In the field of chemistry, the term oxidation is used to describe a process involving a loss of electrons by an atom, ion, or molecule. In a chemical reaction where one reactant is oxidized (i.e., loss of electrons), one or more of the other reactants undergo reduction (i.e., gaining electrons).

An example of a chemical reaction involving oxidation and reduction is the reaction of hydrogen with chlorine (shown below).

$H_2 + Cl_2 \rightarrow 2HCl$

The two reactants on the left side of the chemical equation are both elements with an oxidation number equal to zero. But when these elements react to form the product, $HCl$, the hydrogen has a higher oxidation number ($+1$) and the chlorine has a lower oxidation number ($-1$). In this reaction, the hydrogen has undergone oxidation while the chlorine has undergone reduction.

When writing down an electrochemical half reaction, it is generally quite clear when the half reaction is written as an oxidation half reaction. If the electrons appear as products (rather than reactants) in the half reaction, then the half reaction has been written as an oxidation process (see example below).

$Fe^{2+} \rightarrow Fe^{3+} + e^-$

In the example above, the iron(II) cation loses an electron to become iron(III); thus, the iron(II) cation is oxidized.

Related Terms: redox, half reaction, anode, anodic current

Antonyms: reduction