1.1. The following reactivity series shows both familiar and unfamiliar elements in order of decreasing reactivity. Each element is represented by a redox equation.

Rb $\rightleftharpoons$ Rb⁺ + e^–
      Mg $\rightleftharpoons$ Mg²⁺ + 2e^–
      Mn $\rightleftharpoons$ Mn²⁺ + 2e^–
      Zn $\rightleftharpoons$ Zn²⁺ + 2e^–
      H₂ $\rightleftharpoons$ 2H⁺ + 2e^–
      Cu $\rightleftharpoons$ Cu²⁺ + 2e^–
      Hg $\rightleftharpoons$ Hg²⁺ + 2e^–

Two of the uses of the series are to predict the thermal stability of compounds of the metals and to explain their redox reactions.

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i) Define in terms of electron transfer the term oxidation.

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ii) Explain why the positive ions in the above equations are oxidising agents.

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1.2. i) Which metals in the series above do not react with dilute acids to form hydrogen?

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ii) Describe an experiment which would confirm the prediction made in (b)(i).

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1.3. i) Which metal in the series above can form a negative ion which gives a pink / purple solution in water?

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ii) Describe what you would observe when zinc, a reducing agent, is added to this pink / purple solution.

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