NURTURE
CHEMISTRY
Contents
Serial
No.
TOPIC NAME
Page
No.
1.
Mole Concept
1-24
2.
Atomic Structure
25-40
3.
Periodic Table
41-56
4.
Chemical Bonding
57-88
5.
Gaseous State
6.
Redox
109-124
7.
Iupac 2022
125-154
8.
GOC
155-182
9.
Thermodynamics & Thermochemistry
183-206
10.
Chemical Equilibrium & Ionic
207-230
11.
SB,PB,HC
231-258
12.
Isomerism
259-286
89-108
Mole Concept
MOLE CONCEPT
CLASSICAL COMBINATION LAWS
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
SINGLE CORRECT ANSWER TYPE
In the reaction N2(g) + 3H2(g) ¾¾® 2NH3(g), ratio by volume of N2, H2 and NH3 is 1 : 3 : 2 at
same condition of temperature and pressure. This illustrates law of (A) Definite proportion
(B) Multiple proportion
(C) Conservation of mass
(D) Gaseous volumes
Hydrogen and oxygen combine to form H2O2 and H2O containing 5.93% and 11.2% Hydrogen
respectively. The data illustrates(A) Law of conservation of mass
(B) Law of constant proportions
(C) Law of gaseous volume
(D) Law of multiple proportions
Different proportions of oxygen in the various oxides of nitrogen prove the law of (A) Gaseous volume
(B) Multiple proportion
(C) Constant proportion
(D) Conservation of matter
Select incorrect statement
(A) Element can't be decomposed into simpler substances by chemical methods
(B) Compound can be decomposed into simpler substances by chemical methods.
(C) Mixture may have uniform composition
(D) (Petrol + water) form homogenous mixture.
If water samples are taken from sea, rivers, clouds, lake or snow, they will be found to contain
H2 and O2 in the fixed ratio of 1 : 8. This indicates the law of (A) Multiple proportion
(B) Definite proportion
(C) Gaseous volume
(D) None of these.
Law of definite proportion when expressed in terms of volumes becomes (A) Dalton's law
(B) Boyle's law
(C) Gay-Lussac's Law
(D) Avogadro's law
The law of conservation of mass holds good for all of the following except (A) All chemical reactions
(B) Nuclear reactions
(C) Endothermic reactions
(D) Exothermic reactions
Law of multiple proportion can be verified by following compounds (A) CO2, CH4, H2O
(B) N2O, N2O3, N2O5
(C) NaCl, Na2CO3, NaOH
(D) H2O, HCl, NaCl
A sample of calcium carbonate (CaCO3) has the following percentage composition : Ca = 40%,
C = 12%, O = 48%. If the law of constant proportions is true, then the weight of calcium in 4 g of a
sample of calcium carbonate obtained from another source will be
(A) 0.016 g
(B) 0.16 g
(C) 1.6 g
(D) 16 g
If law of conservation of mass was to hold true, then 20.8 g of BaCl2 on reaction with 9.8 g
of H2SO4 will produce 7.3 g of HCl and BaSO4 equal to (A) 11.65 g
(B) 23.3 g
(C) 25.5 g
(D) 30.6 g
1
JEE-Chemistry
PROBLEMS ON MOLE CALCULATION
SINGLE CORRECT ANSWER TYPE
1.
What is the of mass of 200 oxygen
(A) 3200 amu
2.
9.
13.
(B) 6.023 × 1026
(C) 6.023 × 1024
(D) 6.023 × 1023
(B) 75
(C) 74
(D) 73
(B) 6.023 × 105 amu
(C) 6.023 × 106 amu
(D) 6.023 × 107 amu
(B) 0.166 × 10–4
(C) 1.66 × 10–4
(D) 0.166 × 10–5
(D) 8.023 × 1012 molecules
Mass of 18.069 × 1023 molecule of O3 is
(B) 14.4 g
(C) 72 g
(D) 48g
(C) 1.505 × 105
(D) 1.2046 × 1013
(C) 30
(D) 60
Number of He atom in 10–10 g sample is
(B) 1.505 × 1013
Number of moles of H2O in 1080 g is
(B) 108
Four containers of 2L capacity contains dinitrogen as described below. Which one contains
maximum number of molecules under similar conditions.
(A) 2.5 g-molecules of N2
(B) 4 g-atom of nitrogen
(C) 3.01 × 1024 N atoms
(D) 84 g of dinitrogen
A person counts 1coin/sec. How many years it will take for him to count 0.5 mole coins ?
(B) 8.56 × 1015 yrs
(C) 7.56 × 1015 yrs
(D) 6.56 × 1015 yrs
What is the total number of cations present in 196g of Mohr’s salt [(NH4)2SO4.FeSO4.6H2O] on
dissolving it in water ?
(A) 1.3NA
15.
(D) 6.023 × 1020.
(C) 7.024 × 1012 molecules
(A) 9.56 × 1015 yrs
14.
(C) 6.023 × 1018
(B) 6.023 × 1012 molecules
(A) 54
12.
(B) 6.023 × 1019
(A) 5.023 × 1012 molecules
(A) 1.2046 × 105
11.
(D) 6.312 × 10–20g
How many molecules of H2SO4 weigh 9.8 × 10–10g.
(A) 144 g
10.
(C) 6.312 × 10–22g
How many mole are present in 1020 atoms ?
(A) 0.166 × 10–2
8.
(B) 5.312 × 10–22g
What is the mass of 10–20 mole CaCO3 in amu ?
(A) 6.023 × 107 amu
7.
(D) 400 amu
If mass of single atom of an element is 1.245 × 10–22 g. Find the atomic mass of element
(A) 76
6.
(C) 800amu
How many amu are present in 1kg mass ?
(A) 6.023 × 1025
5.
(B) 1600 amu
How many amu are present in 10–3 g ?
(A) 6.023 × 1017
4.
O isotope in amu ?
What is the mass of 20 oxygen atom in g ?
(A) 1.0624 × 10–21g
3.
16
8
(B) 1.4NA
(C) 1.5NA
(D) 1.2NA
How many mole of protons are present in 90g of H2O ?
(A) 50 mole
(B) 60 mole
(C) 70 mole
2
(D) 40 mole
Mole Concept
PERFECTION IN UNITARY MATHOD
SINGLE CORRECT ANSWER TYPE
1.
How many gram of carbon is present in 560 g of CaCO3 ?
(A) 65.2 g
2.
(C) 129 g
(D) 130 g
(B) 85.5
(C) 86.5
(D) 87.5
(B) 200 g
(C) 500 g
(D) 600 g
13.4 g of Na2SO4.xH2O gives 6.3 g H2O on strong heating. What is the value of x ?
(A) 6
6.
(B) 128 g
How much CaCO3 can be prepared by 280 g of CaO ?
(A) 300 g
5.
(D) 68.2 g
How many gram of KClO4 contain 40 g oxygen ? [Given : M.M. of KClO4 = 138.5]
(A) 84.5
4.
(C) 67.2 g
How many g of oxygen is needed to prepare 284 g of Na2SO4 ?
(A) 126 g
3.
(B) 66.2 g
(B)7
(C) 8
(D) 9
Calculate no of kilogram of Cu in 3.67 × 103 kg of CuFeS2 (chalcopyrite)
[Given : Atomic mass of Cu =63.5, Fe = 56, S = 32]
(A) 1230
7.
(C) 1270
(D) 1260
What is the formula of hydrated salt of barium chloride if 36.6 g of salt on strong heating gives
5.4 g H2O ? [Given : Atomic mass of Ba = 137]
(A)BaCl2.7H2O
8.
(B) 1250
(B) BaCl2.2H2O
(C) BaCl2.3H2O
(D) BaCl2.5H2O
What is the mass of H2O present in 499 g of CuSO4.5H2O ?
(A)180 g
(B) 170 g
(C) 150 g
(D) 160 g
MULTIPLE CORRECT ANSWER TYPE
9.
In 40 g of Fe2O3 [Fe = 56] mass of
(A) Fe is 28 g
10.
(B) Oxygen is 12 g
(C) Fe is 8 g
A sample of MgSO4 is found to contain 8 × 1020 atoms of O.
(A) Mass of S present in the sample is 1.06 × 10–2 g
(B) Number of Mg atoms in the sample is 8 × 1020
(C) Total number of atoms in the sample is 1.2 × 1021
(D) Mass of Mg present in the sample is 1.06 × 10–6 g
3
(D) Oxygen is 32 g
JEE-Chemistry
PROBLEMS ON AVERAGE ATOMIC MASS,
AVERAGE MOLECULAR MASS & VAPOUR DENSITY
SINGLE CORRECT ANSWER TYPE
1.
A mixture of blue & green balls contains 25% by number blue balls. Mass of each blue ball is 40 g &
mass of each green ball is 20 g. Calculate
(i)
average mass of ball
(A) 22
(ii)
(B) 40
(C) 21
Find average atomic weight of a mixture containing 25% by mol
(A) 36.55
3.
(C) 27
(D) 28
% by mass of blue ball
(A) 30
2.
(B) 25
(B) 36.52
(D) 60
Cl35
& 75% by mol Cl37.
(C) 36.58
The mass spectrum of carbon shows 98.9% by mole carbon atoms are
(D) 36.50
12
6
C (12.000 amu) and 1.1%
by mole is 13
6 C (13.003 amu). What is atomic wt. of naturally occuring carbon.
(A) 12.011 amu
4.
(B) 55%
(C) 50%
(D) 45%
(B) 15% and 85%
(C) 25% and 95%
(D) 35 % and 75%
(B) 28.6
(C) 28.8
(D) 29.2
(B) 0.2
(C) 0.5
(D) 0.8
A mixture of O2 and gas "Y" (mol. wt. 80) in the mole ratio a : b has a mean molecular weight 40.
What would be mean molecular weight, if the gases are mixed in the ratio b : a under identical
conditions ? (gases are non-reacting):
(A) 40
10.
(D) 9.9
The vapour density of a mixture containing NO2 and N2O4 is 27.6. The mole fraction of N2O4 in the
mixture is:
(A) 0.1
9.
(C) 10
The air consist of oxygen and nitrogen gases. The composition of air is O2 = 20% and N2 is 80% by
mole (approximately). Find average molecular weight of air.
(A)29.5
8.
(B) 9.8
If an element have average atomic mass 51.7, find %age abundance of element having mass
number 50 and 52 respectively.
(A) 10% and 75%
7.
(D) 14.011 amu
Natural Silver exist in two isotopic forms, Ag107 & Ag109 . The average atomic mass of Silver is
108.1. Find % by mole of Ag107 isotope.
(A) 35%
6.
(C) 10.011 amu
Natural Boron exist in two isotopic forms, B11 & BA . The isotopic abundances are 80% and 20%
respectively. The average atomic mass of Boron is 10.8. Find A
(A) 9.7
5.
(B) 11.011 amu
(B) 48
(C) 62
(D) 72
Calculate density of a gaseous mixture which consist of 3.01 ´ 1024 molecules of N2 and 32 g of O2
gas at 3 atm pressure and 860 K temperature (Given : R = 1/12 atm L/mole.K)
(A) 0.6 g/L
(B) 1.2 g/L
(C) 0.3 g/L
4
(D) 12 g/L
Mole Concept
PROBLEMS ON EMPIRICAL FORMULA, MOLECULAR
FORMULA & % COMPOSITION
SINGLE CORRECT ANSWER TYPE
1.
The simplest formula of a compound containing 50% of element X (atomic mass 10) and 50%
element Y (atomic mass 20) by weight is
(A) X3Y
2
(B) X2Y3
(C) X2Y
(D) X4Y
Given that an organic compound has the following % composition by mass :
C = 60%, O = 32%, H = 8%
Find empirical formula of the compound.
(A) C5H12O2
3.
(B) C5H5ON2
(C) C2H3O2N
(D) C3H7ON
(B) M3N2
(C) M3N5
(D) M3N
A compound containing C,H & O was found to contain 40% C & its molecular formula mass was
equal to 60 amu. The ratio of no. of atom of ‘H’ to ‘O’ atom is 2 : 1. Find E.F. of the compound.
(A) C2H2O
6.
(D) C5H10O2
When 0.273 g of M is heated strongly in N2 gas atmosphere, a chemical reaction occur. The
product of reaction weigh 0.378 g. What is the empirical formula of the compound ? ( M = 24)
(A) M2N3
5.
(C) C5H8O2
Elementary analysis showed that an organic compound containing C,H,N,O and weighing 7.3 g was
found to contain 3.6 g carbon, 0.7 g hydrogen and 1.4 g nitrogen. Find empirical formula.
(A) C3H7NO2
4.
(B) C5H8O
(B) CH4O2
(C) CH2O
(D) C2H4O
A compound of nitrogen & oxygen was found to contain 7 : 16 by mass N & O respectively. Caculate
molecular formula if vapour density is 46.
(A) N2O5
(B) NO2
(C) N2O4
(D) N2O3
7.
Calculate the empirical formula of the minerals that have the following compositions by mass :
(i)
ASO4 = 28%, H2O = 72% [At.wt. of A = 16 ]
(A) ASO3. 16H2O ,
(ii)
8.
(A) 3EO.DO2.2H2O
(B) EO.DO2.5H2O
(C) 2EO.DO2.3H2O
(D) EO.DO.H2O
(B) CH4
(C) CH2
(D) CH
The mass % of O in monovalent metal carbonate is 48%. Find the atomic mass of metal
(B) 20
(C) 30
(D) 40
If mass % of CO2 in a bivalent metal carbonate is 25%, find the atomic mass of metal
(A) 90
11.
(D) 3ASO4. 4H2O ,
Find the empirical formula of a hydrocarbon, 1.4 g of which on complete combustion give 4.4 g CO2 and
1.8 g H2O.
(A) 10
10.
(C)ASO4. 16H2O ,
EO = 25% , DO2 = 25%, H2O = 50% [At. wt. of E = 29 ; D = 13]
(A) CH3
9.
(B) ASO4. 12H2O
(B) 140
(C) 120
(D) 116
The mass % of Na in a compound is 11.5%. What is the minimum molecular mass of compound.
[Na = 23]
(A) 100g/mole
(B) 150 g/mole
(C) 50 g /mole
5
(D)200g /mole
JEE-Chemistry
12.
A 0.492g sample of hemoglobin contain 0.34% by mass Fe. If each Hb contain 4Fe atom. What is the
molecular mass of Hb ?
(A) ~61000
13.
(B) ~65000
(C) ~63000
(D) ~62000
The formula of a metal chloride is MCl 2. If it contains 63.96% by mass chlorine. Find the atomic mass
of metal
(A) 30; Na
(B) 20; Ca
(C) 40; Ca
(D) 43; Na
MULTIPLE CORRECT ANSWER TYPE
14.
An organic compound of molar mass greater than 100 contain C, H and N. The % of C is 6 times %
of H while sum of % of C and H is 1.5 time % of N.
(A) Empirical formula of compound is C3H6N2
(B) Least molar mass of compound is 140
(C) Empirical formula mass of compound is 70
(D) Least molar mass of compound is 130
15.
A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's
density is 2.24 g/litre at 300 K and 1.0 atm pressure.
(A) The molecular formula of the compound is C4H8
(B) Empirical formula of compound is C2H4
(C) Vapour Density of compound is 28
(D) Density of the compound relative to methane (CH4) gas is 3.5 in the given condition.
6
Mole Concept
CALCULATION BASED ON BALANCED CHEMICAL EQUATION
SINGLE CORRECT ANSWER TYPE
1.
What mass of CO2 gas can be produced by decomposition of 1000g of CaCO3 ?
[Given : Atomic mass of Ca = 40 ]
CaCO3 ¾¾®
CaO + CO2
D
(A) 420 g
2.
(B) 450 g
(C) 440 g
(D) 400 g
How many g of KClO4is produced by 6.125 g of KClO3 according to the reaction
4KClO3(s) ® 3KClO4 (s) + KCl(s) ?
(A) 5.13
3.
(B) 5.234
(C) 5.193 g
(D) 5.17g
If mass of KCl formed in the reaction
KClO4 ® KCl + 2O2 is
1.625 g, how many litres of O2 gas is produced at 1atm and 273K.
(A) 0.977L
4.
(D) 1.42 L
(B) 0.4 mol
(C) 0.03 mol
(D) 0.5 mol
In a rocket motor, fuelled with butane, C4H10, how many kg of liquid oxygen should be provided
with each kg of butane for its complete combustion?
(A) 1.58 Kg
6.
(C) 1.23 L
Calculate the number of mole of calcium chloride needed to react with excess silver nitrate to produce
8.61 g of AgCl. [Given : Molar mass of AgCl = 143.5 g]
(A) 0.2 mol
5.
(B) 1.02 L
(B) 3.50 Kg
(C) 2.58 Kg
(D) 3.58 Kg
Phosphorus react with Cl2 to produce PCl3(l) according to reaction.
P4 + 6Cl2 (g) ® 4PCl3(l)
If the density of PCl3(l) is 1.2g/cc
How many kg of phosphorus is needed to produce 13.75 litres of PCl3(l)
(A) 3.25 kg
7.
(B) 3.75 kg
(C) 3.70kg
(D) 3.72 kg
One litre of mixture of CO and CO2 is passed through red hot charcoal in a tube. The new volume
become 1.4 L. Find out composiiton of mixture by volume.
CO 2 (g) + C(s) ¾¾
® 2CO(g)
8.
(A) CO=60% and CO2 = 40%
(B) CO=50% and CO2 = 30%
(C) CO= 40% and CO2 = 20%
(D) CO=30% and CO2 = 70%
An hourly energy requirement of an astronaut can be satisfied by the energy released when 34 g of
sucrose are burnt in his body. How many g of O2 would he need to carried in space capsule to meet
his requirement for one day ? [ Sucrose = (C12H22O11) ]
(A) 902.2 g
(B) 908.2 g
(C) 916.2 g
7
(D) 910.2 g
JEE-Chemistry
MULTIPLE CORRECT ANSWER TYPE
9.
For the reaction A(s) + 2B(g) ® 3C(g) + D(g);
{A = 100, B = 50, C= 60, D=20}
Select the correct statements :
(A) 7.5 moles of C is produced by reaction of 250 g of A
(B) 500 g of A will completely react with 500g of B
(C) 75g of D is produced in the reaction, then 375 g each of A and B are consumed.
(D) 16.5 mg (approx.) of A is required to produce 11.2 ml of gas C at STP
10.
The decomposition of potasium chlorate can be represented as
KClO3 ¾® KCl + O2 ;
[K = 39, Cl 35.5; O=16]
(A) 3.267 g of KClO3 is necessary to produce 1.28 g of O2
(B) 2.367 g of KClO3 is necessary to produce 1.28 g of O2
(C) 1.98 g KCl is produced along with this quantity of oxygen
(D) 1.2 g KCl is produced along with this quantity of oxygen
8
Mole Concept
PROBLEMS ON LIMITING REAGENT
SINGLE CORRECT ANSWER TYPE
1.
How many mole of O2 is needed to react completely with 6 mole of Al ?
[Given Atomic maas of Al = 27]
Al + O2 ® Al2O3
(A) 4.5 mole
2.
(C) 6.5 mole
(D) 7.5 mole
What mass of Al2O3 is produced in g when 6 mole of Al is treated with excess of O2 ? [Al = 27]
(A) 307 g
3.
(B) 5.5 mole
For the reaction
(B) 306 g
(C) 305 g
(D) 304 g
2A(s) + 3B(g) ® 4C(s)
10 mole each of A and B were taken. What is the composition of product mixture by moles at the end
of reaction ?
4.
(A) 40/3 mole C and 10/3 mole A
(B) 20/3 mole C and 30/2 mole A
(C) 50/2 mole C and 40/3 mole A
(D) 25/2 mole C and 10/2 mole A
What is the number of mole of Fe(OH)3(s) that can be produced by reacting 1 mole Fe2S3, 2 mole of
H2O and 3 mole of O2 ?
Fe2S3 + O2 + H2O ® Fe(OH)3 + SO2
(A) 4/5 mole
5.
(B) 5/2 mole
(D) 5/2 mole
1g of Mg is burnt in a closed vessel containing 0.5g of O2. What is the composition of product
mixture by mass ?
Mg (s) +
6.
(C) 4/3 mole
1
O 2 ( g ) ® MgO(s)
2
(A) 0.5g of Mg; 1g of MgO
(B) 0.3g of Mg; 1.2 g of MgO
(C) 1.2g of Mg; 1.25 g of MgO
(D) 0.25g of Mg; 1.25 g of MgO
How many moles of Br2(l) is required to react completely with 810g Al and what mass of Al2Br6 solid
is formed in this question ?
[Given : Atomic mass of Br = 80]
7.
(A) 45 mole of Br2 ; 8.01 kg of Al2Br6(s)
(B) 40 mole of Br2 ; 6.01 kg of Al2Br6(s)
(C) 35 mole of Br2 ; 4.01 kg of Al2Br4(s)
(D) 15 mole of Br2 ; 3.01 kg of Al2Br6(s)
2.84 g of Na2SO4 is mixed with 1.08 g of C. Assuming complete reaction, find the composition of
product mixture and volume of CO formed at 273K temperature and 1atm pressure.
Na2SO4 + 4C(s) ® Na2S + 4CO(g)
(A) Na2S = 1.56g ; VCO = 1.792L ; C = 0.12g (B) Na2S = 1.76g ; VCO = 1.792L ; C = 0.12g
(C) Na2S = 1.66g ; VCO = 1.892L ; C = 0.12g (D) Na2S = 1.36g ; VCO = 1.692L ; C = 0.12g
8.
A mixture of N2 and H2 is caused to react in a closed container to form NH3. The reaction ceases
before reactants are completely consumed. At this stage 2 mole each of N2, H2 and NH3 are present.
What was the moles of N2 and H2 originally present.
(A) 2 mole N2 and 4 mole H2
(B) 3 mole N2 and 5 mole H2
(C) 4 mole N2 and 2 mole H2
(D) 5 mole N2 and 3 mole H2
9
JEE-Chemistry
MULTIPLE CORRECT ANSWER TYPE
9.
Lithium reacts with oxygen as
[Given : Atomic mass of Li = 7 ; O = 16 ]
2Li(s) + O2 (g) ® Li2O (s)
Assuming reaction to be quantitative if 20g of Li is taken with 30g of oxygen then
(A) 42.85 g of Li2O is formed
(B) Li is completely consumed and it acts as limiting reagent.
(C) O2 acts as limiting reagents
(D) 50/7 g of O2 remains unused.
10
Mole Concept
% PURITY & % YIELD
1.
2.
3.
4.
5.
6.
7.
8.
9.
SINGLE CORRECT ANSWER TYPE
A 0.71 g sample containing chloride is dissolved, and chloride precipitated as AgCl. The precipitate
was washed, ignited and found to weigh 0.287 g.
(a) The % age of chloride in sample is
(A) 10%
(B) 20%
(C) 30%
(D) 15%
(b) The percentage expressed as NaCl is approximately
(A) 12.5%
(B) 16.5%
(C) 18.5%
(D) 24.5%
The sulfur in a 0.80 g sample is converted to sulfate, and sulfur precipitated as BaSO 4. The precipitate
is washed, ignited and found to weigh 0.233 g.
[Given : Atomic mass of Ba = 137, S = 32, O = 16]
(a) The % age of sulfur in the sample is
(A) 4%
(B) 8%
(C) 12%
(D) 16%
(b) The % age expressed as SO3 is
(A) 40%
(B) 20%
(C) 30%
(D) 10%
The calcium in 0.80 g sample is precipitated as CaC2O4. The precipitate is washed, dried and ignited
to CaCO3 and found to weigh 0.3 g.
The percentage of CaO in the sample is
(A) 42%
(B) 72%
(C) 21%
(D) 32%
20g of NaCl is added to an aqueous solution containing excess of AgNO3. The AgCl is quantatively
precipitated. If 43.05 g of AgCl solid is obtained upon filteration. What is % purity of NaCl ?
(A) 85.55
(B) 84.5
(C) 87.75
(D) 87.65
10g of KClO4 upon heating gives 2.24L of O2 gas at 1atm and 273K. What is the % purity of KClO4 ?
(A) 65.52%
(B) 69.25 %
(C) 68.20 %
(D) 67.2%
What is the amount of lime (CaO) in moles that can be produced by heating 200 kg lime stone that
95% pure CaCO3 ?
(A) 1.9 × 104 mol
(B) 1.9 × 103 mol
(C) 1.9 × 102 mol
(D) 1.9 × 105 mol
What is the mass of KCl produced from 1 mole of KClO3 if % yield of reaction is 80 ?
KClO3 ® KCl + O2
(A) 59.6 g
(B) 74.5 g
(C) 62.84 g
(D) 48.84 g
The conversion of oxygen to ozone occurs to the extent of 15% only. The mass of ozone that can be
prepared from 67.2 L of oxygen at 1atm and 273K will be 3O2 ® 2O3
(A) 14.4 g
(B) 96 g
(C) 640 g
(D) 64 g
What is the mass of coal sample in kg containing 0.05% by mass of iron pyrite (FeS2) that can
produce 44.8 lit of SO2 1 atm & 273 K with 40% reaction yield ?
FeS2 +
(A) 120 kg
5
O ¾® FeO + 2SO2
2 2
(B) 180 kg
(C) 600 kg
11
(D) 300 kg
JEE-Chemistry
PROBLEMS RELATED WITH SEQUENTIAL REACTION AND
PARALLEL REACTIONS & PROBLEMS RELATED WITH
MIXTURE
SINGLE CORRECT ANSWER TYPE
1.
From the following reaction
2 CoF2 + F2 ® 2CoF3
(CH2)n + 4nCoF3 ® (CF2)n + 2nHF + 4nCoF2
Calculate how much F2 will be consumed to produce 1kg of (CF2)n.
(A) 1.52 kg
2.
(B) 1.50 kg
(C) 1.47 kg
(D) 1.48 kg
Sulphur trioxide may be prepared by the following two reactions :
S8 + 8O2(g) ® 8SO2(g)
2SO2(g) + O2(g) ® 2SO3(g)
How many grams of SO3 will be produced from 1 mol of S8?
(A) 160 g
3.
(B) 640 g
(C) 80 g
(D) 512 g
How many g of H2SO4 can be obtained from 1320 g of PbS. According to given reaction
sequence.
[Assume all other reactants in excess]
2PbS(s) + O2 (g) ® 2PbO(s) + 2SO2
3SO2 + 2HNO3 + 2H2O ® 3H2SO4 + 2NO
[Pb = 208]
(A) 539g
4.
(B) 535g
(C) 549 g
(D) 545 g
From the following series of reaction
What is the mass of chlorine needed to produce 27.7g of KClO4 ?
Cl2 + 2KOH ® KCl + KClO + H2O
3KClO ® 2KCl + KClO3
4KClO3 ® 3KClO4 + KCl
(A) 55.5 g
5.
(C) 56.8 g
(D) 57.6 g
If % yield of 2nd step of above sequence of reaction (previous question) is 50%. Calculate the mass
of chlorine needed
(A) 113.6g
6.
(B) 53.4 g
(B) 112.5g
(C) 110.5 g
(D) 112.5 g
For the following sequence of reaction
5A + 6B ® 2C
3C + 4D ® 2E
5E + 6F ® 2G
If, B, D and F are in excess . How many mole of A is required to produce 100 mole G. The % yield
of 1st, 2nd and 3rd reaction are 50%, 60% and 50% respectively.
(A) 3450 mol
(B) 6350 mol
(C) 6250 mol
12
(D) 2220 mol
Mole Concept
7.
If 6 moles of KClO3 are decomposed according to following reactions calculate the moles of KClO4
produced if moles of O2 produced is 1.
KClO3 ¾¾
® KCl + 3/2 O2
4KClO3 ¾¾
® 3KClO4 + KCl
(A) 2 mole
8.
(B) 4 mole
A2 + 2B2 ¾® A2 B4
(C) 3 mole
(D) 5 mole
3
A + 2B2 ¾® A3 B4
2 2
and
Two substance A2 & B2 are allowed to react completely to from A2B4 & A3B4 mixture of leaving
none of the reactants. Using this information calculate the composition of final mixture when mentioned
amount of A2 & B2 are taken.
(i)
If
5
moles of A2 & 2 moles of B2 is taken
4
(A) A3B4 = 0.2 mole, A2B4 = 0.3 mole
(C) A3B4 = 0.5 mole, A2B4 = 0.5 mole
(ii)
If
(B) A3B4 = 0.8 mole, A2B4 = 0.7 mole
(D) A3B4 = 0.4 mole, A2B4 = 0.6 mole
7
moles of A2 & 6 moles of B2 is taken
2
(A) A3B4 = 1 mole, A2B4 = 2
(C) A3B4 = 2 mole, A2B4 = 4
(B)A3B4 = 2 mole, A2B4 = 1
(D) A3B4 = 4 mole, A2B4 = 1
(iii) If 4 moles of A2 & 6 moles of B2 is taken
(A) A3B4 = 2 mole, A2B4 = 3
(B) A3B4 = 2 mole, A2B4 = 1
(C) A3B4 = 4 mole, A2B4 = 1
(D) A3B4 = 3 mole, A2B4 = 2
9.
Four grams of a mixture of calcium carbonate and sand is treated with an excess of hydrochloric acid
and 0.88 gm of CO2 is produced. What is the percentage of CaCO3 in the original mixture?
(A) 40%
(B) 50%
(C) 30%
(D)20%
10. A 5.00 gm sample of a natural gas, consisting of methane CH4, and ethylene, C2H4 was burned in
excess oxygen, yielding
11.
44
gm of CO2 and some H2O as products. What mole % of the sample was
3
ethylene?
(A) 66.66
(B) 25
(C) 50
(D) 33.33
A mixture of NaCl (molecular weight M1) and KCl (molecular weight M2) weighing w1 gm was
treated with aqueous solution of AgNO3 (excess). The resulting AgCl (molecular weight M3) weighed
w2 gm. What was the mass fraction of NaCl in the mixture?
w 2 M1M 2 - w1M1M 3
(A) w (M M - M M )
1
2
3
1
3
w 2 M1M 3 - w1M1M 2
(B) w (M M - M M )
1
2
3
1
3
w 1M1M 3 - w1M1M 2
(C) w (M M - M M )
2
2
3
1
3
w 2 M1M 2 - w1M1M 3
(D) w (M M - M M )
1
1
3
2
3
13
JEE-Chemistry
PROBLEMS ON POAC
SINGLE CORRECT ANSWER TYPE
1.
A sample of K2CO3 weighing W1 g undergoes a series of reactions so as to convert all carbon atom
to K2Zn3[Fe(CN)6]2. How many g of this product were obtained?
[Mol. wt. K2CO3 ¾® M1, mol wt. K2Zn3 [Fe(CN)6]2 = M2]
12M1
(A) W M
1
2
2.
4.
(B) w CO2 = 528g
(C) w CO2 = 520g
(D) w CO2 = 525g
(B) CO2 = 3 moles; CO = 1 mole
(C) CO = 2 moles; CO = 3 moles
(D) CO2 = 1 mole; CO = 1 mole
5 mole of P and 4 mole of O2 are mixed together - they react completely to form P2O5 and P2O3. Find
the mole of P2O5 and P2O3 formed respectively(B) 1 ; 2
(C) 2 ; 2.25
(D) 0.25 ; 2.25
Equal mass of Hg and I 2 are allowed to react completely to form a mixture of Hg2I2 and HgI2.
Leaving none of the reactant, calculate ratio of mole of Hg2I2 and HgI2 formed.
54
246
(B)
54
146
(C)
54
446
(D)
454
654
Equal mass of phosphorus and oxygen are heated in a closed vessel, producing P2O3 and P2O5 in
1 : 1 mole ratio. Find out which component is in excess, and what fraction of excess reagent is left.
(A) O; 6.25%
7.
W1M 2
(D) 12M
1
(A) CO2 = 4 moles; CO = 2 moles
(A)
6.
W1M1
(C) 12M
2
When 2 moles C and 1.5 moles O2 reacted, no residue remained. Find the composition of product.
(A) 2.5 ; 1.5
5.
12WM
1 2
M1
All carbon atom present in KH(C2O4).2H2O weighing 984 g is converted to CO2. How many g of
CO2 were obtained.
(A) w CO2 = 510g
3.
(B)
(B) P; 3.125%
(C) O; 3.125%
(D) P ; 6.25%
Calculate the percentage of P in an organic compound, if 45.6 g of this compound is subjected to
react first with HNO3 and then with (NH 4) 2 MoO 4, it produced 375.4 g of Ammonium
phosphomolybdate [(NH4)3PO4.12MoO3].
[Given : Atomic mass of Mo = 96; P = 31;]
(A) 20.3%
(B) 13.6%
(C) 23.6 %
14
(D) 73%
Mole Concept
CONCENTRATION TERMS
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
SINGLE CORRECT ANSWER TYPE
A sample contains 8gm H2, 64 gm O2 and 34 gm NH3. Calculate mole fractions of each.
(A) X O 2 = 0.30, X H 2 = 0.40, X NH3 = 0.30
(B) X O 2 = 0.20, X H 2 = 0.60, X NH3 = 0.20
(C) X O 2 = 0.25, X H 2 = 0.50, X NH3 = 0.25
(D) X O 2 = 0.40, X H 2 = 0.30, X NH3 = 0.30
Calculate mmole(millimole) of H2SO4 present in 500mL of 0.2M H2SO4
(A) 50 mmole
(B) 200 mmole
(C) 100 mmole
(D) 150 mmole
What mass of NaNO3 is needed to prepare 250mL of 0.7M solution ?
(A) 12.875
(B) 13.875
(C) 14.875
(D) 11.875
Calculate the molarity of water. Given density of water = 1 gm/mL.
(A) 55.55 M
(B) 52.55 M
(C) 45.55 M
(D) 40.55 M
Calculate the molality of water. Given density of water = 1 gm/mL.
(A) 55.55 m
(B) 52.55 m
(C) 45.55 m
(D) 40.551 m
If mole fraction of C2H5OH is an aqueous solution is 0.4, find molality of solution.
(A) 36
(B) 39
(C) 38
(D) 37
Molarity of 98% (by mass) of H2SO4 having density 1.75 gm /cc is
[ Consider H2SO4 is solute ]
(A) 14.5 M
(B) 17.5M
(C) 16.5M
(D) 15.5M
What is the molality of a solution which is 10% (w/w) NaOH ?
(A) 2.57 m
(B) 2.67 m
(C) 2.70 m
(D) 2.77 m
A solution of NaOH is 20% (w/w). What is the molarity of solution if the density of solution is
1.2 gm/cc ?
(A) 5M
(B) 4M
(C) 3M
(D) 6M
What is the molarity of a 10% (w /v) solution of NaOH ?
(A) 4.5M
(B) 3.5M
(C) 2.5M
(D) 3.5M
Establish a relation ship between M, m, dsolution in gm/mL and MA (mol. wt. of solute).
(A)
12.
13.
d
1
MA
=
+
M m 1000
(B)
d
1
M
=
+ A
M m 100
(C)
d
1
M
=
– A
M m
10
(D)
d
1
M
=
+ A
M m
10
MULTIPLE CORRECT ANSWER TYPE
Concentration of 2M CH3COOH with density 1.2 gm/cc in terms of
(A) % (w/w) is 10 % (B) % (w/v) is 12 % (C) molality is 1.85
(D) molality is 1.65
If 40 gm MgO was dissolved in water to form 200 mL of solution, density of solution becomes
1.5 gm/mL, then select the correct statement(s)
(A)
w
40
% & % by mass of the MgO solution are 20% &
% respectively
v
3
(B) molarity of MgO solution is 5M
(C) molality of MgO solution is 3.85 m
(D) mole fraction of solute is 0.065
15
JEE-Chemistry
14.
Select correct statement(s) :
(A) If concentration of CaCO3 is 20 ppm, then molarity of solution is 2 × 10–4 M.
(B) If molarity of MgCO3 solution is 5 × 10–4 M, then its concetration in ppm is 42.
(C) If concentration of NaOH solution is 4 × 10–5 M, then its concentration in ppb is 1600.
(D) Molarity of 4% w/v of NaOH solution is 1 M.
16
Mole Concept
MOLARITY AND MOLALITY OF IONIC COMPOUNDS / ACIDS /
BASES & MIXING OR DILUTION OF SOLUTIONS
SINGLE CORRECT ANSWER TYPE
1.
2.
Find the molarity of various ions in 0.1 M BaCl2 solution, considering degree of dissociation of
BaCl2 as 80%.
(A) [Ba+2] = 0.03M, [Cl¯] = 0.2 M
(B) [Ba+2] =0.08M, [Cl¯] = 0.16 M
(C) [Ba+2] = 0.02M, [Cl¯] = 0.2 M
(D) [Ba+2] = 0.04M, [Cl¯] = 0.8 M
Calculate ‘m’ of all the ions present in the solution of Al2(SO4)3 for 1M solution.
Given dsolution = 2.342 gm/mL.
(A) 2.5 m
(B) 1.25 m
(C) 1.3 m
(D) 1.2 m
3.
A solution is made by mixing 300 mL of 1.5 M Al2(SO4)3, 300 mL 2M CaSO4 and 400 mL 3.5 M
CaCl2.
(i)
What is the total molarity of SO 24 - ion in solution ?
(A) 4.70 M
(ii)
(C) 1.95 M
(D) 1.88 M
(C) 4.25 M
(D) 4 M
(C) 2M
(D) 2.9 M
What is the molarity of anions in solution ?
(A) 4.50 M
(iii)
(B) 1.90 M
(B) 4.75 M
What is the molarity of cations in the solution ?
(A) 2.6 M
(B) 2.8M
4.
200 mL of 1M HCl solution is mixed with 800 mL of 2M HCl solution.
(i)
Calculate the final molarity of the solution.
(A)1.4 M
(ii)
(D) 1.9 M
(B) 1.59 m
(C) 1.69 m
(D)1.65 m
A sample of H2SO4 (density 1.8 g/mL) is 98% by wt. What is the volume of acid that has to be taken
to make 0.2M H2SO4 1L solution ?
(A) V = 12.12 mL
6.
(C)1.8 M
If density of final solution is 1.2 g/mL. Calculate molality ‘m’
(A) 1.62 m
5.
(B)1.5 M
(B) V = 11.11 mL
(C) V = 12.11 mL
(D) V = 10.10 mL
100 mL of 0.1 M Al2 (SO4)3 is mixed with 100 mL of 0.1M AlCl3 solution. Calculate ‘M’ of Al3+ ion
if final solution has density 1.2 g/mL.
(A) 0.14M
(B) 0.15M
(C) 0.14M
7.
Find molarity of following solutions of H2SO4.
(i)
500 mL of 0.1 M H2SO4 is mixed with 500 mL of 0.2 M H2SO4
(A) 0.15 M
(B) 0.25 M
(C) 0.35 M
(D) 0.13M
(D) 0.45 M
(ii). 4.9 g H2SO4 is mixed with 250 mL 0.1 M H2SO4 and 250 mL water is added in resulting solution
(A) 0.20 M
8.
(B) 0.15 M
(C) 0.25 M
(D) 0.35 M
How many mL of two H2SO4 solutions A and B having molarity 1 M and 2 M respectively should be
mixed to produce 1.75L of exactly 1.75M H2SO4
(A) A : 527.5 mL ; B 1352.5 mL
(B) A : 437.5 mL ; B 1312.5 mL
(C) A : 407.5 mL ; B 1302.5 mL
(D) A : 307.5 mL ; B 1212.5 mL
17
JEE-Chemistry
9.
How much water should be added to prepare 1L of 0.646 M HCl starting with 2 M HCl solution.
(A) 677 mL H2O
10.
(C) 627 mL H2O
(D) 570 mL H2O
How much water should be added to 505 mL of 1.25 M HCl to make it exactly 1 M.
(A)126.35 mL
11.
(B) 607 mL H2O
(B) 126.25 mL
(C) 125.25 mL
(D) 123.25 mL
12.6 g of oxalic acid dihydrate was taken in a beaker and water is filled up to 250mL mark.
(a) 10mL of this solution is now taken and diluted to 100mL
(b) Find the number of oxalic acid molecules in 1mL of final solution.
(A) 2.41 × 1019 molecules
(B) 4.40 × 1010 molecules
(C) 2.38 × 1018 molecules
(D) 3.45 × 1012 molecules
12.
There are two stock solution of H2SO4 of molarity 1M and 2M (A and B respectively). What volume
of A and B should be taken to prepare -
(i)
1.5 L of 1.5 M H2SO4
(ii)
(A) 750 mL of A; 750 mL of B
(B) 1000 mL of A; 500 mL of B
(C) 500 mL of A; 100 mL of B
(D) 1250 mL of A; 250 mL of B
2 L of 1.75 M H2SO4
(A) 500 mL of A; 1500 mL of B
(B) 1500 mL of A; 500 mL of B
(C) 1000 mL of A; 1000 mL of B
(D) 1200 mL of A; 800 mL of B
18
Mole Concept
PROBLEMS INVOLVING PRECIPITATION & PROBLEMS
INVOLVING H2O2 & PROBLEMS INVOLVING OLEUM
SINGLE CORRECT ANSWER TYPE
1.
2.
If 200 mL. of 0.1 M NaCl is mixed with 100 mL of 0.2 M AgNO3 solution. Calculate molarity of all
the ions in the final solution.
(A) [Na+] = 0.060 M, [ NO 3- ] = 0.062 M
(B) [Na+] = 0.060 M, [ NO 3- ]= 0.067 M
(C) [Na+] = 0.067 M, [ NO3- ]= 0.067 M
(D) [Na+] = 0.065 M, [ NO3- ]= 0.063 M
What volume of 0.75M Pb(NO3)2 is required to react completely with 175mL of 1.5M NaCl
solution.
Pb(NO3)2 + 2NaCl (aq) ® PbCl2(s) + 2NaNO3(aq)
(A) 160mL
3.
(C) 3 M
(D) 5 M
(B) 6.81 V
(C) 11.35 V
(D) 34.5 V
(C) 5.675 M
(D) 11.35 M
(B) 2 M
What is the percentage strength (% w/V) of 11.35 V H2O2?
(A) 1.7
7.
(B) 6 M
What is the molarity of 11.35 V of H2O2?
(A) 1 M
6.
(D) 175mL
500mL of an aqueous H2O2 solution given out 3405 mL of O2 gas at 1 bar and 273K. What is the
volume strength of H2O2 solution ?
(A) 22.7 V
5.
(C) 140mL
What is the molarity of an aqueous H2O2 solution having volume strength 68.1 V ?
(A) 0.6 M
4.
(B) 150mL
(B) 3.4
(C) 34
(D) None of these
What is the % of free SO3 in an oleum that is labelled as '104.5% H2SO4' ?
(A) 10
(B) 20
(C) 40
(D) None of these
8.
Calculate composition of the final solution if 100 g oleum labelled as 109% is added with
(i)
9 g water
(ii)
(A) pure H2SO4 = 109 g; SO3 = 0 g
(B) pure H2SO4 =105 g; SO3 = 4 g
(C) pure H2SO4 =100 g ; SO3 = 3 g
(D) pure H2SO4 = 90 g; SO3 = 18 g
18 g water
(A) 102 g H2SO4, 16 g H2O;
(B) 109 g H2SO4, 9 g H2O;
(C) 118 g H2SO4, 0 g H2O;
(D) 111 g H2SO4, 7 g H2O;
(iii) 120 g water
9.
(A) 111 g H2SO4, 109 g H2O
(B) 110 g H2SO4, 110 g H2O
(C) 109 g H2SO4, 111 g H2O
(D) 108 g H2SO4, 112 g H2O
9.0 g water is added into 100 g oleum sample labelled as “112%” H2SO4 then the amount of free
SO3 remaining in the solution at 1 atm and 273 K is :
(A) 14.93 L at STP
(B) 7.46 L at STP
(C) 3.73 L at STP
19
(D) 11.2 L at STP
JEE-Chemistry
10.
(i) 18 g water is mixed in 200 g of oleum containing 80% free SO3. What is new labelling of
Oleum ?
(A) ~102%
(B) 108%
(C) ~118%
(D) ~120%
(ii) % of new oleum solution if 6 g water is added to 100 g oleum labelled as 109% is :
(A) 100.52 %
11.
(B) 50.30 %
(C) 102.83 %
(D) 110.5 %
50 g of 104.5% Oleum is mixed with 150 g of 109%. What is the new labeling of resulting Oleum
sample
(A) 113.5%
(B) 108.7 %
( C) 106.75%
20
(D) 107.8%
Mole Concept
ANSWER KEY
CLASSICAL COMBINATION LAWS
1.
(D)
2.
(D)
3.
(B)
4.
(D)
7.
(B)
8.
(B)
9.
(C)
10.
(B)
5.
(B)
6.
(C)
PROBLEMS ON MOLE CALCULATION
1.
(A)
2.
(B)
3.
(D)
4.
(B)
5.
(B)
6.
(B)
7.
(C)
8.
(B)
9.
(A)
10.
(B)
11.
(D)
12.
(D)
13.
(A)
14.
(C)
15.
(A)
6.
(C)
PERFECTION IN UNITARY MATHOD
1.
(C)
2.
(B)
3.
(C)
4.
(C)
5.
7.
(B)
8.
(A)
9.
(A) (B)
10.
(A) (C)
(B)
PROBLEMS ON AVERAGE ATOMIC MASS,
AVERAGE MOLECULAR MASS & VAPOUR DENSITY
1.
(i) (B)
(ii)
(B)
2.
(D)
3.
(A)
4.
6.
(B)
7.
(C)
8.
(B)
9.
(D) 10.
(B)
(C)
5.
(D)
PROBLEMS ON EMPIRICAL FORMULA, MOLECULAR
FORMULA & % COMPOSITION
1.
(C)
2
7.
(i) (C) (ii) (B)
12.
(B)
13.
(C)
(C)
3.
(D)
4.
(B)
5.
(C)
6.
(C)
8.
(C)
9.
(B)
10.
(D)
11.
(D)
14.
(A) (B) (C)
15.
(A)(C) (D)
CALCULATION BASED ON BALANCED CHEMICAL EQUATION
1.
(C)
2.
(C)
3.
(A)
4.
7.
(A)
8.
(C)
9.
(A) (B) (C) (D)
(C)
5.
(D)
10.
(A) (C)
6.
(D)
6.
(A)
9.
(C)
PROBLEMS ON LIMITING REAGENT
1.
(A)
2.
(B)
3.
(A)
4.
7.
(A)
8.
(B)
9.
(A) (B) (D)
5.
(D)
(b) (D)
3.
(C)
(A)
8.
(A)
(C)
% PURITY & % YIELD
1.
(a)
(A) (b) (B)
2.
(a)
4.
(C)
5.
6.
(B)
(B)
(A) 4%
7.
21
JEE-Chemistry
PROBLEMS RELATED WITH SEQUENTIAL REACTION AND
PARALLEL REACTIONS & PROBLEMS RELATED WITH
MIXTURE
1.
(A)
2.
(B)
3.
7.
(B)
8.
(i)(C) (ii)
(A) (iii)(B)
(A)
4.
(C)
5.
(A)
6.
(C)
9.
(B)
10.
(D)
11.
(A)
5.
(B)
6.
(B)
6.
(D)
PROBLEMS ON POAC
1.
(D)
7.
(B)
2.
(B)
3.
4.
(D)
(D)
CONCENTRATION TERMS
1.
(C)
2.
(C)
3.
(C)
4.
(A)
5.
(A)
7.
(B)
8.
(D)
9.
(D)
10.
(C)
11.
(A)
12.
(A)(B) (C) 13.
14.
(A) (B) (C) (D)
(A) (B) (C) (D)
MOLARITY AND MOLALITY OF IONIC COMPOUNDS / ACIDS /
BASES & MIXING OR DILUTION OF SOLUTIONS
1.
(B)
2.
(A)
3.
(i) (C) (ii) (B)
5.
(B)
6.
(B)
7.
(i) (A) (ii). (B)
9.
(A)
10.
(B)
11.
(A)
12.
(iii) (D)
(i) (A)
4.
(i)(C) (ii)
8.
(B)
(ii)
(A)
(B)
PROBLEMS INVOLVING PRECIPITATION & PROBLEMS
INVOLVING H2O2 & PROBLEMS INVOLVING OLEUM
1.
(C)
2.
(D)
3.
7.
(B)
8.
(i) (A) (ii) (B) (iii)
11.
(D)
(B)
(C)
22
4.
(B)
5.
(A)
6.
9.
(C)
10.
(i) (B) (ii) (C)
(B)
Mole Concept
Important Notes
23
JEE-Chemistry
Important Notes
24
ATOMIC STRUCTURE
Atomic Structure
THOMSON MODEL, RUTHERFORD MODEL
SINGLE CORRECT ANSWER TYPE
1.
What important conclusion was reached through the study of cathode rays?
(A) Cathode rays were proven to be light rays indicating that atoms were indeed indivisible.
(B) Cathode rays were shown to be positively charged particles indicating that atoms contained
electric charge.
(C) Cathode rays were shown to be neutral particles with mass.
2.
(D) The charge to mass ratio of particles making up cathode rays was constant,
indicating they were fundamental particles found in all matter.
The zinc sulphide glows when cathode ray strike on screen coated with ZnS . This is due to
(I) flouroscence
(II) Phosphoroscence
(III) Both flouroscence and Phosphoroscence
(IV) Induced radioactivity
(A) (I), (II) and (III) (B) (I), and (III)
3.
(C) (I), (III) and (IV) (D) (I), (II), (III) and (IV)
In cathode ray tube, at very low pressure, the glow of light behind anode is due to
(A) flouroscence caused by cathode ray on glass wall
(B) flouroscence caused by cathode ray inside the tube
(C) phosphoresence caused by X-rays
4.
(D) flouroscence caused by movement of big cation.
How did Thomson establish whether or not cathode rays were light?
(A) He could tell by visual observation.
(B) Thomson knew light rays would be deflected by electric or magnetic fields and he determined
experimentally that they were not deflected.
(C) Thomson knew light rays would not be deflected by electric or magnetic fields and he
determined experimentally that the cathode rays were deflected.
5.
(D) He determined experimentally if the rays would be deflected by gravity; light rays would not
be deflected.
After the existence of the electron was established by Thomson,, Millikan's contribution added
what additional information to atomic theory?
(A) proved electrons had a variable charge.
(B) measured the fixed negative charge of the electron.
(C) proposed the existence of protons.
6.
(D) None of the above.
In a Millikan’s oil drop experiment following charge on oil drop in arbitrary unit was found
–4.8 × 10–19 , –1.6 × 10–19 ; –2.4 × 10–19 ; –4 × 10–19
What is the value of fundamental charge in arbitrary unit ?
(A) 8 × 10–15
(B) 8 × 10–20
(C) 8 × 10–19
25
(D) 8 × 10–18
JEE-Chemistry
7.
9.
10.
11.
12.
13.
14.
After the mass and charge of the electron was known, the next breakthrough in the development
of atomic theory was made by Rutherford. What important result was established by Rutherford?
(A) The atom was of uniform substance containing electrons arranged like raisins in plum pudding.
(B) Rather than being spread out, electrons occupied one half of an atom and the positive charges
occupied the other half.
(C) Electrons disappeared inside an atom. They only existed outside.
(D) All positive charge in an atom was concentrated at a tiny part of the center.
Radius of nucleus of Al is x × 10–15m. Give value of x in the form of nearest integer as 2.2 should
be reported as 2 and 2.8 should be reported as 3. (mass no. Al = 27).
[Given radius of nucleus r = (1.4×10–15) A1/3 m ; where A = mass number of nucleus]
(A) 1
(B) 2
(C) 3
(D) 4
What basis did Bohr have for allowing only specific orbits for electrons in his model of the atom?
(A) Specific orbits were proven experimentally.
(B) Bohr assumed only specific orbits were allowed.
(C) Allowed orbits were predicted from electromagnetic theory.
(D) It was the general harmony of the scientific community.
What is the closest distance of approach of an a-particle of energy 2.5 MeV being scattered by a
gold nucleus (Z = 79) ?
(A) 9.1 × 10–13 meter (B) 9.1 × 10–14 meter (C) 9.1 × 10–15 meter (D) 9.1 × 10–16 meter
The approximate radius of a H-atom is 0.05 nm, and that of proton is 1.5×10–15m. Assuming both
the hydrogen atom and the proton to be spherical, calculate fraction of the space in an atom of
hydrogen that is occipied by the nucleus.
(A) 2.7 × 10–14
(B) 2.7 × 10–10
(C) 5 × 10–14
(D) 2 × 10–16
MULTIPLE CORRECT ANSWER TYPE
Which of the following is/are correct statement(s) according to Rutherford’s atomic model ?
(A) Almost all of the mass of an atom is centered in the nucleus
(B) most of the part inside the atom is empty
(C) the size of nucleus is very small in comparison to the atoms
(D) electrons revolve round the nucleus
The cathode rays experiment demonstrated that
(A) a-perticles are the nuclei of He atoms
(B) the e/m ratio for the particles of the cathode rays varies gas to gas
(C) cathode rays are streams of negatively charge particles
(D) the mass of an atom is essentially all contained its very small nucleus
26
Atomic Structure
ELECTROMAGNETIC RADIATION & PLANCK’S QUANTUM
THEORY
SINGLE CORRECT ANSWER TYPE
1.
Which is true about electromagnetic radiation ?
(I) direction of propagation of electromagnetic wave is perpendicular to electric field.
(II) direction of propagation of electromagnetic wave is both perpendicular to electric and magnetic field vector.
(III) The speed of electromagnetic wave is constant in a given medium.
(IV) The frequency of a monochromatic electromagnetic wave is different in different medium.
(A) II and III
2.
(D) 12400 eV
(B) 3.33
(C) 3
(D) 6
(B) 2.478
(C) 0.068
(D) 0.68
(B) ~32W
(C) ~40W
(D) ~64W
(B) 2 × 104
(C) 2 × 106
(D) 2 × 103
(B)1.72 × 106m–1
(C) 1.70 × 104m–1
(D)1.60 × 106m–1
What is the number of photons emitted by a 60 W bulb in 10 hrs, that emits the light of wavelength
6620 Å.
(A) 7.2 × 1010
10.
(C) 1.240 eV
Yellow light emitted from a sodium lamp has wavelength (l) of 580 nm. Find the wave number
( v ) of the yellow light.
(A)1.92 × 106m–1
9.
(B) 1240 eV
How many photons of wave number 105 cm–1 is equal to 2.48 MeV energy
(A) 2 × 105
8.
(D) 41.4 eV
A light source emit 1020 photons of wavelength 6200Å per second. What is the power output in
Watt ?
(A) ~25W
7.
(C) 4.14 eV
The energy of a photon with n = 1015 Hz is equal to 4.13eV. What is the energy of photon in eV
with n = 6 × 1014 Hz ?
(A) 3.487
6.
(B) 4.14/2 eV
The wave length of an electromagnetic wave is 3720 Å. What is the energy of photon in eV ?
(A) 6.66
5.
(D) I, II and III
The wave number of an emr is 109m–1. What is the energy in eV ?
(A) 12.40 eV
4.
(C) II and IV
The Frequency of an electromagnetic radiation is 2 × 1015 Hz. What is the energy of photon in eV.
(A) 4.14 × 2 eV
3.
(B) II, III and IV
(B) 7.2 × 1020
(C) 7.2 × 1012
(D) 7.2 × 1024
A dye absorbs a photon of wavelength l and re-emits the same energy into two photons of
wavelengths l1 and l2 respectively. The wavelength l, is related with l1 and l2 as :
l1 + l 2
(A) l =
l1 l 2
l1l 2
(B) l = l + l
1
2
(C) l =
27
l12 l 22
l1 + l 2
l1l 2
(D) l = (l + l )2
1
2
JEE-Chemistry
PHOTOELECTRIC EFFECT
SINGLE CORRECT ANSWER TYPE
The photoelectric emission from a surface starts only when the light incident upon the surface
has certain minimum :
(A) intensity
3.
(A) Wavelength of incident light
(B) Frequency of incident light
(C) Velocity of incident light
(D) Atomic mass of an element
According to Einstein's photoelectric equation, the graph between maximum kinetic energy of
photoelectrons ejected and the frequency of the incident radiation is :
K.E.max.
(B)
K.E.max.
(C)
n
(D)
n0
n
K.E.max.
n
n
V0
n
A
V0
B
v
Which graph is correctly plotted ?
(A)
(B)
l
K.E.max.
6.
K.E.max.
In the photoelectric effect, the slope of straight line
graph between stopping potential (V0) and frequency
of incident light (n) gives
(A) charge on electron
(B) Work function of emitter
(C) Plank’s constant
(D) ratio of Plank’s constant to charge on electron.
The stopping potential as a function of frequency is
plotted for two photoelectric surfaces A and B. The
graph show that the work function of A is
(A) Greater than that of B
(B) Smaller than that of B
(C) Same as that of B
(D) Such that no comparison can be done from graphs
K.E.max.
5.
(D) velocity
In photoelectric effect, the maximum kinetic energy of photoelectrons increases linearly with the
(A)
4.
(C) frequency
(C)
(D)
Intensity of
light
l
28
K.E.max.
2.
(B) wavelength
K.E.max
1.
Intensity of
light
Atomic Structure
7.
A light source of wavelength l illuminates a metal and ejects photo-electrons with (K.E.)max = 1
eV
Another light source of wavelength
8.
l
, ejects photo-electrons from same metal with
3
(K.E.)max =4 eV.
Find the value of work function?
(A) 1 eV
(B) 2 eV
(C) 0.5 eV
(D) None of these
Threshold frequency of a metal is f0. When light of frequency v = 2f0 is incident on the metal
plate, maximum velocity of e– emitted is v1. When frequency of incident radiation is 5f0, maximum velocity of emitted e– is v2. Find ratio of
9.
10.
11.
(i)
(ii)
12.
(A) 1 : 4
(B) 1 : 2
(C) 2 : 1
(D) none of these
What is the kinetic energy of a photoelectron emitted by a sodium surface when light of wavelength
400 nm is incident on it ? The work function of sodium is 2.28 eV.
(A) 0.88 eV
(B) 0.84 eV
(C) 0.82 eV
(D) 0.80 eV
Light of wavelength l falls on metal having work function hc/l0. Photoelectric effect will take
place only if :%
(A) l ³ l0
(B) l ³ 2l0
(C) l £ l0
(D) l £ l0/2
Ultraviolet light of wavelength 280 nm is used in an experiment of photoelectric effect with
lithium (Work function = 2.5 eV) cathode. What is the :
Maximum K.E.
(A) 1.70 eV
(B)1.88 eV
(C) 1.93 eV
(D) 1.90 eV
Stopping potential
(A) 1.70 volts
(B) 1.80 volts
(C) 1.91 volts
(D) 1.93 volts
If l0 and l be the threshold wavelength and the wavelength of incident light, the velocity of
photo-electrons ejected from the metal surface is :
(A)
13.
14.
v1
v2 :
2h
(l 0 - l)
m
(B)
2hc
(l 0 - l)
m
(C)
2hc æ l 0 - l ö
m çè ll 0 ÷ø
(D)
2h æ 1 1 ö
m çè l 0 l ÷ø
The ratio of slopes of Kmax versus n and V0 versus n curves in the photoelectric effect gives
(n = frequency, Kmax = maximum kinetic energy, V0 = stopping potential) :
(A) charge of electron
(B) Planck's constant
(C) work function
(D) the ratio of Planck's constant of electronic
charge
MULTIPLE CORRECT ANSWER TYPE
Light wavelength l shines on a metal surface with intensity X, and the metal emits Y electrons
per second of average energy Z, what will happen to Y and Z if X is doubled?
