Cambridge IGCSE Physical Science 0652 — 2014 Oct/Nov Paper 2 · Variant 1

This document consists of 20 printed pages. DC (CW/CGW) 89047/5 © UCLES 2014 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 3 5 1 0 4 3 8 5 9 1 * PHYSICAL SCIENCE 0652/21 Paper 2 (Core) October/November 2014 1 hour 15 minutes Candidates answer on the Question Paper. No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use an HB soft pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. Electronic calculators may be used. You may lose marks if you do not show your working or if you do not use appropriate units. A copy of the Periodic Table is printed on page 20. At the end of the examination, fasten all your work securely together. The number of marks is given in brackets [ ] at the end of each question or part question.

2 0652/21/O/N/14 © UCLES 2014 1 A student is investigating the stretching of a spring. She sets up the apparatus as shown in Fig. 1.1 and measures the length of the spring with different loads. spring pointer load metre ruler Fig. 1.1 (a) Table 1.1 shows some of the student’s results. Table 1.1 load / N length of spring / cm extension / cm 0 12.0 0 1.0 13.3 1.3 2.0 14.8 Calculate the extension when the load is 2.0 N and complete the table. [1]

3 0652/21/O/N/14 © UCLES 2014 [Turn over (b) The student takes three more sets of readings and draws the best-fit line in Fig. 1.2. 0 1.0 2.0 3.0 4.0 5.0 6.0 4.0 2.0 0 extension / cm load / N Fig. 1.2 (i) Using your answer to part (a), plot the point on the graph for a load of 2.0 N. [1] (ii) State the relationship between the load and the extension shown by the best-fit line. … …[1] (c) Fig. 1.3 shows a rectangular block of mass 63 g and dimensions 3.0 cm by 6.0 cm by 2.5 cm. 2.5 cm 3.0 cm 6.0 cm Fig. 1.3 (i) Calculate the volume of the block. volume = … cm3 [1] (ii) Calculate the density of the block and state the unit. density = … unit … [2]

4 0652/21/O/N/14 © UCLES 2014 2 Copper(II) oxide is added to dilute sulfuric acid until there is no further reaction. The mixture is filtered to obtain a blue solution (filtrate). (a) Describe how the positive metal ions in this blue solution can be identified. reagent … result … …[2] (b) Explain how dry crystals of a blue solid can be obtained from this blue solution. … … … …[3] (c) Name this blue solid. …[1]

5 0652/21/O/N/14 © UCLES 2014 [Turn over 3 The burning of hydrogen is a reaction which gives out heat energy. (a) State the term used to describe reactions which give out heat energy. …[1] (b) Write a balanced equation for the burning of hydrogen in air. …[2] (c) (i) State which bonds are broken and which are formed during this reaction. bonds broken … … bonds formed … … [3] (ii) Energy is taken in to break chemical bonds. Energy is released when chemical bonds are formed. Suggest how a chemical reaction can result in an overall release of energy. … … …[1]

6 0652/21/O/N/14 © UCLES 2014 4 Fig. 4.1 shows a bimetallic strip made from copper and an alloy called invar. copper invar Fig. 4.1 (a) Explain what is meant by an alloy. … …[1] (b) When the strip is heated it bends as shown in Fig. 4.2. copper invar Fig. 4.2 Explain why the strip bends in the direction shown in Fig. 4.2. … … …[2]

7 0652/21/O/N/14 © UCLES 2014 [Turn over (c) Fig. 4.3 shows the bimetallic strip used as part of a thermostat switch in an electric oven. heater contacts bimetal strip clamp power supply Fig. 4.3 Explain what happens when the temperature reaches the level set. … … …[2]

8 0652/21/O/N/14 © UCLES 2014 5 Reacting limestone with hydrochloric acid produces carbon dioxide. (a) Complete Fig. 5.1 to show how the carbon dioxide could be collected and its volume measured. [2] limestone hydrochloric acid Fig. 5.1 (b) The main component of limestone is calcium carbonate, CaCO3. Use its formula to show that calcium carbonate contains 12% of carbon by mass. [Ar: Ca, 40; C, 12; O, 16] [2]

