1 (a) Define first ionisation energy. (b) Successive ionisation energies for element A are shown in Table 1.1. Table 1.1 jonisation | 1st | 2nd | 3rd | 4th | 5th | 6th | 7th | 8th ---|---|---|---|---|---|---|---|--- ionisation energy/kJ mol-1 | 1310 | 3390 | 5320 | 7450 | 11000 | 13300 | 71000 | 84 100 Use Table 1.1 to deduce the group of the Periodic Table that A belongs to. Explain your answer. Group (c) Across Period 3 there is a general trend for first ionisation energies to increase due to the increase in attraction between the nucleus and the outer electron. Explain why the first ionisation energy of sulfur is less than the first ionisation energy of phosphorus. (d) In an Al2+ ion the nuclear attraction for the outer electron is stronger than in an atom of Na. Compare the electronic structures of Al2+ and an atom of Na and explain why the third ionisation energy of aluminium is greater than the first ionisation energy of sodium. (e) An isotope of copper has a relative isotopic mass of 65. Complete Table 1.2 for an atom of copper-65. Table 1.2 | | atomic number | nucleon number | number of neutrons | electronic arrangement | |---|---|---|---|---| | copper-65 | | | | | (f) (i) The element copper has a relative atomic mass of 63.5. Calculate how many atoms are present in 1.05g of copper. atoms of copper present = (ii) Copper has a melting point of 1085°C and a high electrical conductivity. Explain these properties of copper by referring to its structure and bonding.