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Higher Grade Chemistry (HS)
1.1
Which of the following is an isomer of
2,2-dimethylpentane?
A CH3CH2CH2CH2CH3
B (CH3)2CHCH2CH(CH3)2
C CH3C(CH3)2CH2CH2CH3
D (CH3)2CHCH2C(CH3)3
1.2
Ethene can be used in the production of polythene.
What type of reaction is used to produce ethene
from ethane?
A addition
B hydrogenation
C cracking
D oxidation
1.3
1.4
1.5
1.6
1.7
Which of the following kinds of pollution from a
car engine is not caused by incomplete
combustion?
A C
B CO
C CO2
D C8H18
Wich of the following hydrocarbons does not have
any isomers?
A pentane
B 2-methylpropane
C propane
D propene
Which of the following would be produced when
bromine, Br2, reacts with pent-2-ene?
A 1,1-dibromopentene
B 2-bromopentane
C 2,2-dibromopentane
D 2,3-dibromopentane
Which of the following represents the complete
combustion of propane?
A C3H6 + 9/2O2  3CO2 + 3H2O
B C3H8 + 5O2  3CO2 + 4H2O
C C3H8 + 7/2O2  3CO + 4H2O
D C5H12 + 8O2  5CO2 + 6H2O
Which of the following represents a cracking
reaction?
A C3H8 + 5O2  3CO2 + 4H2O
B C3H6 + H2  C3H8
C C3H8  C3H6 + H2
D C3H6 + H2O  C3H8O
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Unit 2 “The World of Carbon” Homework
1.8
1.9
1
Which of the following represents an addition
reaction?
A C3H6 + 9/2O2  3CO2 + 3H2O
B C3H6 + H2  C3H8
C C3H8  C3H6 + H2
D C3H8  CH4 + C2H4
3  1022 molecules of methane will weigh;
A 4.8  10 23 g
B 16 g
C 0.8 g
D 5.3  10-22 g
1.10
This hydrocarbon, CH2CHCH(CH3)2
will be called;
A pentane
B 2-methylbut-1-ene
C 3-methylbut-1-ene
D 3,3-dimethylprop-1-ene
1.11
The hydrocarbon with the name
2,3-dimethylbut-2-ene will have the formula
A CH3CHCHCH3
B CH(CH3)2CH(CH3)2
C CH3CH2CH2CHCH2
D CH2CH(CH3)CH(CH3)2
1.12
The ozone layer is thought to be damaged by
A hydrocarbons
B carbon dioxide
C nitrogen oxides
D chlorofluorocarbons
1.13
Which of the following is an unsaturated
hydrocarbon?
A CH3CH2CH2CH2CH2CH3
B (CH3)2CHCH(CH3)2
C CH3CH2CHCHCH2CH3
D (CH3)3CCH2CH3
1.14
When ethene undergoes an addition reaction with
chlorine, Cl2, the main product will be
A CCl2CCl2
B CH3CHCl2
C CH3CH2Cl
D CH2ClCH2Cl
1.15
Which of the following is a saturated
hydrocarbon?
A 2,2-dimethyloct –3-ene
B methylcyclopentane
C 2,3-dimethylhept-1-ene
D but-1,3-diene
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Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
2
Give systematic names for the following hydrocarbons;
1.16
H
a
H
H
H
C
C
H
H
b
H
H
H
H
H
C
C
C
C
C
H
H
H
H
H
H
C
H
H
H
H
H
H
H
C
C
C
C
C
H
H
H
C
H
H
C
H
H
H
C
C
H
H
H
H
c
H
H
H
H
H
H
H
C
C
C
H
H
H
H
H
C
H
C
H
H
C
H
H
H
C
H
C
C
H
H
H
1.17
1.18
Draw the structural formula for;
(a)
methylpropane
(b) 2,4-dimethylpentane
Styrene has the following structure:
H
H
C
C
(c) 2,2,5,5-tetramethylhexane
H
(a)
(b)
(c)
(d)
(e)
1.19
(a)
Give the systematic name for styrene.
