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1. Which of the following substances is an example of a fine chemical?
A. Sodium hydroxide
B. Hydrochloric acid
C. Ethylene
D. Ammonia
Q2 See pages for figures
3. Which of the following substances is a polypeptide?
A. Starch
B. Glycogen
C. Protein
D. Fats
4. Which of the following products could be formed during incomplete combustion of a hydrocarbon? I. Carbon II. Hydrogen III.Carbon(II)oxide
A. I only
B. I and II only
C. I and III only
D. II and III only
5. What quantity of electrons is lost when one mole of iron (II) ions is oxidized to iron (III) ions?
A. 0 moles
B. 1 mole
C. 2 moles
D. 3 moles
6. What is the mass of of silver deposited when 24, 105C of electricity is passed through a solution of silver salt? [Ag = $108$, $1$F = $96$,$500$ C]
A. $432$g
B. $108$g
C. $54$g
D. $27$g
7. Equal masses of calciumtrioxocarbonate (IV) were added to dilute hydrochloric acid at the temperature specified. Under which of the following condition will the reaction be slowest?
A. Calcium trioxocarbonate (IV) chips at $20^0$C
B. Calcium trioxocarbonate (IV) chips at $40^0$C
C. Calcium trioxocarbonate (IV) powder at $20^0$C
D. Calcium trioxocarbonate (IV) powder at $40^0$C
8. The high solubility of ethanol in water is due to.
A. its low boiling point
B. its low freezing point
C. its covalent nature
D. hydrogen bonding
9. Which of the following metals reacts slowly with cold water?
A. Calcium
B. Silver
C. Iron
D. Potassium
10. Whichof the following pairs of properties of alkali metals decreases down the group?
A. First ionization energy and reactivity
B. Melting point and atomic radius
C. Reactivity and electronegativity
D. First ionization energy and melting point
11. The most suitable process of obtaining water from an aqueous solution of sugar is
A. crystallization
B. distillation
C. filtration
D. decantation
12. Group VII elements in their combined states are called.
A. halogens
B. anions
C. halides
D. cations
13. When an ionic bond is broken, bonding electrons are.
A. shared between participating atoms
B. gained by the most electropositive atom
C. gained by the most electronegative atom.
D. lost by both participating atoms.
14. The oxidation state of chlorine in $NaClO_{3}$ is
A. $+1$
B. $+3$
C. $+5$
D. $+6$
15. A balanced chemical equation is based on the law of
A. periodicity
B. constant composition
C. multiple proportion
D. conservation of mass
16. Which of the following pairs of elements has the greatest difference in electronegativity?
A. Na and F
B. Na and Cl
C. Na and Br
D. Na and I
17. A factor that is considered most important when siting a chemical industry is
A. nearness to other industrial establishments
B. nearness of raw materials
C. favorable climate conditions
D. availability of storage facilities
18. The boiling point of pentane is is higher than that of propane because
A. carbon-carbon single bonds are stronger that carbon-hydrogen bonds.
B pentane has more covalent bonds to break.
C. pentane does not burn easily as propane
D. the intermolecular forces in pentane are stronger than those of propane
19. which of the following solids will not decompose on heating?
A. Ammonium chloride
B. Lead (II) trioxonitrate (V)
C. Potassium trioxocarbonate(IV)
D. Sodium hydrogen trioxocarbonate (IV)
20. The following molecules have double covalent bonds between two atoms except
A. oxygen
B. carbon(IV)oxide
C. ethene
D. water
21. The type of isomerism exhibited by cis and trans isomers is
A. positional
B. geometrical
C. functional
D. optical
22. Which of the following compounds has the lowest boiling point?
A. $C_{4}H_{10}$
B. $CH_{3}COOH$
C. $H_{2}O$
D. $C_{2}H_{5}OH$
23. An alkanol containing 60% carbon by mass would have a molecular formula $[H=1.0, C=12.0, O=16.0]$
A. $CH_3OH$
B. $C_2H_5OH$
C. $C_3H_7OH$
D. $C_4H_9OH$
24. Which of the following compounds would release hydrogenwhen reacted with sodium metal? I. $CH_3COOH$, II. $CH_3CH_2OH$, III. $CH_3COOCH_3$
A. I only
B. I and II only
C. II and III only
D. I and III only
25. Which of the following substances is not a reducing agent?
A. $C$
B. $CO$
C. $O_2$
D. $H_2$
26. Which of the following statements is correct for a reaction at equilibrum?
A. All reaction cease to occur
B. The reaction has gone to completion
C. The rate of forward and backward reactions are equal
D. The amount of product equals the amount of reactants
27. WHich of the following terms are always exothermic?I. Neutralization II. Decomposition III. Combustion
A. I and II only
B. I and III only
C. II and III only
D. I, II and III
28. Which of the following standard coditions is not correct about energy changes?
A. A standard temperature is $298$K
B. Standard pressure is 1atm.
C. Concentration of the solution should be $1moldm^{-3}$
D. ${\Delta H}^{\theta}$ at $298$K is the activation energy
29. If $5.0cm^3$ of $0.200 moldm^{-3} Na_2CO_3$ was diluted to $250 cm^3$ solution, what would be the Concentration of the resulting solution?
A. $0.004 moldm^{-3}$
B. $0.020 moldm^{-3}$
C. $0.200 moldm^{-3}$
D. $400 moldm^{-3}$
30. The initial volume and pressure of a given mass of gas is V and $3$P. What is its pressure if its volume is increased to $2$V at constant temperature?
