Chemistry Examination Question for Senior Secondary School (SS1)

24. An atom of an element X gains two electrons. The symbol of the ion formed is?

(a) X⁺ (b) X²⁺ (c) X^2- (d) X^–

25. On heating, the following trioxocarbonate (iv) salts decompose to give solid residue except

(a) ammonium trioxocarbonate (iv)            (b) calcium trioxocarbonate (iv) (c) lead trioxocarbonate (iv) (d) zinc trioxocarbonate (iv)

26. Two elements X and Y are in the same-group on the periodic table because they both have the same

(a) number of electronic shells (b) number of valence electrons (c) atomic size (d) atomic number

27. Which of the following elements is a metalloid?

(a) carbon (b) oxygen (c) silicon (d) sodium

28. Which of the following substances is a constituent of fire extinguisher?

(a) ammonia (b) carbon (iv) oxide               (c) hydrogen sulphide  (d) sulphur (iv) oxide

29. How many protons are there in a metallic ion (x³⁺) which has an inert gas structure and contains 10 electrons?

(a) 3 (b) 7 (c) 10 (d) 13

30. The type of bond formed when two elements ₁₇X and ₁₉Y combine together is

(a) covalent (b) co-ordinate (c) electrovalent (d) hydrogen

31. Which of the following substance is mainly responsible for the depletion of the ozone layer?

(a) chlorofluorocarbon (b) carbon (iv) oxide (c) nitrogen (d) oxygen

32. Which of the following separation techniques would show that black ink is a mixture of chemical compounds?

(a) crystallization (b) chromatography         (c) filtration (d) sublimation

33. The equation p = k/v illustrates

(a) Boyle’s law (b) Charle’s law (c) Dalton’s law (d) Gay Lussac’s law

34. Which of the following elements can conveniently be placed in two groups in the periodic table?

(a) carbon (b) copper (c) hydrogen           (d) oxygen

35. Which of the following electron configurations correctly represents noble gas?

(a) 1s² 2s² 2p⁴ (b) 1s² 2s² 2p⁶ 35₂ (c) 1s² 2s² 2p⁶ 3s² 3p⁴ (d) 1s² 2s² 2p⁶

36. Salts that contain water of crystallization are said to be

(a) anhydrous (b) deliquescent                   (c) efflorescent (d) hydrated

37. How many orbitals are associated with the p-sub orbital?

(a) 2 (b) 3 (c) 5 (d) 6

38. How protons does contain?

(a) 20 (b) 40 (c) 30 (d) 60

39. What is the value of 14⁰C on the Kelvin temperature scale?

(a) 259k (b) 259⁰k (c) 287k (d) 287⁰k

40. Chemicals that are produced in small quantities and with very high degree of purity are

(a) bulk chemicals (b) fine chemicals          (c) heavy chemicals (d) light chemicals

41. How many isotopes has hydrogen?

(a) 2 (b) 3 (c) 4 (d) 5

42. Which of the following metallic oxides is amphoteric?

(a) Al₂O₃ (b) Fe₂O₃ (c) MgO (d) Na₂O

43. The compound that makes palm wine taste sour after exposure to the air for few days is (a) ethanol (b) ethanoic acid (c) methanol (d) methanoic acid
44. The number of atoms in a compound is called

(a) atomic number (b) avogadro number     (c) empirical formula (d) molecular formula

45. Flourine is sometimes added in the treatment of town water to

(a) improve coagulation (b) kill germs and bacteria (c) make the water tasteful           (d) prevent tooth decay

46. The pH value of FeCl₃ solution is likely to be

(a) 3 (b) 9 (c) 7 (d) 11

47. When a metallic oxide reacts with both acids and bases, the oxide is said to be

(a) acidic (b) amphoteric (c) basic              (d) complex

48. The shape of a graphite is(a) tetrahedral (b) pyramidal (c) hexagonal (d) octahedral

49. When a substance changes directly from the gaseous state to the solid state without forming a liquid, the substance is said to

(a) condense (b) evaporate (c) sublime      (d) precipitate

50. The hydrolysis of NH₄Cl gives(a) an acidic solution (b) an alkaline solution (c) a buffer solution (d) a neutral solution

51. Noble gas molecules are held together by(a) van der waals forces (b) hydrogen bonds (c) dative bonds (d) covalent bonds

