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NSW HSC 2009 : CHEMISTRY

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2009 H I G H E R S C H O O L C E R T I F I C AT E E X A M I N AT I O N Chemistry Total marks 100 General Instructions Reading time 5 minutes Working time 3 hours Write using black or blue pen Draw diagrams using pencil Board-approved calculators may be used A data sheet and a Periodic Table are provided at the back of this paper Write your Centre Number and Student Number at the top of pages 9, 11, 13, 15 and 17 S ection I Pages 2 20 75 marks This section has two parts, Part A and Part B Part A 15 marks Attempt Questions 1 15 Allow about 30 minutes for this part Part B 60 marks Attempt Questions 16 26 Allow about 1 hour and 45 minutes for this part S ection II Pages 21 33 25 marks Attempt ONE question from Questions 27 31 Allow about 45 minutes for this section 115 Section I 75 marks Part A 15 marks Attempt Questions 1 15 Allow about 30 minutes for this part Use the multiple-choice answer sheet for Questions 1 15. 1 Which of the following is an important factor in predicting the nuclear stability of an isotope? (A) Atomic radius (B) Nuclear radius (C) The ratio of neutrons to protons (D) The ratio of electrons to protons 2 Unpolluted rain water in New South Wales is slightly acidic. Which substance is the major contributor to this acidity? (A) Ozone (B) Sulfur dioxide (C) Carbon dioxide (D) Nitrogen dioxide 3 Which of the following groups contains ONLY acidic substances? (A) Antacid tablets, baking soda, laundry detergents (B) Blood, oven cleaner, seawater (C) Milk, tea, drain cleaner (D) Vinegar, wine, aspirin 2 4 What flame colour is produced by barium ions in a flame test? (A) Red (B) Blue (C) Green (D) Orange 5 The apparatus shown is used in a first-hand investigation to determine and compare the heat of combustion of three different liquid alkanols. Thermometer Beaker of water Gauze mat Tripod Spirit burner with alkanol Which is the independent variable? (A) Type of alkanol used (B) Amount of water used (C) Amount of alkanol used (D) Temperature change in the water 3 6 Bromine, Br2, dissolves in unsaturated hydrocarbons and reacts immediately. Which of the following is the best description of this process? (A) Bromine is polar and reacts by adding bromine atoms across the double bond. (B) Bromine is polar and reacts by substituting hydrogen atoms with bromine atoms. (C) Bromine is non-polar and reacts by substituting hydrogen atoms with bromine atoms. (D) Bromine is non-polar and reacts by adding bromine atoms across the double bond. 7 What is the conjugate base of HSO4 ? (A) SO3 2 (B) SO42 (C) H2SO4 (D) HSO3 8 Three separate colourless solutions each contain one cation, Na+, Pb2+ or Ca2+. Which of the following would be an appropriate reagent to unambiguously identify the solution containing Pb2+ ? (A) KI (B) K2CO3 (C) K3PO4 (D) AgNO3 9 One test used for random breath testing in NSW involved crystals of potassium dichromate reacting with ethanol. In this reaction the orange dichromate ion, Cr2O72 , changes to the green chromium ion, Cr 3+. Which statement is true for this reaction? (A) Chromium has lost electrons and reached a lower oxidation state. (B) Chromium has lost electrons and reached a higher oxidation state. (C) Chromium has gained electrons and reached a lower oxidation state. (D) Chromium has gained electrons and reached a higher oxidation state. 4 10 Which of the following is the main organic product resulting from the reaction of butanoic acid and pentanol? O (A) H3C H2C H2C C O CH2 CH2 CH2 CH3 O (B) H3C H2C H2C C O CH2 CH2 CH2 CH2 CH3 O (C) H3C H2C H2C H2C C O CH2 CH2 CH2 CH2 CH3 O (D) H3C CH2 CH2 CH2 CH2 C O CH2 CH2 CH2 CH3 11 The following process is used to purify water for drinking. Step 1 Step 2 Step 3 Step 4 Step 5 Screening ? ? ? Chlorination Which sequence represents the correct order of Steps 2, 3 and 4? Step 2 Step 3 Step 4 (A) Flocculation pH adjustment Settling (B) pH adjustment Flocculation Settling (C) pH adjustment Settling Flocculation (D) Flocculation Settling pH adjustment 5 12 What is the IUPAC name of the following compound? CH3 H F C C C C H H Cl Cl H H CH3 (A) 3,4 dichloro 2 fluorohexane (B) 3,4 dichloro 5 fluorohexane (C) 2 fluoro 3,4 dichlorohexane (D) 5 fluoro 3,4 dichlorohexane 13 In a fermentation experiment 6.50 g of glucose was completely converted to ethanol and carbon dioxide. What is the mass of carbon dioxide produced? (A) 1.59 g (B) 3.18 g (C) 9.53 g (D) 13.0 g 14 Citric acid, the predominant acid in lemon juice, is a triprotic acid. A student titrated 25.0 mL samples of lemon juice with 0.550 mol L 1 NaOH. The mean titration volume was 29.50 mL. The molar mass of citric acid is 192.12 g mol 1. What was the concentration of citric acid in the lemon juice? (A) 1.04 g L 1 (B) 41.6 g L 1 (C) 125 g L 1 (D) 374 g L 1 6 The graph shows the maximum dissolved oxygen concentration in water as a function of temperature at normal atmospheric pressure. O2 Concentration (mg L 1) 15 14 12 10 8 6 0 5 10 15 20 25 Temperature ( C) 30 35 What is the volume of O2 that can dissolve in 10.0 L of water at 25 C and normal atmospheric pressure? (A) 62.0 mL (B) 63.5 mL (C) 80.0 mL (D) 124 mL 7 BLANK PAGE 8 Board of Studies NSW 2009 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Part B 60 marks Attempt Questions 16 26 Allow about 1 hour and 45 minutes for this part Student Number Answer the questions in the spaces provided. Show all relevant working in questions involving calculations. Question 16 (3 marks) Describe how to prepare an ester in the school laboratory. Include a specific safety precaution in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 116 9 3 Question 17 (4 marks) Water and ethanol are both used as solvents. Explain the differences and similarities in their solvent behaviour in terms of their molecular structures. Include a diagram in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 10 Board of Studies NSW 2009 4 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Question 18 (5 marks) There has been an increase in the concentration of the oxides of nitrogen in the atmosphere as a result of combustion. Assess both the evidence to support this statement and the need to monitor these oxides. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ........................................................................................................................................ 116a 11 5 Question 19 (6 marks) Outline the chemical and physical processes involved in the production of ONE of the following from a natural raw material: a polyethylene bottle a polyvinyl chloride pipe a polystyrene cup. Include relevant chemical equations in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 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......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 12 Board of Studies NSW 2009 6 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Question 20 (4 marks) (a) Calculate the mass of ethanol that must be burnt to increase the temperature of 210 g of water by 65 C, if exactly half of the heat released by this combustion is lost to the surroundings. 3 The heat of combustion of ethanol is 1367 kJ mol 1. ............................................................................................................................... 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(b) What are TWO ways to limit heat loss from the apparatus when performing a first-hand investigation to determine and compare heat of combustion of different liquid alkanols? ............................................................................................................................... ............................................................................................................................... 117 13 1 Question 21 (6 marks) The graph shows changes in pH for the titrations of equal volumes of solutions of two monoprotic acids, Acid 1 and Acid 2. 14 12 Acid 1 pH 10 Acid 2 8 6 4 2 0 (a) 0 10 20 30 40 50 Volume of KOH(aq) (mL) 60 Explain the differences between Acid 1 and Acid 2 in terms of their relative strengths and concentrations. 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Name the salt produced by the reaction of an acid of the same type as Acid 2 with KOH(aq). 1 ............................................................................................................................... (c) Calculate the concentration of hydrogen ions when 20 mL of KOH(aq) has been added to Acid 1. 1 ............................................................................................................................... ............................................................................................................................... (d) Why would phenolphthalein be a suitable indicator for both titrations? ............................................................................................................................... ............................................................................................................................... 14 Board of Studies NSW 2009 1 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Question 22 (7 marks) The nitrogen content of bread was determined using the following procedure: A sample of bread weighing 2.80 g was analysed. The nitrogen in the sample was converted into ammonia. The ammonia was collected in 50.0 mL of 0.125 mol L 1 hydrochloric acid. All of the ammonia was neutralised, leaving an excess of hydrochloric acid. The excess hydrochloric acid was titrated with 23.30 mL of 0.116 mol L 1 sodium hydroxide solution. (a) Write balanced equations for the TWO reactions involving hydrochloric acid. 2 ............................................................................................................................... ............................................................................................................................... (b) Calculate the moles of excess hydrochloric acid. 1 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Calculate the moles of ammonia. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (d) Calculate the percentage by mass of nitrogen in the bread. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 118 15 2 Question 23 (6 marks) The graph shows the variation in concentration of reactant and products as a function of time for the following system. COCl2(g) Cl2(g) + CO(g) H = + 108 kJ Concentration (mol L 1) 0.14 Cl2 0.12 0.10 CO 0.08 0.06 COCl2 0.04 0.02 0.00 0 2 4 6 8 10 12 Time (min) 14 16 18 Identify and explain each of the changes in conditions that have shaped the curves during the time the system was observed. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 16 Board of Studies NSW 2009 6 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Question 24 (5 marks) Describe the principle of atomic absorption spectroscopy and its application in environmental monitoring. Include a diagram in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ........................................................................................................................................ 119 17 5 Question 25 (7 marks) An analytical chemist determined the phosphate concentration of water samples from three local streams. Using the absorbance values in the table and graph, determine the mean absorbance and mean phosphate concentration for each stream and complete the table. Stream Absorbances measured 1 Mean absorbance 2 0.513, 0.511, 0.514 3 Mean phosphate concentration (mg L 1) 0.090, 0.092, 0.088 0.234, 0.237, 0.234 0.600 0.500 Absorbance (a) 0.400 0.300 0.200 0.100 0.000 0.000 0.050 0.100 0.150 Phosphate concentration (mg L 1) Question 25 continues on page 19 18 0.200 2 Question 25 (continued) (b) The recommended maximum level of phosphate in streams is 0.100 mg L 1. With reference to the recommended maximum level of phosphate for stream water, explain why there are differences between the three streams. 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Why is phosphate concentration a water quality issue? ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 25 19 2 Question 26 (7 marks) An electrochemical cell is constructed using two half cells. One half cell consists of an inert platinum electrode and a solution of Fe2+ and Fe3+. The other half cell consists of a lead electrode and a solution of Pb2+. Current will flow from one electrode to the other electrode when the cell is completed using a voltmeter and a salt bridge. (a) Write relevant half equations and a balanced net ionic equation for the overall cell reaction. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Calculate the standard cell potential (E ). 1 ............................................................................................................................... ............................................................................................................................... (c) Identify the anode, cathode, metals and ions by labelling the following diagram. 3 e V ................... ................... (d) ................... ................... Identify an appropriate electrolyte to use in the salt bridge. ............................................................................................................................... 20 Board of Studies NSW 2009 1 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Section II 25 marks Attempt ONE question from Questions 27 31 Allow about 45 minutes for this section Answer the question in a writing booklet. Extra writing booklets are available. Show all relevant working in questions involving calculations. Pages Question 27 Question 28 Shipwrecks, Corrosion and Conservation ............................ 24 25 Question 29 The Biochemistry of Movement .......................................... 26 27 Question 30 The Chemistry of Art ........................................................... 28 30 Question 31 120 Industrial Chemistry ............................................................. 22 23 Forensic Chemistry .............................................................. 31 33 21 Question 27 Industrial Chemistry (25 marks) (a) Sulfuric acid is one of the world s most significant industrial chemicals because of the variety and importance of its uses. (i) 1 (ii) Outline the industrial process for the manufacture of sulfuric acid from its raw materials. 3 (iii) (b) Identify the major use of sulfuric acid. Account for the safety precautions associated with the industrial transport of sulfuric acid. 2 At a particular temperature, iodine trichloride dissociates into iodine gas and chlorine gas according to the following equation: 2ICl3(g) I2(g) + 3Cl2(g) H = 240 kJ Initially 0.35 mol of ICl3(g) was introduced into a 1.0 L container and allowed to come to equilibrium. At equilibrium there was 0.45 mol L 1 of Cl2(g). (i) Write the equilibrium constant expression for this reaction. 1 (ii) Calculate the value of K at this temperature. 3 (iii) What are TWO consequences of increasing the temperature of the mixture at equilibrium? 2 Question 27 continues on page 23 22 Question 27 (continued) (c) 2 Account for a use of an emulsion in terms of its properties. (e) (i) Explain the cleaning action of soap in terms of its molecular structure. 2 (ii) (d) Soap is one product of saponification. Name the other product and draw its structural formula. 2 The flowchart summarises the fundamental criteria that must be considered in order to find a suitable location for an industrial plant. 7 use raw materials production waste With reference to the flowchart, explain the significance of each criterion to determine a suitable location for an industrial plant to manufacture sodium carbonate. End of Question 27 23 Question 28 Shipwrecks, Corrosion and Conservation (25 marks) (a) Tins and cans are used to store a range of foods, beverages and general household chemicals. ZOOL A OL C in in vinegar Tun e rin b a in (i) Identify the passivating metal used in drink cans in Australia. 1 (ii) Compare the use and effectiveness in preventing corrosion of different protective coatings on containers, such as those shown. 3 (b) Galvanising is used outside the home on water tanks and fencing. Explain the protection provided to iron by galvanising. 2 (c) The roof guttering on a garage has rusted through. (i) Explain, using chemical equations, the cause of this problem. 2 (ii) The owners have decided to replace the guttering. They have steel screws and a choice of aluminium or copper guttering. 4 Justify the course of action the owners should take, based on chemical principles. Question 28 continues on page 25 24 Question 28 (continued) (d) (i) The diagram shows an electrolytic cell used to conserve an iron artefact recovered from the wreck of a ship that sank in the early 1800s. 3 Power supply Stainless steel electrode (or mesh) Iron artefact Sodium hydroxide solution Explain how this process is used to conserve this iron artefact. Describe, with the aid of a diagram, how a nickel spoon could be silver-plated using equipment available in a school laboratory. 3 The flowchart summarises the historical development of the understanding of electron transfer reactions. 7 (ii) (e) Galvani suggests animal electricity Volta makes first battery Davy isolates alkali metals Faraday develops laws of electrolysis With reference to the flowchart, describe how the work of the scientists led to a better understanding of electron transfer reactions. End of Question 28 25 Question 29 The Biochemistry of Movement (25 marks) (a) Identify a factor that will cause denaturation of a protein molecule. 1 (ii) (b) (i) Explain denaturation of a protein in terms of its structure and bonding. 2 All enzymes are proteins. Polyphenoloxidase (PPO) is an enzyme that catalyses the browning of fruit and vegetables. This catalytic action can be studied in the laboratory by monitoring the oxidation of a phenol to a quinone, a red compound. The intensity of the red colour indicates the extent of the reaction. A student studied the enzyme activity of PPO in relation to a number of biological factors, using quinone as the measure of activity. The following table summarises the results of one set of these experiments. pH at 37 C Colour 3.0 4.0 5.0 6.0 7.0 8.0 colourless light red medium red dark red dark red colourless Account for this set of experimental results in terms of the characteristics of reactions involving enzymes. Question 29 continues on page 27 26 3 Question 29 (continued) (c) The following energy diagram shows the energy change associated with the combustion of glucose in kJ mol 1 during cellular respiration. 181 kJ mol 1 Energy Reactants 2997 kJ mol 1 Products Progress of reaction (i) Write a balanced chemical equation for the combustion of glucose. Include the energy released per mole of glucose. 2 (ii) Calculate the energy released per gram of glucose. 2 (iii) An average cyclist uses 80 kJ for every km travelled. If the glucose content of an energy bar is 36.7 g, how far can an average cyclist travel on only one energy bar? 2 (d) Analysing the structure of the glycerol molecule helps explain many of its properties. (i) Explain the viscosity of glycerol and its solubility in water. (ii) Explain the solubility of both fatty acids and triacylglycerols in water in terms of their molecular structures. (e) 3 3 The flowchart summarises a particular biochemical pathway related to muscle cell respiration. 7 glycogen ATP production muscle cell contraction muscle fatigue and cramping With reference to the flowchart, describe how a knowledge of the biochemical reactions involved in muscle cell respiration has led to more informed training programs. Include relevant chemical equations in your answer. End of Question 29 27 Question 30 The Chemistry of Art (25 marks) (a) (i) Name a monodentate ligand. 1 The ethylenediaminetetraacetate ion (EDTA) is a polydentate ligand. It is sometimes used to treat people suffering from heavy metal poisoning. O C CH2 O O C CH2 CH2 N O CH2 N O CH2 CH2 O C C O O EDTA (ii) With reference to EDTA, explain what is meant by the term polydentate ligand. 2 (iii) Using copper as the ion and EDTA as the ligand, explain how bonding occurs between a metal ion and a ligand. 3 Question 30 continues on page 29 28 Question 30 (continued) (b) (i) What is the maximum number of electrons that a p-orbital can hold? (ii) Write the full electron configurations for a Ca atom in the ground state, an excited Ca atom and a Ca+ ion. (c) The graph shows the first ionisation energy of some elements. 1 2 3 First ionisation energy kJ mol 1 2500 2000 1500 1000 500 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 Atomic Number Account for the trends in the graph in terms of the electron configuration of the elements. (d) (i) Gustav Kirchhoff formulated a law that states that a hot gas produces light with spectral lines at discrete wavelengths . 3 Explain the chemical principle that underpins this law. (ii) Describe how a first-hand investigation in the school laboratory could be undertaken to determine the presence of a particular metal in a water sample using a flame test. Give a reason why this method may not work. Question 30 continues on page 30 29 3 Question 30 (continued) (e) The flowchart summarises the development of pigments over time. natural sources refined mineral synthetic inorganic synthetic organic Historically many pigments have contained elements with atomic numbers in the range of 22 to 30. With reference to the flowchart, describe the use of pigments containing these elements and the origin of pigment colour at the atomic level. End of Question 30 30 7 Question 31 Forensic Chemistry (25 marks) (a) (i) This structure represents a biological molecule. Bond H H C C O N C C CH2 O N H H H CH3 O H SH Alanine Cysteine Name the specific type of covalent bond indicated. 1 (ii) Distinguish between the primary, secondary and tertiary structures of proteins. 3 (iii) How could electrophoresis be used to identify the origins of proteins in an investigation of adulterated food? 2 Question 31 continues on page 32 31 Question 31 (continued) (b) An oil spill occurred at a shipping port. To determine which ship was responsible, a sample of the oil was collected and analysed by gas chromatography. Samples of bunker oil were collected from three ships in port at the time and analysed by gas chromatography. The chromatograms of the samples collected are shown. Signal intensity Ship A sample 0 1 2 34567 Retention time / mins 8 9 Signal intensity 10 Ship B sample 0 1 2 34567 Retention time / mins 8 9 Signal intensity 10 Ship C sample 0 1 2 34567 Retention time / mins 8 9 Signal intensity 10 Oil spill sample 0 1 2 34567 Retention time / mins 8 9 10 (i) 1 (ii) (c) By comparing the chromatograms identify whether the oil spill originated from one of these vessels. Explain what the peaks in the chromatograms represent. 2 Describe the features of instrumental chromatography (GLC or HPLC) that allow the analysis of small samples. Question 31 continues on page 33 32 3 Question 31 (continued) (e) (i) Describe how a first-hand investigation in the school laboratory could be used to separate and identify the components of a mixed food dye. 3 (ii) (d) Describe the chemical tests that could be used to distinguish between alkenes, alkanols and alkanoic acids. 3 The flowchart summarises the steps involved in sample processing and presentation of results for a forensic investigation. 7 sample collection initial examination and classification of material instrumental analysis interpretation of results to a non-scientist You are the forensic chemist investigating a crime scene and collecting samples. With reference to the flowchart, describe how you would process the sample and present the results. Illustrate your answer with relevant tests and appropriate analyses. End of paper 33 BLANK PAGE 34 BLANK PAGE 35 BLANK PAGE 36 Board of Studies NSW 2009 2 009 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry DATA SHEET Avogadro constant, NA .................................................................. 6.022 1023 mol 1 Volume of 1 mole ideal gas: at 100 kPa and at 0 C (273.15 K) ...................... 22.71 L at 25 C (298.15 K) .................... 24.79 L Ionisation constant for water at 25 C (298.15 K), Kw ................. 1.0 10 14 Specific heat capacity of water ..................................................... 4.18 103 J kg 1 K 1 Some useful formulae H = m C T pH = log10 [H+ ] Some standard potentials K+ + e 2+ 2+ Ba Ca K(s) 2.94 V + 2e Ba(s) 2.91 V + 2e Ca(s) 2.87 V Na(s) 2.71 V Mg(s) 2.36 V Al(s) 1.68 V + Na + e Mg 2+ 3+ Al + 2e + 3e Mn2+ + 2e Mn(s) H2O + e 1 H2(g) + OH 2 2+ 2+ 2+ + 2e 2+ + 2e 2+ + 2e Zn Fe Ni Sn Pb + 2e Zn(s) 0.76 V + 2e Fe(s) 0.44 V Ni(s) 0.24 V Sn(s) 0.14 V Pb(s) 0.13 V 2 Cu 2+ 1 H2(g) 2 + + 2e + 2e Cu + e 1 I2(s) + e 2 1 I2(aq) + e 2 3+ +e + Ag + e 1 Br2(l ) + e 2 1 Br2(aq) + e 2 1 O2(g) + 2H+ + 2e 2 1 Cl2(g) + e 2 1 Cr2O72 + 7H+ + 3e 2 1 Cl2(aq) + e 2 MnO4 + 8H+ + 5e 1 F2(g) + e 2 120a 0.16 V Cu(s) 0.00 V SO2(aq) + 2H2O + 4H + 2e 1 O2(g) + H2O 2 + Fe 0.83 V H+ + e SO4 1.18 V 0.34 V 0.40 V Cu(s) 0.52 V 2OH 0.54 V I 0.62 V Fe2+ 0.77 V Ag(s) 0.80 V 1.08 V Br 1.10 V H2O 1.23 V Cl 1.36 V 7 Cr3 + + H2O 2 1.36 V I Br Cl Mn F 1.40 V 2+ + 4H2O 1.51 V 2.89 V Aylward and Findlay, SI Chemical Data (5th Edition) is the principal source of data for this examination paper. Some data may have been modified for examination purposes. 37 38 22 Ti 47.87 56 Ba 137.3 Barium 88 Ra [226] Radium 55 Cs 132.9 Caesium 87 Fr [223] Francium Rutherfordium 104 Rf [261] Hafnium 72 Hf 178.5 Zirconium 90 Th 232.0 Thorium Actinoids 89 Ac [227] Actinium Protactinium 91 Pa 231.0 Praseodymium 59 Pr 140.9 Dubnium 105 Db [262] Tantalum 73 Ta 180.9 Niobium 41 Nb 92.91 Vanadium 23 V 50.94 Uranium 92 U 238.0 Neodymium 60 Nd 144.2 Seaborgium 106 Sg [266] Tungsten 74 W 183.8 Molybdenum 42 Mo 95.94 Chromium 24 Cr 52.00 27 Co 58.93 Neptunium 93 Np [237] Promethium Plutonium 94 Pu [244] Samarium 62 Sm 150.4 Hassium Bohrium 61 Pm [145] 108 Hs [277] 107 Bh [264] Americium 95 Am [243] Europium 63 Eu 152.0 Meitnerium 109 Mt [268] Iridium Osmium Rhenium Rhodium 77 Ir 192.2 Ruthenium 45 Rh 102.9 Iron 44 Ru 101.1 Cobalt 26 Fe 55.85 Gold 79 Au 197.0 76 Os 190.2 75 Re 186.2 Technetium 43 Tc [97.91] Manganese 25 Mn 54.94 Atomic Weight Atomic Number KEY 111 Rg [272] Gold 79 Au 197.0 Silver 47 Ag 107.9 Copper 29 Cu 63.55 Curium 96 Cm [247] Gadolinium 64 Gd 157.3 Berkelium 97 Bk [247] Terbium 65 Tb 158.9 Darmstadtium Roentgenium 110 Ds [271] Platinum 78 Pt 195.1 Palladium 46 Pd 106.4 Nickel 28 Ni 58.69 Name of element Symbol of element Californium 98 Cf [251] Dysprosium 66 Dy 162.5 Mercury 80 Hg 200.6 Cadmium 48 Cd 112.4 Zinc 30 Zn 65.41 PERIODIC TABLE OF THE ELEMENTS Einsteinium 99 Es [252] Holmium 67 Ho 164.9 Thallium 81 Tl 204.4 Indium 49 In 114.8 Gallium 31 Ga 69.72 Aluminium 13 Al 26.98 Boron 5 B 10.81 Fermium 100 Fm [257] Erbium 68 Er 167.3 Lead 82 Pb 207.2 Tin 50 Sn 118.7 Germanium 32 Ge 72.64 Silicon 14 Si 28.09 Carbon 6 C 12.01 Mendelevium 101 Md [258] Thulium 69 Tm 168.9 Bismuth 83 Bi 209.0 Antimony 51 Sb 121.8 Arsenic 33 As 74.92 Phosphorus 15 P 30.97 Nitrogen 7 N 14.01 Nobelium 102 No [259] Ytterbium 70 Yb 173.0 Polonium 84 Po [209.0] Tellurium 52 Te 127.6 Selenium 34 Se 78.96 Sulfur 16 S 32.07 Oxygen 8 O 16.00 Argon Chlorine Lawrencium 103 Lr [262] Lutetium 71 Lu 175.0 Astatine 85 At [210.0] Iodine 53 I 126.9 Bromine Radon 86 Rn [222.0] Xenon 54 Xe 131.3 Krypton 36 Kr 83.80 18 Ar 39.95 17 Cl 35.45 35 Br 79.90 Neon 10 Ne 20.18 Helium 2 He 4.003 Fluorine 9 F 19.00 For elements that have no stable or long-lived nuclides, the mass number of the nuclide with the longest confirmed half-life is listed between square brackets. The International Union of Pure and Applied Chemistry Periodic Table of the Elements (October 2005 version) is the principal source of data. Some data may have been modified. Cerium Lanthanum Lanthanoids 57 58 La Ce 138.9 140.1 Actinoids 89 103 Lanthanoids 57 71 Yttrium Strontium Rubidium 40 Zr 91.22 39 Y 88.91 Potassium 38 Sr 87.62 20 Ca 40.08 19 K 39.10 37 Rb 85.47 Magnesium Sodium Scandium 12 Mg 24.31 11 Na 22.99 Calcium Beryllium Lithium Titanium 21 Sc 44.96 4 Be 9.012 3 Li 6.941 Hydrogen 1 H 1.008

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Additional Info : New South Wales Higher School Certificate Chemistry 2009
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