1-Using a wave model of electrons, describe what happens when we bring two hydrogen atoms together?

2-Draw an energy level diagram for O2 showing the atomic orbitals of both oxygen atoms and the molecular orbitals of the O2 molecule. What property of O2 can be accounted for as a result of this diagram?

3-We talked several times about the concept of a non-bonding orbital. How does this arise? Consider the case of the F2H1- anion and explain the bonding.

4-What fundamental assumption did Lewis make when he developed the %u201CLewis dot%u201D model?

5-What fundamental assumption did Gillespie make when formulating VSEPRT?

6-Define electronegativity. Use this concept to explain the concepts of covalent and ionic bonding. A graph might be useful here.

7-Consider CO2 and SO2. Explain why these molecules are polar or non-polar using vector arguments.

8- For the following compounds or ions:

i) Draw the Lewis dot picture

ii) Sketch the three-dimensional structure of the molecule and give the name to this shape

iii) Indicate whether the molecule is polar or non-polar.

a) CHCl3

b) PH3

c) SF6

d) NO31- (ignore the polarity question for this ion)

9- What bonding property is revealed by the Lewis Dot picture of SO3? What is %u201Creally%u201D going on here?

10-Explain London forces. Where does the property of polarizability come into play?

11-Explain hydrogen bonding. Why are hydrogen bonds substantially stronger than dipole-dipole bonds?

12- Explain in gory detail the relationship between temperature and vapor pressure. Lots of pictures might be helpful.

13-Why does water expand when it freezes?