A student adds three metals, L, M and N, to solutions of the nitrates of the other two metals. The table shows the results.
Table: Results of adding three metals to solutions of the nitrates of the other two metals
| Metal added | L nitrate solution | M nitrate solution | N nitrate solution |
|---|---|---|---|
| L | not done | no reaction | reaction |
| M | reaction | not done | reaction |
| N | no reaction | no reaction | not done |
Use the table to place the three metals in order of reactivity, starting with the most reactive.
Metal M forms ions with the formula M2+\text{M}^{2+}M2+ and metal N forms ions with the formula N2+\text{N}^{2+}N2+.
Write the ionic equation for the reaction between metal M and N nitrate solution.
Which species is oxidised in the reaction in part b)? Give one reason for your answer in terms of electrons.
Metal L forms ions with the formula L3+\text{L}^{3+}L3+.
Write the balanced ionic equation for the reaction between metal L and N nitrate solution.
39 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. Each one has a worked solution and a mark scheme showing where the marks go.