Data for General, Organic, and Physical Chemistry

Transcript

1 Data for General, Organic, and Physical Chemistry Copyright 1989 by C.D. Schaeffer, Jr. (Elizabethtown College) C.A. Strausser, M.W. Thomsen, and C.H. Yoder (Franklin & Marshall College) Table of Contents 1. The Elements: Symbols, Atomic Numbers, Atomic Weights, and Pauling Electronegativities 2. Constants and Conversion Factors 3. Standard Enthalpies of Formation of Gaseous Atoms 4. Ionization Energies of Gaseous Atoms 5. Electron Affinities 6. Common Bond Energies and Bond Lengths 7. Standard Heats and Free Energies of Formation, and Absolute Entropies A. Elements and Inorganic Compounds B. Organic Compounds 8. Standard Heats of Formation for Gaseous Complex Ions 9. Lattice Energy A. Madelung Constants (A) for Common Crystal Lattices B. Values of Born Exponent to be Used in Repulsive Function for Lattice Energy C. Lattice Energies (E) for Common Compounds D. Kapustinskii Equation 10. Contributions to Entropies of Solids at 298 K A. Cation Contributions, J/mol K B. Anion Contributions, J/mol K 11. Group Contributions to H f o (g) and S o (g) at 298 K A. Hydrocarbon Groups B. Corrections for Steric Interactions and Rings C. Oxygen-Containing Groups D. Nitrogen-Containing Groups E. Halogen-Containing Groups 12. Metallic, Covalent and Ionic Radii 13. Thermochemical Radii A. Anions B. Cations 14. Standard Formation Data for Aqueous Ions A. Cations B. Anions 15. Absolute Enthalpies of Hydration of Gaseous Ions 16. Solubilities of Gases in Water at 293 K 17. Solubilities of Inorganic Compounds in Water at 293 K 18. Solubility Product Constants, Ksp 19. Acid and Base Dissociation Constants in Water at 298 K A. Acid Constants B. Base Constants 20. Overall Formation Constants of Coordination Compounds 21. Vapor Pressure of Water from 0 o C to 100 o C 22. Hammett Sigma Constants 23. Standard Electrode Potentials A. Acidic Media B. Basic Media 24. Acid-Base Indicators 25. Oxidation-Reduction Indicators 26. Physical Characteristics of Solvents 27. Molal Freezing and Boiling Point Constants 28. Additivity Rules for π-π* Transitions of Enones 29. Characteristic Infrared Absorptions 30. Properties of NMR-Active Nuclei A. I = 1/2 Nuclei B. I > 1/2 Nuclei 31. Common NMR Solvents 32. Carbon-13 Chemical Shift Increments for Substituted Alkanes 33. Carbon-13 Chemical Shifts of Carbonyl Derivatives 34. Additivity Parameters for Carbon-13 Chemical Shifts in Some Substituted Benzenes 35. Proton, Carbon-13 and Nitrogen Chemical Shift Ranges A. Proton B. Carbon-13 C. Nitrogen 36. Character Tables for Common Symmetry Groups A. The Nonaxial Groups B. The C n Groups C. The D n Groups D. The C nv Groups E. The C nh Groups F. The D nh Groups G. The D nd Groups H. The S n Groups I. The Cubic Groups 37. Molecular parameters 38. References

2 Table 1. The Elements: Symbols, Atomic Numbers (Z), Atomic Weights (At. Wt), and Pauling Electronegativities (c) Element Symbol Z Atomic Weight χ Actinium Ac 89 (227) 1.1 Aluminum Al Americium Am 95 (243) 1.3 Antimony Sb Argon Ar Arsenic As Astatine At 85 (210) 2.2 Barium Ba Berkelium Bk 97 (247) 1.3 Beryllium Be Bismuth Bi Boron B Bromine Br Cadmium Cd Calcium Ca Californium Cf 98 (251) 1.3 Carbon C Cerium Ce Cesium Cs Chlorine Cl Chromium Cr Cobalt Co Copper Cu Curium Cm 96 (247) 1.3 Dysprosium Dy Einsteinium Es 99 (254) 1.3 Erbium Er Europium Eu Fermium Fm 100 (257) 1.3 Fluorine F Francium Fr 87 (223) 0.7 Gadolinium Gd Gallium Ga Germanium Ge Gold Au Hafnium Hf Helium He Holmium Ho Hydrogen H Indium In Iodine I Iridium Ir Iron Fe Krypton Kr Lanthanum La Lawrencium Lr 103 (256) Lead Pb Lithium Li Lutetium Lu Magnesium Mg Manganese Mn Mendelevium Md 101 (258) 1.3 Mercury Hg Molybdenum Mo Neodymium Nd Neon Ne Neptunium Np Nickel Ni Niobium Nb Nitrogen N Nobelium No 102 (255) 1.3 Osmium Os Oxygen O Palladium Pd Phosphorus P Platinum Pt Plutonium Pu 94 (244) 1.3 Polonium Po 84 (210) 2.0 Potassium K Praseodymium Pr Promethium Pm 61 (147) 1.1 Protactinium Pa Radium Ra Radon Rn 86 (222) Rhenium Re Rhodium Rh Rubidium Rb Ruthenium Ru Rutherfordium Rf 104 (261) Samarium Sm Scandium Sc Selenium Se Silicon Si Silver Ag Sodium Na Strontium Sr Sulfur S Tantalum Ta Technetium Tc Tellurium Te Terbium Tb Thallium Tl Thorium Th Thulium Tm Tin Sn Titanium Ti Tungsten W Uranium U Vanadium V Xenon Xe Ytterbium Yb Yttrium Y Zinc Zn Zirconium Zr

3 Table 2. Constants and Conversion Factors Constants Constants Avogadro constant, N A x mol -1 Faraday constant, F 96,485 C mol -1 Faraday constant, F 96.5 kj mol -1 Proton charge, e Proton charge, e Electron mass, me Planck constant, h Speed of light, c Gas constant, R Boltzmann constant, k x C 4.80 x esu 9.11 x g x J s x 10 8 m/s J/mol K x J/K Pi Conversion Factors Natural logarithm base, e = kj = x kcal kcal = 23.1 x ev kcal = 2.39 x x erg 1 esu 2 /cm = 1 erg ln y = x log y 1 ev = kj/mol 1 cm -1 = kj/mol 1 atm = 101,325 Pa = 760 torr 1 Å (angstrom) = m = 100 pm 1 amu = 1.66 x g

