(a)[1]
State the name of aluminium’s main ore.
(b)[1]
Name the substance added to aluminium oxide to lower the process temperature.
(c)[1]
Explain why the molten mixture in (b) conducts electricity.
(d(i))[3]
Complete Table 2.1: • Write the number of electrons required to balance the ionic half-equation for the reaction at the anode. • Write the ionic half-equation for the reaction at the cathode.
(d(ii))[1]
State why the process at the anode is an oxidation.
(d(iii))[2]
Explain why the main gas released at the anode is carbon dioxide rather than oxygen.
(e)[1]
State why aluminium is used in food containers.
(f)[3]
Aluminium reacts with fluorine to make the ionic compound aluminium fluoride. Complete the dot-and-cross diagram in Fig. 2.1 of the ions in aluminium fluoride. Give the charges on the ions.