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NSW HSC 2002 : CHEMISTRY

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2002 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, 13, 17 and 21 Section 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 27 Allow about 1 hour and 45 minutes for this part Section II Pages 25 30 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 Which conditions would be best for the fermentation of sugars by yeast? (A) Low oxygen concentration and a temperature between 25 C and 35 C (B) High oxygen concentration and a temperature between 25 C and 35 C (C) Low oxygen concentration and a temperature between 45 C and 60 C (D) High oxygen concentration and a temperature between 45 C and 60 C 2 What is the catalyst for the conversion of ethanol to ethene? (A) NaOH (B) H2SO4 (C) HNO3 (D) Pt 3 Which explanation best describes why an understanding of electrolysis has made a significant impact on the production of materials? (A) Electrolysis reactions do not require an energy source. (B) Electrolysis can be used to split water into hydrogen and oxygen. (C) Electrolysis provides a way to make non-spontaneous reactions occur. (D) Electrolysis can be used to produce aluminium. 4 Which statement concerning galvanic cells is correct? (A) Oxidation occurs at the anode. (B) They are also known as electrolytic cells. (C) The cathode is assigned a negative charge. (D) An external power source must be present. 5 What arrangement of an electrolytic cell would electroplate a silver coin with copper? Cathode Anode Electrolyte (A) copper silver coin copper sulfate (B) silver coin copper silver nitrate (C) copper silver coin silver nitrate (D) silver coin copper copper sulfate 3 6 Which is amphiprotic? (A) H2SO4 (B) NH4+ (C) HCO3 (D) SO42 7 What did the Br nsted Lowry definition of acids identify that made it a significant improvement over earlier definitions? (A) Acids contain hydrogen. (B) Acids are proton donors. (C) Acids contain oxygen. (D) Acids are electron-pair acceptors. 8 In a titration, an acid of known concentration is placed in a burette and reacted with a base that has been pipetted into a conical flask. Burette (acid) Pipette (transfers base to conical flask) Conical flask (base) What should each piece of glassware be rinsed with immediately before the titration? Burette Pipette Conical flask (A) acid base water (B) water water water (C) acid base base (D) water water base 4 9 The following list of steps refers to an experimental plan for making an ester in a flask. Some of the steps in the list may NOT be required for this experiment. The steps are NOT in the correct sequence. 1. 2. 3. 4. 5. 6. 7. Heat the mixture under reflux. Add three drops of concentrated sulfuric acid. Add 1 mL of ethanol. Add 1 mL of ethene. Add 1 mL of ethanoic acid. Distil the mixture. Add three drops of phenolphthalein indicator. Which alternative is the best sequence for making an ester? (A) 3, 5, 7, 1 (B) 4, 3, 7, 6 (C) 5, 4, 2, 6 (D) 5, 3, 2, 1 10 Which equation represents esterification? O (A) O CH3 O C CH3 + H2O H+ O (B) O CH3 O C H + NaOH O (C) CH3 OH + CH3 C OH O (D) CH3 OH + CH3 C OH CH3 OH + CH3 C OH H C ONa + CH3 OH H+ H+ 5 O CH3 CH2 O C H + H2O O CH3 O C CH3 + H2O 11 A car engine burns fuel with insufficient air. Which substance would be emitted in the exhaust in higher levels than from an engine with a correct fuel to air ratio? (A) Carbon dioxide (B) Carbon monoxide (C) Oxygen (D) Water 12 Oxides of nitrogen are produced by the combustion of coal. The percentage of these compounds remaining in emissions can be reduced using the methods named in the graph. 100 90 80 70 Oxides of 60 nitrogen remaining 50 in emissions 40 (%) 30 20 10 0 Low nitrogen oxide burners Reburning technologies Ammoniainjecting scrubbers Selective catalytic scrubbers Which of the following is the most effective method for removing oxides of nitrogen produced by the combustion of coal? (A) Low nitrogen oxide burners (B) Reburning technologies (C) Ammonia-injecting scrubbers (D) Selective catalytic scrubbers 6 13 The Haber Process for producing ammonia was developed early in the twentieth century. What was the major advantage of its development? (A) A government sold the process to other governments. (B) The inventor sold the process for a great deal of money. (C) It provided a source of nitrogen for farming and industry. (D) It provided jobs for many who were unemployed. 14 Ammonia is produced from hydrogen and nitrogen, according to the equation: N2(g) + 3H2(g) 2NH3(g) The graph shows the yield of ammonia produced at 200 C and 100 kPa. 200 C Yield of ammonia Time Which graph shows a correct comparison of the yield of ammonia produced at a temperature of 400 C and 100 kPa with the yield produced at 200 C and 100 kPa? (A) Yield of ammonia (B) 400 C 200 C Yield of ammonia 200 C 400 C Time Time (C) (D) 200 C Yield of ammonia 400 C Time 400 C Yield of ammonia 200 C Time 7 15 The table gives the results of chemical tests for some cations and anions. (ppt = precipitate) Ion Add cold 0.1 M HCl Add 0.1 M KSCN Add 0.1 M Na2CO3 Add 0.1 M AgNO3 Ca2+ no change no change white ppt no change Fe3+ no change red colour brown ppt no change Ba2+ no change no change white ppt no change Pb2+ white ppt no change white ppt no change Cl no change no change no change white ppt When a group of students performed the above tests on an unknown solution they obtained the following results: Add cold 0.1 M HCl Add 0.1 M KSCN Add 0.1 M Na2CO3 Add 0.1 M AgNO3 no change no change white ppt white ppt Which conclusion is consistent with these results? (A) The sample contained both CaCl2 and BaCl2. (B) The sample contained both CaCl2 and PbCl2. (C) The sample contained both FeCl3 and PbCl2. (D) The sample contained both FeCl3 and BaCl2. 