Home | About | Journals | Submit | Contact Us | Français |

**|**HHS Author Manuscripts**|**PMC2971562

Formats

Article sections

Authors

Related links

Coord Chem Rev. Author manuscript; available in PMC 2010 November 3.

Published in final edited form as:

Coord Chem Rev. 2008 February 1; 252(3-4): 384–394.

doi: 10.1016/j.ccr.2007.07.019PMCID: PMC2971562

NIHMSID: NIHMS242574

Department of Chemistry, 104 Chemistry Building, Pennsylvania State University, University Park, PA 16802

Sharon Hammes-Schiffer: ude.usp.mehc@shs

See other articles in PMC that cite the published article.

Theoretical studies of proton-coupled electron transfer (PCET) reactions for model systems provide insight into fundamental concepts relevant to bioenergetics. A dynamical theoretical formulation for vibronically nonadiabatic PCET reactions has been developed. This theory enables the calculation of rates and kinetic isotope effects, as well as the pH and temperature dependences, of PCET reactions. Methods for calculating the vibronic couplings for PCET systems have also been developed and implemented. These theoretical approaches have been applied to a wide range of PCET reactions, including tyrosyl radical generation in a tyrosine-bound rhenium polypyridyl complex, phenoxyl/phenol and benzyl/toluene self-exchange reactions, and hydrogen abstraction catalyzed by the enzyme lipoxygenase. These applications have elucidated some of the key underlying physical principles of PCET reactions. The tools and concepts derived from these theoretical studies provide the foundation for future theoretical studies of PCET in more complex bioenergetic systems such as Photosystem II.

Bioenergetic processes involving energy transformation play a vital role in all living organisms and structures. For example, Photosystem II (PSII) catalyzes the light-driven oxidation of water to molecular oxygen in plants.[1–3] In this process, absorption of light by the primary electron donor chlorophyll P680 leads to charge separation. A redox-active tyrosine residue Y_{Z} is thought to mediate the proton-coupled electron transfer (PCET) reaction between the oxygen evolving Mn_{4} cluster and P680.[4–10] The detailed mechanism of charge separation in PSII is still not well understood.

Given the large size and complexity of bioenergetic systems such as PSII, the fundamental aspects of the PCET mechanisms in these processes are more easily studied with model systems. Numerous experimental studies of model systems have been performed to elucidate the mechanism of tyrosine oxidation.[11–18] In some cases, photoexcitation of the metal in tyrosine-bound metal polypyridyl systems induces electron transfer from the tyrosine to the metal with concurrent proton transfer from the tyrosine to the solvent or the buffer.[14–18] Other experiments involve the chemical oxidation of phenols in solution.[11, 12] Often the data are interpreted in the context of Marcus theory for electron transfer.[19, 20]

A variety of theoretical approaches have been developed to study PCET reactions.[21–30] In the vibronically nonadiabatic formulation for PCET, [25–27] the active electrons and transferring proton are treated quantum mechanically, and the PCET reaction is described in terms of nonadiabatic transitions between pairs of reactant and product mixed electron-proton vibronic states. The dynamics of the proton donor-acceptor mode and the solvent/protein environment can be included in this formulation. Rate expressions based on linear response theory and the Golden Rule have been derived in various well-defined limits.[25,27] Methods for calculating the vibronic couplings in PCET systems have also been developed and implemented.[28,31] These theoretical approaches enable the calculation of rates and deuterium kinetic isotope effects (i.e., the ratio of the rate for hydrogen to the rate for deuterium), as well as their temperature and pH dependences.[32–35] Applications of these theoretical approaches to a wide range of systems have provided insight into fundamental concepts relevant to the PCET mechanisms in bioenergetic processes.

