Unit 2 Atomic Structures
1. The ________________
a. _______________ Tube experiment in __________________
i. Completed by ________ __________________
ii. Atoms not_________________ spheres, composed of _____________ particles
iii. Electrons (_________)
iv. Calculated ____________ to be ________________________ grams
Cathode Ray Tube
b. __________________ oil drop _________________
i. Used ________________ to place a charge on ___________droplets
ii. Applied an _______ ______________ to_______________ charged
_________droplets
iii. Used this to determine the ____________ _____________ of an ___________
1.6 x 10-19 C.
2. ___________ _________________
i. Observed _________ in a ______________tube traveling from the
___________to the cathode.
ii. These were __________________ towards the _____________plate.
iii. Protons! (_______) =______________________grams
iv. Elements seemed to be comprised of an ____________ number of
____________and ____________________.
3. ________________
a. Not discovered until 1932 by _______________ _________________
i. ______________charged particles
ii. (n0) = ____________________ grams
iii. Accounts for _________________- atoms of an element that are
_____________ alike but _____________in _______________.
b. Isotope notation:
𝑦
𝑧𝑋
i. X is the ___________ _______________, y is the ______________ __________,
and z is the ___________ _______________
ii. Atomic number = _________________________________________
iii. Mass number = number of ___________+_____________ of a single_________
Thompson’s Model of the atom
1. Ernest __________________
a. Conducted _____________ _____________ experiment in 1911
i. Shot __________ particles at a _________ of ___________foil surrounded by a
________________ screen.
ii. Expected the___________ particles to go straight through the atoms based on
J.J _________________ plump _____________model of the atom.
Rutherford’s Gold Foil Experiment
iii. Concluded from the______________ that ___________ are ___________
empty _____________ and with a ____________ charged _________, the
________________.
b. ______________ Model
i. ________________ containing _______________and _______________
ii. Surrounded by mostly _____________ space containing _______________.
Rutherford’s Nuclear Model of the Atom
2. Niels________________
a. Proposed that _______________ must have enough _______________ to keep them in
___________________motion around the ___________________.
i. _____________________ can only circle the_______________ at certain
_______________away from the ______________; these are called
_____________ or ___________ _____________.
1. Each __________________has a ________________ amount of
_____________________associated with it.
a. Closer to the _________________ = a____________ orbit =
______________ energy
b. _______________away from the _______________= a
_________orbit = ______________energy
2. ________________- the amount of _______________needed to jump
________________energy levels
a. Proposed by Max ________________
Planetary Model of the atom
3. _______________ _______________ Model – ____________ of ____________ based on the
______________ properties of an ___________________
a. Deals with the ___________________ of finding an _____________ orbiting an
________
b. ________________
i. _____________ region around the _______________ where an
___________can be found
ii. Forms a __________around the _________________
iii. _____________and _____________ of the cloud depends on the ___________
___________ of the ____________
iv. _______________ can exist _______________ in the ____________, but
________between orbitals.
4. Atomic Orbitals/ Quantum Numbers
a. Ewin _______________ developed an _______________that describes
the________________ of finding the position of an ___________________.
b. Describes the _______________ of an ________________ in an _____________
i. ___________________Quantum Number (______)
1. The _________ ______________ the _____________ occupies
2. ______________ numbers ____________
3. The ______________ the number is, the _______________ the
_________ is away from the_________________
4. ___________ is the ______________ number of_____________ in the
__________ ____________
5. Contains _____________ equal to _______
ii. ____________ Quantum Number (_______)
1. The _______________ of________
2. Defines the ____________of the ____________
3. _________is an _______________ from _______________
4. Example- if n = 3 what are all possibilities for 𝓵
5. Each _____________ is expressed as a ____________ s,p,d,f
𝓵 = 0 (_______)
Picture of s
a. _________sublevel
b. _____________
𝓵=1 (_____)
a. ______ sublevels
Pictures of p
b. ______________
𝓵 =2 (_______)
a. __________ sublevels
6. 𝓵 = 3 (______________)
a. ______________sublevels
5. Electromagnetic Spectrum
a. Total ________________ of ______________________ radiation
10
24
10
22
20
10
rays
-16
-14
10
10
10-12
Wavelength (m)
10
18
10
rays
10-10
16
10
14
rays
10-8
10
12
IR
10-6
400 nm
10-4
10
8
6
10
10
10
Microwaves Radio Waves
10-2 100
10-2
Frequency (Hz)
10
102
100
Long Radio Waves
104
106
108
4
700nm
iv. Wavelength (______) – Distance __________ corresponding _________
on adjacent waves
v. Frequency (__________) – ___________of ________ that pass by a point
in a certain _____________ of time.
