Cambridge IGCSE Physical Science 0652 — 2006 Oct/Nov Paper 2 · Variant 1

Centre Number Candidate Number Name UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/02 Paper 2 (Core) October/November 2006 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. 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. For Examiner’s Use 1 2 3 4 5 6 7 8 9 10 11 Total This document consists of 14 printed pages and 2 blank pages. IB06 11_0652_02/2RP  UCLES 2006 [Turn over www.XtremePapers.com

2 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 1 (a) (i) Complete the diagram in Fig. 1.1 for ethanol, C2H6O. H C H H C H H [1] Fig. 1.1 (ii) Calculate the relative molecular mass, Mr, of ethanol, C2H6O. Show your working. Mr = [2] (iii) Complete the diagram in Fig.1.2 for ethanoic acid, C2H4O2. C H C H H Fig. 1.2 [2] (b) Ethanol, C2H6O, can be used as a fuel. (i) Balance the following chemical equation for the products of the complete combustion of ethanol. C2H6O + 3O2 …CO2 + …H2O [1] (ii) Describe a chemical test for the carbon dioxide produced. test result [2] (iii) Describe a chemical test for the water produced. test result [2]

3 © UCLES 2006 0652/02/O/N/06 [Turn over For Examiner's Use (c) A student adds dilute aqueous sodium hydroxide in excess to an aqueous solution of ethanoic acid in a beaker. Suggest how the pH number of the liquid in the beaker changes. [2]

4 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 2 (a) Look at the Periodic Table on page 16. State the number of electrons in the outer shell of an atom of (i) the alkali metal caesium, Cs, [1] (ii) the halogen astatine, At. [1] (b) Describe the formation of each of the ions in caesium astatide, CsAt, from the atoms of caesium and of astatine. [2] (c) A molecule of chlorine, Cl2, has a single covalent bond between the two atoms. A molecule of astatine, At2, has similar bonding. Draw a diagram to show the bonding in a molecule of astatine, At2. Show only the outer electrons. [2]

5 © UCLES 2006 0652/02/O/N/06 [Turn over For Examiner's Use 3 Fig. 3. 1 shows part of a gas thermostat used in an oven. gas in steel case brass burner space Fig. 3.1 (a) Explain why less gas enters the burner as the temperature in the oven gets higher. [2] (b) Fig. 3.2 shows a loaf of bread cooking in the oven. oven burners bread Fig. 3.2 Thermal energy is transferred from the burning gas to the bread by conduction, convection and radiation. Explain, with reference to this example, what is meant by (i) conduction, (ii) convection, (iii) radiation. [4]

6 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 4 A meteorite is a piece of rock which comes from the outer part of the solar system and enters the Earth’s atmosphere. Fig. 4.1 shows the speed of the meteorite as it approaches and finally strikes the Earth. speed time Fig. 4.1 (a) As the meteorite approaches the Earth it is travelling at a high speed and accelerates further. (i) Name the type of energy it has due to its motion. [1] (ii) Suggest why it accelerates as it approaches the Earth. [2] (b) When the meteorite enters the Earth’s atmosphere it slows down rapidly. (i) Mark, with an X, the point on the graph at which the meteorite enters the Earth’s atmosphere. [1] (ii) Using scientific terms explain why the meteorite slows down. [2] (iii) State into what form the energy is converted. [1]

7 © UCLES 2006 0652/02/O/N/06 [Turn over For Examiner's Use 5 A boy holds a long rope at one end and moves it sharply up and down to send waves along the rope. Fig. 5.1 shows the waves moving along the rope. Fig. 5.1 (a) Mark on the diagram (i) the wavelength of the wave and label it λ , (ii) the amplitude of the wave and label it A. [2] (b) Explain how the boy changes the movement of his hand to (i) increase the amplitude of the wave, (ii) increase the frequency of the wave. [3] (c) When a guitar string is plucked a sound is heard. Explain how the sound is produced. [2]

