Cambridge IGCSE Physical Science 0652 — 2008 Oct/Nov Paper 2 · Variant 1

This document consists of 14 printed pages and 2 blank pages. IB08 11_0652_02/3RP © UCLES 2008 [Turn over *0350997671* For Examiner's Use 1 2 3 4 5 6 7 8 9 10 11 12 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/02 Paper 2 (Core) October/November 2008 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 2008 0652/02/O/N/08 For Examiner's Use 1 A student investigates the current-voltage characteristic for a lamp. She builds the circuit shown in Fig. 1.1. A Fig. 1.1 (a) Show where the voltmeter should be connected on Fig. 1.1 [2] (b) From her results the graph in Fig. 1.2 is plotted. 0 1.0 2.0 3.0 4.0 5.0 6.0 7.0 potential difference / V current / A 0.50 0.40 0.30 0.20 0.10 0 Fig. 1.2 (i) What is the current when there is a potential difference of 2.0 V across the bulb? [1]

3 © UCLES 2008 0652/02/O/N/08 [Turn over For Examiner's Use (ii) Calculate the resistance of the lamp when the potential difference is 2.0 V. Show your working. resistance = [3] (iii) Use the graph to deduce what happens to the resistance of the lamp as the current is increased above 0.30 A. Suggest a reason for the change. [2] 2 (a) Complete Table 2.1 by writing in the missing formulae and types of bonding. Table 2.1 compound formula type of bonding sodium chloride NaCl ionic methane potassium bromide [4] (b) Give the names and symbols of the ions present in sodium chloride. ion 1 symbol ion 2 symbol [4]

4 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 3 Fig. 3.1 shows a 0.20 kg mass hanging on a spring. 0.20 kg Fig. 3.1 (a) (i) Calculate the weight of the mass. (g = 10 N / kg) Show your working. weight = (ii) Write down the force acting on the mass due to the spring. force = [3] (b) The mass is pulled down a short distance and released. (i) Draw an arrow on Fig. 3.1 and label it F, to show the direction of the resultant force on the mass immediately after it is released. [1] (ii) State what would happen to the mass immediately after it is released. [2]

5 © UCLES 2008 0652/02/O/N/08 [Turn over For Examiner's Use 4 Bromine can be extracted from seawater. The sodium bromide in seawater is reacted with chlorine to displace the bromine. (a) What is the name given to all of the elements in Group 7 of the Periodic Table? [1] (b) How many electrons are in the outer shell of bromine? [1] (c) Write a balanced equation for the displacement reaction between sodium bromide, NaBr, and chlorine, Cl2. [2] (d) Explain why iodine cannot be used to displace bromine from sodium bromide. [2] (e) Give the name, atomic number and relative atomic mass of another element in the same period of the Periodic Table as chlorine. The Periodic Table is printed on page 16. element atomic number relative atomic mass [3]

6 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 5 Fig. 5.1 shows a liquid-in-glass thermometer. 0 10 20 30 40 50 60 70 80 90 100 110 °C Fig. 5.1 (a) (i) Name a suitable liquid to use in the thermometer. [1] (ii) Explain what happens to the liquid when the thermometer is placed in a beaker of hot water. [2] (iii) Name the main process by which energy is transferred from the hot water to the liquid in the thermometer. [1] (b) The thermometer is now placed in pure boiling water. (i) What temperature would the thermometer show? [1] (ii) Explain what is meant by the term boiling. [2]

7 © UCLES 2008 0652/02/O/N/08 [Turn over For Examiner's Use 6 Table 6.1 gives the names and formulae of some organic compounds Table 6.1 name of compound formula methanol CH3OH ethanol C2H5OH propanol butanol C4H9OH pentanol C5H11OH (a) (i) Name the type of organic compounds listed in the table. [1] (ii) What is the name given to a series of compounds like these? [1] (b) Complete the table by writing in the formula for propanol. [1] (c) Draw the structure of ethanol. [1] (d) Give two uses of ethanol. (i) (ii) [2]

8 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 7 (a) Fig. 7.1 shows a ripple tank with three wavefronts approaching an area of shallow water. shallow water Fig. 7.1 (i) On Fig 7.1, draw four more wavefronts to complete the diagram. [3] (ii) Name the process being demonstrated. [1] (b) Fig. 7.2 shows a similar ripple tank, with waves approaching a barrier that reflects water waves. Fig. 7.2 On Fig. 7.2, draw in four more wavefronts to complete the diagram. [3]

9 © UCLES 2008 0652/02/O/N/08 [Turn over For Examiner's Use 8 Small pieces of metallic gold can be found in the gravel at the bottom of streams. Sodium is obtained by the electrolysis of one of its compounds. Iron is extracted by reduction of its ore with carbon in a blast furnace. (a) (i) Put these three metals in order of reactivity. most reactive least reactive [2] (ii) Suggest where you would place carbon in this list? Explain your answer. [2] (b) Name an ore of iron. [1] (c) Stainless steel is a mixture of iron and chromium. (i) What name do we give to mixtures of metals like stainless steel? [1] (ii) Give a use of stainless steel. [1]

10 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 9 (a) A student arranges two magnets so that magnet B balances as in Fig. 9.1. N S magnet A magnet B Fig. 9.1 (i) Label the poles of magnet B [1] (ii) Explain why magnet B can be balanced in this way. [2] (b) The student brings a magnet near to an iron bar. N S Y X iron bar Fig. 9.2 What happens when: The magnet is brought up to end Y? The magnet is brought up to end X? [1] (c) He wraps a length of wire around the iron bar. He connects the wire to a battery so that there is a current in the wire. He repeats the experiment in (b). Explain how you would expect the results to change [2]

