DEPARTMENT FOR CURRICULUM,
RESEARCH, INNOVATION AND LIFELONG LEARNING
Directorate for Learning and Assessment Programmes
Educational Assessment Unit
Track 2
Annual Examinations for Secondary Schools 2018
YEAR 9
CHEMISTRY
TIME: 2 hours
Name: ______________________________________
Class: ______________________________________
Useful Data
Atomic numbers and relative atomic masses are shown in the periodic table printed on a separate page.
Marks Grid [ For Examiner’s use only ]
Question
No.
1
Max
Mark
10
2
Section A
3
4
5
6
7
10
10
10
10
20
10
Section B
8
9
20
20
Theory
Total
Actual
Mark
Theory Paper: 85%
Chemistry – Year 9 – Track 2 – 2018
Practical: 15%
Final Score: 100%
Page 1 of 12
SECTION A –
Answer ALL questions in the spaces provided.
This section carries 60 marks.
1) With the help of the periodic table of the elements, give the name or symbol of an element
which:
a)
does not form compounds
_______________
b)
is a shiny solid and conducts electricity
_______________
c)
is the gas most abundant in air
_______________
d)
is a liquid metal at room temperature
_______________
e)
is a solid non-metal that burns in air to form an acidic oxide
_______________
f)
is a metal that forms an amphoteric oxide
_______________
g)
is a gas that produces water on combustion
_______________
h)
is a non-metal, one of its oxides sublimes
_______________
i)
has 3 electron shells and 6 electrons in its outer shell
_______________
j)
forms a positive ion with an electronic configuration of 2,8
and a charge of +2
_______________
(1 mark each – Total 10 marks)
2) Matter is made of particles. The physical state of matter can be changed by heating as shown
in the graph below:
a) Which state of matter do the following lines on the graph represent?
CD __________________
EF ___________________
(2)
b) Use the Kinetic Theory of Matter to:
i)
Draw a diagram that represents the arrangement of the particles in AB
(1)
Page 2 of 12
Chemistry – Year 9 – Track 2 – 2018
ii) Explain the arrangement of the particles when the substance is in the physical state
represented by AB.
________________________________________________________________________
________________________________________________________________________
_____________________________________________________________________ (2)
c) In the state represented by EF, the substance is said to be compressible.
i)
Draw the arrangement of particles in the box below.
(1)
ii) Explain why gases are compressible
____________________________________________________________________
____________________________________________________________________
_________________________________________________________________ (1)
d) Give the names of the processes represented by:
BC _____________________
DE _______________________
(2)
e) When heating a substance, heat energy is absorbed by the particles of that substance
and its temperature increases. Explain why during DE, the temperature of the substance
does not increase.
_______________________________________________________________________
_______________________________________________________________________
____________________________________________________________________ (1)
Total: 10 marks
Chemistry – Year 9 – Track 2 – 2018
Page 3 of 12
3) The picture shows how the solubility in water of various solutes changes with temperature.
a) Two of the solutes shown are gases while the others are salts.
State how the solubility of gases and salts in water changes with temperature.
_______________________________________________________________________
____________________________________________________________________ (2)
b) From the graph:
i.
What temperature is required to completely dissolve 45 g of KCl in 100 g of pure
water?
__________________________________________________________________ (1)
ii.
If the solution mentioned in (b)(i) is cooled to 10 °C, how much KCl, in grams, would
crystallizes out of solution?
__________________________________________________________________ (1)
c) Sodium chloride is an ionic substance. Draw a dot-cross diagram of the sodium chloride
ions showing all electron shells.
(3)
Page 4 of 12
Chemistry – Year 9 – Track 2 – 2018
d) Using a dot-cross diagram, draw the bonding in water, H2O, showing outer shells only.
(3)
Total: 10 marks
4) This question is about water hardness.
a) What happens when soap is added to hard water?
____________________________________________
________________________________________
(1)
b) Give the name or formula of a substance that causes:
i) Temporary hardness
____________________________________________
(1)
ii) Permanent hardness
____________________________________________
(1)
c) State a method which removes
i) Temporary hardness only ____________________________________________ (1)
ii) Both temporary and permanent hardness _______________________________
(1)
d) Give one advantage and one disadvantage of water hardness
______________________________________________________________________
______________________________________________________________________
___________________________________________________________________ (2)
e) Hard water usually leaves behind deposits of calcium carbonate (CaCO3) in the form of
limescale, as can be seen in the picture above. Which of the following substances would
be
suitable
to
remove
the
limescale
from
the
water
tap
in
the
picture?
(underline the correct answer)
ammonia solution
(1)
vinegar
dilute sodium hydroxide
f) Carbon dioxide dissolves in rain water to make it slightly acidic.
