IB Chemistry 12 SL – Grade 11 Review
1.
A burette reading is recorded as 27.70 ± 0.05 cm3. Which of the following could be the actual
value?
I.27.68 cm3
2.
3.
II.27.78 cm3
III.27.74 cm3
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
Density can be calculated by dividing mass by volume. 0.20 ± 0.02 g of a metal has a volume of
0.050 ± 0.005 cm3. How should its density be recorded using this data?
A.
4.0 ± 0.025 g cm–3
C.
4.00 ± 0.025 g cm–3
B.
4.0 ± 0.8 g cm–3
D.
4.00 ± 0.8 g cm–3
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
4.
A fixed mass of gas has a certain volume at a temperature of 50 °C. What temperature is required
to double its volume while keeping the pressure constant?
5.
A.
100 K
C.
373 K
B.
323 K
D.
646 K
What is the concentration of NaCl, in mol dm–3, when 10.0 cm3 of 0.200 mol dm–3 NaCl solution
is added to 30.0 cm3 of 0.600 mol dm–3 NaCl solution?
A.
0.450
C.
0.500
B.
0.300
D.
0.800
6.
What mass, in g, of hydrogen is formed when 3 mol of aluminium react with excess hydrochloric
acid according to the following equation?
2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)
7.
A.
3.0
C.
6.0
B.
4.5
D.
9.0
What is the approximate molar mass, in g mol–1, of MgSO4•7H2O?
A.
120
C.
138
B.
130
D.
246
IB Chemistry 12 SL – Grade 11 Review
8.
Chloroethene, C2H3Cl, reacts with oxygen according to the equation below.
2C2H3Cl(g) + 5O2(g) → 4CO2(g) + 2H2O(g) + 2HCl(g)
What is the amount, in mol, of H2O produced when 10.0 mol of C2H3Cl and 10.0 mol of O2 are
mixed together, and the above reaction goes to completion?
9.
A.
4.00
C.
10.0
B.
8.00
D.
20.0
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).
10.
A.
1.68
C.
3.78
B.
2.52
D.
7.56
What is the sum of all coefficients when the following equation is balanced using the smallest
possible whole numbers?
__ C2H2 + __O2 → __CO2 + __H2O
11.
12.
13.
A.
5
C.
11
B.
7
D.
13
How many oxygen atoms are there in 0.20 mol of ethanoic acid, CH3COOH?
A.
1.2 × 1023
C.
3.0 × 1024
B.
2.4 × 1023
D.
6.0 × 1024
8.5 g of NH3 are dissolved in H2O to prepare a 500 cm3 solution. Which statements are correct?
I.
NH3 is the solute and H2O is the solution
II.
The concentration of the solution is 17 g dm–3
III.
[NH3] = 1.0 mol dm–3
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
Which statement about the numbers of p, e and n in an atom is always correct?
A.
The number of neutrons minus the number of electrons is zero.
B.
The number of protons plus the number of neutrons equals the number of electrons.
IB Chemistry 12 SL – Grade 11 Review
14.
15.
16.
17.
18.
19.
20.
C.
The number of protons equals the number of electrons.
D.
The number of neutrons equals the number of protons.
Which of the following is an isotope of
24
12 Mg?
A.
24
2
12 Mg
C.
42
13 Mg
B.
26
12 Mg
D.
26
13 Mg
A sample of element X contains 69 % of 63X and 31 % of 65X. What is the relative atomic mass of
X in this sample?
A.
63.0
C.
65.0
B.
63.6
D.
69.0
Which describes the visible emission spectrum of hydrogen?
A.
A series of lines converging at longer wavelength
B.
A series of regularly spaced lines
C.
A series of lines converging at lower energy
D.
A series of lines converging at higher frequency
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
The relative molecular mass of a gas is 56 and its empirical formula is CH2. What is the molecular
formula of the gas?
A.
CH2
C.
C3H6
B.
C2H4
D.
C4H8
An atom of an element contains 19 electrons. In which group of the periodic table does it occur?
A.
1
C.
5
B.
2
D.
7
Which equation best represents the first ionization energy of magnesium?
A.
Mg(s) → Mg+(s) + e–
C.
Mg(g) → Mg+(g) + e–
B.
Mg(g) → Mg2+(g) + 2e–
D.
Mg(s) → Mg+(g) + e–
IB Chemistry 12 SL – Grade 11 Review
21.
22.
23.
24.
Which species has the largest radius?
A.
Cl–
C.
Na+
B.
K
D.
K+
Which statements about the periodic table are correct?
