Chapter 1 - Structure and bonding
Use a periodic table and a table of charges on ions to help you to answer these
questions.
1
Choose a word from the list to complete each sentence.
a
When metals react with non-metals electrons are ……………………
combined
b
shared
transferred
(1)
When non-metal elements combine their atoms are held together by
…………………… bonds.
covalent
2
ionic
metallic
Choose a description from the list for each of the substances.
giant covalent
3
(1)
giant ionic
metal
simple molecule
a
ammonia, NH3 ………………..
c
lithium, Li ………………….
b
diamond, C ………………….
d
sodium oxide, Na2O ……………….
Choose a number from the list to complete each sentence.
0
a
1
2
3
4
6
7
The elements in Group …. in the periodic table all form ions with
a charge of 1+.
b
(1)
The elements in Group …. in the periodic table all form ions with
a charge of 2−.
c
(1)
The elements in Group 4 in the periodic table all form …. covalent
bonds.
4
(4)
(1)
d
The aluminium ion has a charge of ….+
a
Choose the correct formula from the list for iron(III) chloride.
FeCl
b
Fe3Cl
FeCl3
(1)
Fe3Cl3
(1)
Choose the formula from the list for each of these ionic compounds.
NaS
NaSO4
Na(SO4)2
Na2S
NaS2
Na2SO4
i
sodium sulfide ………………..
(1)
ii
sodium sulfate ………………..
(1)
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5
Calcium hydroxide, Ca(OH)2, is an ionic compound.
Which of the ions in the list are the ions in calcium hydroxide?
Ca+
Ca2+
Ca4+
OH−
OH2−
OH2−
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6
(2)
Sodium reacts with chlorine. The reaction forms sodium chloride.
a
Use words from the list to answer the questions.
compound
element
hydrocarbon
mixture
Which word best describes:
b
i
sodium …………………………
ii
sodium chloride? …………………………
(1)
(1)
When sodium reacts with chlorine the sodium atoms change into sodium ions.
The diagrams represent a sodium atom and a sodium ion.
Use the diagrams to help you explain how a sodium atom turns into a sodium ion.
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c
i
(2)
The diagram below represents a chlorine atom.
When chlorine reacts with sodium the chlorine forms negative chloride ions.
Copy and complete the diagram below to show how the outer electrons are
arranged in a chloride ion (Cl–).
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C2 – Additional Chemistry
ii
Chloride ions are strongly attracted to sodium ions in sodium chloride.
Explain why.
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7
(1)
Chlorine can form compounds with ionic or covalent bonds.
a
Potassium chloride, KCl, has ionic bonds. Draw dot and cross diagrams to show
what happens to potassium atoms and chlorine atoms when they react to form
potassium chloride. You only need to show the outer electrons in your diagrams.
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b
(4)
Hydrogen chloride, HCl, has covalent bonds. Draw a dot and cross diagram to
show the bonding in hydrogen chloride.
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8
Sodium metal is a giant structure of sodium atoms.
Explain how the atoms are held together in sodium metal.
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Rainford High Technology College Chemistry
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Chapter 2 - Structure and properties
1
Match each of the substances in the table with a description from the list.
giant covalent
ionic
metal
simple molecule
Substance
Formula
Melting
point (°C)
Boiling
point (°C)
Does it
conduct
electricity
when liquid?
a
C
3550
4830
No
b
Co
1768
3142
Yes
c
CH4
–182
–164
No
d
CaCl2
1055
1873
Yes
a ………………………………………….
b ………………………………………….
c ………………………………………….
d ………………………………………….
2
(4)
Copper can be hammered into shape.
The structure of copper metal can be represented as shown:
a
Explain why copper can be hammered into shape.
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b
Copper can be mixed with zinc to make the alloy called brass. Brass is much
harder than copper. Explain why.
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c
(2)
Copper can be mixed with zinc and aluminium to make a shape memory alloy.
What is a shape memory alloy?
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3
(2)
Choose a word from the list to complete each sentence.
different
identical
smart
thermosoftening
thermosetting
The polymers low-density poly(ethene) (LDPE) and high-density poly(ethene)
(HDPE) are made from monomers that are ………………………… . The polymers are
produced using catalysts and reaction conditions that are ………………………… . LDPE
melts at 120°C and HDPE melts at 130°C and they have no cross-links between
the polymer chains so they are both…………………………… polymers.
4
(3)
Chloroethene, C2H3Cl, can be polymerised to poly(chloroethene).
a
Explain in terms of its structure why chloroethene is a gas at room
temperature.
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b
Explain in terms of its structure why poly(chloroethene) is a thermosoftening
polymer.
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5
The picture shows a copper kettle being heated on a camping stove.
a In this question you will be assessed on using good English, organising
information
clearly and using specialist terms where appropriate.
