Cambridge IGCSE Physical Science 0652 — 2004 May/June Paper 3 · Variant 1

This document consists of 13 printed pages and 3 blank pages. SP (CW/GR) S62395/2 © UCLES 2004 [Turn over UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 May/June 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. 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. 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/M/J/04 Answer all the questions. Write your answers in the spaces provided. 1 The metal M has a relative atomic mass, Ar, of 30. M is reacted with pure oxygen at room temperature and pressure (r.t.p.) to form the oxide of M. It is found that 5.0 g of M react with exactly 2.0 dm3 of oxygen under these conditions. 1 mole of any gas occupies 24 dm3 at r.t.p. (a) Define the term relative atomic mass. … … …[2] (b) (i) Find the number of moles in 5.0 g of M. number of moles = …[2] (ii) Find the number of moles of oxygen gas that react with 5.0 g of M. number of moles = …[1] (iii) From your answers to (i) and (ii) deduce the number of moles of M that react with 1 mole of oxygen gas. number of moles = …[1] (iv) Write the balanced chemical equation for the reaction between M and oxygen. …[2] For Examiner’s Use © UCLES 2004

3 0652/03/M/J/04 [Turn over (c) Calculate the relative formula mass, Mr , for the oxide. Mr = … [1] 2 Fig. 2.1 shows apparatus used to measure the volume of an irregularly shaped object. Fig. 2.1 (a) Describe how this apparatus might be used in order to measure the volume of an irregularly shaped object. The dimensions of the object are such that it is too large to fit inside the measuring cylinder. … … … … … … … …[3] displacement (eureka) can measuring cylinder For Examiner’s Use © UCLES 2004

4 0652/03/M/J/04 (b) Fig. 2.2 is a table of the density of some metals. Fig. 2.2 (i) State a unit for density. …[1] (ii) A sample of metal of measured volume 0.8 cm3 is found to have a mass of 15.4 g. Calculate the density of the sample. Write down the equation that you use and show your working. [2] (iii) Which of the metals in the table is the sample most likely to be? …[1] (iv) Explain why the value calculated in (ii) may not be exactly the same as any of the values in the table. … … … …[2] For Examiner’s Use © UCLES 2004 aluminium 2.7 copper 8.9 gold 19.3 iron 7.8 lead 11.3 magnesium 1.7 platinum 21.4 uranium 18.7

5 0652/03/M/J/04 [Turn over (c) A second sample of the metal is found to have a mass of 85 g. On the moon it is found to weigh 0.14 N. Calculate the value of the gravitational field strength (g) on the moon. Write down the equation that you use and show your working. value for g on the moon = … [3] 3 Fig. 3.1 contains the melting points of the elements in Period 3 of the Periodic Table. Fig. 3.1 (a) Describe the trend in melting point of the elements in Period 3. … …[1] (b) What does the high melting point of silicon suggest about the structure of solid silicon? … … … …[2] (c) Use your knowledge of the trends in the Periodic Table to deduce which of these elements (i) is the most reactive metal, …[1] (ii) has five electrons in the outer shell of one atom, …[1] (iii) forms an ion with a charge of 2+, …[1] (iv) does not react with any other element. …[1] For Examiner’s Use © UCLES 2004 element Na Mg Al Si P S Cl Ar m.pt./K 371 924 933 1680 317 386 172 84

6 0652/03/M/J/04 (d) Suggest why sodium is a softer metal than magnesium. … … … …[2] 4 Fig. 4.1 shows a circuit used to measure the resistance of different lengths of wire. Fig. 4.1 (a) Mark on Fig. 4.1 where the resistance wire should be connected. [1] (b) The voltmeter shows a value of 4.3 V and the ammeter a value of 2.1 A. Calculate the resistance of the wire. Write down the equation that you use and show your working. resistance of wire = …[3] (c) What would you expect the resistance to be when a wire of the same metal and same diameter but of twice the length replaces the one used in (b)? new resistance = …[1] A V For Examiner’s Use © UCLES 2004

