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.