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NSW HSC 2004 : CHEMISTRY

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2004 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 13, 17, 21 and 25 Section I Pages 2 27 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 27 Allow about 1 hour and 45 minutes for this part Section II Pages 29 38 25 marks Attempt ONE question from Questions 28 32 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. Select the alternative A, B, C or D that best answers the question. Fill in the response oval completely. Sample: 2+4= (A) 2 A (B) 6 (C) 8 B C (D) 9 D If you think you have made a mistake, put a cross through the incorrect answer and fill in the new answer. A B C D If you change your mind and have crossed out what you consider to be the correct answer, then indicate the correct answer by writing the word correct and drawing an arrow as follows. correct A B C 2 D 1 Ethanol can be reacted with ethanoic acid to produce ethyl ethanoate. What type of reaction is this? (A) Esterification (B) Hydration (C) Polymerisation (D) Reduction 2 Why is research into synthetic biopolymers attracting great interest? (A) They decompose more easily than traditional synthetic polymers. (B) They can be produced more cheaply than traditional synthetic polymers. (C) They have superior physical properties compared to traditional synthetic polymers. (D) They have superior chemical properties compared to traditional synthetic polymers. 3 Which of the following cations can be identified using a flame test? (A) Al3+ (B) Cu2+ (C) Mg2+ (D) Zn2+ 4 Which term describes the relationship between the compounds shown below? Br C C H H Br Br H H (A) Allotropes (B) Isomers (C) Isotopes (D) Monomers 3 C C Br H H H H 5 Which statement best represents Davy s definition of an acid? (A) Acids contain oxygen. (B) Acids are proton donors. (C) Acids contain replaceable hydrogen. (D) Acids ionise in solution to form hydrogen ions. 6 Which of the following is the Lewis electron dot formula for ozone? (A) (B) (C) (D) 7 The figure shows the pH values of some substances. Baking Lemon Rain Distilled soda Laundry juice water water solution detergent Stomach acid Wine Milk Seawater Soap Bleach 0 1 2 3 4 5 6 7 8 9 10 11 12 Oven cleaner 13 14 Based on the pH values shown in the figure, which of the following statements about the concentration of hydrogen ions is correct? (A) It is twice as great in milk as that in lemon juice. (B) It is 1 000 000 times greater in soap than in wine. (C) It is three times greater in wine than in bleach solution. (D) It is 1 000 times greater in distilled water than in soap. 4 Which of the following graphs illustrates the layered structure of the atmosphere? (A) Altitude (km) 140 120 Troposphere 100 80 Mesosphere 60 40 Stratosphere 20 200 Thermosphere 100 0 100 Temperature ( C) 200 300 (B) Altitude (km) 140 120 Thermosphere 100 80 Stratosphere 60 40 Mesosphere 20 200 Troposphere 100 0 100 Temperature ( C) 200 300 (C) Altitude (km) 140 120 Troposphere 100 80 Stratosphere 60 40 Mesosphere 20 Thermosphere 200 100 0 100 Temperature ( C) 200 300 140 (D) Altitude (km) 8 120 Thermosphere 100 80 Mesosphere 60 40 Stratosphere 20 Troposphere 200 100 0 100 Temperature ( C) 200 300 Roland Smith, 2000, Conquering Chemistry, 3rd edition (C) McGraw - Hill Australia Pty Ltd. 5 9 Ozone reacts with nitric oxide according to the equation NO(g) + O3(g) NO2(g) + O2(g) 0.66 g NO(g) was mixed with 0.72 g O3(g). What is the maximum volume of NO2(g) produced at 0 C and 100 kPa? (A) 0.34 L (B) 0.37 L (C) 0.45 L (D) 0.50 L 10 Phosgene is prepared from the reaction of carbon monoxide and chlorine in the presence of a catalyst: CO(g) + Cl2(g) COCl2(g) H = 9.93 kJ mol 1 Which of the following sets of conditions would produce the highest yield of phosgene? (A) High temperature, high pressure (B) Low temperature, low pressure (C) Low temperature, high pressure (D) High temperature, low pressure 6 11 In gas chromatography, compounds may be separated based on their molecular weight. The smaller the molecular weight the more quickly the compound