Cambridge IGCSE Chemistry (BES) 0439 — 2017 Oct/Nov Paper 1 · Variant 1

This document consists of 15 printed pages and 1 blank page. IB17 11_0439_11/FP © UCLES 2017 [Turn over *9780951375* Cambridge International Examinations Cambridge International General Certificate of Secondary Education CHEMISTRY (US) 0439/11 Paper 1 Multiple Choice (Core) October/November 2017 45 minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended) READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples, paper clips, glue or correction fluid. Write your name, Center number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you. DO NOT WRITE IN ANY BARCODES. There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D. Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet. Read the instructions on the Answer Sheet very carefully. Each correct answer will score one mark. A mark will not be deducted for a wrong answer. Any rough working should be done in this booklet. A copy of the Periodic Table is printed on page 16. Electronic calculators may be used.

2 © UCLES 2017 0439/11/O/N/17 1 The diagram shows how the arrangement of particles changes when a substance changes state. Which change of state is shown? A boiling B condensation C evaporation D sublimation 2 Which method can be used to separate a mixture of salt and water to obtain both parts of the mixture? A crystallization B distillation C evaporation D filtration 3 A student put 25.0 cm3 of dilute hydrochloric acid into an Erlenmeyer flask. The student added 2.5 g of solid sodium carbonate and measured the change in temperature of the mixture. Which apparatus does the student need to use to obtain the most accurate results? A balance, graduated cylinder, thermometer B balance, pipet, stopwatch C balance, pipet, thermometer D buret, pipet, thermometer 4 Propanone, C3H6O, is a liquid at room temperature. What is the boiling point of pure propanone? A –61 °C to –51 °C B –56 °C C 51 °C to 61 °C D 56 °C

3 © UCLES 2017 0439/11/O/N/17 [Turn over 5 Which statement about the boxes P, Q and R is correct? P Q R A Box P contains two compounds and box R contains two elements. B Box P contains two elements and box Q contains a mixture. C Box P contains two elements and box Q contains one compound. D Box Q contains two compounds and box R contains a mixture. 6 The number of particles in atoms W, X, Y and Z are shown. protons electrons neutrons W 6 6 6 X 6 6 7 Y 7 7 7 Z 7 7 8 Which statement is correct? A W and X are isotopes of carbon. B X and Y are isotopes of nitrogen. C X has a mass number of 12. D Z has an atomic number of 8. 7 Which row describes the type of bonding present in substances 1 and 2? substance 1 substance 2 A methane has ionic bonding graphite has covalent bonding B graphite has ionic bonding potassium chloride has covalent bonding C potassium chloride has ionic bonding methane has covalent bonding D potassium chloride has ionic bonding graphite has ionic bonding

4 © UCLES 2017 0439/11/O/N/17 8 Substances with giant covalent structures can be used as lubricants and as cutting tools for hard materials. The diagram shows how the atoms are arranged in two giant covalent substances, X and Y. X Y key strong covalent bond weak attraction Which statement is correct? A Only X is used as a cutting tool and only Y is used as a lubricant. B Only X is used as a lubricant and only Y is used as a cutting tool. C X and Y are both used as cutting tools. D X and Y are both used as lubricants. 9 The equation shows the thermal decomposition of magnesium carbonate (Mr = 84). MgCO3 → MgO + CO2 Which mass of magnesium oxide is formed when 21.0 g of magnesium carbonate are completely decomposed? A 1.9 g B 4.0 g C 10.0 g D 40.0 g

5 © UCLES 2017 0439/11/O/N/17 [Turn over 10 Electricity is passed through concentrated aqueous sodium chloride. Inert electrodes are used. + – concentrated aqueous sodium chloride What is formed at the negative electrode? A chlorine B hydrogen C oxygen D sodium 11 Two chemical processes are described. ● During the combustion of gasoline, energy is …1… . ● During the electrolysis of sulfuric acid, energy is …2… . Which words complete gaps 1 and 2? 1 2 A given out given out B given out taken in C taken in given out D taken in taken in

