Cambridge IGCSE Physical Science 0652 — 2007 Oct/Nov Paper 3 · Variant 1

This document consists of 14 printed pages and 2 blank pages. IB07 11_0652_03/4RP © UCLES 2007 [Turn over *6304641213* For Examiner's Use 1 2 3 4 5 6 7 8 9 10 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 (Extended) October/November 2007 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 a soft pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. A copy of the Periodic Table is printed on page 16. 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. www.XtremePapers.com

2 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 1 Fig. 1.1 shows the speed of a car as it moves along a straight, level track. 0 0.5 1.0 1.5 time / s 2.0 2.5 3.0 20 15 10 5 0 speed m / s Fig. 1.1 (a) During the first 1.5 s the car travels at a constant speed. State the overall force on the car during this period of time. force = [1] (b) Calculate the acceleration of the car between 1.5 s and 3.0 s. acceleration = [3] (c) The mass of the car is 1200 kg. Calculate the braking force on the car between 1.5 s and 3.0 s. force = [2]

3 © UCLES 2007 0652/03/O/N/07 [Turn over For Examiner's Use 2 Fig. 2.1 shows a view from above as a set of ripples move out from a point when a stone is thrown into a pond. edge of the pond wavefronts Fig. 2.1 (a) (i) Mark on Fig. 2.1 one wavelength and label it λ. (ii) A boy counts 12 waves hitting the bank in 5.0 s. Calculate the frequency of the waves. frequency = (iii) The wavelength of the waves is 0.40 m. Calculate the speed at which the waves move. speed = [5] (b) The water is shallower near the bank and the waves slow down. Suggest what effect that this will have on (i) the wavelength of the waves, (ii) the frequency of the waves. [2]

4 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 3 A student reacts the same mass of calcium carbonate with excess of the same hydrochloric acid solution at different temperatures. At each temperature he measures the time taken for all of the calcium carbonate to react. His results are shown in Fig. 3.1. 120 100 80 60 40 20 00 10 20 30 temperature / °C 40 50 60 time for reaction to finish / s Fig. 3.1 (a) (i) Describe the effect of change in temperature on the rate of this reaction. [2] (ii) State two other factors that may affect the rate of a reaction. 1. 2. [2]

5 © UCLES 2007 0652/03/O/N/07 [Turn over For Examiner's Use (b) At a higher temperature the particles have more energy to react. Energy may also be supplied by light. This happens in the process called photosynthesis. (i) Plants use photosynthesis to make glucose. Name the reactants and the other product of photosynthesis. reactants and other product [3] (ii) What enables the energy from sunlight to be absorbed in this process? [1] (iii) The process is speeded up by the presence of an enzyme. What is an enzyme? [2] (c) Energy from light is also used in photography. Photographic film contains the compound silver bromide. When light falls on the film a photochemical reaction takes place. Silver metal is formed, creating a black area on the film. What type of reaction have the silver ions undergone? [1]

6 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 4 Fig. 4.1 shows a ray of light entering a parallel sided glass block. glass block Fig. 4.1 (a) Complete the path of the light through and as it leaves the block. [1] (b) Calculate the value of the angle of refraction if the glass has a refractive index of 1.54 and the angle of incidence is 53.1°. Show your working. angle of refraction = [4]

7 © UCLES 2007 0652/03/O/N/07 [Turn over For Examiner's Use 5 Copper and aluminium are two commonly used metals. (a) Copper is a metal that can be found ‘native’. (i) Explain this meaning of the term native. [1] (ii) Name one other metal that is commonly found native. [1] (iii) Complete Table. 5.1 to show two uses of copper and the properties on which these uses are based. Table 5.1 use of copper property of copper [4] (b) Aluminium is not found native. It is found as a compound. (i) The main ore of aluminium contains the compound aluminium oxide. Name this ore. [1] (ii) Aluminium foil is used for food containers. Aluminium is a fairly reactive metal, but aluminium foil does not react with food. Explain why. [1] (iii) State another use of aluminium, and explain why it is a good metal for this use. use explanation [2]

8 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 6 Fig. 6.1 shows a design for a battery charger, which is made up from a transformer and component P. 240 V input 12 V output iron core P Fig. 6.1 (a) (i) Name component P. (ii) Explain why P is needed in the circuit. [3] (b) Explain how the transformer converts an input voltage into a different output voltage. [4] (c) The primary coil has 1800 turns. Calculate the number of turns in the secondary coil. number of turns = [3] (d) A battery takes 3 hours to charge with an average current of 200 mA. Calculate the total charge delivered. charge = [2]

