Musselburgh Grammar School
Chemistry Department
Standard Grade
Ink Exercise Booklet
Instructions
The purpose of this booklet is to help you revise previous
work and improve your knowledge & understanding, to
maximise your success in Chemistry
Pupils should complete one exercise per week, as directed
by their teacher.
Pupils will have one week to complete the exercise, this is
to enable you to seek help if having trouble.
DO NOT leave blanks.
Exercises should be completed in homework jotters.
Notes should be used to complete these exercises.
All exercises should be SIGNED BY A PARENT before being
submitted.
Exercise 1
1(a)
Give an example of a halogen
(b)
Give an example of a noble gas
(c)
Give an example of an alkali metal
(d)
Give an example of a liquid element
(Unit 1 The Periodic Table)
2. State 2 ways to speed up a chemical reaction
(Unit 1 Reaction Rates)
3. Write the formulae for the following compounds
Magnesium Bromide Calcium Carbonate Iron(III) Sulphate
(Unit 1 Formula)
(4)
(2)
(3)
4(a) Draw the structural formulae for Butene and Cyclobutane
(b)
Write the molecular formula for each molecule
(c)
What name is given to molecules with same molecular formula but
different structural formula?
(d)
Which of the molecules would decolourise bromine solution?
Explain your answer
(6)
(Unit 2 Hydrocarbons)
Exercise 2
1. Draw a diagram of an atom, showing the position of the nucleus,
electrons, neutrons and protons.
(Unit 3 Atomic Structure)
2. The two most common types of chlorine atom are:
35
(2)
37
17Cl
and
17Cl
a) What name is given to atoms with the same atomic no. but
different mass no.?
b) Write down the no. of electrons, neutrons and protons in each
atom.
(4)
(Unit 3 Atomic Structure)
3.
(a) Name the process used to separate crude oil into fractions
(b) Crude oil is mainly made up of hydrocarbons. What is a hydrocarbon?
(c) What is the definition of a fuel?
(d) Why is it dangerous to burn a fuel in a poorly ventilated room?
(e) What gas is used up when something is burned?
(f) Write the balanced chemical equation for the combustion of methane.
(Unit 2 Fuels)
(7)
Exercise 3
1. (Unit 4: Bonding)
(a) Identify the 2 ionic
substances.
(b) Identify the substance which
exists as a covalent network.
2. (Unit 2: Hydrocarbons)
(c) Explain your answer to (b)
4
(a) Identify the 2 hydrocarbons which would quickly decolourise bromine
solution.
2
(b) Identify the isomer of the hydrocarbon in box D which belongs to a
different homologous series. (Unit 2: Hydrocarbons)
1
3.(Unit 1: Formulae)
Write chemical formula for (a) oxygen (b) sulphur trioxide (c) Iron (III)
oxide
3
Exercise 4
1. (Unit 1: Intro to Chemistry)
(a) Describe the test for oxygen gas.
(b) Explain why this test is not positive with air.
2. (Unit 2: Hydrocarbons)
2
(a) The fuel used in a Bunsen burner is methane,
CH4. What is meant by the term “fuel”?
(b) Methane burns to form carbon dioxide and
water.
(i) Balance this equation:
CH4 + O2  CO2 + H2O
(ii) Name another product which could be formed
in Flame A (air hole half closed).
(c) Draw a diagram to show the shape of a
methane molecule.
4
3. Zinc reacts with hydrochloric acid to produce hydrogen gas.
(a) State the test for hydrogen
1
gas.
(b) During the experiment, the
test tube becomes warm.
What term is used to describe
a reaction which gives out
1
heat?
(c) Plot a line graph of the results
3
of the reaction.
(d) Predict the volume of gas
which would have been given
off after 60s.
1
(e) What could be done to the
reaction conditions to increase
the rate of the reaction?
1
Exercise 5
1. (Unit 3: Structure of the Atom)
(a) Identify the particle
which is a positive ion.
