1. Electron Transfer: Oxidation is an electrochemical reaction that involves the transfer of electrons between species. When a substance undergoes oxidation, it loses electrons, resulting in an increase in its oxidation state.
2. Oxidized Species: The substance that undergoes oxidation is referred to as the "oxidized species" or "reducing agent." It donates electrons to another substance, causing its own oxidation.
3. Oxidizing Agent: The substance that accepts the electrons from the oxidized species is known as the "oxidizing agent" or "oxidant." It undergoes reduction in the process.
4. Change in Oxidation Number: Oxidation generally leads to an increase in the oxidation number of the oxidized species. The oxidation number represents the charge an atom would have if all bonds to other atoms were purely ionic.
5. Examples of Oxidation:
- Combustion: When a substance burns in the presence of oxygen, it undergoes oxidation. For instance, burning methane (CH4) with oxygen (O2) produces carbon dioxide (CO2) and water (H2O).
- Rusting of Iron: Iron exposed to oxygen and moisture undergoes oxidation, forming iron oxide, commonly known as rust.
Overall, oxidation is a fundamental chemical process that drives many reactions in nature and industry. It plays a crucial role in energy production, metallurgy, food preservation, and various other processes where substances interact with oxygen.
