OUTLINE:

I Introduction

II. Review topics
A. Atomic orbitals
1. Orbital diagrams
2. An example of filling an
orbital diagram
3. Valence shells
B. Covalent bonding
C. Lewis structures
1. How to assign dots for
atoms
2. The octet rule
3. The Lewis structure of
molecular chlorine
4. The Lewis structure of
carbon tetrachloride
5. Multiple bonds

III. VSEPR theory
A. Molecular shape
1. Lewis structure and
molecular shape
2. Common molecular
shapes
3. Characteristic bond
angles
B. VSEPR theory
1. Definition of VSEPR
theory
2. VSEPR theory and lone
pairs
3. Explanation of the bond
angles in ammonia
4. Explanation of the bond
angles in water
5. The effects of lone pairs
on shape
6. Determining the shape
of phosphorus
trichloride
7. VSEPR theory and multiple
bonds

IV. Hybrid orbitals
A. Description of hybrid
orbitals
1. Bonding in methane
2. Creation of hybrid orbitals
3. Hybrid orbitals are new
orbital types
4. The shape of hybrid
orbitals
5. Naming types of
hybridization
B. Shapes created by hybrid
orbitals
1. sp3 hybrid orbitals
2. sp3 hybrid orbitals with
lone pairs
3. sp2 hybrid orbitals
4. sp hybrid orbitals
C. Bond types
1. Sigma bonds
2. Pi bonds and double bonds
3. Pi bonding in triple bonds
4. Characteristics of single,
double and triple bonds
5. Pi bonds are nonrotational

V. Polarity
A. Description of polarity
1. Electronegativity
B. Determining polarity from
molecular shape
1. The polarity of ammonia
2. Carbon dioxide is
nonpolar
3. Predicting the polarity of
water
4. Predicting the polarity of
methane

VI. Intermolecular forces
A. The effects of
intermolecular forces
1. The states of matter
2. van der Waals forces
B. Types of intermolecular
forces
1. London forces and
instantaneous dipoles
a. Induced dipoles
b. Effects of London
forces on boiling
points
2. Dipole interactions
a. Effects of dipole
interactions on
boiling points
3. Hydrogen bonding
a. Effects of hydrogen
bonding on
boiling points

VII. Larger molecules

VIII. Conclusion