Trending ▼   ResFinder  

NSW HSC 2001 : CHEMISTRY

34 pages, 82 questions, 0 questions with responses, 0 total responses,    0    0
nsw_hsc
   		+Fave Message
ProfileTimelineUploadsQ & A
 Home > nsw_hsc >

Instantly get Model Answers to questions on this ResPaper. Try now!
NEW ResPaper Exclusive!

Formatting page ...

2001 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 24 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 31 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 Ethene may be converted into poly(ethene). What type of reaction is this? (A) Condensation (B) Hydrolysis (C) Oxidation/reduction (D) Polymerisation 2 Which of the following is a major component of biomass? (A) Cellulose (B) Ethanol (C) Natural gas (D) Oil 3 Which equation best represents catalytic cracking of a petroleum fraction? Al O 23 (A) C16H34(l) C16H34(g) (B) ( )n nC2H4(g) CH2 CH2 (s) (C) 23 C16H34(l) C7H16(l) + 3C2H4(g) + C3H6(g) Al O Al O 23 (D) C7H16(l) + 3C2H4(g) + C3H6(g) C16H34(l) 3 4 Cellulose is a linear polymer which is a basic structural component of plant cell walls. Which is the correct representation of part of a cellulose polymer? O O CH2OH O O CH2OH O O CH2OH O O O O CH2OH O CH2OH (A) CH2OH O CH2OH O O O (B) O O O CH2OH CH2OH CH2OH O O O O (C) O O O O O O O CH2OH CH2OH O O O (D) O O O CH2OH 5 O CH2OH CH2OH CH2OH The pH of unpolluted rainwater is about 6.0. Which substance contributes most to this? (A) CO2 (B) N2 (C) NO2 (D) O3 4 6 The graph shows the colour ranges of the acid base indicators methyl orange, bromothymol blue and phenolphthalein. red Methyl orange yellow yellow Bromothymol blue blue colourless Phenolphthalein 1 2 3 4 5 magenta 6 7 pH 8 9 10 11 12 13 A solution is yellow in methyl orange, blue in bromothymol blue and colourless in phenolphthalein. What is the pH range of the solution? (A) 4.5 to 6.0 (B) 6.0 to 7.5 (C) 7.5 to 8.5 (D) 8.5 to 10.0 7 A group of students produced a red solution by boiling red cabbage leaves in water. When dilute sodium hydroxide was added to the solution, it turned purple. When dilute hydrochloric acid was added to the red solution, no colour change occurred. Which of these substances, when added, is most likely to cause the red solution to change colour? (A) Cleaning solution containing ammonia (B) Concentrated hydrochloric acid (C) Orange juice (D) Vinegar 5 8 The burning of sulfur can be described by the following equation: S(s) + O2(g) SO2(g) What volume of sulfur dioxide gas will be released at 25 C and 101.3 kPa when 8.00 g of sulfur is burnt? (A) 3.06 L (B) 6.12 L (C) 12.24 L (D) 24.47 L 9 An understanding of Le Chatelier s principle is important in the chemical industry. Which prediction can be made using this principle? (A) The identity of products of a chemical reaction (B) The effect of changes in temperature on the rates of reactions (C) The effect of catalysts on the position of equilibrium reactions (D) The effect of changes in the concentration of chemical substances in equilibrium 10 The following equations describe some reactions in the formation of acid rain: SO2(g) + H2O(l) H+(aq) + HSO3 (aq) 2H+(aq) + 2HSO3 (aq) + O2(g) 4H+(aq) + 2SO42 (aq) What would occur if some solid sodium sulfate (Na2SO4) were added to a sample of acid rain? (A) The amount of SO2(g) would increase and the acidity of the solution would decrease. (B) The amount of SO2(g) would increase and the acidity of the solution would increase. (C) The amount of SO2(g) would be unchanged and the acidity of the solution would be unchanged. (D) The amount of SO2(g) would be unchanged and the acidity of the solution would decrease. 6 11 Why is chlorine used to treat local water supplies? (A) To make water suitable for swimming (B) To kill micro-organisms living in the water (C) To promote sedimentation of finely suspended solids (D) To precipitate heavy metal ions such as lead and mercury 12 The atomic absorption spectrophotometer was developed by Sir Alan Walsh and his team at CSIRO in the 1950s. Its development was one of the most significant in Australian chemical technology. What did it provide? (A) A rapid method to monitor chemical pollutants in water supplies (B) The first method for determining the concentrations of metal ions in water supplies (C) A method for determining the concentrations of hydrocarbons at very low concentrations (D) A method for determining the concentrations of metal