Introduction: Oxidation and reduction are two opposite chemical reactions that occur simultaneously. Oxidation is the loss of electrons, and reduction is the gain of electrons. Together, they are known as redox reactions.

Example: The reaction between iron and oxygen is an example of oxidation and reduction occurring side by side. When iron reacts with oxygen, it forms iron oxide.

Oxidation: Iron is oxidized because it loses electrons to oxygen. The iron atoms lose two electrons each and become positively charged ions, Fe2+. This process is represented by the following equation:

Fe → Fe2+ + 2e-

Reduction: Oxygen is reduced because it gains electrons from iron. The oxygen molecules gain two electrons each and become negatively charged ions, O2-. This process is represented by the following equation:

O2 + 4e- → 2O2-

Overall Reaction: The overall reaction can be written as:

4Fe + 3O2 → 2Fe2O3

In this reaction, iron is oxidized and oxygen is reduced. The oxidation and reduction occur simultaneously, which is why the reaction is called a redox reaction.

Conclusion: Oxidation and reduction proceed side by side because electrons cannot be lost or gained without a corresponding electron transfer. In redox reactions, the oxidation and reduction reactions occur simultaneously to maintain the electrical neutrality of the system.

Because when one oxidised then other is reduced