9 0652/21/O/N/14 © UCLES 2014 [Turn over 6 A teacher demonstrates the properties of waves using a ripple tank. A barrier is placed in the ripple tank. Fig. 6.1 shows a view of the ripple tank from above. ripple tank wavefront barrier vibrator Fig. 6.1 The vibrator produces a series of waves of constant frequency. These waves move towards the barrier. (a) On the diagram, draw an arrow (↔) to show one wavelength. [1] (b) (i) Draw on Fig. 6.1 three wavefronts after they hit the barrier. [3] (ii) Name the property of waves shown by the change in direction of these wavefronts. … [1]

10 0652/21/O/N/14 © UCLES 2014 7 Carbon dioxide gas is much more soluble in water than oxygen gas. Fig. 7.1 shows a candle burning inside a bell jar of air. The bell jar is placed in a trough of water. water bell jar candle floating holder trough Fig. 7.1 As the candle burns the water level rises up inside the bell jar. (a) Explain how burning the candle causes the water level to rise. … … …[2] (b) After several minutes the candle stops burning. Name the main gas in the bell jar after the candle has stopped burning. …[1] (c) Candles are made from wax which is a compound of carbon. Explain why it can be dangerous to burn wax in a limited supply of air. … … …[2]

11 0652/21/O/N/14 © UCLES 2014 [Turn over 8 Sodium is a member of Group I of the Periodic Table. (a) State two observations made when sodium reacts with water. 1 … 2 …[2] (b) Name two other members of Group l, one which is more reactive than sodium and one which is less reactive than sodium. one which is more reactive than sodium … one which is less reactive than sodium …[2] (c) Name a metal and a non-metal in the same period as sodium. metal … non-metal …[2] (d) Sodium reacts with chlorine to form sodium chloride, an ionic compound. Draw a diagram to show the electron arrangement of the ions present in sodium chloride. Show all of the electrons in each ion. Label your diagram with the names of the ions. [3]

12 0652/21/O/N/14 © UCLES 2014 9 Fig. 9.1 shows a circuit with a lamp and a cell in series. Fig. 9.1 (a) Fig. 9.2 shows four more circuits. The cells and lamps are identical to those in Fig. 9.1. (i) Compared with the lamp in Fig. 9.1, state under each diagram whether each lamp in the circuit is brighter, less bright, as bright, not lit. 1 … 2 … 3 … 4 … [4] Fig. 9.2

13 0652/21/O/N/14 © UCLES 2014 [Turn over (ii) State in which circuit in Fig. 9.2 the cell(s) stop working the most quickly. Explain your answer. circuit … explanation … …[2] (b) A student wishes to measure the current from the cell in circuit 4. (i) Name the instrument used to measure current. …[1] (ii) In the box below, redraw circuit 4 to include the measuring instrument. [3]

14 0652/21/O/N/14 © UCLES 2014 10 Fig. 10.1 shows an iron rod with a coil of wire wrapped around it. The coil is attached to a power supply. A mixture of small pieces of different types of metal are on the bench near the iron rod. iron rod pieces of metal switch S power supply + – Fig. 10.1 (a) (i) State what happens to the iron rod when switch S is closed. …[1] When switch S is closed, some of the pieces of metal are attracted to the iron rod and stick to it. The other pieces of metal stay on the bench. (ii) Explain why some of the pieces of metal are attracted to the iron rod and some are not attracted. … … …[2]

15 0652/21/O/N/14 © UCLES 2014 [Turn over (b) In a separate experiment, a magnet is used to pick up two metal pins as shown in Fig. 10.2. N S magnet Fig. 10.2 The pins hang at an angle to each other. Explain why the pins do not hang vertically. … … … …[3]

16 0652/21/O/N/14 © UCLES 2014 11 Carbon-12, 12 6C, and carbon-14, 14 6C, are isotopes of carbon. (a) Complete Table 11.1 to show the number of protons, electrons and neutrons in atoms of carbon-12 and carbon-14. Table 11.1 isotope protons electrons neutrons carbon-12 12 6C … … … carbon-14 14 6C … … … [2] (b) Ethane and ethene are hydrocarbons. They each contain two carbon atoms per molecule. (i) Complete Fig. 11.1 to show the structural formulae of ethane and ethene. C C ethane C C ethene [3] Fig. 11.1 (ii) Describe a chemical test to distinguish between ethane and ethene. test … result with ethane … result with ethene …[3] (iii) State one use of ethene. …[1]

