*END OF EXAMINATION*. Chemistry 12 JUNE Course Code = CH. Student Instructions

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1 MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 JUNE Ministry of Education Course Code = CH 1. Place the stickers with your Personal Education Number (PEN) in the allotted spaces above. Under no circumstance is your name or identification, other than your Personal Education Number, to appear on this booklet. 2. Ensure that in addition to this examination booklet, you have a Data Booklet and an Examination Response Form. Follow the directions on the front of the Response Form. 3. Disqualification from the examination will result if you bring books, paper, notes or unauthorized electronic devices into the examination room. Student Instructions 4. When instructed to open this booklet, check the numbering of the pages to ensure that they are numbered in sequence from page one to the last page, which is identified by *END OF EXAMINATION*. 5. At the end of the examination, place your Response Form inside the front cover of this booklet and return the booklet and your Response Form to the supervisor.

2 Question (5) NR Question (5) NR Question (5) NR Question (5) NR Question (5) NR Question (5) NR Question (5) NR Question (5) NR

3 Chemistry 12 JUNE 2004 Course Code = CH

4 GENERAL INSTRUCTIONS 1. Aside from an approved calculator, electronic devices, including dictionaries and pagers, are not permitted in the examination room. 2. All multiplechoice answers must be entered on the Response Form using an HB pencil. Multiplechoice answers entered in this examination booklet will not be marked. 3. For each of the writtenresponse questions, write your answer in the space provided in this booklet. 4. Ensure that you use language and content appropriate to the purpose and audience of this examination. Failure to comply may result in your paper being awarded a zero. 5. This examination is designed to be completed in two hours. Students may, however, take up to 30 minutes of additional time to finish.

5 CHEMISTRY 12 PROVINCIAL EXAMINATION 1. This examination consists of two parts: Value Suggested Time PART A: 60 multiplechoice questions PART B: 8 writtenresponse questions Total: 90 marks 120 minutes 2. The following tables can be found in the separate Data Booklet: Periodic Table of the Elements Atomic Masses of the Elements Names, Formulae, and Charges of Some Common Ions Solubility of Common Compounds in Water Solubility Product Constants at 25 C Relative Strengths of BrønstedLowry Acids and Bases AcidBase Indicators Standard Reduction Potentials of Halfcells No other reference materials or tables are allowed. 3. A calculator is essential for the Chemistry 12 Provincial Examination. The calculator must be a handheld device designed primarily for mathematical computations involving logarithmic and trigonometric functions and may be capable of performing graphing functions. Computers, calculators with a QWERTY keyboard or symbolic manipulation abilities, and electronic writing pads will not be allowed. Students must not bring any external devices (peripherals) to support calculators such as manuals, printed or electronic cards, printers, memory expansion chips or cards, CDROMs, libraries or external keyboards. Students may have more than one calculator available during the examination, of which one may be a scientific calculator. Calculators may not be shared and must not have the ability to either transmit or receive electronic signals. In addition to an approved calculator, students will be allowed to use rulers, compasses, and protractors during the examination. Calculators must not have any information programmed into memory that would not be acceptable in paper form. Specifically, calculators must not have any builtin notes, definitions, or libraries. There is no requirement to clear memories at the beginning of the examination but the use of calculators with builtin notes is equivalent to the use of notes in paper form. Any student deemed to have cheated on a provincial examination will receive a 0 on that examination and will be permanently disqualified from the Provincial Examination Scholarship Program.

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7 PART A: MULTIPLE CHOICE Value: 60 marks INSTRUCTIONS: Suggested Time: 80 minutes For each question, select the best answer and record your choice on the Response Form provided. Using an HB pencil, completely fill in the circle that has the letter corresponding to your answer. 1. Which of the following could represent the units for reaction rate? A. gml B. gmin C. gmol D. mol L 2. Consider the following reaction: Zn( s) 2HCl( aq ) Æ ZnCl2( aq ) H2( g) Which of the following would increase the reaction rate? A. an increase in pressure B. an increase in temperature C. an increase in the concentration of H 2 D. an increase in the concentration of ZnCl 2 3. Consider the following reaction: H2( g) I2( g) Æ 2HI( g) Which of the following is true of the activated complex relative to the reactants? KE Stability A. high stable B. low stable C. high unstable D. low unstable 1 OVER