(A) Y will be doubled
(B) Z will be remain same
(C) Both Y and Z will be doubled
(D) Y will be doubled and Z will be halved.
29
JEE-Chemistry
BOHR’S MODEL
SINGLE CORRECT ANSWER TYPE
1.
What is the total energy of electron in 3rd orbit of H–atom?
(A) –1.54 eV
2.
(D) –1.52 eV
(B) 1.49eV
(C) 1.51eV
(D) 1.52eV
What is the potential energy of electron in 3rd orbit of H–atom ?
(A) –3.02 eV
4.
(C) –1.51 eV
What is the kinetic energy of electron in 3rd orbit of H–atom ?
(A) 1.50eV
3.
(B) –1.53 eV
(B) –3.01
(C) –3.04
The energy level of an atom for 1st, 2nd and third level are E,
(D) –3.05
4E
and 2E respectively. A photon of
3
wavelength l is emitted for a transition 3 to 1. What will be the wavelength of emission for
transition 2 to 1 ?
(A) l’ = 3 l
(B) l’ = 2l
(C) l’ = 4 l
(D) l’ = 5 l
5.
Let n1 be the frequency of series limit of the Lyman series, n2 be the frequency of the first line of
the Lyman series and n3 be the frequency of the series limit of the Balmer series then what is the
relationship between n1, n2 and n3 ?
(A) n 2 =
n1 - n3
2
(B) n3 = n2–n1
*(C) n3 = n1–n2
(D) n3 = n1 -
n2
2
6.
A hydrogen like atom is observed to emit six wavelength originating from all possible transitions
between a group of levels. These levels have energies between – 0.85 eV and – 0.544 eV (including
both these levels)
(i)
What is the atomic number of the atom ?
(A) 2
(ii)
(C) 4
(D) 5
What is the quantum number of the levels between which transition is taking place ?
(A) 10, 12
7.
(B) 3
(B) 11, 16
(C) 15,12
(D) 10, 17
An electron in an atom jumps in such a way that its kinetic energy changes from x to
x
. The
4
change in potential energy will be
3
(A) + x
2
8.
3
(D) - x
4
(B) 2/1
(C) 1/2
(D) 1/3
The ratio of velocity of the electron in the third and fifth orbit of Li2+ would be :
(A) 3 : 5
10.
3
(C) + x
4
What is the ratio of velocity of electron in 1st and second orbit of He+ ion ?
(A) 3/2
9.
3
(B) - x
8
(B) 5 : 3
(C) 25 : 9
(D) 9 : 25
If radius of second stationary orbit (in Bohr’s atom) is R. Then radius of third orbit will be
30
Atomic Structure
(A) R/3
11.
12.
13.
15.
16.
(C) R/9
(D) 2.25 R
What is the frequency of revolution of electron present in 2nd Bohr’s orbit of H-atom?
(A) 1.016 ´ 1016 s–1
(B) 4.065 ´ 1016 s–1
(C) 1.626 ´ 1015 s–1
(D) 8.2 ´ 1014 s–1
If in Bohr's model, for unielectronic atom, time period of revolution is represented as Tn, Z where
n represents shell number and Z represents atomic number then the value of T1, 2 : T2, 1will be :
(A) 8 : 1
(B) 1 : 8
(C) 1 : 1
(D) 1 : 32
If e0 be the permittivity of vacuum and r be the radius of orbit of H -atom in which electron is
revolving then velocity of electron is given by :
(A) v =
14.
(B) 9R
e
4 pe 0 rm
(B) v = e ´
4 pe 0 rm (C) v =
4 pe 0 rm
e
(D) v =
4 pe 0 rm
e2
If the ionization energy of He+ is 19.6 ´ 10–18 J per atom then the energy of Be3+ ion in the second
stationary state is :
(A) –4.9 ´ 10–18 J
(B) –44.1 ´ 10–18 J
(C) –11.025 ´ 10–18 J (D) None of these
Wavelength for high energy EMR transition in H-atom is 91 nm. What energy is needed for this
transition?
(A) 1.36 eV
(B) 1240 eV
(C) 13 eV
(D) 13.6 eV
MULTIPLE CORRECT ANSWER TYPE
According to Bohr’s atomic theory, which of the following is/are incorrect?
(A) Potential energy of electron µ
Z2
n2
(B) The product of velocity of electron in nth orbit and orbit number (n) µ Z2
(C) Frequency of revolution of electron in an orbit is µ
(D) Coulombic force of attraction on the electron µ
17.
Z2
n3
Z2
n2
According to Bohr’s atomic theory, which of the following relations is/are correct ?
(A) Kinetic energy of electron µ
Z3
n2
(B) The product of velocity of electron in nth orbit and orbit number (n) µ Z
(C) Frequency of revolution of the electron in an orbit µ
(D) Coulombic force of attraction on the electron µ
31
Z3
n4
Z3
n4
JEE-Chemistry
LINES SPECTRUM
SINGLE CORRECT ANSWER TYPE
1.
Find the value of wave number ( n ) in terms of Rydberg's constant when transition of electron takes
place between two levels of He+ ion whose sum is 4 and difference is 2.
(A)
2.
8R
9
R
9
(B) 656
(C) 73.0
(D) 486
(B) 1.36 ´ 103
(C) 1.16 ´ 103
(D) 1.78 ´ 103
(B)
9
R
(C)
1
R
(D)
9R
4
(B)
1
3R
(C)
4
4R
(D) None of these
The l of Ha line of the Balmer series is 6500Å. What is the l of Hb line of the Balmer series.
(A) 5814.8 Å
7.
(D) none of these
What is the maximum wavelength line in the Lyman series of He+ ion?
(A) 3R
6.
3R
4
What is the shortest wavelength line in the Paschen series of Li2+ ion?
(A)
5.
(C)
What is the energy (kJ/mol) associated with the de-excitation of an electron from n = 6 to n = 2 in He+
ion?
(A) 1.36 ´ 106
4.
32R
9
What is the wavelength in nm of the spectral line associated with a transition from n = 3 to n = 2 for
the Li2+ ion?
(A) 219
3.
(B)
(B) 4814.8 Å
(C) 3814.8 Å
(D) 2814.8 Å
Which of the following electron transitions in a hydrogen atom will require the largest amount of
energy?
(A) from n = 1 to n = 2 (B) from n = 2 to n = 4
(C) from n = 5 to n = 1
8.
(D) from n = 3 to n = 5
Which electronic transition in a hydrogen atom, starting from the orbit n = 7, will produce infrared
light of wavelength 2170 nm? (Given : RH = 1.09677 x 107 m–1)
(A) n = 7 to n = 6
(B) n = 7 to n = 5
(C) n = 7 to n = 4
(D) n = 7 to n = 3
MULTIPLE CORRECT ANSWER TYPE
9.
As an electron jumps from 4th orbit to the 2nd orbit in Be3+ ion, its
(A) K.E. increases
(B) speed increases
(C) frequency of revolution increases
(D) angular momentum increases
32
Atomic Structure
de-BROGLIE’S RELATIONSHIP & HEISENBERG PRINCIPLE
SINGLE CORRECT ANSWER TYPE
1.
What is the wavelenght associated ?
(i)
With an electron moving with a velocity of 106 m/sec.
(A) 5.27 Å
(ii)
2.
3.
(B) 6.62 × 10–25 meter
(C) 6.60 × 10–34 meter
(D) 6.62 × 10–35 meter
What is the de-Broglie wavelength of an electron accelerated through a potential difference of
(i) 75 volt and (ii) 300 volt respectively ?
(A) (i) 1.40 Å and 0.70 Å
(B) (i) 1.48 Å and 0.60 Å
(C) (i) 1.38 Å and 0.61 Å
(D) (i) 1.41 Å and 0.71 Å
What possibly can be the ratio of the de Broglie wavelengths for two electrons each having zero
initial energy and accelerated through 50 volts and 200 volts ?
(B) 10 : 3
1.23
m
1840
x
1.23
h
(C) l =
m
1.23
V
nm
(D) l =
1.23
V
(B)
x
1840
(C) 1840 x
(D) x
(B) 4pa0
(C) 2pa0
(D) None of these
Number of waves produced by an electron in one complete revolution in nth orbit is :
(B) n2
(C) (n + 1)
(D) (2n + 1)
The mass of a particle is 10–10 g and its radius is 2 ´ 10–4 cm. If its velocity is 10–6 cm sec–1 with
0.0001% uncertainty in measurement, the uncertainty in its position is :
(A) 5.2 ´ 10–8 m
9.
(B) l =
If a0 be the radius of first Bohr's orbit of H-atom, the de-Broglie's wavelength of an electron
revolving in the second Bohr's orbit will be :
(A) n
8.
(D) 2 : 1
An electron travels with a velocity of ‘x’ ms–1. For a proton to have the same de-Broglie wavelength, the velocity will be approximately :
(A) 6pa0
7.
(C) 1 : 2
The de-Broglie wavelength of an electron accelerated by an electric field of V volts is given by:
(A)
6.
(D) 8.27 Å
(A) 6.62 × 10–45 meter
(A) l =
5.
(C) 6.27 Å
With a cricket ball of mass 0.5 kg moving with 20 m/sec.
(A) 3 : 10
4.
(B) 7.27 Å
(B) 5.2 ´ 10–7 m
(C) 5.2 ´ 10–6 m
(D) 5.2 ´ 10–9 m
If Be3+ and a proton are accelerated by the same potential, their de-Broglie wavelengths have the
ratio? (assume mass of proton = mass of neutron) :
[ Be = 9]
(A) 3 : 2
(B) 2:3
(C) 3 3 :1
33
(D) 1: 3 3
JEE-Chemistry
10.
If the uncertainty in the position of an electron is 0.33 pm, what will be the uncertainty in its
velocity?
(A) 1.72 × 108 m/sec (B) 1.77 × 108 m/sec
11.
If H+ is accelerated to 6.62 × 106 m/sec. If error in velocity is ± 1%, then find the uncertainty in
position.
(A) 4.75 × 10–5 m
12.
2 p
m h2
(C) 4.65 × 10–10 m
(D) 4.75 × 10–7 m
(B) Dn =
1
2m
h
p
(C) Dn =
1 p
m h
(D) Dn =
1 h
m p
The momentum (in kg-m/s) of photon having 6 MeV energy is :
(A) 3.2 ´ 10–21
14.
(B) 4.75 × 10–13 m
If uncertainty in position and momentum are equal, show that uncertainity in velocity is(A) Dn =
13.
(C) 1.75 × 108 m/sec. (D)1.79 × 108 m/sec
(C) 1.6 ´ 10–21
(B) 2.0
(D) none of these
The uncertainty in position of an electron is equal to its de Broglie wavelength. The minimum
percentage error in its measurement of velocity under this circumstance will be approximately?
(A) 4
(B) 8
(C) 22
(D) 18
MULTIPLE CORRECT ANSWER TYPE
15.
Uncertainty in measuring speed of a particle is numerically equal to uncertainty in measuring its
position. The value of there uncertainties may be
(A) equal to
h
4pm
(B) less than
h
4pm
(C) greater than
34
h
(D) zero
4pm
Atomic Structure
QUANTUM MECHANICAL MODEL
SINGLE CORRECT ANSWER TYPE
1.
The idea that electrons have wave properties
(A) was never proven and is now discounted. (B) was only proven theoretically.
(C) was proven experimentally.
2.
“The exact path of electron in 2p-orbital cannot be determined." The above statement is based
upon
(A) Hund's Rule
3.
4.
(D) is true, but of no consequence.
(B) Bohr's Rule
(C) Uncertainty principle
(D) Aufbau principle
The wave function y in the Schrodinger wave equation represents
(A) Probability of the electron
(B) Amplitude of the wave
(C) Frequency of the wave
(D) Speed of the wave
For similar orbitals having different values of n :
(A) the most probable distance increases with increase in n
(B) the most probable distance decreases with increase in n
(C) the most probable distance remains constant with increase in n
(D) none of these
5.
6.
In H-atom energy of electron is determined by :
(A) only n
(B) n, l
(C) n, l, m
(D) all the four quantum numbers.
In any subshell, the maximum number of electrons having same value of spin quantum number is
:
(A)
7.
l(l + 1)
(B) l + 2
9.
(D) 4l + 2
If the subsidiary quantum number of a subenergy level is 4, the maximum and minimum values
of the spin multiplicities are :
(A) 9, 1
8.
(C) 2l + 1
(B) 10, 1
(C) 10, 2
(D) 4, –4
The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated, is
(A)
(B)
(C)
(D)
The quantum numbers of four electrons (e1 to e4) are given below :
n
l
m
s
e1
3
0
0
+ 1/2
e3
3
2
2
–1/2
n
l
m
s
e2
4
0
0
1/2
e4
3
1
–1
1/2
35
JEE-Chemistry
The correct order of decreasing energy of these electrons is :
(A) e4 > e3 > e2 > el (B) e2 > e3 > e4 > e1 (C) e3 > e2 > e4 > el (D) el > e4 > e2 > e3
10.
The two electrons have the following sets of quantum numbers :
X : 3, 2, –2, +1/2
Y : 3, 0, 0, +1/2
What is true for the following ?
11.
12.
(A) X and Y have same energy
(B) X and Y have unequal energy
(C) X and Y repesent same electron
(D) None of the statement is correct
Which of the following set of quantum numbers is impossible for an electron?
(A) n = 1, l = 0, ml = 0, ms = +
1
2
(B) n = 9, l = 7, ml = –6, ms = -
1
2
(C) n = 2, l = 1, ml = 0, ms = +
1
2
(D) n = 3, l = 2, ml = –3, ms = +
1
2
The set of quantum numbers, n = 3, l = 2, m1 = 0
(A) describes an electron in a 2s orbital
(B) is not allowed
(C) describes an electron in a 3p orbital
(D) describes one of the five orbitals of same energy
13.
The number of wave made by Bohr electron in an orbit of maximum magnetic quantum number
+2 is
(A) 3
14.
(B) 4
(B) 7d
(C) (2l +1)2
(D) 2(2l + 1)2
5: 7
(B)
(C) 7 : 3
35 : 15
(D)
24 : 15
(B) 2
(C) 3
(D) 4
What is the maximum number of electrons in an atom that can have the quantum numbers n = 3
and l = 2?
(A) 2
19.
(B) 2(2l + 1)
A compound of vanadium has a magnetic moment (m) of 1.73 BM. If the vanadium ion in the
compound is present as Vx+, then, the value of x is?
(A) 1
18.
(D) 7p
The ratio of magnetic moments of Fe (III) and Co (II) is :
(A)
17.
(C) 7s
Maximum number of electrons in a subshell is given by
(A) (2l + 1)
16.
(D) 1
In which of the following orbitals, the electron is on an average closer to the nucleus?
(A) 7f
15.
(C) 2
(B) 5
(C) 6
(D) 10
Which of the following statements about an electron with ml = +2 is incorrect?
(A) The electron could be in the third shell
(B) The electron is in a non-spherical orbital
36
Atomic Structure
(C) The electron may have ms =
20.
21.
(A) Number of angular nodes = n – l –1
(B) Number of radial nodes = l
(C) Total number of nodes = n – 1
(D) All
How many total nodal planes are present in the atomic orbitals for having the principal quantum
number n = 3 ?
(C) 14
(D) 11
(B) [Kr]4s1 3d7
(C) [Ar] 4s2 3d6
(D) [Kr] 4s2 3d6
Which of the following electron configurations is correct for copper, (atomic number 29)?
(A) [Ar] 3d10 4s1
24.
(B) 10
Which of the following electron configurations is correct for iron, (atomic number 26)?
(A) [Kr] 4s1 3d6
23.
(D) The electron is not in a d-orbital
Which of the following statement is correct?
(A) 12
22.
1
2
(B) [Kr] 3d9 4s1
(C) [Ar] 3d9 4s2
(D) [Kr] 3d10 4s1
The electronic configurations of 24Cr and 29Cu are abnormal
(A) Due to extra stability of exactly half filled and exactly fully filled sub shells
(B) Because they belong to d-block
(C) Both the above
(D) None of the above
25.
Among the following series of transition metal ions, the one where all metal ions have same 3d
electronic configuration is:
(A)Ti2+, V3+, Cr4+, Mn5+ (B) Ti3+, V2+, Cr3+, Mn4+
(C) Ti+, V4+, Cr6+, Mn7+
26.
What is the total number of orbitals in the shell in which the g subshell first occur?
(A) 9
27.
(D) Ti4+, V3+, Cr2+, Mn3+
(B) 16
(C) 25
(D) 36
The Schrodinger wave equation for hydrogen atom is
1 æ 1ö
Y 2s =
ç ÷
4 2p è a 0 ø
3/2
æ
r
ç2 a0
è
ö - r / 2a 0
÷e
ø
where a0 is Bohr's radius. If the radial node in 2s be at r0, then r0 would be equal to
(A)
28.
a0
2
(B) 2a0
(C)
2 a0
(D)
a0
Select the correct plot of radial probability function (4pr2R2) for 2s-orbital.
37
2
29.
2
r
2
(D)
4 pr R
r
4pr2R2
r
(C)
2
2
(B)
4pr R
4pr R
(A)
2
2
JEE-Chemistry
r
In case of d x 2 - y 2 orbital
(A) Probability of finding the electron along x-axis is zero.
(B) Probability of finding the electron along y-axis is zero.
(C) Probability of finding the electron is maximum along x and y-axis.
(D) Probability of finding the electron is zero in x-y plane
MULTIPLE CORRECT ANSWER TYPE
30.
Which of the following statement(s) is/are correct ?
(A) Value of l beyond 3 is not used for electrons in the ground state of naturally occurring
elements
(B) There are 10 electrons in Cl– which have magnetic quantum value equal to zero
(C) Magnitude of orbital angular momentum of p-orbital is zero
(D) 2s-atomic orbital is spherically symmetrical with no node
31.
Which of the following statement(s) is/are true ?
(A) For a H-atom, the energies of electron in 2s and 2p orbitals is same
(B) A d-orbital can have a maximum of two electrons with opposite spin
(C) Energy of electron decreases with the increase in (n + l) value
(D) Total number of nodes in 3s orbitals is 2
38
Atomic Structure
ANSWER KEY
THOMSON MODEL, RUTHERFORD MODEL
1.
(D)
2.
(A)
3.
(A)
4.
(C)
5.
(B)
6.
(B)
7.
(D)
8.
(B)
9.
(D)
10.
(B)
11.
(B)
12.
(A)
13.
(A)(B)(C)(D)
14.
(C)
ELECTROMAGNETIC RADIATION & PLANCK’S QUANTUM
THEORY
1.
(D)
2.
(A)
3.
(B)
4.
(B)
7.
(A)
8.
(B)
9.
(D)
10.
(B)
5.
(B)
6.
(B)
(C)
PHOTOELECTRIC EFFECT
1.
(C)
2.
(B)
3.
(C)
4.
(D)
5.
(B)
6.
7.
(C)
8.
(B)
9.
(C)
10.
(C)
11.
(i) (C)
(ii) (D)
12.
(C)
13.
(A)
14.
(A) (B)
BOHR’S MODEL
1.
(C)
2.
(C)
3.
(A)
4.
(A)
5.
(C)
6.
(i)(B)
(ii)
(C)
7.
(A)
8.
(B)
9.
(B)
10.
(D)
11.
(D)
12.
(D)
13.
(A)
14.
(D)
15.
(D)
16.
(B) (D)
17.
(B)(D)
5.
(B)
6.
(B)
LINES SPECTRUM
1.
(B)
2.
(C)
3.
(C)
4.
7.
(A)
8.
(C)
9.
(A) (B) (C)
(C)
de-BROGLIE’S RELATIONSHIP & HEISENBERG PRINCIPLE
1.
(i)
(ii)
(D)
2.
(D)
3.
(D)
4.
(C)
5.
(B)
6.
(B)
7.
(A)
8.
(A)
9.
(D)
10.
(C)
11.
(B)
12.
(B)
13.
(A)
14.
(B)
15.
(A) (C)
(B)
39
JEE-Chemistry
QUANTUM MECHANICAL MODEL
1.
(C)
2.
(C)
3.
4.
(A)
5.
(A)
6.
(C)
7.
(B)
8.
(D)
9.
10.
(B)
11.
(D)
12.
(D)
13.
(A)
14.
(C)
15.
(B)
16.
(B)
17.
(D)
18.
(D)
19.
(D)
20.
(C)
21.
(D)
22.
(C)
23.
(A)
24.
(A)
25.
(A)
26.
(C)
27.
(B)
28.
(B)
29.
(C)
30.
(A) (B)
31.
(A)(B) (D)
(B)
(C)
40
Classification of elements and periodic properties
CLASSIFICATION OF ELEMENTS AND PERIODIC
PROPERTIES
INTRODUCTION
1.
SINGLE CORRECT ANSWER TYPE
Classification of elements in modern periodic table is based on :
(A) Mendeleev’s law
(B) de-Broglie’s equation
(C) Moseley’s law
(D) Bohr’s model
2.
In Moseley’s experiment, a plot of v against atomic number (z) of element gave a : (v =
frequency of X-rays emitted)
(A) Straight line
(B) Parabola
(C) semicircle
(D) Non-linear curve
3.
Modern periodic law is based on :
(A) Atomic mass
(C) Atomic number
(B) Number of neutrons
(D) Atomic volume
4.
What is group number of element having atomic number 32 in long form of periodic table ?
(A) 10
(B) 14
(C) 18
(D) 12
5.
Total how many elements are there in fifth period of long form of periodic table ?
(A) 2
(B) 8
(C) 32
(D) 18
6.
Element having atomic number 117 is placed in which group and block of periodic table ?
(A) 7, d-block
(B) 15, p-block
(C) 17, p-block
(D) 10, d-block
7.
There are 10 neutrons in the nucleus of an element z M19 . This element belongs to which block of
periodic table ?
(A) s-block
(B) d-block
(C) p-block
(D) f-block
8.
Metalloids are present in which block of periodic table ?
(A) s-block
(B) p-block
(C) d-block
9.
10.
11.
(D) f-block
MULTIPLE CORRECT ANSWER TYPE
Select correct option(s) regarding element of atomic number 25 :
(A) It belongs to d-block.
(B) It is present in fourth period in periodic table.
(C) It is present in seventh group in periodic table.
(D) It is a transition element.
Which block of periodic table contain metals ?
(A) d-block
(B) p-block
(C) s-block
(D) f-block
f-block of periodic table contains :
(A) Lanthanoids
(B) Actinoids
(D) Non-metals
(C) Halogens
41
INORGANIC CHEMISTRY
12.
MATRIX MATCH TYPE
Column-I
Column-II
(Atomic number of element)
(Classification of element)
(A) 20
(P) s-block element
(B) 10
(Q) Transition element
(C) 25
(R) Inner transition element
(D) 58
(S) Noble gas
(T) p-block element
13.
INTEGER ANSWER TYPE
Total how many groups are there in p-block of long form of periodic table ?
14.
How many d-block elements are present in third period of periodic table ?
15.
Total how many periods are there in long form of periodic table ?
42
Classification of elements and periodic properties
IUPAC NAMING OF ELEMENTS AND EFFECTIVE NUCLEAR
CHARGE
1.
SINGLE CORRECT ANSWER TYPE
What is the symbol of element having atomic number 108 ?
(A) NuO
(B) Uno
(C) Oun
(D) Uon
2.
What is the correct IUPAC name of element having atomic number 113?
(A) Ununtriium
(B) Unniltrium
(C) Ununbium
(D) Ununtrium
3.
What is group number of element Uuu in periodic table ?
(A) 10
(B) 11
(C) 12
(D) 14
4.
The order of screening effect of electron of the given shell on outer shell electrons follows the
order :
(A) s > d > p > f
(B) f > p > s > d
(C) s > p > d > f
(D) f > d > p > s
5.
The decrease in the force of attraction between nucleus and valence shell electrons due to presence
of inner shell electrons is :
(A) Effective nuclear charge
(B) Screening effect
(C) Nuclear charge
(D) None of these
6.
On last electron of boron atom, screening is due to :
(A) Electrons of K shell only
(B)All the electrons of L shell only
(C) Two electrons of 1s and 2s each
(D)All electrons of K and L shell
7.
On going from left to right across the period in periodic table, effective nuclear charge generally :
(A) decreases
(B) increases
(C) becomes constant
(D) first decreases then increases
8.
Effective nuclear charge on last electron is maximum in
(A) Na+
(B) O–2
(C) Al+3
(D) F–
INTEGER ANSWER TYPE
What is the period number of element Ununpentium in periodic table ?
9.
10.
What is the difference in magnitude between nuclear charge and effective nuclear charge for
hydrogen atom ?
43
INORGANIC CHEMISTRY
ATOMIC RADIUS -I
1.
SINGLE CORRECT ANSWER TYPE
The bond distance in chlorine molecule (Cl2) is 198 pm. The covalent radius of chlorine would be :
(A) 198 pm
(B) 99 pm
(C) 396 pm
(D) 180 pm
2.
The size of which of the following elements can only be represented as non-bonded radii ?
(A) Cl
(B) H
(C) He
(D) Na
3.
The metallic radius of Potassium is 2.30Å . Its covalent radius can be :
(A) 2.62 Å
(B) 2.30 Å
(C) 2.44Å
(D) 2.03Å
4.
Consider the following presentation regarding closest Br2 molecules in solid phase :
Br
Br
Br
Br
618pm
What would be van der Wall’s radius of bromine if its covalent radius is 114 pm ?
(A) 195 pm
(B) 252 pm
(C) 278.5 pm
(D) 335.5 pm
5.
The covalent radius of P is 0.11 nm. The covalent radius of Cl will be :
(A) less than 0.11nm (B) equal to 0.11nm
(C) more than 0.11nm (D) twice of 0.11nm
6.
Select the correct comparison of size
(A) N–3 > O–2 > F– > Na+
(C) Na+ > F– > O–2 > N–3
7.
8.
9.
(B) N–3 > F– > Na+ > O–2
(D) F– > O–2 > N–3 > Na+
If the ionic radii of K+ and F– are nearly same (i.e., 1.34Å), the atomic radii of K and F are respectively:
(A) 1.34 Å, 1.34Å
(B) 0.72Å, 1.96Å
(C) 1.96Å, 0.72Å
(D) 1.96Å, 1.34Å
MULTIPLE CORRECT ANSWER TYPE
The determination of atomic size can not be precise because :
(A) The size of an atom is very small
(B) Electron cloud surrounding the atom does not have a sharp boundary
(C) It is possible to locate exact position of electrons in an atom
(D) All the elements are found in atomic form in nature.
Atomic size is affected by :
(A) Number of shells
(C) Oxidation state
(B) Effective nuclear charge
(D) Shielding effect
44
Classification of elements and periodic properties
10.
The radius of isoelectronic ions,
(A) increases with increase in nuclear charge
(B) decreases with increase in nuclear charge
(C) is not affected by nuclear charge
(D) increases with increase in magnitude of negative charge
11.
Select the correct comparison(s) of size :
(A) Sr2+ < Rb+
(B) Nb5+ < Zr4+
12.
13.
List (I)
(ion)
(I) Rb+
(II) Ca+2
(III) Be2+
(IV) Cs+
(I)
(A) P
(B) Q
(C) R
(D) S
(C) Ba+2 > Cs+
(D) Se–2 < As–3
MATRIX MATCH TYPE
List (II)
Radius (in pm)
(P) 45
(Q) 152
(R) 167
(S) 100
(II)
Q
S
P
R
(III)
R
P
S
Q
(IV)
S
R
Q
P
INTEGER ANSWER TYPE
How many of the following comparison(s) is/are correct regarding size ?
(i) Se > S
(ii) S–2 > Cl–
(iii) P–3 < S–2
(iv) Pb+4 > Pb+2 (v) H– > H+
(vi) Na+ > Mg2+
(vii) P > Sb
(viii) Be < Li
(ix) Si > Cl
14.
How many of the following elements has covalent radius more than radius of corresponding anion?
N, O, F, Cl, Se, Br, I, P, Te
15.
The period number of alkali metal in periodic table having least volume is :
45
INORGANIC CHEMISTRY
ATOMIC RADIUS -II
1.
2.
3.
4.
5.
6.
SINGLE CORRECT ANSWER TYPE
Size of which of the following ion is smallest among given ions ?
(C) K+(aq)
(B) Li+(aq)
(A) Rb+(aq)
(D) Na+(aq)
Choose the correct order of size :
(A) B < Al < Ga
(B) B > Al ; Ga
(C) B > Al > Ga
(D) B < Ga < Al
Which of the following is smallest ion ?
(A) F–
(B) H+
(C) Na+
(D) Li+
Which order of size is incorrect ?
(A) Ti < Zr ; Hf
(B) He < Ne < Kr
(C) Sc > Y ; La
(D) Zn < Cd ; Hg
Which anion is largest in size among given ?
(A) H–
(B) F–
(C) Cl–
(D) Br–
Au and Ag have nearly equal size due to ?
(A) Transition contraction
(C) Actinide contraction
(B) Lanthanide contraction
(D) Equal number of shells
COMPREHENSION TYPE
Paragraph for question no. 7 & 8
It is not possible to measure the atomic radius precisely. The atomic radius generally decreases across
a period and generally increases down the group. Ionic radius of isoelectronic species depends on the
number of protons in their nuclei.
7.
In which group of p-block, atomic size from third period to fourth period does not increase ?
(A) Group-13
(B) Group-14
(C) Group-15
(D) Group-17
8.
Atomic radii of noble gases are larger than the corresponding elements of the same period because :
(A) Noble gases have maximum effective nuclear charge in period.
(B) Atomic radii of noble gases are expressed as van der Wall’s radii
(C) Atomic radii of noble gases are always expressed as covalent radii.
(D) There is poor shielding by inner electrons to outermost electron.
9.
10.
INTEGER ANSWER TYPE
The group number and period number of smallest size s-block metal in periodic table is x and y
respectively. The value of (x + y) is....
Among s-block metal ions, the non radioactive metal which has least extent of hydration belongs to
which period in periodic table ?
46
Classification of elements and periodic properties
IONISATION ENERGY-I
1.
SINGLE CORRECT ANSWER TYPE
In which of the following reaction, DH° value is equal to the first ionisation energy of Ca ?
(A) Ca(g) ® Ca2+(g) + 2e–
(B) Ca(s) ® Ca+(g) + e–
(C) Ca(g) ® Ca+(g) + e–
(D) Ca+(g) ® Ca+2(g) + e–
2.
As compared to the first ionisation potential, the value of second ionisation potential of an element
is :
(A) Always smaller
(B) Neglible
(C) Always greater
(D) Unpredictable
3.
Successive ionisation energy of an element increases regularly due to :
(A) increasing size
(B) increasing effective nuclear charge
(C) increasing number of electrons
(D) increasing number of shells
4.
Select the correct order of first ionisation energy :
(A) Be < B < C < N (B) B < C < Be < N (C) N < C < B < Be
(D) B < Be < C < N
5.
A sudden largest jump between the values of first and second ionisation energy of an element
would be associated with the electronic configuration :
(A) 1s22s22p63s1
(B) 1s22s22p63s23p5
(C) 1s22s22p63s23p3
(D) 1s22s22p63s2
6.
Which of the following has least ionisation energy among given elements ?
(A) Mg
(B) Al
(C) S
(D) Cl
7.
Which of the following isoelectronic ion has the lowest ionisation energy ?
(A) K+
(B) S–2
(C) Ca+2
(D) Cl–
8.
9.
MULTIPLE CORRECT ANSWER TYPE
Select the factor(s) affecting ionisation energy of element ?
(A) Atomic size
(B) Effective nuclear charge
(C) Stability of configuration
(D) Penetration power of orbital
Choose the incorrect comparison(s) of ionisation energy :
(A) Cl < Cl–
(B) O > N
(C) Na+ > Na
COMPREHENSION TYPE
Paragraph for question no. 10 to 12
Ionisation energies of four elements in kJ/mol are given :
Element
Q
R
S
T
IE1
520
1086
899
2081
IE2
7298
2353
1757
3952
47
IE3
11820
4620
14850
6122
(D) N > F
INORGANIC CHEMISTRY
10.
11.
12.
13.
Which element belongs to group-1 ?
(A) S
(B) Q
(C) R
(D) T
Which element is a noble gas ?
(A) Q
(B) R
(C) T
(D) S
Which element belongs to group-2
(A) T
(B) S
(C) Q
(D) R
INTEGER ANSWER TYPE
Removal of outermost electron from isolated gaseous atom requires energy for how many given
elements ?
B, Li, Na, Cs, He, Kr, P, Xe, H
14.
What is the period number of element having maximum ionisation enthalpy among known elements ?
15.
A representative element has successive ionisation enthalpies as :
IE1
940
kJ/mol
IE2
2080
kJ/mol
IE3
3090
kJ/mol
IE4
4140
kJ/mol
IE5
7030
kJ/mol
IE6
7870
kJ/mol
IE7
16000
kJ/mol
How many valence shell electrons are there in an atom of this element ?
48
IE8
19500
kJ/mol
Classification of elements and periodic properties
IONISATION ENERGY-II
1.
SINGLE CORRECT ANSWER TYPE
X(g) ® X+(g) + e–, DH = +720 kJ/mol
What is the amount of energy required to convert 110 mg of ‘X’ atom in gaseous state into X+ (g)
ion ?
(Atomic weight for X = 7 g/mol)
(A) 9.4 kJ
(B) 21.3 kJ
(C) 11.3 kJ
(D) 32.7 kJ
2.
Second ionisation enthalpy of Mg is 348 Kcal/mol and the enthalpy required for the reaction
Mg(g) ® Mg+2(g) + 2e– is 526 Kcal/mol.
What would be first ionisation enthalpy of Mg ?
(A) 874 Kcal/mol
(B) 178 Kcal/mol
(C) 210 Kcal/mol
(D) 348 Kcal/mol
3.
The correct order of second ionisation energy is :
(A) Ne > O > F > N (B) F > Ne > O > N (C) O > F > Ne > N
(D) Ne > F > O > N
Which of the following has maximum third ionisation energy ?
(A) Ti
(B) V
(C) Cr
(D) Mn
4.
5.
6.
7.
8.
9.
Consider the following reactions :
(P) M(s) ® M(g)
(Q) M(s) ® M+2(g) + 2e–
(R) M(g) ® M+(g) + e–
(S) M+(g) ® M+2(g) + e–
+2
–
(T) M(g) ® M (g) + 2e
The second ionisation energy of M could be calculated from energy values associated with :
(A) (P) + (R) + (S)
(B) (Q) – (P) + (R)
(C) (P) + (T)
(D) (T) – (R)
MULTIPLE CORRECT ANSWER TYPE
Which of the following species has maximum ionisation energy in their respective period ?
(A) F
(B) He
(C) Ar
(D) Ba
Third ionisation energy is not defined for :
(A) H
(B) N
(C) He
(D) O
INTEGER ANSWER TYPE
How many elements of second period have second ionisation energy greater than their corresponding
first ionisation energy ?
The first ionisation energy of He is 24.6 eV. The sum of first and second ionisation energies of He
is (9x –2)eV. The value of x is
49
INORGANIC CHEMISTRY
ELECTRON AFFINITY
1.
SINGLE CORRECT ANSWER TYPE
Electron affinity is the property of :
(A) covalently bonded atom
(B) ionic bonded atom
(C) non bonded atom
(D) atom in solid state
2.
Which of the following reaction represent first electron gain enthalpy of chlorine atom ?
(A) Cl(g) ® Cl+(g) + e–
(B) Cl+(g) + e– ® Cl (g)
(C) Cl (g) + e– ® Cl– (g)
(D) Cl–(g) + e– ® Cl2– (g)
3.
On addition of an electron to an anion, the energy is :
(A) released
(B) absorbed
(C) neither released nor absorbed
(D) either released or absorbed
4.
Addition of an electron is the most easy in which of the following species ?
(A) O–
(B) O
(C) O+
(D) O2–
5.
Which of the following species has maximum electron affinity among given ?
(A) S+
(B) He+
(C) Cl+
(D) O+
6.
The electron gain enthalpy of Cl+ ion is –1251 kJ mol–1. The ionisation enthalpy of Cl atom would
be :
(A) –1251 kJ mol–1 (B) +625.5 kJ mol–1 (C) +1251 kJ mol–1 (D) –625.5 kJ mol–1
7.
Arrange N, O and S in order of decreasing electron affinity :
(A) S > O > N
(B) O > S > N
(C) N > O > S
(D) S > N > O
8.
Which of the following processes involve absorption of energy ?
(A) S(g) + e– ® S–(g)
(B) O(g) + 2e– ® O–2(g)
(C) F(g) + e– ® F–(g)
(D) H(g) + e– ® H–(g)
9.
Which of the following element has least electron affinity ?
(A) F
(B) S
(C) Ne
(D) Al
H+(g) + e– ® H(g),
DH for this process would be :
(A) Zero
(B) Positive
(D) Unpredictable
10.
11.
12.
13.
(C) Negative
If the electron gain enthalpy of Z(g) is –4.2 eV, then the ionisation enthalpy of Z(g) at the same
temperature can be :
(A) 4.2 eV
(B) 5.6 eV
(C) 3.4 eV
(D) any of these
MULTIPLE CORRECT ANSWER TYPE
Select the correct order(s) of electron affinity comparisons :
(A) S > O–
(B) Cl > F+
(C) F+ > Cl+
(D) F– > Cl+
Select the incorrect statement(s) :
(A) F– has more electron affinity than O+.
(B) The incoming electron encounters greater repulsion for F atom than for Cl atom.
(C) Noble gases have high tendency of accepting electron.
(D) S has less electron affinity than oxygen.
50
Classification of elements and periodic properties
14.
Select the correct orders of ionisation energy :
(A) Cl– > F–
(B) S– > O–
(C) F– > Cl–
15.
The correct statement(s) is/are :
(A) Magnitude of first ionisation enthalpy of an atom is equal to magnitude of first electron gain
enthalpy of cation of element.
(B) Magnitude of first ionisation enthalpy of an atom is equal to magnitude of first electron gain
enthalpy of anion of element.
(C) Magnitude of first electron gain enthalpy of an atom is equal to magnitude of first ionisation
enthalpy of anion of element.
(D) Magnitude of first electron gain enthalpy of an anion is equal to magnitude of first ionisation
enthalpy of cation of element.
16.
Electron affinity of an element is affected by :
(A) Size
(B) Effective nuclear charge
(C) Electronic configuration
(D) repulsion by inner electrons
17.
Select the correct order of EA comparison :
(A) Na > B > Ne
(B) B > Na > Be
(C) B < C < S
18.
19.
Column-I
(Element)
(A) F
(B) He
(C) H
(D) P
(D) O– > S–
(D) Zn > Ga > Ge
MATRIX MATCH
Column-II
(Property)
(P) Positive electron gain enthalpy
(Q) Negative electron gain enthalpy
(R) Maximum electron affinity in corresponding period
(S) Minimum electron affinity in corresponding period
INTEGER ANSWER TYPE
How many given element(s) have negative electron gain enthalpy ?
He, Be, Ne, Ar, Kr, N, Xe, Ca, Mg
20.
How many given element(s) have positive second electron gain enthalpy ?
O, F, Cl, Br, S, H, He, Na, P
21.
If group number of element having maximum electron affinity among all known elements in long
form of periodic table is : xy, then value of (x + y) is....
22.
Energy is absorbed in how many of given process(es) ?
(i) O ® O–
(ii) N ® N–
(iii) H ® H–
(v) He ® He–
(vi) Cl ® Cl–
(vii) Na+ ® Na
(ix) F ® F–
23.
For a cation A+5 ; the successive electron affinity values (in eV) are 290, 270, 29.9, 18 and 8.2
respectively. How many electrons are expected to be present in outermost subshell of atom ‘A’ which
is a representative element ?
51
(iv) H+ ® H
(viii) O+ ® O
INORGANIC CHEMISTRY
ELECTRONEGATIVITY
1.
SINGLE CORRECT ANSWER TYPE
Electronegativity is the property of :
(A) isolated atom
(B) bonded atom
(C) only gaseous atom (D) none of these
2.
Pauling’s scale of electronegativity is based on :
(A) Only electron affinity data
(B) Properties of non-bonded atom
(C) Bond dissociation energy data
(D) Number of neutrons in atom
3.
If cr is the electronegativity of an element on Pauling’s scale and cM is the electronegativity of
that element on Mulliken’s scale, then choose the correct relation :
(A) 2.8 cM ; cr
4.
(B)
1
cM
; cr
2.8
1
c
M
(C) 0.744 cr ; c (D) c = 2.8
r
M
Select the correct order of electronegativity :
(A) Li > H > Na
(B) Na > H > Li
(C) H > Li > Na
(D) Li > Na > H
5.
If the ionisation energy of an element is IE, electron affinity is EA and electronegativity is c, then
which relation is correct :
(A) 2c – EA – IE = 0(B) 2EA – c – IE = 0
(C) 2IE – c – EA = 0
(D) 2c – EA – 2IE = 0
6.
In a period form left to right, electronegativity :
(A) generally decreases
(B) generally increases
(C) is almost constant
(D) first decreases then increases
7.
Which order of electronegativity is correct ?
(A) Mg > Cl
(B) Al < S
(C) Rb > F
8.
9.
10.
11.
12.
(D) Al > B
Which of the following is least electronegative element among given ?
(A) O
(B) Al
(C) S
(D) N
Polarity of a covalent bond is explained by using :
(A) Electron affinity difference
(B) Ionisation potential
(C) Electronegativity difference
(D) None of these
Which of the following is most electropositive ?
(A) Be
(B) Rb
(C) Cl
(D) N
MULTIPLE CORRECT ANSWER TYPE
Electronegativity of an element depends on :
(A) Atomic size
(B) Oxidation state
(C) Effective nuclear charge
(D) % s-character
Select the correct relation(s) regarding electronegativity comparison(s) :
(A) N > P
(B) C > B
(C) Cl > I
(D) Li < Be
52
Classification of elements and periodic properties
13.
Select correct statement(s) :
(A) With increase in positive oxidation state, electronegativity increases.
(B) With increase in positive oxidation state, electronegativity decreases.
(C) With increasing size, electronegativity decreases.
(D) Fluorine is the most electronegative element.
14.
Electronegativity of which of the following elements is always constant ?
(A) Cl
(B) N
(C) F
(D) None of these
15.
The incorrect order(s) of electronegativity is/are :
(A) F > Br > Cl
(B) N > P > As
(C) O < S < Se
(D) C < Si < Ge
COMPREHENSION TYPE
Paragraph for question no. 16 & 17
Metals have few electrons in their valence shell while non-metals have more electrons in their valence
shell. Metallic character is closely related to atomic radius and ionisation enthalpy. Metallic character
increases from top to bottom in a group and decreases from left to right in a period. Metallic character
is inversely related to electronegativity of element.
The electronegativity of given elements follows the order :
(A) C < N < Si < P (B) N < Si < C < P (C) Si < P < C < N (D) P < Si < N < C
Choose the correct order of metallic character (A) B > Al > Mg > K
(B) Al > K > B > Mg
(C) Mg > Al > K < B
(D) K > Mg > Al > B
INTEGER ANSWER TYPE
What is the maximum value of principal quantum number of electron in most electronegative
element ?
16.
17.
18.
19.
The group number of least electronegative element in periodic table is :
20.
The first ionisation energy of an element is 13.4 eV per atom and electron affinity is 3.6 eV per
atom. What is approximate value of electronegativity of this element on Pauling’s scale ?
53
INORGANIC CHEMISTRY
MISCELLANEOUS
1.
2.
3.
4.
5.
6.
SINGLE CORRECT ANSWER TYPE
Which of the following non-metal oxide is not acidic ?
(A) CO2
(B) N2O5
(C) SO3
(D) NO
Which oxide among given is amphoteric ?
(A) CO
(B) Na2O
(D) CaO
(C) ZnO
Choose the correct order of acidic strength ?
(A) SO2 > SO3
(B) N2O5 > N2O3
(C) Cl2O7 < CaO
(D) MgO > P4O10
Which of the following oxide is the most acidic ?
(A) Cl2O7
(B) SO3
(C) B2O3
(D) SiO2
Select the neutral oxide among given :
(A) NO2
(B) MgO
(C) N2O
(D) CO2
Which order of basic strength is correct ?
(A) Li2O > Na2O > K2O
(C) Cs2O > Rb2O > K2O
(B) K2O > Cs2O > Na2O
(D) Rb2O > Li2O > K2O
7.
Which of the following ion of non-transition element have maximum value of spin only magnetic
moment ?
(A) Fe2+
(B) Cr3+
(C) Mn2+
(D) None of these
8.
In the periodic table, metallic character of elements generally :
(A) Decreases down the group and increases across the period from left to right.
(B) Increases down the group and decreases across the period from left to right.
(C) Increases down the group as well as across the period from left to right.
(D) Decreases down the group as well as across the period from left to right.
9.
10.
11.
MULTIPLE CORRECT ANSWER TYPE
Diagonal relationship is shown by :
(A) Be and Al
(B) Li and Mg
(C) Mg and Al
(D) B and P
The order : F– < Na+ < Mg2+ is correct for
(A) Size
(C) Ionisation energy
(B) Effective nuclear charge
(D) Electron affinity
Select the incorrect option(s) :
(A) O > S : Electron affinity
(C) Cd > Hg : Size
(B) S > P : Ionisation energy
(D) Mg+2 > Li+ : Size
54
Classification of elements and periodic properties
12.
13.
Column-I
(Comparison)
(A) F > Cl > Br > I
(B) Fe3+ > Fe+2 > Fe
(C) I– > I > I+
(D) O > C > B > N
MATRIX MATCH TYPE
Column-II
(True for)
(P) Size
(Q) Ionisation energy
(R) Electron affinity
(S) Electonegativity
INTEGER ANSWER TYPE
How many compounds are amphoteric among given ?
BeO, Ca(OH)2, CO2, Zn(OH)2, Cr2O3, PbO, SnO, PbO2, SO2
14.
Among given compounds, what is the number of basic oxides ?
Li2O, CO, MgO, Na2O, MnO, SnO2, B2O3, Al2O3, Tl2O
15.
How many oxygen atoms are there in a molecule of amphoteric oxide of group-2 of periodic
table ?
55
INORGANIC CHEMISTRY
1.
7.
11.
15.
1.
7.
1.
7.
11.
1.
7.
(C)
(C)
(A)(B)
7
2.
8.
12.
ANSWER KEY
INTRODUCTION
(A)
3.
(C)
4.
(B)
(B)
9.
(A) (B) (C) (D)
(A)-P ; (B)-ST ; (C)-Q ; (D)-R
5.
10.
13.
(D)
6.
(C)
(A) (B) (C) (D)
6
14. 0
IUPAC NAMING OF ELEMENTS AND EFFECTIVE NUCLEAR
CHARGE
(B)
(B)
2.
8.
(B)
2.
(C)
8.
(A) (B) (D)
(A)
(A)
2.
8.
3.
9.
(D)
(C)
4.
10.
(B)
7
5.
(C)
0
ATOMIC RADIUS -I
3.
9.
(B)
(C)
(A) (B)
12.
(D)
4.
(A)
(A) (B) (C) (D)
10.
13. 6
14.
ATOMIC RADIUS -II
3.
9.
(D)
(B)
4.
10.
(B)
4
(C)
6
(B)
6.
(C)
5.
(A)
(B) (D)
0
15.
6.
(A)
2
5.
(A)
6.
(B)
5.
6.
(B)
15.
(A)
10. (B)
6
5.
(D)
6.
(B) (C)
(B)
(B)
6.
12.
17.
21.
(C)
(A) (C)
(A)(C)
8
IONISATION ENERGY-I
1.
7.
11.
(C)
(B)
(C)
2.
8.
12.
2.
8.
(C)
3.
(B)
(A) (B) (C) (D)
(B)
13. 9
4.
(D)
(A)(B)(D)
14. 1
9.
IONISATION ENERGY-II
1.
7.
(C)
(A) (C)
3.
9.
1.
7.
13.
18.
22.
(C)
2.
(C)
(A)
8.
(B)
(A)(B)
14. (A)(B)
(A)-QR ; (B)-PS ; (C)-QR
2
23. 1
1.
7.
12.
15.
20.
(B)
2.
(C)
(B)
8.
(B)
(A) (B) (C) (D)
(A) (C) (D)
3
1.
7.
11.
(D)
2.
(C)
(D)
8.
(B)
(A) (B) (C) (D)
(B)
8
13.
4.
(A)
9
(D)
ELECTRON AFFINITY
3.
(B)
9.
(C)
15. (A)(C)
; (D)-Q
4.
10.
16.
19.
(C)
5.
(C)
11.
(A)(B)(C)(D)
0
20.
9
ELECTRONEGATIVITY
3.
9.
(A)
16.
4.
10.
(B)
(C)
(C) (D)
(C)
(C)
(B)
14.
17.
(D)
5.
(A)
6.
(B)
11. (A) (B) (C) (D)
(D)
18. 2
19. 1
MISCELLANEOUS
12.
3.
(B)
4.
(A)
5.
9.
(A) (B)
10. (B) (C) (D)
(A)-QS ; (B)-QRS ; (C)-P ; (D)-R
56
(C)
6.
(C)
Chemical Bonding
CHEMICAL BONDING
INTRODUCTION
1.
2.
3.
4.
5.
SINGLE CORRECT ANSWER TYPE
When two or more atoms combine together to form a molecule,...
(A) energy is released finally.
(B) energy is absorbed finally.
(C) energy is neither released nor absorbed.
(D) energy may release or absorb.
The energy of a molecule (as compared to the parent elements) is(A) Lower
(B) Higher
(C) Zero
The main reason of bond formation is(A) to attain unstability.
(C) to attain noble gas like configuration only
(D) Unpredictable
(B) to attain stability.
(D) to increase the overall energy.
For the bond formation process, DH (enthalpy change) is(A) Positive
(B) Zero
(C) Negative
(D) Unpredictable
Which of the following is/are types of chemical bond ?
(A) Covalent
(B) Metallic
(C) Electrovalent
(D) All of these
6.
Which bond is formed by the transfer of electron(s) from one atom to other ?
(A) Covalent
(B) Ionic
(C) Both (A) and (B) (D) None of these
7.
Valency expresses :
(A) total number of electrons in an atom.
(C) combining capacity of an element.
8.
(B) oxidation number of an element.
(D) Number of electrons in first shell of element.
The amount of energy released during bond formation is known as :
(A) Transition energy (B) Bond energy
(C) Ionisation energy
(D) Sublimation energy
9.
When two atoms approach to each other :
(A) Attraction arises between nucleus of two atoms.
(B) Attraction arises between nucleus of one atom and electrons of other atom.
(C) Attraction arises between electrons of two atoms.
(D) There is repulsion between nucleus of one atom and its own electrons.
10.
The energy required to break 1 mole of Cl – Cl covalent bond is nearly :
(A) 1 Kcal
(B) 9 Kcal
(C) 57 Kcal
(D) 5 Kcal
57
INORGANIC CHEMISTRY
COVALENCY
SINGLE CORRECT ANSWER TYPE
1.
Covalency is equal to :
(A) Number of unpaired electrons in only ground state.
(B) Number of unpaired electrons in only excited state.
(C) Number of unpaired electrons either in ground state or in excited state.
(D) Number of ions in molecule.
2.
Maximum covalency among given elements is observed in :
(A) H
(B) O
(C) S
3.
(D) N
In which of the following species, central atom has NOT exactly 8 valence electrons?
(A) BF4-
(B) NCl3
(C) PCl+4
(D) SF4
4.
Which statement is true about the most stable Lewis structure for CS2 ?
(A) There is no lone pair in molecule.
(B) Central atom is carbon.
(C) The central atom does not have an octet of electrons.
(D) A sulfur atom must be the central atom for the structure to be stable.
5.
Which of the following species/molecules does not have number of bond pairs equal to number of
lone pairs?
(A) OCN–
(B) H2O
(C) C2H2Cl2
(D) O3
6.
Covalency of P in PO34- and PH3 respectively are :
(A) 5, 4
7.
(B) 3, 5
(C) 3, 4
Octet of central atom is not complete in which of the following molecule ?
(A) CO2
(B) BeH2
(C) F2
(D) NO2+
8.
INTEGER ANSWER TYPE
What covalency is exhibited by chlorine in its first excited state ?
9.
Maximum covalency of a second period element is .....
10.
(D) 5, 3
SUBJECTIVE TYPE
What are covalencies of following elements in their neutral compounds
(i) C
(ii) B
(iii) N
(iv) S
(v) P
(vi) Xe
58
Chemical Bonding
LEWIS STRUCTURES
SINGLE CORRECT ANSWER TYPE
Draw the Lewis structure of following species showing lone pair and bonds :
1.
2.
3.
4.
Species having single central atom :
(i) H2O
(ii) CO2
(iii) NH3
(iv) COCl2
(v) XeF2
(vi) XeOF4
(vii) SO2
(viii) ICl +2
(ix) I3-
(x) NO -2
(xi) NO +2
(xii) CO32-
(xiii) NO3-
(xiv) SO32 -
(xv) XeF5-
(xvi) ClO -2
(xvii) N 3-
(xviii) PCl-6
(xix) SO 24 -
(xx) XeF6
(xxi) NH +4
(xxii) POCl3
(xxiii) O3
(xxiv) PH3
(xxv) SNF3
(xxvi) PSF3
(xxvii) NOF
(xxviii) ICl-4
(xxix) SOCl2
(xxx) SiF4
Species having multiple central atoms :
(i) N2H4
(ii) C2F6
(iii) S2F10
(iv) H2SO4
(v) H3PO4
(vi) S2O72-
(vii) B(OH)3
(viii) N2O5
(ix) (HO)4P2O3
(x) (HO)2S2O5
Cyclic species :
(i) P4
(ii) P4O10
(iii) P4O7
(iv) S8
(v) B3N3H6
(vi) S3O9
(vii) Benzene
(viii) P4S6
Structure of some important species to remember :
(i) N2O3
(ii) N2O
(iii) S2O32-
(iv) S2O52-
(v) S2O82-
(vi) CrO5
(vii) CO
(viii) C3O2
59
INORGANIC CHEMISTRY
VBT (OVERLAPPING OF PURE ATOMIC ORBITALS)
1.
SINGLE CORRECT ANSWER TYPE
Which of the following overlap result into formation of s-bond ?
(A)
2.
3.
4.
5.
(B)
8.
(D) H
(D) d–p
In which of the following, a p- bond is stronger than a s-bond ?
(A) CO2
(B) O3
(C) O2
(D) None of these
Which of the following overlap result into formation of a d-bond ?
+
(B)
+
(C)
(D)
Which order of p-bond strength is correct ?
(A) 2pp– 3pp > 2pp – 2pp
(C) 2pp – 3dp > 2pp – 2pp
(B) 2pp – 2pp > 2pp – 3pp
(D) 2pp – 3pp > 2pp – 3dp
Correct order of s-bond strength is :
(A) 2s – 2s > 2p – 2p (B) 2s – 2p > 2p – 2p (C) 2p – 2p > 2s – 2s
(D) 2s – 2s > 2p – 2s
MULTIPLE CORRECT ANSWER TYPE
py-orbital can not form p-bond by lateral overlap with : (INA = Z)
(A) d z 2 -orbital
9.
(C) C
Which of the following overlap can not form p-bond ?
(A) p–p
(B) s–p
(C) d–d
(A)
7.
(D)
Which atom can not form p-bond ?
(A) O
(B) N
+
6.
(C)
(B) d x 2 - y2 -orbital (C) py-orbital
(D) pz-orbital
Which of the following overlap of orbitals do/does not form bond (if Z-axis is internuclear axis)?
(A) s + py
(B) s + s
(C) pz + px
(D) pz + s
60
Chemical Bonding
COMPREHENSION TYPE
Paragraph for question no. 10 and 11
According to valence bond theory for a covalent bond formation, two atoms must come closer to
each other so that orbitals of one atom overlaps with the other. Overlapping orbitals must have unpaired
electron. Greater is the overlapping extent, lesser will be the bond length, more will be attraction and
more will be bond energy and bond strength.
10.
When two pz orbitals overlap in a particular direction and form s-bond, if two dyz orbitals overlap in
same direction then which of the following type of covalent bond should be formed ?
(A) s-bond
(B) p-bond
(C) both d & p bond (D) either s or p bond
11.
Which combination of overlap is zero overlap ? (INA = Z)
(A) s + pz
(B) py + py
(C) s + px
12.
INTEGER ANSWER TYPE
How many second period elements can form dp-dp bond ?
13.
How many given elements can form p-bond ?
C, O, N, Li, Na, H
14.
The total number of sigma bonds in a C2H2 molecule is-
15.
The total number of p-bonds in N2 molecule is-
61
(D) pz + pz
INORGANIC CHEMISTRY
HYBRIDISATION
SINGLE CORRECT ANSWER TYPE
1.
Hybridisation is mixing of :
(A) Electrons
2.
3.
(B) maximum two electrons
(C) maximum five electrons
(D) maximum ten electrons
Which hybrid orbital always forms p-bond ?
(B) sp2
(C) sp3
(D) dsp2
(B) CO32-
(C) NO3-
(D) SO3
(B) sp
(C) sp3d2
(D) sp2
(C) sp3d2 only
(D) Both sp3 and sp3d2
(C) Benzene
(D) C2H4
Solid PCl5 has hybridisation :
(B) sp3d only
All central atoms are sp hybridised in :
(A) H2O2
9.
(D) None
Square bipyramidal geometry can appear in hybridisation :
(A) sp3 only
8.
(C) sp3
Which species has the same electron geometry as that of NH3 ?
(A) sp3
7.
(B) sp2
Percentage p-character is three times to percentage s-character in which hybrid orbital ?
(A) SO32 6.
(D) Atoms
(A) maximum one electron
(A) sp
5.
(C) Orbitals
A hybrid orbital can have :
(A) sp
4.
(B) Protons
(B) C2H2
In process of hybridisation,
(A) orbitals of same atom mix together
(B) orbitals of different atom mix together
(C) resulting orbitals are symetrical in shape
(D) orbitals having high energy difference are involved
10.
Hybrid orbitals of central atoms are arranged around it in such a way that(A) repulsions between them are maximum
(B) repulsions between them are minimum
(C) they are oriented towards a point
(D) geometry obtained is always planar
62
Chemical Bonding
MATRIX MATCH TYPE
11.
(P)
Column-I
Column-II
(Electron geometry)
(Hybridisation)
Linear
(1)
sp3d2
(Q) Octahedral
(2)
sp3d
(R)
Trigonal bipyramidal
(3)
sp2
(S)
Trigonal planar
(4)
sp
P
Q
R
S
(A) 3
2
4
1
(B)
4
1
2
3
(C)
4
1
3
2
(D) 2
3
1
4
12.
Column-I
Column-II
(Hybridisation )
(Used orbitals)
(A) sp d (Trigonal bipyramidal)
(P)
dxy
(B)
sp3d2 (octahedral)
(Q)
d z2
(C)
sp3d3 (Pentagonal bipyramidal)
(R)
d x 2 - y2
(S)
pz
(T)
px
3
(D) sp3 (Tetrahedral)
INTEGER ANSWER TYPE
13.
Total how many axial orbitals are involved in hybridisation for central atom in a molecule of SF6 ?
14.
The % s-character in hybrid orbital of central atom in BF3 is :
SUBJECTIVE TYPE
15.
