Chem 12 data booklet
- 1. Data Booklet CHEMISTRY 12 Work done in this booklet will not be marked. © Ministry of Education Revised January 2000
- 2. 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 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.
- 3. PERIODIC TABLE OF THE ELEMENTS 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 1 H 2 Hydrogen He Helium 1.0 4.0 14 Atomic Number 3 4 Si Symbol 5 6 7 8 9 10 Li Be Silicon Name B C N O F Ne Lithium Beryllium 28.1 Atomic Mass Boron Carbon Nitrogen Oxygen Fluorine Neon 6.9 9.0 10.8 12.0 14.0 16.0 19.0 20.2 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar Sodium Magnesium Aluminum Silicon Phosphorus Sulphur Chlorine Argon 23.0 24.3 27.0 28.1 31.0 32.1 35.5 39.9 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton 39.1 40.1 45.0 47.9 50.9 52.0 54.9 55.8 58.9 58.7 63.5 65.4 69.7 72.6 74.9 79.0 79.9 83.8 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe –1– Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon 85.5 87.6 88.9 91.2 92.9 95.9 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Ti Pb Bi Po At Rn Cesium Barium Lanthanum Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury Thallium Lead Bismuth Polonium Astatine Radon 132.9 137.3 138.9 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) (222) 87 88 89 104 105 106 107 108 109 Fr Ra Ac Rf Db Sg Bh Hs Mt Francium Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium (223) (226) (227) (261) (262) (263) (262) (265) (266) 58 59 60 61 62 63 64 65 66 67 68 69 70 71 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Based on mass of C12 at 12.00. 140.1 140.9 144.2 (145) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 Values in parentheses 90 91 92 93 94 95 96 97 98 99 100 101 102 103 are the masses of the most Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium stable or best known isotopes for elements which do not occur naturally. 232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262)
- 4. ATOMIC MASSES OF THE ELEMENTS Based on mass of C12 at 12.00. Values in parentheses are the mass number of the most stable or best known isotopes for elements that do not occur naturally. Atomic Atomic Atomic Atomic Element Symbol Element Symbol Number Mass Number Mass Actinium Ac 89 (227) Mercury Hg 80 200.6 Aluminum Al 13 27.0 Molybdenum Mo 42 95.9 Americium Am 95 (243) Neodymium Nd 60 144.2 Antimony Sb 51 121.8 Neon Ne 10 20.2 Argon Ar 18 39.9 Neptunium Np 93 (237) Arsenic As 33 74.9 Nickel Ni 28 58.7 Astatine At 85 (210) Niobium Nb 41 92.9 Barium Ba 56 137.3 Nitrogen N 7 14.0 Berkelium Bk 97 (247) Nobelium No 102 (259) Beryllium Be 4 9.0 