c1 past paper review questions and self...
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HWK Metallic Bonding
1. The diagram below shows a model of the structure of sodium metal.
a. Describe the structure and bonding in a metal and explain, in terms of bonding, why magnesium has a higher melting point that sodium. (5)
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b. Metals can conduct electricity and heat and are malleable and ductile. Explain these properties in terms of the structure of a metal. (6)
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HWK Ionic Bonding
1. Draw o/x diagrams to show the bonding in the following compounds. (9)
a. Potassium bromide b. Sodium oxide c. Calcium iodide
2. Explain why lead(II) bromide will conduct electricity when molten but not when a solid. Give the balanced electron half equations for the reactions that occur at each electrode. (6)
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3. Explain, in terms of bonding, why magnesium sulfide (MgS) has higher melting temperature compared to sodium chloride (NaCl). (2)
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HWK Covalent Bonding – Simple Molecules
1. Draw the o/x diagrams to show the bonding in the following elements and compounds. (10)
a. Bromine, Br2 b. Oxygen, O2 c. Nitrogen, N2 d. Carbon dioxide, CO2 e. Water, H2O
2. Explain, in terms of bonding, why simple covalent molecules are usually gases at room temperature. (2)
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HWK Covalent Bonding – Giant Structures
1. Carbon can form a number of different structures, as shown.
a. Explain, in terms of structure, why diamond has a very high melting temperatures and carbon dioxide has a low boiling temperature, even though the atoms in both are joined by very strong covalent bonds. (4)
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b. Explain, in terms of structure, why graphite is used as electrodes in the electrolysis process. (2)
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c. Explain, in terms of structure, why a carbon nanotube can be used in microelectronic circuits but graphite is not. (2)
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HWK Nanoparticles
1. Nano-silver particles are used to kill bacteria. The graph shows the percentage of Type 1 bacteria killed by different sized nano-silver particles.
The table shows the percentage of Type 2 bacteria killed by different sized nano-silver particles.
Size of nano-silver particles (nm) 8 11 15 18 20
Percentage of Type 2 bacteria killed (%) 92 64 52 48 44
a. On the grid above, plot the size of nano-silver particles against the percentage of Type 2 bacteria killed and draw a suitable line. (3)
b. Describe the main difference in the shapes of the graphs for Type 1 and Type 2 bacteria killed by nano-sized silver particles. (1)
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c. State the relationship between the size of the nano-silver particles and the percentage of bacteria killed. (1)
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d. Suggest why nano-silver particles below 5 nm were not used in this study. (1)
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e. Explain the reason why some people are concerned about the presence of free nano-scale particles in the atmosphere. (2)
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HWK Smart Materials
1. Describe what is meant by a smart material. Use thermochromic and photochromic materials to support your answer, giving everyday uses of each. (6 QER)
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HWK Metallic Bonding
Targets to know/be able to do Self Peer1 Describe the structure and bonding of a metal. (Q1a)
2 Why magnesium has a higher melting point than sodium. (Q1a)
3 The link between the structure and bonding of a metal and its physical properties. (Q1b)
HWK Ionic Bonding
Targets to know/be able to do Self Peer1 Use dot and cross diagrams to show ionic bonding. (Q1)
2 Why ionic compounds conduct electricity when molten but not when solid. (Q2)
3 Write balanced electron half equations for each electrode. (Q2)
4 The link between the melting point of an ionic compound and the charges on the ions. (Q3)
HWK Covalent Bonding – Simple Molecules
Targets to know/be able to do Self Peer1 Use dot and cross diagrams to show covalent bonding.
(Q1)2 Explain why simple covalent molecules are gases at
room temperature. (Q2)
HWK Covalent Bonding – Giant Structures
Targets to know/be able to do Self Peer1 Explain why diamond has a much higher melting point
than carbon dioxide. (Q1a)2 Explain why graphite is used as electrodes in
electrolysis. (Q1b)3 Explain why carbon nanotubes are used in
microelectronic circuits whereas graphite is not. (Q1c)
HWK Nano-Scale Particles
Targets to know/be able to do Self Peer1 Plot points on a curve. (Q1a)
2 Draw a suitable line. (Q1a)
3 Use graphs and data to answer questions. (Q1b,1c,1d)
4 Explain why some people are concerned about free nano-scale particles present in the atmosphere. (Q1e)
HWK Smart Materials
Targets to know/be able to do Self Peer1 What is meant by a smart material. (Q1)
2 Give everyday examples of thermochromic and photochromic materials. (Q1)
HWK Reactions of Acids
1. Nitric acid is a strong acid whereas citric acid is a weak acid. State how universal indicator and pH can be used to prove this. (2)
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2. The diagram shows some reactions of sulfuric acid.