This review centers on PCET reactions that occur in a single chemical step (i.e., the electron and proton transfer simultaneously without an experimentally observable intermediate). In many cases, this type of PCET mechanism enables the system to avoid high-energy intermediates. Alternative sequential electron and proton transfer mechanisms[36] can be investigated with methods designed for studying single electron and single proton transfer reactions. The remainder of the review is organized as follows. Section II summarizes the vibronically nonadiabatic theoretical formulation for PCET reactions, providing the rate expressions in various limits and methods for calculating the vibronic couplings. Section III presents three applications of these theoretical approaches. The first application is the investigation of the detailed mechanism for tyrosyl radical generation in a tyrosine-bound rhenium polypyridyl complex that has recently been studied experimentally.[14,37] The second application is the calculation and analysis of the vibronic couplings for the phenoxyl/phenol and benzyl/toluene self-exchange reactions.[31] The third application is the study of the PCET reaction catalyzed by the enzyme soybean lipoxygenase, with an emphasis on the dynamical role of the enzyme and the magnitude and temperature dependence of the kinetic isotope effect.[34,35] Section IV presents a summary and discussion of potential future directions.

This subsection summarizes the dynamical formulation for PCET reactions.[27] A PCET reaction is vibronically nonadiabatic when the vibronic coupling is significantly less than the thermal energy *k*_{B}*T*. In this formulation, the active electrons and transferring proton are treated quantum mechanically, and the PCET reaction is described in terms of nonadiabatic transitions between pairs of reactant and product mixed electron-proton vibronic states. In the derivation of the rate expression, the nonadiabatic rate constant is expressed as the time integral of the probability flux correlation function, which in turn is expressed in terms of time correlation functions of the energy gap (i.e., the difference between the energies of the reactant and product states) and the *R* coordinate, where *R* is the distance between the proton donor and acceptor. The nonadiabatic coupling *V _{μν}* between the reactant and product vibronic states

$${V}_{\mu \nu}(R)\approx {V}_{\mu \nu}^{(0)}exp\left[-{\alpha}_{\mu \nu}(R-{\overline{R}}_{\mu})\right],$$

(1)

where * _{μ}* is the equilibrium value of the

As will be discussed in the next subsection, the vibronic coupling can be approximated as *V _{μν}* (

Using linear response theory in conjunction with the Golden Rule and the form of the vibronic coupling given in Eq. (1), we derived a series of rate expressions based on well-defined approximations that have been tested for various systems. Two approximations that were found to be valid for the systems studied are: (1) only the initial value of the energy gap correlation function impacts the rate and (2) the *R*-coordinate correlation function can be represented by the analytical expression for an undamped classical mechanical harmonic oscillator. These two approximations lead to the rate expression[38,39]

$$k=\sum _{\mu}{P}_{\mu}\sum _{\nu}\frac{{\left|{V}_{\mu \nu}^{(0)}\right|}^{2}}{\hslash}exp\left[\frac{2{k}_{\text{B}}T{\alpha}_{\mu \nu}^{2}}{M{\mathrm{\Omega}}^{2}}\right]\sqrt{\frac{\pi}{({\lambda}_{\mu \nu}+{\lambda}_{\alpha}){k}_{\text{B}}T}}exp\left[-\frac{{\left(\mathrm{\Delta}{G}_{\mu \nu}^{0}+{\lambda}_{\mu \nu}\right)}^{2}}{4({\lambda}_{\mu \nu}+{\lambda}_{\alpha}){k}_{\text{B}}T}\right],$$

(2)

where the summations are over the reactant and product vibronic states, *P _{μ}* is the Boltzmann probability for the reactant state, is the Boltzmann constant,
$\mathrm{\Delta}{G}_{\mu \nu}^{0}$ is the driving force, Ω and

