chemistry IGCSE

C a m b r i d g e i g cs e e x a m q u e s t i o n s

8 Iron is a transition element. 10 Zinc is extracted from zinc blende, ZnS.

a W hich three of the following six statements a Zinc blende is heated in air to give zinc oxide

about transition elements are correct? and sulfur dioxide.

i The metals are highly coloured e.g. yellow, Most of the sulfur dioxide is used to make sulfur

green, blue. trioxide. This is used to manufacture sulfuric

ii The metals have low melting points. acid. Some of the acid is used in the plant, but

iii Their compounds are highly coloured. most of it is used to make fertilisers.

iv Their compounds are colourless. i Give another use of sulfur dioxide. [1]

v The elements and their compounds are ii Describe how sulfur dioxide is converted

often used as catalysts. into sulfur trioxide. [3]

vi They have more than one oxidation state. [3] iii Name a fertiliser made from sulfuric acid. [1]

b i I n which Period in the Periodic Table b Some of the zinc oxide was mixed with an

is iron? [1] excess of carbon and heated to 1000 °C.

ii Use the Periodic Table to work out the Zinc distils out of the furnace.

number of protons and the number of 2ZnO 1 C    2Zn 1 CO2
  C 1 CO2    2CO
neutrons in one atom of iron. [1]
i Name the two changes of state involved in
c I ron is extracted in a blast furnace. The list

below gives some of the substances used or the process of distillation. [2]

formed in the extraction. ii Why is it necessary to use an excess of

carbon monoxide coke iron ore limestone slag carbon? [2]

i Which substance is a mineral containing c The remaining zinc oxide reacts with

largely calcium carbonate? [1] sulfuric acid to give aqueous zinc sulfate.

ii Which substance is formed when impurities This is electrolysed with inert electrodes

in the ore react with calcium oxide? [1] (the electrolysis is the same as that of

iii Which substance is also called hematite? [1] copper(II) sulfate with inert electrodes).

d State two functions of the coke used in the Ions present: Zn21(aq)  SO422 (aq)  H1(aq)
OH2(aq).
blast furnace. [2]

e M ost of the iron is converted into mild steel i Z inc forms at the negative electrode

or stainless steel. Give one use for each. [2] (cathode). Write the equation for this

Cambridge IGCSE Chemistry 0620 Paper 3 Q1 June 2006 reaction. [1]

9 T he first three elements in Group IV are ii Write the equation for the reaction at

carbon, silicon, germanium. the positive electrode (anode). [2]

a T he element germanium has a diamond-type iii Complete this sentence:

structure. Describe the structure of germanium. The electrolyte changes from aqueous zinc

A diagram is acceptable. [2] sulfate to ................. [1]

b U nlike diamond, graphite is soft and is d Give two uses of zinc. [2]

a good conductor of electricity. Cambridge IGCSE Chemistry 0620 Paper 3 Q4 November 2007

i Explain why graphite has these properties. [3] 11 Aluminium is extracted by the electrolysis of

ii Give a use of graphite that depends on a molten mixture that contains alumina, which

one of these properties. [1] is aluminium oxide, Al2O3.
a The ore of aluminium is bauxite. This contains
c C arbon dioxide and silicon(IV) oxide have

similar formulae but different types of structure. alumina, which is amphoteric, and iron(III)

i Give the formulae of these oxides. [1] oxide, which is basic. The ore is heated with

ii How are their structures different? [2] aqueous sodium hydroxide.

d All these elements form compounds with Complete the following sentences.

hydrogen called hydrides. The saturated The i….…... dissolves to give a solution of
hydrides of carbon are the alkanes. Predict the
formula of the hydride of germanium which ii.……...

The iii……….does not dissolve and can be

contains two germanium atoms. removed by iv……….. [4]

Cambridge IGCSE Chemistry 0620 Paper 3 Q4 June 2006

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Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m

b Complete the labelling of the diagram. c When nitric acid is added to water the following
reaction occurs.
waste gases

carbon anode (+) HNO3  1  H2O    NO32  1  H3O1

i .................. mixture of aluminium Give the name and the formula of the particle
.................. (–) oxide and ii ..................
transferred from nitric acid to water. [2]

iii .................. d This question is about the following oxides.
temperature is iv ..................
aluminium oxide Al2O3
c The ions involved in the electrolysis are
calcium oxide CaO
Al31 and O22.
carbon dioxide CO2
i Write an equation for the reaction at the
carbon monoxide CO
cathode. [2]
magnesium oxide MgO
ii Explain how carbon dioxide is formed at
sulfur dioxide SO2
the anode. [2]
i Which will react with hydrochloric acid but
d G ive an explanation for each of the following.
not with aqueous sodium hydroxide? [1]
i Aluminium is used extensively in the
ii Which will react with aqueous sodium
manufacture of aircraft. [1]
hydroxide but not with hydrochloric acid? [1]
ii Aluminium is used for food containers. [2]
iii Which will react both with hydrochloric acid
iii Aluminium electricity cables have a steel
and aqueous sodium hydroxide? [1]
core. [1]
iv Which will react neither with hydrochloric
Cambridge IGCSE Chemistry 0620 Paper 3 Q6 June 2007
acid nor with aqueous sodium hydroxide? [1]

12 a Four bottles were known to contain aqueous Cambridge IGCSE Chemistry 0620 Paper 3 Q3 June 2006

ammonia, dilute hydrochloric acid, sodium 13 H ydrogen reacts with the halogens to form
hydrogen halides.
hydroxide solution and vinegar, which is dilute
a Bond energy is the amount of energy, in kJ,
ethanoic acid. The bottles had lost their labels. that must be supplied (endothermic) to break
one mole of a bond.
The pH values of the four solutions were 1, 4,

10 and 13. Complete the table. [2]

solution pH bond bond energy in kJ / mol
aqueous ammonia
dilute hydrochloric acid H2H 1436
F2F 1158
sodium hydroxide solution H2F 1562

vinegar Use the above data to show that the following

b T he following apparatus was set up to investigate reaction is exothermic.
the electrical conductivity of dilute acids.
H H 1 F F   2H F [3]
bulb/lamp
b They react with water to form acidic solutions.
+–
 HCl 1 H2O   H3O1 1 Cl2
 HF 1 H2O   H3O1 1 F2

carbon carbon i Explain why water behaves as a base in
anode cathode
both of these reactions. [2]

dilute sulfuric acid ii At equilibrium, only 1% of the hydrogen

bubbles of chloride exists as molecules, the rest has
hydrogen gas
bubbles of formed ions. In the other equilibrium, 97%
oxygen gas
of the hydrogen fluoride exists as molecules,
Dilute sulfuric acid is a strong acid. If it was
only 3% has formed ions. What does this tell
replaced by a weak acid, what two differences in
you about the strength of each acid? [2]
the observations would you expect to make? [2]
iii How would the pH of these two solutions

differ? [1]

Cambridge IGCSE Chemistry 0620 Paper 32 Q7 June 2009

301

C a m b r i d g e i g cs e e x a m q u e s t i o n s iii Complete the equations for the
decomposition of their nitrates.
14 The reactivity series lists metals in order of
reactivity. To find out which is more reactive, 2KNO3    .................  1  ...............
zinc or tin, this experiment could be carried out. 2Ca(NO3)2    ..........  1  .............. 1 .............

piece of zinc [4]
shiny surface
Cambridge IGCSE Chemistry 0620 Paper 31 Q6 November 2008

tin(II) nitrate(aq) zinc surface still 15 The fractional distillation of crude oil usually
shiny means produces large quantities of the heavier fractions.
NO REACTION (NR) The market demand is for the lighter fractions and
for the more reactive alkenes. The heavier fractions
zinc surface covered are cracked to form smaller alkanes and alkenes as
with a grey deposit means in the following example.

REACTION (R)

a The experiment could be carried out with

other metals and the results recorded in a table. C8H18    C4H10 1 C4H8
octane butane butenes
Then the order of reactivity can be deduced.

i The order was found to be: a i Write a different equation for the cracking
of octane.
manganese most reactive

zinc C8H18     ............. 1 .................. [1]

tin ii The cracking of octane can produce isomers

silver least reactive with the molecular formula C4H8. Draw the
structural formulae of two of these isomers.
Copy and complete this table of results

from which the order was determined. [3] [2]

aqueous tin Sn manganese silver zinc b i Give the essential condition for the reaction
solution Mn Ag Zn
between chlorine and butane. [1]
tin(II) nitrate R NR R
ii What type of reaction is this? [1]
manganese(II)
nitrate iii This reaction produces a mixture of products.

silver(I) nitrate Give the names of two products that contain

zinc nitrate four carbon atoms per molecule. [2]

ii W rite the ionic equation for the reaction c Alkenes are more reactive than alkanes and

between tin atoms and silver(I) ions. [2] are used to make a range of organic chemicals.

iii The following is a redox reaction. Propene, CH3–CH5CH2, is made by cracking.
Give the structural formula of the addition
Mn 1 Sn21     Mn21 1 Sn
product when propene reacts with these.

