Cambridge IGCSE Chemistry (BES) 0439 — 2018 Oct/Nov Paper 4 · Variant 1

READ THESE INSTRUCTIONS FIRST Write your Center 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. A copy of the Periodic Table is printed on page 16. You may lose marks if you do not show your working or if you do not use appropriate units. 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. CHEMISTRY (US) 0439/41 Paper 4 Theory (Extended) October/November 2018  1 hour 15 minutes Candidates answer on the Question Paper. No Additional Materials are required. Cambridge International Examinations Cambridge International General Certificate of Secondary Education This document consists of 15 printed pages and 1 blank page. [Turn over IB18 11_0439_41/FP © UCLES 2018 *3646578630*

2 0439/41/O/N/18 © UCLES 2018 1 The following formulae represent different substances. Al Ag CaCO3 CH4 Cl 2 Cu SO2 Answer the following questions using only these substances. Each substance may be used once, more than once or not at all. State which substance is: (a) used to make food containers … [1] (b) added to a blast furnace to remove impurities during the production of iron … [1] (c) the main constituent of natural gas … [1] (d) a cause of acid rain … [1] (e) a gas which bleaches damp litmus paper … [1] (f) a gas which contributes to climate change. … [1] [Total: 6]

3 0439/41/O/N/18 © UCLES 2018 [Turn over 2 The table gives some information about four different particles, A, B, C and D. particle number of electrons number of neutrons number of protons electronic structure charge on particle A 11 12 11 2,8,1 0 B 14 11 2,8,1 0 C 18 20 2,8,8 0 D 18 20 17 (a) Complete the table. The first row has been done for you. [4] (b) Give two particles from the table which are isotopes of each other. … [1] (c) Element Z is in the same group of the Periodic Table as A and is less reactive than A. State the identity of element Z. … [1] (d) C is unreactive. Use information from the table to explain why. … [1]  [Total: 7]

4 0439/41/O/N/18 © UCLES 2018 3 (a) Copper(II) nitrate decomposes when heated. Two gases, oxygen and nitrogen dioxide, and a solid are made in the reaction. A sample of copper(II) nitrate was decomposed using the apparatus shown. X aqueous sodium hydroxide copper(II) nitrate heat water (i) Complete the chemical equation for the reaction. 2Cu(NO3)2 O2 + …NO2 + … [2] (ii) Only oxygen gas is collected at X. Explain why. … … [1] (b) Nitrogen dioxide and other oxides of nitrogen are formed in car engines. Explain how nitrogen dioxide is formed in car engines. … … … … [2]

5 0439/41/O/N/18 © UCLES 2018 [Turn over (c) A teacher heated 18.8 g of copper(II) nitrate. (i) Calculate the number of moles of copper(II) nitrate present in the 18.8 g. … mol [2] (ii) Calculate the maximum number of moles of oxygen that can be made by heating 18.8 g of copper(II) nitrate. … mol [1] (iii) Calculate the maximum volume of oxygen at room temperature and pressure, in cm3, that can be made by heating 18.8 g of copper(II) nitrate. … cm3 [1] (d) A sample of copper(II) nitrate was dissolved in water to form an aqueous solution. The aqueous solution was split into three portions. A separate test was done on each portion as shown. test reagent added result 1 aqueous sodium hydroxide light blue precipitate forms 2 zinc powder solution changes from blue to colorless and a brown solid forms 3 ammonia gas is produced (i) Give the formula of the light blue precipitate formed in test 1. … [1] (ii) Explain the changes seen in test 2. … … … … [3] (iii) Identify the two reagents that must be added to the aqueous copper(II) nitrate in test 3. 1 … 2 …  [2]

6 0439/41/O/N/18 © UCLES 2018 (e) Copper(II) nitrate can be made by reacting copper(II) carbonate with nitric acid. One of the products is carbon dioxide. (i) Write a chemical equation for the reaction of copper(II) carbonate with nitric acid. … [2] (ii) Carbon dioxide is added to the air by living things. Name the chemical process by which living things add carbon dioxide to the air. … [1] (iii) Carbon dioxide is removed from the air by plants. Name the chemical process by which plants remove carbon dioxide from the air. … [1]  [Total: 19]

