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Forces of Attraction · CAPE Chemistry Unit 1

64 past-paper questions on Forces of Attraction, part of Fundamentals in Chemistry, from every CAPE Chemistry Unit 1 paper on Quelpr.

Practise Forces of Attraction
  1. 5(a)(i)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Suggest an explanation for the difference in behaviour of benzene under the stated conditions.
  2. 5(a)(ii)2 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Write an equation to illustrate the reaction between sulphuric acid and nitric acid.
  3. 5(b)(i)4 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Illustrate the reaction mechanism for the nitration of benzene.
  4. 5(b)(ii)1 mark· CAPE Chemistry Unit 1 · 2005 · Paper 1What is the name given to the mechanism outlined for the nitration of benzene?
  5. 6(b)(ii)3 marks· CAPE Chemistry Unit 1 · 2005 · Paper 1Explain why L-threonine has a high melting point and is soluble in water.
  6. 1(b)(i)3 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Suggest the type of intermolecular forces between particles of A and describe how they arise.
  7. 1(b)(ii)3 marks· CAPE Chemistry Unit 1 · 2005 · Paper 2Name and describe the bonding forces present in substance B.
  8. 1(b)(iii)4 marks· CAPE Chemistry Unit 1 · May/June 2019 · Paper 2Use the VSEPR theory to deduce the arrangement of the orbitals and the shape or bond angles around each of the oxygen atom in a molecule of water (H2O) and the hydronium ion (H3O+).
  9. 1(b)(iv)3 marks· CAPE Chemistry Unit 1 · May/June 2019 · Paper 2Explain why the density of ice is lower than expected.
  10. 1(d)(ii)4 marks· CAPE Chemistry Unit 1 · May/June 2022 · Paper 2Explain how the atomic orbitals in the oxygen atom overlap to form a double covalent bond in the oxygen molecule, O2.
  11. 1(d)(iii)4 marks· CAPE Chemistry Unit 1 · May/June 2022 · Paper 2Account for the physical properties that the boiling point of water is higher than expected and ice has a lower density than water.
  12. 1(c)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2State what is meant by the term 'hybridization'.
  13. 1(d)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Benzene exhibits resonance structures. Explain what is meant by 'resonance'.
  14. 1(e)(i)3 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2State THREE criteria used in the valence shell electron pair repulsion (VSEPR) theory to determine the shapes of molecules and ions.
  15. 1(e)(ii)a)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Use the criteria in (e)(i) to determine the shape and bond angles in the beryllium chloride molecule.
  16. 1(e)(ii)b)2 marks· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Use the criteria in (e)(i) to determine the shape and bond angles in the methyl anion, CH3^-.
  17. 1(e)(iii)1 mark· CAPE Chemistry Unit 1 · May/June 2024 · Paper 2Draw a diagram to show the shape of the methyl anion, CH3^-.
  18. 1(c)(i)4 marks· CAPE Chemistry Unit 1 · May/June 2025 · Paper 2Outline fully the steps involved in the procedure that the student would follow in order to obtain the melting point of Substance S.
  19. 1(c)(ii)1 mark· CAPE Chemistry Unit 1 · May/June 2025 · Paper 2Based on the melting point data obtained, the student concludes that S is a covalent compound. Further analysis reveals that it is nonpolar. State whether Substance S will dissolve in water or tetrachloromethane.
  20. 1(c)(iii)2 marks· CAPE Chemistry Unit 1 · May/June 2025 · Paper 2It was determined that Substance S is a solid with a low melting point. Describe the type of forces of attraction that exist between the molecules of Substance S.
  21. 1(e)(i)4 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2Compare bonding in N2 and CaO in terms of electron interaction and polarity.
  22. 1(e)(ii)2 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2State the TWO types of intra-molecular bonds present in the NH4+ structure.
  23. 1(f)4 marks· CAPE Chemistry Unit 1 · May/June 2026 · Paper 2The boiling point of HCl is -85 °C whereas the boiling point of HF is 20 °C. With reference to the electronegativity of the halogen, explain the difference in the boiling point temperatures of HCl and HF.
  24. 1(a)2 marks· Chemistry · Unit 1 Q1 1(a)State the types of bonds (intra-molecular and inter-molecular) that exist in liquid ammonia.
  25. 1(a)2 marks· Chemistry · Unit 1 Q1 1(a)With the aid of an example, define the term 'dative (co-ordinate) covalent bond'.
  26. 1(b)(i)1 mark· Chemistry · Unit 1 Q1 1(b)(i)Place substances A, B and C in order of increasing boiling point (lowest boiling point first).
  27. 1(b)(ii)3 marks· Chemistry · Unit 1 Q1 1(b)(ii)Identify the intermolecular attractive forces found in EACH of the substances in (b) (i) above.
  28. 1(b)(iii)4 marks· Chemistry · Unit 1 Q1 1(b)(iii)Describe the origin of TWO of the intermolecular attractive forces named in (b) (ii).
  29. 1(c)5 marks· Chemistry · Unit 1 Q1 1(c)Complete 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).
