Cambridge IGCSE Sciences - Co-ordinated (Double) 0654 — 2016 May/June Paper 3 · Variant 1

This document consists of 30 printed pages and 2 blank pages. DC (ST/SG) 109969/4 © UCLES 2016 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 2 2 4 1 0 6 0 6 5 5 * CO-ORDINATED SCIENCES 0654/31 Paper 3 (Extended) May/June 2016 2 hours 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 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 32. 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 0654/31/M/J/16 © UCLES 2016 1 Fig. 1.1 shows a house. wind turbine solar panels Fig. 1.1 In the garden of the house there is a wind turbine. (a) The house is painted white. Suggest why houses are often painted white in hot countries. … …[1] (b) The wind turbine generates electricity. State the main energy transformation in the wind turbine. … energy to … energy. [1] (c) There are solar panels on the roof of the house. Energy from the Sun heats 4 kg of water in the panels. The energy falling on the solar panels is 400 000 J. (i) The efficiency of the solar panels is 15%. Calculate the thermal energy gained by the water. thermal energy gained = … J [2]

3 0654/31/M/J/16 © UCLES 2016 [Turn over (ii) Calculate the temperature rise in the 4 kg of water heated in the solar panels. The specific heat capacity of water is 4200 J / kg °C. State the formula you use and show your working. formula working increase in temperature = … °C [2] (d) Wind energy and energy from the Sun are both examples of renewable energy resources. State two other renewable energy resources. 1 … 2 … [2] (e) Visible light from the Sun is part of the electromagnetic spectrum. (i) Place visible light in the correct position in the incomplete electromagnetic spectrum below. X-rays infra-red radio waves [1] (ii) State the speed at which all electromagnetic waves travel. speed = … m / s [1]

4 0654/31/M/J/16 © UCLES 2016 (f) The household circuits use alternating current. Fig. 1.2 shows the graph of current against time. current 0 time Fig. 1.2 On Fig. 1.2, use a double headed arrow ( ) to indicate the amplitude. [1]

5 0654/31/M/J/16 © UCLES 2016 [Turn over 2 (a) Fig. 2.1 shows a flower as seen from the side and the same flower in a horizontal section taken along the line X–X. X X side view of flower horizontal section of flower Fig. 2.1 (i) On the horizontal section, label a sepal and a stamen. [2] (ii) State how it will affect the plant if all the stamens are removed from the flower. … …[1] (iii) This flower is pollinated by insects. State two features, visible in Fig. 2.1, that show it is an insect-pollinated flower. 1 … 2 … [2]

6 0654/31/M/J/16 © UCLES 2016 (b) Fig. 2.2 shows a fruit from a maple tree. ¶ZLQJ·RIIUXLW IUXLWZDOO SRVLWLRQ RIVHHG Fig. 2.2 A student observed the fruits that fell from a maple tree. He measured the horizontal distance from the tree to the place where each fruit landed. Fig. 2.3 shows the student’s results. 40 35 30 25 20 15 10 5 0 0.0–4.9 5.0–9.9 10.0–14.9 15.0–19.9 20.0–24.9 25.0–29.9 30.0–34.9 35.0–100.0 distance from parent tree / m number of fruits Fig. 2.3 (i) State the number of fruits that landed less than 10 m from the parent tree. …[1] (ii) Fig. 2.3 shows the eight different distance ranges chosen by the student. State the distance range within which the most fruits landed. …[1] (iii) Suggest why so many fruits landed within this distance range. … …[1]

7 0654/31/M/J/16 © UCLES 2016 [Turn over (iv) State two advantages for the maple tree of the seeds inside its fruits being dispersed away from the parent tree. 1 … … 2 … … [2] (v) Maple fruits are dispersed by the wind. State one other way in which the fruits or seeds of trees may be dispersed. …[1] (vi) State and explain how you would expect the student’s results to have been different if the tree had been taller, … … the weather had been windier. … … [2]

8 0654/31/M/J/16 © UCLES 2016 (c) Fig. 2.4 shows the outline of the testa of a seed, such as a bean seed. Inside this outline, draw a plant embryo as it would appear in longitudinal section (with the seed cut lengthways). On your drawing, label the radicle, plumule and cotyledon. Fig. 2.4 [4]

9 0654/31/M/J/16 © UCLES 2016 [Turn over Please turn over for Question 3.

