Name: C4 Chemical Changes. Class: 35 Questions. Date: Time: Marks: Comments: Brookvale Groby Learning Trust

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1 C4 Chemical Changes 35 Questions Name: Class: Date: Time: Marks: Comments: Page of 27

2 The ph scale is a measure of the acidity or alkalinity of a solution. (a) Draw one line from each solution to the ph value of the solution. Solution ph value of the solution 5 Acid 7 9 Neutral 3 (2) (b) Which ion in aqueous solution causes acidity? Tick one box. H + Na + O 2 OH () Page 2 of 27

3 (c) When sulfuric acid is added to sodium hydroxide a reaction occurs to produce two products. The equation is: H 2 SO 4 + 2NaOH Na 2 SO 4 + 2H 2 O How many elements are in the formula H 2 SO 4? Tick one box () (d) What is this type of reaction? Tick one box. Decomposition Displacement Neutralisation Reduction () (e) Name the salt produced. () Page 3 of 27

4 (f) Describe how an indicator can be used to show when all the sodium hydroxide has reacted with sulfuric acid. (3) (Total 9 marks) 2 Some students investigated the reactivity of four unknown metals, W, X, Y and Z. The letters are not the symbols of these elements. The students used metal salt solutions of copper nitrate, magnesium sulfate and zinc chloride. This is the method used.. Pour a solution of a metal salt into a glass beaker. 2. Measure the temperature of the solution. 3. Add g of metal to the solution. 4. Measure the temperature of the solution. 5. Calculate the temperature increase. The students did the experiment using each salt solution with each metal. Figure shows the apparatus the students used. Figure Page 4 of 27

5 The table below shows the students results. Temperature increase in C Solution Metal W Metal X Metal Y Metal Z Copper nitrate No change Magnesium sulfate No change No change No change No change Zinc chloride 5 No change No change No change (a) Which metal is least reactive? Tick one box. Metal W Metal X Metal Y Metal Z () (b) How do the results show that magnesium is more reactive than the metals W, X, Y and Z? () (c) How do the results show that the reaction between metal Y and copper nitrate solution is exothermic? () Page 5 of 27

6 (d) One student said that the investigation was not valid (a fair test). Write a plan for the investigation that includes improvements to the method and apparatus. (4) Page 6 of 27

7 (e) Figure 2 shows the reaction profile of an exothermic reaction. Figure 2 What does the energy value of 370 kj represent? Tick one box. Activation energy Products energy Reactants energy Released energy () (f) The overall energy change is 386 kj. What percentage of 370 kj is this? Give your answer to two significant figures. Percentage = % (2) (Total 0 marks) Page 7 of 27

8 3 This question is about making copper salts. The figure below shows the apparatus given to a student. Outline a safe plan the student could use to make pure, dry, crystals of the soluble salt copper sulfate from the insoluble metal oxide and dilute acid. (Total 6 marks) Page 8 of 27

9 4 The figure below shows an apparatus to produce elements from a solution of an ionic compound. (a) What is the name of the process in the figure? Tick one box. Combustion Crystallisation Distillation Electrolysis () Page 9 of 27

10 (b) The table below shows the products formed from three experiments using different compounds and the apparatus shown in the figure above. Compound State Product at cathode Product at anode Copper chloride Molten Copper Chlorine Copper chloride Aqueous solution Copper Chlorine Potassium bromide Molten Potassium Bromine Use the table above to name the products formed at each electrode if using an aqueous solution of potassium bromide. At cathode At anode (2) (c) Explain why copper is formed at the cathode during the electrolysis of its salts. (2) (Total 5 marks) Page 0 of 27

11 5 This question is about calcium. (a) What type of compound is calcium oxide? Tick one box. An acid A base A carbonate A salt () (b) Ionic compounds, such as calcium oxide, have high melting points. Complete the sentences. Use words from the box. bonds forces ions layers Calcium oxide has a giant ionic lattice in which there are strong electrostatic of attraction in all directions. () Page of 27

12 (c) The figure below shows the electronic structure of an oxygen atom and a calcium atom. Describe how the calcium atom and the oxygen atom forms calcium oxide. You should give the charge on each ion formed. (4) (Total 6 marks) Page 2 of 27

13 6 Figure shows a reactor used to produce titanium from titanium(iv) chloride. Figure The chemical equation for the reaction of titanium(iv) chloride with sodium is: TiCl 4 + 4Na Ti + 4NaCl titanium(iv) chloride + sodium titanium + sodium chloride (a) For one reaction: 65 kg titanium(iv) chloride reacted completely with 782 kg sodium 989 kg sodium chloride was produced. Calculate the mass of titanium produced from this reaction. Mass of titanium = kg () Page 3 of 27

14 (b) The table below shows the solubility of sodium chloride in 00 cm 3 of aqueous solution at different temperatures. Solubility of sodium chloride in g per 00cm 3 Temperature in C On Figure 2: plot this data on the grid draw a line of best fit. Figure 2 (3) Page 4 of 27

15 Volume of water = dm 3 (2) (c) The product sodium chloride is dissolved in water to separate it from titanium. At 30 C the solubility of sodium chloride is 36 kg per 00 dm 3. Calculate the minimum volume of water in dm 3, at 30 C, needed to dissolve 989 kg sodium chloride. (d) Calculate the percentage by mass of titanium in titanium(iv) chloride (TiCl 4 ). Give your answer to 3 significant figures. Relative atomic masses (A r ): Cl = 35.5; Ti = 48 Percentage of titanium by mass = % (3) (e) Suggest why the reaction is done in an atmosphere of dry argon instead of air containing water vapour. (3) Page 5 of 27

16 (f) Explain why titanium conducts electricity. (3) (Total 5 marks) 7 Copper can be produced from copper(ii) sulfate solution by two different methods. Method Electrolysis (a) To produce copper by electrolysis a student has inert electrodes, a d.c. power supply, a switch and electrical wires for the external circuit. Draw and label the apparatus set up to produce copper from copper(ii) sulfate solution by electrolysis. (2) (b) Suggest why the colour of the copper(ii) sulfate solution fades during the electrolysis. (3) Page 6 of 27