(b) Identify the 2 particles
which are isotopes
2
(c) Calculate the number of protons, electrons and neutrons in the
following:
(i)
27
Al
13
(ii)
14
N
7
3-
4
2. (Unit 1: Formulae)
Write chemical formula for (i) Sulphur trioxide (ii) Aluminium carbonate
2
3. (Unit 2: Hydrocarbons)
(a) Write the molecular formula for
compound A.
(b) why can compound B be described as an
isomer of compound A?
(c) Name the products formed when these
compounds are completely burned in a
plentiful supply of oxygen.
3
Exercise 6
1. (Unit 3: Hydrocarbons)
Ethyne is the first member of a homologous series of compounds called
the alkynes. All the alkynes contain 1 Carbon to Carbon triple bond.
(a) Give the name of A and write the molecular formula for B.
A
B
(b) Draw the full structural formula for ethyne
(c) Deduce the general formula for the alkynes.
2.
(a)
(CnH ?)
4
(b)
(c)
3
Exercise 7
1 (Unit 4: Bonding)
2 (Unit 4: Bonding)
(a)
(b)
(a) Explain why a d.c. supply is used.
(b) Write ion electron equations to show
the
reaction at the (i) positive electrode (ii)
negative
electrode.(Use p.7 of the data booklet)
(c)
(c) Why does the copper chloride have to
be in a
solution before it can be electrolysed?
(d) Why couldn’t you electrolyse a
glucose solution?
8
3. (Unit 2: Fuels and Combustion)
(a) Describe how nitrogen dioxide is formed in the car engine.
(b) What environmental problem does nitrogen dioxide cause?
1. (Unit 1: Formulae)
Which of the following compounds
contains only 2 elements?
A Magnesium hydroxide
B Magnesium phosphate
C Magnesium sulphite
D Magnesium nitride
3. (Unit 1: Reaction Rates)
Identify the slowest reaction:
A Mg powder + 4mol/l acid
(Unit
1d) + 2mol/l acid
B 4.Mg
ribbon
C Mg powder + 2mol/l acid
D Mg ribbon + 4mol/l acid
2
Exercise 8
2. (Unit 1: The Periodic Table)
Which element is an alkali metal?
A Aluminium
B Calcium
C Copper
D Sodium
4. (Unit 3: Nuclide Notation)
Calculate the number of protons,
electrons and neutrons in
(i)
40
Ca
20
(ii)
31 3-
P
15
7
5. A new air bag is being developed for use in cars. In the reaction,
butane reacts with an oxide of nitrogen:
C4H10 + N2O  CO2 + H2O + N2
(a) Balance this equation
(b) Water is formed in this reaction. Draw a diagram to show how the
outer electrons are shared in a molecule of water.
(Unit 3: Balancing Equations)
Exercise 9
1. (Unit 4: Bonding)
Substance
Melting point
Electrical conductivity
Solid
Solution
Melt
W
High
Non-conductor Non-conductor Non-conductor
X
High
Conductor
Insoluble
Conductor
Y
Low
Non-conductor Non-conductor Non-conductor
Z
High
Non-conductor Conductor
Conductor
(a) Using the information in the table, state whether W,X,Y and Z are
simple covalent, network covalent, ionic or metallic.
(b) Explain why Z cannot conduct in the solid state, but becomes a good
conductor when molten.
3
2. (Unit 3 & 4: Electrolysis)
(a) State what is meant by electrolysis.
(b) Aluminium is extracted by electrolysis of its molten oxide since
aluminium oxide does not react when heated with carbon. Why does
aluminium oxide not react with carbon?
(c) Chlorine is produced by the electrolysis of sodium chloride solution.
Write the ion-electron equation for the formation of chlorine. You may
wish to use the data booklet to help you.
3
3 (Unit 5: Mole Calculations)
Ammonia gas can be produced in the lab by heating ammonium chloride
with sodium hydroxide.
Calculate the mass of ammonia produced by heating 10kg of NH4Cl
NH4Cl + NaOH  NaCl + H2O + NH3
2
2
Exercise 10
1. (Unit 5 Titration Calculations)
(ii) Calculate the number of moles of sodium hydroxide in this average volume.