Rain water dissolves
carbonates of calcium and magnesium that are major constituents of rock. This is also
how natural water becomes hard.
Give a balanced chemical equation that happens when rain water passes through rock.
____________________________________________________________________ (2)
Total: 10 marks
Chemistry – Year 9 – Track 2 – 2018
Page 5 of 12
5) Hydrogen is the first element of the periodic table. It is also the lightest gas and exists as
diatomic molecules.
a) Hydrogen has three isotopes. Their symbols are shown below. Explain what is meant by
the term ‘isotopes’ in terms of protons and neutrons. Use hydrogen as an example.
______________________________________________________________________
______________________________________________________________________
___________________________________________________________________ (2)
b) Hydrogen is produced in the laboratory by reacting a metal with a dilute acid. The following
diagram shows the apparatus used to carry out the reaction. Complete the diagram below
by drawing the apparatus you would use to collect hydrogen gas.
(2)
c) In an experiment, 1.2 g of magnesium are reacted with dilute hydrochloric acid, to produce
hydrogen gas and magnesium chloride solution. The reaction is given below:
Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
(N.B. Relative atomic masses: Mg=24, H=1; Avogadro’s constant = 6x10 23)
By showing your working, calculate:
i)
the amount (in moles) of magnesium reacting.
___________________________________________________________________
_________________________________________________________________ (1)
ii) the amount (in moles) of magnesium chloride produced.
_________________________________________________________________ (1)
iii) the number of ions present in the magnesium chloride produced.
___________________________________________________________________
_________________________________________________________________ (2)
Page 6 of 12
Chemistry – Year 9 – Track 2 – 2018
iv) the mass, in grams, of hydrogen gas produced.
___________________________________________________________________
___________________________________________________________________
_________________________________________________________________ (2)
Total: 10 marks
6) This question is about acidic and basic substances.
a) Complete and balance the following chemical reactions:
i)
__ H2SO4
+
__ NaOH → ___________________________________________ (2)
ii) __ HCl + __ Na2SO3 → ______________________________________________ (2)
iii) __ NaOH + __ NH4Cl → _____________________________________________ (2)
b) Oxides are compounds that oxygen forms with many elements.
Complete the following grid by drawing lines to match the different types of oxides with
the correct description.
Oxides
Neutral
Basic
Amphoteric
Acidic
Definition
React with both acids and alkalis
Give solutions with pH less than 7
React with alkali to give salt + water
Do not react with neither acids nor alkalis
Give solutions with a pH greater than 7
React with acid to give salt + water
(2)
c) Give the name or formula of a basic oxide that is soluble in water.
____________________________________________________________________ (1)
d) Universal indicator was used to show whether the solution obtained in (c) is acidic or
alkaline. State the colour that results when this indicator is added.
Colour: _____________________________________________________________ (1)
Total: 10 marks
Chemistry – Year 9 – Track 2 – 2018
Page 7 of 12
SECTION B – Answer TWO questions ONLY in the spaces provided.
This section carries 40 marks.
7) The Earth’s atmosphere is a mixture of gases.
a) The following setup can be used in a laboratory to remove some gases from the air.
Stage 1: U-tube contains calcium hydroxide solution (limewater).
Stage 2: U-tube contains solid anhydrous copper(II) sulfate.
Stage 3: In the furnace, granules of copper metal are heated strongly.
i)
For each stage,
 Name which gas is removed
(3)
Stage 1:
______________________________
Stage 2:
______________________________
Stage 3:
______________________________
 State what you would observe.
Stage 1:
(3)
_________________________________________________________
_________________________________________________________________
Stage 2:
_________________________________________________________
_________________________________________________________________
Stage 3:
_________________________________________________________
_________________________________________________________________
 Complete and balance the following chemical equations to explain the
observations you mentioned.
Stage 1: Ca(OH)2(aq) +
(6)
________ (g) →
Stage 2: CuSO4(s)
+
Stage 3: Cu(s)
_______ (g) →
+
CaCO3(s) +
_________ (l)
_________ (g) → _________________ (s)
__________ (s)
ii) Predict which gas is mainly collected in the gas syringe.
(1)
___________________________________________________________________
Page 8 of 12
Chemistry – Year 9 – Track 2 – 2018
b) Some gases should not be present at all in our atmosphere. Such gases are considered
as pollutants.
i) Give the name of one such gas. _______________________________________
(1)
ii) Explain how this gas is formed. ___________________________________________
_________________________________________________________________
(1)
iii) Mention one of its harmful effects. ________________________________________
_________________________________________________________________
(1)
c) Hygroscopic substances such as anhydrous copper(II) sulfate readily absorb water
vapour from the air around us to form hydrated crystals. Other substances behave
differently when exposed to air.
