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© 2004 Ministry of Education
MINISTRY USE ONLY
Place Personal Education Number (PEN) here.
MINISTRY USE ONLY
Chemistry 12
APRIL 2004
Course Code = CH
Student Instructions1. Place the stickers with your Personal
Education Number (PEN) in the allottedspaces above. Under no circumstance isyour name or identification, other thanyour Personal Education Number, toappear on this booklet.
2. Ensure that in addition to this examinationbooklet, you have a Data Booklet and anExamination Response Form. Follow thedirections on the front of the Response Form.
3. Disqualification from the examination willresult if you bring books, paper, notes orunauthorized electronic devices into theexamination room.
4. When instructed to open this booklet, checkthe numbering of the pages to ensure thatthey are numbered in sequence from pageone to the last page, which is identified by
*END OF EXAMINATION* .
5. At the end of the examination, place yourResponse Form inside the front cover of thisbooklet and return the booklet and yourResponse Form to the supervisor.
Question 1
0 1 2 3 4 (5) NR.
Question 2
0 1 2 3 4 (5) NR.
Question 3
0 1 2 3 4 (5) NR.
Question 4
0 1 2 3 (5) NR.
Question 5
0 1 2 3 (5) NR.
Question 6
0 1 2 3 4 (5) NR5 .
Question 7
0 1 2 3 4 (5) NR.
Question 8
0 1 2 3 (5) NR.
82841375
Chemistry 12
APRIL 2004
Course Code = CH
GENERAL INSTRUCTIONS
1. Aside from an approved calculator, electronic devices, including dictionaries andpagers, are not permitted in the examination room.
2. All multiple-choice answers must be entered on the Response Form using anHB pencil. Multiple-choice answers entered in this examination booklet will not bemarked.
3. For each of the written-response questions, write your answer in the space providedin this booklet.
4. Ensure that you use language and content appropriate to the purpose and audience ofthis 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.
CHEMISTRY 12 PROVINCIAL EXAMINATION
ValueSuggested
Time1. This examination consists of two parts:
PART A: 60 multiple-choice questions 60 80
PART B: 8 written-response questions 30 40
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 Brønsted-Lowry Acids and Bases• Acid-Base Indicators• Standard Reduction Potentials of Half-cells
No other reference materials or tables are allowed.
3. A calculator is essential for the Chemistry 12 Provincial Examination. Thecalculator must be a hand-held device designed primarily for mathematicalcomputations involving logarithmic and trigonometric functions and may be capable ofperforming graphing functions. Computers, calculators with a QWERTY keyboard orsymbolic manipulation abilities, and electronic writing pads will not be allowed.Students must not bring any external devices (peripherals) to support calculators suchas manuals, printed or electronic cards, printers, memory expansion chips or cards,CD-ROMs, libraries or external keyboards. Students may have more than onecalculator 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 orreceive electronic signals. In addition to an approved calculator, students will beallowed to use rulers, compasses, and protractors during the examination.
Calculators must not have any information programmed into memory that would notbe acceptable in paper form. Specifically, calculators must not have any built-in notes,definitions, or libraries. There is no requirement to clear memories at the beginning ofthe examination but the use of calculators with built-in notes is equivalent to the use ofnotes in paper form. Any student deemed to have cheated on a provincial examinationwill receive a “0” on that examination and will be permanently disqualified from theProvincial Examination Scholarship Program.
THIS PAGE INTENTIONALLY BLANK
OVER- 1 -
PART A: MULTIPLE CHOICE
Value: 60 marks Suggested Time: 80 minutes
INSTRUCTIONS: For each question, select the best answer and record your choice on the ResponseForm provided. Using an HB pencil, completely fill in the circle that has the lettercorresponding to your answer.
Use the following information to answer questions 1 and 2.
When a candle C H20 42( ) burns, the following reaction occurs:
2 61 40 4220 42 2 2 2C H O CO H O heats g g g( ) ( ) ( ) ( )+ Æ + +
1. If the rate of production of CO2 is 0 98. ming , what is the rate of oxygenconsumption?
A. 0 47. mingB. 0 54. ming
C. 0 71. ming
D. 1 1. ming
2. Which of the following properties could best be monitored in order to determine thereaction rate of the burning candle?
A. mass of C H20 42 s( )B. pressure of H O2 g( )C. surface area of C H20 42 s( )D. concentration of C H20 42 s( )
3. Which of the following is true of the kinetic and potential energies as reactantmolecules approach each other to form an activated complex?
KE PE
A. increases decreases
B. decreases increases
C. decreases remains constant
D. remains constant remains constant
- 2 -
4. Which of the following are necessary for successful collisions between reactantmolecules?
I. high concentration
II. sufficient energy
III. correct geometry
IV. presence of a catalyst
A. I and II onlyB. II and III onlyC. III and IV onlyD. I, II and III only
5. Which of the following graphs most likely represents the slowestforward reaction?
A.
PE(kJ)
50
100
Progress of the reaction
B.
PE(kJ)
50
100
Progress of the reaction
C.
PE(kJ)
50
100
Progress of the reaction
D.
PE(kJ)
50
100
Progress of the reaction
OVER- 3 -
6. For an exothermic reaction, which of the following is true?
A. PE PE PEreactants activated complex products> >
B. PE PE PEproducts activated complex reactants> >
C. PE PE PEactivated complex reactants products> >
D. PE PE PEactivated complex products reactants> >
7. Consider the following reaction:
O O Og g g( ) ( ) ( )+ Æ3 22
Which of the following describes how the reaction’s catalyzed PE diagramcompares to the reaction’s uncatalyzed PE diagram?
Ea DH
A. E catalyzed Ea a( ) < unchanged
B. E catalyzed Ea a( ) > unchanged
C. E catalyzed Ea a( ) < D DH catalyzed H( ) <
D. unchanged D DH catalyzed H( ) <
8. Consider the following reaction mechanism:
Step 1. NO O NO O+ Æ +3 2 2
Step 2. O NO NO O+ Æ +2 2
Which of the following substances is the catalyst?