17 (c) Explain how copper is produced from copper(ii) sulfate solution by electrolysis. (4) Method 2 Displacement (d) The chemical equation for the displacement of copper using iron is: CuSO 4 + Fe Cu + FeSO 4 Calculate the minimum mass of iron needed to displace all of the copper from 50 cm 3 of copper(ii) sulfate solution. The concentration of the copper(ii) sulfate solution is 80 g CuSO 4 per dm 3. Relative atomic masses (A r ): O = 6; S = 32; Fe = 56; Cu = 63.5 Give your answer to 2 significant figures. Mass of iron = g (4) (Total 3 marks) Page 7 of 27

18 8 Hydrogen chloride (HCl) is a gas. (a) Complete the diagram to show all of the arrangement of the outer shell electrons of the hydrogen and chlorine atoms in hydrogen chloride. () (b) Hydrochloric acid is a strong acid. Ethanoic acid is a weak acid. Describe a reaction that could be used to show the difference between a weak acid and a strong acid. You should explain why the weak acid and the strong acid give different results. (6) (Total 7 marks) Page 8 of 27

19 9 Exothermic reactions transfer energy to the surroundings. (a) Draw a reaction profile for an exothermic reaction using the axes in Figure. Show the: relative energies of the reactants and products activation energy and overall energy change. Figure (2) Page 9 of 27

20 (b) Combustion is an exothermic reaction. Calculate the overall energy change for the complete combustion of one mole of methane in oxygen. Bond Bond energy in kj / mol Overall energy change = kj / mol (3) Page 20 of 27

21 (c) Figure 2 shows the chemicals given to a student. Figure 2 The student wants to investigate the reactivity of the four metals. Outline a plan the student could use to investigate the relative reactivity of the four metals, W, X, Y and Z. The plan should use the fact that all four metals react exothermically with dilute sulfuric acid. You should name the apparatus used and comment on the safe use of the chemicals. (6) Page 2 of 27

22 (d) Another student used displacement reactions to investigate the relative reactivity of the four metals, W, X, Y and Z. The table below shows the student s results. Observations Solution Metal W Metal X Metal Y Metal Z Copper nitrate Brown layer formed on metal Brown layer formed on metal Brown layer formed on metal No change Magnesium sulfate No change No change No change No change Sulfuric acid Gas bubbles produced Few gas bubbles produced Gas bubbles produced No change Zinc chloride Grey layer formed on metal No change No change No change Give the order of reactivity of metals, W, X, Y and Z. Use the results in the table above to justify your answer. (3) Page 22 of 27

23 (e) The student concluded that these results could also be used to justify the order of reactivity of copper, magnesium, hydrogen and zinc. The student is not completely correct. Use the results in the table above to explain why. Suggest one further experiment that would provide evidence for the student s conclusion. (4) (Total 8 marks) 0 This question is about the reactions of acids. (a) When dilute hydrochloric acid is reacted with sodium hydroxide solution there is a temperature change. Explain how the temperature changes. (2) Page 23 of 27

24 (b) Acids produce hydrogen ions in aqueous solutions. What is the ionic equation for neutralisation reactions? Tick one box. H + (aq) + H 2 O(l) H 3 O + (aq) H + (aq) + OH (aq) H 2 O(l) 2 H 2 O(l) H 3 O + (aq) + OH (aq) H 2 O(l) 2 H + (aq) + O 2 (aq) () (c) Sulfuric acid reacts with copper carbonate to produce a salt, water and carbon dioxide. H 2 SO 4 + CuCO 3 CuSO 4 + H 2 O + CO 2 What is the name of the salt produced? () (d) A student reacted four metals with water and with a dilute acid to work out the order of reactivity of the metals. The table below shows some of the observations. Metal Reaction with water Reaction with dilute acid Calcium Bubbles of gas X Copper Y No bubbles of gas Magnesium Few bubbles of gas Bubbles of gas Zinc No bubbles of gas Bubbles of gas Write the observations for X and Y. Observation at X Observation at Y (2) Page 24 of 27

25 (e) Write the four metals, calcium, copper, magnesium and zinc, in order of reactivity. Start with the most reactive metal. (2) (f) Some gases given off in reactions can be identified by chemical tests. Draw one line from each chemical test to the name of the gas. Chemical test Gas (3) (g) Acids react with bases to produce salts and water (H 2 O). The electronic structure of a hydrogen atom is 2, The electronic structure of an oxygen atom is 2,6 Draw a diagram to show the arrangement of the outer shell electrons in a molecule of water. (2) (Total 3 marks) Page 25 of 27

26 This question is about the electrolysis of two compounds. Figure shows the electrolysis of molten lead bromide. Figure (a) The electrolyte contains lead ions (Pb 2+ ) and bromide ions (Br ). Complete the sentences. Use words from the box. atoms bromide bromine ions lead molecules oxygen At the positive electrode the gas produced is At the negative electrode lead gain electrons and. (3) Page 26 of 27

27 (b) A student measured the volumes of each gas produced during the electrolysis of water. The table below shows the student s results. Time in minutes Volume of gas produced in cm 3 Hydrogen Oxygen Page 27 of 27

28 The student plotted a graph of the results for oxygen. Figure 2 shows the graph. The student did not put a scale on the y axis. On the graph in Figure 2: complete the scale for the y axis plot the results for hydrogen include a line of best fit. Figure 2 (3) Page 28 of 27

29 (c) Use the graph to calculate the mean volume of oxygen produced per second. Mean volume of oxygen produced = cm 3 / s (3) (Total 9 marks) 2 Iron is a metal that has many uses. (a) Iron is extracted from iron ore. Part of the process involves reduction of the ore with carbon monoxide. Iron ore contains iron oxide (Fe 2 O 3 ). Write a balanced equation for the reaction of iron oxide with carbon monoxide. (3) (b) Explain why this reaction is a redox reaction. (2) Page 29 of 27

30 Steel is an alloy of iron. Steel is used to make cars. After its useful life a car is taken to a scrapyard for recycling. (c) Suggest four benefits of recycling a car body. (4) Page 30 of 27

31 (d) Figure shows an electromagnet being used to lift a car in a scrapyard. Figure An electromagnet is made up of a solenoid. Figure 2 shows a solenoid. Figure 2 Draw the magnetic field of the solenoid on Figure 2. (2) Page 3 of 27

