Cambridge IGCSE Science - Combined 0653 — 2015 May/June Paper 2 · Variant 2

This document consists of 21 printed pages and 3 blank pages. DC (LK/CGW) 98908/3 © UCLES 2015 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 8 3 8 2 4 3 4 7 1 7 * COMBINED SCIENCE 0653/22 Paper 2 (Core) May/June 2015 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 an HB soft pencil for any diagrams, graphs, tables or rough working. 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 0653/22/M/J/15 © UCLES 2015 1 (a) Table 1.1 gives some facts about one atom of the element sodium and the position of sodium in the Periodic Table. Table 1.1 element Group proton number nucleon number sodium I 11 23 (i) From the information in Table 1.1, deduce the following information about the atomic structure of sodium. the number of electrons in a sodium atom … the number of neutrons in this sodium atom … [2] (ii) Deduce the number of electrons a sodium atom loses when it forms an ion. number of electrons lost … explanation … …[1] (b) Fig. 1.1 shows a demonstration of the reaction between hydrogen and the oxygen in air. gas jar drops of a colourless liquid cover mixture of hydrogen and air Fig. 1.1 A burning splint is placed over a gas jar containing a mixture of hydrogen and air. The cover is removed. The mixture explodes.

3 0653/22/M/J/15 © UCLES 2015 [Turn over (i) Drops of a colourless liquid are observed inside the gas jar. Describe a chemical test and the result of this test that shows that the liquid is water. test … … result …[2] (ii) Write a word equation for the reaction between hydrogen and oxygen. …[1] (iii) State the type of bond formed between hydrogen and oxygen atoms in this reaction. Explain your answer. type of bond … explanation … …[2]

4 0653/22/M/J/15 © UCLES 2015 2 (a) Most large molecules in living organisms are made by joining many smaller molecules together. An example of this is glycogen which is made from glucose molecules. A short length of glycogen is shown in Fig. 2.1. small molecule part of large molecule glucose glycogen Fig. 2.1 Some of the small molecules that join together to make large molecules in living organisms are shown in Fig. 2.2. glucose fatty acid amino acid glycerol Fig. 2.2 (i) Select molecules from Fig. 2.2 and make drawings in Table 2.1 to show how protein and starch are made up. Your diagrams should be similar to Fig. 2.1. Table 2.1 large molecule small molecule part of large molecule protein starch [4]

5 0653/22/M/J/15 © UCLES 2015 [Turn over (ii) Energy is needed in cells to build large molecules from small ones. Describe how energy is released in cells for this process. … … …[2] (b) (i) A plant usually gets its nitrogen in the form of nitrate ions which are dissolved in the water in the soil. Describe the path taken by nitrate ions from the soil to the leaves. … … …[2]

6 0653/22/M/J/15 © UCLES 2015 (ii) Fig. 2.3 shows a Venus flytrap. This plant grows in areas where the soil does not have enough nitrogen. A source of the element nitrogen is needed to make proteins. leaf Fig. 2.3 The Venus flytrap captures and digests insects. The insect shown in Fig. 2.4 lands on the open leaf. The leaf then traps the insect by closing around it very quickly. insect insect open leaf closed leaf Fig. 2.4 State two characteristics of living things which the Venus flytrap shows when it traps a fly. 1 … 2 …[2] (iii) When the leaves of the Venus flytrap are open they look like flowers in order to attract insects. Suggest two features the leaves may have that would enable them to look like flowers. 1 … 2 …[2]

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8 0653/22/M/J/15 © UCLES 2015 3 The pole vault is an athletics event in which the athlete attempts to get over a very high bar with the help of a long pole. Fig. 3.1 shows an athlete at five stages during a pole vault. stage 1 stage 2 stage 3 stage 4 stage 5 landing mat Fig. 3.1 The athlete runs with his pole, places the pole in the ground and pushes himself upwards. He rises to the height of the bar, remains there for a brief moment, then falls over the bar to the landing mat. Fig. 3.2 shows a simplified graph of the athlete’s speed during the pole vault. 1 1 2 0 3 time/s 4 0 2 3 4 speed m / s 5 A B C Fig. 3.2 (a) The letters A, B and C on the graph in Fig. 3.2 correspond to three of the five stages in the pole vault shown in Fig. 3.1. Explain why A on the graph corresponds to stage 1. … …[1]