Invoking the additional approximation that the *R*-coordinate time correlation function is approximately constant on the timescale of the probability flux correlation function decay leads to the simpler expression[35]

$$k=\sum _{\mu}{P}_{\mu}\sum _{\nu}\frac{{\left|{V}_{\mu \nu}^{(0)}\right|}^{2}}{\hslash}exp\left[\frac{2{k}_{\text{B}}T{\alpha}_{\mu \nu}^{2}}{M{\mathrm{\Omega}}^{2}}\right]\sqrt{\frac{\pi}{{\lambda}_{\mu \nu}{k}_{\text{B}}T}}exp\left[-\frac{{\left(\mathrm{\Delta}{G}_{\mu \nu}^{0}+{\lambda}_{\mu \nu}\right)}^{2}}{4{\lambda}_{\mu \nu}{k}_{\text{B}}T}\right].$$

(3)

This rate expression is similar to the Marcus theory expression for electron transfer except for the factor of
$exp\left[2{k}_{\text{B}}T{\alpha}_{\mu \nu}^{2}/M{\mathrm{\Omega}}^{2}\right]$. It differs from Eq. (2) by the absence of the term *λ _{α}* in the two denominators. Thus, the approximation leading from Eq. (2) to Eq. (3) is equivalent to the assumption that

An alternative derivation of Equation (3) provides additional connections to previous studies. Starting with the nonadiabatic PCET rate expression[25] derived for fixed *R*, the *R*-dependence of the vibronic coupling can be included according to the form in Eq. (1) and thermally averaged over a Boltzmann distribution for *R*. This procedure leads directly to Eq. (3) because

$${\int}_{-\infty}^{\infty}{P}^{\text{cl}}(R)exp\left[-2\alpha (R-\overline{R})\right]dR=exp\left[2{k}_{\text{B}}T{\alpha}^{2}/M{\mathrm{\Omega}}^{2}\right]$$

where

$${P}^{\text{cl}}(R)=exp\left[-M{\mathrm{\Omega}}^{2}{(R-\overline{R})}^{2}/(2{k}_{\text{B}}T)\right]/{\int}_{-\infty}^{\infty}exp\left[-M{\mathrm{\Omega}}^{2}{(R-\overline{R})}^{2}/(2{k}_{\text{B}}T)\right]dR.$$

This approach is based on the assumptions that the reorganization energy and reaction free energy are independent of *R*, the *R* mode behaves as a classical harmonic oscillator, and the vibronic coupling depends exponentially on *R*. This relation provides a connection to the rate expression of Kuznetsov and Ulstrup[46] as implemented by Klinman and coworkers, [47,48] where the Marcus theory expression for nonadiabatic electron transfer is modified by the inclusion of *R*-dependent Franck-Condon overlap terms for the transferring hydrogen, thermally averaged over a Boltzmann distribution for *R*. Their rate expression leads to Eq. (3) if the overlap between the reactant and product proton vibrational wavefunctions is assumed to depend exponentially on *R*, as in Eq. (1) with
${V}_{\mu \nu}^{(0)}={V}^{\text{el}}{S}_{\mu \nu}^{(0)}$. Thermal averaging over a Boltzmann distribution for *R* can also be performed numerically for a general form of the overlap between the reactant and product proton vibrational wavefunctions.

All of the quantities in the rate expressions above can be calculated from classical molecular dynamics simulations on the reactant surface and quantum mechanical calculations of the vibronic couplings. In linear response theory, the reorganization energy *λ _{μν}* can be expressed in terms of the energy gap variance
$\langle \mathcal{E}{\mathcal{E}}_{\mu \nu}^{2}\rangle $ as

$${\lambda}_{\mu \nu}=\frac{\langle \mathcal{E}{\mathcal{E}}_{\mu \nu}^{2}\rangle}{2{k}_{\text{B}}T},$$

