# Electron transfer In Oxidation And Reduction

## What is oxidation?

You get to hear the terms like oxidation and reduction a lot in CBSE class $12^{th}$ Chemistry but have you understood it? This article looks at oxidation and reduction from two different points of view.

• Oxidation and Reduction in terms of Oxygen transfer
• Oxidation and Reduction in terms of electron transfer

### Oxidation and Reduction in terms of Oxygen transfer

In early chemistry, oxidation and reduction were terms associated with oxygen. Oxidation meant gaining oxygen and Reduction meant losing oxygen. The term ‘reduction’ comes from Latin and means ‘-to lead back’. Therefore anything that leads back to the free metal state is referred to as a reduction reaction.

Magnesium undergoes both oxidation and reduction in reactions with different reactants.

### Oxidation and Reduction in terms of Electron transfer

This is the most commonly used definition of oxidation and reduction and most widely applicable. In this case, Oxidation is the loss of electrons and Reduction is the gain of electrons. A very clever mnemonic to remember this concept is oil rig.
OIL                                 RIG
Oxidation is loss          Reduction is gain

Oxidation and Reduction reactions are always interlinked. Because electrons are neither created nor destroyed in a chemical reaction, oxidation and reduction always occur in pairs, it is impossible to have one without the other. In the below reaction Magnesium gets oxidized by losing two electrons to oxygen which gets reduced by accepting two electrons from magnesium.

Since oxidation and reduction cannot occur individually, they as a whole are called  ‘Redox Reactions’. The reactant that oxidizes the other reactants is called as the Oxidizing agent and reactant that reduces is called Reducing agent. There is quite some confusion about the aspect whether oxidizing agents accept or give away electrons.