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CAPE Chemistry Unit 1 · 2010 · Paper 2

42 questions and parts from this paper. Open one to see it in full, then practise it on Quelpr and get it marked against the mark scheme.

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  1. 1(a)2 marksState the types of bonds (intra-molecular and inter-molecular) that exist in liquid ammonia.
  2. 1(b)(i)2 marksWrite a balanced chemical equation for the reaction between calcium oxide and ammonium chloride.
  3. 1(b)(ii)2 marksCalculate the mass of ammonium chloride needed to produce 1 dm³ of ammonia at RTP (room temperature and pressure). (Molar volume = 24 dm³ at RTP)
  4. 1(c)(i)1 markUnder which of the following sets of conditions, I, II or III, would the deviation be LEAST?
  5. 1(c)(ii)2 marksState TWO assumptions of the kinetic theory as it pertains to ideal gases.
  6. 1(c)(iii)1 markWhich assumption of the kinetic theory as it pertains to ideal gases would MOST likely account for your answer to (c) (i) above?
  7. 1(d)5 marksDescribe an experiment that would determine the concentration of the aqueous ammonia.
  8. 2(a)(i)2 marksDefine EACH of the following terms: Standard electrode potential of a half-cell
  9. 2(a)(ii)2 marksDefine EACH of the following terms: Standard cell potential of an electrochemical cell
  10. 2(b)(i)a)5 marksOn the diagram in Figure 1, label the ions in Solution A and Solution B
  11. 2(b)(i)b)1 markOn the diagram in Figure 1, label the salt bridge
  12. 2(b)(i)c)1 markOn the diagram in Figure 1, label the cathode and anode
  13. 2(b)(i)d)1 markOn the diagram in Figure 1, label the direction of electron flow.
  14. 2(b)(ii)1 markState what would be observed at the cathode after the electrochemical cell in Figure 1 has been running for a few hours.
  15. 2(b)(iii)2 marksState the experimental conditions used in the preparation of the cell in Figure 1. Temperature, Concentration of Solutions A and B
  16. 2(b)(iv)3 marksUse the information in your Data Booklet to calculate the standard cell potential, Ecell, for the electrochemical cell in Figure 1.
  17. 3(a)5 marksRecord in Table 1 the observation expected for EACH of the tests below.
  18. 3(b)(i)3 marksCalculate the oxidation number of vanadium in EACH of the following species: VOSO4
  19. 3(b)(ii)1 markCalculate the oxidation number of vanadium in EACH of the following species: VO2+
  20. 3(b)(iii)1 markCalculate the oxidation number of vanadium in EACH of the following species: VO2+
  21. 3(c)4 marksGive an explanation for the observation stated above in terms of the stability constant of the complex ion formed, and write a balanced equation for the reaction.
  22. 3(d)3 marksComplete Table 2 to show the acid/base character of the oxides of Group IV elements in the +2 oxidation state.
  23. 4(a)4 marksCopy and complete Table 3, which provides information on the properties of the simple subatomic particles.
  24. 4(b)(i)1 markName the type of radioactive particle that behaves in the same way as the electron.
  25. 4(b)(ii)6 marksState the product formed from the decay of 216Po by the emission of three β particles and calculate the n/p ratio of BOTH the reactant and product atoms.
  26. 4(b)(iii)1 markComment on the effect that the decay has on the stability of the nucleus of 216Po.
  27. 4(c)(i)2 marksDraw the structures of the atomic orbitals of principal quantum number 2. Include x, y and z axes in the drawing.
  28. 4(c)(ii)1 markUsing s, p, d notation, write the electronic configuration of 24Cr.
  29. 5(a)(i)2 marksDefine EACH of the following terms: pH
  30. 5(a)(ii)2 marksDefine EACH of the following terms: Buffer solution
  31. 5(b)(i)1 markWrite an expression for the acid dissociation constant (Ka) of ethanoic acid.
  32. 5(b)(ii)4 marksCalculate the equilibrium concentration of ethanoic acid in a solution that has a pH of 5.
  33. 5(c)(i)1 markState the effect, on the equilibrium position of a buffer solution, of adding small amounts of H+(aq)
  34. 5(c)(ii)1 markState the effect, on the equilibrium position of a buffer solution, of adding small amounts of OH-(aq).
  35. 5(d)4 marksCalculate the pH of this buffer solution. (Relative atomic mass: H = 1, C = 12, O = 16, Na = 23)
  36. 6(a)(i)2 marksAccount for EACH of the following variations in properties across the period Na to Ar. Electronegativity increases across the period.
  37. 6(a)(ii)2 marksAccount for EACH of the following variations in properties across the period Na to Ar. Melting point of the elements increases from Na to Si.
  38. 6(b)3 marksDescribe the trend in the acid/base character of the oxides of the elements in Period 3.
  39. 6(c)2 marksAccount for the acidic nature of the aluminium chloride solution.
  40. 6(d)2 marksTransition metals have higher melting points than metals such as calcium in the s-block of the periodic table. Suggest TWO reasons for this.
  41. 6(e)(i)2 marksWrite an equation to show how EACH of the following reacts with water. P4O10
  42. 6(e)(ii)2 marksWrite an equation to show how EACH of the following reacts with water. PCl5

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