Indicate on the equation the change which is i  water   ii  bromine [2]
oxidation. Give a reason for your choice. [2]
d Propene reacts with hydrogen iodide to form

iv Explain why experiments of this type cannot 2-iodopropane.

be used to find the position of aluminium CH32CH5CH2 1 HI CH32CHI2CH3

in the reactivity series. [2] 1.4 g of propene produced 4.0 g of 2-iodopropane.
Calculate the percentage yield.
b P otassium and calcium are very reactive

metals at the top of the series. Because their i moles of CH32CH5CH2 reacted  5
ii maximum moles of CH3-CHI-CH3 that could
ions have different charges, K1 and Ca21, their
be formed  5
compounds behave differently when heated. mass of one mole of CH3-CHI-CH3 is 170 g
iii maximum mass of 2-iodopropane that
i Explain why the ions have different could be formed  5
iv percentage yield  5 [4]
charges. [2]
Cambridge IGCSE Chemistry 0620 Paper 3 Q7 June 2006
ii Their hydroxides are heated. If the compound

decomposes, complete the word equation.

If it does not decompose, write ‘no reaction’.

Potassium hydroxide ...............

Calcium hydroxide ............... [2]

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Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m

16 The alcohols form a homologous series. d F or each of the following predict the name of
The first four members are methanol, ethanol,
propan-1-ol and butan-1-ol. the organic product.

a O ne characteristic of a homologous series is that i reaction between methanol and ethanoic
the physical properties vary in a predictable way.
The table below gives the heats of combustion of acid [1]
the first three alcohols.
ii oxidation of propan-1-ol by potassium

dichromate(VI) [1]

alcohol formula heat of iii removal of H2O from ethanol [1]
combustion (dehydration)
in kJ / mole
Cambridge IGCSE Chemistry 0620 Paper 3 Q6 November 2007
2730
methanol CH3OH 17 Copy and complete the following table.
ethanol CH3-CH2-OH 21370
propan-1-ol CH3-CH2-CH2-OH gas test for gas
butan-1-ol CH3-CH2-CH2-CH2-OH –­ 2020 ammonia
bleaches damp litmus paper
i T he minus sign indicates there is less chemical hydrogen
relights a glowing splint
energy in the products than in the reactants. turns limewater milky

In what form is the energy given out? [1]

ii Is the reaction exothermic or endothermic? [1] [5]

iii Complete the equation for the complete Cambridge IGCSE Chemistry 0620 Paper 3 Q1 November 2008

combustion of ethanol.

C2H5OH  1  ....O2    ............... 1 .............. –700 number of carbon atoms per molecule 4
[2] –800 123
–900
iv D etermine the heat of combustion of butan- –1000
1-ol by plotting the heats of combustion of –1100
the first three alcohols against the number –1200
of carbon atoms per molecule. –1300
Label your graph as on the right. –1400
–1500
What is the heat of combustion of [3] –1600
butan-1-ol in kJ / mol? [2] heat of –1700
[2] combustion /
v Describe two other characteristics of kJ / mol –1800
homologous series. –1900
–2000
b G ive the name and structural formula of –2100
an isomer of propan-1-ol. –2200
–2300
c M ethanol is made from carbon monoxide. –2400
–2500
CO (g) 1 2H2 (g)    CH3OH (g) –2600
–2700
The forward reaction is exothermic. –2800

i D escribe how hydrogen is obtained from

alkanes. [2]

ii S uggest a method of making carbon monoxide

from methane. [2]

iii W hich condition, high or low pressure, would

give the maximum yield of methanol? Give a

reason for your choice. [2]

303

from paper 6C A M B R I D G E I G C S E E X A M Q U E S T I O N S

1 The colours present in some blackcurrant sweets 3 A student investigated the addition of four
can be separated by chromatography. The colours different solids, A, B, C and D, to water.
are water-soluble dyes. The diagrams show how Five experiments were carried out.
the colours can be extracted from the sweets.
Experiment 1
B By using a measuring cylinder, 30 cm3 of distilled
water was poured into a polystyrene cup and the
C initial temperature of the water was measured.
A 4 g of solid A was added to the cup and the mixture
stirred with a thermometer. The temperature of
the solution was measured after 2 minutes.

30 30

25 25

a N ame the pieces of apparatus labelled A to C. [3] 20 20
initial temperature final temperature
The apparatus below was used to carry out
the chromatography.

glass cover Experiment 2
Experiment 1 was repeated using 4 g of solid B.
chromatography beaker
paper 30 30

solvent 25 25

20 20
initial temperature final temperature
b i Name the solvent used. [1]
ii Label, with an arrow, the origin on the Experiment 3
Experiment 1 was repeated using 4 g of solid C.
diagram. [1]
c On a larger copy of this 30 20

rectangle, sketch the 25 15
chromatogram you would
expect if two different colours 20 10
were present in the sweets. [1] initial temperature final temperature

Cambridge IGCSE Chemistry 0620 Paper 6 Q1 November 2008 Experiment 4
Experiment 1 was repeated using 4 g of solid D.
2 Describe a chemical test to distinguish between
each of the following pairs of substances. 30 30

Example: hydrogen and carbon dioxide 25 25
test: lighted splint
result: with hydrogen gives a pop 20 20
result: with carbon dioxide splint is extinguished initial temperature final temperature

a  zinc carbonate and zinc chloride [2]
b ammonia and chlorine [3]
c a queous iron(II) sulfate and aqueous

iron(III) sulfate [3]

Cambridge IGCSE Chemistry 0620 Paper 6 Q3 June 2009

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Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m

Experiment 5 4 Hydrogen peroxide 0 10 20 30 40 50
A little of the solution from Experiment 4 was added breaks down to form
to a little of the solution from Experiment 2 in oxygen. The volume gas syringe
a test-tube. The observations were recorded. of oxygen given off
can be measured
observations using this apparatus.
a fast reaction
vigorous effervescence and bubbles produced Solids W and X both catalyse the breakdown of
hydrogen peroxide. The syringe diagrams show
a C opy out the table and use the thermometer the volume of oxygen formed every 20 seconds
diagrams for Experiments 1–4 to record the using these catalysts at 25 °C.
initial and final temperatures. Calculate and
record the temperature difference in the table. time/ s using catalyst W using catalyst X

expt initial final difference 0 0 10 20 30 40 0 10 20 30 40

1 temperature / °C temperature / °C  / °C
2
3 20 0 10 20 30 40 0 10 20 30 40
4
40 0 10 20 30 40 0 10 20 30 40

[4]

60 0 10 20 30 40 0 10 20 30 40

b Draw a labelled bar chart of the results to [4] 80 0 10 20 30 40 0 10 20 30 40
Experiments 1, 2, 3 and 4 on graph paper.
Label your bar chart as shown below.

+10

100 0 10 20 30 40 0 10 20 30 40

+5

temperature 0 a Copy the table. Use the gas syringe diagrams
difference / ºC to complete it.

–5 time / s volume of oxygen / cm3

–10 catalyst W catalyst X
0
Use the results and observations from Experiments 20
40
1 – 5 to answer the following questions. 60
80
c i Which solid dissolves in water to produce 100

an exothermic reaction? [1]

ii Give a reason why you chose this solid. [1]

d W hich Experiment produced the largest [3]

temperature change? [1] b Plot a graph to show each set of results.

e P redict the temperature change that would Clearly label the curves. [6]

happen if c Which solid is the better catalyst in this

i 8 g of solid B was used in Experiment 2, [1] reaction? Give a reason for your choice. [2]

ii 60 cm3 of water was used in Experiment 4. d Why is the final volume of oxygen the same

[1] in each experiment? [1]

iii Explain your answer to e ii. [2] e Sketch a line on the grid to show the shape

f S uggest an explanation for the observations of the graph you would expect if the reaction

in Experiment 5. [2] with catalyst X was repeated at 40 °C. [2]

Cambridge IGCSE Chemistry 0620 Paper 6 Q4 November 2008 Cambridge IGCSE Chemistry 0620 Paper 6 Q6 June 2007

305

C a m b r i d g e i g cs e e x a m q u e s t i o n s

5 An experiment was carried out to determine 7 The diagram shows an experiment to pass
the solubility of potassium chlorate at different electricity through lead bromide. Electricity has
temperatures. The solubility is the mass of no effect on solid lead bromide.
potassium chlorate that dissolves in 100 g of water.
d.c.power supply
The results obtained are shown in the table below.
bulb
temperature / °C 0 10 20 30 40 50 60
14 17 20 24 29 34 40 LEAD
solubility in BROMIDE
g  / 100 g of water
TOXIC
a Draw a smooth line graph to show the solubility
of potassium chlorate at different temperatures.
Label your graph as shown below.

