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Chemistry Workbook
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Richard Harwood and Ian Lodge
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Cambridge IGCSE®
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Physical Science
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Chemistry Workbook
Original material © Cambridge University Press 2016
Prelims_Chem.indd i
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Original material © Cambridge University Press 2016
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Contents v vi
C1 The particulate nature of matter C1.1 Changing physical state C1.2 Plotting a cooling curve
1 1 3
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C2 Experimental techniques C2.1 Diffusion, solubility and separation C2.2 Chromatography at the races
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Introduction Periodic table
7 7 10
C3 Atoms, elements and compounds C3.1 Atomic structure C3.2 The first four periods C3.3 The chemical bonding in simple molecules C3.4 The nature of ionic lattices
12 12 13 15 16
C4 Stoichiometry
17
Formulae of ionic compounds Making magnesium oxide – a quantitative investigation The analysis of titration results Calculating formula masses A sense of proportion in chemistry Finding the mass of 5 cm of magnesium ribbon Reacting volumes of gases
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C4.1 C4.2 C4.3 C4.4 C4.5 C4.6 C4.7
iii
17 19 22 24 26 27 29
C5 Electricity and chemistry C5.1 The nature of electrolysis C5.2 Making and ‘breaking’ copper chloride
31 31 33
C6 Energy changes in chemical reactions C6.1 Energy diagrams C6.2 The collision theory of reaction rates C6.3 The influence of surface area on the rate of reaction C6.4 Finding the rate of a reaction producing a gas
36 36 38 39 43
C7 Acids, bases and salts C7.1 Acid and base reactions – neutralisation C7.2 Types of salt C7.3 Descaling a coffee machine C7.4 Thermochemistry – investigating the neutralisation of an acid by an alkali
46 46 47 48 50
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54 54 56 58
C9 Metals C9.1 The reactivity series of metals C9.2 Energy from displacement reactions C9.3 Metals and alloys
59 59 61 64
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C8 The Periodic Table C8.1 Trends in the halogens C8.2 Displacement reactions of the halogens C8.3 Group I: The alkali metals
66 66 69
C11 Organic chemistry C11.1 Families of hydrocarbons C11.2 Unsaturated hydrocarbons (the alkenes) C11.3 The alcohols as fuels C11.4 Essential processes of the petrochemical industry C11.5 Addition polymerisation
72 73 74 76 79 81
C12 Analysis C12.1 Titration analysis C12.2 Chemical analysis C12.3 Planning a controlled experiment C12.4 Chemical testing and evaluation C12.5 Experimental design
82 82 84 88 91 94
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iv
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C10 Air and water C10.1 Atmospheric pollution, industry and transport C10.2 Clean water is crucial
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Glossary
Introduction This workbook contains exercises designed to help you develop the skills needed for success in Cambridge IGCSE Physical Science.
AO1 Knowledge with understanding AO2 Handling information and problem solving AO3 Experimental skills and investigations.
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The examination tests three different Assessment Objectives, or AOs for short. These are:
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In the examination, about 50% of the marks are for AO1, 30% for AO2 and 20% for AO3. Just learning your work and remembering it is therefore not enough to make sure that you get the best possible grade in the exam. Half of all the marks are for AO2 and AO3. You need to be able to use what you’ve learned in unfamiliar contexts (AO2) and to demonstrate your experimental skills (AO3). This workbook contains exercises to help you to develop AO2 and AO3 further. There are some questions that just involve remembering things you have been taught (AO1), but most of the questions require you to use what you’ve learned to work out, for example, what a set of data means, or to suggest how an experiment might be improved. These exercises are not intended to be exactly like the questions you will get on your exam papers. This is because they are meant to help you to develop your skills, rather than testing you on them.
There’s an introduction at the start of each exercise that tells you the purpose of it – which skills you will be working with as you answer the questions.
v
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For some parts of the exercises, there are self-assessment checklists. You can try marking your own work using these. This will help you to remember the important points to think about. Your teacher should also mark the work and will discuss with you whether your own assessments are right. The exercises cover both Core and Supplement material of the syllabus. The Supplement material can be identified by the Supplement bar in the margin (as shown). This indicates that the exercise is intended for students who are studying the Supplement content of the syllabus as well as the Core.
