1.	In which complexes does iron have an oxidation number of +3?
I.	[Fe(H2O)6]3+
II.	[Fe(H2O)5(CN)]2+
III.	[Fe(CN)6]3–
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

2.	Which molecule has an octahedral shape?
A.	SF6
B.	PCl5
C.	XeF4
D.	BF3
(Total 1 mark)

3.	Which species have delocalized electrons?
		
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

4.	Consider the equations below.
	CH4(g) + O2(g) → HCHO(l) + H2O(l)	∆HO = x
HCHO(l) + O2(g) → HCOOH(l)	∆HO = y
2HCOOH(l) + O2(g) → (COOH)2(s) + H2O(l)	∆HO = z
	What is the enthalpy change of the reaction below?
		2CH4(g) + 3O2(g) → (COOH)2(s) + 3H2O(l)
A.	x + y + z
B.	2x + y + z
C.	2x + 2y + z
D.	2x + 2y + 2z
(Total 1 mark)

5.	Given the enthalpy change for the reaction below:
		2H2(g) + O2(g) → 2H2O(l)	∆HO = –572 kJ
	which statement is correct?
A.	The standard enthalpy change of combustion of H2(g) is –286 kJ mol–1.
B.	The standard enthalpy change of combustion of H2(g) is +286 kJ mol–1.
C.	The standard enthalpy change of formation of H2O(l) is –572 kJ mol–1.
D.	The standard enthalpy change of formation of H2O(l) is +572 kJ mol–1.
(Total 1 mark)

6.	Which is a correct definition of lattice enthalpy?
A.	It is the enthalpy change that occurs when an electron is removed from 1 mol of gaseous atoms.
B.	It is the enthalpy change that occurs when 1 mol of a compound is formed from its elements.
C.	It is the enthalpy change that occurs when 1 mol of solid crystal changes into a liquid.
D.	It is the enthalpy change that occurs when 1 mol of solid crystal is formed from its gaseous ions.
(Total 1 mark)

7.	Which reaction has the largest increase in entropy?
A.	H2(g) + Cl2(g) → 2HCl(g)
B.	Al(OH)3(s) + NaOH(aq) → Al(OH)4–(aq) + Na+(aq)
C.	Na2CO3(s) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l)
D.	BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)
(Total 1 mark)

8.	Consider the following reaction.
		2P + Q → R + S
	This reaction occurs according to the following mechanism.
	P + Q → X	slow
P + X → R + S	fast
	What is the rate expression?
A.	rate = k[P]
B.	rate = k[P][X]
C.	rate = k[P][Q]
D.	rate = k[P]2[Q]
(Total 1 mark)

9.	What happens when the temperature of a reaction increases?
A.	The activation energy increases.
B.	The rate constant increases.
C.	The enthalpy change increases.
D.	The order of the reaction increases.
(Total 1 mark)

10.	What is the effect of an increase of temperature on the yield and the equilibrium constant for the following reaction?
		2H2(g) + CO(g)  CH3OH(l)	∆HO = –128 kJ

	Yield	Equilibrium
constant	
A.	Increases	Increases	
B.	Increases	Decreases	
C.	Decreases	Increases	
D.	Decreases	Decreases	
(Total 1 mark)

11.	Which statements about a liquid are correct?
I.	When the temperature of a liquid in a closed container increases, its vapour pressure increases.
II.	When the pressure on a liquid increases, its boiling point increases.
III.	When the pressure on a liquid increases, its vapour pressure increases.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

12.	Which mixtures act as buffer solutions?
I.	100 cm3 0.1 mol dm–3 ethanoic acid and 100 cm3 0.1 mol dm–3 sodium ethanoate
II.	100 cm3 0.1 mol dm–3 ethanoic acid and 50 cm3 0.1 mol dm–3 sodium hydroxide
III.	100 cm3 0.1 mol dm–3 ethanoic acid and 100 cm3 0.5 mol dm–3 sodium hydroxide
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

13.	Which solutions have a pH less than 7?
I.	Na2CO3(aq)
II.	[Fe(H2O)6]Cl3(aq)
III.	(NH4)2SO4(aq)
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

14.	Equal volumes and concentrations of hydrochloric acid and ethanoic acid are titrated with sodium hydroxide solutions of the same concentration. Which statement is correct?
A.	The initial pH values of both acids are equal.
B.	At the equivalence points, the solutions of both titrations have pH values of 7.
C.	The same volume of sodium hydroxide is needed to reach the equivalence point.
D.	The pH values of both acids increase equally until the equivalence points are reached.
(Total 1 mark)

15.	Bromophenol blue changes from yellow to blue over the pH range of 3.0 to 4.6. Which statement is correct?
A.	Molecules of bromophenol blue, HIn, are blue.
B.	At pH < 3.0, a solution of bromophenol blue contains more ions, In–, than molecules, HIn.
C.	The pKa of bromophenol blue is between 3.0 and 4.6.
D.	Bromophenol blue is a suitable indicator to titrate ethanoic acid with potassium hydroxide solution.
(Total 1 mark)

16.	The following equations indicate reactions that occur spontaneously.
	Fe(s) + NiCl2(aq) → FeCl2(aq) + Ni(s)
	Zn(s) + FeCl2(aq) → ZnCl2(aq) + Fe(s)
	Ni(s) + PbCl2(aq) → NiCl2(aq) + Pb(s)
	Which is the increasing order of the reactivity of the metals?
A.	Fe < Ni < Zn < Pb
B.	Pb < Ni < Fe < Zn
C.	Ni < Zn < Pb < Fe
D.	Zn < Fe < Ni < Pb
(Total 1 mark)

17.	A voltaic cell is made by connecting two half-cells represented by the half-equations below.
	Mn2+(aq) + 2e– → Mn(s)	EO = –1.19 V
Pb2+(aq) + 2e– → Pb(s)	EO = –0.13 V
	Which statement is correct about this voltaic cell?
A.	Mn is oxidized and the voltage of the cell is 1.06 V.
B.	Pb is oxidized and the voltage of the cell is 1.06 V.
C.	Mn is oxidized and the voltage of the cell is 1.32 V.
D.	Pb is oxidized and the voltage of the cell is 1.32 V.
(Total 1 mark)

18.	For the electrolysis of aqueous copper(II) sulfate, which of the following statements is correct?
A.	Cu and O2 are produced in a mol ratio of 1:1
B.	H2 and O2 are produced in a mol ratio of 1:1
C.	Cu and O2 are produced in a mol ratio of 2:1
D.	H2 and O2 are produced in a mol ratio of 2:1
(Total 1 mark)

19.	By which reactants and type of reaction can ethylamine (aminoethane) be produced?

	Reactants	Type of reaction	
A.	CH3Br + NH3	Nucleophilic substitution	
B.	CH3CH2Br + NH3	Reduction	
C.	CH3CN + H2	Nucleophilic substitution	
D.	CH3CN + H2	Reduction	
(Total 1 mark)

20.	Which compound is an amide?
A.	CH3COOCH3
B.	CH3CONH2
C.	CH3NH2
D.	CH2(NH2)COOH
(Total 1 mark)

A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

21.	Which process can produce a polyester?
A.	Addition polymerization of a dicarboxylic acid
B.	Condensation polymerization of a diol and a dicarboxylic acid
C.	Addition polymerization of a diol and dicarboxylic acid
D.	Condensation polymerization of a dicarboxylic acid
(Total 1 mark)

22.	Which statement about stereoisomers is correct?
A.	1,2-dichloroethane has two geometrical isomers.
B.	1,2-dichloroethane has two optical isomers.
C.	1,2-dichloroethene has two geometrical isomers.
D.	1,2-dichloroethene has two optical isomers.
(Total 1 mark)

23.	The molar mass of a compound is approximately 56 g mol–1. Which formula is possible for this compound?
A.	NaNO3
B.	AgOH
C.	MgO
D.	KOH
(Total 1 mark)

24.	Which compound has the empirical formula with the largest mass?
A.	C2H6
B.	C2H4
C.	C2H2
D.	C3H6
(Total 1 mark)

25.	What is the coefficient for O2(g) when the equation for the combustion of 1 mole of pentane is balanced?
		C5H12(g) + _O2(g) → _CO2(g) + _H2O(g)
A.	5
B.	6
C.	8
D.	16
(Total 1 mark)

26.	What is the maximum mass, in g, of magnesium oxide that can be obtained from the reaction of oxygen with 2.4 g of magnesium?
A.	2.4
B.	3.0
C.	4.0
D.	5.6
(Total 1 mark)

