Reduction and oxidation are terms used to describe
any reactions in which electrons are transferred.
A substance that is reduced
takes electrons from the substance that is oxidised.
A reaction in which both oxidation and reduction takes place is called a
the loss of electrons or an increase in oxidation number.
the gain of electrons or a decrease in oxidation number.
Half equations show
electron transfer, which element is oxidised and which is reduced.
Metals tend to be
Non-Metals tend to be
The more electronegative element attracts more
electron(s) and is then reduced.
Oxidising Agent: is
a reagent that oxidises another species by taking electrons from it.
Reducing Agent is
a reagent that reduces another species by adding electrons to it.
Oxidising and reducing agents are always
the whole species (as the chemical appeared in the beginning of the equation).
A disproportionation reaction
is the oxidation and reduction of the same element in a redox reaction, such as Cl2 + H20 --> HCL + HOCl, with chlorine being oxidised and reduced.