Find hybridisation of underlined atoms in following species :
(i) NH3
(ii) OF2
(iii) CS2
(iv) CF4
(v) POCl3
(vi) SO2
(vii) SF4
(viii) SO3
(ix) NO
(xiii) SO
(x) NO
(xiv) SO42-
(xi) NO
(xv) XeF2
(xii) CO32–
–
2
2–
3
+
2
–
3
63
INORGANIC CHEMISTRY
VSEPR THEORY
1.
2.
3.
4.
5.
SINGLE CORRECT ANSWER TYPE
The repulsive interaction of electron pairs decrease in the order :
(A) lone pair-lone pair > lone pair-bond pair > bond pair-bond pair
(B) lone pair-bond pair > bond pair-bond pair > lone pair-lone pair
(C) lone pair-bond pair > lone pair-lone pair > bond pair-bond pair
(D) lone pair-lone pair > bond pair-bond pair > lone pair-bond pair
In SF4, lone pair occupies :
(A) Axial position
(C) Neither axial nor equatorial position
(B) Equatorial position
(D) Both axial and equatorial position
XeF6 is :
(A) Square planar shaped
(C) Distorted tetrahedral shaped
(B) Pentagonal shaped
(D) Distorted octahedral shaped
The number of bonding pair of electrons in SF4 is :
(A) 4
(B) 5
(C) 6
(D) 17
The geometrical arrangement of orbitals and shape of I3- are respectively :
(A) trigonal bipyramidal geometry, linear shape
(B) hexagonal geometry, T-shape
(C) triangular planar geometry, triangular shape
(D) tetrahedral geometry, pyramidal shape
6.
Which of the following pairs of species have identical shapes ?
(A) NO +2 and NO -2
(B) PCl5 and BrF5
(C) XeF4 and ICl4–
(D) TeCl4 and XeO4
7.
The shapes of XeF4, XeF5– and SnCl2 are :
(A) octahedral, trigonal bipyramidal and bent
(B) square pyramidal, pentagonal planar and linear
(C) square planar, pentagonal planar and angular
(D) see-saw, T-shaped and linear
8.
Which molecular geometry is least likely to result from a trigonal bipyramidal electron geometry?
(A) Trigonal planar
(B) See-saw
(C) Linear
(D) T-shaped
9.
Which electron geometry of covalent molecules about a central atom has not been observed ?
(A) Pentagonal bipyramidal
(B) Octahedral
(C) Hexagonal
(D) Tetrahedral
10.
The bond angle in XeF5- is :
(A) 72°
(B) 120°
(C) 109°
64
(D) 180°
Chemical Bonding
11.
MULTIPLE CORRECT ANSWER TYPE
Which of the following is (are) V-shaped ?
(A) S32-
12.
13.
(B) ClO-2
(C) ClO +2
(D) SO2
If ABn4 , type species are tetrahedral, then which of the following is/are correctly matched ? (where A
is central atom, B is surrounding atom and n is charge on species.) ABn
A
B
n
(A) Xe O
0
(B) Se F
0
(C) P
O
–3
(D) N
H
+1
INTEGER ANSWER TYPE
How many species are linear shaped among given ?
CS2 ,S32- ,SO 2 , N 2O, NO2+ , N3- ,ICl2- , NO3- ,C2 H 2
14.
Lone pair occupies axial position in how many given species ?
ClF2 ,XeF2 ,I3- ,SF4 , XeF5- ,XeO 2F2 ,XeOF2 , XeO3 , PCl 3
15.
SUBJECTIVE TYPE
Predict shape of following species :
(i) H2O
(ii) NO -2
(iii) NO3-
(iv) NO +2
(v) PCl+4
(vi) NH +4
(vii) SO32 -
(viii ) SOCl2
(ix) PF6(xiii) XeO2F2
(x) N 3(xiv) XeO3F2
(xi) XeF2
(xii) XeOF2
(xv) XeO4
(xvi) XeF4
(xvii) XeO3
(xviii) XeF3+
(xix) ClO-2
(xx) OF2
(xxi) I3(xxv) SF4
(xxii) ICl +2
(xxiii) ICl-4
(xxiv) ICl +4
65
INORGANIC CHEMISTRY
RESONANCE
1.
2.
3.
SINGLE CORRECT ANSWER TYPE
Resonance is delocalisation of :
(A) Atoms
(B) Electrons
(C) Molecules
The correct order of Cl-O bond order is :
(A) ClO3– < ClO4– < ClO2– < ClO–
(C) ClO– < ClO2– < ClO–3 < ClO4–
(D) All of these
(B) ClO– < ClO4– < ClO3– < ClO2–
(D) ClO4– < ClO3– < ClO2– < ClO–
The correct order of increasing C–O bond strength of CO, CO32–, CO2 is :
(A) CO32 - < CO2 < CO(B) CO2 < CO32 - < CO
(C) CO < CO32 - < CO2
(D) CO < CO2 < CO32 -
5.
N–O bond length is maximum in :
(B) NO3–
(A) NO2+
(D) NO2–
F:
(B) SO 24-
(C) NH +4
(D) N 3-
p-bond order is fractional in:
(B) SO 24 (A) NO -2
(C) PO34-
(D) CO
(A)
6.
(C) NO+
MULTIPLE CORRECT ANSWER TYPE
Lone pair is delocalised in :
: :
4.
INTEGER ANSWER TYPE
is x. The value of 3x is nearly equal to....
7.
p-bond order in CO32-
8.
Lone pair of oxygen is delocalised in how many given species ?
NO-2 , NO3- ,ClO 4- ,O3 ,CH3OH,HCOO - ,CH 3COOH,CO32- , PO34-
9.
SUBJECTIVE TYPE
Find bond order in following species :
(i) CO32(ii) NO+2
(iii) NO3-
(iv) NO-2
(v) PO34-
(vi) ClO-4
(viii) ClO3-
(ix) O3
(x) SO23-
(vii) SO24-
66
Chemical Bonding
BOND PARAMETERS
SINGLE CORRECT ANSWER TYPE
1.
The correct increasing order of bond angle among BF3, PF3 and ClF3 :
(A) BF3 < PF3 < ClF3 (B) PF3 < BF3 < ClF3 (C) ClF3 < PF3 < BF3 (D) BF3 = PF3 = ClF3
2.
Among the following species, which has the least bond angle around the central atom ?
(A) O3
3.
7.
(C) C – Br
(D) C – I
(B) C2H4
(C) C2H2
(D) Benzene
(B) N – N > P – P
(C) O – O > S – S
(D) N º N < P º P
Which of the following statements is incorrect for PCl5 ?
(A) Its three P – Cl bond lengths arc equal.
(B) It involves sp3d hybridization.
(C) Each bond angle is more than 120°.
(D) Its shape is trigonal bipyramidal.
Central atom uses almost pure orbital for bond formation in :
(A) H2O
8.
(B) C – Cl
Select the correct comparison of bond dissociation energy :
(A) F – F < Cl – Cl
6.
(D) XeF5-
C – C bond length is minimum in :
(A) C2H6
5.
(C) NO -2
Bond dissociation energy is maximum in :
(A) C – F
4.
(B) I3-
(B) PH3
(C) NH3
(D) CH4
The highest H – C – H bond angle is present in :
(A) CH2F2
(B) CH4
(C) CH3Cl
(D) CH3F
MULTIPLE CORRECT ANSWER TYPE
9.
Select correct comparison(s):
(A) N2H4 > N2F4 (N – N bond length)
(B) C2H6 > C2F6 (C – C bond length)
(C) In PCl4F : P – Faxial > P – Clequatorial (bond length)
(D) In PCl3F2 : P – Clequatorial > P – Faxial (bond length)
10.
All bond angles are identical in:
(A) CF4
(B) SF6
(C) CH3Cl
67
(D) C2H4
INORGANIC CHEMISTRY
MATRIX MATCH TYPE
11.
Column-I
Column-II
(A)
XeF5-
(P)
(B)
PBr4+
(Q) Non-axial d-orbital is used in hybridisation
(C)
IOF3
(R)
Planar species
(D)
NH -2
(S)
Non-planar species
(T)
Bond angle 109°28' or less than 109°28'
d-orbital with zero nodal plane is used in hybridisation
INTEGER ANSWER TYPE
12.
How many species contain atleast one bond angle of 180º ?
ClO+2 ,C3O 2 , N 3- ,H 2S,OF2 ,I3+ ,C3H 4 , N 2O
13.
How many right angle, bond angles are present in a ClF3 molecule ?
14.
How may hybrid orbitals(s) are used for bond formation in a molecule of H2Te ?
SUBJECTIVE TYPE
15.
Compare bond angles in following :
(i) BF3, BCl3, BBr3, BI3
(ii) CH4,H2O, NH3, CO2
(iii) N2O, NO , NO
(iv) NH4+, NH3, NH2–
–
3
2–
3
–
2
(v) C3O2, CO , CCl4
68
Chemical Bonding
BACK BONDING & BRIDGE BONDING
SINGLE CORRECT ANSWER TYPE
1.
2.
Multicentred bonds are present in :
(A ) Be2H4
(B) (BeH2)n
(C) Al2H6
Al2(CH3)6 contains :
(A) 2c – 2e– bonds only
(C) 2c – 3e– bonds only
(B) 3c – 2e– bonds only
(D) Both 2c – 2e– and 3c-2e– bonds
(D) All of these
3.
The state of hybridisation of central atom in dimer form of both BH3 and BeH2 is respectively.
(A) sp2, sp
(B) sp3, sp2
(C) sp3, sp3
(D) sp2, sp3
4.
The geometry with respect to the central atom of the following molecules are:
N(SiH3)3 ; Me3N ; (SiH3)3P
(A) planar, pyramidal, planar
(B) planar, pyramidal, pyramidal
(C) pyramidal, pyramidal, pyramidal
(D) pyramidal, planar, pyramidal
5.
In which of the following cases, the strength of p-bond (back bond) is maximum ?
(A) PF3
(B) BF3
(C) (H3Si)3N
(D) (SiH3)2O
6.
7.
8.
9.
MULTIPLE CORRECT ANSWER TYPE
Which of the following statement is/are correct for CCl3– and CCl2
(A) Back bonding in both cases is from Cl to C-atom.
(B) Back bonding in both cases is from C to Cl-atom.
(C) Back bonding in CCl3– is from C to Cl but reverse in CCl2 .
(D) CCl2 is planar.
Which of the following molecule(s) is/are having pp–pp bonding ?
(A) BF3
(B) BeF2
(C) B3N3H6
Choose the incorrect statements :
(A) CH3NCS molecule is linear.
(C) SiF4 has pp–pp bonds
Column-I
(A) B2H 6
(B) Be2H 4
(C) Be2Cl4
(D) Al2(CH3)6
(D) BCl3
(B) In SiH3NCS, SiNC bond angle is 180º.
(D) P(SiH3)3 is planar about P
MATRIX MATCH TYPE
Column-II
(P) (3C–4e–) bond
(Q) (3C–2e–) bond
(R) (2C–2e–) bond
(S) sp3 hybridisation of central atom
(T) sp2 hybridisation of central atom
69
INORGANIC CHEMISTRY
10.
Column-I
Column-II
(A) N(SiH3)3
(P)
pp-dp back bonding
(B)
N(CH3)3
(Q)
sp3 hybridisation for underlined atom
(C)
B2 H 6
(R)
pp-pp back bonding
(S)
neither pp-pp nor pp-dp back bonding
(T)
Underlined atom combines with electron rich molecule on reaction.
(D) BF3
INTEGER ANSWER TYPE
11.
Total how many vacant orbitals of all central atoms are involved in hybridisation in formation of a
molecule of Be2H4 ?
12.
How many hybrid orbitals are possessed by a central atom in solid BeCl2 ?
SUBJECTIVE TYPE
13.
Backbonding is present in :
(i) B(CH3)3
(ii) H2B(NH2)
(iii) N(CH3)3
(iv) NF3
(v) O(SiH3)2
(vi) H3Si(NCS)
(vii) AlCl3
(viii) PF3
70
Chemical Bonding
MISCELLENEOUS
1.
SINGLE CORRECT ANSWER TYPE
Odd electron does not occupy hybrid orbital in :
(A) CF 3
2.
3.
(B) NO2
(C) CH3
PH5 does not exist due to :
(A) Steric crowding
(C) p-orbital contraction
(D) ClO3
(B) Lack of d-orbital contraction
(D) Inert pair effect
Coloured, paramagnetic as well as planar species is :
(A) ClO3
(B) NO2
(C) C2H6
(D) CF3
4.
Mean radial distance of 3d-orbital is least in which of the following species ?
(A) SF6
(B) SF4
(C) H2S
(D) S2F2
5.
All bonding orbitals of central atom are equivalent in :
(A) CH3F
(B) BF2Cl
(C) XeO3
(D) None of these
MULTIPLE CORRECT ANSWER TYPE
6.
All hybrid orbitals of central atom are equivalent in :
(A) NH3
7.
(D) O3
All bonding hybrid orbitals of central atom are equivalent in :
(A) NH3
8.
(C) NO3-
(B) CO2
(C) NO3-
(B) CO2
(D) O3
INTEGER ANSWER TYPE
In how many paramagnetic species, all valence electrons of central atom occupy hybrid orbital ?
CF3, NO2, CH3, ClO3, ClO2, C2H6, PCl 6, NO2+, N 2O
9.
SUBJECTIVE TYPE
Select the species which do not exist ?
(i) NCl5
(ii) PCl-6
(iii) BF63-
(iv) BeCl46 -
(v) PH +4
10.
Assign planar/non-planar to the following species :
(i) ClF3
(ii) SF4
(iii) SiF4
(v) NH3
(vi) HC º CH
(vii) H3C – C º CH
+
+
(ix) XeF3
(x) ClO2
71
(iv) H2C = CH2
(viii) XeF5–
INORGANIC CHEMISTRY
DIPOLE MOMENT
1.
SINGLE CORRECT ANSWER TYPE
Which of the following has least polarity in bond?
(A) H–F
(B) H–Cl
(C) H–O
(D) H–S
2.
BeF2 has zero dipole moment whereas H2O has a dipole moment because :(A) Water is linear.
(B) H2O is bent.
(C) F is more electronegative than O.
(D) Hydrogen bonding is present in H2O.
3.
The correct order of dipole moment is :
(A) CH4 < NF3 < NH3 (B) NF3 < CH4 < NH3 (C) NH3 < NF3 < CH4 (D) NF3 < NH3 < CH4
4.
Which one of the following molecules has highest dipole moment ?
(A) H2S
(B) CO2
(C) CCl4
5.
Which of the following hydrocarbons has the lowest dipole moment ?
(A)
6.
(D) BF3
H 3C
H
C
Cl
H
(B) CH3C º CCH3
(C) CH3CH2C º CH
(D) CH3 – CH º CH
Dipole moment is maximum in :
Cl
Cl
Cl
Cl
Cl
(A)
(B)
(C)
(D)
Cl
Cl
Cl
Cl
7.
A diatomic molecule H –X has a dipole moment of 1.2 D. If the bond length is 1.0 × 10–8 cm, what
fraction of charge does exist on each atom ?
(A) 0.25
(B) 0.75
(C) 0.50
(D) 0.33
8.
Which molecule is non polar but contains all polar bonds ?
(A) H2
(B) BF2Cl
(C) CCl4
9.
10.
11.
(D) HCN
MULTIPLE CORRECT ANSWER TYPE
Dipole moment of AX4 type of molecule is zero. The geometry of it can be :
(A) Tetrahedral
(B) Square planar
(C) See-saw
(D) Bent T
Which molecule is/are planar as well as non polar ?
(A) XeF4
(B) CF4
(C) CO2
(D) SF6
Select the INCORRECT order of dipole moment ?
(A) XeF2 > XeO3F2
(B) BF3 > BCl3
(C) CF4 > CH4
(D) NH3 > NF3
72
Chemical Bonding
INTEGER ANSWER TYPE
æ yö
12.
1 Debye = 1 × 10–y esu–cm. The value of ç ÷ isè 2ø
13.
Measured dipole moment of HCl is 3.436 × 10–30 coulomb-meter. Bond length in HCl is
2.29 × 10–10 meter. The percentage ionic character in HCl is x. The approximate value of x is :
14.
How many given species are non-polar as well as non-planar ?
PCl3F2, IF7, SO3, XeF4, CH2Cl2, CCl4, ClF3, PCl2F3, XeF2
SUBJECTIVE TYPE
15.
Assign polar/non-polar to the following species :
(i) CO2
(ii) CH2Cl2
(iii) CCl4
(iv) BF3
(v) NO2
(vi) XeF4
(vii) SF6
(viii) SiF4
(ix) SF4
(x) XeF2
(xi) SO3
(xii) SO2Cl2
(xiii) N2O
(xiv) SO2
(xv) PCl5
(xvi) XeO3F2
(xvii) I2Cl6
(xviii) ClF3
(xix) XeO4
(xx) XeO2F2
73
INORGANIC CHEMISTRY
MOLECULAR ORBITAL THEORY-I
1.
2.
SINGLE CORRECT ANSWER TYPE
The paramagnetic property of oxygen is well explained by:(A) Molecular orbital theory
(B) Resonance theory
(C) Valence bond theory
(D) VSEPR theory
Which of the following has fractional bond order ?
(A) O22 +
3.
(B) O22 -
Which of the following does not exist ?
(A) He2
(B) N2
(C) F22-
(D) H -2
(C) O2
(D) H2
4.
Which of the following statement is not correct regarding bonding molecular orbitals?
(A) Bonding molecular orbitals possess less energy than the combining atomic orbitals.
(B) Bonding molecular orbitals have low electron density between the two nuclei.
(C) Electron in bonding molecular contributes to the attraction between atoms.
(D) They are formed when the lobes of the combining atomic orbitals have the same sign.
5.
How many nodal planes are present in a ss-bonding molecular orbital?
(A) zero
(B) 1
(C) 2
(D) 3
6.
If z-axis is the molecular axis, then s-molecular orbitals can be formed by the overlap of:
(A) s + pz
(B) px + py
(C) pz + py
(D) px + px
7.
MULTIPLE CORRECT ANSWER TYPE
In which of the following, p-bond order is greater than s-bond order?
(A) N2
8.
(D) O-2
Which of the following changes involve the change in magnetic moment?
(A) N 2 ® N 2+
9.
(C) O +2
(B) O2
(B) H +2 ® H 2-
(C) O2 ® O 22-
(D) N +2 ® N -2
If NB is the number of bonding electrons and NA is the number of antibonding electrons of a molecule.
Then choose the incorrect statement(s) for the relationship, NB > NA :
(A) Molecule will always be diamagnetic.
(B) Molecule may have zero value of bond order.
(C) Molecule is only paramagnetic species.
(D) Molecule does not exist.
74
Chemical Bonding
COMPREHENSION TYPE
Paragraph for question no. 10 & 11
According to MOT, two atomic orbitals overlap resulting in the formation of molecular orbitals.
Number of atomic orbitals overlapping together is equal to the molecular orbital formed. The two
atomic orbital thus formed by LCAO (linear combination of atomic orbital) in the same phase or in
the different phase are known as bonding and antibonding molecular orbitals respectively. The energy
of bonding molecular orbital is lower than that of the pure atomic orbital by an amount ... This known
as the stabilization energy. The energy of antibonding molecular orbital is increased by D'
(destabilisation energy).
10.
The bond order of N2 is equal to that of :
(A) O2
11.
(B) O22 -
(C) O 22+
(D) None
Which among the following pairs contain both paramagnetic species ?
(A) O 22+ and N2
(B) O +2 and N2
(C) O2 and N2
(D) O2 and N -2
INTEGER ANSWER TYPE
12.
Total how many molecular orbitals contain electron(s) in B2 molecule ?
13.
The total number of nodal planes in a p*p molecular orbital-
14.
The toal electrons in HOMO(s) of N2 areSUBJECTIVE TYPE
15.
Find bond order and magnetic behaviour of following diatomic species using moleculear orbital
theory :
(i) H +2
(ii) He +2
(iii) N2
(iv) O-2
(v) Li2
(vi) O +2
(vii) C2
(viii) B2
(ix) N +2
(x) O22 -
(xi) O22 +
(xii) N -2
(xiii) H -2
(xiv) F2+
(xv) C22-
(xvi) C+2
(xvii) B+2
(xviii) O2
(xix) F2
(xx) Li +2
75
INORGANIC CHEMISTRY
MOLECULAR ORBITAL THEORY-II
1.
SINGLE CORRECT ANSWER TYPE
In which of the following ionization processes, the bond order has increased and the magnetic behaviour
has changed
(A) NO ® NO+
2.
(C) N 2 ® N +2
(D) C2 ® C2+
Which of the following species will have the minimum bond energy ?
(A) N2
3.
(B) O 2 ® O 2+
(B) N -2
(C) N +2
(D) N -22
Which of the following species exhibits the diamagnetic behaviour ?
(A) O +2
(B) O2
(C) NO
(D) O 22-
4.
Which of the following statements is correct about N2 molecule :(A) It has a bond order of 3.
(B) The number of unpaired electrons present in it is zero.
(C) The order of filling of MOs is p(2px) = p(2py), s(2pz).
(D) All the above three statements are correct.
5.
Using MO theory, predict which of the following species has the shortest bond length?
(A) O-2
6.
7.
(B) O22 -
(C) O 22+
(D) O +2
Increasing order of bond length in NO, NO+ and NO– is :(A) NO > NO– > NO+ (B) NO+ < NO < NO– (C) NO < NO+ < NO– (D) NO < NO+ = NO–
MULTIPLE CORRECT ANSWER TYPE
Bond order of a species can be :
(A) zero
(B) positive
(C) negative
(D) fractional
8.
Which of the following is/are correct order of energy of molecular orbitals ?
(A) s2pz > p2px (O2 molecule)
(B) s2pz > p2py (N2 molecule)
(C) s2pz > p2px (B2 molecule)
(D) s2pz > p2px (F2 molecule)
9.
Which of the following has more no. of bonding molecular orbital electron(s) than its antibonding
molecular orbital electrons ?
(A) B2
(B) N2
(C) O2
(D) H2
10.
Select the correct statement(s) about the compound NO[BF4] :
(A) It has 5s and 2p bonds.
(B) Nitrogen-oxygen bond length is higher than that in nitric oxide (NO).
(C) It is a diamagnetic species.
(D) B–F bond length in this compound is lower than that in BF3.
76
Chemical Bonding
11.
Which of the following molecular species is/are having p*2p as H.O.M.O. (highest occupied molecular
orbital):
(A) Li2
12.
13.
Column-I
(Species)
(A) O2+[BF4]–
(B) KO 2
(C) Na2O 2
(D) O 2
(B) N2
(C) F2
(D) C22-
MATRIX MATCH TYPE
Column-II
(Properties)
(P) Paramagnetic ion
(Q) Diamagnetic ion
(R) Fractional bond order
(S) Bond order ³ 2
(T) HOMO of diatomic ion contains 4 electrons
INTEGER ANSWER TYPE
If Hund's rule is violated then find the total number of species among following which will be
diamagnetic?
B2 ,O 2 , N 2- ,C 2+ , N +2 , F2+ , N 22- , Li +2 ,O +2
14.
Total number of unpaired electron(s) present in both cationic and anionic part of compound O2[PF6].
15.
There are some arrangements of atomic orbitals which are given below :
(i)
(ii)
(iii)
(iv)
(v)
(vi)
(vii)
(viii)
+
(ix)
Then calculate the value of "Q × R – P" where, P, Q and R are no. of arrangements which give
bonding molecular orbitals (positive overlap), antibonding molecular orbitals (negative overlap) and
non-bonding molecular orbitals (zero overlap) respectively.
77
INORGANIC CHEMISTRY
INTRODUCTION OF IONIC BOND
1.
SINGLE CORRECT ANSWER TYPE
An electrovalent bond or ionic bond is formed generally between :(A) Two electronegative atoms.
(B) Two metals.
(C) Electropositive and electronegative atoms. (D) Two electropositive atoms.
2.
The electronegativity of cesium is 0.7 and that of fluorine is 4.0. The bond formed between the two is
(A) Covalent
(B) Electrovalent/ionic (C) Coordinate
(D) Metallic
3.
Element A has 3 electrons in the outermost orbit and element B has 6 electrons in the outermost orbit.
The formula of the compound formed between A and B would be :(A) A2B3
(B) A2B6
(C) A2B
(D) A3B2
4.
Ionic compounds in general possess both :(A) High melting points and non-directional bonds.
(B) High melting points and low boiling points.
(C) Directional bonds and low boiling points.
(D) High solubilities in polar and non-polar solvents.
5.
An ionic compound A+ B– is most likely to be formed when –
(A) Ionization energy of A is low.
(B) Electron affinity of B is high.
(C) Electron affinity of B is low.
(D) Both (A) and (B)
6.
Electrovalent compounds or ionic compounds do not show isomerism. The reason is –
(A) Presence of ions
(B) Strong electrostatic force of attraction
(C) Brittleness
(D) Non - directional nature of ionic bond
7.
Oxide of a metal 'M' has formula M2O3, The formula of nitride of this metal 'M' will be:(A) M3N
(B) MN
(C) M3N2
(D) M2N3
8.
Solid NaCl is a bad conductor of electricity because :
(A) In solid NaCl, there are no ions.
(B) Solid NaCl is a covalent compound.
(C) In solid NaCl, there is no mobility in ions. (D) In solid NaCl, there are no attractive forces.
9.
INTEGER ANSWER TYPE
How many species contain ionic as well as covalent bond(s) ?
CsBr3, NaOH, NH4Cl, Na2CO3, CaSO4, KNO3, KI3, CaC2, Ba(OH)2
10.
The magnitude of electrovalency of group-1 metals is....
78
Chemical Bonding
LATTICE ENTHALPY AND FAJAN’S RULE
1.
2.
SINGLE CORRECT ANSWER TYPE
Which set of compounds in the following pairs has the higher lattice energy?
(i) KCl or MgO
(ii) LiF or LiBr
(iii) Mg3N2 or NaCl
(A) KCl, LiBr, Mg2N2
(B) MgO, LiBr, Mg3N2
(C) MgO, LiF, NaCl
(D) MgO, LiF, Mg3N2
The incorrect order of lattice energy is :
(A) AlF3 > MgF2
(B) Li3N > Li2O
(C) NaCl > LiF
(D) TiC > ScN
3.
From the following sequence, calculate the lattice energy of AB(s) in kJ/mole :A(s) ® A+(g) + e
; DH= 610 kJ mol–1
B(g) + e ® B– (g)
; DH= –260 kJ mol–1
A(s) + B(g) ® AB(s) ; DH = –569 kJ mol–1
(A) –219
(B) –919
(C) +1539
(D) +301
4.
The magnitude of the lattice energy of an ionic solid increases if :(A) The ions are large.
(B) The ions are small.
(C) The ions are of equal size.
(D) Charges on the ions are small.
5.
Lattice energy is maximum in which of the following ?
(A) NaF
(B) MgO
(C) ScN
(D) CsI
6.
Among LiCl, BeCl2, BCl3 and CCl4, the covalent character follows the order :
(A) LiCl < BeCl2 > BCl3 > CCl4
(B) LiCl > BeCl2 < BCl3 < CCl4
(C) LiCl < BeCl2 < BCl3 < CCl4
(D) LiCl > BeCl2 > BCl3 > CCl4
7.
The correct order of decreasing polarisablity of ions is :
(A) Cl– > Br– > I– > F– (B) F– > I– > Br– > Cl– (C) F– > Cl– > Br– > I– (D) I– > Br– > Cl– > F–
8.
According to Fajan's rules, necessary condition to have more covalent character is :
(A) small cation and large anion
(B) small cation and small anion
(C) large cation and large anion
(D) large cation and small anion
9.
Which of the following is correct order of ionic character ?
(A) NaCl < CuCl
(B) NaCl < KCl
(C) Li2CO3 > Ag2CO3 (D) BeSO4 > ZnSO4
10.
Which of the following has maximum covalent charcater ?
(A) PbF4
(B) BiF5
(C) HgF2
11.
(D) TlF3
Among the following, the maximum covalent character is shown by the compound :(A) AlCl3
(B) MgCl2
(C) KCl
(D) CsCl
79
INORGANIC CHEMISTRY
MULTIPLE CORRECT ANSWER TYPE
12.
Polarisation may be called as the distortion of the shape of an anion by an adjacently placed cation.
Which of the following statements is/are not correct?
(A) Low polarization is brought about by a cation of low radius.
(B) A large cation is likely to bring about a large degree of polarisation.
(C) High polarization is brought about by a cation of high charge.
(D) A small anion is likely to undergo a large degree of polarisation.
13.
Which statement is/are correct ?
(A) Higher is the polarisation, higher will be relative solubility in non-polar solvent.
(B) Higher is the polarisation, more will be the electrical conductivity.
(C) With increase in polarisation, covalent character increases.
(D) Higher is the polarisation in metal oxide, more will be ionic character.
INTEGER ANSWER TYPE
14.
How many given ions have pseudo noble gas configuration ?
Li+, K+, Mg2+, Ga3+, Zn2+, Hg2+, Cu+, Pb2+, Ca2+
15.
What is period number of cation of element of group number 2, which has maximum polarising
power in its group ?
80
Chemical Bonding
INERT PAIR EFFECT
1.
2.
SINGLE CORRECT ANSWER TYPE
Inert pair effect is the reluctance of electrons of :
(A) s-orbital to take part in bonding.
(B) p-orbital to take part in bonding.
(C) d-orbital to take part in bonding.
(D) f-orbital to take part in bonding.
Which of the following is an oxidiser ?
(A) PbO2
(B) Bi2O3
(C) SnO
(D) None of these
3.
The stability of dihalides of Si, Ge, Sn and Pb increases in the sequence
(A) GeX2 < SiX2 < SnX2 < PbX2
(B) SiX2 < GeX2 < PbX2 < SnX2
(C) SiX2 < GeX2 < SnX2 < PbX2
(D) PbX2 < SnX2 < GeX2 < SiX2
4.
Which of the following order is incorrect?
(A) Oxidizing power order : SiCl4 < SnCl4 < PbCl4
(B) Reducing power order : CO > CO2
(C) Oxidising power order : PbO2 > SnO2
(D) Reducing power order : PbO > SnO
5.
Which of the following does not exist ?
(A) BI3
(B) BiI3
6.
7.
(C) PbI4
(D) KI
MULTIPLE CORRECT ANSWER TYPE
Correct stability order of metal cation is/are :
(A) Pb2+ < Sn2+
(B) Pb4+ < Pb2+
(C) Sn4+ < Sn2+
(D) Pb4+ < Sn4+
Choose the incorrect option(s) :
(A) PbO is a powerful oxidiser.
(C) BiF3 is unstable.
(B) SnCl4 is a powerful reducer.
(D) PbI4 is more stable than PbI2.
MATRIX MATCH TYPE
8.
Match the Column :
Column-I
(Property)
(A) Cation with pseudo inert gas configuration
(B) Cation with (18 + 2) electronic configuration
(C) Strongest reducing agent out of given four ions
(D) Cation which form most covalent chloride.
Column-II
(ion)
(P) Sn+2
(Q) Sn+4
(R) Pb+2
(S) Bi+3
INTEGER ANSWER TYPE
9.
D
How many mole of diatomic gas is produced in reaction : 2PbO2 ¾¾
®
10.
The magnitude of oxidation state of Tl in TlI3 is....
81
INORGANIC CHEMISTRY
THERMAL STABILITY, SOLUBILITY OF IONIC COMPOUNDS
AND HEATING EFFECTS
SINGLE CORRECT ANSWER TYPE
1.
Which of the following is thermally most stable ?
(A) BeSO4
2.
(B) CaSO4
(C) SrSO4
(D) BaSO4
D
Pb(NO3 ) 2 (s) ¾¾
®
2MOLES
The number of moles of coloured paramagnetic gases obtained is(A) 5
3.
4.
5.
(C) 1
(D) 2
For an ionic compound, more hydration enthalpy supports for :
(A) Its solubility in water.
(B) Its high lattice enthalpy.
(C) Its high thermal stability
(D) More covalent character in it.
Which of the following ionic compound is insoluble in water ?
(A) CaCO3
(B) NaCl
(C) NaOH
(D) Na2CO3
Extent of hydration is maximum in which of the following isoelectronic ion ?
4+
(A) Ce(aq.)
6.
(B) 4
+
(B) La3(aq.)
+
(C) Ba 2(aq.)
+
(D) Cs(aq.)
Select correct order of thermal stability :
(A) Li2O > Na2O > Rb2O
(B) Rb2O >Na2O > Li2O
(C) Na2O > Rb2O > Li2O
(D) Rb2O > Li2O > Na2O
MULTIPLE CORRECT ANSWER TYPE
7.
Which of the following give O2 (g) on thermal decomposition ?
(A) Pb2O3
8.
(B) Pb3O4
(C) HgCO3
Which of the following give CO2(g) on thermal decomposition ?
(A) Ag2CO3
(B) ZnCO3
(C) CaCO3
(D) NaNO3
(D) Li2CO3
INTEGER ANSWER TYPE
9.
How many moles of CO2 are obtained on thermal decomposition of 1 mole Na2CO3 ?
10.
Solubility of an ionic compound in water generally depends on how many of the following factor ?
Lattice enthalpy, Hydration of ions, Temperature, Thermal stability, Inert pair effect, Polarisation.
82
Chemical Bonding
WEAK FORCES
1.
2.
3.
4.
5.
SINGLE CORRECT ANSWER TYPE
Which of the following has maximum boiling point ?
(A) BF3
(B) BCl3
(C) BBr3
(D) BI3
Correct order of boiling points is :
(A) BF3 > BMe3
(B) NF3 > NMe3
(D) He > H2
(C) C5H12 > CH4
Which of the following interaction is strongest ?
(A) Na+ ....OH2
(B) Na+ .....C6H6
(C) Li+ .....OH2
Solubility of Cl2 in water is due to :
(A) Dipole-Dipole interaction.
(C) Ion-dipole interaction.
(D) Li+ ......C6H6
(B) Dipole-induced dipole interaction.
(D) Ion-induced dipole interaction.
Which of the following does not form clathrates ?
(A) Xe
(B) Rn
(C) Kr
(D) He
6.
The molecular size of ICl and Br2 is approximately same, but boiling point of ICl is about 40°C
higher than that of Br2. It is because :
(A) ICl bond is stronger than Br–Br bond.
(B) IE of iodine < IE of bromine.
(C) ICl is polar while Br2 is nonpolar.
(D) I has smaller size than Br.
7.
The correct order of boiling point is :
OH
(I)
OH
F
(A) I > II > III
8.
(II)
OH
Cl
(III)
(B) III > II > I
Br
(C) II > I > III
(D) III > I > II
(C)
(D)
Which is most volatile among given ?
(A)
(B)
9.
INTEGER ANSWER TYPE
The magnitude of Dipole-induced dipole interaction energy is inversely proportional to rx(r = distance
between polar and non-polar molecule). x is equal to ....
10.
What is atomic number of least water soluble noble gas ?
83
INORGANIC CHEMISTRY
HYDROGEN BONDING
1.
2.
SINGLE CORRECT ANSWER TYPE
The correct order of strength of H-bond in the following compound is :
(A) H2O > H2O2 > HF
(B) HF > H2O2 > H2O
(C) HF > H2O < H2O2
(D) HF > H2O > H2O2
Which of the following is most volatile ?
(A) HF
(B) HCl
(C) HBr
(D) HI
3.
Density of water is more than that of ice at 25ºC. Which of the following is responsible for the above
order ?
(A) Intramolecular H-bonding
(B) intermolecular H -bonding
(C) ion-ion interaction
(D) ion-dipole interaction.
4.
Which among the following has maximum boiling point?
(A) CH3 – CH2 – (CH2)2 – CH2OH
(B) CH3 – CH2 – CH2 – CH – CH3
OH
CH3
(C) CH3 – CH2 – CH – CH2 – CH3
(D) CH3 – C – CH2 – CH 3
OH
5.
OH
MULTIPLE CORRECT ANSWER TYPE
The correct order of decreasing boiling points is/are :
(A) NH3 > PH3
(B) H2O > H2Te
(C) CH3COOH > CH3OCH3
(D) CH4 > GeH4 > SiH4
COMPREHENSION TYPE
Paragraph For Question no 6 & 7
Hydrogen bond is the term given to the relatively weak secondary interaction between a hydrogen
atom bound to an electronegative atom and another atom which is also generally electronegative and
which has one ore more lone pairs and can thus acts as a base.
Bond dissociation energy of H-bond ranges from 8 to 42 kJ/mol, and the most commonly encountered
hydrogen bonds are O – H ... O, N – H ... O and F – H ... F.
6.
7.
Strongest H-bond among given is :
(A) H – Cl......H – Cl (B) F– ......H – F
(C) S ......H – O
Which of the following interaction has energy between 8-42 kJ/mol?
(A) Na+ : CCl4
(B) CHCl3 : Br–
(C) C6H6 : CCl4
84
(D) N......H – N
(D) H2O : HCN
Chemical Bonding
INTEGER ANSWER TYPE
8.
How many membered chelate ring is formed in ortho-nitrophenol due to intramolecular hydrogen
bonding ?
9.
How many atoms are capable of forming hydrogen bond in a molecule of Boric acid, B(OH)3 with
other molecules of B(OH)3 ?
SUBJECTIVE TYPE
10.
Select the species forming intermolecular hydrogen bond with their other molecules, forming
intramolecular hydrogen bond and forming no hydrogen bond :
NO2
NO2
(i) C2H5OH
(ii) Cl3C-CH(OH)2
(iii)
COOH
(iv)
HO
NO2
(v) CH3NH2
(vi) CH3COOH
(vii)
(ix) Ortho-fluorophenol
CH2–H
(x) CH3–CHO
85
(viii) H2O
INORGANIC CHEMISTRY
ANSWER KEY
INTRODUCTION
1.
(A)
2.
(A)
3.
(B)
4.
(C)
7.
(C)
8.
(B)
9.
(B)
10.
(C)
5.
(D)
6.
(B)
5.
(D)
6.
(D)
COVALENCY
1.
(C)
2.
(C)
3.
(D)
4.
(B)
7.
(B)
8.
3
9.
4
10.
(i) 4, (ii) 3, (iii) 3, (iv) 2,4,6, (v) 3,5 (vi) 2,4,6,8
VBT (OVERLAPPING OF PURE ATOMIC ORBITALS)
1.
(B)
2.
(D)
3.
7.
(C)
8.
(A)(B)(D) 9.
13.
3
14.
3
15.
(B)
4.
(D)
5.
(B)
6.
(B)
(A)(C)
10.
(B)
11.
(C)
12.
0
6.
(C)
6.
(C)
2
HYBRIDISATION
1.
(C)
2.
(B)
3.
(D)
4.
(C)
5.
(A)
7.
(D)
8.
(B)
9.
(A)
10.
(B)
11.
(B)
12.
(A)-QST ; (B)-QRST ; (C)-PQRST ; (D)-ST
13.
5
14.
33.33
15.
(i) sp3
(ii) sp3
(iii) sp
(iv) sp3
(v) sp3
(vi) sp2
(vii) sp3d
(viii) sp2
(ix) sp2
(x) sp
(xi) sp2
(xii) sp2
(xiii) sp3
(xiv) sp3
(xv) sp3d
VSEPR THEORY
1.
(A)
2.
(B)
3.
(D)
4.
(A)
5.
(A)
7.
(C)
8.
(A)
9.
(C)
10.
(A)
11.
(A)(B)(C(D)
12.
(A)(C)(D) 13.
6
14.
1
15.
(i)Bent
(ii)Bent
(iii) Trigonal planar
(iv) Linear
(v) Tetrahedral
(vi) Tetrahedral
(vii) Trigonal pyramidal
(viii) Trigonal pyramidal
(ix) Octahedral
(x) Linear
(xi) Linear
(xii) Bent-T
(xiii) See-saw
(xiv) Trigonal bipyramidal
(xv) Tetrahedral
(xvi) Square planar
(xvii) Trigonal pyramidal
(xviii) Bent-T
(xix)Bent
(xx) Bent
(xxi) Linear(xxii) Bent
(xxiii) Square planar
(xxiv) See-saw
(xxv) See-saw
RESONANCE
1.
(B)
2.
(C)
3.
(A)
6.
(A)(B)(C) 7.
1
8.
8
9.
(i) 1.33
(ii) 2
(ix) 1.5
(x) 1.33
(iii) 1.33
4.
(iv) 1.5
(B)
(v) 1.25
86
5.
(vi) 1.75
(A)(B)(D)
(vii) 1.5
(viii) 1.67
Chemical Bonding
BOND PARAMETERS
1.
(C)
2.
(D)
3.
(A)
4.
7.
(B)
8.
(A)
9.
(A)(B)(D) 10.
11.
(A)-PQRT ; (B)-ST ; (C)-PST ; (D)-RT
15.
(i) BF3 = BCl3 = BBr3 = BI3
(ii) CO2 > CH4 > NH3 > H2O
(iv) NH4+ > NH3 > NH2–
(v) C3O2 > CO32– > CCl4
12.
(C)
5.
(A)
6.
(C)
13.
0
14.
0
(A)(B)
4
(iii) N2O > NO–3 > NO2–
BACK BONDING & BRIDGE BONDING
1.
(D)
2.
7.
(A)(B)(C)(D)
10.
(A)-P ; (B)-QS ; (C)-QST ; (D)-RT
13.
ii,v,vi,viii
(D)
3.
(B)
4.
8.
(A)(C)(D) 9.
11.
5.
(B)
(B)
6.
(C)(D)
(A)-QRS ; (B)-QRT ; (C)-PRT ; (D)-QRS
2
12.
4
5.
(D)
MISCELLENEOUS
1.
(C)
7.
10.
2.
3.
(B)
4.
(A)
(A)(B)(C)(D)
8.
1
9.
(i), (iii),(iv)
(i) Planar
(iii) Non planar
(B)
(ii) Non planar
(vi) Planar (vii) Non planar (viii) Planar
(iv) Planar
(v) Non planar
(ix) Planar
(x) Planar
6.
(B)(C)
6.
(A)
DIPOLE MOMENT
1.
(D)
2.
(B)
3.
(A)
4.
(A)
5.
(B)
7.
(A)
8.
(C)
9.
(A)(B)
10.
(A)(C)
11.
(A)(B)(C) 12.
13.
9
14.
3
15.
(i) NP
(ii) P
(iii) NP
(iv) NP
(v) P
(vi) NP
(vii) NP
(viii) NP
(ix) P
(x) NP
(xi) NP
(xii) P
(xiii) P
(xiv) P
(xv) NP
(xvi) NP
(xvii) NP
(xviii) P
(xix) NP
(xx) P
9
MOLECULAR ORBITAL THEORY-I
1.
(A)
2.
(D)
3.
(A)
7.
(A)(C)
8.
(A)(C)
9.
(A)(B)(C)(D)
12.
6
13.
2
14.
2
15.
(i) 0.5, p
(ii) 0.5, p
(ix) 2.5, p (x) 1, D
4.
(B)
(A)
6.
(A)
10.
(C)
11.
(D)
(iii) 3, D
(iv)1.5, p
(xi) 3, D
(xii) 2.5, p (xiii) 0.5, p (xiv) 1.5, p (xv) 3, D
(xvii) 0.5, p(xviii )2, p (xix) 1,D
(v) 1.D
5.
(xx) 0.5, p
87
(vi) 2.5, p (vii) 2, D
(viii) 1, P
(xvi) 1.5, p
INORGANIC CHEMISTRY
MOLECULAR ORBITAL THEORY-II
1.
(A)
2.
7.
(A)(B)(C)(D)
11.
(C)
15.
5
12.
(D)
3.
(D)
4.
(D)
8.
(B)(C)
9.
(A)(B)(C)(D)
(A)-PQRS ; (B)-PQR ; (C)-QT ; (D)-S
5.
13.
(C)
3
6.
(B)
10.
(A)(C)
14.
1
6.
(D)
6.
(C)
6.
(B)(D)
9.
1
INTRODUCTION OF IONIC BOND
1.
(C)
2.
(B)
3.
(A)
4.
(A)
7.
(B)
8.
(C)
9.
9
10.
1
5.
(D)
LATTICE ENTHALPY AND FAJAN’S RULE
1.
(D)
2.
(C)
3.
(B)
4.
(B)
5.
(C)
7.
(D)
8.
(A)
9.
(B)
10.
(B)
11.
(A)
12.
(A)(B)(D) 13.
(A)(C)
14.
4
15.
2
5.
(C)
INERT PAIR EFFECT
1.
(A)
2.
7.
(A)(B)(C)(D)
10.
1
(A)
3.
(C)
4.
8.
(A)-Q ; (B)-PRS ; (C)-P ; (D)-Q
(D)
THERMAL STABILITY, SOLUBILITY OF IONIC COMPOUNDS
AND HEATING EFFECTS
1.
(D)
2.
7.
(A)(B)(C)(D)
(B)
3.
(A)
4.
8.
(A)(B)(C)(D)
(A)
5.
(A)
6.
(A)
9.
0
10.
4
5.
(D)
6.
(C)
5.
(A)(B)(C) 6.
(B)
WEAK FORCES
1.
(D)
2.
(C)
3.
(C)
4.
(B)
7.
(B)
8.
(C)
9.
6
10.
2
HYDROGEN BONDING
1.
(D)
2.
(B)
3.
(B)
4.
7.
(D)
8.
6
9.
6
10.
(i), (iv), (v), (vi), (viii) ® form intermolecular H–bond
(A)
(ii), (iii), (ix) ® form intramolecular H-bond
(vii), (x) ® Neither form intermolecular H-bond with their other molecule nor form intramolecular
H-bond
88
Gaseous State
IDEAL STATE
PRESSURE CALCULATION, BAROMETER & MANOMETER
1.
SINGLE CORRECT ANSWER TYPE
An open tank is filled which Hg upto a height of 76cm. What is the pressure at the
(i)
bottom of the tank ?
(A) 3 atm
(ii)
(B) 2 atm
(C) 4 atm
(D) 1 atm
middle of the tank. (If atmospheric pressure is 1 atm) ?
76 cm
(A) 2 atm
2.
(B) 1.0 atm
(C) 2.5 atm
(D) 1.5 atm
What is the the height of water upto which water must be filled to create the same pressure at the
bottom.
as in above problem ? hwdw = h Hg d Hg
(A) 1033.6 cm
3.
(B) 9033.6 cm
(C) 7033.6 cm
(D) 8033.6 cm
What will be the pressure if two immiscible fluid is filled according to given diagram.
Total pressure = h2d2g + h1d1g
d1 > d2
h2
h2d2g
h1
(i)
(ii)
h1d1g
What is the pressure at the bottom of tank ?
(A) Patm + h2d1 g + h1d2 g
(B) Patm + h3d4 g + h2d2 g
(C) Patm + h2d2 g + h1d1 g
(D) Patm + h1d2 g + h2d1 g
What is the pressure at the middle point of bottom layer.
(A) Patm + h2d2 g +
h1
dg
2 1
(B) Patm + h1d2 g +
h2
dg
2 1
(C) Patm + h1d1 g +
h2
dg
4 1
(D) Patm + h1d2 g +
h1
dg
3 2
89
JEE-Chemistry
4.
In the figure the pressure of the confined gas will be
(A) 30 cm of Hg
5.
(B) 40 cm of Hg
(C) 36 cm of Hg
(D) 46 cm of Hg
Calculate the number of moles of gas present in the container of volume 10 L at 300 K. If the
manometer containing glycerin shows 5 m difference in level as shown diagram.
(Given : dglycerin = 2.72 g/mL; dmercury = 13.6 g/mL)
(A) 0.94 mole
(B) 0.49 mole
(C) 0.64 mole
90
(D) none of these
Gaseous State
GAS LAW
1.
SINGLE CORRECT ANSWER TYPE
A gas occupies one litre under atmospheric pressure. What will be the volume of the same amount of
gas under 750 mm of Hg at the same temperature.
(A) 1.0133 lit.
(B) 2.0133 lit.
(C) 3.0133 lit.
(D) 5.0133 lit.
2.
10 g of a gas at STP occupies 5 litres. The temp. at which the volume becomes double for the same
mass of gas at the same pressure is ?
(A) 273K
(B) –2730C
(C) 2730C
(D) 5460C
3.
Figure shows graphs of pressure versus density for an ideal gas at two temperatures T1 and T2. Which
is correct:
(A) T1 > T2
(B) T1 = T2
(C) T1 < T2
(D) None of the above
4.
A gas is initially at 1 atm pressure. To compress it to 1/4 th of initial volume, what will be the pressure
required ? (Assume process is isothermal]
(A) 6 atm
(B) 4 atm
(C) 10 atm
(D) 8 atm
5.
If the temp. of a particular amount of gas is increased from 27ºC to 57ºC, find final volume of the gas,
if inital volume = 1 L and assume pressure is constant.
(A)1.1 L
(B) 2.1 L
(C) 3.1 L
(D) 4.1 L
6.
Four one litre flasks are separately filled with the gases, O2, F2, CH4 and CO2 under the same conditions.
The ratio of number of molecules in these gases :
(A) 2 : 2 : 4 : 3
(B) 1 : 1 : 1 : 1
(C) 1 : 2 : 3 : 4
(D) 2 : 2 : 3 : 4
7.
Which of the following curve does not represent Boyle’s law?
P
log P
(A)
(B)
V
8.
q = 45°
log P
135°
PV
(D)
(C)
log (V–1)
log (V–1)
V versus T curves at constant pressure P1 and P2 for an
ideal gas are shown in figure. Which is correct?
(A) P1 > P2
(B) P1 < P2
(C) P1 = P2
(D) All of these
91
V
P1
P2
V
T
JEE-Chemistry
9.
Which one of these graphs for an ideal gas, the arrow indication is incorrectly marked?
V
(A)
Decreasing
Pressure
(B)
–273ºC
tºC
P
Decreasing Temp.
(C)
(D)
0
10.
1/V
A rubber balloon contains some solid marbles each of volume 10 ml. A gas is filled in the balloon at
a pressure of 2 atm and the total volume of the balloon is 1 litre in this condition. If the external
pressure is increased to 4atm the volume of Balloon becomes 625 ml. Find the number of marbles
present in the balloon.
(A) 30
(B) 20
(C)35
92
(D) 25
Gaseous State
IDEAL GAS EQUATION
1.
SINGLE CORRECT ANSWER TYPE
In the gas equation PV = nRT the value of universal gas constant depends upon –
(A) The nature of the gas
(B) The pressure of the gas
(C) The temperature of the gas
(D) The units of measurement
2.
One litre of an unknown gas weighs 1.25g at N.T.P. which of the following gas pertains to the above
data
(A) CO2
(B) NO2
(C) N2
(D) O2
3.
2.8 g of a gas at 1 atm and 273 K occupies a volume of 2.24 litres, the gas can not be:
(A) O2
(B) CO
(C) N2
(D) C2H4
4.
Equal volumes of two gases which do not react together are enclosed in separate vessels. Their
pressures are 10 mm and 400 mm respectively. If the two vessels are joined together, then what
will be the pressure of the resulting mixture (temperature remaining constant)
(A) 120 mm
(B) 500 mm
(C) 1000 mm
(D) 205 mm
5.
A 0.50 L container is occupied by nitrogen at a pressure of 800 torr and a temperature of 0°C. The
container can only withstand a pressure of 3.0 atm. What is the highest temperature (°C) to which the
container may be heated?
(A) 505
(B) 450
(C) 625
(D) 560
6.
Densities of two gases are in the ratio 1 : 2 and their temperatures are in the ratio 2 : 1, then the ratio
of their respective molar mass at certain pressure is:
(A) 1 : 1
(B) 1 : 2
(C) 2 : 1
(D) 4 : 1
7.(i)
Plot the curve between PT vs T at const V & constant no of moles. ?
PT
PT
(A)
(B)
(C)
T
(ii)
PT
PT
(D)
T
T
T
What is the number of moles of gas taken when the volume of the vessel is 82.1ml and
d
[PT]at300K = 300 for the given curve ?
dT
(A) n =
1
2
(B) n =
1
4
(C) n =
93
1
6
(D) n =
1
8
JEE-Chemistry
8.(i) Radius of a bubble at the bottom of the tank shown below was found to be 1 cm, then find the radius
of the bubble at the surface of water considering the temperature at the surface & bottom being same.
Water
(A) 3 8 cm
(ii)
(B)
3
2 cm
10.336 m
(C) 3 6 cm
(D)
3
4 cm
If absolute temperature at the surface is 4 times that at the bottom, then find radius of bubble at the
surface.
(A) r' = 4 cm
(B) r' = 6 cm
(C) r' = 2 cm
94
(D) r' = 8 cm
Gaseous State
DALTONS LAW
1.
SINGLE CORRECT ANSWER TYPE
The total pressure of a mixture of two gases is equal to :
(A) Sum of their partial pressures
(B) The difference in partial pressures
(C) The product of partial pressures
(D) The ratio of partial pressures
2.
Equal massesof SO2, CH4 and O2 are mixed in empty container at 298K, when total pressure is 2.1 atm.
The partial pressures of CH4 in the mixture is –
(A) 0.5 atm
(B) 0.75 atm
(C) 1.2 atm
(D) 0.6 atm
3.
The partial pressure of hydrogen in a flask containing 2g of H2 & 32g of SO2 is
(A)
1
16
(C)
2
3
of total pressure
of total pressure (D)
(B)
1
8
1
of total pressure
2
of total pressure
4.
Air contains 79% N2 and 21% O2 by volume. If the barometric pressure is 750 mm Hg the partial
pressure of oxygen is :
(A) 157.5 mm of Hg (B) 175.5 mm of Hg (C) 315.0 mm of Hg (D) None
5.
O2 and SO2 gases are filled in ratio of 1 : 3 by moles in a closed container of 3 L at temperature of
27°C. The partial pressure of O2 is 0.60 atm, the concentration of SO2 would be
(A) 0.36
(B) 0.074
(C) 3.6
(D) 36
6.
If 2 lit. of gas A at 1.5 atm and 3 lit. of gas B at 2 atm are mixed in a 5 lit. container then what is the
final pressure, considering all are at same temperature.
(A) 1.6 atm
(B)1.8 atm
(C) 1.7 atm
(D) 1.9 atm
7.
2 moles of NH3(g) and 1 mole of HCl(g) are taken in a container of capacity 8.21 lit at 300 K to
produce NH4Cl(s). Find the total pressure after the reaction.
(A) 3 atm
(B) 4atm
(C) 5atm
(D) 6 atm
8.
One mole of N2 and 3 moles of H2 are taken in a container of capacity 8.21 lit. at 300 K to produce
NH3.
Find the partials pressure of N2 and H2 if partial pressure of NH3 after sufficient time was found to
be 3 atm.
N2 + H2 ¾® NH3
(A) 2.5 atm, 5.5 atm
(B) 1.5 atm, 4.5 atm
(C) 1.1 atm, 4.8 atm
(D) 1.2 atm, 4.1 atm
95
JEE-Chemistry
CONTAINER CAPACITY, CONNECTED CONTAINER GAS
PROBLEM AND PAYLOAD
SINGLE CORRECT ANSWER TYPE
1.
7
of its maximum volume at 27°C. Then calculate the minimum temperature
8
above which it will burst.
(A) 320.8 K
(B) 340.8 K
(C) 360.8 K
(D) 342.8 K
A balloon is inflated to
2.
A gas cylinder containing cooking gas can withstand a pressure of 18 atm. The pressure gauge of
cylinder indicates 12 atm at 27°C. Due to sudden fire in building the temperature start rising at what
temperature will the cylinder explode.
(A) 420 K
(B) 410 K
(C) 450 K
(D) 430 K
3.
A tyre tube of maximum volume 8.21 lit. can withstand a pressure of 10 atm. Initially the tube is
empty.
What is the number of moles required to inflate completely the tube upto a pressure of 1 atm & 300
K temperature ?
(A) 1/4mol
(B) 1/6 mol,
(C) 1/3 mol
(D) 1/2 mol
(i)
(ii)
What is the minimum number of moles required to burst the tyre tube at 300 K ?
(A) 10/3 mol
(B) 30/3 mol
(C) 20/3 mol
(D) 17/3 mol
4.
An open flask contains air at 27°C. Calculate the temperature at which it should be heated so that
(i)
(ii)
5.
1
rd of air measured in the container at 27°C escape out.
3
(A) 150
(B) 250
(C) 350
(D) 450
1
rd of air measured in the container at final temperature escape out.
3
(A) 400
(B) 200
(C) 100
(D) 300
A container of 8.21 lit. capacity is filled with 1 mole of H2 at 300 K and it is connected to another
container of capacity 2 × 8.21 lit. containing 4 moles of O2 at 300 K, then what is the final pressure &
partial pressure of each gas in each container ?
2×8.21
8.21
H2
O2
(A) Pf =8 atm, p H 2 = 3 atm , pO 2 = 4 atm
(B) Pf = 10 atm, p H 2 = 2 atm , pO 2 = 4 atm
(C) Pf = 6 atm, p H 2 = 1 atm , p O 2 = 2 atm
(D) Pf = 5 atm, p H 2 = 1 atm , p O 2 = 4 atm
96
Gaseous State
6.
A 10 lit. container consist of 1 mole of a gas at 300 K. It is connected through very small nozzle to
another empty container having volume 40 lit. then calculate
(i)
Ratio of moles of gas in container B & A at same T.
(A)
(ii)
4
1
(B)
5
2
Pressure of the gas in both container
(A) 0.9826 atm
(B) 0.7826 atm
(C)
6
1
(C) 0.3026 atm
(D)
7
1
(D) 0.4926 atm
(iii)
If temperature of 40 L container is increased to 600 K keeping the other at 300 K. Find the pressure
of each container.
(A) 0.830 atm
(B) 0.820 atm
(C) 0.821 atm
(D) 0.840 atm
7.
A box of 1 L capacity is divided into two equal compartments by a thin partition which are filled with
2g H2 and 16 g CH4 respectively. The pressure in each compartment is recorded as P atm. The total
pressure when partition is removed will be:
(A) P
8.
(D) P/4
(B) 1.64 atm
(C) 0.328 atm
(D) 1 atm
A balloon weighing 50 kg is filled with 685 kg of helium at 1 atm pressure and 25°C. What will be its
pay load if it displaced 5108 kg of air?
(A) 4373 kg
10.
(C) P/2
Consider the following apparatus. Calculate the partial pressure of helium after the opening valve.
The temperature remains constant.
(A) 0.164 atm
9.
(B) 2P
(B) 4423 kg
(C) 5793 kg
(D) none of these
Find the payload which can be attached to a balloon of 821 lit. capacity if it is filled with Helium gas
at 3 atm and 27°C. Given density of air 2 g/L. wt. of material of balloon = 200 g.
(A) 4042 g
(B) 3042 g
(C) 2042 g
(D) 1042 g
97
JEE-Chemistry
DIFFUSION AND EFFUSION
SINGLE CORRECT ANSWER TYPE
1.
Compare the rate of diffusion of CO with a mixture of He and CH4 in 3 : 1 mole ratio under similar
condition.
(A)
2.
8
1
5
4
(B)
9
1
(C)
10
1
(D)
7
1
(B) 1 : 32
(C) 16 : 1
(D) 1 : 16
(B) MY = 4 MX
(C) MX = 4 MY
(D) None of these
(B) V = 32 ml
(C) V = 20 ml
(D) V = 16 ml
(B) 21 steps
(C) 30 steps
(D) 40 steps
A rigid container containing 5 mole H2 gas at some pressure and temperature. The gas has been
allowed to escape by simple process from the container due to which pressure of the gas
becomes half of its initial pressure and temperature become (2/3)rd of its initial. The mass of gas
remaining is :
(A) 7.5 g
8.