(4)

and the driving force can be calculated as
$\mathrm{\Delta}{G}_{\mu \nu}^{0}=-\langle {\mathcal{E}}_{\mu \nu}\rangle -{\lambda}_{\mu \nu}$. The average *R* coordinate and the quantity *k*_{B}*T/M*Ω^{2} = *δR*_{2} can also be calculated directly from the molecular dynamics simulations. The mass *M* and frequency Ω can be determined independently by fitting the *R*-coordinate time correlation function from the classical molecular dynamics to the corresponding analytical expression for an undamped classical harmonic oscillator for the relevant time scale. The magnitude and distance dependence of the vibronic coupling (i.e.,
${V}_{\mu \nu}^{(0)}$ and *α _{μν}* in Eq. (1)) can be determined from quantum mechanical methods described in the next section. For additional simplification, the reorganization energy can be assumed to be the same for all pairs of reactant and product states, so the reorganization energy and driving force can be calculated for the ground reactant and product states (i.e.,

The rate expression in Eq. (3) leads to a relatively simple expression for the KIE because only the first two factors depend on the isotope. If only the nonadiabatic transition between the two ground states is considered, the KIE can be approximated as[35]

$$\text{KIE}\approx \frac{{\mid {S}_{H}\mid}^{2}}{{\mid {S}_{D}\mid}^{2}}exp\left\{\frac{2{k}_{\text{B}}T}{M{\mathrm{\Omega}}^{2}}\left({\alpha}_{H}^{2}-{\alpha}_{D}^{2}\right)\right\},$$

(5)

where *S _{H}* and

The rate expressions above can be modified to include the quantum mechanical effects of the *R* coordinate motion. In this case, *λ _{α}* is replaced by
$\frac{{\lambda}_{\alpha}}{2{k}_{\text{B}}T}\hslash \mathrm{\Omega}coth\left(\frac{\hslash \mathrm{\Omega}}{2{k}_{\text{B}}T}\right)$ in Eq. (2), and
$exp\left[\frac{2{k}_{\text{B}}T{\alpha}_{\mu \nu}^{2}}{M{\mathrm{\Omega}}^{2}}\right]$ is replaced by
$exp\left[\frac{\hslash {\alpha}_{\mu \nu}^{2}}{M\mathrm{\Omega}}coth\left(\frac{\hslash \mathrm{\Omega}}{2{k}_{\text{B}}T}\right)\right]$ in Eqs. (2) and (3). Analogous to the classical treatment of the

$${\int}_{-\infty}^{\infty}{P}^{\text{qu}}(R)exp\left[-2\alpha (R-\overline{R})\right]dR=exp\left[{\alpha}^{2}\hslash coth(\hslash \mathrm{\Omega}/2{k}_{\text{B}}T)/M\mathrm{\Omega}\right]$$

where

$${P}^{\text{qu}}(R)=\sqrt{M\mathrm{\Omega}tanh(\hslash \mathrm{\Omega}/2{k}_{\text{B}}T)/\pi \hslash}exp\left[-M\mathrm{\Omega}tanh(\hslash \mathrm{\Omega}/2{k}_{\text{B}}T){(R-\overline{R})}^{2}/\hslash \right].$$

. Note that these modified expressions lead to the original expressions given above for the classical limit ĦΩ *K*_{B}*T*.

According to the Golden Rule, the rate of a nonadiabatic PCET reaction is proportional to the square of the nonadiabatic vibronic coupling *V _{μν}* between the reactant and product diabatic vibronic states. This vibronic coupling is defined to be the Hamiltonian matrix element between the reactant and product mixed electronic-proton vibrational wavefunctions. The overall reaction is vibronically nonadiabatic with respect to the solvent or protein environment when this vibronic coupling is much less than

Even for vibronically nonadiabatic PCET reactions, the proton tunneling can be electronically nonadiabatic, electronically adiabatic, or in the intermediate regime. Here the electronically nonadiabatic and adiabatic limits for general PCET reactions refer to the relative timescales of the electrons and the transferring proton. The electrons respond instantaneously to the proton motion in the electronically adiabatic limit but not in the electronically nonadiabatic limit. In the electronically nonadiabatic limit, the vibronic coupling
${V}_{\mu \nu}^{(\text{na})}$ can be expressed as the product of the electronic coupling *V*^{el} and the Franck-Condon overlap *S _{μν}* of the reactant and product proton vibrational wavefunctions:

$${V}_{\mu \nu}^{(\text{na})}={V}^{\text{el}}{S}_{\mu \nu}.$$

(6)

