Cambridge IGCSE Sciences - Co-ordinated (Double) 0654 — 2016 Oct/Nov Paper 2 · Variant 2

This document consists of 32 printed pages. DC (SLM) 137306 © UCLES 2016 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education * 2 3 6 5 9 1 9 7 5 8 * CO-ORDINATED SCIENCES 0654/22 Paper 2 (Core) October/November 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 0654/22/O/N/16 © UCLES 2016 1 Scientists can estimate the concentration of carbon dioxide in the Earth’s atmosphere a long time ago. Samples of air can be found trapped in ancient ice. (a) Table 1.1 shows some results. Table 1.1 year carbon dioxide concentration / parts per million 1000 280 1200 275 1400 280 1600 270 1800 280 2000 345 (i) In the year 2000, the carbon dioxide concentration in the trapped air was 345 parts per million. State the two gases that make up most of the rest of the atmosphere. 1 … 2 … [2] (ii) Using the information in Table 1.1, describe how the carbon dioxide concentration in the Earth’s atmosphere changed between the year 1000 and the year 2000. … … … …[3] (b) Name a biological process that (i) releases carbon dioxide into the atmosphere, …[1] (ii) removes carbon dioxide from the atmosphere. …[1]

3 0654/22/O/N/16 © UCLES 2016 [Turn over (c) Suggest and explain the effect on the carbon dioxide concentration in the Earth’s atmosphere of (i) large-scale deforestation, … …[1] (ii) burning fossil fuels. … …[1] (d) An increase in carbon dioxide concentration in the Earth’s atmosphere could cause global warming. State two undesirable effects of global warming. 1 … 2 … [2]

4 0654/22/O/N/16 © UCLES 2016 2 Five test-tubes containing different substances are labelled A, B, C, D and E as shown in Fig. 2.1. Dilute hydrochloric acid is added to each of the five substances. copper A B C D E dilute hydrochloric acid dilute hydrochloric acid copper carbonate magnesium silver nitrate solution sodium hydroxide solution dilute hydrochloric acid dilute hydrochloric acid dilute hydrochloric acid Fig. 2.1 (a) (i) Suggest the letter of the test-tube containing a substance that releases a gaseous element when the dilute hydrochloric acid is added. Name the gaseous element. test-tube … gaseous element … [1] (ii) Suggest the letter of the test-tube containing a substance that releases a gaseous compound when the dilute hydrochloric acid is added. Name the gaseous compound. test-tube … gaseous compound …[1]

5 0654/22/O/N/16 © UCLES 2016 [Turn over (iii) Dilute hydrochloric acid contains chloride ions in solution. State the letter of the test-tube in which the hydrochloric acid reacts to form a white solid. State the name of the white solid produced. test-tube … white solid … [1] (b) Vanadium and its compounds are able to act as catalysts. (i) State the meaning of the term catalyst. … … …[2] (ii) The chemical symbol for vanadium is shown. 51 23V State • the number of neutrons in the nucleus of this atom, … • the number of electrons in a vanadium atom. … [2] (iii) State the name of the collection of metals in the Periodic Table to which vanadium belongs. …[1]

6 0654/22/O/N/16 © UCLES 2016 (c) The industrial production of sulfuric acid involves a chemical reaction that uses vanadium oxide as a catalyst. Fig. 2.2 shows part of the industrial process used to produce sulfuric acid. X Y key Z vanadium oxide catalyst reaction vessel atom of sulfur atom of oxygen Fig. 2.2 Boxes X, Y and Z contain diagrams that represent the molecules in the reaction. (i) State the formula of the molecules shown in box Z. … [1] (ii) Explain which box, X or Y, contains molecules that are oxidised in the reaction vessel. box … explanation … …[1]