27.	5 dm3 of carbon monoxide, CO(g), and 2 dm3 of oxygen, O2(g), at the same temperature and pressure are mixed together. Assuming complete reaction according to the equation given, what is the maximum volume of carbon dioxide, CO2(g), in dm3, that can be formed?
		2CO(g) + O2(g) → 2CO2
A.	3
B.	4
C.	5
D.	7
(Total 1 mark)

28.	Which statement about solutions is correct?
A.	When vitamin D dissolves in fat, vitamin D is the solvent and fat is the solute.
B.	In a solution of NaCl in water, NaCl is the solute and water is the solvent.
C.	An aqueous solution consists of water dissolved in a solute.
D.	The concentration of a solution is the amount of solvent dissolved in 1 dm3 of solution.
(Total 1 mark)

29.	How many protons, neutrons and electrons are present in each atom of 31P?

	Protons	Neutrons	Electrons	
A.	16	15	16	
B.	15	16	15	
C.	15	31	15	
D.	16	31	16	
(Total 1 mark)

30.	Which is correct for the following regions of the electromagnetic spectrum?

	Ultraviolet (UV)	Infrared (IR)	
A.	high energy	short wavelength	low energy	low frequency	
B.	high energy	low frequency	low energy	long wavelength	
C.	high frequency	short wavelength	high energy	long wavelength	
D.	high frequency	long wavelength	low frequency	low energy	
(Total 1 mark)

31.	An element is in group 4 and period 3 of the periodic table. How many electrons are in the highest occupied energy level of an atom of this element?
A.	3
B.	4
C.	12
D.	14
(Total 1 mark)

32.	Which is the best definition of electronegativity?
A.	Electronegativity is the energy required for a gaseous atom to gain an electron.
B.	Electronegativity is the attraction of an atom for a bonding pair of electrons.
C.	Electronegativity is the attraction between the nucleus and the valence electrons of an atom.
D.	Electronegativity is the ability of an atom to attract electrons from another atom.
(Total 1 mark)

33.	What are the correct formulas of the following ions?

	Ammonium	Hydrogencarbonate	Phosphate	
A.	NH4+	HCO32–	PO4–	
B.	NH3+	HCO3–	PO43–	
C.	NH4+	HCO32–	PO42–	
D.	NH4+	HCO3–	PO43–	
(Total 1 mark)

34.	What happens when magnesium metal reacts with chlorine gas?
A.	Each magnesium atom loses two electrons and each chlorine atom gains two electrons.
B.	Each magnesium atom gains one electron and each chlorine atom loses one electron.
C.	Each magnesium atom loses two electrons and each chlorine atom gains one electron.
D.	Each magnesium atom gains one electron and each chlorine atom loses two electrons.
(Total 1 mark)

35.	Which is the best description of ionic bonding?
A.	The electrostatic attraction between positively charged nuclei and an electron pair
B.	The electrostatic attraction between positive ions and delocalized negative ions
C.	The electrostatic attraction between positive ions and delocalized electrons
D.	The electrostatic attraction between oppositely charged ions
(Total 1 mark)

36.	Which is the best description of the bonding present in silicon dioxide, SiO2?
A.	Each silicon atom forms four single covalent bonds to oxygen atoms.
B.	Each silicon atom forms two double covalent bonds to oxygen atoms.
C.	Each silicon atom forms two single covalent bonds to oxygen atoms.
D.	Each silicon atom forms four double covalent bonds to oxygen atoms.
(Total 1 mark)

37.	When some solid barium hydroxide and solid ammonium thiosulfate were reacted together, the temperature of the surroundings was observed to decrease from 15 ºC to – 4 ºC. What can be deduced from this observation?
A.	The reaction is exothermic and ∆H is negative.
B.	The reaction is exothermic and ∆H is positive.
C.	The reaction is endothermic and ∆H is negative.
D.	The reaction is endothermic and ∆H is positive.
(Total 1 mark)

38.	Which process represents the C–Cl bond enthalpy in tetrachloromethane?
A.	CCl4(g) → C(g) + 4Cl(g)
B.	CCl4(g) → CCl3(g) + Cl(g)
C.	CCl4(l) → C(g) + 4Cl(g)
D.	CCl4(l) → C(s) + 2Cl2(g)
(Total 1 mark)

39.	Some water is heated using the heat produced by the combustion of magnesium metal. Which values are needed to calculate the enthalpy change of reaction?
I.	The mass of magnesium
II.	The mass of the water
III.	The change in temperature of the water
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

40.	What is the best definition of rate of reaction?
A.	The time it takes to use up all the reactants
B.	The rate at which all the reactants are used up
C.	The time it takes for one of the reactants to be used up
D.	The increase in concentration of a product per unit time
(Total 1 mark)

41.	Which factors can affect reaction rate?
I.	The state of the reactants
II.	The frequency of the collisions between particles
III.	The average kinetic energy of the particles
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

42.	Equal masses of powdered calcium carbonate were added to separate solutions of hydrochloric acid. The calcium carbonate was in excess. The volume of carbon dioxide produced was measured at regular intervals. Which curves best represent the evolution of carbon dioxide against time for the acid solutions shown in the table below.

	25 cm3 of 2 mol dm–3 HCl	50 cm3 of 1 mol dm–3 HCl	25 cm3 of 1 mol dm–3 HCl	
A.	I	III	IV	
B.	I	IV	III	
C.	I	II	III	
D.	II	I	III	
(Total 1 mark)

43.	Consider the following equilibrium reaction.
		2SO2(g) + O2(g)  2SO3(g)	∆Ho = –197 kJ
	Which change in conditions will increase the amount of SO3 present when equilibrium is re-established?
A.	Decreasing the concentration of SO2
B.	Increasing the volume
C.	Decreasing the temperature
D.	Adding a catalyst
(Total 1 mark)

44.	For equal volumes of 1.0 mol dm–3 solutions of hydrochloric acid, HCl(aq), and methanoic acid, HCOOH(aq), which statements are correct?
I.	HCl dissociates more than HCOOH
II.	HCl is a better electrical conductor than HCOOH
III.	HCl will neutralize more NaOH than HCOOH
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

45.	When equal volumes of four 0.1 mol dm–3 solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?
A.	CH3COOH < HNO3 < CH3CH2NH2 < KOH
B.	HNO3 < CH3COOH < CH3CH2NH2 < KOH
C.	CH3CH2NH2 < HNO3 < CH3COOH < KOH
D.	KOH < CH3CH2NH2 < CH3COOH < HNO3
(Total 1 mark)

46.	What happens at the negative electrode in a voltaic cell and in an electrolytic cell?

	Voltaic cell	Electrolytic cell	
A.	oxidation	reduction	
B.	reduction	oxidation	
C.	oxidation	oxidation	
D.	reduction	reduction	
(Total 1 mark)

47.	Consider how current is conducted in an electrolytic cell. Which statement is correct?
A.	Electrons move through the electrolyte and the external circuit.
B.	Ions move through the electrolyte and the external circuit.
C.	Electrons move through the external circuit and ions move through the electrolyte.
D.	Electrons move through the electrolyte and ions move through the external circuit.
(Total 1 mark)

48.	Which three compounds can be considered to be a homologous series?
A.	CH3OH,     CH3CH2OH,     CH3CH2CH2OH
B.	CH3CH2OH,     CH3CHO,     CH3COOH
C.	CH3CH2CH(OH)CH3,     CH3CH2CH2CH2OH,     (CH3)3COH
D.	CH3CH2CH2CH2OH,     CH3CH2OCH2CH3,     (CH3)2CH2CHO
(Total 1 mark)

49.	What is the IUPAC name for CH3CH2CH(CH3)CH3?
A.	1,1-dimethylpropane
B.	2-ethylpropane
C.	2-methylbutane
D.	3-methylbutane
(Total 1 mark)

50.	When bromine water is shaken with a liquid organic compound, it is rapidly decolorized. What can be determined from this test?
A.	The compound is an alcohol.
B.	The compound is an alkane.
C.	The compound is an alkene.
D.	The compound is an iodoalkane.
(Total 1 mark)

51.	Which conditions are required to obtain a good yield of a carboxylic acid when ethanol is oxidized using potassium dichromate(VI), K2Cr2O7(aq)?
I.	Add sulfuric acid
II.	Heat the reaction mixture under reflux
III.	Distil the product as the oxidizing agent is added
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

52.	A student recorded the volume of a gas as 0.01450 dm3. How many significant figures are there in this value?
A.	3
B.	4
C.	5
D.	6
(Total 1 mark)