10 0654/31/M/J/16 © UCLES 2016 3 (a) In many countries, water for drinking is taken from rivers and lakes. The water contains insoluble materials and microorganisms. (i) Name the process that is used to remove insoluble materials. …[1] (ii) Microorganisms are destroyed by treating the water with chlorine. Suggest the risk to humans if microorganisms are not destroyed before water is sent into homes. … …[1] (b) Fig. 3.1 shows apparatus used to produce chlorine gas. d.c. power supply anode sodium chloride solution chlorine gas gas R cathode Fig. 3.1 Chlorine gas is produced when an electric current passes through a concentrated solution of sodium chloride. (i) Name the process shown in Fig. 3.1. …[1] (ii) Name gas R. …[1]

11 0654/31/M/J/16 © UCLES 2016 [Turn over (iii) Describe a safe chemical test for chlorine and give the positive result: … … …[2] (iv) Before it is used to produce chlorine, the solution of sodium chloride in Fig. 3.1 is neutral. Predict and explain the change in the pH value of the solution during the process. pH changes from … to … explanation … … … [2] (v) Draw a bonding diagram that shows the arrangement of the outer electrons in a chlorine molecule. [2]

12 0654/31/M/J/16 © UCLES 2016 4 (a) Fig. 4.1 shows a graph of the motion of a truck over 40 seconds. 20 25 15 10 5 0 0 10 20 30 40 A B C D E time / s m / s speed Fig. 4.1 (i) Calculate the acceleration of the truck between B and C. Show your working. acceleration = … m / s2 [2]

13 0654/31/M/J/16 © UCLES 2016 [Turn over (ii) The mass of the truck is 2000 kg. Calculate the size of the force needed for the acceleration between B and C. State the formula you use and show your working. State the units. formula working force = … unit = … [3] (iii) Calculate the distance travelled by the truck in the time that the speed is decreasing. Show your working. distance = … m [2]

14 0654/31/M/J/16 © UCLES 2016 (b) The driver stops the truck. He receives an electric shock when he gets out of the truck. (i) Suggest why the driver receives an electric shock. … … … …[2] (ii) The shock is caused by a current of 0.004 A passing for 0.1 ms. Calculate the charge which passes. State the formula you use and show your working. formula working charge = … C [2]

15 0654/31/M/J/16 © UCLES 2016 [Turn over 5 Fig. 5.1 shows part of the carbon cycle. coal, oil and gas gradual production of fossil fuels carbon dioxide in atmosphere X Y Fig. 5.1 (a) Name the processes labelled X and Y. X … Y … [2] (b) Explain how the following human activities increase the amount of carbon dioxide in the air. (i) deforestation … … … … …[3] (ii) using fuels in power stations … …[1]

16 0654/31/M/J/16 © UCLES 2016 6 (a) (i) The elements in the Periodic Table are placed in order of increasing proton number. Define the term proton number. … …[1] (ii) State two differences between the properties of a proton and an electron. 1 … … 2 … … [2] (b) Caesium, Cs, is an element in Group I of the Periodic Table. Iodine, I, is a halogen in Group VII. Caesium combines with iodine to form the compound caesium iodide. (i) State the number of electrons in the outer shells (valence shells) of atoms of these elements. number of outer shell electrons in caesium … number of outer shell electrons in iodine … [1] (ii) Predict the chemical formula for caesium iodide and name the type of bonding involved. chemical formula … type of bonding …[2] (iii) Describe how the arrangements of the electrons in the atoms of caesium and iodine change when they combine. … … …[2]

17 0654/31/M/J/16 © UCLES 2016 [Turn over (c) The graph in Fig. 6.1 shows the maximum mass of caesium iodide that dissolves in 100 cm3 of water at different temperatures. 250 200 150 100 50 0 0 10 20 30 40 50 60 70 80 90 100 temperature / °C mass of caesium iodide dissolved / g Fig. 6.1 (i) Describe the trend shown in Fig. 6.1. … …[1] (ii) State the mass of caesium iodide that dissolves in 100 cm3 of water at 48 °C. mass = … g [1] (iii) Calculate the concentration, in mol / dm3, of the caesium iodide solution at 48 °C. Show your working. concentration = … mol / dm3 [3]

