Diamond and graphite are both crystalline solids made from carbon atoms. Graphite conducts electricity. Diamond does not conduct electricity.

1. (a)(i)Name the type of lattice structure present in the crystalline solids diamond and graphite.[1]
2. (a)(ii)Explain how graphite conducts electricity.[1]
3. (a)(iii)Explain why diamond does not conduct electricity.[1]
4. (b)(i)Separate samples of phosphorus(V) chloride and silicon(IV) chloride are each added to an excess of cold water. Write an equation for each reaction.[2]
5. (b)(ii)Describe the appearance of phosphorus(V) chloride and silicon(IV) chloride at room temperature. phosphorus(V) chloride silicon(IV) chloride[2]
6. (b)(iii)Compare the appearance of the mixtures produced when each reaction is complete.[2]
7. (c)(i)Some oxides are amphoteric. Describe what is meant by amphoteric.[1]
8. (c)(ii)Identify the formula of a Period 3 oxide that is amphoteric.[1]
9. (d)(i)The melting points of different oxides are shown in Table 1.1. Table 1.1 oxide | melting point/°C | force of attraction broken during melting SO2 | -73 | H2O | 0 | SiO2 | 1610 | Na2O | 1132 | MgO | 2852 | Complete Table 1.1 by identifying the strongest force of attraction in each oxide that is broken during melting. Use the abbreviations below. i.d. = instantaneous dipole-induced dipole p.d. = permanent dipole-permanent dipole H = hydrogen bond C = covalent bond I = ionic bond[3]
10. (d)(ii)A student suggests the following hypothesis. The stronger the covalent bond between atoms in non-metal oxides, the higher the melting point. Use Table 1.1 to deduce if this hypothesis is true or false or if there is not enough information to make a conclusion. Explain your answer.[2]