50

40 heat

a i Copy the diagram and clearly label the

30 electrodes. [1]
solubility in
g/100 g water ii S uggest a suitable material to make the

20 electrodes. [1]

b G ive two observations expected when the

10 lead bromide is heated to melting point. [2]

c State two different safety precautions when

0 carrying out this experiment. [2]
0 10 20 30 40 50 60 70
temperature / ºC Cambridge IGCSE Chemistry 0620 Paper 6 Q2 June 2008

[4] 8 Concentrated hydrochloric acid can be electrolysed
b U se your graph to determine the solubility of using the apparatus shown.

potassium chlorate at 70 °C. Show clearly on
the graph how you obtained your answer. [2]
c W hat would be the effect of cooling a saturated
solution of potassium chlorate from 60 °C
to 20 °C? [2]

Cambridge IGCSE Chemistry 0620 Paper 6 Q6 November 2008

6 T he diagram shows the formation of a solution
of magnesium hydroxide from magnesium.

Universal
A indicator

solution

solution of

water magnesium

magnesium magnesium hydroxide
burning to form a Copy the diagram and label the position of
magnesium oxide indicator C
oxide turns
heat blue
the electrodes. [1]
B b Give two observations when the circuit is

a Name the pieces of apparatus labelled A – C. [3] switched on. [2]
c i Name the product at the positive electrode. [1]
b W hat type of chemical reaction is the

burning of magnesium? [1] ii State a test for this product, and the result. [2]

c S uggest a pH for the solution of magnesium Cambridge IGCSE Chemistry 0620 Paper 6 Q2 June 2007

hydroxide. [1]

Cambridge IGCSE Chemistry 0620 Paper 6 Q1 November 2006

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Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m

9 A student investigated the reaction between d About 1 cm3 of aqueous sodium hydroxide was
potassium manganate(VII) and a metallic salt added to a little of the solution in the flask and
solution. Two experiments were carried out. the observation noted.

Experiment 1 observation  red-brown precipitate
a About 1 cm3 of aqueous sodium hydroxide
e i I n which experiment was the greatest volume
was added to a little of the salt solution A
and the observation noted. of potassium manganate(VII) solution used? [1]
observation  green precipitate formed
ii Compare the volumes of potassium
b A burette was filled with potassium manganate(VII)
solution up to the 0.0 cm3 mark. manganate(VII) solution used in

B y using a measuring cylinder, 25 cm3 of Experiments 1 and 2. [2]
solution A of the salt was placed into a conical
flask. The flask was shaken to mix the contents. iii Suggest an explanation for the difference

T he potassium manganate(VII) solution was in the volumes. [2]
added to the flask, and shaken to mix thoroughly.
Addition of potassium manganate(VII) solution f Predict the volume of potassium manganate(VII)
was continued until there was a pale pink colour
in the contents of the flask. solution which would be needed to react

C opy the table of results below. completely with 50 cm3 of solution B. [2]

Burette readings / cm3 g E xplain one change that could be made to the

Experiment 1 Experiment 2 experimental method to obtain more accurate

final reading results. [2]

initial reading h W hat conclusion can you draw about the salt

difference solution from:

i  experiment 1a, [1]

ii  experiment 2d? [1]

Cambridge IGCSE Chemistry 0620 Paper 6 Q4 June 2008

10 This label is from a container of ‘Bite Relief’ solution.

Use this burette diagram 25 BITE RELIEF
to record the volume and 26 FOR FAST RELIEF FROM INSECT
complete the column
for Experiment 1 in BITES AND STINGS
the table.
Active ingredient: ammonia
Also contains water and alcohol

27 DIRECTIONS FOR USE: Use cotton wool to
dab the solution on the affected area of the skin.


final reading
a Give a chemical test to show the presence of
Experiment 2
c Experiment 1b was repeated using a different ammonia in Bite Relief solution.

solution B of the salt, instead of solution A. Give the result of the test. [2]
Use the burette diagrams to record the volumes
b What practical method could be used to
in the table and complete the table.

15 28 separate the mixture of alcohol (b.p. 78 °C)

and water (b.p. 100 °C)? [2]

c Give a chemical test to show the presence

16 29 of water. Give the result of the test. [2]

d What would be the effect of touching the

17 30 alcohol with a lighted splint? [1]
final reading
initial reading Cambridge IGCSE Chemistry 0620 Paper 6 Q7 June 2008

[4]

307

C a m b r i d g e i g cs e e x a m q u e s t i o n s

11 Two solids, S and V, were analysed. S was copper(II) oxide.
The tests on the solids, and some of the observations, are
in the following table. Write down the observations that
are missing from the table.

test observation
tests on solid S black solid
slow effervescence
a Appearance of solid S splint relit
blue solution formed
b H ydrogen peroxide was added to solid S in a test-tube.
A glowing splint was inserted into the tube ………………………………………….………… [1]
……………………………………………….…… [2]
c D ilute sulfuric acid was added to solid S in a test-tube. ………………………………………..…………... [2]
The mixture was heated to boiling point.
……………………………………………………. [2]
The solution was divided into three equal portions
into test-tubes.

i To the first portion of the solution excess sodium
hydroxide was added.

ii To the second portion of the solution, about
1 cm3 of aqueous ammonia solution was added.

Excess ammonia solution was then added.

iii To the third portion of the solution, dilute
hydrochloric acid was added followed by
barium chloride solution.

tests on solid V black solid
d Appearance of solid V
rapid effervescence
e H ydrogen peroxide was added to solid V in a test-tube. splint relit
A glowing splint was inserted into the tube.

f i C ompare the reactivity of solid S and solid V

with hydrogen peroxide. [1]

ii Identify the gas given off in test e. [1]

g What conclusions can you draw about solid V? [2]

Cambridge IGCSE Chemistry 0620 Paper 6 Q5 June 2009

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Y o u r C a m b r i d g e IG C S E c h e m i s t r y e x a m

12 A sample of solid C was analysed. C is a mixture of two
salts, D and E. Solid D is insoluble lead carbonate and
solid E is water-soluble.

The tests on C, and some of the observations are in the
following tables. Complete the observations that would
go in the tables.

tests observations
a Describe the appearance of C. pale green solid

b U sing a spatula, place a little of C in a hard glass test-tube. paper turns blue
Inside the top of the tube suspend a piece of damp indicator pH 8 to 11
paper. Heat C gently until gas comes out of the tube.
c ............................................. [3]
c Using a spatula, place a little of C in a test-tube.
Add about 2 cm3 of dilute nitric acid and test the gas.

Solid C was added to a boiling tube containing distilled observations [2]
water. The tube was shaken to mix the contents. d .............................................
The contents of the boiling tube were filtered.

tests on the residue in the filter paper
d Place the funnel in a test-tube. Pour dilute nitric acid

onto the residue contained in the funnel.
Add 2 cm3 of potassium iodide to the solution collected
in the tube.

tests on the filtrate observations

e Divide the filtrate into three test tubes. white precipitate
green precipitate
i T o the first portion add dilute hydrochloric acid and paper turns blue
about 1 cm3 of aqueous barium nitrate. pH 8 to 11

ii To the second portion of solution add excess aqueous
ammonia.

iii To the third portion of solution, add an equal volume
of aqueous sodium hydroxide. Warm the mixture gently.
Test the gas with indicator paper.

f Name the gas given off in c. [1]
g Name the gas given off in e iii. [1]
h What conclusions can you draw about salt E? [4]