7 0439/41/O/N/18 © UCLES 2018 [Turn over 4 (a) Sulfuric acid is made industrially by a four-step process. step 1 Sulfur is burned in air to produce sulfur dioxide. step 2 Sulfur dioxide is converted into sulfur trioxide. step 3 Sulfur trioxide is reacted with concentrated sulfuric acid to produce oleum. step 4 Oleum is reacted with water to produce concentrated sulfuric acid. (i) Some sulfur is obtained by mining. Name one other major source of sulfur. … [1] (ii) What is the name of the process by which sulfuric acid is made industrially? … [1] (iii) Describe the conversion of sulfur dioxide into sulfur trioxide in step 2. In your answer, include: ● a chemical equation for the reaction ● the essential reaction conditions. … … … … … … … [5] (b) When concentrated sulfuric acid is added to glucose, C6H12O6, a black solid is produced. The concentrated sulfuric acid acts as a dehydrating agent. (i) What is removed from the glucose in this reaction? … [1] (ii) Name the black solid produced in this reaction. … [1]

8 0439/41/O/N/18 © UCLES 2018 (c) The gas hydrogen sulfide, H2S, is produced when concentrated sulfuric acid is added to solid potassium iodide. The reaction involves oxidation. (i) Define the term oxidation in terms of electron transfer. … [1] (ii) Complete the dot-and-cross diagram to show the electron arrangement in a molecule of hydrogen sulfide. Show outer shell electrons only. H H S [2] (iii) Hydrogen sulfide has a simple molecular structure. Explain why hydrogen sulfide has a low boiling point. … … … [2]

9 0439/41/O/N/18 © UCLES 2018 [Turn over (d) Dilute sulfuric acid reacts with aqueous sodium hydrogencarbonate in a neutralization reaction. H2SO4(aq) + 2NaHCO3(aq) Na2SO4(aq) + 2H2O(l) + 2CO2(g) In a titration, 0.200 mol / dm3 aqueous sodium hydrogencarbonate was used to neutralize 20.0 cm3 of dilute sulfuric acid of concentration 0.150 mol / dm3. (i) Calculate the number of moles of dilute sulfuric acid used in the titration. … mol [1] (ii) Calculate the number of moles of sodium hydrogencarbonate needed to neutralize the dilute sulfuric acid. … mol [1] (iii) Calculate the volume, in cm3, of 0.200 mol / dm3 aqueous sodium hydrogencarbonate needed to neutralize the dilute sulfuric acid. … cm3 [1] [Total: 17]

10 0439/41/O/N/18 © UCLES 2018 5 Hydrogen gas reacts with iodine gas. The equation is shown. H2(g) + I2(g) 2HI(g) The reaction is reversible and can reach equilibrium. (a) What is meant by the term equilibrium? … … … [2] (b) The graphs show how pressure affects the yield of hydrogen iodide, HI, at two different temperatures. yield of hydrogen iodide pressure 500 °C 700 °C (i) Explain why the yield at 500 °C does not change as the pressure is increased. … … [1] (ii) What can you conclude from the difference in the yield of hydrogen iodide at the two temperatures shown? Explain your answer. … … … [2]

11 0439/41/O/N/18 © UCLES 2018 [Turn over (c) The graph shows how the concentration of hydrogen iodide, HI, changes after hydrogen gas and iodine gas are mixed together in a sealed container. concentration of hydrogen iodide time (i) When is the rate of reaction fastest? … [1] (ii) The reaction was repeated at the same temperature and pressure but in the presence of a catalyst. Draw a graph on the same axes to show how the concentration of hydrogen iodide changes with time in the presence of a catalyst. [2] (d) A mixture of hydrogen gas and iodine gas is allowed to reach equilibrium. (i) Increasing the pressure of a gas increases its concentration. State and explain the effect of increasing the pressure on the rate of the forward reaction. … … … [2] (ii) State and explain the effect of increasing the temperature on the rate of the reverse reaction. … … … … … [3] [Total: 13]

12 0439/41/O/N/18 © UCLES 2018 6 (a) Ethane, C2H6, is a member of the homologous series called alkanes. Ethanol, C2H5OH, is a member of the homologous series called alcohols. (i) Alkanes are hydrocarbons. What is meant by the term hydrocarbon? … … [2] (ii) All members of a homologous series can be represented by a general formula. State the general formula of: ● alkanes … ● alcohols … [2] (iii) State two characteristics, other than having the same general formula, of members of a homologous series. 1 … … 2 … … [2] (b) Ethane can react with chlorine in a substitution reaction. (i) State one essential reaction condition. … [1] (ii) Draw the structure of the organic product formed by substitution of one of the hydrogen atoms in ethane with chlorine. Show all of the atoms and all of the bonds.  [1] (iii) Name the product of the substitution reaction between ethane and chlorine that does not contain carbon. … [1]