Show your working clearly.
(b) 1 mole of ethanoic acid reacts with 1 mole of sodium hydroxide.
Calculate the concentration in mol/l of ethanoic acid in vinegar. Show your
5
working clearly.
2. (Unit 3 & 5: Hydrocarbons & Mole Calculations)
Iodine can react with propene in the following way:
(a) (i) Name the homologous series to which propene belongs.
(ii) Name the type of chemical reaction which takes place when iodine reacts with
propene.
(b) Calculate the mass of iodine that will react with 100g of propene.
4
3. (Unit 3: Displacement Reactions)
Which of the following metals would react with zinc chloride solution (use page 7 of the
data booklet)
A Copper
B Gold
C Iron
D Magnesium
1
Exercise 11
1. (Unit 5: Salt Preparation)
Metal salts can be made by using different methods.
(a) Barium sulphate can be made by reacting solutions of barium chloride
and sodium sulphate. The ionic equation for this reaction is:
Ba2+(aq) + 2Cl-(aq) + 2Na+(aq) +SO42-(aq) Ba2+SO42-(s) + 2Na+(aq) + 2Cl-(aq)
(i) Rewrite the equation omitting spectator ions.
(ii) Name the type of reaction taking place.
(b) Potassium sulphate can be made by titrating sulphuric acid with
potassium hydroxide solution.
2KOH (aq) + H2SO4 (aq)  K2SO4 (aq) + H2O (l)
If 25cm3 of dilute sulphuric acid were required to react with 20cm3 of
0.1mol/l potassium hydroxide solution, calculate the concentration of the
(4)
sulphuric acid.
2 (Unit 4: Bonding)
Identify the type of bonding that is likely to be present in the following:
(A) Mercury (B) Silver (I) chloride (C) Carbon monoxide (D) Silicon oxide (4)
3. (Unit 5: Making Acids and Alkalis)
A SO2
B CuO
C Na2O
D NO2
(a) Which 2 letters show compounds which will dissolve in water to
produce acidic solutions?
(b) Which letter shows a compound which will dissolve in water to produce
an alkaline solution?
(c) Which letter shows a compound which will form a neutral solution?
Calculations
Exercise 12
1. Ammonia gas can be produced in the lab by heating ammonium chloride with sodium
hydroxide. Calculate the mass of ammonia produced by heating 10kg of ammonium
2
chloride
NH4Cl + NaOH  NaCl + H2O + NH3
(3)
2.
Zinc sulphide, roasted in air, reacts as follows:
3
2ZnS + O2  2ZnO + 2SO2
(a)Calculate the mass of sulphur dioxide produced when 9.7g of zinc sulphide is
completely roasted in air.
(b) Suggest why this process could damage the environment.
3. (a) Calculate the volume of 5moles of a 0.5 mol/l solution of HCl(aq)
4. (a) Write chemical formula for sodium hydroxide.
(b) Calculate the volume of 2moles of 3mol/l sodium hydroxide.
3
5. Potassium sulphate can be made by titrating sulphuric acid with potassium hydroxide
solution.
2KOH (aq) + H2SO4 (aq)  K2SO4 (aq) + H2O (l)
If 25cm3 of dilute sulphuric acid were required to react with 20cm3 of 0.1mol/l
potassium hydroxide solution, calculate the concentration of the sulphuric acid.
2
Exercise 13
(Unit 5: Acids, Alkalis and Neutralisation)
1. Complete the following word equations & write the chemical equation
underneath.
(a) Sodium hydroxide + Nitric acid 
(b) Lithium hydroxide+Hydrochloric acid 
(c) Sodium oxide + Hydrochloric acid 
(d) Calcium oxide + Nitric acid 
(e) Calcium carbonate + Nitric acid 
(f) Copper (II) carbonate+Hydrochloric acid 
12
2. Complete the following equations and circle the precipitate.
(a) Lead nitrate + Magnesium sulphate 
(b) Magnesium nitrate + Sodium hydroxide
(c) Zinc sulphate + sodium carbonate
(i) Write chemical equations for the 3 reactions above, showing ionic
charges, and circle the spectator ions.