32 (e) In a scrapyard, an electromagnet is used to lift and release cars so they can be moved around. Suggest two ways a solenoid could be made to lift and release cars in a scrapyard. Explain why each suggestion would be useful in the scrapyard. (4) (Total 5 marks) 3 In 869 there were 60 known elements. Mendeleev arranged the elements in order of their atomic mass (atomic weight). He realised that elements with similar properties occurred at regular intervals. (a) Suggest why one of the groups that is on today s periodic table was not in Mendeleev s periodic system. () (b) Explain the arrangement of the first 20 elements in today s periodic table. You should answer in terms of atomic structure. (2) Page 32 of 27

33 (c) A student put some potassium bromide solution in a test tube. She added a few drops of chlorine solution and observed the result. She repeated the process using different potassium halide salts and different halogens. The table below shows the student s results. Solution of halogen Potassium chloride solution Potassium bromide solution Potassium iodide solution Chlorine Orange colour forms Brown colour forms Bromine No reaction Brown colour forms Iodine No reaction No reaction Give the order of reactivity of the halogens from the results in the table above. Explain how you used the results to show this order of reactivity. Order Explanation (2) (d) Write a balanced ionic equation for the reaction of chlorine with bromide ions in solution. (3) Page 33 of 27

34 (e) Explain the order of reactivity of Group 7 elements. Include information about atomic structure. (2) (Total 0 marks) 4 Aluminium is produced from an ore called bauxite. Bauxite contains aluminium oxide. Look at Figure. Figure (a) Calculate the percentage of bauxite that is converted into aluminium oxide. Percentage = (2) Page 34 of 27

35 (b) Show by calculation that the mass of aluminium produced is less than that expected from 950 kg aluminium oxide (Al 2 O 3 ). You should state the difference in the mass of aluminium expected and the mass of aluminium produced to three significant figures. Relative atomic masses (A r ): O = 6; Al = 27 (3) (c) Figure 2 shows an electrolysis cell used to extract aluminium. Figure 2 Why does the carbon anode used in the electrolysis cell need to be continually replaced? (3) Page 35 of 27

36 (d) In an electrolysis cell the current is A, at a potential difference of 4V. Calculate the energy transferred by the electrolysis cell in 24 hours. Energy transferred = J (5) (e) The half equation at the cathode is: Al e Al Calculate the number of moles of electrons needed to produce 000 kg of aluminium. Give your answer to three significant figures. Relative atomic mass (A r ): Al = 27 Answer = moles (3) (Total 6 marks) Page 36 of 27

37 5 A student investigates a potassium salt, X. She finds that salt X: has a high melting point does not conduct electricity when it is solid dissolves in water and the solution does conduct electricity. (a) What is the type of bonding in salt X? Tick one box. Covalent Giant molecular Ionic Metallic () (b) What is the name given to solutions that conduct electricity? () (c) Why does a solution of salt X in water conduct electricity? () Page 37 of 27

38 (d) The student electrolyses a solution of potassium chloride. Figure shows the apparatus she uses. Figure When the current is switched on, bubbles of hydrogen gas are given off at the negative electrode. Explain why hydrogen is produced and not potassium. (2) Page 38 of 27

39 (e) The student then compares the relative conductivity of different concentrations of potassium chloride. Figure 2 shows the apparatus she uses. Figure 2 This is the method used.. Add potassium chloride solution to the water one drop at a time. 2. Stir the mixture. 3. Record the reading on the conductivity meter. The table below shows the student s results. Number of drops of potassium chloride solution Relative conductivity of solution Page 39 of 27

40 When there is no potassium chloride in the beaker no electrical charge flows. Suggest why pure water does not conduct electricity. (2) (f) Describe the relationship shown in the table above. (2) (Total 9 marks) 6 The elements in Group of the periodic table are metals. (a) The elements in Group are called the alkali metals. Why are they called the alkali metals? (2) Page 40 of 27

41 (b) Explain the increase in reactivity of elements further down the group. (4) (c) Lithium oxide is an ionic compound. Draw a dot and cross diagram to show how lithium and oxygen combine to form lithium oxide. Only show the electrons in the outer shell of each atom. Give the charges on the ions formed. (4) (Total 0 marks) Page 4 of 27

42 7 The salt copper sulfate can be made by reacting copper carbonate with dilute sulfuric acid. CuCO 3 (s) + H 2 SO 4 (aq) CuSO 4 (aq) + H 2 O(l) + CO 2 (g) (a) Write a method that a student could use to prepare a pure, dry sample of copper You do not need to write a risk assessment or include safety points. (6) (b) Calculate the number of molecules in 4 g of carbon dioxide. Give your answer in standard form. Relative atomic masses (A r ): C = 4; O = 6 Answer = molecules (4) (Total 0 marks) Page 42 of 27

43 8 This question is about magnesium. (a) (i) The electronic structure of a magnesium atom is shown below. Use the correct answer from the box to complete each sentence. electrons neutrons protons shells The nucleus contains protons and The particles with the smallest relative mass that move around the nucleus are called Atoms of magnesium are neutral because they contain the same number of electrons and (3) (ii) A magnesium atom reacts to produce a magnesium ion. Which diagram shows a magnesium ion? Tick ( ) one box. () Page 43 of 27

44 (b) Magnesium and dilute hydrochloric acid react to produce magnesium chloride solution and hydrogen. Mg(s) + 2 HCl(aq) MgCl 2 (aq) + H 2 (g) (i) State two observations that could be made during the reaction.. 2. (2) (ii) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. Describe a method for making pure crystals of magnesium chloride from magnesium and dilute hydrochloric acid. In your method you should name the apparatus you will use. You do not need to mention safety. (6) (Total 2 marks) Page 44 of 27

45 9 This question is about iron and aluminium. (a) Iron is extracted in a blast furnace. Figure is a diagram of a blast furnace. (i) Calcium carbonate decomposes at high temperatures. Complete the word equation for the decomposition of calcium carbonate. calcium carbonate + (2) (ii) Carbon burns to produce carbon dioxide. The carbon dioxide produced reacts with more carbon to produce carbon monoxide. Balance the equation. C(s) + CO 2 (g) CO(g) () Page 45 of 27