18 0654/31/M/J/16 © UCLES 2016 7 (a) Below is a list of materials. aluminium copper glass iron plastic From the list choose one material to match each description below. Each material can be used once, more than once or not at all. • It can be charged by rubbing with a cloth. … • It can be used as the core in a transformer. … • It can be used to make a lens. … • It is used as the conductor in the windings of a transformer. … [2] (b) One nuclide of iron is represented in nuclide notation as 54 26Fe. (i) For one neutral atom of 54 26Fe, state its nucleon number. … [1] (ii) Another isotope of iron has two more neutrons in the nucleus. Use similar notation to that used in (b)(i) to represent this nuclide. … [1] (iii) An isotope of iron is radioactive. It has a half-life of 2.73 years. State what is meant by the term half-life. … … …[1] (c) The boiling point of iron is 2862 °C. Some iron evaporates at a temperature below this. Describe one difference between evaporation and boiling. … …[1]

19 0654/31/M/J/16 © UCLES 2016 [Turn over (d) Fig. 7.1 shows an iron bar suspended by a string. A magnet is brought close to the iron bar. The iron bar is attracted to the magnet. N S direction of movement bar magnet iron bar string wooden stand Fig. 7.1 Explain why the iron bar is attracted to the magnet. … …[1]

20 0654/31/M/J/16 © UCLES 2016 (e) Iron is an example of a solid at room temperature. The three diagrams A, B and C in Fig. 7.2 show the different arrangements of particles in the three states of matter. A B C Fig. 7.2 Use the correct letter A, B or C from Fig. 7.2 to fill in the blank and complete the statement to explain your choice. Diagram … shows solid iron because the particles … … [1] (f) A student is trying to calculate the density of an irregular piece of iron. To do this he must measure the mass and the volume of the piece of iron. Describe how the student could measure the volume of the piece of iron us ing a measuring cylinder. … … … … …[2]

21 0654/31/M/J/16 © UCLES 2016 [Turn over 8 (a) Too much fat in the diet is a form of malnutrition. Describe the harmful effects of too much fat in the diet. … … … …[3] (b) Fig. 8.1 shows the structure of the human alimentary canal and associated organs. Fig. 8.1 (i) On Fig. 8.1, label a gland that secretes bile. [1] (ii) Describe the role of bile in fat digestion. … … …[2] (iii) Describe how the structure of the villi in the small intestine helps in the efficient absorption of fats. … … …[2]

22 0654/31/M/J/16 © UCLES 2016 9 Fig. 9.1 shows a meteorite. Meteorites contain a mixture of iron and nickel. meteorite made of a mixture of iron and nickel Fig. 9.1 (a) (i) Name the collection of metals in the Periodic Table that contains both iron and nickel. …[1] (ii) State two properties that are typical of the collection of metals in (a)(i) that are not shared by all metals. 1 … 2 … [2] (iii) Iron will rust in the presence of air and water. State and explain, in terms of a change in the number of electrons, which particles are oxidised when iron rusts. … … …[2] (iv) Meteorites do not form rust in the presence of air and water. Suggest a reason for this. … …[1]

23 0654/31/M/J/16 © UCLES 2016 [Turn over (b) Iron is extracted from iron compounds found in the Earth’s crust. Fig. 9.2 shows a diagram of the industrial extraction of iron. iron impurities raw materials including iron oxide iron moving down carbon monoxide rising to react with iron oxide Fig. 9.2 (i) Name the industrial apparatus shown in Fig. 9.2. …[1] (ii) Inside the apparatus, iron oxide, Fe2O3, is reduced by carbon monoxide, CO. Write the balanced equation for this reaction. …[2]

24 0654/31/M/J/16 © UCLES 2016 10 (a) A school has a corner in a corridor where the students are likely to collide. To avoid collisions, a plane mirror is placed across the corner. This is shown in Fig. 10.1. Y X corridor plane mirror science laboratory Fig. 10.1 Student X is able to see student Y around the corner by using the mirror. (i) On Fig. 10.1, draw a ray of light from student Y so that it reflects off the mirror and is seen by student X. [1] (ii) Draw and label the normal. [1] (iii) On Fig. 10.1, label the angle of incidence of the ray of light with an i. [1] (iv) At the corner, student X sees her own image in the mirror. Select three words or phrases from the list below that describe her image correctly. larger than object real same size as object smaller than object upright upside down virtual 1 … 2 … 3 … [1]

