91Ó°ÊÓ

How does the molecular orbital diagram for a homonuclear diatomic species differ from that of a heteronuclear diatomic species?

How does the sea-of-electrons model (Chapter 8 ) explain the high electrical conductivity of gold? How does band theory explain this?

Make a sketch showing how two 1 s orbitals overlap to form a \(\sigma_{1s}\) bonding molecular orbital and a \(\sigma_{1 s}^{*}\) antibonding molecular orbital.

Consider the following molecular ions: \(\mathrm{N}_{2}^{+}, \mathrm{O}_{2}^{+}, \mathrm{C}_{2}^{+},\) and \(\mathrm{Br}_{2}^{2-} .\) Using MO theory, (a) write their orbital electron configuration; (b) predict their bond orders; (c) state whether you expect any of these species to exist.

Which of the following molecular ions is expected to have one or more unpaired electrons? (a) \(\mathrm{N}_{2}^{+} ;\) (b) \(\mathrm{O}_{2}^{+} ;\) (c) \(\mathrm{C}_{2}^{2+}\) (d) \(\mathrm{Br}_{2}^{2-} ;\) (e) \(\mathrm{O}_{2}^{-} ;\) (f) \(\mathrm{O}_{2}^{2-} ;\) (g) \(\mathrm{N}_{2}^{2-} ;\) (h) \(\mathrm{F}_{2}^{+}\)

Which of the following molecular ions have electrons in \(\pi\) antibonding orbitals? (a) \(\mathrm{O}_{2}^{-} ;\) (b) \(\mathrm{O}_{2}^{2-} ;\) (c) \(\mathrm{N}_{2}^{2-} ;\) (d) \(\mathrm{F}_{2}^{+}\) (e) \(\mathrm{N}_{2}^{+} ;\) (f) \(\mathrm{O}_{2}^{+} ;(\mathrm{g}) \mathrm{C}_{2}^{2+} ;\) (h) \(\mathrm{Br}_{2}^{2+}\)

The odd-electron molecule ClO affects the atmospheric chemistry of chlorofluorocarbons as illustrated by the reaction (where the \(^{*}\) indicates an excited-state oxygen atom): $$\mathrm{CF}_{2} \mathrm{Cl}_{2}+\mathrm{O}^{*} \rightarrow \mathrm{ClO}+\mathrm{CF}_{2} \mathrm{Cl}$$ Draw a molecular orbital diagram for ClO. Is the odd electron in a bonding or antibonding orbital?

The elusive molecule boron monoxide, \(\mathrm{BO},\) can be stabilized by bonding to platinum. Draw a molecular orbital diagram for BO. Is the odd electron in a bonding or antibonding orbital?

Do the \(1+\) cations of homonuclear diatomic molecules of the second-row elements always have shorter bond lengths than the corresponding neutral molecules?

Do any of the anions of the homonuclear diatomic molecules formed by \(\mathrm{B}, \mathrm{C}, \mathrm{N}, \mathrm{O},\) and \(\mathrm{F}\) have shorter bond lengths than those of the corresponding neutral molecules? Consider only the anions with \(1-\) or \(2-\) charge.