46 (iii) Carbon monoxide reduces iron(iii) oxide: Fe 2 O 3 (s) + 3 CO(g) 2 Fe(s) + 3 CO 2 (g) Calculate the maximum mass of iron that can be produced from 300 tonnes of iron(iii) oxide. Relative atomic masses (A r ): O = 6; Fe = 56 Maximum mass = tonnes (3) (b) Aluminium is extracted by electrolysis, as shown in Figure 2. Figure 2 (i) Why can aluminium not be extracted by heating aluminium oxide with carbon? () Page 46 of 27

47 (ii) Explain why aluminium forms at the negative electrode during electrolysis. (3) (iii) Explain how carbon dioxide forms at the positive electrodes during electrolysis. (3) (Total 3 marks) 20 This question is about metals. (a) Which unreactive metal is found in the Earth as the metal itself? Tick ( ) one box. aluminium gold magnesium () Page 47 of 27

48 (b) Complete the sentence. Aluminium is an element because aluminium is made of only one type of. () (c) Figure shows the electronic structure of an aluminium atom. (i) Use the correct words from the box to complete the sentence. electrons ions protons neutrons shells The nucleus of an aluminium atom contains and. (2) (ii) Complete the sentence. In the periodic table, aluminium is in Group. () Page 48 of 27

49 (d) Aluminium is used for kitchen foil. Figure 2 shows a symbol on a box of kitchen foil. The symbol means that aluminium can be recycled. It does not show the correct chemical symbol for aluminium. (i) What is the correct chemical symbol for aluminium?. () (ii) Give two reasons why aluminium should be recycled. (2) (e) Aluminium has a low density, conducts electricity and is resistant to corrosion. Which one of these properties makes aluminium suitable to use as kitchen foil? Give a reason for your answer. (2) (Total 0 marks) Page 49 of 27

50 2 This question is about electrolysis. (a) Metal spoons can be coated with silver. This is called electroplating. Suggest one reason why spoons are electroplated. () (b) When sodium chloride solution is electrolysed the products are hydrogen and chlorine. (i) What is made from chlorine? Tick ( ) one box. Bleach Fertiliser Soap () (ii) Sodium chloride solution contains two types of positive ions, hydrogen ions (H + ) and sodium ions (Na + ). Why is hydrogen produced at the negative electrode and not sodium? Tick ( ) one box. Hydrogen is a gas. Hydrogen is less reactive than sodium. Hydrogen ions move faster than sodium ions. () Page 50 of 27

51 (iii) Hydrogen and chlorine can be used to produce hydrogen chloride. The diagrams in Figure show how the outer electrons are arranged in an atom of hydrogen and an atom of chlorine. Complete Figure 2 to show how the outer electrons are arranged in a molecule of hydrogen chloride (HCl). () (iv) What is the type of bond in a molecule of hydrogen chloride? Tick ( ) one box. Covalent Ionic Metallic () Page 5 of 27

52 (v) Why is hydrogen chloride a gas at room temperature (20 C)? Tick ( ) two boxes. Hydrogen chloride has a low boiling point. Hydrogen chloride has a high melting point. Hydrogen chloride is made of simple molecules. Hydrogen chloride does not conduct electricity. Hydrogen chloride has a giant structure. (2) (c) Aluminium is produced by electrolysis of a molten mixture of aluminium oxide and cryolite. This is shown in Figure 3. (i) Name a gas produced at the positive electrode. () Page 52 of 27

53 (ii) Aluminium ions move to the negative electrode. Explain why. (2) (iii) At the negative electrode, the aluminium ions gain electrons to produce aluminium. What is this type of reaction called? Tick ( ) one box. Combustion Oxidation Reduction () (iv) Aluminium has layers of atoms, as shown in Figure 4. Complete the sentence. Metals can be bent and shaped because the layers of atoms can () Page 53 of 27

54 (d) Electrodes used in the production of aluminium are made from graphite. (i) Which diagram, A, B or C, shows the structure of graphite? The structure of graphite is shown in diagram () (ii) The temperature for the electrolysis is 950 C. Use the correct answer from the box to complete the sentence. cross links a giant ionic lattice strong covalent bonds The graphite does not melt at 950 C because graphite has. () (Total 4 marks) Page 54 of 27

55 22 A student investigated the temperature change when zinc reacts with copper sulfate solution. The student used a different concentration of copper sulfate solution for each experiment. The student used the apparatus shown below. The student: measured 50 cm 3 copper sulfate solution into a glass beaker measured the temperature of the copper sulfate solution added 2.3 g zinc measured the highest temperature repeated the experiment using copper sulfate solution with different concentrations. The equation for the reaction is: Zn(s) + CuSO 4 (aq) Cu(s) + ZnSO 4 (aq) zinc + copper sulfate solution copper + zinc sulfate solution (a) The thermometer reading changes during the reaction. Give one other change the student could see during the reaction. () (b) Suggest one improvement the student could make to the apparatus. Give a reason why this improves the investigation. Improvement Reason (2) Page 55 of 27

56 (c) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. The student s results are shown in the table. Table Experiment number Concentration of copper sulfate in moles per dm 3 Increase in temperature in C Describe and explain the trends shown in the student s results. (6) Page 56 of 27

57 (Total 9 marks) 23 This question is about compounds. (a) The table gives information about the solubility of some compounds. Soluble compounds All potassium and sodium salts All nitrates Chlorides, bromides and iodides, except those of silver and lead Use information from the table to answer these questions. (i) Name a soluble compound that contains silver ions. () (ii) Name a soluble compound that contains carbonate ions. () (b) Metal oxides react with acids to make salts. What type of compound is a metal oxide? () (c) Lead nitrate solution is produced by reacting lead oxide with nitric acid. (i) State how solid lead nitrate can be obtained from lead nitrate solution. () (ii) Balance the equation for the reaction. PbO + HNO 3 Pb(NO 3 ) 2 + H 2 O () (iii) Give the total number of atoms in the formula Pb(NO 3 ) 2 () Page 57 of 27