Give the molecular formula for styrene.
Calculate the mass of 0.1 moles of styrene.
Styrene contains a benzene ring.
(i)
Describe what you would see if benzene was shaken with bromine water.
(ii)
Explain what is meant by ‘delocalised electrons’.
(iii)
Describe what you would see if styrene was shaken with bromine water.
(iv)
Draw the structural formula for the product of the reaction between styrene and iodine.
Styrene can undergo addition polymerisation.
(i)
What kind of polymerisation will this be?
(ii)
Draw part of the polymer chain showing at least three monomer units.
(iii)
Draw the repeating unit for this polymer.
(iv)
Name the polymer, and give some uses for it.
Draw a neat labelled diagram for the apparatus which could be used in the school lab to perform
the following experiment.
“Liquid hexane was evaporated and passed over a hot alumina catalyst. A mixture of ethene and butane was
made. The mixture of gases was passed through a condenser to remove unreacted hexane, and then through
bromine water to remove one of the gases. The remaining gas was collected over water.”
(b)
(c)
(d)
(e)
(f)
(g)
(h)
Write an equation using shortened structural formulae showing the hexane reacting.
What kind of reaction is this?
Draw the structural formula for the product of the reaction in which one of the gases is removed by
the bromine water.
Name the product of this reaction.
What kind of reaction is this?
What property of the remaining gas allows it to be collected over water?
Analysis of the gas collected at the end shows it to be a mixture of similar compounds. Give a
possible explanation for this.
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carbon monoxide
nitrogen
other gases
A
B
C
D
2.3
Unit 2 “The World of Carbon” Homework
2.6
12
0
50
47
3
82
34
2
32
0
8
44
51
14
2
4
2
4
6
3
Which of the following represents an addition
reaction?
A CH3CH3  CH2CH2 + H2
B CH3CH2OH  CH2CH2 + H2O
C CH2CH2 + H2O  CH3CH2OH
D CH3OH + O2  HCOOH + H2O
C
C
C
H
CH3 CH3 CH3
has the systematic name;
A 1,1,2,2,3,3-hexamethylpropane
B 2,3,3,4,4-pentamethylbutane
C 2,3,4-tetramethylpentane
D 2,3,3,4-tetramethylpentane
2.7
Which of the following statements about the
petrol (gasoline) fraction from the distillation
of crude oil is correct?
A it is the first fraction to distil out
B its boiling range is 180 to 250 oC
C it contains alkane molecules with 5 to 10
carbon atoms per molecule
D it contains alkane molecules with 11 to 16
carbon atoms per molecule
2.8
Which of the following statements is true
about straight chain alkanes?
A they polymerise readily
B only those with small molecules will burn
C they form addition compounds with
halogens
D the melting points increase with molecular
mass
2.9
Compared to diesel, petrol will;
A evaporate less easily
B contain larger molecules
C ignite more easily with a flame
D have a higher viscosity
2.10
Which of the following statements about
benzene is false?
A it is an aromatic compound
B it rapidly decolourises bromine water
C it can be obtained by reforming naphtha
D it contains delocalised electrons
2.11
The gas C2H4 is used on an industrial scale in
the manufacture of;
A bottled gas fuel
B petrol
C explosives
D an addition polymer
2.4
potential energy /kJ mol-1
100
50
reactants
0
-50
-100
products
reaction path 
The enthalpy change for this reaction will be;
-50
A
-150
B
-200
C
D +100
2.5
When ethene undergoes an addition reaction
with chlorine, the product will be;
A CCl2CCl2
B CH3CHCl
C CH2ClCH2Cl
D CH3CH2Cl
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This hydrocarbon;
CH3 CH3 CH3
H
Which fuel in the following table is most like
natural gas?
percentage composition
methane
2.2
Liquified petroleum gas (LPG) is generally a
mixture of ;
A octane and butane
B butane and propane
C propane and ethane
D ethane and methane
hydrogen
2.1
Higher Grade Chemistry (HS)
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Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
4
2.12
(a) Draw two isomers of C5H10, such that one is saturated and one is unsaturated.
