Cambridge IGCSE Physical Science 0652 — 2004 Oct/Nov Paper 3 · Variant 1

This document consists of 15 printed pages and 1 blank page. SP (NF/GR) S65911/3 © UCLES 2004 [Turn over UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 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 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 16. 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 Total www.XtremePapers.com

2 0652/03/O/N/04 Answer all the questions. Write your answers in the spaces provided. 1 Element X burns in excess air to form the oxide XO2. This oxide dissolves in water to form an acid H2XO3. The two reactions are represented by the following equations. X + O2 = XO2 XO2 + H2O = H2XO3 (a) (i) The relative atomic mass, Ar, of element X is 32. Calculate the number of moles in 4.8 g of X. number of moles = …[2] (ii) How many moles of oxygen gas are required to react completely with 4.8 g of X? number of moles of oxygen = …[1] (iii) How many moles of H2XO3 would be formed if all the XO2 formed was dissolved in water? number of moles H2XO3 = …[1] (iv) Calculate the mass of H2XO3 formed. mass of H2XO3 formed = …[2] For Examiner’s Use © UCLES 2004

3 0652/03/O/N/04 [Turn over (b) The acid H2XO3 reacts with aqueous sodium hydroxide to form a salt and water. Complete the following equation which represents this reaction: H2XO3 + 2NaOH = …+… [2] (c) Suggest the identity of element X, stating your reason. X is … because …[1] For Examiner’s Use © UCLES 2004

4 0652/03/O/N/04 2 Fig. 2.1 shows three situations in which forces act on a book. Fig. 2.1 A shows the book resting on a bench. B shows the book being dragged horizontally for a distance of 0.3 m by a net pulling force of 11 N. C shows the book being lifted through a vertical distance of 0.5 m. In B and C the movement takes place over a period of 0.7 s. Calculate the work done and the power used in each case. Show any working that you do and write down any equations that you use. Case A work done = … power used = … [2] Case B work done = … power used = … [3] Case C work done = … power used = … [3] For Examiner’s Use © UCLES 2004 16 N 16 N 11 N 19 N 16 N 16 N A B C 16 N

5 0652/03/O/N/04 [Turn over 3 Use the Periodic Table on page 16 to help you answer the following questions. (a) Use your knowledge of the trends across Period 3 (sodium to argon) to deduce which of these elements (i) is the metal with the lowest melting point, …[1] (ii) is a covalent macromolecule, …[1] (iii) has four electrons in the outer shell of one atom, …[1] (iv) forms an ion with a charge of –2, …[1] (v) is a reactive gas at room temperature. …[1] (b) The boiling point of argon is 87 K. Explain what this very low boiling point suggests about the forces between argon atoms. … … … …[2] (c) Suggest why sodium is a more reactive metal than aluminium. … … … …[2] For Examiner’s Use © UCLES 2004

6 0652/03/O/N/04 4 Fig. 4.1 shows a block of a thermal conductor that is being heated at the left edge. The block is painted silver. Fig. 4.1 (a) With the aid of a diagram explain how heat is transferred along the block. … … … … … …[4] heat thermometers block For Examiner’s Use © UCLES 2004

7 0652/03/O/N/04 [Turn over (b) When the two thermometers show constant temperatures the block is said to be in thermal equilibrium. The block is still being heated. Explain why the block reaches thermal equilibrium. … … … … … …[3] (c) Suggest and explain what difference painting the block a dull black colour would make. … … … … … …[3] For Examiner’s Use © UCLES 2004

8 0652/03/O/N/04 5 (a) (i) Draw the arrangements of the electrons in shells for an atom of carbon and an atom of oxygen. You may wish to refer to the Periodic Table on page 16. electron arrangement of carbon electron arrangement of oxygen [2] (ii) Draw a dot-cross diagram to show how bonds are formed between carbon and oxygen in carbon dioxide. [2] (iii) By referring to your diagram, explain why carbon dioxide is relatively unreactive. … … … …[2] For Examiner’s Use © UCLES 2004