(D)
A mixture contains D2 and CH4 in 1 : 8 mole ratio. If it is desired to enrich the D2 to 80% of the
sample (by moles) making use of relative rates of effusion of D2 and CH4. How many minimum
effusion steps are required.
(A) 5 steps
7.
1
3
32 ml of He effuses through a fine orifice in 1 minute. Then what volume of CH4 will diffuse in 1
minute under the similar condition.
(A) V = 30 ml
6.
(C)
Pressure of 1 g ideal gas X at 300 K is 2 atm. When 2 g of another gas Y is introduced in the same
vessel at same temperature, the pressure become 3 atm then correct relationshs between molar mass
of X and Y is :
(A) MY = 2 MX
5.
1
2
A vessel contains H2 & O2 in the molar ratio of 8 : 1 respectively. This mixture of gases is allowed to
diffuse through a hole, find composition of the mixture coming out of the hole.
(A) 32 : 1
4.
(B)
A mixture of H2 and O2 in 2 : 1 mole ratio is allowed to diffuse through a orifice. Calculate the
composition of gases coming out initially.
(A)
3.
3
4
(B) 1.5 g
(C) 2.5 g
(D) 3.5 g
The rate of diffusion of a sample of a ozonized oxygen (mixture of O2 and O3) is 0.98 times than that
of oxygen. Find the % (by volume) of ozone in the ozonized sample.
(A) 8.25 %
(B) 10.25 %
(C) 4.25 %
98
(D) 6.25 %
Gaseous State
KTG
SINGLE CORRECT ANSWER TYPE
1.
Which of the following is NOT a postulate of the kinetic molecular theory of gases?
(A) The molecules possess a volume that is negligibly small compared to the container
(B) The pressure and volume of a gas are inversely related
(C) Gases consist of discrete particles that are in constant chaotic motion
(D) The average kinetic energy of the molecules is directly proportional to the temperature
2.
Which of the following statements about kinetic energy (K.E.) is true?
(A) All objects moving with the same velocity have the same K.E.
(B) The K.E. of a body will quadruple if its velocity doubles
(C) As the velocity of a body increases, its K.E. decreases
(D) The K.E. of a body is independent of its mass
3.
The Ne atom has 10 times the mass of H2. Which of the following statements is true?
I. At 25°C they both have the same average kinetic energy.
II. Ten moles of H2 would have the same volume as 1 mole of Ne at same temp. and pressure.
III. One mole of Ne exerts the same pressure as one mole of H2 at STP
IV. A H2 molecule travels 10 times faster than Ne atom at same temperature.
V. At STP, one litre of Ne has 10 times the density of 1 litre of H2.
(A) II, IV, V
4.
(B) I, III, V
(A)
æ 3RT ö 2
ç
÷
è Mw ø
1
(B)
1
æ 3P ö 2
ç
÷
è DM w ø
æ 3P ö 2
(C) ç ÷
è D ø
1
æ 3PVm ö 2
(D) ç
÷
è Mw ø
Average K.E. of CO2 at 270C is E. The average kinetic energy of NO2 at the same temperature will be
(A) E
6.
(d) I, II
Which of the following expression does not give root mean square velocity –
1
5.
(C) I, II, III
(B) 22E
(C) E/22
(D) E 2
(C) KENe < KEHe
(D) None of these
The average K.E. of He and Ne at 25°C is :
(A) KENe > KEHe
(B) KENe = KEHe
7.(i) Calculate the pressure exerted by 1023 gas molecules, each mass 10–22 g in a container of volume one
99
JEE-Chemistry
litre. The rms velocity is 105 cm/sec.
(ii)
(A) 3.33 × 107 dyne/cm2
(B) 3.33 × 105 dyne/cm2
(C) 3.33 × 103 dyne/cm2
(D) 3.33 × 102 dyne/cm2
What is the total kinetic energy (in cal) of these particles ?
(A) 1175.0 Cal
(B) 1195.0 Cal
(C) 1155.0 Cal
(D) 1185.0 Cal
(C) 1214.8 K
(D) 2414.8 K
(iii) What must be the temperature ?
(A) 3614.8 K
8.
Consider three one-litre flasks labeled A, B and C filled with the gases NO, NO2, and N2O, respectively each at 1 atm and 273 K. In which flask do the molecules have the highest average kinetic
energy?
(A) Flask C
9.
(B) 2214.8 K
(B) All have the same (C) Flask A
(D) None
If for two gases of molecular weights MA and MB at temperature TA and TB ; TAMB = TBMA, then
which property has the same magnitude for both the gases.
(A) Density
(B) Pressure
(C) KE per mol
100
(D) RMS speed
Gaseous State
MAXWELL’S DISTRIBUTION CURVE & MEAN FREE PATH AND
FREQUENCY PARAMETER
SINGLE CORRECT ANSWER TYPE
1.
At a definite temperature (T), the distribution of velocities is given by the curve. The curve that
indicates that the velocities corresponding to points A, B and C are :
(A) most probable, average and root mean square (B) average, root mean square and most probable
(C) root mean square, average and most probable (D) most probable, root mean square and average
2.
At what temperature will average speed of the molecules of the second member of the series CnH2n be
the same of Cl2 at 627°C?
(A) 259.4 K
3.
6.
(D) None of these
(B) T1 < T2 < T3
(C) T1 = T2 = T3
(D) None of these
6 ´ 1022 gas molecules each of mass 10–24 kg are taken in a vessel of 10 litre. What is the pressure
exerted by gas molecules? The root mean square speed of gas molecules is 100 m/s.
(A) 20 Pa
5.
(C) 532.4 K
If T1, T2 and T3 are the temperature at which the URMS, Uaverage, UMP of oxygen gas are all equal to 1500
m/s then the correct statement is :
(A) T1 > T2 > T3
4.
(B) 400 K
(B) 2 ´ 104 Pa
(C) 2 ´ 105 Pa
(D) 2 ´ 107 Pa
If C1, C2, C3...represent the speeds of n1, n2, n3...molecules respectively, then the root mean square
speed will be:
(A)
n1C12 + n 2 C22 + n3 C32 + ....
n1 + n 2 + n 3 + .....
(C)
(n1C 1 ) (n2 C 2 ) (n3C 3 )
+
+
n1
n2
n3
(B)
(n1 + n 2 + n 3 + ...)2
n1C12 + n 2 C 22 + n 3 C32 + .....
(D)
(n1C1 + n 2 C2 + n 2C3 + ....)2
n1 + n 2 + n 3 + .....
If URMS of a gas is 30 R1/2 ms–1 at 27°C then the molar mass of gas is
(a) 0.02 kg/mol
(b) 0.001 kg/mol
(c) 0.003 kg/mol
(d) 1 kg/mol
101
JEE-Chemistry
7.
If pressure of ideal gas is increased 4 times at constant volume then mean free path [l] :
(A) quadruples
8.
(D) remains same
(B) Decreases
(C) Remains constant (D) can not be determined
An ideal gas present at 300K is heated at constant volume such that its collision frequency (Z11)
becomes double of its initial value. Then final temperature of gas is :
(A) 300 K
10.
(C) half
On increasing pressure of an ideal gas isothermally collision number (Z1)
(A) increases
9.
(B) doubles
(B) 600 K
(C) 800 K
(D) 1200 K
Two flask X and Y have equal volume. X is maintained at 300K and Y at 600K while X contains H2
gas, Y contains equal mass of CH4 gas. Assuming ideal behavour for both the gases and collision
diameters [s] of H2 and CH4 same. Which flask contains molecules with greater mean path [l] :
(A) X
(B) Y
(C) both have same value
(D) can not be determined.
102
Gaseous State
EUDIOMETRY
1.
SINGLE CORRECT ANSWER TYPE
C6H5OH (g) + O2 (g) ¾® CO2 (g) + H2O (l)
Magnitude of volume change if 30 ml of C6H5OH (g) is burnt with excess amount of oxygen, is
(A) 30 ml
2.
(B) 10%
(C) 18%
(D) 2%
(B) 36.4
(C) 54.6
(D) 91.0
(B) 40
(C) 60
(D) 80
(B) C4H10
(C) C3H6
(D) C2H4
16mL of a hydrocarbon gas was exploded with excess of oxygen. On cooling, the volume of the
resulting gasous mixture was reduced by 48mL. When KOH was added, there was a further decrease
of 48mL in the volume. Find the molecular formula of the compound.
(A) C3H8
8.
(D) 560
10mL of a gasous hydrocarbon was burnt completely in 80mL of O2 at 1atm and 273K. The remaining
gas occupied 70mL at 1atm and 273K. This volume became 50mL on treatment with KOH solution.
What is the formula of the hydrocarbon ?
(A) C2H6
7.
(C) 440
20 mL of CO was mixed with 50mL of oxygen and the mixture was exploded. On cooling, the
resulting mixture was shaken with KOH. Find the volume(in ml) of the gas that is left.
(A) 20
6.
(B) 340
What volume (in L) oxygen will be required for the complete combustion of 18.2 litres of propane at
1atm and 273K?
(A) 18.2
5.
(D) 10 ml
When 20 ml of mixture of O2 and O3 is heated, the volume becomes 29 ml and disappears in alkaline
pyrogallol solution. What is the volume percent of O2 in the original mixture?
(A) 90%
4.
(C) 20 ml
The % by volume of C4H10 in a gaseous mixture of C4H10, CH4 and CO is 40. When 200 ml of the
mixture is burnt in excess of O2, find volume (in ml) of CO2 produced.
(A) 220
3.
(B) 60 ml
(B) C3H10
(C) C3H6
(D) C2H8
7.5mL of hydrocarbon gas was exploded with excess of oxygen. On cooling, it was found to have
undergone a contration of 15mL. If the vapour density of the hydrocarbon is 14, determine its molecular
formula.
[C = 12, H =1]
(A) C3H8
9.
(C) C4H10
(D) C2H6
7.5mL of a gasous hydrocarbon was exploded with 36mL of oxygen. The volume of gases on cooling
was found to be 28.5mL, 15mL of which was absorbed by KOH ans the rest was absorbed in a
solution of alkaline pyrogallol. If all volumes are measured under the same condition, deduce the
formula of the hydrocarbon.
(A) C4H10
10.
(B) C2H4
(B) C6H6
(C) C2H4
(D) C2H6
500ml of hydrocarbon gas , burnt in excess of oxygen, yields 2500ml of CO2 and 3 liter of water
vapour, all volumes being measured at the same temperature and pressure. What is the formula of
hydrocarbon.
(A) C5H12
(B) C4H10
(C) C6H6
(D) C2H2
103
JEE-Chemistry
ANSWER KEY
PRESSURE CALCULATION, BAROMETER & MANOMETER
1.
(i)-(B), (ii)-(D)
2.
3.
(A)
(i)-(C), (ii)-(A)
4.
(B)
5.
(A)
5.
(A)
6.
(B)
5.
(A)
6.
(A)
5.
(B)
6.
(B)
GAS LAW
1.
(A)
2.
(C)
3.
(A)
4.
(B)
7.
(C)
8.
(B)
9.
(B)
10.
(D)
IDEAL GAS EQUATION
1.
(D)
2.
7.
(i)-(D), (ii)-(A)
(C)
3.
(A)
4.
8.
(i)-(B), (ii)-(C)
(D)
DALTONS LAW
1.
(A)
2.
(C)
7.
(A)
8.
(B)
3.
(C)
4.
(A)
CONTAINER CAPACITY, CONNECTED CONTAINER GAS
PROBLEM AND PAYLOAD
1.
(D)
2.
6.
(i)-(A),(ii)-(D), (iii)-(C)
(C)
3.
(i)-(C), (ii)-(A)
4.
(i)-(D), (ii)-(A)
5.
(D)
7.
(A)
8.
(A) 9.
(A)
10.
(D)
DIFFUSION AND EFFUSION
1.
(B)
2.
(A)
7.
(A)
8.
(A)
3.
(A)
4.
(B)
5.
(D)
6.
(A)
5.
(A)
6.
(B)
KTG
1.
(B)
2.
7.
(i)-(A), (ii)-(B),(iii)-(D)
(B)
3.
(B)
4.
(B)
8.
(B)
9.
(D)
MAXWELL’S DISTRIBUTION CURVE & MEAN FREE PATH AND
FREQUENCY PARAMETER
1.
(A)
2.
(C)
3.
(B)
4.
(B)
7.
(D)
8.
(A)
9.
(D)
10.
(B)
5.
(A)
6.
(D)
5.
(B)
6.
(D)
EUDIOMETRY
1.
(B)
2.
(C)
3.
(B)
4.
(D)
7.
(C)
8.
(B)
9.
(C)
10.
(A)
104
Gaseous State
REAL GAS
SINGLE CORRECT ANSWER TYPE
1.
2.
3.
A real gas obeying vander waal equation will resemble ideal gas if the
(A) constants a and b are negligibly small
(B) a is large and b is small
(C) a is small and b is large
(D) constant a and b are large
The compressibility factor of real gas is usually greater than one (Z > 1) at high temperature and high
pressure. This is because
(A) the constant a is negligible while b is not
(B) the constant b is negligible while a is not
(C) both a and b are negligible
(D) both a and b are no negligible
The value of vander Waal’s constant ‘a’ for the gases O2, N2, NH3 and CH4 are 1.36 , 1.39, 4.17 and
2.253 L2 atm mol–2, respectively. The gas which can most easily be liquefied is
(A) O2
4.
5.
(B) N2
(C) NH3
(D) CH4
What is not true about the vander waal constant ‘b’ among the statements given below ?
I. It is called excluded volume
II. It accounts for the interparticle forces
III. Its units are mol dm–3
IV. Its value depends on molecular size
(A) I, II
(C) II, III
(B) II, IV
(D) I, IV
Vander Waal’s constant for three different gases are given
Gas
a (L2 atm mol–2) b (L mol–1)
X
3.0
0.025
Y
10.0
0.030
Z
6.0
0.035
Which is correct ?
6.
7.
8
(A) Maximum critical temperature - Y
(B) Most ideal behaviour - X
(C) Maximum molecular volume - Z
(D) All are correct
Consider an ideal gas contained in a vessel. If the intermolecular interaction suddenly begins to act,
which of the following will happen :
(A) the observed pressure decreases
(B) the observed pressure increases
(C) the observed pressure remains same
(D) none of these
A real gas obeying Vander Waals equation will resemble ideal gas, if the :
(A) constants a & b are small
(B) a is large & b is small
(C) a is small & b is large
(D) constant a & b are large
Calculate the compressibility factor for CO2, if one mole of it occupies 0.4 litre at 300 K and 40 atm.
Comment on the result :
(A) 0.40, CO2 is more compressible than ideal gas
(B) 0.65, CO2 is more compressible than ideal gas
(C) 0.55, CO2 is more compressible than ideal gas
(D) 0.62, CO2 is more compressible than ideal gas
105
JEE-Chemistry
9.
10.
11.
12.
13.
Calculate the radius of He atoms if its Vander Waal's constant 'b' is 24 ml mol–1 :
(Note ml = cubic centimeter)
(A) 1.33 Å
(B) 1.314 Å
(C) 1.255 Å
(D) 0.355 Å
The critical constant for water are 374°C, 218 atm and 0.0566 litre mol–1. Calculate a & b.
(A) a = 1.095 litre2 atm mol–2, b = 0.0185 litre mol–1
(B) a = 1.92 litre2 atm mol–2, b = 0.185 litre mol–1
(C) a = 2.095 litre2 atm mol–2, b = 0.0189 litre mol–1
(D) a = 2.95 litre2 atm mol–2, b = 0.1185 litre mol–1
The compressibility of a gas is less than unity at STP. Therefore :
(A) Vm > 22.4 L
(B) Vm < 22.4 L
(C) Vm = 22.4 L
(D) Vm ³ 44.8 L
If two moles of an ideal gas at 546 K occupies a volume of 44.8 litres, the pressure must be :
(A) 2 atm
(B) 3 atm
(C) 4 atm
(D) 1 atm
Consider the following statements :
The coefficient B in the virile equation on state
æ
B
C
ö
+
+ .......... ÷
PVm = RT çç 1 +
2
÷
Vm Vm
è
ø
14.
15.
a : is independent of temperature
b : is equal to zero at boyle temperature
c : has the dimension of molar volume
Which of the above statements are correct.
(A) a and b
(B) a and c
(C) b and c
(D) a, b and c
Consider the following statements : If the vander Waal's parameters of two gases are given as
a (atm lit2 mol–2)
b (lit mol–1)
Gas X : 6.5
0.056
Gas Y : 8.0
0.011
then a : VC (X) < VC (Y)
b : PC (X) < PC (Y)
c : TC (X) < TC (Y)
Select correct alternate :
(A) a alone
(B) a and b
(C) a,b and c
(D) b and c
The temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is :
(A) critical temperature
(B) Boyle temperature
(C) boiling temperature
(D) reduced temperature
ANSWER KEY
1.
7.
13.
(A)
(A)
(C)
2.
8
14.
(A)
(B)
(D)
3.
9.
15.
(C)
(A)
(B)
4.
10.
106
(C)
(C)
5.
11.
(D)
(B)
6.
12.
(A)
(A)
Important Notes
107
Gaseous State
JEE-Chemistry
Important Notes
108
Redox Reaction
REDOX REACTION
CALCULATION OF OXIDATION NUMBER
1.
Fluorine does not show positive oxidation state due to the (A) Absence of s-orbitals
(B) Absence of p-orbitals
(C) Absence of d-orbitals
(D) Highest electronegativity
2.
Oxidation state of hydrogen in CaH 2 is (A) +1
(B) –1
(C) + 2
(D) 0
Oxidation number of C in CH2Cl2 is (A) +2
(B) + 4
(C) – 4
(D) 0
The oxidation number of P is + 3 in (A) H3PO3
(B) H3PO4
(C) HPO3
(D) H4P2O7
Oxidation number of carbon in diamond is (A) – 4
(B) + 4
(C) 0
(D) + 2
3.
4.
5.
6.
7.
The oxidation number of carbon in C 12H22O11 is (A) 0
(B) – 6
(C) + 6
(D) + 2
The oxidation state of iodine in H 4 IO6- is:
(A) +7
(B) –1
(C) +5
(D) +1
8.
In which of the following compounds, the oxidation state of I-atom is highest(A) KI3
(B) KIO4
(C) KIO3
(D) IF 5
9.
The oxidation number of phosphorus in Ba(H 2PO2)2 is(A) + 3
(B) + 2
(C) + 1
(D) – 1
The oxidation number of nitrogen in NH2OH is(A) + 1
(B) – 1
(C) – 3
(D) – 2
Oxygen has the oxidation state of + 2 in(A) SO2
(B) CO2
(D) OF 2
10.
11.
12.
13.
(C) H2O2
The oxidation number of chlorine in HOCl is(A) – 1
(B) 0
(C) + 1
(D) 2
O.N. of hydrogen in KH, MgH 2 and NaH respectively would be(A) –1, – 1 and –1 (B) +1, + 1, and + 1 (C) +2, +1 and –2
(D) –2, –3 and –1
109
JEE-Chemistry
14.
15.
16.
17.
Oxidation number of nitrogen can be(A) From + 5 to – 3
(C) From – 5 to + 3
(B) From – 5 to – 3
(D) From + 10 to + 6
Oxidation Number of Mn can be(A) +2 to +6
(B) +2, +3
(C) +2 to +7
(D) +2, +8
Oxidation number of iodine varies from –
(A) –1 to +1
(B) –1 to +7
(C) +3 to +5
(D) –1 to +5
The oxidation state of Oxygen atom in potassium superoxide is(A) Zero
18.
(B) –
1
2
(C) – 1
The oxidation state of tungsten in Na 2W4O13.10H2O is –
(A) + 7
(B) + 6
(C) + 4
19.
The oxidation number of S in Na2S4O6 is (A) + 2.5
(B) + 2 and + 3 (two S have + 2 and other two have + 3)
(C) + 2 and + 3 (three S have + 2 and one S has + 3)
(D) + 5 and 0 (two S have + 5 and the other two have 0)
20.
Carbon is in the lowest oxidation state in –
(A) CH 4
(B) CCl4
(C) CF4
(D) – 2
(D) + 4.5
(D) CO 2
21.
Oxidation numbers of two Cl atoms in bleaching powder, CaOCl 2 is –
(A) – 1,– 1
(B) + 1, – 1
(C) + 1,+ 1
(D) 0, – 1
22.
In Wustite Fe0.93 O, the oxidation number of iron is
(A) 200/93
(B) 100/93
(C) 0.4
(D) 0.3
The oxidation state of Cr in CrO5 is (A) +6
(B) +10
(D) +4
23.
24.
(C) +5
The oxidation state of C and N in HCN are respectively (A) +2, –3
(B) –2, +3
(C) –2, +2
110
(D) +3, –3
Redox Reaction
CONCEPT OF OXIDATION & REDUCTION REACTIONS
1.
According to classical concept, oxidation involves (A) Addition of oxygen
(B) Addition of electronegative radical
(C) Removal of either hydrogen or some electropositive radical
(D) All of these
2.
According to modern concept, oxidation is (A) Electronation
(B) Deelectronation
(C) Addition of oxygen
(D) Addition of electronegative element
3.
Oxidation takes place with (A) Gain of electrons
(B) Loss of electrons
(C) Increase in the valency of negative part (D) Decrease in the valency of positive part
4.
When SO2 is passed through acidified K2Cr2O7 solution, Cr2(SO4)3 is formed. The change in
oxidation number of Cr is –
(A) + 4 to + 2
(B) + 5 to + 3
(C) + 6 to + 3
(D) + 7 to + 1
5.
In the reaction
2Na2S2O3 + I2 ® Na2S4O6 + 2NaI,
the oxidation state of S is (A) Increased
(B) Decreased
(C) Remains same
(D) None
In the rusting of iron, iron has been(A) Oxidised
(B) Reduced
(C) Vapourised
(D) Decomposed
6.
7.
The conversion of sugar C12H22O11 ¾¾® CO2 is(A) Oxidation
(B) Reduction
(C) Neither oxidation nor reduction
(D) Both oxidation and reduction
8.
Oxidation is defined as(A) Gain of electrons
(C) Loss of electrons
(B) Decrease in positive valency
(D) None
9.
In the reaction MnO4– + SO32– + H+ ¾¾® SO42– + Mn2+ + H2O
(A) MnO4– and H+ both are reduced
(B) MnO4– is reduced and H+ is oxidised
(C) MnO4– is reduced and SO32– is oxidised
(D) MnO4– is oxidised and SO32– is reduced
10.
In a reaction between zinc and iodine, zinc iodide is formed, what is being oxidised(A) Zinc ions
(B) Iodide ions
(C) Zinc atom
(D) Iodine
111
JEE-Chemistry
11.
In which of the following reactions, the underlined element has decreased its oxidation number
during the reaction ?
(A) Fe + CuSO4 ® Cu + FeSO 4
(B) H2 + Cl2 ® 2HCl
(C) C + H2O ® CO + H2
(D) MnO2 + 4HCl ® MnCl2 + Cl2 + 2H2O
12.
In C + H2O ¾¾® CO + H2, H2O acts as(A) Oxidising agent (B) Reducing agent (C) Both
(D) None
Identify oxidising & Reducing AgentPbS + 4H2O2 ® PbSO4 + 4H2O
(A) PbS, H2O2
(B) H2O2, PbS
(D) PbS both
13.
14.
15.
(C) H2O2 both
Which one can act as oxidising & reducing agent both(A) HNO2
(B) H2O2
(C) H2SO3
(D) all
Which compound can not be used as oxidising agent(A) O3
(B) HNO3
(C) KMnO4
(D) NH3
16.
AB4¯ + C+2 ® C+3 + A+2
If the O.N. of B is –2. Choose the true statement for the above change –
(A) O.N. of A decreases by –5
(B) O.N. of C decreases by +1
(C) O.N. of A decreases by + 5 and that of C increases by +1
(D) O.N. of A decreases by +5 and that of C decreases by +1
17.
Which of the following reactions does not involve either oxidation or reduction –
(A) VO2+ ® V2O3
(B) Na ® Na+
(C) Zn+2 ® Zn
(D) CrO4–2 ® Cr2O7–2
18.
H2MoO4 ® MoO2+ in the process H2MoO4 –
(A) Acts as a reducing agent
(B) Acts as an oxidising agent
(C) Acts both as a reducing and oxidising agent
(D) None of these
19.
A species that cannot be a reducing agent is (C) H2SO4
(A) SO2
(B) SO32–
112
(D) S2–
Redox Reaction
TYPE OF REDOX REACTION
1.
The reaction,
2K2MnO4 + Cl2 ® 2KMnO4 + 2KCl
is an example of (A) Oxidation
(B) Reduction
(C) Redox
(D) Chlorination
2.
In the reaction,
3Br2 + 6CO32– + 3H2O ® 5Br– + BrO3–+ 6HCO3–
(A) Bromine is oxidised and carbonate is reduced
(B) Bromine is oxidised as well as reduced
(C) Bromine is reduced and water is oxidised
(D) Br 2 is neither oxidised nor reduced
3.
Which one of the following is a redox reaction ?
(A) H2 + Br2 ® 2HBr
(B) 2NaCl + H2SO4 ® Na2SO4 + 2HCl
(C) HCl + AgNO3 ® AgCl + HNO3
(D) NaOH + HCl ® NaCl + H2O
4.
The reaction
Zn(s) + Cu2+(aq) ® Zn+2(aq) + Cu(s) is (A) Combination redox reaction
(C) Displacement redox reaction
(B) Decomposition redox reaction
(D) None
A redox reaction is (A) Proton transfer reaction
(C) Ion combination reaction
(B) Electron transfer reaction
(D) A reaction in a solution
5.
6.
Which of following is not a redox change ?
(A) 2H2S + SO2 ® 2H2O + 3S
(B) 2BaO + O2 ® 2BaO2
(C) BaO2 + H2SO4 ® BaSO4 + H2O2
(D) 2KClO3 ® 2KCl + 3O2
7.
Which of the following examples does not represent disproportionation ?
(A) MnO2 + 4HCl ® MnCl2 + Cl2 + 2H2O
(B) 2H2O2 ® 2H2O + O2
(C) 4KClO3 ® 3KClO4 + KCl
(D) 3Cl2+ 6NaOH ® 5NaCl + NaClO3 + 3H2O
8.
Which of the following is a disproportionation reaction ?
9.
(A) Cu2O + 2H+ ® Cu + Cu2+ + H2O
(B) 2CrO24- + 2H+ ® Cr2 O 72- + H2O
(C) CaCO3 + 2H+ ® Ca2+ + H2O + CO2
(D) Cr2 O 72- + 2OH¯ ® 2CrO24- + H2O
D
2KClO3 ¾¾
® 2KCl + 3O2 is an example of(A) Inter molecular redox reaction
(B) Combination redox reaction
(C) Decomposition redox reaction
(D) Displacement redox reaction
113
JEE-Chemistry
10.
In the following reaction
4P + 3KOH + 3H2O ¾¾® 3KH2PO2 + PH3
(A) Only phosphorus is oxidised
(B) Only phosphorous is reduced
(C) Phosphorus is both oxidised and reduced
(D) Phosphorus is neither oxidised nor reduced
11.
NH4NO2 ® N2 + 2H2O
The above reaction is called
(A) Disproportionation reaction
(C) Acid base reaction
(B) Comproportionation reaction
(D) Inter molecular redox reaction
12.
Which of the following is a inter molecular redox reaction
(A) KClO 3 ® KClO4 + KCl
(B) KClO3 ® KCl + O2
(C) NH4NO2 ® N2 + 2H2O
(D) KMnO4 + H2C2O4 + H2SO4 ® MnSO4 + CO2 + H2O + K2SO4
13.
For the given reaction the incorrect statement is2KClO3 ® 2KCl + 3O2
(A) KClO 3 is oxidizing agent as well as reducing agent.
(B) Cl present in KClO3 is reduced.
(C) Oxygen present in KClO3 is oxidized.
(D) It is a disproportionation reaction.
14.
(NH4 )2 Cr2O7 ¾¾¾® Cr2O3 + N2 + 4H2O
heat
The above reaction is called(A) Intra molecular redox reaction
(C) Acid base reaction
15.
(B) Inter molecular redox reaction
(D) Unpredictable
Which of the following species, do not show disproportionation reaction.
(D) ClO4–
(C) ClO3–
(A) ClO–
(B) ClO2–
114
Redox Reaction
BALANCING OF REDOX REACTION
1.
For the redox reaction
MnO4– + C2O42– + H+ ® Mn2+ + CO2 + H2O
the correct coefficients for the balanced reaction are –
H+
C2O42–
MnO4–
(A) 2
5
16
(B) 16
5
2
(C) 5
16
2
(D) 2
16
5
2.
For the redox reaction
MnO4– + Fe++ + H+ ® Mn2+ + Fe3+ + H2O
in the balanced equation, correct coefficient are –
Fe2 +
H+
MnO4–
(A) 1
5
8
(B) 16
5
2
(C) 5
16
2
(D) 2
16
5
3.
What will be the value of x, y and z in the following equation –
H2C2O4 + xH2O2 ® yCO2 + zH2O
(A) 2, 1, 2
(B) 1, 2, 2
(C) 2, 2, 1
(D) None
What will be the value of x, y and z in the following equation –
xI2 + yOH– ® IO3– + zI– + 3H2O
(A) 3, 5, 6
(B) 5, 6, 3
(C) 3, 6, 5
(D) 6, 3, 5
Cu + X ¾® Cu (NO3)2 + 2H2O + 2NO2. Here X is(A) 4HNO3
(B) 2HNO3
(C) 4HNO2
(D) 6HNO3
4.
5.
6.
In the reaction:
A - n 2 + xe ® A - n1
Here x will be –
(A) n1 + n2
7.
(B) n2 – n1
(C) n1 – n2
The stoichiometric coefficients of MnO -4 , Pb2+ and H2O in the balanced chemical equation of the
reaction Mn2+ + PbO 2 + H+ ® MnO 4- + Pb2+ + H2O , respectively are (A) 2, 5, 2
(B) 1, 4, 2
(C) 1, 2, 6
8.
(D) n1.n2
Which of the following equations is a balanced one(A) 5 BiO3– + 22H+ + Mn2+ ® 5Bi3+ + 7H2O + MnO4–
(B) 5 BiO3– + 14H+ + 2Mn2+ ® 5Bi3+ + 7H2O + 2MnO4–
(C) 2 BiO3– + 4H+ + Mn2+ ® 2Bi3+ + 2H2O + MnO4–
(D) 6 BiO3– + 12H+ + 3Mn2+ ® 6Bi3+ + 6H2O + 3MnO4–
115
(D) 1, 2, 3
JEE-Chemistry
9.
In the chemical reaction,
K2Cr2O7 + XH2SO4 + YSO2 ® K2SO4 + Cr2(SO4)3 + ZH2O
X, Y and Z are –
(A) 1, 3, 1
(B) 4, 1, 4
(C) 3, 2, 3
(D) 2, 1, 2
10.
In the redox reaction –
10FeC2O4 + x KMnO4 + 24H2SO4 ® 5Fe2 (SO4)3 + 20CO2 + y MnSO4
+ 3 K2SO4 + 24H2O.
The values of x and y are respectively –
(A) 6, 3
(B) 3, 6
(C) 3, 3
(D) 6, 6
116
Redox Reaction
CONCEPT OF EQUIVALENT WEIGHT (PART-I)
1.
When KMnO4 is titrated against FeSO4.(NH4)2SO4.6H2O the equivalent mass of KMnO4 (acidic)
is –
(A) Molecular mass / 10
(B) Molecular mass / 5
(C) Molecular mass / 2
(D) Molecular mass
2.
The equivalent weight of Na2S2O3 (Mol. wt = M) in the reaction,
2Na2S2O3 + I2 ® Na2S4O6 + 2NaI is –
(A) M/4
(B) M/3
(C) M/2
(D) M
3.
In the following unbalanced redox reaction,
Cu3 P + Cr2O72– —® Cu2+ + H3PO4 + Cr3+
Equivalent weight of H3PO4 is (A)
4.
M
3
31
4
8.
M
7
(D)
M
8
(B)
17
4
(C)
17
2
(D)
17
3
(B)
31
3
(C)
31
2
(D) 31 × 4/3
Equivalent weight of H3PO2 when it disproportionates into PH3 and H3PO3 is (mol. wt. of H3PO2
= M)
(A) M
7.
(C)
What is the equivalent weight of P 4 in the following reaction ?
P4 + NaOH ¾¾® NaH2 PO2 + PH3
(A)
6.
M
6
What is the equivalent weight of NH3 in the given reaction ?
3CuO + 2NH3 = 3Cu + N2 + 3H2O
(A) 17
5.
(B)
(B)
3M
4
(C)
M
2
Equivalent weight of FeC2O4 in the change,
FeC2O4 ® Fe3+ + CO2 is
(A) M/3
(B) M/6
(C) M/2
(D)
M
4
(D) M/1
In the following reaction (unbalanced), equivalent weight of As 2S3 is related to molecular
weight M by :
As2S3 + H+ + NO3– ® NO + H2O + AsO43– + SO42–
(A)
M
2
(B)
M
4
(C)
M
28
(D)
M
24
9.
Equivalent weight of Mn3+ in the following reaction is (Mn = 55)
Mn3+ ® Mn2+ + MnO2
(A) 27.5
(B) 55
(C) 110
(D) 165
10.
The eq. wt. of KMnO4 in the reaction isMnO4¯ + Mn 2+ + H2O ¾® MnO2 + H+ (unbalanced)
[mass of KMnO4 = 158]
(A) 52.7
(B) 158
(C) 31.6
117
(D) None of these
JEE-Chemistry
CONCEPT OF EQUIVALENT WEIGHT (PART-II)
1.
The equivalent mass of calcium phosphate Ca3(PO4)2 (Mol. wt. = 310) is (A) 310/2
(B) 310/6
(C) 310/3
(D) 310
2.
The equivalent mass of crystalline oxalic acid (H2C2O4.2H2O) is equal to the equivalent weight
of (A) Na2CO3
(B) HNO3
(C) KOH
(D) CH 3COOH
3.
Molecular mass of tribasic acid is W. Its equivalent mass would be (A) W/2
(B) W/3
(C) W
(D) 3W
4.
Equivalent wt. of H3PO4 in each of the reaction will be respectivelyH3PO4 + OH– ® H2PO4– + H2O
H3PO4 + 2OH– ® HPO 42– + 2H2O
H3PO4 + 3OH– ® PO43– + 3H2O
(A) 98, 49, 32.67
(B) 49, 98, 32.67
(C) 98, 32.67, 49
(D) 32.67, 49, 98
5.
Equivalent mass of NH3 is (NH3 + H+ ¾¾® NH4+)
(A) 17
(B) 17/2
(C) 1.7
(D) 17/3
6.
The equivalent weight of iron in ferric chloride is (At. wt. of Fe = 55.8) –
(A) 25.8
(B) 18.6
(C) 71.8
(D) 23.6
7.
Equivalent mass of a bivalent metal is 32.7. Molecular mass of its chloride is (A) 68.2
(B) 103.7
(C) 136.4
(D) 166.3
8.
Milli equivalents of a solute in a solution can be given by (A) Milli equivalents = M × Vin ml
(B) Milli equivalents = N × Vin ml
(C) Milli equivalents =
9.
× 1000
(D) (B) and (C) both
Equivalent weight of H3BO3 (M = molar mass of H3BO3) would be (A)
10.
wt.
E.wt.
M
2
(B)
M
3
(C) M
(D)
2M
3
The equivalent mass of phosphoric acid (H3PO4) is 49. It behaves as ... acid.
(A) monobasic
(B) dibasic
(C) tribasic
(D) tetrabasic
118
Redox Reaction
CONCEPT OF EQUIVALENCE & NORMALITY
1.
How many gram of KMnO4 are contained in 4 litres of 0.05 N solution? The KMnO4 is to be
used as an oxidant in acid medium.
(Mol. wt. of KMnO4 = 158)
(A) 1.58 g
(B) 15.8 g
(C) 6.32 g
(D) 31.6 g
2.
Amount of oxalic acid required to prepare 250 mL of N/10 solution (Mol. mass of oxalic acid = 126)
is:
(A) 1.5759 g
(B) 3.15 g
(C) 15.75 g
(D) 63.0 g
3.
What mass of Na2S2O3.5H2O is needed to make 500 cm3 of 0.200 N solution for the
reactions
2S2O32– + I2 ® S4O62– + 2I–
(A) 4.8 g
(B) 14.8 g
(C) 24.8 g
(D) 16.8 g
4.
The mass of sodium bromate (molar mass 151 g mol-1) required to prepare 50 ml of 0.6N solution
based on the reaction
BrO3- + 6H+ + 6e - ® Br - + 3H2O
(A) 0.642 g
5.
is
(B) 0.755 g
(C) 0.814 g
(D) 1.51 g
0.115 gm of sodium metal was dissolved in 500 ml of the solution in distilled water. The
normality of the solution would be (A) 0.010 N
(B) 0.0115 N
(C) 0.023 N
(D) 0.046 N
119
JEE-Chemistry
REDOX TITRATION
1.
The mililitres of 0.2M KMnO4 required for the complete oxidation of 0.1 mol Fe2+ in acidic
medium is(A) 200 ml
(B) 100 ml
(C) 400 ml
(D) 50 ml
2.
In the following redox reaction
Cu(OH)2(s) + N2H4(aq) —® Cu(s) + N2(g)
number of mol of Cu(OH)2 reduced by one mol of N2H4 is (A) 1
(B) 2
(C) 3
(D) 4
3.
How many litres of a 0.5 N solution of an oxidising agent are reduced by 2 litres of a 2.0 N
solution of a reducing agent ?
(A) 8
(B) 4
(C) 6
(D) 7 litres
4.
How many grams of I2 are present in a solution which requires 40 ml of 0.11 N Na2S2O3 to
react with it ? (I = 127)
S2O32– + I2 ¾® S4O62– + 2I¯
(A) 12.7 g
(B) 0.558 g
(C) 25.4 g
(D) 11.4 g
5.
What mass of MnO 2 is reduced by 35 ml of 0.16 N oxalic acid in acid solution ?
(Mn = 55)
MnO2 + H+ + H2C2O4 ®CO2 + H2O + Mn2+
(A) 8.7 g
(B) 0.24 g
(C) 0.84 g
(D) 43.5 g
6.
Volume of 0.1 M K2Cr2O7 (acidic) required to oxidise 35 ml of 0.5 M FeSO 4 solution is (A) 29 ml
(B) 87 ml
(C) 175 ml
(D) 145 ml
7.
A 20.0 mL solution of Na2SO3 required 30 mL of 0.01 M K2Cr2O7 solution for the oxidation to
Na2SO4 . Hence, molarity of Na2SO3 solution is (A) 0.015 M
(B) 0.045 M
(C) 0.030 M
(D) 0.0225 M
8.
The number of moles of Cr2O72– need to oxidize 0.034 mole of N2H5+ by the reaction,
N2H5+ + Cr2O72– —® N2 + Cr3+ + H2O is (A) 0.136
(B) 0.272
(C) 0.816
(D) 0.0227
9.
How many milli litre of 0.5 N SnCl2 solution will reduce 600 ml of 0.1 N HgCl2 to Hg2Cl2 (A) 120 ml
(B) 60 ml
(C) 30 ml
(D) 240 ml
10.
KMnO4 reacts with oxalic acid according to the reaction :
2KMnO4 + 5C 2 O 24- + 16H+ ® 2Mn2+ + 10CO2 + 8H2O
Then, 20 mL of 0.1 M KMnO4 is equivalent to:
(A) 30 mL of 0.5 M C2H2O4 (oxalic acid)
(B) 50 mL of 0.1 M C2H2O4 (oxalic acid)
(C) 20 mL of 0.5 M C2H2O4 (oxalic acid)
(D) 10 mL of 0.1 M C2H2O4 (oxalic acid)
120
Redox Reaction
11.
The number of moles of Cr2O72– required to oxidize one mole of FeC2O4 in acidic medium (A) 0.5
(B) 0.6
(C) 0.2
(D) 0.3
12.
The number of moles of MnO4– ions needed to react with one mole of sulphite ions in acidic medium
are (A) 0.8
(B) 0.4
(C) 0.6
(D) 0.5
13.
When the ion Cr2O72– acts as an oxidant in acidic aqueous solution the ion Cr3+ is formed. How
many moles of Sn2+ would be oxidised to Sn4+ by one mole of Cr2O72– ions (A) 2/3
(B) 3/2
(C) 2
(D) 3
14.
The mass of H2O2 that is completely oxidised by 31.6 g of KMnO4 (Molar mass = 158 g mol-1) in acidic
medium is (A) 12 g
(B) 15 g
(C) 17 g
(D) 1 g
121
JEE-Chemistry
ANSWER KEY
CALCULATION OF OXIDATION NUMBER
1.
(D)
2.
(B)
3.
(D)
4.
(A)
5.
(C)
6.
(A)
7.
(A)
8.
(B)
9.
(C)
10.
(B)
11.
(D)
12.
(C)
13.
(A)
14.
(A)
15.
(C)
16.
(B)
17.
(B)
18.
(B)
19.
(D)
20.
(A)
21.
(B)
22.
(A)
23.
(A)
24.
(A)
CONCEPT OF OXIDATION & REDUCTION REACTIONS
1.
(D)
2.
(B)
3.
(B)
4.
(C)
5.
(A)
6.
(A)
7.
(A)
8.
(C)
9.
(C)
10.
(C)
11.
(D)
12.
(A)
13.
(B)
14.
(D)
15.
(D)
16.
(C)
17.
(D)
18.
(B)
19.
(C)
TYPE OF REDOX REACTION
1.
(C)
2.
(B)
3.
(A)
4.
(C)
5.
(B)
6.
(C)
7.
(A)
8.
(A)
9.
(C)
10.
(C)
11.
(B)
12.
(D)
13.
(D)
14.
(A)
15.
(D)
6.
(C)
6.
(B)
6.
(B)
(A)
BALANCING OF REDOX REACTION
1.
(A)
2.
(A)
3.
(B)
4.
(C)
7.
(A)
8.
(B)
9.
(A)
10.
(D)
5.
(A)
CONCEPT OF EQUIVALENT WEIGHT (PART-I)
1.
(B)
2.
(D)
3.
(D)
4.
(D)
7.
(A)
8.
(C)
9.
(C)
10.
(A)
5.
(D)
CONCEPT OF EQUIVALENT WEIGHT (PART-II)
1.
(B)
2.
(B)
3.
(B)
4.
(A)
7.
(C)
8.
(D)
9.
(C)
10.
(B)
5.
(A)
CONCEPT OF EQUIVALENCE & NORMALITY
1.
(C)
2.
(A)
3.
(C)
4.
(B)
5.
(A)
REDOX TITRATION
1.
(B)
2.
(B)
3.
(A)
4.
(B)
5.
(B)
6.
7.
(B)
8.
(D)
9.
(A)
10.
(B)
11.
(A)
12.
13.
(D)
14.
(C)
122
(B)
Important Notes
123
Redox Reaction
JEE-Chemistry
Important Notes
124
Classification & Nomenclature of Organic Compounds
IUPAC NOMENCLATURE
1.
STRUCTURE OF ORGANIC COMPOUNDS AND HYBRIDISATION
SINGLE CORRECT ANSWER TYPE
Which of the following is condensed structural formula?
H H H
| | |
H
C
- C - C - H (C) CH – CH – CH
(B)
3
2
3
| | |
H H H
(a)
2.
3.
(D)
Number of s-bonds and p-bonds (respectively) are in anthracene:
(A) 7, 26
(B) 24, 8
(C) 26, 7
(D) 26, 6
Arrange the following molecules in increasing order of s to p bond ratio
(I)
(II)
(IV)
(III)
N
N
O
H
4.
(A) I < II < III < IV
(B) I < II < IV < III
(C) II < I < IV< III
(D) IV < II < I < III
What is the hybridization of the carbon atoms numbered 1 and 2 respectively in the following
structure?
– CH = CH – C º CH
1
5.
2
(A) sp3, sp2
(B) sp2, sp2
(C) sp, sp
Which carbon(s) in the following molecule is (are) sp hybridized?
(D) sp2, sp
O
CH3 – C – CH2 – C º C – H
1
6.
2
3
4
5
(A) carbon 1
(B) carbon 2
(C) carbon 1, 3
(D) Carbon 4, 5
What is the hybridization of C1, C2, C3 carbon in the following compound?
CH3 – CH2 – CH = CH – C º C – H
1
7.
2
3
(A) sp , sp , sp
(B) sp , sp , sp
(C) sp3, sp2, sp
What is the hybridization of carbon in the following compounds?
3
3
3
3
2
2
(D) sp, sp2, sp2
CH3 – F, CH3 – Cl
8.
(A) sp2, sp2
(B) sp, sp
(C) sp3, sp3
(D) sp3, sp2
The carbon-carbon triple bond of an alkyne is composed of ...........
(A) three s bonds
(B) two s bonds and one p bond
(C) one s bond and two p bonds
(D) three p bonds
9.
How many – CH3 groups are present in given alkane?
(A) 4
(B) 8
(C) 6
125
(D) 7
JEE-Chemistry
CLASSIFICATION OF CARBON AND HYDROGEN
SINGLE CORRECT ANSWER TYPE
1.
How many 1º carbon atom will be present in a simplest open chain hydrocarbon having two 3º and
one 2º carbon atom?
(A) 3
(B) 4
(C) 5
(D) 6
2.
How many 2° carbons are present in above compound?
(A) 4
(B) 5
(C) 6
(D) 7
How many 2° carbons are in the following compound ?
(A) 21
(B) 19
(C) 17
(D) 31
3.
C=C=C
CH3
4.
The structure shown CHCHC
3
2 HCHCHCHCHCH
2
2
3 has
CHCH
2
3
5.
6.
7.
(A) 1° 2° and 3° carbon atoms
(B) 1° and 2° carbon atoms only
(C) 1° and 3° carbon atoms only
(D) 2° and 3° carbon atoms only
How many 1°carbon atom will be present in a simplest hydrocarbon having one 4° carbon atom?
(A) 3
(B) 4
(C) 5
(D) 6
How many secondary carbon atoms does methyl cyclopropane has?
(A) None
(B) One
(C) Two
(D) Three
Number of secondary carbon atoms present in the above compounds are respectively:
,
8.
CHCH
2
3
and
(A) 6,4,5
(B) 4,5,6
(C) 5,4,6
(D) 6,2,1
A compound containing an equal number of primary, secondary and tertiary carbon atoms is:
o
(A) Mesityl Oxide
(B) Mesitylene
COOH
(C) Maleic acid
COOH
(D) Malonic acid
126
COOH
COOH
Classification & Nomenclature of Organic Compounds
CLASSIFICATION OF ORGANIC COMPOUNDS
SINGLE CORRECT ANSWER TYPE
1.
2.
3.
Which of the following pairs have presence of carbocyclic ring in both compounds?
(A) Pyridine, Benzene
(B) Benzene, Cyclohexane
(C) Cyclohexane, Furan
(D) Furan, Pyridine
The group of heterocylic compounds is:
(A) Phenol, Furan
(B) Furan, Thiophene
(C) Thiophene, Phenol
(D) Furan, Aniline
Which of the following is a heterocyclic compound
(A)
4.
HC = CH
|
HC = CH
S
(B)
HC = COOH
|
HC = COOH
(C)
HC = CH
|
HC = CH
(D)
HC = CH
|
HC = CH
Which of the following compounds is not having molecular formula C6H14O?
OH
(A)
5.
6.
OH
(B)
(C)
OH
(D)
OH
How many different functional groups are present in given compound?
(A) 3
(B) 4
(C) 1
(D) 0
OH
HOC
2
O
How many functional groups are present in above compound?
O
O
||
CH 3 - O - C - CH - C - CH 2 - C - OH
|| |
||
O OH O
(A) 2
7.
(B) 3
(C) 4
(D) 5
Which of the following compound has maximum number of p-bonds?
(A)
(B) NºC–CºC–CºCH (C)
127
(D)
JEE-Chemistry
HOMOLOGOUS SERIES
SINGLE CORRECT ANSWER TYPE
1.
In homologous series, successive members have difference of
(A) CH3 –
2.
(B) CH3 – CH2 –
(B) 13
(C) 14
5.
(A) CH3OH, CH3 – O – CH3
(B) CH3OH, CH3SH
(C) CH3–O–CH3, CH3–CH2–OH
(D) CH3OH, CH3CH2OH
Which of the following is smallest homologue of ketone ?
O
(B)
O
(C) H2C = O
(D)
(B) 3
(C) 2
(D) 4
Which of the following is homologue of CH3 NH CH2 CH2 CH3.
(A) CH 3CH2NHCH2CH3
(B) CH3CH2CH2NH2
(C) CH3—CH—NH2
(D) CH3CH2NHCH3
CH3
8.
9.
O
Number of carbon in the first member of ester homologous series are ?
(A) 1
7.
(B) CH3 – CH2 – CH2 – OH
(D) CH3 – CH2 – O – CH2 – CH3
Which of the following pairs is homologue?
(A)
6.
(D) 15
What is the homologue of CH3 – CH2 – OH?
(A) CH3 – CH2 – O – CH3
(C) CH3OCH3
4.
(D) –H
In homologous series, consecutive members have difference of mol. wt. of
(A) 12
3.
(C) –CH2–
O
||
CH3 - CH - C - H
|
CH 3
Identify the homologous series to which compound shown belongs.
(A) Aldehyde
(B) Ketone
(C) Ester
(D) Carboxylic acid
How many maximum number of compounds, among the following belongs to same homologous
series
CH3CHO, CH3CH2OH, CH3–O–CH3 , CH3 –O–CH2–CH3, CH3 – CH2– CH2OH
CH3COOH, CH3COCH3 , CH3CH2COCH3, HCHO, CH3CH2CHO
(A) 0
(B) 1
(C) 2
128
(D) 3
Classification & Nomenclature of Organic Compounds
FUNCTIONAL GROUP IDENTIFICATION
Q.
Circle the functional groups and given the name in the following structures ?
O
NH2
OH
(2)
(1)
(3)
OH
N
OH
O
O
(5)
O
OH
O
O
(4)
O
(6)
Cl
O
H
O
OH
CN
O
NH2
O
(7)
O
(8)
O
(9)
NH2
O
CO2H
O
(10) HCOOCH3
O
(11)
CN
NC
OCH3
(12)
OCOCH3
NC
(13)
O
(14)
(15)
SH
O
O
(16) O
SO3H
(17)
(18)
OH
Cl
O
O
(19)
(20)
COOH
OH
(21)
O
(22)
(23)
(24)
O
(25)
O
O
CHO
N–H
129
O
SH
JEE-Chemistry
O
CH2–C–NH
CH2OCH3
(26)
(27) CH3–CH–COOCH3
(28)
O
CN
Penicillin
I
HO
NH2
(29) HO
S
NH2
CH2CH2
I
O
HO
(30)
I
CH2–CH–COOH
I
Thyroxine
Dopamine
130
NH2
N
COOH
Classification & Nomenclature of Organic Compounds
IUPAC NOMENCLATURE OF ALKANES
SINGLE CORRECT ANSWER TYPE
1.
2.
The compound which has one isopropyl group is:
(A) 2,2,3,3-Tetramethyl pentane
(B) 2,2-Dimethyl pentane
(C) 2,2,3-Trimethyl pentane
(D) 2-Methyl pentane
Give the complete IUPAC name for the Structure below.
CH 3 - CH - CH 2 - CH - CH 3
|
|
CH 3 - CH 2
CH - CH 3
|
CH 2 - CH 3
3.
(A) 3,5,6-Trimethyl octane
(B) 3,4,6-Trimethyl octane
(C) 1, 2, 3, 6-Tetramethyl heptane
(D) None of these
Give the IUPAC name for the following Structure:
(A) 2-Methyl-3-ethylheptane
(C) 5-Isopropyloctane
4.
(B) 3-Ethyl-2-methylheptane
(D) 5-Isopropylnonane
; Correct IUPAC name of the given compound is:
(A) 4-(l,1-Dimethylethyl)-5-ethyloctane
(C) 5-(1,1-Dimethylethyl)-4-ethyloctane
(B) 5-Ethyl-4-(1,1-dimethylethyl) octane
(D) 4-Ethyl-5-(1,1-dimethylethyl) octane
CH 3—CH—CH3
5.
IUPAC name of compound CH3—CH2—CH2—CH—CH—CH2—CH2—CH3 is
CH3—CH—CH3
(A) 4, 5-Diisopropyl octane
(C) 4- Iso Propyl 5-1-methyl propyl octane
(B) 4, 5- Bis iso butyl octane
(D) 5- Iso propyl-4-1-methyl propyl octane
CH2—CH3
6.
IUPAC name of compound CH3—CH2—CH —CH —CH—CH—CH —CH —CH —CH is
2
2
2
2
2
3
CH3—C—CH3
CH3
(A) 5-(1, 1-Dimethyl ethyl)-6-ethyl decane
(C) 6-Ethyl-5-(1,1-dimethyl ethyl) decane
(B) 5-Ethyl-6-(1, 1-Dimethyl ethyl) decane
(D) 6-(1, 1-Dimethyl ethyl)-5 ethyl decane
131
JEE-Chemistry
CH3 C4H9
7.
IUPAC name of CH3–CH2–CH–C–CH2–CH3 is :
CH3
(A) 3,4,4-Trimethylheptane
(B) 4-Ethyl-3,4-dimethyl octane
(C) 2-Butyl-2-methyl-3-ethylbutane
(D) None of these.
CH3
8.
IUPAC name of the given compound CH3 – (CH)
is:
2 4 – CH – C – CH2 – CH2 – CH3
CH3 CH2 – CH3
9.
10.
(A) 4-Ethyl-4,5-dimethyldecane
(B) 3,4-Dimethyl-3-n-propylnonane
(C) 6,7-Dimethyl-7-n-propylnonane
(D) 6,7-Dimethyl-7-ethyldecane
Name of given compound
is
(A) 4-Ethyl-3-methyloctane
(B) 3-Methyl-4-ethyloctane
(C) 2,3-Diethylheptane
(D) 5-Ethyl-6-methyloctane
IUPAC name of the compound
CH3 – CH2 – CH– CH2 – CH – CHCHCH
2
2
3 is
CH3
CH – CH3
CH3
11.
12.
(A) 4-Isopropyl-6-methyloctane
(B) 3-Methyl-5-(1-methylethyl)octane
(C) 3-Methoxy-4-butanol
(D) 1,2-Methoxybutanol
A student named a certain compound as 2, 3-diethyl butane. Its correct IUPAC name is
(A) 2, 3-Dimethyl hexane
(B) 3,4-Dimethylhexane
(C) 2-Ethyl-3-methyl pentane
(D) 2-Ethyl-butane
How many carbon atoms are present in parent carbon chain in the given compound?
(A) 6
(B) 7
(C) 8
132
(D) 9
Classification & Nomenclature of Organic Compounds
13.
Which of the following option is correct regarding names of various groups ?
CH3
(a) – CH – CH2
(i) iso-Butyl
CH3
CH3
(b) – CH2 – CH
(ii) tert-Pentyl
CH3
CH3
(c) – C – CH3
(iii) iso -Pentyl
CH2CH3
(d)
– HC
– CH2
2
CH3 – CH– CH3
(iv) sec-Butyl
(A) a - ii, b - iv, c - ii, d -iii
(B) a - iv, b - i, c - iii, d - ii
(C) a - iv, b - i, c - ii, d - iii
(D) a - iv, b - ii, c - i, d - iii
133
JEE-Chemistry
IUPAC NOMENCLATURE OF ALKENES & ALKYNES
1.
2.
SINGLE CORRECT ANSWER TYPE
Which pair of names refers to the same compound?
(A) Ethyne and Acetylene
(B) Ethyne and Ethene
(C) Ethane and Acetylene
(D) Ethane and Ethene
What is the IUPAC name for the given compound?
CH 2 = C - CH3
|
CH 2
|
CH3
(A) 2-Methyl-1- butene
(C) 2-Methylbut-1-ene
3.
(B) Isopentene
(D) Ethylpropene
What is the IUPAC name for the following alkyne ?
Br
|
CH 3 - C º C - CH 2 - C - CH 3
|
CH 3
(A) 5-Bromo-2-heptyne
(C) 2-Bromo-2-methyl-4-hexyne
(B) 3-Bromo-5-heptyne
(D) 5-Bromo-5-methylhex-2-yne
4.
The molecular formula of the first member of the family of alkenynes and its name is given by the set
(A) C3H2, Alkene
(B) C5H6, Pent-1-en-3-yne
(C) C6H8, Hex-1-en-5-yne
(D) C4H4, But-1-en-3-yne
5.
IUPAC name of the following compound is
(A) Isoprene
(C) 2-methylbuta-1,3-diene
6.
The IUPAC name of
(A) 2-Bromo-3-methylbutg-3-ene
(C) 2-Bromo-3-methylpent-3-ene
(B) 3-methyl,3-butadiene
(D) 2-methyl-2,3-butadiene
Br
is
(B) 4-Bromo-3-methylpent-2-ene
(D) 4-Bromo-2,3-dimethylbut-2-ene
134
Classification & Nomenclature of Organic Compounds
7.
The IUPAC name of
CH3 – C = C — CH – CH 2 – C º CH is
|
|
|
Cl CH3 C 2H5
(A) 2-Chloro-4-ethyl-3-methyl-6-heptyn-2 ene (B) 2-Chloro-4-ethyl-3-methyl-2-hepten-6-yne
(C) 6-Chloro-4-ethyl-5-methyl-1-heptyn-5-ene (D) 6-Chloro-4-ethyl-5-methylhept-5-en-1-yne
8.
The IUPAC name of the given compound
CH2 = CH – CH – CH3
CH3
9.
(A) 1,1-Dimethylprop-2-ene
(B) 3-Methylbut-1-ene
(C) 2-Vinylpropane
(D) 1-Isopropylethylene
IUPAC name of the given compound is
CH3 – C º C – CH – C = CH2
CH3 CH2– CH3
10.
(A) 3-Methylene-4-methyl-5-heptene
(B) 2-Ethyl-3-methylhex-1-en-4-yne
(C) 5-Methylene-5-ethyl-4-methyl-2-heptyne
(D) 5-Ethyl-4-methyl-2-hexyn-5-ene
IUPAC name of given compound CH3 – CH2 – CH2 – CH– CH2 – CH2 – CH3 is
CH= CH2
11.
(A) 4-Ethenylheptane
(B) 3-Propylhex-1-ene
(C) 4-Ethenylhexane
(D) 3-Ethenylheptane
The IUPAC name of the given compound
is
(A) 4,5-Dimethyloct-4-ene
(B) 4,5-Dimethyl-5-octene
(C) 3,4-Dimethyl-5-octene
(D) 2,3-Dipropyl-2-butene
CH3
12.
The IUPAC name of CH3 – C – CH= CH2 is
CH3
13.
(A) 2,2-Dimethyl-3-butene
(B) 2,2-Dimethyl-pent-4-tene
(C) 3,3-Dimethylbut-1-ene
(D) 1-Hexene
The IUPAC name of the given compound is CH3 – CH = CH – C º CH
(A) Pent-3-en-1-yne
14.
(B) 2-Penten-4-yne
(C) 3-Pentyn-1-ene
(D) 2-Pentyn-1-ene
The IUPAC name of the compound is
(A) 2,4,5,6-Tetramethyl-7-ethyldeca-1,7-diene (B) 7-Ethyl-2,4,5,6-tetramethyldeca-1,8-diene
(C) 4-Ethyl-5,6,7,9-tetramethyldeca-2,9-diene (D) none of the above
135
JEE-Chemistry
NOMENCLATURE OF CARBOXYLIC ACID
WRITE IUPAC NAME OF FOLLOWING
1.
