Problem 14
The atoms in a single bond can rotate about the internuclear axis without breaking the bond. The atoms in a double and triple bond cannot rotate about the internuclear axis unless the bond is broken. Why?
Problem 16
As compared with \(\mathrm{CO}\) and \(\mathrm{O}_{2}, \mathrm{CS}\) and \(\mathrm{S}_{2}\) are very unstable molecules. Give an explanation based on the relative abilities of the sulfur and oxygen atoms to form \(\pi\) bonds.
Problem 17
Compare and contrast bonding molecular orbitals with antibonding molecular orbitals.
Problem 18
What modification to the molecular orbital model was made from the experimental evidence that \(\mathrm{B}_{2}\) is paramagnetic?
Problem 19
Why does the molecular orbital model do a better job in explaining the bonding in \(\mathrm{NO}^{-}\) and \(\mathrm{NO}\) the hybrid orbital model?
Problem 20
The three NO bonds in \(\mathrm{NO}_{3}^{-}\) are all equivalent in length and strength. How is this explained even though any valid Lewis structure for \(\mathrm{NO}_{3}^{-}\) has one double bond and two single bonds to nitrogen?
Problem 21
Use the localized electron model to describe the bonding in \(\mathrm{H}_{2} \mathrm{O}\) .
Problem 22
Use the localized electron model to describe the bonding in \(\mathrm{CCl}_{4}\) .
Problem 23
Use the localized electron model to describe the bonding in \(\mathrm{H}_{2} \mathrm{CO}(\text { carbon is the central atom })\)
Problem 24
Use the localized electron model to describe the bonding in \(\mathrm{C}_{2} \mathrm{H}_{2}\) (exists as \(\mathrm{HCCH} )\)