58 (d) An oxide of lead that does not have the formula PbO contains 6.2 g of lead and 0.72 g of oxygen. Calculate the empirical formula of this lead oxide. Relative atomic masses (A r ): O = 6; Pb = 207 You must show your working to gain full marks. Empirical formula = (4) (Total 0 marks) 24 This question is about sodium chloride and iodine. (a) Describe the structure and bonding in sodium chloride. (4) (b) When sodium chloride solution is electrolysed, one product is chlorine. Name the two other products from the electrolysis of sodium chloride solution. (2) Page 58 of 27

59 (c) Many people do not have enough iodine in their diet. Sodium chloride is added to many types of food. Some scientists recommend that sodium chloride should have a compound of iodine added. Give one ethical reason why a compound of iodine should not be added to sodium chloride used in food. () (d) The bonding in iodine is similar to the bonding in chlorine. (i) Complete the diagram below to show the bonding in iodine. Show the outer electrons only. (2) (ii) Explain why iodine has a low melting point. (3) (iii) Explain, in terms of particles, why liquid iodine does not conduct electricity. (2) (Total 4 marks) Page 59 of 27

60 25 Some pollutants cause acid rain. A student tested 25.0 cm 3 samples of three types of rainwater, P, Q and R. The student titrated the samples with sodium hydroxide solution (an alkali). The student recorded the volume of sodium hydroxide solution needed to neutralise the rainwater. The student s results are shown in Table. Table Volume of sodium hydroxide needed to neutralise the rainwater in cm 3 Type of rainwater Titration Titration 2 Titration 3 Titration 4 Titration 5 P Q R (a) (i) The student calculated the mean value for rainwater R as 9.0 cm 3. Show how the student calculated the mean value for rainwater R. (2) (ii) Write down P, Q and R in order of their acidity. Most acidic Least acidic (2) Page 60 of 27

61 (b) A second student repeated the experiment and recorded the results in Table 2. Table 2 Volume of sodium hydroxide needed to neutralise the rainwater in cm 3 Type of rainwater Titration Titration 2 P 7 5 Q 9 R 20 8 Use Table and Table 2 to suggest two improvements the second student could make to obtain more accurate results. (2) (c) The results of the two students show that the experiment is reproducible. Give the reason why. () (Total 7 marks) 26 Iron is extracted from iron oxide in the blast furnace. (a) The equation for one of the reactions in the blast furnace is: Fe 2 O 3 + 3CO 2Fe + 3CO 2 (i) Complete the word equation for this reaction. iron oxide + carbon monoxide + (2) Page 6 of 27

62 (ii) Oxygen is removed from iron oxide in the blast furnace. Draw a ring around the correct answer to complete the sentence. The iron oxide is neutralised. oxidised. reduced. () (b) The diagrams represent pure iron and iron from the blast furnace. Pure iron Iron from the blast furnace (i) Draw one line from each statement to the correct explanation. (2) Page 62 of 27

63 (ii) Explain why iron from the blast furnace is harder than pure iron. Use the diagrams on page 4 to help you. (2) (Total 7 marks) 27 Sulfur is a non-metal. Sulfur burns in the air to produce sulfur dioxide, SO 2 (a) Why is it important that sulfur dioxide is not released into the atmosphere? Tick ( ) one box. Sulfur dioxide causes acid rain. Sulfur dioxide causes global dimming. Sulfur dioxide causes global warming. () (b) Sulfur dioxide dissolves in water. What colour is universal indicator in a solution of sulfur dioxide? Give a reason for your answer. (2) Page 63 of 27

64 (c) Sulfur dioxide is a gas at room temperature. The bonding in sulfur dioxide is covalent. Explain, in terms of its structure and bonding, why sulfur dioxide has a low boiling point. (3) (d) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. Sulfur dioxide is produced when fossil fuels are burned. It is important that sulfur dioxide is not released into the atmosphere. Three of the methods used to remove sulfur dioxide from gases produced when fossil fuels are burned are: wet gas desulfurisation ( W) dry gas desulfurisation ( D) seawater gas desulfurisation ( S). Information about the three methods is given in the bar chart and in Table and Table 2. Method of removing sulfur dioxide Page 64 of 27

65 Table Method Material used How material is obtained W Calcium carbonate, CaCO 3 Quarrying D Calcium oxide, CaO Thermal decomposition of calcium carbonate: CaCO 3 CaO + CO 2 S Seawater From the sea Table 2 Method W D S What is done with waste material Solid waste is sold for use in buildings. Carbon dioxide is released into the atmosphere. Solid waste is sent to landfill. Liquid waste is returned to the sea. Page 65 of 27

66 Evaluate the three methods of removing sulfur dioxide from waste gases. Compare the three methods and give a justified conclusion. (6) (Total 2 marks) Page 66 of 27

67 28 Lead nitrate solution reacts with potassium iodide solution. The reaction produces a solid. Figure shows the reaction occurring. Figure Lead Iodide By Der Kreole (own work) (CC-BY-3.0) via Wikimedia Commons (a) (i) Give the name of this type of reaction. Tick ( ) one box. Combustion Neutralisation Precipitation () (ii) Write the missing state symbols in the chemical equation. Pb(NO 3 ) 2 (aq) + 2KI( ) PbI 2 ( ) + 2KNO 3 (aq) (2) (iii) Complete the word equation for the reaction. lead nitrate + lead iodide + (2) Page 67 of 27

68 (iv) How is solid lead iodide separated from the solution? Draw a ring around the correct answer. Distillation Electrolysis Filtration () (b) A group of students investigated the movement of particles. The students filled a container with water. The students added a crystal of lead nitrate at position X and a crystal of potassium iodide at position Y, as shown in Figure 2. Figure 2 view from above After 3 minutes solid lead iodide started to form at the position shown in Figure 3. Figure 3 view from above (i) Tick ( ) the correct box to complete the sentence. Lead ions and iodide ions move through the water by diffusion. evaporation. neutralisation. () Page 68 of 27

69 (ii) What conclusion can you make about the speed of movement of lead ions compared with iodide ions? Give a reason for your answer. (2) (iii) The students repeated the experiment at a higher temperature. The solid lead iodide formed after a shorter period of time. Explain why, in terms of particles. (2) (Total marks) 29 A student investigated the conductivity of different concentrations of sodium chloride solution. The student set the apparatus up as shown in Figure. Figure Page 69 of 27

