Oxidation is a chemical reaction where a substance loses electrons. It often involves the substance reacting with oxygen, but not always. Here's a breakdown:
Key Points
Loss of electrons: At its core, oxidation is defined by the loss of electrons by a molecule, atom, or ion.
Increase in oxidation state: When a substance loses electrons, its oxidation state increases.
Not always about oxygen: While the term "oxidation" originally came from reactions with oxygen, it now has a broader meaning in chemistry.
Examples of Oxidation
Rusting of iron: When iron reacts with oxygen in the presence of moisture, it forms rust (iron oxide). This is a classic example of oxidation.
Burning: Combustion, or burning, is another oxidation reaction where a substance reacts rapidly with oxygen to produce heat and light.
Browning of fruit: When you cut an apple or banana and it turns brown, that's oxidation happening. Enzymes in the fruit react with oxygen in the air, causing the color change.
Oxidation and Reduction
Oxidation is often paired with reduction. These two processes always occur together in what's called a redox reaction:
Oxidation: Loss of electrons
Reduction: Gain of electrons
If one substance loses electrons (is oxidized), another substance must gain those electrons (be reduced).
Importance of Oxidation
Oxidation is a fundamental chemical process that plays a vital role in many areas:
Energy production: Our bodies use oxidation to get energy from the food we eat.
Industrial processes: Many industrial processes rely on oxidation, such as the production of steel and various chemicals.
Corrosion: Oxidation can cause unwanted corrosion of metals, like rust on iron.