A Chlorine gas (Cl 2 ) is used as a disinfectant in municipal water supplies, although chlorine dioxide (ClO 2 ) and ozone are becoming more widely used. ClO 2 is a better choice than Cl 2 in this application because it leads to fewer chlorinated by-products, which are themselves pollutants. (a) How many valence electrons are in ClO 2 ? (b) The chlorite ion, ClO 2 − , is obtained by reducing ClO 2 . Draw a possible electron dot structure for ClO 2 − . (Cl is the central atom.) (c) What is the hybridization of the central Cl atom in ClO 2 − ? What is the shape of the ion? (d) Which species has the larger bond angle, O 3 or ClO 2 − ? Explain briefly. (e) Chlorine dioxide, ClO 2 , a yellow-green gas, can be made by the reaction of chlorine with sodium chlorite: 2 NaClO 2 (s) + Cl 2 (g) → 2 NaCl(s) + 2 ClO 2 (g) Assume you react 15.6 g of NaClO 2 with chlorine gas, which has a pressure of 1050 mm Hg in a 1.45-L flask at 22 °C. What mass of ClO 2 can be produced?

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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781337399074
BuyFind

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781337399074

Solutions

Chapter 10, Problem 116SCQ
Textbook Problem

A Chlorine gas (Cl2) is used as a disinfectant in municipal water supplies, although chlorine dioxide (ClO2) and ozone are becoming more widely used. ClO2 is a better choice than Cl2 in this application because it leads to fewer chlorinated by-products, which are themselves pollutants.

  1. (a) How many valence electrons are in ClO2?
  2. (b) The chlorite ion, ClO2, is obtained by reducing ClO2. Draw a possible electron dot structure for ClO2. (Cl is the central atom.)
  3. (c) What is the hybridization of the central Cl atom in ClO2? What is the shape of the ion?
  4. (d) Which species has the larger bond angle, O3 or ClO2? Explain briefly.
  5. (e) Chlorine dioxide, ClO2, a yellow-green gas, can be made by the reaction of chlorine with sodium chlorite:

    2 NaClO2(s) + Cl2(g) → 2 NaCl(s) + 2 ClO2(g)

Assume you react 15.6 g of NaClO2 with chlorine gas, which has a pressure of 1050 mm Hg in a 1.45-L flask at 22 °C. What mass of ClO2 can be produced?

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Chapter 10 Solutions

Chemistry & Chemical Reactivity
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