25 0654/31/M/J/16 © UCLES 2016 [Turn over (b) The corridor is very noisy. Sound waves travel through the air by a series of compressions and rarefactions. Describe the difference between a compression and a rarefaction. … …[1] (c) In the school science laboratory, a student builds an electric circuit. Fig. 10.2 shows a circuit diagram for the circuit. 4 1 12 1 V A Fig. 10.2 (i) Name the instruments represented by each symbol. A … V … [1] (ii) Calculate the combined resistance of the two resistors. State the formula you use and show your working. formula working resistance = … Ω [2]

26 0654/31/M/J/16 © UCLES 2016 11 Mice usually have brown fur due to the presence of dominant alleles for brown. (a) (i) Using F for the dominant alleles and f for the recessive alleles, state all the possible genotypes of a brown mouse. …[1] (ii) Suggest why some mice have white fur even though the alleles for white are recessive. … …[1] (b) It is an advantage for mice to have brown fur rather than white fur. (i) Suggest why having brown fur would be an advantage. … …[1] (ii) Explain why a white mouse is less likely than a brown mouse to pass on its alleles to the next generation. … … …[2]

27 0654/31/M/J/16 © UCLES 2016 [Turn over (c) The length of the fur in mice is also genetically determined. Short fur is dominant to long fur. Complete the genetic diagram to show the result of crossing two mice with short fur. Include both genotypes and phenotypes for the offspring and state the ratio of the phenotypes. parents phenotypes short fur short fur genotypes Hh Hh gametes … … … … offspring male gametes … … female gametes … … … … … … … … … … ratio of phenotypes … : … [4]

28 0654/31/M/J/16 © UCLES 2016 12 (a) Fig. 12.1 shows diagrams of the arrangement of atoms in two forms of carbon, L and M. L M Fig. 12.1 (i) Name the structures of carbon shown in Fig. 12.1. L … M … [1] (ii) Explain, in terms of its atoms, why carbon is an example of an element and not a compound. … …[1]

29 0654/31/M/J/16 © UCLES 2016 (iii) Fig. 12.2 shows a pencil line being drawn on paper. The form of carbon used in pencils has one of the structures shown in Fig. 12.1. pencil material containing carbon is transferred from the pencil to the paper Fig. 12.2 Suggest which form of carbon, L or M in Fig. 12.1, is used in pencils. … Explain how the structure of this substance makes it possible for a pencil to draw a line on paper. … … … … [2] (b) Charcoal is a solid fuel that contains carbon. (i) The word equation for the complete combustion of carbon is shown. carbon + oxygen carbon dioxide (reactants) (product) Suggest and explain whether the reactants or the product possess the larger amount of chemical potential energy. … … …[2] (ii) Explain, in terms of collisions involving molecules, why powdered charcoal burns more quickly than large pieces of charcoal. … … … …[2]