is detected. A gas chromatographic analysis was performed on a mixture of 1-hexanol, 1-octanol, 1-heptanol and 1-pentanol. The results are shown in the diagram. Response of detector X Time Which substance does peak X correspond to? (A) 1-hexanol (B) 1-octanol (C) 1-heptanol (D) 1-pentanol 12 Two of the compounds shown below react together to form a new compound with a coordinate covalent bond. H C H H N H H O H H H Which of the following compounds react this way? (A) Methane and ammonia (B) Methane and water (C) Hydrogen fluoride and ammonia (D) Hydrogen fluoride and methane 7 H H F 13 A student used the apparatus below to determine the molar heat of combustion of propanol. Thermometer Can containing 200 g water Burner containing 1-propanol The following results were obtained: Mass of 1-propanol burnt = 0.60 g Mass of water heated = 200 g Initial temperature of water = 21.0 C The molar heat of combustion of 1-propanol is 2021 kJ mol 1. Assuming no heat loss, what would be the final temperature of the water? (A) 24.2 C (B) 29.1 C (C) 45.2 C (D) 48.4 C 8 14 Four metals Pb, x, y and z, were connected in pairs and the voltage was recorded. V Salt bridge Metal electrode Metal electrode The results obtained are set out in the table below. Negative terminal Positive terminal Voltage (V) Pb x 0.35 y Pb 1.10 z Pb 2.60 What is the order of increasing ease of oxidation of the metals? (A) z, y, Pb, x (B) Pb, x, y, z (C) x, y, Pb, z (D) x, Pb, y, z 9 15 Diagram A shows a dry cell. Diagram B shows a lead-acid cell. 3 Lead dioxide on lead plate Carbon 1 2 Lead plate Electrolyte 3 Diagram A Diagram B Roland Smith, 2000, Conquering Chemistry, 3rd edition (C) McGraw - Hill Australia Pty Ltd. Which of the following shows the correctly labelled parts? LABELS 1 2 3 (A) anode cathode negative terminal (B) cathode anode negative terminal (C) anode cathode positive terminal (D) cathode anode positive terminal 10 BLANK PAGE 11 BLANK PAGE 12 Board of Studies NSW 2004 2 004 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Part B 60 marks Attempt Questions 16 27 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. Marks Question 16 (5 marks) (a) Outline the procedure you would use to prepare a standard solution of sodium hydrogen carbonate from solid sodium hydrogen carbonate. 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Calculate the mass of solid sodium hydrogen carbonate required to make 250 mL of 0.12 mol L 1 solution. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 116 13 2 Marks Question 17 (5 marks) The structures of two commercially significant monomers are shown. H2C CH H2C CH Cl (a) Identify the common name of ONE of the monomers. 1 ............................................................................................................................... (b) The uses of polymers are dependent on their properties. 3 Discuss this statement with reference to a polymer made from one of the above monomers. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Draw the structure of a polymer made from one of the above monomers. 14 1 Marks Question 18 (4 marks) Analyse the relationship between the position of elements in the Periodic Table, and the acid base behaviour of their oxides. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... Please turn over 15 4 Marks Question 19 (6 marks) The following experiment was performed to investigate the relative activity of metals. The beaker initially contained 250.0 mL of 0.050 mol L 1 copper sulfate solution. Zinc Copper sulfate solution After several hours the dark blue colour of the solution had become lighter and a red-brown deposit had formed on the piece of zinc metal. (a) Account for the changes observed. Provide a balanced oxidation reduction equation in your answer. 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... The red-brown deposit was removed from the piece of zinc metal and dried. It was found to weigh 0.325 g. (b) Calculate the concentration of copper sulfate solution remaining in the beaker. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 16 Board of Studies NSW 2004 3 2 004 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 20 (6 marks) A schematic figure of an atomic absorption spectrophotometer is shown. Prism (or monochromator) Light source Flame (with sample in it) Lens Detector Roland Smith, 2000, Conquering Chemistry, 3rd edition (C) McGraw - Hill Australia Pty Ltd. (a) What is the purpose of the light source and the flame in the figure? ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 20 continues on page 18 117 17 2 Marks Question 20 (continued) Soil from an industrial site was suspected of being contaminated with mercury. A single sample of the soil was extracted using an approved method. The resulting solution was analysed five times by atomic absorption spectroscopy (AAS). The results are shown in the table. Measurement number Absorbance at 259 nm 1 0.90 2 0.89 3 0.89 4 0.64 5 0.91 The concentration of mercury in the soil sample was calculated using an average absorbance of 0.85. (b) Assess the validity and reliability of the concentration of mercury determined using this procedure. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 20 18 4 Marks Question 21 (7 marks) You have performed first-hand investigations on water samples using qualitative and quantitative analyses. (a) Distinguish between qualitative analysis and quantitative analysis. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Describe TWO factors that affect the concentrations of ions in natural bodies of water. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Complete the following table to show how the anions listed can be identified. Anion Reagent Observations if anion is present Cl PO43 SO42 19 3 Marks Question 22 (3 marks) (a) 1 Define the term amphiprotic. ............................................................................................................................... ............................................................................................................................... (b) Write TWO chemical equations to show that the dihydrogen phosphate ion (H2PO4 ) is amphiprotic. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 20 Board of Studies NSW 2004 2 2 004 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 23 (3 marks) A natural indicator was made by heating yellow flowers with water. The resulting yellow solution was tested with a range of substances. The results are recorded below. Substance Colour 0.1 M hydrochloric acid Red 0.1 M ammonia Yellow Lemon juice Orange Oven cleaner Yellow Pure water Yellow Assess the usefulness of the yellow solution as an acid base indicator. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 118 21 3 Marks Question 24 (5 marks) The diagram shows three reagent bottles containing acids. pH = 3.38 pH = 2.00 0.01 mol L 1 Acetic acid (a) pH = 2.56 0.01 mol L 1 Citric acid 0.01 mol L 1 Hydrochloric acid Calculate the pH after 10.0 mL of 0.01 mol L 1 hydrochloric acid solution is diluted by the addition of 90.0 mL of distilled water. 1 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Explain the use of acetic acid and citric acid as food additives. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 24 continues on page 23 22 2 Marks Question 24 (continued) (c) Explain the difference in pH between the three acids in the diagram. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 24 Please turn over 23 2 Marks Question 25 (5 marks) 5 The table shows properties of some fuels. Fuel Main sources Heat of combustion (kJ g 1) Boiling point ( C) Methane Petrochemical industry 55.6 161.5 Propane Petrochemical industry Natural gas 50.3 42.1 Octane Refined from crude oil 47.9 125.7 Ethanol Hydration of ethene Fermentation 29.7 78.3 Assess the potential of ethanol as an alternative fuel, making use of data from the table. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 24 Board of Studies NSW 2004 2 004 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 26 (4 marks) Discuss the benefits and problems associated with the use of ONE radioactive isotope in industry. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 119 25 4 Marks Question 27 (7 marks) The table shows ozone depletion potential (ODP) for different compounds. Ozone depletion potential CFC 11 CFC 12 CFC 113 CFC 114 1.0 1.0 0.8 1.0 HCFC 22 HCFC 123 HCFC 141b HCFC 142b HFC 32 HFC 125 HFC 134a HFC 143a 0.055 0.02 0.11 0.065 0 0 0 0 http://www.princeton.edu/nchm333/2002/spring/ozone/alternatives_substitutes.htm Discuss the problems associated with the use of CFCs, and assess the suitability of alternative chemicals as replacements, using data in the table. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... Question 27 continues on page 27 26 7 Question 27 (continued) ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... End of Question 27 27 BLANK PAGE 28 Board of Studies NSW 2004 2 004 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Section II 25 marks Attempt ONE question from Questions 28 32 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 28 Question 29 Shipwrecks, Corrosion and Conservation ............................ 32 33 Question 30 The Biochemistry of Movement .......................................... 34 35 Question 31 The Chemistry of Art ................................................................. 36 Question 32 120 Industrial Chemistry ............................................................. 30 31 Forensic Chemistry .............................................................. 37 38 29 Marks Question 28 Industrial Chemistry (25 marks) (b) (i) Identify a safety precaution used when diluting concentrated sulfuric acid. 1 (ii) (a) Many of the steps in the Contact process for the manufacture of sulfuric acid are reversible equilibrium reactions. Identify ONE of these reactions and describe how the product yield can be maximised. 3 The table shows the structures of three different classes of detergents. Type of detergent Structure SO3 Anionic OH Non-ionic Cationic + N Roland Smith, 2000, Conquering Chemistry, 3rd edition (C) McGraw - Hill Australia Pty Ltd. (i) Account for the cleaning action of anionic detergents. 2 (ii) Assess the environmental impacts of the different classes of detergents. 4 Question 28 continues on page 31 30 Marks Question 28 (continued) (c) Chemco Pty Ltd wishes to build two new industrial plants. One will be used for the production of sodium carbonate and the other for production of sodium hydroxide. The map shows three sites, labelled A, B and C, being considered for the location of the industrial plants. 7 Small town Power station River Large city Small town Port Limestone deposits Port Coast KEY Railway line Assess the suitability of the three sites for locating industrial plants to produce each compound. (d) During your practical work you performed a first-hand investigation to gather information and describe the properties of a named emulsion, and you related these properties to its uses. (i) Define the term emulsion. 1 (ii) Outline the procedure used in your investigation, and describe the results obtained. 3 (iii) Explain how the industrial method of producing soap differs from that used in school laboratories. 4 End of Question 28 31 Marks Question 29 Shipwrecks, Corrosion and Conservation (25 marks) (b) (i) Identify ONE origin of minerals in oceans. 1 (ii) (a) Explain the damage that occurs when drying wooden artefacts that have been removed from long-submerged wrecks. 3 The diagram shows an electrolytic cell. Platinum electrode Platinum electrode Solution of KBr (i) 2 (ii) (c) Write half-equations for the main reactions occurring at the cathode and anode. Analyse the impact of the work of Faraday on our understanding of electrolysis. 4 Assess how increasing knowledge of metals and alloys has resulted in materials other than timber being used to construct ships. 7 Question 29 continues on page 33 32 Marks Question 29 (continued) (d) During your practical work you performed a first-hand investigation to compare and describe the rates of corrosion of materials at different oxygen concentrations. (i) Define the term corrosion. 1 (ii) Outline the procedure used in your investigation, and describe the results obtained. 