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Chapter 10: Problem 3
How many atoms are directly bonded to the central atom in a tetrahedral molecule, a trigonal bipyramidal molecule, and an octahedral molecule?
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Sketch the shapes of these molecular orbitals: \(\sigma_{1 s}\), \(\sigma_{1 s}^{\star}, \pi_{2 p},\) and \(\pi_{2 p}^{\star}\) How do their energies compare?
The ionic character of the bond in a diatomic molecule can be estimated by the formula $$ \frac{\mu}{e d} \times 100 \% $$ where \(\mu\) is the experimentally measured dipole moment (in \(\mathrm{C} \mathrm{m}\) ), \(e\) is the electronic charge \((1.6022 \times\) \(10^{-19} \mathrm{C}\) ), and \(d\) is the bond length in meters. (The quantity \(e d\) is the hypothetical dipole moment for the case in which the transfer of an electron from the less electronegative to the more electronegative atom is complete.) Given that the dipole moment and bond length of \(\mathrm{HF}\) are \(1.92 \mathrm{D}\) and \(91.7 \mathrm{pm},\) respectively, calculate the percent ionic character of the molecule.
What is the relationship between the dipole moment and bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?
Describe the hybridization state of arsenic in arsenic pentafluoride \(\left(\mathrm{AsF}_{5}\right)\).
Describe the change in hybridization (if any) of the \(\mathrm{Al}\) atom in this reaction: $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$
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