8 4. Consider the following PE diagram: 150 PE (kj) Progress of the reaction Which of the following is true for the forward reaction? DH kj ( ) PE of Activated Complex kj ( ) A B C D Which of the following could describe a catalyst? A. A substance that increases the reaction time. B. A substance that provides an alternate mechanism with a higher activation energy. C. A substance that is formed in one step and used up in a subsequent step in a reaction mechanism. D. A substance that is used up in one step and reformed in a subsequent step in a reaction mechanism. 2

9 6. The following forward reaction has an Ea = 167 kj : 28 kj H2( g) I2( g) Æ 2HI( g) Which of the PE diagrams below represents this reaction? A. B. PE (kj) 139 kj PE (kj) 167 kj Progress of the reaction Progress of the reaction C. D. 28 kj PE (kj) 195 kj PE (kj) Progress of the reaction Progress of the reaction 7. A small amount of HCl is added to the following equilibrium system: 2 2 2CrO4 ( aq ) 2H ( aq ) Æ Cr2O 7 ( aq ) H2O l 2 How do the [ CrO 4 ] and the reverse reaction rate change as equilibrium is reestablished? 2 [ CrO 4 ] Reverse Rate A. increases increases B. increases decreases C. decreases decreases D. decreases increases ( ) 3 OVER

10 Use the following equilibrium to answer questions 8 and 9. NO Æ ( g) 2NO ( g) colourless brown 8. If NO 2 4 is placed in a flask at a constant temperature, which of the following is true as the system approaches equilibrium? A. The colour gets darker as NO 2 B. The colour gets lighter as NO 2 C. The colour gets darker as NO 2 4 D. The colour gets lighter as NO 2 4 [ ] increases. [ ] decreases. [ ] increases. [ ] decreases. 9. The system above reaches equilibrium. Considering enthalpy and entropy factors, which of the following is true with respect to the forward reaction? A. The entropy is increasing and the reaction is exothermic. B. The entropy is decreasing and the reaction is exothermic. C. The entropy is increasing and the reaction is endothermic. D. The entropy is decreasing and the reaction is endothermic. 10. In which of the following reactions do the tendencies for minimum enthalpy and maximum entropy both favour reactants? A.? 3O2( g) Æ 2O3( g) DH = 285 kj B.? N2( g) 3H2( g) Æ 2NH3( g) DH = 92kJ C.? 2BrCl( g) Æ Br2( g) Cl2( g) DH = 29. 3kJ D.? CaCO3( s) Æ CaO( s) CO2( g) DH = 175 kj 4

11 11. Consider the following equilibrium: CaCO3( s) Æ CaO( s) CO2( g) DH = 175 kj Which of the following diagrams best represents the change in the concentration of CO 2 as temperature is decreased at time t 1? A. B. [ CO 2 ] [ CO 2 ] t 1 Time t 1 Time C. D. [ CO 2 ] [ CO 2 ] t 1 Time t 1 Time 12. Consider the following equilibrium: 2CO( g) O2( g) Æ 2CO2( g) If some CO is added, the equilibrium shifts right. How does reaction kinetics explain this shift to the right? A. The reverse rate decreases. B. The forward rate increases. C. The pressure of the system increases. D. The concentration of CO has increased. 5 OVER

12 13. The Haber Process is used to produce ammonia commercially according to the following equilibrium: N2( g) 3H2( g) Æ 2NH3( g) energy Which of the following conditions will produce the highest yield of ammonia? A. increase temperature and increase pressure B. increase temperature and decrease pressure C. decrease temperature and increase pressure D. decrease temperature and decrease pressure 14. Consider the following equilibrium: ( aq ) ( aq ) 4 ( aq ) 2 ( l ) eq. Cr O 2OH Æ 2CrO H O K = 414 The concentration of ions at equilibrium was measured at a specific 2 temperature and found to be [ Cr2O 7 ] = M and [ OH ] = M. 2 What is the equilibrium CrO 4 M A B C D M M M [ ]? 15. In which of the following equilibria does the concentration of reactants equal the concentration of products? A. NO 2 4( g) Æ 2NO2( g) Keq = 071. B. H ( aq ) OH ( aq ) Æ H2O( l ) Keq = C. CO2( g) H2( g) Æ CO( g) H2O( g) Keq = D. SnO2( s) 2H2( g) Æ Sn( s) 2H2O( g) Keq =

