GCSE 4462/01 CHEMISTRY 1 FOUNDATION TIER SCIENCE A/CHEMISTRY. A.M. Tuesday, 13 January hour JAN W PMT.

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1 Surname Centre Number Candidate Number Other Names 0 GCSE 4462/01 W SCIENCE A/CHEMISTRY CHEMISTRY 1 FOUNDATION TIER A.M. Tuesday, 13 January hour For s use Question Maximum Mark Mark Awarded ADDITIONAL MATERIALS In addition to this paper you will need a calculator and a ruler INSTRUCTIONS TO CANDIDATES Use black ink or black ball-point pen. Do not use gel pen or correction fluid. Write your name, centre number and candidate number in the spaces at the top of this page. Answer all questions. Write your answers in the spaces provided in this booklet Total If you run out of space, use a standard 4-page continuation booklet. Number the question(s) clearly and put your continuation booklet in this question-and-answer booklet. No other style of answer booklet should be used. INFORMATION FOR CANDIDATES The number of marks is given in brackets at the end of each question or part-question. You are reminded of the necessity for good English and orderly presentation in your answers. Assessment will take into account the quality of written communication (QWC) in your answer to question 9. The Periodic Table is printed on the back cover of the examination paper and the formulae for some common ions on the inside of the back cover. JAN SM*(W )

2 2 Answer all questions. 1. (a) Draw lines to match each diagram below with the correct description. One has been done for you. [2] Diagram Description molecule of a compound molecule of an element mixture of two elements atom 02

3 (b) The following diagram shows an atom. 3 A B The box below contains some words that could be used in a description of the atom neutral electron positive negative nucleus orbit Use words from the box to complete the table. [2] Name Charge part A part B Turn over.

4 4 2. It is believed that the Earth s original atmosphere was produced from volcanoes. The following tables show the gases given out by a volcano and the gases present in today s atmosphere. Gas Amount given out by a volcano (%) Gas Amount present in today s atmosphere (%) water vapour 79.0 nitrogen 78.0 carbon dioxide 12.0 oxygen 21.0 sulfur dioxide 6.5 carbon dioxide 0.04 nitrogen 1.5 others 1.0 others including water vapour 0.9 (a) Using the information in the tables describe three differences between the gases given out by a volcano and today s atmosphere. [3] (b) Levels of carbon dioxide and oxygen have remained approximately constant for 3500 million years. Name the two natural processes that have allowed this to happen. [2]... and... (c) Human activity pollutes the atmosphere which leads to environmental problems. Name the gases responsible for the following problems. [2] Global warming... Acid rain

5 5 3. (a) Complete the following table that shows information about some compounds. [4] Compound Formula Number of atoms present Elements present aluminium chloride AlCl 3 4 aluminium and chlorine... CaO 2 calcium and oxygen copper(ii) sulfide CuS and sodium oxide... 3 sodium and oxygen (b) The following diagram represents a molecule of ethanol, C 2 H 5 OH. Give the names of the atoms represented by the following symbols. [2] Turn over.

6 6 4. The following table shows the ph of some common substances. Substance ph limewater 10.5 saliva 6.4 lemon juice 2.2 orange juice 2.6 milk of magnesia 10.0 (a) Use information from the table to answer parts (i) and (ii). (i) Name the strongest acid. [1] (ii) Name the substance closest to being neutral. [1] (b) Milk of magnesia is used to treat indigestion. It contains magnesium hydroxide which reacts with excess hydrochloric acid in the stomach. (i) Complete the following word equation to show the products formed. [2] magnesium hydroxide (ii) hydrochloric acid Another indigestion remedy contains calcium carbonate. Name the gas produced when calcium carbonate reacts with hydrochloric acid and state how this gas can be identified. [2] Gas produced... How this gas can be identified

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8 8 5. (a) Crude oil is a mixture of hydrocarbons. (i) State what is meant by a hydrocarbon. [1] (ii) Describe how crude oil was formed. [2] (b) The following pie chart shows the mass in kg of each fraction present in 200 kg of crude oil. naphtha = 10 kg bitumen = 20 kg kerosene = 16 kg refinery gases = 12 kg petrol = 98 kg diesel (i) Name the two fractions that are not used as fuels. [1]... and... (ii) Calculate the percentage of diesel present in this crude oil. [2] Percentage of diesel =... % 08

9 (iii) The names of some processes are given in the box below. 9 cracking polymerisation distillation electrolysis Name the process by which I. large hydrocarbon molecules can be made into smaller molecules, [1]... II. small reactive molecules can be joined together to produce long chains. [1] Turn over.

10 10 6. Fractional distillation of liquid air is similar to that of crude oil. The diagram below shows the apparatus used to separate the gases in air. Gas Boiling point ( C) nitrogen 196 argon 186 air fractionating column oxygen 183 cooler liquid air krypton and xenon 154 water removed (a) From the diagram, name the gas that has the lowest boiling point. [1] (b) Suggest a reason why krypton and xenon cannot be separated by this process. [1] (c) Air is cooled to 200 C. Give the state (solid, liquid or gas) of the water removed at this temperature and give a reason for your answer. [2] State of water removed... Reason... (d) Argon is used in light bulbs to prevent the filament from burning. State what property of argon makes it useful for this purpose. [1] 5 10

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12 12 7. (a) The following chart shows the melting points and boiling points of the elements in Group 7. fluorine melting point boiling point chlorine bromine iodine astatine Temperature ( C) Give the state (solid, liquid or gas) of bromine at room temperature giving the reasons for your answer. [2] (b) The following table shows the observations made when some Group 7 elements react with hydrogen. Element chlorine bromine iodine Observations explodes in sunlight violent reaction when heated reacts when heated strongly Describe the trend in reactivity within the group and use this trend to predict how astatine would react with hydrogen. [2] 12

13 13 (c) Group 7 elements also react with iron. Balance the following symbol equation that shows the reaction of iron and fluorine. [1] Fe + F 2 FeF 3 (d) Chlorine and iodine can be extracted from seawater by electrolysis. (i) Balance the following electrode equation showing how chlorine is formed. [1] Cl e Cl 2 (ii) Chlorides make up 55 % of the salts present in seawater and it is therefore economically viable to extract chlorine from seawater. Suggest a reason why iodine is no longer extracted in this way. [1] (iii) State the property of chlorine and iodine that make them suitable for use in disinfectants and antiseptics. [1] 8 13 Turn over.

14 14 8. (a) When a mixture of iron(iii) oxide and aluminium powder (thermite) is heated in the apparatus shown below, there is a violent reaction. There is a bright flame, sparks are produced and molten iron is formed. fuse of magnesium ribbon mixture of aluminium powder and iron(iii) oxide sand heat proof mat (i) Write a word equation for the reaction taking place. [2] (ii) Explain this reaction in terms of reactivity. [2] (iii) State how the observations would be different if the mixture were replaced with a mixture of copper powder and aluminium oxide. [1] 14

15 (b) 15 Iron is extracted from its ore in a blast furnace. iron ore, coke and limestone in hot air in slag iron (i) State the purpose of the following raw materials. [3] Iron ore Coke Limestone 15 Turn over.

16 (ii) 16 The following equation shows the reaction taking place. Fe 2 O 3 + CO Fe + CO 2 I. Balance the equation. [1] II. Iron(III) oxide is reduced during the reaction. Give the meaning of reduction. [1] 10 16

17 17 9. Describe the properties of metals and relate these properties to the uses of two metals of your choice. [6 QWC] END OF PAPER 6 17 Turn over.

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19 19 FORMULAE FOR SOME COMMON IONS POSITIVE IONS NEGATIVE IONS Name Formula Name Formula Aluminium Ammonium Barium Calcium Copper(II) Hydrogen Iron(II) Iron(III) Lithium Magnesium Nickel Potassium Silver Sodium Zinc Al 3+ + NH 4 Ba 2+ Ca 2+ Cu 2+ H + Fe 2+ Fe 3+ Li + Mg 2+ Ni 2+ K + Ag + Na + Zn 2+ Bromide Carbonate Chloride Fluoride Hydroxide Iodide Nitrate Oxide Sulfate Br 2 CO 3 Cl F OH I NO 3 O 2 2 SO 4 19 Turn over.

20 20 PERIODIC TABLE OF ELEMENTS 1 2 Group H 4 He 2 Hydrogen Helium 7 Li 3 9 Be B 12 C 6 14 N 7 16 O 8 19 F 9 20 Ne 10 Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon 23 Na Mg Al Si 31 P S Cl Ar Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon K 40 Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rb 88 Sr Y Zr Nb Mo Tc Ru Rh 106 Pd Ag Cd In Sn Sb 128 Te I Xe 54 Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon 133 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 86 Caesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon 223 Fr Ra Ac 89 Francium Radium Actinium Key: Mass number Atomic number A X Element Symbol Z Name 20