4 Table 3. Standard Enthalpies of Formation of Gaseous Atoms Atom H f o (g) kj/mol Atom H f o (g) kj/mol Atom Actinium 385 Holmium 301 Radium 159 Aluminum 326 Hydrogen 218 Radon 0 Antimony 262 Indium 243 Rhenium 770 Argon 0 Iodine 107 Rhodium 556 Arsenic 302 Iridium 665 Rubidium 86 Astatine 92 Iron 418 Ruthenium 643 Barium 180 Krypton 0 Samarium 205 Beryllium 324 Lanthanum 423 Scandium 378 Bismuth 207 Lead 196 Selenium 227 Boron 573 Lithium 161 Silicon 452 Bromine 112 Lutecium 426 Silver 284 Cadmium 112 Magnesium 148 Sodium 109 Calcium 178 Manganese 281 Strontium 164 Carbon 717 Mercury 61 Sulfur 279 Cerium 422 Molybdenum 658 Tantalum 782 Cesium 79 Neodymium 322 Technetium 677 Chlorine 121 Neon 0 Tellurium 197 Chromium 397 Neptunium 439 Terbium 389 Cobalt 425 Nickel 430 Thallium 182 Copper 338 Niobium 726 Thorium 576 Dysprosium 297 Nitrogen 473 Thulium 230 Erbium 318 Osmium 791 Tin 302 Europium 176 Oxygen 249 Titanium 470 Fluorine 79 Palladium 378 Tungsten 849 Francium 92 Phosphorus 315 Uranium 490 Gadolinium 397 Platinum 565 Vanadium 514 Gallium 286 Polonium 144 Xenon 0 Germanium 377 Potassium 90 Ytterbium 150 Gold 366 Praseodymium 355 Ytterium 423 Hafnium 619 Protactinium 527 Zinc 131 Helium 0 Radium 159 Zirconium 609 H f o (g) kj/mol

5 Table 4. Ionization Energies of Gaseous Atoms (kj/mol) Atomic # H 1,312 2 He 2,372 5,251 3 Li ,298 11,815 4 Be ,757 14,849 21,007 5 B ,427 3,660 25,026 6 C 1,086 2,353 4,621 6,223 7 N 1,402 2,856 7,475 9,445 8 O 1,314 3,388 5,301 7,469 9 F 1,681 3,374 6,051 8, Ne 2,081 3,952 6,122 9, Na ,563 6,913 9, Mg ,451 7,733 10, Al ,817 2,745 11, Si ,577 3,232 4, P 1,012 1,903 2,912 4, S ,251 3,361 4, Cl 1,251 2,297 3,822 5, Ar 1,521 2,666 3,931 5, K ,051 4,412 5, Ca ,145 4,912 6, Sc 631 1,235 2,389 7, Ti 658 1,310 2,653 4, V 650 1,414 2,828 4, Cr ,592 2,987 4, Mn ,509 3,249 4, Fe ,561 2,958 5, Co 758 1,646 3,232 4, Ni ,753 3,394 5, Cu ,958 3,554 5, Zn ,733 3,833 5,730 Atomic # Ga ,979 2,963 6, Ge ,537 3,302 4, As 947 1,798 2,736 4, Se ,045 2,974 4, Br 1,140 2,100 3,500 4, Kr 1,351 2,368 3,565 5, Rb ,632 3,900 5, Sr ,064 4,210 5, Y 616 1,181 1,980 5, Zr 660 1,267 2,218 3,313 Atomic # Nb 664 1,382 2,416 3, Mo ,558 2,621 4, Tc 702 1,472 2, Ru 711 1,617 2, Rh 720 1,745 2, Pd 805 1,875 3, Ag ,074 3, Cd ,631 3, In ,821 2,705 5, Sn ,412 2,943 3,930 Atomic # Sb ,595 2,440 4, Te ,790 2,698 3, I 1,008 1,846 3, Xe 1,170 2,047 3, Cs , Ba La ,067 1,850 4, Ce ,047 1,949 3, Pr ,018 2,086 3, Nd ,035 2,130 3,899 Atomic # Pm ,052 2,150 3, Sm ,068 2,260 3, Eu ,085 2,405 4, Gd ,167 1,991 4, Tb ,112 2,114 3, Dy ,126 2,200 4, Ho ,139 2,204 4, Er ,151 2,194 4, Tm ,163 2,544 4, Yb ,176 2,415 4,220 Atomic # Lu ,340 2,022 4, Hf 680 1,440 2,250 3, Ta W Re Os Ir Pt 870 1, Au , Hg 1,007 1,810 3,300 Atomic # Tl ,971 2, Pb ,450 3,082 4, Bi ,610 2,466 4, Po At Rn 1, Fr Ra Ac Th 587 Atomic # 1 91 Pa U Np Pu Am Cm Bk Cf Es Fm Md No 642

6 Table 5. Electron Affinities (EA) a Atom EA (kj/mol) Atom EA (kj/mol) Atom EA (kj/mol) Atom EA (kj/mol) H 73 O 141 P 72 Cu 118 Li 60 F 328 S 200 Br 325 B 8 Na 53 Cl 349 I 295 C 122 Al 44 K 48 Se 195 N 0 Si 134 Ti 20 Te 190 O - (g) + e - O 2- (g) -798S - (g) + e - S 2- (g) -640 a Electron affinities are defined as heat liberated (e.g., H for H(g) + e - H - (g) is -73 kj/mol).

7 Table 6. Common Bond Energies (D ) and Bond Lengths (r) Hydrogen Group 15 Group 14 Bond D (kj/mol) r (pm) Bond D (kj/mol) r (pm) Bond D (kj/mol) r (pm) Bond D (kj/mol) r (pm) H-H N-N C-C Si-Si H-B N=N C=C Si-N 355 H-C H-Si H-Ge H-Sn H-N H-P H-As H-O H-S N N N-O N=O N-F N-Cl P-P P-O P=O P=S P-F C C C-Si C-Ge C-Sn C-Pb C-N C=N C N C-P Si-O Si-S Si-F Si-Cl Si-Br Si-I Ge-Ge Ge-N 257 Ge-F H-Se H-Te H-F H-Cl H-Br H-I P-Cl P-Br 264 P-I 184 As-As As-O As-F As-Cl As-Br As-I Sb-Sb 121 Sb-F 440 Sb-Cl (SbCl 5 ) 248 C-O C=O C O C-B 356 C-S C=S C-F C-Cl C-Br C-I Ge-Cl Ge-Br Ge-I 212 Sn-F 414 Sn-Cl Sn-Br Sn-I Pb-F 331 Pb-Cl Pb-Br 201 Pb-I Sb-Cl (SbCl 3 ) Group 13 Group 16 Group 17 Group 18 Bond D (kj/mol)) r (pm) B-B 293 B-O 536 B-F 613 B-Cl B-Br 377 Bond D (kj/mol) r (pm) O-O O=O O-F S=O S-S (S 8 ) S=S S-F S-Cl Se-Se 172 Bond D (kj/mol) r (pm) F-F Cl-Cl Br-Br I-I At-At 116 I-O 201 I-F I-Cl I-Br 175 Bond D (kj/mol) r (pm) Kr-F (KrF 2 ) Xe-O Xe-F Se=Se