Give the chemical name for the following. (5)
a. Metal A - ……………………………………………….……………………….
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c. Colourless solution C - …………….………………….………………….
d. Blue solution D - …………………………………………………………….
e. Black oxide E - ………………………………………………………………..
f. Write a balanced symbol equation for the reaction of sulfuric acid with metal A. (2)
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3. Milk of magnesia, which contains magnesium hydroxide, is often used to remove excess hydrochloric acid in the stomach. Write a balanced symbol equation for this reaction. (3)
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4. Write the ionic equation (with state symbols) to show how water is formed during a neutralisation reaction and state the source of the ions. (5)
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Source of ions - …………………………………………………………………………………………………………………..…………………………
5. The symbol equation below represents the reaction occurring between barium chloride and sodium sulfate.
BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaCl (aq)
Write the ionic equation for the reaction, including state symbols. (3)
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6. A student says that the name of the salt produced in the reaction between silver and sulfuric acid is silver sulfate. Explain whether the student is correct or not. (2)
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7. Describe the test that is used to identify the carbonate ion. (2)
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HWK Practical Methods
1. The diagrams below show stages in making the compound copper(II) sulfate by reacting copper(II) carbonate with sulfuric acid.
a. Explain what excess means. (1)
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b. Explain why the copper(II) carbonate is added in excess. (1)
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c. What would be observed in stage 1? (1)
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d. Name the process being carried out in stage 2. (1)
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e. State the property of copper(II) carbonate that allows it to be removed in Stage 2. (1)
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f. Name the substance being removed in Stage 3. (1)
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g. Write a balanced symbol equation to show the reaction in Stage 1. (2)
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2. The diagram below shows the apparatus used to find the concentration of a sample of ethanoic acid. A volume of ethanoic acid was added to a known volume of sodium hydroxide until neutralisation occurred.
a. Name apparatus A. (1)
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b. Name a piece of apparatus that could have been used to measure the sodium hydroxide. (1)
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The titration was carried out four times including a rough initial titration. The results obtained are given.
Rough titration
1st
titration2nd
titration3rd
titrationFinal reading (cm3) 24.7 48.0 24.2
Initial reading (cm3) 0.00 24.7 23.4
Volume of ethanoic acid added (cm3) 24.7 23.4 23.2
c. Complete the table. (2)
d. Calculate the mean volume of ethanoic acid required for neutralisation. (2)
e. Explain which solution, ethanoic acid or sodium hydroxide, was the most concentrated. (2)
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HWK Reactions of Acids
Targets to know/be able to do Self Peer1 Using universal indicator and the pH scale to
identify acid strength. (Q1)2 The reactants and products of reactions of
acids. (Q2)3 Write a balanced symbol equation to show
reactions of acids. (Q2f,3)4 Write an ionic equation for neutralisation.
(Q4)5 Write an ionic equation to show the formation
of a precipitate. (Q5)6 The source of ions for an acid and an alkali.
(Q4)7 Explain whether an acid will react with a
metal using the reactivity series. (Q6)8 The test for a carbonate using an acid. (Q7)
HWK Practical Methods
Targets to know/be able to do Self Peer1 The preparation of copper(II) sulfate from
copper(II) carbonate. (Q1a-f)2 Write a balanced symbol equation to show a
reaction of an acid. (Q1g)3 The names of some apparatus needed to carry
out a titration. (Q2a,2b)4 Perform calculations to calculate a mean
value. (Q2c)5 Identify repeatable results. (Q2d)
6 Calculate a mean. (Q2d)
7 Identify the most concentrated acid from given concentration values. (Q2e)
HWK Calculations
1. A student prepared a solution of sodium hydroxide, NaOH, by dissolving 1.20 g of sodium hydroxide pellets in 250 cm3 of water.
a. Calculate the concentration of the sodium hydroxide solution (mol dm-3). (2)
b. Calculate the concentration of the sodium hydroxide solution (g dm-3). (2)
Ar(H) = 1 Ar(Na) = 23 Ar(O) = 16
She then used this solution to determine the concentration of dilute sulfuric acid. She measured exactly 25.0 cm3 of the sodium hydroxide solution and titrated it against the dilute sulfuric acid.