17 0652/21/O/N/14 © UCLES 2014 [Turn over 12 Fig. 12.1 shows a cathode ray tube. There is an electric field between the charged plates. The cathode rays are deflected by this electric field. + + + + + + + – – – – – – – + – path of cathode rays charged plates 200 V Fig. 12.1 (a) Describe the evidence which suggests that the particles which make up cathode rays are negatively charged. … … …[2] (b) Name the type of particle which forms cathode rays. … [1]

18 0652/21/O/N/14 © UCLES 2014 13 A student measures the half-life of a radioactive isotope. She records the results and draws the graph in Fig. 13.1. 1000 800 600 400 200 0 activity / Bq 50 40 30 20 10 0 time / min Fig. 13.1 (a) The points are not exactly on a smooth curve. State the property of radioactive decay which causes this scatter. … …[1] (b) Use the graph to determine the half life of the isotope. Show clearly on the graph in Fig. 13.1, how you obtained this value. half-life = … min [2]

19 0652/21/O/N/14 © UCLES 2014 (c) The isotope decays by emitting an α-particle (alpha-particle). Describe the nature of an α-particle. … … …[2]

20 0652/21/O/N/14 © UCLES 2014 Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the publisher will be pleased to make amends at the earliest possible opportunity. Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. Group 140 Ce Cerium 58 141 Pr Praseodymium 59 144 Nd Neodymium 60 Pm Promethium 61 150 Sm Samarium 62 152 Eu Europium 63 157 Gd Gadolinium 64 159 Tb Terbium 65 162 Dy Dysprosium 66 165 Ho Holmium 67 167 Er Erbium 68 169 Tm Thulium 69 173 Yb Ytterbium 70 175 Lu Lutetium 71 232 Th Thorium 90 Pa Protactinium 91 238 U Uranium 92 Np Neptunium 93 Pu Plutonium 94 Am Americium 95 Cm Curium 96 Bk Berkelium 97 Cf Californium 98 Es Einsteinium 99 Fm Fermium 100 Md Mendelevium 101 No Nobelium 102 Lr Lawrencium 103 1 H Hydrogen 1 7 Li Lithium 3 23 Na Sodium 11 24 Mg Magnesium 12 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 64 Cu Copper 29 65 Zn Zinc 30 70 Ga Gallium 31 27 Al Aluminium 13 11 B Boron 5 12 C Carbon 6 14 N Nitrogen 7 16 O Oxygen 8 19 F Fluorine 9 28 Si Silicon 14 31 P Phosphorus 15 32 S Sulfur 16 35.5 Cl Chlorine 17 40 Ar Argon 18 20 Ne Neon 10 4 He Helium 2 73 Ge Germanium 32 75 As Arsenic 33 79 Se Selenium 34 80 Br Bromine 35 84 Kr Krypton 36 39 K Potassium 19 88 Sr Strontium 38 89 Y Yttrium 39 91 Zr Zirconium 40 93 Nb Niobium 41 96 Mo Molybdenum 42 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 54 137 Ba Barium 56 139 La Lanthanum 57 * 178 Hf Hafnium 72 181 Ta Tantalum 73 184 W 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 Po Polonium 84 At Astatine 85 Rn Radon 86 Fr Francium 87 227 Ac Actinium 89 9 Be Beryllium 4 I II III IV V VI VII 0 85 Rb Rubidium 37 133 Cs Caesium 55 226 Ra Radium 88 The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.). a X b a = relative atomic mass X = atomic symbol b = proton (atomic) number Key *58-71 Lanthanoid series 90-103 Actinoid series DATA SHEET The Periodic Table of the Elements

® IGCSE is the registered trademark of Cambridge International Examinations. CAMBRIDGE INTERNATIONAL EXAMINATIONS Cambridge International General Certificate of Secondary Education MARK SCHEME for the October/November 2014 series 0652 PHYSICAL SCIENCE 0652/21 Paper 2 (Core Theory), maximum raw mark 80 This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. It shows the basis on which Examiners were instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began, which would have considered the acceptability of alternative answers. Mark schemes should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the October/November 2014 series for most Cambridge IGCSE®, Cambridge International A and AS Level components and some Cambridge O Level components.