Cambridge IGCSE Chemistry 0620 Paper 6 Q5 June 2007

309

Reference

Glossary

A B cathode  the negative electrode of an
electrolysis cell
acetylene  a gas (formula C2H2) used as a back reaction  the reaction in which the
fuel, for example in the oxy-acetylene torch product breaks down again, in a reversible cation  another name for a positive ion
reaction
acid rain  rain that is acidic because gases cell (biological)  the building blocks for
such as sulfur dioxide are dissolved in it bacteria  tiny organisms, some of which can animals and plants
(from burning fossil fuels) cause disease; others break down dead plant
and animal material cell (electrical)  a device that converts
acidic solution  has a pH less than 7; an chemical energy to electrical energy
acidic solution contains H 1 ions balanced equation  a chemical equation in
which the number of each type of atom is cement  a substance used in building, made
acid fermentation  the process in which the same on both sides of the arrow from limestone and clay
bacteria convert ethanol to ethanoic acid
base  a metal oxide or hydroxide; a base will ceramic  a hard, ureactive material that can
addition reaction  where a molecule adds neutralise an acid, to form a salt and water withstand high temperatures, made by
onto an alkene, and the C 5 C double bond baking clay in a kiln; ceramics are non-
of the alkene changes to a single bond battery  a portable electrical cell; for conductors
example a torch battery
addition polymerisation  where small chalk  a rock made of calcium carbonate
molecules join to form a very large molecule, biodegradable  will decay naturally in the
by adding on at double bonds soil, with the help of bacteria change of state  a change in the physical
state of a substance – for example from solid
alcohols  a family of organic compounds, biopolymer  a polymer made by bacteria to liquid, or liquid to gas
similar to the alkanes but with the OH
functional group; ethanol is an example blast furnace  the chemical plant in which chemical change  a change in which a new
iron is extracted from its ore, iron(III) oxide chemical substance forms
alkali  a soluble base; for example sodium
hydroxide boiling  the change from a liquid to a gas, chemical equation  uses chemical symbols
which takes place at the boiling point to describe a chemical reaction in a short
alkali metals  the Group I elements of the way
Periodic Table boiling point  the temperature at which a
substance boils chemical reaction  a process in which
alkaline earth metals  the Group II chemical change takes place
elements of the Periodic Table bond energy  the energy needed to break a
bond, or released when the bond is formed; chromatogram  the paper showing the
alkaline solution  has a pH above 7; it is given in kilojoules (kJ) per mole separated coloured substances, after paper
alkaline solutions contain OH 2 ions chromatography has been carried out
bonding  how the atoms are held together
alkanes  a family of saturated hydrocarbons in an element or compound; there are three climate change  how climates around the
with the general formula CnH2n 1 2; types of bonds: ionic, covalent, and metallic Earth are changing, because of the rise in
‘saturated’ means they have only single C–C average air temperatures
bonds brittle  breaks up easily when struck
coagulant  a substance that will make small
alkenes  a family of unsaturated hydro- brine  the industrial name for a particles stick together; coagulants are used
carbons with the general formula CnH2n ; concentrated solution of sodium chloride in in cleaning up water, ready for piping to
their molecules contain a carbon 5 carbon water; it can be made by dissolving rock salt homes
double bond
burette  a piece of laboratory equipment for coke  a form of carbon made by heating
allotropes  different forms of an element; delivering a measured volume of liquid coal
diamond and graphite are allotropes of
carbon burning  an exothermic chemical reaction combination  where two or more
in which the reactant combines with oxygen substances react to form a single substance
alloy  a mixture where at least one other to form an oxide; also called combustion
substance is added to a metal, to improve its combustible  can catch fire and burn very
properties; the other substance is often a C easily
metal too (but not always)
carbon cycle  the way carbon moves non- combustion  another name for burning
amphoteric  can be both acidic and basic in stop between the atmosphere, living things,
its reactions; for example aluminium oxide the land, and the ocean; it moves in the form compound fertiliser  it provides
is an amphoteric oxide of carbon dioxide nitrogen, potassium, and phosphorus
for plants
anion  another name for a negative ion carboxylic acids  a family of organic acids,
which have the COOH functional compound ion  an ion containing more
anode  the positive electrode of a cell group;  ethanoic acid is an example than one element; for example the nitrate
ion NO3–
aquifer  underground rocks holding a large cast iron  iron from the blast furnace that is compound  a substance in which two or
volume of water; it can be pumped out to run into molds to harden; it contains a high more elements are chemically combined
give a water supply % of carbon, which makes it brittle
concentration  tells you how much of one
atmosphere  the layer of gases around the catalyst  a substance that speeds up a substance is dissolved in another; usually
Earth; here at the Earth’s surface, we call it chemical reaction, without itself being used given as grams or moles per dm3
air up in the process
condensation  the physical change in which
atoms  elements are made up of atoms, catalytic converter  a device in a car a gas turns into a liquid on cooling
which contain protons, neutrons, and exhaust, in which catalysts are used to
electrons convert harmful gases to harmless ones condensation polymerisation  where
molecules join to make very large molecules,
Avogadro constant  the number of particles catalytic cracking  where large molecules by eliminating small molecules (such as
in one mole of an element or compound; it of hydrocarbons are split up into smaller water molecules)
is 6.02 3 1023 ones, with the help of a catalyst

310

Reference

condenser  a piece of laboratory equipment electrolyte  the liquid through which the fractional distillation  a method used to
used to cool a gas rapidly, and turn it into a current is passed, in electrolysis; the current separate two or more liquids that have
liquid is carried by ions in the electrolyte different boiling points

conductor  a substance that allows heat or electron distribution  how the electrons in fractions  the different groups of
electricity to pass through it easily an atom are arranged in shells (2 1 8 1 …) compounds that a mixture is separated into,
by fractional distillation; fractions are
Contact process  the industrial process for electron shells  the different energy levels collected one by one
making sulfuric acid which electrons occupy, around the nucleus
freezing  the change from liquid to solid,
corrosion  where a substance is attacked by electronic configuration  another term for  that occurs at the freezing point (5 melting
air or water, from the surface inwards; the electron distribution point)
corrosion of iron is called rusting
electrons  the particles with a charge of 1– fuel  a substance we use to provide energy;
covalent bond  the chemical bond formed and almost no mass, in an atom most fuels are burned to release their energy
when two atoms share electrons (but nuclear fuels are not)
electroplating  coating one metal with
covalent compound  a compound made of another, using electrolysis fuel cell  a cell in which a chemical reaction
atoms joined by covalent bonds provides electricity (to light homes and so
element  a substance that cannot be split on)
cracking  reactions in which long-chain into anything simpler, in a chemical reaction
hydrocarbon molecules are broken down to functional group  the part of the molecule
shorter, more useful molecules empirical  found by experiment of an organic compound, that largely
dictates how it reacts; for example the OH
cross-linking  the chemical bonds between empirical formula  shows the simplest group in molecules of the alcohol family
the long-chain molecules in some polymers, ratio in which the atoms in a compound
that hold the chains together are combined G

crude oil  the fossil fuel formed over millions endothermic  takes in energy from the galvanising  coating iron with zinc, to
of years from the remains of tiny sea plants surroundings prevent the iron from rusting
and animals; it is also called petroleum
enzymes  proteins made by living cells, that giant structure  where a very large number
crystallisation  the process in which act as biological catalysts of atoms or ions are held in a lattice by
crystals form, as a saturated solution cools strong bonds; metals, diamond and ionic
equation  it uses symbols to describe a solids such as sodium chloride are all giant
D chemical reaction (but a word equation uses structures
just words)
decomposition reaction  where a substance global warming  the rise in average
breaks down to give two or more products equilibrium  the state where the forward temperatures taking place around the world;
and back reactions are taking place at the many scientists believe that carbon dioxide
denature  to destroy the structure of an same rate, in a reversible reaction; so there (from burning fossil fuels) is the main cause
enzyme by heat, or a change in pH is no overall change
greenhouse gas  a gas in the atmosphere
degradeable  will break down naturally ester  a compound formed when an alcohol that traps heat, preventing its escape into
(for example through the action of reacts with a carboxylic acid; esters often space; carbon dioxide and methane are
bacteria) smell of fruit or flowers examples

density  tells you how ‘heavy’ something is; evaporation  the physical change where a group  a column of the Periodic Table;
the density of a substance is its mass per liquid turns to a gas at a temperature below elements in a group have similar properties
unit volume; for water it is 1 g / cm3 its boiling point
H
diatomic  a substance is called diatomic if exothermic  gives out energy
its molecules contain two atoms joined by a Haber process  the process for making
covalent bond extract  to remove a metal from its ore ammonia from nitrogen and hydrogen, in
industry
diffusion  the process in which particles F
mix by colliding randomly with each other, half-equation  an equation that shows the
and bouncing off in all directions fermentation  the process in which the reaction taking place at an electrode
enzymes in yeast break down sugars, to
displacement reaction  a reaction in form ethanol and carbon dioxide halogens  the Group VII elements of the
which a more reactive element takes the Periodic Table
place of a less reactive one, in a compound fertilisers  substances added to soil to help
crops grow well heating curve  a graph showing how the
dissolving  the process in which a soluble temperature of a substance changes on
substance forms a solution filtering  separating solids from liquids by heating, while it goes from solid to liquid to
pouring the mixture through filter paper gas
distillation  separating a liquid from a
mixture by boiling it off, then condensing it filtrate  the liquid obtained from filtration homologous series  a family of organic
(after the solid has been removed) compounds, that share the same general
double bond  a covalent bond in which two formula and have similar properties
atoms share two pairs of electrons flammable  burns easily
hydrated  has water molecules built into its
ductile  can be drawn out into a wire; for flue gas desulfurisation  the removal of crystal structure; for example copper(II)
example copper is ductile sulfur dioxide from the waste gases at power sulfate: CuSO4.5H2O
stations, to stop it getting into the hydrocarbon  a compound containing only
dynamic equilibrium  where forward and atmosphere carbon and hydrogen
back reactions take place at the same rate,
so there is no overall change formula  uses symbols and numbers to tell hydrogenation  adding hydrogen
you what elements are in a compound, and
E the ratio in which they are combined hydrogen fuel cell  it uses the reaction
between hydrogen (from a tank), and
electrodes  the conductors used to carry forward reaction  the reaction in which oxygen (from the air), to give an electric
current into and out of an electrolyte; they the product is made, in a reversible reaction current
could be graphite rods, for example
fossil fuels  petroleum (crude oil), natural
electrolysis  the process of breaking down gas, and coal; they are called the fossil fuels
a compound by passing a current through it because they were formed from the remains
of living things, millions of years ago

311

Reference

hydrolysis  the breaking down of metallic bond  the bond that holds the O
a compound by reaction with water atoms together in a metal
ore  rock containing a metal, or metal
hypothesis  a statement you can test by metalloid  an element that has properties of compounds, from which the metal is
doing an experiment and taking both a metal and a non-metal extracted
measurements
microbe  a microscopic (very tiny) living organic chemistry  the study of organic
I organism, such as a bacterium or virus compounds (there are millions of them!)

