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Chapter 8: Q4 E (page 451)
A typical barometric pressure in Redding, California, is about 750mm Hg. Calculate this pressure in atm and kPa.
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Use valence bond theory to explain the bonding in\({{\rm{F}}_2},{\rm{HF}}\), and\({\rm{ClBr}}\). Sketch the overlap of the atomic orbitals involved in the bonds.
Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.
Compare the atomic and molecular orbital diagrams to identify the member of each of the following pairs that has the highest first ionization energy (the most tightly bound electron) in the gas phase:
(a) \({\rm{H}}\) and \({{\rm{H}}_{\rm{2}}}\)
(b) \({\rm{N}}\)and \({{\rm{N}}_{\rm{2}}}\)
(c) \({\rm{O}}\)and \({{\rm{O}}_{\rm{2}}}\)
(d) \({\rm{C}}\)and \({{\rm{C}}_{\rm{2}}}\)
(e) \({\rm{B}}\)and \({{\rm{B}}_{\rm{2}}}\)
Determine the bond order of each member of the following groups, and determine which member of each group is predicted by the molecular orbital model to have the strongest bond.
(a) \({{\rm{H}}_{\rm{2}}}{\rm{,}}{{\rm{H}}_{\rm{2}}}{\rm{ + ,H}}_{\rm{2}}^{\rm{ - }}\)
(b) \({{\rm{O}}_{\rm{2}}}{\rm{,O}}_{\rm{2}}^{{\rm{2 + }}}{\rm{,O}}_{\rm{2}}^{{\rm{2 - }}}\)
(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{,B}}{{\rm{e}}_{\rm{2}}}{\rm{ + ,B}}{{\rm{e}}_{\rm{2}}}\)
(d) \({{\rm{F}}_{\rm{2}}}{\rm{,\;}}{{\rm{F}}_{\rm{2}}}{\rm{ + ,}}\;\;\;{\rm{F}}_{\rm{2}}^{\rm{ - }}\)
(e) \({{\rm{N}}_{\rm{2}}}{\rm{,\;N}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\;\;\;{\rm{N}}_{\rm{2}}^{\rm{ - }}\)
Label the molecular orbital shown as σ or Π, bonding or antibonding, and indicate where the node occurs.
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