5.1 Explain how the methods of extraction if the metals in this section are related to their positions in the reactivity series

The reactive series

Anything LESS reactive than carbon can be displaced from its ore by carbon (e.g.: iron)
Anything MORE reactive than carbon can't and so is extracted by electrolysis (e.g.: aluminium)

5.3 Write ionic half-equations for the reactions at the electrodes in aluminium extraction

These are the two equations you need to know (all thanks go to Hannah Help)

Al³⁺ + 3e^- > Al

• 2O^2- → O₂ + 4e^-

(btw, the Al and the O2 come from the aluminium oxide which is broken down via electrolysis)

5.4 Describe and explain the main reactions involved in the extraction of iron from iron ore (haematite), using coke, limestone and air in a blast furnace

Figure 1: All the equations you need to know

Figure 2

Coke, which contains carbon, burns in air to produce heat (and CO2), meaning that it is exothermic. The CO2 reacts with MORE C to form carbon monoxide, which is needed to reduce iron oxide.

Limestone, which contains calcium carbonate, is used to get rid of impurities: it reacts with them to produce molten slag, which can be used to build roads.

Hot air is needed so the coke can burn.

Because carbon is higher up in the reactivity series than iron, it displaces iron in the reaction Fe₂O₃ + 3CO  →   2Fe + 3CO₂

In that reaction, iron oxide is reduced to iron and carbon monoxide is oxidised to produce carbon dioxide.