A. OB. O2
C. NOD. NO2
- 4 -
9. Which of the following is true for an endothermic reaction?
A. forward E reverse Ea a>B. reverse E forward Ea a>C. forward E reverse Ea a=D. forward E reverse Ea a+ = 0
10. Some Fe3+ and SCN- were mixed and established the following equilibrium:
Fe SCN FeSCNaq aq aq( )+
( )-
( )++ Æ̈3 2
What happened to the reverse rate and Fe3+[ ] as equilibrium was established?
A. The reverse rate decreased and Fe3+[ ] increased.
B. The reverse rate increased and Fe3+[ ] increased.
C. The reverse rate decreased and Fe3+[ ] decreased.
D. The reverse rate increased and Fe3+[ ] decreased.
11. Which of the following forward reaction changes would result in the most products?
Entropy Enthalpy
A. decreasing decreasing
B. increasing decreasing
C. decreasing increasing
D. increasing increasing
12. In which of the following equations does entropy most favour reactants?
A. 12 2 2 2N O NOg g g( ) ( ) ( )+ Æ̈
B. 4 63 4 2PH P Hg g g( ) ( ) ( )Æ̈ +
C. NH Cl NH Cl4 4s aq aq( ) ( )+
( )-Æ̈ +
D. SnO H Sn H O2 2 22 2s g s g( ) ( ) ( ) ( )+ Æ̈ +
OVER- 5 -
13. The following equation represents the catalyzed decomposition of O3 (ozone):
Cl O O O Clg g g g g( ) ( ) ( ) ( ) ( )+ + Æ̈ +3 22
Which of the following is true?
A. The catalyst O speeds up only the forward rate.B. The catalyst Cl speeds up only the forward rate.C. The catalyst O speeds up both the forward and reverse rates.D. The catalyst Cl speeds up both the forward and reverse rates.
14. When the temperature of an exothermic equilibrium is increased, which of thefollowing will happen?
A. Equilibrium will shift left and products[ ] will increase.
B. Equilibrium will shift left and products[ ] will decrease.
C. Equilibrium will shift right and reactants[ ] will increase.
D. Equilibrium will shift right and reactants[ ] will decrease.
15. The following equilibrium is established in a 1 0. L container:
heat CH H S CS H+ + Æ̈ +( ) ( ) ( ) ( )4 2 2 22 4g g g g
If some CH4 is added to the system, what happens to the net concentration of CH4and the value of Keq ?
A. CH4[ ] is decreased and Keq increases.
B. CH4[ ] is increased and Keq increases.
C. CH4[ ] is decreased and Keq remains constant.
D. CH4[ ] is increased and Keq remains constant.
- 6 -
16. Consider the following equilibrium:
2 22 2 2N O N Og g g( ) ( ) ( )Æ̈ +
Initially, 0 800 2. mol N O is placed in a 1 0. L container. At equilibrium, the N2[ ] isfound to be 0 780. M. What is the value of Keq ?
A. 1 7 10 3. ¥ -
B. 1 5 101. ¥
C. 5 9 102. ¥
D. 1 2 103. ¥
17. Consider the following equilibrium:
CO H CH OHg g g( ) ( ) ( )+ Æ̈2 2 3
Some CO, H2 and CH OH3 were placed in a 1 0. L container. When equilibriumwas established, the CO[ ] had increased. Which of the following is true?
A. Trial K Keq eq> so reaction shifted left to reach equilibrium.
B. Trial K Keq eq< so reaction shifted left to reach equilibrium.
C. Trial K Keq eq> so reaction shifted right to reach equilibrium.
D. Trial K Keq eq< so reaction shifted right to reach equilibrium.
18. Which of the following would form a saturated solution when 0 010. mol of thesolid solute is added to 100 mL of water?
A. BaCO3
B. FeSO4
C. NaCN
D. Pb NO3 2( )
OVER- 7 -
19. Which net ionic equation best describes the reaction that exists in a solution preparedby mixing equal volumes of 0 20 3 2. M Ca NO( ) and 0 20 2 3. M Na CO ?
A. Ca CO CaCOaq aq s( )+
( )-
( )+ Æ̈232
3
B. Na NO NaNOaq aq s( )+
( )-
( )+ Æ̈3 3
C. Ca NO Na CO NaNO CaCO3 2 2 3 3 32( ) + Æ̈ +( ) ( ) ( ) ( )aq aq s s
D. Ca NO Na CO NaNO CaCO3 2 2 3 3 32( ) + Æ̈ +( ) ( ) ( ) ( )aq aq aq s
20. Which compound will have the greatest solubility in water?
A. CuCl
B. FeCO3
C. MgSO4
D. Cu PO3 4 2( )
21. Which cation below can be used to separate SO42 - from S2 - ions by precipitation?
A. Sr2 +
B. Pb2 +
C. Cs+
D. Be2 +
22. What will be the effect of adding some solid AgNO3 to a saturated solutionof AgCl ?
A. The AgNO3 will not dissolve.
B. More solid AgCl will dissolve.C. More solid AgCl will be produced.D. The AgNO3 will not affect the AgCl equilibrium.
- 8 -
23. For a saturated solution, the Ksp expression does not contain any solid solute term.
What is the reason for this?
A. The solid solute is a product.B. The solid solute is a reactant.C. The solid solute continues to change in amount.D. The solid solute does not change in concentration.
24. Which of the statements below describes the Ksp expression for the salt
barium phosphate?