8 Table 7. Standard Heats and Free Energies of Formation, and Absolute Entropies of Inorganic and Organic Substances A. Elements and Inorganic Compounds Name H o f (kj/mol) G o f (kj/mol) S o (J/mol K) H 2 (g) H(g) Li(s) Li(g) Li 2 O(s) Li 2 O 2 (s) LiH(s) LiCl(s) LiF(s) LiI(s) Na(s) Na(g) NaH(s) NaF(s) NaCl(s) NaBr(s) NaI(s) Na 2 SO 4 (s) NaNO 3 (s) NaNO 2 (s) Na 2 CO 3 (s) Na 2 O(s) Na 2 O 2 (s) NaO 2 (s) NaC 2 H 3 O 2 (s) NaOH(s) K(s) K(g) KF(s) KCl(s) KClO 3 (s) K 2 O(s) K 2 O 2 (s) KO 2 (s) KOH(s) KNO 3 (s) KClO 4 (s) Rb(s) Name H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Rb(g) RbF(s) RbCl(s) Rb 2 O(s) Rb 2 O 2 (s) RbO 2 (s) Cs(s) Cs(g) CsF(s) CsCl(s) CsI(s) Cs 2 O(s) Cs 2 O 2 (s) CsO 2 (s) Be(s) Be(g) BeCl 2 (s) Mg(s) Mg(g) MgF 2 (s) MgCl 2 (s) MgO(s) MgSO 4 (s) Mg(NO 3 ) 2 (s) Ca(s) Ca(g) CaH 2 (s) CaO(s) Ca(OH) 2 (s) CaF 2 (s) CaCl 2 (s) CaCO 3 (s) Sr(s) Sr(g) SrCl 2 (s) Ba(s) Ba(g) BaCl 2 (s) Name H f o (kj/mol) G f o (kj/mol) S o (kj/mol) BaCl 2.2H 2 O(s) BaCO 3 (s) B(s) B 2 O 3 (s) BF 3 (g) BCl 3 (g) B 2 H 6 (g) Al(s) Al 2 O 3 (s) Al 2 (SO 4 ) 3 (s) C(s, graphite) C(s, diamond) C(g) CF 4 (g) CCl 4 (g) CCl 4 (l) Cl 2 CO(g) CO(g) CO 2 (g) OCS(g) CS 2 (g) HCN(g) Si(s) SiO 2 (s) SiH 4 (g) SiCl 4 (g) SiCl 4 (l) Ge(s) GeCl4(l) Sn(s) SnO(s) SnO 2 (s) SnCl 2 (s) SnCl 4 (l) N 2 (g) NH3(g) N 2 H 4 (g) NO(g) NO 2 (g) N 2 O(g) N 2 O 4 (g) NH 4 Cl(s) NH 4 NO 3 (s) NH 4 NO 2 (s) -264 Name H f o (kj/mol) G f o (kj/mol) S o (kj/mol) HNO 3 (l) P 4 (s, white) P 4 (s, red) P 4 (s, black) P 4 O 10 (s) PH 3 (g) PCl 3 (g) PCl 5 (g) As(s) AsH 3 (g) Sb(s) SbCl 3 (s) SbCl 5 (l) O 2 (g) O 3 (g) H 2 O(g) H 2 O(l) H 2 O 2 (l) OCl 2 (g) S 8 (s, rhombic) H 2 S(g) SF 6 (g) SO 2 (g) SO 3 (g) H 2 SO 4 (l) Se(s) H 2 Se(g) SeO 2 (s) -236 Te(s) H 2 Te(g) F 2 (g) HF(g) Cl 2 (g) HCl(g) Br 2 (l) Br 2 (g) HBr(g) BrF(g) BrF 3 (g) I 2 (s) I 2 (g) HI(g) IF 5 (g) ICl 3 (s) Name H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Co(s) CoCl 2 (s) Cr(s) Cr 2 O 3 (s) CrCl 2 (s) CrCl 3 (s) Fe(s) FeO(s) Fe 2 O 3 (s) Ni(s) NiCl 2.6H 2 O(s) Ti(s) TiCl 4 (l) TiO 2 (s) Cu(s) CuO(s) CuCl 2.2H 2 O(s) CuSO 4 (s) Zn(s) ZnO(s) ZnCl 2 (s) Cd(s) CdS(s) Hg(l) HgCl 2 (s) Hg 2 Cl 2 (s) HgO(s) Ag(s) AgF(s) AgCl(s) AgBr(s) AgI(s) AgNO 3 (s)

