Cambridge IGCSE Physical Science 0652 — 2013 Oct/Nov Paper 2 · Variant 2

This document consists of 24 printed pages. IB13 11_0652_22/FP © UCLES 2013 [Turn over *9272258430* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/22 Paper 2 (Core) October/November 2013 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 pencil for any diagrams or graphs. Do not use staples, paper clips, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. Electronic calculators may be used. You may lose marks if you do not show your working or if you do not use appropriate units. A copy of the Periodic Table is printed on page 24. 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 2013 0652/22/O/N/13 For Examiner's Use 1 A student investigates the composition of four different inks using paper chromatography. Fig. 1.1 shows the results of his experiment after one hour. A B C D solvent front starting position of inks beaker water Fig. 1.1 (a) Explain why the water level in the beaker must be below the ink dots at the start of the experiment. [1] (b) Suggest why ink A did not move during the experiment. [1] (c) (i) State how many different components ink D contains. [1] (ii) State one similarity and one difference in the compositions of inks B and C. similarity difference [2]

3 © UCLES 2013 0652/22/O/N/13 [Turn over Please turn over for Question 2.

4 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 2 A metre rule is clamped to a ramp. Fig. 2.1 shows the experimental set up. 0 10 20 30 40 50 60 70 80 90 100 ramp metre ruler Fig. 2.1 • The ramp is tilted and a toy car is held at the top of the ramp. • The car is given a gentle push and it moves down the ramp. • The positions of the car after successive time intervals of 0.20 s are shown. (a) (i) Read off the positions of the front of the car after each time interval. Record the values, to the nearest centimetre, in Table 2.1. Table 2.1 time / s 0.0 0.20 0.40 0.60 0.80 position / cm 99 [1] (ii) Describe the pattern in the data in Table 2.1 which suggests that the car is travelling at constant speed. [2] (iii) Calculate the speed of the car as it moves down the ramp. Show your working in the box. speed = unit [3]

5 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use (b) • In a separate experiment the angle of the ramp is increased. • The car is given a gentle push and it moves down the ramp. • Fig. 2.2 shows the positions of the car in successive 0.20 s intervals. 0 10 20 30 40 50 60 70 80 90 100 Fig. 2.2 Describe the motion of the car in this experiment. [1]

6 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 3 (a) Potassium nitrate can be made by reacting an acid with an alkali. Name these reagents. acid alkali [2] (b) State the name given to the reaction of an acid with an alkali. [1] (c) The potassium nitrate formed is in aqueous solution. Describe how you could obtain dry crystals of potassium nitrate from this solution. [2]

7 © UCLES 2013 0652/22/O/N/13 [Turn over Please turn over for Question 4.

8 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 4 Fig. 4.1 shows apparatus used to demonstrate one method of transfer of thermal energy. smoke goes down smoke goes up candle smoke generator Fig. 4.1 (a) (i) Name the method of thermal energy transfer this experiment demonstrates. [1] (ii) Explain how the candle makes the smoke rise up the right hand tube. [3]

9 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use (b) Fig. 4.2 shows an eagle gliding round a thermal. A thermal is a column of rising hot air. hot dark rocks Fig. 4.2 (i) The rocks are heated by electromagnetic radiation from the sun. Name the type of electromagnetic radiation that heats the rocks. [1] (ii) Explain how the thermal is formed. [1]

10 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 5 Hydrogen has been described as ‘a clean fuel which produces no pollution’. (a) Write a balanced equation for the burning of hydrogen in air. [2] (b) State why the burning of hydrogen is an oxidation reaction. [1] (c) Explain why the burning of hydrogen does not produce pollution. [1] (d) Give one disadvantage of using hydrogen as a fuel instead of petrol. [1]

11 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use 6 Fig. 6.1 shows water waves in a ripple tank. The wavefronts pass from the deep water to the shallow water. wavefront deep water shallow water Fig. 6.1 (a) Name the wave behaviour this experiment demonstrates. [1] (b) State the change, if any, to these properties as the waves enter shallow water. (i) wavelength (ii) frequency (iii) speed [3] (c) Fig. 6.2 shows the electromagnetic spectrum. radio waves micro- waves infra-red visible Y X-rays γ-rays Fig. 6.2 (i) Name the type of radiation found in region Y. [1] (ii) When the Sun moves from behind a cloud we feel an increase in warmth and see an increase in brightness at the same time. State what this suggests about the speeds of different types of electromagnetic radiation. [1]

12 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 7 Chlorine is a member of Group VII of the Periodic Table. (a) Use the electron configuration of chlorine to explain why it is in Group VII. [1] (b) Chlorine is a gas at room temperature. Name another element in Group VII that is a gas at room temperature. [1] (c) Name an element in Group VII that is less reactive than chlorine. [1] (d) (i) Name the compound formed when chlorine reacts with sodium. [1] (ii) Name the type of bonding in this compound. [1] (e) Name a metal in the same period as chlorine. [1]

13 © UCLES 2013 0652/22/O/N/13 [Turn over Please turn over for Question 8.

