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Chapter 10: Problem 60

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{PCl}_{3} ;\) (b) \(\mathrm{SO}_{4}^{2-}\); (c) \(\mathrm{SOCl}_{2} ;\) (d) \(\mathrm{SO}_{3} ;\) (e) \(\mathrm{BrF}_{4}^{+}\).

Short Answer

Expert verified
The geometric shapes are (a) PCl3 - trigonal pyramidal; (b) SO42- - tetrahedral; (c) SOCl2 - trigonal planar; (d) SO3 - trigonal planar; (e) BrF4+ - square planar.

Step by step solution

01

Determine the Electron Domains (PCl3)

First, identify the central atom (P) and its bonding (3 from Cl) and non-bonding electron pairs. Phosphorus (P), in the 5th group of the Periodic Table, has 5 valence electrons. There are 3 Chlorines (Cl), each contributes an electron for bonding. So there are 3 bonding pairs and one lone pair in PCl3.
02

Predict the Shape (PCl3)

Four domains in total (3 bonding, 1 non-bonding) suggest a tetrahedral arrangement. However, due to the lone pair, the actual shape realized is 'trigonal pyramidal'.
03

Determine the Electron Domains (SO42-)

Sulfur (S) is the central atom. It has 6 valence electrons. Oxygen atoms contribute 4 electrons for bonding. Taking into consideration 2 additional electrons due to the negative charge (2-), there are 6 pairs in total: 4 bonding and 2 non-bonding.
04

Predict the Shape (SO42-)

Six domains in total suggest an octahedral arrangement. However, considering 2 non-bonding pairs, the actual shape is tetrahedral.
05

Repeat for Rest of the Molecules/Ions

Repeat steps 1 and 2 for each remaining molecule/ion. This should lead to the following shapes: SOCl2 - 'trigonal planar', SO3 - 'trigonal planar', and BrF4+ - 'square planar'.

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Most popular questions from this chapter

Without referring to tables or figures in the text other than the periodic table, indicate which of the following atoms, \(\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As},\) or \(\mathrm{Mg},\) has the intermediate value when they are arranged in order of increasing electronegativity.

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?

Each of the following is either linear, angular (bent), planar, tetrahedral, or octahedral. Indicate the correct shape of (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{N}_{2} \mathrm{O}_{4} ;\) (c) \(\mathrm{HCN} ;\) (d) \(\mathrm{SbCl}_{6}^{-}\); (e) \(\mathrm{BF}_{4}^{-}\)

Write acceptable Lewis structures for the following molecules: (a) \(\mathrm{H}_{2} \mathrm{NNH}_{2}\); (b) HOClO; (c) (HO) \(_{2}\) SO; (d) HOOH (e) SO \(_{4}^{2-}\).
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