7 0652/03/M/J/04 [Turn over (d) It is likely that the temperatures of the two lengths of wire would be different as a result of the different currents flowing through the wires. State and explain the effect that this is likely to have on the resistances of the wires. … … … … … …[3] (e) Explain why using a very short length of resistance wire could damage the ammeter. … … … …[2] (f) Name a device that could be used to measure the p.d. instead of the voltmeter. …[1] For Examiner’s Use © UCLES 2004

8 0652/03/M/J/04 5 (a) (i) Using the Periodic Table on page16, write down the electronic structures of calcium and fluorine. electronic structure of calcium …[1] electronic structure of fluorine …[1] (ii) By reference to these structures, describe how calcium and fluorine form calcium fluoride. [2] (iii) State the formula of calcium fluoride. …[1] (b) Solid calcium fluoride does not conduct electricity but molten calcium fluoride does. Liquid fluorine does not conduct electricity. Explain these observations in terms of the structures of these substances. … … … … … …[3] For Examiner’s Use © UCLES 2004

9 0652/03/M/J/04 [Turn over 6 (a) Light travels at a speed of 3 × 10nm/s in a vacuum. Write down the value for n. n = …[1] (b) Sound waves travel with a speed of approximately 340 m/s. Calculate the time that it takes sound to travel a distance of 80 m. Write down the equation that you use and show your working. [2] (c) Fig. 6.1 shows a method of measuring the speed of sound. An observer watches an assistant fire a gun. On seeing the smoke he starts a stopwatch and on hearing the sound of the gun he stops the watch. It is important that this experiment is performed in a large open space. Fig. 6.1 (i) Explain how this experiment depends upon the speed of sound being much less than the speed of light. … … … … … …[2] 80 m For Examiner’s Use © UCLES 2004

10 0652/03/M/J/04 (ii) Why is it important to carry out this experiment in an open space? … … … … … …[2] (d) A particular sound wave has a frequency of 3.5 kHz. What is its wavelength? Write down the equation that you use and show your working. wavelength of sound = …[3] For Examiner’s Use © UCLES 2004

11 0652/03/M/J/04 [Turn over 7 When an aqueous solution of sugars is fermented to form ethanol the resulting solution contains about 15% of ethanol. (a) State two essential conditions for fermentation to occur. 1. … 2. …[2] (b) (i) The boiling point of ethanol is 78 °C. State the name of the method used to separate ethanol from the solution. …[1] (ii) Sketch a labelled diagram of the apparatus that would be used in the laboratory to carry out this separation. [4] For Examiner’s Use © UCLES 2004

12 0652/03/M/J/04 8 (a) Complete the following passage relating to measuring temperatures. Temperatures indicate the degree of “hotness” of an object and can be measured using a … . These are devices that must have a property which … with temperature. Ideally this property shows a linear relationship with temperature. This means that the property changes by equal amounts for … changes in temperature. The maximum temperature minus the minimum temperature that the device can register is known as the … of the device. Devices for which the chosen property makes a large change for a small change in temperature are said to be very … . [5] (b) Name a specific type of temperature measuring device and the property on which its operation depends. device … property …[2] 9 Three substances are added to a blast furnace during the extraction of iron from its ore. Haematite, Fe2O3, is the ore. Limestone, CaCO3, and coke are the other substances needed. The main products are iron, slag and oxides of carbon. (a) State the reason for adding limestone to the furnace. …[1] (b) Write balanced equations for the reactions that occur when (i) limestone decomposes, … (ii) haematite is reduced. …[4] (c) Iron and steel can be prevented from rusting by galvanising. When the covering is complete this prevents the iron being exposed to the air. However, unlike painting, galvanising continues to prevent rusting even when the coating is damaged. Explain this difference between painting and galvanising. … … … …[2] For Examiner’s Use © UCLES 2004

15 0652/03/M/J/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/M/J/04 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 © UCLES 2004