9 0653/22/M/J/15 © UCLES 2015 [Turn over (b) The energy of the athlete changes during this pole vault. He starts with chemical energy in his muscles. State the main energy changes that follow between stages 3 and 5 before he lands on the mat. from chemical energy to kinetic energy to … energy to … energy [2] (c) (i) Describe the motion of the athlete between points B and C. …[1] (ii) Explain why the motion described in (i) occurs between points B and C. …[1] (d) Calculate the distance travelled by the athlete in the first 2 seconds shown on the graph in Fig. 3.2. State the formula that you use and show your working. formula: working: distance = … m [2] (e) The pole used by the athlete is made of metal. In the box below, draw a diagram to show the arrangement of atoms in the solid metal. One atom has been drawn for you. You need to draw at least 11 more. [2]

10 0653/22/M/J/15 © UCLES 2015 4 (a) Fig. 4.1 shows a sample of rock containing bands of iron oxide. quartz (silicon dioxide) iron oxide Fig. 4.1 Some information about the formation of this rock is shown below: • this rock was formed about 2.5 billion years ago; • oxygen was produced by bacteria in the oceans; • iron compounds were dissolved in the oceans; • iron compounds were oxidised by reacting with oxygen to make insoluble iron oxide; • iron oxide settled on the ocean bed to produce the dark layers in the rock. (i) State one physical change and one chemical change that occurred when the rock shown in Fig. 4.1 was formed. physical change … … chemical change … …[2] (ii) Describe the difference between a physical change and a chemical change. … …[1]

11 0653/22/M/J/15 © UCLES 2015 [Turn over (b) Fig. 4.2 shows the approximate composition of the Earth’s atmosphere 3 billion years ago. nitrogen carbon dioxide Fig. 4.2 Describe two differences and one similarity between this and our present day atmosphere. difference 1 … difference 2 … similarity …[3] (c) Another type of rock contains copper oxide. When a piece of this rock is added to dilute hydrochloric acid, the pH of the solution increases. Explain why this occurs. … …[1] (d) Copper metal can be extracted from the rock containing copper oxide. (i) Explain why the extraction of copper from copper oxide is called reduction. …[1] (ii) Describe how copper can be extracted from copper oxide in the laboratory. … … …[2]

12 0653/22/M/J/15 © UCLES 2015 5 Fig. 5.1 shows the internal structure of the heart. B A left ventricle Fig. 5.1 (a) On Fig. 5.1 (i) draw a label line and the letter P to show the pulmonary artery, [1] (ii) draw arrows to show the direction of blood flow through the left side of the heart. [2] (b) (i) A and B are valves. Describe the function of the valves in the heart. … …[1] (ii) Explain why valve A closes when the left ventricle contracts. … …[1] (c) The red cells in the blood contain haemoglobin. Describe the function of haemoglobin. … …[1]

13 0653/22/M/J/15 © UCLES 2015 [Turn over (d) The blood also contains platelets. Describe the function of platelets and explain why this is important. … … …[2]

14 0653/22/M/J/15 © UCLES 2015 6 (a) Electromagnetic waves have many uses. Name one type of electromagnetic wave and state one example of a use for that type of wave. name … use … …[2] (b) Fig. 6.1 shows apparatus called a ripple tank. This is used by students for experiments to investigate water waves. The electric motor causes the board to vibrate. At a constant speed of rotation the motor produces waves at a constant rate. power supply water waves water waves vibrating board shallow tank of water electric motor Fig. 6.1 Fig. 6.2 shows a close-up side view of some water waves during an experiment in the tank. direction of travel of waves P Fig. 6.2 (i) Describe what is meant by wave motion, using the water waves shown in Fig. 6.2 as an example. … … …[2]

15 0653/22/M/J/15 © UCLES 2015 [Turn over (ii) Fig. 6.2 shows a change in the wave pattern at point P. From the diagram in Fig. 6.2 state one property of the wave motion that changes at point P and describe how this changes, … … one property of the wave motion that does not change at point P. … [3] (c) As the speed of the motor is increased, the board vibrates more rapidly. When the board is vibrating at 10 vibrations per second, the students cannot hear any sound. When the board is vibrating at 30 vibrations per second, the students can hear a sound with a low pitch. Explain why the students cannot hear any sound when the board makes 10 vibrations per second. … …[1]

16 0653/22/M/J/15 © UCLES 2015 7 (a) A copper compound contains two carbon atoms and four oxygen atoms for every copper atom. Write the chemical formula for the compound. …[2] (b) Fig. 7.1 shows the electrolysis of copper chloride solution. copper chloride solution carbon electrodes power supply + – Fig. 7.1 Copper is deposited on one of the electrodes. (i) Describe the appearance of the copper that is deposited. … …[1] (ii) State the polarity of the electrode where the copper is deposited. … [1] (iii) State the name of the electrode where the copper is deposited. … [1]

17 0653/22/M/J/15 © UCLES 2015 [Turn over (c) A student carries out experiments to compare the reactivity of some metals. Fig. 7.2 shows test-tubes containing pieces of calcium and magnesium. Some water is added to each test-tube. test-tube 1 calcium test-tube 2 water magnesium Fig. 7.2 Describe what the student observes in each test-tube and state, with a reason, which metal is the more reactive. test-tube 1 … test-tube 2 … This means that … is the more reactive metal because … …[2] (d) (i) Use the Periodic Table on page 24 to write the first three members of Group I, the alkali metals, in order of reactivity. most reactive ……………………… ……………………… least reactive ……………………… [1] (ii) When a piece of sodium is dropped into a trough of water it melts, skims over the surface and produces bubbles of gas. Describe how the observations would be different if a piece of potassium is used instead of sodium. … …[1]

18 0653/22/M/J/15 © UCLES 2015 8 (a) Large areas of forest are cleared in some parts of the world so that the land can be used to grow crops. Fig. 8.1 shows the burning of trees to clear forests. 3. wind carries smoke to neighbouring trees 1. trees being felled 2. combustion of wood Fig. 8.1 When the trees burn, smoke is produced that contains carbon particles. The wind carries the smoke to neighbouring trees. This affects the rate of photosynthesis in these trees. Complete the sentences below using words from the list. You may use each word once, more than once, or not at all. carbon dioxide chlorophyll increased light oxygen reduced unchanged water The rate of photosynthesis is … because particles of carbon landing on the upper surface of the leaves prevent … being absorbed by the leaf. The rate of photosynthesis is … because particles of carbon blocking the stomata in the leaves prevent … being absorbed by the leaf. [4] (b) Deforestation causes the concentration of carbon dioxide in the Earth’s atmosphere to increase. Describe one consequence of an increase in the carbon dioxide concentration of the Earth’s atmosphere. … …[1] (c) Describe the undesirable effects of deforestation on the animal life in the forest. … … …[2]

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20 0653/22/M/J/15 © UCLES 2015 9 A student is building a model motorcycle. Fig. 9.1 shows a circuit he designs for the electrical equipment he wants on the motorcycle. sidelamp headlamp rear lamp 12 V Fig. 9.1 (a) Fig. 9.2 shows the lamps he uses for his model. The markings on the lamps are shown below the pictures. sidelamp headlamp 12 V, 0.5 A rear lamp 12 V, 0.5 A 12 V, 2 A Fig. 9.2 State and explain what is meant by the quantity ‘12 V’ on the lamps. … …[2]

21 0653/22/M/J/15 © UCLES 2015 [Turn over (b) When the student switches on the circuit in Fig. 9.1, the lamps glow only very faintly. He has not designed his circuit correctly. On Fig. 9.3 complete the circuit diagram to show the sidelamp and rear lamp connected so that all the lamps glow brightly. headlamp 12 V Fig. 9.3 [2] (c) The sidelamp is replaced with a new lamp that uses a lower current when connected to the 12 V battery. State the property of the new lamp that is different from the old lamp in order to use less current and describe how it is different. … …[1]

22 0653/22/M/J/15 © UCLES 2015 (d) Each lamp contains a thin wire filament surrounded by a glass bulb attached to a metal base. The space inside the glass bulb is filled with a gas. When the lamp is lit, the filament reaches a very high temperature. wire filament glass bulb, filled with gas metal base After the lamps have been lit for a few minutes, the glass bulbs become hot. Describe and explain two ways by which heat energy can be transferred from the hot filament to the glass bulb. 1 … … 2 . … … [4]

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24 0653/22/M/J/15 © UCLES 2015 To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series. Group 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 91 238 231 147 237 244 243 247 247 251 252 257 258 259 260 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 82 209 209 210 222 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 55 226 223 Ra Radium 88 a X b a = relative atomic mass X = atomic symbol b = atomic (proton) number Key DATA SHEET * 58–71 Lanthanoid series † 90–103 Actinoid series The volume of one mole of any gas is 24dm3 at room temperature and pressure (r.t.p.).

® IGCSE is the registered trademark of Cambridge International Examinations. CAMBRIDGE INTERNATIONAL EXAMINATIONS Cambridge International General Certificate of Secondary Education MARK SCHEME for the May/June 2015 series 0653 COMBINED SCIENCE 0653/22 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 May/June 2015 series for most Cambridge IGCSE®, Cambridge International A and AS Level components and some Cambridge O Level components.