O
H3C
H2C
2.
H3C
3.
CH3
OH
O
HO
CH3
CH2
O
HO
OH
CH3
4.
CH3
5.
Br
CH3
O
HO
NOMENCLATURE OF ACID ANHYDRIDE
WRITE IUPAC NAME OF FOLLOWING
CH3
O
1.
Cl
CH3
O
O
O
2.
O
O
O
CH3
3.
CH3
O
O
Br
CH3
CH2
CH2
4.
O
O
O
O
CH3
O
O
5.
HC
NOMENCLATURE OF ESTER
WRITE IUPAC NAME OF FOLLOWING
CH3
H 3C
1.
H3C
O
O CH3
2.
O
CH3
CH3
4.
CH2 O
O
5.
O
O
H 3C
CH3
136
O
H3C
3.
Br
CH3
O
CH 3
O
Classification & Nomenclature of Organic Compounds
NOMENCLATURE OF HALO CARBONYL
WRITE IUPAC NAME OF FOLLOWING
1.
H3 C
CH3
H 3C
2.
O
CH3
CH3
Cl
H3 C
5.
Cl
3.
O
Cl
CH3
HC
3
4.
Cl
O
Cl
H3C
H3C
CH3
Cl
Cl
O
CH3
O
NOMENCLATURE OF AMIDE
WRITE IUPAC NAME OF FOLLOWING
O
1.
CH3
2.
H 2N
O
H 2N
CH3
HN
CH3
H 2N
CH2
H3C
4.
3.
H 2N
O
O
CH3
O
CH3
5.
CH
NOMENCLATURE OF CYANIDE
WRITE IUPAC NAME OF FOLLOWING
1.
2.
N
3.
N
H 3C
CH3
N
N
H3 C
CH3
4.
H3 C
CH3
5.
N
CH
137
JEE-Chemistry
NOMENCLATURE OF ALDEHYDE
WRITE IUPAC NAME OF FOLLOWING
1.
H3C
2.
CH3
O
4.
5.
H3C
CH3
H3C
O
O
3.
O
CH2
H3C
H 3C
O
O
NOMENCLATURE OF KETONE
WRITE IUPAC NAME OF FOLLOWING
H3C
O
H3C
1.
2.
4.
H2C
CH3
O
CH3
O
5.
H2C
3.
H3C
CH3
H2C
O
O
HC
CH3
CH3
NOMENCLATURE OF ALCOHOL
WRITE IUPAC NAME OF FOLLOWING
HO
H3C
H3C
CH3
1.
2.
H3C
CH2
OH
5.
H3C
CH3
OH
4.
HO
H 2C
CH3
OH
138
CH3
3.
Classification & Nomenclature of Organic Compounds
NOMENCLATURE OF AMINE
WRITE IUPAC NAME OF FOLLOWING
1.
CH3
H 3C
H 3C
2.
NH2
NH2
H3C
3.
CH3
H2N
CH
CH2
H3 C
CH3
4.
NH2
5.
(CH3CH2)2NCH3
NOMENCLATURE OF HALOALKANES, HALOALKENES &
HALOALKYNES
WRITE IUPAC NAME OF FOLLOWING
1.
H
H
Br
H
5.
7.
H
H
H
Br
H
9.
CH3
H
Br
H
H
Cl
CH3
H
Br
H3C
H
H 3C
H
10.
6.
H3 C
CH3
H
Br 8.
H
CCl4
H3C
CH3
H
Br
H
H3 C
H 3C
3.
ClCH2–CHCl2
H
H3 C
4.
2.
CH3–CCl3
H
Br
HO
Cl
CH
NOMENCLATURE OF ETHER
1.
4.
C6H5OCH 3
CH3O – CH – CH3
WRITE IUPAC NAME OF FOLLOWING
2.
C6H5OCH 2CH 3
3.
C6H5O(CH2)6 – CH3
5.
C6H 5 – O – CH2 – CH2 – CH – CH3
CH3
CH3
139
JEE-Chemistry
IUPAC NOMENCLATURE OF COMPOUNDS CONTAINING ONLY
SINGLE FUNCTIONAL GROUP
SINGLE CORRECT ANSWER TYPE
1.
Cl
The IUPAC name of
is
O
(A) 2-Ethyl-3-methyl butanoyl chloride
(C) 3,4-Dimethyl pentanoyl chloride
(B) 2,3-Dimethylpentanoyl chloride
(D) 1-Chloro-1-oxo-2,3-dimethyl pentane
O
2.
The IUPAC name of
– C – NH – CH
6 5
is
(A) N-Cyclohexyl benzamide
(C) N-phenyl-N-cyclohexyl methanamide
3.
(B) N-Cyclohexyl-N-phenyl methyl amide
(D) N-Phenylcyclohexane carboxamide
The IUPAC name of the given compound is
CH3
|
CH 3 - C - CH 2 - CHO
|
CH 3
(A) 1,1-Dimethylbutanal
(C) 1,1,1-Trimethylpropanal
4.
(B) 3,3-Dimethylbutanal
(D) 3,3,3-Trimethylpropanal
IUPAC name of the given compound is
CH 3 - CH 2 - CH - CONH 2
|
CH 3
(A) 2-Ethylbutanamide
(C) 2-Methylbutanamide
5.
(B) 1-Amino-3-methylpropane
(D) 3-Methylbutanamide
IUPAC name of the given compound is
NC – CH– CH2 – CH3
CN
(A) 2-Ethylpropane-1,3-dinitrile
(B) 1,2-Dicyanopropane
(C) 1,2-Dicyanobutane
(D) 2-Cyanobutane-1-nitrile
140
Classification & Nomenclature of Organic Compounds
6.
Which of the following compound has INCORRECT IUPAC name?
(A) CH3 – CH2 – CH2 – COOCHCH
2
3
(B) CH3 – CH – CH2 – CHO
Ethyl butanoate
CH3
3-Methylbutanal
(C) CH3 – CH– CH2 – CH3
7.
(i)
(D) CH3 – CH – C– CH2 – CH3
OH CH3
CH3 O
2-Methylbutan-3-ol
2-Methylpentan-3-one
OH
and (ii)
CHCHOH
2
2
True statement for the above compounds is :
(A) (i) is phenol while (ii) is alcohol
(B) Both (i) and (ii) are primary alcohol
(C) (i) is primary and (ii) is secondary alcohol (D) (i) is secondary and (ii) is primary alcohol
8.
The IUPAC name of
CH – OH is :
CH3
(A) 1-Hydroxy-1-cyclopropylethane
(B) 1-Hydroxyethylcyclopropane
(C) 2-Cyclopropylethanol
(D) 1-Cyclopropylethanol
141
JEE-Chemistry
IUPAC NOMENCLATURE OF COMPOUNDS CONTAINING MORE
THAN ONE FUNCTIONAL GROUP
SINGLE CORRECT ANSWER TYPE
1.
The IUPAC name of the compound is
COOH
CH3 – CH2 – CH2 – C – CH2 – CH3
COOH
2.
(A) 2-Propyl-2-ethylpropane-1,3-dioic acid
(B) 2-Ethyl-2-propylpropane-1,3-dioic acid
(C) 2-Ethyl-2-carboxypentanoic acid
(D) 2-Carboxy-2-ethylpentanoic acid
The IUPAC name of the given compound is
CH2 – CH3
CH3 – CH– CH2 – C – OH
OH
3.
CH2 – CH3
(A) 2,4-Hexanediol
(B) 4-Ethylhexane 2,4-diol
(C) 2,4-Hexanediol-2-ethyl
(D) 3,3-Diethyl-1,3-butanediol
The IUPAC name of the given compound is
CH2 – CH – CH2
CN
CN
CN
(A) 1,2,3-Tricyanopropane
(B) 3-Cyanopentanedinitrile
(C) Propane -1,2,3-tricarbonitrile
(D) Propane tricarbonitrile
O O
4.
The correct IUPAC name of H – C – C – His
(A) Formylmethanal
(B) 1,2-Ethanedione
(C) 2-Oxethanal
(D) Ethane-1,2-dial
CHO
2 H
5.
6.
IUPAC name of given compound is
(A) 3,7-Dimethylocta-2,6-dien-1-ol
(B) 2,6-Dimethylocta-2,6-diene-8-ol
(C) 1-Hydroxy-3,7-dimethylocta-2,6-diene
(D) None of the above
The correct IUPAC name of the given compound is
O
(A) Pent-4-en-2-one
(B) 3-Buten-1-al
(C) 3-Methylhex-4-en-1-yne
(D) 4-Methyl-2-hexen-5-yne
142
Classification & Nomenclature of Organic Compounds
7.
The principal functional group of following compound is
O
OH
CICH 2CH CH–
2 C– CHNO
2
2
(A) nitro
8.
(B) Alcohol
(C) Alkyl halide
The IUPAC name of CH3CH(OH)CH2CH2COOH is
(A) 4-Hydroxypentanoic acid
(B) 1-Carboxybutan-3-ol
(C) 1-Carboxybutan-4-ol
9.
(D) ketone
(D) 4-Carboxybutan-2-ol
The IUPAC name of compound is
CH3 O
CH3–C – C–CH 2–CH2OH
H
10.
(A) 1-Hydroxy-4-methylpentan-3-one
(B) 2-Methyl-5-hydroxypentan-3-one
(C) 4-Methyl-3-oxopentan-l-ol
(D) Hexan-1-ol-3-one
The IUPAC name of the given compound
CH3
O
Br
C
CH
CH
COOH is :
I
11.
(A) 4-Keto-3-bromo-2-iodopentanoic acid
(B) 2-Iodo-3-bromo-4-keto-pentanoic acid
(C) 3-Bromo-2-iodo-4-ketopentanoic acid
(D) 4-Carboxy-3-bromo-4-iodopentanoic acid
The correct systematic IUPAC name of the given compound is
OH
CH2 – C – CH2 – C – NH2
HN
2 CO
12.
CONH2
O
(A) 3-Carbamoyl-3-hydroxybutanediamide
(B) 2-Hydroxypropane-1,2,3-tricarbamoyl
(C) 2-Hydroxypropane-1,2,3-tricarboxamide
(D) 2-Bis(carbamoyl)-2-hydroxyethanamide
The correct IUPAC name of the given compound is
NH2
O
CH2 —C —CH2 —C —OH
COOHCOOH
(A) 3-Carboxy-3-hydroxy butane dioic acid
(B) 2-Aminopropane-1,2,3-tricarboxylic acid
(C) 3-Amino butanedioic acid
(D) 2-Bis(carboxymethyl)-2-hydroxy ethanoic acid
143
JEE-Chemistry
13.
The correct IUPAC name of picric acid is :
(A) 1,3,5-Trinitrophenol
(B) 1,2,5-Trinitrophenol
(C) 2,4,6-Trinitrophenol
(D) 2,3,5-Trinitrophenol
O
14.
CH3 – CH – CH2 – C – O – CH2 – CH – CH3
Cl
Br
Select the correct IUPAC name among the following:
15.
(A) 3-Chlorobutyl-2-bromopropanoate
(B) 2-Chlorobutyl-3-bromopropanoate
(C) 2-Bromopropyl-3-chlorobutanoate
(D) 2-Bromopropyl-1- chlorobutyrate
The IUPAC name of the compound is
OH
O
O
16.
(A) 5-Ethyl-1-hydroxyoctan-1,4-dioic acid
(B) 2-Carboxyethyl-3-hexyl ketone
(C) 3-(3-Hexylcarbonyl) propanoic acid
(D) 5-Ethyl-4-ketooctanoic acid
What is the common name for the following compound ?
O
CH3CHCH2COH
Cl
17.
(A) l - chlorobutanoic acid
(B) b - chlorobutanoic acid
(C) b - chlorobutyric acid
(D) l - chlorobutyric acid
What is the IUPAC name for the following compound ?
O
CH3CCHCH2CHCH 3
CH3
18.
Cl
(A) 5-chloro-3-methylhexanone
(B) l-Chloro-1.3-dimethyl-4-pentanone
(C) 5-chloro-3,5-dimethyl-2-pentanone
(D) 5-chloro-3-methylhexan-2-one
The correct IUPAC name of compound is: CH 3 - CH 2 C - CH - CHO
||
|
O CN
?
(A) 2-Cyano-3-oxopentanal
(B) 2-Formyl-3-oxopentanenitrile
(C) 2 Cyano-1,3 pentancdione
(D) 1,3 Dioxo-2- cyanopentane
144
Classification & Nomenclature of Organic Compounds
CO2H
19.
The IUPAC name of compound CH3–C
Cl
C–CH–CH3 ?
NH2
20.
21.
22.
(A) 2-Amino -3-chloro-2-methylpent-2-enoic acid
(B) 3-Amino-4-Chloro-2-methylpent-2-enoic acid
(C) 4-Amino-3-Chloro-2-methylpent-2-enoic acid
(D) All of the above
Which of the following compound is wrongly named ?
(A) CH 3 CH 2 CH 2 CHCOOH
|
Cl
; 2-Chloropentanoic acid
(B) CH3 C º CCHCOOH
|
CH3
; 2-Methyl hex-3-enoic acid
(C) CH 3 CH 2 CH = CHCOCH 3
; Hex-3-en-2-one
(D) CH 3 - CHCH 2 CH 2 CHO
|
CH 3
; 4-Methyl pentanal
The correct IUPAC name of CH3 - CH 2 - C - COOH is :
||
CH 2
(A) 2-Methyl butanoic acid
(B) 2-Ethylprop-2-enoic acid
(C) 2-Carboxy-l-butene
(D) None of these
The suffix of the principal group, the prefixes for the other groups and the name of the parent in the
structure
HO - CH 2 - CH - CH = C - CH 2 - C - C - OH are respectively
|
|
|| ||
CH 3
Cl
O O
(A) -oic acid, chloro, hydroxy, oxo, ethyl, hept-4-ene
(B) -oic acid, chloro, hydroxy, methyl, oxo, hept-4-ene
(C) -one, carboxy, chloro, methyl, hydroxy, hept-4-ene
(D) -one, carboxy, chloro, methyl, hydroxy, hept-4-ene
23.
OH
|
The IUPAC name of CH3 - CH - COOH
(A) 2-Hydroxypropanoic acid
(C) 1-Hydroxyethane carboxylic acid
(B) 1 -Hydroxypropanoic acid
(D) l-Hydroxyethanoic acid
145
JEE-Chemistry
24.
25.
Cl
|
The IUPAC name of CH3 - C - CH 2 CH = CHCH 3
|
OH
(A) 5-Chloro-2-hydroxyhexene
(B) 2-Chloro-5-hydroxyhexene
(C) 2-Chloro-2-hydroxy-5-hexene
(D) 2-Chlorohex-4-en-2-ol
Which of the following compound has 4 carbon atoms in the parent chain ?
(A) OH
(C)
OH
OH
(B)
(D)
146
O
Br
Classification & Nomenclature of Organic Compounds
IUPAC NOMECLATURE OF ALICYCLIC COMPOUNDS
1.
SINGLE CORRECT ANSWER TYPE
The IUPAC name of the given compound
2.
(A) Octylcyclopentane
(B) 3-Cyclopentyloctane
(C) Cyclopentaneoctane
(D) 6-Cyclopentyloctane
Which of the following name will be incorrect?
(A)
(C)
3,6-Dimethylcyclohexene
6,6-Dimethylcyclohexene
(B)
(D)
1,6-Dimethylcyclohexene
1,5-Dimethylcyclohexene
3.
The IUPAC name of the following compound is
4.
(A) Cyclopropylcyclohexane
(B) 4-Cyclopropyl-1-tert. butyl cyclohexane
(C) 1-Cyclopropyl hexyl-2,2-dimethylpropane (D) 1-Dimethyl ethyl-4-cyclopropyl cyclohexane
Select the correct IUPAC name of the compound:
(A) 3-Ethyl-1,5-dimethylcyclopentane
(C) 4-Ethyl-1,2-dimethylcyclopentane
(B) 1-Ethyl-3, 4-dimethylcyclopentane
(D) 2-Ethyl-4, 5-dimethylcyclopentane
OH
5.
The name of the given compound is
Br
6.
(A) 2-Bromo-4-hydroxycyclohexene
(C) 3-Bromo-cyclohex-4-ene-1-ol
IUPAC name of the given molecule is
(B) 3-Bromocyclohex-3-en-1-ol
(D) None of the above
CH2OH
COOH
(A) 4-Hydroxymethyl 1-carboxy cyclohex-3-ene
(B) 4-Hydroxymethyl cyclohex-3-ene carboxylic acid
(C) 1-Hydroxymethyl cyclohexene-4-carboxylic acid
(D) 4-(Hydroxymethyl cyclohex-3-enyl)methanoic acid
147
JEE-Chemistry
7.
IUPAC name of the given molecule is
COOH
8.
Br
COOH
(A) 2-Bromo cyclo hexa-2,5-di en-1,4-dioic acid
(B) 2-Bromo cyclo hex-2,5-diene-1,4-dicarboxylic acid
(C) 2-Bromocyclo hexa-2,5-diene-1,4- dicarboxylic acid
(D) 3-Bromocyclo hexa-3,6-diene-1,6-dicarboxylic acid
Correct IUPAC name of the given compound is:
Br
Cl
OH
(A) 2-Bromo-3 - ethy1-4-chlorocyclobutanol
(B) 4-Bromo-1-chloro-3-ethylcyclobutanol
(C) 2-Bromo-4-chloro-3-ethyl cyclohydroxybutane
(D) 2-Bromo-4-chloro-3-ethylcyclobutan-1-ol
CH3
9.
IUPAC name of given compound is
OH
CH
CH3
CH3
(A) 5-methyl -2-(1'-Methylethyl)cyclohexanol
(B) 1-(1'-Methylethyl)-4-methyl cyclohexan-2-ol
(C) 2-Propyl-5-methyl cyclohexanol
(D) None of the above
O
10.
Cl
C – NH 2
Which of the following is the correct IUPAC name of the above compound?
(A) p-Acetamido chlorocyclohexane
(B) 4-Chloro cyclohexane carboxamide
(C) Amido chlorocyclohexane
(D) None of the above
148
Classification & Nomenclature of Organic Compounds
IUPAC NOMENCLATURE OF BENZENE RING CONTAINING
COMPOUNDS
SINGLE CORRECT ANSWER TYPE
COOH
Br
1.
IUPAC name of the following compound HO
(A) 2-Bromo-5-hydroxy-3-nitro benzoic acid
(C) 3-Nitro-2-bromo-5-hydroxy benzoic acid
2.
NO2 is :
(B) 6-Bromo-5-nitro-3-hydroxy benzoic acid
(D) None of these
What is the structure of 3-Phenylpentane ?
CHCHCHCHCH
3
2
2
3
CHCHCHCHCHCH
3
2
2
2
3
O
(B)
(A)
CHCHCHCHCH
3
2
2
3
COOH
(C)
(D)
COOH
3.
What is the IUPAC name of the following compound ?
CH3
NO2
Br
(A) o-Nitro-m-bromotoluene
(C) m-Bromo-O-nitrotoluene
4.
(B) 3-Bromo-6-nitrotoluene
(D) 5-Bromo-2-nitrotoluene
What is the common name of the compound below ?
OH
CHCHCHCH
2
2
2
3
(A) 1-Phenoxyethane
(C) o-Butylhydroxybenzene
(B) Ethyl phenyl ether
(D) m-Butylphenol
149
JEE-Chemistry
5.
Which of the following structures has the correct locants?
5
O
COOH
6
(A) Cl C 4
1
3
CN
O
2
COH
2
1
6.
6
4
COCH
2
3
COH
2
6
1
(B) Cl C 5
2
(C) Cl C 3
CN
COCH
2
3
O
2
CN
4
3
O
6
5
(D) Cl C 1
5
CN
COH
2
4
2
3
What is the IUPAC name for the following compound ?
C N
(A) Benzenecarbonitrile
(C) Phenylisocyanide
(B) Benzenecyanide
(D) Cyanophenyl
150
COCH
2
3
COCH
2
3
Classification & Nomenclature of Organic Compounds
ANSWER KEY
STRUCTURE OF ORGANIC COMPOUNDS AND HYBRIDISATION
SINGLE CORRECT ANSWER TYPE
1.
(C)
2.
(C)
3.
(C)
7.
(C)
8.
(C)
9.
(B)
4.
5.
(D)
6.
(D)
(C)
CLASSIFICATION OF CARBON AND HYDROGEN
1.
(B)
2.
(B)
7.
(A)
8.
(B)
3.
4.
(A)
5.
(A)
(B)
6.
(C)
CLASSIFICATION OF ORGANIC COMPOUNDS
1.
(B)
7.
(B)
2.
3.
(B)
4.
(A)
(D)
5.
(B)
6.
(C)
5.
(A)
6.
(C)
HOMOLOGOUS SERIES
1.
(C)
2.
(C)
3.
(B)
7.
(D)
8.
(A)
9.
(D)
4.
(D)
FUNCTIONAL GROUP IDENTIFICATION
1.
1°amine, alcohol
2.
3°amine, carboxylic acid
3.
alcohol, ketone, carboxylic acid
4.
Ketone, Aldehyde
5.
Alkene, Acid chloride
6.
ester, carboxylic acid
7.
Acid Anhydride
8.
1°amine, ketone, amide
9.
cyanide, isocyanide, ether
10.
Ester
11.
Alkene, ketone, Aldehyde
12.
Alkene, Carboxylic acid
13.
Alkene, cyanide, aldehyde
14.
Alkene, isocyanide
15.
Thioalcohol, ester
17.
Alkene, Alkyne, Sulphonic acid
18.
Ketone, alcohol, Thio alcohol
19.
Acid Anhydride
20.
Alkene, alcohol (enol) 21.
Alkene, Carboxylic acid
22.
Alkene, Aldehyde
23.
Ketone
24.
Alkene, ester
25.
Amide
26.
Ether, cyanide
27.
1°amine, ester
28.
2°-Amide, Thio ether, Carboxylic acid, 3°-Amide
30.
Phenol, ether, 1°amine, Carboxylic acid, Iodine
16.
Aldehyde, Acid chloride
29.
Phenol, 1°amine
IUPAC NOMENCLATURE OF ALKANES
1.
(D)
2.
(B)
3.
(D)
4.
(A)
5.
(A)
6.
(A)
7.
(B)
8.
(A)
9.
(A)
10.
(B)
11.
(B)
12.
(C)
13.
(C)
151
JEE-Chemistry
IUPAC NOMENCLATURE OF ALKENES & ALKYNES
1.
(A)
2.
(C)
3.
(D)
4.
(D)
5.
(C)
6.
(B)
7.
(D)
8.
(B)
9.
(B)
10.
(B)
11.
(A)
12.
(C)
13.
(A)
14.
(B)
NOMENCLATURE OF CARBOXYLIC ACID
1.
Ethanoic acid
2.
2-Methylhex-5-en-1-oic acid
3.
2-Ethyl-4-methylhept-6-en-1-oic acid
4.
3-Bromo-2-ethylbutanoic acid
5.
2-Ethylheptanoic acid
NOMENCLATURE OF ACID ANHYDRIDE
1.
Ethanoic anhydride
2.
3.
2-Bromoethanoic-2-chloropropanoic anhydride
4.
But-3-enoic pentanoic anhydride
5.
Butanoic ethanoic anhydride
But-3-enoic but-3-ynoic anhydride
NOMENCLATURE OF ESTER
1.
Methyl ethanoate
2.
Methyl-2-methylpentanoate
3.
Methyl-3-bromo-2-ethylpentanoate
4.
Methyl-2-methyloct-7-en-1-oate
5.
Phenylethanoate
NOMENCLATURE OF HALO CARBONYL
1.
2-Methylpropanoyl chloride
2.
3.
4-Methyl-2-(1-methylethyl)pentanoyl chloride 4.
5.
4, 7-Dichloro-2-ethylnonanoyl chloride
2-Methylpentanoyl chloride
2, 6-Dimethyloct-7-en-1-oyl chloride
NOMENCLATURE OF AMIDE
1.
Butanamide
2.
Hexanamide
3.
But-3-en-1-amide
4.
2-Methylbut-3-yn-1-amide
5.
N-1-methylethyl)ethanamide
NOMENCLATURE OF CYANIDE
1.
3,3-Dimethylbutan-1-nitrile
2.
But-3-yne-1-nitrile
4.
2-Propylpentanenitrile
5.
2, 5-Dimethylhept-6-yne-1-nitrile
152
3.
2-Methylpentanenitrile
Classification & Nomenclature of Organic Compounds
NOMENCLATURE OF ALDEHYDE
1.
2-Ethylbutanal
2.
2,4-Dimethylhex-5-en-1-al
3.
2-Methylpropanal
4.
Ethane-1,2-dial
5.
But-2-en-1-al
NOMENCLATURE OF KETONE
1.
Pentan-2-one
2. 3-Methylbutan-2-one
3.
But-3-en-2-one
4.
5.
But-3-yn-2-one
3-Ethenylpent-4-en-2-one
NOMENCLATURE OF ALCOHOL
1.
Hexan-3-ol
2.
4-Methylhexan-2-ol
4.
Prop-2-en-1-ol
5.
Hexa-1,5-dien-1-ol
3.
4-Ethylhexan-3-ol
NOMENCLATURE OF AMINE
1.
Ethanamine
2.
4-Methylhex-5-yn-2-amine
3.
6-Methyloct-7-en-2-amine
4.
Hexan-3-amine
5.
N-Ethyl-N-Methylethanamine
NOMENCLATURE OF HALOALKANES, HALOALKENES &
HALOALKYNES
3.
1.
1,1,1-Trichloroethane
2.
1, 1, 2-Trichloroethane
4.
4-Bromopent-2-ene
5.
3-Bromo-2-methylbut-1-ene 6.
7.
1-Bromo-2-methylbut-2-ene
9.
3-Bromo-2-methylpropene
10.
4-Bromo-2,3-dichlorohex-5-yn-1-ol
8.
Tetrachloromethane
4-Bromo-3-methylpent-2-ene
1-Bromobut-2-ene
NOMENCLATURE OF ETHER
1.
Methoxybenzene(Anisole)
2.
Ethoxybenzene(Phenetole)
3.
Heptyloxybenzene
4.
2-Methoxypropane
5.
3-Methylbutoxybcnzene
153
JEE-Chemistry
IUPAC NOMENCLATURE OF COMPOUNDS CONTAINING ONLY
SINGLE FUNCTIONAL GROUP
1.
(B)
2.
(D)
7.
(D)
8.
(D)
3.
(B)
4.
(C)
5.
(A)
6.
(C)
IUPAC NOMENCLATURE OF COMPOUNDS CONTAINING MORE
THAN ONE FUNCTIONAL GROUP
1.
(B)
2.
(B)
3.
(C)
4.
(D)
5.
(A)
6.
(A)
7.
(D)
8.
(A)
9.
(A)
10.
(C)
11.
(C)
12.
(B)
13.
(C)
14.
(C)
15.
(D)
16.
(C)
17.
(D)
18.
(B)
19.
(B)
20.
(B)
21.
(B)
22.
(B)
23.
(A)
24.
(D)
25.
(A)
IUPAC NOMECLATURE OF ALICYCLIC COMPOUNDS
1.
(B)
2.
(C)
3.
(A)
4.
(C)
7.
(C)
8.
(D)
9.
(A)
10.
(B)
5.
(B)
6.
(B)
IUPAC NOMENCLATURE OF BENZENE RING CONTAINING
COMPOUNDS
1.
(A)
2.
C
3.
4.
(D)
154
(D)
5.
(B)
6.
((A)
General Organic Chemistry
GENERAL ORGANIC CHEMISTRY
INDUCTIVE EFFECT
SINGLE CORRECT ANSWER TYPE
1.
Inductive effect refers to
(A) Electron displacement along a carbon chain
(B) Complete transfer of one of the shared pair of electrons to one of the atoms joined by a double
bond
(C) Complete transfer of electrons from one atom to another
(D) None of the above
2.
Maximum -I effect is exerted by the group
(A) C6H5–
(B) –OCH3
(C) –Cl
(D) –NO2
3.
Which of the following is correct order of increasing + I effect ?
(A) (CH3)3C— < (CH3)2CH— < CH3CH2— (B) CH3CH2— < (CH3)2CH— < (CH3)3C—
(C) (CH3)2CH— < (CH3)3C— < CH3CH2— (D) (CH3)3C— < CH3CH2— < (CH3)2CH—
4.
Which of the following is correct for inductive effect ?
(A) It decreases with increases in distance
(B) It is independent of distnace
(C) It indicates the transfer of p pair of electrons from less electronegative atom to non-electronegative atom in a molecules
(D) It show the transfer of lone pair of electrons
5.
Inductive effect of Cl-atom operates in
(A) CH3 – CH2 – CH2 – Cl
(B) CH2 = CH – CH = CH – Cl
Cl
(C)
6.
7.
8
(D) All of these
What is the correct order of +I effect of the following groups ?
–O– –CO2– –CR3 –R2CH –D –H
a
b
c
d
e f
(A) a > b > c > d > e > f
(C) a > c > b > d > f > e
(B) a > c > d > b > e > f
(D) a > f > b > d > e > c
Which of the following has strong +I effect ?
(A) – O (B) –Et
(C) –CH3
Which of the following compound does not show inductive effect ?
(A) CH3–CH2–Br
(B) CH3– CH = CH2 (C) CH3 – C º CH
155
(D) –NH–CH3
(D) CH3 – CH2 – CH3
JEE-Chemistry
9.
In which of the following compound, +I effect of alkene is operating ?
(A) CH3 – CH = CH2
(B) CH3 – CH2 – CH = CH2
(C) HC º C – CH = CH2
(D) H2C = CH – CH = CH2
C CH
CH3
;
10.
(a)
;
(b)
In compound (a) and (b) relative inductive effect of phenyl group with respect to the groups attached
to it is :
(A) + I, + I
(B) –I, + I
(C) –I, – I
(D) +I, –I
156
General Organic Chemistry
RESONANCE
SINGLE CORRECT ANSWER TYPE
Resonating structures :
1.
Select the molecule in which p bonds are conjugated ?
H
(A) H2C = CH – CH2 – CH = CH2
H
(C) H
2.
C= C
(B)
C = C= C
H
H
H
H
C=O (D) Both (A) and (C)
H
Which of the following is not a valid resonance structures ?
O–
O
–
(A)
–2
O
O
(B)
(C)
(D)
–
3.
How many neutral resonating structures are possible for Napthalene ?
(A) 1
(B) 2
(C) 3
(D) 4
+
4.
Number of resonating structures of compound
(A) 1
5.
(B) 2
(C) 3
(D) 4
In which of the following compounds lone pair of oxygen is delocalized ?
(A)
6.
is :
(B)
(C)
(D)
In which of the following resonating structures extra bond will form?
+
-
(A) H2 C = CH – CH 2
Å
(C) H3C - CH - O - CH3
CH2
(B)
(D)
+
157
+
JEE-Chemistry
7.
In which of the following compounds d-orbital resonance takes place ?
-
-
(A) Cl - CH 2
8.
(B) CH3 - S - CH 2
(B) H – N
O
–
N– H
S
(C) S
–
(D)
–
–
Which of the following compound has localized lone pair ?
NH2
CH2 –NH2
(A)
10.
(D) All of these
Which of the following carbanions is resonance stabilized ?
(A) O
9.
(C) –CCl3
(B)
CH–CH3
(C)
(D)
N
|
H
Which of the following compounds has delocalized lone pair ?
O
(A)
11.
(B)
(D)
N
N
N
H
H
H
N
Which of the following has two equivalent resonating structure ?
O
||
(A) H - C - NH 2
12.
(C)
O
||
H
C
- OH
(C)
O
|| (B) H - C - O
O
||
(D) H - C - CH3
Which of the following is not a resonance structure of the others ?
O–
(A)
O
(B)
O
O
–
–
(C)
(D)
–
Stability of resonating structures :
13.
Stability order of the following resonating structure will be :
–
O
–
O
+
+
O
O
+
–
(I)
(II)
(III)
(IV)
(A) I > II > III > IV
(B) II > I > III > IV
(C) III > II > I > IV
(D) I > III > II > IV
158
General Organic Chemistry
14.
15.
Compare relative stability of following resonating structure :
-
OO
||
|
Å
CH 3 - C - OH ¬¾
CH
C
= O- H
®
3
(a)
(b)
O
|
- OH
CH
C
3
¬¾
®
Å
(A) a > b > c
(C) b > a > c
(c)
(B) a > c > b
(D) c > a > b
Most stable resonating structure of given cation is :
O
(A)
(B)
O
16.
(C)
(D)
O
O
O
Compare relative stability of following resonating structure :
Å
-
CH 3 - NH = CH - CH - CH = CH 2
(a)
-
CH 3 - NH - CH = CH - CH = CH 2
(b)
Å
CH 3 - NH - CH - CH = CH - CH 2
(c)
(A) a > b > c
17.
(B) b > a > c
(C) b > c > a
(D) a > c > b
Rank the resonance structure in each group in order of increasing contribution to the resonance hybrid :
CH3
CH 3
CH3
|
··
|
|
Å
¬¾
®
CH
C
N
- NH 2
3
CH3 - C = N - NH2 ¬¾
® CH 3 - C - N = NH 2
Å
Q
Q
(I)
(A) I < II < III
(III)
(II)
(B) II < I < III
(C) III < II < I
159
(D) III < I < II
JEE-Chemistry
Resonance Energy :
18.
If we consider four resonating structure of formic acid. Then structure II corresponds to
IV
III
II
I
E
Formic acid
-
O
||
H
C
- OH
(A)
Q
19.
O
|Å
(B) H - C - OH
Å
Q
O|
Å
(C) H - C = O- H
OÅ
|
- OH
H
C
(D)
Q
Å
O = C = O; O - C º O; O - C = O
(I)
(II)
(III)
I, II and III are represented by (where E = Potential energy):
III
II
(A) E
20.
I, II, III
(B) E
II
(C) E
I
III
(D) E
I
Compar resonance energy of following:
O
21.
I, III
II
O
O
(I)
(II)
(III)
(A) I > II > III
(B) II > I > III
(C) II > III > I
(D) I > III > II
Which of the following has highest resonance energy ?
O
O
(A)
O
(B)
O
(C)
(D)
Resonance (Miscellaneous) :
22.
In which of the following molecules p – electron density in ring is minimum :
(A)
23.
(B)
(D)
Å
Resonance hybrid of H 2 C = CH - CH 2 is :
d+
d+
–CH–CH2
(A) HC
2
24.
(C)
d–
d–
d–
(B) H2C –CH–CH2
d–
d
–
(C) H2C–CH–CH2
–
=CH–CH2
(D) HC
2
Which of the following group(s) cannot participate in resonance when attached to benzene ring?
Å
(A) - NH 3
Å
(B) - PH3
Å
(C) - C H 2
160
(D) -COO
General Organic Chemistry
MULTIPLE CORRECT ANSWER TYPE
25.
E
A &B
A and B is/are resonating structure of :
O
||
(A) CH3 - C - OH
26.
(B)
O
|| Q
(C) CH3 - C - O
(D) CH 2 = CH - CH 2 +
Which of the following compound(s) can show resonance ?
(A)
27.
O
(B)
(C)
(D)
In which of the following molecule/s resonance is absent ?
–
CH2
(A)
(B)
(C)
(D) CH -2 - CH 2 - CH = CH 2
+
161
JEE-Chemistry
HYPERCONJUGATION
1.
SINGLE CORRECT ANSWER TYPE
Which of the following has maximum number of a -hydrogen ?
(A)
(B)
(C)
(D)
2.
Number of a -hydrogen in given compound is :
(A) 4
(B) 5
(C) 6
3.
Number of possible hyper conjugative structures of
(A) 9
4.
5.
(B) 8
(D) 7
are ?
(C) 7
(D) 6
(C) 15
(D) 16
Sum of a -hydrogen in :
(I)
(II)
(I) + (II) = ?
(A) 13
(B) 14
Sum of a -hydrogen in:
(I) 1 - hexene,
(II) 2-hexene,
(I) + (II) + (III) = ?
(A) 8
(B) 10
(III) 3-hexene
(C) 11
(D) 12
6.
Hyperconjugation is best described as:
(A) Delocalisation of p electrons into a nearby empty orbital.
(B) Delocalisation of s electrons into a nearby empty orbital.
(C) The effect of alkyl groups donating a small amount of electron density inductively into a carbocation.
(D) The migration of a carbon or hydrogen from one carbocation to another.
7.
In which of the following alkene hyperconjugation does not take place ?
(A)
(B)
(C)
162
(D)
CH= CH
General Organic Chemistry
8.
Which of the following represent hyperconjugation in carbocation ?
H
O
E
H
(A) H – C – C
H
9.
10.
H
E
+
(B) H C – C
H
H
+
(C) H2C CH CH2
(D)
H
Which of the following is different from others
(A) no bond resonance
(B) excessive conjungation
(C) Hyper conjugation
(D) electromeric effect
MULTIPLE CORRECT ANSWER TYPE
Which of the following can show hyper conjugation :
·
·
(B) ( CH3 ) C
3
(A) CH3
11.
O
H
·
(C) CH 3 C H 2
(D)
Which of the following compound (s) do not have alpha hydrogen ?
O
(A)
CH
O
O
(B) H – C – H
(C)
CH3O
– CH
(D) CHC
3
CH3
163
JEE-Chemistry
HEAT OF HYDROGENATION/HEAT OF COMBUSTION
1.
2.
3.
4.
5.
SINGLE CORRECT ANSWER TYPE
Arrange the following in decreasing order of heat of combustion.
(I)
(II)
(III)
(IV)
(A) I > II > III > IV
(B) II > III > IV > I
(C) III > I > II > IV
(D) I > III > II > IV
Arrange the following in decreasing order of heat of combustion.
(I)
(II)
(III)
(IV)
(A) I > II > III > IV
(B) II > III > IV > I
(C) III > IV > II > I
(D) III > II > IV > I
Arrange the following in decreasing order of heat of hydrogenation (HOH).
(I)
(II)
(III)
(IV)
(A) II > III > I > IV
(B) I > II > IV > III
(C) I > II > III > IV
(D) III > II > I > IV
Arrange the following in decreasing order of heat of hydrogenation (HOH).
(I)
(II)
(III)
(IV)
(A) I > II > III > IV
(B) II > III > IV > I
(C) I > II > III > IV
(D) IV > III > II > I
Arrange the following in decreasing order of heat of hydrogenation (HOH).
(I)
(II)
(III)
(A) III > I > II
(B) I > II > III
(C) III > II > I
164
(D) II > III > I
General Organic Chemistry
AROMATICITY
1.
SINGLE CORRECT ANSWER TYPE
Which of the following is anti-aromatic ?
+
+
(A)
Å
+
(B)
(C)
(D)
N
Å
H
2.
How many p electrons are there in the following species :
(A) 2
3.
(B) 4
(B)
(B)
(B)
Br
(C)
(D) All of these
(C)
(D) All of these
(C) r1 = r2
(D) r2 >> r1
Br
AgNO3
r1;
AgNO3
Rate of reaction r1 and r2 is :
(A) r1 > r2
(B) r2 > r1
7.
(D)
Which of the following is non-Aromatic?
(A)
6.
(C)
Which of the following is Aromatic?
(A)
5.
(D) 8
Which of the following is aromatic compound?
(A)
4.
(C) 6
r2
Which of the following statements is incorrect about benzene?
(A) All of the carbon atoms are sp hybridized
(B) It has delocalized p electrons
(C) The carbon-carbon bond lengths are all the same
(D) The carbon-hydrogen bond lengths are all the same
165
JEE-Chemistry
8.
Which of the following is Anti-aromatic?
(A)
9.
(B)
(B)
(C)
(D)
In which of the following reaction product is aromatic?
Cl
Br
AgNO3
¾¾¾
® (B)
(A)
11.
(D)
Which of the following is not Aromatic compounds :
(A)
10.
(C)
Li
¾Ph
¾-¾
®
D
¾AgNO
¾¾
¾3 ® (D)All of these
D
(C)
In which of the following compound resonance does not takes place ?
O
(B)
(A)
12.
(C)
MULTIPLE CORRECT ANSWER TYPE
Which of the structures below would be aromatic?
+
+
(A)
13.
(D)
(B)
(C)
+
(D)
Select the correct statement/s
;
(A)
..
N
Both are aromatic but the conjugate acid of (II) is not aromatic
H
(II)
(B)
Br
(I)
;
Both are nonaromatic but (I) gives precipitate of AgBr with aq. AgNO3
(II)
(C)
(D)
Br
;
;
(I) is antiaromatic but (II) is nonaromatic.
Both liberate H2 gas on reaction with K, and turn into aromatic salts.
166
General Organic Chemistry
14.
Which of the following species should be aromatic ?
(A)
15.
..
S
..
(B)
(C)
..
O
(D)
[10] Annulene
Using Huckel rule, predict which of the following hydrocarbons will exhibit aromatic stabilisation :
..-
(A)
16.
(B)
(C)
+
(D)
Which of the following are aromatic compound ?
(A)
(B)
(C)
167
(D)
JEE-Chemistry
REACTION INTERMEDIATES
Carbocation :
Arrange the following in decreasing order of stability of following reactions intermediates (for
question 1-7) :
1.
CH 3
|
Å
Å
CH3 - CH 2 CH3 - CH - CH3 CH 3 - C Å
|
(II)
CH 3
(I)
(III)
(A) I > II > III
(B) III > II > I
(C) II > I > III
(D) III> I > II
(C) II >III > I
(D) III> I > II
(C) II >III > I>IV
(D) III> I > II>IV
(C) II >III > I
(D) III> I > II
Å
Å
2.
(I)
Å
(II)
(A) I > II > III
(III)
(B) III > II > I
Å
Å
Å
Å
(III)
(IV)
3.
(I)
(II)
(A) IV>I > II > III
(B) IV>III > II > I
CH2Å
CH2Å
Å
CH2
OH
4.
OH
(I)
(II)
(A) I > II > III
5.
OH
(III)
(B) III > II > I
CHÅ
2
CHÅ
2
CH2Å
CH2Å
CH3
CH2Me
CH Me2
CMe3
(I)
(II)
(III)
(IV)
(A) I > II > III>IV
(B) IV>III > II > I
(C) II >III > I>IV
168
(D) III> I > II>IV
General Organic Chemistry
Å
Å
CH2
6.
CH2
Å
CH2
H
C H
H
H C H
H
(I)
(II)
(A) I > II > III
H
C H
H
(III)
(B) III > II > I
+
+
+
(I)
(II)
(III)
(C) II >III > I
(D) III> I > II
(C) II >III > I
(D) III> I > II
7.
(A) I > II > III
8.
(B) III > II > I
Which of the following carbocation is resonance stabilized ?
+
+
(A)
9.
+
(B)
(C)
(A)
+
+
(D)
(B)
+
(C)
(D)
+
+
Which of the following is the most stable carbocation ?
(A)
CH3
CH3
(B)
+
+
(C)
CH3
+
+
(D)
Which of the following carbocation is the most stable ?
Å
(I) CH 3 CH CH 3
(A) I
13.
(C)
+
Most stable structure of carbocation C4H9Å is :
CH3
12.
+
(B)
(A)
11.
(D)
Which of the following carbocation is most stable ?
+
10.
+
CH 3
|
Å
(II) CH 3 - C
|
CH 3
(B) II
(IV)
(C) III
(D) IV
Correct order of stability of carbocations is:
Å
Å
(I)
(A) I > II > III > IV
(II)
(B) I > II > IV > III
+
Å
(III) CH3CH 2CH 2
Å
(III)
(C) II > I > III > IV
169
Å
(IV)
(D) II > I > IV > III
JEE-Chemistry
Carboanion :
Arrange the following in decreasing order of stability of following reactions intermediates (for
question 14-19) :
14.
CH3 – CH2
CH3
|
CH3 – C–
|
CH3
CH3 – CH – CH3
(I)
(II)
(A) I > II > III
(III)
(B) III > II > I
(C) II > I > III
(D) III> I > II
(C) II > I > III
(D) III> I > II
(C) II > I > III
(D) III> I > II
(C) II > I > III
(D) III> I > II
–
–
–
15.
(I)
(II)
(III)
(A) I > II > III
(B) III > II > I
–
–
16.
–
(I)
(II)
(A) I > II > III
-
17.
HC º C
(I)
(B) I > III > II
-
-
CH 2 = CH CH 3 - CH 2
(II)
(III)
(A) I > II > III
(B) III > II > I
–
–
CH2
CH2
18.
Cl
O
N
(I)
(II)
(A) I > II > III > IV
–
(I)
(A) I > II > III
O
–
–
CH2
CH2
C ºN
(III)
(IV)
(B) I > II > IV > III
O
19.
(III)
O
–
(II)
(C) II > III >I > IV
(D) II > I > IV > III
(C) II > I > III
(D) III> I > II
O
–
(III)
(B) III > II > I
170
General Organic Chemistry
Free radical :
Arrange the following in decreasing order of stability of following reactions intermediates (for
question 20-25) :
20.
CH3 – CH2
CH3
|
CH3 – C
|
CH3
(III)
CH3 – CH – CH3
(I)
(II)
(A) I > II > III
(B) III > II > I
(C) II > I > III
(D) III> I > II
(C) II > I > III
(D) III> I > II
(C) II > III> I
(D) III> I > II
(C) II > I > III
(D) III> I > II
21.
(I)
(II)
(A) I > II > III
(III)
(B) I > III > II
22.
(I)
(II)
(A) I > II > III
·
23.
(III)
(B) III > II > I
·
·
CH º C CH 2 = C H CH3 - CH 2
(I)
(II)
(III)
(A) I > II > III
(B) III > II > I
CH2
CH2–CH2
(I)
(II)
24.
(III)
(A) I > II > III
25.
(B) III > II > I
(C) II > I > III
(D) III> I > II
MULTIPLE CORRECT ANSWER TYPE
Which of the following is/are correct :
Å
Å
(A) CH3O CH 2 is more stable than CH3 CH 2
Å
Å
(B) Me 2 CH is more stable than CH 3CH 2 CH2
Å
Å
(C) CH 2 = CH - CH2 is more stable than CH 3 CH 2 CH 2
Å
Å
(D) CH 2 = CH is more stable than CH3 CH 2
171
JEE-Chemistry
BOND PARAMETER
SINGLE CORRECT ANSWER TYPE
Bond order and bond strength :
1.
Rank the indicated bond in the given compound in order of decreasing bond strength is :
b
a
c
C
C
(A) a > b > c
2.
(B) b > a > c
(C) b > c > a
Rank the indicated bond in the given compound in order of decreasing bond strength:
a
CH3
b
–N
N
H
(A) a > b > c
3.
4.
(D) a > c > b
c
Cº N
(B) c > b > a
(C) b > c > a
(D) c > a > b
Among the following molecules, the correct order of C – C bond length is
(A) C2H6 > C2H4 > C6H6 > C2H2
(B) C2H6 > C6H6 > C2H4 > C2H2(C6H6 is benzene)
(C) C2H4 > C2H6 > C2H2 > C6H6
(D) C2H6 > C2H4 > C2H2 > C6H6
¬
¾®
¬
¾®
These are three canonical structures of naphthalene. Examine them and find correct statement among
the following :
(A) All C – C bonds are of same length
(B) C1 – C2 bond is shorter than C2 – C3 bond.
(C) C1 – C2 bond is longer than C2 – C3 bond (D) None
5.
Find out the correct statement(s) about the given compound?
8
1
7
2
6
3
5
4
(A) Bond length between C2 and C3 = Bond length between C5 and C6
(B) Bond length between C1 and C2 = Bond length between C6 and C7
(C) Bond length between C6 and C7 < Bond length between C3 and C4
(D) Bond length between C2 and C3 < Bond length between C3 and C4
172
General Organic Chemistry
Bond energy :
6.
Instuction For question no 6 to 8 : Consider homolytic bond cleavage
Arrange the following hydrogen in decreasing order of bond energy :
Ha Hb
CH3
HC
= CH– CH –CH– C – CH–
2
2 Hd
Hc
(A) Ha > Hc > Hb > Hd
(C) Hd > Hc > Hb > Ha
7.
(B) Ha > Hd > Hb > Hc
(D) Hd > Hb > Hc > Ha
Arrange the following in decreasing order of bond energy :
Ha
CH CH2
Hb
Hc
(A) Ha > Hc > Hb
8.
(B) Hc > Hb > Ha
(C) Hb > Ha > Hc
(D) Hb > Hc > Ha
Arrrange the following in decreasing order of bond energy :
Ha
Hb
Hc
(A) Ha > Hc > Hb
(B) Ha > Hb > Hc
(C) Hb > Ha > Hc
173
(D) Hb > Hc > Ha
JEE-Chemistry
DETERMINANTION OF ACIDIC STRENGTH
SINGLE CORRECT ANSWER TYPE
Arrange the following in decreasing order of acidic strength (for question1-7) :
1.
2.
O
||
(I) NO 2 - CH 2 - C - O - H
O
||
(II) F - CH - C - O - H
2
O
||
(III) Ph - CH 2 - C - O - H
O
||
(IV) CH 3 - CH 2 - C - O - H
(A) II > I > III > IV
(C) III > I > II > IV
(B)IV > III > II > I
(D) I > II > III > IV
O
||
(II) CH 3 - CH - CH 2 - C - O - H
|
F
O
||
(I) CH 3 - CH 2 - CH - C - O - H
|
F
O
||
(III) CH 2 - CH 2 - CH 2 - C - O - H
|
F
(A) I > II > III
(B) I > III > II
(C) III > II > I
(D) II > I > III
CH3
3.
4.
5.
(I) CH3–CH2–O–H
(II) CH 3 - CH - O - H (III) CH3–C–O–H
|
CH3
CH 3
(A) II > I > III
(B) III > II > I
(C) I > II > III
(I)
(II)
(III)
COOH
(A) III > II > I
COOH
(I) |
COOH
COOH
(B) II > I > III
(II) CH2
COOH
COOH
(C) III > I > II
(D) II > III > I
(D) I > II > III
CH 2 - COOH
(III) |
CH 2 - COOH
(A) II > I > III
COOH
(B) I > II > III
(C) III > I > II
(D) I > III > II
6.
(I) CH4
(A) II > I > III > IV
(II) NH3
(B) IV> III > II > I
(III) H2O
(C) I > II > III > IV
(IV) H–F
(D) I > III > III > IV
7.
(I) F–CH2–CH2–O–H
(II) NO2–CH2–CH2–O–H
(III) Br–CH2–CH2–O–H
(IV) NH3 - CH2 - CH2 - O - H
(A) IV> II > I > III
(C) IV > II > I > III
(B) IV> III > II > I
Å
174
(D) I > II > III > IV
General Organic Chemistry
Write correct order of acidic strength of following compounds (for question 8-14) :
O–H
O–H
8.
(I)
N
(II)
O–H
O
O
O–H
NO2
(III)
NO2
(A) I > II > III > IV
(B) III > II > IV > I
O–H
9.
O–H
(I)
NO2
(A) IV > I > II > III
O–H
10.
N
(I)
(III)
Cl
(B) II > I > III > IV
CH3
(C) I > IV > II > III
O
(A) I > II > III > IV
(II)
O
N
O
O
(C) II > III > I > IV
(D) IV > I > III > II
O–H
(II)
12.
(I)
(II)
(IV)
CH 3
(C) II > I > III > IV
(D) III > II > I > IV
O–H
O–H
O–H
Cl
O–H
(III)
(B) IV > II > III > I
O–H
O–H
(IV)
CH3
(A) IV > III > II > I
(D) III > II > I > IV
(III)
O–H
CH 3
(I)
CN
O
(B) III > I > II > IV
O–H
(IV)
O–H
O–H
NO2
O–H
(II)
O
NO2
NO2
(D) IV > III > II > I
O–H
N
11.
(C) I > III > IV > II
(IV)
(III)
(IV)
(B) II > I > III> IV
Cl
(C) III > II > I > IV
(D) III > I > II > IV
COOH
COOH
Cl
(A) I > II > III > IV
COOH
13.
(I)
N
O
O
(A) II > III > I > IV
(II)
(III)
NO2
COOH
(IV)
NO2
(B) I > II > III > IV
(C) II > I > III > IV
175
(D) III > I > II > IV
JEE-Chemistry
COOH
14.
COOH
COOH
(I)
CH3
(II)
COOH
(III)
(IV)
CH3
(A) II > I > III > IV
15.
16.
(B) I > II > III > IV
(C) III > II > I > IV
(I)
(II)
(III)
(A) III > I > II
(B) I > II > III
(C) II > I > III
(D) III > II > I
The most acidic among the following compound is :
(A) Cl – CH2 – CH2 – OH (B)
OH
(C)
OH
(D)
NO2
CH3
(C) I > IV > II > III
(D) I > IV > III > II
Rank these protons in order of decreasing acidity :
(III)
O
(II)
NH2 OH
NH2
(I)
(IV)
(A) IV > I > III > II
H–O
(a)
(B) I > II > IV > III
OH(b)
O
18.
(D) IV > I > II > III
Rank the following in decreasing order of acidity :
OH
17.
CH 3
NH 3(c)
SO3H(d) ; Order of acidic strength is :
+
(A) d > c > b > a
19.
(B) d > a > b > c
(C) d > a > c > b
(D) a > d > c > b
In the following compunds :
OH
OH
OH
OH
NO2
(I)
CH3
(II)
the order of acidity is :
(A) III > IV > I > II
(B) I > IV > III > II
(III)
NO2
(IV)
(C) II > I > III > IV
176
(D) IV > III > I > II
General Organic Chemistry
DETERMINATION OF BASIC STRENGTH
1.
SINGLE CORRECT ANSWER TYPE
Write in increasing/decreasing order of basic strength of following:
(I) NH3
(II) MeNH2
(III) Me2NH
(IV) Me3N (in H2O)
(A) I > II > III > IV
(B) II > I > III > IV
(C) III > II > IV > I
(D) IV > I > III > II
2.
(I) NH3
(A) II > I > III > IV
(II) MeNH2
(B) I > II > III > IV
(III) Me2NH
(C) IV > III > II > I
3.
(I) R–NH2
(II) Ph–NH2
(III) R - C - NH 2
||
O
(A) I > II > III
(B) II > I > III
(C) III > II > I
N
N
4.
(I)
(III)
Me
(A) III > II > I
(I)
7.
(C) I > II > III
(III)
··
· ·
(B) II > I > III > IV
(D) I > II > III > IV
··
(II) CH3–CH= NH
(B) II > III > I
··
H
(C) III > IV > II > I
··
NH2
(IV)
CH3
Cl
(I) CH3–CH2– N H 2
(A) I > II > III
(D) II > III > I
NH2
NH2
(II)
Å
NH3
(A) I > II > IV > III
6.
F
(B) II > I > III
NH2
5.
(D) III > I > II
N
(II)
O2N
(IV) Me3N (in Gas)
(D) I > II > III > IV
(III) CH3–Cº N
(C) I > III > II
· ·
(D) III > II > I
· ·
(II) CH3–CH2– NH 2
(III) CH 3 - C - N H 2
||
N
H
··
(IV) NH 2- C - N H 2
||
N
H
··
(A) I > II > III > IV
(B) IV > III > II > I
(C) I > II > III > IV
(D) I > II > III > IV
NH2
8.
· ·
(I) CH 3 - C - NH 2
||
O
(I)
N
H
(A) I > II > III
(II)
N
(B) II > I > III
(III)
(C) III > II > I
177
(D) II > III > I
JEE-Chemistry
NH2
9.
NH2
(I)
(II)
NO2
(B) I > II > III > IV
(I)
NH2
(C) IV > III > II > I
(D) II > I > III > IV
NH2
(II)
NO2
(III)
NO2
NO2
(A) I > II > III
(B) II > I > III
NMe2
11.
(IV)
OMe
NH2
NH2
10.
(III)
CN
(A) I > III > II > IV
NH2
NH2
(C) III > II > I
Me
NMe2
(I)
(II)
N
(D) II > III > I
Me
OMe
(III)
OMe
OMe
(A) III > I > II
(B) II > I > III
(C) III > II > I
(D) II > III > I
O
12.
(I)
(II)
(A) III > II > I
(B) II > I > III
14.
(III)
(C) II > III > I
NH2 H
C H
NH2
13.
NH–CH2–CH3
NH2
NH–C–CH3
(I)
(II)
(A) III > I > II
(B) II > I > III
H
(D) II > III > I
NH2
(III)
(C) I > II > III
(D) II > III > I
Which of the following is strongest base ?
O
··
(A) H – N
··
NH2
··
NH
··
N– H
·
(B) H – N·
··
N– H
(C)
178
··
N
(D)
General Organic Chemistry
H
O
N
15.
16.
;
N
N
N
H
(a)
H
(b)
H
(c)
Compare basic strength
(A) a > b > c
(B) c > a > b
Which of the following is strongest base ?
NH2
(C) b > a > c
NH2
(D) c > b > a
NH2
CH2 – NH2
CH3
(A)
(B)
(C)
CH3
CH3
17.
Which of the following is strong base ?
(A) NH2 – C
18.
NH
CH3
(B) NH2 – C
O
NH2
CH3
(C) NH2 – CH
CH3
(D) NH2 – C
(A) N
CF3
(B) N
CH3
CH3
NH2
CH3
CF3
CF3
(C) N
CH3
CF3
(D) N
CH3
CF3
CF3
Which of the following is weakest base ?
NH2
O
NH
(A) CH3
C
(B) CH3
CH
NH(C) CH3
C
NH2
(D)
NH2
20.
NH
Which of the following compound is virtually non-basic ?
CH3
19.
(D)
Which of the following is weakest base ?
Q
(A) Ph - O
O
||
(B) Ph - C- OQ
O
||
Q
(C) Ph - S - O
||
O
179
Q
(D) PH - CH 2
JEE-Chemistry
SIR EFFECT
1.
SINGLE CORRECT ANSWER TYPE
Which of the following carbocation is not resonance stabilized ?
+
+
CH2
CH– CH3
(A)
2.
(B)
+
CH3 – C – CH3
CH3
CH3
(C)
(D)
In which of the following compound maximum Steric inhibition of resonance effect will operate ?
CH3
NO2
CH3
NO2
CH3
NO2
CH3
CH3
(B)
(A)
3.
+
CH3 – C – CH3
CH3
CH3
(C)
CH3
(D)
In which of the following lone pair of nitrogen is not involved in reasonance ?
CH3
CH3
N
CH3
(A)
CH3
(B)
CH3
N
CH3
CH3
CH3
N
CH3
(C)
(D)
CH3
4.
CH3
Which of the following is the strongest base ?
CH3
NH2
(A)
CH3
N
(B)
NH2
NO2
CH3
NO2
(C)
N
NO2
CH3
NO2
(D)
NO2
NO2
180
N
CH3
CH3
General Organic Chemistry
5.
Which of the following compound has highest Ka value ?
OH
OH
ON
2
(A)
NO2
(B)
ON
2
NO2
NO2
NO2
OH
OH
NO2
(C)
NO2
(D)
NO2
NO2
6.
NO2
Correct order of basic strength of following compounds is :
Me
NH2
Me
O
N
(A) I > III > II
O
N
Me
Me
(II) Me
(I)
Me
NH2
O
Me
N
(B) III > II > I
Me
(III)
O
O
N
(C) I > II > III
181
O
(D) II > III > I
JEE-Chemistry
ANSWER KEY
INDUCTIVE EFFECT
1.
7.
(A)
(A)
2.