7 0654/22/O/N/16 © UCLES 2016 [Turn over 3 (a) Three identical kettles have each been filled with the same volume of water at 25 °C. Fig. 3.1 shows the three kettles a few minutes later. A B C heating element Fig. 3.1 Kettle A contains water that remains at 25 °C. Kettle B contains water that is just starting to boil at 100 °C. Kettle C contains water that has been boiling for a few minutes but is still at 100 °C. (i) The volume of water in kettle A stays the same. There is a small increase in the volume of water in kettle B. Explain why the water volume increases in kettle B. … …[1] (ii) Explain why there is a large difference in the volume of water between kettles B and C. … …[1] (iii) Pure water has a boiling point of 100 °C. State the meaning of the term boiling point. … …[1]

8 0654/22/O/N/16 © UCLES 2016 (iv) When the water boils, some becomes water vapour in the air. Fig. 3.2 shows the arrangement of particles in a gas, liquid and solid. A B C Fig. 3.2 State and explain which diagram, A, B or C, best represents: water at 25 °C, … explanation … … water vapour. … explanation … … [2] (b) The kettles shown in Fig. 3.1 each have a heating element at the bottom. Name the method by which thermal energy is transferred through the water in the kettles. … [1] (c) A kettle is connected to a 250 V supply. There is a current of 8 A in the heating element. Calculate the resistance of the heating element. State the formula you use, show your working and state the unit. formula working resistance = … unit = … [3]

9 0654/22/O/N/16 © UCLES 2016 [Turn over (d) Fig. 3.3 shows a kettle with a mains lead connected to a plug. Inside the plug there is a fuse. heating element mains lead plug with fuse inside Fig. 3.3 A fuse in the plug protects a person using the kettle from an electric shock. Describe what happens to the fuse when a short circuit occurs in the kettle. Explain why this happens. description … … explanation … … [2]

10 0654/22/O/N/16 © UCLES 2016 4 A gardener increases the number of trees by taking cuttings. The gardener cuts off part of a stem (the cutting) and places it in water, as shown in Fig. 4.1. cutting removed cutting placed in water water Fig. 4.1 The cutting develops roots as shown in Fig. 4.2. The gardener then plants the cutting in the ground. developing roots cutting water Fig. 4.2 (a) The cutting grows into a new tree. This is an example of asexual reproduction. (i) Define the term asexual reproduction. … … …[2] (ii) For a particular gene, the parent plant has the genotype Aa. Predict what would be the genotype of the cutting. genotype … [1]

11 0654/22/O/N/16 © UCLES 2016 [Turn over (b) Before the roots develop on a cutting, the gardener encloses the cutting in a plastic bag, as shown in Fig. 4.3. This prevents the cutting from losing too much water before its new roots have grown. string cutting plastic bag Fig. 4.3 (i) State the name of the cells in the roots of a plant that absorb most of the water, … the tissue that carries water up from the roots to the leaves, … the process of evaporation of water from the surfaces of the cells in the leaves. … [3] (ii) Explain why the plastic bag in Fig. 4.3 reduces the amount of water lost from the leaves of the cutting. … …[1] (iii) State two ways in which the cutting uses the water that it has absorbed. 1 … 2 …[2]

12 0654/22/O/N/16 © UCLES 2016 (c) As the cutting develops, it also needs nitrate ions and magnesium ions. These are added to the water. Describe the importance to the developing cutting of (i) nitrate ions, … …[1] (ii) magnesium ions. … …[1]

13 0654/22/O/N/16 © UCLES 2016 [Turn over 5 (a) Fig. 5.1 shows the apparatus a teacher uses to demonstrate the reaction between hot magnesium and steam. magnesium steam heat white solid S gas G burning Fig. 5.1 During the reaction a white solid, S, and a flammable gas, G, are produced. (i) Name solid S and gas G. solid S … gas G … [2] (ii) Predict and explain what is observed, if anything, when the teacher repeats the experiment using copper instead of magnesium. observation … explanation … … [2]

14 0654/22/O/N/16 © UCLES 2016 (b) Fig. 5.2 shows the apparatus and materials a student uses to study the reaction between magnesium ribbon and excess copper sulfate solution. She measures the temperature of the solution for ten minutes. thermometer insulated beaker copper sulfate solution magnesium ribbon lid Fig. 5.2 Fig. 5.3 shows a graph of her results. 0 1 2 3 4 5 time / minutes temperature 6 7 8 9 10 Fig. 5.3 (i) Explain why the results in Fig. 5.3 show that an exothermic reaction occurs between the magnesium and the copper sulfate solution. … …[1]