incomplete combustion  the burning of minerals  compounds that occur naturally in organic compound  a compound containing
fuels in a limited supply of oxygen; it gives the Earth; rocks contain different minerals carbon, and usually hydrogen; petroleum is a
carbon monoxide instead of carbon dioxide mixture of many organic compounds
mixture  contains two or more substances
indicator  a chemical that shows by its that are not chemically combined oxidation  a chemical reaction in which a
colour whether a substance is acidic or substance gains oxygen, or loses electrons
alkaline molar solution  contains one mole of a
substance in 1 dm3 (1 litre) of water oxidation state  every atom in a formula
inert  does not react (except under extreme can be given a number that describes its
conditions) mole  the amount of a substance that oxidation state; for example in NaCl, the
contains the same number of elementary oxidation states are +I for sodium, and – I
inert electrode  is not changed during units as the number of carbon atoms in 12g for chlorine
electrolysis; all it does is conduct the current of carbon-12; you obtain it by weighing out
the Ar or Mr of the substance, in grams oxide  a compound formed between oxygen
in excess  more than is needed for a molecular  made up of molecules and an other element
reaction; some will be left at the end
molecule  a unit of two or more atoms held oxidising agent  a substance that brings
insoluble  does not dissolve in a solvent together by covalent bonds about the oxidation of another substance

insulator  a poor conductor of heat or monatomic  made up of single atoms; for ozone  a gas with the formula O3
electricity example neon is a monatomic element ozone layer  the layer of ozone up in the
atmosphere, which protects us from harmful
intermolecular forces  forces between monomers  small molecules that join UV radiation from the sun
molecules together to form polymers
P
ion  a charged atom or group of atoms N
formed by the gain or loss of electrons paper chromatography  a way to separate
native  describes a metal that is found in the the substances in a mixture, using a solvent
ionic bond  the bond formed between ions Earth as the element and special paper; the substances separate
of opposite charge because they travel over the paper at
negative electrode  another name for the different speeds
ionic compound  a compound made up of cathode, in an electrolysis cell
ions, joined by ionic bonds percentage composition  it tells you which
negative ion  an ion with a negative charge elements are in a compound, and what % of
ionic equation  shows only the ions that each is present by mass
actually take part in a reaction, and ignores neutral (electrical)  has no charge
any other ions present; the other ions are period  a horizontal row of the Periodic
called spectator ions neutral (oxide)  is neither acidic nor basic; Table; its number tells you how many
carbon monoxide is a neutral oxide electron shells there are
isomers  compounds that have the same
formula, but a different arrangement of neutral (solutions)  neither acidic nor periodicity  the pattern of repeating
atoms alkaline; neutral solutions have a pH of 7 properties that shows up when elements are
arranged in order of proton number; you
isotopes  atoms of the same element, that neutralisation  the chemical reaction can see it in the groups in the Periodic Table
have a different numbers of neutrons between an acid and a base or a carbonate,
giving a salt and water Periodic Table  the table showing the
L elements in order of increasing proton
neutron  a particle with no charge and a mass number; similar elements are arranged in
lattice  a regular arrangement of particles of 1 unit, found in the nucleus of an atom columns called groups

lime  the common name for calcium oxide nitrogenous fertiliser  it provides nitrogen petroleum  a fossil fuel formed over millions
for plants, in the form of nitrate ions or of years from the remains of tiny sea plants
limewater  a solution of the slightly soluble ammonium ions and animals; it is also called crude oil
compound calcium hydroxide, which is used
to test for carbon dioxide noble gases  the Group 0 elements of the pH scale  a scale that tells you how acidic or
Periodic Table; they are called ‘noble’ alkaline a solution is; it is numbered 0 to 14
locating agent  used to show up colourless because they are so unreactive
substances, in chromatography; it reacts photochemical reaction  a reaction that
with them to give coloured substances non-metal  an element that does not show depends on light energy; photosynthesis is
metallic properties: the non-metals lie to the an example
M right of the zig-zag line in the Periodic Table,
(except for hydrogen, which sits alone) photodegradeable  can be broken down by
macromolecule  a very large molecule; for light
example a molecule in a polymer non-renewable resource  a resource such
as petroleum that we are using up, and photosynthesis  the process in which plants
malleable  can be bent or hammered into which will run out one day convert carbon dioxide and water to glucose
shape and oxygen
non-toxic  not harmful health
mass spectrometer  an instrument used to physical change  a change in which no new
find the masses of atoms and molecules nucleon number  the number of protons chemical substance forms; melting and
plus neutrons in an atom of an element boiling are physical changes
melting point  the temperature at which a
solid substance melts nuclear fuel  contains radioisotopes such physical properties  properties such as
as uranium-235; these are forced to break density and melting point (that are not
melting  the physical change from a solid to down, giving out energy about chemical behaviour)
a liquid
nucleus  the centre part of the atom, made
metal  an element that shows metallic up of protons and neutrons
properties (for example conducts
electricity, and forms positive ions)

312

Reference

pipette  a piece of laboratory equipment refining (metals)  the process of purifying structural formula  the formula of a
used to deliver a known volume of liquid, a  metal; copper is refined using electrolysis compound displayed to show the bonds
accurately between the atoms as lines; we often show
relative atomic mass (Ar)  the average organic compounds this way
plastics  a term used for synthetic polymers mass of the atoms of an element, relative to
(made in factories, rather than in nature) the mass of an atom of carbon-12 T

pollutant  a substance that causes harm if it relative formula mass (Mr)  the mass of thermal decomposition  the breaking
gets into the air or water one formula unit of an ionic compound; you down of a compound by heating it
find it by adding together the relative atomic
pollution  when harmful substances are masses of the atoms in the formula thermite process  the redox reaction
released into the environment between iron oxide and aluminium, which
relative molecular mass  the mass of a produces molten iron
polymer  a compound containing very large molecule; you find it by adding the relative
molecules, formed by polymerisation atomic masses of the atoms in it titration  a laboratory technique for finding
the exact volume of an acid solution that will
polymerisation  a chemical reaction in renewable resource  a resource that will react with a given volume of alkaline
which many small molecules join to form not run out; for example water, air, sunlight solution, or vice versa
very large molecules; the product is called a
polymer residue  the solid you obtain when you toxic  poisonous
separate a solid from a liquid by filtering
positive ion  an ion with a positive charge transition elements  the elements in the
respiration  the reaction between glucose wide middle block of the Periodic Table; they
precipitate  an insoluble chemical and oxygen that takes place in the cells of all are all metals and include iron, tin, copper,
produced during a chemical reaction living things (including you) to provide and gold
energy
precipitation reaction  a reaction in which trend  a gradual change; the groups within
a precipitate forms reversible reaction  a reaction that can go the Periodic Table show trends in their
both ways: a product can form, then break properties; for example as you go down
product  a chemical made in a chemical down again; the symbol is used to show a Group I, reactivity increases
reaction reversible reaction
triple bond  the bond formed when two
protein  a polymer made up of many rusting  the name given to the corrosion of atoms share three pairs of electrons; a
different amino acid units joined together iron; oxygen and water attack the iron, and nitrogen molecule has a triple bond
rust forms
proton number  the number of protons in U
the atoms of an element; it is sometimes S
called the atomic number universal indicator  a paper or liquid you
sacrificial protection  allowing one metal can use to find the pH of a solution; it
proton  a particle with a charge of 1+ and a to corrode, in order to protect another metal changes colour across the whole range of pH
mass of 1 unit, found in the nucleus of an
atom salt  an ionic compound formed when an unreactive  does not react easily
acid reacts with a metal, a base, or a
pure  there is only one substance in it carbonate unsaturated compound  an organic
compound with at least one double bond
Q saturated compound  an organic between carbon atoms
compound in which all the bonds between
quicklime  another name for calcium oxide carbon atoms are single covalent bonds V

R saturated solution  no more of the solute valency  a number that tells you how many
will dissolve in it, at that temperature electrons an atom gains, loses or shares, in
radioactive isotopes (radioisotopes)  forming a compound
unstable atoms that break down, giving out single bond  the bond formed when two
radiation atoms share just one pair of electrons valency electrons  the electrons in the
outer shell of an atom
random motion  the zig-zag path a particle slaked lime  another name for calcium
follows as it collides with other particles and hydroxide variable valency  an element shows
bounces away again variable valency if its atoms can lose
solubility  the amount of solute that will different numbers of electrons, in forming
rate of reaction  how fast a reaction is dissolve in 100 grams of a solvent, at a given compounds; for example copper forms Cu+
temperature and Cu2 1 ions
reactant  a starting chemical for a chemical
reaction soluble  will dissolve in a solvent viscosity  a measure of how runny a liquid
is; the more runny it is, the lower its viscosity
reactive  tends to react easily solute  the substance you dissolve in the
solvent, to make a solution viscous  thick and sticky
reactivity  how readily a substance reacts
solution  a mixture obtained when a solute volatile  evaporates easily, to form a vapour
reactivity series  the metals listed in order is dissolved in a solvent
of their reactivity W
solvent  the liquid in which a solute is
recycling  reusing resources such as scrap dissolved, to make a solution water of crystallisation  water molecules
metal, glass, paper and plastics built into the crystal structure of a
sonorous  makes a ringing noise when compound; for example in copper(II) sulfate,
redox reaction  any reaction in which struck CuSO4.5H2O
electrons are transferred; one substance is weak acids  acids in which only some of the
oxidised (it loses electrons) and another is spectator ions  ions that are present in a molecules are dissociated, to form H 1 ions;
reduced (it gains electrons) reaction mixture, but do not actually take ethanoic acid is a weak acid
part in the reaction
reducing agent  a substance which brings Y
about the reduction of another substance stable  unreactive
yield  the actual amount of a product
reduction  when a substance loses oxygen, state symbols  these are added to an obtained in a reaction; it is often given as a
or gains electrons equation to show the physical states of the % of the theoretical yield (which you can
reactants and products (g 5 gas, l 5 liquid, work out from the equation)
refining (petroleum)  the process of s 5 solid, aq 5 aqueous)
separating petroleum (crude oil) into groups
of compounds with molecules fairly close in
size; it is carried out by fractional distillation