(b) Give the systematic name for each of the isomers.
2.13
“Markovnikov’s Rule refers to the most common way in which asymmetric molecules will add across double
bonds. In general, when an asymmetric molecule such as HCl adds across a double bond, the hydrogen atom
will attach to the carbon atom which already has the greater number of hydrogen atoms.”
(a) What does ‘asymmetric’ mean?
(b) Use the reaction between HCl and but-1-ene to show how Markovnikov’s Rule works.
(c) Explain why Markovnikov’s Rule does not apply to but-2-ene.
(d) Draw the full structural formula for the product of the reaction between HCN and propene if it follows
Markovnikov’s rule.
(e) Explain why this is an important synthesis route in organic chemistry.
2.14
Draw full structural formulae for the following hydrocarbons;
(a) 2,2,4-trimethylpentane
(b) 4,4-dimethylpent-2-ene
(c) 2-phenylpropane
Give systematic names for;
(a)
C
(c)
2.15
C
C
C
(b)
C
C
C
C
C
C
C
C
C
C
C
C
C
C
C
2.16
(a) Explain why unleaded petrol must contain a larger proportion of branched chain hydrocarbons than
leaded petrol.
(b) Describe how these branched chain hydrocarbons could be made from naphtha.
(c) Name three polluting gases produced in car engines.
(d) Give a few details about the problems which one of these polluting gases could cause.
2.17
(a) How many atoms are in 2.5 g of ethene?
(b) What is the mass of 3  1030 molecules of ethane?
(c) What mass of hydrogen gas will be produced when 4.5 g of magnesium reacts with 200 cm3 of 2 mol l-1
nitric acid according to the equation;
Mg + 2HNO3  Mg(NO3)2 + H2
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3.1
3.2
3.3
Higher Grade Chemistry (HS)
Which of the following molecules is an alcohol?
A CH3CH2CHCH2
B CH3OCH2CH3
C CH3CH2COOH
D CH3CH(OH)CH3
Which of the following is true for propane and
propan-1-ol?
A soluble in water
B burns to give carbon dioxide and water
C reacts with sodium to give hydrogen
acidified potassium dichromate solution
D
changes colour from orange to green
Which of the following represents a tertiary
alcohol?
A (CH3)2C(OH)CH2CH3
B CH3CH(OH)CH2CH3
C CH3CH2CH2CH2OH
D (CH3)2CHCH(OH)CH3
3.4
The kind of reaction involved in converting
propene into propan-2-ol is
A oxidation
B addition
C cracking
D dehydrogenation
3.5
The insecticide DDT has a molecular mass of
354.5 and contains 50% by mass of chlorine.
The number of chlorine atoms per molecule will
be;
A 2
B 3
C 4
D 5
3.6
Which of the following is a secondary alcohol
and also an isomer of pentan-1-ol?
A
B
C
D
H
H
H
H
H
OH H
H
H
C
C
C
C
C
H
H
H
H
H
H
H
H
H
OH
C
C
C
C
C
H
H
H
H
H
H
H
H
H
H
H
C
O
C
C
C
C
H
H
H
H
H
H
H
O
H
H
C
C
C
C
C
O
H
H
H
H
Unit 2 “The World of Carbon” Homework
3.7
Which of the following reactions represents
reforming?
A C6H14  C2H4 + C4H10
B C4H8 + H2  C4H10
C nC2H4  {C2H4}n
D C6H14  C6H6 + 4H2
3.8
100 cm3 of ethane gas is mixed with 600 cm3 of
oxygen and the mixture is ignited. What is the
volume of the resulting gases? (all volumes
measured at room temperature and pressure)
100 cm3
A
200 cm3
B
450 cm3
C
650 cm3
D
3.9
PVC, poly(chloroethene) is;
A a man made polymer produced by a
condensation reaction using a synthetic
monomer
B a natural polymer modified by the addition
of various side groups
C a man made polymer produced by a
condensation reaction using a natural
monomer
D a man made polymer produced by an
addition reaction using a synthetic
monomer
3.10
Which statement about toluene (methylbenzene,
C6H5CH3) will be correct?