Page 2 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0652 21 © Cambridge International Examinations 2014 1 (a) 2.8 (cm) ; [1] (b) (i) point correctly marked to < ½ a square (e.c.f.) ; [1] (ii) extension is proportional to load ; [1] (c) (volume =) 3 × 6 × 2.5 = 45 cm3 ; [1] (i) density = mass/volume / (63 / 45) = 1.4 ; g/cm3 ; [2] [Total: 6] 2 (a) aqueous sodium hydroxide / ammonia ; with sodium hydroxide: blue precipitate insoluble (in excess) ; OR with ammonia: blue precipitate dissolving to deep blue solution ; [max 2] (b) boil / evaporate ; (crystallise and) filter / pour off liquid / wash ; dry in oven / dry with filter paper ; [3] (c) copper sulfate ; [1] [Total: 6] 3 (a) exothermic ; [1] (b) 2H2 + O2 → 2H2O ;; [2] (1 for formulae, 1 for balancing) (c) (i) bonds broken: H – H ; O – O ; bonds made: H – O ; (allow names) [3] (ii) making bonds gives out more energy than that needed to break bonds ; [1] [Total: 7]

Page 3 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0652 21 © Cambridge International Examinations 2014 4 (a) a mixture of two (or more) metals ; [1] (b) metals expand ; copper more than invar ; [2] (copper expands faster than invar, 1 mark max) (c) strip bends away from contact ; breaking the circuit / switching off heater ; [2] [Total: 5] 5 (a) collection over water or in gas syringe ; graduations shown on collection vessel ; [2] (collection by displacement of air – 1 mark only) (b) molar mass of calcium carbonate is 100 ; contains 1 atom / 12 u of carbon (therefore 12%) ; [2] [Total: 4] 6 (a) wavelength correctly marked ; [1] (b) (i) 3 (or more) wavefronts drawn moving slightly left of top centre of the tank ; wavefront direction so angle of incidence = angle of reflection (by eye) ; wavelength constant and equal to incident wave train ; [3] (ii) reflection ; [1] [Total: 5] 7 (a) oxygen used up (by combustion) ; forms carbon dioxide which dissolves (in the water) ; lower pressure ; [max 2] (b) nitrogen ; [1] (c) carbon monoxide formed ; toxic / poisonous / prevents blood carrying oxygen ; [2] [Total: 5]

Page 4 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0652 21 © Cambridge International Examinations 2014 8 (a) fizzes / bubbles formed ; floats ; ‘scoots’ about surface ; [2] (b) potassium / rubidium / caesium / francium ; lithium ; [2] (c) magnesium / aluminium ; silicon / phosphorus / sulfur / chlorine / argon ; [2] (d) 2,8 for sodium ; 2,8,8 for chlorine ; sodium and chloride (NOT chlorine) ; [3] [Total: 9] 9 (a) (i) 1 less bright ; 2 brighter ; 3 not lit ; 4 as bright ; [4] (ii) circuit 4 (accept 2) ; largest current taken from the cells ; [2] (b) (i) ammeter ; [1] (ii) correct symbol for ammeter (if voltmeter is answer in (i) e.c.f. for this mark only) ; circuit copied correctly and meter measuring a current ; ammeter correctly placed to measure current through cells ; [3] [Total: 10] 10 (a) (i) iron rod is magnetised ; [1] (ii) ferromagnetic materials / steel / iron are attracted ; non-(ferro)magnetic materials / not all metals magnetic ; [2] (b) pins become induced magnets ; like poles at the bottom (can be scored from diagram) ; like poles repel ; [3] [Total: 6]

Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2014 0652 21 © Cambridge International Examinations 2014 11 (a) 6, 6, 6 ; 6, 6 8 ; [2] (b) (i) H H H H | | | | H — C — C — H and C = = C | | | | H H H H 6 hydrogens in ethane ; 4 hydrogens in ethane ; single bond in ethane and double bond in ethane ; [3] (ii) bromine / bromine water ; no change with ethane ; decolourises with ethane ; [3] (iii) used to make polythene / plastics / named addition polymer / ethanol ; [1] [Total: 9] 12 (a) deflected by an electric field / attracted / repelled to charged plate ; towards the positive plate / away from negative plate ; [2] (b) electrons ; [1] [Total: 3] 13 (a) any mention of randomness of decay ; [1] (b) clear lines within ± 2.5 minutes of correct answer from the axes showing the points chosen ; 24.5 or 2.5 (min) ; [2] (c) contains 2 protons ; 2 neutrons ; [2] (allow: helium nucleus / He2+ for 2 marks OR helium ion / atom 1 mark max) [Total: 5]