A. K Ba POsp = [ ][ ]+ -24
3
B. K Ba POsp = [ ] [ ]+ -2 3
43 2
C. K Ba POsp = [ ][ ]+ -3 224
3
D. K Ba POsp = [ ] [ ]+ -3 22 3
43 2
25. What is the solubility of Fe OH( )2 ?
A. 4 9 10 17. ¥ - M
B. 1 2 10 17. ¥ - M
C. 3 7 10 6. ¥ - M
D. 2 3 10 6. ¥ - M
26. Which of the following ions would have the highest concentration in 0 1 32. M CO - ?
A. Ba2 +
B. Ca2 +
C. Sr2 +
D. Mg2 +
OVER- 9 -
27. Which net ionic equation best describes the reaction between NaOH and H S2 ?
A. OH H H Oaq aq( )-
( )+
( )+ Æ̈2 l
B. 2 22 22OH H S H O Saq aq aq( )
-( ) ( ) ( )
-+ Æ̈ +l
C. 2 22 2 2NaOH H S H O Na Saq aq aq( ) ( ) ( ) ( )+ Æ̈ +l
D. 2 2 2 2 222
2Na OH H S H O Na Saq aq aq aq aq aq( )+
( )-
( )+
( )-
( ) ( )+
( )-+ + + Æ̈ + +l
28. Which of the following is a general characteristic of Arrhenius acids?
A. They produce H+ in solution.
B. They accept an H+ from water.
C. They turn bromthymol blue a blue colour.
D. They react with H O3+ ions to produce H2.
29. Identify a conjugate pair from the equilibrium provided:
PO HCO HPO CO43
3 42
32- - - -+ Æ̈ +
A. CO and PO32
43- -
B. PO and HCO43
3- -
C. PO and HPO43
42- -
D. HCO and HPO3 42- -
30. Which of the following best describes a weak acid?
A. Its 0 10. M solution will have pH = 1 00. .B. It may be very soluble, but only partly ionized.C. It must be very soluble and completely ionized.D. It must be of low solubility and completely ionized.
- 10 -
31. Which of the following solutions will have the lowest OH-[ ] ?
A. NaFaq( )
B. NaClaq( )
C. NaHCO3 aq( )
D. NaHPO4 aq( )
32. Water has the greatest tendency to act as an acid with which of the following?
A. Cl-
B. NO2-
C. H PO2 4-
D. CH COO3-
33. Which of the following statements is true for an acidic solution at 25∞C ?
A. pH > 7 0.
B. pOH < 7 0.
C. H O OH3+ -[ ] < [ ]
D. H O OH3+ -[ ] > [ ]
34. What is the OH-[ ] in 0 025. M HCl ?
A. 2 5 10 16. ¥ - M
B. 4 0 10 13. ¥ - M
C. 2 5 10 2. ¥ - M
D. 2 5 1012. ¥ M
OVER- 11 -
35. What is the equilibrium expression for the predominant equilibriumin NaHCO3 aq( ) ?
A. KHCO
H O COa =
[ ][ ][ ]
-
+ -
3
3 32
B. KHCO
H CO OHb =
[ ][ ][ ]
-
-
3
2 3
C. KH O CO
HCOa =
[ ][ ][ ]
+ -
-
3 32
3
D. KH CO OH
HCOb =
[ ][ ][ ]
-
-
2 3
3
36. What is true about an acid that has a large Ka value?
A. The acid is weak.
B. The acid is strong.
C. The acid has a large Kb value.
D. The acid has a large pH value.
37. Consider the following reaction:
NO H O HNO OH2 2 2aq aq aq( )-
( ) ( ) ( )-+ Æ̈ +l
This reaction represents which of the following?
A. the titration of NO2-
B. the ionization of HNO2
C. the hydrolysis of NaNO2
D. the dissociation of NaNO2
- 12 -
38. Which of the following salts will be basic?
A. KClB. NH Cl4
C. KHSO4
D. K HPO2 4
39. Consider the following indicator equilibrium:
HIn H O H O Inyellow blue
+ Æ̈ +( ) ( )
+ -2 3
What is the result of adding CH COOH3 to this indicator?
Equilibrium Shift Colour
A. left blue
B. left yellow
C. right blue
D. right yellow
40. An indicator changes colour when 4 0. M HCl is added. If the indicator has aKa = ¥ -1 10 10 , identify the indicator and the pH at its transition point.
Indicator pH
A. phenolphthalein 4 0.
B. phenolphthalein 10 0.
C. thymolphthalein 4 0.
D. thymolphthalein 10 0.
OVER- 13 -
41. What term describes the chemical that is used to detect the end point ofan acid-base titration?
A. bufferB. standardC. indicatorD. primary standard
42. The strong acid, HNO3 aq( ), is titrated with the weak base, NH3 aq( ).What is the net ionic equation for this reaction?
A. H OH H Oaq aq( )+
( )-
( )+ Æ 2 l
B. H NH NHaq aq aq( )+
( ) ( )++ Æ3 4
C. HNO NH NH NO3 3 4 3aq aq aq( ) ( ) ( )+ Æ
D. H NO NH NH NOaq aq aq aq aq( )+
( )-
( ) ( )+
( )-+ + Æ +
3 3 4 3
43. What H O3+[ ] results when 25 0 1 0. .mL of M HCl is mixed
with 15 0 0 30. .mL of M KOH ?
A. 0 020. MB. 0 51. MC. 0 70. MD. 0 82. M
44. What typically happens to the pH of a buffer solution when a small amount of acidis added?
A. The pH increases slightly.B. The pH decreases slightly.C. The pH always remains the same.D. The pH first increases then decreases to its original value.
- 14 -
45. Consider the following buffer equilibrium:
HF H O H O Faq aq aq( ) ( ) ( )+
( )-+ Æ̈ +2 3l
What would limit the buffering action if acid were added?
A. F-[ ]B. HF[ ]C. H O2[ ]D. H O3
+[ ]
46. Identify an environmental problem associated with acid rain.
A. increasing the pH of lakesB. depletion of the ozone layerC. chemical decomposition of rainwaterD. chemical erosion of limestone structures
47. Which of the following is not a redox equation?
A. Zn S ZnS+ ÆB. Cl NaI NaCl I2 22 2+ Æ +C. Sn Fe Fe Sn4 2 3 22 2+ + + ++ Æ +D. K PO AgNO Ag PO KNO3 4 3 3 4 33 3+ Æ +
48. Consider the following equation:
8 5 5 442 3 2
2H MnO Fe Fe Mn H O+ - + + ++ + Æ + +
Which ion is the reducing agent?