A it is an isomer of cycloheptane
B it will take part in addition reactions
C it will not decolourise bromine water
D it will not react with oxygen
3.11
Which of the following alcohols will not be
oxidised easily by acidified potassium
dichromate?
A CH3CH2CH2CH2CH2OH
B (CH3)2C(OH)CH2CH3
C (CH3)2CH2CH(OH)CH3
D CH3CH2CH(OH)CH2CH3
3.12
Which of the following compounds is a ketone?
A CH3CH2CH2CH2CH2OH
B CH3CH2CH2CH2CHO
C (CH3)2CHCH2COOH
D CH3CH2COCH2CH3
H
H
H
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3.13
Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
6
This diagram shows some of the reactions of hydrogen.
1
2
3
4
5
6
7
8
H2
H2
H2
H2
H2
H2
H2
H2
+
+
+
+
+
+
+
+
reagent
CO
Na
F2
Cl2
O2
S
N2
C18H32O2
conditions used
ZnO + Cr2O3 catalyst
heat
heat
light
heat
heat
Fe catalyst, 200 atm pressure
Ni catalyst








main product
CH3OH
NaH
HF
HCl
H2O
H2S
NH3
C18H36O2
methanol
sodium hydride
ammonia
a saturated fatty acid
(a) (i) Name the type of reaction for reaction 8.
(ii) Give a use for the product.
(b) Which two products will be bases?
(c) (i) In which reaction is hydrogen acting as an oxidiser?
(ii) Write ion electron half equations for this reaction.
(d) Hydrogen fluoride exhibits a high degree of hydrogen bonding. Explain the cause of the hydrogen
bonding, and suggest some properties which will result.
(e) (i) Write a balanced symbol equation for the manufacture of methanol.
(ii) Assuming an 85% conversion, what mass of methanol will be made from 200 litres of hydrogen at stp.
(f) What role does light play in the formation of hydrogen chloride?
(g) The enthalpy of combustion of hydrogen is negative, and yet energy must be supplied to make water.
Explain why this is.
(h) What is the chemical test for hydrogen?
The mass of a pure nickel crucible decreased by 0.0012 g during strong heating. How many nickel atoms
have been lost from the crucible?
3.14
3.15
A pupil performed the following experiments, and noted these observations;
experiment
1
2
3
observation
stays clear and
colourless
add sodium iodide solution to a fresh starch solution
bubble chlorine gas through sodium iodide solution,
then add the mixture to fresh starch solution
boil fresh starch solution with dilute hydrochloric acid for 15
minutes.
add some of the sodium iodide solution from experiment 2
goes blue/black
stays clear
(slightly yellow)
(a) What causes the blue/black colour in experiment 2?
(b) Write ion-electron half equations for the reactions in the first part of experiment 2.
(c) Explain why there was no blue/black colour in experiment 3.
3.16
10 g of sodium carbonate were weighed out, dissolved in 50 cm3 of water and transferred to a 100 cm3
standard flask which was topped up to the mark with water. 20 cm3 of this solution were pipetted into a
conical flask and a few drops of methyl orange indicator were added. The sodium carbonate solution was
then titrated with hydrochloric acid. The following results were obtained;
(a) What is the concentration of the sodium carbonate solution?
titre
volume /cm3
3
(b) How many moles of sodium carbonate are in the 20 cm pipetted into the
1
19.8
conical flask?
2
19.2
(c) What volume should be used for the acid?
3
19.1
(d) Calculate the concentration of the hydrochloric acid.
4
19.2
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4.1
H
Higher Grade Chemistry (HS)
The processes;
H
H
H
C
C
1
H  C
H
H
H
H
H
H
2
C  H
C
C
H
H
H
4.3
4.4
4.7
Which of the following statements is not true
about both of the following compounds?