Osmium Os 76 190.2 Bismuth Bi 83 209.0 Oxygen O 8 16.0 Boron B 5 10.8 Palladium Pd 46 106.4 Bromine Br 35 79.9 Phosphorus P 15 31.0 Cadmium Cd 48 112.4 Platinum Pt 78 195.1 Calcium Ca 20 40.1 Plutonium Pu 94 (244) Californium Cf 98 (251) Polonium Po 84 (209) Carbon C 6 12.0 Potassium K 19 39.1 Cerium Ce 58 140.1 Praseodymium Pr 59 140.9 Cesium Cs 55 132.9 Promethium Pm 61 (145) Chlorine Cl 17 35.5 Protactinium Pa 91 231.0 Chromium Cr 24 52.0 Radium Ra 88 (226) Cobalt Co 27 58.9 Radon Rn 86 (222) Copper Cu 29 63.5 Rhenium Re 75 186.2 Curium Cm 96 (247) Rhodium Rh 45 102.9 Dubnium Db 105 (262) Rubidium Rb 37 85.5 Dysprosium Dy 66 162.5 Ruthenium Ru 44 101.1 Einsteinium Es 99 (252) Rutherfordium Rf 104 (261) Erbium Er 68 167.3 Samarium Sm 62 150.4 Europium Eu 63 152.0 Scandium Sc 21 45.0 Fermium Fm 100 (257) Selenium Se 34 79.0 Fluorine F 9 19.0 Silicon Si 14 28.1 Francium Fr 87 (223) Silver Ag 47 107.9 Gadolinium Gd 64 157.3 Sodium Na 11 23.0 Gallium Ga 31 69.7 Strontium Sr 38 87.6 Germanium Ge 32 72.6 Sulphur S 16 32.1 Gold Au 79 197.0 Tantalum Ta 73 180.9 Hafnium Hf 72 178.5 Technetium Tc 43 (98) Helium He 2 4.0 Tellurium Te 52 127.6 Holmium Ho 67 164.9 Terbium Tb 65 158.9 Hydrogen H 1 1.0 Thallium Tl 81 204.4 Indium In 49 114.8 Thorium Th 90 232.0 Iodine I 53 126.9 Thulium Tm 69 168.9 Iridium Ir 77 192.2 Tin Sn 50 118.7 Iron Fe 26 55.8 Titanium Ti 22 47.9 Krypton Kr 36 83.8 Tungsten W 74 183.8 Lanthanum La 57 138.9 Uranium U 92 238.0 Lawrencium Lr 103 (262) Vanadium V 23 50.9 Lead Pb 82 207.2 Xenon Xe 54 131.3 Lithium Li 3 6.9 Ytterbium Yb 70 173.0 Lutetium Lu 71 175.0 Yttrium Y 39 88.9 Magnesium Mg 12 24.3 Zinc Zn 30 65.4 Manganese Mn 25 54.9 Zirconium Zr 40 91.2 Mendelevium Md 101 (258) –2–
- 5. NAMES, FORMULAE, AND CHARGES OF SOME COMMON IONS * Aqueous solutions are readily oxidized by air. ** Not stable in aqueous solutions. Positive Ions (Cations) Al3+ Aluminum Pb4+ Lead(IV), plumbic NH4+ Ammonium Li+ Lithium Ba2+ Barium Mg2+ Magnesium Ca2+ Calcium Mn2+ Manganese(II), manganous Cr2+ Chromium(II), chromous Mn4+ Manganese(IV) Cr3+ Chromium(III), chromic Hg 22+ Mercury(I)*, mercurous Cu + Copper(I)*, cuprous Hg2+ Mercury(II), mercuric Cu2+ Copper(II), cupric K+ Potassium H+ Hydrogen Ag+ Silver H 3 O+ Hydronium Na+ Sodium Fe 2+ Iron(II)*, ferrous Sn2+ Tin(II)*, stannous Fe 3+ Iron(III), ferric Sn4+ Tin(IV), stannic Pb 2+ Lead(II), plumbous Zn2+ Zinc Negative Ions (Anions) Br − Bromide OH− Hydroxide CO3 2− Carbonate ClO− Hypochlorite ClO3 − Chlorate I− Iodide Cl − Chloride HPO 42− Monohydrogen phosphate ClO2 − Chlorite NO3− Nitrate CrO4 2− Chromate NO2− Nitrite CN − Cyanide C 2O 