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Chapter 22: Problem 44
Give an appropriate formula for each of the following compounds: (a) calcium sulfate dihydrate; (b) hydrosulfuric acid; (c) sodium hydrogen sulfate; (d) disulfuric acid.
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Without per frming detailed calculations, determine which of the following compounds has the greatest percent oxygen by mass: dinitrogen tetroxide, aluminum oxide, tetraphosphorus hexoxide, or carbon dioxide.
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.
In \(1988,\) G. J. Schrobilgen, professor of chemistry at McMaster University in Canada, reported the synthesis of an ionic compound, \([\mathrm{HCNKrF}]\left[\mathrm{AsF}_{6}\right],\) which consists of \(\mathrm{HCNKr} \mathrm{F}^{+}\) and \(\mathrm{AsF}_{6}^{-}\) ions. In the \(\mathrm{HCNKr} \mathrm{F}^{+}\) ion, the krypton is covalently bonded to both fluorine and nitrogen. Draw Lewis structures for these ions, and estimate the bond angles.
Give a specific example of a chemical equation that illustrates the (a) reaction of a metal sulfide with \(\mathrm{HCl}(\mathrm{aq})\) (b) action of a nonoxidizing acid on a metal sulfite; (c) oxidation of \(\mathrm{SO}_{2}(\mathrm{aq})\) to \(\mathrm{SO}_{4}^{2-}(\mathrm{aq})\) by \(\mathrm{MnO}_{2}(\mathrm{s})\) in acidic solution; (d) disproportionation of \(S_{2} \mathrm{O}_{3}^{2-}\) in acidic solution.
Use VSEPR theory to predict the probable geometric structures of (a) \(\mathrm{XeO}_{3} ;\) (b) \(\mathrm{XeO}_{4} ;\) (c) \(\mathrm{XeF}_{5}^{+}\).
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