Pearson Edexcel Merged Question Paper + Mark Scheme (Results) Summer 2022 Pearson Edexcel GCSE In Combined Science (1SC0) Paper 1CF Centre Number Candidate Number *P69481A0120* Turn over Total Marks Candidate surname Other names

Pearson Edexcel Merged Question Paper + Mark Scheme (Results) Summer 2022 Pearson Edexcel GCSE In Combined Science (1SC0) Paper 1CF Centre Number Candidate Number *P69481A0120* Turn over Total Marks Candidate surname Other names Please check the examination details below before entering your candidate information Paper reference   P69481A ©2022 Pearson Education Ltd. Q:1/1/ Pearson Edexcel Level 1/Level 2 GCSE (9–1) You must have: Calculator, ruler Time 1 hour 10 minutes 1SC0/1CF Combined Science PAPER 2 Foundation Tier Instructions • Use black ink or ball-point pen. • Fill in the boxes at the top of this page with your name, centre number and candidate number. • Answer all questions. • Answer the questions in the spaces provided – there may be more space than you need. • Calculators may be used. • Any diagrams may NOT be accurately drawn, unless otherwise indicated. • You must show all your working out with your answer clearly identified at the end of your solution. Information • The total mark for this paper is 60. • The marks for each question are shown in brackets – use this as a guide as to how much time to spend on each question. • In questions marked with an asterisk (*), marks will be awarded for your ability to structure your answer logically, showing how the points that you make are related or follow on from each other where appropriate. • There is a periodic table on the back cover of the paper. Advice • Read each question carefully before you start to answer it. • Try to answer every question. • Check your answers if you have time at the end. *P69481A0220* 2  Answer ALL questions. Write your answers in the spaces provided. Some questions must be answered with a cross in a box . If you change your mind about an answer, put a line through the box and then mark your new answer with a cross . 1 Figure 1 shows a metal spoon and two test tubes being heated in a water bath. One test tube contains a piece of chocolate, the other some liquid egg white. metal spoon chocolate egg white heat Figure 1 After heating, the spoon, the chocolate and the egg white are allowed to cool to room temperature. Figure 2 shows the state of the three different substances before heating, when hot and after cooling. substance before heating when hot after cooling metal spoon solid solid solid chocolate solid liquid solid egg white liquid solid solid Figure 2 *P69481A0320* Turn over 3  (a) Describe the differences in the arrangement and movement of the particles in a solid and in a liquid. (2) difference in arrangement of particles ................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... difference in movement of particles .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (b) What name is given to the process when the chocolate changes from a solid to a liquid? (1) A condensing B evaporating C freezing D melting (c) Give a reason why the metal spoon has not changed state during the experiment. (1) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (d) Explain how we know the change to the egg white is a chemical change rather than a physical change. 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(Total for Question 1 = 6 marks) *P69481A0420* 4  2 Potable water is water that is suitable for drinking. (a) River water can be treated to make it potable. Chlorination, filtration and sedimentation are three of the processes involved in making the river water potable. (i) Which row of the table shows these three processes in the order in which they are carried out? (1) A B C D first second third chlorination sedimentation filtration chlorination filtration sedimentation sedimentation filtration chlorination sedimentation chlorination filtration (ii) State the reason why chlorine is added during the water treatment. (1) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (iii) Describe how sedimentation is carried out. (2) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... *P69481A0520* Turn over 5  (iv) Figure 3 shows the results of an analysis of a sample of potable water. ion concentration in mg dm−3 chloride 60.70 fluoride 0.24 nitrate 24.90 sulfate 71.40 copper 0.05 magnesium 9.10 Figure 3 Using this information, explain why this sample of potable water is not the same as pure water. (2) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... *P69481A0620* 6  (b) A student wanted to distil a sample of potable water. Figure 4 shows apparatus the student used. heat potable water X Figure 4 (i) Name the piece of equipment labelled X in Figure 4. (1) .................................................................................................................................................................................................................................................................................... (ii) The student made an error when setting up the equipment in Figure 4. This error meant no water could be collected in the test tube. Explain what the student needs to do so water can be collected. 