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WAEC past questions and answers on Chemistry 2022 [Objective Test – Paper 1]

Instruction: Answer all the questions. Do all rough work on this question paper

  1. The by-product of fermentation of sugar is
    • A. carbon(IV) oxide
    • B. ethanoic acid
    • C. propanol.
    • D. propan-1,2,2- triol.
  2. Which of the following sugars is a product of the condensation of monosaccharides?
    • A. Galactose
    • B. Maltose
    • C. Glucose
    • D. Fructose
  3. The cleaning effect of soap is low in acidic water because of
    • A. the formation of unionized fatty acid.
    • B. increase in the pH of the soap molecules.
    • C. anti-biodegradable effect of hydrogen ions
    • D. the hardness of the acidic water.
  4. The following compounds are condensation polymers except
    • A. nylon
    • B. protein
    • C. starch
    • D. polyethene
  5. What amount of electricity is required to deposit one mole of aluminium from a solution of AlCl3?
    • A. One Faraday
    • B. One sampere
    • C. Three Faradays
    • D. Three amperes
  6. Which of the following compounds would react rapidly with bromine?
    • A. Benzene
    • B. Hexane
    • C. Hexene
    • D. Hexanol
  7. Alkanols can be manufactured from alkenes by the initial reaction of alkenes with
    • A. bromine in tetrachloromethane
    • B. concentrated tetraoxosulphate (VI) acid.
    • C. aqueous potassium tetraoxomanganate (VII)
    • D. sodium hydroxide solution
  8. Which of the following statements about the standard hydrogen electrode is not correct?
    • A. The hydrogen gas is at a pressure of 1 atmosphere
    • B. A solution containing 1 mol dm-3 of H+(aq) ions is used
    • C. A platinum electrode is used
    • D. The temperature is kept at 200C
  9. If 60g of M combines with 24g of oxygen, what would the empirical formula of the oxide be? [0 = 16.0, M = 120]
    • A. MO
    • B. MO2
    • C. MO3
    • D. MO4
  10. The products of the electrolysis of dilute sodium chloride using carbon electrodes are Anode/Cathode
    • A. chlorine and sodium
    • B. oxygen and hydrogen
    • C. chlorine and hydrogen
    • D. hydrogen and oxygen
  11. Determine the quantity of electricity used when a current of 0.20 amperes is passed through an electrolytic cell for 60 minutes.
    • A. 12 C
    • B. 120 C
    • C. 360 C
    • D. 720 C
  12. Oxochlorate (I) acid is used as a bleaching agent because it is
    • A. a weak acid
    • B. a reducing agent
    • C. an oxidizing agent
    • D. a strong acid
  13. The IUPAC name for CH3CHCH3CHCLCHCH3CH2CH3 is
    • A. 2, 4 – dimethyl – 3 – chlorohexane
    • B. 3, 5 – dimethyl – 4 – chlorohexane
    • C. 4 – chloro -3, 5 – dimethylhexane
    • D. 3 – chloro -2, 4 – dimethylhexane.
  14. A colourless gas with a pungent smell is evolved when dilute hydrochloric acid is added to a sample of a salt. The gas evolved could turn
    • A. acidified K2Cr2 O7 solution colourless
    • B. acidified KMnO4 solution colourless
    • C. Fe(NO3)2 solution green
    • Pb(NO3)2 paper black
  15. If 5.0g of marble reacts with 25.0cm3 hydrochloric acid, which of the following combination has the fastest reaction rate?
    • A. Marble chips and 2.0 mol dm-3 HCL(aq)
    • B. Marble chips and 2.0 mol dm-3 HCL(aq)
    • C. Powered marble and 2.5 mol dm-3 HCL(aq)
    • C. Powered marble and 2.0 mol dm-3 HCL(aq)
  16. Increasing the temperature generally
    • A. decreases the solubility of a solid in a liquid but increases the solubility of a gas in a liquid
    • B. increases the solubility of a solid in a liquid but decreases the solubility of a gas in a liquid
    • C. increases the solubility of both a solid and gas in a liquid
    • D. decreases the solubility of both a solid and a gas in a liquid.
  17. A white precipitate was formed when BaCl2(aq) was added to an aqueous solution of a salt X. The precipitate dissolved in dilute HCL with rapid effervescence. Salt X is likely to contain
    • A, SO42- ions
    • B. SO32- ions
    • C. NO3ions
    • D. CO32- ions
  18. Before a reaction could take place, the should be
    • A. ionization of reactant particles
    • B. breakage of bonds of products
    • C. breakage of bonds of reactants
    • D. ionization of product particles
  19. Consider the following reaction equation: CaO + SiO2 → CaSiO3 Silicon(IV) oxide is acting as
    • A. a basic oxide
    • B. a reducing agent
    • C. an acidic oxide
    • D. an oxidizing agent
  20. Which of the following acids would form normal salt only?
    • A . Tetraoxosulphate (IV) acid
    • B. Trioxonitrate (V) acid
    • C. Tetraoxophosphate (V) acid
    • D. Trioxosulphate (IV) acid
  21. What is the partial pressure of oxygen at s.t.p. in a gaseous mixture containing 100cm3 of oxygen and 900 cm3 of nitrogen gas?