8 Board of Studies NSW 2002 2002 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 (6 marks) You have carried out a first-hand investigation to compare the reactivity of an alkene with its corresponding alkane. (a) 1 State the name of the alkene. ............................................................................................................................... (b) Outline a procedure to compare the reactivity of this alkene with its corresponding alkane. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Describe the results obtained from this first-hand investigation and include relevant chemical equations. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 116 9 3 Marks Question 17 (3 marks) Explain why alkanes and their corresponding alkenes have similar physical properties, but very different chemical properties. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 10 3 Marks Question 18 (6 marks) (a) 1 Name the type of polymerisation shown in the following reaction: O n HO C O C OH + n HO CH2 CH2 OH O OC O C O CH2 CH2 O + H2O n ............................................................................................................................... (b) Assess current developments in the use of biopolymers. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 11 5 BLANK PAGE 12 Board of Studies NSW 2002 2002 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 19 (5 marks) (a) Describe the conditions under which a nucleus is unstable. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 19 continues on page 14 117 13 2 Marks Question 19 (continued) The following is a flow diagram showing the sequence of products released during the decay of uranium. U 238 Pa Th 230 Mass number (b) U Th Ra 222 214 Rn Pb Pb 206 Bi Po Po Bi Po Pb 82 84 86 88 Atomic number 90 92 Use examples from the flow diagram to describe processes by which an unstable isotope undergoes radioactive decay. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 19 14 3 Marks Question 20 (4 marks) (a) 1 Identify ONE common household base. ............................................................................................................................... (b) A student used indicators to determine whether three colourless solutions were acidic or basic. The indicators used are shown in the table. Indicator Colour change pH range Methyl orange red to yellow 3.2 4.4 Methyl red red to yellow 4.8 6.0 Thymol blue yellow to blue 8.0 9.6 Alizarin red to purple 11.0 12.4 Samples of each solution were tested with the indicators. The colours of the resulting solutions are shown in the table. Indicator added Colour of solution A Colour of solution B Colour of solution C Methyl orange yellow yellow yellow Methyl red yellow yellow yellow blue blue yellow purple red red Thymol blue Alizarin The student concluded that each of the three solutions tested was basic. Assess the validity of this conclusion. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 15 3 Marks Question 21 (7 marks) Evaluate the impact of industrial sources of sulfur dioxide and nitrogen oxides on the environment, making use of appropriate chemical equations. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 16 Board of Studies NSW 2002 7 2002 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 22 (5 marks) Solutions of hydrochloric acid, acetic acid and sulfuric acid were prepared. Each of the solutions had the same concentration (0.01 mol L 1). The pH of the acetic acid solution was 3.4. 0.01 mol L 1 hydrochloric acid (a) 0.01 mol L 1 acetic acid 0.01 mol L 1 sulfuric acid pH = 3.4 Calculate the pH of the hydrochloric acid solution. 1 ............................................................................................................................... (b) Compare the pH of the sulfuric acid solution to the pH of the hydrochloric acid solution. Justify your answer. (No calculations are necessary.) 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Explain why the acetic acid solution has a higher pH than the hydrochloric acid solution. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 118 17 2 Marks Question 23 (4 marks) A bottle of soft drink was placed on an electronic balance and weighed. The cap was removed and placed next to the bottle on the balance. The mass of the cap, bottle and its contents was monitored. The results are shown in the graph. The experiment was conducted at 25 C and 101.3 kPa. Assume that no evaporation has occurred. 630 Mass of cap, bottle and contents (g) 625 620 615 (a) Time 1 Identify the gas released. ............................................................................................................................... (b) Calculate the volume of the gas released. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 18 3 Marks Question 24 (4 marks) Assess the impact of atomic absorption spectroscopy (AAS) on the scientific understanding of the effects of trace elements. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 19 4 BLANK PAGE 20 Board of Studies NSW 2002 2002 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 25 (6 marks) (a) What is the systematic name of the CFC in the diagram? 1 Cl Cl F C C F F F ............................................................................................................................... (b) Identify the bonding within ozone, using a Lewis electron-dot diagram. 2 (c) Discuss how CFCs damage the ozone layer, using relevant equations. 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 119 21 Marks Question 26 (5 marks) Water can be described as either hard or soft . (a) Describe a test you have used to determine whether a given sample of water is hard or soft . 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (b) A sample of hard water contains 6 10 4 mol L 1 of magnesium carbonate. Calculate the mass, in mg, of magnesium carbonate in 150 mL of this sample. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 22 3 Marks Question 27 (5 marks) Describe the physical and chemical processes needed to purify and sanitise a town water supply. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 23 5 BLANK PAGE 24 Board of Studies NSW 2002 2002 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. Page Question 28 Question 29 Shipwrecks and Salvage ............................................................ 27 Question 30 The Biochemistry of Movement ................................................ 28 Question 31 The Chemistry of Art ................................................................. 29 Question 32 120 Industrial Chemistry ................................................................... 26 Forensic Chemistry .................................................................... 30 25 Marks Question 28 Industrial Chemistry (25 marks) (b) (i) Define saponification. 1 (ii) (a) Account for the cleaning action of soap. 3 One of the reactions used to form sulfuric acid is the reaction of oxygen with sulfur dioxide under equilibrium conditions to form sulfur trioxide. 4 Before the reaction, the concentration of sulfur dioxide was 0.06 mol L 1 and the concentration of oxygen was 0.05 mol L 1. After equilibrium was reached, the concentration of sulfur trioxide was 0.04 mol L 1. Calculate the equilibrium constant, K, for the reaction. Show relevant working. (c) Use a chemical equation to describe what happens when sulfuric acid is added to water in a laboratory. 2 (ii) (d) (i) Describe the use of sulfuric acid as an oxidising agent, as a dehydrating agent and as a means of precipitating sulfates. Use chemical equations to illustrate your answer. 3 During your practical work, you performed a first-hand investigation involving an equilibrium reaction. (i) 2 (ii) (e) Outline the procedure you used. Explain how you analysed the equilibrium reaction qualitatively. 4 Evaluate changes in industrial production methods for sodium hydroxide. 26 6 Marks Question 29 Shipwrecks and Salvage (25 marks) (i) Name the type of electrochemical cell that produces a spontaneous reaction. 1 (ii) (a) Calculate the voltage required to operate the cell shown in the diagram as an electrolytic cell, showing relevant half-equations in your working. 3 V Salt bridge Iron Copper Fe2+ (1 mol L 1) (b) Cu2+ (1 mol L 1) Describe how the work of early scientists increased our understanding of electron transfer reactions. 4 (d) (i) Name ONE method for removing salt from an artefact recovered from a wreck. 1 (ii) (c) Explain, using an example, chemical procedures used to clean and preserve artefacts from wrecks. 4 During your practical work you performed a first-hand investigation to compare and describe the rate of corrosion of materials in different acidic and neutral solutions. (i) Outline the procedure used. 2 (ii) It is hypothesised that acidic environments accelerate the corrosion of shipwrecks. 4 Explain how data obtained from the procedure in part (d) (i) does or does not support this hypothesis. (e) Analyse the effect of ocean depth on corrosion of metallic objects. 27 6 Marks Question 30 The Biochemistry of Movement (25 marks) (a) (i) To what class of compounds do these molecules belong? H CH3 O H H N C C O H HO H N C C O H H H Using the two compounds in part (a) (i), describe the formation of a peptide bond, illustrating your answer with a chemical equation. Clearly indicate the peptide bond. 3 Explain why triacylglycerols (TAGs) are an important energy store for humans. 4 (ii) (b) 1 (d) (i) Name the acid that builds up in muscles in anaerobic respiration. 1 (ii) (c) Discuss the characteristics of muscle cells used for light exercise and those of muscle cells used for heavy exercise. 4 During your practical work you performed a first-hand investigation to demonstrate the effect of various factors on the reaction of a named enzyme. (i) 2 (ii) (e) Name the enzyme and outline the procedure used to demonstrate the effect of ONE of these factors on the reaction. Explain how the results obtained from the experiment in part (d) (i) can be used to indicate changes in the structure of the enzyme investigated. 