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Chapter 23: Problem 66

The only important compounds of \(\mathrm{Ag}(\mathrm{II})\) are \(\mathrm{AgF}_{2}\) and AgO. Why would you expect these two compounds to be stable, but not other silver(II) compounds such as \(\mathrm{AgCl}_{2}, \mathrm{AgBr}_{2},\) and \(\mathrm{AgS} ?\)

Short Answer

Expert verified
AgF2 and AgO are stable because Fluorine and Oxygen have high electron affinities that result in strong ionic bonds with Silver. Other elements like Chlorine, Bromine and Sulfur have less electron affinity and thus form unstable bonds with Silver.

Step by step solution

01

Understand the role of electron affinity

Different elements have different affinities for electrons. Fluorine (F) has the highest electron affinity, meaning it attracts electrons more readily than other elements. When Ag donates an electron to F, it forms a strong ionic bond resulting in the formation of AgF2. This is why AgF2 is stable.
02

Understanding the Role of Oxygen

Oxygen has a high electronegativity and tends to form a -2 charge when it gains two electrons. When silver donates two electrons to oxygen, it forms a strong ionic bond, forming AgO. This is why AgO is also a stable compound.
03

Understand the instability of other compounds

Chlorine (Cl), Bromine (Br), and Sulfur (S) have lower electron affinity than fluorine and oxygen. This means they are less capable to attract electrons from silver to form stable ionic bonds. Hence, AgCl2, AgBr2 and AgS are not stable compounds.

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Most popular questions from this chapter

Nickel can be determined as nickel dimethylglyoximate, a brilliant scarlet precipitate that has the composition \(20.31 \% \mathrm{Ni}, 33.26 \% \mathrm{C}, 4.88 \% \mathrm{H}, 22.15 \% \mathrm{O},\) and \(19.39 \%\) N. \(\mathrm{A} 15.020 \mathrm{g}\) steel sample is dissolved in concentrated HCl(aq). The solution obtained is suitably treated to remove interfering ions, to establish the proper \(\mathrm{pH},\) and to obtain a final solution volume of \(250.0 \mathrm{mL} .\) A \(10.00 \mathrm{mL}\) sample of this solution is then treated with dimethylglyoxime. The mass of purified, dry nickel dimethylglyoximate obtained is \(0.104 \mathrm{g}\) (a) What is the empirical formula of nickel dimethylglyoximate? (b) What is the mass percent nickel in the steel sample?

In the metallurgical extraction of silver and gold, an alloy of the two metals is often obtained. The alloy can be separated into Ag and Au either with concentrated \(\mathrm{HNO}_{3}\) or boiling concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4},\) in a process called parting. Write chemical equations to show how these separations work.

What products are obtained when \(\mathrm{Mg}^{2+}(\mathrm{aq})\) and \(\mathrm{Cr}^{3+}(\mathrm{aq})\) are each treated with a limited amount of NaOH(aq)? With an excess of \(\mathrm{NaOH}(\) aq)? Why are the results different in these two cases?A certain steel is to be analyzed for \(\mathrm{Cr}\) and \(\mathrm{Mn}\). By suitable treatment, the Cr in the steel is oxidized to \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) and the \(\mathrm{Mn}\) to \(\mathrm{MnO}_{4}(\mathrm{aq}) . \mathrm{A} 10.000 \mathrm{g}\) sample of steel is used to produce \(250.0 \mathrm{mL}\) of a solution containing \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) and \(\mathrm{MnO}_{4}^{-}(\mathrm{aq}) . \mathrm{A} 10.00 \mathrm{mL}\) portion of this solution is added to \(\mathrm{BaCl}_{2}(\mathrm{aq}),\) and by proper adjustment of the \(\mathrm{pH}\), the chromium is completely precipitated as \(\mathrm{BaCrO}_{4}(\mathrm{s}) ; 0.549 \mathrm{g}\) is obtained. A second \(10.00 \mathrm{mL}\) portion of the solution requires exactly \(15.95 \mathrm{mL}\) of \(0.0750 \mathrm{M} \mathrm{Fe}^{2+}(\mathrm{aq})\) for its titration in acidic solution. Calculate the \(\%\) Cr and \% \(\mathrm{Mn}\) in the steel sample. [Hint: In the titration \(\mathrm{MnO}_{4}^{-}(\mathrm{aq})\) is reduced to \(\mathrm{Mn}^{2+}(\mathrm{aq})\) and \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) is reduced to \(\left.\mathrm{Cr}^{3+}(\mathrm{aq}) ; \text { the } \mathrm{Fe}^{2+}(\mathrm{aq}) \text { is oxidized to } \mathrm{Fe}^{3+}(\mathrm{aq}) \cdot\right]\)

Balance the following oxidation-reduction equations. $$\text { (a) } \mathrm{Fe}_{2} \mathrm{S}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{S}(\mathrm{s})$$ $$\begin{aligned} &\text { (b) } \mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\\ &&\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}$$ $$\begin{aligned} &\text { (c) } \mathrm{Ag}(\mathrm{s})+\mathrm{CN}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\\\ &&\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \end{aligned}$$

Write plausible equations for the following reactions occurring in the hydrometallurgy of the coinage metals. (a) Copper is precipitated from a solution of copper(II) sulfate by treatment with \(\mathrm{H}_{2}(\mathrm{g})\) (b) Gold is precipitated from a solution of \(\mathrm{Au}^{+}\) by adding iron(II) sulfate. (c) Copper(II) chloride solution is reduced to copper(I) chloride when treated with \(\mathrm{SO}_{2}(\mathrm{g})\) in acidic solution.
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