15 0654/22/O/N/16 © UCLES 2016 [Turn over (ii) Suggest the time it takes for all of the magnesium to react in this experiment. Give a reason for your answer. … … …[2] (iii) Suggest one change the student could make, other than using a catalyst, to increase the rate of this reaction. … …[1]

16 0654/22/O/N/16 © UCLES 2016 6 Fig. 6.1 shows an electric train. Fig. 6.1 The train starts from rest and accelerates with constant acceleration. The train reaches 45 m / s after 60 seconds. The train then continues at this constant speed for 150 seconds. (a) (i) On the grid below sketch a speed / time graph for the train. 0 0 20 40 60 80 10 30 50 70 50 100 time / s speed m / s 150 200 250 [2]

17 0654/22/O/N/16 © UCLES 2016 [Turn over (ii) Calculate the distance travelled by the train between 60 seconds and 210 seconds. Show your working. distance = …m [2] (b) The train track is made from lengths of steel rail. The steel rails are made from steel blocks. Each rail is made using 512 000 cm3 of steel. The density of steel is 8.0 g / cm3. Calculate the mass of a steel rail. State the formula you use and show your working. formula working mass = …g [2]

18 0654/22/O/N/16 © UCLES 2016 (c) Fig. 6.2 shows the two horizontal forces acting on the train when it is moving. Force D is the driving force from the engine. Force F is the frictional force from air resistance and the wheels. force F frictional force force D driving force from engine Fig. 6.2 State what can be said about the two forces D and F acting on the train when the train is accelerating, … … travelling at a constant speed. … … [2] (d) The power station that supplies the electrical energy for the overhead cables on the railway uses natural gas as its energy source. (i) Describe the processes and energy transfers involved in generating electrical energy from natural gas. processes … … … energy transfers … … … [4] (ii) Natural gas is a non-renewable energy source. Name one other non-renewable energy source and one renewable energy source. non-renewable source … renewable source … [1]

19 0654/22/O/N/16 © UCLES 2016 [Turn over Please turn over for Question 7.

20 0654/22/O/N/16 © UCLES 2016 7 (a) Use the terms in the list to complete the sentences about homeostasis. Each term may be used once, more than once, or not at all. arterioles capillaries environment shiver sweat temperature vasoconstriction vasodilation veins Homeostasis is defined as the maintenance of a constant internal … . If a person’s body temperature gets too low, the person may … to raise their temperature again. Also, in the skin, … may undergo … , reducing the blood flow to the … near the skin surface. [5] (b) Fig. 7.1 shows how a person’s body temperature changes over a period of three hours. 15:00 35 36 37 38 body temperature / °C 39 16:00 17:00 time of day / hours 18:00 Fig. 7.1 (i) State the time at which the person’s body temperature is highest. … [1]

21 0654/22/O/N/16 © UCLES 2016 [Turn over (ii) During the three hour period, the external environment stays the same. Suggest why the person’s body temperature starts to rise at 16:00 hours, … falls again after that. … [2] (iii) Describe the role of fatty tissue in the skin in the control of body temperature. … … …[2]

22 0654/22/O/N/16 © UCLES 2016 8 (a) Fig. 8.1 shows sodium burning in chlorine gas. The product of this reaction is a white solid compound. chlorine gas jar clouds of a white solid compound sodium burning Fig. 8.1 (i) Write the word equation for the reaction shown in Fig. 8.1. … … … [2] (ii) Fig. 8.2 shows some of the particles that are bonded together in the white solid. These particles have electrical charges as shown. + + + – + + – – – Fig. 8.2 Add the chemical symbols for the metal, Na, and non-metal, Cl, to the particles in Fig. 8.2. [1] (iii) Describe, in terms of electrons, how a chlorine atom becomes a chloride ion. … …[1]