52. Which of the following phenomena leads to decrease in volume of liquid in an open container?

(a) Brownian motion (b) diffusion (c) evaporation (d) sublimation

53. The solution which has pH > 7 is

(a) FeCl₃ (b) CuSO₄ (c) KNO_3(aq) (d) Na₂CO_{3 (aq)}

54. An aqueous solution of Na₂CO₃ is

(a) acidic (b) alkaline (c) amphoteric          (d) neutral

55. The oxidation number of sulphur in Fe₂(SO₄)₃ is

(a) +2 (b) +3 (c) +4 (d) +6

56. The purity of a solid sample can best be determined by its

(a) boiling point (b) melting point                (c) conductivity (d) solubility

57. An element X with electronic configuration 1s²2s²2p63s²

(a) X₂Y₅ (b) X₂Y₃ (c) XY₃ (d) XY₂

58. The basicity of H₂SO₄ is _________________
59. CFC means ___________________________
60. What is the term used to describe an oxide whose aqueous solution turns blue litmus red?

(a) strong electrolyte (b) acid anhydride      (c) amphoteric oxide (d) basic oxide

61      Which of the following compounds is not a double salt? (a) Zn (oH) N^O₃ (b) KAl (So₄)₂    (c) KCr (So₄)₂ (d) (NH₄) F_e (So₄)₂

62      Which of the following decreases in mass on exposure to air? (a) NaOH (b) Fe (c) FeCl₃ (d) Na₂Co₃.10H₂O

63      The laboratory apparatus used in keeping salts is _____________

64. Fractional distillation of petroleum depends on difference in

(a) molar masses (b) densities (c) rate of diffusion (d) free points

65. Separating funnel is used for separating of mixture of

(a) liquids with different boiling points (b) sediments of a liquid (c) liquids with different colours (d) liquids that are immiscible

66. Which of the following is not a separation technique?

(a) sieving (b) dissolution (c) filtration        (d) sublimation

67. The method used to separate the components of iodine and alom is _________
68. Which of the following represents a noble gas configuration

(a) 2, 8, 8, 2 (b) 2, 8, 2 (c) 2, 8 (d) 2, 6

69. What is the family name of group 7 elements is ___________
70. Na and Na⁺ have the same

(a) chemical properties (b) electrical charge (c) electronic configuration (d) number of proton

71. Which allotrope of carbon is a constituent of a lead pencil?

CLASS: SS 3       SUBJECT:  CHEMISTRY      TIME: 2 HOURS

SECTION A – OBJECTIVES [50MARKS]

Instructions: Answer all questions

1. The atoms of four elements are represented as ₂₀Q, ₁₆R, ₁₀S and ₈ which of the elements would be unreactive A. Q  B. R  C. S  D. T
2. The type of chemical bond that exists between potassium and oxygen in potassium oxide is A. Ionic Metallic C. Covalent   D. Dative
3. Chlorine atom forms Cl^– by A. Losing one electron Sharing one electron  C. Donating one pair of electrons   D. Gaining one electron
4. An element Z has a combining power of 3. Which of the following formulae is correct of its compound A. ZSO₃ Z₃Cl₂  C. Z₂O₃  D. ZS₃
5. The gas evolved when dilute tetraoxosulphate(iv) acid reacts with sodium hydrogentrioxocarbonate(iv) is A. Hydrogen Oxygen
6. Carbon(iv)oxide D. Sulphur(vi)oxide
7. If a solution has a p^H of 2, it can be concluded that it A. Is a weak electrolyte has hydrogen concentration of 0.2moldm^-3 C. Is twice as acidic as a solution of p^H,  D. Will produce effervescence with magnesium ribbon
8. Chemical equilibrium is attained when A. Reactants in the system are used up B. Concentrations of the products are greater than those of the reactants  Concentrations of the reactants and products remain constant  D. reactants stop forming the products
9. An iron nail placed in a solution of copper(ii)tetraoxosulphate(vi) is soon covered with a deposit of copper. Which of the following equations represents the reaction?
10. Fe²⁺_(aq) + Cu(s)   Fe³⁺_(aq)
11. Fe²⁺_(aq) + Cu_(s)      Fe_(s) + Cu²⁺_(aq)
12. Fe_(s) + Cu²⁺_(aq)       Fe²⁺_(aq) + Cu²⁺_(aq)
13. Fe_(s) + Cu²⁺_(aq) Fe²⁺_(aq)
14. Which of the following non-metals reacts most readily with metals? A. Nitrogen Chlorine  C. Sulphur  D. Carbon
15. A radioactive substance is best stored Under paraffin oil  B. Under ultravidet light  C. In a cool, dark cupboard  D. In a box lined with lead

