Copper is used in electrical equipment. It has a melting point of 1085 °C.

1. (a)(i)Identify the lattice structure of copper.[1]
2. (a)(ii)Draw a labelled diagram to show the bonding present in copper.[1]
3. (b)The relative isotopic masses and natural abundances of the two isotopes in a sample of copper are shown in Table 1.1. Table 1.1 isotope relative isotopic mass % abundance 63Cu 62.930 69.15 65Cu 64.928 30.85
4. (b)(i)Define the unified atomic mass unit.[1]
5. (b)(ii)Define relative atomic mass, Ar, in terms of the unified atomic mass unit.[1]
6. (b)(iii)Calculate the relative atomic mass, Ar, of copper in this sample using the data in Table 1.1. Show your working. Ar =[1]
7. (c)The mass spectrum of a sample of pure copper is shown in Fig. 1.1. [Figure 1.1] Identify the ion with an abundance of 23% in the sample.[1]
8. (d)When KI(aq) is added to CuSO4(aq) the blue-coloured solution turns brown and a white precipitate of CuI(s) is seen. The reaction between copper ions and iodide forms only two products.
9. (d)(i)Complete the equation for this reaction. .Cu2+ + .......I- → .......CuI + .......[1]
10. (d)(ii)Identify the oxidising agent in this reaction. Explain your answer in terms of electron transfer.[1]
11. (d)(iii)State the full electronic configuration of Cu2+.[1]

This question uses a diagram from the original paper, which isn't shown here. Open the full paper from the past papers archive to see it.