The Group 14 elements show a change from non-metallic to metallic character down the group.

1. (a)Table 3.1 shows some properties of two Group 14 elements, C and Sn, in their standard states. The table is incomplete. [Table 3.1]
2. (a)(i)Complete Table 3.1.[3]
3. (a)(ii)Identify the lattice structure shown by graphite.[1]
4. (a)(iii)Explain why Sn has good electrical conductivity.[1]
5. (b)Carbon is found in inorganic compounds such as carbonates.
6. (b)(i)Write an equation for the reaction of magnesium carbonate with dilute HCl(aq).[1]
7. (b)(ii)Describe the thermal stability of the carbonates down Group 2.[1]
8. (b)(iii)Ammonium carbonate undergoes an acid-base reaction with NaOH(aq). Explain this statement.[2]
9. (c)Fig. 3.1 shows a sketch of some of the ionisation energies of silicon, Si. [Fig. 3.1]
10. (c)(i)Complete the graph in Fig. 3.1 to show the third to sixth ionisation energies of Si.[2]
11. (c)(ii)Construct an equation to represent the second ionisation energy of Si.[1]
12. (d)Fig. 3.2 shows the boiling points of the simplest hydrides of the Group 14 elements, C to Pb. [Fig. 3.2]
13. (d)(i)Explain the trend in the boiling points of the Group 14 hydrides shown in Fig. 3.2.[2]
14. (d)(ii)Deduce the shape of a molecule of SiH₄.[1]
15. (e)Silicon readily reacts with elements of high electronegativity.
16. (e)(i)Write an equation for the formation of SiCl₄ from its constituent elements.[1]
17. (e)(ii)Describe what is observed when a small sample of SiCl₄ is added to water.[1]
18. (e)(iii)SiO₂ is a white solid that melts above 1700°C. SiCl₄ is a colourless liquid at room temperature. Explain the difference in the melting points of these two compounds with reference to their structure and bonding.[2]
19. (f)Tin forms an amphoteric oxide, SnO₂. Suggest the formula of the tin compound that forms when SnO₂ reacts with H₂SO₄ in an acid-base reaction.[1]

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