    • A. 1.0 atm
    • B. 0.1 atm
    • C. 9.0 atm
    • D. 0.9 atm
  22. Graphite is used as a dry lubricant due to the presence of
    • A. mobile electrons
    • B. free electrons
    • C. octahedral structures
    • D. layered structures
  23. Which of the following gases is alkaline?
    • A. NO2
    • B. CO2
    • C. NH3
    • D. N20
  24. Which of the following statements about an equilibrium system is correct?
    • A. Forward and backward reactions occur at the same rate.
    • B. The concentrations of reactants must equal that of the products
    • C. The concentrations of reactants and products can be changes by adding a catalyst.
    • D. The concentrations of reactants and products are not affected by a change in temperature.
  25. Consider the following reaction equation: N2(g) + 3H2(g) ⇌ 2NH3(g); H = -92kJ. Increasing the temperature of the reaction would
    • A. Shift the equilibrium to the right
    • B. increase the yield of ammonia.
    • C. decrease the amount of hydrogen
    • D. decrease the yield of ammonia.
  26. When air in a syringe is compressed such that there is no change in temperature, the
    • A. air liquefies
    • B. pressure increases
    • C. intermolecular space increases.
    • D. density decreases
  27. Which of the following statements about liquids is/are true? I.) Liquids maintain their volume at constant temperature. II.) Liquids have fixed shape. III.) Liquids do not diffuse. IV.) Change in pressure affects volume of liquids.
    • A. I only
    • B. IV only
    • C. I and IV only
    • D. II and III ONLY
  28. A hydrogen chloride gas reacted with oxygen gas to yield water and chloride gas. The mole ratio of the hydrogen chloride gas to water is
    • A. 1:3
    • B. 2:1
    • C. 3:1
    • D. 4:1
  29. What number of moles of oxygen would exert a pressure of 10 atm at 320 K in an 8.2 dm3 cylinder? [R = 0.082 atm dm-3 mol-1 K-1]
    • A. 0.32
    • B. 1.52
    • C. 3.13
    • D. 31.25
  30. If 50cm3 of a saturated solution of KN03 at 40OC contained 5.05g of the salt, its solubility at the same temperature would be [KNO3 = 101]
    • A. 1.0 mol dm-3.
    • B. 1.5 mol dm-3.
    • C. 2.0 mol dm-3.
    • D. 5.0 mol dm-3.
  31. Which of the following elements would displace copper from a solution of copper ions?
    • A. Silver
    • B. Gold
    • C. Lead
    • D. Mercury
  32. What is the percentage composition of carbon in Ca(HCO3)2? [ Ca = 40.0, O = 16.0, C = 12.0, H = 1.0]
    • A. 22.2 %
    • B. 14.8 %
    • C. 7.4 %
    • D. 3.7 %
  33. Which of the following bond types is intermolecular?
    • A. Covalent bond
    • B. Hydrogen bond
    • C. Ionic bond
    • D. metallic bond
  34. The maximum number of covalent bonds formed by nitrogen is
    • A. 1.
    • B. 2.
    • C. 3.
    • D. 4
  35. The IUPAC name of the compound CH3CH(CH3)CHCH2 is
    • A. 2 – methyl but – 1 – ene
    • B. 2 – methyl but – 2 – ene
    • C. 3 – methyl but – 1 – ene
    • D. 3 – methyl but – 2 – ene
  36. Ionization energy increases across the period in the periodic table because
    • A. atomic number increases.
    • B. effective nuclear charge increases.
    • C. mass number decreases
    • D. screening effect decreases.
  37. Which of the following properties indicate that an element is a metal. It (I) reacts with oxygen to form an acidic oxide. (II) forms ionic chlorides. (III) has variable oxidation states. (IV). displaces hydrogen from dilute HCL.
    • A. I and III only
    • B. I and II only
    • C. II and IV only
    • D. I, II, III and IV
  38. The electron configuration of carbon atom in its excited state is
    • A. 1s22s22px22Py0
    • B. 1s22s22px12py1
    • C. 1s22s12px12py12pz1
    • D. 1s12s22px12py12pz1
  39. An oxide has the following properties. It (I). is a white powder. (ii) react with HCL. (III) reacts with NaOH (IV) in insoluble in water. The oxide is
    • A. alkaline
    • B. amphoteric
    • C. acidic
    • D. nuetral
  40. Which of the following statement about atoms of a metal is correct? They
    • A. readily accept electrons
    • B. are soft
    • C. are held together by covalent bond
    • D. are held together by a sea of electron cloud
  41. Which of the following sketches is a graphical representation of Boyle’s law?
  42. The atom with the electron configuration 1s22s22p63s23p63d104s24p4 is in
    • A. period 4, p- block
    • B. period 3, p- block
    • C. period 4, d-block
    • D. period 3, d-block
  43. Electropositivity of elements across the periodic table normally
    • A. remains constant down the group
    • B. increases across the period
    • C. decreases across the period
    • D. decreases down the group
  44. Consider the following table
SubstanceMelting point/ 0CBoiling point/OC

