Cambridge IGCSE Sciences - Co-ordinated (Double) 0654 — 2010 Oct/Nov Paper 3 · Variant 2

This document consists of 25 printed pages and 3 blank pages. IB10 11_0654_32/3RP © UCLES 2010 [Turn over *8813001337* For Examiner's Use 1 2 3 4 5 6 7 8 9 10 Total UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education CO-ORDINATED SCIENCES 0654/32 Paper 3 (Extended) October/November 2010 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 a soft pencil for any diagrams, graphs, tables or rough working. Do not use staples, paper clips, highlighters, glue or correction fluid. DO NOT WRITE IN ANY BARCODES. Answer all questions. A copy of the Periodic Table is printed on page 28. 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. www.XtremePapers.com

2 © UCLES 2010 0654/32/O/N/10 1 (a) Fig. 1.1 shows apparatus used in the electrolysis of copper chloride solution. copper chloride solution d.c. power supply test-tube electrolysis cell anode cathode Fig. 1.1 (i) Describe what is observed at the cathode. [1] (ii) Chloride ions have a single negative electrical charge, Cl -. For every copper ion in the solution, two chloride ions are present. Deduce the electrical charge of a copper ion. Show how you obtained your answer. [2]

3 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (iii) Fig. 1.2 shows diagrams of two particles L and M. Each of these particles have 17 protons in their nucleus. Only the outer shell of each particle is shown. Cl particle L × × × × × × × × Cl particle M × × × × × × × Fig. 1.2 State and explain which one of these particles, L or M, would move towards the anode during electrolysis. particle [2] (iv) The bubbles of gas which rise from the anode contain diatomic molecules of chlorine. Complete the bonding diagram below to show how the outer electrons are arranged in a chlorine molecule. Cl Cl [2]

4 © UCLES 2010 0654/32/O/N/10 For Examiner's Use (b) The apparatus shown in Fig. 1.3 can be used to investigate the reaction between lead oxide, PbO, and carbon. strong heat mixture of lead oxide and powdered carbon glass rod drop of limewater Fig. 1.3 When the mixture is heated, a redox reaction occurs in which lead oxide is reduced. The drop of limewater suspended on the glass rod turns cloudy. (i) Name the gas which is produced in this redox reaction. [1] (ii) Suggest the balanced symbolic equation for the redox reaction between lead oxide and carbon. [2] (iii) A student suggested carrying out a similar redox reaction to that shown in Fig. 1.3, using potassium oxide instead of lead oxide. Potassium is an alkali metal in Group 1 of the Periodic Table. Predict and explain whether or not there would be a redox reaction between potassium oxide and carbon. [2]

5 © UCLES 2010 0654/32/O/N/10 [Turn over BLANK PAGE Please turn over for Question 2.

6 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 2 (a) Fig. 2.1 shows an electric circuit. A2 A1 A4 A3 Fig. 2.1 Complete Table 2.1 to show the reading on each ammeter. Table 2.1 ammeter current / amps A1 0.7 A2 A3 A4 0.3 [2] (b) Fig. 2.2 shows how the current in a circuit varies with voltage. 0 2 4 voltage / V current / A 6 8 10 2.0 1.5 1.0 0.5 0 Fig. 2.2 (i) Is Ohm’s Law obeyed in this circuit? Explain your answer. [1]

7 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (ii) Predict the current in the circuit when the voltage is 13 V. Explain your answer. [2] (c) Fig. 2.3 shows a transformer. a.c. input a.c. output iron core Fig. 2.3 (i) Explain why the core of the transformer is made of iron. [2] (ii) The transformer has 10 000 turns on the primary coil and 1000 turns on the secondary coil. The voltage across the primary coil is 200 V. Use the formula Vp / Vs = Np / Ns to calculate the voltage across the secondary coil. Show your working. [1]

