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NSW HSC 2008 : CHEMISTRY

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2008 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, 15, 17 and 21 S ection I Pages 2 23 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 28 Allow about 1 hour and 45 minutes for this part S ection II Pages 25 35 25 marks Attempt ONE question from Questions 29 33 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 radiations is measured with a Geiger counter? (A) Beta (B) Infrared (C) Microwave (D) Ultraviolet 2 What are the volumes of one mole of argon, Ar, and one mole of fluorine, F2, at 0 C and 100 kPa? Volume (litres) Ar (A) 12.40 24.79 (B) 22.71 22.71 (C) 22.71 45.42 (D) 3 F2 24.79 24.79 Which term describes the relationship between oxygen and ozone? (A) Allotropes (B) Conjugates (C) Isomers (D) Isotopes 2 4 What is the main constituent of the atmosphere at ground level? (A) Water (B) Oxygen (C) Nitrogen (D) Carbon dioxide 5 Why is ethanol used in preference to water as the main ingredient of perfume? (A) Ethanol is cheaper to produce. (B) Ethanol has no detectable odour. (C) Ethanol dissolves esters more readily. (D) Ethanol has a significantly lower density. 6 What is the specific heat of a compound? (A) The quantity of heat required to boil 1 g of the compound (B) The quantity of heat required to melt 1 g of the compound (C) The quantity of heat required to increase the temperature of the compound by 1 C (D) The quantity of heat required to increase the temperature of 1 g of the compound by 1 C 7 Which of the following changes will always shift this equilibrium reaction to the right? 2HI(g) H2(g) + I2(g) H = 52 kJ (A) Adding a catalyst (B) Increasing the pressure (C) Increasing the temperature (D) Adding more of the reactant 8 According to the Arrhenius theory of acids and bases, an acid is a substance that (A) tastes sour. (B) is capable of donating a hydrogen ion. (C) can accept a pair of electrons to form a co-ordinate covalent bond. (D) increases the concentration of hydrogen ions in an aqueous solution. 3 9 Which of the following lower atmosphere pollutant gases is produced directly by the smelting of mineral ores? (A) Carbon monoxide (B) Nitrogen dioxide (C) Ozone (D) Sulfur dioxide 10 The molar heat of combustion of ethanol is 1367 kJ mol 1. What quantity of ethanol must be combusted to raise the temperature of 1.0 kg water from 50 C to boiling point at sea level (assuming no loss of heat to the surroundings)? (A) 6.5 g (B) 7.0 g (C) 209 g (D) 300 g 11 In which of the following alternatives are the three compounds listed in order of increasing boiling point? (A) Pentane, butan-1-ol, propanoic acid (B) Propanoic acid, butan-1-ol, pentane (C) Propanoic acid, pentane, butan-1-ol (D) Butan-1-ol, propanoic acid, pentane 4 12 Samples of water were collected from a river at four different sites: forest, mine, town and estuary. Forest sampling site Forest catchment Copper mine discharge Mine sampling site Town sewage treatment plant discharge Town sampling site Estuary sampling site Ocean The results of various analyses of the water samples are shown. Site 1 Site 2 Site 3 Site 4 6.8 305 32 18 6.8 85 2 2 7.8 7600 2 2 5.9 290 3 2 pH Total Dissolved Solids (mg/L) Biochemical Oxygen Demand (mg/L) E. coli (CFU/100 mL) Using the data from the table above identify each of the sampling sites. Site 1 Site 2 Site 3 Site 4 (A) Town Forest Estuary Mine (B) Estuary Forest Town Mine (C) Mine Town Forest Estuary (D) Town Mine Estuary Forest 5 13 Some reactions of the metals Q, R and S are given below. Metal Reaction in air Reaction with water Q Burns to form metallic oxide Reacts with steam to form hydrogen R Reacts slowly to Does not react form metallic oxide S Reacts to form metallic oxide Reaction with dilute hydrochloric acid Hydrogen is formed Does not react Does not react Hydrogen is formed In a galvanic cell, Q+, R+ and S+ would represent cations of these metals. Which galvanic cell will produce the greatest voltage? (A) (B) Q(s) S(s) V salt bridge Q+(aq) S(s) S+(aq) S+(aq) (C) Q(s) V salt bridge Q+(aq) (D) Q(s) R(s) V salt bridge Q+(aq) S(s) S+(aq) R+(aq) 6 R(s) V salt bridge R+(aq) 14 20 mL of 0.08 mol L 1 HCl is mixed with 30 mL of 0.05 mol L 1 NaOH. What is the pH of the resultant solution? (A) 1.1 (B) 2.7 (C) 4.0 (D) 7.0 15 A 2.45 g sample of lawn fertiliser was analysed for its sulfate content. After filtration and drying, 2.18 g of barium sulfate was recovered. What is the % w/w of sulfate in the lawn fertiliser? (A) 16.8 (B) 36.6 (C) 46.2 (D) 89.0 7 BLANK PAGE 8 Board of Studies NSW 2008 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Part B 60 marks Attempt Questions 16 28 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) The process of fractional distillation is used to separate crude oil into different fractions. One of the compounds obtained from fractional distillation is C10H22. This compound undergoes catalytic cracking as follows: C10H22 C8H18 + C2H4 (a) Complete the table below to identify the products and the homologous series to which they belong. C8H18 2 C2H4 Name of compound Name of series (b) Using examples from your first-hand investigation, explain how you distinguished between these two series of compounds. Include a relevant equation in your answer. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 116 9 3 Marks Question 17 (5 marks) Using TWO examples, analyse how the features of catchment areas will determine the water treatment necessary to make the water safe to drink. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 10 Board of Studies NSW 2008 5 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Student Number Marks Question 18 (5 marks) (a) Draw Lewis electron dot structures for oxygen and ozone. (b) Account for the differences in the properties of oxygen and ozone on the basis of their molecular structure and bonding. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 117 11 2 3 Marks Question 19 (5 marks) A laboratory assesses the amount of zinc in dietary supplement tablets. A chemist prepared 4 tablet samples for analysis by dissolving the tablets individually in 10% nitric acid. Each tablet solution was made up to a final volume of 100 mL. Five standard solutions of zinc were also prepared. The absorbances of the standard and sample solutions were determined by atomic absorption spectroscopy at 213.9 nm. The results are presented in the table. Standard zinc solutions (mg L 1) 0.00 0.000 1.00 0.170 2.00 0.330 3.00 0.503 4.00 0.680 Tablet samples: mean absorbance (a) Absorbance 0.280 Plot a calibration curve for the standard zinc solutions on the grid. Question 19 continues on page 13 12 3 Marks Question 19 (continued) (b) Using the mean absorbance of the tablet samples, calculate the mean amount of zinc per tablet in mg. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 19 Question 20 (3 marks) 1.22 g of an unknown gas has a volume of 15.0 L at 100 kPa and 25 C. (a) 2 Calculate the molar mass of the gas. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Identify the gas. 1 ............................................................................................................................... ............................................................................................................................... 13 BLANK PAGE 14 Board of Studies NSW 2008 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Student Number Marks Question 21 (4 marks) The graph shows the concentration of CCl3F known as CFC-11, as measured at the Cape Grim Baseline Air Pollution Station, in north-western Tasmania. Awaiting copyright (a) Explain the changes in concentration of CFC-11 as illustrated by the graph. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) Why is it important to monitor the concentration of CFC-11? ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 118 15 2 Marks Question 22 (5 marks) The following extract was taken from the website of a leading car manufacturer. Awaiting copyright Critically evaluate the extract with reference to ethanol being a carbon-neutral fuel. Support your answer with relevant chemical equations. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 16 Board of Studies NSW 2008 5 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Student Number Marks Question 23 (4 marks) Using Le Chatelier s principle, justify the choice of temperature and pressure conditions used to optimise the yield in the Haber process. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 118a 17 4 Marks Question 24 (5 marks) The table shows four fuels and their various properties. Property Petrol Kerosene Hydrogen Ethanol Heat of combustion (kJ mol 1) 5460 10 000 285 1370 Boiling point ( C) 126 300 253 78 0.69 0.78 n/a 0.78 114 210 2 46 Density (g mL 1) 1 Average molar mass (g mol ) (a) Which fuel provides the greatest amount of energy per gram? 1 ............................................................................................................................... ............................................................................................................................... (b) A car has an 80 L petrol tank. Calculate the energy released by the complete combustion of one full tank of petrol. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) How many litres of hydrogen gas at 25 C and 100 kPa would be needed to supply the same amount of energy as 80 L of petrol? ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 18 2 Marks Question 25 (5 marks) A galvanic cell under standard conditions is represented below. Ni(s) v Pt(s) salt bridge Cl2(g) in KNO3(aq) Ni(NO3)2(aq) (pale green) (a) KCl(aq) (colourless) On the diagram, clearly label the anode, the cathode and the direction of electron flow. (b) Write a balanced net ionic equation for the overall cell reaction. 1 1 ............................................................................................................................... ............................................................................................................................... (c) Calculate the standard cell potential (E ). 1 ............................................................................................................................... ............................................................................................................................... (d) Explain any colour changes observed in this cell as the reaction proceeds. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 19 2 BLANK PAGE 20 Board of Studies NSW 2008 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I (continued) Student Number Marks Question 26 (4 marks) Explain how a buffer works with reference to a specific example in a natural system. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 119 21 4 Marks Question 27 (4 marks) (a) Classify these salts as forming acidic, basic or neutral solutions. Salt 2 Classification of solution Ammonium chloride Sodium ethanoate Sodium chloride Ammonium nitrate (b) From the table, choose a salt that forms an acidic or basic solution, and justify its classification. Include an equation to illustrate your answer. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 22 2 Marks Question 28 (6 marks) A standard solution was prepared by dissolving 1.314 g of sodium carbonate in water. The solution was made up to a final volume of 250.0 mL. (a) Calculate the concentration of the sodium carbonate solution. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... This solution was used to determine the concentration of a solution of hydrochloric acid. Four 25.00 mL samples of the acid were titrated with the sodium carbonate solution. The average titration volume required to reach the end point was 23.45 mL. (b) Write a balanced equation for the titration reaction. 1 ............................................................................................................................... (c) Calculate the concentration of the hydrochloric acid solution. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 23 3 BLANK PAGE 24 Board of Studies NSW 2008 2 008 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Section II 25 marks Attempt ONE question from Questions 29 33 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 29 Question 30 Shipwrecks, Corrosion and Conservation ............................ 28 29 Question 31 The Biochemistry of Movement .......................................... 30 31 Question 32 The Chemistry of Art ........................................................... 32 33 Question 33 120 Industrial Chemistry ............................................................. 26 27 Forensic Chemistry .............................................................. 34 35 25 Marks Question 29 Industrial Chemistry (25 marks) (a) The following diagram illustrates the process used to extract sulfur from underground deposits. Awaiting copyright (i) Copy and complete this table in your writing booklet to identify which fluid is pumped through each pipe. Pipe 2 Fluid Pipe 1 Do NOT write your answers here. Pipe 2 Pipe 3 (ii) Explain why this process can be used to extract sulfur. 2 (iii) What possible environmental issues are associated with this process? 2 Question 29 continues on page 27 26 Marks Question 29 (continued) (b) A first-hand investigation was performed to observe the electrolysis of sodium chloride. (i) 3 (ii) Identify the reactions that occur at the anode and at the cathode and give equations for these reactions. 2 (iii) (c) Describe an appropriate procedure. What condition would need to be changed to produce sodium metal as a product? 1 Consider the following mixture of gases in a closed 5.0 L vessel at 730 C. Gas Quantity (mol) CH4 2.00 H2O 1.25 CO 0.75 H2 0.75 The following reaction occurs: CH4(g) + H2O(g) CO(g) + 3H2(g) H = +206 kJ The equilibrium constant, K, is 0.26 at 730 C. (i) 3 (ii) (d) Determine whether the system is at equilibrium. Explain how conditions in this reaction could be adjusted to increase the quantity of products. 