CH3CH2CH2OH and CH3CH(OH)CH3
A they have the molecular formula C3H8O
B they are isomers
C they are primary alcohols
D they can be oxidised by acidified potassium
dichromate solution
4.8
Which of the following anhydrous compounds
will react with sodium to give hydrogen gas?
A CH3CH2CH2CHO
B CH3COCH2CH3
C CH3CH(OH)CH2CH3
D CH3CH2COOCH2CH3
4.9
Which of the following formulae represents the
organic compound formed by the oxidation of;
CH3CH2CH2CH(OH)CH3
A CH3CH2CH2COOCH3
B CH3CH2CH2COCH3
C CH3CH2CH2CH2CHO
D CH3CH2CH2CH2COOH
4.10
Compound X has the molecular formula C3H8O.
It is readily oxidised to compound Y with the
molecular formula C3H6O. X is most likely to
be;
A a primary alcohol
B a secondary alcohol
C an aldehyde
D a ketone
4.11
A hydrocarbon contains 92.3% carbon by mass.
A possible formula for the compound would be;
A C6H6
B C2H4
C C3H6
D C4H6
OH
are;
A condensation followed by oxidation
B cracking followed by condensation
C oxidation followed by hydration
D cracking followed by addition
4.2
Unit 2 “The World of Carbon” Homework
Which of the following chemicals has weak van
der Waal’s forces between its molecules?
A SiO2
B C60
C CuI2
D Na
Excess oxygen was added to 2 moles of
hydrogen gas and 1 mole of methane gas, and
the mixture was ignited. How many moles of
oxygen were used up?
A 1 mole
B 2 moles
C 3 moles
D 4 moles
The systematic name for this compound;
H
H
OH H
C
C
H
H
H
H
C
C
H
H
is;
A
B
C
D
4.5
4.6
butanol
methylpropanol
butan-2-ol
2-methylpropan-2-ol
4.12
Which of the following hydrocarbons is formed
when pentan-1-ol is dehydrated under suitable
conditions?
A cyclopentane
B pentane
C pent-1-ene
D pent-3-ene
The mass of one silver atom will be;
A 1.08  102 g
B 1.8  10-22 g
C 5.6  1021 g
D 6.5  1025 g
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4.13
The mass of 1  1020 molecules of ethane, C2H6,
is;
A 5.5  10-6 g
B 180.6 kg
C 30 g
D 0.005 g
10 cm3 of a 0.1 mol l-1 potassium carbonate
solution will contain;
A 0.003 moles of carbonate ions
B 1 mole of carbon atoms
C 0.002 moles of potassium ions
D 0.002 moles of ions
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4.14
Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
This table shows the approximate percentages of pollutants converted at different temperatures in the catalytic
converter in a car exhaust system.
O
temperature
C
150
200
250
300
350
400
450
500
550
600
carbon monoxide
%
9
30
55
80
98
100
100
100
100
100
nitrogen oxides
%
6
12
18
22
25
19
12
10
8
4
(a) Draw line graphs for these data on the same axes.
(b) Which operating temperature would you choose for the catalytic converter?
(c) Suggest a reason for the shape of the nitrogen oxides graph.
4.15
8
Compound P reacts slowly with sodium to produce hydrogen gas and an alkaline liquid.
Compound P also reacts as follows;
C6H12O
P

C6H10
Q

C6H12
R
and
C6H10
Q

C6H11Br
S
(a) What can be deduced about the structure of P from its reaction with sodium?
(b) Given that compound R does not readily undergo further addition reactions, deduce possible structural
formulae for P, Q and R.
(c) What reagent could be used to convert Q into S?
4.16
Draw the full structural formulae for;
(a) pentan-2-ol
(b) cyclobutene
(c) a tertiary alcohol with five carbon atoms.
(d) hexanal
4.17
Methanol can be made from synthesis gas by the following reaction;
CO + 2H2  CH3OH
(a) Draw the full structural formula for methanol.
(b) Explain why methanol is soluble in water.