313

Reference

I II The Periodic Table of the Elements III IV V
Group

1

H

Hydrogen
1

7 9 45 48 51 52 55 56 59 59 64 65 11 12 14

Li Be Sc Ti V Cr Mn Fe Co Ni Cu Zn B C N

Lithium Beryllium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Boron Carbon Nitrogen
3 4 23 24 25 26 27 28 29 30 5 6 7
21 22
23 24 93 101 103 106 108 112 27 28 31
89 91 96
Na Mg Nb Ru Rh Pd Ag Cd A Si P
Y Zr Mo Tc
Sodium Magnesium Niobium Ruthenium Rhodium Palladium Silver Cadmium Aluminium Silicon Phosphorus
11 12 Yttrium Zirconium 41 Molybdenum Technetium 44 45 46 47 48 13 14 15
39 40 42 43
39 40 181 190 192 195 197 201 70 73 75
139 178 184 186
K Ca Ta Os Ir Pt Au Hg Ga Ge As
La Hf W Re
Potassium Calcium Tantalum Osmium Iridium Platinum Gold Mercury Gallium Germanium Arsenic
19 20 Lanthanum Hafnium 73 Tungsten Rhenium 76 77 78 79 80 31 32 33

85 88 57 * 72 140 74 75 115 119 122

Rb Sr Ce In Sn Sb

Rubidium Strontium Cerium Indium Tin Antimony
37 38 58 49 50 51

133 137 232 204 207 209

Cs Ba Th T Pb Bi

Caesium Barium Thorium Thallium Lead Bismuth
55 56 90 81 82 83

Fr 226 227

Francium Ra Ac
87
Radium Actinium
88 89 †

*58–71 Lanthanoid series 141 144 Pm 150 152 157 159 163 165 167
†90–103 Actinoid series
Pr Nd Promethium Sm Eu Gd Tb Dy Ho Er
61
Praseodymium Neodymium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium
59 60 62 63 64 65 66 67 68

238 Np Pu Am Cm Bk Cf Es Fm

Pa U Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium
93 94 95 96 97 98 99 100
Protactinium Uranium
91 92

The symbols and proton numbers of the elements

Element Symbol Proton Element Symbol Proton Element Symbol Proton Element Symbol Proton
number number number number
actinium Ac calcium Ca francium Fr lawrencium Lw 103
aluminium Al 89 californium Cf 20 gadolinium Gd 87
americium Am 13 carbon C 98 gallium Ga 64 lead Pb 82
antimony Sb 95 cerium Ce germanium Ge 31 3
argon Ar 51 chlorine Cl 6 gold Au 32 lithium Li
arsenic As 18 chromium Cr 58 hafnium Hf 79 71
astatine At 33 cobalt Co 17 helium He 72 lutetium Lu 12
barium Ba 85 copper Cu 24 holmium Ho 25
berkelium Bk 56 curium Cm 27 hydrogen H 2 magnesium Mg 101
beryllium Be 97 dysprosium Dy 29 indium In 67 80
bismuth Bi einsteinium Es 96 iodine I manganese Mn 42
boron B 4 erbium Er 66 iridium Ir 1 60
bromine Br 83 europium Eu 99 iron Fe 49 mendelevium Md 10
cadmium Cd fermium Fm 68 krypton Kr 53 93
caesium Cs 5 fluorine F 63 lanthanum La 77 mercury Hg 28
35 100 26 41
48 36 molybdenum Mo 7
55 9 57
neodymium Nd

neon Ne

neptunium Np

nickel Ni

niobium Nb

nitrogen N

314

Reference

Key Relative atomic masses (Ar)
for calculations
a
IV V VI VII 0 Element Symbol Ar
X 27
19 4 aluminium Al 80
b bromine Br 40
F He calcium Ca 12
a = relative atomic mass carbon C 35.5
Fluorine Helium X = atomic symbol chlorine Cl 64
9 2 b = proton number copper Cu 19
fluorine F 4
12 14 16 35.5 20 helium He 1
hydrogen H 127
C N O C Ne iodine I 56
iron Fe 207
Carbon Nitrogen Oxygen Chlorine Neon lead Pb
6 7 8 17 10 lithium Li 7
magnesium Mg 24
28 31 32 80 40 manganese Mn 55
neon Ne 20
Si P S Br Ar nitrogen N 14
oxygen O 16
Silicon Phosphorus Sulfur Bromine Argon phosphorus P 31
14 15 16 35 18 potassium K 39
silver Ag 108
73 75 79 127 84 sodium Na 23
sulfur S 32
Ge As Se I Kr zinc Zn 65

Germanium Arsenic Selenium Iodine Krypton
32 33 34 53 36

119 122 128 At 131

Sn Sb Te Astatine Xe
85
Tin Antimony Tellurium Xenon
50 51 52 54

207 209 Po Rn

Pb Bi Polonium Radon
84 86
Lead Bismuth
82 83

165 167 169 173 175

Ho Er Tm Yb Lu

Holmium Erbium Thulium Ytterbium Lutetium
67 68 69 70 71

Es Fm Md No Lr

Einsteinium Fermium Mendelevium Nobelium Lawrencium
99 100 101 102 103

Element Symbol Proton Element Symbol Proton Element Symbol Proton
number number number
nobelium thallium
osmium No 102 rhodium Rh 45 thorium Tl 81
oxygen Os 76 rubidium Rb 37 thulium Th 90
palladium O 8 ruthenium Ru 44 tin Tm 69
phosphorus Pd 46 samarium Sm 62 titanium Sn 50
platinum P 15 scandium Sc 21 tungsten Ti 22
plutonium Pt 78 selenium Se 34 uranium W 74
polonium Pu 94 silicon Si 14 vanadium U 92
potassium Po 84 silver Ag 47 xenon V 23
praseodymium K 19 sodium Na 11 ytterbium Xe 54
promethium Pr 59 strontium Sr 38 yttrium Yb 70
protactinium Pm 61 sulfur S 16 zinc Y 39
radium Pa 91 tantalum Ta 73 zirconium Zn 30
radon Ra 88 technetium Tc 43 Zr 40
rhenium Rn 86 tellurium Te 52
Re 75 terbium Tb 65