3 Synthetic detergents have been developed over the past 60 years. Compare anionic, cationic and non-ionic synthetic detergents in terms of their use and chemical composition and the impact that these detergents have had on the environment. End of Question 29 27 7 Marks Question 30 Shipwrecks, Corrosion and Conservation (25 marks) (a) Underground gas pipelines are often made of steel. To prevent the pipe from rusting it is connected at regular intervals to metal rods. ground conducting wire steel pipe metal rod moist soil (i) 3 (ii) (b) Identify a suitable metal for the rod and explain how this prevents corrosion of the pipe. Support your answer with relevant chemical equations. Suggest TWO other methods that could be used to protect the pipe from corrosion and explain how each of these methods is effective. 3 A first-hand investigation was performed to compare the rate of corrosion of iron and a named steel. (i) Describe an appropriate procedure. 3 (ii) Explain the results obtained using relevant equations. 2 (iii) How can steel composition be modified to increase corrosion resistance? 1 Question 30 continues on page 29 28 Marks Question 30 (continued) (c) A 1.0 mol L 1 solution of silver nitrate was electrolysed using platinum electrodes. Silver was produced at one electrode and a gas was produced at the other. (i) 2 (ii) Identify the reactions that occur at the anode and the cathode and give equations for these reactions. 2 (iii) (d) Draw a labelled diagram to represent this cell. Identify FOUR factors that affect the rate of deposition of silver. 2 Several maritime archaeological projects exist around Australia. Compare the conservation and restoration techniques used in TWO of these projects with reference to the chemistry applied. 7 End of Question 30 29 Marks Question 31 The Biochemistry of Movement (25 marks) (a) The following flowchart outlines a specific section of an important biochemical process. X Y + P Cytochrome chain enzymes catalyse reaction of NADH + H+ and FADH2 with X to produce Y. Energy released by this reaction converts ADP + P to ATP. ADP ATP (i) 1 (ii) Identify this biochemical process and the specific section outlined by the flowchart. 2 (iii) (b) Identify X and Y in your writing booklet. With reference to X and Y explain the role of the co-factors NADH and FADH2. Include equations in your answer. 3 A first-hand investigation was performed to observe the effects of changes in temperature on the reaction of a named enzyme. (i) Describe an appropriate procedure. 3 (ii) Sketch an appropriate graph to represent the results. 2 (iii) Identify the group of biochemical compounds to which this enzyme belongs. 1 Question 31 continues on page 31 30 Marks Question 31 (continued) (c) The nutrition information below appeared on the packaging of a food item. Awaiting copyright (i) Identify THREE major nutrient groups listed in the panel that are required for human cellular metabolic processes. 1 (ii) Quantitatively compare the total energy of the contents of this package with the suggested average daily adult intake. 2 (iii) Explain how the contents of this package could meet the metabolic requirements of human Type 1 skeletal muscle fibres. 3 (d) With reference to the body s metabolic processes, analyse how modern athletes might modify their diet over time to cope with a change in focus from less strenuous exercise to sprinting. 7 End of Question 31 31 Marks Question 32 The Chemistry of Art (25 marks) The diagram below shows the ground state electron configuration of two complexes of cobalt in aqueous solution. Energy (a) [CoCl4 ]2 [Co(H2O)6 ] 2+ blue solution red solution (i) 2 (ii) Explain the difference in the colour of the two complexes. 3 (iii) (b) Identify the block in the periodic table to which cobalt belongs and write the electron configuration of cobalt metal in its ground state. Why are solutions of zinc complexes colourless? 1 A first-hand investigation was performed to demonstrate the oxidising strength of potassium permanganate. (i) Describe an appropriate procedure. 3 (ii) Explain the results obtained with the use of half equations. 2 (iii) A solution of potassium permanganate was added to solutions of the following three compounds: potassium iodide, potassium bromide and potassium fluoride. 1 Identify which of these solutions would react with the potassium permanganate. Question 32 continues on page 33 32 Marks Question 32 (continued) (c) An acidified solution of VO2+(aq) is poured into a flask containing zinc metal. When the flask is swirled the following sequence of colour changes is observed. yellow green blue violet VO2 +(aq) VO2+(aq) V3+(aq) V2+(aq) (i) Sketch the expected absorption spectrum for the violet V2+(aq) solution and justify the shape of the curve you have drawn. 3 (ii) Use the following unbalanced half equations to give the overall equation for the colour change from yellow to violet. 