Name: _____________________________________ Date: ____________ Period: _______ Page#: _____
CHAPTER 6 REVIEW – COVALENT BONDING
1. List the properties of covalent compounds.
1.
2.
4.
5.
3.
2. To name covalent compounds: USE ___________________!
Number of Atoms
Prefixes
1
2
3
4
5
6
7
8
9
10
NO CRISS CROSS!!
3. Name the following compounds or write the formula:
Compound Name
Compound Formula
AsF2
C2O2
NF3
S2O3
disilicon nonafluoride
pentaphosphorous deciodide
bromine pentachloride
disulfur heptoxide
4. Identify the shared pair and lone pairs in the diagram below:
How many valence electrons are
shown in this structure? _______
5. Draw an example of a compound with a:
Single Bond
Double Bond
Triple Bond
6. Draw the Lewis Structures for:
CH4
NF3
H2O
CO2
SiO2
SF2
7. Describe the amount of transfer of electrons for:
An ionic bond:
A polar covalent bond:
A nonpolar covalent bond:
8. Identify the type of bond that exists with these electronegativity differences:
0 – 0.3
0.4 – 1.6
 1.7
9. Using the table of electronegativities, identify the bond type between the following elements:
Electronegativity
Elements
Element 1
Element 2
Electronegativity
Difference
Bond Type
Ca to F
N to O
Se to I
Fe to C
10. What is the difference between intermolecular and intramolecular forces?
11. Define each type of intermolecular force. Then draw a picture of what this force looks like.
Type of Force: Defined
Hydrogen Bonding:
Picture
Dipole-Dipole:
Dipole-Induced Dipole:
London Dispersion Forces:
12. List all the properties of liquids that are affected by intermolecular forces.