Copper is a good material for making a kettle because it has a high melting
point.
Explain why copper, like many other metals, has a high melting point. You should
describe the structure and bonding of a metal in your answer.
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b
(6)
An aeroplane contains many miles of electrical wiring made from copper. This
adds to the mass of the aeroplane.
It has been suggested that the electrical wiring made from copper could be
replaced by lighter carbon nanotubes.
The diagram shows the structure of a carbon nanotube.
i
What does the term ‘nano’ tell you about the carbon nanotubes?
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ii
Like graphite, each carbon atom is joined to three other carbon
atoms. Explain why the carbon nanotube can conduct electricity.
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Chapter 3 - How much?
1
a
An atom of phosphorus can be represented as:
31
15
P
b
i
What is the number of protons in this atom of phosphorus? …………..
(1)
ii
What is the number of neutrons in this atom of phosphorus? …………
(1)
iii
What is the number of electrons in this atom of phosphorus? ………..
(1)
A different atom of phosphorus can be represented as:
32
15
P
i
What are these two atoms of phosphorus known as? ……………………
ii
Give one way in which these two atoms of phosphorus are different.
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2
(1)
(1)
Toothpastes often contain fluoride ions to help protect teeth from attack by
bacteria.
Some toothpastes contain tin(II) fluoride. This compound has the formula SnF2.
a
Calculate the relative formula mass (Mr) of SnF2.
(Relative atomic masses: F = 19; Sn = 119)
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b
Calculate the percentage by mass of fluorine in SnF2.
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c
(2)
(2)
A tube of toothpaste contains 1.2 g of SnF2. Calculate the mass of fluorine in
this tube of toothpaste.
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3
The diagram shows what happens when ammonium chloride is heated.
The reaction that takes place is:
NH4Cl (s)
a
NH3 (g) + HCl (g)
What does
in the equation mean?
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b
(1)
Explain why the white solid appears near the top of the test tube.
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4
(2)
The diagram shows the main parts of an instrumental method called gas
chromatography linked to mass spectroscopy (GC–MS).
This method separates a mixture of compounds and then helps to identify each of
the compounds in the mixture.
a
In which part of the apparatus:
i
is the mixture separated?
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ii
(1)
is the relative molecular mass of each of the compounds in the mixture
measured?
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iii
are the results of the experiment recorded?
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b
i
(1)
Athletes sometimes take drugs because the drugs improve their performance.
One of these drugs is ephedrine.
Ephedrine has the formula:
C10H15NO
What relative molecular mass (Mr) would be recorded by GC–MS if ephedrine was
present in a blood sample taken from an athlete? Show clearly how you work out your
answer.
(Relative atomic masses: H = 1; C = 12; N = 14; O = 16.)
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ii
(2)
Another drug is amphetamine which has the formula: C9H13N
The relative molecular mass (Mr) of amphetamine is 135.
Calculate the percentage by mass of nitrogen in amphetamine.
(Relative atomic mass: N = 14.)
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c
(2)
Athletes are regularly tested for drugs at international athletics events.
An instrumental method such as GC-MS is better than methods such as titration.
Suggest why.
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5
A chemist thought a liquid hydrocarbon was hexane, C6H14.
Relative atomic masses: H = 1; C = 12
a
Calculate the percentage of carbon in hexane.
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b
(2)
The chemist analysed the liquid hydrocarbon and found that it contained 85.7%
carbon. Calculate the empirical formula of the hydrocarbon based on this
result. You must show your working to gain full marks.
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c
(4)
Was the liquid hydrocarbon hexane? Explain your answer.
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Rainford High Technology College Chemistry
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Chapter 4 - Rates and energy
1
A glue is made by mixing together two liquids.
a
When the liquids are mixed an exothermic reaction takes place. Complete the
sentence below using a word or phrase from the list.
decrease
increase
stay the same
During the reaction the temperature of the mixture will …………………….
b
(1)
The time taken for the glue to set at different temperatures is given in the
table below.
Temperature (°C)
Time taken for the glue to
set
20
3 days
60
6 hours
90
1 hour
Complete the sentences below using words or phrases from the list.
decreases
i
increases
stays the same
When the temperature is increased the time taken for the glue to set
……………………........
ii
When the temperature is increased the rate of the setting reaction
………………………….
c
(2)
Which two of the following are reasons why an increase in temperature affects
the rate of reaction? (circle your answers)
It gives the particles more energy.
It increases the concentration of the particles.
It increases the surface area of the particles.
It makes the particles move faster.
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2
Instant cold packs are used to treat sports injuries.
One type of cold pack has a plastic bag containing water. Inside this bag is a smaller
bag containing ammonium nitrate.