8
3.
9.
(D)
(D)
(B)
(C)
4.
10.
(A)
(B)
5.
(D)
6.
(A)
5.
11.
17.
23.
(C)
(B)
(C)
(A)
6.
12.
18.
24.
(C)
(D)
(C)
(A)
5.
11.
(C)
6.
(A)(B)(C)(D)
RESONANCE
1.
7.
13.
19.
25.
(C)
(D)
(A)
(C)
(C)(D)
2.
8.
14.
20.
26.
(D)
(C)
(A)
(B)
(A)(B)(D)
3.
9.
15.
21.
27.
(C)
(B)
(B)
(D)
(A)(D)
4.
10.
16.
22.
(C)
(C)
(B)
(D)
HYPERCONJUGATION
1.
7.
(A)
(D)
2.
8.
(C)
(B)
3.
9.
(A)
(D)
4.
10.
(C)
(B)(C)
(B)
HEAT OF HYDROGENATION/HEAT OF COMBUSTION
1.
(A)
2.
(D)
3.
(B)
4.
(C)
5.
(C)
5.
11.
16.
(D)
6.
(D)
12.
(A)(C)(D)
AROMATICITY
1.
7.
13.
(A)
2.
(A)
8.
(A)(B)(C)(D)
(C)
(D)
3.
9.
14.
(B)
4.
(C)
10.
(A)(B)(C) 15.
(D)
(D)
(A)(C)
(A)
(C)(D)
REACTION INTERMEDIATES
1.
7.
13.
19.
25.
(B)
(C)
(C)
(B)
(A)(B)(C)
2.
8.
14.
20.
(C)
(C)
(A)
(B)
3.
9.
15.
21.
(B)
(A)
(A)
(B)
4.
10.
16.
22.
(D)
(C)
(B)
(C)
5.
11.
17.
23.
(A)
(D)
(A)
(B)
6.
12.
18.
24.
(D)
(B)
(C)
(A)
5.
(C)
6.
(D)
6.
12.
18.
(B)
(A)
(C)
BOND PARAMETER
1.
7.
(C)
(B)
2.
8.
(B)
(D)
3.
(B)
4.
(B)
DETERMINANTION OF ACIDIC STRENGTH
1.
7.
13.
19.
(D)
(C)
(D)
(D)
2.
8.
14.
(A)
(D)
(A)
3.
9.
15.
(C)
(C)
(D)
4.
10.
16.
(A)
(B)
(C)
5.
11.
17.
(B)
(B)
(B)
DETERMINATION OF BASIC STRENGTH
1.
7.
13.
19.
(C)
(B)
(C)
(C)
2.
8.
14.
20.
(C)
(D)
(B)
(C)
3.
9.
15.
(A)
(C)
(B)
4.
10.
16.
(D)
(B)
(D)
5.
11.
17.
(C)
(A)
(D)
6.
12.
18.
(A)
(A)
(D)
5.
(B)
6.
(B)
SIR EFFECT
1.
(D)
2.
(C)
3.
(B)
4.
182
(D)
Thermodynamics
THERMODYNAMICS
BASIC DEFINITION
1.
2.
SINGLE CORRECT ANSWER TYPE
Out of molar entropy (I), specific volume (II), heat capacity (III), volume (IV), extensive
properties are
(A) I, II
(B) I, II, IV
(C) II, III
(D) III, IV
Thermodynamic equilibrium involves
(A) Chemical equilibrium
(C) Thermal equilibrium
(B) Mechanical equilibrium
(D) All of above simultaneously
3.
A well stoppered thermos flask contains some ice cubes. This is an example of :–
(A) Closed system
(B) Open system
(C) Isolated system
(D) Non-thermodynamic system
4.
Which of the following is a closed system?
(A) Jet engine
(B) Tea placed in a covered cup
(C) open kettle
(D) Rocket engine during propulsion
5.
Select the correct order in the following :
(A) 1 erg > 1 joule > 1 cal
(C) 1 erg > 1 cal > 1 joule
6.
7.
8.
9.
(B) 1 cal > 1 joule > 1 erg
(D) 1 joule > 1 cal > 1 erg
Which of of the following is state function ?
(A) Temperature
(B) Potential energy
(C) Internal Energy
(D) All of these
Thermodynamics is not concerned about......
(A) Energy changes involved in a chemical reation
(B) The extent to which a chemical reaction proceeds
(C) the rate at which a reaction proceeds
(D) the feasibility of a chemical reaction
MULTIPLE CORRECT ANSWER TYPE
Which of the following statements is correct ?
(A) The presence of reacting species in a covered beaker is an example of open system
(B) There is an exchange of energy as well as matter between the system and the surrounding in
a close system
(C) The presence of reactants in a closed vessel made up of copper is an example of a closed
system
(D) The presence of reactants in a thermos flask or any other closed insulated vessel is an example
of a isolated system
Which of the following is an extensive property ?
(A) Kinetic energy
(B) Potential energy
(C) Internal Energy
183
(D) Temperature
JEE-Chemistry
FLOT, DU & W CALCULATION
1.
SINGLE CORRECT ANSWER TYPE
In a closed insulated container a liquid is stirred with a paddle to increase the temperature only.
Which of the following is true?
(A) DE = W ¹ 0, q = 0
(B) DE = W = q ¹ 0
(C) DE = 0, W = q ¹ 0
(D) W = 0, DE = q ¹ 0
2.
The change in the internal energy for an isolated system at constant volume is
(A) DU ¹ 0
(B) DU = Dq + DW (C) DU = 0
(D) None of these
3.
A system is provided 50 J of heat and work done on the system is 10 J. The change in internal energy
during the process is :(A) 40 J
(B) 60 J
(C) 80 J
(D) 50 J
4.
An ideal gas expands against a constant external pressure of 2.0 atmosphere from 20 litre to
40 litre and absorb 10 kJ of heat from surrounding. What is the change in internal energy of the
system? (Given: 1 atm-litre = 101.3 J)
(A) 4052 J
(B) 5948 J
(C) 14052 J
(D) 9940 J
5.
A system undergoes a process in which DE = + 300 J while absorbing 400 J of heat energy and
undergoing an expansion against 0.5 bar. What is the change in the volume (in L)?
(A) 4
(B) 5
(C) 2
(D) 3
6.
One mole of an ideal gas at 25°C expands in volume from 1.0 L to 4.0 L at constant temperature.
What work (in J) is done if the gas expands against vacuum (Pexternal = 0)?
(A) –4.0 ´ 102
(B) –3.0 ´ 102
(C) –1.0 ´ 102
(D) zero
7.
At 25°C, a 0.01 mole sample of a gas is compressed from 4.0 L to 1.0 L at constant temperaure. What
is the work done for this process if the external pressure is 4.0 bar?
(A) 1.6 ´ 103 J
(B) 8.0 ´ 102 J
(C) 4.0 ´ 102 J
(D) 1.2 ´ 103 J
8.
What is the change in internal energy when a gas contracts from 377 mL to 177 mL under a constant
pressure of 1520 torr, while at the same time being cooled by removing 124 J heat?
(A) 40.52 J
(B) –83.48 J
(C) –248 J
(D) None of these
9.
A gas absorbs 200 J of heat and expands against the external pressure of 1.5 atm from a volume of 0.5
L to 1.0 L. Calculate the change in internal energy.
(A)120.025 J
(B) 115.025 J
(C) 135.025 J
(D) 124.025 J
10.
The temperature of 1 mole of an ideal gas is increased by 1°C at constant pressure. The work done is
(A) –R
(B) – 2R
(C) – R/2
(D) – 3R
11.
When freezing of a liquid takes place in a system
(A) may have q > 0 or q < 0 depending on the liquid
(B) is represented by q > 0
(C) is represented by q < 0
(D) has q = 0
184
Thermodynamics
12.
13.
Mechanical work is specially important in systems that contain
(A) gas-liquid
(B) liquid-liquid
(C) solid-solid
(D) amalgam
Calculate work done for an ideal gas in going from state A to state B (ln 2 = 0.7)
B
Patm
2
1
A
1/22.4
1/11.2
(1/V)L
(A) 15.68 L–atm
14.
15.
(B) 25.68 L–atm
(C) 30.68 L–atm
(D) 35.68 L–atm
20
(where P in atm and V in L). During
V
expansion from volume of 1 litre to 10 litre, the gas undergoes a change in internal energy of 400 J.
How much heat is absorbed by the gas during expansion?
(A) 46 J
(B) 4660 J
(C) 5065.8 J
(D) 4260 J
A gas expands against a variable pressure given by P =
A sample of an ideal gas is expanded 1 m3 to 3 m3 in a reversible process for which P = KV2, with
K = 6 bar/m6. Work done by the gas is
(A) 5200 kJ
(B) 15600 kJ
(C) 52 kJ
(D) 5267.6 kJ
185
JEE-Chemistry
CALCULATION OF DH, DU, Q & W
1.
SINGLE CORRECT ANSWER TYPE
A given mass of gas expands reversibly from the state A to the state B by three paths 1, 2 and 3 as
shown in the figure. If w1, w2 and w3 respectively be the work done by the gas along three paths then
P
A
3
12
B
V
(A) w1 > w2 > w3
2.
(B) w1 < w2 < w3
(C) w1 = w2 = w3
(D) w2 < w3 < w1
Which of the following expressions is true for an ideal gas?
æ ¶V ö
(A) çè
÷ =0
¶T ø P
æ ¶P ö
(B) ç ÷ = 0
è ¶T ø v
æ ¶U ö
(C) çè
÷ =0
¶V ø T
æ ¶U ö
(D) çè
÷ =0
¶T ø V
3.
Calculate the maximum work done when pressure on 10 g of hydrogen is reduced form 20 to 1 atm
at a constant temperature of 273 K. The gas behaves ideally.
(A) 6180 calories.
(B) 8180 calories.
(C) 7180 calories.
(D) 9180 calories.
4.
A liquid of volume of 100 L and at the external pressure of 10 atm is confined inside an adibatic bath.
external pressure of the liquid is suddenly increased to 100 atm and the liquid gets compressed by 1 L
against this pressure then find DH
(A) 6000 lit atm.
(B)2000 lit atm.
(C) 9000 lit atm.
(D) 1200 lit atm.
5.
For 1 mole of ideal gas. Calculate w = ?
44.8
V
22.4
273
(A) – 283 R
6.
(B) – 253 R
T
546
(C) – 263 R
(D) – 273 R
For 1 mole of monoatomic gas. Calculate DH.
4
Patm
3
300K
400K
T
(A) 250 R
(B) 240 R
(C) 230 R
186
(D) 220 R
Thermodynamics
7.
2 mole of an ideal gas at 27°C expands isothermally and reversibly from a volume of 4 litre to 40 litre.
The work done (in kJ) by the gas is
(A) w = – 28.72 kJ
(B) w = – 11.488 kJ (C) w = – 5.736 kJ
(D) – 4.988 kJ
8.
For two mole of an ideal gas
(A) CV – CP = R
(B) CP – CV = 2R
9.
(C) CP – CV = R
(D) CV – CP = 2R
A thermodynamic process is shown in the following figure. In the process AB, 600 J of heat is added to
the system and in BC, 200 J of heat is added to the system. The change in internal energy of the system
in the process AC would be given
PA = 3 × 104 Pa, VA = 2 × 10–3 m3,
PB = 8 × 104 Pa, VC = 5 × 10–3 m3
B
C
P
A
O
10.
V
(A) 560 J
(B) 800 J
(C) 600 J
(D) 640 J
Calculate the work performed when 2 moles of hydrogen expand isothermally and reversibly at
25ºC form 15 to 50 litres.
(A) –1236 calories
(B) –1436 calories
(C) –1036 calories
(D) –1536 calories
11.
5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against
a constant external pressure of 1 atm. wirr at 300 K is :
(A) –15.921 kJ
(B) –11.224 kJ
(C) –110.83 kJ
(D) None of these
12.
If a gas at a pressure of 10 atm at 300 K expands against a constant external pressure of 2 atm from a
vol. of 10 litres to 20 litres find work done ? [Isothermal process]
(A) –10 L atm
(B) –20 L atm
(C) –30 L atm
(D) –40 L atm
13.
During an expansion of ideal gas the work done by gas is 100 J and the heat capacity of process is
found to be + 2 J/ºC find DE of gas if the final temperature of gas is 25ºC higher than its initial
temperature.
(A) –40J
(B) –50J
(C) –70J
(D)–35J
14.
Calculate DE for the conversion of 1 mole of water into 1 mole of steam at a temperature of
100ºC and at a pressure of 1 atmosphere. Latent heat of vaporisation of water is 9720 cal/mole.
(A) 7979 calories
(B) 6979 calories.
(C) 5979 calories.
(D) 8979 calories.
15.
During an adiabatic process, the pressure of gas is found to be proportional to the cube of its absolute
temperature. The ratio of (Cp,m/Cv,m) for gas is
(A)
3
2
(B)
5
3
(C)
187
7
2
(D)
4
3
JEE-Chemistry
16.
If w1, w2, w3 and w4 for an ideal gas are magnitude of work done in isothermal, adiabatic, isobaric
and isochoric reversible expansion processes, the correct order will be
(A) w1 > w2 > w3 > w4 (B) w3 > w2 > w1 > w4 (C) w3 > w2 > w4 > w1 (D) w3 > w1 > w2 > w4
17.
In an adiabatic process, no transfer of heat takes place between system and surroundings.
Choose the correct option for free expansion of an ideal gas under adiabatic condition from
the following:
(A) q = 0, DT ¹ 0, W = 0
(B) q ¹ 0, DT = 0, W = 0
(C) q = 0, DT = 0, W = 0
(D) q = 0, DT < 0, W ¹ 0
18.
One mole of an ideal gas undergoes a change of state (2.0 atm, 3.0 L) to (2.0 atm, 7.0 L) with a
change in internal energy (DU) = 30 L-atm. The change in enthalpy (DH) of the process in
L-atm
(A) 22
(B) 38
(C) 25
(D) None of these
19.
The work done by the gas in reversible adiabatic expansion process is
(A)
20.
21.
P2 V2 - P1V1
g -1
(B)
nR (T1 - T2 )
g -1
(C)
P2 V2 - P1V1
g
(D) None of these
With what minimum pressure (in kPa), a given volume of an ideal gas (Cp,m = 7/2 R), originally at 400
K and 100 kPa pressure can be compressed irreversibly adiabatically in order to raise its temperature
to 600 K :
(A) 362.5 kPa
(B) 275 kPa
(C) 437.5 kPa
(D) 550 kPa
5 ö
æ
One mole of an ideal gas çè Cv,m = R÷ø at 300 K and 5 atm is expanded adiabatically to a final
2
external pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is
(A) 270 K
(B) 273 K
(C) 248.5 K
(D) 200 K
22.
10 litre of a non linear polyatomic ideal gas at 127°C and 2 atm pressure is suddenly released to 1 atm
pressure and the gas expanded adiabatically against constant external pressure, the final temperature
and volume of the gas respectively are.
(A) T = 350K; V = 17.5L
(B) T = 300K; V = 15L
(C) T = 250K; V = 12.5L
(D) None of these
23.
One mole of an ideal gas is expanded isothermally at 300 K from 10 atm to 1 atm. Calculate
work done under the following conditions.
(i)
Expansion is carried out reversibly.
(A) –595.9R
(B) –795.9R
(C) -690.9R
(D) –395.9R
Expansion is carried out irreversibly.
(A) –370R
(B) –770R
(C) –270R
(D) –570R
(ii)
188
Thermodynamics
24.
One mole of a non linear triatomic ideal gas is expanded adiabatically at 300 K from 16 atm to
1 atm.
(i)
Find the final temperature if expansion is carried out reversibly.
(A) 140K
(B) 150K
(C) 160K
(D) 120K
Calculate work done if expansion is carried out irreversibly.
(A) –220.93R
(B) –360.93R
(C) –450.93R
(D) –210.93R
A gas expands adiabatically & reversibly such that T µ V–1/2.
The value of g (Cp,m./Cv,m) of the gas will be
(A) 1.30
(B) 1.50
(C) 1.70
(D) 2
(ii)
25.
189
JEE-Chemistry
CYCLIC PROCESS & POLYTROPIC PROCESS
1.
SINGLE CORRECT ANSWER TYPE
Heat absorbed by a system in going through a cyclic process shown in figure is
V (in L)
30
10
30
10
P (in kPa)
(A) 107 p J
2.
(B) 106 p J
(C) 102 p J
(D) 104 p J
In the cyclic process shown in P-V diagram, the magnitude of the work done is
V2
V1
P2 P
P1
æ P2 - P1 ö
(A) p ç
è 2 ÷ø
3.
2
æ V2 - V1 ö
(B) p ç
è 2 ÷ø
2
(C)
p
(P2 - P1 ) (V2 - V1 ) (D) p (V2 – V1)2
4
An ideal gas is taken around the cycle ABCA as shown in P–V diagram. The magnitude of net work
done during the cycle is equal to
B
Pressure
6P1
P1
C
A
V1
Volume
(A) 12P1V1
4.
(B) 6P1V1
3V1
(C) 5P1V1
(D) P1V1
In diagram (1 to 4), variation of volume with changing pressure is shown. A gas is taken along the
path ABCDA. The change in internal energy of the gas will be
D
C
V
(1)
A
(1)
B
P
V
(2)
D
C
A
B
V
(3)
(2) P
(A) Positive in all the cases (1) to (4)
(B) Positive in cases (1), (2), (3) but zero in case (4)
(C) Negative in cases (1), (2), (3) but zero in case (4)
(D) Zero in all the cases
190
D
C
A
B
(3)
P
(4)
V D
C
A
B
(4)
P
Thermodynamics
5.
A cyclic process ABCD is shown in P-V diagram for an ideal gas. Which of the following diagram
represents the same process?
(A)
6.
(B)
(C)
For 1 mole of ideal monoatomic gas if
(D)
P
= constant and initial temperature is 100 K. If gas is
V2
expanded from 1 L to 2 L then :
(Assume R = 0.0821 Latm mol -1K -1 , 1 L atm = 24 cal)
(i) Heat capacity (in cal) is
(A)
11
3
(B)
11
6
(C)
(ii) The total heat absorbed (in cal) is
(A) 1966.66
(B) 2566.66
(C) 566.66
(iii) Approximate value of work done (in cal) is
(A) –460
(B) –650
(C) –378
7.
22
3
(D)
44
3
(D) 4566.66
(D) –540
1
mol of an ideal monatomic gas undergoes a reversible process for which PV2 = C. The gas is
22.4
expanded from initial volume of 1 L to final volume of 2 L starting from initial temperature of 273 K.
Find the heat exchanged during the process (in L atm).
R=
22.4
L atm mole–1 K–1.
273
(A) –0.50
(B) –0.75
(C) –0.10
191
(D) –0.25
JEE-Chemistry
SLOT
1.
2.
SINGLE CORRECT ANSWER TYPE
DS for the reaction; MgCO3(s) ¾® MgO(s) + CO2(g) will be :
(A) 0
(B) –ve
(C) +ve
Change in entropy is negative for :(A) Bromine (l ) ¾® Bromine (g)
(C) N2(g, 1 atm) ¾® N2 (g, 0.1 atm)
(D) ¥
(B) C(s) + H2O(g) ¾® CO(g) + H2(g)
(D) Fe(at 400 K) ¾® Fe(at 300 K)
3.
For which reaction from the following, D S will be maximum ?
(A) Ca(s) + 1/2 O2(g) ¾® CaO(s)
(B) CaCO3(s) ¾® CaO(s) + CO2(g)
(C) C(s) + O2(g) ¾® CO2 (g)
(D) N2(g) + O2(g) ¾® 2NO(g)
4.
In which reaction DS is positive :(A) H2O (l) ® H2O (s)
(C) H2O (l) ® H2O (g)
(B) 3O2 (g) ® 2O3 (g)
(D) N2(g) + 3H2(g) ® 2NH3 (g)
When two gases are mixed the entropy :–
(A) Remains constant (B) Decreases
(C) Increases
(D) Becomes zero
Unit of molar entropy is :(A) JK–1 mol–1
(B) J mol–1
(C) J–1K–1 mol–1
(D) JK mol–1
5.
6.
7.
8.
When you make ice cubes, the entropy of water
(A) Does not change
(B) Increases
(C) Decreases
(D) May either increase or decrease depending on the process used
5 ö
æ
When two mole of an ideal gas çè Cp,m = R÷ø heated from 300 K to 600 K at constant pressure.
2
The change in entropy of gas (DS) is :
(A)
9.
3
(B) - R ln 2
2
(C) 5R ln 2
(D)
5
R ln 2
2
(D)
DH + DG
T
The entropy change for a phase transformation is :
(A)
10.
3
R ln 2
2
DU
g + dT
(B)
DT
DH
(C)
DH
T
What is the melting point of benzene if DHfussion = 9.95kJ/mol and DSfusion = 35.7 J/K-mol?
(A) 278.7°C
(B) 278.7 K
(C) 300 K
(D) 298 K
192
Thermodynamics
11.
When one mole of an ideal gas is compressed to half of its initial volume and simultaneously heated
to twice its initial temperature, the change in entropy of gas (DS) is :
(A) Cp,m ln 2
(B) Cv,m ln 2
(C) R ln 2
(D) (Cv,m – R) ln 2
12.
What is the change in entropy when 2.5 mole of water is heated from 27°C to 87°C?
Assume that the heat capacity is constant? (Cp,m (H2O) = 4.2 J/K-mol ln (1.2) = 0.18)
(A) 16.6 J/K
(B) 9 J/K
(C) 34.02 J/K
(D) 1.89 J/K
13.
The entropy of vaporization of benzene is 85 JK–1 mol–1. When 117g benzene vaporize at it's normal
boiling point, the entropy change of surrounding is :
(A) –85 JK–1
(B) –85 ´ 1.5 JK–1
(C) 85 ´1.5 JK–1
(D) None of these
14.
One mole of an ideal gas expands isothermally and reversibly at 25ºC from a volume of 10 litres to
a volume of 20 litres.
What is the change in entrogy of the gas?
(A) 2.76 J/K.
(B) 3.76 J/K.
(C) 4.76 J/K.
(D) 5.76 J/K.
(i)
(ii)
How much work is done by the gas?
(A) 1851 J.
(B) 1718 J.
(iii) What is q ?
(A)1318 J.
(B) 1418 J.
(C) 2.78 J.
(D) 1518 J.
(C) 1718 J.
(D) 1518 J.
(iv) What is the change in the entropy of the surroundings?
(A) – 7.76 J/K.
(B) – 5.76 J/K.
(C) – 3.76 J/K.
193
(D) – 2.76 J/K.
JEE-Chemistry
GIBB’S FREE ENERGY
1.
SINGLE CORRECT ANSWER TYPE
Identify the correct statement regarding entropy
(A) At absolute zero temperature, the entropy of perfectly crystalline substances is +ve
(B) At absolute zero temperature entropy of perfectly crystalline substance is taken to be zero
(C) At 0°C the entropy of a perfectly crystalline substance is taken to be zero
(D) At absolute zero temperature, the entropy of all crystalline substances is taken to be zero
2.
For a process to be spontaneous at constant T and P :
(A) (DG)system, must be negative
(B) (DG)system must be positive
(C) (DS)system must be positive
(D) (DS)system must be negative
3.
For a reaction to occur spontaneously (A) D S must be negative
(C) (D H + T D S) must be negative
(B) (D H – TD S) must be negative
(D) D H must be negative
4.
Which of the following pairs of a chemical reaction is certain to result in a spontaneous reaction.?
(A) endothermic and decreasing disorder
(B) exothermic and increasing disorder
(C) endothermic and increasing disorder
(D) exothermic and decreasing disorder
5.
What is the sign of D G for the process of ice melting at 283 K ?
(A) D G > 0
(B) D G = 0
(C) D G < 0
(D) None of these
6.
Which of the following reaction is expected never to be spontaneous :–
(A) 2O3 ® 3O2
DH = – ve, DS = + ve
(B) Mg + H2 ® MgH2
DH = – ve, DS = – ve
(C) Br2(l) ® Br2(g)
DH = + ve, DS = + ve
(D) 2Ag + 3N2 ® 2AgN3
DH = + ve, DS = – ve
7.
Which of the following is true for the reaction H2O(l)
H2O(g) at 1000C and 1 atmosphere
(A) D S = 0
(B) D H = 0
(C) D H = D U
(D) D H = TD S
8.
For a perfectly crystalline solid Cp,m = aT3, where a is constant. If Cp,m is 0.42 J/K-mol at 10 K, molar
entropy at 20 K is :
(A) 0.42 J/K mol
(B) 0.14 J/K mol
(C) 1.12 J/K mol
(D) zero
9.
Consider the following spontaneous reaction 3X2(g) ® 2X3(g). What are the sign of DH, DS
and DG for the reaction?
(A) +ve, +ve, +ve (B) +ve, –ve, –ve
(C) –ve, +ve, –ve
(D) –ve, –ve, –ve
10.
For the reaction 2H(g) ® H2(g), the sign of DH and DS respectively are :
(A) +, –
(B) +, +
(C) –, +
(D) –, –
194
Thermodynamics
11.
12.
For a reaction to occur spontaneously :
(A) DS must be negative
(C) DH + TDS must be negative
(B) (–DH + T DS) must be positive
(D) DH must be negative
The free energy change DG = 0, when
(A) the system is at equilibrium
(C) reactants are initially mixed thoroughly
(B) catalyst is added
(D) the reactants are completely consumed
13.
Suppose that a reaction has DH = –40kJ and DS = –50 J/K. At what temperature range will it change
from spontaneous to non-spontaneous?
(A) 0.8 K to 1 K
(B) 799 K to 800 K (C) 800 K to 801 K (D) 799 K to 801 K
14.
18 gm of ice is converted into water at 0°C and 1 atm. The entropies of H2O(s) and H2O(l) are 38.2
and 60 J/mol-K respectively. The enthalpy change for this conversion is
(A) 5951.4 J/mol
(B) 595.14 J/mol
(C) –5951.4 J/mol (D) None of these
15.
At what temperature, will the following process would not be spontaneous ?
A(g) ¾¾® A (l)
DH = – 20 kJ
DS = – 50 J/K
(A) > 200 K
(B) > 300 K
(C) 350 K
(D) > 400 K
16.
Calculate standard entropy change in the reaction
Fe2O3(s) + 3H2(g) ® 2Fe(s) + 3H2O (l)
Given : S°m (Fe2O3, S) = 87.4, S°m (Fe, S) = 27.3
S°m (H2, g) = 130.7, S°m (H2O, l) = 69.9 JK–1 mol
(A) –212.5 JK–1 mol–1 (B) –215.2 JK–1 mol–1 (C) –120.9 JK–1 mol–1 (D) None of these
17.
18.
Calculate DG° (kJ/mol) at 127°C for a reaction with Kequilibrium = 105 :
(A) –38.294
(B) –16.628
(C) –9.16
(D) None of these
When reaction is carried out at standard states then at the equilibrium :
(A) DH° = 0
(B) DS° = 0
(C) equilibrium constant K = 0
(D) equilibrium constant K = 1
195
JEE-Chemistry
ANSWER KEY
BASIC DEFINITION
1.
7.
(D)
(C)
2.
8.
(D)
(C)(D)
3.
9.
(C)
4.
(A)(B)(C)
1.
7.
13.
(A)
(D)
(A)
2.
8.
14.
(C)
(B)
(C)
3.
9.
15.
(B)
(D)
(A)
4.
10.
1.
7.
13.
19.
24.
(B)
2.
(B)
8.
(B)
14.
(A)
20.
(i)-(B) ; (ii)-(D)
(C)
(B)
(D)
(B)
3.
9.
15.
21.
25.
(B)
(A)
(A)
(C)
(B)
4.
10.
16.
22.
1.
6.
(C)
2.
(C)
(i)-(A) ; (ii)-(B) ; (iii)-(A)
3.
7.
(C)
(D)
4.
1.
7.
13.
(C)
(C)
(B)
2.
8.
14.
(D)
3.
(B)
4.
(C)
(C)
9.
(C)
10. (B)
(i)-(D) ; (ii)-(B) ; (iii)-(C) ; (iv)-(B)
1.
7.
13.
(B)
(D)
(D)
2.
8.
14.
(A)
(C)
(A)
(B)
5.
(B)
6.
(D)
(C)
(C)
6.
12.
(D)
(A)
(D)
6.
(B)
12.
(C)
18.
(i)-(C) ; (ii)-(C)
(A)
(B)
(B)
FLOT, DU & W CALCULATION
(B)
(A)
5.
11.
CALCULATION OF DH, DU, Q & W
(C)
(B)
(D)
(A)
5.
11.
17.
23.
CYCLIC PROCESS & POLYTROPIC PROCESS
(D)
5.
(C)
5.
11.
(C)
(D)
6.
12.
(A)
(D)
5.
11.
17.
(C)
(B)
(A)
6.
12.
18.
(D)
(A)
(D)
SLOT
GIBB’S FREE ENERGY
3.
9.
15.
(B)
(D)
(D)
4.
10.
16.
196
(B)
(D)
(B)
Thermochemistry
THERMOCHEMISTRY
PROBLEMS RELATED WITH DU & DH
1.
2.
SINGLE CORRECT ANSWER TYPE
Enthalpy change during a reaction does not depend upon :
(A) Allotropic form of the element
(B) Temperature
(C) Physical state of reactants and products
(D) Number of steps in the reaction
D H for transition of carbon in the diamond form to carbon in the graphite form is – 453.5 cal. This
suggests that :
(A) Graphite is chemically different from
(C) Graphite is more stable than diamond
(B) Graphite is as stable as diamond diamond
(D) Diamond is more stable than graphite
3.
For the reactions,
(i) H2(g) + Cl2(g) ¾® 2HCl(g) + xKJ
(ii) H2(g) + Cl2(g) ¾® 2HCl(l) + yKJ
Which one of the following statement is correct :
(A) x > y
(B) x < y
(C) x = y
(D) More data required
4.
1150 kcal heat is released when following reaction is carried out at constant volume 27°C
C7H16(l) + 11O2(g) ® 7CO2(g) + 8H2O(l)
Find the heat change at const. pressure :
DH = DU + DngRT
(A) –1052.4 KCal
(B) –1232.4 KCal
(C) –1062.4 KCal
(D) –1152.4 KCal
5.
For the reaction : PCl5(g) ® PCl3(g) + Cl2(g):
(A) DH = DE
(B) DH > DE
(C) DH < DE
(D) None of the above
6.
Consider the reaction at 300 K
H2(g) + Cl2(g) ® 2HCl(g); DH° = –185 kJ mol–1
If 2 mole of H2 completely react with 2 mole of Cl2 to form HCl. What is DU° for this reaction?
(A) 0
(B) –185 J
(C) 370 kJ
(D) None of these
7.
Which of the indicated relationship is correct for the following exothermic reaction carried out at
constant pressure?
CO(g) + 3H2(g) ® CH4(g) + H2O(g)
(A) DE = DH
(B) DE > DH
(C) w < 0
(D) q > 0
8.
Consider the reaction at 300 K
15
O (g) ® 6CO2(g) + 3H2O(l); DH = –3271 kJ mol–1
2 2
What is DU for the combustion of 1.5 mole of benzene at 27°C?
(A) –3267.25 kJ
(B) –4900.88 kJ
(C) –4906.5 kJ
(D) –3274.75 kJ
C6H6(l) +
9.
At 5 ´ 105 bar pressure density of diamond and graphite are 3 g/cc and 2 g/cc respectively, at certain
temperature ‘T’. Find the value of DU – DH for the conversion of 1 mole of graphite to 1 mole of
diamond at temperature ‘T’:
(A) 100 kJ/mol
(B) 50 kJ/mol
(C) –100 kJ/mol
(D) None of these
197
JEE-Chemistry
ENTHALPY OF FORMATION & COMBUSTION
SINGLE CORRECT ANSWER TYPE
1.
Which of the following value of DH °f represent that the product is least stable ?
(A) –94.0 kcal mol–1 (B) –231.6 kcal mol–1 (C) + 21.4 kcal mol–1 (D) +64.8 kcal mol–1
2.
Given :
C(diamond) + O2 ® CO2 ; DH = –395 kJ mol–1
C(graphite) + O2 ® CO2 ; DH = –393 kJ mol–1
The enthalpy of formation of diamond from graphite is
(A) +2.0 kJ
(B) –1.5 kJ
(C) –788 kJ
(D) 788 kJ
3.
Which of the following equations represents a reaction that provides the enthalpy of formation of
CH3Cl?
(A) C(s) + HCl(g) + H2(g) ® CH3Cl (g)
(B) C(s) + 3H(g) + Cl(g) ® CH3Cl(g)
(C) C(s) + 3/2H2(g) + l/2Cl2(g) ® CH3Cl(g) (D) CH4(g) + Cl2(g) ® CH3Cl(g) + HCl(g)
4.
Use the given standard enthalpies of formation (in kJ/mol) to determine the enthalpy of reaction of the
following reaction :
NH3(g) + 3F2(g) ® NF3(g) + 3HF(g)
DH °f (NH3, g) = –46.2 kJ mol–1;
DH °f (NF3, g) = –113.0 kJ mol–1;
DH °f (HF, g) = –269.0 kJ mol–1
(A) –335.8 kJ/mol
(B) –873.8 kJ/mol
(C) –697.2 kJ/mol
(D) –890.4 kJ/mol
5.
The standard enthalpy of formation of octane (C8H18) is –250 kJ/mol. Calculate the enthalpy of
combustion of C8H18 . The enthalpy of formation of CO2(g) and H2O(l) are –394 kJ/mol and
–286 kJ/mol respectively:
(A) –5200 kJ/mol
(B) –5726 kJ/mol
(C) –5476 kJ/mol
(D) –5310 kJ/mol
6.
Determine the enthalpy of formation of B2H6(g) in kJ/mol of the following reaction :
B2H6(g) + 3O2(g) ® B2O3(s) + 3H2O(g);
Given : D r H° = –1941 kJ/mol; DH °f (B2O3, s) = –1273 kJ/mol;
DH °f (H2O, g) = –241.8 kJ/mol
(A) –75.6
7.
(B) +75.6
(C) –57.4
(D) –28.4
Consider the following reactions :
C(s) + O2(g) ® CO2(g) + x kJ
CO(g) +
1
O (g) ® CO2(g) + y kJ
2 2
The heat of formation of CO(g) is :
(A) –(x + y) kJ/mol (B) (x – y) kJ/mol
(C) (y – x) kJ/mol
198
(D) None of these
Thermochemistry
8.
What amount of energy (kJ) is released in the combustion of 5.8 g of C4H10(g)?
2C4H10(g) + 13O2(g) ® 8CO2(g) + 10H2O(l); DH° = –756kJ mol–1
(A) 575.6
(B) 37.8
(C) 182
(D) 57.56
9.
Calculate heat of the following reaction at constant pressure,
F2O(g) + H2O(g) ® O2 (g) + 2HF(g)
The heats of formation of F2O (g), H2O(g) and HF (g) are 5.5 kcal mol–1, –57kcal mol–1 and –64 kcal
mol–1 respectively.
(A) – 76.5 kcal mol–1 (B) – 78.5 kcal mol–1 (C) – 86.5 kcal mol–1 (D) – 77.9 kcal mol–1
10.
Calculate the enthalpy change of the following reaction
3C2H2(g) ¾¾® C6H6(g)
Given Enthalpy of combustion of C2H2(g) = – 1.30 kJ mol–1 and that of C6H6(g) = – 3.30 kJ
mol–1
(A) –0.60 kJ/mol
(B) –0.70 kJ/mol
(C) –0.80 kJ/mol
(D) –0.90 kJ/mol
11.
A gas mixture of 3.67 litres (at 1 atm) of ethylene and methane on complete combustion at 25ºC
produces 6.11 litres of CO2 (at 1 atm). Find out the amount of heat evolved on burning this gas
mixture. The heats of combustion of ethylene and methane are – 1423 and –891 kJ mol-1 at 25ºC.
(A) 182.85 KJ
(B) 186.85 KJ
(C) 196.85 KJ
(D) 166.80 kJ
199
JEE-Chemistry
BOND ENTHALPY
1.
SINGLE CORRECT ANSWER TYPE
The entropies of H2(g) and H(g) are 130.6 and 114.6 J mol–1 K–1 respectively at 298 K. Using the
data given below calculate the bond energy of H2 (in kJ/mol) :
H2(g) ® 2H(g); DG° = 406.6 kJ mol–1
(A) 377.2
(B) 436.0
(C) 425.5
(D) 430.5
2.
The enthalpy change for the following reaction is 368 kJ. Calculate the average O—F bond energy.
OF2(g) ® O(g) + 2F(g)
(A) 184 kJ/mol
(B) 368 kJ/mol
(C) 536 kJ/mol
(D) 736 kJ/mol
3.
Calculate P—Cl bond enthalpy
Given : D f H (PCl3, g) = 306 kJ/mol;
DHatomization(P, s) = 314 kJ/mol;
D f H (Cl, g) = 121kJ/mol
(A) 123.66 kJ/mol
(B) 371 kJ/mol
(C) 19 kJ/mol
(D) None of these
4.
Calculate the enthalpy for the following reaction using the given bond energies (kJ/mol)
(C—H = 414; H—O = 463; H — Cl = 431, C — Cl = 326; C — O = 335)
CH3—OH(g) + HCl(g) ® CH3 — Cl(g) + H2O(g)
(A) –23kJ/mol
(B) –42 kJ/mol
(C) –59kJ/mol
(D) –511kJ/mol
5.
Based on the values of B.E. given, D f H° of N2H4(g) is :
Given : N – N = 159 kJ mol–1; H–H = 436 kJ mol–1
N º N = 941 kJ mol–1; N – H = 398 kJ mol–1
(A) 711 kJ mol–1 (B) 62 kJ mol–1
(C) –98 kJ mol–1
6.
7.
Find the bond enthalpy of S – S bond from the following data :
DfH° of C2H5 – S – C2H5(g) = – 147.23 kJ mol–1
DfH° of C2H5 – S – S – C2H5(g) = –201.92 kJ mol–1
DfH° of S(g) = 222.80 kJ mol–1
(A) 277.49 kJ mol–1
(B) 288.49 kJ mol–1
(C) 299.49 kJ mol–1
(D) –711 kJ mol–1
(D) 177.49 kJ mol–1
Using the bond enthalpy data given below, calculate the enthalpy change for the reaction
C2H4(g) + H2(g) ¾¾® C2H6(g)
Data :
Bond
C–C
C=C
C–H
H–H
(A) –120.08 kJ mol–1
Bond enthalpy
336.81 kJ mol–1
606.68 kJ mol–1
410.87 kJ mol–1
431.79 kJ mol–1
(B) –130.08 kJ mol–1
(C) –150.08 kJ mol–1
200
(D) –160.08 kJ mol–1
Thermochemistry
OTHER TYPE OF ENTHALPY REACTION
1.
2.
SINGLE CORRECT ANSWER TYPE
Hess's law states that :
(A) the standard enthalpy of an overall reaction is the sum of the enthalpy changes in individual
reactions.
(B) enthalpy of formation of a compound is same as the enthalpy of decomposition of the compound
into constituent elements, but with opposite sign.
(C) at constant temperature the pressure of a gas is inversely proportional to its volume
(D) the mass of a gas dissolved per litre of a solvent is proportional to the pressure of the gas in
equilibrium with the solution
An imaginary reaction X ® Y takes place in three steps
X ® A, DH = –q1;
B ® A, DH = –q2;
B ® Y, DH = –q3
If Hess’s law is applicable, then the heat of the reaction (X ® Y) is :
(A) q1 – q2 + q3
(B) q2 – q3 – q1
(C) ql – q2 – q3
(D) q3 – q2 – q1
3.
The enthalpy change for a reaction does not depend upon :
(A) the physical states of reactants and products
(B) use of different reactants for the same product
(C) the number of intermediate reaction steps
(D) the differences in initial or final temperatures of involved substances
4.
Calculate the standard enthalpy of reaction for the following reaction using the listed
enthalpies of reaction :
3Co(s) + 2O2(g) ® Co3O4(s)
2Co(s) + O2(g) ® 2CoO(s); DH1° = –475.8 kJ mol–1
(A) –891.2 kJ
5.
6CoO(s) + O2(g) ® 2Co3O4(s); DH °2 = –355.0 kJ mol–1
(B) –120.8 kJ
(C) +891.2 kJ
(D) –830.8 kJ
From given following equations and DH°values, determine the enthalpy of reaction at 298 K for the
reaction :
C2H4(g) + 6F2(g) ® 2CF4(g) + 4HF(g)
H2(s) + F2(g) ® 2HF(g); DH1° = –537 kJ mol–1
C(s) + 2F2(g) ® CF4(g) ; DH °2 = –680 kJ mol–1
2C(s) + 2H2(g) ® C2H4(g); DH °3 = 52 kJ mol–1
(A) –1165
(B) –2486
(C) +1165
(D) +2486
6.
If D f H° (C2H4) and D f H° (C2H6) are x1 and x2 kcal mol–1, the heat of hydrogenation of C2H4 is
(A) xl + x2
(B) x1 – x2
(C) x2 – x1
(D) xl + 2x2
7.
Heat of combustion of ethanol at constant pressure and at temperature T K is found to be
–q J mol–1 . Hence, heat of combustion (in J mol–1) of ethanol at the same temperature at
constant volume will be :
(A) RT – q
(B) –(q + RT)
(C) q – RT
(D) q + RT
201
JEE-Chemistry
8.
If the enthalpy of formation and enthalpy of solution of HCl(g) are –92.3 kJ/mol and
–75.14 kJ/mol respectively then find enthalpy of formation of Cl–(aq):
(A) –17.16 kJ/mol
(B) –167.44 kJ/mol
(C) 17.16 kJ/mol
(D) None of these
9.
At 25°C, 1 mole of MgSO4 was dissolved in water, the heat evolved was found to be 91.2 kJ. One
mole of MgSO 4 . 7H 2O on dissolution gives a solution of the same composion
accompanied by an absorption of 13.8 kJ, The enthalpy of hydration, i.e., DH for the reaction
MgSO4(s) + 7H2O(l) ® MgSO4 . 7H2O(s) is:
(A) –105 kJ/mol
(B) –77.4 kJ/mol
(C) 105 kJ/mol
(D) None of these
10.
The magnitude of heat of solution ..... on addition of solvent to solution
(A) Decreases
(B) Increases
(C) Remains constant (D) Increases or decreases
11.
Enthalpy of neutralization of HCl by NaOH is –57.1 kJ/mol and by NH4OH is –51.1 kJ/mol. Calculate
the enthalpy of dissociation of NH4OH.
(A) 6.0 kJ/mol
(B) 7.0 kJ/mol
(C) 8.0 kJ/mol
(D) 9.0 kJ/mol
12
The enthalpy of formation of H2O(l) is –285.83 kJ mol–1 and enthalpy of neutralization of a strong
acid and a strong base is –55.84 kJ mol–1. What is the enthalpy of formation of OH¯ ions ?
(A) –229.99 kJ mol–1 (B) –339.99 kJ mol–1 (C) –449.99 kJ mol–1 (D) –338.99 kJ mol–1
13.
Calculate DH° for the reaction
Ag+(aq) + Cl¯(aq) ¾¾® AgCl(s)
at 25°C. Given DfH° (Ag+, aq) = 105.58 kJ mol–1, DfH° (Cl°, aq) = –167.16 kJ mol–1
and DfH°(AgCl, s) = – 127.07 kJ mol–1
(A) –65.49 kJ mol–1
(B) –60.49 kJ mol–1
(C) –50.49 kJ mol–1
(D) –70.49 kJ mol–1
14.
Calculate the enthalpy change when one mole of HCl(g) is dissolved in a very large amount of water
at 25°C. The change in state is HCl(g) + aq ¾¾® H+(aq) + Cl¯(aq)
Given : DfH (HCl, g) = – 92.31 kJ mol–1 and DfH° (Cl¯, aq) = – 167.16 kJ mol–1
(A) – 74.85 kJ mol–1 (B) – 80.85 kJ mol–1 (C) – 70.85 kJ mol–1 (D) – 66.85 kJ mol–1
15.
Calculate the resonance energy of N2O from the following data :
DHfº of N2O = 82 kJ mol-1 . Bond energy of N º N, N = N, O = O & N = O bonds is 946, 418,
498 & 607 kJ mol-1 respectively .
(A) – 88 kJ mol–1
(B) – 78 kJ mol–1
(C) 98 kJ mol–1
(D) – 108 kJ mol–1
16.
The standard molar enthalpies of formation of cyclohexane (l) & benzene (l) at 25°C are
-156 & + 49 kJ/mol respectively . The standard enthalpy of hydrogenation of cyclohexene(l) at 25º
is - 119 kJ mol-1. Use these data to estimate the magnitude of the resonance energy of
benzene.
(A) 200 kJ mol-1
(B) 152 kJ mol-1
(C) 100 kJ mol-1
(D) 211 kJ mol-1
17.
The enthalpy of formation of ethane, ethylene and benzene from the gaseous atoms are –2839.2,
–2275.2 and –5506 kJmol–1 respectively. Calculate the resonance energy of benzene. The bond
enthalpy of C–H bond is given as equal to + 410.87 kJ/mol.
(A) – 80.68 kJ/mol
(B) – 23.68 kJ/mol
(C) –96.68 kJ/mol
(D) – 46.68 kJ/mol
202
Thermochemistry
18.
Calculate the enthalpy of combustion of methyl alcohol at 298 K from the following data
Bond
C-H
C-O
O-H
O=O
C=O
Bond Enthalpy(kJ mol-1) 414
351.5
464.5
494
711
-1
Resonance energy of CO2 = - 143 kJ mol
Latent heat of vaporisation of methyl alcohol = 35.5 kJ mol-1.
Latent heat of vaporisation of water = 40.6 kJ mol-1.
(A) – 669.7 kJ mol-1 (B) – 329.7 kJ mol-1
(C) – 69.7 kJ mol-1
(D) – 889.7 kJ mol-1
19.
Set up a Born-Haber cycle to find the lattice energy of NaCl crystal. Given DHf° (NaCl) = –410 kJ
mol–1 . Ionization enthalpy of Na = 495 kJ mol–1 , electron affinity of chlorine = 365 kJ mol–1 ,
sublimation enthalpy of Na = 315 kJ mol–1 and dissociation enthalpy of Cl2(g) = 240 kJ mol–1 .
(A) –975 kJ/mol
(B) –860 kJ/mol
(C) –750 kJ/mol
(D) –675 kJ//mol
20.
Enthalpy of neutralization of HCl by NaOH is –55.84 kJ/mol and by NH4OH is –51.34 kJ/mol. The
enthalpy of ionization of NH4OH is :
(A) 107.18 kJ/mol
(B) 4.5 kJ/mol
(C) –4.5 kJ/mol
(D) None of these
COMPREHENSION TYPE
Paragraph for question no 21 to 23
Enthalpy of neutralization is defined as the enthalpy change when 1 mole of acid/base is
completely neutralized by base/acid in dilute solution.
For strong acid and strong base neutralization net chemical change is
H+ (aq) + OH–(aq) ® H2O(l); DrH° = –55.84 kJ/mol
DH°ionization of aqueous solution of strong acid and strong base is zero.
When a dilute solution of a weak acid or base is neutralized, the enthalpy of neutralization is some
what less because of the absorption of heat in the ionization of the weak acid or base, for weak acid/
base
DH °neutralization = DH °ionization + D r H° (H + + OH - ® H 2 O)
21.
If enthalpy of neutralization of CH 3COOH by NaOH is –49.86 kJ/mol then enthalpy of
ionization of CH3COOH is :
(A) 5.98 kJ/mol
(B) –5.98 kJ/mol
(C) 105.7 kJ/mol
(D) None of these
22.
What is DH° for complete neutralization of strong diacidic base A(OH)2 by HNO3?
(A) –55.84 kJ
(B) –111.68 kJ
(C) 55.84 kJ/mol
(D) None of these
23.
Under the same conditions how many mL of 0.1 M NaOH and 0.05 M H2A (strong diprotic acid)
solution should be mixed for a total volume of 100 mL produce the highest rise in
temperature :
(A) 25 : 75
(B) 50 : 50
(C) 75 : 25
(D) 66.66 : 33.33
203
JEE-Chemistry
CALORIMETRY
1.
SINGLE CORRECT ANSWER TYPE
1.0 g of a sample of graphite was burnt in a bomb calorimeter in excess of oxygen at 298 K and 1 atm
pressure according to equation C(graphite) +O2(g) ® CO2(g). When it was completely burnt, the
temperature rose to 299 K. If heat capacity of bomb calorimeter and its contents is 20.7 kJ K–1. What
is the enthalpy change for the above reaction ?
(A) – 248.4 kJ mol–1 (B) – 348.4 kJ mol–1 (C) – 148.4 kJ mol–1 (D) – 448.4 kJ mol–1
2.
A 0.05 L, sample of 0.2 M aqueous hydrochloric acid is added to 0.05 L of 0.2 M aqueous ammonia
in a calorimeter. Heat capacity of entire calorimeter system is 480 J/K. The temperature increase is
1.09 K. Calculate DrH° in kJ/mol for the following reaction :
HCl(aq.) + NH3(aq.) ® NH4Cl(aq.)
(A) –52.32
(B) –61.1
(C) –55.8
(D) –58.2
3.
A coffee cup calorimeter initially contains 125 g of water, at a temperature of 24.2°C. 8 g ammonium
nitrate (NH4NO3), also at 24.2°C, is added to the water and the final temperature is 18.2°C. What is
the heat of solution of ammonium nitrate in kJ/mol? The specific capacity of the solution is 4.2 J/°C g.
(A) 33.51 kJ/mol
(B) 39.5 kJ/mol
(C) 32.2 kJ/mol
(D) 37.3 kJ/mol
204
Thermochemistry
ANSWER KEY
PROBLEMS RELATED WITH DU & DH
1.
(D)
2.
(C)
3.
(B)
7.
(B)
8.
(B)
9.
(A)
4.
(D)
5.
(B)
6.
(D)
6.
(C)
6.
(A)
ENTHALPY OF FORMATION & COMBUSTION
1.
(D)
2.
(A)
3.
(C)
4.
(B)
5.
(C)
7.
(C)
8.
(B)
9.
(A)
10.
(A)
11.
(B)
5.
(B)
BOND ENTHALPY
1.
(B)
7.
(A)
2.
(A)
3.
(A)
4.
(A)
OTHER TYPE OF ENTHALPY REACTION
1.
(A)
2.
(B)
3.
(C)
4.
(A)
5.
(B)
6.
(C)
7.
(A)
8.
(B)
9.
(A)
10.
(C)
11.
(A)
12
(A)
13.
(A)
14.
(A)
15.
(A)
16.
(B)
17.
(B)
18.
(A)
19.
(A)
20.
(B)
21.
(A)
22.
(B)
23.
(B)
CALORIMETRY
1.
(A)
2.
(A)
3.
(A)
205
JEE-Chemistry
Important Notes
206
Chemical Equilibrium
CHEMICAL EQUILIBRIUM
CHARACTERISTIC OF CHEMICAL EQUILIBRIUM
1.
SINGLE CORRECT ANSWER TYPE
The reaction : 3Fe(s) + 4H2O(g)
Fe3O4(s) + 4H2(g), is reversible if it is carried out
(A) at constant pressure
(B) at constant temperature
(C) in an open vessel
(D) in a closed vessel.
2.
Which of the following is a characteristic of a reversible reaction ?
(A) It never proceeds to completion.
(B) It can be completed in finite time.
(C) It proceeds only in the forward direction.
(D) Number of moles of reactants and products are equal.
3.
Which of the following statement is false in case of equilibrium state –
(A) There is no apparent change in measurable properties with time.
(B) It is dynamic in nature.
(C) It can be attained from either side of the reaction.
(D) It can be attained from the side of reactants only.
4.
A chemical reaction is in equilibrium when
(A) Formation of product is minimum
(B) Reactants are completely transformed into products
(C) Rates of forward and backward reactions are equal
(D) Equal amounts of reactants and products are present.
5.
The state of chemical equilibrium of a reversible reaction is not influenced by
(A) pressure
(B) catalyst
(C) concentration of the reactants
(D) temperature.
6.
For the reaction : R ƒ P, Variation of concentration is plotted against time :
P
Concentration III
II I
R
Time ®
Which of the following regions show(s) state of equilibrium ?
(A) III
(B) II
(C) I
207
(D) both II and III
JEE-Chemistry
7.
Which of the following represents the rate of forward reaction (rf) and rate of backward reaction (rb)
at equilibrium ?
(A) Rate of
reaction
rf
(B) Rate of
Time
Rate of
(C) reaction
rb
rf
reaction
rb
Time
rb
Rate of
(D) reaction
rf
rf
rb
Time
Time
In case of gaseous homogeneous reaction, the active mass of the reactant is obtained by the expression
(A)
(B)
P
RT
(C)
RT
P
(A)
H2
N2
NH3
(B)
n
RT .
V
2NH3 in the Haber process, the attain-
H2
N2
NH3
Time
NH3
H2
(D)
N2
Molar
concentration
Time
(C)
(D)
Molar
concentration
For the synthesis of ammonia by the reaction N2 + 3H2
ment of equilibrium is correctly predicted by the curve
Molar
concentration
9.
PV
RT
Molar
concentration
8.
NH3
N2
H2
Time
Time
208
Chemical Equilibrium
PROBLEMS BASED UPON EQUILIBRIUM CONSTANT
1.
2.
SINGLE CORRECT ANSWER TYPE
ˆˆ† 2NH , the value of K does not depends upon :For a reaction : N2 + 3H2 ‡ˆˆ
3
C
(a) Initial concentration of the reactants
(b) Pressure
(c) Temperature
(d) Catalyst
(A) Only c
(B) a, b, c
(C) a, b, d
(D) a, b, c, d
Equilibrium constant for the reaction : 2NO(g) + Cl 2(g)
expression
(A) K =
[2NOCl]
[2NO][Cl 2 ]
(B) K =
[NOCl]2
[NO]2 [Cl 2 ]
(C) K =
2NOCl(g), is correctly given by
[NO]2 [Cl2 ]2
[NO]2 + [Cl2 ]
(D) K =
[NO]2 + [Cl]2
[NOCl]
3.
The unit of equilibrium constant for the reversible reaction : H2 + I2
(A) mol-4 litre
(B) mol-2 litre
(C) mol litre-1
4.
For a reaction : H2(g) + I2(g)
2HI(g), at 721 K, the value of equilibrium constant is 50. If 0.5
moles each of H2 and I2 is added to the system the value of equilibrium constant at same temperature
will be
(A) 0.02
(B) 0.2
(C) 50
(D) 25.
5.
ˆˆ† 2CO(g), the partial pressure of CO and CO are 2.0 and
For the reaction : C(s) + CO2(g) ‡ˆˆ
2
4.0 atm. respectively at equilibrium. The KP for the reaction is (A) 0.5
(B) 4.0
(C) 8.0
(D) 1
6.
ˆˆˆ
†
In a chemical equilibrium for the reaction : A + B ‡ˆˆ
ˆ C + D, when one mole each of the reactants
are mixed, 0.4 mole each of the products are formed. The equilibrium constant is :(A) 1
(B) 0.36
(C) 2.25
(D) 0.44
7.
Match List –I (hypothetical reactions) with List–II (ratio
correct answer using the code given below :ˆˆˆ
†
(a) A2(g) + 3B2(g) ‡ˆˆ
ˆ 2AB3(g)
ˆˆˆ
†
(b) A2(g) + B2(g) ‡ˆˆ
ˆ 2AB(g)
ˆˆˆ
†
(c) A(s) + 1.5 B2(g) ‡ˆˆ
ˆ AB3(g)
ˆˆˆ
†
(d) AB2(g) ‡ˆˆˆ AB(g) + 0.5 B2(g)
Codes :
(a)
(b)
(c)
(d)
(A)
(i)
(ii)
(iii)
(iv)
(B)
(ii)
(i)
(iv)
(iii)
(C)
(i)
(iv)
(iii)
(ii)
(D)
(i)
(ii)
(iv)
(iii)
KP
for the given reactions) and select the
KC
(i) (RT)–2
(ii) (RT)0
(iii) (RT)1/2
(iv) (RT)–1/2
209
2HI, is
(D) unit less
JEE-Chemistry
8.
In a reversible reaction : A
B, If the initial concentrations of A and B are a and b (in mole per
litre )and the equilibrium concentrations are ( a - x) and (b + x) respectively; express 'x' in terms of k1,
k2, a and b.
k1a - k 2b
(A) k +k
1 2
k1a - k 2b
(B) k -k
1 2
(C)
k1a - k 2b
k1k 2
k1a + k 2b
(D) k +k
1 2
9.
3.1 moles of FeCl3 and 3.2 moles of NH4SCN are added to one litre of water. At equilibrium
3.0 moles of FeSCN2+ are formed. The equilibrium constant KC of the reacion
2+
ˆˆˆ
†
Fe3+(aq) + SCN–(aq) ‡ˆˆ
ˆ FeSCN (aq) will be :
(A) 6.66 ´ 10–3
(B) 0.30
(C) 3.30
(D) 150
10.
ˆˆˆ
†
X2(g) + Y2(g) ‡ˆˆ
ˆ 2XY(g) reaction was studied at a certain temperature. In the beginning 1 mole of
X2 was taken in a one litre flask and 2 moles of Y2 was taken in another 2 litre flask, after joining what
is the equilibrium concentration of X2 and Y2 ?
(Given : Equilibrium concentration of [XY] = 0.6 mol/L).
æ1
ö æ2
ö
æ1
ö æ2
ö
(A) ç - 0.3 ÷ , ç - 0.3 ÷
(B) ç - 0.6 ÷ , ç - 0.6 ÷
è3
ø è3
ø
è3
ø è3
ø
(C) (1 – 0.3), (2 – 0.3)
11.
(D) (1 – 0.6), (2 – 0.6)
20.0 grams of CaCO3(s) were placed in a closed vessel, heated & maintained at 727º C under
ˆˆ† CaO(s) + CO2(g) and it is found that 75 % of CaCO3 was decomposed.
equilibrium CaCO3(s) ‡ˆˆ
What is the value of Kp ? The volume of the container was 15 litres.
(A) 0.182
(B) 0.821
(C) 0.524
(D) 0.245
12.
The reaction : A(g) + B(g)
C(g) + D(g), is studied in a one litre vessel at 250°C. The initial
concentration of A was 3n and that of B was n. When equilibrium was attained, equilibrium
concentration of C was found to the equal to the equilibrium concentration of B. What is the
concentration of D at equilibrium?
(A) n/2
(B) (3n – n/2)
(C) (n – n/3)
(D) n
[ NO2 ]
N 2 O4 (g) ƒ 2NO 2 (g) is K =
[ N2O4 ]
2
13.
The equilibrium constant for the following reaction :
Which of the following graphs is correct ?
(A) [NO ]
2
(B)
[N2O4]
(C)
[NO2]
(D)
[NO2]
[N2O4]
[N2O4]
210
[NO2]
[N2O4]
Chemical Equilibrium
14.
For a reaction : 2A(g) + B(g) ƒ C(g) + D(g), the value of K p will be :
(A) K p =
nCn D V
n 2A n B RT 2
(B) K p =
n Cn D P
n 2A n B RT
(C) K p =
n C n D RT 2
n 2A n B V
(D) K p =
n Cn D V
n 2A n B RT
15.