6. ________________ can be described as _____________or _____________
a. ______________states – when____________ are boosted to ___________
energy levels
b. _____________________state – the _____________ energy level
c. When _____________ go to a ________________ energy state they __________
a _______________ of energy.
vi. This _____________ is in the form of ______________, called a
____________.
7. _____________ Uncertainty Principle
a. _____________Physicist
b. Determined it’s ___________ possible to measure both _____________and the
___________of an ______________ at the same ___________.
8. Bright light emission spectrum.
a. Certain ____________ levels emit certain___________ when an __________
falls from them.
b. Each ____________ has a particular ____________ associated with it and so emit
a specific _____________ of _______________.
1. Electron configurations
a. Written notation to show how _____________ are distributed within ________________
1s2
b. Examples:
i. Nitrogen
ii. Potassium
c. Exceptions:
i. Cr
ii. Cu
d. Nobel Gas configurations:
i. Potassium
ii. Bromine
e. Rules for orbital diagrams:
i. Aufbau Principle –_______________ must occupy the _____________energy
level ______________.
ii. Hund’s Rule - Orbital's of ____________energy will occupy an _________
______________ before ___________________ occurs.
iii. Pauli ______________Principle – no two ______________ can have all
_________quantum numbers the ______________.
How did you organize your candy?
1. History of the periodic table
a. Demitriy ________________
i. Realized that the ________________ and _________________properties of the
______________________ repeated in an __________________ way when he
organized the elements according to increasing _______________ ___________.
ii. Elements with ________________properties were placed in the ____________
horizontal _____________.
iii. Table showed that ____________________ of elements ____________ in an
__________________way from row to row.
iv. Mendeleev’s table left some ________________ spaces; this suggested that there
were___________________ that had not yet been _________________.
v. Using the table Mendeleev could ______________ the properties of these
unknown elements.
Properties of Eka- Aluminum (Germanium)
Property
Predicted (1869)
Atomic mass
72 amu
Color
Dark gray
Density
5.5 g/ml
Melting point
Very high
Formula of oxide
EsO2
Density of oxide
4.7 g/ml
Oxide solubility in HCl
Slight
Formula of chloride
EsCl4
Actual (1886)
Gray-white
5.32 g/ml
937 0C
GeO2
4.70 g/ml
none
GeCl4
b. ______________________- tendency to ___________at regular ______________.
i. Mendeleev was so confident in ________________ that he placed some elements
in groups with others of _______________ properties even though this
__________________ did not go strictly by _____________ ____________.
c. Henry _________________
i. Organized his ______________table by _____________ _______________.
2. Modern Periodic Table
a. __________________ Law –_______________ and _________________ properties of
elements _______________ in a regular _______________ when they are arranged by
_______________ atomic number.
3 Undiscovered Elements
1.
2.
3.
8. Family Characteristics
a) Group 1 (Alkali metals)
i) Soft and highly reactive.
ii) Alkali
(1) Produce alkaline (basic) solutions
(2) Slippery to the touch
iii) Metal
(1) Malleable
(3) Conducts heat and electricity
(2) Ductile
(4) Luster
iv) Have 1 electron in highest energy level.
b) Group 2 (Alkaline earth metals)
i) Harder and more dense than alkali metals.
ii) Not as reactive as alkali metals.
iii) Contain 2 electrons in their highest energy level.
c) Group 3 - 12 (Transition elements)
i) All are metals.
ii) Not as reactive as alkali or alkaline earth metals.