315

Index

Index

Where several page numbers ammonium ion, test for  285 butane 252 changes of state  8–11
are given and one is bold, amphoteric oxides  157 butanoic acid  258 charcoal 234
look that one up first. anode 104 but-1-ene 254 charge (for blast
aqueous solution  17
A Ar 70 C furnace) 198
acetone 17 argon  37, 48, 172–173 calamine lotion  153 charge (on sub-atomic
acetylene 213 artificial elements  30, 167 calcium
acidic oxides  157 artificial fertilisers  228 particles) 32
acidity 150 atmosphere 210 reaction with oxygen  93 chemical change  46, 47
atoms 30, 32 reactivity of  184, 188 chemical equations  68–69
and pH number  149 Avogadro constant  76 calcium compounds chemical properties  42
acid rain  214, 225 Avogadro’s Law  80 carbonate  236, 241 chemical reaction  47
acids 148–155 aquifer 218 hydroxide  16, 148, 241 chlorine
oxide  93, 199, 205,
and pH  149 B as a member of Group
as proton donors  154, 155 back reaction  124 240, 241 VII  170–­ 171
carboxylic 258–259 bacteria  35, 141, 142, 218 calcium ions, test for  286
reactions of  152–153 baking soda  52, 153 calculations from bonding in  55
strong and weak 148, 150 balancing equations  68–69 from electrolysis of
addition barium sulfate  160, 287 equations 78–79
polymerisation 264–265 bases 152–153 cancer treatment by brine 108
air 210–213 reaction with sodium 
alanine 274 alkalis (soluble radioisotopes 35
alcoholic drinks  256 bases) 148–152 carbohydrates 272–273 48–50
alcohols 256–257 uses of  109
algae 229 and acids  152–153 complex 273 chlorine water  171
alkali metals  166, 168–169 as proton acceptors  155 carbon  chloromethane 253
alkaline earth metals  166, reactions of  152 chlorophyll 144
182 basic oxides  156 allotropes of  61 chromatogram 23
alkalis 148–152 batteries 122–123 as a reducing agent  196 chromatography (paper) 
alkanes  250, 251, 252–253 bauxite (aluminium in steel  204, 205 23–25
alkenes 254–255 ore) 195, 200 isotopes of  34 chromium  175, 204
allotropes (of carbon)  61, biological catalysts  140 reactivity compared to use in plating  111
234 biological detergents  141 citric acid  148
alloys  203, 204  bio-polymers 271 metals 186, 188 climate change  239
alumina (aluminium bitumen 247 carbon-12  34, 70, 76 coal 214, 244
oxide)  200, 201 blast furnace  198–199 carbonates 236 cobalt chloride  124
aluminium bleaching carbon cycle  234–235 coke 198
alloys of  203 by chlorine  285 carbon dioxide  236 collision theory (for reaction
apparent unreactivity  191 by hydrogen peroxide  87 rate) 138–139
corrosion in  191, 201 by sulfur dioxide  231 and global warming  combustion  93, 114
extraction of  200–201 boiling (change of state)  11 238–239 competition among
in the Earth’s crust  194 boiling points  9 metals 186–187
in the reactivity series  188 and purity  19 and the carbon cycle  compound ions  53
ore  195, 197, 200 for ionic compounds  59 234­–235 compounds 46
properties of  201 for molecular and mixtures  46
uses of  200, 202 bonding in  57 covalent  56–57, 58–59
aluminium ions, test for  286 substances  54, 59 in photosynthesis  235 forming 48
aluminium oxide  195, bond breaking and properties of  236 ionic  50–51, 58–59
197, 201 carbonic acid  148, 236 names and formulae 
amide linkage  266, 274 making 116 carbon monoxide  236
amino acids  24, 274, bond energies  116 as a reducing agent  196 66–67
276, 277 bonding carboxyl functional percentage composition
ammonia 225–227 group 258  
as an alkali  148, 151 between ions  50–51 carboxylic acids  258–259 of 73
bonding in  57 i n giant covalent car exhausts  215 compression of gases  12
Haber process for  226 cast iron  199 concentration of a
in making fertilisers  229 structures 60–61 catalysts 140–141
laboratory in metals  62 biological (enzymes)  140, solution 82–83
in molecules  54–57 finding by titration 
preparation 225 brass 203 142–143 162–163
manufacture 126–127, breathalyser test  99 in car exhausts  215
brine 108 transition elements concrete 241
226–227 electrolysis of  108–109 condensation 11
test for  285 bromide ion, test for  287 as  141, 175 condensation
ammonium compounds bronze 206 cathode 104
chloride 225 burning of fuels  114, cell (producing polymerisation 263,
nitrate  225, 228 118–119 266–267
energy from  118, 119 electricity) 120 condenser 22
cellulose 263 conductivity of metals  42,
cement 241 63, 103
chain length conductors 102–103
Contact process  232
and boiling point  251
and homologous

series 251
in polythene  264

316

index

copper 174 electroplating 111 effect of temperature indicators 149
bonding in  62 elements 30–31 on 12 indigestion 155
in reactivity series  188 empirical formula  84–85 insoluble salts  160–161
refining of  110 endothermic reactions  115 pressure in  12 insulators 102
uses of  202 energy changes during gasoline (petrol)  247 iodide ion, test for  287
giant covalent structures  iodine 170
copper ion, test for  286 reactions 114–115
copper(II) oxide  92 energy from fuels  118–119 60–61 displacement of  171
copper(II) sulfate  158 energy level diagram  114, 115 global warming  238–239 ionic bonds  50–51
enzymes  140, 141, 142–143 glucose 272, 273 ionic compounds  50, 51
electrolysis of equations 68–69 glycerol 275
solution 110 glycine 274 and electrolysis  104
calculations using  78–79 gold 195 formulae of  52
in testing for water  124 half-equations 94 graphite 61 names of  52–53
corrosion ionic equations  95, 154 greenhouse gases  238 properties of  59
equilibrium (in reversible groundwater 218 ions  49, 52, 53
of aluminium  191 reactions) 125 groups in Periodic Table  compound ions  53
of iron  216–217 ester linkage  259, 267, 275 mass of  71
covalent bond  54–55 esters 259 31, 166 iron  174, 175
covalent compounds  56–57 ethane 252 Group 0 (noble alloys of  204–205
covalent giant structures  ethanoates 259 gases) 172–173 corrosion (rusting)
60–61 ethanoic acid  258, 259 Group I (alkali
cracking of ethanol  256, 257 metals) 168–169 of 216–217
hydrocarbons 248–249 ethene  254, 255 Group II (alkaline earth extraction of  198–199
crude oil (petroleum)  evaporation 11 metals) 166 in the Earth’s crust  194
244–245 exothermic reactions  114 Group VII (halogens)  in reactivity series  188
crystallisation 20 explosions 137 170–171 ore 198
cysteine 274 extraction of metals  196–197 properties of  174, 175, 204
gypsum 241 iron ions, test for  286
D F iron(III) oxide  156, 198
decay (radioactivity)  34 fats 275 H iron sulfide  46
denature (enzymes)  141 fatty acids  275 Haber process  226–227 isomers  253, 255
density 182 fermentation 142, 256 haemoglobin  236, 274 isotopes  34, 70
detergents (biological)  141 fertilisers 228–229 half-equations 94
diamond 60 filtering 20 halides 170 K
diaphragm cell  108 filtrate 20 halogens 170–171 kerosene 247
diatomic 54 flue gas desulfurisation  241 heating curve  9 kilojoule (kJ)  114
dichloromethane 253 fluoride (in water helium  37, 172, 173 kinetic particle theory  11
diesel (fraction from hematite (iron ore)  198 krypton  172, 173
supply) 219 homologous series  251
petroleum) 247 formulae  46, 66 hydrocarbons  251, 252, 254 L
diffusion  7, 13 hydrochloric acid  148, 150 lattice  50, 58
displacement reactions  171, empirical 84–85 lead
molecular 86–87 electrolysis of dilute  105
185, 187 of compounds  66–67 electrolysis of and extraction
dissolving 16 of ionic compounds  52–53 methods 196
distillation 22 formula mass  71 concentrated 105
distilled water  22 forward reaction  124 hydrogen 224 ‘lead’ in pencils  61
double bonds  55 fossil fuels  244 reactivity of  185, 186, 188
fountain experiment  225 as a fuel  119, 121 lead bromide, electrolysis
in alkenes  254 fractional distillation  22 bonding in  54 of  104, 106
ductile (of metals)  63, 182 fractions in fractional displacement of  185 Le Chatelier’s principle  126
dynamic equilibrium  125 distillation 246 from electrolysis of light (and photochemical
fractions from refining reactions) 144–145, 253
E petroleum 247 brine 108 lime  153, 240
Earth’s crust  194 freezing 8 in Periodic Table  167 limestone 153, 240–241
electricity 102 freezing point  8 reactivity relative to limewater  241, 285
electrode 104 fuel cell  121 liquids 8–11
electrolysis 102–111 fuel oil  247 metals 188 lithium 123, 168, 169
fuels 118–119 test for  285 litmus 148
in extraction of functional group  251, 254, uses of  109 locating agent  25
aluminium 201 256, 258 hydrogen chloride  116, 150 lubricating fraction  247
bonding in  56
in extraction of G hydrogen ions, in acids  M
metals 196–197 galena (ore)  230 150, 154 macromolecules 262,
galvanising  191, 217 hydrogen sulfide  67, 230
of brine  108 gas chromatography  26 hydrolysis 272–275
of copper(II) sulfate gases  8, 10, 12–13 in digestion  276 magnesium  51, 132, 185
in the lab  277 magnesium chloride  51,
solution 110 and Avogadro’s Law  80 hydroxide ions (and
of molten compounds  104 compression of  12 alkalinity) 151 132, 185
of solutions  105 diffusion in  13 hydroxides  152, 184, 189 magnesium oxide  51, 85, 186
electrolyte 103 magnesium sulfate (Epsom
electron distribution  36–37 I
electrons  32, 36 impurities 18–17 salts) 52
electron shells  36 incomplete combustion  252
electron transfer (in redox
reactions) 94