53.	Which species possesses only two unpaired electrons?
A.	Zn
B.	Mg
C.	Ti2+
D.	Fe2+
(Total 1 mark)

54.	Which statements are correct for the reactions of Cl2, MgCl2 and SiCl4 with water?

	Cl2	MgCl2	SiCl4	
A.	forms a neutral solution	forms a neutral solution	no reaction	
B.	forms an acidic solution	forms an acidic solution	forms an acidic solution	
C.	forms an acidic solution	forms an acidic solution	no reaction	
D.	forms a neutral solution	forms a neutral solution	forms an acidic solution	
(Total 1 mark)

55.	Which transition element, or compound of a transition element, is used as a catalyst in the Contact process?
A.	Fe
B.	MnO2
C.	V2O5
D.	Ni
(Total 1 mark)

56.	Which statements best describe the structure of sodium chloride, NaCl?
I.	Each sodium ion is surrounded by six chloride ions.
II.	The chloride ions are arranged octahedrally around each sodium ion.
III.	The lattice forms a cubic structure.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

57.	Which molecule contains a dative covalent (coordinate) bond?
A.	HCN
B.	H2O2
C.	CO2
D.	CO
(Total 1 mark)

58.	Identify the hybridization of carbon atoms in this molecule

	1	2	3	4	
A.	sp3	sp2	sp2	sp2	
B.	sp2	sp2	sp2	sp	
C.	sp3	sp	sp2	sp	
D.	sp	sp2	sp	sp2	
(Total 1 mark)

59.	Which structure has delocalized π electrons?
A.	O3
B.	CO
C.	HCN
D.	CO2
(Total 1 mark)

60.	1.0 g of sodium hydroxide, NaOH, was added to 99.0 g of water. The temperature of the solution increased from 18.0 ºC to 20.5 ºC. The specific heat capacity of the solution is
4.18 J g–1 K–1.
Which expression gives the heat evolved in kJ mol–1?
A.	
B.	
C.	
D.	
(Total 1 mark)

61.	Which reaction has the greatest increase in entropy?
A.	C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
B.	H2(g) + Cl2(g) → 2HCl(g)
C.	N2(g) + 3H2(g) → 2NH3(g)
D.	C2H4(g) + H2(g) → C2H6(g)
(Total 1 mark)

62.	The reaction between but-1-ene and water vapour produces butan-1-ol.
		C4H8(g) + H2O(g) → C4H9OH(l)
	The standard entropy values (SO) for but-1-ene, water vapour and butan-1-ol are 310, 189 and 228 J K–1 mol–1 respectively. What is the standard entropy change for this reaction in
J K–1 mol–1?
A.	–271
B.	+271
C.	–107
D.	+107
(Total 1 mark)

63.	This question refers to the following reaction.
		X2 + 2Y → 2XY
	The reaction occurs in a series of steps.
	X2 → 2X	slow
X + Y → XY	fast
	What is the rate-determining step for this reaction mechanism?
A.	X2 + 2Y → 2XY
B.	X2 + Y → XY + X
C.	X2 → 2X
D.	X + Y → XY
(Total 1 mark)

64.	This question refers to the following reaction.
		X2 + 2Y → 2XY
	The reaction occurs in a series of steps.
	X2 → 2X	slow
X + Y → XY	fast
	What is the rate expression for this reaction?
A.	rate = k[XY]
B.	rate = k[X2][Y]2
C.	rate = k[X2]
D.	rate = k[2X]
(Total 1 mark)

65.	Consider the following reversible reaction.
		Cr2O72–(aq) + H2O(l)  2CrO42–(aq) + 2H+(aq)
	What will happen to the position of equilibrium and the value of Kc when more H+ ions are added at constant temperature?

	Position of equilibrium	Value of Kc	
A.	shifts to the left	decreases	
B.	shifts to the right	increases	
C.	shifts to the right	does not change	
D.	shifts to the left	does not change	
(Total 1 mark)

66.	Consider this equilibrium reaction in a sealed container:
		H2O(g)  H2O(l)
	What will be the effect on the equilibrium of increasing the temperature from 20 ºC to 30 ºC?
A.	More of the water will be in the gaseous state at equilibrium.
B.	More of the water will be in the liquid state at equilibrium.
C.	At equilibrium the rate of condensation will be greater than the rate of evaporation.
D.	At equilibrium the rate of evaporation will be greater than the rate of condensation.
(Total 1 mark)

67.	What is the correct expression for the ionic product constant of water, Kw?
A.	KW = 
B.	KW = 
C.	KW = [H+] + [OH–]
D.	KW = [H+][OH–]
(Total 1 mark)

68.	Which mixtures could act as buffers?
I.	NaOH(aq) and HCl(aq)
II.	NaOH(aq) and CH3COOH(aq)
III.	HCl(aq) and CH3COONa(aq)
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

69.	What is the approximate pH of a 0.01 mol dm–3 ammonia solution?
A.	2
B.	More than 2 but less than 7
C.	More than 7 but less than 12
D.	12
(Total 1 mark)

70.	Which conditions are usually stated for a standard hydrogen electrode?
I.	Hydrogen gas at a pressure of 1.01 × 105 Pa (1 atm)
II.	1.0 mol dm–3 solution of any acid
III.	Temperature of 25 ºC (298 K)
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

71.	Consider these standard electrode potentials.
	Mg2+(aq) + 2e–  Mg(s)	EO = –2.36 V
Zn2+(aq) + 2e–  Zn(s)	EO = –0.76 V
	What is the cell potential for the voltaic cell produced when the two half-cells are connected?
A.	–1.60 V
B.	+1.60 V
C.	–3.12 V
D.	+3.12 V
(Total 1 mark)

72.	Identify the functional group present in HCOCH2CH3.
A.	Ester
B.	Ketone
C.	Aldehyde
D.	Alcohol
(Total 1 mark)

73.	What is the IUPAC name for HCOOCH2CH2CH3?
A.	Butanoic acid
B.	Butanal
C.	Methyl propanoate
D.	Propyl methanoate
(Total 1 mark)

74.	Which statements about substitution reactions are correct?
I.	The reaction between sodium hydroxide and 1-chloropentane predominantly follows an SN2 mechanism.
II.	The reaction between sodium hydroxide and 2-chloro-2-methylbutane predominantly follows an SN2 mechanism.
III.	The reaction of sodium hydroxide with 1-chloropentane occurs at a slower rate than with 1-bromopentane.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

75.	What is the organic product of the reaction between methylamine and ethanoic acid?
A.	CH3COONH4
B.	CH3NHCOCH3
C.	CH3COCH2NH2
D.	CH3CH2CONH2
(Total 1 mark)

76.	Which compound can exist as stereoisomers?
A.	CH3CH2CHO
B.	CH3CH2COCH3
C.	CH3CH(CH3)2
D.	CH3CH2CHOHCH3
(Total 1 mark)

77.	What is the number of oxygen atoms in one mole of CuSO4•5H2O?
A.	5
B.	9
C.	6.0 × 1023
D.	5.4 × 1024
(Total 1 mark)

78.	Which sample has the greatest mass?
A.	6.0 × 1025 molecules of hydrogen
B.	5.0 mol of neon atoms
C.	1.2 × 1024 atoms of silver
D.	1.7 × 102 g of iron
(Total 1 mark)

79.	What volume of sulfur trioxide, in cm3, can be prepared using 40 cm3 sulfur dioxide and 20 cm3 oxygen gas by the following reaction? Assume all volumes are measured at the same temperature and pressure.
		2SO2(g) + O2(g) → 2SO3(g)
A.	20
B.	40
C.	60
D.	80
(Total 1 mark)

80.	Which sample of nitrogen gas, N2, contains the greatest number of nitrogen molecules?
A.	1.4 g N2
B.	1.4 dm3 of N2 at 1.01 × 105 Pa and 273 K
C.	1.4 × 1023 N2 molecules
D.	1.4 mol N2
(Total 1 mark)

81.	What is the atomic number of a neutral atom which has 51 neutrons and 40 electrons?
A.	40
B.	51
C.	91
D.	131
(Total 1 mark)

82.	What is the relative atomic mass of an element with the following mass spectrum?
		
A.	24
B.	25
C.	26
D.	27
(Total 1 mark)

83.	Which is the correct definition of the mass number of an atom?
A.	The total mass of neutrons and protons in the nucleus of the atom
B.	The total mass of neutrons, protons and electrons in the atom
C.	The number of protons in the nucleus of the atom
D.	The total number of neutrons and protons in the nucleus of the atom
(Total 1 mark)

84.	Which statement describes the trends of electronegativity values in the periodic table?
A.	Values increase from left to right across a period and increase down a group.
B.	Values increase from left to right across a period and decrease down a group.
C.	Values decrease from left to right across a period and increase down a group.
D.	Values decrease from left to right across a period and decrease down a group.
(Total 1 mark)

