Chapter 9: Molecular Geometry and Bonding Theories
Definitions:

Molecular Shape:
o Bond Angle:

VSEPR Model:
o Electron Domain:

Bonding Pair:

Nonbonding Pair:
o Electron Domain Geometry:
o Molecular Geometry:

Effect Due to Multiple Bonds:

Effect Due to Nonbonding Pairs:

Bond Dipole:

Valence – Bond Theory:

Hybrid Orbitals:
o Hybridization:

Sigma Bonds:

Pi Bonds:
o Localized:
o Delocalized:
Table 1: VSEPR Model
Number of
Domains
Electron
DomainGeometry
Bond
Angle
2
3
4
5
6
Free Response:
1. For the Compound: H2CO3
a. Draw the Lewis Structure:
Hybrid
Orbital
Number of
Bonds
Number of
Free
Electron
Pairs
Molecular
Geometry
b. Determine the Molecular Geometry for Each Element (Exclude Repeats and
Elements bonded to only One Atom)
c. Estimate the Bond Angles for Every Bond (Exclude Repeats)
d. List the Hybridization for Every Bond (Exclude Repeats)
e. How many Sigma Bonds are Present and how many Pi Bonds are Present?
f. Are any bonds delocalized?
2. For the Compound: C6H12O6
a. Draw the Lewis Structure: (It includes a Ring!)
b. If Hydrogen has a Electronegativity of 2.2, Oxygen has an electronegativity of
3.44, and Carbon has an electronegativity of 2.55; what is the polarity of each
bond?
c. What is the polarity of the overall molecule?
3. For the Compound: SO42–
a. Draw the Lewis Structure:
b. Determine the Molecular Geometry for Each Element (Exclude Repeats and
Elements bonded to only One Atom)
c. Estimate the Bond Angles for Every Bond (Exclude Repeats)
d. List the Hybridization for Every Bond (Exclude Repeats)
e. How many Sigma Bonds are Present and how many Pi Bonds are Present?
f. Are any bonds delocalized?
g. If Sulfur has a Electronegativity of 2.58 and Oxygen has an electronegativity of
3.44, what is the polarity of each bond?
h. What is the polarity of the overall molecule?