A. H+
B. Fe2+
C. Fe3+
D. MnO4-
OVER- 15 -
49. What is the oxidation number of chromium in the complex ion Cr H O Br2 4 2( ) + ?
A. -1B. +1C. +2D. +3
50. Three elements (X, Y, and Z) and solutions of their anions were combined.The results are shown in the following data table:
X aq( )- Y aq( )
- Z aq( )-
X — No reaction No reaction
Y Reaction — Reaction
Z Reaction No reaction —
Which of the following best describes the strength of the ions acting asreducing agents?
A. X Y Z- - -> >
B. X Z Y- - -> >
C. Y Z X- - -> >
D. Z Y X- - -> >
51. When the skeletal equation Cr O Cr2 72 3- +Æ is balanced in acidic solution
H+ and e- will appear. Which of the following best describes the H+ and e-
for the balanced half-reaction?
A. 7H+ on the left and 1e- on the right
B. 14H+ on the left and 9e- on the left
C. 14H+ on the left and 6e- on the left
D. 14H+ on the left and 6e- on the right
- 16 -
52. The titration of a 25 0 2. mL SnCl sample, in acidic solution, requires 14 4. mLof 0 030 2 2 7. M K Cr O . The balanced equation for the reaction is shown below:
Cr O H Sn Sn Cr H O2 72 2 4 3
214 3 3 2 7- + + + ++ + Æ + +
What is the number of moles of SnCl2 in the original sample?
A. 1 4 10 4. ¥ - mol
B. 4 3 10 4. ¥ - mol
C. 1 3 10 3. ¥ - mol
D. 5 2 10 2. ¥ - mol
53. Consider the following reaction:
Ni Ag Ag Ni2 2 2+ ++ Æ +
Which of the following is true?
E∞ Reaction
A. -1 06. V non-spontaneous
B. -0 54. V non-spontaneous
C. +0 54. V spontaneous
D. +1 06. V spontaneous
OVER- 17 -
Use the following diagram to answer questions 54 to 56.
Anion movement
1.0 M Ni2+ 1.0 M Pd2+
PdNi PorousBarrier
VOLTMETER
0.88V
Cation movement
54. What is the half-cell reaction at the anode?
A. Ni Ni eÆ ++ -2 2
B. Pd Pd eÆ ++ -2 2
C. Ni e Ni2 2+ -+ ÆD. Pd e Pd2 2+ -+ Æ
55. What best describes the flow of electrons?
A. from Ni to PdB. from Pd to NiC. from cathode to anodeD. into the solution around the Ni electrode
56. What is the voltage for the oxidation half-reaction of Pd?
A. -0 62. VB. +0 62. VC. +0 88. VD. +1 14. V
- 18 -
Use the following diagram to answer questions 57 and 58.
1.0 M K2SO4
DCPowerSource
CuPt(inert)
+ –
57. What is the equation for the anode reaction?
A. K K eÆ ++ -
B. Cu Cu eÆ ++ -2 2
C. 2 242
2 82SO S O e- - -Æ +
D. H O O H M e212 2
72 10 2Æ + ( ) ++ - -
58. Which of the following best describes the mass of the copper electrode and thedirection of cation movement as the cell operates?
Mass of the copper electrode
Cationmovement
A. increases to the left
B. stays the same to the left
C. stays the same to the right
D. decreases to the right
OVER- 19 -
59. Consider the following diagram:
1.0
M KNO
3
Fe nail
Cu
1.0 M Cu2+ 1.0 M Fe3+
DCPowerSource
+ –
Which of the following statements describes why the cell would not be used toelectroplate an Fe nail with copper?
A. Fe3+ will react with Cu2 +.
B. The cell reaction is non-spontaneous.
C. Cu2 + ions do not collide with the nail.
D. The power supply is connected backwards.
60. In the electro-refining of an ore, the ore is dissolved and the solution placed in anelectrolytic cell. A specific ore produces a solution which contains Na+ , Cu2+ ,
Pb2+ and Ag+ . Which of these metals can be plated out from the solution byelectrolysis?
A. all four metalsB. Cu and Pb onlyC. Na, Cu and Pb onlyD. Cu, Pb and Ag only
This is the end of the multiple-choice section.Answer the remaining questions directly in this examination booklet.
- 20 -
PART B: WRITTEN RESPONSE
Value: 30 marks Suggested Time: 40 minutes
INSTRUCTIONS You are expected to communicate your knowledge and understanding of chemicalprinciples in a clear and logical manner. Your steps and assumptions leading to asolution must be written in the spaces below the questions. Answers must includeunits where appropriate and be given to the correct number of significant figures.For questions involving calculations, full marks will NOT be given forproviding only an answer.
1. Consider the following equilibrium:
Al H O OH Al H O OH H2 4 2 3 3( ) ( ) Æ̈ ( ) ( ) +( )+
( ) ( )+
2 aq s aq
a) Some HCl aq( ) is added to the equilibrium. What happens to the amount of solid
Al H O OH2 3 3( ) ( ) ? Explain. (2 marks)
b) The HCl is added at time t1 and equilibrium is re-established at time t2.On the axis below, sketch what happens to the reverse reaction rate. (2 marks)
ReverseReaction
Rate
t1 t2
Time
OVER- 21 -
2. Consider the following diagram for the equilibrium:
N O NO H kJ2 4 22 59g g( ) ( )Æ̈ = +D
t2
Concentration(M)
0.60
t3
0.62
0.64
NO2
N2O4
Time
t1
0.66
a) Calculate the value of Keq at t1. (1 mark)
b) Calculate the value of Keq at t 3. (1 mark)
c) What stress was applied at time t2 ? Explain. (2 marks)
Stress:
Explanation:
- 22 -
3. Calculate the mass of solid AgNO3 that can be added to 2 0. L of a 0 10 2 4. M K CrOsolution in order to just start precipitation. (4 marks)
OVER- 23 -
4. a) Write the formula equation to represent the complete neutralization reactionbetween household vinegar (acetic acid) and drain cleaner (sodium hydroxide). (2 marks)
b) Write the formula for the conjugate base of the reactant acid. (1 mark)
5. A sample of pure NaOH s( ) is dissolved in water to make 10 0. L of solution and a
pH = 10 75. results. Calculate the mass of pure NaOH that was dissolved. (3 marks)
- 24 -
6. Calculate the pH of M NH0 70 3. . Start by writing the equation for the predominantequilibrium reaction. (5 marks)
- 25 -
7. Balance the following redox reaction in basic solution: (4 marks)
ClO N H NO Cl3 2 4 3- - -+ Æ + (basic)
8. A 1 0. M solution of CoSO4 is electrolyzed using inert electrodes.
a) Write the anode and cathode half-reactions that would occur. (2 marks)
Anode:
Cathode:
b) What is observed when bromthymol blue is added to the solutionaround the anode? (1 mark)
END OF EXAMINATION
THIS PAGE INTENTIONALLY BLANK
© Ministry of Education Revised January 2000
Work done in this bookletwill not be marked.