70 The student measured the conductivity of the pure water with a conductivity meter. The reading on the conductivity meter was zero. (a) The student: added sodium chloride solution one drop at a time stirred the solution recorded the reading on the conductivity meter. The student s results are shown in the table below. Number of drops of sodium chloride solution added Relative conductivity of solution Page 70 of 27

71 (i) The student plotted the results on the grid shown in Figure 2. Plot the four remaining results. Draw a line of best fit, ignoring the anomalous result. Figure 2 Number of drops of sodium chloride added (3) (ii) One of the points is anomalous. Suggest one error that the student may have made to cause the anomalous result. () Page 7 of 27

72 (iii) The student wanted to compare the conductivity of sodium chloride solution with the conductivity of potassium chloride solution. State one variable he should keep constant when measuring the conductivity of the two solutions. () (b) (i) Explain, in terms of bonding, why pure water does not conduct electricity. (2) (ii) Explain why sodium chloride solution conducts electricity. (2) (iii) After he had added sodium chloride solution, the student noticed bubbles of gas at the negative electrode. Complete the sentence. The gas produced at the negative electrode is () (Total 0 marks) Page 72 of 27

73 30 Use the periodic table and the information in the table below to help you to answer the questions. The table shows part of an early version of the periodic table. Group Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 H Li Be B C N O F Na Mg Al Si P S Cl (a) Hydrogen was placed at the top of Group in the early version of the periodic table. The modern periodic table does not show hydrogen in Group. (i) State one similarity between hydrogen and the elements in Group. () (ii) State one difference between hydrogen and the elements in Group. () (b) Fluorine, chlorine, bromine and iodine are in Group 7, the halogens. The reactivity of the halogens decreases down the group. Bromine reacts with a solution of potassium iodide to produce iodine. Br 2 + 2KI 2KBr + I 2 (i) In the reaction between bromine and potassium iodide, there is a reduction of bromine to bromide ions. In terms of electrons, what is meant by reduction? () (ii) Complete the half equation for the oxidation of iodide ions to iodine molecules. 2I (2) Page 73 of 27

74 (iii) Explain, in terms of electronic structure, why fluorine is the most reactive element in Group 7. (3) (Total 8 marks) 3 A student was trying to produce hydrogen gas. Figure shows the apparatus she used. Figure (a) No gas was produced. The student s teacher said that this was because the substances in the flask did not react. (i) Suggest why the substances in the flask did not react. () Page 74 of 27

75 (ii) Which two substances could the student have put in the flask to produce hydrogen safely? Tick ( ) one box. Gold and dilute hydrochloric acid Potassium and dilute hydrochloric acid Zinc and dilute hydrochloric acid () (b) Another student did produce hydrogen from two substances. Figure 2 shows the apparatus the student used to collect and measure the volume of the hydrogen gas. Figure 2 Give the name of the apparatus labelled X. () Page 75 of 27

76 Mean volume = cm 3 (2) (c) The student did the experiment four times. Her results are shown in the table below. Experiment Volume of hydrogen collected in one minute in cm (i) One of the results is anomalous. Which result is anomalous? Write your answer in the box. Give a reason for your choice. (2) (ii) Calculate the mean volume of hydrogen collected in one minute. (iii) Give a reason why the experiment should be repeated several times. () Page 76 of 27

77 (d) A teacher collected two tubes full of hydrogen gas, as shown in Figure 3. Figure 3 She tested tube A with a lighted splint as soon as she took the bung out. She tested tube B with a lighted splint a few seconds after taking the bung out. (i) Suggest why tube B gave a much louder pop than tube A. () (ii) Complete and balance the chemical equation for the reaction that takes place when the hydrogen reacts in this test. H 2 + O 2 (2) (Total marks) Page 77 of 27

78 32 A student investigated displacement reactions of metals. The student added different metals to copper sulfate solution and measured the temperature change. The more reactive the metal is compared with copper, the bigger the temperature change. The apparatus the student used is shown in Figure. Figure (a) State three variables that the student must control to make his investigation a fair test (3) Page 78 of 27

79 (b) Figure 2 shows the thermometer in one experiment before and after the student added a metal to the copper sulfate solution. Figure 2 Before adding metal After adding metal Use Figure 2 to complete Table. Table Temperature before adding metal in C Temperature after adding metal in C Change in temperature in C (3) Page 79 of 27

80 (c) The student repeated the experiment three times with each metal. Table 2 shows the mean temperature change for each metal. Table 2 Metal Mean temperature change in C Cobalt 4.5 Gold 0.0 Magnesium 0.0 Nickel 3.0 Silver 0.0 Tin.5 (i) On Figure 3, draw a bar chart to show the results. Figure 3 (3) (ii) Why is a line graph not a suitable way of showing the results? () Page 80 of 27

81 (iii) Use the results to work out which metal is the most reactive. Give a reason for your answer. Most reactive metal Reason (2) (iv) Explain why there was no temperature change when silver metal was added to the copper sulfate solution. (2) (v) It is not possible to put all six metals in order of reactivity using these results. Suggest how you could change the experiment to be able to put all six metals into order of reactivity. (2) (Total 6 marks) Page 8 of 27

82 33 This question is about copper. (a) Most of the copper extracted is used in electric circuits. The figure below shows how impurities change the electrical conductivity of copper. Percentage of impurities in copper Copper extracted by smelting is about 99% pure. The 99% pure copper produced by smelting is purified to % pure copper by electrolysis. Use values from the graph to explain why copper is purified to %. (2) Page 82 of 27

83 (b) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. Read the information in the box. Copper extraction World demand for copper for the year 20 was about 20 million tonnes. World reserves of copper are estimated to be 700 million tonnes. Most of the copper used is obtained from copper ores, which are mined. The copper ore chalcopyrite is heated in a furnace to produce copper sulfide, CuS The furnace is heated by burning fossil fuels. Air is then blown through the hot copper sulfide, to produce copper and sulfur dioxide. CuS + O 2 Cu + SO 2 A scientist made the statement: Copper should be recycled. Use the information in the box and your own knowledge and understanding to justify the scientist s statement. Page 83 of 27

