CAPE Chemistry Unit 1 · 2014 · Paper 2

43 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)(i)2 marksDefine the term 'mole'.
2. 1(a)(ii)2 marksDefine the term 'molar mass' (include the units).
3. 1(b)(i)a)2 marksCalculate the number of moles of M₂CO₃.
4. 1(b)(i)b)2 marksCalculate the relative molecular mass of M₂CO₃.
5. 1(b)(ii)2 marksDeduce the identity of M.
6. 1(c)5 marksOutline the experimental steps required to carry out the reaction described in (b) on page 2.
7. 2(a)(i)1 markState the Brønsted-Lowry theory of acids and bases.
8. 2(a)(ii)2 marksDistinguish between a 'strong acid' and a 'weak acid'.
9. 2(b)(i)2 marksIn the space below, sketch the curve which is expected to illustrate the changes that take place during titration.
10. 2(b)(ii)2 marksSuggest an indicator, giving a reason for your choice.
11. 2(c)(i)1 markDeduce the order of the reaction.
12. 2(c)(ii)2 marksCalculate the rate constant for the decomposition.
13. 2(d)(i)1 markMagnesium filings were added to the remaining solution at 2(c). What observation is expected?
14. 2(d)(ii)4 marksOutline an alternative experimental method to determine the rate of decomposition of HOX at room temperature.
15. 3(a)2 marksDefine the term 'transition element'.
16. 3(b)(i)1 markDeduce the oxidation number of the platinum atom.
17. 3(b)(ii)1 markSuggest the shape of the cisplatin molecule.
18. 3(c)(i)a)2 marksComplete the diagrams below by inserting arrows to show the electronic configuration of Fe²⁺ ion.
19. 3(c)(i)b)2 marksComplete the diagrams below by inserting arrows to show the electronic configuration of Mn²⁺ ion.
20. 3(c)(ii)2 marksUse the information in (c)(i)b) to explain why Mn²⁺ ions resist oxidation to Mn³⁺ ions.
21. 3(d)(i)3 marksList the colour of the following ions: B, C, D.
22. 3(d)(ii)2 marksSketch the arrangement of bonds in the ion labelled C.
23. 3(e)2 marksState the changes that would be observed when a solution of copper(II) ions is treated with concentrated hydrochloric acid followed by concentrated ammonia.
24. 4(a)(i)1 markState the electronic configuration of carbon in its ground state using sp notation.
25. 4(a)(ii)3 marksAccount for the number and type of orbitals around EACH carbon atom in a molecule of ethane.
26. 4(a)(iii)3 marksUse the VSEPR theory to deduce the arrangement of the orbitals and the bond angles around EACH carbon atom in a molecule of dichloroethane, CH₂ClCH₂Cl.
27. 4(b)(i)3 marksState THREE assumptions of the kinetic theory as it pertains to ideal gases.
28. 4(b)(ii)1 markUnder what conditions of temperature and pressure will a real gas deviate from ideal gas behaviour?
29. 4(c)4 marksCalculate the relative molecular mass (Mᵣ) of the gas.
30. 5(a)(i)2 marksDefine the term 'solubility'.
31. 5(a)(ii)2 marksDefine the term 'solubility product'.
32. 5(b)(i)2 marksCalculate the solubility, in mol dm⁻³, of the lead(II) azide.
33. 5(b)(ii)2 marksWrite the expression for the solubility product of lead(II) azide.
34. 5(b)(iii)2 marksCalculate the solubility product of lead(II) azide.
35. 5(c)(i)2 marksSketch a diagram showing the distribution of energies in a gas at a given temperature, T₁.
36. 5(c)(ii)1 markOn the same diagram as in 5(c)(i), insert another curve showing the distribution of energies of the molecules at a higher temperature, T₂.
37. 5(c)(iii)2 marksUsing your sketch, explain the difference in the rates of reaction at temperatures T₁ and T₂.
38. 6(a)2 marksDefine the term 'polarization'.
39. 6(b)(i)1 markState the trend in ionic size of the elements from Na to Al.
40. 6(b)(ii)7 marksExplain the following observation. (Include relevant equations to support your answer.)
41. 6(c)(i)1 markState the name of the halide ion in A.
42. 6(c)(ii)2 marksWrite the formula equation for the reaction of A with chlorine.
43. 6(c)(iii)2 marksDescribe an additional simple test to confirm the identity of the halide ion in A.