(c) In the manufacture of methanol, 14 tonnes of carbon monoxide was found to produce 10 tonnes of
methanol. Calculate the percentage yield of the reaction.
(d) Write a balanced equation for the complete combustion of methanol.
(e) Calculate the heat energy released when 1 kg of methanol is burned in excess oxygen.
4.18
Pentan-2-ol can take part in several different reactions.
combustion


pentan-2-ol
dehydration


oxidation
condensation with an organic acid
(a) Write a balanced symbol equation for the complete combustion of pentan-2-ol.
(b) Draw the apparatus which could be used to perform the dehydration reaction and collect the gaseous
product.
(c) Dehydration of pentan-2-ol gives two isomeric products. Draw the structural formulae for the two
isomers.
(d) Name a chemical which could be used to oxidise the pentan-2-ol, and state the colour change.
(e) Name the product of the oxidation of propan-2-ol, and draw its full structural formula.
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5.1
5.2
Higher Grade Chemistry (HS)
Which of the following would cause an iron nail to
rust quickest when in contact with the nail in
water?
A iron
B magnesium
C tin
D zinc
A pupil found that neutralising 50 cm3 of lithium
hydroxide solution with 2 mol l-1 hydrochloric acid
gave a final volume of 115 cm3. Which of the
following statements is true?
A 15 cm3 of water are formed during the
reaction
B the lithium hydroxide solution is more
concentrated than the hydrochloric acid
C the final solution has a pH greater than 7
D the final volume is about 100 cm3 when the
salt has been removed
Unit 2 “The World of Carbon” Homework
9
The following formulae refer to questions 5.8 and 5.9
A C3H7OH
B C2H5COOH
C C2H5CHO
D CH3COCH3
5.8
Which of the above will give a positive test with
Benedict’s solution?
5.9
Which of the above reacts with sodium carbonate
to give carbon dioxide?
5.10
H
H
H
OH
C
C
C
H
H
H
H
C
H
H
5.3
Which of these gases has the lowest density at stp?
A CH4
B NO
C CO
D O2
5.4
Which of the following gases will contain the
smallest number of atoms? (all measurements at the same
temperature and pressure)
A
B
C
D
5.5
5.6
5.7
If the above molecule is oxidised by acidified
potassium dichromate solution, the product will be
called;
A 2-methylpropan-1-ol
B butanal
C 2-methylpropanone
D 2-methylpropanal
5.11
Excess silver nitrate solution was added to 10 cm3
of sea water. The resulting precipitate was
filtered, dried, and found to weigh 0.359 g. The
concentration of chloride ions in the sea water was:
A 2.5  10-5 mol l-1
B 0.14 mol l-1
C 0.20 mol l-1
D 0.25 mol l-1
5.12
Which type of bonding can be described as
intermolecular?
A metallic
B ionic
C covalent
D van der Waal’s
5.13
Using the density quoted in the data booklet, how
many atoms will be in a 10 litre container of
oxygen gas at stp?
A 2.6  1023
B 5.3  1023
C 2.7  1029
D 5.3  1020
10 g of fluorine
pentane
pent-1-ene
pent-3-ene
One mole of calcium nitrate contains;
A two moles of ions
B five moles of atoms
C two moles of negative ions
D two moles of positive ions
A white compound was burned in oxygen and gave
carbon dioxide and water as products. What is the
most that can be said about he compound?
A it is a hydrocarbon
B it is a carbohydrate
C it contains carbon and hydrogen
D it contains carbon, hydrogen and oxygen
The name of this compound (CH3)2CHCOCH3 is;
A
B
C
D
2-methylbutan-3-one
1,1-dimethylpropan-2-one
3-methylbutan-2-one
3-methylbutanal
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5.14
Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
10
“An aldehyde can be prepared by oxidation of the corresponding alcohol. Aldehydes themselves are easily
oxidised, and this makes it difficult to stop the oxidation of the alcohol at the correct stage. One way to
avoid this difficulty is to use ‘catalytic dehydrogenation’, usually with copper as the catalyst. A second way
to avoid the difficulty is to use the fact that aldehydes generally have lower boiling points than the
corresponding alcohol. Adding a powerful oxidiser to some boiling alcohol will result in the aldehyde being
made, and boiling out of the mixture before it can be oxidised further.”
