Draw four different Lewis electron-dot formulas for the SeO₂ molecule. (HINT: One should have two single bonds, two have a single and a double bond, and one two double bonds).

a. Are there any electron-dot formulas that you expect to give the best description? How would you describe the bonding in terms of electron-dot formulas?

b. Describe the bonding in SeO₂ in valence bond terms. If there is delocalized bonding, note this in your description and explain how molecular orbital theory can be useful here.

c. Determine the arrangement of electron pairs about Se in the SeO₂ molecule. What would you expect for the molecular geometry of the SeO₂ molecule?

d. Would you expect the O-Se-O angle in the SeO₂ molecule to be greater than, equal to, or less than 120°. Explain your answer.

e. Draw an electron-dot formula for the H₂Se molecule and determine its molecular geometry.

f. Compare the H-Se-H bond angle to the O-Se-O bond angle. Is it larger or smaller? Explain.

g. Determine whether the H₂Se and SeO₂ molecules have dipole moments. Describe how you arrived at your answer.