2017 Chemistry WAEC SSCE (School Candidates) May/June

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Chemistry 1 - Objective Test Questions

1. Which of the following species determines properties of an atom?
   1. Electron
   2. Neutron
   3. Nucleus
   4. Proton
2. The following glasses are are used to measure the volume of liquids except
   1. graduated beaker
   2. pipette.
   3. test tube.
   4. burette
3. Pauli exclusion principle is related to
   1. quantity of electrons in the valence shell.
   2. filling the orbitals with lower energy first.
   3. the filling of degenerated orbitals.
   4. quantum numbers of electrons.
4. The species with no electron in the 3d-orbital is
   1. Option a
   2. Option b
   3. Cu
   4. Mn
5. The separation of oxygen from nitrogen by fractional distillation of air is possible because A. nitrogen Is less dense than oxygen. B. oxygen is more reactive than nitrogen. _C. of the difference in their
   1. nitrogen Is less dense than oxygen.
   2. oxygen is more reactive than nitrogen.
   3. of the difference in their boiling points.
   4. they belong to the same period.
6. The purity of a Solid sample can best be determined by its
   1. boiling point.
   2. melting point.
   3. conductivity.
   4. Solubility
7. The mass of one mole of XX is
   1. 66.0g.
   2. 76.0g.
   3. 80.0g
   4. 96.0g
8. Atomic orbital is
   1. the circular path through which electrons revolve round the nucleus.
   2. a region around the nucleus where electrons are most likely to be found.
   3. the path around the nucleus through which electrons move.
   4. the path around the nucleus through which protons move.
9. The property of elements which increases down a group of the Periodic Table is
   1. electronegativity.
   2. electron affinity.
   3. ionic radius.
   4. ionization energy.
10. The reason for the decrease in the atomic size of elements across a period is that
    1. nuclear charge increases While the outermost electrons are drawn closer to the nucleus.
    2. nuclear charge decreases while the outermost electrons are drawn closer to the nucleus.
    3. valence electrons increase across the period while the valence shell remains constant.
    4. nuclear charge decreases while the distance of the valence shell from the nucleus is increasing.
11. The oxidation number of nitrogen in
    1. +2.
    2. +3.
    3. +4.
    4. +5.
12. Which of the following arrangements indicates the correct decreasing order of ionization energy of period 3 elements?
    1. Na, Al, P, Cl
    2. Cl, P, Al, Na
    3. Na, P, Cl, Al
    4. Al, Na, P, Cl
13. Which of the following metals has the strongest metallic bond?
    1. Option a
    2. Option b
    3. Option c
    4. Option d
14. Question 14
    1. Option a
    2. Option b
    3. Option c
    4. Option d
15. Question 15
    1. Option a
    2. Option b
    3. Option c
    4. Option d
16. Question 16
    1. Option a
    2. Option b
    3. Option c
    4. Option d
17. Question 17
    1. Option a
    2. Option b
    3. Option c
    4. Option d
18. Question 18
    1. Option a
    2. Option b
    3. Option c
    4. Option d
19. Question 19
    1. Option a
    2. Option b
    3. Option c
    4. Option d
20. Question 20
    1. Option a
    2. Option b
    3. Option c
    4. Option d
21. Question 21
    1. Option a
    2. Option b
    3. Option c
    4. Option d
22. Question 22
    1. Option a
    2. Option b
    3. Option c
    4. Option d
23. Question 23
    1. Option a
    2. Option b
    3. Option c
    4. Option d
24. Question 24
    1. Option a
    2. Option b
    3. Option c
    4. Option d
25. Question 25
    1. Option a
    2. Option b
    3. Option c
    4. Option d
26. Question 26
    1. Option a
    2. Option b
    3. Option c
    4. Option d
27. Question 27
    1. Option a
    2. Option b
    3. Option c
    4. Option d
28. Question 28
    1. Option a
    2. Option b
    3. Option c
    4. Option d
29. Question 29
    1. Option a
    2. Option b
    3. Option c
    4. Option d
30. Question 30
    1. Option a
    2. Option b
    3. Option c
    4. Option d
31. Question 31
    1. Option a
    2. Option b
    3. Option c
    4. Option d
32. Question 32
    1. Option a
    2. Option b
    3. Option c
    4. Option d
33. Question 33
    1. Option a
    2. Option b
    3. Option c
    4. Option d
34. Question 34
    1. Option a
    2. Option b
    3. Option c
    4. Option d
35. Question 35
    1. Option a
    2. Option b
    3. Option c
    4. Option d
36. Question 36
    1. Option a
    2. Option b
    3. Option c
    4. Option d
37. Question 37
    1. Option a
    2. Option b
    3. Option c
    4. Option d
38. Question 38
    1. Option a
    2. Option b
    3. Option c
    4. Option d
39. Question 39
    1. Option a
    2. Option b
    3. Option c
    4. Option d
40. Question 40
    1. Option a
    2. Option b
    3. Option c
    4. Option d
41. Question 41
    1. Option a
    2. Option b
    3. Option c
    4. Option d
42. Question 42
    1. Option a
    2. Option b
    3. Option c
    4. Option d
43. Question 43
    1. Option a
    2. Option b
    3. Option c
    4. Option d
44. Question 44
    1. Option a
    2. Option b
    3. Option c
    4. Option d
45. Question 45
    1. Option a
    2. Option b
    3. Option c
    4. Option d
46. Question 46
    1. Option a
    2. Option b
    3. Option c
    4. Option d
47. Question 47
    1. Option a
    2. Option b
    3. Option c
    4. Option d
48. Question 48
    1. Option a
    2. Option b
    3. Option c
    4. Option d
49. Question 49
    1. Option a
    2. Option b
    3. Option c
    4. Option d
50. Question 50
    1. Option a
    2. Option b
    3. Option c
    4. Option d

Chemistry 2 - Theory Questions

Section A - For All Candidates

1. 1. 1. What is an acid-base indicator?
      2. Give-one: example: of an acid-base indicator.
   2. State the property exhibited by nitrogen(IV) oxide in each of the following equations:
      1. ${\ce {4 Cu +2 NO2 -> 4 CuO + N2}}$
      2. ${\ce {H2O +2 NO2 -> HNO3 + HNO2}}$
   3. 1. Define enthalpy of combustion.
      2. State why the enthalpy of combustion is always negative.
   4. 1. Distinguish between a primary cell and a secondary cell.
      2. Give an example of each of the cells stated in 1(d)(i).
   5. Define the term mole.
   6. Calculate the amount of hydrochloric acid in 40.0 $cm^{3}$ of $0.40moldm^{-}3$ of dilute HCL.
   7. Name two substances which can be used as electrodes during the electrolysis of acidified water.
   8. List two forces of attraction that can exist between covalent molecules.
   9. Name the products formed when butane undergoes incomplete combustion.
   10. Write the electron configuration of ${\ce {_{26}Fe^3+}}$

Section B

2. 1. 1. I State the periodic law. II What is meant by the term periodic property of elements?
      2. List three properties of an element which show periodicity
      3. Explain briefly how each of the properties listed in 2(a)(i) in varies across the period.
   2. Define relative atomic mass.
   3. 1. What phenomenon is exhibited by an element Z which exist as ${\ce {^{35}_{17}Z}}$ and ${\ce {^{37}_{17}Z}}$?
      2. What accounts for the difference in the mass numbers of the element Z?
      3. Calculate the relative atomic mass of Z if the percentage abundance of ${\ce {^{37}_{17}Z}}$ is 75%.
   4. 1. State the method used for collecting each of the following gases: I ${\ce {CO2}}$ II ${\ce {HCl}}$ III ${\ce {H2}}$
      2. Give a reason for your answer stated in and 2(d)(i) I and I
3. 1. Consider the following reaction equation: ${\ce {C12H26 ->[{Al2O3}][{350°C}] X +C8H18}}$
      1. What type of reaction is represented by the equation?
      2. Write the molecular of formula of X.
      3. Draw the structure of two isomers of X.
      4. Name the isomers drawn in 3(a)(iii).
      5. Write a balanced equation for the reaction between X and hydrogen.
   2. Describe one test for fats.
   3. Sulphur (IV) oxide is converted to tetraoxosulphate (VI) acid according to the following equation: ${\ce {2SO2_{(g)}+O2_{(g)}+2H2O_{(}l)->2H2SO4_{(}aq)}}$. If 1.5 moles of oxygen reacts with Sulphur (IV) oxide, calculate the mass of tetraoxosulphate (VI) acid produced. [H = 1.0; O = 16.0; S = 32.0]
   4. Consider the following neutralization reactions:${\ce {CH3COOH + NaOH ->CH3COONa + H2O}}$, ${\ce {CH3COOH + NH4OH ->CH3COONH4 + H2O}}$${\ce {NaOH+HCl ->NaCl + H2O}}$
      1. Arrange the enthalpy changes for the reactions in order of increasing magnitude.
      2. Explain briefly your order in 3(d)(i).
   5. Consider the following substances, State the substance(s) which: ${\ce {Cu_{(}s)}}$, ${\ce {BeCl2_{(}s)}}$, ${\ce {NaH_{(}s)}}$, ${\ce {HF_{(}l)}}$ and ${\ce {CCl4_{(}l)}}$
      1. can conduct electricity;
      2. is/are soluble in water.