23 0654/22/O/N/16 © UCLES 2016 [Turn over (b) A student was asked to produce some chlorine. Fig. 8.3 shows the apparatus and most of the materials that he was given to complete the task. d.c. power supply switch beaker copper chloride crystals carbon electrodes – + Fig. 8.3 (i) Describe how the student should use the apparatus and materials to produce chlorine. Include in your answer any other materials that are required. … … … … …[3] (ii) Describe how the appearance of the carbon cathode changes during the electrolysis of copper chloride. Explain your answer. change in appearance … … explanation … … [2]

24 0654/22/O/N/16 © UCLES 2016 (c) The bell in Fig. 8.4 is made from a mixture of copper and tin. bell Fig. 8.4 (i) State the word that is used for a mixture of metals. … [1] (ii) The metal used to make the bell is less malleable than pure copper and pure tin. State the meaning of the term malleable. … …[1] (iii) Suggest an advantage of making the bell from a metal that is not malleable. … …[1]

25 0654/22/O/N/16 © UCLES 2016 [Turn over 9 (a) A nuclear power station uses the energy from nuclear fission to generate electricity. (i) Describe what happens to the nucleus of an atom when it undergoes nuclear fission. … …[1] (ii) Place alpha (α), beta (β) and gamma (γ) radiations in order of their ionising ability. most ionising … … … least ionising [1] (iii) Alpha radiation sources are more dangerous to humans, when they are breathed in or swallowed, than alpha radiation sources remaining outside the body. Explain this observation. … …[1] (b) An overhead power cable transmits electrical power from a power station to a town. The resistance of the cable is 6 Ω. (i) State the effect on the resistance of the cable if the diameter of the cable is increased. …[1] (ii) State one way to change the resistance of the cable, other than changing the diameter. … …[1]

26 0654/22/O/N/16 © UCLES 2016 10 (a) Fig. 10.1 shows the human female reproductive system. X uterus oviduct Z Y Fig. 10.1 (i) Name the parts labelled X, Y and Z. X … Y … Z … [3] (ii) State one function of part X. …[1] (b) (i) State where in the female reproductive system the egg is fertilised. …[1] (ii) Outline the early development of the zygote after fertilisation. … … … …[3]

27 0654/22/O/N/16 © UCLES 2016 [Turn over 11 Fig. 11.1 shows apparatus used to investigate the compounds produced when ethanol burns. ethanol burner balance cobalt chloride paper cold water limewater pump draws combustion products through the apparatus U-tube Fig. 11.1 (a) (i) Before the ethanol burner is lit, the cobalt chloride paper is blue and the limewater is colourless. Predict and explain the changes in appearance of the cobalt chloride paper and the limewater shortly after the burner is lit. cobalt chloride paper … explanation … limewater … explanation … [4] (ii) Predict what happens to the reading on the balance during the experiment. …[1]

28 0654/22/O/N/16 © UCLES 2016 (b) Fig. 11.2 shows diagrams of molecules, I, J and K. H H H H C C H I H O H H H H C C K H H H H C C H J H Fig. 11.2 (i) Molecule J is a saturated hydrocarbon. State what is meant by the terms hydrocarbon, … … saturated. … … [2] (ii) Name molecules I and K. I … K … [2] (iii) State the chemical formula of the molecule that reacts with molecule K to form molecule I. … [1]

29 0654/22/O/N/16 © UCLES 2016 [Turn over 12 (a) A star emits γ-rays and visible light. γ-rays and visible light are parts of the electromagnetic spectrum. Place γ-rays and visible light in their correct positions in the incomplete electromagnetic spectrum shown in Fig. 12.1. [1] X-rays infra-red waves microwaves Fig. 12.1 (b) Below are four terms used to describe a wave. Draw a line from each term to its definition. term definition amplitude how far the wave travels in one second frequency the distance from any point on one wave to the same point on the next wave speed the distance from the centre of a wave to the top or to the bottom of the wave wavelength the number of waves passing a fixed point in one second [2]