CHEMISTRY 12
DataBooklet
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 Brønsted-Lowry Acids and Bases
7 Acid-base Indicators
8 Standard Reduction Potentials of Half-cells
REFERENCE
D.R. Lide, CRC Handbook of Chemistry and Physics, 80th edition, CRC Press, Boca Raton, 1999.
CONTENTS
Bas
ed o
n m
ass
of C
12 a
t 12.
00.
Valu
es in
par
enth
eses
are
the
mas
ses
of th
e m
ost
stab
le o
r be
st k
now
n is
otop
es fo
rel
emen
ts w
hich
do
not o
ccur
nat
ural
ly.
PER
IOD
IC T
AB
LE
OF
TH
E E
LE
ME
NT
S
12
34
56
78
910
1112
1314
1516
1718
4 Be
Bery
llium
9.0
11 Na
Sodi
um
23.0
12 Mg
Mag
nesi
um
24.3
19 KPo
tass
ium
39.1
20 Ca
Cal
cium
40.1
37 Rb
Rub
idiu
m
85.5
55 Cs
Ces
ium
132.
9
56 Ba
Bariu
m
137.
3
87 Fr
Fran
cium
(223
)
88 Ra
Rad
ium
(226
)
21 Sc
Scan
dium
45.0
22 Ti
Tita
nium
47.9
39 YYt
trium
88.9
40 Zr
Zirc
oniu
m
91.2
57 La
Lant
hanu
m
138.
9
72 Hf
Haf
nium
178.
5
89 Ac
Actin
ium
(227
)
104
Rf
Rut
herfo
rdiu
m
(261
)
23 VVa
nadi
um
50.9
24 Cr
Chr
omiu
m
52.0
41 Nb
Nio
bium
92.9
42 Mo
Mol
ybde
num
95.9
73 TaTa
ntal
um
180.
9
74 WTu
ngst
en
183.
8
105
Db
Dub
nium
(262
)
106
Sg
Seab
orgi
um
(263
)
25 Mn
Man
gane
se
54.9
26 Fe
Iron
55.8
43 Tc
Tech
netiu
m
(98)
44 Ru
Rut
heni
um
101.
1
75 Re
Rhe
nium
186.
2
76 Os
Osm
ium
190.
2
107
Bh
Bohr
ium
(262
)
108
Hs
Has
sium
(265
)
27 Co
Cob
alt
58.9
45 Rh
Rho
dium
102.
9
77 IrIri
dium
192.
2
109
Mt
Mei
tner
ium
(266
)
28 Ni
Nic
kel
58.7
78 Pt
Plat
inum
195.
1
29 Cu
Cop
per
63.5
47 Ag
Silv
er
107.
9
79 Au
Gol
d
197.
0
30 Zn
Zinc
65.4
48 Cd
Cad
miu
m
112.
4
80 Hg
Mer
cury
200.
6
5 B Boro
n
10.8
13 Al
Alum
inum
27.0
31 Ga
Gal
lium
69.7
49 In Indi
um
114.
8
81 Tl
Thal
lium
204.
4
6 CC
arbo
n
12.0
14 Si
Silic
on
28.1
32 Ge
Ger
man
ium
72.6
50 Sn
Tin
118.
7
82 Pb
Lead
207.
2
7 NN
itrog
en
14.0
15 PPh
osph
orus
31.0
33 As
Arse
nic
74.9
51 Sb
Antim
ony
121.
8
83 Bi
Bism
uth
209.
0
8 OO
xyge
n
16.0
16 SSu
lphu
r
32.1
34 Se
Sele
nium
79.0
52 TeTe
lluriu
m
127.
6
84 Po
Polo
nium
(209
)
9 FFl
uorin
e
19.0
17 Cl
Chl
orin
e
35.5
35 Br
Brom
ine
79.9
53 IIo
dine
126.
9
85 At
Asta
tine
(210
)
10 Ne
Neo
n
20.2
18 Ar
Argo
n
39.9
36 Kr
Kryp
ton
83.8
54 Xe
Xeno
n
131.
3
86 Rn
Rad
on
(222
)
2 He
Hel
ium
4.0
58 Ce
Cer
ium
140.
1
90 Th
Thor
ium
232.
0
59 Pr
Pras
eody
miu
m
140.
9
91 Pa
Prot
actin
ium
231.
0
60 Nd
Neo
dym
ium
144.
2
92 UU
rani
um
238.
0
61 Pm
Prom
ethi
um
(145
)
93 Np
Nep
tuni
um
(237
)
62 Sm
Sam
ariu
m
150.
4
94 Pu
Plut
oniu
m
(244
)
63 Eu
Euro
pium
152.
0
95 Am
Amer
iciu
m
(243
)
64 Gd
Gad
olin
ium
157.
3
96 Cm
Cur
ium
(247
)
65 Tb
Terb
ium
158.
9
97 Bk
Berk
eliu
m
(247
)
66 Dy
Dys
pros
ium
162.
5
98 Cf
Cal
iforn
ium
(251
)
67 Ho
Hol
miu
m
164.
9
99 Es
Eins
tein
ium
(252
)
68 Er
Erbi
um
167.
3
100
Fm
Ferm
ium
(257
)
69 Tm
Thul
ium
168.