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(Total for Question 2 = 9 marks) *P69481A0720* Turn over 7  BLANK PAGE *P69481A0820* 8  3 (a) An atom of aluminium has an atomic mass of 27. Aluminium has an atomic number of 13. State the number of electrons, neutrons and protons in this atom. (3) number of electrons = .............................................................. number of neutrons = .............................................................. number of protons = .............................................................. (b) Aluminium reacts with bromine to form aluminium bromide. A sample of aluminium bromide contains 1.35g of aluminium atoms and 12.00g of bromine atoms. Calculate the empirical formula of this sample of aluminium bromide. (relative atomic masses: Al = 27.0, Br = 80.0) (3) ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... empirical formula = .............................................................. *P69481A0920* Turn over 9  (c) Gallium is in the same group in the periodic table as aluminium and in the same period in the periodic table as bromine. (i) State in which group and period of the periodic table gallium can be found. You may want to refer to the periodic table. (2) group = .............................................................. period = .............................................................. (ii) Gallium had not been discovered when Mendeleev created his first periodic table. Figure 5 shows some properties of gallium that Mendeleev predicted and some of the actual properties of gallium. property predicted property actual property relative atomic mass about 68 70 density in g/ cm3 about 6.0 5.9 melting point lower than 40°C 29.8°C density of oxide in g/ cm3 about 5.5 5.9 Figure 5 Describe how Mendeleev predicted these properties of gallium. 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(Total for Question 3 = 10 marks) *P69481A01020* 10  4 (a) 3.14g of solid copper sulfate was dissolved in water and made up to 250cm3 of solution. concentration (gdm−3) = mass of solid (g) volume of solution (dm ) 3 Calculate the concentration of this copper sulfate solution in g dm−3. (2) ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... concentration = .............................................................. gdm−3 (b) Sodium hydroxide solution was added to a solution of copper sulfate. A precipitate of copper hydroxide and a solution of sodium sulfate were formed. (i) State what would be seen in the reaction. (1) ..................................................................................................................................................................................................................................................................................... (ii) Complete the balanced equation for the reaction by adding a number in front of NaOH. (1) ................NaOH + CuSO4 → Cu(OH)2 + Na2 SO4 (iii) Describe how to obtain a pure, dry sample of the precipitate of copper hydroxide from the reaction mixture. (3) ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... *P69481A01120* Turn over 11  (c) Figure 6 shows the equipment used to electrolyse a sample of sodium sulfate solution. 6V d.c. supply sodium sulfate solution graphite electrode graphite electrode + − Figure 6 Graphite electrodes are used in the electrolysis of sodium sulfate solution. Graphite is used because it is inert and conducts electricity. (i) Figure 7 shows the ions in the sodium sulfate solution. Draw a circle around each of the ions in Figure 7 that are attracted to the negative graphite electrode during the electrolysis. (1) H+ OH− Na+ SO4 2− Figure 7 (ii) State why it is important that the electrodes are inert. (1) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (iii) Explain, in terms of its structure, how graphite conducts electricity. (2) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (Total for Question 4 = 11 marks) *P69481A01220* 12  5 Barium hydroxide reacts with dilute hydrochloric acid to form barium chloride and water. (a) The equation for the reaction is Ba(OH)2 (s) + 2HCl(aq) → BaCl 2 (aq) + 2H2 O(l) Which row of the table shows the correct state of each of the substances in the equation for the reaction? (1) A B C D barium hydroxide hydrochloric acid barium chloride water solid aqueous aqueous liquid solid liquid solid aqueous aqueous aqueous solid liquid aqueous liquid aqueous aqueous (b) A student wanted to investigate how the pH of the mixture changes as barium hydroxide is added to dilute hydrochloric acid. They followed this method. step 1 measure out 50.0cm3 of dilute hydrochloric acid into a beaker using a measuring cylinder step 2 use a glass rod to place a drop of the acid onto a piece of universal indicator paper and record the pH step 3 add 0.2g of barium hydroxide to the acid in the beaker and stir step 4 use the glass rod to place a drop of the mixture onto a new piece of universal indicator paper and record the pH again step 5 repeat steps 3–4 until there is no further change in the pH. (i) Name a piece of equipment which could be used to measure out 50.0cm3 of dilute hydrochloric acid more accurately than the measuring cylinder. (1) .................................................................................................................................................................................................................................................................................... *P69481A01320* Turn over 13  (ii) Describe how the pH of the mixture is determined when a drop of it is placed on the universal indicator paper. 