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Chapter 22: Problem 90

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\). The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from \(\mathrm{GeO}_{2}\).

Short Answer

Expert verified
The balanced chemical equations for the various steps involved in preparing ultrapure germanium (Ge) from germanium dioxide (GeO鈧�) are as follows: 1. Reduction of GeO鈧� with carbon (C): \(GeO_{2} + C \rightarrow Ge + CO_{2}\) 2. Conversion of Ge to GeCl鈧� using Cl鈧�: \(Ge + 2 Cl_{2} \rightarrow GeCl_{4}\) 4. Hydrolysis of GeCl鈧� in water: \(GeCl_{4} + 2 H_{2}O \rightarrow GeO_{2} + 4 HCl\) 5. Reduction of GeO鈧� with H鈧�: \(GeO_{2} + 2 H_{2} \rightarrow Ge + 2 H_{2}O\)

Step by step solution

01

Reduction of GeO鈧� with Carbon

To reduce germanium dioxide (GeO鈧�) with carbon (C), we can use the following balanced chemical equation: \[GeO_{2} + C \rightarrow Ge + CO_{2}\]
02

Conversion of Ge to GeCl鈧� using Cl鈧�

To convert germanium (Ge) to germanium tetrachloride (GeCl鈧�) using chlorine (Cl鈧�), we can use the following balanced chemical equation: \[Ge + 2 Cl_{2} \rightarrow GeCl_{4}\]
03

Purification of GeCl鈧� by distillation

The purification of GeCl鈧� by distillation is a physical process, not a chemical reaction. Therefore, no chemical equation is needed for this step.
04

Hydrolysis of GeCl鈧� in water

To hydrolyze germanium tetrachloride (GeCl鈧�) in water (H鈧侽), we can use the following balanced chemical equation: \[GeCl_{4} + 2 H_{2}O \rightarrow GeO_{2} + 4 HCl\]
05

Reduction of GeO鈧� with H鈧�

To reduce germanium dioxide (GeO鈧�) with hydrogen gas (H鈧�), we can use the following balanced chemical equation: \[GeO_{2} + 2 H_{2} \rightarrow Ge + 2 H_{2}O\]

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Most popular questions from this chapter

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) chlorate ion, (b) hydroiodic acid, (c) iodine trichloride, (d) sodium hypochlorite, (e) perchloric acid, (f) xenon tetrafluoride.

Complete and balance the following equations: (a) \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (f) \(\mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow\)

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}{ }^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\). Nitrogen and the Other Group 5A Elements (Sections 22.7 and 22.8)

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) nitric oxide, (b) hydrazine, (c) potassium cyanide, (d) sodium nitrite, (e) ammonium chloride, (f) lithium nitride.
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