14 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 8 Fig. 8.1a shows a long conducting wire connected to a switch and power supply. A small plotting compass is placed near the wire. switch S compass power supply switch S compass power supply Fig. 8.1a Fig. 8.1b Switch S is closed and the plotting compass needle moves to the position shown in Fig. 8.1b. (a) State the conclusion that can be made from this experiment. [1]

15 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use (b) A student takes a similar wire and wraps it around a cylindrical piece of soft ion. She connects it to a switch and a power supply. She holds the soft iron above some light iron nails which are on the work bench, as shown in Fig. 8.2. power supply switch soft iron wire iron nails Fig. 8.2 (i) State what the student observes when the switch is closed. Give a reason for your answer. observation reason [2] (ii) State what the student observes when the switch is opened again. Give a reason for your answer. observation reason [2] (iii) She replaces the soft iron with a steel cylinder of the same size. Describe what she observes when she closes the switch, opens the switch. [2]

16 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 9 (a) The treatment of water to make it safe for domestic use involves two main steps. Name these steps. step 1 step 2 [2] (b) Anhydrous copper(II) sulfate can be used to test for the presence of water. Describe the change that shows water is present. [1] (c) Describe how you could show that a liquid is pure water. [2]

17 © UCLES 2013 0652/22/O/N/13 [Turn over Please turn over for Question 10.

18 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 10 Fig. 10.1 shows a circuit diagram with a battery of e.m.f. 6.0 V, an ammeter, and two resistors of 4.0 Ω and 8.0 Ω. A 4.0 Ω 6.0 V 8.0 Ω Fig. 10.1 (a) (i) Calculate the resistance in the circuit. resistance = Ω [1] (ii) Calculate the current in the circuit and give the unit. current = unit [2] (b) A teacher wants to show his students the potential difference across the 4.0 Ω resistor. (i) Name the instrument that he should use. [1] (ii) On Fig. 10.1, show how the instrument should be connected. [1] (iii) Calculate the potential difference across the 4.0 Ω resistor and give the unit. potential difference = unit [2]

19 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use (c) The teacher rearranges the resistors so that they are in parallel. (i) Complete Fig. 10.2 to show this circuit. [1] A Fig. 10.2 (ii) State how the current from the battery in Fig. 10.2 compares with the current from the battery in Fig. 10.1. Explain your answer. [2]

20 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 11 Organic compounds are often arranged in homologous series. (a) Give two characteristics of an homologous series. 1 2 [2] (b) The alkanes are an homologous series. Complete Table 11.1. Table 11.1 alkane C H H C H H C H H H H H C H H H structural formula molecular formula C2H6 methane ethane propane [3] (c) State one use of methane. [1]

21 © UCLES 2013 0652/22/O/N/13 [Turn over For Examiner's Use (d) The alkenes are another homologous series. (i) Describe the difference in bonding between alkanes and alkenes. [2] (ii) Describe a chemical test to show that a compound is an alkene rather than an alkane. test result [2]

22 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 12 Fig. 12.1 shows some of the principal parts of a nuclear reactor used to generate electricity. reactor core steam generator steel lined concrete pressure vessel steam out to turbine water in steam out to turbine water in Fig. 12.1 The reactor is fuelled with uranium which undergoes nuclear fission. (a) (i) Explain what is meant by nuclear fission. [2] (ii) During the fission process particles are released with very high speeds. Name the form of energy that these particles have due to their motion. [1] (b) Suggest a reason why the pressure vessel is made from steel and thick concrete. [1]

23 © UCLES 2013 0652/22/O/N/13 For Examiner's Use 13 Potassium nitrate, KNO3, and potassium phosphate, K3PO4, are both used as fertilizers. (a) Calculate the relative molecular mass of potassium nitrate. [relative atomic masses, Ar : K, 39; N, 14; O, 16] Write your working in the box. answer [1] (b) Show, by calculation, that potassium phosphate contains more than 50% potassium by mass. [relative atomic masses, Ar : K, 39; O, 16; P, 31;] Write your working in the box. [3]

24 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 2013 0652/22/O/N/13 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

CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the October/November 2013 series 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 should be read in conjunction with the question paper and the Principal Examiner Report for Teachers. Cambridge will not enter into discussions about these mark schemes. Cambridge is publishing the mark schemes for the October/November 2013 series for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level components and some Ordinary Level components.

