Cambridge IGCSE Physical Science 0652 — 2010 Oct/Nov Paper 3 · Variant 1

This document consists of 17 printed pages and 3 blank pages. IB10 11_0652_03/4RP © UCLES 2010 [Turn over *3983879930* For Examiner's Use 1 2 3 4 5 6 7 8 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 (Extended) October/November 2010 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 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 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 1 Fig. 1.1 shows apparatus used to react dilute solutions of sodium hydroxide and sulfuric acid. burette sodium hydroxide flask sulfuric acid Fig. 1.1 (a) Sodium hydroxide is added slowly from the burette to the flask until in it is in excess. (i) Suggest a value for the pH of the acid before any sodium hydroxide solution is added. pH = [1] (ii) Describe the changes in the pH of the liquid in the flask as the sodium hydroxide is added until in excess. [2] (iii) Suggest how you could observe the change in pH. [1] (iv) Write a balanced equation for the reaction that takes place. [2]

3 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (b) During the reaction protons are transferred from one reagent to the other. Identify the source of the protons and explain what is happening. [3]

4 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 2 Fig. 2.1 shows a side view of a shallow pool. A C B movement of the waves Fig 2.1 Some waves move across the surface of the water. (a) (i) Mark on the diagram, between A and B, one wavelength of the waves. [1] (ii) Explain why the wavelength of the waves changes as the waves go across the pool from B to C. [2] (b) The wavelength of the waves between A and B is 12 cm. They move across the pool at a speed of 90 cm/s. Calculate the frequency of these waves. Show your working. frequency [2]

5 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (c) When the pool is perfectly calm, a boy observes that an image of a lamp is formed as shown in Fig. 2.2. boy lamp image Fig. 2.2 (i) On Fig. 2.2, draw a ray from the lamp to the boy’s eye to show how the image is formed. [2] A breeze blows and ripples form. The appearance of the side view of the surface of the pool is shown in Fig. 2.3. boy lamp Fig. 2.3 (ii) Explain why a single image of the lamp is no longer seen. Draw suitable rays on Fig. 2.3 to help with your explanation. [3]

6 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 3 Ethanol can be made by two different processes: • fermentation, • addition of steam to ethene. (a) (i) Describe how ethanol is made by fermentation. [3] (ii) Complete and balance this equation to show the formation of ethanol by fermentation. C6H12O6 → [2] (b) Steam is reacted with ethene according to this equation. C2H4 + H2O → C2H5OH Calculate the volume of ethene, measured at room temperature and pressure, which reacts to produce 1.0 dm3 of ethanol. Ethanol has a density of 0.8 kg/dm3. [Ar: C, 12; H,1; O,16.] [At room temperature and pressure 1 mole of any gas has a volume of 24 dm3.] Show your working. volume of ethene = dm3 [4]

7 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (c) Ethene is made by the cracking of hydrocarbons obtained from crude oil. Describe this process. [3]

8 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 4 Fig. 4.1 shows two conducting spheres. Sphere B is connected to earth through a sensitive ammeter. Sphere A has a very large positive charge on it. When sphere B is brought near to A, a spark jumps between the two spheres and the ammeter needle moves rapidly up the scale and then back to zero. sphere A insulating stand sphere B A safety resistor 50 000 Ω earth Fig. 4.1 (a) (i) Explain why the ammeter needle moves. [2] (ii) Describe the energy changes that occur when the spark jumps between the two spheres. [3] (b) (i) The average current through the ammeter is 0.0012 mA. Calculate the average potential difference across the safety resistor. potential difference = [2]

9 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (ii) The current lasts for 1.5 ms. Calculate the charge which flows through the ammeter. charge = [2] (iii) Calculate the energy transferred in the resistor. energy = [2]

10 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 5 Table 5.1 shows the elements in a period of the Periodic Table. Table 5.1 group I II III IV V VI VII element Li Be B C N O F (a) Describe the relationship between group number and the number of outer shell electrons in the atoms of these seven elements. [1] (b) Describe how the character of the elements changes from left to right across these seven elements. [1] (c) Lithium forms an ion Li+. Oxygen forms an ion O2−. (i) What is the formula for the ionic compound lithium oxide? [1] (ii) Describe, in terms of electrons, how lithium and oxygen atoms form the compound lithium oxide. [3]