3 (iii) The diagram shows the locations of two identical steel ships that were wrecked at the same time near a tropical island. 4 30 m Explain how differences in oxygen concentration and temperature experienced by the two wrecks have resulted in different levels of corrosion. End of Question 29 33 Marks Question 30 The Biochemistry of Movement (25 marks) (a) (i) 1 Identify the following molecule: H (ii) (b) C C H H OH H O C OH Compare the formation of this molecule by anaerobic respiration with the process of fermentation. 3 The diagram illustrates schematically the current model of muscle contraction. Protein A Protein B Metal ion ATP C ADP + Pi (i) Identify protein A, protein B, and metal ion C. 2 (ii) Explain why different energy sources are used in sprinting and light exercise. 4 Question 30 continues on page 35 34 Marks Question 30 (continued) (c) Assess the importance of oxidative phosphorylation as an energy source, referring to the roles of cytochromes and oxygen. (d) 7 During your practical work you performed a first-hand investigation on the effect of pH on the reaction of an enzyme. (i) Define the term enzyme. 1 (ii) Outline the procedure used in your investigation, and describe the results obtained. 3 (iii) Explain the possible effects of varying pH on the primary, secondary and tertiary structures of enzymes. 4 End of Question 30 35 Marks Question 31 The Chemistry of Art (25 marks) (a) The formulae of three coordination complexes containing chromium(III) are shown below. [Cr(H O) ] [Cr(H O) Cl] [Cr(H O) Cl ] 3+ 2 6 2+ 2 5 + 2 4 2 (i) 1 (ii) (b) What is the electron configuration of chromium metal in the ground state? Draw a Lewis structure of ONE of these coordination complexes, and explain the bonding in this molecule. 3 The diagram shows the emission spectrum of sodium seen through a spectroscope. 700 600 500 400 nm (i) Draw an energy level diagram to represent the origin of these spectral lines. 2 (ii) Explain how the Bohr model of the atom was developed using the emission spectrum of hydrogen, and outline its limitations. 4 (c) Assess the potential health risks associated with chemicals found in cosmetics that were used in an ancient culture. 7 (d) During your practical work you performed a first-hand investigation to observe the colour changes of a named transition element as it changed in oxidation state. (i) Define the term transition element. 1 (ii) Outline the procedure used in your investigation, and describe the results obtained. 3 (iii) Explain why transition elements may have more than one oxidation state. 4 36 Marks Question 32 Forensic Chemistry (25 marks) (a) Identify the technique used to separate amino acids on the basis of differences in their charge. 1 (ii) (b) (i) Explain how a mass spectrometer operates, and identify its usefulness for forensic science. 3 Oxytocin and vasopressin are small proteins consisting of nine amino acids. A forensic scientist decided to determine the amino acid composition of both proteins using paper chromatography. Samples of both proteins were first hydrolysed into their constituent amino acids using a mixture of enzymes. The resulting protein hydrolysates were spotted onto a sheet of filter paper together with eleven reference amino acids. After the filter paper had been placed in a suitable solvent and developed, the chromatogram below was obtained. KEY Solvent front Ty = Tyrosine As = Asparagine Ph = Phenylalanine Va = Valine Gly = Glycine Le = Leucine Glu = Glutamic acid Hi = Histidine Ar = Arginine Il = Isoleucine Pr = Proline S1 = Vasopressin hydrolysate S2 = Oxytocin hydrolysate Solvent flow Start point Ty As Ph Va Gly Le Glu Hi Ar Il Pr S1 S2 (i) Contrast the amino acid composition of both proteins after analysing the chromatogram. 2 (ii) Explain how variations in the composition and structure of proteins affect their biological functions. 4 Question 32 continues on page 38 37 Marks Question 32 (continued) (c) Assess the usefulness of distinguishing tests for carbohydrates and metal ions used in the school laboratory, compared with technology used by forensic chemists in laboratories, for the same purposes. (d) 7 During your practical work you performed a first-hand investigation to identify the range of solvents that may be used for chromatography to separate and identify mixtures. (i) Define the term chromatography. 