13 16. Consider the following equilibrium: C( s) H2O( g) Æ CO( g) H2( g) At equilibrium, mol H 2, mol CO, mol H2O and mol C were present in a 1. 0L container. What is the value of K eq? A B C. 63. D Consider the following equilibrium: ( ) Æ ( ) ( ) 2COF2 g CO2 g CF4 g Initially, 012. M CO 2 and 020. M CF 4 are placed in a container. At equilibrium, it is found that the COF 2. M. What is the value of K eq? A B C. 80. D. 11 [ ] is Which of the solutes below can form an ionic solution with the highest conductivity? A. PbS B. CH3Cl C. NaNO 3 D. CH3COOH 7 OVER

14 19. The following data was collected to determine the solubility of a substance: Mass of solute dissolved 500. g Volume of solvent ml Molar mass of solute g mol Molar mass of solvent g mol Which of the following best describes its solubility? A gml B mol C mol D mol L 20. Which value best represents the total ion concentration when 010. moles of K3PO 4 is present in 05. L of solution? A. 01. M B. 02. M C. 04. M D. 08. M 21. What will happen when equal volumes of 020. M NH4 2S are mixed? A. SrS precipitates. B. NH4 OH precipitates. C. Both NH4 OH and SrS precipitate. D. No precipitate forms. ( ) and 020. M Sr( OH) Which anion would be most effective in removing the cations responsible for hard water? A. S 2 B. Cl C. PO 4 3 D. SO 4 2 8

15 23. Which of the following is the K sp expression for barium phosphate? 2 3 sp = [ ][ 4 ] sp = [ ] [ 4 ] 2 3 sp = [ 3 ][ 2 4 ] sp = [ 3 ] [ 2 4 ] A. K Ba PO B. K Ba PO C. K Ba PO D. K Ba PO The solubility of Mg OH A B C D ( ) 2 is found to be M. What is its K sp? 25. Which of the following is true for the salt SrF 2 at 25 C? A. It has a high solubility. B. It will not dissolve at all. C. Its solubility is M. D. Its solubility is M. 26. Which of the following ions could be used in the lowest concentration to remove Ag ions from a polluted water sample? A. I B. Br C. BrO 3 D. CO OVER

16 27. Which of the following best describes an acidic solution? Litmus Colour Reaction with Zn A. red reaction B. red no reaction C. blue no reaction D. blue reaction 28. Identify the common acid found in the stomach. A. nitric acid B. sulphuric acid C. perchloric acid D. hydrochloric acid 29. Consider the following equilibrium: HCO H PO Æ HPO H CO What are the BrønstedLowry acids in this equilibrium? A. HCO 3 and HCO 2 3 B. HCO 3 and HPO 4 2 C. HPO 2 4 and HCO 2 3 D. HPO and HPO Which of the following solutions would typically show the greatest electrical conductivity? A. 10. M weak acid B. 08. M weak base C. 05. M strong acid D. 01. M strong base 10

17 31. Given a 1. 0M solution of HI, which sequence best describes the equilibrium concentration of the substances in the solution? [ 3 ] > [ ] > [ ] > [ ] A. HO I OH HI [ ] > [ 3 ] > [ ] > [ ] [ ] > [ 3 ] = [ ] > [ ] [ 3 ] > [ ] > [ ] > [ ] B. HI H O I OH C. HI H O I OH D. HO HI I OH 32. Which of the following are amphiprotic in aqueous solutions? I. HBO 3 3 II. HBO 2 3 III. HBO 3 2 IV. BO 3 3 A. I only B. IV only C. I and II only D. II and III only 33. What happens to the ion concentrations in water when a small amount of HCl( aq ) is added? 7 [ 3 ] = [ ] = A. HO OH M [ ] and [ OH ] both increase [ ] increases and [ OH ] decreases [ ] increases and [ OH ] is unchanged B. HO 3 C. HO 3 D. HO 3 11 OVER

18 34. Which of the following is a typical ph value for dishwashing solutions? A. 20. B. 40. C D What is the poh of 005. M Sr( OH) 2? A. 10. B. 13. C D Consider the following equilibrium: aq aq aq CH3NH2( ) H2O( l) Æ CH3NH OH 3 ( ) ( ) Which of the following is true? [ CH NH ][ OH ] A. K eq = 3 3 CH NH H O [ ][ ] [ CH NH ][ OH ] 3 3 B. Ka = CH NH [ ] 3 2 [ CH NH ][ OH ] 3 3 C. Kb = CH NH [ ] 3 2 sp = [ 3 3 ][ ] D. K CH NH OH 12