9
101
Md
Men
dele
vium
(258
)
70 Yb
Ytte
rbiu
m
173.
0
102
No
Nob
eliu
m
(259
)
71 Lu
Lute
tium
175.
0
103
Lr
Law
renc
ium
(262
)
1 HH
ydro
gen
1.0
46 Pd
Palla
dium
106.
4
38 Sr
Stro
ntiu
m
87.6
3 Li
Lith
ium
6.9
14 Si
Silic
on
28.1
Ato
mic
Num
ber
Sym
bol
Nam
eA
tom
ic M
ass
14 Si
Silic
on
28.1
– 1 –
ATOMIC MASSES OF THE ELEMENTSBased on mass of C12 at 12.00.
Values in parentheses are the mass number of the most stable or bestknown isotopes for elements that do not occur naturally.
– 2 –
ActiniumAluminumAmericiumAntimonyArgonArsenicAstatineBariumBerkeliumBerylliumBismuthBoronBromineCadmiumCalciumCaliforniumCarbonCeriumCesiumChlorineChromiumCobaltCopperCuriumDubniumDysprosiumEinsteiniumErbiumEuropiumFermiumFluorineFranciumGadoliniumGalliumGermaniumGoldHafniumHeliumHolmiumHydrogenIndiumIodineIridiumIronKryptonLanthanumLawrenciumLeadLithiumLutetiumMagnesiumManganeseMendelevium
AcAlAmSbArAsAtBaBkBeBiBBrCdCaCfCCeCsClCrCoCuCmDbDyEsErEuFmFFrGdGaGeAuHfHeHoHInIIrFeKrLaLrPbLiLuMgMnMd
891395511833855697
483
535482098
658551724272996
10566996863
1009
876431327972
267
1495377263657
10382
3711225
101
(227)27.0
(243)121.8
39.974.9
(210)137.3
(247)9.0
209.010.879.9
112.440.1
(251)12.0
140.1132.9
35.552.058.963.5
(247)(262)162.5
(252)167.3152.0
(257)19.0
(223)157.3
69.772.6
197.0178.5
4.0164.9
1.0114.8126.9192.2
55.883.8
138.9(262)207.2
6.9175.0
24.354.9
(258)
MercuryMolybdenumNeodymiumNeonNeptuniumNickelNiobiumNitrogenNobeliumOsmiumOxygenPalladiumPhosphorusPlatinumPlutoniumPoloniumPotassiumPraseodymiumPromethiumProtactiniumRadiumRadonRheniumRhodiumRubidiumRutheniumRutherfordiumSamariumScandiumSeleniumSiliconSilverSodiumStrontiumSulphurTantalumTechnetiumTelluriumTerbiumThalliumThoriumThuliumTinTitaniumTungstenUraniumVanadiumXenonYtterbiumYttriumZincZirconium
HgMoNdNeNpNiNbNNoOsOPdPPtPuPoKPrPmPaRaRnReRhRbRuRfSmScSeSiAgNaSrSTaTcTeTbTlThTmSnTiWUVXeYbYZnZr
80426010932841
7102
768
461578948419596191888675453744
10462213414471138167343526581906950227492235470393040
200.695.9
144.220.2
(237)58.792.914.0
(259)190.2
16.0106.4
31.0195.1
(244)(209)
39.1140.9
(145)231.0
(226)(222)186.2102.9
85.5101.1
(261)150.4
45.079.028.1
107.923.087.632.1
180.9(98)127.6158.9204.4232.0168.9118.747.9
183.8238.0
50.9131.3173.0
88.965.491.2
Element Symbol AtomicNumber
AtomicMass Element Symbol Atomic
NumberAtomicMass
NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air.** Not stable in aqueous solutions.
Negative Ions(Anions)
Positive Ions(Cations)
Aluminum
Ammonium
Barium
Calcium
Chromium(II), chromous
Chromium(III), chromic
Copper(I)*, cuprous
Copper(II), cupric
Hydrogen
Hydronium
Iron(II)*, ferrous
Iron(III), ferric
Lead(II), plumbous
Al3+
NH4+
Ba2+
Ca2+
Cr2+
Cr3+
Cu+
Cu2+
H+
H3O+
Fe2+
Fe3+
Pb2+
Lead(IV), plumbic
Lithium
Magnesium
Manganese(II), manganous
Manganese(IV)
Mercury(I)*, mercurous
Mercury(II), mercuric
Potassium
Silver
Sodium
Tin(II)*, stannous
Tin(IV), stannic
Zinc
Pb4+
Li+
Mg2+
Mn2+
Mn4+
Hg22+
Hg2+
K+
Ag+
Na+
Sn2+
Sn4+
Zn2+
Bromide
Carbonate
Chlorate
Chloride
Chlorite
Chromate
Cyanide
Dichromate
Dihydrogen phosphate
Ethanoate, acetate
Fluoride
Hydrogen carbonate, bicarbonate
Hydrogen oxalate, binoxalate
Hydrogen sulphate, bisulphate
Hydrogen sulphide, bisulphide
Hydrogen sulphite, bisulphite
Br−
CO32−
ClO3−
Cl−
ClO2−
CrO42−
CN−
Cr2O72−
H2PO4−
CH3COO−
F−
HCO3−
HC2O4−
HSO4−
HS−
HSO3−
Hydroxide
Hypochlorite
Iodide
Monohydrogen phosphate
Nitrate
Nitrite
Oxalate
Oxide**
Perchlorate
Permanganate
Phosphate
Sulphate
Sulphide
Sulphite
Thiocyanate
OH−
ClO−
I−
HPO42−
NO3−
NO2−
C2O42−
O2−
ClO4−
MnO4−
PO43−
SO42−
S2−
SO32−
SCN−
– 3 –
SOLUBILITY OF COMMON COMPOUNDS IN WATER
The term soluble here means > 0.1 mol/L at 25°C.