(a) Give another name for ‘aldehyde’.
(b) Name the alcohol which could be used to prepare propanal.
(c) If propanal was further oxidised, what would be formed?
(d) What is meant by ‘catalytic dehydrogenation’?
(e) Name the chemical which could be used to produce butanal by catalytic dehydrogenation.
(f) Calculate the O:H ratio for the reactant and product in (e) and decide if the reaction is an oxidation or
a reduction.
(g) Explain why catalytic dehydrogenation is a good method for preparing an aldehyde.
(h) Give the boiling points for ethanal and ethanol.
(i) Explain why these compounds have different boiling points.
(j) Name a suitable oxidiser for the second method for making aldehydes.
(k) Describe the colour changes you would see during the reaction.
(l) When 1.32 g of butanol is oxidised, 0.98 g of butanal is produced. Calculate the percentage yield of
this reaction.
5.15
What mass of nitrogen gas will contain 4  1025 protons?
5.16
The smell of honey is mainly due to the chemical ethyl phenylethanoate, which has the structural formula;
H
O
C
C
O
H
(a)
(b)
(c)
(d)
(e)
5.17
5.18
H
H
C
C
H
H
H
To which two families of chemicals does this molecule belong?
Give some possible physical properties for this chemical.
Describe how you would hydrolyse this chemical in the lab.
Draw the full structural formulae for the products of the hydrolysis, and give their systematic names.
What mass of carbon dioxide will be produced by the complete combustion of 10 g of this chemical.
Draw full structural formulae for the following chemicals;
(a) hexan-3-ol
(b) butanoic acid
(c) butyl methanoate
(d) 3,3-diethylhexane
(e) cyclopentene
Draw the full structural formula, and give the systematic name, for the main product of each of the following
reactions;
(a) C2H2 + Br2 
(b) CH3CH(OH)CH2CH3 + K2Cr2O7 + H+ 
(c) CH3CH2OH + HCOOH 
(d) C2H6 + O2 
(e) C2H5OH + Na 
(f) C2H5OH  hot Al2O3 catalyst 
(g) CH3CH2CH2CHO + K2Cr2O7 + H+ 
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6.1
Higher Grade Chemistry (HS)
Which of the following gases will have the
highest density at stp?
A C2H6
B C2H4
C C2H2
D CH4
Unit 2 “The World of Carbon” Homework
6.9
Silicon carbide is often used as
A the ‘lead’ in a pencil
B an electrical conductor in a computer
C an abrasive powder
D a lubricating oil
6.10
Tetrachloromethane, CCl4, is a non-polar solvent
because;
A the C-Cl bond is not polar
B the bonds in the molecule are arranged
symmetrically
C chlorine atoms have a higher
electronegativity than carbon atoms
D only water is a polar solvent
6.11
The difference in covalent radius between
chlorine and iodine is mainly due to the
difference in
A the number of protons in the nucleus
B the mass number of the atoms
C the number of electron energy levels
D the number of neutrons in the nucleus
6.12
The molecule below dissolves in water to give an
acidic solution.
These formulae refer to questions 6.2, 6.3 and 6.4
A CH3CH2CH2CH2CHOH
B CH3CH(CH3)CH(OH)CH3
C CH3CH(CH3)(OH)CH2CH3
D CH3CH2CH2CH2CHO
6.2
Identify the primary alcohol.
6.3
Identify the alcohol which could be oxidised to
give a ketone.
6.4
Identify the alkanal.