9 Table 7. Standard Heats and Free Energies of Formation, and Absolute Entropies of Inorganic and Organic Substances B. Organic Compounds Compound State H o f (kj/mol) G o f (kj/mol) S o (J/mol K) Class Methane g alkane Ethane g alkane Propane g alkane Butane g alkane Pentane g alkane Pentane l alkane Hexane g alkane Hexane l alkane 2-Methylpropane g alkane 2-Methylbutane g alkane 2-Methylbutane l alkane 2,2-Dimethylpropane g alkane Cyclopropane g alkane Cyclobutane g alkane Cyclopentane g alkane Cyclopentane l alkane Cyclohexane g alkane Cyclohexane l alkane cis-1,2-dimethylcyclohexane l alkane trans-1,2-dimethylcyclohexane l alkane Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Propene g alkene 1,3-Butadiene g alkene 1-Butene g alkene Z-2-Butene g alkene E-2-Butene g alkene 2-Methylpropene g alkene 2-Methyl-1-butene g alkene 2-Methyl-2-butene g alkene 3-Methyl-1-butene g alkene Cyclohexene l alkene Cyclohexene g alkene 1-Methylcyclopentene g alkene 3-Methylcyclopentene g alkene 4-Methylcyclopentene g alkene Ethene g alkene Ethyne g alkyne Propyne g alkyne 1-Butyne g alkyne 2-Butyne g alkyne Benzene g aromatic Benzene l aromatic Styrene l aromatic Toluene g aromatic Toluene l aromatic Ethylbenzene l aromatic m-xylene l aromatic o-xylene l aromatic p-xylene l aromatic n-propylbenzene l aromatic Isopropylbenzene (cumene) l aromatic Nitrobenzene l aromatic Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class 1,2-Dibromobutane g alkyl halide 1,3-Dichloropropane g alkyl halide 1-Bromobutane g alkyl halide 1-Bromopropane g alkyl halide 1-Chloro-2-methylpropane g alkyl halide 1-Chlorobutane g alkyl halide 1-Chloropropane g alkyl halide 2,3-Dibromobutane g alkyl halide 2-Bromo-2-methylpropane g alkyl halide 2-Bromobutane g alkyl halide 2-Bromopropane g alkyl halide 2-Chloro-2-methylpropane g alkyl halide 2-Chlorobutane g alkyl halide 2-Chloropropane g alkyl halide Benzyl bromide g alkyl halide Bromomethane g alkyl halide Chloroform g alkyl halide Chloroform l alkyl halide Chloromethane g alkyl halide Dichloromethane g alkyl halide Dichloromethane l alkyl halide Diiodomethane g alkyl halide Fluoromethane g alkyl halide Iodomethane g alkyl halide Iodomethane l alkyl halide Tetrachloromethane g alkyl halide Tetrafluoroethene g alkyl halide Tetrafluoromethane g alkyl halide Tribromomethane (bromoform) g alkyl halide Trifluoromethane g alkyl halide Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Methanol l alcohol Methanol g alcohol Ethanol l alcohol Ethanol g alcohol 1-Propanol l alcohol 1-Propanol g alcohol 2-Propanol l alcohol 2-Propanol g alcohol 1-Butanol l alcohol 1-Butanol g alcohol 2-Butanol g alcohol 2-Methyl-2-propanol g alcohol 2-Methyl-2-propanol l alcohol 2-Methyl-2-propanol s alcohol 1-Pentanol l alcohol 1-Pentanol g alcohol 2-Methyl-2-butanol l alcohol 2-Methyl-2-butanol g alcohol Cyclohexanol l alcohol Cyclohexanol g alcohol Benzyl alcohol l alcohol Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Diethyl ether (ether) g ether Diethyl ether (ether) l ether Dimethyl ether g ether Diphenyl ether l ether Ethyl vinyl ether g ether Ethylene oxide g ether Ethylene oxide l ether Methyl ethyl ether g ether Methyl isopropyl ether g ether Methyl phenyl ether (anisole) l ether Methyl propyl ether g ether Propylene oxide g ether Propylene oxide l ether Tetrahydrofuran l ether Benzaldehyde l aldehyde Butanal g aldehyde Butanal l aldehyde Ethanal g aldehyde Methanal g aldehyde 2-Methylbutanal l aldehyde Propanal g aldehyde Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Ethyl ethanoate l ester Ethyl methanoate l ester Ethyl propionate l ester Methyl benzoate l ester Methyl ethanoate l ester Methyl methanoate g ester Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class 2-Butanone g ketone 2-Butanone l ketone 2-Pentanone g ketone 2-Pentanone l ketone 2-Propanone (acetone) g ketone 2-Propanone (acetone) l ketone 3-Pentanone g ketone Acetophenone l ketone Cyclohexanone g ketone Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Phenol g phenol Phenol s phenol 2-Nitrophenol s phenol 3-Nitrophenol s phenol 4-Nitrophenol s phenol 2-Methylphenol (o-cresol) g phenol 3-Methylphenol (m-cresol) g phenol 4-Methylphenol (p-cresol) g phenol Hydroquinone s phenol Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Acetyl chloride g acid halide Benzoyl chloride l acid halide Benzoyl bromide l acid halide Acetic anhydride g anhydride Acetic anhydride l anhydride Benzoic anhydride s anhydride Acetamide s amide Formamide l amide Acetanilide s amide Benzamide s amide Benzanilide s amide Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Methylamine g amine Ethylamine g amine Dimethylamine g amine n-propylamine g amine Trimethylamine g amine n-butylamine g amine Diethylamine g amine 2-Aminobutane g amine 2-Amino-2-methylpropane g amine Triethylamine g amine N,N-Dimethylaniline g amine N,N-Dimethylaniline l amine N-Ethylaniline g amine N-Ethylaniline l amine Aniline g amine Aniline l amine 2-Nitroaniline s amine 3-Nitroaniline s amine 4-Nitroaniline s amine Compound State H o f (kj/mol) G o f (kj/mol) S o (kj/mol) Class Acetonitrile g nitrile Acetonitrile l nitrile Benzonitrile g nitrile Propionitrile g nitrile Propionitrile l nitrile Methyl radical g radical Ethyl radical g radical 1-Propyl radical g radical 2-Propyl radical g radical 2-Methyl-2-propyl radical g radical 2-Methyl-1-propyl radical g radical Allyl radical g radical Benzyl radical g radical Phenyl radical g radical Cyclohexyl radical g radical Cyclohexen-3-yl radical g radical 1,3-Cyclohexadien-5-yl g radical Vinyl radical g radical Trifluoromethyl radical g radical Trichloromethyl radical g radical Perfluoroethyl radical g radical Ethynyl radical g radical Methylene (carbene) g radical Dichlorocarbene g radical Difluorocarbene g radical Methyoxyl radical g radical Ethoxyl radical g radical 2-Methyl-2-propoxyl radical g radical Acyl radical g radical

10 Table 8. Standard Heats of Formation for Gaseous Complex Ions, Calculated and (Experimental) Group H f o (kj/mol) Group H f o (kj/mol) Group H f o (kj/mol) Group H f o (kj/mol) OH (-143) HS BF IO NH 2-63 CN - 36 (60) NCO ClO BH N SeO CO HF O 2 - (-49) ClO HCO SO O NO BrO CrO CH 3 CO AlCl SiF SnCl PbCl TiCl HfCl PtCl TiBr NH WBr

11 Table 9. Lattice Energy A. Madelung Constants (A) for Common Crystal Lattices a Structure Constant Sodium chloride 1.75 Cesium chloride 1.76 Zinc blende 1.64 Wurtzite 1.64 Fluorite 5.04 Rutile 4.82 b Corundum b a The Madelung constant, A, is used in the equation E = AZ 2e 2/r, where r is the sum of the ionic radii, e is the charge on an electron, and Z is the highest common denominator of the absolute values of the integral charges on the ions (e.g., for MgCl 2, Z = 1; for CaO, Z = 2). b Depends on exact structure.

12 Table 9. Lattice Energy B. Values of Born Exponent to be Used in Repulsive Function for Lattice Energy c Ion Type Example n He-He LiH 5 Ne-Ne NaF, MgO 7 Ar-Ar KCl, CaS, CuCl 9 Kr-Kr RbBr, AgBr 10 Xe-Xe CsI 12 c For compounds of mixed ion types, use the average value (e.g., for NaCl, n = 8).