4 Discuss the oxidation of fatty acids as an inhibitor of the conversion of pyruvate to acetyl CoA, with reference to the dietary needs of sprinting athletes. 6 28 Marks Question 31 The Chemistry of Art (25 marks) (b) (i) Identify the metal ion that will produce a yellow colour in a flame test. 1 (ii) (a) Explain how some metal ions produce a characteristic colour in a flame. 3 Using an example from medicine or biological research, describe the bonding in a coordination complex. 4 (d) (i) Explain what is meant by a reflectance spectrum. 2 (ii) (c) Outline how infrared light and ultraviolet light are used to determine the chemical composition of pigments. 3 During your practical work you performed a first-hand investigation to determine the oxidising strength of potassium permanganate. (i) 1 (ii) Outline the procedure used to determine the oxidising strength of potassium permanganate. 2 (iii) (e) State the electronic configuration of manganese in terms of subshells. Using your results from the procedure in part (d) (ii), justify a conclusion about the oxidising strength of potassium permanganate. Use half-equations in your answer. 3 Analyse trends in the physical properties of the first transition series. 29 6 Marks Question 32 Forensic Chemistry (25 marks) (b) (i) Identify the functional group in glycerol. 1 (ii) (a) Compare the reactions of both glycerol and 1-propanol when they react with cold dilute KMnO4. 3 Discuss the value of electron spectroscopy and scanning tunnelling microscopy in the analysis of small samples in forensic chemistry. 4 (d) (i) What class of compounds is used to break proteins into fragments of different lengths? 1 (ii) (c) Describe the processes of electrophoresis and chromatography in separating organic compounds. 4 During your practical work you performed a first-hand investigation to describe the emission spectrum of sodium. (i) 1 (ii) Outline the procedure that you used in this investigation. 2 (iii) (e) Name the piece of equipment you used to analyse the emission spectrum of sodium in the laboratory. Explain how the emission spectrum was produced. 3 Discuss the uses of DNA analysis in forensic chemistry. End of paper 30 6 BLANK PAGE 31 BLANK PAGE 32 Board of Studies NSW 2002 2002 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry DATA SHEET Avogadro s constant, NA ............................................................... 6.022 1023 mol 1 Volume of 1 mole ideal gas: at 101.3 kPa (1.00 atm) and at 273 K (0 C) ........................... 22.41 L at 298 K (25 C) ......................... 24.47 L Ionisation constant for water at 298 K (25 C), 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 2+ + 2e Mg 3+ Al + 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 2+ Cu 1 H2(g) 2 + + 2e H2O + 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) + 2 + 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 2+ Fe 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 Br Cl 1.40 V 2+ Mn F + 4H2O 1.51 V 2.89 V Aylward and Findlay, SI Chemical Data (4th Edition) is the principal source of data for this examination paper. Some data may have been modified for examination purposes. 33 34 Yttrium 57 71 Calcium 38 Sr 87.62 Strontium 56 Ba 137.3 Barium 88 Ra [226.0] Radium Potassium 37 Rb 85.47 Rubidium 55 Cs 132.9 Caesium 87 Fr [223.0] Francium 22 Ti 47.87 Rutherfordium 104 Rf [261.1] Hafnium 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 23 V 50.94 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 24 Cr 52.00 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 25 Mn 54.94 Plutonium 94 Pu [239.1] Samarium Americium 95 Am [241.1] Europium 63 Eu 152.0 Curium 96 Cm [244.1] Gadolinium 64 Gd 157.3 Ununnilium Meitnerium Hassium 62 Sm 150.4 110 Uun 109 Mt [268] 108 Hs [265.1] Platinum 78 Pt 195.1 Palladium 46 Pd 106.4 Nickel 28 Ni 58.69 111 Uuu Gold 79 Au 197.0 Silver 47 Ag 107.9 Copper 29 Cu 63.55 Berkelium 97 Bk [249.1] Terbium 65 Tb 158.9 Unununium Name of element Symbol of element Iridium 77 Ir 192.2 Rhodium 45 Rh 102.9 Cobalt 27 Co 58.93 Gold 79 Au 197.0 KEY Osmium 76 Os 190.2 Ruthenium 44 Ru 101.1 Iron 26 Fe 55.85 Atomic Weight Atomic Number Californium 98 Cf [252.1] Dysprosium 66 Dy 162.5 Ununbium 112 Uub Mercury 80 Hg 200.6 Cadmium 48 Cd 112.4 Zinc 30 Zn 65.39 PERIODIC TABLE OF THE ELEMENTS 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 Aluminium 13 Al 26.98 Boron 5 B 10.81 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 Mendelevium 101 Md [258.1] Thulium 69 Tm 168.9 115 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 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 72 Hf 178.5 Zirconium 40 Zr 91.22 20 Ca 40.08 19 K 39.10 Titanium Magnesium Sodium 39 Y 88.91 12 Mg 24.31 11 Na 22.99 Scandium Beryllium Lithium 21 Sc 44.96 4 Be 9.012 3 Li 6.941 Hydrogen 1 H 1.008 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 Sulfur 16 S 32.07 Oxygen 8 O 16.00 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 9 F 19.00 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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