CAPE Chemistry Unit 1 · 2006 · Paper 1

52 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 marksCalculate the relative atomic mass Aᵣ of titanium.
2. 1(b)3 marksUse the data booklet and the mass spectrum given above to determine the number of protons and neutrons of the most abundant isotope of titanium.
3. 1(c)1 markUsing s, p, d, f notation, write the electronic configuration of titanium.
4. 1(d)2 marksDraw the shapes of the orbitals of principal quantum number n = 2 in the titanium atom.
5. 1(e)2 marksAnother isotope of titanium, ⁵¹Ti, decays by β-emission. A β-particle has no mass and a single negative charge. Write an equation to represent the decay of a ⁵¹Ti atom.
6. 2(a)2 marksSketch the shape of BOTH the water and ammonia molecules.
7. 2(b)(i)3 marksExplain the difference in the bond angles of the ammonia and water molecules.
8. 2(b)(ii)2 marksExplain the difference in the boiling points of water and ammonia.
9. 2(c)(i)1 markSuggest the shape of a molecule of hydrogen sulphide.
10. 2(c)(ii)2 marksHow would the boiling point of hydrogen sulphide compare with that of ammonia? Explain your answer.
11. 3(a)1 markDefine the term 'enthalpy change of solution'.
12. 3(b)(i)1 markState Hess' Law.
13. 3(b)(ii)5 marksUse the data in Table 2 and apply Hess' Law to determine the enthalpy of solution of hydrogen fluoride gas.
14. 3(b)(iii)3 marksAny chemical change involves processes of bond making and bond breaking. Classify EACH process as exothermic or endothermic and, hence, explain the value obtained in (b)(ii) on page 5.
15. 4(a)(i)1 markWhich of the functional groups present in aspartame would react with ethanol?
16. 4(a)(ii)2 marksWhich of the functional groups present in aspartame would react with dilute hydrochloric acid?
17. 4(a)(iii)1 markWhich of the functional groups present in aspartame would react with ethanoyl chloride?
18. 4(b)1 markName the OTHER chemical that is required for the reaction with ethanol to occur.
19. 4(c)(i)1 markDraw the structural formula of B.
20. 4(c)(ii)2 marksState the reagents and conditions required for the conversion of B to C.
21. 4(c)(iii)2 marksState ONE physical property that is characteristic of BOTH Compound C and that obtained in the reaction described in (b) above. Explain your answer.
22. 5(a)2 marksState TWO reasons why carbon can form straight chains and rings.
23. 5(b)1 markWrite the molecular formula of Dopa.
24. 5(c)(i)1 markDefine the term 'isomerism'.
25. 5(c)(ii)2 marksState TWO types of isomerism which can be exhibited by a molecule with formula A.
26. 5(c)(iii)4 marksDraw the full structural formulae of TWO isomers for each type of isomerism stated in (c)(ii) on page 8.
27. 6(a)(i)1 markHow many monomer units are present in this portion of the macromolecule?
28. 6(a)(ii)2 marksDraw the displayed structure of two monomers used to make A.
29. 6(b)2 marksTo what class of compounds do the monomers and macromolecule, A, belong?
30. 6(c)(i)1 markName the type of reaction that occurs when nylon 6.6 or A is boiled with concentrated hydrochloric acid.
31. 6(c)(ii)1 markCopy the structure of A and use it to illustrate the changes that occur during the reaction described in (c)(i) above.
32. 6(c)(iii)1 markDraw the fully displayed structure of ONE product of the reaction described in (c)(i) above.
33. 6(d)2 marksState ONE common structural feature and ONE different structural feature in nylon 6.6 and A.
34. 7(a)3 marksState THREE characteristics of ethanedioic acid that make it a suitable primary standard.
35. 7(b)2 marksIn preparing the solution of ethanedioic for titration against the permanganate, two pieces of laboratory equipment with a high degree of accuracy are required. Name these TWO pieces of equipment.
36. 7(c)(i)1 markCalculate the number of moles MnO₄⁻ used.
37. 7(c)(ii)1 markCalculate the number of moles Fe²⁺ in the 25.0 cm³ of aqueous M.
38. 7(c)(iii)1 markCalculate the number of moles Fe²⁺ in 1.0 dm³ of M (aq).
39. 7(c)(iv)1 markCalculate the mass of Fe²⁺ in 1 dm³ of M (aq).
40. 7(c)(v)1 markCalculate the % Fe²⁺ in the compound [The mass concentration of M is 40.90 g dm⁻³].
41. 8(a)(i)1 markWhat is meant by retention time as applied to gas liquid chromatography (GLC)?
42. 8(a)(ii)2 marksDistinguish between a stationary phase and a mobile phase used in chromatography.
43. 8(a)(iii)2 marksGive ONE example EACH of commonly used stationary and mobile phases in GLC.
44. 8(b)(i)2 marksCalculate the Rᶠ values for the TWO samples.
45. 8(b)(ii)3 marksDeduce whether the same red dye is used to make both types of ink. Give TWO reasons for your answer.
46. 9(a)3 marksInfra red (IR) spectroscopy is widely used to determine the structure of molecules. State the principles upon which infra red (IR) spectroscopy is based.
47. 9(b)2 marksEven though air consists of 78% N₂ and 21% O₂, these gases do not contribute to global warming. Explain this phenomenon.
48. 9(c)1 markExplain how the IR spectra may be used to distinguish between functional groups in organic compounds.
49. 9(d)1 markThe carbonyl group, >C=O, has absorption peaks in the region of 1680 to 1750 cm⁻¹, while the peaks for the alkene group, >C=C<, are manifested in the region of 1610 to 1680 cm⁻¹. What does this say about the bond…
50. 9(e)1 markSuggest ONE reason why HCl has only one peak in its IR spectrum.
51. 9(f)(i)1 markGive ONE reason why the monochromator and sample cell are not constructed of glass or quartz.
52. 9(f)(ii)1 markWhat material may be used instead of quartz or glass?