An oxidation number is a number assigned to an element in chemical combination that represents the number of electrons lost (or gained, if the number is negative), by an atom of that element in the compound.
The term redox comes from the two concepts of reduction and oxidation. It can be explained in simple terms:
- Oxidation describes the loss of electrons by a molecule, atom or ion
- Reduction describes the gain of electrons by a molecule, atom or ion
Whether an electron is gained or lost can be easily memorised by the abbreviation OIL RIG, which stands for, "Oxidation Is Loss," or losing electrons, and "Reduction Is Gain," or gaining electrons. Redox reactions can also happen by sharing electrons to form a product by covalent bonding.
In an oxidation reduction reaction, the cation gives an electron to the anion because both ions will have a different charge to attract each other with. In an oxidation reduction reaction, the oxidizing reagent pulls an electron from the other atom to have a net positive charge. The reducing reagent gives an electron to have a net negative charge. However, there are exceptions.
- Now elementary iron has been processed.
- This can be a simple redox process, such as the oxidation of carbon to yield carbon dioxide, the reduction of carbon by hydrogen to yield methane (CH4), or a complex process such as the oxidation of sugar in the human body, through a series of very complex electron transfer processes.
- Oxidation and reduction properly refer to a change in oxidation number – the actual transfer of electrons may never occur. Thus, oxidation is better defined as an increase in oxidation number, and reduction as a decrease in oxidation number. In practice, the transfer of electrons will always cause a change in oxidation number, but there are many reactions which are classed as "redox" even though no electron transfer occurs (such as those involving covalent bonds).
|The English Wikibooks has more information on:|