42− Oxalate Cr 2O7 2− Dichromate O 2− Oxide** H2 PO4 − Dihydrogen phosphate ClO4− Perchlorate CH3 COO − Ethanoate, acetate MnO4− Permanganate F− Fluoride PO 43− Phosphate HCO3 − Hydrogen carbonate, bicarbonate SO 42− Sulphate HC2O 4 − Hydrogen oxalate, binoxalate S2− Sulphide HSO4 − Hydrogen sulphate, bisulphate SO 32− Sulphite HS − Hydrogen sulphide, bisulphide SCN− Thiocyanate HSO3 − Hydrogen sulphite, bisulphite –3–
- 6. SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/L at 25°C. Negative Ions Positive Ions Solubility of (Anions) (Cations) Compounds All Alkali ions: Li+ , Na + , K + , Rb + , Cs + , Fr + Soluble All Hydrogen ion: H + Soluble All Ammonium ion: NH 4 + Soluble Nitrate, NO3 − All Soluble Chloride,Cl − All others Soluble or − Bromide, Br or Iodide, I − Ag+ , Pb 2+ , Cu + Low Solubility All others Soluble Sulphate, SO4 2− Ag+ , Ca 2+ , Sr 2+ , Ba2+ , Pb2+ Low Solubility Alkali ions, H + , NH 4 + , Be2+ , Mg2+ , Ca2+ , Sr2+ , Ba2+ Soluble Sulphide, S2− All others Low Solubility Alkali ions, H + , NH 4 + , Sr 2+ Soluble Hydroxide, OH − All others Low Solubility Phosphate, PO4 3− Alkali ions, H + , NH 4 + Soluble or Carbonate, CO32− or Sulphite, SO3 2− All others Low Solubility –4–
- 7. SOLUBILITY PRODUCT CONSTANTS AT 25°C Name Formula K sp Barium carbonate BaCO3 2.6 × 10 −9 Barium chromate BaCrO4 1.2 × 10−10 Barium sulphate BaSO4 1.1 × 10 −10 Calcium carbonate CaCO3 5.0 × 10 −9 Calcium oxalate CaC2 O4 2.3 × 10−9 Calcium sulphate CaSO4 7.1 × 10−5 Copper(I) iodide CuI 1.3 × 10 −12 Copper(II) iodate ( )2 Cu IO 3 6.9 × 10 −8 Copper(II) sulphide CuS 6.0 × 10 −37 Iron(II) hydroxide Fe OH( )2 4.9 × 10−17 Iron(II) sulphide FeS 6.0 × 10 −19 Iron(III) hydroxide Fe OH( )3 2.6 × 10 −39 Lead(II) bromide PbBr2 6.6 × 10 −6 Lead(II) chloride PbCl2 1.2 × 10−5 Lead(II) iodate ( )2 Pb IO3 3.7 × 10−13 Lead(II) iodide PbI2 8.5 × 10−9 Lead(II) sulphate PbSO4 1.8 × 10−8 Magnesium carbonate MgCO3 6.8 × 10 −6 Magnesium hydroxide ( ) Mg OH 2 5.6 × 10 −12 Silver bromate AgBrO3 5.3 × 10−5 Silver bromide AgBr 5.4 × 10 −13 Silver carbonate Ag2 CO3 8.5 × 10−12 Silver chloride AgCl 1.8 × 10−10 Silver chromate Ag2 CrO4 1.1 × 10 −12 Silver iodate AgIO3 3.2 × 10 −8 Silver iodide AgI 8.5 × 10−17 Strontium carbonate SrCO3 5.6 × 10 −10 Strontium fluoride SrF2 4.3 × 10 −9 Strontium sulphate SrSO 4 3.4 × 10 −7 Zinc sulphide ZnS 2.0 × 10 −25 –5–