Page 2 Mark Scheme Syllabus Paper IGCSE – October/November 2013 0652 22 © Cambridge International Examinations 2013 1 (a) to prevent ink dissolving/running into the water/samples mix ; [1] (b) insoluble (in water) ; [1] (c) (i) three [1] (ii) both have one colour/spot in common/both composed of 2 colours ; both have one colour different ; [2] [Total: 5] 2 (a) (i) 75, 51, 27, 3 – all correct ±1 cm ; [1] (ii) travels equal distances ; in equal time intervals ; [2] (iii) choice of any two correct distances and times, e.g. (0,0) and (96, 0.80) ; use of change of distance/time ; 120 cm/s ; [3] (b) (constant) acceleration ; [1] [Total: 7] 3 (a) nitric acid ; potassium hydroxide/potassium carbonate ; [2] (b) neutralisation ; [1] (c) any two valid points: evaporate (to concentrate solution) ; cool/allow crystals to form ; filter and dry ; [max 2] [Total: 5] 4 (a) (i) convection ; [1] (ii) candle heats the air (accept heats smoke) ; air expands ; becomes less dense (so rises) ; [3] (b) (i) infra-red radiation/visible light ; [1] (ii) the hot rocks heat the air ; [1] [Total: 6]

Page 3 Mark Scheme Syllabus Paper IGCSE – October/November 2013 0652 22 © Cambridge International Examinations 2013 5 (a) 2H2 + O2 → 2H2O (correct formulae – 1 mark ; correct balancing – 1 mark) ; [2] (accept H2 + O → H2O for 1c) (b) oxygen added / oxidation number increases / loses an electron ; [1] (c) only water produced / no carbon dioxide produced / no acidic gases produced ; [1] (d) needs to be manufactured / not found naturally / made from methane / etc. ; [1] [Total: 5] 6 (a) refraction ; [1] (b) (i) decreases ; [1] (ii) unchanged ; [1] (iii) decreases ; [1] (c) (i) ultraviolet ; [1] (ii) travel at the same speed ; [1] [Total: 6] 7 (a) 7 electrons in outer shell ; [1] (b) fluorine (accept bromine) ; [1] (c) bromine / iodine / astatine ; [1] (d) (i) sodium chloride (accept common salt) ; [1] (ii) ionic ; [1] (e) sodium / magnesium / aluminium ; [1] [Total: 6]

Page 4 Mark Scheme Syllabus Paper IGCSE – October/November 2013 0652 22 © Cambridge International Examinations 2013 8 (a) an electric current has a magnetic field ; [1] (b) (i) nails move towards the iron (accept attracted to) ; iron is magnetised ; [2] (ii) nails fall to the ground ; iron loses magnetism / iron is easily demagnetised / does not retain magnetism ; [2] (iii) nails move towards the steel (accept attracted to) ; nails remain on the steel when switch is opened ; [2] [Total: 7] 9 (a) filtration ; chlorination / ozonation ; [2] (b) turns blue / white to blue ; [1] (c) boil / freeze ; 100 oC (at 1 atm pressure)/0oC; [2] [Total: 5] 10 (a) (i) 12 (Ω) ; [1] (ii) use of V = IR → I = 6/12 = 0.5 A ; [2] (b) (i) voltmeter ; [1] (ii) in parallel over the 4 Ω resistor ; [1] (iii) Use of V = IR = 0.5 × 4 (ecf); = 2 V ; [2]

Page 5 Mark Scheme Syllabus Paper IGCSE – October/November 2013 0652 22 © Cambridge International Examinations 2013 (c) (i) correct connection ; [1] (ii) current greater than in 5.1 ; with simple explanation e.g. resistance less in parallel circuit ; [2] [Total: 10] 11 (a) any two from: similar chemical properties ; members differ from each other by CH2 ; gradation in physical properties ; same functional group ; [max 2] (b) CH4 ; ; C3H8 ; [3] (c) fuel ; [1] (d) (i) alkanes have only single bonds / saturated ; alkenes have (at least one) double bond / unsaturated ; [2] (ii) bromine water / bromine ; [1] decolourised ; [1] [2] [Total: 10] 12 (a) (i) splitting of an atomic nucleus ; detail; e.g. into two (more or less) equal parts / with the release of energy / large nucleus ; [2] (ii) kinetic energy ; [1] (b) very high pressure or temperature / shield outside from radioactive emissions / to protect in case of catastrophic failure ; [1] [Total: 4] 13 (a) 101 ; [1] H C H H C H H H

Page 6 Mark Scheme Syllabus Paper IGCSE – October/November 2013 0652 22 © Cambridge International Examinations 2013 (b) potassium is 39 × 3 = 117(g) ; whole molecule is 212 or PO4 is 95; which is less than triple potassium or which is less than K3 ; [3] (accept correct calculation of % potassium, etc.) [Total: 4]