Titration number 1 2 3 4Volume of sulfuric acid
used (cm3)17.3 15.9 16.1 16.0
c. Calculate the mean volume of sulfuric acid used. (2)
Sulfuric acid reacts with sodium hydroxide solution according to the following equation –
H2SO4 + 2NaOH Na2SO4 + 2H2O
d. Use the mean volume of sulfuric acid and the equation shown to calculate the concentration of the acid (mol dm-3). (3)
2. 25.0 cm3 of HCl reacts completely with 12.5 cm3 of NaOH of concentration 2.00 mol dm-3. Calculate the concentration of the HCl. (3)
NaOH + HCl NaCl + H2O
3. 25.0 cm3 of H2SO4 reacts completely with 20.0 cm3 of NaOH of concentration 0.500 mol dm-3. Calculate the concentration of the H2SO4 solution. (3)
2NaOH + H2SO4 Na2SO4 + 2H2O
HWK Acid Strength
1. Explain the difference between a concentrated acid and a strong acid. (2)
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2. Ethanoic acid is a weak acid and sulfuric acid is a strong acid but both react with sodium hydroxide solution. Give the similarities and differences in the reactions. (4)
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3. Two experiments were carried out to investigate the volume of carbon dioxide (CO2) given off when sodium carbonate reacted with two acids (A and B). The acids were of equal concentrations and were added separately to equal masses of sodium carbonate powder. The results are shown below.
Time (s) 0 10 20 30 40 50 60
Volume of CO2 from acid A (cm3) 0 15 27 37 44 49 50
Volume of CO2 from acid B (cm3) 0 25 40 48 50 50 50
a. Plot the results for acid A and draw a suitable fit. The line for acid B has been done. (3)
b. Calculate the initial rate of reaction for acid B. (3)
c. Explain which acid is the strongest. (2)
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HWK Calculations
Targets to know/be able to do Self Peer1 Calculate the concentration of a solution in mol dm-3
when given a volume and mass. (Q1a)2 Calculate the concentration of a solution in g dm-3.
(Q1b)3 Identify repeatable results. (Q1c)
4 Calculate a mean. (Q1d)
5 Calculate the concentration of a solution in mol dm-3 when given a volume and concentration. (Q1d,2,3)
HWK Acid Strength
Targets to know/be able to do Self Peer1 The difference between a concentrated and strong
acid. (Q1)2 The similarities and differences in the reaction of a
strong and weak acid. (Q2)3 Plot points on a graph. (Q3a)
4 Draw a suitable line. (Q3a)
5 Calculate an initial rate of a reaction by drawing a tangent. (Q3b)
6 Explain which acid is the strongest. (Q3c)
HWK Electrolysis
1. A student tried to electrolyse potassium chloride.
a. Explain why the student found that solid potassium chloride does not conduct electricity. (2)
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b. State two things the student could do to the potassium chloride to make it conduct electricity. (2)
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c. During electrolysis, the potassium ions move to the negative electrode and the chloride ions move to the positive electrode. Explain why this happens and write balanced electron half equations for the reactions that occur at each electrode. (6)
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2. Electroplating is used to coat a cheap metal with a thin layer of an expensive metal. In the diagram, a teaspoon made of nickel is being coated with silver. Explain fully why the nickel teaspoon becomes coated in silver. Include balanced electron half equations in your answer. (QER 6)
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3. The diagram shows an apparatus used for the electrolysis of sodium chloride solution.
