Oxidative Reactions

 Oxidative reactions, also known as oxidation reactions, involve the transfer of electrons between chemical species. In these reactions, one substance loses electrons (is oxidized), while another gains those electrons (is reduced). Oxidation reactions are fundamental to many biological and chemical processes.

Key Concepts:

1. Oxidation: Loss of electrons from a substance.
2. Reduction: Gain of electrons by a substance.
3. Oxidizing Agent: The substance that accepts electrons and gets reduced.
4. Reducing Agent: The substance that donates electrons and gets oxidized.

Examples of Oxidative Reactions:

1. Combustion: A common example where a fuel (like hydrocarbons) reacts with oxygen to produce carbon dioxide and water, releasing energy.

   • ${\text{CH}}_4+2{\text{O}}_2\to {\text{CO}}_2+2{\text{H}}_2\text{O}$

2. Cellular Respiration: Biological oxidative reaction where glucose is oxidized to produce ATP.

   • ${\text{C}}_6{\text{H}}_{12}{\text{O}}_6+6{\text{O}}_2\to 6{\text{CO}}_2+6{\text{H}}_2\text{O}$

3. Corrosion: Metals like iron react with oxygen to form oxides, a process known as rusting.

   • $4\text{Fe}+3{\text{O}}_2\to 2{\text{Fe}}_2{\text{O}}_3$

Importance:

• Metabolism: Oxidative reactions drive the breakdown of nutrients to produce energy in living organisms.
• Industry: Oxidation is vital in processes like metal refining, production of chemicals, and energy generation.