Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 22: Problem 88

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 GeCl_ by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; GeCl_ is then hydrolyzed in water to 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 GeO \(_{2} .\)

Short Answer

Expert verified
The balanced chemical equations for each step in the formation of ultrapure germanium are as follows: 1. Reduction of GeO2 with carbon: \[GeO_{2}(s) + C(s) \rightarrow Ge(s) + CO_{2}(g)\] 2. Conversion of Ge to GeCl4: \[Ge(s) + 2\,Cl_{2}(g) \rightarrow GeCl_{4}(g)\] 3. Reduction of GeCl4 to elemental germanium with H2: \[GeCl_{4}(g) + 2\,H_{2}(g) \rightarrow Ge(s) + 4\,HCl(g)\]

Step by step solution

01

Reduction of GeO2 with Carbon

In this step, GeO2 reacts with carbon (C) to form germanium (Ge) and carbon dioxide (CO2). The balanced chemical equation for this reaction can be written as follows: \[GeO_{2}(s) + C(s) \rightarrow Ge(s) + CO_{2}(g)\]
02

Conversion of Ge to GeCl4

Germanium reacts with chlorine gas (Cl2) to form germanium tetrachloride (GeCl4). The balanced chemical equation for this reaction is: \[Ge(s) + 2\,Cl_{2}(g) \rightarrow GeCl_{4}(g)\]
03

Purification of GeCl4 by Distillation

In this step, germanium tetrachloride (GeCl4) undergoes purification through distillation. This step does not involve a chemical reaction, so there is no balanced chemical equation for distillation.
04

Reduction of GeCl4 to Elemental Germanium with H2, and Zone Refining

In this final step, germanium tetrachloride reacts with hydrogen gas (H2) to form elemental germanium and hydrochloric acid (HCl). The balanced chemical equation for this reaction is: \[GeCl_{4}(g) + 2\,H_{2}(g) \rightarrow Ge(s) + 4\,HCl(g)\] After this reaction, the germanium undergoes zone refining, which is a purification process that does not involve a chemical reaction, so there is no balanced equation for this final step.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid.(c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.

Write a balanced chemical reaction for the condensation reaction between \(\mathrm{H}_{3} \mathrm{PO}_{4}\) molecules to form \(\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10} .\)

Write the formulas for the following compounds, and indicate the oxidation state of the group 4 A element or of boron in each: (a) boric acid, (b) silicon tetrabromide, (c) lead(II) chloride, (d) sodium tetraborate decahydrate (borax), (e) boric oxide, (f) germanium dioxide.

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over catalyst at \(800^{\circ} \mathrm{C} .\) Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.

Although the \(\mathrm{ClO}_{4}^{-}\) and \(\mathrm{IO}_{4}^{-}\) ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\) was not synthesized until \(1965 .\) The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free