1. Watch the demonstrations
Write a chemical equation for the reaction
State and explain the type of reaction

2. Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)
Write out half equations for the following reactions
Describe each half equation as oxidation or reduction
Indicate which species is oxidised and which is reduced
Identify the oxidising agent and the reducing agent
Ca(s) + I2(s) → CaI2(s)
Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

3. Rules for assigning oxidation numbers
Elements – oxidation number is zero
Simple ions - oxidation number is equal to the charge on the ion
Compounds – the sum of oxidation numbers equals zero
Complex ions - the sum of oxidation numbers is equal to the charge on the ion
Usually, in compounds and ions:
F -1 Cl -1 Group 1 +1
O Group 2 +2
H Aluminium +3

4. 2H2 (g) + O2 (g) → 2H2O (g)
Deduce the oxidation states of each element before and after the reaction
Which elements are oxidised and which are reduced?

5. Oxidation numbers N2 NH3 NO3-
State and explain the oxidation number for nitrogen in these substances: N2
NH3
NO3-

6. combustion of magnesium
Identify the element that is oxidised
Show that the demonstrations you observed are redox reactions using oxidation numbers:
combustion of magnesium
displacement reaction between magnesium and copper
Identify the element that is reduced
Name the oxidising agent and the reducing agent