Cambridge IGCSE Physical Science 0652 — 2004 Oct/Nov Paper 2 · Variant 1

This document consists of 12 printed pages. SP (NF/GR) S63775/2 © UCLES 2004 [Turn over UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/02 Paper 2 October/November 2004 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 in the spaces provided on the Question Paper. 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. Answer all questions. The number of marks is given in brackets [ ] at the end of each question or part question. A copy of the Periodic Table is printed on page 12. Centre Number Candidate Number Name If you have been given a label, look at the details. If any details are incorrect or missing, please fill in your correct details in the space given at the top of this page. Stick your personal label here, if provided. For Examiner’s Use 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 Total www.XtremePapers.com

2 0652/02/O/N/04 1 Fig. 1.1 shows a current carrying coil in a magnetic field. There is a force of 5.0 N on each side of the coil acting as shown. Fig. 1.1 (a) (i) Calculate the moment about the axle produced by the force on the right hand side of the coil. Show your working and state the unit. moment = … (ii) Write down the moment about the axle produced by the force on the left hand side of the coil. … (iii) Calculate the total moment on the axle. moment = … [5] (b) (i) State the effect on the total moment about the axle of increasing the current in the coil. … (ii) State the effect on the total moment about the axle of decreasing the number of turns of wire in the coil. …[2] (c) Name a device or a piece of apparatus which relies on the turning effect on a coil in a magnetic field. …[1] 8.0 cm 5.0 N 5.0 N axle For Examiner’s Use © UCLES 2004

3 0652/02/O/N/04 [Turn over 2 Using a microscope, the small drops of fat in milk can be seen moving about slowly in a random way. (a) Name this type of movement. … [1] (b) Use words from the list below to complete the sentences describing this type of movement. You may use each word once, more than once or not at all. collide combine electrons larger molecules smaller The … of water are moving about quickly. They … with the drops of fat. The drops of fat move slowly because they are much … than the … of water. [4] For Examiner’s Use © UCLES 2004

4 0652/02/O/N/04 3 Fig. 3.1 shows a hot water system for a house. Fig. 3.1 (a) (i) Name the main process by which hot water rises from the boiler to the hot water tank. … (ii) Explain why this process occurs. … …[3] (b) (i) Name the main process by which the energy is transferred through the boiler wall to the water. … (ii) Complete the sentences below, which describe the energy changes as the gas is burnt. When the gas is burnt … energy of the gas is converted into … energy which raises the temperature of the water. The combustion process is an … change. [4] (c) Energy is lost from the hot water tank causing the water to cool. Suggest a way in which this loss could be minimised. …[1] cold water tank gas boiler hot water hot water tank hot water cold water hot tap hot cold For Examiner’s Use © UCLES 2004

5 0652/02/O/N/04 [Turn over 4 A student uses paper chromatography to investigate three substances, X, Y and Z. The result of her experiment in Fig. 4.1 shows three components, P, Q and R. Fig. 4.1 (a) State and explain which substance is a mixture of the other two. … …[2] (b) State and explain which component is most soluble in the solvent. … …[2] R Q P X Y Z start line solvent reaches here substances components For Examiner’s Use © UCLES 2004

6 0652/02/O/N/04 5 Fig. 5.1 Use the information in Fig. 5.1 to describe the structures of (i) graphite, … … …[2] (ii) diamond. … … …[2] 6 (a) (i) Describe how a potassium atom, K, forms a potassium ion. … …[1] (ii) Describe how an iodine atom, I, forms an iodide ion. … …[1] (b) Hence describe how potassium iodide is formed from potassium and iodine. … …[2] graphite diamond For Examiner’s Use © UCLES 2004

7 0652/02/O/N/04 [Turn over 7 Fig. 7.1 shows a circuit being used to light two identical bulbs. Fig. 7.1 Ammeter A1 reads 0.75 A and the potential difference across the two bulbs is 4.5 V. (a) (i) What is the reading on ammeter A2? … A (ii) Calculate the total resistance in the circuit. Show your working and state the unit. resistance = … (iii) What is the resistance of one bulb? resistance = … [5] Fig. 7.2 Fig. 7.2 shows another circuit which could be used to light the two bulbs. Both ammeter A1 and ammeter A2 read 1.5 A. (b) What would ammeter A3 read? … A [1] (c) Explain whether the bulbs would be brighter in the circuit in Fig. 7.1 or Fig. 7.2. … …[2] A1 A3 A2 A1 A2 For Examiner’s Use © UCLES 2004

