View source for Redox Reaction

==Key Stage 4==
===Meaning===
====Foundation====
A '''redox reaction''' is a [[Chemical Reaction|chemical reaction]] in which [[Oxygen]] is lost from one [[compound]] ([[Reduction]]) and gained by another [[compound]] ([[Oxidation]]).
====Higher====
A '''redox reaction''' is a [[Chemical Reaction|chemical reaction]] in which [[ion]]s of a less [[reactivity|reactive]] [[metal]] gain [[electron]]s ([[Reduction]]) and [[atom]]s of a more [[Reactivity|reactive]] [[metal]] lose [[electron]]s ([[Oxidation]]).

===About Redox Reactions===
====Foundation====
: [[Displacement Reaction|Displacement reactions]] between [[metal]]s and [[Metal Oxide|metal oxides]] are a type of '''redox reaction'''.
: During a '''redox reaction''' a less [[reactivity|reactive]] [[metal]] in a [[Metal Oxide|metal oxide]] is [[Displacement Reaction|displaced]] by the more [[reactivity|reactive]] [[metal]] [[element]].
In the following '''redox reaction''':
: [[Aluminium]] + [[Iron Oxide]] → [[Aluminium Oxide]] + [[Iron]]
: <chem>2Al+Fe2O3->Al2O3+2Fe</chem>
The [[Aluminium]] is [[Oxidation|oxidised]] and the [[Iron]] is [[Reduction|reduced]].

====Higher====
: [[Displacement Reaction|Displacement reactions]] between [[metal]]s and [[metal]] [[compound]]s are a type of '''redox reaction'''.
: During '''redox reaction''' the less [[reactivity|reactive]] [[metal]] [[ion]] is [[reduction|reduced]] when it gains [[electron]]s and the more [[reactivity|reactive]] [[metal]] [[element]] is [[oxidation|oxidised]] when it loses [[electron]]s.
'''Redox Reactions''' can be described by two [[Half Equation|half equations]].
: [[Aluminium]] + [[Iron Oxide]] → [[Aluminium Oxide]] + [[Iron]]
: [[Oxidation]] of [[Aluminium]]: <chem>Al - 3e^- -> Al^3+</chem>
: [[Reduction]] of [[Iron]]: <chem>Fe^3+ + 3e^- -> Fe</chem>
To remember whether [[electron]]s are gained or lost the [[acronym]] '''OIL RIG''' can be used: [[Oxidation]] is lost, [[Reduction]] is gained.