8 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 3 A healthy plant growing in a pot was watered and placed in a sunny window. A transparent plastic bag was placed over the plant, as shown in Fig. 3.1. soil pot transparent plastic bag Fig. 3.1 (a) The temperature near the window fell overnight. The next morning, small droplets of water were visible on the inside of the plastic bag. Explain why the droplets of water appeared on the inside of the plastic bag. [4]

9 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (b) The plastic bag was then removed from the plant. The next day was warm and sunny, and by the end of the day the plant had wilted. Fig. 3.2 shows the wilted plant. Fig. 3.2 (i) Explain why the plant wilted. [2] (ii) Explain why the main stem of the plant remained upright, even when the rest of the plant wilted. [1]

10 © UCLES 2010 0654/32/O/N/10 For Examiner's Use (iii) Fig. 3.3 shows a cell from the plant leaf before it wilted. Fig. 3.3 In the space below, draw the same cell to show its appearance after the plant had wilted. [3]

11 © UCLES 2010 0654/32/O/N/10 [Turn over BLANK PAGE Please turn over for Question 4.

12 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 4 (a) Below is a list of some types of waves. gamma infra-red microwave sound ultrasound ultraviolet visible light State one wave from the list that is (i) a longitudinal wave, [1] (ii) emitted by hot objects but cannot be seen by the human eye, [1] (iii) the transverse wave with the highest frequency. [1] (b) A sound wave has a frequency of 50 000 Hz. (i) Explain the meaning of the term frequency. [1] (ii) Explain whether a person would be able to hear this sound. [1] (iii) Sound waves travel through the air at 330 m / s. Calculate the wavelength of the sound wave. State the formula that you use and show your working. formula used working [3]

13 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use 5 In many countries, river water is collected and treated to make it safe for humans to drink. (a) Explain which one of the treatments shown below might not remove all the harmful bacteria from water which is to be used for drinking. chlorination distillation filtration treatment [1] (b) Sometimes large numbers of tiny pieces of insoluble solid material become dispersed in river water, forming a colloid. Fig. 5.1 shows a simplified diagram of a colloid. dispersed solid particles water Fig. 5.1 Explain in terms of light rays, why colloids are not transparent. You may draw some light rays on Fig. 5.1 to help you to answer this question. [2]

14 © UCLES 2010 0654/32/O/N/10 For Examiner's Use (c) A chemist wanted to find the concentration in mol / dm3 of sulfuric acid in a sample of acidic lake water. Fig. 5.2 shows the apparatus and materials that he used. beaker containing 1.0 dm3 of acidic lake water burette containing 0.05 mol / dm3 sodium hydroxide solution tap Fig. 5.2 The chemist slowly added 0.05 mol / dm3 sodium hydroxide solution to 1.0 dm3 of acidic lake water contained in a beaker until the acid had just been neutralised. The chemist found that it required 12.5 cm3 of 0.05 mol / dm3 sodium hydroxide solution to neutralise the acid. (i) State the number of moles of sodium hydroxide which are dissolved in 1.0 dm3 of the sodium hydroxide solution. [1] (ii) Calculate the number of moles of sodium hydroxide which are dissolved in 12.5 cm3 of the sodium hydroxide solution. Show your working. [2]

15 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (iii) The balanced equation for the neutralisation reaction is 2NaOH + H2SO4 → Na2SO4 + 2H2O Calculate the number of moles of sulfuric acid which were contained in 1.0 dm3 of acidic lake water. Show your working. [2]

16 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 6 Fig. 6.1 shows the speed-time graph for a car for the first 24 seconds of a journey. 0 2 4 6 8 10 12 14 16 18 20 22 24 20 18 16 14 12 10 8 6 4 2 0 time / s speed m / s Fig. 6.1 (a) On the graph, label with an A a section when the car is accelerating. [1] (b) Calculate the distance covered in the first 8 seconds. Show your working. [2]

17 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (c) The mass of the car is 800 kg. Calculate the kinetic energy of the car when travelling at its maximum speed on this journey. State the formula that you use and show your working. formula used working [3] (d) When the speed of a car doubles, its momentum also doubles but its kinetic energy is four times greater. Explain why. [2]