13 Table 9. Lattice Energy C. Lattice Energies (E) for Common Compounds Compound E (kj/mol) Compound E (kj/mol) Compound E (kj/mol) LiH 906 NaH 811 KH 714 LiF 1009 NaF 904 KF 801 LiCl 829 NaCl 769 KCl 698 LiBr 789 NaBr 736 KBr 672 LiI 734 NaI 688 KI 632 CuCl 979 AgF 969 AuCl 1042 CuBr 976 AgCl 916 AuI 1050 CuI 958 AgBr 900 TlCl 748 MgF AgI 895 BaF MgBr CaF TiF VF CaI ZnF FeF CaO 3464 ZnS 3619 CuF CaS 3093 CdS 3402 MnF CrF HgS 3573 CoF NiF Al 2 O 3 15,326

14 Table 9. Lattice Energy D. Kapustinskii Equation E = 108,000 Z c Z a ν/r, where Z c and Z a are absolute integral values of charges on the cation and anion, ν is the number of ions in the simplest formula, and ris the sum of the ionic radii. When r is in pm, E will result in kj/mol.

15 Table 10. Contributions to Entropies of Solids at 298 K A. Cation Contributions Cation J/mol K Ag 54 Al 33 As 48 Au 64 B 21 Ba 57 Be 18 Bi 65 C 22 Ca 39 Cd 54 Ce 58 Co 44 Cr 43 Cs 57 Cu 45 Fe 44 Ga 47 Ge 47 Hf 62 Hg 64 In 54 Ir 64 K 38 La 58 Li 15 Mg 32 Mn 43 Mo 51 N 24 Na 31 Nb 51 Ni 44 Os 63 Pb 65 Pd 53 Pt 64 Ra 66 Rb 50 Re 63 Rh 52 Ru 52 Sb 55 Sc 41 Si 34 Sn 55 Sr 50 Ta 62 Tc 52 Ti 41 Tl 64 U 67 V 42 W 63 Y 50 Zn 46 Zr 51

16 Table 10. Contributions to Entropies of Solids at 298K B. Anion Contributions, J/mol K Charge on Positive Ion Anion F Cl Br I O S Charge on Positive Ion Anion Se Te OH CN NO NO CO Charge on Positive Ion Anion HCO C 2 O ClO BrO IO MnO SO SO CrO PO

17 Table 11. Group Contributions to H f o (g) and S o (g) at 298 K a A. Hydrocarbon Groups Group H f o (kj/mol) S o (J/mol K) Group H f o (kj/mol) S o (J/mol K) C-(H) 3 (C) C-(C d )(C) 2 (H) C-(H) 2 (C) C-(C d )(C B )(H) C-(H)(C) C-(C B )(C) 2 (H) C-(C) C-(C B )(C)(H) C d -(H) C-(C B )(C) C d -(H)(C) C B -(H) C d -(C) C B -(C) C d -(C d )(H) C B -(C d ) C d -(C d )(C) [C B -(C t )] [C d -(C B )(H)] C B -(C B ) C d -(C B )(C) C-(C t )(C) 2 (H) [C d -(C t )(H)] C-(C t )(C)(H) C-(C d )(C)(H) C t -(C) C-(C d ) 2 (H) C t -(H) C-(C d )(C) C t -(C d ) C a C t -(C B ) a The subscripts "d" and "t" designate carbon atoms in carbon-carbon double and triple bonds; "a", an allenic carbon; "B", an aromatic carbon; "A", a nitrogen atom in a nitrogen-nitrogen double bond; and "I", a nitrogen atom in a nitrogen-carbon double bond. Bracketed values are estimated.

18 Table 11. Group Contributions to H f o (g) and S o (g) at 298 K a B. Corrections for Steric Interactions and Rings H f o (kj/mol) S o (J/mol K) Alkane, gauche correction 3.3 Alkene, gauche correction 2.1 cis correction 4.2 ortho correction Cyclopropane Cyclopropene Cyclobutane Cyclobutene Cyclopentane Cyclopentene Cyclohexane Cyclohexene Cycloheptane Cycloheptene 22.6 Cyclooctane

19 Table 11. Group Contributions to H f o (g) and S o (g) at 298 K a C. Oxygen-Containing Groups Group H o f (kj/mol) S o (J/mol K) Group H o f (kj/mol) S o (J/mol K) CO-(CO)(C) O-(C) CO-(O)(C d ) O-(C)(H) CO-(O)(C B ) C d (CO)(O) 26.3 CO-(O)(C) CO-(C d )(H) [CO-(O)(H)] C d -(CO)(C) 39.3 CO-(C B ) [C d -(CO)(H)] 32.2 CO-(C B )(C) [C d -(O)(C d )] 37.2 [CO-(C B )(H)] [C d -(O)(C)] 43.0 CO-(C) [C d -(O)(H)] 36.0 CO-(C)(H) C B -(CO) 40.5 Group H o f (kj/mol) S o (J/mol K) Group H o f (kj/mol) S o (J/mol K) CO-(C)(H) C B -(CO) 40.5 CO-(H) C B -(O) O-(CO) C-(CO) 2 (H) O-(CO)(O) C-(CO)(C) [O-(CO)(C d )] C-(CO)(C) 2 (H) O(CO)(C) C-(CO)(C)(H) O-(CO)(H) [C-(CO)(H) 3 ] O-(O)(O) C-(O) 2 (C) O-(O)(C) C-(O) 2 (C)(H) O-(O)(H) C-(O) 2 (H) Group H o f (kj/mol) S o (J/mol K) Group H o f (kj/mol) S o (J/mol K) O-(C d ) C-(O)(C B )(H ) O-(C d )(C) C-(O)(C d )(H ) O-( C B ) C-(O)(C ) O-(C B )(C) C-(O)(C) 2 (H) [O-(C B )(H)] C-(O)(C)(H ) [C-(O)(H) 3 ] a The subscripts "d" and "t" designate carbon atoms in carbon-carbon double and triple bonds; "a", an allenic carbon; "B", an aromatic carbon; "A", a nitrogen atom in a nitrogen-nitrogen double bond; and "I", a nitrogen atom in a nitrogen-carbon double bond. Bracketed values are estimated.