30 0654/22/O/N/16 © UCLES 2016 (c) Telescopes used to observe stars contain mirrors. Fig. 12.2 shows a ray of light reflecting from a plane mirror. incident ray reflected ray mirror Fig. 12.2 (i) On Fig. 12.2 label with an r the angle of reflection. [1] (ii) The angle of incidence is 36°. State the angle of reflection. Explain your answer. angle of reflection … explanation … … [1] (d) Fig. 12.3 shows a comet seen in the sky by an astronomer. Fig. 12.3 The astronomer observes the comet in a mirror. Draw an image of the comet that the astronomer sees in the mirror. [1]

31 0654/22/O/N/16 © UCLES 2016 (e) Telescopes also contain lenses. Rays of light from a star pass through a lens, as shown in Fig. 12.4. Fig. 12.4 (i) On Fig. 12.4, label the principal focus of the lens with the letter P. [1] (ii) On Fig. 12.4, use a double-headed arrow ( ) to indicate the focal length of the lens. [1] (iii) As light passes through the lens, the direction of the light is changed. State the name of this process. … [1] (f) An explosion in space produces both light waves and sound waves. (i) Explain why an astronomer on Earth would be able to see the light wave through a telescope but would not be able to hear the sound wave produced by the explosion. … … …[1] (ii) State one other difference between a light wave and a sound wave. … …[1]

32 0654/22/O/N/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 119 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 Cn 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 11 printed pages. © UCLES 2016 [Turn over Cambridge International Examinations Cambridge International General Certificate of Secondary Education CO-ORDINATED SCIENCES 0654/22 Paper 2 Core Theory October/November 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 October/November 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 – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 1(a)(i) nitrogen ; oxygen ; 2 1(a)(ii) little change / no overall change ; (but) some fluctuations ; increases from 1800 ; by 65 ppm ; max 3 1(b)(i) respiration / decomposition / excretion ; 1 1(b)(ii) photosynthesis ; 1 1(c)(i) increase, because less photosynthesis ; 1 1(c)(ii) increase, because CO2 released by combustion ; 1 1(d) flooding ; melting ice-caps ; extinction / migration of species ; hurricanes / unpredictable weather patterns ; increased agricultural pests ; max 2 Total: 11 Question Answer Marks 2(a)(i) C and hydrogen ; 1 2(a)(ii) B and carbon dioxide ; 1 2(a)(iii) D and silver chloride ; 1 2(b)(i) substance / material that speeds up / alters rate of a chemical change / reaction ; is itself not permanently changed ; 2

Page 3 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 2(b)(ii) 28 ; 23 ; 2 2(b)(iii) transition (series / metals) ; 1 2(c)(i) SO3 ; 1 2(c)(ii) (Y) oxygen has been added to the molecules ; 1 Total: 10 Question Answer Marks 3(a)(i) water has expanded because it is hotter ; 1 3(a)(ii) some of the water has boiled away / evaporated ; 1 3(a)(iii) temperature at which all the liquid can turn into a gas ; 1 3(a)(iv) (water is) B most particles are touching and random arrangement ; (water vapour is) C particles are spread out (and random arrangement) ; 2 3(b) Convection ; 1 3(c) R = V / I or = 250 / 8 ; = 31.25 ; Ω ; 3 3(d) fuses cut electricity to a device if there is a power surge / too much current flows / a fault ; (too much current) causes fuse to melt ; 2 Total: 11

Page 4 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 4(a)(i) production of genetically identical offspring ; from one parent ; 2 4(a)(ii) Aa ; 1 4(b)(i) root hair (cells) ; xylem ; transpiration ; 3 4(b)(ii) retains water in the air around the leaves / increases humidity ; 1 4(b)(iii) photosynthesis ; transport ; support ; AVP ; max 2 4(c)(i) for protein synthesis ; 1 4(c)(ii) for chlorophyll synthesis ; 1 Total: 11

