- 1. The hydrolysis of proteins by diluting mineral acids produces
A) sucrose
B) amino acids
C) glucose
D) fatty acids
- 2. Which of the following oxide causes acid rain?
A) H2O2
B) NO2
C) CO
D) NO
- 3. The ratio of carbon atoms of hydrogen atoms in a hydrocarbon is 1:2. If its molecular mass is 56, what is its molecular formula?
A) C2H4
B) C4H8
C) CH2
D) C3H6
- 4. What is the relative molecular mass of the compound below?
A) 64
B) 59
C) 136
D) 137
- 5. Cathodic protection of metals is based on
A) relative tendencies of oxidation
B) nature of oxides formed
C) standard electrode potential of hydrogen
D) its electrical conductivity
- 6. If humid air is polluted by chlorine discharged, the air can be restored by sprinkling
A) acidified KMnO4
B) acidified FeSO4
C) solid MnO2
D) saturated NaCl(aq)
- 7. The alkanol represented by the structure above is
A) secondary and monohydric
B) secondary and dihydric
C) primary and dihydric
D) tertiary and dihydric
- 8. Which of the following pairs of compounds would form a precipitate when their aqueous solutions are mixed?
A) KCl and NaNO3
B) NH4NO3 and Na2CO3
C) NaCl and KNO3
D) K2SO4 and BaCl2
- 9. Study the graphs below (I, II, III, IV) and use them to answer questions 9 to 11.
Which of the graphs illustrates the variation of the rate of evolution of a gas from a given length of magnesium ribbon (y-axis) with increase in the concentration of the acid added (x-axis)?
A) II
B) IV
C) III
D) I
- 10. Study the graphs below (I, II, III, IV) and use them to answer questions 9 to 11.
Which of the graphs illustrates the variation of the pH of a given volume of strong acid solution (y-axis) with the volume of strong base titrated against it (x-axis)?
A) I
B) IV
C) II
D) III
- 11. Study the graphs below (I, II, III, IV) and use them to answer questions 9 to 11.
Which of the graphs illustrates the variation of the solubility of a salt in water (y-axis) with increase in temperature (x-axis), if the dissolution process is exothermic?
A) IV
B) II
C) I
D) III
- 12. The formation of ethene from dehydration of ethanol can be described as
A) an addition reaction.
B) an elimination reaction.
C) an oxidation reaction.
D) a substitution reaction.
- 13. Which of the following gases is highly soluble in water at room temperature?
A) Carbon (IV) oxide
B) Chlorine
C) Nitrogen
D) Ammonia
- 14. A molecule of phosphorus is
A) a monoatomic.
B) a triatomic.
C) a diatomic.
D) a tetraatomic.
- 15. The most common method of preparing insoluble salts is by
A) decomposition.
B) neutralization.
C) filtration.
D) double decomposition.
- 16. What number of moles of oxygen would exert a pressure of 10 atm at 320K in an 8.2dm³ cylinder? [R=0.082 atm dm³mol⁻¹K⁻¹]
A) 1.56
B) 3.13
C) 31.25
D) 0.32
- 17. The basic property of salts used as drying agents is
A) hygroscopy.
B) high melting point.
C) low solubility.
D) efflorescence.
- 18. What would be observed when aqueous ammonia is added in drops and then in excess to a solution of copper (II) ions?
A) A blue precipitate is formed which is soluble in excess ammonia
B) A green precipitate is formed which is insoluble in excess ammonia
C) A white precipitate is formed which is soluble in excess ammonia
D) A brick red precipitate is produced which is insoluble in excess ammonia
- 19. When CuSO4(aq) is added to Pb(NO3)2(aq),
A) a white precipitate would be formed.
B) the resulting solution would become colourless.
C) a blue precipitate would be formed.
D) there would be no visible change.
- 20. Consider the structure below (a carbon chain with -OH, a C2H5 branch, and a C=O group). How many carbon atoms does the parent chain contain?
A) 4
B) 5
C) 3
D) 2
- 21. Under which conditions of pressure (P) and temperature (T) would the volume of an inflated balloon increase? When
A) both T and P are increased
B) both T and P are decreased
C) T is increased and P is decreased
D) T is decreased and P is increased
- 22. The collision between ideal gas molecules are considered to be perfectly elastic because
A) their average kinetic energy is variable.
B) they move randomly in straight lines.
C) they collide without losing energy.
D) the distance between them is large compared to their sizes.
- 23. Elements with high ionization energies would
A) have high effective nuclear charges.
B) lose electrons easily.
C) have low atomic numbers.
D) have large atomic radii.
- 24. Which of the following statements about Group VII elements is correct?
A) They exist as monoatomic molecules
B) They are strong reducing agents
C) Their reactivity decreases down the group
D) They are present in the same physical state
- 25. Consider the diagram below and use it to answer questions 25 and 26 (electrochemical cell with crystals A and B, A(aq)3+ and B(aq)2+).
Which of the following cell notations represent the diagram?
A) B/B2+//A/A3+
B) A/A3+//B2+/B
C) A3+/A//B/B2+
D) B2+/B//A/A3+
- 26. Consider the diagram below and use it to answer questions 25 and 26 (electrochemical cell with crystals A and B, A3+ (aq) and B2+ (aq).