8 0652/02/O/N/04 8 A saturated hydrocarbon gas is given off from decaying rubbish. (a) One molecule of this hydrocarbon contains one carbon atom and four hydrogen atoms. (i) Write the molecular formula of this hydrocarbon. … [1] (ii) Use the information in the Periodic Table on page 12 to calculate the relative molecular mass, Mr, of this hydrocarbon. Mr = … [1] (b) This gas burns completely in air to form carbon dioxide and water. hydrocarbon gas + oxygen → carbon dioxide + water Construct a balanced chemical equation for this reaction. …[2] 9 (a) Copper oxide heated in hydrogen forms copper and water. Use this example to explain the meaning of reduction. … …[2] (b) State two properties of copper that show this metal is a transition element. 1 … 2 … [2] 10 A student prepares magnesium sulphate by adding pieces of magnesium to dilute sulphuric acid until there is excess magnesium and the reaction stops. (a) Describe how the student can obtain crystals of magnesium sulphate from the mixture of aqueous magnesium sulphate and excess magnesium. … … …[2] (b) Hydrogen is also produced in the first experiment. Describe a test to identify this gas. test … result …[2] For Examiner’s Use © UCLES 2004

9 0652/02/O/N/04 [Turn over 11 Fig. 11.1 shows a beam of light being shone on a pond. Fig. 11.1 (a) (i) Complete the two rays, which mark the edges of the beam of light, to show the path of the beam after it enters the water. (ii) For one of the rays, mark the angle of incidence and label it i. (iii) Name the effect that this experiment demonstrates. … [4] Fig. 11.2 shows the front of a police car. Fig. 11.2 (b) Explain, using appropriate scientific terms, why the car has the mirror writing on the front. … … …[2] torch beam of light pond For Examiner’s Use © UCLES 2004

10 0652/02/O/N/04 12 (a) A student adds aqueous bromine to a colourless solution of potassium iodide. The solution changes colour, showing a reaction has occurred. (i) State the product of this reaction that causes the change of colour. … [1] (ii) In terms of the reactivity of the halogens, explain why there is a reaction in this experiment. … …[1] (b) Another student adds aqueous bromine to a colourless solution of potassium chloride. There is no reaction. In terms of the reactivity of the halogens, explain why there is no reaction in this experiment. … …[1] 13 State and explain the purpose of the two main steps in the purification of the water supply for domestic purposes. step 1 … …[2] step 2 … …[2] For Examiner’s Use © UCLES 2004

11 0652/02/O/N/04 14 (a) Draw the structures of ethane, C2H6, and ethene, C2H4. Show all the atoms and all the bonds. ethane ethene [2] (b) Explain why alkenes, such as ethene, do react with steam whereas alkanes, such as ethane, do not react with steam. … …[2] 15 The isotope 90 38Sr is a radioactive isotope which emits β-particles. (a) (i) Explain what is meant by the term isotope. … …[2] (ii) Explain what a β-particle is. … …[2] (b) (i) Complete the table in Fig. 15.1 which describes the make up of a neutral atom of 90 38Sr. Fig. 15.1 (ii) Which type of particle, listed in Fig. 15.1, is not found in the nucleus of an atom? … [4] (c) Complete the equation below which describes the decay of 90 38Sr. 90 38Sr → … 90Y + … –1β + energy [2] For Examiner’s Use © UCLES 2004 University of Cambridge International Examinations is part of the University of Cambridge Local Examinations Syndicate (UCLES) which is itself a department of the University of Cambridge. Number of protons Number of neutrons Number of electrons

12 0652/02/O/N/04 © UCLES 2004 Group DATA SHEET The Periodic Table of the Elements 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

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the NOVEMBER 2004 question paper 0652 PHYSICAL SCIENCE 0652/02 Paper 2 , maximum raw mark 80 This mark scheme is published as an aid to teachers and students, to indicate the requirements of the examination. It shows the basis on which Examiners were initially instructed to award marks. It does not indicate the details of the discussions that took place at an Examiners’ meeting before marking began. Any substantial changes to the mark scheme that arose from these discussions will be recorded in the published Report on the Examination. 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 discussion or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the November 2004 question papers for most IGCSE and GCE Advanced Level syllabuses. www.XtremePapers.com

Grade thresholds taken for Syllabus 0652 (Physical Science) in the November 2004 examination. minimum mark required for grade: maximum mark available A C E F Component 2 80 n/a 47 34 25 The threshold (minimum mark) for B is set halfway between those for Grades A and C. The threshold (minimum mark) for D is set halfway between those for Grades C and E. The threshold (minimum mark) for G is set as many marks below the F threshold as the E threshold is above it. Grade A* does not exist at the level of an individual component.