• In the electrolytic extraction of aluminum from puried alumina; molten cryolite is added in order to A. lower the melting point of the alumina

1. Prevent the aerial oxidation of the molten aluminum C. Lower the activation energy of the reaction D. Form a protective  crust on top of the electrolyte

13. When iron rusts, it undergoes A. Deliquescence Chemical decomposition  C. Hydrolysis  D. Redox reaction
14. Which of the following involves the decomposition of a sugar by enzymic action? A. Esterification Fermentation  C. Dehydration
15. Polymerization
16. If a reaction is said to be exothermic, which of the following statements is a correct deduction from the information? The reaction vessel gets hotter as the reaction proceeds  B.  for the reaction is positive  C. The rate of the reaction increases with time  D. The activation energy of the reaction is high
17. A dye s suspected to have contaminated a lollipop. Which of the following is the best method by which the contaminant may be isolated?
18. Fractional distillation B. Recrystallization C. Filtration  D. Paper Chromatography
19. Which of the following accounts for the difference in the mode of conduction of electricity by metals and aqueous salt solutions?
20. Electrons are present in metals but not in salt solutions B. Metals are conducted while salts are electrolytes C. Electricity is carried by mobile electrons in metals but by ions in aqueous  salt solution  D. Salts ionize in aqueous solutions while metals do not.
21. A positive brown ring test indicates the presence of A. NO^–_3­ Fe³⁺
22. D. Cu⁺
23. The following statements about graphite are correct EXCEPT that it A. Is used as a lubricant Has a network structure  C. Contains  mobile free electrons  D. Is a good conductor
24. Which of the following hydrocarbons is unsaturated? A. Ethane
25. Benzene C. Propane D. Z-methylbutane
26. Which of the following is an alloy of mercury? A. Stainless steel Soft solder  C. Coinage bronze  D. Amalgam
27. Metals which react with steam only when they are red-hot include
28. Copper B. Sodium C. Calcium  D. Iron
29. An arrangement of two different metals in aqueous solutions of their salts to produce an electric current is known as A. Electrochemical cell Activity series  C. Thermocouple   D. Volmeter
30. Which of the following exhibits resonance? A. Benzene Butane
31. Pentene D. Octane
32. Which of the following metals will be the most suitable for use where lightness and resistance to corrosion are of important? A. Lead
33. Copper C. Iron D. Aluminum
34. What is the most probable group of an element which is a soft, silvery-white solid and reacts violently with water? A. Group O  Group 1
35. Group 4 D. Group 6
36. Which of the following ions will migrate to the cathode during electrolysis? Zinc ions  B. Chloride ions   C. Suphide ions
37. Tetraoxosulphate(vi)ions
38. Which of the following radioactive decays involve an emission?
39. B. C.
41. The following oxides react with both acids and bases to form salts except A. Zinc oxide Lead (ii) oxide  C. Aluminium oxide   D. Carbon(iv)oxide
42. Which of the following metals is NOT extracted by electrolysis? A. Iron  Sodium  C. Calcium  D. Magnesium
43. Which of the following is an ore of aluminum? A. Haematite
44. Magnetite C. Siderite D. Bauxite
45. Which of the following statements is/are correct about metals? They I. Are good conductors of electricity II. Have mobile electrons III are reducing agent IV. Form acidic oxides I and II only  B. I, II and III only  C. I, II, III and IV   D. None of the above.
46. The main type of reaction that occurs in the blast furnace during the extraction of Iron is A. reduction reaction Decomposition
47. Exothermic reaction D. Combustion
48. Which of the following compounds can be represented by the molecule formula C₂H₆O A. Propanal Ethanol  C. Methanoic acid   D. Glucose
49. The following compounds are hydrocarbons EXCEPT
50. Methylpropanoate B. Z-methylbutane C. Benzene  D. Cyclohexane

