What is Oxidation?

Oxidation

According to the classical concept of oxidation, it may be defined as “Oxidation” is a process which involves the addition of oxygen or any other electro­negative element or radical to an element or a compound or the removal of hydroge­n any electro-positive element or radical from a compound.

For example:

Addition of oxygen or any other electro-negative element

• C + O₂ –> CO₂

Here, carbon adds oxygen and is thus oxidized to CO₂.

• Cu + Cl₂ –> CaCl₂

Here, chlorine has been added to copper and thus it is oxidized to CuC1₂.

• 2FeCl₂ + Cl₂ –> 2FeCl₃

In this reaction FeCl₂ gains electro-negative atom that is chlorine (Cl^–) and is therefore oxidized to FeCl₃.

According to the electronic concept oxidation is a process which involves loss of electrons by an atom or group of atoms. Due to this loss of electrons there will be an increase in positive charge and simultaneously will decrease in negative charge.

Example:

Sodium reacts with chlorine forming NaCI.

2Na + Cl₂ –> 2NaCI

In the above reaction sodium (Na) looses one electron and thus has become oxidized.

Na –> Na⁺ + e (Oxidation)