19 37. What is the K b value for HPO 2 4? A B C D Which of the following is the net ionic equation that describes the hydrolysis that occurs in a KCO 2 3 solution? 2 A. 2K ( aq ) CO3 ( aq ) Æ K2CO3( s) 2 B. KCO 2 3( aq ) Æ 2K ( aq ) CO3 ( aq ) 2 aq aq aq C. CO3 ( ) H2O( l) Æ HCO3 ( ) OH ( ) 2 3( aq ) 2 ( l) 2 3( aq ) ( aq ) aq D. KCO 2HO Æ HCO 2K 2OH ( ) 39. Which of the following amphiprotic ions will act predominantly as a base in solution? A. HSO 3 B. HSO 4 C. HPO 4 2 D. HPO Consider the indicator equilibrium: HIn H O Æ H O In yellow 2 3 Which of the following is true about the transition point of this indicator? A. ph = 70. [ ] = [ ] [ ] > [ ] B. HIn In C. HIn In D. moles of H O = moles of In 3 red 13 OVER

20 41. What is one of the K a values for thymol blue? A B C D A ml sample of a diprotic weak acid is titrated with ml of M NaOH. What is the concentration of the acid? A M B M C M D M 43. Which of the following is the complete ionic equation for the titration of HCl ( aq ) with KOH ( aq )? A. H ( aq ) OH ( aq ) Æ H 2 O( l ) B. HCl KOH Æ KCl H 2 O l ( aq ) ( aq ) ( aq ) ( ) ( aq ) ( aq ) ( aq ) ( aq ) Æ ( aq ) 2 ( l) aq aq aq aq aq aq C. H Cl K OH KCl H O D. H ( ) Cl ( ) K ( ) OH ( ) Æ K ( ) Cl ( ) H2O l ( ) 44. What is always true about the ph at the equivalence point when a weak acid is titrated with a strong base? A. ph < 68. B. ph > 70. C. ph = 70. D. ph = What happens to the ph of a buffer solution if a small amount of base is added? A. The ph remains constant. B. The ph increases slightly. C. The ph decreases slightly. D. The ph decreases significantly. 14

21 46. What would be a reasonable [ HO 3 ] value for a sample of rainwater to be classified as acid rain? A M B M C M D M 47. Consider the following redox equation: MnO 5Fe 8H Æ Mn 5Fe 4H O Which of the following statements is false? A. Iron is oxidized. B. Hydrogen is reduced. C. Manganese is reduced. D. The equation is balanced Consider the following unbalanced redox equation: Which chemical species is oxidized? A. Pt B. Cl C. HO 2 D. NO Pt NO Cl Æ PtCl NO H O What is the oxidation number of carbon in the ethanoate ion CHO 2 3 2? A. 1 B. 0 C. 1 2 D OVER

22 50. What reaction will occur when a solution containing 1. 0M MgSO4 and 10. M CoCl 2 is stored in a galvanized (Zn coated) bucket? A. Mg( s) Cl ( g) Æ MgCl B. Co SO4 Æ CoSO4( s ) 2 2 C. Co Zn( s) Æ Zn Co( s) 2 2 D. Mg Zn( s) Æ Zn Mg( s) 51. When the skeletal equation Br Æ BrO is balanced in acidic solution, 2 3 HO 2, H and e will appear. Which of the following are the correct balancing coefficients? HO 2 H e A B C D Consider the following balanced redox equation in acidic solution: HO 2CoCl OCl Æ 2Co( OH) 5Cl 4H Which of the following describes the amounts and locations of OH the equation is balanced in basic solution? and H O 2 if A. 1HOon 2 the left and no OH B. 1HOon 2 the left and 4OH on the left C. 5HOon 2 the left and 4OH on the left D. 1HOon 2 the left and 4OH on the right 16

23 53. Consider the numbered components in the following diagram: Which of the following would best describe the components of this electrochemical cell? Component 1 Component 2 Component 3 (Contents) A. nonmetal power supply NaNO 3 ( aq ) B. metal light bulb NaNO 3 ( aq ) C. metal voltmeter CH OH 3 aq ( ) D. metal power supply CH OH 3 aq ( ) 17 OVER