9 0652/03/O/N/04 [Turn over (b) Magnesium oxide has a similar relative formula mass to carbon dioxide, but magnesium oxide is a very high melting point solid. Explain this difference in terms of the structures of the two oxides. … … … …[2] For Examiner’s Use © UCLES 2004

10 0652/03/O/N/04 6 Fig. 6.1 shows how the ripples in a pond spread out as they pass through a gap between two concrete pillars. Fig. 6.1 (a) Name the process by which the waves spread out after passing through the gap between the pillars. …[1] (b) Mark on the diagram the wavelength of the waves. [1] (c) The diagram is drawn
  th full size. The frequency of the waves is 3 Hz. Calculate the speed of the waves. Show all your working and write down any equation that you use. wave speed = … [3] wave fronts concrete pillars For Examiner’s Use © UCLES 2004

11 0652/03/O/N/04 [Turn over (d) Explain how you would use the pond and any other necessary apparatus to demonstrate (i) reflection and (ii) refraction of waves. In each case draw a diagram to help your explanation. reflection … … … … …[3] refraction … … … … …[3] For Examiner’s Use © UCLES 2004

12 0652/03/O/N/04 7 (a) A number of pollutants may be found in car exhaust gases. Explain how the following pollutants are formed: (i) oxides of nitrogen …[2] … (ii) carbon monoxide … …[1] (b) Name one other pollutant formed in car exhaust gases. …[1] (c) Explain how nitrogen oxides in the atmosphere can cause damage to limestone buildings. … … … …[2] (d) Both nitrogen monoxide, NO, and carbon monoxide, CO, can be removed from exhaust fumes by using a catalyst to make them react together. The products are carbon dioxide and nitrogen. Write a balanced equation for this reaction. …[2] 8 Fig. 8.1 shows a transformer. The output is connected to a lamp rated at 6 V, 1.8 W and the input is connected to a 220 V supply. Fig. 8.1 (a) (i) Name the type of transformer used. …[1] 220 V 6 V, 1.8 W For Examiner’s Use © UCLES 2004

13 0652/03/O/N/04 [Turn over (ii) Calculate the ratio of the number of turns on the secondary to the number of turns on the primary. Write down the equation that you use and show your working. turns ratio = … [2] (b) (i) Calculate the normal working current for the lamp. Write down the equation that you use and show your working. current = … [3] (ii) Calculate the working resistance of the lamp. Write down the equation that you use and show your working. resistance = … [2] (iii) Explain why the initial current for the lamp is likely to be higher than the normal working current. … … … … … …[3] For Examiner’s Use © UCLES 2004

14 0652/03/O/N/04 9 The salt lead(II) chloride is insoluble in cold water, whereas the salt lead(II) nitrate is soluble. (a) Lead(II) chloride is to be prepared from a solution of lead(II) nitrate. (i) What other solution should be added to the solution of lead(II) nitrate? …[1] (ii) How would you decide when to stop adding this solution? …[1] (iii) How would you separate a sample of lead(II) chloride from the mixture? … … …[2] (b) Draw a labelled diagram of the apparatus to carry out the separation described in (a)(iii). [2] For Examiner’s Use © UCLES 2004

15 0652/03/O/N/04 BLANK PAGE 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.

16 0652/03/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 0652/03 Paper 3 (Extended), 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 3 80 43 31 19 14 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: 0652/03 PHYSICAL SCIENCE Paper 3 (Extended)

Page 1 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 3 © University of Cambridge Local Examinations Syndicate 2005 Question1 (a) (i) ratio 4.8/32 seen or else molar mass of X = 32 g 1 0.15 (no unit penalty) 1 (ii) 0.15 1 (iii) 0.15 1 (iv) relative molecular mass = 82 1 mass formed = 12.3 g (unit penalty) 1 (b) Na2XO3 + 2H2O both formulae correct 1 balanced 1 (c) X is sulphur (or S) because it has a relative atomic mass of 32 1 [9] Question 2 case A zero 1 zero 1 case B 3.3 J 1 4.7 W 1 case C 1.5 J 1 2.1(4) W 1 equations W = F s and P = W/t score two when seen anywhere 2 [8]

