Fig. 1.1 shows the variation in melting point of some Period 3 elements in their standard states at room temperature and pressure.

1. (a)Complete Table 1.1 using relevant information from the Periodic Table. Table 1.1 nucleon number proton number number of electrons Mg2+ 24 Al3+ 27[2]
2. (b)State and explain the difference in the ionic radius of Al3+ compared to Mg2+.[3]
3. (c)Draw a labelled diagram to show the structure and bonding in sodium.[1]
4. (d)(i)Explain why Si has a high melting point.[1]
5. (d)(ii)Complete Fig. 1.1 to show the variation in the melting points of the elements P, S and Cl.[2]
6. (e)(i)Two Period 3 elements react with an excess of oxygen at room pressure. Complete Table 1.2. Table 1.2 1 Period 3 element 2 state of oxide at room temperature and pressure Na S 3 approximate pH of solution made when oxide is added to water[2]
7. (e)(ii)The solutions made in column 3 of Table 1.2 are mixed together. Name the type of reaction that occurs.[1]
8. (e)(iii)Write an equation to describe the reaction between P4O10 and an excess of water.[1]
9. (f)(i)Aluminium hydroxide is amphoteric. Explain what is meant by amphoteric.[1]
10. (f)(ii)Write an equation to describe the reaction that occurs when aluminium hydroxide, Al(OH)3, reacts with NaOH(aq).[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.