24 Use the following diagram to answer questions 54 to 56. Volts Cl 2 Ag 1.0 M KNO3 Pt (inert) 1.0 M NaCl 1.0 M AgNO Which of the following represents the anode halfcell reaction? A. Ag Æ Ag e B. Ag e Æ Ag C. Cl2 2e Æ 2Cl D. 2Cl Æ Cl 2e What changes in mass occur to the anode and cathode? Anode Mass Cathode Mass A. decreases increases B. decreases no change C. increases decreases D. increases no change 56. What is the voltage for this cell under standard conditions? A V B V C V D V 18

25 57. Consider the following diagram: VOLTMETER Zn Porous Barrier Pb 1.0 M Zn(NO 3 ) M Pb(NO 3 ) 2 As the cell operates, the voltage gradually changes. Which of the following is responsible for this change? A. The Pb 2 B. The Pb 2 C. The Zn 2 [ ] is increasing. [ ] is decreasing. [ ] is decreasing. D. The mass of the Pb( s ) electrode is decreasing. 19 OVER

26 Use the following diagram to answer questions 58 and 59. DC Power Source A B 1.0 M CuSO The above cell is constructed in order to copper plate an object. For best results, which of the following should be used for electrodes A and B? Electrode A Electrode B A. object pure copper B. pure copper object C. object any conductor D. any conductor object 59. A student tries to use the above apparatus to copper plate a zinc object. What will happen if the student places the zinc object at A and the copper electrode at B? Electrode A Electrode B A. Cu ( s) forms Cu dissolves B. Zn dissolves Zn ( s) forms C. Zn dissolves Cu ( s) forms D. Bubbles form Bubbles form 20

27 60. Which of the following occurs during the electrolysis of molten KCl? A. Oxygen forms at the anode. B. Potassium forms at the anode. C. Chlorine forms at the cathode. D. Potassium forms at the cathode. This is the end of the multiplechoice section. Answer the remaining questions directly in this examination booklet. 21 OVER

28 PART B: WRITTEN RESPONSE Value: 30 marks INSTRUCTIONS: Suggested Time: 40 minutes You are expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in the spaces below the questions. Answers must include units where appropriate and be given to the correct number of significant figures. For questions involving calculations, full marks will NOT be given for providing only an answer. 1. When solid sodium is placed in water at room temperature, an immediate, violent reaction occurs: 2Na ( s) 2H2O( l) Æ 2NaOH( aq) H2( g) energy a) Describe two methods that could be used to experimentally determine the rate of reaction. (2 marks) Method 1: Method 2: b) Would you expect the activation energy of this reaction to be high or low? Explain, using collision theory. (2 marks) 22

29 2. Consider the following equilibrium: N2( g) O2( g) Æ 2NO( g) Keq = Initially, 0. 15mol N 2 and 0. 15mol O 2 were placed in a 1. 0L container. Calculate the concentration of all species at equilibrium. (4 marks) 23 OVER

30 3. a) How would a saturated solution be prepared at room temperature? (1 mark) b) Write a chemical equation to illustrate the equilibrium that exists in a saturated solution of Be PO ( ). (2 marks) Using calculations, show why the electrical conductivity of 10. M H2CO 3 will be less than that for 010. M HCl. (4 marks) 24

31 5. Water, at 60 C, has a K w = a) Write an equation representing the ionization of water. Include the heat of reaction 57. 1kJ ( ) in the equation. (2 marks) b) If a small amount of NaOH is added to water, what happens to the value of K w? (1 mark) 25 OVER

32 6. Calculate the ph of 30. M Na2CO 3. Start by writing the equation for the predominant equilibrium reaction. (5 marks) 26

33 7. An impure sample of CaC 2 O 4 weighing g is titrated with ml of M KMnO 4. The net reaction is MnO 5C O 16H Æ 2Mn 10CO 8H O 2 2 What is the percent by mass of the CaC O 2 4 in the original sample? (4 marks) 8. A sample of Zn corrodes in moist air. a) Write the reduction halfreaction. (1 mark) b) What metal could be attached to the sample to prevent the corrosion of the zinc? Explain. (2 marks) END OF EXAMINATION 27

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35 Data Booklet CHEMISTRY 12 Work done in this booklet will not be marked. Ministry of Education Revised January 2000

36 CONTENTS Page Table 1 Periodic Table of the Elements 2 Atomic Masses of the Elements 3 Names, Formulae, and Charges of Some Common Ions 4 Solubility of Common Compounds in Water 5 Solubility Product Constants at 25 C 6 Relative Strengths of BrønstedLowry Acids and Bases 7 Acidbase Indicators 8 Standard Reduction Potentials of Halfcells REFERENCE D.R. Lide, CRC Handbook of Chemistry and Physics, 80 th edition, CRC Press, Boca Raton, 1999.