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32 0654/31/M/J/16 © UCLES 2016 Group The Periodic Table of Elements 1 H hydrogen 1 2 He helium 4 I II III IV V VI VII VIII 3 Li lithium 7 4 Be beryllium 9 atomic number atomic symbol Key name relative atomic mass 11 Na sodium 23 12 Mg magnesium 24 19 K potassium 39 20 Ca calcium 40 37 Rb rubidium 85 38 Sr strontium 88 55 Cs caesium 133 56 Ba barium 137 87 Fr francium – 88 Ra radium – 5 B boron 11 13 Al aluminium 27 31 Ga gallium 70 49 In indium 115 81 Tl thallium 204 6 C carbon 12 14 Si silicon 28 32 Ge germanium 73 50 Sn tin 117 82 Pb lead 207 22 Ti titanium 48 40 Zr zirconium 91 72 Hf hafnium 178 104 Rf rutherfordium – 23 V vanadium 51 41 Nb niobium 93 73 Ta tantalum 181 105 Db dubnium – 24 Cr chromium 52 42 Mo molybdenum 96 74 W tungsten 184 106 Sg seaborgium – 25 Mn manganese 55 43 Tc technetium – 75 Re rhenium 186 107 Bh bohrium – 26 Fe iron 56 44 Ru ruthenium 101 76 Os osmium 190 108 Hs hassium – 27 Co cobalt 59 45 Rh rhodium 103 77 Ir iridium 192 109 Mt meitnerium – 28 Ni nickel 59 46 Pd palladium 106 78 Pt platinum 195 110 Ds darmstadtium – 29 Cu copper 64 47 Ag silver 108 79 Au gold 197 111 Rg roentgenium – 30 Zn zinc 65 48 Cd cadmium 112 80 Hg mercury 201 112 Cr copernicium – 114 Fl flerovium – 116 Lv livermorium – 7 N nitrogen 14 15 P phosphorus 31 33 As arsenic 75 51 Sb antimony 122 83 Bi bismuth 209 8 O oxygen 16 16 S sulfur 32 34 Se selenium 79 52 Te tellurium 128 84 Po polonium – 9 F fluorine 19 17 Cl chlorine 35.5 35 Br bromine 80 53 I iodine 127 85 At astatine – 10 Ne neon 20 18 Ar argon 40 36 Kr krypton 84 54 Xe xenon 131 86 Rn radon – 21 Sc scandium 45 39 Y yttrium 89 57–71 lanthanoids 89–103 actinoids 57 La lanthanum 139 89 Ac lanthanoids actinoids The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.) actinium – 58 Ce cerium 140 90 Th thorium 232 59 Pr praseodymium 141 91 Pa protactinium 231 60 Nd neodymium 144 92 U uranium 238 61 Pm promethium – 93 Np neptunium – 62 Sm samarium 150 94 Pu plutonium – 63 Eu europium 152 95 Am americium – 64 Gd gadolinium 157 96 Cm curium – 65 Tb terbium 159 97 Bk berkelium – 66 Dy dysprosium 163 98 Cf californium – 67 Ho holmium 165 99 Es einsteinium – 68 Er erbium 167 100 Fm fermium – 69 Tm thulium 169 101 Md mendelevium – 70 Yb ytterbium 173 102 No nobelium – 71 Lu lutetium 175 103 Lr lawrencium – 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.

® IGCSE is the registered trademark of Cambridge International Examinations. This document consists of 8 printed pages. © UCLES 2016 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education CO-ORDINATED SCIENCES 0654/31 Paper 3 Extended Theory May/June 2016 MARK SCHEME Maximum Mark: 120 Published 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 2016 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 2016 0654 31 © Cambridge International Examinations 2016 1 (a) white surfaces are better reflectors of thermal energy / white surfaces are poorer absorbers of thermal energy ; [1] (b) kinetic to electrical ; [1] (c) (i) efficiency = energy out / energy in or energy used = 15 / 100 × 400 000 ; = 60 000 (J) ; [2] (ii) (temperature rise =) energy / mass × shc or 60 000 / (4 × 4200) ; 3.6 (°C) ; [2] (d) tidal, wave, geothermal, HEP, (named) biomass: any two ;; [2] (e) (i) in space of left of infra-red ; X rays visible light infra-red radio waves [1] (ii) 300 000 000 / 3 × 108 (m / s) ; [1] (f) amplitude correctly indicated ; either : [1] [Total: 11]

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Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2016 0654 31 © Cambridge International Examinations 2016 (b) (i) CO2 used for photosynthesis ; less CO2 absorbed / less photosynthesis ; CO2 produced by burning timber / CO2 produced by decomposition / AW [3] (ii) because combustion produced CO2 ; [1] [Total: 6] 6 (a) (i) number of protons in the nucleus / one atom ; [1] (ii) proton positive(ly charged) and electron negative(ly charged) ; proton has greater mass ; [2] (b) (i) caesium 1 and iodine 7 ; [1] (ii) CsI ; ionic ; [2] (iii) caesium atom loses one / its outer electron ; iodine atom gains one electron ; [2] (c) (i) the higher the temperature the greater mass of solid dissolves ; [1] (ii) 130 (g) [1] (iii) calculation of Mr [CsI] 133 + 127 / 260 ; change volume units from 100 cm3 to dm3 mass dissolving in 1 dm3 = 1300 g ; calculation of concentration in moles / dm3 1300 ÷ 260 = 5 (mol / dm3) ; OR calculation of Mr [CsI] 133 + 127 / 260 ; calculation of concentrarion in mol / 100 cm3 130 / 260 = 0.5 mol / 100 cm3 ; change volume units from 100 cm3 to dm3 concentration = 5 mol / dm3 ; [3] [Total: 13] 7 (a) plastic / glass iron glass / plastic copper 4 correct = 2 marks, 3 or 2 correct = 1 mark ;; [2] (b) (i) 54 ; [1] (ii) 56 26Fe [1]