6.5
A positively charged particle with the same
electron arrangement as argon could be
A an aluminium ion
B a sulphide ion
C a potassium ion
D a calcium atom
The table below refers to questions 6.6 and 6.7,
and gives information about four chemicals
conduction of
chemical melting point oC
electricity
A
1310
non-conductor
B
502
conductor
C
534
non-conductor
D
3520
conductor
6.6
In which substance will van der Waal’s bonds be
broken as the chemical melts?
6.7
Which substance is most likely to be graphite?
6.8
The systematic name for this compound,
C
H
H
C
C
6.13
H
C
A
O
O
H
O
H
C
C
C
C
H
H
C
H
B
H
H
H
O
C
C
C
O
D
O
C
C
H
H
O
C
C
H
H
O
C
C
O
H
H
H
H
H
H
H
is;
A
B
C
D
H
H
H
D
hexanoic acid
2,2-dimethylbutanoic acid
3,3-dimethylbutanoic acid
3,3-dimethylbutanal
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H
Which of the following molecules is an ester?
O
H
A
H
H
B
Which letter identifies the hydrogen atom which
becomes a hydrogen ion in solution.
H
H
11
H
C
O
C
H
H
O
H
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C
H
H
H
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Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
12
6.14
Give the systematic name and the full structural formula for the alcohols which would produce the following
compounds on oxidation;
(a) CH3CHO
(b) CH3CH2CH2COOH
(c) CH3CH2COCH3
(d) (COOH)2
(e) CH3COCH2COCH3
(f) HCHO
6.15
Name the main products of the hydrolysis of the following compounds:
(a) protein
(b) starch (using acid)
(c) starch (using amylase)
(d) CH3COOCH3
6.16
Give the name and full structural formulae for the products of the following reactions:
(a) ethene + hydrogen chloride 
(b) propene + steam 
(c) pent-2-ene + bromine 
(d) ethyne + hydrogen bromide 
(e) hex-3-ene + hydrogen chloride 
6.17
A company wishes to make the solvent 1,1,2,2-tetrabromoethane.
(a) Draw the full structural formula for 1,1,2,2-tetrabromoethane.
The company has the following feedstocks available;
ethane; ethene; ethyne; bromine; hydrogen bromide.
(b) Which feedstocks should the company use?
(c) Draw a simple reaction sequence to show how the product will be made.
(d) What must the company consider when choosing a feedstock?
6.18
Beginning with ethene, how could you make:
(a) ethanol
(b) ethanal
(c) bromoethane
(d) 1,2-dichloroethane
6.19
A pupil has several chemicals in bottles.
A
CH3CH(OH)CH2CH3
C
E
CH3CH2COOH
CH3COCH2CH3
B
D
F
CH3CH(CH3)CHO
CH3C(CH2)CH2CH3
CH3OCOCH2CH3
(a) Which chemical would give a ‘silver mirror’ test with ammoniacal silver nitrate solution (Tollen’s
Reagent)? Give the shortened structural formula for the product.
(b) Which chemical would rapidly decolourise bromine water? Give the systematic name for the product.
(c) Which chemical would produce an alkanone on oxidation? Suggest a reagent which could be used to
bring about this oxidation, and say what colour change you would see.
(d) Which two would react together to form an ester? Draw the full structural formula for the ester.
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2.18
Higher Grade Chemistry (HS)
Unit 2 “The World of Carbon” Homework
13
“Ammonia gas can be produced by heating ammonium sulphate with soda lime (a mixture of sodium
hydroxide and calcium hydroxide). The ammonia can be dried by passing it through a container packed with
pieces of quick lime (calcium oxide), and it can then be passed over heated copper oxide. The resulting
nitrogen gas can then be collected.”
(a) Draw a labelled diagram of the apparatus used for this experiment.
(b) How could you detect the ammonia coming from the first reaction?
(c) Why will there be no ammonia mixed with the nitrogen at the end?
(d) The following information was obtained from this experiment;
mass of weighboat
123.4 g
mass of weighboat and copper oxide
130.6 g
mass of weighboat and solid product
129.8 g
What is the empirical (simplest) formula for the copper oxide?
(e) Write a symbol equation for the reaction between ammonia and hot copper oxide.
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