Which of the following half reaction equations represent the reaction at the cathode?
A) A3+(aq)+3e⁻→A(s)
B) B2+(aq)+2e⁻→B(s)
C) B(s)→B2+(aq)+2e⁻
D) A(s)→A3+(aq)+3e⁻
- 27. The reactivity of fluorine is high because of
A) its high electronegativity.
B) the availability of d-orbitals.
C) the small size of the fluorine atom.
D) the strong F-F bond.
- 28. How many coulombs of electricity would liberate 1.08g of Ag from a solution of silver salt? [Ag=108.0; 1F=96500C]
A) 96500C
B) 9.65C
C) 9650C
D) 965C
- 29. The Bohr model of the atom proposed
A) nucleons.
B) electron shells.
C) neutrons.
D) the existence of the nucleus.
- 30. At 25°C, evaporation of a 100cm³ solution of K2CO3 to dryness gave 14g of the salt. What is the solubility of K2CO3 at 25°C? [K2CO3=138]
A) 10.0 mol dm⁻³
B) 0.01 mol dm⁻³
C) 0.101 mol dm⁻³
D) 1.01 mol dm⁻³
- 31. Student X titrated 25cm³ of Na2CO3 with 0.1mol dm⁻³ HCl, using methyl orange as indicator. Student Y carried out the same exercise but used phenolphthalein as indicator. Which of the following statements about the titration is true?
A) Hydrogen chloride gas was released in the reactions in both titrations
B) The titre values obtained from the titrations are equal
C) The titre value obtained by Y is twice that of X
D) The titre value obtained by X is twice that of Y
- 32. What is the concentration of a solution which contains 0.28g of potassium hydroxide in 100cm³ of solution? [KOH=56]
A) 0.05 mol dm⁻³
B) 0.50 mol dm⁻³
C) 0.10 mol dm⁻³
D) 0.01 mol dm⁻³
- 33. What is the empirical formula of a hydrocarbon containing 0.160 moles of carbon and 0.640 moles of hydrogen?
A) CH2
B) CH3
C) C2H4
D) CH4
- 34. Which of the following species has the largest ionic radius?
A) Ca2+
B) S2-
C) Cl-
D) K+
- 35. Which of the following statements is correct about ionization energy? It
A) results in the formation of an anion
B) decreases down the group
C) decreases across the periods
D) causes metallic nuclei to disintegrate
- 36. Potassium trioxonitrate (V) can be obtained from its solution by
A) distillation.
B) crystallization.
C) evaporation.
D) filtration.
- 37. An element, Q, contains 69.0% of 63Q and 31% of 65Q. What is the relative atomic mass of Q?
A) 63.6
B) 63.0
C) 69.0
D) 65.0
- 38. The following ions have the same electron configuration except ____
A) Mg2+
B) Al3+
C) O2-
D) Cl⁻
- 39. The region around the nucleus where electrons can be located is called
A) a spectra.
B) a quanta.
C) an orbital.
D) a field.
- 40. Protons and electrons are called fundamental particles because they
A) are the lightest particles.
B) are found in all matter.
C) have different charges.
D) are indivisible.
- 41. Consider the following energy profile diagram (Potential Energy vs Reaction Co-ordinates) and use it to answer questions 41 to 43.
The activation energy of the reaction is
A) ED
B) EA
C) EB
D) EC
- 42. Consider the following energy profile diagram (Potential Energy vs Reaction Co-ordinates) and use it to answer questions 41 to 43.
The enthalpy change of the reaction is
A) EC
B) EA
C) EB
D) ED
- 43. Consider the following energy profile diagram (Potential Energy vs Reaction Co-ordinates) and use it to answer questions 41 to 43.
The energy profile diagram illustrates
A) a spontaneous reaction.
B) a redox reaction.
C) an exothermic reaction.
D) an endothermic reaction.
- 44. How many molecules of oxygen would occupy a volume of 2.24cm³ at s.t.p.?
[Molar volume at s.t.p.=22,400cm³;
Avogadro's number = 6.02×10²³]
A) 6.02×10¹⁹
B) 3.01×10²¹
C) 3.01×10²⁰
D) 6.02×10²⁷
- 45. The relationship between x, y and z is
A) xy<z.
B) x<z<y.
C) x>y>z.
D) x=y=z.
- 46. Which of the following pairs of molecules form hydrogen bonds?
A) NH3 and SO2
B) H2S and CH4
C) C2H5OH and CH3OH
D) C6H6 and Br2
- 47. Which of the following statements about elements in Group VII is correct?
A) Br will oxidize Cl⁻
B) F2 has the least tendency to be reduced
C) Cl2 will oxidize I⁻
D) I2 is a stronger oxidizing agent than F2
- 48. Electrovalent compounds normally
A) conduct electricity in the solid state.
B) have low boiling points.
C) have mobile electrons.
D) dissolve in polar solvents.
- 49. A coordinate covalent bond could be formed between
A) NH3 and PCl3.
B) BCl3 and NH3.
C) H+ and AlCl3.
D) BCl3 and AlCl3.
- 50. Which of the following scientists discovered the electron?
A) Joseph J. Thompson
B) Ernest Rutherford
C) Amedeo Avogadro
D) James Chadwick
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