The equilibrium constant for a reaction : N2(g) + O2(g)
2 NO(g), is 4 x 10-4 at 2000 K. In the
presence of catalyst, the equilibrium constant is attained 10 times faster. The equilibrium constant in
the presence of catalyst,
(A) 40 × 10-4
(B) 4 × 10-4
(C) 4 × 10-2
(D) Insufficent data.
16.
Calculate the partial pressure (in atm) of carbon mono-oxide from the following data :
CaCO3(s)
(A) 0.2
CaO(s) + CO2
(B) 0.4
; Kp = 8 x 10-2 & CO2(g) + C(s)
(C) 1.6
211
2CO(g) ; Kp = 2
(D) 4.
JEE-Chemistry
REACTION QUOTIENT &APPLICATION OF EQUILIBRIUM
CONSTANT
1.
SINGLE CORRECT ANSWER TYPE
Which of the following is favours of forward reaction :–
(A) Q = Kc
(B) Q > Kc
(C) Q < Kc
(D) None
2.
Kc for a reaction : A(g) + B(g)
C(g) + D(g), is 10 at 25ºC. If a container contains 1,
2, 3, 4 mol per litre of A, B, C and D respectively at 25ºC, the reaction shall :
(A) proceed from left to right
(B) proceed from right to left
(C) be at equilibrium
(D) none of these
3.
In which of the following cases, the reaction goes farthest to completion
(A) K = 103
(B) K = 10–2
(C) K = 10
(D) K = 100.
4.
Some gaseous equilibria have following relation in equilibrium constants
K
K
K
CO + H2O ‡ˆˆ
ˆˆˆ
†
ˆˆˆ
†
ˆˆˆ
†
ˆ CO2 + H2 ; CO + O2 ‡ˆˆ
ˆ CO2 ; H2 + O2 ‡ˆˆ
ˆ H2O
1
(A) K = K1K2
5.
2
(B) K = (K1K2)2
AO
1
1
A2 +
O ; K = 5 × 105
2
2 2
BO
1
1
B2 +
O ; K = 1.10 × 1012
2
2 2
CO
1
1
C2 +
O ; K = 2.3 × 1018
2
2 2
DO
1
1
D2 +
O ; K = 1.4 × 1021
2
2 2
which oxide is most stable?
(A) AO
(B) BO
(C) K = (K1K2)–1/2
(D) K = K1/ K2
(C) CO
(D) DO
6.
B, B
C, C
D, equilibrium constants are K1, K2 and K3
For reactions : A
respectively. What is the value of equilibrium constant for A
D :
(A) K1 + K2 + K3 (B) K1 × K2 × K3 (C) K1K2/K3
(D) K1/K2K3
7.
For the following isomerisation reaction :
Cyclohexane ƒ hexane-1-ene, K = 1.732
A
P(hexane-1-ene)
60°
Pcyclohexene
Which of the following statements holds good at point 'A' ?
(A) Q > K
(B) Q < K
(C) Q = K= 1
212
(D) Q = K= 1.732
Chemical Equilibrium
8.
2 mole each of SO3, CO, SO2 and CO2 is taken in a one litre vessel. If Kc for the raction :
SO3(g) + CO(g)
SO2(g) + CO2(g) is 1/9 then
(A) Total number of moles at equilibrium are less than 8
(B) n(SO3) + n(CO2) = 4
(C) [n(SO2)/n(CO)] < 1
(D) Both (B) and (C).
9.
ˆˆˆ
†
For the reaction A(g) + 2B(g) ‡ˆˆ
ˆ C(g) + D(g) ; Kc = 1012 .
If the initial moles of A,B,C and D are 0.5, 1, 0.5 and 3.5 moles respectively in a one litre vessel.
What is the equilibrium concentration of B (mol/L )?
(A) 10–4
(B) 2 × 10–4
(C) 4 ×10–4
(D) 8 × 10–4
213
JEE-Chemistry
THERMODYNAMICS OF EQUILIBRIUM
1.
2.
3.
SINGLE CORRECT ANSWER TYPE
For a reversible reaction at equilibrium DG° =0, the equilibrium constant K =
(A) 0
(B) 1
(C) 2
(D) 10
For the reaction : H2(g) + I2(g)
reaction has
(A) DH = positive
(C) DH = zero
Variation of log K with
is :
1
T
2HI(g), Kc = 66.9 at 350°C and Kc = 50.0 at 448°C. The
(B) DH = negative
(D) DH sign can not be determined
is shown by the following graph in which straight line is at 45°, hence DH°
log10 K A
(A) + 4.606 cal
(B) – 4.606 cal
1/T
(C) 2 cal
(D) – 2cal
4.
The equilibrium constant for, 2H2S (g)
2H2(g) + S2(g) is 0.0118 at 1300 K while the heat of
dissociation is 597.4 kJ. The equilibrium constant of the reaction at 1200 K is :
(A) 1.180 × 10–4
(B) 11.80
(C) 118.0
(D) cannot be calculated from given data
5.
For a reversible reaction : aA + bB
K
º
é 1
cC + dD ; the variation of K with temperature is given by
1ù
- DH
2
ê - ú then,
log K =
2.303R ë T2 T1 û
1
(A) K2 > K1 if T2 > T1 for an endothermic change
(B) K2 < K1 if T2 > T1 for an endothermic change
(C) K2 > K1 if T2 > T1 for an exothermic change
(D) K1 < K2 if T2 > T1 for an exothermic change
6.
For the reaction 3Fe2O3(s)
2Fe3O4(s) +
1
O (g)
2 2
DHº298K = 55.5 kcal/mol and DGº298K = 46.5 kcal/mol. The equilibrium constant Kp at 298
K for this reaction is :
(A) 1.3 × 10–34
(B) 1.3 × 10–35
(C) 4 × 10–35
(D) 8 × 10–35
1/T
(C)
(D)
1/T
1/T
214
ln Kp
(B)
ln Kp
(A)
ln Kp
Which of the following graph represents an exothermic reaction
ln Kp
7.
1/T
Chemical Equilibrium
1/T
1/T
(D)
1/T
For the chemical equilibrium, CaCO3(s) ƒ CaO(s) + CO2(g)
2
(B)
log PCO
(A)
log PCO
2
D r H 0 can be determined from which one of the following graphs ?
(D)
log T
log PCO
(C)
2
1/T
2
1/T
log PCO
9.
(C)
log T
215
log Kp
(B)
log Kp
(A)
log Kp
ˆˆˆ
†
ˆ H2(g) + I2(g); DH = positive, Which of the following plot is correct ?
For the reaction 2HI(g) ‡ˆˆ
log Kp
8.
1/T
JEE-Chemistry
DEGREE OF DISSOCIATION &VAPOUR DENSITY
1.
2.
SINGLE CORRECT ANSWER TYPE
If concentration of N2, H2 and NH3 are 1, 2 and 3 respectively, their concentration at equilibrium
will be :
N2(g) + 3H2(g)
2NH3(g)
(A) (1 – x)
(2 – 3x)
2x
(B) (1 – x/3) (2 – x)
2x/3
(C) (1 – x)
(2 – x)
(3 + x)
(D) (1 – x)
(2 – 3x)
(3 + 2x)
4 moles of PCl5 are heated at constant temperature in closed container. If degree of dissociation of
PCl5 is 0.5, then calculate total number of moles at equilibrium :- PCl5(g) ƒ PCl3(g) + Cl2(g)
(A) 4.5
(B) 6
(C) 3
(D) 4
3.
ˆˆ† 2CO(g) + O (g). If 2 moles of CO are
The dissociation of CO2 can be expressed as 2CO2(g) ‡ˆˆ
2
2
taken initially and 40% of the CO2 is dissociatated. What is the total number of moles at equilibrium
(A) 2.4
(B) 2.0
(C) 1.2
(D) 5
4.
ˆˆ† PCl (g) + Cl (g), the partial pressure of PCl , Cl and PCl are 0.3,
For the reaction : PCl5(g) ‡ˆˆ
3
2
3
2
5
0.2 and 0.6 atm respectively. If partial pressure of PCl3 and Cl2 is increased to twice, what will be the
partial pressure of PCl5 at new equilibrium (in atm) :(A) 0.3
(B) 1.2
(C) 2.4
(D) 0.15
5.
In a closed container, equilibrium N2O4 (g)
2NO2 (g) is attained at 25°C. The total equilibrium
pressure in container is 380 torr. If equilibrium constant of above equilibrium is 0.667 atm, then
degree of dissociation of N2O4(g) at this temperature will be :
(A) 0.33
(B) 0.5
(C) 0.66
(D) 0.25
6.
For the reaction : N2(g)+ O2(g)
2NO(g), equilibrium constant Kc = 2. If equal moles
of N2 and O2 are present then find degrees of dissociation of N2 and O2 are :
(A)
1
1
,
1+ 2 1- 2
(B)
1
1
,
1- 2 1+ 2
(C) both are
1
1+ 2
(D)
2
2
,
1+ 2 1- 2
7.
40% of a mixture of 0.2 mole of N2(g) and 0.6 mole of H2(g) react to give NH3(g) according
to the equation : N2(g) + 3H2(g)
2NH3(g), at constant temperature and pressure. Then
the ratio of the final volume to the initial volumes of gases are as :
(A) 4 : 5
(B) 5 : 4
(C) 7 : 10
(D) 8 : 5
8.
The vapour density of PCl5 is 104.16 but when heated to 230º C its vapour density is reduced to 62.
The degree of dissociation of PCl5 at this temperature will be :
(A) 6.8%
(B) 68%
(C) 46%
(D) 64%
216
Chemical Equilibrium
9.
ˆˆˆ
†
ˆ nB(g), the degree of dissociation is measured from vapour
For the general reaction : A(g) ‡ˆˆ
density measurements. If the degree of dissociation, the observed and theoretical vapour densities be
a, d0 and dt respectively, then
dO - dt
(A) a = d n + 1
)
t (
(B) a =
dO - d t
dt
(C) a =
( dO - dt )(n - 1)
dt
dt - d0
(D) a = d (n - 1)
0
10.
For the reaction N2O4 (g)
2NO2 (g), if percentage dissociation of N2O4 are 20%, 45%, 65% &
80%, then the sequence of observed vapour densities will be :
(A) d20 > d45 > d65 > d80
(B) d80 > d65 > d45 > d20
(C) d20 = d45 = d65 = d80
(D) (d20 = d45) > ( d65 = d80)
11.
The degree of dissociation (a) of PCl5 obeying the equilibrium : PCl5(g)
approximately related to the presure at equilibrium by (given a << 1) :
(A) a µ P
12.
(B) a µ
1
(C) a µ
P
1
P
PCl3(g) + Cl2(g) , is
(D) a µ
2
1
P4
In the dissociation of N2O4(g) into NO2(g), (1 + a) values with the vapour densities ratio
æDö
ç ÷
èdø
is
given by : [a-degree of dissociation, D-vapour density before dissociation, d-vapour density after
dissociation]
(A) (1 + a)
(C) (1 + a)
(B) (1 + a)
D
d
13.
a
(A)
14.
D
d
D
d
In the above question, a varies with
D
d
D
d
D
d
according to :
a
(B)
(D) (1 + a)
a
(C)
D
d
a
D
d
(D)
D
d
Before equilibrium is set-up for the chemical reaction N2O4(g)
2NO2(g), vapour density d of the
gaseous mixture was measured. If D is the theoretical value of vapour density, variation of a with D/d
is given by the graph. What is the value of D/d at point A ?
a
A
D
d
(A) 0
(B) 0.5
(C) 1
217
(D) 1.5
JEE-Chemistry
LE-CHATELIER'S PRINCIPLE
1.
SINGLE CORRECT ANSWER TYPE
In which of the following equilibrium reactions, the equilibrium would shift to right side, if total
pressure is decreased :ˆˆ† 2NH (g)
ˆˆ† 2HI(g)
(A) N2(g) + 3H2(g) ‡ˆˆ
(B) H2(g) + I2(g) ‡ˆˆ
3
ˆˆ† 2NO (g)
ˆˆ† 2NO(g)
(C) N2O4(g) ‡ˆˆ
(D) N2(g) + O2(g) ‡ˆˆ
2
2.
For the reaction CO(g) + H2O(g)
CO2(g) + H2(g) at a given temperature the equilibrium amount
of CO2 (g) can be increased by :
(A) adding a suitable catalyst
(B) adding an inert gas
(C) decreasing the volume of container
(D) increasing the amount of CO(g)
3.
An equilibrium mixture in a vessel of capacity 100 litre contains 1 mole N2(g), 2 mole O2(g) and 3
mole NO(g). Number of moles of O2 to be added so that at new equilibrium the concentration of NO
is found to be 0.04 mol/L :
(A) (101/18)
(B) (101/9)
(C) (202/9)
(D) (18/101)
4.
When pressure is applied to the equilibrium
Ice
Water
Which of the following phenomenon will happen ?
(A) More ice will be formed
(B) Water will evaporate
(C) More water will be formed
(d) Equilibrium will not be achived.
5.
In a two step exothermic reaction : A2(g) + B2(g)
3C(g)
D(g), step 1 & 2 are
favoured by :
(A) high pressure, high temperature & low pressure, low temperature respectively.
(B) low pressure, low temperature & high pressure, low temperature respectively.
(C) high pressure, low temperature & low pressure, high temperature respectively.
(D) low pressure, high temperature & high pressure, high temperature respectively.
6.
For a reaction if Kp > Kc, the forward reaction is favoured by (T > 15K)
(A) High temperature (B) Low temperature (C) Low pressure
(D) High pressure.
7.
In a given reaction : 2X(g) + Y(g)
2Z(g) + 80 kcal
Which combination of pressure and temperature gives the highest yield of Z at equilibrium
(A) 1000 atm and 200°C
(B) 500 atm and 500°C
(C) 1000 atm and 100°C
(C) 500 atm and 100°C
8.
ˆˆ† CO2(g) , DH = positive
On decreasing temperature of following system at equilibrium CO2(s) ‡ˆˆ
:(A) There is no effect on the equilibrium state
(B) More CO2 gas is formed
(C) More solid CO2 is obtained
(D) None of above
218
Chemical Equilibrium
9.
MULTIPLE CORRECT ANSWER TYPE
For the reaction : PCl5 (g)
PCl3 (g) + Cl2 (g), The forward reaction at constant temperature is
favoured by
(A) introducing chlorine gas at constant volume (B) introducing an inert gas at constant pressure
(C) increasing the volume of the container
(D) introducing PCl5 at constant volume
10.
For the following reaction at equilibrium : N2(g) + 3H2(g)
2NH3(g). Some inert gas at constant
pressure is added to the system. Predict which of the following facts will be observed.
(A) More NH3(g) is produced
(B) Less NH3(g) is produced
(C) No affect on the equilibrium
(D) Kp of the reaction is decreased
11.
2CaSO4(s)
2CaO(s) + 2SO2(g) + O2(g), DH > 0
Above equilibrium is established by taking some amount of CaSO4(s) in a closed container at 1600
K. Then which of the following may be correct option(s).
(A) moles of CaO(s) will increase with the increase in temperature
(B) If the volume of the container is doubled at equilibrium then partial pressure of SO2(g) will
change at new equilibrium.
(C) If the volume of the container is halved partial pressure of O2(g) at new equilibrium will remain
same
(D) If two moles of the He gas is added at constant pressure then the moles of CaO(s) will increase.
219
JEE-Chemistry
SIMULTANEOUS EQUILIBRIUM
1.
SINGLE CORRECT ANSWER TYPE
Two solids X and Y disssociate into gaseous products at a certain temperature as follows:
X(s) ƒ A(g) + C(g), and Y(s) ƒ B(g) + C(g). At a given temperature, pressure over excess solid
X is 40 mm and total pressure over solid Y is 60 mm. Calculate the ratio of moles of A and B in
vapour state over a mixture of X and Y
(A) 2/3
(B) 9/4
(C) 4/9
(D) 3/2
2.
The two equilibria, AB(aq)
A+(aq) + B-(aq) and AB(aq) + B-(aq)
AB2-(aq) are
simultaneously maintained in a solution with equilibrium constants, K1 and K2 respectively. The ratio
of concentration of A+ to AB2- in the solution is :
(A) directly proportional to the concentration of B– (aq).
(B) inversely proportional to the concentration of B– (aq).
(C) directly proportional to the square of the concentration of B– (aq).
(D) inversely proportional to the square of the concentration of B– (aq).
3.
In the preceeding problem, if [A+] and [AB2-] are y and x respectively, under equilibrium produced
by adding the substance AB to the solvents, then K1/K2 is equal to
4.
(A)
y
( y - x )2
x
(B)
y 2 ( x + y)
x
(C)
y 2 ( x + y)
x
(D)
y
( x - y)
x
MULTIPLE CORRECT ANSWER TYPE
The two equilibria, AB
A+ + B- and AB + BAB2- are simultaneously maintained in a
solution with equilibrium constants, K1 and K2 respectively. If [A+] and [AB2-] are y and x respectively,
under equilibrium produced by adding the substance AB(s) to the solvents, then
(A) k1/k2 =
y
( y - x)2
x
(B) k1/k2 =
y
( x - y)
x
(C) [B¯]eq. = y – x
220
(D) None of these
Chemical Equilibrium
ANSWER KEY
CHARACTERISTIC OF CHEMICAL EQUILIBRIUM
1.
(D)
2.
(A)
3.
(D)
7.
(A)
8.
(B)
9.
(A)
4.
(C)
5.
(B)
6.
(C)
PROBLEMS BASED UPON EQUILIBRIUM CONSTANT
1.
(C)
2.
(B)
3.
(D)
4.
(C)
5.
(D)
6.
(D)
7.
(D)
8.
(A)
9.
(D)
10.
(A)
11.
(B)
12.
(A)
13.
(A)
14.
(D)
15.
(B)
16.
(B)
REACTION QUOTIENT &APPLICATION OF EQUILIBRIUM
CONSTANT
1.
(C)
2.
(A)
3.
(A)
7.
(D)
8.
(D)
9.
(B)
4.
(D)
5.
(A)
6.
(B)
6.
(A)
THERMODYNAMICS OF EQUILIBRIUM
1.
(B)
2.
(B)
3.
(B)
7.
(D)
8.
(B)
9.
(A)
4.
(A)
5.
(A)
DEGREE OF DISSOCIATION &VAPOUR DENSITY
1.
(D)
2.
(B)
3.
(A)
4.
(C)
5.
(B)
6.
(C)
7.
(A)
8.
(B)
9.
(D)
10.
(A)
11.
(B)
12.
(A)
13.
(B)
14.
(C)
6.
(C)
LE-CHATELIER'S PRINCIPLE
1.
(C)
2.
(D)
3.
(A)
4.
7.
(C)
8.
(C)
9.
(B)(C)(D) 10.
(C)
5.
(B)
(B)
11.
(A)(C)(D)
SIMULTANEOUS EQUILIBRIUM
1.
(C)
2.
(D)
3.
(A)
4.
221
(A)(C)
JEE-Chemistry
Important Notes
222
Ionic Equilibrium
IONIC EQUILIBRIUM
OSTWALD'S DILUTION LAW & ACID BASE CONCEPT
1.
2.
SINGLE CORRECT ANSWER TYPE
Ostwald's dilution law is not applicable for strong electrolytes because:(A) Strong electrolytes are completely ionised
(B) Strong electrolytes are volatile
(C) Strong electrolytes are unstable
(D) Strong electrolytes often contain metal ions
For a solution K = 4.41 × 10–5 , C = 0.1 M then a will be :(A) 2.1 × 10–2
(B) 4.41 × 10–4
(C) 1.5 × 10–1
(D) 2.1 × 10–1
3.
A solution of acetic acid is 1.0% ionised. Determine the molar concentration of acid
(Ka = 1.8 ´ 10–5) and also the [H+].
(A) 1.8 ´ 10–5 M
(B) 1.8 ´ 10–6 M
(C) 1.8 ´ 10–3 M
(D) 1.8 ´ 10–4 M
4.
BF3 is acid according to :(A) Lewis
(B) Arrhenius
5.
(C) Bronsted and Lowery (D) Madam Curie
Consider the following reactions :+ H2O
(i) CO 23
HCO 3- + OH–
(ii) CO2 + H2O
H2CO3
(iii) NH3 + H2O
NH4OH
(iv) HCl + H2O
Cl– + H3O+
Which of the pairs of reactions proves that water is basic in character :(A) (i), (ii) and (iii)
(B) only (iii)
(C) only (iv)
(D) (i), (ii), (iii) and (iv)
6.
The conjugated base for bicarbonate ion is:(A) CO32 -
7.
(C) CO2
(D) H2CO3
Which of the following is strongest conjugate base:(A) ClO -4
8.
(B) HCO 3-
(B) HCO 3-
(C) F–
(D) HSO -4
In which of the following reactions NH3 acts as acid :(B) NH3 + H+ ® NH4+
(A) NH3 + HCl ® NH4Cl
1
(C) NH3 + Na ® NaNH2+ H2
2
(D) NH3 cannot act as acid
223
JEE-Chemistry
IONIC PRODUCT OF WATER (KW)
1.
2.
3.
4.
5.
6.
SINGLE CORRECT ANSWER TYPE
For water at 25° C, 2 × 10–7 moles per litre is the correct answer for which one of the following
(A) [H+] + [OH–]
(B) [H+]2
(C) [OH–]2
(D) [H+] – [OH–]
The units of ionic product of water (KW) are:(A) Mol–1 Lit.–1
(B) Mol2– Lit.–2
(C) Mol2– Lit.–1
(D) Mol2 Lit–2
Degree of dissociation of water at 25ºC is
(A) 1.8 × 10–7 %
(B) 1.8 × 10–5 %
(D) 1.8 × 10–2 %
(C) 1.8 × 10–3 %
At 80ºC, Kw = 10–13 pH of neutral point is
(A) 7
(B) 6.5
(C) 8
(D) 9
Molar concentration of water (density = 1gm/cc) is
(A) 55.55 M
(B) 1 M
(C) 20 M
(D) 18 M
What is the value of Kw in 0.01 M NaOH at 25ºC ?
(A) 1 × 10–15
(B) 1 × 10–13
(C) 1 × 10–16
(D) 1 × 10–14
pH OF SOLUTION
1.
2.
3.
SINGLE CORRECT ANSWER TYPE
0.001 M KOH solution has the pH :(A) 10–1
(B) 3
(C) 11
(D) 2
10–6 M HCl is diluted to 100 times. Its pH is:(A) 6.0
(B) 8.0
(C) 6.95
(D) 9.5
The pH of a 10–10 M NaOH solution is nearest to :(A) 10
(B) 7
(C) 4
(D) – 10
4.
The pH of a 0.02 M ammonia solution which is 5% ionised will be :(A) 2
(B) 11
(C) 5
(D) 7
5.
Pure water is kept in a vessel and it remains exposed to atmospheric CO2 which is absorbed. Then
the pH will be :(A) Greater than 7
(B) Less than 7
(C) 7
(D) Depends on ionic product of water
6.
pH of 10–1 M formic acid is:(A) 1
(B) > 1
7.
(C) < 1
(D) 13
How many moles of HCl must be removed from 1 litre of aqueous HCl solution to change its pH
from 2 to 3 :(A) 1
(B) 0.02
(C) 0.009
(D) 0.01
224
Ionic Equilibrium
8.
Calculate pH of a solution whose 100 ml contains 0.2 g NaOH dissolved in it :(A) 10.699
(B) 11.699
(C) 12.699
(D) 13.699
9.
[H3O+] in 0.1 M H2SO4 at two stages
(A) 0.1 M, 0.1 M
H2SO4
H+ + HSO4–
HSO4–
H+ + SO42–
(B) 0.1 M, > 0.01 M (C) > 0.1 M, > 0.1 M
are :
(D) 0.1 M, < 0.1 M
10.
When the pH changes from 4 to 2, the hydrogen ion concentration will increase by a factor –
(A) 2
(B) 1/2
(C) 102
(D) 100.5
11.
1 cc of 0.1 M HCl is added to 99 cc solution of NaCl. The pH of the resulting solution will be
(A) 7
(B) 3
(C) 4
(D) 1
12.
The first and second dissociation constants of an acid H2A are 1.0 × 10–5 and 5.0 × 10–10 respectively.
The overall dissociation constant of the acid will be :
(A) 5.0 ×10–5
(B) 5.0 ×1015
(C) 5.0 ×10–15
(D) 0.2 ×105
13.
0.001 mol of the strong electrolyte M(OH)2 has been dissolved to make a 20 mL of its saturated
solution. Its pH will be : - [Kw = 1 × 10–14]
(A) 13
(B) 3.3
(C) 11
(D) 9.8
14.
MULTIPLE CORRECT ANSWER TYPE
In the following reaction:
[Cu(H2O)3 (OH)]+ + [Al(H2O)6]3+
A
B
[Cu(H2O)4]2+ + [Al(H2O)5(OH)]2+
C
D
(A) A is an acid and B the base
(B) A is a base and B the acid
(C) C is the conjugate acid of A, and D is the conjugate base of B
(D) C is the conjugate base of A, and D is the conjugate acid of B
15.
Which of the following will suppress the ionization of phthalic acid in an aqueous
solution.
(A) KCl
(B) H2SO 4
(C) HNO3
(D) NaOH
225
JEE-Chemistry
TYPES OF SALT AND SALT HYDROLYSIS
1.
2.
SINGLE CORRECT ANSWER TYPE
Which of the following is not an acidic salt :(A) NaHSO4
(B) HCOONa
(C) NaH2PO3
(D) None of them
Which is a basic salt :–
(A) PbS
(B) PbCO3
(D) 2PbCO3 Pb(OH)2
(C) PbSO4
3.
The process of neutralisation invariably results in the production of :(A) H+ ions
(B) OH— ions
(C) Both H+ and OH— ions
(D) Molecules of water
4.
At 900 C, the pH of 0.1M NaCl aqueous solution is :(A) < 7
(B) > 7
(C) 7
5.
HCOO– + H2O
is related :(A) h =
6.
Kh
(D) 0.1
HCOOH + OH–
(B) h =
Kh
C
(C) h =
The pH of aqueous solution of sodium acetate is
(A) 7
(B) Very low
(C) > 7
Kh
V
(D) Kh =
hc
(D) < 7
7.
A salt 'X' is dissolved in water of pH = 7. The resulting solution becomes alkaline in nature. The
salt is made up of:(A) A strong acid and strong base
(B) A strong acid and weak base
(C) A weak acid and weak base
(D) A weak acid and strong base
8.
Degree of Hydrolysis of
(A) 2.7 ´ 10–3
9.
M
solution of KCN is (Given Ka = 1.4 ´ 10–9)
100
(B) 2.7 ´ 10–2
(C) 2.7 ´ 10–4
(D) 2.7 ´ 10–5
The pH of 1M NH4Cl(aq) at 25o C should be:–
(A) zero
(B) between 6 and 7 (C) 7
(D) above 7
10.
The Ka value for the acid HA is 1.0 × 10–6. What is the value of K for the reaction ?
A– + H3O+
HA + H2O
–8
(A) 1.0 × 10
(B) 1.0 × 108
(C)1.0 × 10–3
(D) 1.0 × 106
11.
pH of 0.01 M aqueous solution of NaX, NaY and NaZ are 8, 9 and 10 respectively. Strongest acid
among HX, HY and HZ is –
(A) HX
(B) HY
(C) HZ
(D) can’t be predicted
Four solutions of NH4Cl are taken with concentrations 1 M, 0.1 M, 0.01 M and 0.001 M. Their
12.
226
Ionic Equilibrium
degree of hydrolysis are h1, h2, h3 and h4. What is the gradation of degree of hydrolysis ?
(A) h1 > h2 > h3 > h4 (B) h1 = h2 = h3 = h4 (C) h4 > h3 > h2 > h1 (D) none of these
13.
The degree of hydrolysis of a salt of weak acid and weak base in it’s 0.1 M solution is found to be
50%. If the molarity of the solution is 0.2 M, the percentage hydrolysis of the salt should be
(A) 100%
(B) 50%
(C) 25%
(D) none of these
14.
A saturated solution of barium formate (HCOO)2 Ba contains 0.6 mole in 2 litre solution. pOH of
solution is 4.6. pka of formic acid (HCOOH) is ?
(A) 4.8 + log 0.6
(B) 4.8 + log 0.3
(C) 9.4 – log 0.6
(D) 4.8 – log 0.6
BUFFER SOLUTION
1.
SINGLE CORRECT ANSWER TYPE
20 mL of 0.2 M NaOH is added to 50 mL of 0.2 M CH3COOH. Hence (pH – pKa) is –
(A) log
3
2
(B) log
2
3
(C) log 2
(D) 2 log 2
2.
Which buffer solution has maximum pH ?
(A) mixture which is 0.1 M in CH3COOH and 0.1 M in CH3COONa [pKa (CH3COOH) = 4.74]
(B) mixture which is 0.2 M CH3COOH and 0.2 M in CH3COONa
(C) mixture which is 0.1 M in NH4Cl and 0.1 M in NH4OH [pKa (NH4+) = 9.26]
(D) all the solution have equal pH which is 4.74
3.
pH of mixture of HA and A– buffer is 5. Kb of A– = 10–10. Hence [HA]/[A–] will be :
(A) 1
(B) 10
(C) 0.1
(D) 100
4.
A flask contains 100.00 mL of 0.100 M HOAc. To prepare a buffer with pH = pKa which of the
following samples of barium acetate solution should be added to the flask?
(A) 50.00 mL of 0.400 M Ba (OAc)2
(B) 25.00 mL of 0.200 M Ba (OAc)2
(C) 50.00 mL of 0.200 M Ba (OAc)2
(D) 100.00 mL of 0.100 M Ba (OAc)2
5.
The pH of a solution containing 0.10 M H3BO3 and 0.18 M Na[B(OH)4] is
(Ka of H3BO3 = 7.3 ´ 10–10)
[Use log 4.1 = 0.61]
(A) 4.39
(B) 9.39
(C) 12.39
(D) 11.39
6.
Ka for HCN is 5 x 10–10 at 250C. For maintaining a constant pH of 9, the volume of 5M KCN
solution required to be added to 10mL of 2M HCN solution is(A) 4 mL
(B) 7.95 mL
(C) 2 mL
(D) 9.3 mL
7.
A basic - buffer will obey the equation pOH - pKb = 1 only under condition:(A) [Conjugate acid] : [base] = 1 : 10
(B) [Conjugate acid] = [base]
(C) [Conjugate acid] : [base] = 10 : 1
(D) N.O.T
8.
Half of the formic acid solution is neutralised on addition of a KOH solution to it. If
Ka (HCOOH) = 2 × 10–4 then pH of the solution is : (log 2 = 0.3010)
(A) 3.6990
(B) 10.3010
(C) 3.85
(D) 4.3010
227
JEE-Chemistry
9.
MULTIPLE CORRECT ANSWER TYPE
All of the following are acid-base conjugate pairs:
(A) HONO, NO2–
(B) H3O+, OH–
(C) CH3NH3+, CH3NH2 (D) HS–, S2–
10.
pH of the following solution is not affected by dilution:
(A) 0.01 M CH3COONa
(B) 0.01 M NaHCO3
(C) buffer of 0.01 M CH3COONa and 0.01 M CH3COOH
(D) 0.01 M CH3COONH4
11.
Which of the following mixtures constitute a buffer?
(A) CH3COOH + CH 3COONa
(B) Na2CO 3 + NaHCO3
(C) NaCl + HCl
(D) NH4Cl + (NH4)2SO 4
SOLUBILITY & SOLUBILITY PRODUCT (KSP)
1.
SINGLE CORRECT ANSWER TYPE
The correct relation between Ksp and solubility for the salt KAl(SO4)2 is
(A) 4s3
(B) 4s4
(C) 27s4
(D) None
2.
If s is the molar solubility of Ag 2SO4, then –
(A) 3 [Ag+] = s
(B) [Ag+] = s
(C) [2Ag+] = s
(D) [ SO 2–
4 ] = s
3.
The aqueous solution of which of the following sulphides would contain maximum concentration of
S2– ions–
(A) MnS (Ksp = 1.1 × 10–21 )
(B) ZnS (Ksp = 1.1 × 10–23 )
(C) PbS (Ksp = 1.1 × 10–35 )
(D) CuS (Ksp = 1.1 × 10–30 )
4.
Which of the following salts has maximum solubility –
(A) HgS, Ksp = 1.6 × 10–54
(B) PbSO4 , Ksp = 1.3 × 10–8
(C) ZnS, Ksp = 7.0 × 10–26
(D) AgCl, Ksp = 1.7 × 10–10
5.
At 250C, the Ksp value of AgCl is 1.8 × 10–10. If 10–5 moles of Ag+ are added to solution then Ksp will
be :(A) 1.8 × 10–15
(B) 1.8 × 10–10
(C) 1.8 × 10–5
(D) 18 × 10+10
6.
The solubility product of As2S3 is given by the expression :(A) Ksp = [As3+][S–2]
(B) Ksp = [As3+]1 [S–2]1
(C) Ksp = [As3+]3 [S–2]2
(D) Ksp = [As3+]2 [S–2]3
7.
If the solubility of lithium sodium hexafluoro aluminate Li3Na3(AlF6)2 is 's' moles/litre. Its solubility
product is equal to :(A) s8
(B) 12 s3
(C) 18 s3
(D) 2916 s8
228
Ionic Equilibrium
8.
9.
If the maximum concentration of PbCl2 in water is 0.01 M at 298 K,
in 0.1 M NaCl will be:(A) 4 × 10–3 M
(B) 0.4 × 10–4 M
(C) 4 × 10–2 M
In which of the following, the solubility of AgCl will be maximum
(A) 0.1 M AgNO3
(B) Water
(C) 0.1 M NaCl
Its maximum concentration
(D) 4 × 10–4 M
:(D) 0.1 M KCl
10.
At 30ºC, the solubility of Ag2CO3 (Ksp = 8 × 10–2 ) will be maximum in –
(A) 0.05 M Na2CO3 (B) 0.05 M AgNO3 (C) Pure water
(D) 0.05 NH3
11.
What will happen if the pH of the solution of 0.001 M Mg(NO3)2 solution is adjusted to
pH = 9 (Ksp of Mg(OH)2 = 8.9 × 10-12)
(A) ppt will take place
(B) ppt will not take place
(C) Solution will be saturated
(D) None of these
12
Solubility of Ag2CO3 could be calculated by the following formula :(A)
FK I
GH 8 JK
sp
(B)
3
æ K SP ö
ç 4 ÷
è
ø
(C)
3
æ K SP ö
ç
÷
è 2 ø
(D)
3
æ K SP ö
ç
÷
è 8 ø
13.
Solubility product of AgCl at 100°C is 1.44 × 10–4, solubility of AgCl in boiling water may be:(A) 0.72 × 10–4 M
(B) 1.20 × 10–2 M
(C) 0.72 × 10–2 M
(D) 1.20 × 10–4 M
14.
Relation between solubility & solubility product of AxBy type salt is :(A) Ksp = xx yy sx–y (B) Ksp = sx+y
(C) Ksp = xyyxsx+y
(D) Ksp = xx yy sx+y
15.
Solubility of PbCl2 is :(A)
K sp
(B)
3
K sp
(C)
3
K sp
4
(D)
K sp
4
16.
If solubility product of AgCl at 25° C is 5 × 10–13 then solubility of its :(A) 5 × 10–13
(B) 7.1 × 10–7
(C) 2.5 × 10–13
(D) 2.5 × 10–6
17.
The solubility products of Al(OH)3 and Zn(OH)2 are 8.5 × 10–23 and 1.8 × 10–14 at room temperature.
If the solution contains same concentration of Al3+ and Zn2+ ions, the ion first precipitated by adding
NH4OH is –
(A) Al3+
(B)Zn2+
(C) both (A) & (B)
(D) none of these
18.
The necessary condition for saturated solution is –
(A) Product of ionic concentrations = Solubility product
(B) Product of ionic concentrations < Solubility product
(C) Product of ionic concentrations > Solubility product
(D) None of the above
229
JEE-Chemistry
19.
20.
Which of the following would increase the solubility of Pb (OH) 2 –
(A) Add hydrochloric acid
(B) Add a solution of Pb(NO3)2
(C) Add a solution of NaOH
(D) The solubility of a compound is constant at constant temperature
MULTIPLE CORRECT ANSWER TYPE
When HCl(g) is passed through a saturated solution of common salt, pure NaCl is
precipitated because
(A) HCl is highly soluble in water
(B) the ionic product [Na+] [Cl¯] exceeds its solubility product (K sp)
(C) the Ksp of NaCl is lowered by the presence of Cl¯ ions
(D) HCl causes precipitation
ANSWER KEY
OSTWALD'S DILUTION LAW & ACID BASE CONCEPT
1.
(A)
2.
(A)
7.
(B)
8.
(C)
3.
(C)
4.
(A)
5.
(C)
6.
(A)
IONIC PRODUCT OF WATER (KW)
1.
(A)
2.
(D)
3.
(A)
4.
(B)
5.
(A)
6.
(D)
pH OF SOLUTION
1.
(C)
2.
(C)
3.
(B)
4.
(B)
5.
(B)
6.
(B)
7.
(C)
8.
(C)
9.
(D)
10.
(C)
11.
(B)
12.
(C)
13.
(A)
14.
(B)(C)
15.
(B)(C)
TYPES OF SALT AND SALT HYDROLYSIS
1.
(B)
2.
(D)
3.
(D)
4.
(A)
5.
(B)
6.
(C)
7.
(D)
8.
(B)
9.
(B)
10.
(D)
11.
(A)
12.
(C)
13.
(B)
14.
(D)
5.
(B)
6.
(C)
BUFFER SOLUTION
1.
(B)
2.
(C)
3.
(C)
4.
7.
(C)
8.
(A)
9.
(A)(C)(D) 10.
(B)
(B)(C)(D) 11.
(A)(B)
SOLUBILITY & SOLUBILITY PRODUCT (KSP)
1.
(B)
2.
(D)
3.
(A)
4.
(B)
5.
(B)
6.
(D)
7.
(D)
8.
(D)
9.
(B)
10.
(D)
11.
(B)
12
(B)
13.
(B)
14.
(D)
15.
(C)
16.
(B)
17.
(A)
18.
(A)
19.
(A)
20.
(B)(D)
230
s-Block
GENERAL PHYSICAL AND ATOMIC PROPERTIES OF GROUP -1
METALS
1.
2.
SINGLE CORRECT ANSWER TYPE
Melting point is least for which of the following alkali metal ?
(A) Na
(B) K
(C) Rb
(D) Cs
In Flame test, which colour is shown by potassium ?
(A) Golden yellow
(B) Crimson red
(C) Violet
(D) Apple green
3.
The ionic mobility of alkali metal ions in aqueous solution is maximum for :
(A) Rb+
(B) Li+
(C) Na+
(D) K+
4.
Pick the incorrect statement from the following about alkali metals :
(A) Alkali metals are soft.
(B) Alkali metals have low melting point.
(C) They have very high density.
(D) They have low ionisation energy.
5.
Which is not correct for Lithium ?
(A) Lithium is softer than other alkali metals.
(B) Hydrated Lithium ion is the largest among hydrated alkali metal ions.
(C) The melting and boiling points of Li are comparatively high.
(D) The ionisation enthalpy and electronegativity of Li are higher than other alkali metals.
6.
(1)
(2)
(3)
(4)
(A)
(B)
(C)
(D)
7.
(1)
(2)
(3)
(4)
(A)
(B)
(C)
(D)
Metal
Na
Li
Cs
Rb
(1) (2) (3) (4)
P
Q
R
S
S
P
Q
R
Q
R
S
P
R
S
P
Q
Order
Cs> Rb > Na > K > Li
Li > Na > K > Rb > Cs
Cs > Rb > K >Na > Li
Li+ > Na+ > K+ > Rb+
(1) (2) (3) (4)
R
S
P
Q
P
Q
R
S
S
P
Q
R
Q
R
S
P
MATRIX MATCH TYPE
Property
(P) alkali metal having least density
(Q) alkali metal having maximum atomic volume
(R) Red violet colour in flame test
(S) Most abundant alkali metal in earth’s crust
Correct for property
(P) metallic radius
(Q) hydrated ionic radii
(R) density
(S) melting point
8.
INTEGER ANSWER TYPE
How many alkali metals do not respond to flame test ?
[Do not consider radioactive alkali metals]
9.
Total number of valence electrons in an alkali metal is ......
10.
How many alkali metals are present in first period of the periodic table ?
231
JEE-Chemistry
GENERAL CHEMICAL PROPERTIES OF GROUP-1 METALS
1.
SINGLE CORRECT ANSWER TYPE
Which of the following alkali metals reacts with water least vigorously ?
(A) Li
(B) Na
(C) K
(D) Cs
2.
Sodium reacts with water more vigorously than lithium because it :
(A) has higher atomic weight
(B) is a metal
(C) has lower melting point
(D) is more electronegative
3.
The reducing power of a metal depends on various factors. Suggest the factor which makes Li, the
strongest reducing agent in aqueous solution :
(A) Sublimation enthalpy
(B) Ionisation enthalpy
(C) Hydration enthalpy (D) Electron- gain enthalpy
4.
The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the
individual ions. Amongst fluorides of alkali metals, the lowest solubility of LiF in water is due to :
(A) Ionic natue of lithium fluoride
(B) High lattice enthalpy
(C) High hydration enthalpy for lithium ion
(D) Low ionisation enthalpy of lithium atom
5.
Which of the following alkali metal carbonate is the least stable and decomposes readily ?
(A) Li2CO3
(B) Na2CO3
(C) K2CO3
(D) Cs2CO3
6.
On dissolving small amount of sodium metal in liquid NH3 at low temperature, which one of the
following does not occur ?
(A) Blue coloured solution is obtained.
(B) Solvated Na+ ions are formed in the solution.
(C) Solution becomes good conductor of electricity.
(D) Solution is diamagnetic.
7.
Alkali metal are powerful reducing agents because :
(A) these are non metals.
(B) these are monovalent.
(C) their ionic radii are large.
(D) their ionization potentials are low.
8.
Which is the most soluble in ether ?
(A) NaCl
(B) KCl
9.
10.
MULTIPLE CORRECT ANSWER TYPE
Paramagnetic species are formed in
(B) KO2 + H 2 O ®
(excess)
12.
(D) RbCl
A blue coloured solution of sodium in liquid NH3 acts as strong reducing agent, because of (A) ammoniated sodium
(B) Ammonia dissociation
(C) Sodium nitride formed
(D) ammoniated electron
(A) K + NH3 (l) ®
11.
(C) LiCl
(C) Li2 O + H 2 O ®
Which of the following carbonates do not evolve CO2 on heating ?
(A) Li2CO3
(B) MgCO3
(C) Na2CO3
KO + CO ® (a)
2
(2 mole)
(1mole)
(compound )
+
D
(D) Li 2 CO 3 ¾¾
®
(D) K2CO3
(b)
(diatomic gas)
Select the correct statement(s):
(A) (b) is paramagnetic.(B) (b) is colourless.
(C) (a) is thermally stable.
(D) bond order in (b) is 2.
232
s-Block
13.
14.
Bicarbonate(s) which are known in solid state is/are
(A) LiHCO3
(B) NaHCO3
(C) KHCO3
(D) CsHCO3
Select the correct statement(s)/comparisons about alkali metal halides :
(A) LiF > LiCl > LiBr > LiI : Melting point
(B) Enthalpy of formation of KI is positive.
(C) CsI is less soluble in water due to low lattice enthalpy.
(D) LiCl < NaCl < KCl < RbCl < CsCl : Negative DfHº
15.
MATRIX MATCH TYPE
Column-II
(Metal ‘M’ = )
Column-I
(Reaction )
D
® Peroxide (major)
(A) M + O 2 ¾¾
(P)
(exc)
(B)
D
M + O 2 ¾¾
®
paramagnetic (major)
Li
(Q) Na
(exc)
16.
17.
(C)
in dry
® tarnished
M ¾¾¾
air
(R)
Rb
(D)
N2 , D
® Nitride
M ¾¾¾
(S)
K
Column-I
(Reaction )
Column-II
(Products/properties of products)
(A)
D
Na + HC º CH ¾¾
®
(P)
(B)
KO 2 + H 2 O ¾¾
®
(Q) Basic oxide/Peroxide/superoxide/Hydroxide
(C)
D
LiNO3 ¾¾
®
(R)
Paramagnetic gas
(D)
D
Cs + exc. O 2 ¾¾
®
(S)
(T)
Yellow orange paramagnetic solid
Reddish-brown gas
Colourless gas
INTEGER ANSWER TYPE
Total number of alkali metals (non-radioactive) which produce mainly superoxide when burn with
excess of O2 is :
18.
On heating a mixture containing 3 moles each of Li2CO3 and K2CO3, how many moles of CO2 are
evolved ?
19.
Consider following reactions : (Ignore balancing)
(I) Na + H2O ¾¾
® NaOH + H2 ­
(II) NaH + H2 O ¾¾
® NaOH + H2 ­
D
(III) Na + N2 ¾¾
® Na3N
(IV) Li3 N + H2O ¾¾
® N2 + LiOH
D
D
(V) Na2CO3 ¾¾
(VI) NaHCO3 ¾¾
® Na2O + CO2
® Na2CO3 + H2O + CO2
How many reactions give products as indicated ?
20.
25 ° C
Na2O2 + H2SO4 ¾¾¾
®
How many moles of H2O2 are obtained finally?
233
JEE-Chemistry
SOME IMPORTANT ALKALI METAL COMPOUNDS
1.
SINGLE CORRECT ANSWER TYPE
Which of the following substance is not related to Solvay process ?
(A) CaCO3
(B) NaHCO3
(C) Na2CO3
(D) KCl
2.
Which of the following statement is INCORRECT ?
(A) Reaction of S and NaOH, gives Na2S and Na2S2O3.
(B) Reaction of Cl2 with cold and dilute NaOH, gives NaCl and NaOCl.
(C) Reaction of Cl2 with hot and conc. NaOH, gives NaCl and NaClO3.
(D) Reaction of P4 and NaOH, gives NaH2PO2 only.
3.
Which of the following element is insoluble in excess of NaOH ?
(A) Pb
(B) Pt
(C) Zn
(D) Sn
4.
In the synthesis of sodium carbonate, the recovery of ammonia is done by treating NH4Cl with
Ca(OH)2. The by product obtained in this process is :
(A) CaCl2
(B) KCl
(C) Na2O
(D) KO2
5.
Which disproportionates on heating with NaOH ?
(A) P4
(B) S
(C) Cl2
(D) All of these
6.
When NaOH is added dropwise to a mixture of two compounds, A white precipitate appears but on
adding excess of NaOH amount of precipitate decreases but not completely finished from solution.
The possible compounds are(A) AlCl3, MnCl2
(B) ZnCl2, PbO2
(C) BeCl2, ZnSO4
(D) Al2O3, SnO2
7.
Which systematic diagram represents the correct sequence of Solvay process ?
CO2
+ H2O
(Excess)
in NH4OH
in NH4OH
CO2
+ H2O
(Excess)
NH4HCO3
(NH4)2CO3
KCl
CaCl2
(A)
(B)
CO2 + K2CO3
D
KHCO3
in NH4OH
CO2
+ H2O
(Excess)
NH4Cl
CO2 + Na2CO3
D
CaO
D
CaCO3
in Ca(OH)2
CO2
+ H2O
(Excess)
NH4HCO3
NaCl
(C)
CO2 +
CO2 + CaO
234
Ca(HCO3)2
Na2CO3
(D)
NaHCO3
2NH4Cl
D
CaCO3 + 2NaHCO3
s-Block
8.
MULTIPLE CORRECT ANSWER TYPE
Choose correct statement for sodium carbonate :
(A) White crystalline solid
(B) Soluble in water
(C) It’s anhydrous white powder form is known as soda ash
(D) Its aqueous solution is alkaline.
9.
Which of the following statement are correct for NaOH ?
(A) It is an ionic solid.
(B) NaOH solution at the surface reacts with CO2 in the atmosphere to form Na2CO3.
(C) It is a deliquescent solid.
(D) It is obtained along with O2 gas on treatment of sodium amalgam with water.
10.
Which of the following bicarbonate has hydrogen bond in solid state ?
(A) NaHCO3
(B) KHCO3
(C) RbHCO3
(D) Ba(HCO3)2
11.
Choose the correct orders of solubility :
(A) NaCl > CaCl2
(B) MgCl2 > NaCl
(C) KHCO3 > NaHCO3 (D) LiF > CsF
MATRIX MATCH TYPE
12.
Column-I
(Reaction/Process)
Column-II
(Used for preparation
of compound)
(A)
Electrolysis
Brine solution ¾¾¾¾¾¾¾
®
in Castner - Kel ln er cell
(P)
Baking soda
(B)
add NaCl
D
NH 3 + H 2 O + CO 2 ¾¾
® solution ¾¾¾¾
® ppt ¾¾
®
(Q)
Table salt
(C)
Saturation by CO 2
®
Na 2 CO3 (aq) ¾¾¾¾¾¾
(R)
Caustic soda
(S)
Washing soda
min. H 2O
saturation with HCl
(D) Crude salt from sea water ¾¾¾¾
® solution ¾¾¾¾¾¾
®
13.
INTEGER ANSWER TYPE
How many of given species are soluble in excess NaOH?
Al(OH)3, Be(OH)2, Cu(OH)2, Fe(OH)3, Zn(OH)2, AgCl, PbO, SnO, Al2O3
14.
How many water molecules are lost by Na2CO3.10H2O on heating at 100ºC ?
15.
In the reaction with sodium hydroxide, how many of the following substances are oxidised ?
Be, Al, Sn, Pb, NH4Cl , FeCl3, AlCl3, Mg, Li
235
JEE-Chemistry
GENERAL PHYSICAL , ATOMIC AND CHEMICAL PROPERTIES
OF GROUP -2 METALS
1.
SINGLE CORRECT ANSWER TYPE
A substance which gives brick red flame and breaks down on heating to give oxygen and a brown
gas is :
(A) Magnesium nitrate (B) Calcium nitrate
(C) Barium nitrate
(D) Berrylium nitrate
2.
One mole of magnesium nitride on reaction with excess of water gives :
(A) Two mole of HNO3
(B) Two mole of NH3
(C) 1 mole of NH3
(D) 1 mole of HNO3
3.
Reactivity order of group 2 elements with water is :
(A) Be > Mg > Ca > Sr > Ba
(B) Ba > Sr > Ca > Mg > Be
(C) Ba > Mg > Sr > Ca > Be
(D) Be > Ba > Sr > Ca > Mg
4.
Which of the following sulphates is most stable for following change ?
D
MSO4 ¾¾
® MO + SO3
(A) BeSO4
(B) MgSO4
(C) CaSO4
(D) BaSO4
5.
Which of the following gas is produced when group 2 metal reacts with HCl ?
(A) Cl2
(B) OCl2
(C) H2
(D) O2
6.
Beryllium hydride is obtained by :
(A) Heating Be in atmosphere of H2
(C) Action of BeCl2 with LiAlH4
(B) Action of Be with CaH2
(D) None of these
7.
Anhydrous MgCl2 can be prepared by heating MgCl2. 6H2O :
(A) in a current of dry HCl(g)
(B) with carbon
(C) until it fuses
(D) with CaO
8.
The hydride from amongst the following that cannot be obtained directly by reaction with hydrogen
is :(A) CaH2
(B) MgH2
(C) BeH2
(D) NaH
9.
Alkaline earth metals forms basic hydroxide. Which of the following metal hydroxide is the least
basic ?
(A) Mg(OH)2
(B) Ca(OH)2
(C) Sr(OH)2
(D) Ba(OH)2
10.
Pick the incorrect statements about beryllium :
(A) Compounds of beryllium are readily hydrolysed.
(B) BeCl2 fumes in moist air.
(C) solid BeH2 is planar.
(D) BeCl2 (like AlCl3) is covalent.
236
s-Block
11.
Beryllum shows diagonal relationship with aluminium. Which are of the following properties is not
shown by both ?
(A ) BeO & A l 2O2 are amphoteric.
(B) Be2C & Al4C3 are methanides.
(C) Both have same maximum covalency.
(D) Both become passive in conc. HNO3 .
12.
Which of the following gives precipitate only on heating .
(A) BaCO3(s)
(B) Mg(HCO3)2(aq)
(C) KHCO3(aq)
(D) All
13.
Which of the following is formed on reaction of Be with excess KOH ?
(A) BeO + H2
(B) K2[Be(OH)4] + H2 (C) BeH2 + K2O
(D) None of these
14.
High temp.
X + C + Cl2 ¾¾¾¾
® Y + CO
Y + 2H2O ¾¾
® Z + 2 HCl
Compound Y is found as polymeric chain structure and is an electron deficient molecule. The compound
Y is:
(A) BeO
(B) BeCl2
(C) Be(OH)2
(D) BeO.Be(OH)2
15.
16.
MULTIPLE CORRECT ANSWER TYPE
Compounds which are almost insoluble in water is/are
(A) Be(OH)2
(B) BaSO4
(C) Be(NO3)2
(D) Ba(OH)2
Which form blue coloured solution with liquid NH3?
(A) Be
(B) Ca
(C) Sr
(D) Ba
17.
Halides (Cl, Br and I) of alkaline earth metals which can not be dehydrated by heating alone is/
are:
(A) Ca
(B) Mg
(C) Ba
(D) Be
18.
Which carbide produces ethyne when it reacts with water ?
(A) Be2C
(B) BaC2
(C) CaC2
(D) Mg2C3
COMPREHENSION TYPE
Several group-2 metals dissolve in excess of liquid NH3 and form solution. This solution is example
of true solution.
19.
20.
Solution is bright blue coloured due to :
(A) High extent of hydration.
(C) Ammoniated metal ions
Bright blue solution is/has :
(A) Diamagnetic
(C) non-conducting nature
(B) Solvated electrons
(D) Hydrated metals
(B) Reducing ability
(D) excellent oxidiser
237
JEE-Chemistry
21.
Element
(1) Be
(2) Ba
(3) Sr
(4) Ca
Codes :
(1) (2)
(A) R
P
(B) P
S
(C) S
Q
(D) Q
R
MATRIX MATCH TYPE
Property
(P) least density among group ‘2’ elements
(Q) Highest second ionisation energy among group ‘2’ elements
(R) strongest reducing ability among group ‘2’ elements
(S) crimson colour in flame test
(3)
S
Q
P
S
(4)
Q
R
R
P
22.
INTEGER ANSWER TYPE
How many element(s) are called alkaline earth metals?
Be, Ba, Ca, Mg, Sr, K, Rb, Cs
23.
The maximum covalency of Be can be :
24.
How many of the following react with both acid and base?
Be, Mg, Ca, Sr, Ba
25.
On heating calcium hexa ammoniate, NH3 and H2 are evolved. How many moles of NH3 are
evolved when 1.5 moles of calcium ammoniate are heated ?
238
s-Block
SOME IMPORTANT GROUP -2 METAL COMPOUNDS
1.
2.
SINGLE CORRECT ANSWER TYPE1
By adding gypsum to cement :
(A) setting time of cement becomes less
(B) setting time of cement increases
(C) colour of cement becomes light
(D) shining surface is obtained
The alkaline earth metal present in chlorophyll is :
(A) Be
(B) Mg
(C) Sr
(D) Ba
3.
Which of the following statement is true about Ca(OH) 2?
(A) It does not react with HCl (aq.)
(B) Its suspension in water is called lime water
(C) It is water insoluble
(D) It is a base
4.
The process of setting of cement under water is essentially :
(A) An oxidation process
(B) A reduction process
(C) A double decomposition process
(D) A hydration process
5.
Gypsum CaSO4.2H2O on heating to about 120ºC forms plaster of paris which has chemical
composition represented by :
(A) 2CaSO4.3H2O
(B) CaSO4.H2O
(C) 2CaSO4.H2O
(D) CaSO4
6.
On passing excess of CO2 in lime water, its milky appearance disappears because (A) Soluble Ca(OH)2 is formed
(B) Soluble Ca(HCO3)2 is formed
(C) Reaction becomes reversible
(D) Calcium compound evaporated
7.
Ca(OH)2 + dry Cl2 ® A ; A is
(A) washing soda
(B) Bleaching powder (C) Quick lime
8.
D
CaO + P4O10 ¾¾
® products ; products are :
(A) Ca3P2 + O2
9.
10.
11.
(D) Calcium chloride
(B) Ca3(PO4)2
(C) Ca3P2 + P4
(D) None of these
MULTIPLE CORRECT ANSWER TYPE
Portland cement does not contain
(A) Ca3(PO4)2
(B) Ca3Al2O6
(C) BeCl2
(D) BaCO3
CaCO3 gives CO2 on :
(A) Thermal decomposition
(C) reaction with NaCl
Compound
(1) CaO(s)
(2) Ca(OH)2 (s)
(3) CaCO3 (s)
(4) Ba(OH)2 (aq.)
(B) reaction with dil.HCl
(D) reaction with dil. H2SO4
MATRIX MATCH TYPE
Name
(P) Lime stone
(Q) Baryta water
(R) Quick lime
(S) slaked lime
239
JEE-Chemistry
Codes :
(1)
(A) R
(B) P
(C) S
(D) Q
(2)
S
S
Q
R
(3)
P
Q
P
S
(4)
Q
R
R
P
INTEGER ANSWER TYPE
12.
Gypsum on heating to 120ºC gives a hemihydrate (X). The difference in molar mass of gypsum
and X is 9Y. What is the value of Y ?
13.
When 1mole CaSO4. 2H2O(s) is heated at 393 K, number of moles of water molecules removed is
14.
For a good quality of cement, mass ratio ç SiO + Al O + Fe O ÷ ; x . What is the value of x ?
è
2
2 3
2 3 ø
15.
How many water of crystallisations are there in dead burnt plaster ?
æ
CaO
240
ö
s-Block
MISCELLANEOUS
1.
SINGLE CORRECT ANSWER TYPE
Which of the following pairs can be distinguished by the action of heat ?
(I) Na2CO3 &CaCO3
(II) MgCl2 . 6H2O & CaCl2 .6H2O
(III) Ca(NO3)2 & NaNO3
(A) I & II only
(B) I, II & III all
(C) I & III only
(D) I Only
2.
Which of the following is used for taking X-ray spectra of the digestive system?
(A) K2CO3
(B) BaSO4
(C) Mg(OH)2
(D) NaOH
3.
One mole of a substance (A) on reacting with excess of water, gives two mole of readily combustible
gas and alkaline solution. The alkaline solution gives white turbidity with CO2. The substance (A) is
(A) CaH2
(B) NaH
(C) Ca(OH)2
(D) NaNO3
4.
5.
6.
7.
8.
9.
10.
MULTIPLE CORRECT ANSWER TYPE
Which of the following pair give at least one common hydrolysis product ?
(A) NaH and CaH2
(B) AlN and Mg3N2
(C) CaC2 and Li2C2
(D) Mg3N2 and Li3N
Which s-block element shows crimson red colour in flame ?
(A) Lithium salt
(B) Rubidium salt
(C) Barium salt
(D) Strontium salt
Which of the following compounds is polymeric in nature?
(A) BeCl2(g)
(B) NaH(s)
(C) BeCl2(s)
(D) BeH2(s)
Which of the following are correct for comparison : Be > Li ?
(A) Hardness
(B) Density
(C) Reactivity
(D) Melting point
Select the correct statement(s) :
(A) Common salt absorbs water due to presence of impurities of Ca, Mg compounds.
(B) Size of Li+ is more than that of Mg2+.
(C) Mg is more electropositive than Na
(D) Mg(OH)2 is less basic than NaOH
INTEGER ANSWER TYPE
Consider following compounds:
Na2O2, CsO2, O2, KO3, Li2O, Na in liq. NH3 (concentrated solution), BaO2, Ca in liq
NH3(dil.solution) , Mg3N2
How many are paramagnetic ?
