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Reduction

The gain of electrons by a reactant (or loss of oxygen).

Oxidation

The loss of electrons by a reactant (or gain of oxygen).

Redox Reaction

A chemical reaction in which oxidation and reduction occur simultaneously.

Oxidising Agent

A substance that accepts electrons, causing another reactant to be oxidized by being reduced itself.

Reducing Agent

A substance that donates electrons, helping another reactant to be reduced by being oxidized itself.

Electrochemical Series

A chart that ranks elements based on their ability to act as oxidizing or reducing agents, with oxidizing agents on the bottom left and reducing agents on the top right.

Strongest Reducing Agents

Found in Group 1 of the Periodic Table.

Strongest Oxidising Agents

Found in Group 7 of the Periodic Table.

Uses of Oxidising Agents

Used to kill fungi and bacteria and also as a bleach.

Balanced Ion-Electron Equation

An equation that shows the balanced movement of ions and electrons in a redox reaction.

Step 1 of Balancing Ion-Electron Equations

Balance the chromium ions in the equation.

Step 2 of Balancing Ion-Electron Equations

Balance the oxygen by adding water.

Step 3 of Balancing Ion-Electron Equations

Balance the hydrogen by adding hydrogen ions.

Step 4 of Balancing Ion-Electron Equations

Balance the charge by adding electrons.

Overall Redox Reaction

The combined reaction of oxidation and reduction processes after balancing the number of electrons.