Oxidation Number Rules
1. The oxidation number of un-combined elements is zero.
2. In simple ions the oxidation number of the element is the charge on the ion
3. The sum of the oxidation numbers in a neutral compound is zero.
4. The sum of the oxidation numbers for an ion is the charge on the ion.
5. Some elements have fixed oxidation numbers in all their compounds
Group I metals +1 hydrogen +1 (except in metal hydrides, H-)
Group II metals +2 fluorine -1
Aluminium +3 oxygen -2 (except in peroxides O22- and compounds with fluorine).
chlorine -1 (except in compounds with oxygen / fluorine).
1. Calculate the oxidation state of sulphur in the sulphate ion (SO42-)
Step 1: Allocate known charges
x = charge on sulphur
overall charge = -2
charge on each oxygen = -2
Step 2: Write equation
x + (4×-2) = -2
x – 8 = -2
x = -2+8
x = +6
Oxidation state of sulphur in SO4-2 = +6
Always remember to include the fact that these are positive or negative – DON’T Assume!
2. Calculate the charge on the manganese in the MnO4- ion.
3. Calculate the charge on the chromium in Cr2O72-.
Calculate the oxidation states of the starred ions in these compounds.
1. Br*O- 2. Br*O3- 3. HBr 4. N*H4+
5. P*Cl5 6. S*O32- 7. N*O2- 8. S*2O32-
Some formulae have roman numerals e.g. iron (II) bromide. This number gives the oxidation states of the iron.
The compound CuSO4½H2O is commonly called copper (II) sulphate. Its correct name is tetraaquocopper (II) tetraoxosulphate (VI)-1-water. However very few chemists call is this and copper (II) sulphate is acceptable.
Write the formulae of these compounds.
a) tin (II) oxide
b) tin (IV) oxide
c) sodium chlorate (III)
d) iron (III) nitrate (V)
e) potassium chromate (VI)
Use the concept of oxidation states to help you balance these equations, state what is oxidised and which is reduced.
a) Fe + Br2 ? FeBr3
b) F2 + H2O ? HF + O2
c) IO3- + H+ + I- ? I2 + H2O
d) S2O32- + I2 ? S4O62- + I-e) Cl2 + OH- ? Cl- + ClO- + H2O