Oxidation & Reduction (Edexcel IGCSE Chemistry)
Revision Note
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Chemistry Lead
Oxidation & Reduction
Oxidation & reduction in terms of oxygen
- The reactions of metals with oxygen, such as in iron rusting can be classified as oxidation
- Oxidation is any reaction in which a substance gains oxygen
- The opposite of oxidation is reduction
- Reduction is a reaction in which a substance loses oxygen
- For example, the displacement reaction between zinc and copper(II)oxide can be classified as a redox reaction
Zn + CuO → ZnO + Cu
zinc + copper(II) oxide → zinc oxide + copper
- Oxidation cannot occur without reduction happening simultaneously, hence these are called redox reactions
- The copper(II)oxide supplies the oxygen, so it is the oxidising agent
- The zinc is the reducing agent because it removes the oxygen
Oxidation & Reduction in terms of electrons
- Displacement reactions can be analysed in terms redox reactions by studying the transfer of electrons
- For the example of magnesium and copper sulfate, a balanced equation can be written in terms of the ions involved:
Mg (s) + Cu2+ (aq) + SO42- (aq) → Mg2+ (aq) + SO42- (aq) + Cu (s)
- The sulfate ions, SO42-, appear on both sides of the equation unchanged hence they are spectator ions and do not participate in the chemistry of the reaction so can be omitted:
Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)
- This equation is an example of a balanced ionic equation which can be further split into two half equations illustrating oxidation and reduction individually:
Mg → Mg2+ + 2e–
Cu2+ + 2e–→ Cu
- The magnesium atoms are thus oxidised as they lose electrons
- The copper ions are thus reduced as they gain electrons
- These equations illustrate the broader definition of oxidation and reduction in terms of electron transfer:
- Oxidation is the loss of electrons
- Reduction is the gain of electrons
'OIL RIG' is a useful mnemonic to help remember the definitions of oxidation and reduction
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