11 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (d) In the box below, draw a diagram to show the arrangement of all electrons in a molecule of nitrogen. [3]

12 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 6 Jane is given a radioactive source. She finds out what type or types of radiation it emits. (a) Describe one safety precaution she must take when using the source. [1] (b) She sets up a GM-tube and finds there is a count of 12 in one minute with no source present. State why there is a count with no source present. [1] (c) She places the source a few centimetres from the GM-tube. Table 6.1 shows the results she obtains using different absorbers between the GM-tube and the source. Table 6.1 absorber reading 1 / counts per minute reading 2 / counts per minute reading 3 / counts per minute none 4352 4429 4388 thin card 1265 1321 1272 2 mm aluminium 1269 1247 1285 4 cm lead 33 45 37 (i) Explain why, when there is no absorber present, the readings vary. [1]

13 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (ii) Complete Table 6.2 and indicate whether each of the three types of radiation are present or absent. Use the evidence from Table 6.1 to explain the presence or absence of each of the three types of radiation. Table 6.2 type of radiation present (✓) absent () reason alpha beta gamma [4] (d) In a research project a small amount of an alpha emitting isotope is injected into a cancerous tumour in a mouse. (i) Suggest why alpha radiation might be especially effective at destroying tumours. [2] (ii) Explain why a beam of alpha particles is not aimed at the tumour from outside the body of the mouse. [2]

14 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 7 Fig. 7.1 shows a blast furnace producing iron from iron ore. gas outlet iron ore, coke and limestone brick lining 1000 °C 2000 °C 1500 °C hot air molten slag molten iron Fig. 7.1 In the blast furnace iron(III) oxide is reduced by carbon monoxide to produce iron metal. Fe2O3 + 3CO → 2Fe + 3CO2 (a) Carbon monoxide is formed from coke in two stages in the blast furnace. (i) Describe the two stages to show how carbon monoxide is formed in the blast furnace. stage 1 stage 2 [2] (ii) Write balanced equations for the two stages that are involved in this formation of carbon monoxide. stage 1 stage 2 [2]

15 © UCLES 2010 0652/03/O/N/10 [Turn over For Examiner's Use (b) A blast furnace produces 60 000 tonnes of iron per week. Calculate the mass of iron(III) oxide used to produce this iron. [Ar: Fe, 56; O,16.] mass = tonnes [3] (c) Mild steel and stainless steel are two alloys of iron. (i) How are alloys of iron produced? [1] (ii) Give a reason for producing alloys of iron. [1] (d) Aluminium ore contains aluminium oxide, Al2O3. Why is aluminium not extracted from this ore using a blast furnace? [1]

16 © UCLES 2010 0652/03/O/N/10 For Examiner's Use 8 A student measures the density of an irregularly shaped stone. (a) (i) Name two pieces of apparatus he might use. 1. 2. [2] (ii) State the measurements he makes. [2] (iii) Explain how he uses his results to find the density of the stone. [2] (b) A beaker contains 280 g of sea water, which has a density of 1.12 g/cm3. Calculate the volume of sea water in the beaker. volume = cm3 [2]

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20 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 2010 0652/03/O/N/10 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

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the October/November 2010 question paper for the guidance of teachers 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, which would have considered the acceptability of alternative answers. 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 2010 question papers for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses.

Page 2 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0652 03 © UCLES 2010 1 (a) (i) any value below 7 ; [1] (ii) pH rises ; (ecf from (i)) to above 7 / stated value above 7 ; [2] (iii) use the universal indicator / pH meter ; (not litmus or just indicator) [1] (iv) H2SO4 + 2NaOH → Na2SO4 + 2H2O ;; (one mark for all formulae correct, one mark for balance if formulae correct) [2] (b) proton source is (sulfuric) acid ; base is proton acceptor ; H+ / H ion & OH– / O ion form H2O / water ; [3] [Total: 9] 2 (a) (i) wavelength marked correctly ; [1] (ii) depth decreases ; so speed reduces ; [2] (b) use of v = fλ ; F = 7.5 Hz ; [2] (c) (i) ray from lamp to boy’s eye reflecting off water, i = r ; traced back to the lamp ; [2] (ii) ray drawn from lamp to boy’s eye, i ¸ r ; second ray drawn from lamp to boy’s eye, i ¸ r ; explanation such as diffuse reflection* ; (*an outstanding explanation which shows real understanding, could score 2 marks if only 1 mark is scored in the diagram) [3] [Total: 10]

