Oxidising agents
An oxidising agent:
- is normally a non-metal or positive ion
- cause oxidation reactions to take place
- gains electrons from other atoms or ions (is itself reduced)
For example, chlorine and copper ions are both oxidising agent which are themselves reduced as follows:
\(Cl_{2}(g)+2e^{-}\rightarrow 2Cl^{-}(aq)\)
\(Cu^{2+} (aq) + 2e^{-} \rightarrow Cu(s)\)
The strongest oxidising agents are highly electronegative elements like the halogens (Group 7).
Uses of oxidising agents
Oxidising agents are frequently used because of the effectiveness with which they can kill fungi and bacteria, and can inactivate viruses. Group ions such as dichromate (Cr2O72-) and permanganate (MnO4-) ions are strong oxidising agents in acidic solutions.
They are useful in the chemistry lab when forming aldehydes, ketones and carboxylic acids from alcohol molecules.
Hydrogen peroxide (H2O2) is an example of a molecule which is a strong oxidising agent.
It is used in everyday life as a means of breaking down coloured compounds, whether in clothes or hair.