A student investigated the voltage produced by different pairs of metal electrodes in a chemical cell.
One electrode was always made of iron (Fe\text{Fe}Fe). The other electrode (Electrode A) was varied. Both electrodes were placed in a 1.0 mol/dm31.0\text{ mol/dm}^31.0 mol/dm3 sodium chloride solution.
The table below shows the results of the investigation:
| Electrode A | Symbol of metal | Voltage in volts |
|---|---|---|
| Aluminium | Al\text{Al}Al | +1.22+1.22+1.22 |
| Copper | Cu\text{Cu}Cu | −0.78-0.78−0.78 |
| Iron | Fe\text{Fe}Fe | 0.000.000.00 |
| Magnesium | Mg\text{Mg}Mg | +1.93+1.93+1.93 |
| Tin | Sn\text{Sn}Sn | −0.30-0.30−0.30 |
Write the symbols of the five metals in the table in order of reactivity, from most reactive to least reactive. Justify your answer.
5 exam-style questions on AQA GCSE Chemistry 4.1 Reactivity of metals, covering 4.1.1 Metal oxides, 4.1.2 The reactivity series, 4.1.3 Extraction of metals and reduction, and 4.1.4 Oxidation and reduction in terms of electrons (HT only). Each one has a worked solution and a mark scheme showing where the marks go.