SolubleAlkali ions: Li+ , Na + , K+ , Rb+ , Cs+ , Fr +All
SolubleHydrogen ion: H+All
SolubleAmmonium ion: NH4+All
All SolubleNitrate, NO3−
Soluble
Low Solubility
All others
or
or
Ag+ , Pb2+ , Cu+
Chloride,Cl−
Bromide, Br−
Iodide, I−
Soluble
Low Solubility
All others
Ag+ , Ca2+ , Sr 2+ , Ba2+ , Pb2+
Sulphate, SO42−
Soluble
Low SolubilityAll others
Alkali ions, H+ , NH4+ , Be2+ , Mg2+ , Ca2+ , Sr2+ , Ba2+
Sulphide, S2−
Soluble
Low SolubilityAll others
Alkali ions, H+ , NH4+ , Sr 2+
Hydroxide, OH−
Soluble
Low SolubilityAll othersor
orAlkali ions, H+ , NH4
+
Sulphite, SO32−
Phosphate, PO43−
Carbonate, CO32−
– 4 –
Negative Ions(Anions)
Positive Ions(Cations)
Solubility ofCompounds
SOLUBILITY PRODUCT CONSTANTS AT 25°C
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
Name Formula
CuS
FeS
( )
AgBr
AgCl
AgI
ZnS
BaCO3
BaCrO4
BaSO4
CaCO3
CaC2O4
CaSO4
CuI
Cu IO3( )2
( )Fe OH 2
Fe OH 3
PbBr2
PbCl2
Pb IO3( )2
PbI2
PbSO4
MgCO3
Mg OH( )2
AgBrO3
Ag2CO3
Ag2CrO4
AgIO3
SrCO3
SrF2
SrSO4
2.6 × 10−9
1.2 × 10−10
1.1 × 10−10
5.0 × 10−9
2.3 × 10−9
7.1 × 10−5
1.3 × 10−12
6.9 × 10−8
6.0 × 10−37
4.9 × 10−17
6.0 × 10−19
2.6 × 10−39
6.6 × 10−6
1.2 × 10−5
3.7 × 10−13
8.5 × 10−9
1.8 × 10−8
6.8 × 10−6
5.6 × 10−12
5.3 × 10−5
5.4 × 10−13
8.5 × 10−12
1.8 × 10−10
1.1 × 10−12
3.2 × 10−8
8.5 × 10−17
5.6 × 10−10
4.3 × 10−9
3.4 × 10−7
2.0 × 10−25
– 5 –
K sp
RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASESin aqueous solution at room temperature.
Name of Acid Base Acid Ka
Perchloric HClO H ClO
Hydriodic HI H I
Hydrobromic HBr H Br
Hydrochloric HCl H Cl
Nitric HNO H NO
Sulphuric H SO H HSO
Hydronium Ion H O H H O
Iodic HIO H IO
Oxalic H C O
4 4
3 3
2 4 4
3 2
3 31
2 2
1 0
1 7 10
→ +
→ +
→ +
→ +
→ +
→ +→← +→← + ×
+ −
+ −
+ −
+ −
+ −
+ −
+ +
+ − −
very large
very large
very large
very large
very large
very large
.
.
44 2 42
2 2 2 3 32
4 42 2
3 4 2 43
2 6
3
5 9 10
1 5 10
1 2 10
7 5 10
→← + ×
+( ) →← + ×→← + ×→← + ×
( ) →← +
+ − −
+ − −
− + − −
+ − −
+ +
H HC O
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 HIII
.
.
.
.
, ( ) FeFe H O OH
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 ion Cr HIII
2 52 3
3 6 5 7 2 6 5 74
2 24
4
4
6 0 10
7 1 10
4 6 10
3 5 10
1 8 10
( ) ( ) ×→← + ×→← + ×→← + ×→← + ×
+ −
+ − −
+ − −
+ − −
+ − −
.
.
.
.
, .
, ( ) 22 6
32 5
2 4
6 5 6 55
2 4 2 42 5
3 35
2 6 5
1 5 10
6 5 10
6 4 10
1 8 10
O H Cr H O OH
Benzoic C H COOH H C H COO
Hydrogen oxalate ion HC O H C O
Ethanoic acetic CH COOH H CH COO
Dihydrogen citrate ion H C H
( ) →← + ( ) ( ) ×→← + ×→← + ×→← + ×
+ + + −
+ − −
− + − −
+ − −
.
.
.
, .
OO H HC H O
Al H O H Al H O OH
H O H CO H HCO
Monohydrogen citrate ion HC H O H C H O
7 6 5 72 5
2 6
32 5
2 5
2 2 3 37
6 5 72
6 5 73
1 7 10
1 4 10
4 3 10
− + − −
+ + + −
+ − −
− + −
→← + ×
( ) →← + ( ) ( ) ×
+( ) →← + ×→← +
.
.
.
Hexaaquoaluminum ion, aluminum ion
Carbonic CO2
44 1 10
1 0 10
9 1 10
6 2 10
7 3 10
5 6 10
7
3 32 7
28
2 4 42 8
3 3 2 310
4 3
.
.
.
.
.
.
×→← + ×→← + ×→← + ×→← + ×→← + ×
−
− + − −
+ − −
− + − −
+ − −
+ +
Hydrogen sulphite ion HSO H SO
Hydrogen sulphide H S H HS
Dihydrogen phosphate ion H PO H HPO
Boric H BO H H BO
Ammonium ion NH H NH −−
+ − −
+ − −
− + − −
+ − −
− + − −
→← + ×→← + ×→← + ×→← + ×→← + ×
10
10
6 5 6 510
3 32 11
2 2 212
42
43 13
2
4 9 10
1 3 10
5 6 10
2 4 10
2 2 10
Hydrocyanic HCN H CN
Phenol C H OH H C H O
Hydrogen carbonate ion HCO H CO
Hydrogen peroxide H O H HO
Monohydrogen phosphate ion HPO H PO
Water H
.
.
.
.
.
OO H OH
Hydroxide ion OH H O very small
Ammonia NH H NH very small
→← + ×
← +
← +
+ − −
− + −
+ −
1 0 10 14
2
3 2
.
