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Chapter 8: Q34E (page 450)
If molecular orbitals are created by combining five atomic orbitals from atom A and five atomic orbitals from atom B combine, how many molecular orbitals will result?
Ten molecular orbitals will result.
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Use valence bond theory to explain the bonding in\({{\rm{O}}_{\rm{2}}}\). Sketch the overlap of the atomic orbitals involved in the bonds in \({{\rm{O}}_{\rm{2}}}\).
For the first ionization energy for an \({{\rm{N}}_2}\) molecule, what molecular orbital is the electron removed from?
What is the hybridization of the central atom in each of the following?
(a) \({\rm{Be}}{{\rm{H}}_{\rm{2}}}\)
(b) \({\rm{S}}{{\rm{F}}_{\rm{6}}}\)
(c) \({\rm{PO}}_{\rm{4}}^{{\rm{3 - }}}\)
(d) \({\rm{PC}}{{\rm{l}}_{\rm{5}}}\)
Draw the orbital diagram for carbon in showing how many carbon atom electrons are in each orbital.
For each of the following molecules, indicate the hybridization requested and whether or not the electrons will be delocalized: (a) ozone (\({{\rm{O}}_{\rm{3}}}\)) central \({\rm{O}}\) hybridization (b) carbon dioxide (\({\rm{C}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{C}}\) hybridization (c) nitrogen dioxide (\({\rm{N}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{N}}\) hybridization (d) phosphate ion (\({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\)) central \({\rm{P}}\) hybridization.
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