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Chapter 8: Q9 E (page 446)
Why is the concept of hybridization required in valence bond theory?
Hybridization is necessary to determine the molecular geometry of complex.
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The bonding molecular orbital in \({{\rm{H}}_2}\) is lower in energy than an electron in \({\rm{1s}}\) orbital because the bonding molecular is more stable.
Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds: (a) \({\rm{ClNO}}\) (\({\rm{N}}\) is the central atom) (b) \({\rm{C}}{{\rm{S}}_{\rm{2}}}\) (c) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (\({\rm{C}}\) is the central atom) (d) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\) (\({\rm{S}}\) is the central atom) (e) \({\rm{S}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{S}}\) is the central atom) (f) \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{Xe}}\) is the central atom) (g) \({\rm{ClO}}{{\rm{F}}_{\rm{2}}}^{\rm{ + }}\) (\({\rm{Cl}}\) is the central atom).
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 \({{\rm{O}}_{\rm{2}}}\).
Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions.
(a) \({\rm{N}}{{\rm{a}}_{\rm{2}}}^{{\rm{2 + }}}\)
(b) \({\rm{M}}{{\rm{g}}_{\rm{2}}}^{{\rm{2 + }}}\)
(c) \({\rm{A}}{{\rm{l}}_{\rm{2}}}^{{\rm{2 + }}}\)
(d) \({\rm{S}}{{\rm{i}}_{\rm{2}}}^{{\rm{2 + }}}\)
(e) \({\rm{P}}_{\rm{2}}^{{\rm{2 + }}}\)
(f) \({{\rm{S}}_{\rm{2}}}^{{\rm{2 + }}}\)
(g) \({{\rm{F}}_{\rm{2}}}^{{\rm{2 + }}}\)
(h) \({\rm{A}}{{\rm{r}}_{\rm{2}}}^{{\rm{2 + }}}\)
For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains \({\rm{77}}{\rm{.55\% }}\)Xe and \({\rm{22}}{\rm{.45\% \;F}}\)by mass.
(a) What is the formula of the compound?
(b) Write a Lewis structure for the compound.
(c) Predict the shape of the molecules of the compound.
(d) What hybridization is consistent with the shape you predicted?
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