ST
RO
NG
WE
AK
ST
RO
NG
WE
AK
ST
RE
NG
TH
OF
AC
IDS
TR
EN
GT
H O
F B
AS
E
– 6 –
ACID-BASE INDICATORS
Indicator
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 –
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 WhichColour Change Occurs
Colour Changeas pH Increases
0.0 – 1.6
1.2 – 2.8
1.4 – 2.8
3.2 – 4.4
3.8 – 5.4
4.8 – 6.0
5.2 – 6.8
6.0 – 7.6
6.6 – 8.0
6.8 – 8.0
8.0 – 9.6
8.2 – 10.0
9.4 – 10.6
10.1 – 12.0
11.4 – 13.0
SO H e H SO H O
Cu e Cu
Sn e Sn
S H e H S
H e H
Pb e Pb
Sn
42
2 3 2
2
4 2
2
22
4 2 0 17
0 15
2 0 15
2 2 0 14
2 2 0 00
2 0 13
− + −
+ − +
+ − +
( )+ −
( )+ −
( )+ −
( )
+ + →← + +
+ →← +
+ →← +
+ + →← +
+ →← +
+ →← −
.
.
.
.
.
.
s g
g
s
22
2
3 4 3 3 2
2
2
3 2
2
2 0 14
2 0 26
2 2 0 28
2 0 28
2 2 0 40
0 41
2
+ −( )
+ −( )
+ −
+ −( )
( )+ −
+ − +
+ →← −
+ →← −
+ + →← + −
+ →← −
+ + →← −
+ →← −
e Sn
Ni e Ni
H PO H e H PO H O
Co e Co
Se H e H Se
Cr e Cr
H
s
s
s
s
.
.
.
.
.
.
OO e H OH M
Fe e Fe
Ag S e Ag S
Cr e Cr
Zn e Zn
Te H e H
s
+ →← + ( ) −
+ →← −
+ →← + −
+ →← −
+ →← −
+ + →←
− − −
+ −( )
( )−
( )−
+ −( )
+ −( )
( )+ −
2 2 10 0 41
2 0 45
2 2 0 69
3 0 74
2 0 76
2 2
27
2
22
3
2
2
.
.
.
.
.
s
s
s
s
s TeTe
H O e H OH
Mn e Mn
Al e Al
Mg e Mg
Na e Na
Ca e Ca
Sr
−
+ →← + −
+ →← −
+ →← −
+ →← −
+ →← −
+ →← −
+
−( )
−
+ −( )
+ −( )
+ −( )
+ −( )
+ −( )
+
0 79
2 2 2 0 83
2 1 19
3 1 66
2 2 37
2 71
2 2 87
2 22
3
2
2
2
.
.
.
.
.
.
.
g
s
s
s
s
s
22 2 89
2 2 91
2 93
2 98
3 03
3 04
2
e Sr
Ba e Ba
K e K
Rb e Rb
Cs e Cs
Li e Li
−( )
+ −( )
+ −( )
+ −( )
+ −( )
+ −( )
→← −
+ →← −
+ →← −
+ →← −
+ →← −
+ →← −
s
s
s
s
s
s
.
.
.
.
.
.
STANDARD REDUCTION POTENTIALS OF HALF-CELLSIonic concentrations are at 1M in water at 25°C.
Reducing AgentsOxidizing AgentsS
TR
ON
GW
EA
KS
TR
ON
GW
EA
K
OverpotentialEffect
OverpotentialEffect
F e F
S O e SO
H O H e H O
MnO H e Mn H O
Au e Au
BrO H e
2
2 82
42
2 2 2
42
2
3
3
2 2 2 87
2 2 2 01
2 2 2 1 78
8 5 4 1 51
3 1 50
6 5
g
s
( )− −
− − −
+ −
− + − +
+ −( )
− + −
+ →← +
+ →← +
+ + →← +
+ + →← + +
+ →← +
+ + →←
.
.
.
.
.112 2 2
4 2
2
2 72 3
2
12 2 2
2
3 1 48
8 8 4 1 39
2 2 1 36
14 6 2 7 1 23
2 2 1 23
Br H O
ClO H e Cl H O
Cl e Cl
Cr O H e Cr H O
O H e H O
MnO
l( )− + − −
( )− −
− + − +
( )+ −
(
+ +
+ + →← + +
+ →← +
+ + →← + +
+ + →← +
.
.
.
.
.
g
g
s))+ − +
− + −( )
( )− −
− −( )
−
− + −( )
+ + →← + +
+ + →← + +
+ →← +
+ →← + +
+ + →← + +
4 2 2 1 22
6 5 3 1 20
2 2 1 09
3 4 1 00
4 3 2 0
22
312 2 2
2
4
3 2
H e Mn H O
IO H e I H O
Br e Br
AuCl e Au Cl
NO H e NO H O
.
.
.
.
s
s
g
l
..
.
.
.
.
.
96
2 0 85
2 10 2 0 82
2 4 2 2 0 80
0 80
0 80
2
12 2
72
3 2 4 2
12 2
2
3
Hg e Hg
O H M e H O
NO H e N O H O
Ag e Ag
Hg e Hg
Fe e
+ −( )
( )+ − −
− + −
+ −( )
+ −( )
+
+ →← +
+ ( ) + →← +
+ + →← + +
+ →← +
+ →← +
+
l
l
g
s
−− +
( )+ −
− −( )
−
( )− −
+ −( )
+ −( )
→← +
+ + →← +
+ + →← + +
+ →← +
+ →← +
+ + →← +
Fe
O H e H O
MnO H O e MnO OH
I e I
Cu e Cu
H SO H e S H
g
2
2 2 2
4 2 2
2
2 3 2
0 77
2 2 0 70
2 3 4 0 60
2 2 0 54
0 52
4 4 3
.
.
.
.
.
s
s
s
s OO
Cu e Cu
+
+ →← ++ −( )
0 45
2 0 342
.
.s
ST
RE
NG
TH
OF
OX
IDIZ
ING
AG
EN
TS
TR
EN
GT
H O
F R
ED
UC
ING
AG
EN
TE° Volts( )
– 8 –