18 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 7 (a) Mammals are vertebrates. State two characteristic visible features of mammals that distinguish them from all other classes of vertebrates. 1 2 [2] (b) Mammals are able to maintain a constant internal body temperature. Describe how vasodilation helps to cool the body when it gets too hot. [3] (c) The maintenance of a constant internal body temperature is part of homeostasis. Homeostasis also includes the regulation of blood glucose concentration and the removal of toxic waste products, such as urea, from the body. (i) Describe how blood glucose concentration is brought back to normal if it rises too high. [3]

19 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (ii) Urea is removed from the body dissolved in water, forming urine. Fig. 7.1 is an incomplete diagram of the kidneys and other organs involved in the removal of urea from the body. to heart from heart kidney bladder Fig. 7.1 Complete Fig. 7.1 by drawing and labelling: • the renal arteries • the renal veins • the ureters • the urethra [4]

20 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 8 (a) A scientist uses a Geiger counter to measure radiation from a radioactive source. Fig. 8.1 shows the graph of her results. 0 5 10 15 20 25 200 180 160 140 120 100 80 60 40 20 0 time / hours reading on Geiger counter / counts per second Fig. 8.1 Calculate the half-life of the radioactive source. Show your working. [2]

21 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use (b) Alpha radiation is a form of ionising radiation. (i) Explain the meaning of the term ionising radiation. [1] (ii) An alpha radiation source is less harmful to humans than a gamma radiation source if it is outside the body. An alpha radiation source is more harmful than to humans than a gamma radiation source if it is inside the body. Explain why. [2] (c) Nuclear fission and nuclear fusion are both sources of energy. (i) Describe how these two processes differ. [2] (ii) There are safety concerns about the use of nuclear fission as an energy resource. Describe and explain one of these safety concerns. [2]

22 © UCLES 2010 0654/32/O/N/10 For Examiner's Use 9 (a) The chemical symbols for the atoms shown below include proton (atomic) numbers and nucleon (mass) numbers. O 16 8 P 31 15 S 32 16 Ga 70 31 Complete Table 9.1 which shows the names and the numbers of protons and neutrons in two of the atoms shown above. Table 9.1 element name protons neutrons oxygen 15 16 [2] (b) Fig. 9.1 shows part of a chart of the melting points in kelvins (K) of some elements. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 4000 3500 3000 2500 2000 1500 1000 500 0 melting point / K proton (atomic) number Fig. 9.1

23 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use The melting points of the elements in Period 2 and Period 3 of the Periodic Table show a periodic pattern. (i) Use Fig. 9.1 and your understanding of the term periodic pattern to predict the element which has the highest melting point in Period 3. Explain your choice briefly. element explanation [2] (ii) Carbon, proton number 6, and nitrogen, proton number 7, have very different melting points. Explain the difference in terms of the structures of these elements. In your answer you should include the phrases, giant structure and simple molecular structure. You may wish to draw diagrams as part of your answer. [3]

24 © UCLES 2010 0654/32/O/N/10 For Examiner's Use (c) Carbon and hydrogen combine to form a very large number of hydrocarbons. Ethene, C2H4, is a gaseous, unsaturated hydrocarbon, which is of industrial importance. (i) Complete the displayed formula of the ethene molecule below. H C [2] (ii) Unsaturated hydrocarbons are made in industry from fractions obtained by the fractional distillation of oil (petroleum). Name the process which is used to make unsaturated hydrocarbons and describe briefly how it is done. name of process description [3] (iii) Describe, in terms of changes to chemical bonds, what happens when ethene molecules react to form molecules of poly(ethene). [2]