The outer bag is squeezed so that the inner bag bursts. The pack is shaken and
quickly gets very cold as the ammonium nitrate dissolves in the water.
a
Explain why the pack gets cold.
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b
(2)
Suggest and explain why the pack is shaken after the inner bag has burst.
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3
(2)
A student reacted small pieces of zinc with dilute acid to make hydrogen gas. The
graph shows how the volume of hydrogen gas produced changed with time.
a
Describe, as fully as you can, how the rate of this reaction changes with time.
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b
The student wanted to make the reaction go faster.
Which suggestion would make the reaction go faster? (circle your answer)
Use bigger pieces of the same total mass of zinc.
Use more of the dilute acid.
Use zinc powder.
c
(1)
The student decided to increase the concentration of the acid. Explain, in
terms of particles, why increasing the concentration of the acid increases the
rate of reaction.
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d
(2)
The student increased the temperature of the reaction by 10°C. The student
found that the reaction went twice as fast. Explain, as fully as you can, why an
increase in temperature increases the rate of the reaction.
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4
(3)
Platinum is used as a catalyst in many industrial processes. Platinum is a very
expensive metal. The catalysts often contain only about 1% platinum dispersed on an
inert support such as aluminium oxide to give a surface area of about 200 m2 per
gram. Cobalt catalysts with nanosized particles have been developed as an
alternative to platinum catalysts for use in some industrial processes.
a
Suggest two reasons why platinum is used as a catalyst, even though it is very
expensive.
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(2)
b
Explain, in terms of particles, why catalysts like platinum should have a very
large surface area.
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c
(2)
Suggest an economic reason and an environmental reason why cobalt catalysts
have been developed as alternatives to platinum catalysts.
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d
(2)
Suggest three reasons why the use of catalysts is important in industrial
processes.
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Chapter 5 - Salts and electrolysis
1
Hydrogen chloride gas reacts with water to make hydrochloric acid. The equation
for the reaction is:
HCl (g) → H + (aq) + Cl− (aq)
a
b
Which of the following shows that an acid has been made? (circle your answer)
A
An aqueous solution has been made.
B
Hydrogen ions have been made.
C
Chloride ions have been made.
Choose a number from the list for the pH of hydrochloric acid.
1
c
(1)
7
12
…………………….
(1)
Hydrochloric acid reacts with sodium hydroxide solution to produce a salt and
water.
i
Choose a word from the list that describes sodium hydroxide.
alcohol
ii
alkali
insoluble
.…………………….
Choose a word from the list to complete the sentence.
The reaction between hydrochloric acid and sodium hydroxide is an example
of ……………………..
combustion
iii
neutralisation
oxidation
Name the salt made when hydrochloric acid reacts with sodium hydroxide.
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2
(3)
Lead chloride is a white insoluble salt. It can be made by mixing lead nitrate
solution with sodium chloride solution. Both of these solutions are colourless.
a
What would you see when lead nitrate solution is mixed with sodium chloride
solution?
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b
(1)
Write a word equation for the reaction.
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c
A mining company produces wastewater that contains dissolved lead ions.
Suggest how the company could treat the wastewater to reduce the
concentration of lead ions.
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3
(2)
In this question you will be assessed on using good English, organising information
clearly and using specialist terms where appropriate.
Copper( II) oxide is an insoluble base.
Describe how you could make crystals of copper( II) sulfate from copper( II) oxide.
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4
The diagram shows a nickel spoon being coated with silver.
a
Explain why silver ions in the solution move towards the spoon.
b
Use words from the list to complete the sentence.
gaining
losing
sharing
electron
neutron
(2)
proton
When silver ions reach the spoon they change into silver atoms
by .……………………. an .……………………..
c
(2)
Suggest one reason why spoons made from nickel are coated with silver.
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5
(1)
Magnesium is manufactured by the electrolysis of molten magnesium chloride. The
container is made of steel, which is the negative electrode. Carbon (graphite) is used
for the positive electrode.
a
Steel and carbon (graphite) both conduct electricity.
i
Suggest one other reason why the negative electrode is made of steel.
......................................................................................................................................................................................
ii
(1)
Suggest one other reason why the positive electrode is made of carbon
(graphite).
......................................................................................................................................................................................
b
(1)
Magnesium chloride melts at 950°C. It is mixed with sodium and calcium
chloride so that it can be electrolysed at 750°C.
i
Suggest one way this benefits the manufacturer.
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(1)
ii
Suggest one way this benefits the environment.
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c
(1)
Complete and balance the equations for the reactions at the electrodes.
i
At the negative electrode:
….Mg2+ + ….e– → ….Mg
(1)
ii
At the positive electrode:
….Cl− → ….Cl2 + ….e−
(1)
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[H]