Cambridge IGCSE Physical Science 0652 — 2011 Oct/Nov Paper 2 · Variant 2

This document consists of 16 printed pages. IB11 11_0652_22/FP © UCLES 2011 [Turn over *4403521531* For Examiner's Use 1 2 3 4 5 6 7 8 9 10 11 12 13 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/22 Paper 2 (Core) October/November 2011 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.

2 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 1 A list of apparatus commonly found in the laboratory is shown below. balance beaker burette spatula thermometer Choose the item from the list which you would use to carry out each of the following actions. (a) weigh 0.5 g of copper(II) carbonate (b) measure 25.0 cm3 of water (c) find the temperature of boiling ethanol (d) react together an acid and an alkali [4] 2 Two cars are being tested on a straight level track. Fig. 2.1 shows the speed-time graphs for the two cars, each of mass 1500 kg. speed m / s car car A car car B 60 40 20 0 0 10 20 30 40 time / s car A car B Fig. 2.1 (a) Determine the maximum speed of car A. maximum speed = m / s [1]

3 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use (b) Describe the motion of car B during the last 2.5 s of the test. [2] (c) Use the graph to determine the distance travelled by car B during the first 10 s of the test. distance = m [2] (d) From 10.0 s to 37.5 s car B is travelling at constant speed in a straight line. (i) State the resultant force on the car during this time. force = [1] (ii) Explain why the car engine must continue to do work during this period. [1] (e) At the beginning of the test both cars accelerate from rest. Explain which car produces the greater accelerating force. [2]

4 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 3 (a) Give an example of an ionic compound and an example of a covalent compound. ionic compound covalent compound [2] (b) Describe two differences in the properties of ionic and covalent compounds. 1 2 [2] (c) Draw a dot and cross diagram to show the electron arrangement in an atom of magnesium. [2]

5 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use 4 (a) Name the main ore of aluminium. [1] (b) Explain why aluminium is not extracted from its ore by heating with carbon. [2]

6 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 5 A student is investigating the melting of fruit flavoured crushed ice. Initially, the temperature of the ice is -10 °C. He measures the temperature every 30 s. Fig. 5.1 shows the apparatus he uses. thermometer stirrer ice bench Fig. 5.1 (a) (i) Explain why the student stirs the crushed ice just before taking each temperature reading. [1] (ii) Suggest why, in the first two minutes of the experiment, the temperature of the ice rises, even though there is no apparent heat source. [2]

7 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use The graph in Fig. 5.2 shows how the temperature of the ice changes with time. 5 0 –5 –10 1 2 3 4 1 2 3 4 temperature / °C time / minutes Fig. 5.2 (b) Determine the temperature at which this sample of ice melts. temperature = °C [1] (c) Explain in terms of the kinetic theory what is happening to the sample from two minutes to four minutes. [2]

8 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 6 (a) Complete Table 6.1 by putting in the missing names, formulae and molar masses. Table 6.1 name formula mass of 1 mole / g H2O hydrogen chloride 36.5 sodium fluoride 42 N2 [4] (b) Give the symbols for the ions in sodium fluoride and the number of protons present in each ion. sodium ion number of protons fluoride ion number of protons [2] 7 The radioactive isotope 105 45 Rh decays by emitting a beta-particle (β-particle). (a) (i) State the number of protons in the nucleus of this isotope. number of protons = [1] (ii) Calculate the number of neutrons in the nucleus. number of neutrons = [1]

9 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use (b) (i) What is a beta-particle? [1] (ii) Describe the changes in the nucleus when a beta-particle is emitted. [2] 8 (a) Give an advantage and a disadvantage of using hydrogen as a fuel for motor vehicles. advantage disadvantage [2] (b) Write a balanced equation for the burning of hydrogen in air. [2] (c) Describe a test for hydrogen and state the expected result. test result [2] (d) The reaction between hydrogen and nitrogen is an important industrial process. (i) Name the gas formed. [1] (ii) Name this industrial process. [1]

10 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 9 A student experiments with a rubber band. She stretches it between two retort stands and notices that it produces a sound when she plucks it. The apparatus is shown in Fig. 9.1. rubber band Fig. 9.1 (a) Explain why the sound is produced. [2] (b) The student sets up a cathode ray oscilloscope and a microphone as shown in Fig. 9.2 to display the sound trace produced by the apparatus in Fig. 9.1. microphone cathode ray oscilloscope Fig. 9.2

11 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use (i) She now plucks the rubber band so that a quieter note of the same frequency is heard. Draw, on Fig. 9.3, the trace that is now seen. [2] Fig. 9.3 (ii) She moves the stands further apart. She plucks the band again. The frequency of the sound now heard is greater than before. Explain what is meant by the term frequency and state the unit used to measure it. unit [2]

12 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 10 Chlorine is in Group VII of the Periodic Table. (a) Name this Group. [1] (b) Name another element in this Group. [1] (c) State one use of chlorine. [1] (d) Name the Group II element which is in the same period as chlorine. [1] (e) Describe how, using chlorine, you can show that a solution contains bromide ions. [2] (f) Write down the number of electrons in a bromine atom and in a bromide ion. bromine atom bromide ion [2]

13 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use 11 Fig. 11.1 shows an electric circuit. The e.m.f. of the battery is 9.0 V. V X R 9.0 V A Fig. 11.1 (a) Name component X. [1] (b) The resistance of resistor R is 12 Ω and the resistance of component X is 8.0 Ω. (i) Calculate the combined resistance of R and X. resistance = Ω [1] (ii) Calculate the current measured by the ammeter. current = [2] (iii) Calculate the reading on the voltmeter. reading = V [2]

