Oxidation
Introduction:
Oxidation is the process in which an atom, ion, or molecule loses one or more electrons during a chemical reaction. Although the term was originally coined to describe reactions involving oxygen, modern chemistry defines it more broadly as the fundamental transfer of electrons between substances.
Redox reaction brief: Reactions often involve electrons moving between substances. When a substance loses electrons, it is oxidized. The substance that gains those electrons is said to be reduced.
This usually happens during a redox reaction (reduction–oxidation reaction), where both oxidation and reduction occur at the same time.
How oxidation occurs:
• Atoms try to become more stable
• To achieve this, electrons may move between atoms
• When an atom loses electrons, it is oxidized
• When another atom gains those electrons, it is reduced
This process happens only when:
• There is a driving force (one atom attracts electrons more strongly).
• There is a path for electrons to move.
Conditions that allow oxidation to continue:
1. Presence of an electron acceptor
• Oxidation cannot occur independently
• A second substance must be available to accept electrons
2. Suitable medium for transfer
• In many cases, a medium such as water facilitates the movement of ions
• This supports the continuation of the overall process
3. Energy favorability
• The reaction must be energetically favorable, generally resulting in a more stable system