- 8. RELATIVE STRENGTHS OF BR¯NSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature. Name of Acid Acid Base Ka Perchloric HClO 4 → H + + ClO 4 − very large STRONG + − Hydriodic HI → H +I very large + − Hydrobromic HBr → H + Br very large + − Hydrochloric HCl → H + Cl very large + − Nitric HNO 3 → H + NO 3 very large + − Sulphuric H 2 SO 4 → H + HSO 4 very large Hydronium Ion H 3O + → H + + H 2 O ← 1.0 WEAK Iodic HIO → H + + IO − ←3 3 1.7 × 10 −1 Oxalic H 2 C 2 O 4 → H + + HC 2 O 4 − ← 5.9 × 10 − 2 Sulphurous (SO 2 + H 2 O) H 2 SO 3 ← → H + + HSO − 3 1.5 × 10 − 2 − → + 2− Hydrogen sulphate ion HSO 4← H + SO 4 1.2 × 10 − 2 Phosphoric H 3 PO 4 → H + + H 2 PO 4 − ← 7.5 × 10 − 3 Fe(H 2 O)6 ← H + Fe(H 2 O)5 (OH) 3+ → + 2+ Hexaaquoiron ion, iron( III ) ion 6.0 × 10 − 3 Citric H 3C 6 H 5 O 7 → H + + H 2 C 6 H 5O 7 − ← 7.1 × 10 − 4 Nitrous HNO → H + + NO − ← 2 2 4.6 × 10 − 4 STRENGTH OF ACID Hydrofluoric HF → H + + F − ← 3.5 × 10 − 4 Methanoic, formic HCOOH → H + + HCOO − ← 1.8 × 10 − 4 Cr(H 2 O)6 → H + + Cr(H O) (OH)2 + 3+ Hexaaquochromium ion, chromium( III ) ion ← 2 5 1.5 × 10 − 4 Benzoic C H COOH ← → H + + C H COO − 6.5 × 10 − 5 STRENGTH OF BASE 6 5 6 5 Hydrogen oxalate ion HC 2 O 4 − → H + + C 2 O 4 2 − ← 6.4 × 10 − 5 Ethanoic, acetic CH 3COOH ← → H + + CH COO − 1.8 × 10 − 5 3 − → + 2− Dihydrogen citrate ion H C H O 2 6 5 ← H + HC H O 7 6 5 7 1.7 × 10 − 5 Al(H 2 O)6 H + + Al(H 2 O)5 (OH)2 + 3+ → Hexaaquoaluminum ion, aluminum ion ← 1.4 × 10 − 5 Carbonic (CO 2 + H 2 O) H 2 CO 3 → ← H + + HCO 3 − 4.3 × 10 − 7 HC 6 H 5O 7 2 − → H + + C 6 H 5O 7 3 − 4.1 × 10 − 7 Monohydrogen citrate ion ← Hydrogen sulphite ion HSO 3 − → ← H + + SO 3 2 − 1.0 × 10 − 7 Hydrogen sulphide H 2 S → H + + HS− ← 9.1 × 10 − 8 − → + 2− Dihydrogen phosphate ion H 2 PO 4 ← H + HPO 4 6.2 × 10 − 8 Boric H BO → H + + H BO − 3 ← 3 2 3 7.3 × 10 −10 → H + + NH + 5.6 × 10 −10 Ammonium ion NH 4 ← 3 Hydrocyanic HCN ←→ H + + CN − 4.9 × 10 −10 Phenol C 6 H 5OH → H + + C 6 H 5O − ← 1.3 × 10 −10 Hydrogen carbonate ion HCO − → H + + CO 2 − ←3 3 5.6 × 10 −11 Hydrogen peroxide H 2 O 2 → H + + HO 2 − ← 2.4 × 10 −12 WEAK 2− → + 3− Monohydrogen phosphate ion HPO 4 ← H + PO 4 2.2 × 10 −13 STRONG Water H O → H + + OH − ←2 1.0 × 10 −14 Hydroxide ion OH − ← H + + O 2 − very small + − Ammonia NH 3 ← H + NH 2 very small Ð6Ð
- 9. ACID-BASE INDICATORS pH Range in Which Colour Change Indicator Colour Change Occurs as pH Increases Methyl violet 0.0 – 1.6 yellow to blue Thymol blue 1.2 – 2.8 red to yellow Orange IV 1.4 – 2.8 red to yellow Methyl orange 3.2 – 4.4 red to yellow Bromcresol green 3.8 – 5.4 yellow to blue Methyl red 4.8 – 6.0 red to yellow Chlorophenol red 5.2 – 6.8 yellow to red Bromthymol blue 6.0 – 7.6 yellow to blue Phenol red 6.6 – 8.0 yellow to red Neutral red 6.8 – 8.0 red to amber Thymol blue 8.0 – 9.6 yellow to blue Phenolphthalein 8.2 – 10.0 colourless to pink Thymolphthalein 9.4 – 10.6 colourless to blue Alizarin yellow 10.1 – 12.0 yellow to red Indigo carmine 11.4 – 13.0 blue to yellow –7–