Section C - For Candidates in Nigeria, Sierra Leone, The Gambia and Liberia

4. 1. 1. Describe briefly the industrial preparation of ammonia.
      2. Write a balanced equation for the reaction in 4(a)(1).
      3. State one way of increasing the yield of ammonia in 4(a)(1).
      4. State two uses of ammonia.
   2. Describe briefly, one chemical test for each of the following gases in the laboratory:
      1. hydrogen;
      2. carbon(IV) oxide;
      3. oxygen
   3. 1. State the composition of water gas.
      2. List two uses of water gas.
   4. Describe briefly a simple experiment to determine the type of hardness in a sample of water.
5. 1. 1. Describe briefly how trioxonitrate (V) ions could be tested for in the laboratory.
      2. State two uses of each of the following compounds: I. sodium chloride; II. sodium trioxocarbonate (IV).
   2. 1. Write balanced equations for the reactions involved in the extraction of iron in the blast furnace.
      2. State Faraday first law of electrolysis.
      3. State two applications of electrolysis.
   3. Concentrated tetraoxosulphate (VI) acid is added to sugar crystals in a beaker, State what would be observed. Explain briefly your answer.
   4. Write an equation for the reaction of zinc powder with:
      1. dilute tetraoxosulphate (VI) acid;
      2. concentrated tetraoxosulphate (VI) acid.
   5. What property of concentrated tetraoxosulphate (VI) acid is shown in 5 (d)(ii)?

Chemistry 3 - Practical Questions

1. A is $0.200moldm^{-}3$ of HCI. C is a solution containing 14.3g of ${\ce {Na2CO3XH2O}}$ in 500 $cm^{3}$ of solution.
   1. Put A into the burette and titrate it against 20.0 $cm^{3}$ or 25.0 $cm^{3}$ portions of C using methyl orange as indicator, Repeat the titration to obtain Consistent titre values. Tabulate your results and calculate the average volume of A used, The equation for the reaction is: ${\ce {Na2CO3*XH2O}}$ ${\ce {+2HCl_{(}aq)->NaCl_{(}aq)}}$ ${\ce {+CO2_{(}g)}}$${\ce {+ (x + 1)H2O}}$
   2. From your results and the information provided. calculate the:
      1. concentration of C in moldmn-3:
      2. concentration of C in gdin-3;
      3. molar mass of Na2CO3 . XH20:
      4. the value of X in NaxCO3 . XH20.
   3. Sub-question c
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   4. Sub-question d
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   5. Sub-question e
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   6. Sub-question f
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
2. Question 2
   1. Sub-question a
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   2. Sub-question b
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   3. Sub-question c
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   4. Sub-question d
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   5. Sub-question e
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   6. Sub-question f
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
3. Question 3
   1. Sub-question a
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   2. Sub-question b
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   3. Sub-question c
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   4. Sub-question d
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   5. Sub-question e
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v
   6. Sub-question f
      1. Sub-question i
      2. Sub-question ii
      3. Sub-question iii
      4. Sub-question iv
      5. Sub-question v