36. When alkynes are hydrogenated completely, they produce compounds with the general molecular formula C_nH_n   B. C_nH_2n+2   C. C_nH_2n
37. C_nH_2n-2
38. Which of the following alloys does not contain copper? I. Brass Bronze  III. Steel  A. I only  B. II only  C. III only  D. II and III only
39. The major product in the solvay process is A. NaOH Na₂CO₃  C. NH₃  D. H₂SO₄
40. 100g of radioactive mass has a half-life of 5 days. Calculate the mass decayed off after 15 days. A. 25g 50g   C. 12.5g  D. 6.25g
41. A solution of sodium trioxocarbonate(iv) contains 10.6g in 250cm³ of solution. Calculate the concentration of the solution. A. 0.4moldm^-3
42. 1.0moldm^-3 C. 10.6moldm^-3 D. 25.0moldm^-3
43. The rate of chemical reaction of solids are not affected by A. Catalyst
44. pressure C. Particle size  D. Temperature
45. The energy change that accompanies the addition of an electron to an isolated gaseous atom is A. Bond energy electronegativity  C. electron affinity  D. Ionization energy
46. Which of the following metals could be used as sacrificial anode for preventing the corrosion of iron? A. Copper Lead  C. Magnesium
47. Silver
48. What mass of copper would be formed when a current of 10.0A is passed through a solution of CuSO₄ for 1hour? A. 5.9_g 11.8_g   C. 23.7_g
49. 47.3_g­
50. The volume occupied by 0.4_­­g of hydrogen gas at t.p is A.2.2dm³
51. 4.48dm³ C. 22.4dm³ D. 44.8dm³
52. The oxidation number of Fe in [Fe(CN)₆]^3- is A. +3 +2  C. -2 D. -3
53. Which of the following substances is mainly responsible for the depletion of the ozone layer? A. Oxygen Chlorofluorocarbon  C. Carbon(ii)oxide  D. Nitrogen(ii)oxide
54. Which of the following reactions is common to all hydrocarbons?
55. Combustion B. Addition C. Polymerization  D. Condensation
56. A hydrocarbon compound contains 92.3% carbon. Determine its empirical formula A. CH CH₂  C. CH₃ D. C₂H₃
57. Reduction is the process of A. Loss of electron Loss of hydrogen
58. loss of oxygen D. Addition of electronegative elements

SECTION B – THEORY

Instruction: This section is divided into two parts, answer only two questions from each part.

PART I [ 50 MARKS]

1.(a)   What are nucleons?

(b)   State Graham’s law of diffusion

(c)   Explain briefly why aluminum does not corrode easily

(d)   State THREE examples of periodic properties and their variations in the periodic  table of elements

(e)   State TWO reasons why real gases deviate from ideal gas behave iour

(f)    List THREE uses of fractional distillation in industry

(g)   What factors determine the selective discharge of ions at the electrodes during electrolysis?

(h)  Consider the reaction represented by the following equation

Na₂CO_3(aq) + M_gCl₂           2NaCl_(aq) + M_gCO_3(aq)

2a.     Consider the following atoms

1. State the phenomenon exhibited by the two atoms
2. What is the difference between the atoms?

iii.    Give two examples of elements that exhibit the phenomenon stated in   2(a)(i)

iv     If T is 17, write the electron configuration of the element

b(i)     State two differences between metals and non-metals with respect to their: I. Physical properties              (ii) Chemical properties

b (ii)   Give one example of each of the following compounds

• An amphoteric oxide
• A hydride which evolves hydrogen when reacted with water;
• A trioxocarbonate(iv) salt which is readily decomposed on heating
• A chloride salt which is readily hydrolyzed in water

c(i)     State THREE characteristic properties of transition metals

(ii)      Write the electro configuration of ₃₀Zn

(iii)     Explain briefly why zinc is not considered as a typical transition element

3(ai)   State Graham’s Law of diffusion

(aii)  If 100cm³ of oxygen diffused in 4seconds and 50cm³ of gas Y diffused in 3 seconds, Calculate the relative molecular mass of gas Y

(b)      Consider the following equilibrium reaction:

X_(g)+2Y_(g                 XY_2(g)­  = -52KJmol^-1

1. i) State what happens to the yield of XY₂ when the temperature is increased

(ii)      Explain the effect of decrease in pressure on the equilibrium position

(iii)     State the effect of a catalyst on the

1. Position of equilibrium
2. Activation energy

c.(i)    State two differences between the solubilities of solids and gases in liquids

c.(ii)   Name the physical  properties used in choosing separation techniques for the following mixtures I. Kerosene and Petrol II. Calcium trioxocarbonate (iv) and potassium chloride III. Ammonium chloride and sodium chloride

d(i)     State a method of preparing each of the following salts;

1. Sodium Chloride
2. Lead (II) Trioxocarbonate (iv)

• Iron (ii) Chloride

1. Copy and complete the table below

Acid                      Basicity

H₃PO₄

CH₃COOH

HNO₃

D(i)    State the difference between analydrous and hydrated salts

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