Summary
Redox Summary Sheet
- Institution
- CCEA
Summary study book Chemistry for CCEA AS Level of Dr Wingfield Glassey, Dr Wingfield Glassey (Redox) - ISBN: 9781780731018 (Redox Summary Sheet)
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RedoxOxidation Reduction
Loss of electrons Gain of electrons
Gain of oxygen Loss of oxygen
Increase in oxidation Decrease in oxidation state
Oxidation State: The charge on a simple ion or the difference in the number of electrons associated
with an element in a compound compared with the atoms of the element
Oxidation state of an atom is 0, even diatomic
Always written as +2 not 2+
Fractional oxidation states are possible e.g. Fe304
Oxygen is nearly always -2 except in peroxides e.g. H202 = -1, and in F20, = +2 as fluorine is
more electronegative than oxygen
Group 1 always have an oxidation state of +1
Group 2 always have an oxidation state of +2 in compounds
Oxidation state of simple ions in a compounds= charge on ion e.g. Iron(II) Chloride, Iron= +2
Total of oxidation states in a compound must equal 0
Total of oxidation stats in a molecular ion must equal charge of ion
Oxidation states of P and D block elements vary, with the highest being ‘+group number’
Oxidising Agent: Is an electron acceptor
Reducing Agent: Is an electron donor
An oxidising agent is a chemical that causes oxidation in another species, the reducing agent
causes reduction in another species by being oxidised.
Half Equations
Mg → Mg2+ + 2e-
Cl2 + 2e- → 2Cl-
Balance Oxygen atoms with water.
Balance H atoms with H+
Balance charge with e-
Then, to add together, ensure that each equation has the same no. of e-
One species is reduced and one oxidised
Disproportionation: Reaction in which the same element is oxidised and reduced
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