The elements phosphorus, sulfur and chlorine are in Period 3 of the Periodic Table. Table 1.1 shows some properties of the elements P to Cl. The first ionisation energy of S is not shown. Table 1.1 property P S Cl number of electrons in 3p subshell total number of unpaired electrons first ionisation energy /kJ mol⁻¹ 1060 1260 formula of most common anion P³⁻ S²⁻ Cl⁻

1. (a)(i)Complete Table 1.1 to show the number of electrons in the 3p subshell and the total number of unpaired electrons in an atom of P, S and Cl.[2]
2. (a)(ii)Construct an equation to represent the first ionisation energy of P.[1]
3. (a)(iii)Three possible values for the first ionisation energy of S are given. 1000 kJ mol⁻¹ 1160 kJ mol⁻¹ 1320 kJ mol⁻¹ Circle the correct value. Explain your choice by comparing your chosen value to those of P and Cl.[4]
4. (b)(i)Give the full electronic configuration of P³⁻.[1]
5. (b)(ii)State the trend in ionic radius shown by P³⁻, S²⁻ and Cl⁻. Explain your answer.[2]
6. (c)A student does three tests on separate samples of NaCl(aq). Complete Table 1.2 with the observations the student makes in each test. Table 1.2 test observations 1 addition of a few drops of Br₂(aq) 2 addition of a few drops of concentrated H₂SO₄ 3 addition of a few drops of dilute AgNO₃(aq)[3]
7. (d)(i)Explain how the information in (d) suggests the structure and bonding of POCL₃ is simple covalent.[2]
8. (d)(ii)Construct an equation for the reaction of POCL₃ with water. POCL₃ + →[1]
9. (d)(iii)POCL₃ contains a double covalent bond between P and O. Complete the dot-and-cross diagram, in [Figure 1.1], to show the bonding in POCL₃. Show outer shell electrons only.[2]
10. (e)(i)Define enthalpy change of formation, ΔHᶠ.[2]
11. (e)(ii)Calculate the bond energy of P=O in POCl₃ using the data in Table 1.3. Show your working.[2]