84 Extra space (6) (c) Phytomining is used to obtain copper from land that contains very low percentages of copper compounds. Describe how copper compounds are obtained by phytomining. (3) (Total marks) Page 84 of 27

85 34 Where copper ore has been mined there are areas of land that contain very low percentages of copper compounds. One way to extract the copper is to grow plants on the land. The plants absorb copper compounds through their roots. The plants are burned to produce copper oxide. The copper oxide produced from plants can be reacted to produce copper or copper sulfate solution, as shown in Figure. Figure (a) Draw a ring around the correct answer to complete each sentence. (i) Copper ores contain enough copper to make extraction of the metal carbon neutral. economical. reversible. () (ii) Using plants to extract metals is called photosynthesis. phytomining. polymerisation. () (iii) Copper oxide reacts with carbon to produce copper and carbon dioxide. oxygen. sulfur dioxide. () (b) Copper is produced from copper sulfate solution by displacement using iron or by electrolysis. (i) Complete the word equation. copper sulfate + iron + (2) Page 85 of 27

86 (ii) Figure 2 shows the electrolysis of copper sulfate solution. Figure 2 Why do copper ions go to the negative electrode? () (c) Suggest two reasons why copper should not be disposed of in landfill sites. (2) (Total 8 marks) Page 86 of 27

87 35 Some students investigated reactions to produce magnesium. (a) The students used electrolysis to produce magnesium from magnesium chloride, as shown in the figure below. (i) Magnesium chloride contains magnesium ions and chloride ions. Why does solid magnesium chloride not conduct electricity? () (ii) One of the products of the electrolysis of molten magnesium chloride is magnesium. Name the other product. () (iii) Why do magnesium ions (Mg 2+ ) move to the negative electrode? () (iv) At the negative electrode, the magnesium ions (Mg 2+ ) gain electrons to become magnesium atoms. How many electrons does each magnesium ion gain? () Page 87 of 27

88 (b) The students did the experiment four times and weighed the magnesium produced. The table below shows their results. Experiment Mass of magnesium produced in grams (i) There is an anomalous result. Suggest one possible reason for the anomalous result. () (ii) Calculate the mean mass of magnesium produced, taking account of the anomalous result. Mean mass = g (2) Page 88 of 27

89 (c) The formula of magnesium chloride is MgCl 2 The relative formula mass of magnesium chloride is 95. The relative atomic mass of magnesium is 24. (i) Use the equation to calculate the percentage mass of magnesium in magnesium chloride. Percentage mass of magnesium = 00% Percentage mass of magnesium in magnesium chloride = % (2) (ii) Draw a ring around the relative mass of chlorine in MgCl () (d) Magnesium is also produced from the reaction of magnesium oxide with silicon. (i) The equation for the reaction is: 2 MgO(s) + Si(s) SiO 2 (s) + 2 Mg(s) What is the meaning of this symbol? Draw a ring around the correct answer. neutralisation reaction precipitation reaction reversible reaction () (ii) The forward reaction is endothermic. Draw a ring around the correct answer to complete the sentence. decreases. In an endothermic reaction the temperature of the surroundings increases. stays the same. () (Total 2 marks) Page 89 of 27

90 Mark schemes (a) extra lines from solution negate the mark 2 (b) H + (c) 3 (d) (e) (f) Neutralisation sodium sulfate Add indicator to sodium hydroxide solution allow add indicator to sulfuric acid Add sulfuric acid (gradually) allow add sodium hydroxide solution (gradually) allow ph probe until indicator just changes (colour) or until universal indicator turns green or shows ph7 [9] 2 (a) Z (b) magnesium sulfate does not react with any of the metals allow there is no change / increase in temperature with any of the metals (c) temperature increase Page 90 of 27

91 (d) Level 2 (3 4 marks): A detailed and coherent plan covering all the steps. The steps include the improvements and are set out in a logical manner. Level ( 2 marks): Simple statements of improvements to the apparatus or steps are made but they may not be set out in a logical manner. 0 marks: No relevant content Indicative content Simple statements stir the solution use the same amount of each solution use the same concentration of solution put insulation or a lid on the beaker measure how high temperature goes (e) Coherent statements in a logical order pour a fixed, measured volume of the metal salt solution into a plastic / polystyrene cup measure and record the temperature of the solution stir and add g of metal to the solution (put a lid on the cup) measure and record the temperature after a set time or measure and record the greatest / highest temperature calculate and record the temperature increase (repeat each individual experiment at least two more times and calculate the mean temperature increase) Activation energy 4 (f) 386 (kj) / % [0] Page 9 of 27

92 3 Level 3 (5 6 marks): A coherent method is described with relevant detail, which demonstrates a broad understanding of the relevant scientific techniques, procedures and safety precautions. The steps in the method are logically ordered with the dependent and control variables correctly identified. The method would lead to the production of valid results. Level 2 (3 4 marks): The bulk of a method is described with mostly relevant detail, which demonstrates a reasonable understanding of the relevant scientific techniques, procedures and safety precautions. The method may not be in a completely logical sequence and may be missing some detail. Level ( 2 marks): Simple statements are made which demonstrate some understanding of some of the relevant scientific techniques, procedures and safety precautions. The response may lack a logical structure and would not lead to the production of valid results. 0 marks: No relevant content Indicative content Named chemicals copper oxide sulfuric acid copper sulfate Correct use of apparatus stirring rod spatula beaker filter funnel and filter paper evaporating basin Bunsen burner tripod and gauze bench mat conical flask Method add (excess) copper oxide to sulfuric acid heat the mixture filter the mixture method to evaporate some of the water from the filtrate eg using a water bath or evaporating to half volume leave solution (to cool and) to form crystals remove and dry crystals Safety wearing of safety glasses / goggles care with use of sulfuric acid as corrosive warming not boiling mixture of copper oxide and sulfuric acid hold beaker containing warm mixture with tongs whilst filtering [6] Page 92 of 27