a. Explain, in terms of bonding, why pure water does not conduct electricity but sodium chloride solution does. (3)
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b. Explain why hydrogen gas is formed at the cathode and not sodium metal. (2)
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c. Explain how an increase in the concentration of the sodium chloride solution affects the volume of hydrogen gas produced in a certain time (during the electrolysis process). (2)
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HWK Aluminium Extraction
1. The diagram shows the industrial extraction of aluminium metal from aluminium oxide.
a. State the meaning of the term electrolysis. (1)
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b. Write a balanced symbol equation for the electrolysis of aluminium oxide. (3)
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c. Write balanced electron half equations for the reactions that occur at each electrode. (5)
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d. Explain, in terms of electrons, the reason that the electrolysis of aluminium oxide is a redox process. (2)
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e. Give the reasons that the aluminium oxide is dissolved into molten cryolite. (2)
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HWK Iron Extraction
1. The diagram shows where materials enter and leave the blast furnace in the extraction of iron.
a. Complete the table. (5)
Letter What it representsA
B
C
D
E
b. Name the:
i. Fuel used. (1)
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ii. Gas needed for the fuel to burn. (1)
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iii. Substance used to remove impurities. (1)
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2. One of the reactions that occur during the extraction of iron in the blast furnace is shown as a word equation below.
iron(III) oxide + carbon iron + carbon dioxide
a. Explain which substance is reduced and which is oxidised during the reaction. (2)
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b. Write the balanced symbol equation for the reaction that occurs. (3)
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c. Calculate the mass of carbon that would be needed to completely react with 100 tonnes of iron(III) oxide. (3)
Ar(C) = 12 Ar(Fe) = 56 Ar(O) = 16
3. In the blast furnace, the iron(III) oxide can be reduced by carbon monoxide to produce iron and carbon dioxide. In the reaction, the iron(III) ions are reduced to iron metal.
a. Write the balanced symbol equation for the reaction. (3)
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b. Write the electron half equation for the reduction of the iron(III) ions. (2)
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c. In a blast furnace, the percentage (%) yield of iron obtained from iron(III) oxide was found to be 78 %. Calculate the mass of iron that can be obtained from 200 tonnes of iron(III) oxide. (4)
Ar(Fe) = 56 Ar(O) = 16
HWK Reactivity Series
1. When a mixture of powdered magnesium and copper(II) oxide is heated, a violent reaction takes place. In the reaction, the magnesium is oxidised and the copper(II) oxide reduced. The magnesium atoms are changed into magnesium ions, while the copper(II) ions are changed into copper atoms.
a. Write a balanced symbol equation to show this reaction. (2)
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b. Write balanced electron half equations to show what happens during the reaction. (4)
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c. Explain the meaning of the terms oxidised and reduced. (2)
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2. Tin does not react with iron(III) oxide but can reduce lead(II) oxide, forming tin(ll) oxide as one of the products.
a. Write the balanced symbol equation and balanced electron half equations for the reaction that occurs between tin and lead(II) oxide. (6)
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b. Explain why tin cannot reduce iron(III) oxide but can reduce lead(II) oxide. (2)
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3. A pupil had four metals A, B, C and D. He placed each metal in turn into separate solutions of the nitrate of the other three. The results were:
A displaced D
B displaced A
B displaced D
C displaced A, B and D
a. Place the metals in order of reactivity (starting with the most reactive). (1)
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b. A and D are both Group 2 metals. Write the balanced symbol equation (using the letters A and D to represent the metals) for the reaction between A and the solution of the nitrate of D. (2)
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4. The following table show the observations made when some metals were added to solutions of compounds of other metals.
Metal Solution Observation
Zinc Copper(II) sulfate Orange-brown solid forms on surface of zinc
Copper Zinc sulfate No change
Magnesium Zinc sulfate Dark grey solid forms on surface of magnesium
Zinc Magnesium sulfate No change
a. Use the information in the table to put the metals in order of reactivity, starting with the most reactive. (2)
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b. Write balanced symbol equations for the reactions that occur. (4)
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HWK Transition Metals
1. Write balanced symbol and ionic equations, with state symbols, for the following reactions.
a. Copper(II) chloride solution and sodium hydroxide solution. (8)
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b. Iron(III) nitrate solution and sodium hydroxide solution. (8)
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2. Sodium is a typical Group 1 metal and iron is a typical transition metal. State the ways in which these two metals are different from each other in terms of their properties. (QER 6)
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HWK Electrolysis
Targets to know/be able to do Self Peer1 Explain why a solid ionic compound does not conduct
electricity. (Q1a)2 State how to make an ionic compound conduct electricity.
(Q1b)3 Explain why ions move to electrodes during electrolysis.
(Q1c)4 Write balanced electron half equations for each electrode.
