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CHEMISTRY (Objective Questions And Answers)


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THEORY QUESTIONS
WAEC SYLLABUS

WASSCE 2013

Objectives



1. Which of the following instruments is used in detecting the presence of radiation?

A. Cathode ray tube

B. Geiger-Muller counter

C. Mass spectrometer

D. X-ray tube


2. The molecule which has a linear shape is

A. CH4

B. NH3

C. H2S

D. C02.


3. The formula of the compound formed between a trivalent metal, M and a divalent non-metal, Y is

A. M2Y3

B. M3Y2

C. MY

D. M3Y.


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

A. X+

B.X2+

C.X2-

D. X


5. Which of the following statements is correct?

A. Atomic size decreases down the group

B. Atomic size increases across the period

C. Anions are smaller than the parent atom

D. Cations are smaller than the parent atom


ANSWERS

6. Which of the following arrangements represents the correct order of electronic energy level?

A. IS 2P 2S 3P 3S 3D 4S

B. IS 2S 2P 3S 3P 3D 4S

C. IS 2S 2P 3S 3P 4S 3D

D. IS 2S 3S 2P 3P 4S 3D


7. The element with electron configuration IS2 2s2 2PF 3s2 3P1 belongs to

A. s - block, period 3, group 1

B. P - block, period 3, group 2

C. s - block, period 3, group 3

D. P - block, period 3, group 3


8. In the periodic table, all the elements within the same group have the same

A. number of neutrons

B. number of valence electrons

C. number of isotopes

D. atomic number


9. Which of the following halogens is liquid at room temperature?

A. Iodine

B. Chlorine

C. Bromine

D. Fluorine


10. Rare gases are stable because they

A. are chemically active

B. contain equal number of protons and neutrons.

C. contain more electrons than protons

D. have octet structures


ANSWERS

11. In the periodic table, alkaline earth metals can be found in group

A. I

B. ll

C. VI

D. VII


12. In which of the following scries are the atoms arranged in order of increasing ionization energy?

A. Li, Na, K

B. B, Be, Li

C. O, F, Ne

D. Be, Mg, Ca


13. Which of the following bond types is responsible for the high boiling point of water?

A. Metallic bond

B. Covalent bond

C. Ionic bond

D. Hydrogen bond


14. In metallic solid, the forces of attraction is between the mobile valence electrons and the

A. atoms

B. neutrons

C. negative ions

D. positively charged nuclei


15. The bonds in crystalline ammonium chloride are

A. covalent and dative

B. ionic and covalent

C. ionic, covalent and dative

D. ionic, covalent and hydrogen bond


ANSWERS

16. Which of the following elementslis diatomic?

A. Sodium

B. Oxygen

C.Iron

D. Neon


17. Noble gas molecules are held together by

A. van der Waals feces

B. hydrogen bonds

C. dative bonds

D. covalent bands


18. Which of the following statements about nuclear reaction is correct? The reaction

A. involves neutrons only

B. takes place inside the nucleus

C. is governed by temperature and pressure

D. involves protons and electrons only


19. Consider the reaction represented by the following equation: C2H2 + yH2 ----» C2H6. The value of y in the reaction is

A. 4

B. 3

C. 2

D. 1.


20. The volume of 0.25 MOLDNR3 solution of KOH that would yield 6.5 G of solid KOH on evaporation is [K = 39.0 0 = 16.0 H= 1.00]

A. 464.30 cm3

B. 625.00 cm3

C. 1000.00cm3

D. 2153.80cm3


ANSWERS

21. The percentage by mass of calcium in Ca(OCI)2 is [ Ca = 40.0 CI = 35.5 0= 16.0]

A. 28.0%

B. 31.6%

C. 43.8%

D. 44.5%.


22. The gas law which describes the relationship between volume and temperature is

A. Boyle's law

B. Charles' law

C. Dalton's law

D. Graham's law


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

A. Brownian motion

B. Diffusion

C: Evaporation

D. Sublimation


24. The pressure exerted by a gas is a function of the

A. total volume of the gas.

B. speed of the gaseous molecules. \

C. mass of each gaseous molecule.

D. frequency of collision between gaseous molecules.


25. Which of the following gases are arranged in increasing order of diffusion rate? [ H = 1.0 C = 12 N = 14 O = 16 S = 32 ]

