Chlorine dioxide gas (ClO2) is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (a)What is the Lewis structure for ClO2? (b) Why do you thinkthat ClO2 is reduced so readily? (c) When a ClO2 moleculegains an electron, the chlorite ion, ClO2-, forms. Draw theLewis structure for ClO2-. (d) Predict the O—Cl—O bondangle in the ClO2- ion. (e) One method of preparing ClO2is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s)------>2 ClO2(g) + 2 NaCl(s)If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorinegas at a pressure of 1.50 atm at 21 °C, how many gramsof ClO2 can be prepared?

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Chlorine dioxide gas (ClO₂) is used as a commercial bleaching
agent. It bleaches materials by oxidizing them. In the
course of these reactions, the ClO₂ is itself reduced. (a)
What is the Lewis structure for ClO₂? (b) Why do you think
that ClO₂ is reduced so readily? (c) When a ClO₂ molecule
gains an electron, the chlorite ion, ClO₂^-, forms. Draw the
Lewis structure for ClO₂^-. (d) Predict the O—Cl—O bond
angle in the ClO₂^- ion. (e) One method of preparing ClO₂
is by the reaction of chlorine and sodium chlorite:
Cl₂(g) + 2 NaClO₂(s)------>2 ClO₂(g) + 2 NaCl(s)
If you allow 15.0 g of NaClO₂ to react with 2.00 L of chlorine
gas at a pressure of 1.50 atm at 21 °C, how many grams
of ClO₂ can be prepared?

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