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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 14, Problem 26E
Textbook Problem
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Draw Lewis structures for each chemical reaction, and identify what is oxidized and what is reduced:

a . 2K+Cl 2 2KCl b .4Al+3O 2 2Al 2 O 3 c . CH 4 +2O 2 CO 2 +2H 2 O

Interpretation Introduction

Interpretation:

The Lewis structures of each chemical equation is to be drawn and oxidized and reduced elements are to be identified.

Concept introduction:

Lewis structures are also known as Lewis dot formulas and are diagrams that show the bonding of atoms and the lone pairs of electrons that exist in the molecule.

Oxidation is the addition of an electronegative element or the removal of an electropositive element in a chemical reaction.

Reduction is the addition of an electropositive element or the removal of an electronegative element in a chemical reaction.

An oxidizing agent is a substance that has the capacity to oxidize other substances and get reduced in a chemical reaction.

A reducing agent is a substance that has the capacity to reduce other substances and get oxidized in a chemical reaction.

Explanation of Solution

a) 2K+Cl22KCl

The equation for the reaction of K with Cl2 is as follows.

2K+Cl22KCl

An oxidizing agent gains electron easily and a reducing agent loses electrons easily in a chemical reaction.

2K0+Cl202K+1Cl1

In this chemical reaction, the oxidation state of K is increased from 0 to +1 and loss of electrons occurs. Therefore, K is oxidized.

In this chemical reaction, the oxidation state of Cl2 is reduced from 0 to 1 and gain of electrons occurs. Therefore, Cl2 is reduced.

The Lewis structure of the above redox reaction is as follows.

.

b) 4Al+3O22Al2O3.

The equation for the reaction of Al with O2 is as follows.

4Al+3O22Al2O3.

An oxidizing agent gains electrons easily and a reducing agent loses electrons easily in a chemical reaction.

4Al0+3O202Al2+3O32

In this chemical reaction, the oxidation state of Al is increased from 0 to +3 and loss of electrons occurs

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Chapter 14 Solutions

Chemistry In Focus
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