9 © UCLES 2007 0652/03/O/N/07 [Turn over For Examiner's Use 7 Table 7.1 gives information about some of the elements in Group II of the Periodic Table. Table 7.1 element atomic number formula of oxide melting point in °C reaction with cold water magnesium 12 MgO 649 slow calcium 20 CaO 839 steady strontium 38 SrO 769 rapid barium 56 BaO 725 (a) Three of these elements show a trend in a physical property. (i) Describe this physical trend. [2] (ii) Which element does not fit in with this trend? [1] (b) The elements in Table 7.1 show a trend in a chemical property. Describe this chemical trend. [2] (c) When a small piece of calcium is added to cold water, a steady stream of bubbles is given off. This is hydrogen gas. When the reaction is completed, a test with Universal Indicator shows the water to have a pH of 12. Calcium hydroxide has been formed. (i) Write a balanced symbol equation for the reaction of calcium with cold water. [2] (ii) What does the test with Universal Indicator show about the properties of calcium hydroxide? [1] (iii) What would you see when a small piece of barium is added to cold water? [2]

10 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 8 Fig. 8.1 shows the structure of a cathode ray tube. K A X-plates Y-plates Fig. 8.1 (a) Explain how parts K and A produce cathode rays. [4] (b) Fig. 8.2 shows an experiment to measure the speed of sound. Two microphones are placed 8.0 m apart and connected to a cathode ray oscilloscope. A loudspeaker is placed in front of them. 8.0 m loudspeaker microphones cathode ray oscilloscope Y-input Fig. 8.2 The loudspeaker produces a sharp pulse of sound which is detected by the microphones and displayed on the cathode ray oscilloscope screen.

11 © UCLES 2007 0652/03/O/N/07 [Turn over For Examiner's Use Fig. 8.3 shows the screen in more detail. The time base is set to 5 ms / square. Fig. 8.3 (i) What is the time interval between the pulses received from the two microphones? time = (ii) Calculate the speed of the sound. speed = [3]

12 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 9 Copper(II) oxide reacts with dilute sulphuric acid according to the following equation. CuO + H2SO4 CuSO4 + H2O A student uses this reaction to prepare crystals of copper(II) sulphate. (a) To make sure that the crystals are pure, an excess of copper(II) oxide must be used. (i) Explain why an excess of copper(II) oxide must be used to ensure purity of the crystals. [1] (ii) The student uses 10.0 g of copper(II) oxide and 100 cm3 of 1.0 mol / dm3 sulphuric acid. Show by calculation that the copper(II) oxide is in excess. [Ar : Cu, 64; O,16.] [4] (b) Describe how the student should carry out the preparation to obtain pure, dry crystals of copper(II) sulphate. [4]

13 © UCLES 2007 0652/03/O/N/07 For Examiner's Use 10 Fig. 10.1 shows the apparatus used to identify the radioactive emissions from different isotopes source absorber detector counter Fig. 10.1 Table 10.1 shows the count obtained in 2 minutes from an isotope of the element americium, using different absorbers. Table 10.1 count with no absorber count with paper absorber count with aluminium absorber count with lead absorber 5854 1649 1644 103 State, with reasons, the type or types of radiation emitted by the source. [3]

16 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. University of 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. © UCLES 2007 0652/03/O/N/07 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 Sulphur 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

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the October/November 2007 question paper 0652 PHYSICAL SCIENCE 0652/03 Paper 3 (Extended), 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. All Examiners are instructed that alternative correct answers and unexpected approaches in candidates’ scripts must be given marks that fairly reflect the relevant knowledge and skills demonstrated. Mark schemes must be read in conjunction with the question papers and the report on the examination. • CIE will not enter into discussions or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the October/November 2007 question papers for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses. www.XtremePapers.com

Page 2 Mark Scheme Syllabus Paper IGCSE – October/November 2007 0652 03 © UCLES 2007 1 (a) zero accept good comment re sideways force only 1 [1] (b) use of gradient OR (v2 – v1)/(t2 – t1) OR (3.5 – 20)/(3.0 – 1.5) 1 11.0 m/s2 (do not penalise sig. figs) 1 Recognition of deceleration either by statement or minus sign 1 (c) use of F = ma = 1200 x 11 1 13 200 N 1 [5] [Total: 6] 2 (a) (i) wavelength correctly marked (within 1 mm, by eye) 1 (ii) f = 12/5 1 = 2.4 Hz (or per s) 1 (iii) Speed = f x λ or 2.4 x 0.4 (ecf) 1 = 0.96 m/s 1 [5] (b) (i) gets shorter/smaller (accept wavelengths get closer) 1 (ii) remains the same/no change 1 [2] [Total: 7] 3 (a) (i) increase in rate with increase in temperature or vice versa 2 [2] (increase/decrease in rate without clear reference to temperature 1, incorrect linking – 0) (ii) Any two of: concentration; particle size (accept surface area); catalyst (not accept a named catalyst) ANY 2 [2] (b) (i) water; carbon dioxide; 2 oxygen (accept correct formulae) 1 [3] (ii) chlorophyll (ignore spelling errors) 1 [1] (iii) an organic compound/protein; that catalyses a reaction/is a catalyst 2 [2] (c) reduction/gains electrons/endothermic 1 [1] [Total: 11]