85.	Which statement is correct for all elements in the same period?
A.	They have the same number of electrons in the highest occupied energy level.
B.	They have the same chemical reactivity.
C.	They have the same number of occupied energy levels.
D.	They have the same number of neutrons.
(Total 1 mark)

86.	Which statement best describes the intramolecular bonding in HCN(l)?
A.	Electrostatic attractions between H+ and CN– ions
B.	Only van der Waals’ forces
C.	Van der Waals’ forces and hydrogen bonding
D.	Electrostatic attractions between pairs of electrons and positively charged nuclei
(Total 1 mark)

87.	Which statement best describes metallic bonding?
A.	Electrostatic attractions between oppositely charged ions
B.	Electrostatic attractions between a lattice of positive ions and delocalized electrons
C.	Electrostatic attractions between a lattice of negative ions and delocalized protons
D.	Electrostatic attractions between protons and electrons
(Total 1 mark)

88.	Metal M has only one oxidation number and forms a compound with the formula MCO3.
Which formula is correct?
A.	MNO3
B.	MNH4
C.	MSO4
D.	MPO4
(Total 1 mark)

89.	Which molecule has the shortest bond between carbon atoms?
A.	C2H6
B.	C2H4
C.	C2H2
D.	C2H4Cl2
(Total 1 mark)

90.	What is the energy, in kJ, released when 1.00 mol of carbon monoxide is burned according to the following equation?
		2CO(g) + O2(g) → 2CO2(g)	ΔHo = –564 kJ
A.	141
B.	282
C.	564
D.	1128
(Total 1 mark)

91.	The specific heat of iron is 0.450 J g–1 K–1. What is the energy, in J, needed to increase the temperature of 50.0 g of iron by 20.0 K?
A.	9.00
B.	22.5
C.	45.0
D.	450
(Total 1 mark)

92.	Which of the following reactions are exothermic?
I.	CH4 + 2O2 → CO2 + 2H2O
II.	NaOH + HCl → NaCl + H2O
III.	Br2 → 2Br
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

93.	Consider the reaction between magnesium and hydrochloric acid. Which factors will affect the reaction rate?
I.	The collision frequency of the reactant particles
II.	The number of reactant particles with E ≥ Ea
III.	The number of reactant particles that collide with the appropriate geometry
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

94.	What is the function of iron in the Haber process?
A.	It shifts the position of equilibrium towards the products.
B.	It decreases the rate of the reaction.
C.	It provides an alternative reaction pathway with a lower activation energy.
D.	It reduces the enthalpy change of the reaction.
(Total 1 mark)

95.	What effect will an increase in temperature have on the Kc value and the position of equilibrium in the following reaction?
		N2(g) + 3H2(g)  2NH3(g)	ΔH = –92 kJ

	Kc	Equilibrium position	
A.	increases	shifts to the right	
B.	decreases	shifts to the left	
C.	increases	shifts to the left	
D.	decreases	shifts to the right	
(Total 1 mark)

96.	Which statement is always correct for a chemical reaction at equilibrium?
A.	The rate of the forward reaction equals the rate of the reverse reaction.
B.	The amounts of reactants and products are equal.
C.	The concentration of the reactants and products are constantly changing.
D.	The forward reaction occurs to a greater extent than the reverse reaction.
(Total 1 mark)

97.	Which are definitions of an acid according to the Brønsted-Lowry and Lewis theories?

	Brønsted-Lowry theory	Lewis theory	
A.	proton donor	electron pair acceptor	
B.	proton acceptor	electron pair acceptor	
C.	proton acceptor	electron pair donor	
D.	proton donor	electron pair donor	
(Total 1 mark)

98.	Which list contains only strong acids?
A.	CH3COOH,   H2CO3,   H3PO4
B.	HCl,   HNO3,   H2CO3
C.	CH3COOH,   HNO3,   H2SO4
D.	HCl,   HNO3,   H2SO4
(Total 1 mark)

99.	An example of a strong acid solution is perchloric acid, HClO4, in water. Which statement is correct for this solution?
A.	HClO4 is completely dissociated in the solution.
B.	HClO4 exists mainly as molecules in the solution.
C.	The solution reacts only with strong bases.
D.	The solution has a pH value greater than 7.
(Total 1 mark)

100.	Which species is oxidized in the following reaction?
		2Ag+(aq) + Cu(s) → 2Ag(s) + Cu2+(aq)
A.	Ag+
B.	Cu
C.	Ag
D.	Cu2+
(Total 1 mark)

101.	Which list represents the halogens in increasing order of oxidizing strength (weakest oxidizing agent first)?
A.	Cl2   I2   Br2
B.	I2   Br2   Cl2
C.	I2   Cl2   Br2
D.	Cl2   Br2   I2
(Total 1 mark)

102.	What is the product of the oxidation of butan-2-ol?
A.	But-2-ene
B.	Butanoic acid
C.	Butanal
D.	Butanone
(Total 1 mark)

103.	Which is a tertiary halogenoalkane?
A.	CH3CH2CH2Br
B.	CH3CH2CH(CH3)Cl
C.	C(CH3)3Br
D.	CH3CHClCH2CH3
(Total 1 mark)

104.	What is the IUPAC name of the following compound?
		
A.	2-methylbutane
B.	Ethylpropane
C.	3-methylbutane
D.	Pentane
(Total 1 mark)

105.	Which equations represent the incomplete combustion of methane?
I.	CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
II.	CH4(g) + 1½O2(g) → CO(g) + 2H2O(g)
III.	CH4(g) + O2(g) → C(s) + 2H2O(g)
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

106.	Which would be the best method to decrease the random uncertainty of a measurement in an acid-base titration?
A.	Repeat the titration
B.	Ensure your eye is at the same height as the meniscus when reading from the burette
C.	Use a different burette
D.	Use a different indicator for the titration
(Total 1 mark)

107.	The table below shows the number of protons, neutrons and electrons present in five species.

Species	Number of protons	Number of neutrons	Number of electrons	
X	6	8	6	
Y	7	7	7	
Z	7	7	8	
W	8	8	8	
Q	8	10	8	
	Which two species are isotopes of the same element?
A.	X and W
B.	Y and Z
C.	Z and W
D.	W and Q
(Total 1 mark)

108.	What is the order of increasing energy of the orbitals within a single energy level?
A.	d < s < f < p
B.	s < p < d < f
C.	p < s < f < d
D.	f < d < p < s
(Total 1 mark)

109.	What is the electron configuration of the Cr2+ ion?
A.	[Ar] 3d5 4s1
B.	[Ar] 3d3 4s1
C.	[Ar] 3d6 4s1
D.	[Ar] 3d4 4s0
(Total 1 mark)

110.	Which equation best represents the first ionization energy of magnesium?
A.	Mg(s) → Mg+(s) + e–
B.	Mg(g) → Mg2+(g) + 2e–
C.	Mg(g) → Mg+(g) + e–
D.	Mg(s) → Mg+(g) + e–
(Total 1 mark)

111.	What are the products of the reaction between chlorine and water?
A.	O2, H2 and HCl
B.	H2 and OCl2
C.	HCl and HOCl
D.	HOCl, H2 and Cl2
(Total 1 mark)

112.	How many bonding pairs and lone pairs of electrons surround the sulfur atom in the SF4 molecule?

	Bonding pairs	Lone pairs	
A.	4	1	
B.	4	0	
C.	6	0	
D.	8	2	
(Total 1 mark)

113.	Which of the following best describes the formation of π bonds?
A.	They are formed by the sideways overlap of parallel orbitals.
B.	They are formed by the axial overlap of orbitals.
C.	They are formed by the sideways overlap of an s and p orbital.
D.	They are formed by the axial overlap of either s or p orbitals.
(Total 1 mark)

114.	What is the standard entropy change, ∆SO, for the following reaction?
		2CO(g) + O2(g) → 2CO2(g)

	CO(g)	O2(g)	CO2(g)	
SO/J K–1 mol–1	198	205	214	
A.	–189
B.	–173
C.	+173
D.	+189
(Total 1 mark)

115.	Which step(s) is/are endothermic in the Born-Haber cycle for the formation of LiCl?
A.	½Cl2(g) → Cl(g) and Li(s) → Li(g)
B.	Cl(g) + e– → Cl–(g) and Li(g) → Li+(g) + e–
C.	Li+(g) + Cl–(g) → LiCl(s)
D.	½Cl2(g) → Cl(g) and Cl(g) + e– → Cl–(g)
(Total 1 mark)