iii) Electron configuration can change within a group in order to better stabilize the atom.
d) Lanthanide Series
– 71Lu
i)
58Ce
ii)
Rare earth elements.
iii) Most are radioactive
e) Actinide series
i)
ii)
90Th
– 103Lr
All are radioactive.
iii) Have unstable electron configurations.
f) Group 13 – 18 (Main block elements)
i) Represent a wide range of chemical and physical properties.
ii) Contain metals, metalloids, non-metals and noble gases.
g) Group 17 (Halogens – salt formers)
i) Readily combine with alkali metals or alkaline earth metals to form a “salt”
ii) Most reactive non-metals.
iii) Have 7 electrons in the highest energy level.
h) Group 18 (Noble Gases)
i) The group of Noble gases were originally proposed by Strutt and Ramsey when they
discovered the element Argon.
ii) Have a full s and p orbitals
iii) Stable configuration, or, resists change (inert).
i) Hydrogen (Own family)
i) Behaves like no other element.
ii) Has only one electron.
iii) Rare on earth in its free state, usually found in combination with other atom(s).
(1) Ex. H2O, CH3CH2OH, CH3CH2CH2CH2CH2CH2CH2CH3
8. Octet Rule- in order for an element to be _____________ it must possess full ____ and
______orbitals
a. Have _________ electrons in its _______________energy level!
b. Elements will react _________________, or nuclearly to achieve this ________.
Periodic Trends
1. Atomic Radius- ____________ of an ________________
a. _________________of the distance between the ________________ of
_______________elements
i. Diatomic ________________- elements that e_________ in nature as a
______________
1. _____________ diatomic elements
a.
b. _______________ down a group
i. The more _____________ ______________ there are the _____________
the atom is.
c. _______________________ from left to right across a period
i. ________________ effect- ________________ of the attraction between a
__________________and its ____________
electrons due to the ______________ effect of the
______________electrons.
2. Ionization Energy
a. ___________- an atom that has ____________ or _____________electron(s)
giving it a __________________
i. ______________- an ion that has _______________ electron(s)
1. Have a _________________charge
ii. _______________- an ion that has ____________ electron(s)
1. Have a _________________charge
b.________________ electrons- electrons in the ___________________energy _________of an
atom.
i.
Responsible for _______________of the chemical ______________ between
atoms
ii. Electrons _______________ or _________________will be ______________ electrons
How to find the number of valence electrons: The Bhor model of the atom:
To draw the bohr model of the atom: example: Ne
1. Start by placing the correct number of protons and neutrons of the element in the center
a. Protons are found from the atomic number.
b. Neutrons are found from subtracting the atomic number from the mass number of
the most stable isotope.
2. Add enough energy levels for the element in question
a. You can figure this out by counting the number of rows on the periodic table.
3. Figure out how many electrons can go in each energy level.
a. 2n2 rule
4. Add as many electrons as are in the element filling the energy levels starting closest to
the nucleus.
a. The number of electrons is equal to the number of protons.
b. ________________ energy- energy required to __________________an
________________from an element.
i. ________________ down a _________________
1. ________________ that are held more tightly to the__________
will be _______________________ to remove
a. The _________________ an atom is the __________
energy required to______________an _____________.
ii. _______________ from left to right in a ________________
a. The _________________an atom is the
___________energy required to ___________an electron.
3. ______________________- the tendency of an ___________________ to attract
__________________ to itself when forming a ______________________.
a. The higher the__________________, the more likely an ___________ is to attract
______________.
i. _________ has the highest at _________________
b. ________________ down a _________________
i. The _____________________ the ________________ are held by the ______________,
the greater the ____________________ is.
ii. As the_____________ gets _____________ the__________________ gets
______________________.
c. _______________________ from left to right in a _______________.
i. As the atomic_______________
gets________________ the
____________________gets
___________________.
Martian Periodic Table
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0
1
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-1
2
3
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Element List
A
B
C
D
E
F
G
H
I
J
K
L
M
N
O
P
Q
R
S
T
U
V
W
X
Y
Z
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