ions at very low concentrations 13 Four students analysed a sample of fertiliser to determine its percentage of sulfate. Each student: weighed an amount of fertiliser; dissolved this amount in 100 mL of water; added aqueous barium nitrate; filtered, dried and weighed the barium sulfate precipitate. Their results and calculations are shown in the table. Student Mass of fertiliser used (g) Mass of BaSO4 weighed (g) Percentage of sulfate in fertiliser (%) A 11.6 19.5 69.2 B 10.4 16.9 66.9 C 10.268 22.612 90.6 D 11.1 18.2 67.5 The percentage of sulfate calculated by Student C was significantly higher than that of the other students. Which is the most likely reason for this? (A) Student C did not dry the sample for long enough. (B) Student C added more Ba(NO3)2 solution than the other students. (C) Student C used a balance capable of measuring weight to more decimal places. (D) Student C waited longer than the other students for the Ba(NO3)2 to react completely with the sulfate. 7 14 Which diagram represents the most effective design for a microscopic membrane filter to purify contaminated water? (A) (B) KEY Clean water Contaminated water (C) Microscopic membrane (D) Movement of water Trapped contamination 15 Four students were asked to test a solution for the presence of a cation by using various anions. The students obtained these results: Student Chloride Sulfate Carbonate A no precipitate no precipitate precipitate B precipitate precipitate no precipitate C precipitate precipitate precipitate D no precipitate precipitate no precipitate Each student concluded that Pb2+ was present. Which student had results consistent with this conclusion? (A) A (B) B (C) C (D) D 8 Board of Studies NSW 2001 200 1 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 (3 marks) Radioisotopes are used in industry, medicine and chemical analysis. For ONE of these fields, relate the use of a named radioisotope to its properties. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 116 9 3 Marks Question 17 (6 marks) Students were asked to perform a first-hand investigation to determine the molar heat of combustion of ethanol. The following extract is from the practical report of one student. Apparatus used: Thermometer 500 mL Beaker Wire gauze Tripod Spirit burner containing ethanol Lab data: Mass of water Initial mass of burner Final mass of burner Initial temperature of water Final temperature of water (a) = = = = = 250.0 g 221.4 g 219.1 g 19.0 C 59.0 C After completing the calculations correctly, the student found that the answer did not agree with the value found in data books. Suggest ONE reason for this. 1 ............................................................................................................................... ............................................................................................................................... (b) Propose TWO adjustments that could be made to the apparatus or experimental method to improve the accuracy of the results. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... Question 17 continues on page 11 10 2 Marks Question 17 (continued) (c) Calculate the molar heat of combustion of ethanol, using the student s data. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 17 Please turn over 11 3 Marks Question 18 (6 marks) A galvanic cell was made by connecting two half-cells. One half-cell was made by putting a copper electrode in a copper (II) nitrate solution. The other half-cell was made by putting a silver electrode in a silver nitrate solution. The electrodes were connected to a voltmeter as shown in the diagram. V Copper electrode Silver electrode Copper (II) nitrate solution (1 mol L 1) Silver nitrate solution (1 mol L 1) (a) Complete the above diagram by drawing a salt bridge. 1 (b) Using the standard potentials table in the data sheet, calculate the theoretical voltage of this galvanic cell. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) A student removes the voltmeter from the circuit and replaces it with an electrical generator. The generator causes the copper electrode to increase in mass. Explain, using an equation, why the copper electrode will increase in mass. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 12 Board of Studies NSW 2001 3 200 1 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 19 (7 marks) Name ONE type of cell, other than the dry cell or lead acid cell, you have studied. Evaluate it in comparison with either the dry cell or lead acid cell, in terms of chemistry and the impact on society. Include relevant chemical equations in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 117 13 7 Marks Question 20 (4 marks) A 0.1 mol L 1 solution of hydrochloric acid has a pH of 1.0, whereas a 0.1 mol L 1 solution of citric acid has a pH of 1.6. (a) State ONE way in which pH can be measured. 1 ............................................................................................................................... (b) Explain why the two solutions have different pH values. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 14 3 Marks Question 21 (4 marks) Barium hydroxide and sulfuric acid react according to the following equation: Ba(OH)2(aq) + H2SO4(aq) BaSO4(s) + 2H2O(l) (a) 1 Name this type of chemical reaction. ............................................................................................................................... A 20 mL sample of barium hydroxide was titrated with 0.12 mol L 1 sulfuric acid. The conductivity of the solution was measured throughout the titration and the results graphed, as shown. Conductivity (b) mL of H2SO4 added Explain the changes in conductivity shown by the graph. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 15 3 BLANK PAGE 16 Board of Studies NSW 2001 200 1 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 22 (6 marks) Justify the procedure you used to prepare an ester in a school laboratory. Include relevant chemical equations in your answer. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 118 17 6 Marks Question 23 (4 marks) A household cleaning agent contains a weak base of general formula NaX. 1.00 g of this compound was dissolved in 100.0 mL of water. A 20.0 mL sample of the solution was titrated with 0.1000 mol L 1 hydrochloric acid and required 24.4 mL of the acid for neutralisation. (a) What is the Br nsted Lowry definition of a base? 1 ............................................................................................................................... ............................................................................................................................... (b) What is the molar mass of this base? 3 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 18 Marks Question 24 (6 marks) In the early twentieth century, Fritz Haber developed a method for producing ammonia, as shown by the equation: N2(g) + 3H2(g) (a) 2NH3(g) Ammonia is used as a cleaning agent. State ONE other use of ammonia. 1 ............................................................................................................................... (b) Explain the effect of liquefying the ammonia on the yield of the reaction. 2 ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... (c) Explain why it is essential to monitor the temperature and pressure inside the reaction vessel. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... 19 3 BLANK PAGE 20 Board of Studies NSW 2001 200 1 HIGHER SCHOOL CERTIFIC ATE EXAMINATION Chemistry Centre Number Section I Part B (continued) Student Number Marks Question 25 (6 marks) Explain the need for monitoring the products of a chemical reaction such as combustion. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 119 21 6 Marks Question 26 (4 marks) A university student decided to measure the concentration of lead (Pb) in the soil around his home. He prepared five standard lead solutions of known concentration. The absorbance of these solutions was measured. These results are shown in the table. Concentration of lead standard (ppm) 0 0.00 1 0.15 2 0.31 3 0.44 4 0.59 5 0.75 1 Draw a line graph of these data. 1.00 0.90 0.80 0.70 Absorbance (a) Absorbance 0.60 0.50 0.40 0.30 0.20 0.10 0 0 1 2 3 Concentration of lead (ppm) 4 Question 26 continues on page 23 22 5 Marks Question 26 (continued) (b) The student prepared solutions from four different soil samples around his home. These solutions were also analysed using the same method. The results are shown in the table. 1 Solutions made from soil samples Area sampled Absorbance Front garden bed 0.19 Back garden bed 0.09 Mail box 0.22 Back fence 0.11 Determine the highest concentration of lead in the soil around the home. ............................................................................................................................... (c) State an hypothesis to account for the variation in lead concentration around the student s home. ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... ............................................................................................................................... End of Question 26 Please turn over 23 2 Marks Question 27 (4 marks) Oxygen exists in the atmosphere as the allotropes oxygen and ozone. The graph shows a typical change in ozone concentration with changing altitude. 60 Mesosphere Upper atmosphere Altitude (km) 50 Stratosphere 40 30 10 0 Lower atmosphere 20 Troposphere 1 2 3 4 5 Ozone concentration (ppm) Compare the environmental effects of the presence of ozone in the upper and lower atmosphere. ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... ......................................................................................................................................... 24 Board of Studies NSW 2001 4 200 1 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 and Salvage ................................................. 27 Question 30 The Biochemistry of Movement .................................... 28 Question 31 The Chemistry of Art ............................................... 29 30 Question 32 120 Industrial Chemistry ....................................................... 26 Forensic Chemistry ........................................................ 31 25 Marks Question 28 Industrial Chemistry (25 marks) Electrolysis is an important industrial process. (b) (i) Define electrolysis. 1 (ii) (a) Compare the reaction products from the electrolysis of molten sodium chloride and concentrated aqueous sodium chloride. 2 Carbonyl chloride, COCl2 , is a colourless, poisonous gas that is also known as phosgene. It is needed for the production of insecticides, polyurethane plastics and polycarbonate. It is produced from the exothermic equilibrium reaction of carbon monoxide gas and chlorine gas. When the reaction vessel is cooled below 8 C the phosgene is a liquid. Carbon monoxide Chlorine Phosgene Tap for removal of phosgene Reaction vessel for the formation of phosgene at 4 C (i) 2 (ii) (c) Write a balanced equation for the formation of phosgene. Explain how industry could maximise the production of phosgene. 2 Explain why sulfuric acid is an important industrial chemical. Include balanced chemical equations in your answer. 5 Name the chemical process used to make soap. 1 Outline the procedure for making soap in the school laboratory. 2 (iii) (e) (i) (ii) (d) Describe a safety risk associated with the procedure outlined in part (ii), and suggest a safe work practice to minimise the risk. 3 Evaluate how environmental issues are addressed in the Solvay process. 26 7 Marks Question 29 Shipwrecks and Salvage (25 marks) (a) (d) 1 Although aluminium is a very reactive metal, with a very low reduction potential, it is used in many structures exposed to oxidising conditions. Explain why aluminium can be used in this way. 2 (i) Give an example of a metal commonly used as a sacrificial anode. 1 (ii) (c) Identify the main metal used to construct ships. (ii) (b) (i) Explain why sacrificial anodes are added to metal-hulled ships. 3 Describe the effect of adding other elements to iron on the properties and uses of steels. 5 Define corrosion. 1 (ii) Outline a procedure that could be used to compare the corrosion rates of different metals or alloys in the school laboratory. 2 (iii) (e) (i) Describe ways in which accuracy and reliability could be improved in the procedure described in part (ii). 3 For ONE specific metal, evaluate the steps that can be used to clean, stabilise and preserve artefacts recovered from shipwrecks. 7 27 Marks Question 30 The Biochemistry of Movement (25 marks) (b) (i) Name the molecule that stores energy for nearly all metabolic processes. 1 (ii) (a) Explain how the biologically important part of the molecule in part (i) provides energy for cellular metabolism. 2 Energy for our bodies to function is provided by the oxidation of fuels. Fats and glucose are used as fuels. A summary of the oxidation of fats and glucose is shown. Fats and oils Polysaccharides Hydrolysis and oxidation Hydrolysis and glycolysis Molecule X Citric acid cycle O2 CO2 Oxidative phosphorylation H2O + energy (i) 2 (ii) (c) Identify molecule X and state its function. Analyse the role of oxidative phosphorylation in energy production. 