How many metals dissolve in excess of aq. NH3 to form blue coloured solution ?
Na, Be, Ca, Mg, Ba, K, Rb, Sr, Li
241
JEE-Chemistry
ANSWER KEY
GENERAL PHYSICAL AND ATOMIC PROPERTIES OF GROUP -1
METALS
1.
(D)
2.
(C)
3.
(A)
4.
(C)
7.
(A)
8.
0
9.
1
10.
0
5.
6.
(A)
(B)
GENERAL CHEMICAL PROPERTIES OF GROUP-1 METALS
1.
(A)
2.
(C)
3.
(C)
4.
(B)
5.
(A)
7.
(D)
8.
(C)
9.
(D)
10.
(A) (B)
11.
(C)(D)
12.
(A)(B)(C)(D)
13.
(B)(C)(D) 14.
(A)(D)
15.
A- Q; B- R,S; C-P,Q,R,S ; D-P
17.
3
18.
3
19.
3
6.
16.
A- P; B-P,Q,R; C-P,Q,R,T ; D-Q,S
20.
zero
(D)
SOME IMPORTANT ALKALI METAL COMPOUNDS
1.
(D)
2.
(D)
3.
7.
(C)
8.
(A) (B) (C) (D)
12.
A-R; B-S; C-P; D-Q
(B)
13.
6
4.
(A)
5.
9.
(A)(B)(C) 10.
14.
9
15.
6.
(D)
(A)(B)(C) 11.
(A)
(B)(C)
4
GENERAL PHYSICAL , ATOMIC AND CHEMICAL PROPERTIES
OF GROUP -2 METALS
1.
(B)
2.
(B)
3.
(B)
4.
(D)
5.
(C)
6.
(C)
7.
(A)
8.
(C)
9.
(A)
10.
(C)
11.
(C)
12.
(B)
13.
(B)
14.
(B)
15.
(A)(B)
16.
(B)(C)(D) 17.
(B)(D)
18.
(B)(C)
19.
(B)
20.
(B)
21.
(D)
22.
23.
4
24.
1
25.
6
SOME IMPORTANT GROUP -2 METAL COMPOUNDS
1.
(B)
2.
(B)
3.
(D)
4.
7.
(B)
8.
(B)
9.
(A)(C)(D) 10.
13.
1.50
14.
2
15.
0
(D)
5.
(A)(B)(D) 11.
(C)
6.
(B)
(A)
12.
3
MISCELLANEOUS
1.
(B)
2.
(B)
3.
6.
(C) (D)
7.
(A) (B)(D) 8.
(A)
4.
(A) (B) (D)9.
242
5.
(A) (B) (C) (D)
4
10.
0
(A) (D)
Hydrogen & Its Compounds
HYDROGEN & ITS COMPOUNDS
H2, HYDRIDES, H & ITS ISOTOPES
1.
2.
SINGLE CORRECT ANSWER TYPE
The most abundant isotope of hydrogen is :(A) Tritium
(B) Deuterium
(C) Protium
Nascent hydrogen consists of
(A) Hydrogen ions in excited state
(C) Solvated protons
(D) Para hydrogen
(B) Hydrogen ions with excess energy
(D) Hydrogen atom
3.
Ordinary hydrogen at room temperature is a mixture of :(A) 75% o-Hydrogen + 25% p-Hydrogen
(B) 25% o-Hydrogen + 75% p-Hydrogen
(C) 50% o-Hydrogen + 50% p-Hydrogen
(D) 1% o-Hydrogen + 99% p-Hydrogen
4.
When the same amount of zinc is treated separately with excess of dilute sulphuric acid and excess of
sodium hydroxide, the ratio of volumes of hydrogen evolved is :(A) 1 : 1
(B) 1 : 2
(C) 2 : 1
(D) 9 : 4
5.
Ionic hydrides are formed by :(A) Transition metals (B) Ca, Sr, Ba
6.
(C) Carbon
(D) Boron
In Bosch's process which gas is utilised to increase the production of hydrogen :(A) Producer gas
(B) Water gas
(C) Coal gas
(D) Natural gas
MULTIPLE CORRECT ANSWER TYPE
7.
8.
9.
10.
11.
12.
At absolute zero :(A) para hydrogen exists
(C) Both para and ortho hydrogen exists
(B) no ortho hydrogen exists
(D) % of ortho hydrogen is more than para hydrogen
The adsorption of hydrogen by metals is called :(A) Dehydrogenation (B) Hydrogenation
(C) Occlusion
(D) Adsorption
Which of the following is / are same for Ortho and Para hydrogen :(A) In the number of protons
(B) In the molecular mass
(C) In the nature of spins of nucleus
(D) In the nature of spin of electrons
MATRIX MATCH TYPE
Column-I
Column-II
(Hydride)
(Classification)
(A) BaH2
(P) Covalent hydride
(B) SiH4
(Q) Polymeric hydride
(C) B2H6
(R) Salt like hydride
(D) (BeH2)n
(S) Electron defecient hydride
INTEGER ANSWER TYPE
Find out the sum of protons, electrons and neutrons in the heaviest isotope of hydrogen.
Find out the value of 'x' in ion [HxO4]+ .
243
JEE-Chemistry
H2O, D2O, H2O2
1.
2.
3.
SINGLE CORRECT ANSWER TYPE
High boiling point of water is due to
(A) Its high specific heat
(B)Hydrogen bonding
(C) High dielectric constant
(D) Low dissociation constant
Calgon is an industrial name given to
(A) Normal sodium phosphate
(C) Sodium hexametaphosphate
(B) Sodium meta-aluminate
(D) Hydrated sodium aluminium silicate
Water softening by Clarke’s process uses
(A) Calcium bicarbonate
(C) Potash alum
(B) Sodium bicarbonate
(D) Calcium hydroxide
4.
The bleaching properties of H2O2 are due to its
(A) Reducing properties
(B) Oxidising properties
(C) Unstable nature
(D) Acidic nature
5.
Hydrogen peroxide has a
(A) Linear structure
(C) Closed book type structure
6.
7.
(B) Pyramidal structure
(D) Half open book type structure
The hybridisation of the orbitals of oxygen in H2O2 is: (A) sp3d
(B) sp
(C) sp2
H2O2 is always stored in dark bottles because
(A) It is highly unstable
(C) It undergoes auto decomposition in light
(D) sp3
(B) Its enthalpy of decomposition is high
(D) None of these
8.
The reaction, H2S + H2O2 ® S + 2H2O manifests:
(A) Acidic nature of H2O2
(B) Alkaline nature of H2O2
(C) Oxidising nature of H2O2
(D) Reducing nature of H2O2
9.
Determine the degree of hardness of a sample of water containing 30 ppm of MgSO4.
(A) 20 ppm
(B) 25 ppm
(C) 30 ppm
(D) 35 ppm
10.
Which of the following metal does not give hydrogen gas on reacting with dil.HCl ?
(A) Zn
(B) Na
(C) K
(D) Au
1.
7.
11.
1.
7.
(C)
(A)(B)
4
(B)
(C)
2.
8.
12.
2.
8.
ANSWER KEY
H2, HYDRIDES, H & ITS ISOTOPES
(D)
(C)(D)
9
(C)
(C)
3.
9.
3.
9.
(A)
4.
(A)(B)(D) 10.
(A)
5.
(B)
6.
(B)
(A)-(R),(B)-(P), (C)-(P)(S), (D)-(P)(Q)(S)
H2O, D2O, H2O2
(D)
(B)
4.
10.
244
(B)
(D)
5.
(D)
6.
(D)
p-Block Elements
BORON FAMILY- I
1.
SINGLE CORRECT ANSWER TYPE
Boron has an extremely high melting point because of :
(A) The strong vander Waals forces between its atoms
(B) The strong binding forces in the covalent polymer
(C) Its ionic crystal structure
(D) Allotropy
2.
Aluminium does not react with pure water as (A) Impurities in water are essential for the reaction to occur
(B) It is protected by a film of aluminium oxide
(C) It is light metal
(D) It is not a reactive metal
3.
The possible oxidation state of Tl are:
(A) +1 and + 2
(B) +2 and + 3
(C) +1 and -1
(D) +1 and + 3
4.
For which of the following element, there is maximum difference in its melting and boiling point ?
(A) B
(B) Al
(C) Ga
(D) In
5.
Select correct statement :
(A) Trihalides of boron do not act as Lewis acid.
(B) Ga has more density in solid state than in liquid state.
(C) Ga has unusually high boiling point.
(D) Ga has high melting point.
6.
Consider following reaction(s).
(I) H2 gas is evolved on reaction of Al with conc HNO3.
(II) H2 gas is evolved on reaction of Al with dil.HCl.
(III) H2 gas is evolved on reaction of Al with aqueous NaOH solution
Correct statement (s) is/are:
(A) I &II only
(B) II & III Only
(C) I&III only
(D)All
7.
M+X2 ® M+1 (X3)-1
For which combination of metal and halogen, the above reaction is correct ?
(A) M = Boron, X = F2
(B) M = Boron, X = I2
(C) M = Thallium, X= F2
(D) M= Thallium, X = I2
8.
Choose correct statement(s) regarding group-13 :
(A) All trihalides of Al exist in dimeric form
(B) Fluoride being ionic do not dimerize, so AlF3 is monomeric
(C) Only AlF3 dimerize while rest exist in monomeric form
(D) none of these .
245
JEE-Chemistry
9.
MULTIPLE CORRECT ANSWER TYPE
Mark the correct statement(s) regarding BF3 :
(A) It acts as a Lewis acid
(B) If forms an addition compound with NH 3
(C) It is a Volatile liquid at room temperature
(D) It combines with ether to form an adduct
10.
Which of the following is/are incorrect in case of boron nitride :
(A) It is also called borazine
(B) It is aromatic
(C) It contains B-H bonds
(D) It has no s-bond
11.
Choose the correct statement(s) regarding group-13 elements :
(A) Stability of +1 oxidation state increases down the group.
(B) Ability to form multiple bonds with other second period elements is maximum for boron.
(C) Stability of +3 oxidation state decreases down the group.
(D) Boron is a typical non-metal and forms covalent bond.
12.
Choose correct statement(s) :
(A) Al2O3 and Ga2O3 are amphoteric oxides.
(B) Boron reacts with dil.HCl to evolve H2 gas.
(C) Aluminium becomes passive in conc.HNO3.
(D) Boron reacts with molten NaOH to form Na3BO3 & evolve H2 gas.
13.
How many exist in dimeric form in gaseous state ?
(A) BH3
(B) BF3
(C) AlF3
14.
15.
(D) AlCl3
INTEGER ANSWER TYPE
How many of the following properties do not strictly increase or decrease down the group (gp 13)?
Ionisation energy, melting point, boiling points, electronegativity, density
Maximum how many atoms are in single plane in B2H6?
246
p-Block Elements
BORON FAMILY- II
SINGLE CORRECT ANSWER TYPE
1.
Heat
Heat
Na2B4O7·10H2O ¾¾¾
® X + NaBO2 + H2O, X + Cr2O3 ¾¾¾®
X and Y are :
(A) Na3BO3 and Cr(BO2)3
(C) B2O3 and Cr(BO2)3
2.
Y
(Green coloured)
;
(B) Na2B4O7 and Cr(BO2)3
(D) B2O3 and CrBO3
Borax is converted into crystalline boron by the following steps:
Y
X
D
® B
Borax ¾¾
® H3BO3 ¾¾® B2O3 ¾¾
D
X and Y are respectively:
(A) HCl, Mg
(B) HCl, C
(C) C, Al
(D) HCl, Al
3.
Which mixed sulphate is not an alum ?
(A) K2SO4.Al2(SO4)3.24H2O
(C) Na2SO4.Fe2(SO4)3.24H2O
(B) K2SO4.Cr2(SO4)3.24H2O
(D) CuSO4.Al2(SO4)3.24H2O
4.
Reactivity of borazole is greater than that of benzene because : (A) Borazole is non-polar compound
(B) Borazole contains polar bonds
(C) Borazole is electron deficient compound
(D) of delocalized electrons in it
5.
On hydrolysis, diborane produces :
(A) H3BO2 + H2O2 (B) H3BO3 + H2
6.
(C) B2O3 + O2
(D) H3BO3 + H2O2
By which of the following reactions is borazine prepared ?
low temperatur e
(A) B2H6 + NH3 (excess) ¾¾
¾ ¾¾ ¾
¾®
high temperatur e
(B) B2H6 + NH3 (excess) ¾¾
¾ ¾¾ ¾
¾®
( ratio 2NH3 : 1B2H6 )
¾¾ ¾¾¾
¾®
(C) B2H6 + NH3 ¾¾high
temperatur e
(D) None of these
7.
Anhydrous aluminium chloride fumes in moist air owing to the formation of:
(A) gaseous aluminium chloride
(B) chlorine
(C) chlorine dioxide
(D) hydrogen chloride
8.
Potash Alum is a double salt made up of two salts
(A) Salt of a (SA + WB) + Salt of a (WA + WB)
(B) Salt of a (SA + SB) + Salt of a (SA + WB)
(C) Salt of a (SA + SB) Salt of a (WA + WB)
(D) Salt of a (SA + WB) + Salt of a (WA + WB)
247
JEE-Chemistry
9.
Alum is found to contain hydrated monovalent cation [M(H2O)6]+, trivalent cation [M’(H2O)6]+3
and SO42– in the ratio of :
(A) 1 : 1 : 1
(B) 1 : 1 : 2
(C) 1 : 2 : 2
(D) 1 : 2 : 3
10.
Choose correct order of acidic strength :
(A) H3BO3 > HCl
(B) Al2O3 > B2O3
(C) Tl2O > Tl2O3
11.
Al2O3 can be converted to anhydrous AlCl3 by heating :
(A) hydrated Al2O3 with Cl2 gas
(B) Al2O3 with aqueous HCl
(C) Al2O3 with NaCl in solid state
(D) a mixture of Al2O3 and carbon in dry Cl2 gas
12.
D
cooling
B2O3 + Al ¾¾
® X + Al2O3 ; X ¾¾¾
® Y
Y is obtained in :
(A) Liquid state
(C) Amorphous form
(B) Crystalline form
(D) None of these
13.
When borax is treated with mineral acids, the product formed is
(A) Boron oxide
(B) Orthoboric acid
(C) Metaboric acid
(D) Pyroboric acid
14.
Choose correct order:
(I) BCl3 > AlCl3 (lewis acidic strength)
(II) BF3 > BCl3 (lewis acidic strength)
(A) I only
(B) II only
15.
16.
17.
(D) None of these
(C) Both
(D)None
Potash alum on reaction with excess of NaOH solution gives following species :
(A) Al3+(aq), SO24- (aq), K+ (aq)
(B) Al(OH)3¯, SO24- (aq), K+(aq)
(C) [Al(OH)4]–1(aq), SO24- (aq), K+(aq)
(D) Al2O3¯, SO24- (aq), K+(aq)
MULTIPLE CORRECT ANSWER TYPE
Identify correct statement(s) regarding structure of diborane :
(A) There are two bridging hydrogen atoms.
(B) Each boron atom forms four bonds.
(C) All hydrogen atoms are not in the same plane.
(D) Each boron atom is in sp3 hybridised state.
Al2(SO4)3 + NH4OH ® X(contains Al) ; X is
(A) A white gelatinous precipitate.
(B) Insoluble in excess of NH4OH.
(C) Soluble in excess of NaOH.
(D) Amphoteric in nature.
248
p-Block Elements
18.
19.
In how many of the reactions at least one product is common?
(I): B2H6 + H2O ®
D
(II): H3BO3 + C2H5OH ¾¾
®
(III): B2H6 + C2H5OH ®
(A) I & II
(B) II & III
(C) I & III
(D) none of these
In which of the following reaction(s), B2O3 is obtained as one of the product(s)?
D
D
(A) B2H6 + O2 ¾¾
(B) Na2B4O7.10H2O ¾¾
®
®
(D) B2H6 + H2O ®
Strong
®
(C) H3BO3 ¾¾¾
heating
COMPREHENSION TYPE
A white precipitate (X) is formed when a mineral (A) is boiled with Na2CO3 solution. The precipitate
is filtered and filtrate contains two compounds (Y) and (Z).
The compound (Y) is removed by crystallization and when CO2 is passed through the filtrate obtained
after crystallization, then (Z) changes to (Y). When compound (Y) is heated, it gives two compounds
(Z) and (T).
Compound (T) on heating with cobalt oxide produces blue coloured substance (S).
20.
The mineral (A) is :
(A) Na2B6O11
(B) CaCO3
(C) Ca2B6O11·5H2O
(D) B2O3
21.
The compound (Y) in the filtrate, when (A) is boiled with Na2CO3, is :
(A) NaBO2
(B) Na2B4O7
(C) Na3BO3
(D) CaO
22.
When cobalt oxide is heated with (Y), then a bead (S) is formed which is blue in colour. The bead (S)
is
(A) CoCO3
(B) Co(BO2)2
(C) CoO
(D) B2O3
MATRIX MATCH TYPE
Property
(P) Amphoteric element
(Q) Highest melting point in group 13 elements
(R) Oxide(E2O3) is basic
(S) +1 oxidation state is more stable than +3
(T) Least melting point in group 13 elements
23.
(Element)
(A) B
(B) Al
(C) Ga
(D) Tl
24.
Match the following List-I and List-II
List-I
List-II
(A) A1Cl3
(P) Lewis acid
(B) BCl3
(Q) Forms acidic solution
(C) B2H 6
(R) Sublimes on heating
(D) Alum
(S) Swells on heating
249
JEE-Chemistry
25.
List-I
(A) H3BO 3
(B) B2H 6
(C) Al2O3
(D) TlOH
List-II
(P) Hydrogen bonds
(Q) Amphoteric oxide
(R) Basic
(S) Lewis acid
26.
INTEGER ANSWER TYPE
No. of p-bonds in a molecule of borazole is :
27.
In borax, the number of boron atoms involved in sp3 hybridisation is :
28.
The number of water molecules co-ordinated to each monovalent cation in alum is :
29.
Number of tetrahedral boron atoms in colemanite, Ca2B6O11.5H2O, is :
30.
B2H6 + LiH ® product
How many orbitals are utilised by each boron atom in hybridisation in product ?
250
p-Block Elements
CARBON FAMILY- I
1.
2.
3.
4.
5.
SINGLE CORRECT ANSWER TYPE
Which of the following is most abundant group 14 element in earth’s crust ?
(A) C
(B) Si
(C) Ge
(D) Sn
Which halide is most stable towards hydrolysis ?
(A) CX4
(B) SiX4
(C) PbX4
(D) SnX4
C-C bond length is maximum among given for :
(A) Graphite
(B) Diamond
(C) H2C = CH2
(D) Benzene
Diamond is highly unreactive due to :
(A) High C-C bond order
(C) Strong C-C covalent bond
(B) Presence of impurities
(D) High bond polarity
CO2 is not produced in :
(A) CaCO3 + HCl(aq.) ®
D
(B) NaHCO3 ¾¾
®
(D) K4[Fe(CN)6] + H2SO4(conc) ®
(C) Fe2O3 + CO ®
6.
Which of the following is called sheet silicate ?
–
O
–O
(A)
–O
O
–
O
–
(B)
–
O
O O O
O
–
O
–
O–
O
(C)
O
O
–
O
(D)
O
O
–
O
7.
Mg(SixOy).Mg(OH)2 is formula of Talc. It is a sheet silicate. The value of x is :
(A) Less than y.
(B) More than y.
(C) equal to y.
(D) Zero.
8.
Choose the incorrect statement about buckminster fullerene , C60 :
(A) It has 60 vertices having C atom(s) at each vertex.
(B) Has 20 hexagons & 12 pentagons.
(C) hexagon can fuse with only hexagon but pentagon can fuse with both hexagon and pentagon
(D) Since no dangling bonds are present, so fullerenes are purest form of carbon.
9.
Which is thermodynamically most stable allotrope of carbon ?
(A) Diamond
(B) Graphite
(C) Fullerenes
10.
(D) None of these
MULTIPLE CORRECT ANSWER TYPE
Which is/are not affected by H2O(l) at 25°C ?
(A) C
(B) Si
(C) Ge
(D) Pb
251
JEE-Chemistry
11.
C-C covalent bond exists in :
(A) Al4C3
(B) CaC2
(C) Mg2C3
12.
Oxidation state of Si is +4 in :
(A) Single chain silicate(B) double chain silicate
(C) Cyclic silicate
(D) Sheet silicate
13.
The amphoteric oxide(s) is/are :
(A) SnO
(B) SnO2
(C) PbO
(D) Be2C
(D) PbO2
14.
Which of the following is/are correct for group 14 element ?
(A) The stability of dihalides are in the order CX2 < SiX2 < SnX2 < PbX2.
(B) The ability to form pp – pp multiple bonds among themselves increases down the group.
(C) The tendency for catenation decreases down the group.
(D) Dioxides are more acidic than coresponding monoxides.
15.
Choose correct statement(s) :
(A) CO> SnO > PbO (reducing power)
(C) CO2 > SnO2 > PbO2 (acidic strength)
16.
17.
Column-I
Compound
(A) CaC2
(B) B4C
(C) WC
(D) Be2C
(B) CO2 > SnO2 > PbO2 (Oxidising power)
(D) SnO > PbO (basic strength)
MATRIX MATCH TYPE
Column-II
Property
(P) Ionic carbide
(Q) Covalent carbide
(R) Interstitial carbide
(S) Acetylide
(T) Methanide
INTEGER ANSWER TYPE
How many of the following have three dimensional structure ?
Diamond, fullerenes, SiO2, CO2, Cyclic silicate, C3O2
18.
Consider following oxides :
CO, CO2, SiO2, SnO, SnO2, PbO, PbO2
Let the number of neutral oxides = x and the number of amphoteric oxides = y
Find x + y :
19.
The sum of covalencies per atom (for all different elements) present in a non-elemental compound
(x) formed in the given reaction is :
D
C + SiO2 ¾¾
® X + CO
20.
Total number of covalent bonds in C3O2 is :
252
p-Block Elements
CARBON FAMILY- II
1.
2.
3.
4.
5.
6.
7.
Si
O Si linkage is present in :
(A) Straight chain silicone
(C) Cross-linked silicone
(B) Cyclic silicone
(D) All of these
SnCl2 can reduce ;
(A) FeCl3
(C) Hg2Cl2
(B) HgCl2
(D) All of these
A colourless diatomic gas is produced in :
D
(A) PbO2 + HCl ¾¾
®
(C) SnO2 + HCl ®
D
(B) Pb3O4 + H2SO4 ¾¾
®
(D) CO + I2O5 ®
Most acidic oxide among given is :
(A) CO
(B) CO2
(C) SnO
(D) PbO
Most stable allotrope of Sn is :
(A) Grey tin
(B) White tin
(C) Rhombic tin
(D) None of these
Maximum catenation ability is shown by :
(A) C
(B) Si
(C) Ge
(D) Pb
Which of the following gives paramagnetic gas readily on heating ?
(A) PbO
(B) SnO
(C) PbO2
(D) CO2
8.
In which of the following silicates, only two corners per tetradron are shared ?
(I) Pyrosilicate
(II) Cyclic silicate
(III) Double chain silicate
(IV) Single chain silicate
(V) 3D silicate
(VI) Sheet silicate
(A) I, II, III
(B) IV and VI only
(C) I & VI only
(D) II and IV only
9.
SnCl
SnCl2 + HgCl2 ® products ¾¾¾
® A(grey ppt)
A is :
(A) SnCl4
(B) Hg2Cl2
(C) Hg
2
(D) Sn
10.
Choose correct statement(s) regarding zeolites:
(A) They are 3 – D silicates
(B) Hydrated zeolites are used as water softeners
(C) ZSM–5 catalyses conversion of alchols to gasoline
(D) All of these
11.
An inorganic compound (A) made by two most occurring elements in the earth crust has polymeric
tetrahedral network structure. With carbon, compound (A) produces a poisonous gas (B) which is the
most stable diatomic molecule. Compound (A) and (B) will be
(A) SiO2, CO2
(B) SiO2, CO
(C) SiC, CO
(D) SiO2, N2
253
JEE-Chemistry
12.
13.
14.
15.
16.
When oxalic acid is heated with cone. H2SO4, two gases produced are neutral and acidic in nature
respectively. Potassium hydroxide absorbs one of the two gases. The product formed during this
absorption and the gas which is absorbed, are respectively :
(A) K2CO3 and CO2 (B) H2CO3 and CO2 (C) K2CO3 and CO
(D) KHCO3 and CO
MULTIPLE CORRECT ANSWER TYPE
In silcones, R2SiO is repeating unit ; where R can be :
(A) Alkyl group
(B) Aryl group
(C) Hydrogen
(D) Nitrogen
Mixed oxide of Pb is/are :
(A) PbO2
(B) Pb3O4
(C) Pb2O3
(D) PbO
Allotropy is exhibited by :
(A) Si
(B) C
(C) Sn
(D) Pb
Which of the following carbides yield CH4 gas on hydrolysis ?
(A) Al4C3
(B) Be2C
(C) Mg2C3
(D) Na2C2
17.
Consider following reaction:
PbO2 + HCl ®
Now choose correct option.
(A) Since PbO2 is amphoteric, it will act as base
(B) PbO2 will oxidize HCl to Cl2 & itself get reduced to PbCl2
(C) PbO2 wil undergo intramolecular redox to form PbCl2 and O2 in presence of HCl as medium
(D) None of these
18.
D
PbO2 + H2SO4 ¾¾
® X(g) + Y + H2O
D
H2O2 + Z ¾¾
® Y + H2O
Choose correct options:
(A) X is a paramagnetic gas
(C) Z is PbS
(B) X is diamagnetic
(D) Y is insoluble in water
COMPREHENSION TYPE
Carbides are of three types;
Ionic, covalent and interstitial. CaC2 is one of the commercially important ionic carbide.
D
X+C ¾¾
® CaC2+CO
D
CaC2 + Y ¾¾
® Z+C
Z + H2O ® NH3 + CaCO3
‘Z’ is an important nitrogenous fertilizer.
19.
‘X’ is
(A) CaO
(B) CaCO3
(C) Ca (OH)2
254
(D) CaCl2
p-Block Elements
20.
21.
22.
Y and Z respectively are:
(A) N2O and CaCN2
(C) N2 and Ca(CN)2
(B) (CN)2 and CaCN2
(D) N2 and CaCN2
Column-I
(Silicate)
(A) Sheet silicate
(B) 3D silicate
(C) Double chain silicate
(D) Pyrosilicate
MATRIX MATCH TYPE
Column-II
(No. of oxygen shared by each tetrahedral unit)
(P) 2
(Q) 3
(R) 4
(S) 1
INTEGER ANSWER TYPE
What is the value of x in given silicate :
II
III
Na 2 Fe3 Fe x [Si 4 O11 ]2 (OH) 2
23.
In how many of the following given species, all the atoms are present in same plane?
C3O2, C3H4, CO2, C60, diamond, silica, cross linked silicones, chain silicones and orthosilicates.
24.
A compound (X) when heated with conc.H2SO4 gives only one gaseous product, which under
pressure forms sodium methanoate (HCOONa) with NaOH. How many of the following can be X
?
HCOOH, K4[Fe(CN)6], H2C2O4, PCl5
25.
12In cyclic silicate ion Si6 O18
, the number of oxygen atoms shared is :
255
JEE-Chemistry
ANSWER KEY
BORON FAMILY- I
1.
(B)
2.
(B)
3.
(D)
4.
7.
(D)
8.
(B)
9.
(A)(B)(D) 10.
12.
(A)(C)(D) 13.
(A)(D)
14.
3
15.
(C)
5.
(A)(C)(D) 11.
(C)
6.
(B)
(A)(B)(C)(D)
6
BORON FAMILY- II
1.
(C)
2.
(D)
3.
(D)
4.
(B)
5.
(B)
6.
(C)
7.
(D)
8.
(B)
9.
(B)
10.
(D)
11.
(D)
12.
(B)
13.
(B)
14.
(A)
15.
(C)
16.
(A)(B)(C)(D)
17.
(A)(B)(C)(D)
18.
(B)(C)
19.
(A)(B)(C) 20.
(C)
21.
(B)
22.
(B)
24.
(A)-PQR ; (B)-PQ ; (C)-PQ ; (D)-QS
26.
3
23.
27.
(A)-Q; (B)-P ; (C)-P,T ; (D)-R,S
2
28.
6
25.
(A)-PS ; (B)-S ; (C)-Q ; (D)-PR
29.
4
30.
4
5.
(D)
CARBON FAMILY- I
1.
(B)
2.
(A)
3.
(B)
4.
(C)
7.
(A)
8.
(C)
9.
(B)
10.
(A)(B)(C)(D)
12.
(A)(B)(C)(D)
13.
(A)(B)(C)(D)
16.
(A)-P,S ; (B)-Q ; (C)-R ; (D)-P,T
20.
8
17.
4
6.
(C)
11.
(B)(C)
14.
(A)(C)(D) 15.
(A)(C)
18.
5
19.
8
CARBON FAMILY- II
1.
(D)
2.
(D)
3.
(B)
4.
(B)
5.
(B)
6.
(A)
7.
(C)
8.
(D)
9.
(C)
10.
(D)
11.
(B)
12.
(A)
13.
(A)(B)
14.
(B)(C)
15.
(A)(B)(C) 16.
(A)(B)
17.
(B)
18.
(A)(C)(D) 19.
(A)
20.
(D)
23.
2
2
25.
6
24.
21.
256
(A)-Q, (B)-R, (C)-PQ, (D)-S 22.
2
p-Block Elements
Important Notes
257
JEE-Chemistry
Important Notes
258
Isomerism
ISOMERISM
STRUCTURAL ISOMERISM (EXCEPT TAUTOMERISM)
SINGLE CORRECT ANSWER TYPE
1.
(A)
(B)
(A) Chain isomers
OH
2.
(A)
OH
; compound (A) and (B) are related as :
(B) Positional isomers (C) Metamers
OH OH ; compound (A) and (B) are related as :
(B)
(A) Chain isomers
(C) Metamers
3.
(B) Positional isomers
(D) Functional isomers
; compound X and Y are related as :
X
Y
(A) Chain isomers
(C) Metamers
4.
(B) Position isomers
(D) Functional isomers
CH3 - CH 2 - CH 2 - CO 2H CH3 - CH - CH3 ; correct relation between compound (A) and (B) is
(A)
|
CO2 H
(B)
(A) Chain isomer
(B) Ring chain isomer (C) Functional isomer (D) Metamer
O
O
5.
CH3–CH2–C–O–C2H 5
X
; CH3–CH2–CH2–C–O–CH3 ; compound X and Y are mutually :
Y
(A) Chain isomers
(C) Metamers
6.
(D) Functional isomes
(B) Position isomers
(D) Functional isomers
O
O
(A)
; compounds (A) and (B) are related as :
(B)
(A) Chain isomers
(B) Functional isomers(C) Metamers
259
(D) Position isomers
JEE-Chemistry
OH
7.
(B)
(A)
(A) Chain isomer
8.
OH ; correct relation between compound (A) and (B) is :
(B) Functional isomer (C) Metamers
(D) Homologues
Which of the following pairs represent isomers ?
(A) CH3 - CH3 , CH3 - CH 2 - CH3
(B) H 2 C = CH - OH,CH 3 - O - CH3
(C) CH3 - CH 2 - CH2 - CH3 , CH3 - CH - CH 3
(D)
|
CH 3
,
9.
Which of the following represent pair of chain isomers?
(A) n-pentane, Iso-pentane
(B) n-pentane, Neo-pentane
(C) Iso-pentane, Neo-pentane
(D) All of these
10.
CH 3 - CH 2 - CH 2 - C º N; CH 3 - CH - CH 3
|
(A)
CN
(B)
Compound (A) is related to compound (B) as:
(A) Chain isomer
(B) Position isomer
(C) Functional isomer
(D) Metamers
11.
Given compound shows which type of isomerism ?
O
S—O
O
and
S—O
O
O
(A) Chain isomerism
(C) Metamerism
12.
(B) Position isomerism
(D) Functional group isomerism
MULTIPLE CORRECT ANSWER TYPE
Find correct relation for compound I, II & III :
O
CH3 – CH2 – CH2 – CHO
(I)
CH3
CH3 – CH2 – C – CH3
(II)
CH3 – CH – CHO
(III)
(A) I and III are chain isomers
(B) I and II are functional isomers
(C) II and III are position isomers
(D) I and III are metamers
260
Isomerism
13.
Which of the following pairs of structures represent isomers ?
and
(A)
(B)
O
and
O
O
OH
(C)
14.
15.
and
O
O
and
Which of the following are chain isomers ?
CH 3
|
(A) CH3CH2CH2–Cl & CH 3 - CH - Cl
CN
|
(B) CH3CH2CH2–CN & CH 3 - CH - CH 3 ( C )
CH3CH2CH2CH3 & CH 3 - CH - CH 3
|
CH 3
(D)
&
CH3
Et
Select the pair that are not chain isomers
(A )
(C)
16.
(D)
COOH
COOH
OH
(B)
and
Et
(D)
and Et
OH
and
NH2
and
Which of the following is/are the pair(s) of functional isomers ?
O
(A)
and
OH
O
(B)
O
C—O—H
and
H—C—O—
O
(C)
and
O
(D) CH3 – CH2 – O– CH2 – CH3 and CH3 – CH2 – CH2 – O – CH3
261
N
JEE-Chemistry
17.
Which of the following has CORRECT relation ?
Me
(A)
Pr
Pr
&
Me
Et
Me
(B)
Pr
&
Et
(C)
Pr
identical
Pr
positional isomers
Et
&
positional isomers
Pr
Me
Me
(D)
Pr
&
Et
homologues
18.
Which functional group cannot be present in compound having molecular formula C4H10O ?
(A) Aldehyde
(B) Ketone
(C) Acid
(D) Alcohol
19.
CH 3 - O - CH 2 - CH 2 - CH 3 ; CH 3 - CH 2 - O - CH 2 - CH 3
(B)
(A)
Possible relations between compound (A) and (B) is/are :
(A) Chain isomer
(B) Positional isomer
(C) Functional isomer
(D) Metamers
20.
Compound CH3CH2OCH3 and CH3CH2CH2OH are not :
(A) constitutional isomer
(B) configurational isomer
(C) conformational isomer
(D) stereochemical isomer
262
Isomerism
STRUCTURAL ISOMERISM (TAUTOMERISM)
SINGLE CORRECT ANSWER TYPE
O
OH
O
1.
(II)
(I)
(III)
The tautomer of compound II is :
(A) I
(B) III
(C) both I and III
O
O
(D) none of these
O
O
2.
CH3
CH3
CH3
CH3
CH3
(I)
(III)
(II)
Identify which can exhibit tautomerism?
(A) I only
(B) II only
3.
(C) III only
Among the following compounds, the one which will not show keto-enol tautomerism is :
O
O
O
(A)
4.
(D) all of these
(B)
O
CH3 (C)
CH3
(D)
O
Tautomer of the following compound is :
O
O
C – CH2 – C
(A)
C – CH = C
O
(C)
C – CH2 – C
OH
OH
CH – CH = CH
OH
(B)
(D)
C – CH2 – C
O
OH
263
O
OH
O
JEE-Chemistry
5.
Which statement is correct for Keto-enol tautomerism ?
(A) Tautomersim is catalysed by either acid or base.
(B) Tautomers are present in dynamic equilibrium state.
(C) Generally keto form is more stable than enol form.
(D) All of the above
O
O
O
O
O
6.
O
(I)
(II)
(III)
Which among the above compounds can exhibit tautomerism ?
(A) I only
(B) II only
(C) I and II
O
7.
OH
(D) II and III
OH
+
(X)
(Y)
(Z)
8.
Stability order among these tautomer is :
(A) X > Y > Z
(B) Y > X > Z
(C) Z > X > Y
(D) Y > Z > X
Keto and enol forms of a compound are related to each other as:
(A) resonance structures
(B) conformations
(C) configurational isomers
(D) constitutional isomers
9.
Which of the following compound will not undergo tautomerism ?
OH
(A)
10.
O
O
O
(B)
(C)
(D)
Which of the following compound will undergo tautomerism ?
O
O
(A)
(B)
O
O
O
(C)
O
264
C
H
(D)
CH3
Isomerism
MULTIPLE CORRECT ANSWER TYPE
11.
Which of the following statements is/are not correct?
(A) Metamerism belongs to the category of structural isomerism
(B) Tautomeric structures are the resonating structures of a molecule
(C) Keto form is always more stable than the enol form
(D) Geometrical isomerism is shown only by alkenes
12.
13.
Which of the following compounds show tautomerism?
O
||
(A) NH 2 - C - NH 2
S
||
(B) NH 2 - C- NH 2
O
||
(C) CH3 - C - CH3
(D) HO
N=O
Which of the following compound can show tautomerism ?
O
OH
(A)
N
(B)
OH
(C)
(D) None of these
N=O
14.
Which of the following compound(s) show tautomerism in triad system ?
O
(A) CH3COCH3
15.
(B) CH3CH2NO2
(C)
(D) HCN
Keto-enol tautomerism is observed in :
O
||
(A) C 6 H 5 - C - H
O
||
C
H
C
- CH 3
(B) 6 5
O
||
(C) Ph - C - Ph
O
O
||
||
(D) Ph - C - CH 2 - C - CH3
265
JEE-Chemistry
16.
Which of the following statement(s) is/are correct about tautomers?
(A) They posses different electronic and atomic rearrangement
(B) They posses different electronic but same atomic arrangement
(C) They have different atomic arrangement but same electronic arrangement
(D) They exist in equilibrium
17.
Which compound does not show tautomerism ?
O
CH3
CH3
(A)
18.
Cl
(B)
O
O
Br (C)
(D)
O
O
O
Which of the following can undergo tautomerisation ?
(A) CH3 – CN
(B) CH3 – NO2
(C) CH3 – NO
266
(D)
CH3
CH3 – C = N – CH 3
Isomerism
GEOMETRICAL ISOMERISM
1.
2.
SINGLE CORRECT ANSWER TYPE
Geometrical isomerism can result when molecule
(A) has a plane of symmetry
(B) has a centre of symmetry
(C) has restricted rotation
(D) rotates the plane of polarized light
Which of the following compound shows cis and trans isomerism ?
(A)
3.
Cl
Cl
(B)
Br
CH3
Cl
C =C
CH3
H
C=C=C
CH3
H
H
Cl
(D) Cl – CH = CH – Cl
CH3
Cl
C=C
H
H
(D) All of these
Cl
(B)
(C)
C=C
H
Br
and
Cl
CH3
C=C
Cl
Cl
(D) All of these
H
Br
(A) Configurational isomers
(C) Constitutional isomers
(B) conformational isomers
(D) Structural isomers
Which of the following will not show geometrical isomerism ?
Me
Me
(A)
8.
CH3
What is the correct relationship between the following compounds ?
CH3
7.
CH3
Which of the following compound do not show geometrical isomerism ?
(A)
6.
C
(C)
(B) CH3 - C º C - CH3 (C)
Cl
5.
H
Which of the following compound will not show geometrical isomerism ?
(A)
4.
Br
C =C
(B)
Me
Geometrical isomerism is possible in:
(A) isobutene
(C) acetophenone oxime
(C)
Cl
(D)
(B) acetone oxime
(D) benzophenone oxime
(i) CH2 = CH – CH2 – CH = CH2
(ii) CH2 = CH – CH =CH – CH3
(iii) CH3 – CH = CH – CH = CH – CH3
The numbers of possible geometrical isomers for the above compounds are respecitvely :
(A) 0, 2, 4
(B) 2, 2, 4
(C) 0, 3, 3
(D) 0, 2, 3
267
JEE-Chemistry
9.
For a hydrocarbon, the minimum number of carbon atoms to show position and geometrical isomerism
is be :
(A) 4, 3
10.
(B) 4, 4
(C) 3, 4
(D) 4, 2
The number of pairs of geometrical isomers in 1, 2-Dichlorocyclohexane is
(A) 1
(B) 2
(C) 3
(D) 4
MULTIPLE CORRECT ANSWER TYPE
11.
For the compound H3C – CH = CH – CH = CH – CH = CH – CH3 .
Which of the following is/are true ?
(A) There are total 6 geometrical isomers
(B) There are total 8 geometrical isomers
(C) There are five geometrical isomers with at least one configuration as cis.
(D) There are five geometrical isomer with at least one configuration as trans.
12.
13.
Which of the following does not have zero dipole moment ?
(A) trans-1, 2-Dichloroethene
(B) cis-1, 2-Dichloroethene
(C) Benzene-1, 4-diol
(D) 1, 4-Dichlorobenzene
What characteristics of cis-but-2-ene and trans-but-2-ene are not common ?
(A) Constitution
(B) boiling point
(C) heat of hydrogenation
(D) Dipole moment
268
Isomerism
CALCULATION OF GEOMETRICAL ISOMERS
1.
SINGLE CORRECT ANSWER TYPE
How many geometrical isomer are possible for given compound ?
(A) 0
2.
(C) 2
How many geometrical isomers are possible for
(A) 0
3.
(B) 1
(B) 1
(D) 3
?
(C) 2
(D) 3
How many geometrical isomers are possible for :
Cl
Cl
Cl
(A) 0
(B) 1
(C) 2
(D) 3
4.
How many geometrical isomers are possible for : CH 3 - CH = C = CH - CH = CH - CH 3
(A) 0
(B) 1
(C) 2
(D) 3
5.
How many geometrical isomers are possible for
CH 3 - CH = C = C = C = CH - CH = CH - CH 3
(A) 1
(B) 2
(C) 3
6.
CH3
How many geometrical isomers are possible for
(A) 2
(B) 3
(D) 4
CH3
H
H
(C) 4
(D) 6
7.
How many geometrical isomers are possible for, CH3–CH=CH–CH=CH–Cl ?
(A) 2
(B) 3
(C) 4
(D) 5
8.
How many geometrical isomers are possible for, Ph–CH=CH–CH=CH–Ph ?
(A) 2
(B) 3
(C) 4
(D) 5
9.
How many geometrical isomers are possible for,
(A) 0
(B) 1
(C) 2
269
?
(D) 3
?
JEE-Chemistry
10.
Select the compound with correct number of geometrical isoemers :
Compound
Number of geometrical isomers
(A)
6
(B)
6
(C)
(D)
Cl
Cl
4
8
270
Isomerism
ELEMENTS OF SYMMETRY
SINGLE CORRECT ANSWER TYPE
1.
How many planes of symmetry are present in
(A) 1
2.
(B) 2
H
H
H
C= C
?
(C) 3
How many planes of symmetry are present in
(A) 3
H
(B) 5
(D) 4
(Benzene) ?
(C) 7
(D) 9
COH
2
3.
H
OH
H
OH
COH
2
Number of plane of symmetry in above compound is :
(A) 1
(B) 2
(C) 3
(D) 4
H
H
4.
Cl
Cl
How many planes of symmetry are present in above compound ?
(A) 0
(B) 1
(C) 2
(D) 3
How many planes of symmetry are present in above compound ?
(A) 1
(B) 2
(C) 3
(D) 4
5.
6.
Which of the following compound has plane of symmetry and center of symmetry?
F
F
F
F
F
(A)
(B)
F
F
F
F
F
F
F
(C)
F
F
F
(D) All of these
F
F
F
271
JEE-Chemistry
7.
Which compound has plane of symmetry and C2 axis of symmetry ?
F
O
(A)
(B)
H
8.
H
Cl
C
C
H
H
(C)
(D) All of these
F
Which species has a plane of symmetry?
(A)
9.
Cl
(B)
(C)
(D)
Which of the following compound has plane of symmetry ?
Cl
Cl
Cl
(A)
(B)
CH3
Br
(C)
Cl
I
C
H
(D)
CH3
Cl
Cl
10.
Cl
Cl
Number of planes of symmetry in above compound are :
(A) 0
(B) 1
(C) 2
272
CH3
(D) 3
CH3
Isomerism
DETERMINATION OF STEREO CENTRES
1.
SINGLE CORRECT ANSWER TYPE
Which of the following has asymmetric carbon atom?
C l Br
|
|
(A) H - C - C - H
|
|
H H
2.
H Cl
|
|
(B) H - C - C - C l
|
|
H H
H H
|
|
(D) H - C - C - CH 3
|
|
Br OH
H Cl
|
|
(C) H - C - C - H
|
|
H H
Whcih of the following compound is chiral?
H
O
(A)
(B)
(C)
F
CH3
F
Cl
F
CH3
(D) Cl
H
H
3.
Which of the following is a chiral compound ?
(A)
(B)
(C)
(D)
OH
4.
(a) (Number of chiral center)
O
(b) (Number of chiral center)
COH
2
sum of (a + b = ?) :
(A) 3
CH3
(B) 4
(C) 5
(D) 6
CH3
5.
How many chiral centers are present in above compound ?
(A) 1
(B) 2
(C) 3
273
C
(D) 4
Br
JEE-Chemistry
CH3
6.
Number of chiral center present in above compounds are :
(A) 0,1
(B) 0, 2
(C) 0, 3
O
(D) 1, 2
O
N
7.
Number of chiral carbons present in above compounds are :
(A) 1, 2
(B) 2, 2
(C) 2, 1
(D) 2, 3
CH3
CH3
8.
O+
O
H
Number of chiral carbons present in above compounds are :
(A) 1, 1
(B) 1, 2
(C) 2, 2
9.
H
Et
|
|
CH
C
-D
3
CH 3 - C - H
|
|
T
CH3CH 2 - CH 3
Number of chiral carbons present in above compounds are :
(A) 0, 0
(B) 1, 0
(C) 1, 1
10.
(D) 2, 3
(D) 2, 2
Number of stereocenters present are :
CH 3 - CH = CH - CH - CH 3
|
Cl
(A) 0
(B) 3
(C) 4
274
(D) 5
Isomerism
DETERMINATION OF ABSOLUTE CONFI GURATION
1.
SINGLE CORRECT ANSWER TYPE
IUPAC name of the given compound is :
(A) (2S, 3S)-2-chloropentan-3-ol
(C) (2R, 3R)-2-chloro-3-pentanol
2.
(B) (2S, 3R)-2-chloro-3-pentanol
(D) (2R, 3S)-2-chloro-3-pentanol
IUPAC name of the compound
is
(A) (2R,3R)-3-chloropentan-2-ol
(C) (2S,3R)-3-chloropentan-2-ol
3.
The R/S configuration of these compounds are respectively.
HO
H
CF3
(A) R,R,R
4.
H
HS
H
NH2
CH3
CHO
COOH
(B) R,S,R
(C) R,S,S
(D) S,S,S
Which of the following combinations amongst the four Fischer projections represents the same absolute
configurations?
(A) (II) and (III)
5.
(B) (2R,3S)-3-chloropentan-2-ol
(D) (2S,3S)-3-chloropentan-2-ol
(B) (I) and (IV)
(C) (II) and (IV)
Which of the following operations on the Fischer formula
(D) (III) and (IV)
does not change its absolute
configuration?
(A) Exchanging one horizontal & one vertical groups
(B) Exchanging two vertical groups
(C) Exchanging three groups in clockwise or in anticlockwise direction keeping 4th group fixed
(D) Exchanging two horizontal groups
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6.
Which of the following compound has S configuration?
Cl
(A) H
CHCl
2
(B) H
CH3
CHCl
2
7.
CH3
(C) CH3
CHCl
2
Cl
Which of the following compound has R configuration ?
(A) CHCH
3
2
CH= CH2
Br
(B) Br
CH = CH2
H
CHCH
2
3
CHCH
2
3
CHCH
2
3
(C) Br
H
(D) CH2 = CH
CH = CH2
Br
H
Which of the following group has the highest priority using the Cahn, Ingold, Prelog rules ?
O
||
(A) - C - OH
9.
Cl
(D) CH3
H
Cl
H
8.
H
CHCl
2
O
||
(B) - C - H
(C) – OH
(D) – O –CH3
What is the configuration of the following compound?
CH3
H
Cl
Cl
H
CHC
2 H3
(A) 2S,3R
10.
(B) 3R,3S
(C) 2S,3R
(D) 2S,3S
In the Fischer projection below, what are the configurations of the two asymmetric centers?
COH
2
H
CH3
H
CH3
CHCHO
2
2 H
(A) 2R,3R
(B) 2R,3S
(C) 2S,3R
276
(D) 2S, 3S
Isomerism
RELATIONSHIP BETWEEN STEREOISOMERS
1.
2.
SINGLE CORRECT ANSWER TYPE
Meso-tartaric acid and d-tartaric acid are
(A) positional isomers (B) enantiomers
(C) diastereomers
The structures shown here are related as :
(I)
(A) conformers
(C) geometrical isomers
3.
(D) racemic mixture
(II)
(B) enantiomers
(D) diastereomers
The two compounds given below are
(A) enantiomers
(B) identical
(C) optically inactive
(D) diastereomers
4.
Which of the following statements is/are correct?
(A) A meso compound has chiral centres but exhibits no optical activity
(B) A meso compound has no chiral centres and thus are optically inactive.
(C) meso compounds are molecules which are nonsuperimposable on their mirror images even though
they contain chiral centres
(D) A meso compound is optically inactive because the rotation caused by any molecule is cancelled
by an equal and opposite rotation caused by another molecule that is the mirror image of the first.
5.
Which of the following is not having D-configuration ?
(A)
(B)
(C)
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(D)
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6.
Which of the following is a 'threo' isomer?
CHO
H
OH
(A) H
OH
HO
(B) H
H
OH
COOH
H
Cl
(C) H
OH
COOH
NH2
(D) H
H
OH
CH3
CH3
CH2OH
7.
CH3
CH3
Identify meso compound :
CH3
Cl
H
Cl
(A) Cl
H
CH3
Cl
CH3
(C)
(B)
(D)
Cl
Cl
Cl
H
Br
Cl
H
CH3
8.
(A)
(B)
Relation between (A) and (B) is :
(A) Diastereomers
(B) Enantiomer
(C) Identical
(D) Structural isomer
MULTIPLE CORRECT ANSWER TYPE
9.
Which of the following statements is/are not correct for D-(+) glyceraldehyde?
(A) The symbol D indicates the dextrorotatory nature of the compound
(B) The sign (+) indicates the dextrorotatory nature of the compound
(C) The symbol D indicates that hydrogen atom lies left to the chiral centre in the Fischer projection
diagram
(D) The symbol D indicates that hydrogen atom lies right to the chiral centre in the Fischer projection
diagram
10.
Which of the following statements for a meso compound is/are correct?
(A) The meso compound may has either a plane or a centre of symmetry
(B) The meso compound has non-zero optical rotation
(C) The meso compound is achiral
(D) The meso compound is formed when equal amounts of two enantiomers are mixed
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Isomerism
11.
12.
Which of the following pairs of compound is/are identical?
(A)
(B)
(C)
(D)
Which of the following molecule is not identical with that represented by
(A)
(B)
(C)
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(D)
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CALCULATION RELATED WITH OPTICAL ISOMERISM
1.
SINGLE CORRECT ANSWER TYPE
What is optical purity of 6 gm (d) and 4 gm (l) ?
(A) 40%
(B) 20%
(C) 10%
O
2.
Cl
O
(A)
(A) + 500
(D) 60%
Cl
What is the optical rotation of (A) ?
(B) – 500
(C) 00
(D) 1000
3.
If (S)-glyceraldehyde has a specific rotation of -8.7°, what is the specific rotation of
(R)-glyceraldehyde?
(A) –8.7°
(B) +8.7°
(C) 0.0°
(D) cannot be determined from the information given
4.
The specific rotation of a pure substance is 1.68°. What is the specific rotation of a mixture containing
75% of this isomer and 25% of the (–) isomer?
(A) +1.68°
(B) 0°
(C) +1.26°
(D) +0.84°
5.
(–)-Mandelic acid has a specific rotation of –160°. What would be the specific rotation of a solution
which contains 40% (–)-mandelic acid and 60° (+)-mandelic acid?
(A) +95°
(B) +63°
(C) +32°
(D) –32°
(E) –63°
6.
The number of optically active compounds in the isomers of C4H9Br is
(A) 1
(B) 2
(C) 3
(D) 4
7.
How many stereoisomers can exist for the following acid
H - C(OH).CO 2H
|
H - C.CO 2 H
|
H - C(OH).CH 3
8.
(A) Two
(B) Four
(C) Eight
(D) Sixteen
Sum of total number of stereoisomers of both compound given below is :
(A) 5
(B) 6
NH2
F
OH
Cl
(C) 7
280
(D) 8
Isomerism
9.
CH3
|
CH 2 = C - CH2 - CH = CH - CH- CH3
|
Cl
Total number of stereoisomers are:
(A) 4
(B) 6
10.
(C) 8
(D) 12
How many stereoisomers exist for the compound below?
COH
2
H
H
HO
OH
OH
H
CHO
2 H
(A) 2
(B) 4
(C) 8
(D) 7
MULTIPLE CORRECT ANSWER TYPE
11.
The incorrect number of chiral center(s) and stereoisomers are :
CH 2 - CO2 H
|
CH - CO2 H
|
HO - CH - CO2 H
(A) 1, 2
12.
(B) 2, 4
(C) 2, 3
(D) 3, 8
For the given compound which of the following statements is/are correct ?
CH 3–CH(OH)–CH(OH)–CH(OH)–CH3
(A) number of stereoisomers are 6.
(B) number of meso forms are 2.
(C) number of optically active isomers are 2.
(D) molecule contains three tertiary carbon atoms.
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CONFORM ATI ONS
1.
SINGLE CORRECT ANSWER TYPE
This is the Newman projection formula of
(A) 2-Bromo-3-chloro-2-fluoropentane
(B) 3-Bromo-2-chloro-3-fluoropentane
(C) 3-Bromo-2-chloro-2-fluoropentane
(D) 2-Bromo-2-chloro-2-fluoropentane
H
F
CH3
CH
2 5
Br
Cl
2.
Which of the following statements about conformers is correct?
(A) Conformers exist in a state of dynamic equillibrium
(B) At equillibrium, population of more stable conformers will be more than that of less stable
conformer
(C) Conformers cannot be separated
(D) All of these
3.
Which of the following causes is correct to develope torsional strain in the molecule?
(A) Bond pair-bond-pair repulsion
(B) Steric repulsion
(C) vander Waals repulsion
(D) Dipole-dipole repulsion
4.
Translating this staggered Newman projection formula of 2,3-dibromobutane into staggered sawhorse projection appears as
H
Br
H Br
CH3
(A)
Br
5.
(A)
7.
CH3
(B)
Br
H
CH3
Br
H
H
CH3
Br
H
CH3
(C)
H
H
CH3
(D) all of these
Br
Most stable form of meso-2,3-diflouro-2,3-butandiol is Me
6.
CH3.
Br
CH3
F
Me
OH
HO
F
OH
(B)
Me
OH
F
HO
Me
(C)
F
Me
OH
F
Me
Which is the most stable conformer of glycol ?
(A) anti
(B) gauche
(C) eclipsed
Compound
(A) Cyclohexane
Me
F
(D)
Me
OH
OH
F
F
(D) fully eclipsed
is projection formula of :
(B) Cyclopentane
(C) Cyclobutane
282
(D) Cyclopropane
Isomerism
8.
Which of the following is an achiral molecule?
(A)
(B)
(C)
(D)
9.
The most stable conformation of 3-fluorobutan-2-ol is :
(A) Fully eclipsed form
(B) Partially eclipsed form
(C) Gauche form
(D) Anti form
10.
Which of the following statements regarding the projections shown below is true.
(A) ‘a’ and ‘b’ both represent the same configuration
(B) Both ‘a’ and ‘b’ are optically active
(C) ‘b’ alone is optically active
(D) ‘a’ alone is optically active
11.
MULTIPLE CORRECT ANSWER TYPE
The two structures I & II do not represents :-
(I)
(A) Conformational isomers
(C) Constitutional isomers
12.
(B) Stereoisomers
(D) Identical
Which of the Newman projections shown below do not represent the conformation about the
C1–C2 bond of 1 Bromo –2–methylpropane?
(A)
13.
(II)
(B)
(C)
(D)
Which of the following do not represent the staggered conformation with dihedral angle f = 60 ?
(A)
(B)
(C)
283
(D)
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14.
Which of the following sawhorse representation is incorrect for the given newman projection.
(A)
(B)
(C)
(D)
284
Isomerism
ANSWER KEY
STRUCTURAL ISOMERISM (EXCEPT TAUTOMERISM)
1.
(A)
2.
(B)
3.
(A)
4.
(A)
5.
(C)
6.
(B)
7.
(D)
8.
(C)
9.
(D)
10.
(A)
11.
(C)
12.
(A)(B)
13.
(A)(B)(C) 14.
(B)(C)
15.
(B)(C)(D) 16.
18.
(A)(B)(C) 19.
(A)(D)
20.
(B)(C)(D)
6.
(B)
6.
(A)
(A)(B)(C) 17.
(A)(C)(D)
STRUCTURAL ISOMERISM (TAUTOMERISM)
1.
(C)
2.
(D)
3.
(B)
4.
(A)
5.
(D)
7.
(A)
8.
(D)
9.
(D)
10.
(D)
11.
(B)(C)(D)
12.
(A)(B)(C)(D)
13.
(A)(C)
14.
(A)(B)(C)
15.
(B)(D)
17.
(A)(B)
18.
(A)(B)(C)(D)
16.
(A)(D)
GEOMETRICAL ISOMERISM
1.
(C)
2.
(D)
3.
(D)
4.
(D)
5.
(A)
7.
(C)
8.
(D)
9.
(B)
10.
(A)
11.
(A)(C)(D) 12.
13.
(B)(C)(D)
(B)(C)
CALCULATION OF GEOMETRICAL ISOMERS
1.
(C)
2.
(C)
3.
(C)
4.
(C)
7.
(C)
8.
(B)
9.
(C)
10.
(C)
5.
(B)
6.
(A)
(D)
6.
(C)
6.
(C)
ELEMENTS OF SYMMETRY
1.
(C)
2.
(C)
3.
(A)
4.
(B)
7.
(D)
8.
(D)
9.
(D)
10.
(B)
5.
DETERMINATION OF STEREO CENTRES
1.
(D)
2.
(D)
3.
(D)
4.
(C)
7.
(C)
8.
(A)
9.
(C)
10.
(B)
5.
(C)
DETERMINATION OF ABSOLUTE CONFIGURATION
1.
(A)
2.
(A)
3.
(A)
4.
(C)
7.
(A)
8.
(D)
9.
(D)
10.
(A)
5.
(C)
6.
(B)
RELATIONSHIP BETWEEN STEREOISOMERS
1.
(C)
2.
(D)
3.
(A)
4.
(A)
5.
(B)
6.
7.
(D)
8.
(A)
9.
(A)(D)
10.
(A)(C)
11.
(A) 12.
(B)(C)
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(B)
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CALCULATION RELATED WITH OPTICAL ISOMERISM
1.
(B)
2.
(C)
3.
(B)
4.
(D)
7.
(C)
8.
(D)
9.
(A)
10.
(C)
11.
(A)(C)(D) 12.
5.
(C)
6.
(B)
6.
(B)
(A)(B)(C)(D)
CONFORMATIONS
1.
(C)
2.
(D)
3.
(A)
4.
(A)
5.
(C)
7.
(D)
8.
(A)
9.
(C)
10.
(C)
11.
(A)(B)(D)
12.
(A)(B)(D) 13.
(A)(C)(D) 14.
(A)(B)(C)
286