In the electronically adiabatic limit, the proton dynamics occur on the electronically adiabatic ground state potential energy surface, and the vibronic coupling ${V}_{\mu \nu}^{(\text{ad})}$ can be calculated by standard semiclassical methods.[49,50] For a symmetric system, the vibronic coupling ${V}_{\mu \nu}^{(\text{ad})}$ is half the splitting between the symmetric and antisymmetric proton vibrational states for the electronic ground state potential energy surface.

In general, PCET reactions can be in the intermediate regime between the electronically nonadiabatic and adiabatic limits. Georgievskii and Stuchebrukhov[28] derived a semiclassical expression for the general vibronic coupling ${V}_{\mu \nu}^{(\text{sc})}$:

$${V}_{\mu \nu}^{(\text{sc})}=\kappa {V}_{\mu \nu}^{(\text{ad})}$$

(7)

where the factor κ is defined as

$$\kappa =\sqrt{2\pi p}\frac{{e}^{\mathit{p}lnp-p}}{\mathrm{\Gamma}(p+1)}.$$

(8)

In Eq. (8), Γ(*x*) is the gamma-function and *p* is the proton adiabaticity parameter defined as

$$p=\frac{{\mid {V}^{\text{el}}\mid}^{2}}{\hslash \mid \mathrm{\Delta}F\mid {v}_{t}},$$

(9)

where *v _{t}* is the tunneling velocity of the proton at the crossing point of the two proton potential energy curves and |Δ

$${v}_{t}=\sqrt{\frac{2({V}_{c}-E)}{m}}.$$

(10)

In the electronically adiabatic limit, *p*1, κ = 1, and the vibronic coupling simplifies to
${V}_{\mu \nu}^{(\text{ad})}$. In the electronically nonadiabatic limit, *p*1,
$\kappa =\sqrt{2\pi p}$, and the vibronic coupling reduces to
${V}_{\mu \nu}^{(\text{na})}$, as given in Eq. (6).

The adiabaticity of a general PCET reaction can be viewed in terms of the relative times of the proton tunneling and the electronic transition. Within the semiclassical framework, the time spent by the tunneling proton in the crossing region (i.e., the proton tunneling time) is

$${\tau}_{\text{p}}\sim \frac{{V}^{\text{el}}}{\mid \mathrm{\Delta}F\mid {\nu}_{t}}$$

(11)

and the time required to change the electronic state (i.e., the electronic transition time) is

$${\tau}_{\text{e}}\sim \frac{\hslash}{{V}^{\text{el}}}.$$

(12)

The adiabaticity parameter is simply the ratio of these two times:

$$p=\frac{{\tau}_{\text{p}}}{{\tau}_{\text{e}}}.$$

(13)

When the proton tunneling time is much longer than the electronic transition time, the electronic states have enough time to mix completely and the proton transfer occurs on the electronically adiabatic ground state surface (i.e., the reaction is electronically adiabatic). When the proton tunneling time is much less than the electronic transition time, the reaction is electronically nonadiabatic because the electronic states no longer have enough time to mix completely during the proton tunneling process.