11 © UCLES 2008 0652/02/O/N/08 [Turn over For Examiner's Use 10 Fig. 10.1 shows an experiment to measure the volume of oxygen in 100 cm3 of air. Oxygen reacts with iron to form a solid compound. water air iron filings Fig. 10.1 (a) What do we call reactions which involve the addition of oxygen? [1] (b) What type of compound is formed when an element reacts with oxygen? [1] (c) (i) What volume of gas remains in the tube when all the oxygen has reacted? [1] (ii) Name the main gas in the tube after the oxygen has reacted. [1]

12 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 11 The iodine isotope, 131 53 I, decays by emitting a β–particle. (a) Explain what is meant by a β–particle. [2] (b) (i) Complete the equation which describes the decay. I = 131 53 … … … … X + β (ii) Use the Periodic Table, on page 16, to identify the element X and comment on its reactivity. [4]

13 © UCLES 2008 0652/02/O/N/08 For Examiner's Use 12 A sample of copper chloride is made by reacting excess copper carbonate with hydrochloric acid. (a) Balance the equation for this reaction. …..CuCO3 + ….. HCl → ….. CuCl2 + ….. CO2 + ….. H2O [1] (b) (i) Name the gas evolved. [1] (ii) Describe a test for this gas. [2] (c) How could you obtain pure copper chloride crystals from the resulting mixture ? [2]

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 2008 0652/02/O/N/08 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 2008 question paper 0652 PHYSICAL SCIENCE 0652/02 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. 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 2008 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 2008 0652 2 © UCLES 2008 1 (a) (i) voltmeter in parallel with main circuit (1) across the bulb (+1) [2] (b) (i) 0.25A (1) [1] (ii) use of V = IR (1) = 8.0 (1) ohms (give this even if working incorrect) (1) [3] (iii) resistance increases (1) because the filament/bulb gets hot (1) [2] [Total: 8] 2 (a) CH4 covalent [2] KBr ionic [2] (b) sodium Na+ [2] chloride (not chlorine) Cl – [2] [Total: 8] 3 (a) (i) use of weight = mass × g (1) = 2.0 N (1) [2] (ii) 2.0 N OR consistent with (i) (1) [1] (b) (i) arrow vertically upwards (allow without label if clear) (1) [1] (ii) accelerate (1) upwards (1) [2] [Total: 6]

Page 3 Mark Scheme Syllabus Paper IGCSE – October/November 2008 0652 2 © UCLES 2008 4 (a) halogens [1] (b) 7 [1] (c) Cl2 + 2NaBr → Br2 + 2NaCl [2] (formulae – 1 mark: then correct balancing – 1 mark) (d) iodine is less reactive (1) than bromine (1) [2] (accept bromine is more reactive than iodine for both marks) (e) element in period 2 named (not chlorine) (1) corresponding atomic number (1) corresponding relative atomic mass (1) [3] (give these last 2 marks even if the named element is not in the correct period) [Total: 9] 5 (a) (i) mercury/alcohol (not ethanol) [1] (ii) The liquid moves up the capillary tube (1) because it expands (1) [2] (iii) conduction [1] (b) (i) 100 °C (accept 97–101) [1] (ii) change (of state) from liquid to vapour/gas without change in temperature throughout the liquid/forms (vapour) bubbles ANY TWO (1 + 1) [2] [Total: 7]

Page 4 Mark Scheme Syllabus Paper IGCSE – October/November 2008 0652 2 © UCLES 2008 6 (a) (i) alcohols [1] (ii) homologous [1] (b) C3H7OH [1] (c) correct structural formula including hydrogens [1] (d) two correct uses (ANY TWO) e.g. alcoholic drinks fuel solvent etc. (1+1) [2] [Total: 6] 7 (a) (i) waves change direction on entering shallow water (1) refraction correct (1) wavelength in deep water constant AND in shallow water (1) [3] (If only 3 wavefronts drawn max. 2; 2 drawn max. 1) (ii) refraction (1) [1] (b) (i) clear reflected waves (1) angle i = angle r (approx. by eye) (1) wavelength equal throughout (1) [3] (if only 3 wavefronts drawn max. 2; 2 drawn max. 1) [Total: 7] 8 (a) (i) sodium most reactive (1) gold least reactive (1) [2] (ii) between iron and sodium/above iron/below sodium (1) carbon removes oxygen from iron/carbon reduces iron ore/oxide (1) [2] (b) hematite/magnetite/etc. [1] (c) (i) alloy [1] (ii) correct use e.g. cutlery/medical instruments/etc [1] [Total: 7]

Page 5 Mark Scheme Syllabus Paper IGCSE – October/November 2008 0652 2 © UCLES 2008 9 (a) (i) N&S labelled correctly [1] (ii) like poles repel (1) upward force = gravitational force (1) [2] (b) Y attract, X attract (must have both) [1] (c) iron bar would be magnetised (1) one end would now repel (1) [2] [Total: 6] 10 (a) oxidation [1] (b) oxide [1] (c) (i) 79 cm3 (accept 80) [1] (ii) nitrogen [1] [Total: 4] 11 (a) electron (1) fast/energetic/from the nucleus (1) [2] (b) (i) nucleon numbers correct: 131, 0 (1) proton numbers correct: 54, –1 (1) [2] (ii) Xenon (1) Nobel gas/inert (1) [2] [Total: 6] 12 (a) 1 2 1 1 1 (accept correct multiples) [1] (ones may be omitted) (b) (i) carbon dioxide [1] (ii) mention of limewater (1) turns milky/cloudy/white precipitate (1) [2] (must have carbon dioxide to score in this section) (c) filter (1) evaporate/boil/heat (+1) [2] [Total: 6]