Page 5 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 5(a)(i) S is magnesium oxide ; G is hydrogen ; 2 5(a)(ii) no change / reaction ; copper too unreactive / less reactive than hydrogen ; 2 5(b)(i) the temperature (initially) increases ; 1 5(b)(ii) 3 minutes ; no heat given out after this time / temperature no longer increases ; 2 5(b)(iii) increase concentration of copper sulfate solution ; increase (starting) temperature of copper sulfate solution ; use powdered magnesium / increase surface area of magnesium ; max 1 Total: 8 Question Answer Marks 6(a)(i) acceleration line gradient correct ; constant speed line correct at 45m / s for 150 s anywhere ; 2 6(a)(ii) distance = speed × time ; = 45 × 150 = 6750 (m) ; 2 6(b) mass = density × volume or 8 × 512 000 ; = 4 096 000 (g) ; 2 6(c) D is greater than F ; D is equal (and opposite) to F ; 2

Page 6 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 6(d)(i) fuel is burned ; chemical energy to thermal energy ; water is turned into steam ; thermal to kinetic energy ; steam drives turbine / generator ; kinetic to electrical ; max 4 6(d)(ii) example of non-renewable and example of renewable ; 1 Total: 13 Question Answer Marks 7(a) environment ; shiver ; arterioles ; vasoconstriction ; capillaries ; 5 7(b)(i) 16.30 ; 1 7(b)(ii) exercise / activity ; sweating / vasodilation ; 2 7(b)(iii) is a good insulator ; reduces heat loss to the environment ; 2 Total: 10

Page 7 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 8(a)(i) sodium + chlorine → sodium chloride ;; LHS and RHS 2 8(a)(ii) 1 8(a)(iii) atom gains (an) electron / completes its outer shell ; 1 8(b)(i) make copper chloride into a(n aqueous) solution ; add solution to the beaker so electrodes are immersed ; close the switch ; 3 8(b)(ii) changes from black to brown / pink / copper coloured ; copper is deposited (on the cathode) ; 2 8(c)(i) alloy ; 1 8(c)(ii) malleable refers to ability to be shaped (without breaking) / does not break / change shape when subjected to a force / other correct ; 1 8(c)(iii) less likely to be dented when rung / owtte ; 1 Total: 12

Page 8 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 9(a)(i) (nucleus) splits ; 1 9(a)(ii) α β γ ; 1 9(a)(iii) alpha (is ionising but) has low penetration ; 1 9(b)(i) resistance reduced ; 1 9(b)(ii) length / material / temperature ; 1 Total: 5 Question Answer Marks 10(a)(i) X = ovary ; Y = cervix ; Z = vagina ; 3 10(a)(ii) release of female gametes ; 1 10(b)(i) oviduct ; 1 10(b)(ii) divides ; forms a ball of cells ; implants ; in lining / wall of uterus ; max 3 Total: 8

Page 9 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 11(a)(i) cobalt chloride paper goes pink ; showing water (vapour in the combustion products) ; limewater turns milky ; showing carbon dioxide (in the combustion products) ; 4 11(a)(ii) decreases ; 1 11(b)(i) hydrocarbon contains hydrogen and carbon only ; saturated it contains only single bonds / it fits the general formula CnH2n + 2 ; 2 11(b)(ii) I is ethanol ; K is ethene ; 2 11(b)(iii) H2O ; 1 Total: 10

Page 10 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 12(a) gamma – box to left of X rays and visible light – box to left of infra-red ; 1 12(b) amplitude = 3rd answer, frequency = 4th answer, speed = 1st answer, wavelength = 2nd answer 4 correct = 2 marks , 3, 2 or 1 correct = 1 mark ;; 2 12(c)(i) angle of reflection correctly indicated ; 1 12(c)(ii) 36° angle of incidence = angle of reflection ; 1 12(d) mirror image of comet drawn laterally inverted and same size ; 1 12(e)(i) principal focus identified ; 1 12(e)(ii) focal length identified ; 1 12(e)(iii) refraction ; 1

Page 11 Mark Scheme Syllabus Paper Cambridge IGCSE – October/November 2016 0654 22 © UCLES 2016 Question Answer Marks 12(f)(i) sound requires a medium / sound cannot travel through vacuum ; 1 12(f)(ii) light waves are electromagnetic / sound waves are not ; light waves are transverse / sound waves are longitudinal ; max 1 Total: 11