Page 2 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 3 © University of Cambridge Local Examinations Syndicate 2005 Question 3 (a) (i) Na 1 (ii) Si 1 (iii) Si 1 (iv) S 1 (v) Cl 1 (b) weak (attractive) forces 1 little energy needed to separate particles 1 (c) sodium has 1 electron in outer shell, aluminium has 3 1 attraction between electron and nucleus is weaker for sodium 1 Or single electron lost more easily Or comment about extra protons in nucleus of Al meaning stronger force [9] Question 4 (a) diagram showing vibrating molecules 1 mention of vibration 1 mention of molecular collisions 1 mention of kinetic/potential/vibrational energy passed from molecule to molecule 1 mention of conduction 1 Max 4 (b) strip loses heat 1 to surroundings 1 when heat received = heat given out thermal equilibrium established 1 (c) temperatures would be lower/strip cooler 1 more heat given out (per unit time) 1 black better radiator of energy (thermal radiation/i.r.) 1 [10]

Page 3 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 3 © University of Cambridge Local Examinations Syndicate 2005 Question 5 (a) (i) carbon – two shells with 2.4 pattern 1 oxygen – two shells with 2.6 pattern 1 (ii) two double bonds between carbon and oxygen 1 8 electrons around each symbol 1 (iii) double bonds need more energy to break than single bonds 1 bonds must be broken to start the reaction 1 carbon dioxide contains only double bonds 1 each atom has noble gas configuration 1 Max 2 (b) CO2 – simple covalent with weak forces 1 MgO – ionic lattice with strong forces between ions 1 [compensation CO2 covalent and MgO ionic] reject ionic bond is stronger than covalent bond [8] Question 6 (a) diffraction 1 (b) correct wavelength marked at any point 1 (c) wavelength measured and correctly scaled (0.2 m) 1 c = fλ or substituted values including candidate’s value for λ 1 correct speed with candidate’s value in appropriate units (0.6 m/s) (unit penalty) 1 (d) evidence of use of barrier (either plane or curved) 1 incident and reflected waves seen 1 correct reflection for barrier given (constant λ) 1 evidence of means of changing depth 1 incident and refracted waves shown 1 correct refraction with reduced λ over shallowest water 1 [11]

Page 4 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 3 © University of Cambridge Local Examinations Syndicate 2005 Question 7 (a) (i) reaction between nitrogen and oxygen 1 at high temperature 1 (ii) incomplete combustion (of hydrocarbon fuel) 1 (b) sulphur dioxide or trioxide, “lead”, lead compounds not sulphur or CO2 1 (c) acid rain 1 reacts with buildings/limestone (not corrode) 1 (d) 2NO + 2CO N2 + 2CO2 all formulae correct 1 correct formulae correctly balanced 1 [8] Question 8 (a) (i) step down 1 (ii) Ns/Np = Vs/Vp 1 6/220 or 0.027 (or 220/6, if clearly Np:Ns) 1 (b) (i) P = IV or substituted values 1 0.3 1 A 1 (ii) R=V/I or substituted values 1 20 Ω [or ecf = 6/6(b)(i)] 1 (iii) lamp has lower resistance 1 cold 1 as its temperature rises resistance increases or explanation in terms of electron collisions 1 [11]

Page 5 Mark Scheme Syllabus Paper IGCSE – NOVEMBER 2004 0652 3 © University of Cambridge Local Examinations Syndicate 2005 Question 9 (a) (i) hydrochloric acid or any soluble chloride 1 (ii) no more precipitate (formed on addition) 1 (iii) filter 1 wash residue (not filtrate) with water 1 (b) filter funnel and filter paper seen 1 reasonable diagram with correct labels 1 [6]