Chapter 4 - Redox Reactions

The gain of electrons. For example: Fe²⁺+ (aq) + 2e⁻ → Fe (s)

The loss of electrons. For example: Fe (s) → Fe²⁺+ (aq) + 2e⁻

An equation that describes one half of a redox reaction (either reduction or oxidation). For example: O2 + 4e⁻ →2O²⁻

A type of chemical reaction where reduction and oxidation are both taking place. For example: 2Mg + O2 → 2MgO

The substance that causes oxidation (gets reduced) in a redox reaction. Usually non-metals or a metal cation.

The substance that causes reduction (gets oxidised) in a redox reaction. Usually a metal or non-metal anion.

The product formed from a reducing agent. (i.e. the product of oxidation).

The product formed from an oxidising agent (i.e. the product of reduction).

A number assigned to an element which represents the number of electrons lost/gained by an atom of that element in a specific compound. e.g. ON of S in SO2 is +4.