12
Exercise 14
1. (Unit 6: Carbohydrates)
(a) State the colour change when a sugar reacts with benedict’s solution.
(b) Which sugar does not react with benedict’s?
(c) State the test for starch.
(d) Glucose and fructose both have the formula C6H12O6 but they have different
structures. What name is given to such compounds which have the same formula but
different structure?
4
2. (Unit 3: Metal Extraction)
A Na2O
B ZnO
C SnO2
D PbO
E CuO
F Hg2O
(a) Which oxide could be broken down by heat alone?
(b) i.Which oxide could not be broken down by heating with carbon?
ii. What process would have to be carried out on this oxide, to extract
the metal?
3
3 (Unit 1 & Unit 5: The Periodic Table and Acids & Alkalis)
A Silicon Dioxide
B Carbon Dioxide
C Sodium Oxide
D Iron Oxide
E Sulphur Dioxide
F Copper Oxide
(a) Identify which 2 oxides contain transition metals
(b) Identify the oxide which reacts with water in the atmosphere to
make acid rain
(c) Identify the oxide which, when added to water, produces a solution
with a greater concentration of hydroxide(OH-) ions than hydrogen ions
(H+).
4. (Unit 2: Hydrocarbons)
Draw full structural formula for the following:
(a) pentane (b) Cyclohexane (c) ethene (d) but-2-ene.
4
4
Exercise 15
1. The grid shows some statements which could be applied to a solution
A
It does not react with magnesium
B
It has a pH less than 7
C
It does not conduct electricity
D
It produces chlorine gas when electrolysed
E
It contains more H+ ions than pure water
Identify the two statements which are true for both dilute hydrochloric
acid and dilute sulphuric acid.
2. The table contains information about some substances
2
Substance
Melting point/ o C
Boiling point/ o C
Conducts as solid
Conducts as a liquid
A
B
C
D
E
F
-7
98
-39
547
-78
1700
59
883
357
1265
-33
2230
No
Yes
Yes
No
No
No
No
Yes
Yes
Yes
No
No
(a) Identify the substance which is a gas at O0C
(b) Identify the two substances that exist as molecules
(c) Identify the covalent network substance
(d) Identify the ionic substance
4
3. David was studying the reactions of some metals and their compounds.
He carried out experiments involving magnesium, copper, zinc, nickel,
silver and unknown metal X
Listed below are some of his observations
A
X was more easily oxidised than copper
B
X oxide was more stable to heat than silver oxide
C
Magnesium displaced X from a solution of X nitrate
D
X reacted more vigorously than nickel, with dilute acid
E
Compounds of X were more readily reduced than compounds of zinc
David produced the following order of reactivity
MOST
Magnesium > Zinc > Nickel > Copper > X > Silver
REACTIVE
LEAST
REACTIVE
Identify the two observations which can be used to show that X has been
wrongly placed.
2
4. Calculate the percentage, by mass, of calcium in fluorite(CaF2)
Showing your working clearly
2
5. Iron can be extracted by heating haematite (Fe2O3) with carbon
monoxide. Carbon dioxide is also produced in the reaction.
Write an equation, using symbols and formulae, for this reaction
Exercise 16
1
1. (Unit 5: Salt Preparation)
The grid shows some ionic compounds
A Aluminium Bromide
B Sodium Chloride
C Potassium Hydroxide
D Sodium Sulphate
E Potassium Bromide
F Calcium Chloride
(a) Identify the base
(b) Identify the two compounds whose solutions would form a precipitate
when mixed
(c) Identify the compound with a formula of the type XY2, where X is a
metal.
3
2.(Unit 7: Corrosion)
(a) Which pair of metals would produce a flow of
electrons in the same direction as shown in the diagram
and produce a blue colour round metal B?
