Chapter 4 - Redox Reactions

Question 1

Reduction

Answer 1

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

Question 2

Oxidation

Answer 2

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

Question 3

Half Equation

Answer 3

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

Question 4

Redox Reaction

Answer 4

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

Question 5

Oxidising Agent

Answer 5

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

Question 6

Reducing Agent

Answer 6

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

Question 7

Conjugate Oxidising Agent

Answer 7

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

Question 8

Conjugate Reducing Agent

Answer 8

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

Question 9

Oxidation Number

Answer 9

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 SO_{2 is +4.}