Ch. 7-8 Review
Sheet
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1. What are the properties of IONIC
substances?
These substances:
-Solid Hard and brittle (like salt) at room temp
-Conduct electricity when dissolved in water
-High boiling/melting points
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2. What are the properties of
COVALENT substances?
These substances:
-MOST are liquids/gases at room temp
-Do not conduct electricity when dissolved in
water
-Most can not dissolve in water
-Low boiling/melting points
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3. What’s the difference between ionic
BONDING and covalent BONDING?
Ionic
Covalent
Transfer electrons
Shared electrons
Metal/nonmetals
Nonmetals
Has a charge
No charge
Single bonds only
Can have double/triple
bonds
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4. Why do atoms form bonds?
Atoms are trying to fill their valence orbit with a
stable octet of electrons- in the case of
hydrogen it’s a duet
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5. What are diatomic molecules?
Name 7 of them.
Diatomic molecules are molecules that are
made up of 2 identical atoms to become a
molecule.
H2, N2, O2, F2, Cl2, Br2, I2
KNOW THESE!!!~!!!
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6. How many electrons are involved in
covalent bonding?____
2 shared electrons or a pair of electrons
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7. What is bond dissociation energy?
The energy needed to separate a covalent bond
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8. What properties determine bond
strength?
C-C longer and weaker
O=O not so long and stronger
N=N short and strong
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9. Provide the Lewis structure, the VSEPR shape
and determine the polarity for the following
Lewis
Structure
SO3
VSEPR shape
Trig planar
CI4
Tetrahedral
SeO2
Bent
HF
Iinear
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IMF
DD
Dispersion
DD
HB
10. What are the 10 prefixes to
molecular compound naming?
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Non-9
Deca- 10
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11. What is the difference between a nonpolar
covalent bond and a polar covalent bond?
Provide an example.
Nonpolar covalent bond is where the electrons are
shared equally between the atoms. Ex: Cl-Cl
Polar covalent bond is where the electrons are not
shared equally between the atoms. Ex: H-Cl
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12. Can a molecule have polar covalent bonds
and be nonpolar? Explain your answer.
Yes, they can.
Overall– Nonpolar molecule
BUT it does have polar bonds
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13. Match the following- answers can be used more than
once or have multiple answers.
1. Induced dispersion
2. Dipole-dipole
3. Hydrogen bonding
a.
b.
c.
d.
H-H _____
1
3
H-F _____
C-Cl____
2
O-O ____
1
1
e. nonpolar covalent____
f. polar covalent____
2 or 3
1
g. attraction to nucleus & electrons ___
1, 2, 3
h. attraction to adjacent atoms___
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Name or Formula
Ionic or
Covalent
Li2O
Ionic
Nitrogen dibromide
Covalent
SBr6
Covalent
Aluminum phosphide
Boron sulfide
SO2
CN2
Potassium nitride
Chlorine trifluoride
Nitrogen disulfide
Magnesium phosphide
Ionic
Ionic
Covalent
Covalent
Ionic
Covalent
Covalent
Ionic
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ANSWER
Lithium oxide
NBr2
Sulfur hexabromide
AlP
B2S3
Sulfur dioxide
Carbon dinitride
K3N
ClF3
NS2
Mg3P2
I Can
•
•
•
•
Describe covalent bonding.
Provide the names or formulas for molecules.
Draw Lewis dot structures of molecules.
Use Lewis dot structures and VSPER theory to
determine the shape of a molecule.
• Predict the intermolecular forces between
molecules by using molecular shapes.
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To Know List- Ch. 3-9
• Look at your reading notes from Ch. 9
– 9.1- Covalent bonds
• Why bonds form?
• Diatomic Molecules- Name them.
• Lewis structures- bonding verse lone pairs
• Double/Triple bonds
• Bond length verse bond strength
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To Know List- Ch. 3-9
• Look at your reading notes from Ch. 9 (75%)
– 9.2 and 9.5 – Naming and Molecular structure
• Binary molecules- what are they?
• Naming molecules- Prefixes and rules for mono
• 3 Exceptions to the octet rule
• Know the 8 basic shapes of Molecules
• Electronegativity and polarity relationship
• Non polar molecules vs Polar molecules
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To Know List- Ch. 3-9 Test
• Concentration of MOSTLY Ch. 9 (75%)
– Ionic Bonding- Ch. 8
• Ionic Bonding
• Naming/Formula of ionic substances
• Properties of Ionic bonds
– Periodic trends- Ch. 6
– Energy levels-light, E-dot/valence-Ch. 5
– Particles- Protons, Electrons Neutrons-Ch. 4
– Physical chemical properties/changes-Ch. 3
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20%
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