37 PERIODIC TABLE OF THE ELEMENTS Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine H He Hydrogen Helium Ne Neon Atomic Number Symbol Name Atomic Mass 3 Li Lithium Si Silicon Na Mg Sodium Magnesium Aluminum Silicon Phosphorus Sulphur Chlorine Argon Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Ni Cu Zn Ga Ge As Se Br Kr Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Nickel Rb Y Zr Nb Mo Tc Ru Rh Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon (98) Sr Pd Ag Cd In Sn Sb Te I Xe Cs Ba Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon (209) (210) (222) Fr Ra La Hf Ac Rf Ta Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (223) (226) (227) (261) (262) (263) (262) (265) (266) 74 W Db Sg Re Os Bh Hs Ir Mt Pt Au Hg Tl Pb Bi Po At Rn 58 Ce Cerium Based on mass of C 12 at Th Thorium Pr Praseodymium Pa Protactinium Nd Neodymium U Uranium Pm Promethium (145) 93 Np Neptunium (237) 62 Sm Samarium Pu Plutonium (244) 63 Eu Europium Am Americium (243) 64 Gd Gadolinium Cm Curium (247) 65 Tb Terbium Bk Berkelium (247) 66 Dy Dysprosium Cf Californium (251) 67 Ho Holmium Es Einsteinium (252) 68 Er Erbium Fm Fermium (257) 69 Tm Thulium Md Mendelevium (258) 70 Yb Ytterbium No Nobelium (259) 71 Lu Lutetium Lr Lawrencium (262) Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. 1

38 ATOMIC MASSES OF THE ELEMENTS Based on mass of C 12 at Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally. 2 Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curium Dubnium Dysprosium Einsteinium Erbium Europium Fermium Fluorine Francium Gadolinium Gallium Germanium Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanum Lawrencium Lead Lithium Lutetium Magnesium Manganese Mendelevium Ac Al Am Sb Ar As At Ba Bk Be Bi B Br Cd Ca Cf C Ce Cs Cl Cr Co Cu Cm Db Dy Es Er Eu Fm F Fr Gd Ga Ge Au Hf He Ho H In I Ir Fe Kr La Lr Pb Li Lu Mg Mn Md (227) 27.0 (243) (210) (247) (251) (247) (262) (252) (257) 19.0 (223) (262) (258) Mercury Molybdenum Neodymium Neon Neptunium Nickel Niobium Nitrogen Nobelium Osmium Oxygen Palladium Phosphorus Platinum Plutonium Polonium Potassium Praseodymium Promethium Protactinium Radium Radon Rhenium Rhodium Rubidium Ruthenium Rutherfordium Samarium Scandium Selenium Silicon Silver Sodium Strontium Sulphur Tantalum Technetium Tellurium Terbium Thallium Thorium Thulium Tin Titanium Tungsten Uranium Vanadium Xenon Ytterbium Yttrium Zinc Zirconium Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr (237) (259) (244) (209) (145) (226) (222) (261) (98) Element Symbol Atomic Number Atomic Mass Element Symbol Atomic Number Atomic Mass