- 10. STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic concentrations are at 1M in water at 25°C. Oxidizing Agents Reducing Agents E° (Volts ) F2( g ) + 2 e − → 2 F − ← + 2.87 S2 O 8 2 − + 2 e − → 2SO 4 2 − WEAK ← + 2.01 STRONG H 2 O 2 + 2H + + 2e − → 2H 2 O ← +1.78 MnO 4 − + 8H + + 5e − → Mn 2 + + 4 H 2 O ← +1.51 Au 3 + + 3e − → Au ( s ) ← +1.50 BrO 3 − + 6H + + 5e − → 1 Br2(l ) + 3H 2 O ← 2 +1.48 ClO 4 − + 8H + + 8e − → Cl − + 4 H 2 O ← +1.39 Cl + 2 e − → 2Cl − 2( g )← +1.36 Cr2 O 7 2 − + 14 H + 6e − → 2Cr 3 + + 7H 2 O ← + +1.23 1 2O + 2H + + 2e − → H O 2( g ) ← 2 +1.23 MnO 2( s ) + 4 H + + 2 e − → Mn 2 + + 2 H 2 O ← +1.22 IO 3 − + 6H + + 5e − → 1 I 2( s ) + 3H 2 O ← 2 +1.20 Overpotential Br2(l ) + 2 e − → 2 Br − ← +1.09 Effect AuCl 4 − + 3e − → Au ( s ) + 4Cl − ← +1.00 NO 3 + 4 H + + 3e − → NO ( g ) + 2 H 2 O − ← + 0.96 Hg 2 + + 2 e − → Hg (l ) ← + 0.85 1 + ( −7 2 O 2 ( g ) + 2 H 10 M + 2 e ) − → ← H2O + 0.82 2 NO − + 4 H + + 2 e − → N O + 2 H O 3 ← 2 4 2 + 0.80 Ag + + e − → Ag ( s ) ← + 0.80 1 2 Hg 2 2+ + e − → Hg (l ) ← + 0.80 Fe 3 + + e − → Fe 2 + STRENGTH OF REDUCING AGENT ← + 0.77 STRENGTH OF OXIDIZING AGENT O 2( g ) + 2 H + + 2e − → H 2 O 2 ← + 0.70 MnO 4 − + 2 H 2 O + 3e − → MnO 2( s ) + 4OH − ← + 0.60 I 2( s ) + 2e − → 2 I − ← + 0.54 Cu + + e − → Cu ( s ) ← + 0.52 H SO + 4 H + + 4e − → S + 3H O 2 3 ← (s) 2 + 0.45 Cu 2 + + 2 e − → Cu ( s ) ← + 0.34 SO 4 2 − + 4 H + + 2 e − → H 2 SO 3 + H 2 O ← + 0.17 Cu 2 + + e − → Cu + ← + 0.15 Sn + 2 e → 4+ − ← Sn 2 + + 0.15 S( s ) + 2 H + + 2 e − → ← H 2 S( g ) + 0.14 2H + + 2e − → ← H 2( g ) + 0.00 Pb 2 + + 2 e − → ← Pb ( s ) − 0.13 Sn 2 + + 2 e − → Sn ( s ) ← − 0.14 Ni 2 + + 2 e − → Ni ( s ) ← − 0.26 H 3 PO 4 + 2 H + + 2 e − → H 3 PO 3 + H 2 O ← − 0.28 Co 2 + + 2 e − → Co ( s ) ← − 0.28 Se ( s ) + 2 H + + 2 e − → H 2 Se ← − 0.40 Cr 3 + + e − → Cr 2 + ← − 0.41 2 H 2 O + 2 e − → H 2 + 2OH − 10 −7 M ← ( ) − 0.41 Fe 2 + + 2 e − → Fe ← (s) − 0.45 Overpotential Ag 2 S( s ) + 2 e − → 2 Ag (s) + S2 − ← − 0.69 Effect Cr 3 + + 3e − → Cr( s ) − 0.74 ← Zn 2 + + 2 e − → Zn ← (s) − 0.76 Te ( s ) + 2 H + + 2 e − → H 2 Te ← − 0.79 2H O + 2e − → H 2 ← + 2OH − 2( g ) − 0.83 Mn 2+ + 2 e − → Mn ( s ) ← −1.19 Al + 3e − → Al 3+ ← (s) −1.66 Mg 2 + + 2 e − → Mg ( s ) ← − 2.37 Na + + e − → Na ← (s) − 2.71 Ca 2 + + 2 e − → Ca ( s ) ← − 2.87 Sr 2 + + 2 e − → Sr(s) ← − 2.89 STRONG Ba 2 + + 2 e − → Ba ← (s ) − 2.91 K + + e − → K (s ) ← − 2.93 WEAK Rb + + e − → Rb (s) ← − 2.98 Cs + + e − → Cs ← (s) − 3.03 Li + + e − → Li ( s ) ← − 3.04 Ð8Ð