317

Index N oxygen mask  213 changing properties
names for compounds  52– oxygen tent  213 of 268
malleable (of metals)  63, 174 oxygen, test for  285
manganese (and variable 53, 66–67 uses of  269
naphtha  247, 249 P potassium (as Group I
valency) 96 natural gas  118, 244 painting (against rust)  217
manganese(IV) oxide  natural polymers  263 palmitic acid  275 metal) 168–169
neon 48, 172–173 paper chromatography  23, reactivity  184, 185, 188
122, 140 neutralisation reactions  153,
mass of atoms, molecules 24­–25 potassium compounds
154–155 paraffin (kerosene)  247 bromide, and
and ions  70–71 neutral liquids (and pH)  149 particles in matter  6–7, displacement 171
melting  8, 9, 10 neutral oxides  157 bromide, and
melting points  8, 9 neutrons  32, 33 10–11 electrolysis 105
nickel 174 evidence for 6, 7 bromide, and
and purity  19 ninhydrin 25 photography 161
of ionic compounds  59 nitrate ion, test for  287 pentane 250 dichromate(VI), as
of metals  62 nitrates  152, 160, 189 percentage composition of oxidising agent  99
of molecular covalent nitric acid  148 iodide, and
nitrogen 224 compounds 73 displacement 171
compounds 59 percentage purity  73, 88–89 iodide, as reducing
of giant covalent bonding in  55 percentage yield  88 agent 99
for plants  228 Periodic Table  166–167, hydroxide  148, 151, 184
structures 60 production in manganate(VII) and
metallic bonds  62 178–179 diffusion 7
metalloids 176 industry 212 petrol (gasoline)  87, 247 manganate(VII), as
metal oxides  156, 157 uses 213 petroleum (crude oil)  oxidising agent  98
metals  42, 43, 182–183 nitrogen oxides as
pollutants 214 244–245 potassium for plants  228
bonding in  62–63 noble gases  172–173 and pollution  214 power stations  118, 119,
compared with non- electron distribution in  48 refining of  246–247
in Periodic Table  166 sulfur extraction from  230 231, 241 
metals 42–43 uses of  173 precipitation 160–161
extraction from ores  non-conductor 102 pH scale  149 pressure in gases  12
non-metals  42, 43 phenolphthalein 149 propane 250, 252
196–197 compared with metals  42 phosphorus propane-1,2,3-triol
in Earth’s crust  194 in Periodic Table  31
in Periodic Table  182 reactions with oxygen  157 combustion in oxygen  157 (glycerol) 275
in reactivity series  188 non-renewable resource  245 impurity in steel- propanoic acid  258
ores 195 nuclear fuels  119 propanone 17
properties of  182–183 nucleon number  33 making 205 propene 254
reactions with nucleus of atoms  32 for plants  228 proteins 263, 272
nylon  266, 269 phosphorus pentoxide  157
oxygen 156 photographic film  145, 161 from polymerisation of
reactivity of  184–188 O photosynthesis  144, 234 amino acids  274
stability of oil (petroleum)  244–245 physical change  47
physical properties  42 hydrolysis of  276, 277
compounds 189 and pollution  214 phytoplankton 235 proton donors and
transition elements  refining of  246–247 plastics 262, 268–269
sulfur extraction from  230 and pollution  270–271 acceptors 155
174–175 ores  195, 196 made by proton number  32, 33
uses of 175, 202–203 organic chemistry  237 protons 32
metal salts  152, 158–161 organic compounds  237, 250 polymerisation 264–267 purity 18
methane 252 oxidation 92 platinum
as fuel (natural gas) 244 and electron transfer  94–95 and melting and boiling
as greenhouse gas  238 oxidation state  96–97 in catalytic converters  215 points 19
bonding in  56 oxides 156–157 in the Earth’s crust  194
methanoic acid  252, 258 oxidising agents  98–99 for inert electrodes  104 percentage  73, 88, 89
methyl orange indicator 149 oxy-acetylene torch  213 pollution PVC (polychloroethene) 
mild steel  204 oxygen  in air  214–215
mining of metal ores  195 in air  210–211 by plastic  270–271 265, 269
mixtures 16 bonding in the polyamide 266
compared with poly(chloroethene) or Q
molecule 55 PVC 265 quartz 60
compounds 46 bonding in ionic polyester 267 quicklime  240, 241
mobile phase (in polymerisation  255, 263,
compounds 51 264–267 R
chromatography) 26 reaction with metals and polymers  262–263, 264–267 radiation  34, 35
molar volume of a gas  80 poly(propene) 265 radioactivity 34–35
molar solution  82 non-metals 156–157 polysaccharide 273 radioisotopes 34
mole 76 separation from air  212 polystyrene 265 random motion of
molecular formulae  uses 213 polythene, or
poly(ethene) 262, 264 particles 6
46, 66 and chain lengths  264 rate of reaction  131,
molecular substances  and pollution  270
130–145
54–57, 59 and catalysts  140–141
molecules 54 and concentration  134, 138

masses of  71
monomer  262, 264, 266
monosaccharides 273
Mr 71

318

and photochemical sand 60 starch  263, 272 index
reactions 140–141 saturated compounds from polymerisation of
glucose 273 U
and surface area  136–137, (alkanes) 252 hydrolysis of  276, 277 universal indicator  149
139 saturated solutions  17 unsaturated (organic
scientific method  280 state symbols  68 compounds) 254
and temperature  135, 139 semi-conductors 177 steel 175
measuring  131, 132–137 separation methods  20–25 test for unsaturation  255
reactants 68 shells (electron)  36 electroplating of  111 unsaturated fats  275
reactions, equations for  silicon dioxide (silica)  60, galvanising of  191
68–69 manufacture of  204–205 V
energy changes in  114–115 61, 66 recycling of  205 valency  66, 67, 176
reversible 124–125 silver (a transition styrene 265 valency electrons  166
reactivity substitution reaction  253 variables (in experiments)  280
of Group I metals  168–169 element) 174 sulfates 152 vinegar 258
of Group VII and electroplating  111 solubility of  160 vinyl chloride  265
in film photography  145 sulfur 30, 230 viscosity  247, 251
(halogens) 170–171 reactivity of  184, 185, 188 sulfur dioxide  157, 231 volatile liquids  17, 246
of Group 0 (noble and flue gas voltage (of cells)  190
silver bromide  145, 161 vulcanizing 230
gases) 172 single bond  54 desulfurisation 241
of metals  184–187 slag  199, 205 as pollutant  214, 231 W
reactivity series of slaked lime  153, 241 sulfur trioxide  232 water 224
metals 188 smoke particles  6 sulfuric acid  233
recycling iron and steel  205 soap 277 manufacture of  232 as solvent  16, 17
redox reactions  92–97 sodium properties  233 bonding in  56
and electron transfer  sulfurous acid  231 changes of state for  8
as alkali metal  168–169 surface area of solid formula of  46
94–95 extraction of  196 heating curve for  9
and oxidation state  96–97 properties of  168–169 reactant reaction with metals  184
reducing agent  98, 99 sodium chloride  48 and rates of tests for  124
reduction 92–95 bonding in  48, 50 reaction  136–137, 139 uses of  218
in metal extraction  196 electrolysis of molten and risk of explosions  137 water supply  218–219
refining petroleum (oil)  22, symbols for elements  30 water vapour  8
246–247 compound 105 synthetic polymers  262
relative atomic mass, Ar 70 electrolysis of X
relative formula mass, Mr 71 T xenon  172, 173
relative molecular mass, solutions  105, 106–108 Teflon  265, 269
Mr 71 structure and Terylene  267, 269 Y
residue from filtration  20 tests in the laboratory yeast 142, 256
respiration 234, 235 properties  58, 59 yield 88
reversible reactions  124–125 sodium hydroxide  184 for anions and
Rf value  25  cations 286–287 in making ammonia  126,
rock salt  195 as alkali  148, 151 227
rotary kiln  240 from electrolysis of for gases  285
rubber (vulcanizing of)  230 for unsaturation  255 Z
rusting and its prevention brine 108 for water  124 zinc  174, 182
216–217 uses of  109 tetrachloromethane 253
soil acidity  153, 240 thermal decomposition  189, extraction of  197
S solidifying 11 240, 248 reactivity of  184–186, 188
sacrificial protection  191, solids  8, 11 thermite process  190 uses of  202
solutions 16–17 tin (for plating steel)  111 zinc blende (ore)  197
217 concentration of  82–83 titanium 108, 206, 207, 264 zinc chloride  185
salt (sodium chloride)  50, 58 electrolysis of  105, titrations 159, 162–163 zinc oxide  157
salts 152 tracers 35 zinc sulfate  131
106–107 transition elements  167,
making in laboratory  solvents  16, 17 174–175
158–161 sonorous 182 as catalysts  141, 175
stability of metal trichloromethane 253
solubility of some  160
compounds 189
stainless steel  204, 205
standard solution  162

319

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Dino O./Shutterstock; P150b: Rob Cruse/Istockphoto; P151: RMG; P152t: OUP; P152m:
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P157t: OUP; P157b: Jodi Jacobson/Istockphoto; P158: Canis Maior/Shutterstock; P159:
Laurence Gough/Istockphoto; P160: OUP; 161t: Brenda Carson/Shutterstock; 161bl:

320

Complete Authors
RoseMarie Gallagher
Chemistry Paul Ingram

for Cambridge IGCSE®

Second Edition

Complete Chemistry for Cambridge IGCSE® provides clear and comprehensive RoseMarie Gallagher
support for the Cambridge International Examinations syllabus for Chemistry. This and Paul Ingram are
bestselling resource now includes a CD with past paper questions and revision a well-known author
checklists to fully develop understanding. team with a wealth of
teaching, examining
Oxford and Cambridge are world leaders in international education. Our combined and authoring
expertise and knowledge shape Oxford’s resource packages for Cambridge IGCSE. experience.
You can rely on:

● Fully comprehensive, endorsed student textbooks, mapped to the Cambridge
syllabus, equipping students to tackle complex theory

● Customisable digital Teacher Kits endorsed by Cambridge and loaded with
digital material to support effective delivery

● Thorough revision support focused on building exam confidence and supporting
achievement

Step-by-step approach simplifies complex ideas

Application boxes link learning to the real world

Also available: 978 0 19 913881 4
978 0 19 915266 7

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