  30. 1(c)(i)2 marks· Chemistry · Unit 1 Q1 1(c)(i)What kind of bonding is present in halides of X?
  31. 1(c)(ii)1 mark· Chemistry · Unit 1 Q1 1(c)(ii)What kind of bonding is present in halides of Y?
  32. 1(e)7 marks· Chemistry · Unit 1 Q1 1(e)L, M and N are examples of three solid compounds which are ionic, polar and covalent respectively. Using the format in Table 1, describe THREE simple laboratory tests, stating the corresponding observations, to show the…
  33. 21 mark· Chemistry · Unit 1 Q2 2The intermolecular forces present in ice are
  34. 2(a)2 marks· Chemistry · Unit 1 Q2 2(a)Sketch the shape of BOTH the water and ammonia molecules.
  35. 2(b)(i)3 marks· Chemistry · Unit 1 Q2 2(b)(i)Explain the difference in the bond angles of the ammonia and water molecules.
  36. 2(b)(ii)2 marks· Chemistry · Unit 1 Q2 2(b)(ii)Explain the difference in the boiling points of water and ammonia.
  37. 2(c)(i)1 mark· Chemistry · Unit 1 Q2 2(c)(i)Suggest the shape of a molecule of hydrogen sulphide.
  38. 2(c)(ii)2 marks· Chemistry · Unit 1 Q2 2(c)(ii)How would the boiling point of hydrogen sulphide compare with that of ammonia? Explain your answer.
  39. 31 mark· Chemistry · Unit 1 Q3 3Which of the following pairs of elements combine to produce naturally occurring compounds with formulae type XY?
  40. 41 mark· Chemistry · Unit 1 Q4 4Which of the following diagrams represents a pi (π) bond?
  41. 41 mark· Chemistry · Unit 1 Q4 4Which of the following diagrams represents a pi (π) bond?
  42. 4(a)1 mark· Chemistry · Unit 1 Q4 4(a)State the basic principle behind the VSEPR theory.
  43. 4(a)3 marks· Chemistry · Unit 1 Q4 4(a)Apply the concept of the 'hybridization of atomic orbitals' to explain the planarity of the ethene molecule.
  44. 4(a)(i)4 marks· Chemistry · Unit 1 Q4 4(a)(i)Describe how the bonds are formed in EACH of the solids, potassium chloride and iodine.
  45. 4(a)(ii)3 marks· Chemistry · Unit 1 Q4 4(a)(ii)Account for the number and type of orbitals around EACH carbon atom in a molecule of ethane.
  46. 4(a)(ii)2 marks· Chemistry · Unit 1 Q4 4(a)(ii)Complete Table 3 by comparing the physical properties of potassium chloride (KCl) and iodine (I₂).
  47. 4(a)(iii)3 marks· Chemistry · Unit 1 Q4 4(a)(iii)Use the VSEPR theory to deduce the arrangement of the orbitals and the bond angles around EACH carbon atom in a molecule of dichloroethane, CH₂ClCH₂Cl.
  48. 4(b)(i)2 marks· Chemistry · Unit 1 Q4 4(b)(i)Using the VSEPR theory, state the shapes of the hydroxonium (H3O+) and ammonium (NH4+) ions.
  49. 4(b)(i)2 marks· Chemistry · Unit 1 Q4 4(b)(i)State TWO principles which form the basis of the valence-shell electron pair repulsion (VSEPR) theory.
  50. 4(b)(i)3 marks· Chemistry · Unit 1 Q4 4(b)(i)Account for EACH of the following statements: The boiling point of H₂O is higher than that of H₂S.
  51. 4(b)(ii)4 marks· Chemistry · Unit 1 Q4 4(b)(ii)Use the VSEPR theory to account for the difference in shape between the ammonia molecule (NH₃) and the ammonium ion (NH₄⁺). Ammonia molecule (NH₃): Ammonium ion (NH₄⁺):
  52. 4(b)(ii)2 marks· Chemistry · Unit 1 Q4 4(b)(ii)Using suitable diagrams, illustrate the shape of EACH ion in (b) (i).
  53. 4(b)(ii)3 marks· Chemistry · Unit 1 Q4 4(b)(ii)Account for EACH of the following statements: The molecules of aluminium fluoride in the presence of ammonia forms a white solid of formula NH₄AlF₄. (Include an appropriate equation in your account.)
  54. 4(b)(iii)4 marks· Chemistry · Unit 1 Q4 4(b)(iii)Account for the shape of EACH of the species, H3O+ and NH4+.
  55. 4(c)3 marks· Chemistry · Unit 1 Q4 4(c)Explain the difference between the shapes of NH₃ and NH₄⁺.
  56. 4(c)(i)4 marks· Chemistry · Unit 1 Q4 4(c)(i)The experimental determination of the relative molecular mass of ethanoic acid (CH3CO2H) produces a value of 120 g. Your answer should include a suitable diagram.
  57. 4(c)(ii)2 marks· Chemistry · Unit 1 Q4 4(c)(ii)The boiling point of propanone (acetone) is greater than the boiling point of butane.
  58. 6(a)2 marks· Chemistry · Unit 1 Q6 6(a)Define the term 'polarization'.
  59. 71 mark· Chemistry · Unit 1 Q7 7Which of the following structures correctly illustrates the co-ordinate bonding between BF₃ and NH₃?
  60. 111 mark· Chemistry · Unit 1 Q11 11Which of the following groups of solids contains substances that ALL have giant structures?
  61. 111 mark· Chemistry · Unit 1 Q11 11Which of the following groups of solids contains substances that ALL have giant structures?
  62. 151 mark· Chemistry · Unit 1 Q15 15A student was asked to carry out an experiment to investigate the properties of ionic and covalent compounds. Which of the following experiments should the student use?
  63. 311 mark· Chemistry · Unit 1 Q31 31Which of the following ions has the GREATEST polarizing power?
  64. 311 mark· Chemistry · Unit 1 Q31 31Which of the following ions has the GREATEST polarizing power?

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