Uscript; available in PMC 2011 December 8.Warren et al.Pagereduced forms, given by the pKas of XH?/X?and XH/X- pairs; the reduction potentials of the protonated and deprotonated substrate, E XH?/XH] and E X?X-], and the homolytic bond dissociation free energy, the BDFE (see below). All of these parameters are free energies, and it is simple to convert them all into the same units (eqs 4 and 5, where R is the gas constant, T = temperature, and F = Faraday constant). The E?is a free MG516 site energy for the chemical reaction that is the sum of the half reaction of interest, such as X?+ e- X-, and the half reaction for the standard redox couple (NHE for aqueous values). For a reaction such as HX + Y X + HY, the pKa and E?NSC309132MedChemExpress 4-Deoxyuridine values for the HX and HY systems determine the free energies of PT, ET, and H?transfer steps.(4)NIH-PA Author Manuscript NIH-PA Author Manuscript NIH-PA Author Manuscript(5)The pKa values in many cases can be determined by titration either versus pH (in aqueous media) or versus a standard acid or base (in organic solvents). As discussed below in more detail, there are extensive acid/base data available in organic solvents from the respective work of Izutsu,28 Bordwell29 and K t.30 The redox potentials are typically determined electrochemically. The average of the anodic and cathodic peaks in the cyclic voltammogram, E1/2, is typically used as a good measure of the thermodynamic potential E? 31 Parenthetically, we note that it is strongly preferred to reference non-aqueous potentials to the ferrocene (Cp2Fe+/0) couple.32 Aqueous potentials are reference to normal hydrogen (NHE) in this review. Useful conversions between common electrochemical references are available for acetonitrile33 and water34 and potentials of Cp2Fe+/0 in organic solvents versus aqueous NHE have been reviewed.35 The thermodynamic parameters E?and pKa, if they are to be used in the same Scheme or equation, should be determined under conditions that are as similar as possible. For instance, if the electrochemical data are determined using solutions containing supporting electrolyte (as is typical), then the pKa values should ideally be determined in the presence of the same electrolyte. Because the data tabulated below often come from different sources and different types of measurements, this requirement for similar conditions is not always met, which introduces some (usually relatively small) uncertainty into any composite values. A valuable check on the consistency of the data can be obtained using Hess’ law, which states that the energy change is independent of path, and that the energy change around any closed cycle is zero. This means that there are actually only 3 independent parameters in Scheme 4. It also implies, perhaps counter-intuitively, that in free energy terms the change in the pKa values upon oxidation is identical to the change in redox potential upon deprotonation (eq 6).(6)3.1 X Bond Dissociation Free Energies HAT reactions have historically been analyzed using the Bell-Evans-Polyani relation,36 which uses bond dissociation enthalpies (BDEs, which are not exactly the same as bond dissociation energies37). It is, however, more appropriate to use bond dissociation free energies (BDFEs) because all modern theories of ET, PT, and CPET use free energies rather than enthalpies. Our group has shown, for an iron system where the BDE and BDFE areChem Rev. Author manuscript; available in PMC 2011 December 8.Warren et al.Pagequite different, that CPET.Uscript; available in PMC 2011 December 8.Warren et al.Pagereduced forms, given by the pKas of XH?/X?and XH/X- pairs; the reduction potentials of the protonated and deprotonated substrate, E XH?/XH] and E X?X-], and the homolytic bond dissociation free energy, the BDFE (see below). All of these parameters are free energies, and it is simple to convert them all into the same units (eqs 4 and 5, where R is the gas constant, T = temperature, and F = Faraday constant). The E?is a free energy for the chemical reaction that is the sum of the half reaction of interest, such as X?+ e- X-, and the half reaction for the standard redox couple (NHE for aqueous values). For a reaction such as HX + Y X + HY, the pKa and E?values for the HX and HY systems determine the free energies of PT, ET, and H?transfer steps.(4)NIH-PA Author Manuscript NIH-PA Author Manuscript NIH-PA Author Manuscript(5)The pKa values in many cases can be determined by titration either versus pH (in aqueous media) or versus a standard acid or base (in organic solvents). As discussed below in more detail, there are extensive acid/base data available in organic solvents from the respective work of Izutsu,28 Bordwell29 and K t.30 The redox potentials are typically determined electrochemically. The average of the anodic and cathodic peaks in the cyclic voltammogram, E1/2, is typically used as a good measure of the thermodynamic potential E? 31 Parenthetically, we note that it is strongly preferred to reference non-aqueous potentials to the ferrocene (Cp2Fe+/0) couple.32 Aqueous potentials are reference to normal hydrogen (NHE) in this review. Useful conversions between common electrochemical references are available for acetonitrile33 and water34 and potentials of Cp2Fe+/0 in organic solvents versus aqueous NHE have been reviewed.35 The thermodynamic parameters E?and pKa, if they are to be used in the same Scheme or equation, should be determined under conditions that are as similar as possible. For instance, if the electrochemical data are determined using solutions containing supporting electrolyte (as is typical), then the pKa values should ideally be determined in the presence of the same electrolyte. Because the data tabulated below often come from different sources and different types of measurements, this requirement for similar conditions is not always met, which introduces some (usually relatively small) uncertainty into any composite values. A valuable check on the consistency of the data can be obtained using Hess’ law, which states that the energy change is independent of path, and that the energy change around any closed cycle is zero. This means that there are actually only 3 independent parameters in Scheme 4. It also implies, perhaps counter-intuitively, that in free energy terms the change in the pKa values upon oxidation is identical to the change in redox potential upon deprotonation (eq 6).(6)3.1 X Bond Dissociation Free Energies HAT reactions have historically been analyzed using the Bell-Evans-Polyani relation,36 which uses bond dissociation enthalpies (BDEs, which are not exactly the same as bond dissociation energies37). It is, however, more appropriate to use bond dissociation free energies (BDFEs) because all modern theories of ET, PT, and CPET use free energies rather than enthalpies. Our group has shown, for an iron system where the BDE and BDFE areChem Rev. Author manuscript; available in PMC 2011 December 8.Warren et al.Pagequite different, that CPET.
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