6 © UCLES 2017 0439/11/O/N/17 12 When dilute sulfuric acid reacts with aqueous sodium hydroxide, the temperature of the solution increases. Which words describe this reaction? A endothermic and neutralization B endothermic and redox C exothermic and neutralization D exothermic and redox 13 The mass of a beaker and its contents is plotted against time. Which graph represents what happens when sodium carbonate reacts with an excess of dilute hydrochloric acid in an open beaker? mass time A mass time B mass time C mass time D 0 0 0 0 0 0 0 0 14 When blue copper(II) sulfate is heated, a white solid and water are formed. The white solid turns blue and gives out heat when water is added to it. Which terms describe the blue copper(II) sulfate and the reactions? the blue copper(II) sulfate is reactions A a mixture can be reversed B a mixture cannot be reversed C hydrated can be reversed D hydrated cannot be reversed 15 Which changes increase the rate of reaction between calcium carbonate and dilute hydrochloric acid? 1 increasing the concentration of the acid 2 increasing the temperature 3 increasing the size of the pieces of calcium carbonate A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

7 © UCLES 2017 0439/11/O/N/17 [Turn over 16 The equations for two reactions P and Q are given. P 2NaNO2 + O2 → 2NaNO3 Q 2HgO → 2Hg + O2 In which of these reactions does oxidation of the underlined substance occur? P Q A   B   C   D   17 What is not a typical characteristic of acids? A They react with alkalis producing water. B They react with all metals producing hydrogen. C They react with carbonates producing carbon dioxide. D They turn blue litmus paper red. 18 Magnesium, phosphorus and chlorine are elements in the same period of the Periodic Table. Which row describes the type of oxide formed by each of these elements? magnesium phosphorus chlorine A acidic acidic basic B acidic basic basic C basic acidic acidic D basic basic acidic 19 Zinc sulfate is made by reacting an excess of zinc oxide with dilute sulfuric acid. The excess zinc oxide is then removed from the solution. Which process is used to obtain solid zinc sulfate from the solution? A crystallization B dissolving C filtration D fractional distillation

8 © UCLES 2017 0439/11/O/N/17 20 What is used to test for chlorine? A a glowing splint B damp litmus paper C limewater D potassium manganate(VII) solution 21 Which statements about the trends across a period of the Periodic Table are correct? 1 Aluminum is more metallic than sodium. 2 Beryllium is more metallic than carbon. 3 Boron is more metallic than lithium. 4 Magnesium is more metallic than silicon. A 1 and 2 B 1 and 3 C 2 and 4 D 3 and 4 22 Astatine is an element in Group VII of the Periodic Table. Astatine is …1… reactive than iodine. The melting point of astatine is …2… than the melting point of iodine. Astatine is …3… in color than bromine. Which words complete gaps 1, 2 and 3? 1 2 3 A less higher darker B less lower lighter C more higher darker D more lower lighter 23 Which row describes the properties of a typical transition element? melting point forms colored compounds can act as a catalyst A high no no B high yes yes C low no yes D low yes no

9 © UCLES 2017 0439/11/O/N/17 [Turn over 24 Why is argon gas used to fill electric lamps? A It conducts electricity. B It glows when heated. C It is less dense than air. D It is not reactive. 25 What is a property of all metals? A conduct electricity B hard C low melting points D react with water 26 Which material is not involved in the large-scale extraction of iron from iron ore? A bauxite B calcium carbonate (limestone) C carbon (coke) D hematite

10 © UCLES 2017 0439/11/O/N/17 27 Some reactions of three metals are listed in the table. metal metal reacts with dilute hydrochloric acid metal oxide is reduced by carbon P yes no Q no yes R yes yes What is the order of reactivity of the metals? most reactive least reactive A P R Q B Q P R C R P Q D R Q P 28 Which uses of the metals shown are both correct? aluminum stainless steel A aircraft bodies cutlery B car bodies aircraft bodies C chemical plant food containers D food containers car bodies 29 The flow chart shows stages in the treatment of river water to produce drinking water. drinking water stage Y stage X settling tank river water What occurs at stages X and Y? X Y A distillation chlorination B distillation filtration C filtration chlorination D filtration distillation