93 4 (a) electrolysis (b) Cathode hydrogen Anode bromine (c) copper ions are positive so the copper ions are attracted to the negative cathode allow so the copper ions gain electrons from the cathode to form copper atoms [5] 5 (a) A base (b) forces (c) calcium loses electrons and oxygen gains electrons max 3 for incorrect reference to atom / ion or to oxygen / oxide two electrons are transferred calcium has a 2 + charge oxide has a 2 charge [6] 6 (a) 408 kg (b) all points correct ± ½ small square allow mark if 5 points correct 2 best fit line (c) 5525 dm 3 Page 93 of 27

94 (d) relative formula mass of TiCl 4 is % Answer given to 3 significant figures = 25.3 % 25.23% with or without working gains 3 marks (e) (f) argon is unreactive water (vapour) would react with sodium allow water (vapour) would react with titanium(iv) chloride and air contains oxygen that would react with reactants allow and air contains oxygen that would react with products (titanium conducts electricity) because electrons in the outer shell of the metal atoms are delocalised and so electrons are free to move allow the delocalised electrons in the metal carry electrical charge through the metal through the whole structure [5] 7 (a) electrodes connected to d.c. power supply by wires for this diagram ignore the material used for the electrodes as long as they are made from carbon or metals that are inert electrodes labelled anode (+) and cathode ( ) (b) copper ions cause the blue colour answer must be in terms on copper ions copper ions are reduced / converted to copper ions so the concentration of copper ions decreased Page 94 of 27

95 (c) if no other mark awarded allow mark for copper ions are used up during electrolysis copper ions are positive so are attracted to the inert cathode or inert negative electrode copper ions gain electrons at the inert cathode or inert negative electrode so they are reduced to form copper atoms (d) 50 cm 3 contains 4 g CuSO 4 M r CuSO 4 = g CuSO 4 reacts with 56 g Fe =.40(43877) =.4 (g) accept.4(g) with no working shown for 4 marks allow.40(43887) without working shown for 3 marks [3] 8 (a) bonded pair of electrons and 6 non-bonded electrons on chlorine Page 95 of 27

96 (b) Level 3 (5 6 marks): A detailed and coherent explanation of comparative results of a reaction in terms of concentration and ionisation. The response makes logical links between the points raised and uses sufficient examples to support these links. Level 2 (3 4 marks): A description of a reaction with results is given but may miss some details. Links are made but may not be fully articulated and / or precise. Level ( 2 marks): Simple statements are made. The response may fail to make logical links between the points raised. 0 marks: No relevant content Indicative content Simple statements / descriptions of a reaction correct comparative ph, such as, 0 3 (strong) 4 6 (weak) named reaction, such as, with a reactive metal or a named carbonate comparative results or observations of the named reaction, such as, faster reaction (strong) or greater volume of gas produced in a given time (strong) Explanations of different results weak acids are only partially ionised in aqueous solution strong acids are completely ionised in aqueous solution / greater concentration of H + ions aqueous solutions of acids at the same concentration / same state of division of metal / powder, same temperature 6 [7] 9 (a) the relative energies of the reactants, products and the overall energy change the activation energy Page 96 of 27

97 (b) (4 43) + (2 498) = (2 805) + (4 464) = ( =) 88 (kj / mol) allow max 2 marks for one ecf Page 97 of 27

98 (c) Level 3 (5 6 marks): A coherent method is described with relevant detail, which demonstrates a broad understanding of the relevant scientific techniques and procedures. The steps in the method are logically ordered with the dependent and control variables correctly identified. The method would lead to the production of valid results. Level 2 (3 4 marks): The bulk of a method is described with mostly relevant detail, which demonstrates a reasonable understanding of the relevant scientific techniques and procedures. The method may not be in a completely logical sequence and may be missing some detail. Level ( 2 marks): Simple statements are made which demonstrate some understanding of some of the relevant scientific techniques and procedures. The response may lack a logical structure and would not lead to the production of valid results. 0 marks: No relevant content Indicative content Named apparatus thermometer measuring cylinder stirring rod spatula plastic cup (with lid) or beaker stopwatch filter paper or watch glass balance Method weigh the same mass of each metal in each same state of division eg powder measure a set volume of sulfuric acid into a plastic cup or beaker measure and record the temperature of the sulfuric acid add metal W into the plastic cup or beaker stir and record the highest temperature or record the temperature after a set time calculate the increase in temperature repeat the method for metals X, Y and Z repeat for each metal at least three times to calculate a mean Safe use comment on safe use should include wearing safety glasses 6 Page 98 of 27

99 (d) (e) W>Y>X>Z reason for position of W and Z W reacts with most solutions whereas Z reacts with none of the solutions reason for position of X and Y Y is more reactive than X because Y reacts more with sulfuric acid magnesium is most reactive because not displaced by any metal zinc is second most reactive because displaced by only one metal copper and hydrogen cannot be placed in order of reactivity or are least reactive because they both are displaced by the most / three metals experiment add sulfuric acid to copper because copper is less reactive than hydrogen then copper would not react with sulfuric acid to displace hydrogen [9] 0 (a) it goes up / increases because the reaction is exothermic or transfers energy to the surroundings allow gives out thermal / heat energy (b) H + (aq) + OH (aq) H 2 O(l) (c) (d) (e) copper sulfate X bubbles of gas Y no bubbles of gas calcium>magnesium>zinc>copper if not all correct allow mark for at least two metals in the correct position 2 Page 99 of 27

100 (f) Chemical test Gas extra lines from a test negate the mark 3 (g) two pairs of shared electrons oxygen has four other electrons not bonded [3] (a) bromine ions atoms (b) correct scale on y axis points correctly plotted using the scale ± ½ small square best-fit line drawn (c) value for oxygen divided by corresponding time 60 Page 00 of 27

101 = 0.05 (cm 3 / s) allow 0.05 with no working shown for 3 marks [9] 2 (a) Fe 2 O CO 2Fe + 3 CO 2 correct formulae of reactants correct formulae of products correct balancing (b) (c) (d) iron loses oxygen reduction carbon gains oxygen oxidation any four from: resources for manufacture are limited recycling reduces the use of resources reduces energy consumption in extraction / manufacture reduces waste from processing and extraction reduces environmental impact of extraction 4 field lines going through and around coil correct directional arrows Page 0 of 27

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