Give ONE word to describe the following substances and give ONE example of each:
i) Compounds that absorb so much water from the atmosphere that they form a
solution.
___________________________________________________________________
Example: _________________________________________________________ (2)
ii) Substances that lose their water of crystallization to form the anhydrous salt.
___________________________________________________________________
Example: _________________________________________________________ (2)
Total: 20 marks
8) This question is about salts and their preparation.
a) Anhydrous copper(II) chloride, CuCl2, is a soluble salt and can be prepared in the
laboratory by reacting an insoluble salt of copper with a dilute acid. The diagram below
shows the method used.
i) From the following list, choose the correct reactants that can be used in this
experiment.
Solid salts:
Cu(NO3)2
or
CuO
Dilute acids:
HCl
or
HNO3
Salt: ________________
Acid: ________________
Chemistry – Year 9 – Track 2 – 2018
(2)
Page 9 of 12
ii) Write a balanced equation for the reaction between the reactants you have chosen to
prepare copper(II) chloride. Include state symbols.
__________________________________________________________________ (3)
iii) The amount of solid salt used must be in excess of the quantity of acid. Explain why
this is important.
_____________________________________________________________________
__________________________________________________________________ (1)
iv) Why is filtration required in the second step of the method?
__________________________________________________________________ (1)
v) The above setup is not suitable to obtain hydrated crystals. Draw the correct
apparatus that should be used in the final step to obtain hydrated copper(II)
chloride crystals.
(3)
b) Zinc carbonate, ZnCO3, was prepared by precipitation by mixing a solution containing
27.2 g of zinc chloride and a solution containing ammonium carbonate.
(Relative atomic masses: Zn=65, Cl=35.5, C=12, O=16)
i)
Complete and balance the equation for the reaction. Include state symbols.
ZnCl2(aq) + (NH4)2CO3(aq) → ______________________________
(3)
ii) Work out the relative formula mass of zinc chloride, ZnCl 2
________________________________________________________________
(1)
iii) Calculate the number of moles of zinc chloride in the 27.2 g of ZnCl2 used.
____________________________________________________________________
____________________________________________________________________
________________________________________________________________
(2)
iv) Use the equation to work out the number of moles of ZnCO3 produced.
____________________________________________________________________
_________________________________________________________________ (2)
v) Calculate the mass, in grams, of zinc carbonate obtained.
____________________________________________________________________
____________________________________________________________________
_________________________________________________________________ (2)
Total: 20 marks
Page 10 of 12
Chemistry – Year 9 – Track 2 – 2018
9) This question is about Oxygen.
a) Oxygen can be prepared in the laboratory by the catalytic action of manganese(IV) oxide
(MnO2) on hydrogen peroxide (H2O2).
i)
On the diagram label the reagents used for the reaction.
(2)
ii) Complete the diagram to show how you would collect the oxygen over water. Label
your drawing.
iii) Give a balanced chemical equation for the reaction.
(3)
(2)
____________________________________________________________________
iv) State how you would test and confirm that the gas produced is oxygen.
(1)
____________________________________________________________________
v) Explain the function of manganese(IV) oxide in this reaction.
(2)
____________________________________________________________________
____________________________________________________________________
b) Rusting is a term used to refer to the corrosion of iron. In the experiment shown in the
diagram, would you expect the iron nail in tubes B and C to rust? Explain your answer.
Chemistry – Year 9 – Track 2 – 2018
Page 11 of 12
Tube B: ________________________________________________________________
____________________________________________________________________ (2)
Tube C: ________________________________________________________________
____________________________________________________________________ (2)
c) Oxygen, nitrogen and some noble gases can be obtained on a large scale from air. Give
the name of the industrial process used.
____________________________________________________________________ (1)
d) An allotrope of oxygen in the Earth’s atmosphere filters harmful radiation from the sun.
Give its name or formula.
____________________________________________________________________ (1)
e) Oxygen and nitrogen can form various gases between them. One such gas contains
30.43 % nitrogen and 69.57 % oxygen by mass.
i)
Calculate the number of moles of nitrogen atoms in the compound.
(RAM Nitrogen = 14).
___________________________________________________________________
________________________________________________________________ (1)
ii)
Calculate the number of moles of oxygen atoms in the compound.
(RAM Oxygen = 16).
___________________________________________________________________
________________________________________________________________ (1)
iii) Find the mole ratio between nitrogen and oxygen in this compound.
___________________________________________________________________
________________________________________________________________ (1)
iv) Given that one mole of this gas has a mass of 46 g, work out the molecular
formula of this gas.
___________________________________________________________________
___________________________________________________________________
________________________________________________________________ (1)
Total: 20 marks
Page 12 of 12
Chemistry – Year 9 – Track 2 – 2018