(Q1c,2)5 The process of electroplating. (Q2)
6 Explain why pure water does not conduct electricity but a solution of an ionic compound does. (Q3a)
7 Explain why hydrogen gas is sometimes formed at the cathode. (Q3b)
8 Explain how an increase in concentration of a solution affects the volume of gas produced in a certain time. (Q3c)
HWK Aluminium Extraction
Targets to know/be able to do Self Peer1 The meaning of electrolysis. (Q1a)
2 Write a balanced symbol equation to show the electrolysis of aluminium oxide. (Q1b)
3 Write balanced electron half equations for each electrode. (Q1c)
4 Explain a redox reaction in terms of gaining and losing electrons. (Q1d)
5 The reasons cryolite is used to extract aluminium. (Q1e)
HWK Iron Extraction
Targets to know/be able to do Self Peer1 The names and locations of the materials that enter and
leave the blast furnace. (1a)2 The fuel used in the blast furnace. (Q1bi)
3 The gas needed for the fuel to burn in the blast furnace.(Q1bii)
4 The substance used to remove impurities in the blast furnace. (Q1biii)
5 Reduction and oxidation in terms of gaining and losing oxygen. (Q2a)
6 Write balanced symbol equations to show reactions in the blast furnace. (Q2b,3a)
7 Write balanced electron half equations for each electrode. (Q3b)
8 Calculate a mass of substance produced in a reaction using moles. (Q2c,3c)
HWK Displacement Reactions
Targets to know/be able to do Self Peer1 Write balanced symbol equations to show displacement
reactions. (Q1a,2a,4b)2 Write balanced electron half equations for each
electrode. (Q1b,2a)3 Explain the meaning of the terms oxidised and reduced.
(Q1c)4 Explain displacement reactions in terms of how reactive
metals are. (Q2b)5 Place metals in order of reactivity using given
information. (Q3a,4a)
HWK Transition Metals
Targets to know/be able to do Self Peer1 Write balanced symbol equations to show reactions of a
transition metal compound. (Q1a,b)2 Write ionic equations to show the formation of a precipitate.
(Q1a,b)3 The general properties of transition metals and Group 1
metals. (Q2)
HWK Bond Energies
1. When hydrogen reacts with chlorine, hydrogen chloride is formed.
The relative amounts of energy needed to break the bonds in the above equation are shown.
Bond Energy needed to break the bond (kJ)
H-H 436
Cl-Cl 243
H-Cl 432
Using the bond energy values in the table, calculate the energy –
a. Needed to break all the bonds in the reactants. (2)
b. Released when all the bonds in the products are formed. (2)
c. Explain why the relative overall energy change is exothermic. (1)
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2. Hydrogen peroxide, H2O2, decomposes to produce water and oxygen gas. The reaction is shown by the following equation.
The relative amounts of energy needed to break the bonds in the above equation are shown.
Bond Energy needed to break the bond (kJ)
H-O 464
O=O 498
O-O 144
a. Use the bond energy values to calculate the overall energy change for this reaction. (5)
b. Draw an energy profile for this reaction and label the axes, reactants, products, activation energy and the overall energy change. (6)
3. When hydrogen burns in air, water is formed. This is shown by the following equation.
a. The overall relative energy change during the reaction is -486 kJ and the total energy needed to break all the bonds in the reactants is 1370 kJ. Calculate the energy released when the bonds in the products are formed. (2)
b. Calculate the amount of energy released in forming an O-H bond. (1)
4. State what is meant by the activation energy of a reaction. (1)
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HWK Bond Energies
Targets to know/be able to do Self Peer1 Use bond energy data to calculate the energy needed
to break bonds in reactants. (Q1a,3a)2 Use bond energy data to calculate the energy released
when the bonds in products are formed. (Q1b)3 Use bond energy data to identify whether a reaction is
exothermic or endothermic. (Q1c)4 Use bond energy data to calculate the overall energy
change of a reaction. (Q2a)5 Draw a labelled energy profile diagram. (Q2b)
6 Calculate a bond energy from given data. (Q3b)
6 The definition of activation energy. (Q4)
HWK Crude Oil
1. Crude oil is a mixture of hydrocarbons which can be separated into fractions in a fractionating column.
a. State the relationship between the chain length of a hydrocarbon and its boiling point. (1)
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b. Explain why physical processes occur in the column and not chemical processes. (1)
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c. Explain why all fractions, apart from the petroleum gases, leave the column as liquids. (1)
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d. Explain why it is difficult to identify the fraction which contains the compound with the formula C9H20. (1)
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e. Explain why each fraction is separated over a temperature range. (2)
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HWK Burning Fuels
1. Charcoal is mainly carbon. When charcoal burns in air the only product is carbon dioxide. Write a balanced symbol equation for this reaction. (2)
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2. Write a balanced symbol equation to show the combustion reaction of propane (C3H8). (3)
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3. Methanol, ethanol, propanol and butanol are compounds that can be used as fuels. An experiment was carried out to find which one gives out the most energy when burned.
