Redox

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The two parts of a redox reaction
Rusting iron
A bonfire. Combustion consists of redox reactions involving free radicals.

Redox (shorthand for reduction/oxidation) describes all chemical reactions in which atoms have their oxidation number (oxidation state) changed.[1]

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

Which gains and loses electrons 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.

But there are exceptions.[2]

Chemical process[change | change source]

Redox is a chemical process. It can be described within chemical formulas. This example describes the process that occurs in a blast furnace, where iron (Fe) reacts with carbon (C):

\mathrm{1) \ C + O_2 \longrightarrow CO_2}
\mathrm{2) \ CO_2 + C \rightleftharpoons 2 \ CO}
\mathrm{3) \ Fe_2O_3 + 3 \ CO \longrightarrow 3 \ CO_2 + 2 \ Fe}
Now elementary iron has been processed.

References[change | change source]

  1. 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.
  2. 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).

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