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Chapter 22: Problem 7

Use VSEPR theory to predict the probable geometric structures of (a) \(\mathrm{XeO}_{3} ;\) (b) \(\mathrm{XeO}_{4} ;\) (c) \(\mathrm{XeF}_{5}^{+}\).

Short Answer

Expert verified
Using the VSEPR theory: (a) \(\mathrm{XeO}_{3}\) predicts a trigonal pyramidal structure. (b) \(\mathrm{XeO}_{4}\) predicts a tetrahedral structure. (c) \(\mathrm{XeF}_{5}^{+}\) predicts a square pyramidal structure.

Step by step solution

01

Determine the Total Number of Electrons

Count the total number of valence electrons around the central atom (Xe). For \(\mathrm{XeO}_{3}\), the count is 8 (from Xe) + 3(6) (from each O) = 26 electrons. For \(\mathrm{XeO}_{4}\), the count is 8 (from Xe) + 4(6) (from each O) = 32 electrons. For \(\mathrm{XeF}_{5}^{+}\), the count is 8 (from Xe) + 5(7) (from each F) = 43 electrons, but we subtract one electron due to the +1 charge for a total of 42 electrons.
02

Place Electrons and Determine the Steric Number

For \(\mathrm{XeO}_{3}\), placing the electrons, we have 1 bond with each O (6 electrons), and one lone pair on Xe (2 electrons). This gives us a steric number of 4. For \(\mathrm{XeO}_{4}\), we have one bond with each O (8 electrons), and no lone pairs giving us a steric number of 4. For \(\mathrm{XeF}_{5}^{+}\), we have one bond with each F (10 electrons), and one lone pair on Xe (2 electrons). This gives us a steric number of 6.
03

Predict the Shape

Using the steric number, we can predict the shape. For \(\mathrm{XeO}_{3}\) with a steric number of 4 and 1 lone pair, the shape is trigonal pyramidal. For \(\mathrm{XeO}_{4}\) with a steric number of 4 and no lone pairs, the shape is tetrahedral. For \(\mathrm{XeF}_{5}^{+}\) with a steric number of 6 and 1 lone pair, the shape is square pyramidal.

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Most popular questions from this chapter

Give an appropriate formula for each of the following compounds: (a) calcium sulfate dihydrate; (b) hydrosulfuric acid; (c) sodium hydrogen sulfate; (d) disulfuric acid.

In water, \(\mathrm{O}^{2-}\) is a strong base. If \(50.0 \mathrm{mg}\) of \(\mathrm{Li}_{2} \mathrm{O}\) is dissolved in \(750.0 \mathrm{mL}\) of aqueous solution, what will be the pH of the solution?

Give a practical laboratory method that you might use to produce small quantities of the following gases and comment on any difficulties that might arise: (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{NO} ;\) (c) \(\mathrm{H}_{2} ;\) (d) \(\mathrm{NH}_{3} ;\) (e) \(\mathrm{CO}_{2}\).

Use the following electrode potential diagram for basic solutions to classify each of the statements below as true or false. Assume standard conditions. $$\begin{aligned}\mathrm{SO}_{4}^{2-} \stackrel{-0.936 \mathrm{V}}{\longrightarrow} \mathrm{SO}_{3}^{2-} & \stackrel{-0.576 \mathrm{V}}{\longrightarrow} \\\& \mathrm{S}_{2} \mathrm{O}_{3}^{2-} \stackrel{-0.74 \mathrm{V}}{\longrightarrow} \mathrm{S} \stackrel{-0.476 \mathrm{V}}{\longrightarrow} \mathrm{S}^{2-}\end{aligned}$$ (a) Sulfate \(\left(\mathrm{SO}_{4}^{2-}\right)\) is a stronger oxidant than thiosulfate \(\left(\mathrm{S}_{2} \mathrm{O}_{3}^{2}\right)\) in basic solution. (b) \(S^{2-}\) can be used as a reducing agent in basic solutions. (c) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) is stable with respect to disproportionation to \(\mathrm{SO}_{3}^{2-}\) and \(\mathrm{S}\) in basic solution.

What mass of \(\mathrm{Na}_{2} \mathrm{SO}_{3}\) was present in a sample that required \(26.50 \mathrm{mL}\) of \(0.0510 \mathrm{M} \mathrm{KMnO}_{4}\) for its oxidation to \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in an acidic solution? \(\mathrm{MnO}_{4}^{-}\) is reduced to \(\mathrm{Mn}^{2+}\).
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