25 © UCLES 2010 0654/32/O/N/10 [Turn over For Examiner's Use 10 Fig. 10.1 shows some stages in the formation of a human fetus. ball of cells fetus zygote egg cell sperm cell amnion amniotic fluid Fig. 10.1 (a) Most human cells contain 46 chromosomes. (i) State the number of chromosomes in a sperm cell. [1] (ii) State the number of chromosomes in a zygote. [1] (iii) Name the part of the cell in which chromosomes are found. [1] (b) Name the part of the female reproductive system in which each of these events occurs. (i) The zygote is produced. [1] (ii) The fetus develops. [1] (c) Describe the function of the amnion. [2]

26 © UCLES 2010 0654/32/O/N/10 For Examiner's Use (d) Mutations sometimes occur in the chromosomes of a cell. Mutations are generally harmful, but sometimes a mutation may increase an organism’s ability to survive in its environment. Explain how this could lead to a change, over time, in the characteristics of a population of organisms. [4]

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28 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. 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. © UCLES 2010 0654/32/O/N/10 Group 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 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 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 DATA SHEET The Periodic Table of the Elements

UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education MARK SCHEME for the October/November 2010 question paper for the guidance of teachers 0654 CO-ORDINATED SCIENCES 0654/32 Paper 3 (Extended Theory), maximum raw mark 100 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 must be read in conjunction with the question papers and the report on the examination. • CIE will not enter into discussions or correspondence in connection with these mark schemes. CIE is publishing the mark schemes for the October/November 2010 question papers for most IGCSE, GCE Advanced Level and Advanced Subsidiary Level syllabuses and some Ordinary Level syllabuses. www.XtremePapers.com

Page 2 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 1 (a) (i) pink / orange / brown / copper (layer) ; [1] (ii) 2+ ; two negative charges from chloride must balance the charge on the copper ion / owtte ; [2] (iii) (L) it is a negative ion / has a negative charge / has more electrons than protons ; reference to attraction between opposite charges ; [2] (iv) × × × × × × × × × × × × × × Cl Cl one shared pair ; all other electrons correctly shown ; [2] (b) (i) carbon dioxide ; [1] (ii) 2PbO + C → 2Pb + CO2 ;; (correct formula then look for balance) [2] (iii) (no reaction) idea that carbon is less reactive than potassium ; and so cannot remove / combine with the oxygen ; [2] (allow 1 mark for saying potassium is too reactive) [Total: 12] 2 (a) ammeter current / amps A1 0.7 A2 0.3 A3 0.4 A4 0.3 ;; [2] (b) (i) (yes – no mark) straight line on graph so current is directly proportional to voltage ; [1] (ii) 2 amps ; explanation e.g. 13 × 0.15 A or 2 × 1 A ; [2] Cl Cl

Page 3 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 (c) (i) make magnetic field stronger ; only magnetic while the current is on ; so that magnetic field can be reversed ; [max 2] (ii) Vs = Vp × Ns / Np = 200 × 1000 / 10000 = 20 V ; [1] [Total: 8] 3 (a) water vapour lost from plant’s leaves ; transpiration ; condensation ; water vapour cooled ; gas changed to liquid / water vapour changed to water (droplets) ; ref. to particles and (kinetic) energy ; [max 4] (b) (i) loss of turgor (in leaf cells) / cells become flaccid ; because water lost from the cells ; [2] (ii) (supported by) xylem / lignin ; (reject if reason is that xylem contains water) [1] (iii) approximately similar shaped cell, with all parts shown ; outer cell wall slightly caved in ; vacuole much smaller ; cytoplasm pulled away from cell wall ; [max 3] [Total: 10] 4 (a) (i) sound / ultrasound ; [1] (ii) infra-red ; (iii) gamma ; [1] (b) (i) number of, waves / oscillations, per, second / unit time ; [1] (ii) (no – no mark) maximum human frequency about 20 000 Hz ; [1] (iii) v = f × λ ; wavelength = 330 / 50 000 ; = 0.0066 m ; [3] [Total: 8]