Page 6 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2016 0654 31 © Cambridge International Examinations 2016 (iii) time taken for a sample of radioactive isotope to decay by half/ time taken for count rate of radioactive isotope to decrease by half ; [1] (c) evaporation can occur at any temperature / boiling only happens at the boiling point ; evaporation happens only at the surface / boiling happens throughout the liquid ; evaporation lets only the molecules with the highest kinetic energy out / boiling taken energy in (endothermic) to occur ; evaporation can occur using the internal energy of the system / boiling requires an external source of heat ; evaporation produces cooling / boiling does not produce cooling ; evaporation is a slow process / boiling is a rapid process ; [max 1] (d) reference to induced magnetism ; [1] (e) A (no mark) regular arrangement ; [1] (f) workable method of measurement of displacement ; ref to displacement / subtraction of two volumes ; [2] [Total: 10] 8 (a) obesity ; blocking coronary arteries ; (leading to) (coronary) heart disease ; [3] (b) (i) liver labelled on Fig. 1.1 ; [1] (ii) emulsifies ; increases surface area for, enzyme action / faster digestion ; [2] (iii) large surface area ; thin wall ; lacteals ; [max 2] [Total: 8] 9 (a) (i) transition (metals / series / elements) ; [1]

Page 7 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2016 0654 31 © Cambridge International Examinations 2016 (ii) elements or their compounds can behave as catalysts ; compounds have colours other than white ; [2] (iii) iron atoms ; reference to electrons being lost ; [2] (iv) this alloy does not rust ; [1] b (i) blast furnace ; [1] (ii) Fe2O3 + 3CO → 2Fe + 3CO2 formulae ; balancing ; [2] [Total: 9] 10 (a) (i) ray of light correctly drawn from Y to X ; [1] (ii) normal correctly drawn ; [1] (iii) angle of incidence correctly labelled ; [1] (iv) same size as object, upright, virtual ; [1] (b) compression: particles close together / rarefaction: further apart OR compression: region of high pressure / rarefaction: region of low pressure ; [1] (c) (i) ammeter and voltmeter ; [1] (ii) 1 / RT = 1 / R1 + 1 / R2 or 1 / RT = 1 / 12 + 1 / 4 = 1 / 3 or RT = R1R2 / (R1 + R2) or RT = 48 / 16 ; RT = 3 (Ω) ; [2] [Total: 8] 11 (a) (i) FF and Ff ; [1] (ii) have ff genotype ; [1] (b) (i) camouflage / AW ; [1] (ii) less well adapted / less likely to survive / more likely to be preyed on ; (so) less likely to reproduce ; [2]

Page 8 Mark Scheme Syllabus Paper Cambridge IGCSE – May/June 2016 0654 31 © Cambridge International Examinations 2016 (c) (correct gametes) H, h, H, h ; (correct genotypes) HH, Hh, Hh, hh ; (correct phenotypes) short fur, short fur, short fur, long fur ; (correct ratio) 3 short : 1 long ; [4] [Total: 9] 12 (a) (i) L diamond and M graphite ; [1] (ii) contains only one type of atom ; [1] (iii) (M) reference to the layer structure ; reference to (layers) sliding ; reference to weak (attractive) forces (between layers) ; [max 2] (b) (i) (reactants) energy is transferred from reactants ; as thermal energy / reaction is exothermic ; [2] (ii) powder has a large surface area ; the idea that the probability / frequency of collision (between oxygen molecules and the solid surface / carbon atoms) is higher ; [2] [Total: 8]