14 © UCLES 2011 0652/22/O/N/11 For Examiner's Use 12 Methane and ethane are hydrocarbons. They are members of the same homologous series. (a) Name this homologous series. [1] (b) Give the name and formula of the next member of this series. name formula [2] (c) Explain why ethanol, C2H5OH, is not a hydrocarbon. [2]

15 © UCLES 2011 0652/22/O/N/11 [Turn over For Examiner's Use 13 (a) Fig. 13.1 shows a stiff copper rod suspended between two magnetic poles. The copper rod is freely hinged at the top. switch N S liquid mercury stiff copper rod metallic hinge Fig. 13.1 (a) Draw, on Fig. 13.1, the magnetic field between the poles. [3] (b) Explain why a current passes through the circuit when the switch is closed. [2] (c) State what will be observed when switch is closed. [2] (d) The connections to the battery are reversed so that the current in the circuit is in the opposite direction. State how the observations change. [1]

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 2011 0652/22/O/N/11 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 2011 question paper for the guidance of teachers 0652 PHYSICAL SCIENCE 0652/22 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, 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. • Cambridge will not enter into discussions or correspondence in connection with these mark schemes. Cambridge is publishing the mark schemes for the October/November 2011 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 2011 0652 22 © University of Cambridge International Examinations 2011 1 (a) balance ; [1] (b) burette ; [1] (c) thermometer ; [1] (d) beaker OR burette ; [1] [Total: 4] 2 (a) 50 (m / s) ; [1] (b) deceleration ; constant ; [2] (c) use of area under graph, S = ½ × 30 × 10 ; 150 (m) ; [2] (calculation 30 × 10 = 300 m – max 1) (d) (i) zero ; [1] (ii) mention of frictional force ; [1] (e) car A ; larger gradient ; greater acceleration ; [max 2] [Total: 9]

Page 3 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 22 © University of Cambridge International Examinations 2011 3 (a) suitable example of ionic compound e.g. sodium chloride ; suitable example of covalent compound e.g. ammonia ; [2] (b) suitable example for ionic compound ; e.g. conduct electricity when molten or in aqueous solution / giant ionic structure / high melting and boiling points / etc. suitable example for covalent compound ; e.g. does not conduct electricity when molten / simple molecular structure / low melting and boiling points / etc. [2] (c) diagram showing 2 electrons in outer shell ; 3 shells with 2 electrons in first shell and 8 in middle shell ; [2] [Total: 6] 4 (a) bauxite ; [1] (b) aluminium too reactive ; more reactive than carbon / carbon not reactive enough / will not replace carbon ; [2] [Total: 3] 5 (a) (i) so that the mean temperature of the ice is measured ; [1] (ii) sample is below room temperature ; so absorbs energy from the surroundings ; [2] (b) – 2(°C) ; [1] (c) temperature remains constant / ice melting ; molecules gain potential energy / bonds are broken ; [2] [Total: 6]

Page 4 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 22 © University of Cambridge International Examinations 2011 6 (a) name formula mass of 1 mole / g water H2O 18 ; hydrogen chloride HCl 36.5 ; sodium fluoride NaF 42 ; nitrogen N2 28 ; [4] (b) Na+ AND 11 ; F– AND 9 ; [2] [Total: 6] 7 (a) (i) 45 ; [1] (ii) 60 ; [1] (b) (i) (a fast moving) electron ; [1] (ii) loses 1 neutron ; gains proton ; (‘neutron changes to proton’ gains 2 marks) [2] [Total: 5] 8 (a) suitable advantage, e.g. no pollution, etc. ; suitable disadvantage, e.g. needs to be made, etc. ; [2] (b) 2H2 + O2 → 2H2O ;; [2] (correct formulae – 1 mark and correct balancing – 1 mark) (c) lighted splint ; pops ; [2] (d) (i) ammonia ; [1] (ii) Haber / Haber-Bosch ; [1] [Total: 8]

Page 5 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 22 © University of Cambridge International Examinations 2011 9 (a) the (vibrating) rubber hits air molecules ; causing them to vibrate / forming a sound wave ; [2] (no mention of vibration 1 max.) (b) (i) same frequency (approximately) ; smaller amplitude ; [2] (ii) number of waves (or vibrations) per second ; Hz or hertz ; [2] [Total: 6] 10 (a) halogens ; [1] (b) fluorine / bromine / iodine / astatine ; [1] (c) correct use of chlorine ; [1] e.g. water sterilization / making plastics / etc. (d) magnesium ; [1] (e) bubble chlorine into the solution ; turns brown / yellow ; [2] (f) 35 ; 36 (allow e.c.f. on number in atom, i.e. atom + 1 for a max 1) ; [2] [Table: 8] 11 (a) lamp / bulb ; [1] (b) (i) 20 Ω ; [1] (ii) use of I = V / R (= 9 / 20) ; = 0.45 A ; [2] (iii) use of V = IR (= 0.45 × 12) ; = 5.4 V ; [2] [Total: 6]

Page 6 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2011 0652 22 © University of Cambridge International Examinations 2011 12 (a) alkanes ; [1] (b) propane ; C3H8 ; [2] (c) contains oxygen ; hydrocarbons contain hydrogen and carbon only ; [2] [Total: 5] 13 (a) straight lines between poles ; all lines start on one pole and finish on the other, none touch each other ; arrows pointing north to south ; [3] (b) complete circuit ; mercury is a conductor ; [2] (c) the rod will kick ; towards / away from the observer ; [2] (d) kick / move in the opposite direction ; [1] [Total: 8]