(b) Which pair of metals would produce the biggest
voltage? (Page 7 data book)
2
3.(Unit 3: Metal Extraction and Reactivity)
Siobhan carried out some experiments
with 4 metals (W, X, Y and Z) and some of
their compounds. She made the following
observations:
(a) Name the gas formed when metal Y
reacts with water.
(b) Suggest names for metals W and Y.
(c) Place the 4 metals in order or reactivity
(most reactive first)
(d) Name the type of chemical reaction
which takes place when a metal is extracted
from its oxide.
4
Exercise 17
1.(Unit 5: Mole Calculations)
(a) Calculate the formula mass of sodium carbonate
(b) Calculate the mass of solute (sodium carbonate ) present in 100cm3 of sodium
hydroxide solution, concentration 0.2mol/l
5
(c) Mg +
H2SO4

MgSO4 +
H2
Use the above equation to calculate the mass of hydrogen released when 12g of Mg is
added to excess sulphuric acid.
2. (Unit 4: Hydrocarbons)
Dienes are a homologous series of hydrocarbons which contain 2 double bonds per
molecule.
4
(a) What is meant by the term “homologous series”?
(b) Suggest a general formula for the dienes. (CnH? )
(c) Write the full structural formula for the product of the complete reaction of penta1,3-diene with bromine.
3. (Unit 4, 5 & 7)
Reactions can be represented using chemical equations
A
Fe2+ (aq) + 2e-  Fe (s)
B
Fe2+ (aq)  Fe3+ (aq) + e
C
2H2 (g) + O2 (g)  2H2O (g)
D
2H2O (l) +O2(g) + 4e-  4OH- (aq)
E
SO2 (g) + H2O (l)  2H+ (aq) + SO32- (aq)
(a) Identify the equation which shows the formation of acid rain
(b) Identify the equation which represents a combustion reaction
(c) Identify the two equations which are involved in the corrosion of iron
Exercise 18
1. (Unit 8: Plastics)
When superglue sets, a polymer is formed. The polymer has the following structure.
(a) Draw the structural formula for the repeating unit.
(b) Draw the structural formula for the monomer in superglue.
Q1 continued
(c) Name a toxic gas given off when superglue burns.
(d) As the polymer forms, it releases large amounts of heat. What name is given to this
type of reaction?
3
4
2. (Unit 7: Corrosion)
2
3.
(ii)
(i)
Which of the following compounds dissolves
in water to give a solution with a pH greater
than 7?
A Ammonia
B Carbon Dioxide
C Sulphur Dioxide
D Sodium chloride
(iii)Draw a section of the polymer
formed when 3 propene monomers
combine
3
Exercise 19
1. (Unit 8: Plastics)
(a) Ethene can be used to make poly (ethene). Draw the structure of the polymer
showing three ethene units joined together.
(b) Poly (ethene) is a thermoplastic. Explain the meaning of the term thermoplastic.
(c) Poly(ethene) can’t be described as biodegradable. What does biodegradable mean?
(d) Name a biodegradable polymer
(e) What is the raw material used to make all synthetic plastics?
5
2. (Unit 6: Carbohydrates)
A Nitrogen
B Oxygen
C Water
D Carbon Dioxide
E Methane
F Ethanol
(a) Identify the substances used by plants during photosynthesis
(b) Identify the two substances produced during fermentation of glucose
solution
(c) Identify the substances produced during respiration in humans
(d) The substance used up in the combustion of starch
4
3. (Unit 6: Making Fertilisers)
A Nitrogen Dioxide
B Hydrogen
C Oxygen
D Carbon Dioxide
E Ammonia
F Nitrogen
Identify
(a) The two gases used as reactants in the Haber Process
(b) The two gases used as reactants in the Ostwald Process
(c) The gas that is produced during lightning storms and near spark plugs
in car engines
(d) The gas that makes up 80% of the air
(e) The gas that dissolves to give an alkaline solution
(f) The gas that is produced by the Haber Process
6