91Ó°ÊÓ

Describe the molecular orbitals formed by the overlap of the following atomic orbitals. (Assume that the bond lies along the \(z\) axis of the coordinate system.) (a) \(2 s+2 s\) (b) \(2 p_{x}+2 p_{x}\) (c) \(2 p_{y}+2 p_{y}\) (d) \(2 p_{z}+2 p_{z}\) (e) \(2 s+2 p_{z}\)

Write the electron configuration for the following diatomic molecules and calculate the bond order in each molecule. (a) \(\mathrm{H}_{2}\) (b) \(\mathrm{C}_{2}\) (c) \(\mathrm{N}_{2}\) (d) \(\mathrm{O}_{2}\) (e) \(\mathrm{F}_{2}\)

Use molecular orbital theory to predict whether the \(\mathrm{H}_{2}^{+}, \mathrm{H}_{2}^{-}\), and \(\mathrm{H}_{2}{ }^{2-}\) ions should be more stable or less stable than a neutral \(\mathrm{H}_{2}\) molecule.

Use molecular orbital theory to explain why the oxygen-oxygen bond is stronger in the \(\mathrm{O}_{2}\) molecule than in the \(\mathrm{O}_{2}^{2-}\) (peroxide) ion.

Use molecular orbital theory to predict whether the bond order in the superoxide ion, \(\mathrm{O}_{2}^{-}\), should be larger or smaller than the bond order in a neutral \(\mathrm{O}_{2}\) molecule.

Use molecular orbital theory to predict whether the peroxide ion, \(\mathrm{O}_{2}{ }^{2-}\), should be paramagnetic.

Write the electron configuration for the following diatomic molecules. Calculate the bond order in each molecule. (a) \(\mathrm{HF}\) (b) \(\mathrm{CO}\) (c) \(\mathrm{CN}^{-}\) (d) \(\mathrm{ClO}^{-}\) (e) \(\mathrm{NO}^{+}\)

Classify the following molecules as paramagnetic or diamagnetic. (a) HF (b) \(\mathrm{CO}\) (c) \(\mathrm{CN}^{-}\) (d) NO (e) \(\mathrm{NO}^{+}\)