Page 3 Mark Scheme Syllabus Paper IGCSE – October/November 2007 0652 03 © UCLES 2007 4 (a) ray continues and emergent ray parallel to incident ray 1 [1] (b) n = sin i/sin r or variation 1 1.54 = sin 53.1/sin r 1 sin r = 0.519 1 r = 31.3o ignore sig. figs., accept 31 1 [4] (Each stage in the calculation need not be shown, full credit can be scored, for the bare answer.) [Total: 5] 5 (a) (i) not combined with another element/not in a compound/ as the free element/found (in the ground) as a metal 1 (ii) gold/platinum 1 (iii) electrical wiring; good conductor of electricity; cooking utensils; good conductor of heat 4 [6] ornaments, jewellery, coins; can be polished/ malleable, low reactivity roofing; malleable ANY TWO USES 1 +1 ANY TWO RELEVANT PROPERTIES 1 +1 [4] (b) (i) bauxite 1 (ii) aluminium is covered by a layer of oxide; 1 (iii) e.g. aircraft parts; low density window frames/malleable bicycles; low density ANY USE 1 ANY RELEVANT PROPERTY 1 [4] [Total: 10] 6 (a) (i) diode (not rectifier) 1 (ii) produces d.c. (output) 1 from a.c. (input) +1 [3] (b) input current induces a magnetic field in the core 1 field links (through core) to secondary coil 1 current continuously changing so field also changing 1 induces emf/voltage/pd in secondary coil 1 different number of turns on primary and secondary step up/step down V 1 [ANY 4] (c) N1/N2 = V1/V2 or variation 1 N2 = 1800 x 12 /240 1 = 90 1 [3] (d) Use of Q = It OR = 0.2 x 3 x 60 x 60 1 = 2160 C 1 [2] (give 1 mark for 216000C) [Total: 12]

Page 4 Mark Scheme Syllabus Paper IGCSE – October/November 2007 0652 03 © UCLES 2007 7 (a) (i) melting point; 1 decreases with increase in atomic number/down the group +1 (ii) magnesium +1 [3] (b) reactivity (with water); 1 increases with increase in atomic number/down the group +1 [2] (c) (i) Ca + 2H2O → Ca(OH)2 + H2 all formlae correct 1 balanced +1 (ii) (it forms an) alkaline (solution) 1 (iii) bubbles of gas/hydrogen; given off very/more quickly white precipitate/ goes cloudy ANY TWO 2 [5] [Total: 10] 8 (a) K is the cathode/is negative 1 K/cathode hot 1 emits electrons 1 A is anode/ positive 1 accelerates/atracts electrons (not accept accelerates cathode rays) 1 [ANY 4] (b) (i) 25 ms 0.025 s 1 (ii) v = 8.0/2.5 x 10–3 ecf 1 = 320 m/s 1 [3] [Total: 7] 9 (a) (i) otherwise sulphuric acid would be left unreacted (to contaminate the crystals)/ no sulphuric acid left 1 [1] (ii) molar mass of CuO 64 + 16 = 80 (g) 1 10/80 (=0.125) moles of Cu) used 1 0.1 moles of acid used 1 thus more CuO than acid 1 [4] (b) add copper(II) oxide to sulphuric acid (warm and stir); 1 filter off excess copper(II) oxide; 1 evaporate filtrate to small volume; 1 leave to crystallise; 1 filter off crystals; 1 wash with a little cold water and leave to dry 1 [ANY 4] (if ‘filter off excess copper(II) oxide’ step is omitted, maximum 3 marks) [Total: 9]

Page 5 Mark Scheme Syllabus Paper IGCSE – October/November 2007 0652 03 © UCLES 2007 10 (a) alpha and gamma 1 alphas stopped by paper 1 gammas go through aluminium but stopped by lead 1 [3] (If β α, and γ  are given lose first mark, but score last two marks on merit, so long as they refer to the experiment.) [Total: 3]