Chapter 4, Problem 4.39P

Interpretation Introduction

(a)

Interpretation:

The oxidized and reduced species should be identified.

Concept Introduction:

When in a reaction a species gets oxidized and the other gets reduced, it is known as a Redox reaction.

Loss of electrons is Oxidation.

Addition of Oxygen is Oxidation.

Removal of Hydrogen is Oxidation.

For example-

$\text{Na(g)}\stackrel{}{\to }{\text{Na}}^{\text{+}}{\text{+e}}^{\text{-}}$

Gain of electrons is Reduction.

Removal of Oxygen is Reduction.

Addition of Hydrogen is Reduction.

$\raisebox{1ex}{$\text{1}$}\!\left/ \!\raisebox{-1ex}{$\text{2}$}\right.{\text{Cl}}_{\text{2}}{\text{(g)+e}}^{\text{-}}\stackrel{}{\to }{\text{Cl}}^{\text{-}}$.

Interpretation Introduction

(b)

Interpretation:

The species which acts as an oxidizing agent and which acts a reducing agent should be identified.

Concept Introduction:

When in a reaction a species gets oxidized and the other gets reduced, it is known as a Redox reaction.

Loss of electrons is Oxidation.

Addition of Oxygen is Oxidation.

Removal of Hydrogen is Oxidation.

For example-

$\text{Na(g)}\stackrel{}{\to }{\text{Na}}^{\text{+}}{\text{+e}}^{\text{-}}$

Gain of electrons is Reduction.

Removal of Oxygen is Reduction.

Addition of Hydrogen is Reduction.

$\raisebox{1ex}{$\text{1}$}\!\left/ \!\raisebox{-1ex}{$\text{2}$}\right.{\text{Cl}}_{\text{2}}{\text{(g)+e}}^{\text{-}}\stackrel{}{\to }{\text{Cl}}^{\text{-}}$.