CAPE Chemistry Unit 1 · 2012 · Paper 2

49 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.

1. 1(a)2 marksWith the aid of an example, define the term 'dative (co-ordinate) covalent bond'.
2. 1(b)(i)1 markPlace substances A, B and C in order of increasing boiling point (lowest boiling point first).
3. 1(b)(ii)3 marksIdentify the intermolecular attractive forces found in EACH of the substances in (b) (i) above.
4. 1(b)(iii)4 marksDescribe the origin of TWO of the intermolecular attractive forces named in (b) (ii).
5. 1(c)5 marksComplete Table 1 by indicating whether EACH of the substances, potassium bromide, acetone and solid iodine are soluble or insoluble in the two solvents, water (polar solvent) and toluene (non-polar solvent).
6. 2(a)5 marksDescribe, using FIVE essential steps, an experiment which can be used to determine the solubility product of Ca(OH)2 at room temperature.
7. 2(b)(i)1 markDefine the term 'solubility product'.
8. 2(b)(ii)1 markWrite the equation for the dissociation of calcium carbonate.
9. 2(b)(iii)2 marksWrite the solubility constant expression for calcium carbonate.
10. 2(c)(i)2 marksCalculate the solubility of calcium carbonate (Ksp = 5.0 × 10⁻⁹ mol² dm⁻⁶ at 25°C) in pure water.
11. 2(c)(ii)3 marksCalculate the solubility of calcium carbonate (Ksp = 5.0 × 10⁻⁹ mol² dm⁻⁶ at 25°C) in 0.1 mol dm⁻³ Na₂CO₃ solution.
12. 2(d)1 markWhat is responsible for the difference between the solubilities in (c) (i) and (c) (ii) above?
13. 3(a)(i)3 marksDescribe the reaction of Fluorine with hydrogen.
14. 3(a)(ii)3 marksDescribe the reaction of Chlorine with hydrogen.
15. 3(a)(iii)3 marksDescribe the reaction of Bromine with hydrogen.
16. 3(b)(i)2 marksIdentify the gases observed in Test Tube II and Test Tube III.
17. 3(b)(ii)2 marksWrite a balanced equation to represent the reaction occurring in Test Tube II.
18. 3(b)(iii)2 marksUsing the relevant information provided in the data booklet, explain the trend in the observations recorded in Table 2.
19. 3(b)(iv)1 markWhat would you observe if hydrogen fluoride was used in the experiment?
20. 3(c)(i)1 markState what would be observed in the case of sodium chloride.
21. 3(c)(ii)2 marksState what would be observed in the case of sodium bromide.
22. 3(d)2 marksThe products of the reaction in (c) (i) above were passed into water and the resultant solution treated with AgNO3(aq) followed by aqueous ammonia. State what would be observed.
23. 4(a)3 marksState THREE factors which affect the first ionisation energy of the elements.
24. 4(b)(i)5 marksWrite the s, p and d electronic configuration of Cu.
25. 4(b)(ii)5 marksWrite the s, p and d electronic configuration of O²⁻.
26. 4(b)(iii)5 marksWrite the s, p and d electronic configuration of Mn²⁺.
27. 4(b)(iv)5 marksWrite the s, p and d electronic configuration of Fe³⁺.
28. 4(b)(v)5 marksWrite the s, p and d electronic configuration of Ca.
29. 4(c)3 marksExplain how ionization energy data provide evidence for shells and subshells.
30. 4(d)(i)1 markWrite the electronic configuration of the element represented in Figure 1.
31. 4(d)(ii)1 markSuggest an identity for the element.
32. 4(d)(iii)2 marksWrite a balanced equation to illustrate the first ionisation of the element.
33. 5(a)(i)3 marksCopy and complete Table 3 to show the type of equilibrium for the selected equilibrium systems.
34. 5(a)(ii)2 marksState TWO characteristics of the equilibrium represented by System 1 in Table 3.
35. 5(b)(i)1 markWrite the expression for the equilibrium constant.
36. 5(b)(ii)1 markWhat deduction can be made when the equilibrium constant is much greater than 1?
37. 5(c)(i)2 marksExplain why the white precipitate, BiOCl, disappears on the addition of aqueous HCl to the equilibrium mixture.
38. 5(c)(ii)3 marksExplain what would be observed if a large volume of water was added to the equilibrium mixture.
39. 5(d)3 marksCalculate the concentration of Cl2 in the mixture.
40. 6(a)(i)1 markState the general trend in atomic radii in moving from left to right across Period 3 (from sodium to argon).
41. 6(a)(ii)1 markGive a reason for the trend stated in (i) above.
42. 6(b)(i)3 marksWhich structure is exhibited by Magnesium?
43. 6(b)(ii)3 marksWhich structure is exhibited by Silicon?
44. 6(b)(iii)3 marksWhich structure is exhibited by Sulphur?
45. 6(c)3 marksWith reference to structure and bonding, account for the variation in melting points shown in the figure.
46. 6(d)(i)2 marksSketch a similar diagram to Figure 2 given in 6 (c) to illustrate the variation in the electrical conductivity of the elements in Period 3.
47. 6(d)(ii)3 marksWith reference to structure, explain the variations shown on your sketch in (d) (i) above.
48. 6(e)(i)1 markDescribe the reaction which occurs when magnesium is heated in dry chlorine gas.
49. 6(e)(ii)1 markWrite an equation to represent the reaction in (e)(i) above.