2 Zn(s) Zn2+(aq) + e VO2+(aq) + H+(aq) + e V2+(aq) + H2O(l) (iii) (d) Identify the class of reaction to which the reactions in part (ii) belong. A painting is discovered in a disused storeroom of a local museum. The style suggests the painting is approximately 500 years old. Describe some methods a chemist would use to identify pigments in the painting and to check the estimated age of the painting. End of Question 32 33 1 7 Marks Question 33 Forensic Chemistry (25 marks) (a) At a crime scene secured by police, it appears a motor vehicle has been driven into a plate glass window. Display cases inside the window are empty and the vehicle is gone. The forensic examiner made the following annotated sketch. TELEVISION ELECTRONICS SHOP 112 Fingerprints on shelves Blood drops on glass Threads of cloth Glass s shards Muddy tyre dy y tracks acks Glass fragm g Glass fragments headlight g headlight glass Oily patch Glass shards from window, paint flakes on glass shards (i) Identify FOUR pieces of evidence that could be collected to help solve the crime. 2 (ii) Identify TWO instrumental techniques and explain how each could be used to analyse the evidence collected from this crime scene. 4 Question 33 continues on page 35 34 Marks Question 33 (continued) (b) A first-hand investigation was performed to identify reducing and non-reducing sugars. (i) 3 (ii) Account for the results obtained in terms of the chemical differences between reducing and non-reducing sugars. 2 (iii) (c) Describe an appropriate procedure. Suggest an instrumental method for identifying different sugars. 1 An athlete provided a urine sample to be tested for steroids. The sample and the steroid standards were treated and then analysed by gas chromatography with mass spectrometric detection. Below are chromatograms of a standard mixture containing four different steroids, and the sample from the athlete. 1 2 3 4567 Time (min) Sample from athlete 8 Intensity 4. Prednisolone 3. Stanozolol 2. Norandrosterone Intensity 1. Nandrolone Standard steroid mixture 9 1 2 3 4567 Time (min) 8 9 (i) 1 (ii) What properties of compounds would lead a forensic chemist to use high pressure liquid chromatography over gas chromatography? 2 (iii) (d) Identify which steroid, if any, the athlete has taken. Describe the principle of operation of the mass spectrometer. Include a diagram in your answer. 3 With reference to a named example, explain the theory behind emission spectra and how such information could be useful in determining the origins of a mixture. 7 End of paper 35 BLANK PAGE 36 Board of Studies NSW 2008 2 008 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 Ba 2+ Ca 2+ K(s) 2.94 V Ba(s) 2.91 V Ca(s) 2.87 V Na(s) 2.71 V Mg(s) 2.36 V Al(s) 1.68 V + 2e + 2e + Na + e Mg 2+ + 2e Al3+ + 3e Mn 2+ + 2e Mn(s) 1 H2(g) 2 H2O + e 2+ 1.18 V + OH 0.83 V Zn(s) 0.76 V Fe(s) 0.44 V Ni(s) 0.24 V Sn(s) 0.14 V Pb2+ + 2e Pb(s) 0.13 V Zn Fe 2+ Ni 2+ Sn 2+ + 2e + 2e + 2e + 2e + 1 H2(g) 2 2 SO4 2+ Cu + + 4H + 2e + 2e 1 O2(g) + H2O 2 + + 2e Cu + e 1 I2(s) + e 2 1 I2(aq) + e 2 3+ Fe +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 H +e 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 1.10 V I Br Br H2O 1.23 V Cl 1.36 V 7 Cr3 + + H2O 2 1.36 V 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 4 Be 9.012 12 Mg 24.31 Magnesium 20 Ca 40.08 Calcium 38 Sr 87.62 Strontium 56 Ba 137.3 Barium 88 Ra [226] Radium Lithium 11 Na 22.99 Sodium 19 K 39.10 Potassium 37 Rb 85.47 Rubidium 55 Cs 132.9 Caesium 87 Fr [223] Francium Rutherfordium 104 Rf [261] Hafnium 72 Hf 178.5 Zirconium 40 Zr 91.22 Titanium 22 Ti 47.87 Cerium 90 Th 232.0 Thorium Lanthanum Actinoids 89 Ac [227] Actinium Lanthanoids 57 58 La Ce 138.9 140.1 Actinoids 89 103 Lanthanoids 57 71 Yttrium 39 Y 88.91 Scandium 21 Sc 44.96 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 Hassium Bohrium Neptunium 93 Np [237] Promethium Plutonium 94 Pu [244] Samarium 62 Sm 150.4 108 Hs [277] 107 Bh [264] 61 Pm [145] Osmium 76 Os 190.2 Ruthenium 44 Ru 101.1 Iron 26 Fe 55.85 Rhenium 75 Re 186.2 Technetium 43 Tc [97.91] Manganese 25 Mn 54.94 Atomic Weight Atomic Number Americium 95 Am [243] Europium 63 Eu 152.0 Meitnerium 109 Mt [268] Iridium 77 Ir 192.2 Rhodium 45 Rh 102.9 Cobalt 27 Co 58.93 Gold 79 Au 197.0 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 6 C 12.01 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 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 Boron 13 Al 26.98 Carbon 5 B 10.81 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 Lawrencium 103 Lr [262] Lutetium 71 Lu 175.0 Astatine 85 At [210.0] Iodine 53 I 126.9 Bromine 35 Br 79.90 Chlorine 17 Cl 35.45 Fluorine 9 F 19.00 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 Radon 86 Rn [222.0] 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. Beryllium 3 Li 6.941 Hydrogen 1 H 1.008

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