Unit 6 Studyguide/Review Packet:
Test:
B: Thursday 17 Dec 2015
A: Friday 18 Dec 2015
Ionic/Metallic Bonds:
types of particles bonding
force holding atoms together
difference in electronegativity (only ionic)
properties
how delocalized electrons explain properties of metals
Covalent Bonds:
Classify bond types based on EN differences
NPC: from 0 to 0.20
PC: from 0.20 to 1.67
I: greater than or equal to 1.67
What is a molecule?
Determine valence electrons of atoms and molecules
name/write formulas for molecules using prefixes
State and Apply the octet rule
Write Lewis Dot Structures
Fill in the chart: see example on next page
Describe the three main intermolecular forces in terms of strength and
“Weird” Atoms that do not follow the octet rule:
Element
Symbol
Number of electrons in
valence:
2
hydrogen
H
4
beryllium
Be
6
boron
B
If a central atom has 5 bonded atoms it may have 10 valence eIf a central atom has 6 bonded atoms it may have 12 valence e-
Write T for true and F for false. If a statement is false, replace the underlined word or
phrase with one that will make the statement true, and write your correction in.
True
a. Dispersion forces are the only attractive forces that attract between
non-polar molecules.
False, can
b. Molecules cannot exhibit both dipole-dipole forces and hydrogen bonding.
True
c. A non-polar molecule can have polar bonds. If true, then when?
When the molecule is SYMMETRIC
False, polar
d. Water is a non-polar molecule that has polar bonds.
Fill in the chart:
molecular
formula
carbon
tetrachloride
CCl4
number
of
(total)
valence
e32
water
H 2O
8
CHCl3
26
nitrogen
tribromide
NBr3
26
lewis dot
structure
Cl
Cl - C– Cl
Cl
..
H-O–H
..
Cl
Cl - C– Cl
H
..
Br - N – Br
Br
number
of
bonded
atoms
(B)
number
of lone
pair (E)
type of
molecule
(A B E)
molecular
shape
polarity
of
molecule
(P or
NP)
4
0
AB4
tetrahedral
NP
2
2
AB2E2
bent
P
4
0
AB4
tetrahedral
P
3
1
AB3E
trigonal
pyramid
P
Practice:
1.
Pairs of electrons that bond two atoms in a molecule are called ___shared pairs_____.
2. Pair of electrons that are unshared are called lone pair.
3. Because each of the bond angles of methane equals 109.5⁰, its molecular shape is a perfect
tetrahedron.
4. Define “dipole” in your own words! DO NOT use the same definition from your notes,
paraphrase and simplify!
polar molecule
5. Are the bonds in a polar molecule arranged symmetrically or asymmetrically?
6. Matching (write the roman numeral beside the letter it matches)
iii a. a non-polar molecule in which the charge
i. dispersion forces
distribution is very briefly asymmetrical
i
b. forces generated by instantaneous dipoles
ii. dipole-dipole forces
v
c. forces between molecules
iii. instantaneous dipole
iv
d. forces within a molecule
iv. intramolecular forces
ii
e. attractive forces between two molecules
v. intermolecular forces
of the same or different substance that
are both “permanent” dipoles
0
