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Igcse Combined Science Past Paper Paper 2 0653/21 October/November 2010

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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education *1144188971* COMBINED SCIENCE Paper 2 (Core) 0653/21 October/November 2010 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.

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Answer all questions. A copy of the Periodic Table is printed on page 20. 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 Total This document consists of 20 printed pages. IB10 11_0653_21/4RP © UCLES 2010 [Turn over 2 1 (a) State the word equation for photosynthesis. For Examiner’s Use + + [2] (b) (i) Name the green pigment found in plant leaves which absorbs energy from sunlight.

[1] (ii) Fig. 1. 1 is a diagram of a plant cell.

On the diagram, draw a label line to where this green pigment would be found, and label it P. Fig. 1. 1 [1] © UCLES 2010 0653/21/O/N/10 3 (c) A student fixed a piece of black paper over a leaf, which was still attached to the plant. He left the plant in the sun for two days. He then removed the leaf from the plant and tested it for starch, after removing the paper. (i) Using the letters given, list the correct sequence of the steps he took. A Add iodine solution to the leaf. For Examiner’s Use B Place the leaf in boiling water. C Dip the leaf into water to soften it. D Place the leaf in hot ethanol. E

Spread the leaf on a white tile. [3] (ii) Fig. 1. 2 shows the leaf before and after he did the starch test. black paper before testing after testing Fig. 1. 2 Iodine solution is orange-brown. It turns blue-black when it is in contact with starch. Complete the diagram of the leaf after testing in Fig. 1. 2. Do not colour the diagram. Use labels to show which parts would look orange-brown and which parts would look blue-black. [2] © UCLES 2010 0653/21/O/N/10 [Turn over 4 2 Fig. 2. 1 shows the apparatus a student used to measure the rate of reaction between some powdered metal and dilute hydrochloric acid.

For Examiner’s Use test-tube full of water conical flask 1. 0 g powdered metal dilute hydrochloric acid water Fig. 2. 1 When the student tilted the conical flask, the acid mixed with the powdered metal. If a reaction occurred, any gas which was produced bubbled up into the test-tube, pushing the water out. The student timed how long it took for the test-tube to fill with gas. (a) Describe how the student could test the gas to show that it was hydrogen. [2] (b) The student used the apparatus in Fig. 2. 1 to compare the rates of reaction between dilute hydrochloric acid and three powdered metals, X, Y and Z.

The results the student obtained are shown in Table 2. 1. Table 2. 1 metal mass of metal / g X Y Z 1. 0 1. 0 1. 0 time for gas to fill the test-tube / seconds 150 45 no gas was produced (i) One of the metals used was copper. State and explain which metal, X, Y or Z, was copper. metal explanation [2] © UCLES 2010 0653/21/O/N/10 5 (ii) Suggest two ways, other than using a catalyst, in which the student could increase the rate of reaction between metal X and dilute hydrochloric acid. 1 For Examiner’s Use 2 [2] (c) Fig. 2. 2 shows another experiment in which the student added zinc carbonate to dilute sulfuric acid.

A gas was given off and, when the bubbling stopped, some solid zinc carbonate remained in the mixture. zinc carbonate solid zinc carbonate remaining dilute sulfuric acid Fig. 2. 2 (i) State the chemical formula of sulfuric acid. [1] (ii) Explain why the reaction eventually stopped even though some zinc carbonate powder remained. [1] © UCLES 2010 0653/21/O/N/10 [Turn over 6 3 Fig. 3. 1 shows a rock that is falling from the top of a cliff into the river below. For Examiner’s Use cliff falling rock river Fig. 3. 1 (a) (i) As the rock falls, it gains kinetic energy.

Name the form of energy the rock had at the top of the cliff. [1] (ii) Suggest what happens to the kinetic energy of the rock when the rock hits the water. [2] (b) Fig. 3. 2 shows a speed-time graph for the motion of the rock. 25 20 speed m/s 15 10 5 0 0 1 2 3 4 time / s 5 6 7 Fig. 3. 2 (i) After how many seconds was the speed of the rock 15 m / s? s [1] © UCLES 2010 0653/21/O/N/10 7 (ii) The rock is accelerating. Explain the meaning of the term accelerating. For Examiner’s Use [1] (c) The rock contains radioactive substances emitting high levels of ionising radiation. (i) State how the radioactivity could be detected. 1] (ii) Explain why it would be dangerous for a person to handle this rock without proper protection. [1] © UCLES 2010 0653/21/O/N/10 [Turn over 8 4 Copper metal reacts with oxygen gas to form the black solid, copper oxide. (a) (i) Use this example to describe one difference between elements and compounds. For Examiner’s Use [2] (ii) State why this reaction is an example of oxidation. [1] (iii) Name the type of chemical bonding found in copper oxide. [1] (b) Fig. 4. 1 shows apparatus used in the electrolysis of copper chloride solution. – power supply + Fig. 4. 1 (i) On the diagram, clearly label the anode and the electrolyte. ii) Copper chloride solution contains copper ions and chloride ions in water. State briefly two differences between a chlorine atom and a chloride ion. [2] [2] © UCLES 2010 0653/21/O/N/10 9 (iii) Copper is a pink/orange metal and chlorine is a gas. Describe what would be observed at the positive and negative electrodes during electrolysis of copper chloride solution. observation at positive electrode For Examiner’s Use observation at negative electrode [2] © UCLES 2010 0653/21/O/N/10 [Turn over 10 5 (a) Fig. 5. 1 shows some of the different types of radiation in the electromagnetic spectrum. For Examiner’s Use gamma ltraviolet visible light infrared radio waves Fig. 5. 1 Write the names of the missing types of radiation in the two empty spaces. [2] (b) Fig. 5. 2 shows a ray of light hitting a mirror. air mirror 50° Fig. 5. 2 (i) On Fig. 5. 2, label the normal. (ii) On Fig. 5. 2, draw the reflected ray. (iii) State the value of the angle of reflection. ° [1] [1] [1] (c) A sound wave has a frequency of 500 Hz. (i) Explain the meaning of the term frequency. [1] (ii) State the approximate range of audible frequencies detected by the normal human ear. [1] © UCLES 2010 0653/21/O/N/10 11 (d) Fig. 5. 3 shows the wave traces made by four sounds.

For Examiner’s Use trace A trace B trace C trace D Fig. 5. 3 (i) Which trace shows the sound wave with the lowest pitch? [1] (ii) Which trace shows the sound wave with the smallest amplitude? [1] © UCLES 2010 0653/21/O/N/10 [Turn over 12 6 (a) Complete the sentences about the human nervous system, using some of the words in the list. For Examiner’s Use biceps nerves brain detectors effectors receptors Specialised cells in the human nervous system detect external stimuli. These cells are called . They convert the stimulus into electrical impulses in , which carry the impulse to the central nervous system.

The central nervous system then sends impulses to parts of the body that respond to the stimulus, such as muscles or glands. These parts are called . [3] (b) When we smell food, the salivary glands respond by secreting saliva. Saliva contains the enzyme amylase, which breaks down large starch molecules to smaller sugar molecules. (i) Explain what is meant by the term enzyme. [2] (ii) Name the process by which large molecules are broken down to small ones in the alimentary canal. [1] (iii) Explain why this process is necessary. [2] © UCLES 2010 0653/21/O/N/10 13 7 (a) Complete Table 7. to show the correct symbols of these electrical components. One symbol has been drawn for you. Table 7. 1 component lamp ammeter fixed resistor [2] (b) A student set up the electric circuit in Fig. 7. 1. It contained three lamps L1, L2 and L3. It contained three switches S1, S2 and S3. electrical symbol For Examiner’s Use S1 S3 L1 L2 L3 S2 Fig. 7. 1 In Table 7. 2, write the words ‘on’ or ‘off’ to show when each lamp is lit or not lit for each set of switch positions. Table 7. 2 switch position S1 S2 S3 closed open open [3] © UCLES 2010 0653/21/O/N/10 lamp ‘on’ or ‘off’ L1 L2 L3 losed closed closed closed closed open [Turn over 14 (c) The student then set up another electric circuit shown in Fig. 7. 2. For Examiner’s Use lamp A lamp B Fig. 7. 2 She noticed that neither lamp A nor lamp B lit up.

She found nothing wrong with lamp A but the filament in lamp B was broken. (i) Explain why lamp A did not light up. [1] (ii) She replaced lamp B with a new lamp C. The resistance of both lamp A and lamp C was 5 ohms when lit. Calculate the combined resistance of both lamps in the working circuit. State the formula that you use and show your working. formula used working ohms [2] UCLES 2010 0653/21/O/N/10 15 (d) Fig. 7. 3 shows an electrical device. For Examiner’s Use primary coil 20 turns 23 V a. c. secondary coil 200 turns Fig. 7. 3 (i) Name the device. [1] (ii) Calculate the output voltage. Use the formula Vp / Vs = Np / Ns. Show your working. V [1] © UCLES 2010 0653/21/O/N/10 [Turn over 16 8 In jet engines, hydrocarbon molecules from the jet fuel mix with air and burn. This releases a large amount of energy and produces a mixture of waste gases. These waste gases pass out through the back of the jet engine into the atmosphere. For Examiner’s Use waste gases air jet engine a) Fig. 8. 1 shows a molecule of octane, which is a typical hydrocarbon molecule in jet fuel. octane key carbon atom hydrogen atom Fig. 8. 1 (i) State the chemical formula of octane. [1] (ii) Complete the word equation below for the complete combustion of octane. octane + + [2] (iii) Explain why the mixture of gases coming from the rear of the jet engine contains a large amount of nitrogen. [2] (iv) Explain why the metallic parts of the jet engine become hot when it is working. [1] © UCLES 2010 0653/21/O/N/10 17 (b) (i) A carbon atom has a proton (atomic) number 6 and a nucleon (mass) number 12.