8 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 6 (a) Balloons are used to lift radio equipment high in the atmosphere to measure pressure, temperature and ozone levels. Explain why helium, not hydrogen, is used to fill these balloons. [2] (b) Filament lamps have a thin wire of tungsten that glows white hot when connected to the electrical supply. Explain why argon, not air, is used to fill these lamps. [2] (c) An atom of helium has the notation He. 4 2 An atom of argon has the notation Ar. 40 18 Complete Fig. 6.1 for these atoms. notation of atom He 4 2 Ar 40 18 number of protons in nucleus 2 number of neutrons in nucleus 22 arrangement of electrons in shells in the atom 2 [3] Fig. 6.1

9 © UCLES 2006 0652/02/O/N/06 [Turn over For Examiner's Use 7 Fig. 7.1 shows a circuit. The e.m.f. of the battery is 12 V. iron core A Fig. 7.1 (a) What is the total resistance in the circuit when the ammeter reads 2 A? Show your working and state the unit. resistance = [3] (b) Two soft iron nails are attracted to the core as shown in Fig. 7.2. S N iron core nails Fig. 7.2 (i) Complete Fig. 7.2 to show the poles induced on the nails. [2] (ii) Explain what happens to the nails when the current is gradually reduced to zero. [3]

10 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 8 (a) Iron, Fe, is described as a transition element. State two properties of iron that are common to transition elements. 1. 2. [2] (b) Iron reacts with dilute hydrochloric acid. Fe(s) + 2HCl(aq) FeCl2(aq) + H2(g) State two ways of increasing the speed of this reaction. 1. 2. [2] (c) Iron goes rusty in damp air. State two ways to prevent iron from rusting. 1. 2. [2] (d) Rust is a form of iron oxide. When this is heated in carbon monoxide, iron and carbon dioxide are formed. Explain this reaction in terms of oxidation and reduction. oxidation reduction [2]

11 © UCLES 2006 0652/02/O/N/06 [Turn over For Examiner's Use 9 An experiment is done to measure the half-life of an isotope of neon. The results are shown in Fig. 9.1 count rate/Bq 180 150 125 104 85 70 60 51 42 time/s 0 10 20 30 40 50 60 70 80 Fig. 9.1 (a) The first four points are already plotted on the grid in Fig. 9.2. (i) Plot the remaining points. (ii) Draw a smooth curve through the points. 20 40 time / s count rate / Bq 60 80 200 150 100 50 0 [3] Fig. 9.2 (b) Use the graph to find the half-life of the isotope. half-life = s [2] (c) The isotope decays by emission of a beta-particle (β-particle). Complete the equation to show the decay. Ne Na + 23 10 … … β … … [2]

12 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 10 (a) Energy is needed to convert a boiling liquid, at constant temperature, into a gas. Use the kinetic particle theory of matter to explain this fact. [2] (b) Explain why evaporation from the surface of a liquid causes the temperature of the remaining liquid to cool. [2] (c) (i) Fig. 10.1 shows two liquids being boiled for several minutes. xxxxxxxxxxxxxx heat liquid P thermometer xxxxxxxxxxxxxx heat liquid Q thermometer Fig. 10.1 Liquid P continues to boil at a constant temperature. Liquid Q continues to boil at a temperature that increases with time. Explain these observations. [2] (ii) Name one example of a liquid that behaves like liquid Q. [1]

13 © UCLES 2006 0652/02/O/N/06 For Examiner's Use 11 (a) Describe how a polythene rod can be charged. [1] (b) Fig. 11.1 shows a negatively charged polythene rod suspended by an insulating thread. A B insulating thread polythene rod Fig. 11.1 State what happens when (i) a negatively charged rod is brought up to end A, (ii) a positively charged acetate rod is brought up to end A, (iii) a positively charged acetate rod is brought up to end B, (iv) an uncharged glass rod is brought up to end A. [4]

15 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 University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge. 0652/02/O/N/06 BLANK PAGE

16 0652/02/O/N/06 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 AAluminium 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 CChlorine 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 TThallium 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 2006 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 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. The grade thresholds for various grades are published in the report on the examination for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses. • CIE will not enter into discussions or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the October/November 2006 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 - OCT/NOV 2006 0652 2 © UCLES 2006 General Rules. + marks can only be scored if the previous mark has been scored. In calculations, if the working/equation has not been asked for, and the answer is correct, then all the marks for that section must be scored. Words in brackets preferable but not obligatory.