I.
Elements in period 3 have similar chemical properties.
II.
Elements in group 7 show a gradual change in physical properties.
III.
The position of an element in period 3 is related to the number of electrons in the
highest occupied energy level.
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
Which properties of the alkali metals decrease going down group 1?
A. First ionization energy and reactivity
C. Reactivity and electronegativity
B. Melting point and atomic radius
D. First ionization energy and melting
point
Which oxides produce an acidic solution when added to water?
I.
25.
26.
27.
P4O10
II.
MgO
III.
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
SO3
Which property decreases down group 7 in the periodic table?
A.
Melting point
C.
Atomic radius
B.
Electronegativity
D.
Ionic radius
Which property generally decreases across period 3?
A.
Atomic number
C.
Atomic radius
B.
Electronegativity
D.
First ionization energy
Which is the best description of the bonding present in the ammonium ion, NH4+?
A.
Sharing of electrons between atoms
B.
Electrostatic attraction between ions
C.
Electrostatic attraction between positive ions and delocalized electrons
D.
Sharing of electrons between atoms and electrostatic attraction between ions
IB Chemistry 12 SL – Grade 11 Review
28.
29.
Which pair of compounds is arranged in correct order of relative boiling points?
Lower Boiling Point
Higher Boiling Point
A.
H2S
H2O
B.
NH3
PH3
C.
HF
HCl
D.
CH3COOH
CH3CH2OH
The Lewis structure of SO2 is given below.
..
..
: O ―S
..
O:
..
What is the shape of the SO2 molecule?
30.
31.
A.
Bent (V-shaped)
C.
T-shaped
B.
Linear
D.
Triangular planar
Which compound forms hydrogen bonds in the liquid state?
A.
C2H5OH
C.
CH3CHO
B.
CHCl3
D.
(CH3CH2)3N
How do the bond angles in CH4, NH3 and H2O compare?
A.
CH4
=
NH3
=
H2O
C.
NH3
<
CH4
<
H2O
B.
CH4
<
NH3
<
H2O
D.
H2O
<
NH3
<
CH4
32. What type of solid materials are typically hard, have high melting points and poor electrical
conductivities?
I.
II.
III.
33.
Ionic
Metallic
Covalent-network
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
Which species contain a dative covalent bond?
I.
HCHO
II.
CO
III.
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
H3O+
IB Chemistry 12 SL – Grade 11 Review
34.
The electronegativities of four different elements are given below (the letters are not their
chemical symbols).
Element
W
X
Y
Z
Electronegativity
0.9
1.2
3.4
4.0
Based on this information which statement is correct?
35.
36.
37.
38.
39.
40.
A.
W is a non-metal.
C.
Y is a metal.
B.
W and X form an ionic
compound.
D.
Y and Z form a covalent
compound.
Which molecule has a non-bonding (lone) pair of electrons on the central atom?
A.
BF3
C.
CO2
B.
SO2
D.
SiF4
How many electrons are used in the carbon-carbon bond in C2H2?
A.
4
C.
10
B.
6
D.
12
Which molecule is polar?
A.
CH2Cl2
C.
Cl2
B.
BCl3
D.
CCl4
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.
Which particles are responsible for electrical conductivity in metals?
A.
Anions
C.
Electrons
B.
Cations
D.
Protons
Which equation represents the bond enthalpy for the H–Br bond in hydrogen bromide?
A.
HBr(g) → H(g) + Br(g)
B.
HBr(g) → H(g) + Br(l)
C.
HBr(g) → H(g) +
1
Br2(1)
2
D.
HBr(g) → H(g) +
1
Br2(g)
2
IB Chemistry 12 SL – Grade 11 Review
41.
Use the average bond enthalpies below to calculate the enthalpy change, in kJ, for the following
reaction.
H2(g) + I2(g) → 2HI(g)
42.
43.
44.
Bond
Bond energy / kJ mol–1
H–H
440
I–I
150
H–I
300
A.
+290
C.
–10
B.
+10
D.
–290
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.
Which statement is correct given the enthalpy level diagram?
A.
The reaction is endothermic and the products are more
thermodynamically stable than the reactants.
B.
The reaction is exothermic and the products are more
thermodynamically stable than the reactants.
C.
The reaction is endothermic and the reactants are more thermodynamically stable than the
products.
D.
The reaction is exothermic and the reactants are more thermodynamically stable than the
products.
Which types of reaction are always exothermic?