State the number of neutrons and electrons in this carbon atom. number of neutrons number of electrons [2] For Examiner’s Use (ii) State the chemical symbol of another element which is in the same group in the Periodic Table as carbon. [1] © UCLES 2010 0653/21/O/N/10 [Turn over 18 9 The gray wolf is a predator that lives in North America. For Examiner’s Use (a) The gray wolf’s diet consists mainly of white-tailed deer, beavers and snowshoe hares. These are all herbivores. They eat plants. (i) Construct a food web including all the organisms mentioned above. 3] (ii) State what the arrows in your food web represent. [1] (iii) Name the producers in the food web you have drawn. [1] © UCLES 2010 0653/21/O/N/10 19 (b) Some of the chemicals in a gray wolf’s body contain carbon. When a wolf dies, its body is broken down by decomposers and the carbon is returned to the air. (i) Name one type of chemical in a wolf’s body that contains carbon. [1] (ii) Explain how the carbon from a wolf’s body is returned to the air after the wolf dies. For Examiner’s Use [2] (c) Some gray wolves are born with darker fur than others. They can pass this fur colour to their offspring.

If wolves live in cold places, they grow longer fur than wolves that live in warm places. They cannot pass their fur length to their offspring. Tick two boxes to show the cause of each of these types of variation in wolves’ fur. cause genes only environment only genes and environment [2] fur colour fur length © UCLES 2010 0653/21/O/N/10 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.

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. © UCLES 2010 DATA SHEET The Periodic Table of the Elements Group III 1 I H Hydrogen II IV V VI VII 0 4 He Helium 1 11 12 14 16 19 2 20 7 9 Li Boron Carbon Be 5 27 28 6 7 B C N Nitrogen O Oxygen F Fluorine Ne Neon Lithium Beryllium 3 4 8 31 32 35. 5 10 40 23 24 Na Aluminium Mg 13 51 52 55 56 59 59 64 65 70 Al 14 Si Silicon P Phosphorus S Sulfur Cl Chlorine Ar Argon Sodium Magnesium 11 12 15 73 75 16 79 17 80 18 84 39 40 45 48 K Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Ca 23 93 96 101 103 106 108 112 24 25 26 27 28 29 30 Sc Ti V Cr Mn Fe Co Ni Cu Zn 31 Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Potassium Calcium Scandium Titanium 19 20 21 22 32 115 119 33 122 34 128 35 127 36 131 20 85 88 89 91 Rb Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Sr 41 181 184 186 190 192 195 197 42 43 44 45 46 47

Y Zr Nb Mo Tc Ru Rh Pd Ag 48 Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon 0653/21/O/N/10 49 201 Rubidium Strontium Yttrium Zirconium 37 38 39 40 50 204 207 51 209 52 53 54 133 137 139 178 Cs Tantalum Iridium Tungsten Rhenium Osmium Platinum Ba 73 77 74 75 76 78 La Ta W Re Os Pt Hf Ir 79 Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium At Astatine Rn Radon Caesium Barium Lanthanum Hafnium 55 56 57 * 72 80 81 82 83 84 85 86 226 227 Fr 140 141 144 150 Ra Ac 152 157 159 162 165 167 169 173 175 Francium Radium Actinium 87 88 89 *58-71 Lanthanoid series 90-103 Actinoid series Ce

Cerium Praseodymium Neodymium Promethium Pr 59 60 238 61 Nd Pm 62 Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium 58 232 63 64 65 66 67 68 69 70 71 a a = relative atomic mass Key Th Thorium Protactinium Uranium X Pa 91 92 X = atomic symbol 90 U 93 Np Neptunium Pu Plutonium Am Americium Cm Curium Bk Berkelium Cf Californium Es Einsteinium Fm Fermium Md Mendelevium No Nobelium Lr Lawrencium b b = proton (atomic) number 94 95 96 97 98 99 100 101 102 103 The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r. t. p. ).

Cite this Igcse Combined Science Past Paper Paper 2 0653/21 October/November 2010

Igcse Combined Science Past Paper Paper 2 0653/21 October/November 2010. (2017, Jan 31). Retrieved from https://graduateway.com/igcse-combined-science-past-paper-paper-2-065321-octobernovember-2010/

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