CAPE Chemistry Unit 1 · May/June 2022 · Paper 2

30 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)4 marksComplete Table 1 by filling in the blanks for the relative mass, relative charge, or location of electron, proton, and neutron labeled (i), (ii), (iii), and (iv).
2. 1(b)2 marksDescribe the evidence that disproved Dalton's postulate stating that 'Atoms of the same element are identical in mass and properties', and state the modifications made to this postulate.
3. 1(c)(i)2 marksDefine the term 'relative atomic mass'.
4. 1(c)(ii)2 marksCalculate the relative atomic mass of neon containing 90.9% 20Ne, 0.3% 21Ne, and 8.8% 22Ne.
5. 1(d)(i)1 markWrite the s, p electronic configuration of the oxygen atom in its ground state.
6. 1(d)(ii)4 marksExplain how the atomic orbitals in the oxygen atom overlap to form a double covalent bond in the oxygen molecule, O2.
7. 1(d)(iii)4 marksAccount for the physical properties that the boiling point of water is higher than expected and ice has a lower density than water.
8. 1(e)(i)1 markDefine the term 'bond energy'.
9. 1(e)(ii)5 marksUsing the bond energy values in Table 2, determine the enthalpy change for the reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g) Show all working.
10. 1(f)5 marksOutline the experimental steps required to determine the enthalpy of neutralization reaction between 50 cm^3 of 1.00 M sodium hydroxide solution and 50 cm^3 of 1.00 M hydrochloric acid to obtain an accurate value.…
11. 2(a)(i)1 markDefine the term 'pH'.
12. 2(a)(ii)2 marksCalculate the hydrogen ion concentration of the colourless liquid with pH 4.2.
13. 2(a)(iii)4 marksTwenty cm^3 of a solution with the same pH as the extracted liquid is titrated with 1 x 10^-4 mol dm^-3 aqueous sodium hydroxide. Sketch the titration curve that will be obtained.
14. 2(a)(iv)3 marksUsing Table 3 showing pH ranges of indicators, suggest with reasons which indicator is the most suitable for use in the titration in (iii).
15. 2(b)(i)2 marksDefine the term 'rate of reaction'.
16. 2(b)(ii)4 marksExplain how catalysts and surface area affect the rate of a chemical reaction.
17. 2(c)(i)4 marksUse ONLY the data in Table 4 to determine the order of reaction with respect to S2O8^2- and I^-.
18. 2(c)(ii)1 markBased on your answer in (c)(i), determine the overall order of the reaction.
19. 2(c)(iii)2 marksDetermine the rate law for the reaction.
20. 2(d)(i)2 marksDefine the term 'standard electrode potential of a half cell'.
21. 2(d)(ii)5 marksDraw a labelled diagram to show how the standard electrode potential of the Fe3+(aq)/Fe2+(aq) half cell can be determined.
22. 3(a)(i)3 marksExplain how the boiling point of the halogens changes going down the group.
23. 3(a)(ii)3 marksExplain how the oxidizing power of the halogens changes going down the group.
24. 3(b)(i)2 marksWrite a balanced equation for the reduction of H2SO4 to SO2 by Br^-.
25. 3(b)(ii)2 marksWrite a balanced equation for the reduction of H2SO4 to H2S by I^-.
26. 3(b)(iii)2 marksWrite a balanced equation for the reaction between H2SO4 and Cl^-.
27. 3(c)5 marksComplete the table to show how both AgNO3(aq) and NH3(aq) can be used to distinguish between solutions of NaCl(aq) and NaBr(aq), specifying the test and observations.
28. 3(d)4 marksDiscuss the values of the physical properties (melting point, density, atomic radius) shown in Table 5 in terms of the structure and bonding of the elements calcium and iron.
29. 3(e)(i)4 marksInsert arrows into EACH of the boxes in Figure 1 to show the electronic configuration (3d and 4s orbitals) of Fe3+, Mn2+, Cr, and Ni2+.
30. 3(e)(ii)5 marksConsidering the electronic configurations given for Cu+ (1s2 2s2 2p6 3s2 3p6 3d10) and Cu2+ (1s2 2s2 2p6 3s2 3p6 3d9), discuss the fact that some copper(I) compounds are colourless but most copper(II) compounds are…