20 Table 11. Group Contributions to H f o (g) and S o (g) at 298 K a D. Nitrogen-Containing Groups Group H f o (kj/mol) S o (J/mol K) Group H f o (kj/mol) S o (J/mol K) [C-(N)(H) 3 ] N A -(N) 96.1 C-(N)(C)(H) CO-(N)(H) C-(N)(C) 2 (H) CO-(N)(C) C-(N)(C) N-(CO)(H) C- (N A )(C)(H) N-(CO)(C)(H) C- (N A )(C) 2 (H) N-(CO)(C B )(H) 1.7 C-(N A )(C) N-(CO) 2 (H) Group H f o (kj/mol) S o (J/mol K) Group H f o (kj/mol) S o (J/mol K) N-(C) (H) N-(CO) 2 (C) 24.7 N-(C) 2 (H) N-(CO) 2 (C B ) -2.1 N- (C) C-(CN)(C) (H) N-(N) (H) C- (CN)(C) 2 (H) N- (N)(C)(H) C-(CN) (C) N-(N)(C ) C-(CN) 2 (C) N- (N)(C B )(H) 92.4 Cd-(CN)(H) NI-(C) 89.0 Cd-(CN ) NI-(C B ) 69.8 Ct-(CN) C B -(CN) Cd-(NO 2 )(H) N A -(H) C-(NO 2 )(C) (H) N A -(C) C- (NO 2 )(C) 2 (H) N-(C B )(H) C-(NO 2 )(C) N- (C B )(C)(H) 62.3 C- (NO 2 ) 2 (C)(H) N-(C B )(C) O-(NO)(C) N-(C B ) 2 (H) 68.1 O-(NO) 2 (C) C B -(N) a The subscripts "d" and "t" designate carbon atoms in carbon-carbon double and triple bonds; "a", an allenic carbon; "B", an aromatic carbon; "A", a nitrogen atom in a nitrogen-nitrogen double bond; and "I", a nitrogen atom in a nitrogen-carbon double bond. Bracketed values are estimated.

21 Table 11. Group Contributions to H f o (g) and S o (g) at 298 K a E. Halogen-Containing Groups Group H o f (kj/mol) S o (J/mol K) Cd-(F) Cd-(Cl) Cd-(F)(H) Cd-(Cl)(H) Cd-(Br)(H) Cd-(I)(H) CB-(F) CB-(Cl) CB-(Br) CB-(I) C-(CB)(F) C-(CB)(Br)(H) C-(CB)(I)(H) C-(F) 3 (C) C-(F) 2 (H)(C) C-(F)(H) 2 (C) C-(F) 2 (C) C-(F)(H)(C) C-(F)(C) C-(F) 2 (Cl)(C) C-(Cl) 3 (C) C-(Cl) 2 (H)(C) C-(Cl)(H) 2 (C) C-(Cl) 2 (C) C-(Cl)(H)(C) C-(Cl)(C) C-(Br)(H) 2 (C) C-(Br)(H)(C ) C-(Br)(C) C-(I)(H) 2 (C) C-(I)(H)(C ) C-(I)(C) C-(Cl)(C)(O)(H) a The subscripts "d" and "t" designate carbon atoms in carbon-carbon double and triple bonds; "a", an allenic carbon; "B", an aromatic carbon; "A", a nitrogen atom in a nitrogen-nitrogen double bond; and "I", a nitrogen atom in a nitrogen-carbon double bond. Bracketed values are estimated.

22 Table 12. Metallic, Covalent and Ionic Radii (r) a (Note: 1 Å = 100pm) Atom/Ion r (pm) Ag 144 Ag Al 143(140) Al Ar (95) As (122) As Au 144 Au B (90) Ba 224 Ba Be 112(125) Be Bi 182 Bi Br 114 Br C (77) Ca 197 Ca Cd 152 Cd Ce 182 Ce Cl (99) Cl- 184 Co 125 Co Co Cr 129 Cr Cs 272 Cs Cu 128 Cu + 77 Cu F (71) F Fe 126 Fe Atom/Ion r (pm) Fe Ga 153 Ga Ge 139(122) H (37) He (32) Hf 159 Hg 155 Hg I (133) I- 220 In 167 In Ir 136 Ir K 235 K Kr (110) La 188 La Li 157 Li + 76 Lu 172 Lu Mg 160 Mg Mn 137 Mn N (75) Na 191 Na Ne (69) Ni 125 Ni O (73) O Os 135 P (110) Pb 175 Pb Pd 137 Atom/Ion r (pm) Pd Po 153 Pt 139 Pt Pt Rb 250 Rb Rh 134 Rn (145) Ru 134 S (102) S Sb 161(143) Sb Sc 164 Sc Se (117) Se Si (118) Sn 158(140) Sn Sr 215 Sr Te (135) Te Th 180 Ti 147 Ti Tl 171 Tl Tl U 156 V 135 V W 141 Xe (130) Y 182 Y Zn 137 Zn Zr 160 a Metallic radii for 12-coordination are given for all metals. Covalent radii are in parentheses. Ionic radii are for six-coordination.

23 Table 13. Thermochemical Radii A. Anions Ion r(pm) Ion r(pm) Ion r(pm) Ion r(pm) BO BF GeCl WBr BrO BeF IrCl ZnBr CO CoF PbCl PtI ClO CrF PdCl SnI ClO MnF PtCl ZnI CrO NiF PtCl BH IO SiF RuCl CH 3 CO IO PtF SeCl CN MnO RhF SnCl CNS NO TiF TiCl N NO AlCl UCl NCO PO BCl WCl NH SeO HCl2-201 ZnCl O SeO CeCl PtBr OH SiO CoCl SnBr OCN SO CuCl TeBr HCO TeO FeCl TiBr HCO VO GaCl UBr HS - 207

24 Table 13. Thermochemical Radii B. Cations Ion r(pm) Cd(NH 3 ) Co(H 2 O) Co(NH 3 ) 5 Cl Co(NH 3 ) Fe(NH 3 ) Mg(H 2 O) Mn(H 2 O) Mn(NH 3 ) NH N(CH 3 ) Ni(H 2 O) Ni(NH 3 ) PH Zn(H 2 O) Zn(NH 3 ) Fr + 172

25 Table 14. Standard Formation Data for Aqueous Ions A. Cations Ion H o f (kj/mol) G o f (kj/mol) S o (J/mol K) H Li Na K Rb Cs Cu Ag Tl NH Be Mg Ca Sr Ba Cr Mn Fe Co Ni Cu Zn Cd Hg Sn Pb Al Ga In Tl Cr Fe Co Ag(NH 3 )

26 Table 14. Standard Formation Data for Aqueous Ions B. Anions Ion H o f (kj/mol) G o f (kj/mol) S o (J/mol K) F Cl Br I ClO ClO ClO ClO BrO IO OH SH S HSO SO SO SeO SeO NO NO N PO CO HCO CN BF MnO CrO Cr 2 O

27 Table 15. Absolute Enthalpies of Hydration of Gaseous Ions Ion H h o (kj/mol) H Li Na K Rb Cs In Tl Cu Ag Au NH Be Mg Ca Sr Ba Ti Cr Mn Fe Co Ni Cu Pt Zn Cd Hg Sn Pb Al Sc Y Ga In Tl Cr Fe Co F Cl Br I NO OH

28 Table 16. Solubilities of Gases in Water at 293 K Gas Solubility a Acetylene Ammonia 52.9 Bromine 14.9 Carbon dioxide Carbon monoxide Chlorine Ethane Ethylene Hydrogen Hydrogen sulfide Methane Nitrogen Oxygen Sulfur dioxide a Grams of gas dissolved in 100 g of water when the total pressure above the solution is 1 atm.

