What is the Difference Between Oxidation Reaction and Reduction Reaction?

The main difference between oxidation and reduction reactions lies in the transfer of electrons and the change in the oxidation numbers of the reactants. Here are the key differences between the two types of reactions:

• Oxidation:

1. Involves the loss of electrons by a reactant.
2. Results in an increase in the oxidation number of the reactant.
3. Occurs in the presence of oxidizing agents (e.g., ozone, bleach, peroxide).
4. Releases energy.
5. Examples include the rusting of iron and the combustion of hydrocarbons.

• Reduction:

1. Involves the gain of electrons by a reactant.
2. Results in a decrease in the oxidation number of the reactant.
3. Occurs in the presence of reducing agents (e.g., metals).
4. Stores energy.
5. Examples include the extraction of metals from their ores and the reduction of oxygen to water during cellular respiration.

In summary, oxidation reactions involve the loss of electrons and an increase in the oxidation number of the reactant, while reduction reactions involve the gain of electrons and a decrease in the oxidation number of the reactant. These reactions often occur simultaneously in a process called a redox reaction.

Comparative Table: Oxidation Reaction vs Reduction Reaction

Here is a table comparing the differences between oxidation and reduction reactions:

In an oxidation reaction, a molecule loses electrons, and its oxidation state increases. On the other hand, in a reduction reaction, a molecule gains electrons, and its oxidation state decreases. These reactions often occur simultaneously in a process called redox (reduction-oxidation) reaction.