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(iii) In the method, universal indicator paper is used to determine the pH. Explain why litmus paper would not be a suitable indicator to use in this experiment. (2) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... *P69481A01420* 14  (iv) Figure 8 shows the student’s results. mass of barium hydroxide in g pH of mixture 0.0 1 0.2 1 0.4 1 0.6 1 0.8 2 1.0 7 1.2 12 1.4 13 1.6 13 Figure 8 On the grid opposite: • Add suitable scales to the vertical and horizontal axes. • Plot a graph of the pH of the mixture against the mass of barium hydroxide. (3) *P69481A01520* Turn over 15  pH of the mixture mass of barium hydroxide in g *P69481A01620* 16  (c) Figure 9 shows a hazard symbol placed on a container of barium hydroxide. Figure 9 (i) What is the meaning of the hazard symbol in Figure 9? (1) A flammable B health hazard C oxidising D toxic (ii) Barium hydroxide is also corrosive. Give one precaution that the student should take when using barium hydroxide. (1) .................................................................................................................................................................................................................................................................................... .................................................................................................................................................................................................................................................................................... (Total for Question 5 = 11 marks) *P69481A01720* Turn over 17  6 Magnesium carbonate has the formula MgCO3 . (a) Magnesium carbonate contains Mg2+ and CO3 2− ions. (i) The atomic number of magnesium is 12. What is the electronic configuration of the Mg2+ ion? (1) A 2 B 2.8 C 2.8.2 D 2.8.4 (ii) Explain why solid magnesium carbonate cannot conduct electricity but solid magnesium can. (3) ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... (b) Calculate the percentage by mass of magnesium in magnesium carbonate, MgCO3 . (relative atomic masses: C = 12.0, O = 16.0, Mg = 24.0) (3) ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... ..................................................................................................................................................................................................................................................................................... percentage by mass of magnesium = .............................................................. *P69481A01820* 18  *(c) A student has two separate test tubes containing sulfuric acid. The student adds a spatula measure of magnesium carbonate, MgCO3 , to the first test tube and a piece of magnesium to the second test tube. Explain what the student would see in each test tube and the tests that they should carry out to identify the gases produced. Your answer should include word equations for the reactions that would take place. 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(Total for Question 6 = 13 marks) TOTAL FOR PAPER = 60 MARKS *P69481A02020* 20    The periodic table of the elements * The elements with atomic numbers from 58 to 71 are omitted from this part of the periodic table. The relative atomic masses of copper and chlorine have not been rounded to the nearest whole number. 1 2 3 4 5 6 7 0 Key 1 H hydrogen 1 4 He helium 2 7 Li lithium 3 9 Be beryllium 4 relative atomic mass atomic symbol name atomic (proton) number 11 B boron 5 12 C carbon 6 14 N nitrogen 7 16 O oxygen 8 19 F fluorine 9 20 Ne neon 10 23 Na sodium 11 24 Mg magnesium 12 27 Al aluminium 13 28 Si silicon 14 31 P phosphorus 15 32 S sulfur 16 35.5 Cl chlorine 17 40 Ar argon 18 39 K potassium 19 40 Ca calcium 20 45 Sc scandium 21 48 Ti titanium 22 51 V vanadium 23 52 Cr chromium 24 55 Mn manganese 25 56 Fe iron 26 59 Co cobalt 27 59 Ni nickel 28 63.5 Cu copper 29 65 Zn zinc 30 70 Ga gallium 31 73 Ge germanium 32 75 As arsenic 33 79 Se selenium 34 80 Br bromine 35 84 Kr krypton 36 85 Rb rubidium 37 88 Sr strontium 38 89 Y yttrium 39 91 Zr zirconium 40 93 Nb niobium 41 96 Mo molybdenum 42 [98] Tc technetium 43 101 Ru ruthenium 44 103 Rh rhodium 45 106 Pd palladium 46 108 Ag silver 47 112 Cd cadmium 48 115 In indium 49 119 Sn tin 50 122 Sb antimony 51 128 Te tellurium 52 127 I iodine 53 131 Xe xenon 54 133 Cs caesium 55 137 Ba barium 56 139 La* lanthanum 57 178 Hf hafnium 72 181 Ta tantalum 73 184 tungsten 74 186 Re rhenium 75 190 Os osmium 76 192 Ir iridium 77 195 Pt platinum 78 197 Au gold 79 201 Hg mercury 80 204 Tl thallium 81 207 Pb lead 82 209 Bi bismuth 83 [209] Po polonium 84 [210] At astatine 85 [222] Rn radon 86 Mark Scheme (Results) Summer 2022 Pearson Edexcel GCSE In Combined Science (1SC0) Paper 1CF Edexcel and BTEC Qualifications Edexcel and BTEC qualifications are awarded by Pearson, the UK’s largest awarding body. 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