116.	Consider the following reaction.
		5Br–(aq) + BrO3–(aq) + 6H+(aq) → 3Br2(aq) + 3H2O(l)
	The rate expression for the reaction is found to be:
		rate = k[Br–] [BrO3–][H+]2
	Which statement is correct?
A.	The overall order is 12.
B.	Doubling the concentration of all of the reactants at the same time would increase the rate of the reaction by a factor of 16.
C.	The units of the rate constant, k, are mol dm–3 s–1.
D.	A change in concentration of Br– or BrO3– does not affect the rate of the reaction.
(Total 1 mark)

117.	The rate expression for a reaction is:
		rate = k [X][Y]
	Which statement is correct?
A.	As the temperature increases the rate constant decreases.
B.	The rate constant increases with increased temperature but eventually reaches a constant value.
C.	As the temperature increases the rate constant increases.
D.	The rate constant is not affected by a change in temperature.
(Total 1 mark)

118.	Consider the following reaction mechanism.
Step 1	H2O2 + I– → H2O + IO–	slow
Step 2	H2O2 + IO– → H2O + O2 + I–	fast
	Which statement correctly identifies the rate-determining step and the explanation?
A.	Step 2 because it is the faster step
B.	Step 1 because it is the slower step
C.	Step 1 because it is the first step
D.	Step 2 because it is the last step
(Total 1 mark)

119.	Which statement is correct for the equilibrium H2O(l)  H2O(g) in a closed system at 100 °C?
A.	All the H2O(l) molecules have been converted to H2O(g).
B.	The rate of the forward reaction is greater than the rate of the reverse reaction.
C.	The rate of the forward reaction is less than the rate of the reverse reaction.
D.	The pressure remains constant.
(Total 1 mark)

120.	100 cm3 of a NaOH solution of pH 12 is mixed with 900 cm3 of water. What is the pH of the resulting solution?
A.	1
B.	3
C.	11
D.	13
(Total 1 mark)

121.	Ammonia acts as a weak base when it reacts with water. What is the Kb expression for this reaction?
A.	
B.	
C.	
D.	
(Total 1 mark)

122.	The indicator, HIn is used in a titration between an acid and base. Which statement about the dissociation of the indicator, HIn is correct?
	HIn (aq)  H+ (aq) + In– (aq)
colour A	colour B
A.	In a strongly alkaline solution, colour B would be observed.
B.	In a strongly acidic solution, colour B would be observed.
C.	[In–] is greater than [HIn] at the equivalence point.
D.	In a weakly acidic solution colour B would be observed.
(Total 1 mark)

123.	At the same concentration, which acid would have the lowest pH?
A.	HNO2	Ka = 5.6 × 10–4 mol dm–3
B.	HF	Ka = 6.8 × 10–4 mol dm–3
C.	C6H5COOH	Ka = 6.3 × 10–5 mol dm–3
D.	HCN	Ka = 4.9 × 10–10 mol dm–3
(Total 1 mark)

124.	What is the cell potential, in V, for the reaction that occurs when the following two half-cells are connected?
	Fe2+(aq) + 2e–  Fe(s)	EO = –0.44 V
	Cr2O72–(aq) + 14H+(aq) + 6e–  2Cr3+(aq) + 7H2O(l)	EO = +1.33 V
A.	+ 0.01
B.	+ 0.89
C.	+ 1.77
D.	+ 2.65
(Total 1 mark)

125.	What structural feature must a molecule have in order to undergo addition polymerization?
A.	Two functional groups
B.	A carbon–carbon double bond
C.	Carbon atoms singly bonded together
D.	A polar covalent bond
(Total 1 mark)

126.	What is the organic product of the reaction between CH3CH2NH2 and CH3CH2COOH?
A.	CH3CH2NHCOCH2CH3
B.	CH3CH2CH2NHCOCH3
C.	CH3CH2NHCOCH3
D.	CH3NHCOCH3
(Total 1 mark)

127.	What is the IUPAC name of the compound CH3CH2COOCH2CH3?
A.	Ethyl ethanoate
B.	Propyl ethanoate
C.	Ethyl propanoate
D.	Pentyl propanoate
(Total 1 mark)

128.	Which statement is correct about the enantiomers of a chiral compound?
A.	Their physical properties are different.
B.	All their chemical reactions are identical.
C.	A racemic mixture will rotate the plane of polarized light.
D.	They will rotate the plane of polarized light in opposite directions.
(Total 1 mark)

129.	Which non-metal forms an oxide XO2 with a relative molecular mass of 60?
A.	C
B.	N
C.	Si
D.	S
(Total 1 mark)

130.	How many oxygen atoms are there in 0.20 mol of ethanoic acid, CH3COOH?
A.	1.2 × 1023
B.	2.4 × 1023
C.	3.0 × 1024
D.	6.0 × 1024
(Total 1 mark)

131.	4.00 mol of a hydrocarbon with an empirical formula of CH2 has a mass of 280 g. What is the molecular formula of this compound?
A.	C2H4
B.	C3H6
C.	C4H8
D.	C5H10
(Total 1 mark)

132.	What will be the concentration of sulfate ions in mol dm–3 when 0.20 mol of KAl(SO4)2 is dissolved in water to give 100 cm3 of aqueous solution?
A.	0.2
B.	1.0
C.	2.0
D.	4.0
(Total 1 mark)

133.	The volume of an ideal gas at 27.0 °C is increased from 3.00 dm3 to 6.00 dm3. At what temperature, in °C, will the gas have the original pressure?
A.	13.5
B.	54.0
C.	327
D.	600
(Total 1 mark)

134.	Which species have the same number of electrons?
I.	S2–
II.	Cl–
III.	Ne
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

135.	Which gives the correct order of these processes in a mass spectrometer?
A.	ionization	deflection	acceleration
B.	ionization	acceleration	deflection
C.	acceleration	ionization	deflection
D.	deflection	acceleration	ionization
(Total 1 mark)

136.	What happens when sodium is added to water?
I.	A gas is evolved
II.	The temperature of the water increases
III.	A clear, colourless solution is formed
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

137.	An atom of an element contains 19 electrons. In which group of the periodic table does it occur?
A.	1
B.	2
C.	5
D.	7
(Total 1 mark)

138.	What compound is formed when lithium reacts with selenium?
A.	LiSe
B.	Li2Se
C.	LiSe2
D.	Li2Se2
(Total 1 mark)

139.	How many non-bonding pairs of electrons are there in a nitrogen molecule?
A.	0
B.	1
C.	2
D.	3
(Total 1 mark)

140.	Which molecule contains a bond angle of approximately 120°?
A.	CH4
B.	C2H2
C.	C2H4
D.	C2H6
(Total 1 mark)

141.	Which compound does not form hydrogen bonds between its molecules?
A.	CH3NH2
B.	CH3COCH3
C.	CH3COOH
D.	CH3CH2OH
(Total 1 mark)

142.	Which substance does not conduct electricity?
A.	Solid zinc
B.	Molten zinc
C.	Solid zinc chloride
D.	Molten zinc chloride
(Total 1 mark)

143.	Which is true for a chemical reaction in which the products have a higher enthalpy than the reactants?

	Reaction	∆H	
A.	endothermic	positive	
B.	endothermic	negative	
C.	exothermic	positive	
D.	exothermic	negative	
(Total 1 mark)

144.	In a reaction that occurs in 50 g of aqueous solution, the temperature of the reaction mixture increases by 20 °C. If 0.10 mol of the limiting reagent is consumed, what is the enthalpy change (in kJ mol–1) for the reaction? Assume the specific heat capacity of the solution
= 4.2 kJ kg–1 K–1.
A.	–0.10 × 50 × 4.2 × 20
B.	–0.10 × 0.050 × 4.2 × 20
C.	
D.	
(Total 1 mark)

145.	Use the average bond enthalpies below to calculate the enthalpy change, in kJ, for the following reaction.
		H2(g) + I2(g) → 2HI(g)

Bond	Bond energy / kJ mol–1	
H–H 	440 	
I–I 	150 	
H–I 	300 	
A.	+290
B.	+10
C.	–10
D.	–290
(Total 1 mark)

146.	Hydrochloric acid is reacted with large pieces of calcium carbonate, the reaction is then repeated using calcium carbonate powder. How does this change affect the activation energy and the collision frequency?