Page 4 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 5 (a) (filtration) microorganisms will pass through the filter / owtte ; [1] (allow idea that chlorination and distillation kill microorganisms whereas filtration does not) (b) light rays are scattered ; by reflection from dispersed material ; transparency requires most rays to be undeviated / owtte ; [max 2] (first two points could come from diagram of scattered rays) (c) (i) 0.05 ; [1] (ii) relevant working e.g. 0.05 × 12.5 / 1000; = 0.000625 ; [2] (iii) evidence of the use of molar ratio. e.g. 2 mols of alkali neutralise one mole of acid / acid to alkali = 1:2 / 0.000625 ÷ 2 ; = 0.00031(25) ; [2] [Total: 8] 6 (a) A written anywhere between 0 and 13 seconds ; [1] (b) area under graph / other working ; ½ × 12.8 × 8 = 51.2 m ; [2] (c) maximum speed = 16 m / s KE = ½ mv2 ; = 0.5 × 800 × 16 × 16 = 102 400 J ; [3] (d) momentum is directly proportional to v / momentum = mv ; KE is directly proportional to v2 / explained using numbers ; [2] [Total: 8] 7 (a) hair / fur ; mammary glands ; different types of teeth ; pinnae / ear flaps ; [max 2] (b) arterioles ; delivering blood to skin surface ; dilate / get wider ; so more blood flows close to skin surface ; loses heat (by radiation to air) ; [max 3]

Page 5 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 (c) (i) sensed by pancreas ; pancreas secretes insulin ; insulin affects liver ; causes liver to take glucose from blood ; (liver) converts glucose to glycogen ; [max 3] (ii) to heart from heart kidney bladder urethra ureter renal vein renal artery one renal artery and vein drawn and labelled ; two renal arteries and veins drawn ; (at least one) ureter drawn and labelled ; urethra drawn and labelled ; [4] [Total: 12] 8 (a) working ; 5 hours ; (allow leeway if carefully shown on graph) [2] (b) (i) causes, atoms / molecules, to lose electrons / to become ions ; [1] (ii) alpha is less penetrating and is stopped by, the air / clothes / skin ; alpha is more ionising and so causes more damage when close to cells ; [2]

Page 6 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 (c) (i) fusion is joining and fission is splitting (of atoms / nuclei) ; of nuclei ; [2] (ii) radiation leaks / ref. Chernobyl ; cancer / mutations in, local people / animals ; or disposal of waste ; needs to be stored safely for a long period ; [max 2] [Total: 9] 9 (a) Table 9.1 element name protons neutrons (oxygen) 8 8 phosphorus (15) (16) ;; (1 mark per row) [2] (b) (i) silicon / Si ; periodic pattern refers to (repeating) patterns (of properties) across periods / every eight elements / owtte ; silicon is eight elements further on (in Periodic Table) from element No. 6 / carbon ; [max 2] (ii) carbon has a giant structure and nitrogen is simple molecular ; much energy needed to, melt / break down, giants / converse for molecular ; because strong bonds must be broken / converse for molecular ; because many bonds must be broken / converse for molecular ; [max 3] (c) (i) H C H H C H ;; (2C and 4H bonded and double bond shown) [2] (ii) (catalytic / thermal) cracking ; fractions are boiled / vaporised / heated ; passed over (hot) catalyst / subjected to very high temperature and pressure ; [3] (iii) double bonds become single ; single bonds form between molecules to form a long chain ; [2] (marks can be obtained by clear diagrams) [Total: 14]

Page 7 Mark Scheme: Teachers’ version Syllabus Paper IGCSE – October/November 2010 0654 32 © UCLES 2010 10 (a) (i) 23 ; [1] (ii) 46 ; [1] (iii) nucleus ; [1] (b) (i) oviduct / fallopian tube ; [1] (ii) uterus / womb ; [1] (c) produces / contains, amniotic fluid ; protects / supports, embryo ; [2] (d) individual with the mutation is more likely to survive ; individual with the mutation is more likely to reproduce ; passing mutation on to its offspring ; repeated over many generations ; most / all, of population have the mutation ; and the characteristic that the mutated gene produces ; [max 4] [Total: 11]