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Chapter 22: Problem 43

Give an appropriate name to each of the following compounds: (a) \(\mathrm{ZnS} ;\) (b) \(\mathrm{KHSO}_{3} ;\) (c) \(\mathrm{K}_{2} \mathrm{S}_{2} \mathrm{O}_{3} ;\) (d) \(\mathrm{SF}_{4}\).

Short Answer

Expert verified
The names for the respective compounds are: (a) Zinc Sulfide, (b) Potassium Hydrogen Sulfite, (c) Potassium Thiosulfate, (d) Sulfur Tetrafluoride

Step by step solution

01

Identify the elements in the compound

To name a chemical compound, one needs to identify the individual elements from their chemical symbol. For example, for compound (a) \(Zn\) stands for Zinc and \(S\) stands for Sulfur.
02

Apply naming guidelines

For ionic compounds, the metal ion keeps its name (in this case, Zinc) and the nonmetal ion takes its root and attaches '-ide' at the end. So, \(ZnS\) is named Zinc Sulfide.
03

Repeat Steps 1 and 2 for the remaining compounds

Repeat the same process for each compound. For compound (b) \(K\) stands for Potassium, \(H\) for Hydrogen, \(S\) for Sulfur and \(O\) for oxygen. This compound is named as Potassium Hydrogen Sulfite. Similarly, (c)\(K_{2}S_{2}O_{3}\) is named Potassium Thiosulfate and (d) \(SF_{4}\) is named Sulfur Tetrafluoride.

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Most popular questions from this chapter

A 25.0 L sample of a natural gas, measured at \(25^{\circ} \mathrm{C}\). and 740.0 Torr, is bubbled through \(\mathrm{Pb}^{2+}(\mathrm{aq}),\) yielding \(0.535 \mathrm{g}\) of \(\mathrm{PbS}(\mathrm{s}) .\) What mass of sulfur can be recovered per cubic meter of this natural gas?

Joseph Priestley, a British chemist, was credited with the discovering oxygen in \(1774 .\) In his experiments, he generated oxygen gas by heating \(\mathrm{HgO}(\mathrm{s}) .\) The other product of the decomposition reaction is \(\mathrm{Hg}(1) .\) What volume of wet \(\mathrm{O}_{2}(\mathrm{g})\) is obtained from the decomposition of \(1.0 \mathrm{g} \mathrm{HgO}(\mathrm{s}),\) if the gas is collected over water at \(25^{\circ} \mathrm{C}\) and a barometric pressure of \(756 \mathrm{mmHg} ?\) The vapor pressure of water is \(23.76 \mathrm{mmHg}\) at \(25^{\circ} \mathrm{C}\).

Suppose that the sulfur present in seawater as \(\mathrm{SO}_{4}^{2-}\) \(\left(2650 \mathrm{mg} \mathrm{L}^{-1}\right)\) could be recovered as elemental sulfur. If this sulfur were then converted to \(\mathrm{H}_{2} \mathrm{SO}_{4},\) how many cubic kilometers of seawater would have to be processed to yield the average U.S. annual consumption of about 45 million tons of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

The trichloride ion, \(\mathrm{Cl}_{3}^{-1}\), is not very stable in aqueous solution. The equilibrium constant for the following dissociation reaction is 5.5 at \(25^{\circ} \mathrm{C}\) : $$\mathrm{Cl}_{3}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Cl}_{2}(\mathrm{aq})$$ (a) Draw a Lewis structure for the \(\mathrm{Cl}_{3}^{-}\) ion and predict the geometry. (b) Calculate the equilibrium concentration of \(\mathrm{Cl}_{3}^{-}\) if 0.0010 moles each of \(\mathrm{KCl}\) and \(\mathrm{Cl}_{2}\) are dissolved in water at \(25^{\circ} \mathrm{C}\) to make \(1.0 \mathrm{L}\) of solution.

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.
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