	Activation energy	Collision frequency	
A.	increases	increases	
B.	stays constant	increases	
C.	increases	stays constant	
D.	stays constant	stays constant	
(Total 1 mark)

147.	Which statement is true about using sulfuric acid as a catalyst in the following reaction?
		CH3–CO–CH3(aq) + I2(aq)  CH3–CO–CH2–I(aq) + HI(aq)
I.	The catalyst increases the rate of reaction.
II.	The catalyst lowers the activation energy for the reaction.
III.	The catalyst has been consumed at the end of the chemical reaction.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

148.	An increase in temperature increases the amount of chlorine present in the following equilibrium.
		PCl5(s)  PCl3(l) + Cl2(g)
	What is the best explanation for this?
A.	The higher temperature increases the rate of the forward reaction only.
B.	The higher temperature increases the rate of the reverse reaction only.
C.	The higher temperature increases the rate of both reactions but the forward reaction is affected more than the reverse.
D.	The higher temperature increases the rate of both reactions but the reverse reaction is affected more than the forward.
(Total 1 mark)

149.	What will happen when at a constant temperature, more iodide ions, I–, are added to the equilibrium below?
		I2(s) + I–(aq)  I3–(aq)
A.	The amount of solid iodine decreases and the equilibrium constant increases.
B.	The amount of solid iodine decreases and the equilibrium constant remains unchanged.
C.	The amount of solid iodine increases and the equilibrium constant decreases.
D.	The amount of solid iodine increases and the equilibrium constant remains unchanged.
(Total 1 mark)

150.	What is the formula of the conjugate base of the hydrogenphosphate ion, HPO42–?
A.	H2PO4–
B.	H3PO4
C.	HPO4–
D.	PO43–
(Total 1 mark)

151.	Which pH value is that of an aqueous solution of carbon dioxide?
A.	2.1
B.	5.6
C.	9.8
D.	12.2
(Total 1 mark)

152.	Which are redox reactions?
I.	2FeCl2 + Cl2 → 2FeCl3
II.	Mg + 2HNO3 → Mg(NO3)2 + H2
III.	H2O + SO3 → H2SO4
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

153.	Magnesium is higher in the reactivity series than zinc. In the cell shown, in which direction do the electrons flow in wire X and which metal is oxidized?

	Electron flow	Oxidized	
A.	Zn to Mg	Zn	
B.	Mg to Zn	Zn	
C.	Zn to Mg	Mg	
D.	Mg to Zn	Mg	
(Total 1 mark)

154.	How many structural isomers exist with the formula C3H5Cl3?
A.	3
B.	4
C.	5
D.	6
(Total 1 mark)

155.	Which substance is produced by the reaction of hydrogen with a vegetable oil?
A.	Margarine
B.	Nylon
C.	Polypropene
D.	Soap
(Total 1 mark)

156.	Which substance is not produced during the combustion of alkanes?
A.	CO2
B.	CO
C.	C
D.	H2
(Total 1 mark)

157.	Propene is converted to propanone in a two stage process.
		Propene → X → Propanone
	What is the formula of compound X?
A.	CH3CHBrCH3
B.	CH3CH2CH2Br
C.	CH3CHOHCH3
D.	CH3CH2CH2OH
(Total 1 mark)

158.	Which are likely to be reduced when an experiment is repeated a number of times?
A.	Random errors
B.	Systematic errors
C.	Both random and systematic errors
D.	Neither random nor systematic errors
(Total 1 mark)

159.	Which coefficients would balance this equation?
		__ MnO2 + __ HCl → __ MnCl2 + __ Cl2 + __ H2O

	MnO2	HCl	MnCl2	Cl2	H2O	
A.	1	2	1	1	1	
B.	1	3	1	1	1	
C.	1	4	1	1	2	
D.	1	4	1	2	2	
(Total 1 mark)

160.	What volume of carbon dioxide, in dm3 under standard conditions, is formed when 7.00 g of ethene (C2H4, Mr = 28.1) undergoes complete combustion?
A.	
B.	
C.	
D.	
(Total 1 mark)

161.	Between which ionization energies of boron will there be the greatest difference?
A.	Between 1st and 2nd ionization energies
B.	Between 2nd and 3rd ionization energies
C.	Between 3rd and 4th ionization energies
D.	Between 4th and 5th ionization energies
(Total 1 mark)

162.	Which species has the largest radius?
A.	Cl–
B.	K
C.	Na+
D.	K+
(Total 1 mark)

163.	Which process is responsible for the colour of a transition metal complex?
A.	The absorption of light when electrons move between s orbitals and d orbitals
B.	The emission of light when electrons move between s orbitals and d orbitals
C.	The absorption of light when electrons move between different d orbitals
D.	The emission of light when electrons move between different d orbitals
(Total 1 mark)

164.	What is the correct order if the compounds are arranged in order of increasing boiling point?
A.	CH4 < CH3Cl < SiH4 < CH3OH
B.	CH3OH < CH4 < CH3Cl < SiH4
C.	CH3OH < CH3Cl < SiH4 < CH4
D.	CH4 < SiH4 < CH3Cl < CH3OH
(Total 1 mark)

165.	What is the bond angle in the H3O+ ion?
A.	104°
B.	107°
C.	109°
D.	120°
(Total 1 mark)

166.	How many atoms is each carbon directly bonded to in its allotropes?

	Diamond	Graphite	C60 fullerene	
A.	3	3	3	
B.	4	3	3	
C.	4	3	4	
D.	4	4	3	
(Total 1 mark)

167.	What is the type of hybridization of the silicon and oxygen atoms in silicon dioxide?

	Silicon	Oxygen	
A.	sp3	sp3	
B.	sp3	sp2	
C.	sp2	sp3	
D.	sp2	sp2	
(Total 1 mark)

168.	Which ionic compound has the most endothermic lattice enthalpy?
A.	NaCl
B.	KCl
C.	NaF
D.	KF
(Total 1 mark)

169.	Which change leads to an increase in entropy?
A.	CO2(g) → CO2(s)
B.	SF6(g) → SF6(l)
C.	H2O(l) → H2O(s)
D.	NaCl(s) → NaCl(aq)
(Total 1 mark)

170.	Two species, P and Q, react together according to the following equation.
		P + Q → R
	The accepted mechanism for this reaction is
		P + P  P2	fast
	P2 + Q → R + P	slow
	What is the order with respect to P and Q?

	P	Q	
A.	1	1	
B.	1	2	
C.	2	1	
D.	2	2	
(Total 1 mark)

171.	The activation energy of a reaction may be determined by studying the effect of a particular variable on the reaction rate. Which variable must be changed?
A.	pH
B.	Concentration
C.	Surface area
D.	Temperature
(Total 1 mark)

172.	Which affects the equilibrium vapour pressure of a liquid in a sealed container, assuming that there is always some of the liquid present?
A.	The temperature of the liquid
B.	The surface area of the liquid
C.	The volume of the liquid
D.	The volume of the container
(Total 1 mark)

173.	According to the Brønsted-Lowry theory, how does each species act in the equilibrium below?
		CH3COOH + H2SO4  CH3COOH2+ + HSO4–

	CH3COOH	H2SO4	CH3COOH2+	HSO4–	
A.	acid	base	base	acid	
B.	acid	base	acid	base	
C.	base	acid	base	acid	
D.	base	acid	acid	base	
(Total 1 mark)

174.	If 20 cm3 samples of 0.1 mol dm–3 solutions of the acids below are taken, which acid would require a different volume of 0.1 mol dm–3 sodium hydroxide for complete neutralization?
A.	Nitric acid
B.	Sulfuric acid
C.	Ethanoic acid
D.	Hydrochloric acid
(Total 1 mark)

175.	Which mixture of acid and alkali would produce a buffer solution?

	Acid	Alkali	
A.	40 cm3 0.1 mol dm–3 HCl	60 cm3 0.1 mol dm–3 NaOH	
B.	60 cm3 0.1 mol dm–3 HCl	40 cm3 0.1 mol dm–3 NaOH	
C.	40 cm3 0.1 mol dm–3 HCl	60 cm3 0.1 mol dm–3 NH3	
D.	60 cm3 0.1 mol dm–3 HCl	40 cm3 0.1 mol dm–3 NH3	
(Total 1 mark)

176.	Which aqueous solution would have a pH > 7?
A.	Sodium sulfate
B.	Ammonium nitrate
C.	Sodium ethanoate
D.	Aluminium nitrate
(Total 1 mark)

177.	Which indicator would be the most appropriate for titrating aqueous ethylamine, CH3CH2NH2, with nitric acid, HNO3?
A.	Bromophenol blue (pKa = 4.1)
B.	Bromothymol blue (pKa = 7.3)
C.	Phenol red (pKa = 8.0)
D.	Thymolphthalein (pKa = 10.0)
(Total 1 mark)

178.	Which compound contains nitrogen with an oxidation number of +3?
A.	NH4Cl
B.	HNO3
C.	N2O4
D.	KNO2
(Total 1 mark)

179.	In the electrolytic cell shown, at which electrode will chlorine form, and what is the process taking place there?

	Electrode	Process	
A.	P	reduction	
B.	Q	reduction	
C.	P	oxidation	
D.	Q	oxidation	
(Total 1 mark)

