Table 16.1 Some common minerals and their metals.

Figure 16.3 The magnesium oxide coating needs to be removed when performing experiments with magnesium ribbon.

Figure 16.4 Copper wire placed in a silver nitrate solution forms deposits of silver crystals.

Figure 16.5 The relationship between oxidants and reductants in oxidation reduction reactions.

Table 16.2 An electrochemical series.

Figure 16.7 The apparatus used to demonstrate electron flow during oxidation–reduction reactions.

Figure 16.8 An electrochemical cell demonstrating a flow of electrons in a redox reaction.

Figure 16.10 An electrochemical cell made up by linking an Ag+(aq)/Ag(s) half cell and a Cu2+(aq)/Cu(s) half cell.

Figure 16.12 This Viking sword has a gold and silver handle, and an iron blade. Which is the most reactive metal?

Figure 16.14 Microscopic view of rust flakes.

Figure 16.15 Wet corrosion operates like a mini galvanic cell, where electrons are transferred though the iron, and ions flow through the water droplets.

Figure 16.19 These 450 kg aluminium alloy anodes are attached to bare steel structures of offshore gas platforms to protect them against corrosion. These areas will be under water when the platform is in service. The aluminium is more reactive than iron and will be oxidised preferentially. Aluminium anodes of this size are designed to last the life of the platform.

Figure 16.21 These displacement reactions demonstrate the nature of sacrificial protection. Magnesium is attached to the nail in the left container, and tin to the nail on the right.