13 0439/41/O/N/18 © UCLES 2018 [Turn over (c) Propan-1-ol is an alcohol. The structure of propan-1-ol is shown. C H H H C H H C H H O H Propan-1-ol reacts with ethanoic acid to form an ester. Give the name of the ester formed in this reaction. … [1] (d) Ester Y has the structure shown. C H H H C H H H H C C H ester Y H O C O H (i) Give the molecular formula of ester Y. … [1] (ii) Draw the structures of the carboxylic acid and the alcohol used to make ester Y. Show all of the atoms and all of the bonds. Give the name of the carboxylic acid and the alcohol. structure of the carboxylic acid name of the carboxylic acid … structure of the alcohol name of the alcohol … [4]

14 0439/41/O/N/18 © UCLES 2018 (e) Nylon is a polyamide. Complete the diagram to show the structure of nylon. Show all of the atoms and all of the bonds present in the linkages. [3] [Total: 18]

15 0439/41/O/N/18 © UCLES 2018 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. 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. 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. BLANK PAGE

16 0439/41/O/N/18 © UCLES 2018 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 cesium 133 56 Ba barium 137 87 Fr francium – 88 Ra radium – 5 B boron 11 13 Al aluminum 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 –

This document consists of 9 printed pages. © UCLES 2018 [Turn over Cambridge Assessment International Education Cambridge International General Certificate of Secondary Education CHEMISTRY (US) 0439/41 Paper 4 Extended Theory October/November 2018 MARK SCHEME Maximum Mark: 80 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 International will not enter into discussions about these mark schemes. Cambridge International is publishing the mark schemes for the October/November 2018 series for most Cambridge IGCSE™, Cambridge International A and AS Level components and some Cambridge O Level components.

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 2 of 9 Generic Marking Principles These general marking principles must be applied by all examiners when marking candidate answers. They should be applied alongside the specific content of the mark scheme or generic level descriptors for a question. Each question paper and mark scheme will also comply with these marking principles. GENERIC MARKING PRINCIPLE 1: Marks must be awarded in line with: • the specific content of the mark scheme or the generic level descriptors for the question • the specific skills defined in the mark scheme or in the generic level descriptors for the question • the standard of response required by a candidate as exemplified by the standardisation scripts. GENERIC MARKING PRINCIPLE 2: Marks awarded are always whole marks (not half marks, or other fractions). GENERIC MARKING PRINCIPLE 3: Marks must be awarded positively: • marks are awarded for correct/valid answers, as defined in the mark scheme. However, credit is given for valid answers which go beyond the scope of the syllabus and mark scheme, referring to your Team Leader as appropriate • marks are awarded when candidates clearly demonstrate what they know and can do • marks are not deducted for errors • marks are not deducted for omissions • answers should only be judged on the quality of spelling, punctuation and grammar when these features are specifically assessed by the question as indicated by the mark scheme. The meaning, however, should be unambiguous. GENERIC MARKING PRINCIPLE 4: Rules must be applied consistently e.g. in situations where candidates have not followed instructions or in the application of generic level descriptors.

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 3 of 9 GENERIC MARKING PRINCIPLE 5: Marks should be awarded using the full range of marks defined in the mark scheme for the question (however; the use of the full mark range may be limited according to the quality of the candidate responses seen). GENERIC MARKING PRINCIPLE 6: Marks awarded are based solely on the requirements as defined in the mark scheme. Marks should not be awarded with grade thresholds or grade descriptors in mind.