Which of the substances is a liquid at room temperaturw and rapidly evaporates on exposure to air?

  • A. P
  • B. Q
  • C. R
  • D. S
  • 45. Which of the following oxides is amphoteric?
    • A. Carbon (II) oxide
    • B. Nitrogen (IV) oxide
    • C. Lead (II) oxide
    • D. Calcium oxide
  • 46. Which of the following processes occur during fractional distillation of petroleum?
    • A. Condensation and diffusion
    • B. Diffusion and evaporation
    • C. Diffusion and sublimation
    • D. Evaporation and condensation
  • 47. If the molar mass of X(HCO3)2 is 162g mol-1, determine the relative atomic mass of X. [H = 1.0, C = 12.0, O = 16.0]
    • A. 40
    • B. 48
    • C. 61
    • D. 101
  • 48. Charcoal is used in the decolourization of sugar because of its
    • A. absorption property
    • B. amorphous property
    • C. oxidizing property
    • D. adsorption property
  • 49. The first defination of an element was made by
    • A. J. Dalton
    • B. A. Lavoisier
    • C. R. Boyle
    • D. J. J. Thompson
  • 50. Which of the following scientists formulated the law of conservation of mass?
    • A. A. Lavoisier
    • B. J. Dalton
    • C. R. Boyle
    • D. J. Proust
OBJECTIVE ANSWERS [WAEC past questions and answers on Chemistry 2022]


THEORY ANSWERS [WAEC past questions and answers on Chemistry 2022]

Question 1

(a) (i) An electron electron pair acceptors [2marks]

(ii) AlCl3, BCl3, H2O, H+, Transition metal ions [1mark]

(1a) (i) An electron electron pair acceptors [2marks]
(ii) AlCl3, BCl3, H2O, H+, Transition metal ions [1mark]

(1b) Is the addition of NaCl (1) to the reaction mixture (1) in soap production to facilitate the precipitation of soap (1) from the mixture [3marks]

Reagent – AgNO3 in NH3(aq) / Ammoniacal silver trioxonitrate (v)
Condition – Heat [2marks]

(1d) Is the fraction of a given isotope (1) in a mixture of isotopes of the same element (1) OR
The % of an isotope with a specific atomic mass (1) found in a naturally accruing sample of an element (1).

(1e) (i) because the element is/has

  • unreactive
  • stable
  • inert
  • a noble gas
  • completely filled outermost shell

(ii) Because of a weak forces between the molecules (1) hence not much heat (1) is needed to break the forces (1) [3marks]

  • (1f)
  • (Conc) HNO3 produces brown fumes (1) (of NO2) when copper tunings are added (1) to it / copper (II) salt is added but H2S04 will not react with the copper tuning / copper (II) salt (1).
  • When Concentrated H2SO4 is added to sugar (1) it chars (1) the sugar but Concentrated HN03 will not (1)
  • Add BaCl2 solution to each acid (1) white precipitate indicates H2SO4 (1) no precipitate indicates HNO3 (1) Any 1 x 3 = 3marks

