Although we have studied in detail about redox reaction in class XI, here we shall just focus on the electronic aspect of redox reactions.
In our daily life, formation of rust from Iron, combustion of carbon, sulphur or phosphorus and fading of colours of our cloths are some examples of oxidation reactions. Industrial process of extraction of metals (Al, Na Cu, Fe etc.) from their ores, removal of stains from cloths and generation of electricity in batteries are some examples of reduction reactions.
Electronically, oxidation is a process involving loss of electrons (de-electronation) and the reduction process involves gain of electrons (electronation). Since the net balanced chemical reaction is neutral (i.e. neither loss nor gain of electrons), the oxidation and reduction processes must occur simultaneously. Such reactions involving both reduction and oxidation are called ?Redox reaction?. For example,
Oxidizing agents (Oxidants) : Species which gains one or more electrons.
Reducing agents (Reductants): Species which losses one a more electrons.