Chapter 20, Problem 66A

Interpretation Introduction

Interpretation: The necessity of oxidizing and reducing agents in a redox reaction is to be explained.

Concept introduction: The reaction which involves the oxidation and reduction process simultaneously is defined as the redox reaction.

Answer to Problem 66A

In a redox reaction, t is very important to have an oxidizing and reducing agent since the electron lost by a reducing agent must be accepted by an oxidizing agent.

Explanation of Solution

The reducing agent is a chemical species that is found to undergo oxidation by the loss of electrons. While an oxidizing agent is the species that undergo reduction by the gain of electrons. In a redox reaction, there must be a reducing agent that is ready to lose the electrons present in them. It will create an unbalance if there are no chemical species available to accept the electrons donated by those reducing agents and that is oxidizing agents. For example, in $NaCl$ .

Oxidation: $Na\to N{a}^{+}+e^{-}$

Reduction: $Cl+e^{-}\to C{l}^{-}$

So, oxidation is always accompanied by reduction. And also, there must be oxidizing and reducing agents in a redox reaction.