(1g) Any 2 x 1 = 2marks

Electrochemical cellElectrolytic cell
– the node is negative/ cathode is positive– anode is positive / cathode is negative
– chemical energy is converted to electrical energy– electrical energy is converted to chemical energy
– the two half cells are in separate containers and connected by a salt bridge– the two half cells are in the same container
– reaction is spontaneous– non-spontaneous
– current is generated from within the cell– current is generated from external source / battery
[WAEC past questions and answers on Chemistry 2022]

group 1 element reacts by forming positive ions, the higher the ionization energy, the more difficult it is to lose the electron hence the lower the reactivity of the element. OR

Ionization energy decreases down group 1 elements, the lower the ionization energy, the easier to loose an electron, hence the higher the reactivity of the elements. [3marks]

(1i) Molecular formula shows the actual number of atoms of each element in a molecule. [2marks]

(1j) (i)

(1j) (i) NH₃ will deviate more [1mark]
(ii) This is because it has a larger volume and also it has a stronger intermolecular forces. [2marks]

Question 2

Ionization energy can be defined as the energy required to remove one electron from a mole of a gaseous atom. OR

Is the minimum energy required to convert one mole of a gas of atom into one mole of a gaseous plus 1 ions. [2marks]

2aii) 4Be : 1s2 2s2
5B: 1s2 2s2 2p1 The electron to be removed from Be is in the 2s orbital which is closer to the nucleus; nuclear attraction is greater hence first ionization energy is greater but the electron to be removed from B is in the 2p orbital which is farther away from the nucleus; hence nuclear attraction is weaker; hence first ionization energy is smaller. OR 2p has less energy than 2s (1). So it is easier to remove an electron from 2p (1) as the nuclear charge is weaker in 2p (1) because 2p is further away from the nucleus (1). Hence, first ionization energy is small. 4marks

I = 0.12A, t = 500seconds, Q = It, Q = 0.12 x 500 = 60C
m = 0.015g, 1 F =96500C
M = 48.0, Charge = ?
m = MIt/CF
C = MIt/mF
C = (48×0.12×500)/(0.015×96500) Hence charge = +2

(2ci) Alumina (Al2O3) mixed with molten cryolite (Na3AlF6)

(i) Abundant deposits of bauxite
(ii) Cheap source of electricity

2d) (i) Is the ability of a substance to be attracted strongly into a magnetic field. [2marks]

(i) ₂₄Cr²⁺ – 1s22s22p63s23p63d4 unpaired electron = 4
₂₄Cr⁶⁺ – 1s22s22p63s23p6 = unpaired electrons = 0

(ii) ₂₄Cr²⁺

(iii) the greater the number of unpaired electrons in the 3d – orbital (1), the greater the paramagnetism (1)


This can be defined as the number of particles (atoms, molecules, ions etc) present in one mole of a substance. OR Number of particles present in 12.0g of carbon – 12

Mass/m.m = no. of molecules/Avogadro’s number
(2.30/m.m) × (3.01×10²²/6.02×10²³)
m.m = (2.30×6.02×10²³)/3.01×10²²
m.m = 46g/mol

Let Nx Oy be the formula of the oxide or 14x + 16y = 46
:. x = 1, y = 2
ie. 14(1) + 16(2) = 46
:. formula of x = NO2

(i) Two layers are formed / no reaction / immiscible
(ii) There is a reaction / hydrolysis (1) with steamy fumes / white fumes

The reaction occurs by interaction of the lone pair of electrons of water binding to the central atom (1) (silicon or carbon) / attaching to the central atom. In silicon, the 3d – orbital is available to accept the pairs of electrons (1) but in carbon there is no vacant orbitals for bonding (1). OR Water is pola (1) hence the reaction with SiCl4 (1). But CCl4 is non polar (1) hence there is no reaction.

  • (3ci)
  • Extraction of copper
  • Electroplating
  • Purification of metals / copper

(i) CuSO₄
(ii) CuCl2(aq) (iii) Cu(NO3)2

Cu(s) → Cu²⁺(aq) + 2e⁻(aq)

Using; m = ZIt, t = 3min, 13 sec, = 193 sec
Z = m/It
Z = 3.2/(50×193)
Z = 3.2/9650
Z = 0.000332g/C


Temperature : 350 – 5000C/high temperature
Pressure : 150 – 1000 atm / high pressure
Catalyst: (Finely divided) Iron

Rate of the reaction increases (1) as particles are closer together / more particles per unit volume (1). There are more collision per second / collisions are more often

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