1 g of each fuel was used to heat 100 g of water and the results are shown.
Fuel Initial temperature of water (⁰C)
Final temperature of water (⁰C)
Energy given out (J/g)
Ethanol 20 45
Butanol 20 50
The energy given out by each fuel can be calculated using the formula:
Energy given out = mass of water x 4.2 x temperature change
a. Use this information to calculate the energy given out per gram of ethanol and butanol burned. (4)
b. Apart from using 1 g of each fuel and 100 g of water, give two other ways the experiment could be made a fair test. (2)
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The theoretical values for the energy given out by each fuel are below.
Fuel Theoretical energy given out (J/g)
Ethanol 29,700
Butanol 36,100
c. Suggest a reason for the difference between the experimental and theoretical values. (1)
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4. Hydrogen can be burned as a fuel.
a. Write a balanced symbol equation for the burning of hydrogen in air. (3)
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b. Give an advantage and disadvantage of using hydrogen as a fuel. (2)
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5. State a different firefighting method for each of the following situations. Use the fire triangle to explain your method in each case.
a. A person with their clothes on fire. (2)
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b. A waste paper bin on fire. (2)
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c. Oil in a chip pan on fire. (2)
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HWK Alkanes and Alkenes
1. The structural formulae of three hydrocarbons are shown.
a. Name the hydrocarbons A, B, C and give their molecular formulae. (6)
A - ………………………………………………………………………………………………………………………..….……………………….
B - ………………………………………………………………………………………………………………………….………………………….
C - ………………………………………………………………………………………………….………………………………………………….
b. Give the letter of the unsaturated hydrocarbon and explain your choice. (2)
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c. State how a student could distinguish between A and B. (3)
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2. Give the general formula of an alkane and alkene. (2)
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3. Draw the structural formulae for the branched chain isomers of the alkane with the molecular formula C5H12. (2)
4. Complete the following equation for the reaction between ethene and bromine, showing the product as a structural formula. (2)
5. Explain how polymers are produced from monomers. (3)
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6. Draw the repeating unit for the polymer PVC. (1)
7. Write a symbol equation for the making of the polymer PTFE. (3)
8. Give the chemical name for PTFE. (1)
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9. Give two reasons, apart from cost, why the recycling of plastics is important. (2)
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HWK Crude Oil
Targets to know/be able to do Self Peer1 The relationship between the chain length and the boiling
point of a hydrocarbon. (Q1a)2 Why chemical processes do not occur during fractional
distillation. (Q1b)3 Why nearly all the fractions are collected as liquids during
fractional distillation. (Q1c)4 Explain why it is difficult to identify a fraction using given
information. (Q1d)5 Explain why each fraction is separated over a temperature
range. (Q1e)
HWK Burning Fuels
Targets to know/be able to do Self Peer1 Write a balanced symbol equation. (Q1,2,4a)
2 Calculate the energy given out, per gram, of a fuel. (Q3a)
3 How to make an investigation a fair test. (Q3b)
4 Make a comparison of experimental and theoretical results. (Q3c)
5 An advantage and disadvantage of using hydrogen as a fuel. (Q4b)
6 Use the fire triangle to explain different firefighting methods. (Q5a,b,c)
HWK Alkanes and Alkenes
Targets to know/be able to do Self Peer1 Name a hydrocarbon when given a structural formula.