2 Discuss the use of models in developing an understanding of enzyme function. 5 Define viscosity. 1 Outline a procedure that could be used to compare the viscosity of pure glycerol and a glycerol solution. 2 (iii) (e) (i) (ii) (d) Describe ways in which accuracy and reliability could be improved in the procedure described in part (ii). 3 The energy requirements for different types of skeletal muscle are met by the interaction of separate energy output systems. 7 Analyse the role and interaction of the energy output systems used by skeletal muscle. 28 Marks Question 31 The Chemistry of Art (25 marks) (b) (i) Identify the mineral source of a pigment. 1 (ii) (a) Describe the use of a named separation process to obtain a pigment. 2 A sample of a mineral used as a pigment was subjected to spectroscopic analysis. The spectrum is shown. Ba Sr Cu Cd Cr Li Mineral (nm) 300 400 500 600 (i) Identify the elements in the mineral sample. 2 (ii) Explain how a line spectrum is produced. 2 Question 31 continues on page 30 29 Marks Question 31 (continued) (c) (d) Describe the Bohr model of the atom, and identify ONE merit and ONE limitation of the model. 5 Name a transition element. 1 (ii) Outline a first-hand investigation to demonstrate the colour changes of a named transition element as it changes in oxidation state. 2 (iii) (e) (i) Describe a safety risk associated with the procedure outlined in part (ii), and suggest a safe work practice to minimise the risk. 3 With reference to TWO pigments, explain how the metallic components produce colour. 7 End of Question 31 30 Marks Question 32 Forensic Chemistry (25 marks) (b) (i) Define organic compounds. 1 (ii) (a) For ONE class of organic compound, describe a chemical test that identifies this class. 2 The table shows fatty acid composition of some common oils and fats. Fatty acids present (% by weight) Lauric Palmitic Stearic Oleic Linoleic Butter 2 3 23 26 10 13 30 40 4 5 Lard <1 28 30 12 18 41 48 6 7 Tallow <1 24 32 14 32 35 38 2 4 45 51 4 10 1 5 2 10 0 2 Fat or oil hydrolysed Coconut An oily sample was hydrolysed and the fatty acids analysed. Fatty acids present (% by weight) Lauric Oil sample Palmitic Stearic Oleic Linoleic <1 29 28 36 4 (i) (d) 1 (ii) (c) Which fat or oil has been identified? Explain the solubility in water of fatty acids, in terms of their structure. 3 Assess the usefulness of mass spectrometry in providing forensic evidence. 5 Name ONE technique used by forensic chemists to separate a mixture of organic compounds. 1 (ii) In your study of Forensic Chemistry, you performed a first-hand investigation to separate a mixture of organic materials. Outline the procedure. 2 (iii) (e) (i) Describe ways in which accuracy and reliability could be improved in the procedure described in part (ii). 3 Discuss the uses of DNA analysis in forensic chemistry. End of paper 31 7 BLANK PAGE 32 Board of Studies NSW 2001 200 1 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 H = m C T pH = log10 [H+ ] Some standard potentials + K +e 2+ 2+ Ba Ca K(s) 2.94 V + 2e Ba(s) 2.91 V + 2e Ca(s) 2.87 V Na(s) 2.71 V Mg(s) 2.36 V Al(s) 1.68 V + Na + e Mg 2+ 3+ Al + 2e + 3e Mn2+ + 2e Mn(s) H2O + e 1 H2(g) + OH 2 2+ + 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 I2(aq) + e 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 2+ Fe 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 (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 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

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

Formatting page ...

 

  Print intermediate debugging step

Show debugging info


 

Additional Info : New South Wales Higher School Certificate Chemistry 2001
Tags : new south wales higher school certificate chemistry 2001, nsw hsc online chemistry, nsw hsc chemistry, nsw hsc chemistry syllabus, chemistry model exam papers, chemistry sample papers, chemistry course., australia new south wales, nsw hsc online, nsw hsc past papers, nsw hsc papers, nsw hsc syllabus, nsw board of studies, higher school certificate new south wales, nsw australia, hsc syllabus, nsw hsc exams, nsw hsc question papers, nsw hsc solved question papers, nsw hsc previous exam papers, nsw university.  

© 2010 - 2025 ResPaper. Terms of ServiceContact Us Advertise with us

 

nsw_hsc chat