29 Table 17. Solubilities of Inorganic Compounds in Water at 293 K (g per 100 g water) Fluorides AlF BaF MnF NiF KF 94.9 AgF 172 NaF 4.06 Chlorides AlCl NH 4 Cl 37.2 BaCl 2.2 H 2 O 35.8 CaCl 2.6 H 2 O 74.5 CsCl 187 CoCl CuCl FeCl FeCl 3.6 H 2 O 91.8 PbCl LiCl 83.5 MgCl MnCl HgCl NiCl KCl 34.2 NaCl 35.9 Nitrates Al(NO 3 ) NH 4 NO Ba(NO 3 ) Cd(NO 3 ) Ca(NO 3 ) 2.4 H 2 O 129 CsNO 3 23 Co(NO 3 ) Cu(NO 3 ) Fe(NO 3 ) 2.6 H 2 O 140 Fe(NO 3 ) 3.9 H 2 O 138 Pb(NO 3 ) LiNO KNO AgNO NaNO Sulfates Al 2 (SO 4 ) (NH 4 ) 2 SO CdSO CaSO 4.2 H 2 O 0.26 CoSO CuSO 4.5 H 2 O 32.0 FeSO 4.7 H 2 O 48 Li 2 SO MgSO K 2 SO Ag 2 SO Na 2 SO ZnSO Carbonates Li 2 CO K 2 CO Na 2 CO Perchlorates Ba(ClO 4 ) 2.3 H 2 O 336 Cd(ClO 4 ) 2.6 H 2 O 188 Fe(ClO 4 ) LiClO KClO NaClO 4 201

30 Table 18. Solubility Product Constants, K sp Bromides PbBr x 10-6 Hg 2 Br 2 AgBr 1.3 x x Carbonates BaCO x 10-9 CdCO x CaCO x 10-9 CuCO x FeCO 3 5 x PbCO x MgCO 3 8 x NiCO x 10-7 Ag 2 CO x SrCO x 10-9 ZnCO x 10-7 Chlorides AgCl 1.8 x PbCl x 10-4 Hg 2 Cl x Cyanides Hg 2 (CN) 2 5 x AgCN 1.6 x Chromates PbCrO x Ag 2 CrO x BaCrO x CuCrO x 10-6 CaCrO x 10-4 Hg 2 CrO x 10-9 Fluorides BaF x 10-6 CaF 2 4 x LiF 5 x 10-3 PbF 2 4 x 10-8 MgF 2 6 x 10-9 SrF 2 3 x 10-9 Hydroxides Al(OH) 3 4 x Cd(OH) 2 2 x Ca(OH) 2 6 x 10-6 Cr(OH) 3 7 x Co(OH) 3 1 x Co(OH) 2 3 x Cu(OH) 2 2 x Fe(OH) 3 6 x Fe(OH) 2 2 x Pb(OH) 2 4 x Mg(OH) x Mn(OH) 2 2 x Ni(OH) 2 2 x Zn(OH) 2 5 x Iodides Hg 2 I 2 5 x AgI 8 x PbI x 10-8 Oxalates BaC 2 O x 10-7 CaC 2 O x 10-9 MgC 2 O x 10-5 SrC 2 O x 10-8 Ag 2 C 2 O x PbC 2 O 4 3 x Phosphates Ag 3 PO x Ca 3 (PO 4 ) 2 1 x Mg 3 (PO 4 ) 2 4 x Sulfates BaSO x CaSO 4 2 x 10-5 PbSO x 10-8 Hg 2 SO 4 7 x 10-7 Ag 2 SO 4 6 x 10-5 SrSO 4 3 x 10-7 Sulfides CdS 1 x CoS 1 x CuS 1 x FeS 1 x PbS 1 x MnS 1 x HgS 1 x NiS 1 x Ag 2 S 1 x SnS 1 x ZnS 1 x 10-23

31 Table 19. Acid and Base Dissociation Constants in Water at 298 K A. Acid Constants Compound Ka Compound Ka HF 3.5 x 10-4 o-fc 6 H 4 COOH 5.4 x 10-4 HOCl 3.0 x 10-8 m-fc 6 H 4 COOH 1.4 x 10-4 HClO x 10-2 p-fc 6 H 4 COOH 7.2 x 10-5 H 2 S 5.7 x 10-8, 1.2 x o-clc 6 H 4 COOH 1.2 x 10-3 H 2 SO x 10-2, 5.6 x 10-8 m-clc 6 H 4 COOH 1.5 x 10-4 H 2 Se 2.0 x 10-4, 1.0 x p-clc 6 H 4 COOH 1.0 x 10-4 H 2 Te 2.5 x 10-3, 5.0 x o-no 2 C 6 H 4 COOH 7.0 x 10-3 HNO x 10-4 m-no 2 C 6 H 4 COOH 3.4 x 10-4 HCN 4.9 x p-no 2 C 6 H 4 COOH 3.9 x 10-4 H 2 CO x 10-7, 4.8 x p-ch 3 C 6 H 4 COOH 4.2 x 10-5 H 2 C 2 O x 10-2, 6.4 x 10-5 p-ch 3 O 2 C 6 H 4 COOH 3.4 x 10-5 H 3 PO x 10-3, 6.2 x 10-8, p-h 2 NC 6 H 4 COOH 1.2 x x C 2 H 5 SH 2.5 x Compound Ka Compound Ka HOOCCH 2 COOH 1.5 x 10-3, 2.0 x 10-6 BrCH 2 COOH 1.4 x 10-3 HCOOH 1.8 x 10-4 ICH 2 COOH 7.6 x 10-4 CH 3 COOH 1.8 x 10-5 CH 3 CH 2 COOH 1.3 x 10-5 FCH 2 COOH 2.2 x 10-3 C 6 H 5 COOH 6.5 x 10-5 F 2 CHCOOH 6.0 x 10-2 o-c 6 H 4 (COOH) x 10-3, 3.9 x 10-6 F 3 CCOOH 6.0 x 10-1 C 6 H 5 OH 1.3 x ClCH 2 COOH 1.4 x 10-3 o-no 2 C 6 H 4 OH 6.8 x 10-8 Cl 2 CHCOOH 3.3 x 10-2 m-no 2 C 6 H 4 OH 5.3 x 10-9 Cl 3 CCOOH 2.0 x 10-1 p-no 2 C 6 H 4 OH 7.0 x 10-8

32 Table 19. Acid and Base Dissociation Constants in Water at 298 K B. Base Constants Compound Kb Compound Kb NH x 10-5 C 6 H 5 NH x H 2 NNH x 10-6 C 6 H 5 N(CH 3 ) x 10-9 H 2 NOH 1.1 x 10-8 o-fc 6 H 4 NH x (CH 3 ) 3 N 6.5 x 10-5 m-fc 6 H 4 NH x (C 2 H 5 ) 3 N 4.0 x 10-4 p-fc 6 H 4 NH x (C 2 H 5 ) 2 NH 1.3 x 10-3 o-no 2 C 6 H 4 NH x C 2 H 5 NH x 10-4 m-no 2 C 6 H 4 NH x C 6 H 5 CH 2 NH x 10-5 p-ch 3 C 6 H 4 NH x 10-9 (C 2 H 5 ) 3 P 5.0 x 10-8 p-ch 3 OC 6 H 4 NH x 10-9 (C 2 H 5 ) 3 As 5.0 x pyridine 1.4 x 10-9

33 Table 20. Overall Formation Constants of Coordination Compounds Halo Complexes Amine Complexes AlF x Co(NH 3 ) x 10 4 AgCl x 10 5 Co(NH 3 ) x AgCl x 10 6 Ni(NH 3 ) x 10 8 HgCl x Cu(NH 3 ) x AgBr x 10 9 Cu(NH 3 ) x CdBr x 10 3 Ag(NH 3 ) x 10 7 HgBr x Zn(NH 3 ) x 10 9 PbBr x 10 4 Cd(NH 3 ) x 10 7 AgI x CdI x 10 6 HgI x PbI x 10 6 Cyano Complexes Cu(CN) x Ni(CN) x Fe(CN) x Fe(CN) x Ag(CN) x Cd(CN) x Hg(CN) x Zn(CN) x Other Complexes AgI x Ag(C 2 O 4 ) x 10 2 Fe(C 2 O 4 ) x Al(C 2 O 4 ) x HgS x Fe(NCS) x 10 3 Hg(NCS) x Pb(C 2 H 3 O 2 ) x 10 3 Cu(en) x Ni(en) x Co(en) x Co(en) x Ca(EDTA) x Mg(EDTA) x 10 8

34 Table 21. Vapor Pressure of Water from 0 o C to 100 o C T ºC P(torr) T ºC P(torr) T ºC P(torr) T ºC P (torr)

35 Table 22. Hammett Sigma Constants a Group σmeta σpara σi σ v π E s MR H CH C 2 H n-c 3 H i-c 3 H n-c 4 H t-c 4 H H 2 C=CH* C 6 H 5 * CH 2 Cl CF CN CHO COCH CO 2 H* Si(CH 3 ) F Cl Br I OH OCH OCH 2 CH SH SCH NO 2 * NO NH NHCHO NHCOCH N(CH 3 ) N(CH 3 ) a σ meta, σ para = Hammett constants; σ I = inductive sigma constant; σ v = Charton's v (size) values; π = hydrophobicity parameter; E s = Taft size parameter; MR = molar refractivity (polarizability) parameter. An asterisk indicates that the group is in the most sterically hindered conformation.

36 Table 23. Standard Electrode Potentials A. Acidic Media Half-reaction E o, V F 2 (g) + 2H + + 2e - = 2HF(aq) 3.06 F 2 + 2e - = 2 F S 2 O e - = 2SO Co 3+ + e - = Co H 2 O 2 + 2H + + 2e - = 2H 2 O 1.78 MnO H + + 3e - = MnO 2 (s) + 2H 2 O 1.70 H 5 IO 6 + H + + 2e - = IO H 2 O 1.64 Ce 4+ + e - = Ce BrO H + + 5e - = 1/2 Br 2 (l) + 3H 2 O 1.52 MnO H + + 5e - = Mn H 2 O 1.51 PbO 2 + 4H + + 2e - = Pb H 2 O 1.46 Cl 2 + 2e - = 2Cl Cr 2 O H + + 6e - = 2Cr H 2 O 1.33 MnO 2 (s) + 4H + + 2e - = Mn H 2 O 1.23 O 2 (g) + 4H + + 4e - = 2H 2 O(l) 1.23 IO H + + 5e - = 1/2 I 2 + 3H 2 O 1.20 Br 2 (aq) + 2e - = 2Br VO H + + e - = VO 2+ + H 2 O 1.00 HNO 2 + H + + e - = NO(g) + H 2 O 1.00 NO H + + 2e - = HNO 2 + H 2 O Hg e - = Hg Ag + + e - = Ag 0.80 Hg e - = 2Hg(l) 0.79 NO H + + e - = NO 2 + H 2 O 0.78 Fe 3+ + e - = Fe O 2 (g) + 2H + + 2e - = H 2 O 2 (aq) 0.68 Hg 2 SO 4 (s) + 2e - = 2Hg + SO H 3 AsO 4 (aq) + 2H + + 2e - = HAsO 2 + 2H 2 O 0.56 I e - = 3I I 2 + 2e - = 2I Cu + + e - = Cu 0.52 O 2 + 2H 2 O + 4e - = 4OH VO H + + e - = V 3+ + H 2 O 0.36 [Fe(CN) 6 ] 3- + e - = [Fe(CN) 6 ] Cu e - = Cu 0.34 UO H + + 2e - = U H 2 O 0.33 BiO+ + 2H + + 3e - = Bi + H 2 O 0.32 Hg 2 Cl 2 (s) + 2e - = 2Hg + 2Cl Half-reaction E o, V AgCl(s) + e - = Ag + Cl SbO + + 2H + + 3e - = Sb + H 2 O 0.21 SO H + + 2e - = H 2 SO 3 + H 2 O 0.17 Sn e - = Sn S(rhombic) + 2H + + 2e - = H 2 S(aq) 0.14 CuCl + e - = Cu + Cl TiO H + + e - = Ti 3+ + H 2 O 0.10 S 4 O e - = 2S 2 O AgBr(s) + e - = Ag + Br H + + 2e - = H 2 (g) 0.00 Pb e - = Pb Sn e - = Sn(white) AgI(s) + e - = Ag + I Mo e - = Mo Ni e - = Ni V 3+ + e - = V Co e - = Co [Ag(CN) 2 ] - + e - = Ag + 2CN Cd e - = Cd Cr 3+ + e - = Cr Fe e - = Fe CO 2 + 2H + + 2e - = H 2 C 2 O U 4+ + e - = U Cr e - = Cr Zn e - = Zn Mn e - = Mn Zr e - = Zr Ti e - = Ti Al e - = Al Th e - = Th Mg e - = Mg Ce e - = Ce La e - = La Na + + e - = Na Ca e - = Ca Sr e - = Sr Ba e - = Ba Cs + + e - = Cs K + + e - = K Li + + e - = Li -3.04