November 2004 INTERNATIONAL GCSE MARK SCHEME MAXIMUM MARK: 80 SYLLABUS/COMPONENT: 0652/02 PHYSICAL SCIENCE Paper 2

Page 1 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 2 © University of Cambridge International Examinations 2005 1 (a)(i) Moment = 5 ×8 [1] = 40 Ncm [2] (-1 for incorrect/no unit) (ii) 40 Ncm (ecf) [1] (iii) 80 Ncm (ecf) [1] (b)(i) Increases the moment [1] (ii) Decreases the moment [1] (c) (Electric) motor/ammeter etc. NOT generator/dynamo etc. [1] Total [8] 2 (a) Brownian (motion) [1] (b) molecules [1] collide [1] larger [1] molecules [1] Total [5] 3 (a)(i) Convection [1] (ii) Water expands on heating [2] Becomes less dense ANY TWO Rises (b)(i) Conduction [1] (ii) Chemical [1] Heat/Thermal Internal [1] Exothermic (accept irreversible) [1] (c) Insulating/lagging the tank – DO NOT accept vacuum or paint silver [1] Total [8] 4 (a) Z [1] because this contains P and Q from X and R from Y [1] (b) R [1] because this has travelled furthest with the (moving) solvent or [1] equivalent idea Total [4]

Page 2 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 2 © University of Cambridge International Examinations 2005 5 (i) Graphite √ 3 (covalent) bonds for each atom [2] √ two dimensional structure √ layers ANY TWO √ strong bonds in layer and weak bonds between layers (ii) Diamond √ 4 (covalent) bonds for each atom [2] √ three dimensional structure ANY TWO √ tetrahedral √ all strong bonds For both: NOT properties, NOT uses Total [4] 6 (a)(i) Loss of one (outer) electron [1] (ii) Gain of one (outer) electron [1] (b) Transfer of (one) electron from K to I [1] To form ions that attract each other (K+ and I-) [1] Can be answered mainly by diagram Total [4] 7 (a)(i) 0.75 A [1] (ii) Use of R = V/ I [1] R = 6 [1] ohm [1] (iii) 3 (ohm) (ecf) [1] (b) 3.0 A [1] (c) Fig 7.2 [1] larger current through each bulb (necf) [1] Total [8] 8 (a)(i) CH4 [1] (ii) (12 + 4) 16 (ignore any unit) [1] (b) CH4 + 2O2 → CO2 + 2H2O) (error carried forward) all correct formulae [1] correct balancing [1] Total [4]

Page 3 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 2 © University of Cambridge International Examinations 2005 9 (a) Oxygen is removed [1] from the copper oxide [1] (or in terms of electron exchange) (b) √ high density [2] √ coloured compounds √ high melting point ANY TWO √ can be used as a catalyst (element or in compound) Total [4] 10 (a) Filter (to remove excess magnesium) [1] leave filtrate to crystallise or equivalent [1] (b) Use lighted splint NOT ‘glowing’ splint [1] “pops” (necf) [1] Total [4] 11 (a)(i) One ray correctly deflected towards the normal [1] Second ray correct and consistent (not parallel to first not converging) [1] (ii) Normal drawn and i correctly marked [1] (iii) Refraction [1] (b) Some explanation that the writing will be seen in a mirror [1] Use of the term lateral inversion [1] Total [6] 12 (a)(i) Iodine [1] (ii) Bromine is more reactive than iodine or equivalent [1] (b) Bromine is less reactive than chlorine or equivalent [1] Total [3] 13 Step 1 Filtration [1] to remove mud etc. +[1] Step 2 Chlorination (do not accept boiling) [1] to kill bacteria etc. + [1] (If in wrong order, mark as though in correct order but ignore the first mark scored) Total [4]

Page 4 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 2 © University of Cambridge International Examinations 2005 14 (a) [2] (b) Alkenes have a double (carbon) bond [1] but alkanes have only single bonds (accept but alkanes do not), [1] (Must have the double statement for both marks) Total [4] 15 (a)(i) Nuclides with same number of protons [1] but different number of neutrons + [1] (ii) Electron [1] very fast moving/emitted in radioactive decay + [1] (b)(i) 38 [1] 52 [1] 38 [1] (ii) Electron [1] (c) 39 [1] 0 [1] Total [10]