Page 3 Mark Scheme Syllabus Paper IGCSE - OCT/NOV 2006 0652 2 © UCLES 2006 1 (a) (i) –OH or –O―H (do not accept HO) 1 (ii) 24 + 6 +16 1 = 46 1 (iii) ═ O 1 ― OH 1 5 (b) (i) 2 (CO2) + 3 (H2O) (both) 1 (ii) test - (bubble through) limewater 1 result - (from clear) to cloudy [necf] 1 (iii) test - use (anhydrous) copper sulphate/cobalt chloride 1 result - from white to cloudy/blue to red [necf] 1 5 (no need for white/red if anhydrous used in test) (c) rises/increases 1 from <7 to >7 (accept any corresponding figures) 1 2 Total 12 2 (a) (i) Cs … 1 1 (ii) At … 7 1 2 (b) transfer of electron(s) 1 from Cs to At or to form Cs + and At - 1 2 (accept At loses an electron and Cs gains an electron for 2) diagram showing shared pair of electrons 1 both shells with 8 electrons +1 2 Total 6 3 (a) brass expands (more than steel) 1 making entry gap smaller 1 2 (b) (i) energy is passed from molecule to molecule 1 (ii) hot air from the bottom (of the oven) rises 1 (iii) waves or (better) infra red 1 some correct reference to the example somewhere 1 4 Total 6 4 (a) (i) kinetic 1 (ii) mention of gravity 1 either Earth's gravity or gravity pulls it 1 3 (b) (i) anywhere from where the rate of increase of the curve's gradient starts to decrease to the vertical line 1 (ii) work is done (any mention of work) 1 against friction (any mention of friction) / air resistance 1 (iii) kinetic energy is converted to heat/ (any mention of heat) 1 4 Total 7

Page 4 Mark Scheme Syllabus Paper IGCSE - OCT/NOV 2006 0652 2 © UCLES 2006 5 (a) (i) wavelength correctly marked 1 (ii) amplitude correctly marked 1 2 (b) (i) move the hand further (up and down) 1 (ii) move the hand up and down faster 1 clear that it means more times per second +1 3 (c) string vibrates 1 causing the air molecules to vibrate 1 2 Total 7 6 (a) hydrogen is flammable/explosive 1 helium is inert or equivalent 1 2 (b) in air the (hot) tungsten/filament would oxidize/burn/react 1 argon is inert or equivalent 1 2 (c) number of protons in argon nucleus – 18 1 number of neutrons in helium nucleus – 2 1 arrangement of electrons in argon – 2,8,8 1 3 Total 7 7 (a) V = IR or R = V/I or R = 12/2 1 = 6 1 Ω 1 3 (b) (i) top pole on top pin south 1 remainder all correct 1 (ii) fall off 1 one by one 1 because the iron loses its magnetism 1 5 Total 8

Page 5 Mark Scheme Syllabus Paper IGCSE - OCT/NOV 2006 0652 2 © UCLES 2006 8 (a) high density high melting point coloured compounds good conductor (of either heat or electricity) catalysts ANY TWO 1+1 2 (b) increase the concentration of the acid increase the temperature decrease the size of the pieces of iron use a catalyst ANY TWO 1+1 2 (c) coating with: grease/oil paint plastic zinc or galvanising ANY TWO 1+1 2 (d) oxidation: carbon monoxide gains oxygen OR is oxidized 1 reduction: iron loses oxygen OR is reduced 1 2 Total 8 9 (a) remaining points correctly plotted (-1 for each incorrect) 2 good curve going through all points 1 3 (b) 38 s +/- 2s 2 (38 s +/- 4s………..1) 2 (c) top line 23 & 0 1 lower line 11 & -1 1 2 Total 7 10 (a) work must be done 1 to overcome the attractive forces OR to separate the particles 1 (accept bond breaking (is exothermic) for one mark maximum) 2 (b) energy is needed to escape (from the surface) 1 comes from the liquid itself 1 (OR the fastest/most energetic molecules tend to escape 1 the slower/less energetic molecules are left behind 1) 2 (c) (i) P is a single substance 1 Q is a mixture 1 (ii) any valid example; e.g. crude oil, fermented liquor, liquid air 1 3 Total 7 11 (a) rub it (with a cloth) 1 1 (b) (i) repel 1 (ji) attract 1 (iii) attract 1 (iv) attract 1 4 Total 5