Learn about Molecular Bonding, Shape, and Intermolecular Forces.
Bonding II: Molecular
Bonding, Shape, and Intermolecular Forces
Molecular Bonding, Shape, and Intermolecular Forces starts with a review of electron orbitals and Lewis structures leading to VSEPR theory. Examples with three-dimensional models facilitate understanding and prediction of molecular shapes. Hybridization of orbitals and the formation of sigma and pi bonds are also covered. Understanding three-dimensional structure provides a framework for discussing polarity and electronegativity. Three-dimensional models and animations show interactions leading to polarity. Forces acting between molecules are described, explaining the states of matter and boiling and melting points.
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
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A. Atomic orbitals 