39 NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air. ** Not stable in aqueous solutions. Positive Ions (Cations) Al 3 Aluminum Pb 4 Lead(IV), plumbic NH 4 Ammonium Li Lithium Ba 2 Barium Mg 2 Magnesium Ca 2 Calcium Mn 2 Manganese(II), manganous Cr 2 Chromium(II), chromous Mn 4 Manganese(IV) Cr 3 Chromium(III), chromic Hg 2 2 Mercury(I)*, mercurous Cu Copper(I)*, cuprous Hg 2 Mercury(II), mercuric Cu 2 Copper(II), cupric K Potassium H Hydrogen Ag Silver H 3 O Hydronium Na Sodium Fe 2 Iron(II)*, ferrous Sn 2 Tin(II)*, stannous Fe 3 Iron(III), ferric Sn 4 Tin(IV), stannic Pb 2 Lead(II), plumbous Zn 2 Zinc Negative Ions (Anions) Br Bromide OH Hydroxide CO 3 2 Carbonate ClO Hypochlorite ClO 3 Chlorate I Iodide Cl Chloride HPO 4 2 Monohydrogen phosphate ClO 2 Chlorite NO 3 Nitrate CrO 4 2 Chromate NO 2 Nitrite CN Cyanide C 2 O 4 2 Oxalate Cr 2 O 7 2 Dichromate O 2 Oxide** H 2 PO 4 Dihydrogen phosphate ClO 4 Perchlorate CH 3 COO Ethanoate, acetate MnO 4 Permanganate F Fluoride PO 4 3 Phosphate HCO 3 Hydrogen carbonate, bicarbonate SO 4 2 Sulphate HC 2 O 4 Hydrogen oxalate, binoxalate S 2 Sulphide HSO 4 Hydrogen sulphate, bisulphate SO 3 2 Sulphite HS Hydrogen sulphide, bisulphide SCN Thiocyanate HSO 3 Hydrogen sulphite, bisulphite 3

40 SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/l at 25 C. Negative Ions (Anions) Positive Ions (Cations) Solubility of Compounds All Alkali ions: Li,Na,K,Rb,Cs,Fr Soluble All Hydrogen ion: H Soluble All Ammonium ion: NH 4 Soluble Nitrate, NO 3 All Soluble or or Chloride,Cl Bromide, Br Iodide, I All others Ag,Pb 2,Cu Soluble Low Solubility Sulphate, SO 4 2 All others Ag,Ca 2,Sr 2,Ba 2,Pb 2 Soluble Low Solubility Sulphide, S 2 Alkali ions, H,NH 4,Be 2,Mg 2,Ca 2,Sr 2,Ba 2 All others Soluble Low Solubility Hydroxide, OH Alkali ions, H,NH 4,Sr 2 All others Soluble Low Solubility or or Phosphate, PO 4 3 Carbonate, CO 3 2 Sulphite, SO 3 2 Alkali ions, H,NH 4 All others Soluble Low Solubility 4

41 SOLUBILITY PRODUCT CONSTANTS AT 25 C Name Barium carbonate Barium chromate Barium sulphate Calcium carbonate Calcium oxalate Calcium sulphate Copper(I) iodide Copper(II) iodate Copper(II) sulphide Iron(II) hydroxide Iron(II) sulphide Iron(III) hydroxide Lead(II) bromide Lead(II) chloride Lead(II) iodate Lead(II) iodide Lead(II) sulphate Magnesium carbonate Magnesium hydroxide Silver bromate Silver bromide Silver carbonate Silver chloride Silver chromate Silver iodate Silver iodide Strontium carbonate Strontium fluoride Strontium sulphate Zinc sulphide Formula BaCO 3 BaCrO 4 BaSO 4 CaCO 3 CaC 2 O 4 CaSO 4 CuI Cu IO 3 CuS FeS ( ) AgBr AgCl AgI ZnS ( ) 2 Fe( OH) 2 Fe OH 3 PbBr 2 PbCl 2 ( ) 2 Pb IO 3 PbI 2 PbSO 4 MgCO 3 ( ) 2 Mg OH AgBrO 3 Ag 2 CO 3 Ag 2 CrO 4 AgIO 3 SrCO 3 SrF 2 SrSO 4 K sp

