0620_s11_qp_22.pdf

ww ap eP m e tr .X w om .c s er UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education *0710019578* CHEMISTRY 0620/22 Paper 2 May/June 2011 1 hour 15 minutes Candidates answer on the Question Paper. No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number, candidate number and name in the spaces at the top of this page. Write in dark blue or black pen. You may need to use a pencil for any diagrams, graphs 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 16. 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. For Examiner’s Use 1 2 3 4 5 6 7 Total This document consists of 14 printed pages and 2 blank pages. IB11 06_0620_22/4RP © UCLES 2011 [Turn over ... + – + – – + – + + – + – – + – + [1] [Total: 9] © UCLES 2011 0620/22/M/J/11 ..... is shared between two ......... (vi) an atom with a complete outer shell of electrons? [6] (b) Atoms D and F can combine to form a covalent molecule......... (ii) an atom containing six protons. B.. Which structure represents (i) an atom in Period 3 of the Periodic Table.. [2] (ii) Which one of the following structures represents an ionic compound? Tick one box.. atoms electrons ions neutrons solids A covalent bond is formed when a pair of ..... (iii) an atom of a Group I metal. C.. (iv) an atom of phosphorus....2 1 For Examiner’s Use The diagram shows the electronic structures of six atoms... E or F.. (v) an atom with six electrons in its outer shell.. more than once or not at all.. . (i) Complete the following sentence using words from the list... A B C D E F (a) Answer the following questions by choosing from the structures A........ You can use each structure once... D. ..........CO → ............................. iron................................................Fe + 3CO2 [2] (iii) In the blast furnace... ................................................................................... state the names of two other raw materials used in the blast furnace for the extraction of iron.......... [2] (ii) Complete this equation for the reaction of iron(III) oxide with carbon....................................................................... CO2 + C → 2CO Which substance gets reduced during this reaction? Explain your answer............................................ [1] (b) Iron is extracted by heating iron ore with carbon in a blast furnace......... ....... [1] (iii) State the name of the main ore of aluminium................................................................. carbon dioxide reacts with red hot carbon to form carbon monoxide..................... .................................. The table shows the temperatures required to produce different metals from their oxides by heating with carbon...................................... .................................................................................... ........................ [2] © UCLES 2011 0620/22/M/J/11 [Turn over ...... least reactive most reactive [1] (ii) Suggest why aluminium is extracted by electrolysis rather than by heating with carbon..............................3 2 Many metal oxides can be reduced with carbon........................................................................... Fe2O3 + .................... reaction temperature / °C aluminium oxide → aluminium 2100 iron oxide → iron 425 nickel oxide → nickel 475 zinc oxide → zinc 925 For Examiner’s Use (a) (i) Use the information in the table to arrange aluminium................................................. ............... and ............. nickel and zinc in order of their reactivity. (i) Apart from iron ore and carbon (coke)...... ................................................................. ............................................ ........................................................................... .....................................4 For Examiner’s Use (iv) State one adverse effect of carbon monoxide on health................................................................................ [1] (ii) Mild steel is an alloy.............................................................................. (i) What do you understand by the term alloy ? ................................................. State one use of mild steel......................................................................................................... [1] (v) The reaction between carbon dioxide and red hot carbon is endothermic................................ [1] (c) Iron is usually made into steel alloys................................... [1] [Total: 13] © UCLES 2011 0620/22/M/J/11 ................................... What do you understand by the term endothermic ? ....... .......................... [1] (c) State one use of copper........................................... [1] © UCLES 2011 0620/22/M/J/11 [Turn over ........................ [1] (ii) the mass of the wire in the tube............ [2] (b) The percentage of oxygen in air can be found using the apparatus shown below................. suggest what happens to (i) the total volume of air in the gas syringes............................................................................ nitrogen oxygen other gases (a) (i) What is the percentage of nitrogen in the air? ................................... [1] (ii) Apart from nitrogen and oxygen.................. ... The copper reacts with oxygen in the air.................................................................................... air copper wire air gas syringe heat Air is passed backwards and forwards over the heated copper using the syringes................. state the names of two gases present in unpolluted air.............................. copper + oxygen → copper(II) oxide As the experiment proceeds.................. .................................................................................................................................................. ........ and .....5 3 For Examiner’s Use The pie chart shows the composition of air............. ............................................................. ....................................................................................................................................... [3] [Total: 9] © UCLES 2011 0620/22/M/J/11 .................................... ...................................................................................... .................................... ............................................................... – + copper electrode steel spoon to be electroplated electrolyte Give a description of this electroplating............................ ● changes to the spoon....................6 For Examiner’s Use (d) A steel spoon can be electroplated using the apparatus shown.. In your answer...................................................................................................... ......................... ....................................................... .................... refer to: ● a suitable electrolyte that can be used..................................................................................... ● the anode and the cathode.............................................................................................................................................. ...... ................................... test .............................................................. + ethanol [1] (ii) State the conditions needed for fermentation.................................................... group......................... series...... [3] [Total: 12] © UCLES 2011 0620/22/M/J/11 [Turn over ............ Describe a test for an unsaturated hydrocarbon.............................. ................................. chemical properties because they contain the same .............................................................................................................. different functional homologous similar unreactive unsaturated Ethanol is a member of the alcohol .. result ........................................................................... [2] (d) Complete these sentences using words from the list.......................................................... glucose → .......... C 2H 4 H H C C H H + → H2O C2H5OH → + [2] (ii) Ethene is an unsaturated hydrocarbon......................... (a) (i) Complete the word equation for fermentation..... All alcohols have ......... State the names of the products formed when ethanol undergoes complete combustion. .................... [2] (b) (i) Complete the equation for the catalytic addition of steam to ethene by drawing the structures of water and ethanol in the boxes...................................................... and .............................. [2] (c) Ethanol can be used as a fuel...................7 4 For Examiner’s Use Ethanol can be produced by fermentation or by the catalytic addition of steam to ethene............................................................................ .................. Cl Cl Cl Cl C Cl C Cl C C Cl C Cl C Cl Cl Cl Cl What is the molecular formula of this compound? .................... [1] © UCLES 2011 0620/22/M/J/11 . ............................................................................................................................................... .................................................................................................................... covalent diatomic giant macromolecule molecule structure diamond .......................................................................................................................................................... .................................................................. chlorine ...........................8 5 For Examiner’s Use The structures of diamond and chlorine are shown below............................ diamond chlorine = carbon atom = chlorine atom (a) Describe the structure of these two substances............................................................................................................................................................................. ................................................................................................. [4] (b) The structure of a compound containing carbon and chlorine is shown below........................................................................................... Use the list of words to help you... .................... + ......................................................... ........................................................................................................................................................ ............................................................................................................................56 bromine –7 iodine red-brown +114 4.................................. [2] [Total: 13] © UCLES 2011 0620/22/M/J/11 [Turn over ...................................................................51 yellow chlorine –35 1............................. .. [1] (d) (i) Complete the word equation for the reaction of bromine with aqueous potassium iodide..... [1] (iii) Describe the trend in boiling point of the halogens down the group....................... ................................... .......................... electrical conductivity? .................................. bromine + potassium iodide → ...............................................................................................................................................93 grey-black Use the information in the table to answer the following questions.................................................. How do most ionic and molecular substances differ in their solubility in water.................................. (i) State the colour of chlorine................ .......................................................... (ii) Predict the density of liquid bromine.......... element boiling point / °C density in liquid state / g per cm3 colour fluorine –188 1............ ..................................................................... [2] (ii) Explain why bromine does not react with aqueous potassium chloride................9 For Examiner’s Use (c) Chlorine is a halogen................... ................................... [1] The table shows some properties of the halogens......... [1] (e) Potassium chloride is an ionic substance but iodine is a molecular substance......... ........................................................................................ [1] (c) Many centuries ago........................ Drops of a colourless liquid appeared at the mouth of the test-tube and the iron(II) sulfate turned white........................................................................... in a test-tube............. ........................ Write down the symbol which shows that a reaction is reversible.............................................. [1] (iv) The reaction in part (iii) can be reversed... sulfuric acid was made from iron(II) sulfate.............. result ...... (i) Describe what you would observe when sulfuric acid is added to blue litmus paper........................................................... Sulfuric acid is a typical acid.............................. (a) Describe how you can prepare pure dry crystals of iron(II) sulfate from iron powder and dilute sulfuric acid....... ........................................................................................................... (i) What is the meaning of the symbol (II) in this formula? .... [2] © UCLES 2011 0620/22/M/J/11 ....................... .............................................10 6 For Examiner’s Use Iron(II) sulfate is a light green salt................................................................................................................................................................. .................................. ..........7H2O............................ ..................... [1] (ii) Describe a test for iron(II) ions..................... [3] (b) The formula for iron(II) sulfate is FeSO4................................................................... [3] (iii) A student warmed a sample of iron(II) sulfate........................................................................................................................................................................................................ iron powder....................... FeSO4................................... ..................................................................................... Explain these observations........................................................... test ...... .............................................................................7H2O............. ..11 (ii) Farmers can add a solution of dilute sulfuric acid to their fields if the soil is too alkaline...................... [1] (iii) Which one of the following pH values best describes a solution which is slightly alkaline? Put a ring around the correct answer.. Explain why farmers do not want their fields to become too alkaline............................................................................................................ pH 1 pH 6 pH 7 pH 8 pH 14 [1] (iv) Give the name of a compound which farmers add to the soil to make it less acidic.............................................................................. [1] [Total: 14] © UCLES 2011 0620/22/M/J/11 [Turn over ................. For Examiner’s Use ........................... . ................................... The students in row C could smell the ammonia after 40 seconds....................................................................... ................................................................................... .................................................. [1] (ii) Explain these results using ideas about moving particles...... ............................ [3] (b) Ammonium carbonate has the formula (NH4)2CO3....................................................................................... [3] © UCLES 2011 0620/22/M/J/11 For Examiner’s Use .......................... Ammonium carbonate breaks down slowly at room temperature to release ammonia gas................................................ ammonium carbonate C B A The students in row A could smell the ammonia 10 seconds after the smelling salts had been put on the bench..................................... essential for plant growth............... [1] (c) Ammonia is used to make fertilisers such as ammonium sulfate.......................... (i) Suggest how long it took the students in row B to smell the ammonia....... Calculate the relative formula mass of ammonium carbonate.................12 7 Smelling salts are sometimes used to ‘wake up’ people who feel faint..... ............... ammonium carbonate → ammonia + carbon dioxide + water (a) A few crystals of ammonium carbonate were put on a bench at the front of a classroom................. that are present in fertilisers....................... The main chemical in smelling salts is ammonium carbonate.............. ................................. (i) State the names of the three chemical elements.............. Ammonium sulfate can be made by adding sulfuric acid to ammonia. 96 g of ammonium carbonate is formed. When ammonium sulfate is added to a solution of barium chloride. [1] (d) Ammonium carbonate is made by heating ammonium sulfate with excess calcium carbonate.13 For Examiner’s Use (ii) Which one of the following statements about ammonium sulfate is correct? Tick one box. [1] [Total: 10] © UCLES 2011 0620/22/M/J/11 . Farmers add ammonium sulfate to the soil to make it alkaline. ammonium sulfate + calcium carbonate → ammonium carbonate + calcium sulfate When 132 g of ammonium sulfate is reacted with calcium carbonate. When ammonium sulfate is heated with sodium hydroxide. carbon dioxide is given off. Calculate the mass of ammonium sulfate needed to make 240 g of ammonium carbonate. a blue precipitate is formed. 14 BLANK PAGE © UCLES 2011 0620/22/M/J/11 . 15 BLANK PAGE © UCLES 2011 0620/22/M/J/11 . ). Every reasonable effort has been made by the publisher (UCLES) to trace copyright holders.© UCLES 2011 Magnesium Sodium Calcium 0620/22/M/J/11 Strontium 89 Key b X a 72 b = proton (atomic) number X = atomic symbol a = relative atomic mass *58-71 Lanthanoid series 90-103 Actinoid series 88 Ac Actinium Ra Radium Fr Francium 87 * Hafnium Lanthanum 57 178 Hf 40 Zirconium Zr 91 Titanium 139 Yttrium 22 48 Ti La 39 Y 89 Scandium 21 227 56 Barium Caesium 45 Sc 226 55 137 Ba 133 Cs 38 Rubidium 37 88 Sr 85 Rb 20 Potassium 19 40 Ca 39 12 24 Mg 23 Na Beryllium 4 Lithium K 11 3 9 Be 7 II Li I 93 Ta 181 Niobium Nb 90 58 73 52 96 Mo W 184 Protactinium Thorium 55 Tc 186 Re 144 Nd 92 60 Uranium U 238 Neodymium 75 Rhenium 43 Technetium 25 Manganese Mn 27 59 28 59 29 64 30 65 5 Ru 101 Iron 190 Pm Osmium Os 93 Np Neptunium 61 Promethium 76 44 Ruthenium 26 56 Fe Sm 150 Iridium 94 Pu Plutonium 62 152 Eu 95 Am Americium 63 Europium 78 Platinum 195 Pt 192 46 Palladium Pd 106 Nickel Ni Ir Samarium 77 45 Rhodium Rh 103 Cobalt Co Gd 157 Gold Au 197 Silver 96 64 Curium Cm Gadolinium 79 47 Ag 108 Copper Cu 201 Bk Terbium Tb 159 Mercury Hg 97 Berkelium 65 80 48 Cadmium Cd 112 Zinc Zn 11 6 Dy 162 Thallium Tl 204 Indium 98 Cf Californium 66 Es Holmium Ho 165 Lead Pb 207 Tin 99 Einsteinium 67 82 50 119 Sn 115 32 Germanium Ge 73 Silicon In Gallium Dysprosium 81 49 31 70 Ga 14 28 Si Carbon 27 Aluminium 13 12 C Al Boron B 7 14 75 Sb 122 Arsenic As Bi 209 Fermium Fm Erbium Er 167 Bismuth 100 68 83 51 Antimony 33 15 Phosphorus P 31 Nitrogen N 8 Se 79 Sulfur S 32 Oxygen Po 169 Md Thulium Tm 101 Mendelevium 69 84 Polonium 52 Tellurium Te 128 Selenium 34 16 16 O 9 Yb 173 Astatine At Iodine I 127 Bromine Br 80 Chlorine No 102 Nobelium 70 Ytterbium 85 53 35 17 Cl 35.p. University of Cambridge International Examinations is part of the Cambridge Assessment Group. but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.5 Fluorine F 19 Lr Lutetium Lu 175 Radon Rn Xenon Xe 131 Krypton Kr 84 Argon Ar 40 Neon 103 Lawrencium 71 86 54 36 18 10 Ne 20 Helium 2 0 Hydrogen VII 4 VI He V 1 IV H III The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r. 91 Pa Th 232 Praseodymium Cerium 59 141 Pr 140 74 Tungsten 42 Molybdenum 24 Chromium Cr Ce Tantalum 41 23 Vanadium V 51 1 Group DATA SHEET The Periodic Table of the Elements 16 Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. which is itself a department of the University of Cambridge.t. . Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES).