Chemistry 12 PERIODIC TABLE OF THE ELEMENTS 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 1 18 2 H Hydrogen He 1.0 Helium 14 14 3 4 Li Be Silicon Silicon Lithium Beryllium 6.9 9.0 28.1 28.1 Si Si 4.0 Atomic Number Symbol Name Atomic Mass 5 6 7 8 9 10 B C N O F Ne Boron Carbon Nitrogen Oxygen Fluorine Neon 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 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 Tl 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) 109 87 88 89 104 105 106 107 108 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) Based on mass of C12 at 12.00. Data Page Values in parentheses are the masses of the most stable or best known isotopes for elements which do not occur naturally. 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 140.1 140.9 144.2 (145) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 103 90 91 92 93 94 95 96 97 98 99 100 101 102 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 232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262) 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. Element 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 Data Page Symbol Atomic Number Atomic Mass 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 89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 101 (227) 27.0 (243) 121.8 39.9 74.9 (210) 137.3 (247) 9.0 209.0 10.8 79.9 112.4 40.1 (251) 12.0 140.1 132.9 35.5 52.0 58.9 63.5 (247) (262) 162.5 (252) 167.3 152.0 (257) 19.0 (223) 157.3 69.7 72.6 197.0 178.5 4.0 164.9 1.0 114.8 126.9 192.2 55.8 83.8 138.9 (262) 207.2 6.9 175.0 24.3 54.9 (258) Element 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 Symbol Atomic Number Atomic Mass 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 80 42 60 10 93 28 41 7 102 76 8 46 15 78 94 84 19 59 61 91 88 86 75 45 37 44 104 62 21 34 14 47 11 38 16 73 43 52 65 81 90 69 50 22 74 92 23 54 70 39 30 40 200.6 95.9 144.2 20.2 (237) 58.7 92.9 14.0 (259) 190.2 16.0 106.4 31.0 195.1 (244) (209) 39.1 140.9 (145) 231.0 (226) (222) 186.2 102.9 85.5 101.1 (261) 150.4 45.0 79.0 28.1 107.9 23.0 87.6 32.1 180.9 (98) 127.6 158.9 204.4 232.0 168.9 118.7 47.9 183.8 238.0 50.9 131.3 173.0 88.9 65.4 91.2 Chemistry 12 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+ NH4+ Ammonium Li+ Lead(IV), plumbic Lithium Ba2+ Barium Mg2+ Magnesium Ca2+ Calcium Mn2+ Manganese(II), manganous Cr2+ Chromium(II), chromous Mn4+ Manganese(IV) Cr3+ Chromium(III), chromic Hg22+ Mercury(I)*, mercurous Cu+ Copper(I)*, cuprous Cu2+ Hg2+ K+ Copper(II), cupric Mercury(II), mercuric Potassium Hydrogen Ag+ Silver Hydronium Na+ Sodium Fe2+ Iron(II)*, ferrous Sn2+ Tin(II)*, stannous Fe3+ Iron(III), ferric Sn4+ Tin(IV), stannic Pb2+ Lead(II), plumbous Zn2+ Zinc Bromide OH– Hydroxide CO32– Carbonate ClO– Hypochlorite ClO3– Chlorate I– Cl– Chloride HPO42– ClO2– Chlorite NO3– Nitrate Chromate NO2– Nitrite H+ H3O+ Negative Ions (Anions) Br– CrO42– CN– Cr2O72– Dichromate H2PO4– Dihydrogen phosphate CH3COO – F– HCO3– Ethanoate, acetate C2O42– O2– ClO4– MnO4– Monohydrogen phosphate Oxalate Oxide** Perchlorate Permanganate Fluoride PO4?– Phosphate Hydrogen carbonate, bicarbonate SO42– Sulphate S2– Sulphide HC2O4– Hydrogen oxalate, binoxalate HSO4– Hydrogen sulphate, bisulphate SO32– Sulphite HS– Hydrogen sulphide, bisulphide SCN– Thiocyanate HSO3– Chemistry 12 Cyanide Iodide Hydrogen sulphite, bisulphite Data Page SOLUBILITY OF COMMON COMPOUNDS IN WATER The term soluble here means > 0.1 mol/L at 25°C. Positive Ions (Cations) Solubility of Compounds All Alkali ions: Li+, Na+, K+, Rb+, Cs+, Fr+ Soluble All Hydrogen ion: H+ Soluble All Ammonium ion: NH4+ Soluble Nitrate, NO3– All Soluble All others Soluble – Bromide, Br Sulphate, SO42– 123 Iodide, I– Sulphide, S 123 or Chloride, Cl– 2– 123 or 14243 Negative Ions (Anions) Hydroxide, OH or or Data Page 14253 – Phosphate, PO43– 2– Carbonate, CO3 Sulphite, SO32– Ag+, Pb2+, Cu+ All others Low Solubility Soluble Ag+, Ca2+, Sr2+, Ba2+, Pb2+ Alkali ions, H+, NH4+, Be2+, Mg2+, Ca2+, Sr2+, Ba2+ Low Solubility Soluble All others Alkali ions, H+, NH4+, Sr2+ ? Low Solubility Soluble Low Solubility All others Alkali ions, H+, NH4+ All others Soluble Low Solubility Chemistry 12 SOLUBILITY PRODUCT CONSTANTS AT 25°C Chemistry 12 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 CaC2O4 2.3 10–9 Calcium sulphate CaSO4 7.1 10–5 Copper(I) iodide CuI 1.3 10–12 Copper(II) iodate Cu(IO3)2 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 Pb(IO3)2 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 Ag2CO3 8.5 10–12 Silver chloride AgCl 1.8 10–10 Silver chromate Ag2CrO4 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 SrSO4 3.4 10–7 Zinc sulphide ZnS 2.0 10–25 Data Page RELATIVE STRENGTHS OF BRØNSTED-LOWRY ACIDS AND BASES in aqueous solution at room temperature. STRONG Name of Acid Iodic Oxalic H2C2O4 H 2 SO 3 Hydrogen sulphate ion HSO 4 − Phosphoric H 3 PO 4 Citric Nitrous Hydrofluoric Methanoic, formic Fe(H 2 O)6 3 + H 3C 6 H 5 O 7 HNO 2 HF HCOOH Hexaaquochromium ion, chromium( III ) ion Cr(H 2 O)6 3 + Benzoic C 6 H 5COOH Hydrogen oxalate ion Ethanoic, acetic HC 2 O 4 − CH 3COOH Dihydrogen citrate ion H 2 C 6 H 5O 7 − Hexaaquoaluminum ion, aluminum ion Al(H 2 O)6 3 + Carbonic (CO 2 + H 2 O) Monohydrogen citrate ion Hydrogen sulphite ion Hydrogen sulphide Dihydrogen phosphate ion Boric Ammonium ion Hydrocyanic Phenol Hydrogen carbonate ion H 2 CO 3 HC 6 H 5O 7 2 − HSO 3 − H 2S H 2 PO 4 − H 3 BO 3 NH 4 + HCN C 6 H 5OH HCO 3 − → → → → → → → ← H+ H+ H+ H+ H+ H+ H+ Ka + ClO 4 − + I− + Br − + Cl − + NO 3 − + HSO 4 − + H2O − + → ← H + IO 3 − + → ← H + HC 2 O 4 − + → ← H + HSO 6.0 × 10 − 3 7.1 × 10 − 4 + 2+ → ← H + Cr(H 2 O)5 (OH) + − → ← H + C 6 H 5COO 2− + → ← H +C O 1.5 × 10 − 4 2 3.5 × 10 − 4 1.8 × 10 − 4 4 6.5 × 10 − 5 6.4 × 10 − 5 + − → ← H + CH 3COO 2− + → ← H + HC 6 H 5O 7 + 2+ → ← H + Al(H O) (OH) 1.8 × 10 − 5 − + → ← H + HCO 3 3− + → ← H + C 6 H 5O 7 → H + + SO 2 − ← 3 + − → ← H + HS → H + + HPO 2 − ← 4 − + → H + H BO ← 2 3 + → ← H + NH 4.3 × 10 − 7 2 3 − 5 1.7 × 10 − 5 1.4 × 10 − 5 4.1 × 10 − 7 1.0 × 10 − 7 9.1 × 10 − 8 6.2 × 10 − 8 7.3 × 10 −10 5.6 × 10 −10 + → ← H + CN + − → ← H + C 6 H 5O 2− + → ← H + CO 4.9 × 10 −10 2.4 × 10 −12 3 ← H + + O2 − NH 3 + ← H + NH 2 1.3 × 10 −10 5.6 × 10 −11 2.2 × 10 −13 1.0 × 10 −14 very small − very small STRONG OH − Data Page 7.5 × 10 − 3 4.6 × 10 − 4 Hydroxide ion Ammonia 7 1.2 × 10 − 2 → H + + NO ← 2 + − → H + F ← + − → ← H + HCOO H2O HPO 4 2 − 1.5 × 10 − 2 6 5 − Water Monohydrogen phosphate ion H2O2 5.9 × 10 − 2 + → ← H + SO 4 − + → ← H + H 2 PO 4 + 2+ → ← H + Fe(H 2 O)5 (OH) − + → ← H +H C H O 2 large large large large large large 1.7 × 10 −1 3 2− → H + + HO − ← 2 3− + → H + PO ← 4 + − → ← H + OH Hydrogen peroxide very very very very very very 1.0 STRENGTH OF BASE STRENGTH OF ACID HIO 3 Sulphurous (SO 2 + H 2 O) Hexaaquoiron ion, iron( III ) ion WEAK HClO 4 HI HBr HCl HNO 3 H 2 SO 4 H 3O + Base WEAK Perchloric Hydriodic Hydrobromic Hydrochloric Nitric Sulphuric Hydronium Ion Acid Chemistry 12 ACID-BASE INDICATORS Indicator Chemistry 12 pH Range in Which Colour Change Occurs Colour Change 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 Data Page STANDARD REDUCTION POTENTIALS OF HALF-CELLS Ionic concentrations are at 1M in water at 25°C. Oxidizing Agents F2 (g) + 2 e − STRONG + 2e − H 2 O 2 + 2H + + 2e − MnO 4 − + 8H + + 5e − Au 3+ + 3e − BrO 3 − + 6H + + 5e − ClO 4 − + 8H + + 8e − Cl 2 (g) + 2 e − Cr2 O 7 2 − + 14H + + 6e − 1 2 O 2 (g) + 2 H + + 2 e − MnO 2 (s) + 4H + + 2 e − IO 3 − + 6H + + 5e − Br2 (l) + 2 e − AuCl 4 − + 3e − NO 3 − + 4H + + 3e − Hg 2 + + 2 e − 1 2 O 2 (g) + 2 H + (10 −7 M ) + 2 e − 2 NO 3 − + 4H + + 2 e − Ag + + e − 1 2 Hg 2 2 + + e − STRENGTH OF OXIDIZING AGENT O 2 (g) + 2 H + + 2 e − MnO 4 − + 2 H 2 O + 3e − I 2 (s) + 2 e − Cu + + e − H 2 SO 3 + 4H + + 4e − Cu 2 + + 2 e − SO 4 2 − + 4H + + 2 e − Cu 2+ +e − Sn 4 + + 2 e − S(s) + 2 H + + 2 e − 2H + + 2e − Pb 2 + + 2 e − Sn 2 + + 2 e − Ni 2 + + 2 e − H 3 PO 4 + 2 H + + 2 e − Co 2 + + 2 e − Se(s) + 2 H + + 2 e − Cr 3+ + e − 2H 2 O + 2e − Overpotential Effect Fe 2+ + 2e − Ag 2 S(s) + 2 e − Cr 3+ + 3e − Zn 2 + + 2 e − Te(s) + 2 H + + 2 e − 2H 2 O + 2e − Mn 2 + + 2 e − Al 3+ + 3e − Mg 2 + + 2 e − → Mn + 4H O ← 2 → ← Au(s) 1 → Br (l) + 3H O ← +1.51 + 2.01 +1.78 2 2+ +1.50 2 +1.48 − → ← Cl + 4H 2 O − → ← 2Cl 3+ → ← 2Cr + 7H O +1.36 2 2 2 → ← H2O 2+ → ← Mn + 2 H 2 O 1 → I (s) + 3H O ← 2 2 2 − → ← 2 Br → ( ) + 4Cl − Au s ← → ( ) + 2H O NO g ← 2 → ← Hg(l) → ← H2O → ← N 2 O 4 + 2H 2 O → Ag(s) ← → ← Hg(l) 2+ → ← Fe +1.39 +1.23 +1.23 +1.22 +1.20 +1.09 +1.00 + 0.85 + 0.82 + 0.80 + 0.80 + 0.80 + 0.77 → ← H2O2 − → ← MnO 2 (s) + 4OH − → ← 2I + 0.70 → ← Cu(s) → ← S(s) + 3H 2 O → ← Cu(s) + 0.52 → ← H 2 SO 3 + H 2 O + → ← Cu 2+ → Sn ← + 0.17 + 0.60 + 0.54 + 0.45 + 0.34 + 0.15 + 0.15 → ← H 2 S(g) → ← H 2 (g) → ← Pb(s) + 0.14 → ← Sn(s) → ← Ni(s) → H PO + H O ← 3 3 2 → ← Co(s) → ← H Se − 0.14 2 2+ + 0.00 − 0.13 − 0.26 − 0.28 − 0.28 − 0.40 → ← Cr − −7 → ← H 2 + 2 OH (10 M ) − 0.41 → ← Fe(s) 2− → ← 2 Ag(s) + S → ← Cr(s) − 0.45 → ← Zn(s) → ← H 2 Te − → ← H (g) + 2 OH − 0.76 → ← Mn(s) → ← Al(s) → ← Mg(s) −1.19 2 − 0.41 − 0.69 − 0.74 − 0.79 − 0.83 −1.66 − 2.37 − 2.93 Cs + + e − → ← K(s) → ← Rb(s) → ← Cs(s) − 3.03 Li + + e − → ← Li(s) − 3.04 2+ + 2e − Ba 2 + + 2 e − K+ + e− Rb + + e − − 2.87 − 2.89 − 2.91 − 2.98 STRONG Sr 2 + + 2 e − Overpotential Effect + 0.96 − 2.71 Ca WEAK + 2.87 → ← Na(s) → ← Ca(s) → ← Sr(s) → ← Ba(s) Na + + e − Data Page − → ← 2F 2− → ← 2SO 4 → ← 2H O STRENGTH OF REDUCING AGENT Fe 3+ + e − E° (Volts) WEAK S2 O 8 2− Reducing Agents Chemistry 12