1 (ii) Outline the procedure used in your investigation, and describe the results obtained. 3 (iii) Describe precautions used to prevent contamination of forensic samples, and explain why they are needed. 4 End of paper 38 BLANK PAGE 39 BLANK PAGE 40 Board of Studies NSW 2004 2004 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 pH = log10 [H+ ] H = m C T 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+ + 2e 2+ 2+ 2+ + 2e 2+ + 2e Zn Fe Ni Sn Pb Zn(s) 0.76 V + 2e Fe(s) 0.44 V + 2e Ni(s) 0.24 V Sn(s) 0.14 V Pb(s) 0.13 V 2 Cu 2+ 1 H2(g) 2 + + 4H + 2e + 2e 1 O2(g) + 2 + H2O + 2e Cu + e +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 1 I2(s) + e 2 1 I (aq) + e 2 2 3+ Fe 0.83 V H+ + e SO4 1.18 V 0.34 V 0.40 V Cu(s) 0.52 V 2OH I 0.54 V I 0.62 V Fe2+ 0.77 V Ag(s) 0.80 V Br 1.08 V Br 1.10 V H2O 1.23 V 1.36 V Cl 7 Cr3 + + H2O 2 Cl Mn F 1.36 V 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. 41 42 Yttrium 57 71 Strontium 56 Ba 137.3 Barium 88 Ra [226.0] Radium Rubidium 55 Cs 132.9 Caesium 87 Fr [223.0] Francium Rutherfordium 104 Rf [261.1] Hafnium 72 Hf 178.5 Zirconium 90 Th 232.0 Thorium Actinides 89 Ac [227.0] Actinium Protactinium 91 Pa 231.0 Praseodymium 59 Pr 140.9 Dubnium 105 Db [262.1] Tantalum 73 Ta 180.9 Niobium 41 Nb 92.91 Vanadium Uranium 92 U 238.0 Neodymium 60 Nd 144.2 Seaborgium 106 Sg [263.1] Tungsten 74 W 183.8 Molybdenum 42 Mo 95.94 Chromium Neptunium 93 Np [237.0] Promethium 61 Pm [146.9] Bohrium 107 Bh [264.1] Rhenium 75 Re 186.2 Technetium 43 Tc [98.91] Manganese Platinum 78 Pt 195.1 Palladium 46 Pd 106.4 Nickel Plutonium 94 Pu [239.1] Samarium Americium 95 Am [241.1] Europium Curium 96 Cm [244.1] Gadolinium 64 Gd 157.3 Meitnerium Hassium 63 Eu 152.0 Ununnilium 109 Mt [268] 108 Hs [265.1] 62 Sm 150.4 110 Uun Iridium 77 Ir 192.2 Rhodium 45 Rh 102.9 Cobalt Osmium 76 Os 190.2 Ruthenium 44 Ru 101.1 Iron 28 Ni 58.69 Berkelium 97 Bk [249.1] Terbium 65 Tb 158.9 Unununium 111 Uuu Gold 79 Au 197.0 Silver 47 Ag 107.9 Copper Californium 98 Cf [252.1] Dysprosium 66 Dy 162.5 Ununbium 112 Uub Mercury 80 Hg 200.6 Cadmium 48 Cd 112.4 Zinc Einsteinium 99 Es [252.1] Holmium 67 Ho 164.9 113 Thallium 81 Tl 204.4 Indium 49 In 114.8 Gallium 31 Ga 69.72 Fermium 100 Fm [257.1] Erbium 68 Er 167.3 Ununquadium 114 Uuq Lead 82 Pb 207.2 Tin 50 Sn 118.7 Germanium 32 Ge 72.61 Silicon 14 Si 28.09 Carbon 6 C 12.01 9 F 19.00 Sulfur Phosphorus Mendelevium 101 Md [258.1] Thulium 69 Tm 168.9 115 Bismuth 83 Bi 209.0 Antimony 51 Sb 121.8 Arsenic Nobelium 102 No [259.1] Ytterbium 70 Yb 173.0 Ununhexium 116 Uuh Polonium 84 Po [210.0] Tellurium 52 Te 127.6 Selenium 34 Se 78.96 16 S 32.07 15 P 30.97 33 As 74.92 Oxygen Nitrogen Lawrencium 103 Lr [262.1] Lutetium 71 Lu 175.0 117 Astatine 85 At [210.0] Iodine 53 I 126.9 Bromine 35 Br 79.90 Chlorine 17 Cl 35.45 Fluorine 8 O 16.00 7 N 14.01 Where the atomic weight is not known, the relative atomic mass of the most common radioactive isotope is shown in brackets. The atomic weights of Np and Tc are given for the isotopes 237Np and 99Tc. Cerium Lanthanum Lanthanides 57 58 La Ce 138.9 140.1 Actinides 89 103 Lanthanides 39 Y 88.91 38 Sr 87.62 40 Zr 91.22 Titanium Scandium Calcium 27 Co 58.93 30 Zn 65.39 37 Rb 85.47 26 Fe 55.85 29 Cu 63.55 Potassium 25 Mn 54.94 Aluminium 24 Cr 52.00 20 Ca 40.08 19 K 39.10 23 V 50.94 Magnesium Sodium 22 Ti 47.87 13 Al 26.98 Boron 12 Mg 24.31 Name of element 11 Na 22.99 Atomic Weight Gold Beryllium Symbol of element Lithium 21 Sc 44.96 5 B 10.81 79 Au 197.0 3 Li 6.941 Atomic Number KEY 4 Be 9.012 PERIODIC TABLE OF THE ELEMENTS Hydrogen 1 H 1.008 Ununoctium 118 Uuo Radon 86 Rn [222.0] Xenon 54 Xe 131.3 Krypton 36 Kr 83.80 Argon 18 Ar 39.95 Neon 10 Ne 20.18 Helium 2 He 4.003

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Additional Info : New South Wales Higher School Certificate Chemistry 2004
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