(Q1a)2 Write a molecular formula when given a structural
formula. (Q1a)3 Identify, with a reason, an unsaturated hydrocarbon. (Q1b)
4 The test for an alkene. (Q1c)
5 The general formula for an alkane and alkene. (Q2)
6 The structural formulae of isomers when given a molecular formula. (Q3)
7 Draw a structural formula to balance an equation. (Q4)
8 Explain how polymers are produced from monomers. (Q5)
9 Draw a repeating unit in a polymer. (Q6)
10 Write a balanced equation showing the formation of a polymer. (Q7)
11 The chemical name for PTFE. (Q8)
12 The importance of recycling plastics. (Q9)
HWK Alcohols
1. Draw the structural formula of 2-methylpropan-1-ol. (1)
2. Name the following compound. (1)
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3. Ethanol can be converted into a carboxylic acid when it is exposed to the air for a period of time.
a. Name the carboxylic acid that ethanol is converted into and the type of reaction that occurs in this conversion. (2)
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b. Draw the structural formula of the carboxylic acid formed. (1)
c. Describe a chemical test that would allow you to identify ethanol. (2)
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4. Ethanol can be oxidised to produced ethanoic acid and water. Write a balanced symbol equation for this reaction. (2)
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5. Yeast contains enzymes. The following graph shows the amount of activity of an enzyme, A, over a temperature range.
a. Describe fully what happens to the activity of enzyme A when the temperature increases. (5)
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b. Sketch on the graph the activity of a different enzyme, B, which is active between 0 and 55 ⁰C and has its greatest activity at 30 ⁰C. (2)
6. Explain why bioethanol is considered a carbon neutral fuel. (2)
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HWK Analysis
1. The structural formulae of four compounds are shown.
The data in the table below shows some bonds and their corresponding absorption value or wavenumber.
Bond Absorption value or wavenumber/cm-1
C-H 2800 – 3100C=C 1620 – 1670C-O 1000 – 1300C=O 1650 – 1750O-H 2500 - 3550
Use this information to answer the following questions.
a. One of the compounds shows an absorption at 1630 cm-1 and at 2900 cm-1 in its spectrum. Give the letter of this compound and the bonds that give rise to the absorptions. (3)
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b. Under certain conditions, compound C can be formed from compound B. What would be the main difference be in the infrared spectra of compounds B and C? (2)
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c. Give the molecular formula of compound C. (1)
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HWK Organic Chemistry
Targets to know/be able to do Self Peer1 Draw a structural formula when given a name of a
compound. (Q1)2 Name a compound when given a structural
formula. (Q2)3 The name of the carboxylic formed from an alcohol
and the type of reaction that occurs. (Q3a)4 Draw a structural formula of a carboxylic acid.
(Q3b)5 How to identify an alcohol. (Q3c)
6 Write a balanced symbol equation to show the oxidation of ethanol. (Q4)
7 Describe a set of results. (Q5a)
8 Use a set of infrared results to identify a compound. (Q5b)
9 What a carbon neutral fuel is. (Q6)
10 Use infrared spectroscopy data to answer questions. (Q7a,b)
11 Write a molecular formula when given a structural formula. (Q7c)
HWK Analysis
Targets to know/be able to do Self Peer1 Use infrared spectroscopy data to answer
questions. (Q1a,b)2 Write a molecular formula when given a structural
formula. (Q1c)
HWK Haber Process
1. Ammonia, NH3, was first made commercially over a hundred years ago by a German chemist called Fritz Haber. He succeeded in reacting two elements to make the gas ammonia.
a. Write a balanced symbol equation to show this reaction. (2)
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b. State the type of reaction. (1)
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c. State the role of iron in the reaction. (1)
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d. Describe how a scientist could carry out a test to identify ammonia gas. (2)
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2. The graphs show the % yields of ammonia at different pressures and temperatures.
a. State what temperature is needed to obtain 25 % yield of ammonia at a pressure of 200 atmospheres. (1)
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b. State the percentage yield of ammonia at a pressure of 350 atmospheres and a temperature of 350 ⁰C. (1)
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c. State how the % yield of ammonia changes with temperature and pressure. (4)
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3. The conditions used in industry are a temperature of 450 ⁰C and a pressure of 250 atmospheres. The % yield of ammonia would increase if a lower temperature or a higher pressure was used. Explain why these conditions are not used.
