FOR THE
IB DIPLOMA
PROGRAMME
THIRD EDITION
Chemistry
Christopher Talbot
Chris Davison
David Fairley
Practice
Exam-style
Questions
,Contents
Structure . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1 Models of the particulate nature of matter . . . . . . 000
S1.1 Introduction to the particulate nature of matter . . . . . . . . . . . . . . . 000
S1.2 The nuclear atom . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1.3 Electron configuration . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1.4 Counting particles by mass: the mole. . . . . . . . . . . . . . . . . . . . . . . 000
S1.5 Ideal gases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2 Models of bonding and structure . . . . . . . . . . . . . . . . 000
S2.1 The ionic model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.2 The covalent model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.3 The metallic model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.4 From models to materials . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S3 Classification of matter . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S3.1 The periodic table: classification of elements . . . . . . . . . . . . . . . . . 000
S3.2 Functional groups: classification of compounds . . . . . . . . . . . . . . . 000
Reactivity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1 What drives chemical reactions? . . . . . . . . . . . . . . . . . 000
R1.1 Measuring enthalpy changes . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.2 Energy cycles in reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.3 Energy from fuels . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.4 Entropy and spontaneity (HL) . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R2 How much, how fast and how far? . . . . . . . . . . . . . . 000
R2.1 How much? : the amount of chemical change . . . . . . . . . . . . . . . . . 000
R2.2 How fast? : the rate of chemical change . . . . . . . . . . . . . . . . . . . . . 000
R2.3 How far? : the extent of chemical change. . . . . . . . . . . . . . . . . . . . 000
R3 What are the mechanisms of chemical change? . 000
R3.1 Proton transfer reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.2 Electron transfer reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.3 Electron sharing reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.4 Electron pair sharing reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
,S1.1 Introduction to the particulate nature of matter
■ Paper 1 6 Which physical processes could be used to separate
1 Which equation represents sublimation? decane (C10H22) and water. The two liquids are
immiscible and have different boiling points.
A 2Al (s) + 3Cl2 (g) → 2AlCl3 (s)
1 distillation
B C10H16O (s) → C10H16O (g)
2 filtration
C CO2 (g) → CO2 (s)
3 sublimation
MgCO3 (s) + MgCl2 (aq) +
D → 4 use of a separating funnel
2HCl (aq) H2O (l) + CO2 (g)
2 Which statements about mixtures are correct? A 1, 2, 3 and 4
I The components may be elements or compounds. B 1, 2 and 3 only
II All mixtures are homogeneous. C 1 and 2 only
III The components can be separated by D 1 and 4 only
physical means. 7 A colourless solid crystalline sample was heated from
A I and II only a temperature of 25 °C (standard conditions) until
B I and III only it completely melted to form a colourless liquid. As
the temperature starts to rise again the state change
C II and III only
is complete.
D I, II and III
3 Which change of state is exothermic?
Temperature / °C
Z
A I2 (s) → I2 (g)
B NH3 (l) → NH3 (g)
C H2O (g) → H2O (l)
D Cu (s) → Cu (l) Time / s
4 Which statement about sodium oxide is true? State which of the following statements best explains the
A It is a homogenous mixture. shape of the graph at region Z.
B It melts overs a range of temperature. A There was no further heating.
C It has a fixed composition by mass. B The particles do not have any kinetic and
D It can be separated into sodium and oxygen by potential energy.
physical means. C A chemical reaction has taken place as the solid
5 A new substance was discovered and a series of was melted.
experiments were carried out on it. Which observation D Heat energy is used to separate the solid particles
suggests that the substance cannot be an element? from their fixed positions in the lattice.
A Electrolysis of the molten substance gave 8 Benzenecarboxylic acid is widely used in the food
two products. industry as a food preservative. The melting and boiling
B It reacted and dissolved in water to give a points of benzenecarboxylic acid are given below.
colourless solution and a gas. melting point of 122 °C boiling point of 249 °C
C It has fixed melting and boiling points (under Which of the following will occur to the molecules of
standard conditions). benzenecarboxylic acid when it is cooled from 260 °C
D When heated in oxygen it can form two oxides. to 100 °C?
Distance between molecules Kinetic energy of particles
A decreases decreases
B increases decreases
C increases increases
D decreases increases
Chemistry for the IB Diploma Programme S1.1 Introduction to the particulate nature of matter 1
, 9 Which of the following is not true about the Kelvin 13 The diagrams below show the arrangement of particles
scale of temperature? in a substance at the same pressure and at temperatures
A The values on the absolute scale are directly −90 °C and −70 °C.
proportional to the average kinetic energy of the
particles.