A. S02,02, NH3, H2

B. H2S,NH2,02,S02

C. C02, N20, 02, S02

D. NH3, N02, N2, C02


ANSWERS

26. Which of the following variables is a measure of the average kinetic energy of the molecule of a gas?

A. Density

B. Pressure

C. Temperature

D. Volume


27. When heat is absorbed during a chemical reaction, the reaction is said to be

A. adiabatic

B. endothermic

C. exothermic

D. isothermal


28. The aqueous solution which has pH > 7 is

A. FeCI3(aq)

B. CuS04(aq)

C. KN03(aq)

D. Na2C03(aq)


29. Which of the following acids would readily react with CaC03 to liberate C02?

A. CH3COOH

B. H2S04

C. H2S03

D. HN03


30. Which of the following compounds crystallizes without water of crystallization?

A. MgS04

B. Na2C04

C. NaCI

D. FeS04


ANSWERS

31. A substance is said to be impure if

A. its melting point range is wide

B. it dissolves in water with difficulty

C. it has a Low melting point

D. it is coloured


32. The following factors affect the solubility of a solid in a given solvent except

A. nature of solute

B. nature of solvent

C. pressure

D. temperature


33. Consider the reaction represented by the equation: N2O4(aq) <=====> 2N02(g) AH = +xkJmol-1 What happens when the temperature is reduced at equilibrium?

A. Concentration of N204(g) decreases

B. Concentration of N2O4(g) increases

C. Pressure exerted by the gases increases

D. Pressure exerted by the gases remains constant


34. Which of the following cells produce electrical energy from chemical reactions? I. Lead-acid battery? II. Dry cell III. Daniell cell IV. Electrolytic cell

A. I and II only

B. I, II and III only

C. II, III and IV only

D.I, III and IV only


35. What happens at the cathode during electrolysis? The

A. anion is oxidized

B. anion loses electrons

C. cation is oxidized

D. cation is discharged.


ANSWERS

36. Which of the following substances are electrolytes? I. PbBr2(/) II. NaCI(aq) III. NaCl(s) IV C6H1206(aq)

A. I and II only

B. I, II and IV only

C. Ill and IV only

D. I and III only


37. Consider the redox reaction as represented by the following equation: I2(aq) + 2S2O32- (aq) 2I- (aq) + Which of the species in the equation is reduced?

A. S4O62- (aq)

B. S2O32- (aq)

C. I2(aq)

D. I- (aq)


38. The separation of petroleum fractions depends on the differences in their

A. melting points

B. molar masses

C. solubilities

D. boiling points.


39. The major product formed by the reaction between ethanoic acid and aqueous sodium hydroxide is

A. soap

B. sodium ethanoate

C. sodium methoxide

D. water.


40. Which of the following organic compounds would decolourize bromine water?

A. Benzene

B. Cyclobutane

C. Hexane

D. Pentane


ANSWERS

41. How many isomers has C3H6Cl2?

A.2

B. 3

C. 4

D. 5


42. The IUPAC name of the compound (CH3)2CHCH2CHOOH is

|

NH2

A. 2 - amino hexanoic acid

B. 2 - amino -4 - methyl pentanoic acid

C. 2, 4 - dimethyl butanoic acid

D. 4 - amino pentanoic acid.


43. Which of the following reactions is common to all hydrocarbons?

A. Combustion

B. Addition

C. Polymerization

D. Condensation


44. A hydrocarbon compound contains 92.3% carbon. Determine its empirical formula. [H=1.00 C=12.0J

A. CH

B. CH2

C. CH3

D. C2H3


45. The main function of limestone in the blast furnace is to

A. act as catalyst

B. act as a reducing agent

C. remove impurity

D. supply carbon (IV) oxide


ANSWERS

46. Which of the following raw materials is used in a plastic industry?

A. E'hene

B. Methane

C. Calcium

D. Hydrogen


47. Which of the following statements about thermoplastic materials is correct? They

A. do not melt on heating

B. harden on heating

C. decompose on heating

D. soften and melt on heating


48. Bronze is a mixture of

A. Cu and Mg

C. Cu and Zn

B. Cu and Sn

D. Cu and Pb


49. Which of the following statements about fine chemical is correct? It

A. is injurious to health

B. has low degree of purity

C. is produced in relatively small amount.

D. can be stored for a long time


50. Which of the following materials is classified as a non-biodegradable pollutant?

A. Animal hide

B. Paper

C. Plastic

D. Wood



WASSCE JUNE 2013 CHEMISTRY OBJECTIVE TEST

ANSWERS

​1. B 2. D 3. A 4.C 5.D 6.C 7.D 8. B 9. C 10.D

11. B 12. C. 13. D 14. 15. 16. B 17. A 18. B 19. B 20. A

21. A 22. B. 23. C 24. D 25. A 26. C 27. B 28. D 29. D 30. C

31. A 32. C 33. B 34. B 35. D 36. A 37. D 38. D 39. B 40. C

41. 42. 43. A 44. A 45. C 46. A 47. D 48. B 49. C 50. C


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