Covalent Bonds – Review 2013
Name____________________________
1. Define the HONC1234 rule:
Use the HONC1234 rule to make structural formulas out of the following molecular formula
C4H11N
C2H6O
C6H12O2
C3OH2
C3H3N
2. Define isomer.
Create 3 isomers for the following structural formula using the HONC1234 rule:
C3H5O2N
3. Draw Lewis dot symbols for the following elements and determine how many covalent bonds they can
make:
C
F
Te
Ge
S
P
H
4. Be able to draw Lewis Dot Diagrams for molecules. Be able to locate the shared pairs and the lone
pairs in the diagrams.
Formul Lewis Dot Diagram
Number of
Number of
a
Bonding
Lone Pairs
Pairs
CBr4
H2S
PF3
5. Draw Lewis dot structure and structural formula for the following molecules (include lone pairs in the
structural formulas)
Molecular
formula
Lewis Dot structure
Structural formula (with lone
pairs)
C2H6O2
C2H4
O2
N2H2
P2
6. Define polar bond, non-polar bond and ionic bond: Give the electronegativity difference for each.
7. Polarity: be able to look at a molecule or molecular formula and figure out if it is polar covalent, nonpolar covalent, or ionic. Identify the bond type between the following atoms.
 Li and S
 Cu and P
 As and Br
 I and I
 Se and Cl
 N and F
 Sn and Cl
8. For each of the following molecules
a. calculate the difference in polarity for each bond.
b. Include dipoles for each polar bond.
c. Determine if the molecule is polar or non-polar. Include dipole of molecule if polar.
d. Label molecule as polar or non-polar and give your reasons for your decision.
9. Match the following compounds to the bond types.
NPC) Non Polar Covalent PC) Polar Covalent
I) Ionic
___1.
KBr
___4.
CaCl2
___8.
ZnI2
___2.
CO2
___5.
Br2
___9.
NaCl
___3.
CH4
___6.
Na2O
___10. C3H8
___7.
SiO2
10. Explain why CO2 is a nonpolar molecule even though its bonds are polar.
11. Define: molecule, covalent bond, octet rule, electronegativity, structural formula, molecular
formula, dipole