B To convert a temperature on the Celsius scale
to the absolute scale, subtract 273.15 from the
Celsius temperature.
C A kelvin has the same size as Celsius degree.
−90−90
°C °C −70−70
°C °C
D Absolute zero corresponds to the absence
of molecular movement. Which of the following could be the property of
10 The black and white balls represent atoms of the substance?
different elements. Melting point / °C Boiling point / °C
A −100 −75
AA CC
B −110 −65
C −66 −32
D −80 −60
14 Which statement about the kinetic molecular theory is
not true?
BB DD A It explains why ionic salts have different
solubilities in water.
B It explains the changes of state, boiling and freezing.
C It explains the difference in physical properties
of solids, liquids and gases.
D It explains the diffusion of gases in air.
Which diagram shows a mixture of only compounds? 15 Which of the following best explains why iodine slowly
11 Which statement most clearly indicates that diamond sublimes under standard conditions?
and graphite are forms of pure elemental carbon? A The iodine molecules at the surface reacts
A Both are crystalline solids. with oxygen.
B Complete combustion of equal masses of both B The iodine is heated and decomposes to form a
solids at high temperature produces equal masses gaseous product.
of carbon dioxide. C Solid iodine is unstable.
C Graphite is an electrical conductor, but diamond D Iodine molecules at the surface gain sufficient
is an electrical insulator. kinetic energy to escape as gas.
D Under high pressure graphite can be partially 16 Which one of the following correctly describes the
converted to diamond. properties of a molecular liquid?
12 It is suspected that a coloured juice contains a low A Hard to compress; has a fixed shape and a
concentration of a poisonous green dye with a boiling fixed volume.
point of 75 °C in addition to two harmless yellow and B Hard to compress; has no fixed shape but has a
green dyes with boiling points of 72 °C and 75 °C. fixed volume.
Which is the most suitable separation technique by C Easy to compress; has no fixed shape but a
which the green dye may be detected? fixed volume.
A recrystallization D Easy to compress; has a fixed shape, but no
B fractional distillation fixed volume.
C paper chromatography
D evaporation
Chemistry for the IB Diploma Programme S1.1 Introduction to the particulate nature of matter 2
IB DIPLOMA
PROGRAMME
THIRD EDITION
Chemistry
Christopher Talbot
Chris Davison
David Fairley
Practice
Exam-style
Questions
,Contents
Structure . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1 Models of the particulate nature of matter . . . . . . 000
S1.1 Introduction to the particulate nature of matter . . . . . . . . . . . . . . . 000
S1.2 The nuclear atom . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1.3 Electron configuration . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S1.4 Counting particles by mass: the mole. . . . . . . . . . . . . . . . . . . . . . . 000
S1.5 Ideal gases . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2 Models of bonding and structure . . . . . . . . . . . . . . . . 000
S2.1 The ionic model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.2 The covalent model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.3 The metallic model . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S2.4 From models to materials . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S3 Classification of matter . . . . . . . . . . . . . . . . . . . . . . . . . . 000
S3.1 The periodic table: classification of elements . . . . . . . . . . . . . . . . . 000
S3.2 Functional groups: classification of compounds . . . . . . . . . . . . . . . 000
Reactivity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1 What drives chemical reactions? . . . . . . . . . . . . . . . . . 000
R1.1 Measuring enthalpy changes . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.2 Energy cycles in reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.3 Energy from fuels . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R1.4 Entropy and spontaneity (HL) . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R2 How much, how fast and how far? . . . . . . . . . . . . . . 000
R2.1 How much? : the amount of chemical change . . . . . . . . . . . . . . . . . 000
R2.2 How fast? : the rate of chemical change . . . . . . . . . . . . . . . . . . . . . 000
R2.3 How far? : the extent of chemical change. . . . . . . . . . . . . . . . . . . . 000
R3 What are the mechanisms of chemical change? . 000
R3.1 Proton transfer reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.2 Electron transfer reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.3 Electron sharing reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
R3.4 Electron pair sharing reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . 000
,S1.1 Introduction to the particulate nature of matter
■ Paper 1 6 Which physical processes could be used to separate
1 Which equation represents sublimation? decane (C10H22) and water. The two liquids are
immiscible and have different boiling points.
