Oxidation and Reduction Reactions

When oxidation and reduction take place one after the other. Then it is called a redox reaction. Oxygen is added to the reactant in an oxidation reaction, whereas hydrogen is removed from the reactant, This is termed as oxidation reaction. The reduction reaction is the opposite of the oxidation reaction. As in a reduction reaction, Oxygen is removed from the reactant, and hydrogen is added to the reactant. Also, the reactant gains electrons in the reduction process, and in the oxidation process, the reactant loses electrons. When both processes occur simultaneously, it is known as a redox reaction. The one that gives Oxygen is called oxidising agents, and the one that gives hydrogen is called reducing agents. 

Difference between oxidation and reduction reactions:

One of the major differences between the oxidation and reduction reactions is that, in oxidation, the loss of electrons occurs. Whereas in the reduction reaction, a gain of electrons occurs. The oxidation reaction is the addition of Oxygen to the reactant and removal of hydrogen from the reactant. In the reduction reaction, the removal of Oxygen occurs, and hydrogen is added to the substance. When both the reactions occur one after the other, it is known as an oxidation-reduction reaction or redox reaction. 

Let us discuss the oxidation-reduction reaction examples. It takes place in two halves; in the first half, oxidation is done, and in the next half, a reduction reaction occurs. 

Example of Reaction Between Hydrogen and Fluorine

In the chemical reaction of hydrogen and fluorine, the hydrogen used gets oxidised, whereas the fluorine used gets reduced. The chemical reaction is mentioned below:-

H₂ + F₂→ 2HF

In first half oxidation-reaction takes place: H₂ → 2H+ + 2e–

In second half reduction-reaction takes place: F₂ + 2e–→ 2F–

Then both the ions combine and produce hydrogen fluoride.

Example of Reaction Between Zinc and Copper

It is an example of a metal displacement reaction. In this reaction, copper metal is acquired. The zinc is used to displace the Cu2+ion in the copper sulphate solution. The complete reaction can be written as:-

Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)

In the first half, the oxidation reaction can be written as Zn → Zn2+ + 2e–

In the next half, reduction-reaction can be written as: Cu2+ + 2e– → Cu

Both the process is oxidation and reduction takes place one after the other. It is known as an oxidation-reduction reaction. The one reactant is oxidised, and the other reactant gets reduced. 

Example of Reaction between Iron and Hydrogen Peroxide

In this reaction, hydrogen peroxide acid is present. The Fe2+ changes to Fe3+. The complete reaction can be written as:-

2Fe2+ + H₂O₂ + 2H+ → 2Fe3+ + 2H2O

In the first half oxidation-reaction occurs: Fe2+  → Fe3+ + e–

In the next half, reduction-reaction occurs: H₂O₂ + 2e– → 2 OH–

With the reduction of hydrogen peroxide, hydroxide ions form, and it combines with the proton contributed by the acidic medium to form H₂O.

Example of reaction between Hydrazine and Oxygen

N₂H₄ (hydrazine) + O₂ (oxygen) –> N₂ (Nitrogen) + 2H₂O (Water)

Hydrazine is oxidised to nitrogen in the reaction, and Oxygen is reduced to water.

Hydrazine loses hydrogen, whereas Oxygen gains hydrogen. An oxidation and reduction reaction occurs in the given reaction, as first it is oxidised and then reduces. 

Conclusion:

When oxidation and reduction occur one after another, the process is known as an oxidation-reduction reaction. The one substance gets oxidised, whereas the other one gets reduced. The oxidation-reduction not only emphasises labs but also has many real-life uses. Like it is used in bleaching materials. Sanitization of water can be done with the help of these reactions. Manufacturing some chemicals like caustic soda and chlorine oxidation-reduction reactions seems very useful. When gains of electrons occur in a reaction, it is called a reduction reaction. And the loss of electrons occurs in the oxidation reaction.