Page 3 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0652 03 © UCLES 2010 3 (a) (i) sugar / named carbohydrate source e.g. grapes / starch / bread ; mixed with yeast ; kept warm / at 35 °C at correct temperature ; [3] (ii) C6H12O6 → 2C2H5OH + 2CO2 ;; (one mark for all formulae correct, one mark for balance if formulae correct) [2] (b) C2H5OH = 46 ;; 0.8 / 46 ; = 417 (accept 420 / 417.3 / 417.4) ; [4] (c) any three from: long chain hydrocarbons / alkanes broken down ; to form short chain hydrocarbons / alkanes and alkenes ; using heat ; and a catalyst ; (if distillation is discussed zero marks are scored) [max 3] [Total: 12] 4 (a) (i) charge moves from A to B / or electrons move from B to A / A discharges through B ; current is a movement of charge / current to Earth through ammeter ; (reject current in the first part) [2] (ii) electrical (potential) energy ; goes to thermal / heat energy / light energy ; and sound energy ; (any mention of kinetic energy only the first mark can be scored) [3] (b) (i) use of V = IR = (0.0012 × 10–3 × 50 000) ; 60 mV, 0.060 V ; [2] (ii) use of q = It (= 0.0012 × 10–3 × 1.5 × 10–3 ; 1.8 × 10–9 C ; [2] (iii) use of E = VQ or VIt (= 0.0012 × 10–3 × 1.5 × 10–3 × 0.06) ; 1.08 × 10–10 J ; [2] [Total: 11]

Page 4 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0652 03 © UCLES 2010 5 (a) group number is the same as the number of electrons in the outer shell ; [1] (b) changes from metallic to non-metallic / metallic to covalent ; [1] (c) (i) Li2O ; [1] (ii) electron(s) transferred ; from (outer shell of) lithium atom to (outer shell) of oxygen atom ; from two lithium atoms transfer one electron each to one oxygen atom ; (accept a clearly labelled diagram) (reference to covalent bonding no marks) [3] (d) diagram showing two nitrogen atoms with at least one shared pair of electrons ; three shared pairs of electrons in total, with no other electrons in outer shell ; inner shell with two electrons ; [3] [Total: 9] 6 (a) use of tongs / forceps / protective clothing / gloves / lead shielding / not point source ; (reject exposure time / goggles / storing in lead) [max 1] (b) background radiation or very clear source ; [1] (c) (i) random variation of emissions ; [1] (ii) alpha
beta  gamma
; alpha – significant change with thin card ; beta – no significant change with aluminium ; gamma – significant penetration through lead / reading above background ; (the answer must refer to the experiment not general properties and the explanation cannot be given the mark unless the presence / absence is correct) [4] (d) (i) very highly ionising ; high chance of collision with cancerous cells ; [2] (ii) alpha very short range ; would not reach tumour / would damage healthy cells on the way ; [2] [Total: 11]

Page 5 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0652 03 © UCLES 2010 7 (a) (i) carbon / coke is burned to make carbon dioxide ; carbon dioxide is reduced by more carbon / coke to carbon monoxide ; (one mark only for carbon / coke reacts with oxygen to form carbon monoxide) [2] (ii) C + O2 → CO2 ; CO2 + CO → 2CO ; (one mark only for 2C + O2 → 2CO) [2] (b) 112 (tonnes iron produced) or 160 tonnes iron(III) oxide ; 160 / 112 or 60 000 / 112 ; = 85 714 tonnes ; (treat use of wrong formula as an arithmetic error so first mark only is lost) [1] (c) (i) by using additives / by adding other metals / by adding other elements ; [1] (ii) to change / improve properties / to make harder / to prevent rusting / stronger ; [1] (d) aluminium is more reactive than carbon / carbon will not reduce aluminium oxide ; [1] [Total: 10] 8 (a) (i) balance (accept scale(s) / measuring scales) ; measuring cylinder (reject beaker) ; [2] (ii) volume of water in cylinder (v1) AND volume of water plus stone (v2) ; mass of stone (m) ; [2] (iii) v2 – v1 ; divide mass by volume ; [2] (b) use of density = mass / volume = 1.12 = 280 / v ; 250 (cm3) ; [2] [Total: 8]