A 2Al (s) + 3Cl2 (g) → 2AlCl3 (s)
1 distillation
B C10H16O (s) → C10H16O (g)
2 filtration
C CO2 (g) → CO2 (s)
3 sublimation
MgCO3 (s) + MgCl2 (aq) +
D → 4 use of a separating funnel
2HCl (aq) H2O (l) + CO2 (g)
2 Which statements about mixtures are correct? A 1, 2, 3 and 4
I The components may be elements or compounds. B 1, 2 and 3 only
II All mixtures are homogeneous. C 1 and 2 only
III The components can be separated by D 1 and 4 only
physical means. 7 A colourless solid crystalline sample was heated from
A I and II only a temperature of 25 °C (standard conditions) until
B I and III only it completely melted to form a colourless liquid. As
the temperature starts to rise again the state change
C II and III only
is complete.
D I, II and III
3 Which change of state is exothermic?
Temperature / °C
Z
A I2 (s) → I2 (g)
B NH3 (l) → NH3 (g)
C H2O (g) → H2O (l)
D Cu (s) → Cu (l) Time / s
4 Which statement about sodium oxide is true? State which of the following statements best explains the
A It is a homogenous mixture. shape of the graph at region Z.
B It melts overs a range of temperature. A There was no further heating.
C It has a fixed composition by mass. B The particles do not have any kinetic and
D It can be separated into sodium and oxygen by potential energy.
physical means. C A chemical reaction has taken place as the solid
5 A new substance was discovered and a series of was melted.
experiments were carried out on it. Which observation D Heat energy is used to separate the solid particles
suggests that the substance cannot be an element? from their fixed positions in the lattice.
A Electrolysis of the molten substance gave 8 Benzenecarboxylic acid is widely used in the food
two products. industry as a food preservative. The melting and boiling
B It reacted and dissolved in water to give a points of benzenecarboxylic acid are given below.
colourless solution and a gas. melting point of 122 °C boiling point of 249 °C
C It has fixed melting and boiling points (under Which of the following will occur to the molecules of
standard conditions). benzenecarboxylic acid when it is cooled from 260 °C
D When heated in oxygen it can form two oxides. to 100 °C?
Distance between molecules Kinetic energy of particles
A decreases decreases
B increases decreases
C increases increases
D decreases increases
Chemistry for the IB Diploma Programme S1.1 Introduction to the particulate nature of matter 1
, 9 Which of the following is not true about the Kelvin 13 The diagrams below show the arrangement of particles
scale of temperature? in a substance at the same pressure and at temperatures
A The values on the absolute scale are directly −90 °C and −70 °C.
proportional to the average kinetic energy of the
particles.
B To convert a temperature on the Celsius scale
to the absolute scale, subtract 273.15 from the
Celsius temperature.
C A kelvin has the same size as Celsius degree.
−90−90
°C °C −70−70
°C °C
D Absolute zero corresponds to the absence
of molecular movement. Which of the following could be the property of
10 The black and white balls represent atoms of the substance?
different elements. Melting point / °C Boiling point / °C
A −100 −75
AA CC
B −110 −65
C −66 −32
D −80 −60
14 Which statement about the kinetic molecular theory is
not true?
BB DD A It explains why ionic salts have different
solubilities in water.
B It explains the changes of state, boiling and freezing.
C It explains the difference in physical properties
of solids, liquids and gases.
D It explains the diffusion of gases in air.
Which diagram shows a mixture of only compounds? 15 Which of the following best explains why iodine slowly
11 Which statement most clearly indicates that diamond sublimes under standard conditions?
and graphite are forms of pure elemental carbon? A The iodine molecules at the surface reacts
A Both are crystalline solids. with oxygen.
B Complete combustion of equal masses of both B The iodine is heated and decomposes to form a
solids at high temperature produces equal masses gaseous product.
of carbon dioxide. C Solid iodine is unstable.
C Graphite is an electrical conductor, but diamond D Iodine molecules at the surface gain sufficient
is an electrical insulator. kinetic energy to escape as gas.
D Under high pressure graphite can be partially 16 Which one of the following correctly describes the
converted to diamond. properties of a molecular liquid?
12 It is suspected that a coloured juice contains a low A Hard to compress; has a fixed shape and a
concentration of a poisonous green dye with a boiling fixed volume.
point of 75 °C in addition to two harmless yellow and B Hard to compress; has no fixed shape but has a
green dyes with boiling points of 72 °C and 75 °C. fixed volume.
Which is the most suitable separation technique by C Easy to compress; has no fixed shape but a
which the green dye may be detected? fixed volume.
A recrystallization D Easy to compress; has a fixed shape, but no
B fractional distillation fixed volume.
C paper chromatography
D evaporation
Chemistry for the IB Diploma Programme S1.1 Introduction to the particulate nature of matter 2