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 4 of 9 Question Answer Marks 1(a) Al / aluminium 1 1(b) CaCO3/ calcium carbonate 1 1(c) CH4/ methane 1 1(d) SO2/ sulfur dioxide 1 1(e) Cl2/ chlorine 1 1(f) CH4/ methane 1 Question Answer Marks 2(a) M1 11 M2 18 M3 2.8.8 M4 –1 4 2(b) A and B 1 2(c) Li / Lithium 1 2(d) it has a complete or full or 8 electrons in the outer shell 1 Question Answer Marks 3(a)(i) 4NO2 2CuO M1 CuO as a product (1) M2 rest fully correct (1) 2 3(a)(ii) nitrogen dioxide is acidic OR nitrogen dioxide reacts with sodium hydroxide 1

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 5 of 9 Question Answer Marks 3(b) M1 nitrogen and oxygen (from the air) M2 (react) at high temperatures (in engine) or (electrical) spark (in engine) 2 3(c)(i) M1 188 M2 (18.8 / 188) = 0.1(00) 2 3(c)(ii) 0.05 1 3(c)(iii) 1200 1 3(d)(i) Cu(OH)2 1 3(d)(ii) Any three from: 1 zinc more reactive than copper 2 displacement / redox reaction OR zinc displaces copper OR zinc reacts with copper ions 3 copper is solid / copper is brown 4 zinc nitrate is colourless (solution) OR blue colour disappears because Cu2+ ions removed (from solution) max 3 3(d)(iii) M1 sodium hydroxide / NaOH M2 aluminium / Al 2 3(e)(i) CuCO3 + 2HNO3 Æ Cu(NO3)2 + CO2 + H2O M1 carbon dioxide and water as products M2 rest correct 2 3(e)(ii) respiration 1 3(e)(iii) photosynthesis 1

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 6 of 9 Question Answer Marks 4(a)(i) from petroleum or (crude) oil or fossil fuels 1 4(a)(ii) Contact (process) 1 4(a)(iii) M1 vanadium pentoxide or vanadium(V) oxide or V2O5 (catalyst); 1 M2 1–5 atmospheres; (Units required) 1 M3 450°C; units required 1 M4 2SO2 + O2 Æ 2SO3 ; 1 M5 equilibrium / reversible reaction in equation or text 1 4(b)(i) water / H2O 1 4(b)(ii) carbon / C 1 4(c)(i) (oxidation is) loss of electrons 1 4(c)(ii) M1 one shared pair between each H and S 1 M2 four unpaired electrons on S giving S a total of 8 outer shell electrons and no other unpaired electrons 1 4(c)(iii) M1 weak (attractive) forces OR (attractive) forces need little energy to overcome 1 M2 forces between molecules / intermolecular 1 4(d)(i) 0.003 1 4(d)(ii) 0.006 1 4(d)(iii) 30 1

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 7 of 9 Question Answer Marks 5(a) M1 forward and back reactions occur at equal rates 1 M2 concentration (of substances) remains constant 1 5(b)(i) equal / same number of moles on each side or amount / molecules (of gas) on each side is the same 1 5(b)(ii) M1 (forward) reaction exothermic or reverse reaction endothermic M2 yield lower at higher temperature or (position of) equilibrium moves left at higher temperature ORA 2 5(c)(i) at the start / beginning 1 5(c)(ii) M1 new line is steeper than printed line and starts at origin 1 M2 new line reaches same final volume as printed line 1 5(d)(i) M1 Faster and More particles per unit volume / dm3 / cm3 M2 More collisions per second / unit time or greater collision rate 2 5(d)(ii) Reaction faster and (particles) have more energy or (particles) move faster 1 more collisions per second or greater collision rate 1 more (of the) particles / collisions have energy greater than the activation energy or more particles / collisions have sufficient energy to react or a greater percentage / proportion / fraction of collisions are successful 1

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 8 of 9 Question Answer Marks 6(a)(i) M1 (compound that) contains carbon and hydrogen 1 M2 and no other elements / only 1 6(a)(ii) Alkanes: CnH2n+2 1 Alcohols CnH2n+1OH OR CnH2n+2O 1 6(a)(iii) any two from: Similar / same chemical properties Same functional group Trend or gradual change in physical properties (Neighbouring) members differ by CH2 max 2 6(b)(i) ultraviolet light / sunlight 1 6(b)(ii) 1 6(b)(iii) hydrogen chloride 1 6(c) propyl ethanoate 1 6(d)(i) C5H10O2 1

0439/41 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2018 © UCLES 2018 Page 9 of 9 Question Answer Marks 6(d)(ii) M1 1 M2 methanoic acid 1 M3 1 M4 butan-2-ol 1 6(e) M1 correct amide link between at least one pair of boxes M2 all three amide linkages between boxes are correct M3 continuation bonds shown 3