42 RELATIVE STRENGTHS OF BRØNSTEDLOWRY ACIDS AND BASES in aqueous solution at room temperature. Name of Acid Acid Base K a STRONG STRENGTH OF ACID WEAK 4 4 Perchloric HClO H ClO Hydriodic HI H I Hydrobromic HBr H Br Hydrochloric HCl H Cl 3 3 Nitric HNO H NO very large very large very large very large very large Sulphuric H2SO4 H HSO4 very large Hydronium Ion H O 3 H H2O Iodic HIO 3 H IO Oxalic H C O H HC O ( 2 ) 2 3, ( III) 6 Fe( H2O) ( OH) ( ) Sulphurous SO H O H SO H HSO Hydrogen sulphate ion HSO H SO Phosphoric H PO H H PO Hexaaquoiron ion iron ion Fe H O H Citric H C H O H H C H O Nitrous HNO H NO Hydrofluoric HF H F Methanoic, formic HCOOH H HCOO ( ) ( ) ( ) Hexaaquochromium ion, chromium( III) ion Cr H2O H Cr H 6 2O OH Benzoic C6H5COOH H C6H5COO Hydrogen oxalate ion HC2O 4 H C2O Ethanoic, acetic CH3COOH H CH3COO Dihydrogen citrate ion H C H O H HC H O ( ) ( ) ( ) Hexaaquoaluminum ion, aluminum ion Al H2O H Al H O OH Carbonic ( CO HO 2 ) HCO H HCO Monohydrogen citrate ion 2 3 HC6H5O 7 H C6H5O Hydrogen sulphite ion HSO3 H SO Hydrogen sulphide H2S H HS Dihydrogen phosphate ion H2PO4 H HPO Boric H3BO3 H H2BO Ammonium ion NH4 H NH Hydrocyanic HCN H CN Phenol C 6H5OH H C6H5O Hydrogen carbonate ion HCO3 H CO Hydrogen peroxide H2O2 H HO Monohydrogen phosphate ion 2 HPO4 H PO Water H O H OH Hydroxide ion OH H O very small 3 2 Ammonia NH H NH very small WEAK STRENGTH OF BASE STRONG 6

43 ACIDBASE INDICATORS Indicator Methyl violet Thymol blue Orange IV Methyl orange Bromcresol green Methyl red Chlorophenol red Bromthymol blue Phenol red Neutral red Thymol blue Phenolphthalein Thymolphthalein Alizarin yellow Indigo carmine ph Range in Which Colour Change Occurs Colour Change as ph Increases yellow to blue red to yellow red to yellow red to yellow yellow to blue red to yellow yellow to red yellow to blue yellow to red red to amber yellow to blue colourless to pink colourless to blue yellow to red blue to yellow 7

44 STANDARD REDUCTION POTENTIALS OF HALFCELLS Ionic concentrations are at 1M in water at 25 C. Oxidizing Agents Reducing Agents E ( Volts ) STRONG STRENGTH OF OXIDIZING AGENT WEAK Overpotential Effect F2( g) 2e 2F SO 2e 2SO HO 2H 2e 2HO MnO 8H 5e Mn 4H O Au 3e Au( s) BrO3 6H 5e 1 Br 2 2( l) 3H2O ClO 8H 8e Cl 4H O Cl2( g) e Cl O 2 2( g) H e H2O 2 MnO2( s) ( s) 2 Br2( l) e Br AuCl4 e Au( s) Cl 3 ( g) 2 2 Hg e Hg( l) 1 7 O 2 2( g) H M e H2O Ag e Ag( s) 1 2 Hg 2 2 e Hg( l) 3 2 O ( ) H e 2 g H2O ( s) I2( s) e I Cu e Cu( s) ( s) 3 2O 2 Cu e Cu( s) SO 4H 2e H SO H O Cu e Cu Sn 2e Sn S( ) 2H 2e s H2S( g) 2H 2e H2( g) 2 Pb 2e Pb( s) 2 Sn 2e Sn( s) Ni 2e Ni( s) HPO 2H 2e HPO HO Co e Co( s) Se( s) H e H2Se Cr e Cr H2 2 2 Fe e Fe( s) 2 Ag2S( s) e Ag() s S 3 Cr e Cr( s) 2 Zn e Zn( s) ( s) Te HO 2 e H2( g) OH 2 Mn e Mn( s) 3 Al e Al( s) 2 Mg e Mg( s) Na e Na( s) 2 Ca e Ca( s) 2 Sr e Sr( s) 2 Ba e Ba( s) K e K( s) Rb e Rb( s) Cs e Cs( s) Li e Li( s) O 2e H 2OH ( 10 M) Te H e H Cr O 14H 6e 2Cr 7H O H 2e Mn 2H O 122. IO 6H 5e I 3H O NO 4H 3e NO 2H O ( 10 ) NO 4H 2e N O 2H O Fe e Fe MnO 2H O 3e MnO 4OH HSO H e S H Overpotential Effect WEAK STRENGTH OF REDUCING AGENT STRONG