11 © UCLES 2017 0439/11/O/N/17 [Turn over 30 Which gas is over 30% of air? A argon B carbon dioxide C nitrogen D oxygen 31 Iron is a metal that rusts in the presence of oxygen and water. Mild steel is used for …1… and is prevented from rusting by …2… . Stainless steel does not rust. It is produced by …3… iron with another metal. Which words complete gaps 1, 2 and 3? 1 2 3 A car bodies greasing covering B car bodies painting mixing C cutlery greasing covering D cutlery painting mixing 32 A mixture produces a gas both when it reacts with an acid and when it reacts with an alkali. Which ions are present in the mixture? A ammonium ions and carbonate ions B ammonium ions and oxide ions C hydrogen ions and carbonate ions D hydrogen ions and oxide ions 33 Some marble chips (calcium carbonate) are heated strongly and substances X and Y are formed. Substance X is a white solid that reacts with water, giving out heat. Substance Y is a colorless gas. What are substances X and Y? X Y A calcium chloride oxygen B calcium hydroxide carbon dioxide C calcium oxide carbon dioxide D calcium sulfate oxygen

12 © UCLES 2017 0439/11/O/N/17 34 The structures of some organic molecules are shown. C C CH3 H H3C H C CH3 H H H C CH3 H C CH3 H H H C H H C CH3 H CH3 H C H H 2 1 3 4 Which structures represent an alkane with four carbon atoms? A 1 only B 2 and 3 C 2 and 4 D 3 and 4 35 Some of the fractions obtained from the fractional distillation of petroleum are used as fuels for vehicles. Which two fractions are used as fuels for vehicles? A bitumen fraction and gasoline fraction B bitumen fraction and naphtha fraction C gasoline fraction and kerosene fraction D kerosene fraction and lubricating fraction 36 Burning fossil fuels releases heat energy. Which substance is not a fossil fuel? A coal B hydrogen C natural gas D petroleum 37 X, Y and Z are three hydrocarbons. X CH2=CH2 Y CH3–CH=CH2 Z CH3–CH2–CH=CH2 What do compounds X, Y and Z have in common? 1 They are all alkenes. 2 They are all part of the same homologous series. 3 They all have the same boiling point. A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

13 © UCLES 2017 0439/11/O/N/17 [Turn over 38 The table shows bonds that are present and bonds that are not present in compound X. bond C–C  C=C  C–H  C–O  C=O  O–H  What type of compound is X? A a carboxylic acid B an alcohol C an alkane D an alkene 39 The diagram shows a reaction sequence. butane ethene ethanol carbon dioxide and water X Y Z Which row names the processes X, Y and Z? X Y Z A cracking fermentation respiration B cracking hydration combustion C distillation fermentation respiration D distillation hydration combustion

14 © UCLES 2017 0439/11/O/N/17 40 Molecules of a substance react together as shown. H H H H C C H H H H C C H H C H H C H H C H H C H H C H H C H H H H C C + + Which type of reaction has taken place? A cracking B oxidation C polymerization D reduction

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16 © UCLES 2017 0439/11/O/N/17 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 –

® IGCSE is a registered trademark. This document consists of 3 printed pages. © UCLES 2017 [Turn over Cambridge Assessment International Education Cambridge International General Certificate of Secondary Education CHEMISTRY (US) 0439/11 Paper 1 Multiple Choice (Core) October/November 2017 MARK SCHEME Maximum Mark: 40 Published This mark scheme is published as an aid to teachers and candidates, to indicate the requirements of the examination. 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 2017 series for most Cambridge IGCSE®, Cambridge International A and AS Level components and some Cambridge O Level components.

0439/11 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2017 © UCLES 2017 Page 2 of 3 Question Answer Marks 1 D 1 2 B 1 3 C 1 4 D 1 5 C 1 6 A 1 7 C 1 8 B 1 9 C 1 10 B 1 11 B 1 12 C 1 13 B 1 14 C 1 15 B 1 16 B 1 17 B 1 18 C 1 19 A 1 20 B 1 21 C 1 22 A 1 23 B 1 24 D 1 25 A 1 26 A 1 27 A 1 28 A 1 29 C 1

0439/11 Cambridge IGCSE – Mark Scheme PUBLISHED October/November 2017 © UCLES 2017 Page 3 of 3 Question Answer Marks 30 C 1 31 B 1 32 A 1 33 C 1 34 C 1 35 C 1 36 B 1 37 B 1 38 A 1 39 B 1 40 C 1