Oxidation-Reduction
Oxidation-Reduction or Redox is a type of chemical reaction where the oxidation states of atoms are changed. Redox reactions are characterized by the transfer of electrons between chemical species, most often with one species (the oxidant) undergoing oxidation (losing electrons) while another species (the reductant) undergoes reduction (gains electrons).
Overview[edit | edit source]
The term 'redox' comes from two concepts involved with electron transfer: 'reduction' and 'oxidation'. It can be explained in simple terms:
- Oxidation is the loss of electrons or an increase in the oxidation state of an atom, an ion, or of certain atoms in a molecule.
- Reduction is the gain of electrons or a decrease in the oxidation state of an atom, an ion, or of certain atoms in a molecule.
Redox reactions[edit | edit source]
In redox processes, the reductant transfers electrons to the oxidant. Thus, in the reaction, the reductant or reducing agent loses electrons and is oxidized, and the oxidant or oxidizing agent gains electrons and is reduced.
Examples[edit | edit source]
Some examples of redox reactions are:
- The reaction between hydrogen and fluorine is an example of an oxidation-reduction process:
2H2 + F2 → 2HF
- The rusting of iron is a redox reaction:
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
See also[edit | edit source]
| Oxidation-Reduction Resources | |
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