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II
a = relative atomic mass
X
b
X = atomic symbol b = proton (atomic) number
F
9
Ne
Helium 4 10
He
Group
8
2
VIII / 0
O
Neon 20 18
VII
7
Ar
VI
N
Fluorine 19 17
Argon 40 36
V
6
Cl
Kr
IV
C
Chlorine 35.5 35
III
H
5
S
Oxygen 16 16
Br
1
Hydrogen 1
B
Sulfur 32 34
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I
a
P
Nitrogen 14 15
Se
4
Carbon 12 14
Phosphorus 31 33 30
3
Key
Si
As
Zn
Be
Boron 11 13
Silicon 28 32 29
Li
Al
Ge
Cu
Beryllium 9 12
Aluminium 27 31 28
Mg
Ga
Ni
Lithium 7 11
22
27
Na
Ti
Co
25
21
26
Mn
Sc Fe
24
Krypton 84 54
Cr
Xe
V
I
Bromine 80 53
23
Selenium 79 52
Magnesium 24 20
Te
Ca
Arsenic 75 51
Sodium 23 19
Sb
K
Germanium 73 50 Iron 56 44
Sn Ru
Gallium 70 49
Manganese 55 43
In Tc
Zinc 65 48
Chromium 52 42
Cd
Mo
Copper 64 47
Vanadium 51 41
Ag
Nb
Zr
Titanium 48 40
Y
Scandium 45 39
Nickel 59 46
Calcium 40 38
Pd
Sr
Cobalt 59 45
Potassium 39 37
Rh
Rb
Xenon 131 86
–
Rn
Technetium
Iodine 127 85
Rhodium 103 77
At
Ir
Tellurium 128 84
Ruthenium 101 76
Po
Os
Antimony 122 83 75
Bi
Re
Tin 119 82
Molybdenum 96 74
Pb
W
Indium 115 81
Niobium 93 73
Tl
Ta
Zirconium 91 72
Cadmium 112 80
Hf
Yttrium 89 57 *
Hg
La
Silver 108 79
Strontium 88 56
Au
Ba
Platinum 195 110
Palladium 106 78
Rubidium 85 55
Ds
Pt
Cs
Indium 192 109
Radon 222 118
Mt
Uuo
Osmium 190 108
Astatine 210 117
Hs
Uus
Rhenium 186 107
Polonium 209 116
Bh
Lv
Tungsten 184 106
Bismuth 209 115
Sg
Uup
Tantalum 181 105
Fl
Db
Lead 207 114
Rf
Hafnium 179 104
Thallium 204 113
Lanthanum 139 † 89
Uut
Ac
Mercury 201 112
Barium 137 88
Cn
Ra
Gold 197 111
Caesium 133 87
Rg
Fr
Ununoctium
Meitnerium 268
Eu
63
Gd
64
Bk
Terbium 159 97
Tb
65
Cf
Dysprosium 163 98
Dy
66
Es
Holmium 165 99
Ho
67
Fm
Erbium 167 100
Er
68
–
Md
Thulium 169 101
Tm
69
–
No
Ytterbium 173 102
Yb
70
Lr
Lutetium 175 103
Lu
71
Lawrencium 262
–
62
Gadolinium 157 96
–
Hassium 265
Sm
Cm
Ununpentium Livermorium
61
Europium 152 95
Nobelium 259
–
Bohrium 264
Pm
Am
Mendelevium 258
Flerovium
60
Samarium 150 94
Fermium 257
–
Seaborgium 263
Nd
Pu
Einsteinium 252
–
59
Promethium 145 93
Californium 251
Darmstadtium Roentgenium 281 273 Dubnium 262
Pr
Np
Berkelium 247
Rutherfordium 261
Original material © Cambridge University Press 2016
Ununseptium
Actinium 227
Ununtrium
Radium 226
Copernicium
Francium 223
Praseodymium
U
Neodymium 144 92
Curium 247
58
141 91
Americium 243
Ce
*58–71 Lanthanoid series
Pa
Plutonium 244
Cerium 140 90
Neptunium 237
Th
†90–103 Actinoid series
Uranium 238 Protactinium 231
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Thorium 232
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The Periodic Table
C1: The particulate nature of matter DEFINITIONS TO LEARN
physical state: the three states of matter are solid, liquid and gas condensation: the change of state from gas to liquid freezing: the change of state from liquid to solid at the melting point
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melting: the change of state from solid to liquid boiling: the change of state from liquid to gas at the boiling point of the liquid evaporation: the change of state from liquid to gas below the boiling point sublimation: the change of state directly from solid to gas (or the reverse)
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crystallisation: the formation of crystals when a saturated solution is left to cool
Exercise C1.1 Changing physical state
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The graph shows the heating curve for a pure substance. The temperature rises with time as the substance is heated.
Temperature / ÂşC
This exercise will develop your understanding of the kinetic model and the energy changes involved in changes of physical state.
1
D
115
C B
17
A 0
0
Time
a What physical state(s) is the substance in at points A, B, C and D? A
C
B
D
b What is the melting point of the substance? c What is its boiling point?
d What happens to the temperature while the substance is changing state?
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Cambridge IGCSE Physical Science
e The substance is not water. How do we know this from the graph?