Page 2 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2015 0653 22 © Cambridge International Examinations 2015 1 (a) (i) 11 ; 12 ; [2] (ii) 1 because sodium is in group 1 / atom has 1 electron in outer shell ; [1] (b) (i) cobalt chloride (test paper) / anhydrous cobalt chloride ; goes (from blue to) pink ; OR anhydrous copper sulfate ; goes (from white to) blue ; [2] (ii) hydrogen + oxygen → water ; [1] (iii) covalent ; hydrogen and oxygen are non-metals / description of covalency in terms of electron sharing ; (allow forms a liquid at room temperature) [2] [Total: 8] 2 (a) (i) amino acid correct ; glucose molecule correct ; two or more amino acids joined together and two or more glucose molecules joined together ; continuation bonds shown / any indication that the molecules continue ; [4] (ii) by respiration ; nutrient / glucose molecules are broken down by chemical reactions ; [2] (b) (i) taken up / absorbed by root (hair cells) ; through xylem ; through stem ; [max 2] (ii) sensitivity ; movement ; [2] (iii) (bright) colour ; large size ; similar shape to petals / look like petals ; avp ; [max 2] [Total: 12]

Page 3 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2015 0653 22 © Cambridge International Examinations 2015 3 (a) running at constant speed ; [1] (b) (gravitational) potential (energy) ; kinetic (energy) ; [2] (c) (i) decelerates then accelerates ; [1] (ii) gravitational force / weight (accept gravity) ; [1] (d) (distance =) speed × time (in any form) ; = 4 × 2 = 8 (m) ; [2] (e) or acceptable equivalent with at least 12 spheres in total regular pattern ; most touching ; [2] [Total: 9] 4 (a) (i) physical: (iron oxide) settled / produced layers in rock / iron compounds dissolved ; chemical: compounds oxidised to iron oxide / oxygen produced by bacteria ; [2] (ii) chemical change produces a new substance / v.v. ; [1] (b) differences: no oxygen in ancient atmosphere / v.v. ; more carbon dioxide in ancient atmosphere / v.v. ; (assume reference to ancient atmosphere if not specified) similarity : nitrogen largest component ; [3]

Page 4 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2015 0653 22 © Cambridge International Examinations 2015 (c) copper oxide neutralises the acid ; [1] (d) (i) reduction is removal of oxygen ; [1] (ii) carbon / charcoal / etc. ; heat ; allow other workable method [2] [Total: 10] 5 (a) (i) pulmonary artery correctly labelled ; [1] (ii) arrow going from atrium to ventricle ; arrow going from ventricle through the aorta ; [2] (b) (i) makes the blood flow in one direction ; [1] (ii) (valve A closes) because the pressure (of blood) in the ventricle is greater than in the atrium ; [1] (c) to carry oxygen ; [1] (d) needed for clotting of blood ; prevents excessive blood loss / prevents entry of pathogens ; [2] [Total: 8] 6 (a) gamma rays / X-rays / ultra-violet / visible / infrared / microwave / radio (any one) ; relevant useful job for type selected ; [2] (b) (i) up and down motion / oscillation / vibration / owtte ; correct reference to wavelength / amplitude shown in diagram ; [2] (ii) wavelength ; decreases ; or speed ; slows down ; frequency / amplitude / direction of wave flow ; [3] (c) frequency less than lower limit of hearing ; [1] [Total: 8]

Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2015 0653 22 © Cambridge International Examinations 2015 7 (a) symbols: Cu, C and O ; CuC2O4 ; allow elements in any order [2] (b) (i) brown / pink (solid) ; [1] (ii) negative ; [1] (iii) cathode ; [1] no ecf (c) more bubbles / more heat produced, in test-tube 1 than in test-tube 2 ; (allow no bubbles apparent with magnesium) calcium (is more reactive) ; because gas is displaced / evolved, more quickly ; [max 2] (d) (i) (most reactive) potassium sodium (least reactive) lithium ; [1] (ii) ignition / skims faster / bubbles produced faster / avp ; [1] [Total: 9] 8 (a) reduced ; light ; reduced ; carbon dioxide ; [4] (b) increases global warming / description of effect ; [1] (c) loss of habitat ; killed in fire / leave the forest ; loss of food supply ; [max 2] [Total: 7]

Page 6 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2015 0653 22 © Cambridge International Examinations 2015 9 (a) V represents voltage / volts / potential difference ; needed to drive the (required) current through the lamp ; 12 V is a safe maximum requirement for the bulb to work properly / above this voltage the bulb would break ; [max 2] (b) side and rear lamps in parallel with headlamp ; side and rear lamps in parallel with each other ; [2] (c) new lamp has higher resistance / thinner filament / longer filament ; [1] (d) any two pairs from: conduction… ; …from filament to metal (filament and base) ; convection… ; …of heated gas / through gas ; radiation ;… … of infra-red / absorbed by glass ; [max 4] [Total: 9]