Cambridge IGCSE Physical Science 0652 — 2003 May/June Paper 3 · Variant 1

This document consists of 13 printed pages and 3 blank pages. BR (PW) S41651/4 © CIE 2003 [Turn over CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education PHYSICAL SCIENCE 0652/03 Paper 3 May/June 2003 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

1 Fig. 1.1 shows the trends in some of the properties of the elements in Group V of the Periodic Table. Fig. 1.1 (a) (i) Describe the structure and bonding in nitrogen. … … (ii) Explain how this structure relates to the properties shown above. … …[3] (b) Suggest, with a reason, the type of oxide you would expect arsenic to form. … … …[2] (c) Antimony is a metallic element. Suggest why you would expect antimony to have a higher melting point than bismuth. … … … …[2] (d) Write down the formula that you would expect for a chloride of phosphorus. …[1] nitrogen phosphorus arsenic antimony bismuth non-metal gas at 20°C acidic oxide metal basic oxide solid at 20°C 2 0652/03/M/J/03 For Examiner’s Use

3 0652/03/M/J/03 [Turn over 2 A child throws a beach ball, of mass 0.075 kg, vertically upwards from the ground. The ball takes 0.3 s to accelerate from rest to 11 m/s. (a) Calculate the acceleration of the ball. Write down the equation that you use and show all your working. acceleration = … [3] (b) Calculate the maximum kinetic energy of the ball. Write down the equation that you use and show all your working. maximum kinetic energy = … [3] (c) The ball reaches a vertical height of 2.7 m. Calculate the maximum gravitational potential energy of the ball. Write down the equation that you use and show all your working. [g = 10 N/kg] maximum gravitational potential energy = … [3] (d) (i) Explain what is meant by the term efficiency. … … …[2] (ii) Discuss whether or not the energy conversion from kinetic to gravitational potential has been done efficiently. … … …[2] For Examiner’s Use

4 0652/03/M/J/03 3 Many substances need to be kept under carefully controlled conditions. Use your knowledge of the reactions of the substances involved to explain each of the following. (a) Silver nitrate is stored in dark brown bottles. … … …[2] (b) Sodium metal is stored immersed in liquid paraffin. … … …[2] (c) Anhydrous copper(II) sulphate is stored in a desiccator. … … …[2] (d) Bromine should be kept cold and in a fume cupboard. … … …[2] For Examiner’s Use

5 0652/03/M/J/03 [Turn over 4 An object of height 2.0 cm is placed 3.0 cm to the left of a converging (convex) lens of focal length 5.0 cm. (a) On the grid below draw a ray diagram to show the formation of the image by the lens. The central line shows the centre of the lens. [3] (b) Write down three properties of the image. … … …[3] (c) Suggest a use for a lens forming an image in this way. … …[1] For Examiner’s Use

6 0652/03/M/J/03 5 The two diagrams in Fig. 5.1 represent the structures of a pure metal and one of its alloys. Fig. 5.1 (a) State what holds the positive metal ions together. … …[1] (b) By referring to the diagrams, explain why pure metals are more malleable than alloys. … … … … … …[4] (c) Both the metals in the alloy belong to Group II in the Periodic Table. The smaller circles represent magnesium ions. (i) Suggest what ions the larger circles represent. … [1] (ii) Describe two changes that you would expect to observe if a sample of the pure metal were placed in cold water. … … … …[2] ++ + + ++ ++ ++ ++ ++ + + + + + + ++ ++ ++ ++ ++ + + ++ ++ + + + + + + + + + + + + ++ ++ ++ ++ + metal alloy For Examiner’s Use

7 0652/03/M/J/03 [Turn over 6 Fig. 6.1 shows a coil of copper wire wound on a cardboard tube. The ends of the coil are connected to a cathode ray oscilloscope (c.r.o.) and a magnet is released so that it falls vertically down the tube. Fig. 6.2 shows the trace seen on the c.r.o., along with its y-gain and time-base settings. Fig. 6.1 Fig. 6.2 (a) Write down the voltages at A and B. voltage at A = …V voltage at B = …V [2] (b) Explain why these voltages are produced. … … … …[2] A B voltage (y-gain): 0.2V/division time-base: 20ms/division S N magnet to c.r.o. coil of copper wire cardboard tube to c.r.o. For Examiner’s Use

8 0652/03/M/J/03 (c) State and explain two things about the shape of the trace. … … … … … … … …[4] For Examiner’s Use

9 0652/03/M/J/03 [Turn over 7 The equation for the reaction between copper(II) carbonate and dilute hydrochloric acid may be written as shown below. CuCO3(s) + 2HCl(aq) →CuCl2(aq)+ H2O(l) + CO2(g) (a) (i) What do you understand by the symbol (II) after the word copper? … …[1] (ii) Why is it not necessary to write this symbol after calcium in the name calcium carbonate? … …[1] (b) In an experiment copper(II) carbonate is added to 50 cm3 of hydrochloric acid of concentration 1 mol/dm3, until no more will react. (i) Calculate the number of moles of HCl in the 50 cm3 of acid. number of moles of HCl … [1] (ii) Calculate the number of moles of copper(II) carbonate that will react with this acid. number of moles of copper(II) carbonate …[1] (iii) Calculate the relative formula mass, Mr, of copper(II) carbonate. [Ar: C, 12; O, 16; Cu, 64] Mr of copper(II) carbonate …[2] (iv) Calculate the mass of copper(II) carbonate that will react with this acid. mass of copper(II) carbonate …[2] For Examiner’s Use

10 0652/03/M/J/03 8 Fig. 8.1 shows a circuit with a high-resistance voltmeter being used to measure the e.m.f. of a cell. Fig. 8.1 (a) Explain the meaning of the term e.m.f. … … …[2] (b) Explain why the voltmeter must have a high resistance if it is to measure an accurate value of the e.m.f. … … …[2] (c) Fig. 8.2 shows a cell with an internal resistance of 2 Ω. A voltmeter which has a resistance of 100 Ωis connected across the cell. The e.m.f. of the cell is 1.50 V. Fig. 8.2 V 2 Ω internal resistance 100 Ω V For Examiner’s Use

11 0652/03/M/J/03 [Turn over (i) Calculate the current in the circuit. current = … [3] (ii) Calculate the potential difference across the voltmeter. potential difference = … [2] (iii) The potential difference in (ii) is not equal to the e.m.f. of the cell. Explain why this is the case and state what change you would make in order to give a value much closer to the e.m.f. of the cell. … … … … …[3] For Examiner’s Use

12 0652/03/M/J/03 9 Ethene, C2H4, is the first member of the homologous series of alkenes. (a) Draw a diagram to show the arrangement of the outer shell electrons in a molecule of ethene. [2] (b) In most homologous series the first member contains only one carbon atom. Explain why this is not the case with alkenes. … … … …[2] (c) Ethene and hydrogen can be produced from saturated hydrocarbons by cracking. (i) Write an equation for the cracking of butane, C4H10, to produce ethene and hydrogen. …[2] (ii) State two essential conditions for cracking to occur. … …[2] For Examiner’s Use

16 0652/02/O/N/03 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