CIE Nov 2014 v3 Paper 2 Q1

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Answer all the questions in the spaces provided. PMT (a) Successive ionisation energies for the elementsuorine, F, to bromine, Br, are shown on the graph. 12 000 10 000 ionisation energy / kJ mol1 8000 6000 4000 2000 Cl Br electrons removed (i) Explain why therst ionisation energies decrease down the group.[3] (ii) Explain why there is an increase in the successive ionisation energies ofuorine.[2]UCLES 2014 9701/23/O/N/14<br /> PMT (b) Group VII is the only group in the Periodic Table containing elements in all three states of matter at room conditions. State and explain, in terms of intermolecular forces, the trend in the boiling points of the elements down Group VII.[4] (c) Compounds containing different halogen atoms covalently bonded together are called interhalogen compounds. (i) One interhalogen compound can be prepared by the reaction between iodine anduorine. This compound has Mr = 222 and the percentage composition by mass: F, 42.8; I, 57.2. Calculate the molecular formula of this interhalogen compound. molecular formula[3] (ii) Another interhalogen compound has the formula ICl. Draw a dot-and-cross diagram of a molecule of this compound, showing outer shell electrons only. Explain whether or not you would expect this molecule to be polar.[2]UCLES 2014 9701/23/O/N/14 [Turn over<br /> PMT (d) Some reactions involving chlorine and its compounds are shown in the reaction scheme below. NaCl (aq) + W(aq) cold NaOH(aq) Cl 2(g) H2(g) UV Y(g) hot NaOH(aq) bubble into water NaCl (aq) + X(aq) Z(s) AgNO3(aq) Y(aq) (i) Give the formulae of W, X, Y and Z. WXYZ[4] (ii) Write an equation for the reaction of chlorine with hot NaOH(aq).[2] (iii) State the oxidation numbers of chlorine at the start and at the end of the reaction in (ii).[2] (iv) Write an ionic equation for the reaction of Y with AgNO3(aq). Include state symbols.[1] [Total: 23]UCLES 2014 9701/23/O/N/14<br /> PMT Question 2 starts on the next page.UCLES 2014 9701/23/O/N/14 [Turn over<br />

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