# Practice Problem

10D.1. (a) The individual bonds in $\mathrm{PCl}_{5}$ are polar, yet the molecule as a whole is nonpolar. Explain how this is so.
(b) How do the bond angles in $\mathrm{PCl}_{5}$ compare to the "ideal" angles for the general geometric pattern predicted by VSEPR?
(c) Repeat part b for $\mathrm{PCl}_{3}$.

10D.2. (i) Do the parallel example problems without looking at the key, then check yourself against the key.
(ii) Determine the molecular geometry of the following molecules using VSEPR.
(iii) Give the hybridization of the central atom and the geometry of the following molecules from valence bond theory. In cases where lone pairs are present, indicate how the bond angle will differ from "ideal."
a) $\mathrm{BF}_{3}$
c) $\mathrm{BrF}_{5}$
b) $\mathrm{NH}_{3}$
d) $\mathrm{IBr}_{3}$

10D.3. Predict the electron-domain geometry and the hybridization of the central atom in
(a) $\mathrm{SO}_{3}{ }^{2-}$
(b) $\mathrm{SF}_{6}$
10D.4. In each of the following pairs, which ion or molecule has the smaller bond angle(s)?
a) $\mathrm{SF}_{6}$ or $\mathrm{H}_{2} \mathrm{~S}$
b) $\mathrm{BF}_{3}$ or $\mathrm{NH}_{4}^{+}$
c) $\mathrm{H}_{2} \mathrm{O}$ or $\mathrm{NH}_{3}$

Question

# Practice Problem

10D.1. (a) The individual bonds in $\mathrm{PCl}_{5}$ are polar, yet the molecule as a whole is nonpolar. Explain how this is so.
(b) How do the bond angles in $\mathrm{PCl}_{5}$ compare to the "ideal" angles for the general geometric pattern predicted by VSEPR?
(c) Repeat part b for $\mathrm{PCl}_{3}$.

10D.2. (i) Do the parallel example problems without looking at the key, then check yourself against the key.
(ii) Determine the molecular geometry of the following molecules using VSEPR.
(iii) Give the hybridization of the central atom and the geometry of the following molecules from valence bond theory. In cases where lone pairs are present, indicate how the bond angle will differ from "ideal."
a) $\mathrm{BF}_{3}$
c) $\mathrm{BrF}_{5}$
b) $\mathrm{NH}_{3}$
d) $\mathrm{IBr}_{3}$

10D.3. Predict the electron-domain geometry and the hybridization of the central atom in
(a) $\mathrm{SO}_{3}{ }^{2-}$
(b) $\mathrm{SF}_{6}$
10D.4. In each of the following pairs, which ion or molecule has the smaller bond angle(s)?
a) $\mathrm{SF}_{6}$ or $\mathrm{H}_{2} \mathrm{~S}$
b) $\mathrm{BF}_{3}$ or $\mathrm{NH}_{4}^{+}$
c) $\mathrm{H}_{2} \mathrm{O}$ or $\mathrm{NH}_{3}$

StudyXY · Accepted Answer

I'll provide detailed solutions for each part of the practice problems. (a) The individual bonds in $\mathrm{PCl}_{5}$ are polar due to the difference in electronegativity between phosphorus (P) and chlorine (Cl). (ii) Using VSEPR, we can determine the molecular geometry of the following molecules: (a) The electron-domain geometry of $\mathrm{SO}_{3}{ }^{2-}$ is trigonal planar, and the central sulfur atom is sp$^2$ hybridized. (a) $\mathrm{SF}_{6}$ has a larger bond angle compared to $\mathrm{H}_{2} \mathrm{~S}$. However, $\mathrm{NH}_{3}$ has a smaller deviation from the ideal bond angle compared to $\mathrm{H}_{2} \mathrm{O}$.

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QuestionAnatomy and Physiology

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Step 1
I'll provide detailed solutions for each part of the practice problems.

Step 2
(a) The individual bonds in $\mathrm{PCl}_{5}$ are polar due to the difference in electronegativity between phosphorus (P) and chlorine (Cl).

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