Edexcel Jan 2016 (IAL) Paper 1 Q19

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19 The first ionization energies for the elements in Period 3 of the Periodic Table are Element First ionization energy / kJ mol1 Na 496 Mg 738 Al Si Cl Ar 578 789 1012 1000 1251 1521 (a) (i) Complete the electronic configuration of phosphorus, using the electrons-in-boxes notation. Write the symbols for the sub-shells on the dotted lines. (cid:110)(cid:112) 1s*(ii) The first ionization energies generally increase from left to right across the period. Explain why the first ionization energy of sulfur is lower than that of phosphorus. (2) (2)(iii) Write an equation, with state symbols, to show the third ionization energy of phosphorus. (2) 14 *P46937A01424* D O N O T W R I T E I N T H I S A R E A D O N O T W R I T E I N T H I S A R E A D O N O T W R I T E I N T H I S A R E A<br /> *(b) (i) Explain why the first ionization energy of nitrogen is greater than the first ionization energy of phosphorus. (3)(ii) Draw a dot and cross diagram to show the bonding in a molecule of nitrogen. Show outer electrons only. (c) Solid white phosphorus exists as P4 molecules. Calculate the number of molecules in 24.8 g of white phosphorus. [The Avogadro constant, L = 6.021023 mol1] (2) (2) A E R A S I H T N I E T I R W T O N O D A E R A S I H T N I E T I R W T O N O D A E R A S I H T N I E T I R W T O N O D (Total for Question 19 = 13 marks) *P46937A01524* 15 Turn over<br />

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