Complete the passage using the words given below. different
diffusion
gas
spread
particles
diffuse
random
lattice
vibrate
temperature
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f
in a liquid and a
The kinetic model states that the
are in constant motion. In a gas, the particles are far apart from each other and their motion is said to be
. The particles in a solid are held in fixed positions in a regular
positions.
about their fixed
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. In a solid, the particles can only
Liquids and gases are fluid states. When particles move in a fluid, they can collide with each other. When they collide, they bounce off each other in mixed, the different types of particle
directions. If two gases or liquids are
out and get mixed up. This process is called
.
2
particles that have a lower mass move faster than those with higher
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At the same
mass. This means that the lighter particles will spread and mix more quickly; the lighter particles are said to faster than the heavier particles.
g Use the data given for the substances listed below to answer the questions that follow on their physical state at a room temperature of 25 °C and atmospheric pressure.
Substance sodium
Melting point / °C
Boiling point / °C
98
883
−71
−62
ethanol
−117
78
cobalt
1492
2900
nitrogen
−210
−196
propane
−188
−42
16
118
radon
ethanoic acid
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C1: The particulate nature of matter
i
Which substance is a liquid over the smallest range of temperature?
ii
Which two substances are gaseous at −50 °C? and Which substance has the lowest freezing point?
iv
Which substance is liquid at 2500 °C?
v
A sample of ethanoic acid was found to boil at 121 °C at atmospheric pressure. Use the information in the
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iii
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table to comment on this result.
Exercise C1.2 Plotting a cooling curve
This exercise presents data obtained practically for plotting a cooling curve. It will help develop your skills in handling the data and interpreting what changes the different regions of the curve represent. Examples of sublimation are also discussed.
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A student, carried out the following data-logging experiment as part of a project on changes of state. An organic crystalline solid was melted by placing it in a tube in a boiling water bath. A temperature sensor was placed in the liquid.
computer
3
temperature sensor
bath of boiling water
magnetic stirrer
The temperature change was followed as the liquid was allowed to cool down. The data shown in the table below are taken from the computer record of the temperature change as the liquid cooled down to room temperature. Time / min
0
0.5
1.0
1.5
2.0
2.2
2.4
2.6
2.8
3.0
3.5
4.0
4.5
5.0
Temperature / °C 96.1 89.2
85.2
82.0
80.9
80.7
80.6
80.6
80.5
80.3
78.4
74.2
64.6
47.0
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Cambridge IGCSE Physical Science
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4
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a On the grid below, plot a graph of the temperature change taking place in this experiment.
b What change is taking place over the second minute of the experiment?
c Why does the temperature remain almost constant over this period of time? Give your explanation in terms of what is happening to the organisation of the molecules of the substance.
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C1: The particulate nature of matter
d What change would need to be made to carry out the experiment using a compound with a melting point greater than 100 °C?
e A similar experiment was carried out to demonstrate the cooling curve for paraffin wax. In the space below, sketch the shape of the graph you would expect to produce.
ii
Explain why the curve is the shape you have drawn.
f
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i
5
Sublimation occurs when a substance passes between the solid and gaseous states without going through
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the liquid phase. Both carbon dioxide and water can sublime under certain conditions of temperature and pressure.
‘Dry ice’ is the solid form of carbon dioxide used in commercial refrigeration. At atmospheric pressure it has a ‘sublimation point’ of –78.5°C. i
What difference can you see between solid carbon dioxide and water ice at atmospheric pressure?
ii
If you gently shake a carbon dioxide fire extinguisher, you will feel the presence
CO2
of liquid within the extinguisher. What conditions within the extinguisher mean that the CO2 is liquid in this case?
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Cambridge IGCSE Physical Science
iii
Complete the following paragraph about a particular type of frost using the words listed below. surrounding
liquid
colder
white
crystals
ice
Hoar frost is a powdery
humid
frost caused when solid
air. Water vapour is deposited on a surface as fine ice
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6
phase.
without
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going through the
than the
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air. The solid surface on which it is formed must be
forms from
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Cambridge IGCSE Physical Science
Exercise C12.3 Planning a controlled experiment
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The questions in this exercise illustrate the issues faced when designing experiments that will give you results that are clear. They will help you think through which conditions need to be controlled in a given situation so that a fair test can be carried out. They do not show all possible situations but will give an idea of the range of investigations you may encounter.
a Sudso is a washing powder which has been designed to work best at 30 °C. ‘Mr Jones’ has always done her
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washing at 50 °C and thinks that that temperature will work better.
Fo ro u res tstan ult din sa g t
30 °
C!
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88
lts at resu nding a t s t u For o
! 30 °C
Devise an experiment to discover which temperature is best for the washing powder Sudso.
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