A. $3P$
B. $2P$
C. $^{3/_2}$
D. $^{2}/_3$
31. What volume of oxygenat s.t.p is required to burn completely 7.5${dm}^3$ of methane according to the following equation? $CH_{4(g)} + 2O_{2(g)} \longrightarrow CO_{2(g)} + H_2O_{(g)}$
A. $3.75dm^{3}$
B. $7.50dm^{3}$
C. $15.0dm^{3}$
D. $30.0dm^{3}$
32. When $250cm^3$ of saturated solution of $C_{u}SO_4$ at $30^0C$ was evaporated to dryness, $5.0_g$ of the salt was obtained. what is the solubility of the salt at $30^{0}C$? [$C_{u}SO_4 = 160$]
A. $0.031$
B. $0.125$
C. $0.640$
D. $1.560$
33. The bond between $NH_{3}$ and and $H^{+}$ in ${NH_{4}}^{+}$ is
A. Dative
B. Covalent
C. Hydrogen
D. electrovalent
34. Which of the following oxides has a giant covalent structure?
A. $Al_{2}O_{3}$
B. $Na_2O$
C. $P_4O_{10}$
D. $SiO_2$
35. Which of the following hydroxides is not readily soluble in water?
A. $NH_4OH$
B. $Ca(OH)_2$
C. $NaOH$
D. $KOH$
36. Which of the following statements about the solubilityof salt is correct?
A. A salt whose solubility increases with temperature would not crystallize quickly on cooking.
B. A salt whose solubility is independent of temperature would normally crystallize out on cooling.
C. Crystallization would be efficient in separating out a salt whose solubility increases considerably with temperature.
D. Solubility of a solid does not affect its crystallization.
37. How many moles of $H_{2}SO_4$ are there in $50cm^{3}$ of $0.108 moldm^{3}$ solution of the acid?
A. $5.4 \times 10$
B. $5.4 \times 10^{-1}$
C. $5.4 \times 10^{-2}$
D. $5.4 \times 10^{-3}$
38. If $20cm^{3}$ of sodium hydroxide was neutralized by $20cm^{3}$ of $0.01 mol dm^{3}$ tetraoxosulphate(VI) acid, what is the Concentration of the solution?
A. $0.010$
B. $0.020$
C. $0.100$
D. $0.150$
39. "Electrons always occupy the lowest empty energy level" is a statement of
A. Aufbau Principle
B. Hund's rule
C. Pauli Exclusion Principle
D. Periodic law
40. Which of the following metals do not react to water to produce hydrogen?
A. Lithium
B. Potassium
C. Sodium
D. Zinc
41. Which of the following arrangements of elements is decreasing order of electronegativity?
A. Na, Mg, Al, Si
B. Na, Al, Mg, P, Si
C. P, Mg, Na, Si, Al
D. P, Si, Al, Mg, Na
42. The metallic bond in magnessium is stronger than that in calcium because magnessium has a
A. larger atomic size
B. smaller atomic size
C. greater number of valence electrons
D. lower melting point
43. Consider the reaction represented by the following eguation: $AgNO_{3(aq)}$ + NaCl $\longrightarrow$ $AgCl_{(s)} NaNO_{2(aq)}$ The steps that could be taken to obtain pure dry sample of AgCl(s)from the mixture includes.
A. heating to saturation and drying
B. filtering and evaporation to dryness
C. filtering, washing and drying
D. crystallizing and allowing to cool
44. How many electrons does $^{31}_{15}P^{3-}$ contain?
A. $12$
B. $15$
C. $16$
D. $18$
45. The atomic number of an atom would be equal to its mass number if it
A. has a totally filled valence shell.
B. has a high charge to mass ratio
C. does not contain neutrons
D. exhibits isotopy
46. Which of the following processes is not exhibited by atoms in order to attain more stable electron configuration?
A. Gaining of electrons.
B. Hybridization of orbitals
C. Losing electrons
D. Sharing electrons
47. Which of the following quantities is a molar quantity?
A. Molarity
B. Molar mass
C. Mass concentration
D. Molality
48. Dilution factor is the
A. amount of distilled water that is added to the concentrated solution to dilute it.
B. quantity of distilled water added to 1${dm}^{3}$ of the concentrated solution to give the dilute solution.
C. number of times the volume of the concentated solution to give the dilute solution
D. act of diluting the concentrated to obtain the dilute solution
49. Calcium chloride is an ionic compound, which of the following statements account for its ionic character? I. calcium has high ionization energy II. Calcium has low ionization energy III. Chlorine has high electron affinity IV. Chlorine has high ionization energy.
A. I and II only
B. I, II and IV only
C. II, III and IV only
D. I,II,III and IV
50. An example of a biodegradable pollutant is
A. Plastic
B. sewage
C. carbon (II) oxide
D. hydrogen sulphide
ANSWERS
1
B
21
B
41
C
2
D
22
A
42
B
3
C
23
B
43
A
4
C
24
A
44
D
5
B
25
C
45
C
6
C
26
C
46
B
7
A
27
B
47
B
8
B
28
A
48
C
9
A
29
A
49
C
10
C
30
C
50
B
11
A
31
C
12
A
32
B
13
B
33
A
14
C
34
C
15
D
35
B
16
A
36
C
17
B
37
D
18
A
38
A
19
A
39
A
20
B
40
D