180.	How do the products compare at each electrode when aqueous 1 mol dm–3 magnesium bromide and molten magnesium bromide are electrolysed?
		EO / V
		Mg2+(aq) + 2e–  Mg(s)	–2.37
	½Br2(l) + e–  Br–(aq)	+1.07
	½O2(g) + 2H+(aq) + 2e–  H2O(l)	+1.23

	Positive electrode (Anode)	Negative electrode (Cathode)	
A.	same	same	
B.	same	different	
C.	different	same	
D.	different	different	
(Total 1 mark)

181.	Which reaction occurs via a free-radical mechanism?
A.	C2H6 + Br2 → C2H5Br + HBr
B.	C2H4 + Br2 → C2H4Br2
C.	C4H9I + OH– → C4H9OH + I–
D.	(CH3)3CI + H2O → (CH3)3COH + HI
(Total 1 mark)

182.	Which compound could rotate the plane of polarization of polarized light?
A.	(CH3)2CHCH2Cl
B.	CH3CH2CH2CH2Cl
C.	CH3CH2CHClCH3
D.	(CH3)3CCl
(Total 1 mark)

183.	What is the name of the ester formed when CH3CH2COOH and CH3OH react together?
A.	Ethyl methanoate
B.	Methyl ethanoate
C.	Propyl methanoate
D.	Methyl propanoate
(Total 1 mark)

184.	Which formula represents a polyamide?
A.	 ( CH2–CHCl ) n
B.	 ( NH–(CH2)6–NH–CO–(CH3)4–CO ) n
C.	 ( CF2–CF2 ) n
D.	 ( O–(CH2)2–O–CO––CO ) n
(Total 1 mark)

185.	How many hydrogen atoms are in one mole of ethanol, C2H5OH?
A.	1.00×1023
B.	3.61×1024
C.	5.00
D.	6.00
(Total 1 mark)

186.	What is the coefficient for H2SO4(aq) when the following equation is balanced, using the smallest possible integers?
__Mg3N2(s) + __H2SO4(aq) → __MgSO4(aq) + __(NH4)2SO4(aq)
A.	1
B.	3
C.	4
D.	7
(Total 1 mark)

187.	Air bags in cars inflate when sodium azide decomposes to form sodium and nitrogen:
	2NaN3(s) → 2Na(s) + 3N2(g)
	Calculate the amount, in moles, of nitrogen gas produced by the decomposition of 2.52 mol of NaN3(s).
A.	1.68
B.	2.52
C.	3.78
D.	7.56
(Total 1 mark)

188.	What volume, in cm3, of 0.200 mol dm–3 HCl(aq) is required to neutralize 25.0 cm3 of 0.200 mol dm–3 Ba(OH)2(aq)?
A.	12.5
B.	25.0
C.	50.0
D.	75.0
(Total 1 mark)

189.	Which species has 54 electrons and 52 protons?
A.	
B.	
C.	
D.	
(Total 1 mark)

190.	What is the correct sequence for the processes occurring in a mass spectrometer?
A.	vaporization, ionization, acceleration, deflection
B.	vaporization, acceleration, ionization, deflection
C.	ionization, vaporization, acceleration, deflection
D.	ionization, vaporization, deflection, acceleration
(Total 1 mark)

191.	Which series is arranged in order of increasing radius?
A.	Ca2+ < Cl– < K+
B.	K+ < Ca2+ < Cl–
C.	Ca2+ < K+ < Cl–
D.	Cl– < K+ < Ca2+
(Total 1 mark)

192.	What is the formula of the compound formed when aluminium reacts with oxygen?
A.	Al3O2
B.	Al2O3
C.	AlO2
D.	AlO3
(Total 1 mark)

193.	Which statement is true for compounds containing only covalent bonds?
A.	They are held together by electrostatic forces of attraction between oppositely charged ions.
B.	They are made up of metal elements only.
C.	They are made up of a metal from the far left of the periodic table and a non-metal from the far right of the periodic table.
D.	They are made up of non-metal elements only.
(Total 1 mark)

194.	How many electrons are used in the carbon-carbon bond in C2H2?
A.	4
B.	6
C.	10
D.	12
(Total 1 mark)

195.	Which compound has the highest boiling point?
A.	CH3CH2CH3
B.	CH3CH2OH
C.	CH3OCH3
D.	CH3CHO
(Total 1 mark)

196.	What type of solid materials are typically hard, have high melting points and poor electrical conductivities?
	I.	Ionic
II.	Metallic
III.	Covalent-network
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

197.	How much energy, in joules, is required to increase the temperature of 2.0 g of aluminium from 25 to 30 °C? (Specific heat of Al = 0.90 J g–1 K–1).
A.	0.36
B.	4.5
C.	9.0
D.	54
(Total 1 mark)

198.	Which combination is correct for a chemical reaction that absorbs heat from the surroundings?
	Type of reaction	ΔH at constant pressure	
A.	Exothermic	Positive	
B.	Exothermic	Negative	
C.	Endothermic	Positive	
D.	Endothermic	Negative	
(Total 1 mark)

199.	Using the equations below:
	C(s) + O2(g) → CO2(g)	∆Hο = –394 kJ mol–1
	Mn(s) + O2(g) → MnO2(s)	∆Hο = –520 kJ mol–1
	What is ∆H, in kJ, for the following reaction?
	MnO2(s) + C(s) → Mn(s) + CO2(g)
A.	914
B.	126
C.	–126
D.	–914
(Total 1 mark)

200.	Excess magnesium, was added to a beaker of aqueous hydrochloric acid. A graph of the mass of the beaker and contents was plotted against time (line 1).

	What change in the experiment could give line 2?
A.	The same mass of magnesium in smaller pieces
B.	The same volume of a more concentrated solution of hydrochloric acid
C.	A lower temperature
D.	A more accurate instrument to measure the time
(Total 1 mark)

201.	Which quantities in the enthalpy level diagram are altered by the use of a catalyst?

A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

202.	The sequence of diagrams represents the system as time passes for a gas phase reaction in which reactant X is converted to product Y.

	Which statement is correct?
A.	At t = 5 days the rate of the forward reaction is greater than the rate of the backward reaction.
B.	At t = 7 seconds the reaction has reached completion.
C.	At t = 10 minutes the system has reached a state of equilibrium.
D.	At t = 5 days the rate of the forward reaction is less than the rate of the backward reaction.
(Total 1 mark)

203.	What changes occur when the temperature is increased in the following reaction at equilibrium?
	Br2(g) + Cl2(g)  2BrCl(g)	∆Hο = +14 kJ mol–1
	Position of equilibrium	Value of equilibrium constant	
A.	Shifts towards the reactants	Decreases	
B.	Shifts towards the reactants	Increases	
C.	Shifts towards the products	Decreases	
D.	Shifts towards the products	Increases	
(Total 1 mark)

204.	Which species can act as a Lewis acid?
A.	BF3
B.	OH–
C.	H2O
D.	NH3
(Total 1 mark)

205.	Which substance, when dissolved in water, to give a 0.1 mol dm–3 solution, has the highest pH?
A.	HCl
B.	NaCl
C.	NH3
D.	NaOH
(Total 1 mark)

206.	What is the reducing agent in this reaction?
Cu(s) + (aq) + 4H+(aq) → Cu2+(aq) + 2NO2(g) + 2H2O(l)
A.	Cu(s)
B.	(aq)
C.	Cu2+(aq)
D.	H+(aq)
(Total 1 mark)

207.	A particular voltaic cell is made from magnesium and iron half-cells. The overall equation for the reaction occurring in the cell is
	Mg(s) + Fe2+(aq) → Mg2+(aq) + Fe(s)
	Which statement is correct when the cell produces electricity?
A.	Magnesium atoms lose electrons.
B.	The mass of the iron electrode decreases.
C.	Electrons flow from the iron half-cell to the magnesium half-cell.
D.	Negative ions flow through the salt bridge from the magnesium half-cell to the iron half-cell.
(Total 1 mark)

208.	What process occurs at the cathode in a voltaic cell and at the anode in an electrolytic cell?
	Cathode of voltaic cell	Anode of Electrolytic cell	
A.	Oxidation	Reduction	
B.	Oxidation	Oxidation	
C.	Reduction	Oxidation	
D.	Reduction	Reduction	
(Total 1 mark)

209.	Which statement about successive members of all homologous series is correct?
A.	They have the same empirical formula.
B.	They differ by a CH2 group.
C.	They have the same physical properties.
D.	They differ in their degree of unsaturation.
(Total 1 mark)

210.	The following is a three-dimensional representation of an organic molecule.

	Which statement is correct?
A.	The correct IUPAC name of the molecule is 2-methylpentane.
B.	All the bond angles will be approximately 90°.
C.	One isomer of this molecule is pentane.
D.	The boiling point of this compound would be higher than that of pentane.
(Total 1 mark)

211.	Which compound forms when hydrogen bromide is added to but-2-ene?
A.	2-bromobutane
B.	2,3-dibromobutane
C.	1-bromobutane
D.	1,2-dibromobutane
(Total 1 mark)

212.	Which products can be potentially obtained from crude oil and are economically important?
	I.	Plastics
II.	Margarine
III.	Motor fuel
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

213.	Propane, C3H8, undergoes incomplete combustion in a limited amount of air. Which products are most likely to be formed during this reaction?
A.	Carbon monoxide and water
B.	Carbon monoxide and hydrogen
C.	Carbon dioxide and hydrogen
D.	Carbon dioxide and water
(Total 1 mark)

214.	The following diagram shows a set of experimental data points, X, determined when one experimental measurement was repeated three times. The centre of the diagram represents the ideal value calculated from theory. What statement is correct about these measurements?
	