I.Neutralization
II.Decomposition
III. Combustion
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
IB Chemistry 12 SL – Grade 11 Review
45. A pure aluminium block with a mass of 10 g is heated so that its temperature increases from 20 °C
to 50 °C . The specific heat capacity of aluminium is 8.99 × 10–1 J g–1 K–1. Which expression gives the
heat energy change in kJ?
46.
A.
10 × 8.99 × 10–1 × 303
B.
10 × 8.99 × 10–1 × 30
C.
10  8.99  10 1  303
1000
D.
10  8.99  10 1  30
1000
Consider the two reactions involving iron and oxygen.
2Fe(s) + O2(g) → 2FeO(s)
4Fe(s) + 3O2(g) → 2Fe2O3(s)
∆HO = –544 kJ
∆HO = –1648 kJ
What is the enthalpy change, in kJ, for the reaction below?
4FeO(s) + O2(g) → 2Fe2O3(s)
47.
A.
–1648 – 2(–544)
C.
–1648 – 544
B.
–544 – (–1648)
D.
–1648 – 2(544)
Which is the correct classification of these alcohols?
1
2
1
48.
2
3
3
A.
tertiary
secondary
primary
B.
tertiary
primary
secondary
C.
tertiary
tertiary
secondary
D.
secondary
primary
secondary
Halogenoalkanes can undergo SN1 and SN2 reactions with aqueous sodium hydroxide.
Which halogenoalkane will react fastest with a 0.1 mol dm–3 solution of aqueous sodium
hydroxide?
A.
2-chloro-2-methylpropane
C.
1-chlorobutane
B.
2-iodo-2-methylpropane
D.
1-iodobutane
IB Chemistry 12 SL – Grade 11 Review
49. Which type of reaction occurs when 2-iodo-2-methylpropane, C(CH3)3I, reacts with aqueous
sodium hydroxide, NaOH(aq)?
50.
51.
52.
53.
54.
A.
Addition
C.
SN1
B.
Free-radical substitution
D.
SN2
Which reaction pathway describes how ethanol can be formed?
A.
addition
elimination
 chloroethane 
  ethanol
ethene  
B.
substitution
nucleophilic substitution
 chloroethane 

 ethanol
ethane   
C.
substitution
 ethanol
ethene   
D.
addition
 ethanol
ethane  
Which of the following pairs are members of the same homologous series?
A.
CH3CH2CH2OH and CH3CH2CHO
B.
CH3CH(OH)CH3 and CH3CH2CH(OH)CH3
C.
CH3COCH3 and CH3CH2COOH
D.
CH3COCH2CH3 and CH3CH2CHO
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
Which equations represent the incomplete combustion of methane?
I.
CH4(g) + 2O2(g) → CO2(g) + 2H2
II.
CH4(g) + 1½O2(g) → CO(g) + 2H2O(g)
III.
CH4(g) + O2(g) → C(s) + 2H2O(g)
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
When bromine water is shaken with a liquid organic compound, it is rapidly decolorized. What is
the identity of the compound?
A.
alcohol.
C.
B.
alkane.
D.
alkene.
iodoalkane
IB Chemistry 12 SL – Grade 11 Review
55.
56.
Which of the following are isomers of pentane?
I.
2-methylpentane
II.
methylbutane
III.
dimethylpropane
A.
I and II only
C.
II and III only
B.
I and III only
D.
I, II and III
What is the product of the following reaction?
2

Cr2 O 7 /H


CH3CH(OH)CH3 
57.
58.
59.
60.
A.
CH3COOH
C.
CH3CH2COOH
B.
CH3COCH3
D.
CH3CH2CH3
What is the structural formula of 2,3-dibromo-3-methylhexane?
A.
CH3CHBrCHBrCH(CH3)CH2CH3
B.
CH3CHBrCBr(CH3)CH2CH2CH3
C.
CH3CH2CHBrCBr(CH2CH3)2
D.
CH3CHBrCHBrCH(CH2CH3)2
What is the IUPAC name for CH3CH2CH(CH3)CH3?
A.
1,1-dimethylpropane
C.
2-methylbutane
B.
2-ethylpropane
D.
3-methylbutane
Which of the following statements about alkenes is not correct?
A.
They have reactive double bonds.
C.
They react mainly by substitution.
B.
They can form addition polymers.
D.
They can react with water to form
alcohols.
Which statement about bonding is correct?
A.
Bond breaking is endothermic and requires energy.
B.
Bond breaking is endothermic and releases energy.
C.
Bond making is exothermic and requires energy.
D.
Bond making is endothermic and releases energy.