a. Lower temperature. (1)
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b. Higher pressure. (1)
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4. Explain what happens to the unreacted nitrogen and hydrogen in the process. (2)
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HWK Contact Process
1. Sulfuric acid is produced industrially by the Contact process, as shown.
Sulfur reacts with oxygen to
produce gas A
Gas A reacts with oxygen to
produce gas B
Gas B is used to produce sulfuric
acid
Stage 1 Stage 2 Stage 3
a. State the raw materials used in the Contact Process. (1)
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b. Write a balanced symbol equation for stage 2. (3)
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c. Explain why a high pressure is not used in stage 2. (2)
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d. Name the catalyst used in the process. (1)
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e. Give balanced symbol equations showing how gas B is used to produce sulfuric acid. (5)
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f. The table shows the % yield of sulfur trioxide at different temperatures. Plot the points of the % yield of sulfur trioxide at different temperatures on the grid and draw a suitable line. (3)
Temperature (⁰C)
400 450 500 550 600 650
Yield(%)
99 98 96 91 74 44
g. State how changing the temperature affects the % yield of sulfur trioxide. (2)
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h. Give the temperature range to be used to obtain a yield of sulfur trioxide above 90 %. (1)
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i. If a temperature of 300 ⁰C is used, the yield of sulphur trioxide is almost 100 %. Explain why this temperature is not used in this process. (1)
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2. Concentrated sulfuric acid can act as a dehydrating agent. When added to hydrated copper(II) sulfate crystals, anhydrous copper(II) sulfate and water are produced.
CuSO4.5H2O CuSO4 + 5H2O
a. Describe the changes that would be observed during the reaction. (2)
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b. Calculate the percentage (%) by mass of oxygen in hydrated copper(II) sulfate, giving your answer to one decimal place. (2)
Ar(Cu) = 63.5 Ar(H) = 1 Ar(O) = 16 Ar(S) = 32
c. Calculate the percentage (%) loss in mass due to the dehydration, giving your answer to one decimal place. (2)
Ar(Cu) = 63.5 Ar(H) = 1 Ar(O) = 16 Ar(S) = 32
HWK Fertilisers
1. One of the main uses of ammonia is in the production of nitrogenous fertilisers. The table shows the content of three types of fertiliser.
Percentage present
Fertiliser Nitrogen Phosphate Potash Sulfur
A 34 0 0 0
B 21 0 0 24
C 0 0 32 12
a. Explain which fertiliser, A, B or C, is not made from ammonia. (2)
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b. Explain which one of the fertilisers, A, B or C, is produced when ammonia is neutralised by sulfuric acid. (2)
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2. Write the balanced symbol equation for the reaction taking place when ammonia solution is neutralised by hydrochloric acid. (2)
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3. Give the test and the expected result for the ammonium ion. (2)
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4. Give one advantage and one disadvantage of the use of nitrogenous fertilisers. (2)
Advantage
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5. Write the balanced symbol equation for the reaction taking place when ammonia solution is neutralised by sulfuric acid. (3)
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HWK The Haber Process
Targets to know/be able to do Self Peer1 Write a balanced symbol equation to show
the Haber process. (Q1a)2 Identify a reversible reaction. (Q1b)
3 The role of iron in the Haber process. (Q1c)
4 How to identify ammonia gas. (Q1d)
5 Use graphs to answer questions about percentage yield. (Q2a,b,c)
6 Explain the conditions used in the Haber process. (Q3a,b)
7 Explain what happens to the unreacted nitrogen and hydrogen. (Q4)
HWK The Contact Process
Targets to know/be able to do Self Peer1 The raw materials needed. (Q1a)
2 Write balanced symbol equations to show reactions in the contact process. (Q1b,e)
3 Explain why a high pressure is not used. (Q1c)
4 Name the catalyst used in the contact process. (Q1d)
5 Plot points on a graph. (Q1f)
6 Draw a suitable line. (Q1f)
7 Analyse results. (Q1g)
8 Use a set of results to give a range.(Q1h)
9 Explain why the temperature used is not 300 OC. (Q1i)
10 Describe the changes of a dehydration reaction. (Q2a)
11 Calculate a percentage (%) composition. (Q2b)
12 Calculate a percentage (%) loss in mass. (Q2c)
HWK Fertilisers
Targets to know/be able to do Self Peer1 Identify a fertiliser, with reasons, from
given information. (Q1a,b)2 Write balanced symbol equations to show
the formation of fertilisers. (Q2,5)3 Test for the ammonium ion. (Q3)
4 An advantage and disadvantage of using fertilisers. (Q4)