A.	The measurements involve low accuracy and low precision.
B.	The measurements involve low accuracy and high precision.
C.	The measurements involve high accuracy and low precision.
D.	The measurements involve high accuracy and high precision.
(Total 1 mark)

215.	What is the electron configuration for the copper(I) ion, (Z = 29)?
A.	[Ar]4s23d9
B.	[Ar]4s13d10
C.	[Ar]4s13d9
D.	[Ar]3d10
(Total 1 mark)

216.	Which salts form coloured solutions when dissolved in water?
	I.	FeCl3
II.	NiCl2
III.	ZnCl2
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

217.	How many sigma (σ) and pi (π) bonds are present in the structure of HCN?
	σ	π	
A.	1	3	
B.	2	3	
C.	2	2	
D.	3	1	
(Total 1 mark)

218.	How many lone pairs and bonding pairs of electrons surround xenon in the XeF4 molecule?
	Lone pairs	Bonding pairs	
A.	4	8	
B.	0	8	
C.	0	4	
D.	2	4	
(Total 1 mark)

219.	Which reaction has the most negative ∆Hο value?
A.	LiF(s) → Li+(g) + F–(g)
B.	Li+(g) + F–(g) → LiF(s)
C.	NaCl(s) → Na+(g) + Cl–(g)
D.	Na+(g) + Cl–(g) → NaCl(s)
(Total 1 mark)

220.	Which equation represents the electron affinity of calcium?
A.	Ca(g) →Ca+(g) + e–
B.	Ca(g) →Ca–(g) + e–
C.	Ca(g) + e– → Ca–(g)
D.	Ca+(g) + e– → Ca(g)
(Total 1 mark)

221.	Which reaction causes a decrease in the entropy of the system?
A.	CaCO3(s) → CaO(s) + CO2(g)
B.	2H2(g) + O2(g) → 2H2O(l)
C.	2C(s) + O2(g) → 2CO(g)
D.	2SO3(g) → 2SO2(g) + O2(g)
(Total 1 mark)

222.	What are the signs of ∆Hο and ∆Sο for a reaction that is non-spontaneous at low temperature but spontaneous at high temperature?
	DHο	DSο	
A.	–	–	
B.	+	–	
C.	–	+	
D.	+	+	
(Total 1 mark)

223.	What is the order of reaction with respect to NO2(g) and F2(g) given the following rate data at a certain temperature?
[NO2(g)] / mol dm–3	[F2(g)] / mol dm–3	Rate / mol dm–3 min–1	
0.1	0.2	0.1	
0.2	0.2	0.4	
0.1	0.4	0.2	

	Order with respect to NO2(g)	Order with respect to F2(g)	
A.	first	first	
B.	first	second	
C.	second	first	
D.	second	second	
(Total 1 mark)

224.	For the reaction below:
	H2(g) + I2(g)  2HI(g)
	at a certain temperature, the equilibrium concentrations, in mol dm–3, are
	[H2(g)] = 0.30, [I2(g)] = 0.30, [HI(g)] = 3.0
	What is the value of Kc?
A.	1.0×10–2
B.	10
C.	33
D.	1.0×102
(Total 1 mark)

225.	A liquid and its vapour are at equilibrium inside a sealed container. Which change will alter the equilibrium vapour pressure of the liquid in the container?
A.	Adding more liquid
B.	Adding more vapour
C.	Decreasing the volume of the container
D.	Decreasing the temperature
(Total 1 mark)

226.	Which methods will distinguish between equimolar solutions of a strong base and a strong acid?
I.	Add magnesium to each solution and look for the formation of gas bubbles.
II.	Add aqueous sodium hydroxide to each solution and measure the temperature change.
III.	Use each solution in a circuit with a battery and lamp and see how bright the lamp glows.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

227.	Which values are correct for a 0.010 mol dm–3 solution of NaOH(aq) at 298 K?
(Kw = 1.0×10–14 mol2 dm–6 at 298 K)
A.	[H+] = 1.0×10–12 mol dm–3 and pH = 12.00
B.	[OH–] = 1.0×10–12 mol dm–3 and pH = 12.00
C.	[H+] = 1.0×10–12 mol dm–3 and pOH = 12.00
D.	[OH–] = 1.0×10–12 mol dm–3 and pOH = 12.00
(Total 1 mark)

228.	At 25 °C, Ka for an acid is 1.0×10–2. What is the value of Kb for its conjugate base?
A.	1.0×102
B.	1.0×10–2
C.	1.0×1012
D.	1.0×10–12
(Total 1 mark)

229.	Which statement about indicators is always correct?
A.	The mid-point of the pH range of an indicator is 7.
B.	The pH range is greater for indicators with higher pKa values.
C.	The colour red indicates an acidic solution.
D.	The pKa value of the indicator is within its pH range.
(Total 1 mark)

230.	Consider the following reaction:
H2SO3(aq) + Sn4+(aq) + H2O(l) → Sn2+(aq) + HSO4–(aq) + 3H+(aq)
	Which statement is correct?
A.	H2SO3 is the reducing agent because it undergoes reduction.
B.	H2SO3 is the reducing agent because it undergoes oxidation.
C.	Sn4+ is the oxidizing agent because it undergoes oxidation.
D.	Sn4+ is the reducing agent because it undergoes oxidation.
(Total 1 mark)

231.	Which processes occur during the electrolysis of molten sodium chloride?
	I.	Sodium and chloride ions move through the electrolyte.
II.	Electrons move through the external circuit.
III.	Oxidation takes place at the anode.
A.	I and II only
B.	I and III only
C.	II and III only
D.	I, II and III
(Total 1 mark)

232.	Which equation represents the reduction process occurring in the standard hydrogen electrode?
A.	H2(g) → 2H+(aq) + 2e–
B.	H+(aq) + OH–(aq) → H2O(l)
C.	2H+(aq) + 2e– → H2(g)
D.	O2(g) + 4H+(aq) + 4e– → 2H2O(l)
(Total 1 mark)

233.	Which statement is correct about the value of Eο?
A.	The more positive the value of Eο, the greater the driving force for reduction.
B.	The more negative the value of Eο, the greater the driving force for reduction.
C.	The more positive the value of Eο, the greater the rate of reaction.
D.	The more negative the value of Eο, the greater the rate of reaction.
(Total 1 mark)

234.	Which combination is correct for the complex ion in [Co(NH3)4(H2O)Cl]Br?
	Oxidation state of cobalt	Shape of the complex ion	Overall charge of the
complex ion	
A.	+2	Octahedral	+2	
B.	+3	Octahedral	–1	
C.	+2	Octahedral	+1	
D.	+2	Tetrahedral	+1	
(Total 1 mark)

235.	What is the product of the following reaction?
	CH3CH2CH2CN + H2 
A.	CH3CH2CH2NH2
B.	CH3CH2CH2CH3
C.	CH3CH2CH2CH2CH3
D.	CH3CH2CH2CH2NH2
(Total 1 mark)

236.	What is the correct IUPAC name for the following compound?

A.	4-methylbutanenitrile
B.	4-methylpentanenitrile
C.	2-methylbutanenitrile
D.	2-methylpentanenitrile
(Total 1 mark)

237.	What is the organic product of the reaction between ethanol and ethanoic acid in the presence of sulfuric acid?
A.	CH3CHO
B.	CH3COOCH3
C.	CH3CH2COOCH3
D.	CH3COOCH2CH3
(Total 1 mark)

238.	Which compound can exist as optical isomers?
A.	H2NCH2COOH
B.	H3CCONH2
C.	H3CCHBrI
D.	HCOOCH3
(Total 1 mark)