The vibronic couplings can be calculated with several different methods. As shown in Ref. [31], the input quantities for the semiclassical vibronic coupling expressions given above can be calculated with conventional electronic structure methods. Alternatively, the Hamiltonian matrix element between the reactant and product diabatic vibronic states can be calculated with the nuclear-electronic orbital (NEO) method.[51] In the NEO method, mixed nuclear-electronic wavefunctions are calculated with molecular orbital techniques. The diabatic vibronic states can be defined to be the two nonorthogonal localized nuclear-electronic wavefunctions obtained at the NEO-HF (Hartree-Fock) level. The Hamiltonian matrix element between these two diabatic vibronic states can be calculated with the NEO-NOCI (nonorthogonal configuration interaction) approach.[52] The NEO-NOCI method has been shown to agree well with the semiclassical methods for the phenoxyl/phenol system.[53]

Numerous experimental studies of model systems have been performed to study the fundamental mechanism of tyrosine oxidation.[11–18] For example, Sjodin et al. studied tyrosine-bound ruthenium-tris-bipyridine model systems with the flash-quench method.[15–18] In these experiments, the excited state of Ru is quenched by an external quencher, followed by electron transfer from the tyrosine to the photo-oxidized Ru. Sjödin et al. explained the pH dependence of the experimentally measured rate constant in terms of a PCET mechanism in which the proton transfers from tyrosine to bulk water.[15–18] Our theoretical calculations on this model system were consistent with this interpretation.[32] Alternative interpretations of this type of pH-dependence have also been proposed.[12,36] To avoid the use of external quenchers, Reece and Nocera designed and studied tyrosine-bound rhenium polypyridyl complexes.[14] In these experiments, tyrosine radicals are produced directly from the metal-to-ligand charge transfer (MLCT) excited state without an external quencher. The rate constant for emission quenching for this complex increases with pH in the range 4 < pH < 9 in the presence of phosphate buffer. In addition, the rate constant is independent of pH for 4 < pH < 8 in the absence of the phosphate buffer, and the dependence of the rate on phosphate buffer concentration is absent at low pH, where the dominant buffer species is H_{2}PO_{4}^{−}.[54] These experimental observations are consistent with a PCET mechanism in which the proton is transferred from the tyrosine to the phosphate buffer species HPO_{4}^{2−} for 4 < pH < 9.[54]

Recently, we used our multistate continuum theory[24–26] for PCET reactions to investigate the detailed mechanism for tyrosyl radical generation in the [Re(P-Y)(phen)(CO)_{3}]PF_{6} system, where phen denotes 1,10-phenanthroline and P-Y denotes triphenylphosphine-tyrosine. This system is depicted in Figure 1. We evaluated two different models for tyrosyl radical generation in this system. In the phosphate-acceptor model, the phosphate buffer species HPO_{4}^{2−} serves as the proton acceptor, and the pH-dependence of the overall rate arises from the titration between the HPO_{4}^{2−} and H_{2}PO_{4}^{−} forms of the phosphate buffer. In the water-acceptor model, bulk water serves as the proton acceptor. Our calculations indicate that the phosphate-acceptor model can successfully reproduce the experimentally observed pH-dependence of the overall rate and H/D KIE, whereas the water-acceptor model is not physically reasonable for this system. The phosphate buffer species HPO_{4}^{2−} is favored over water as the proton acceptor in part because the proton donor-acceptor distance is ~0.2 Å smaller for the phosphate acceptor due to its negative charge. This smaller proton donor-acceptor distance leads to a larger vibronic coupling because of the greater overlap between the reactant and product proton vibrational wavefunctions. Other factors differentiating these two mechanisms include the slightly smaller outer-sphere reorganization energy for PCET in the phosphate-acceptor model and the differences in driving forces for PCET.

Here we review the results and analysis for the favored phosphate-acceptor model. In this model, the pH-dependence of the overall rate arises from the titration between the HPO_{4}^{2−} and H_{2}PO_{4}^{−} forms of the phosphate buffer, and the proton is assumed to transfer to HPO_{4}^{2−} but not to H_{2}PO_{4}^{−}. These assumptions are consistent with the experimental observations described above. Given these assumptions, the overall rate constant for tyrosine oxidation can be expressed as[54]

$${k}_{q}=\chi \left({\text{HPO}}_{4}^{2-}\right)\u2022{[\text{Phosphate}]}_{\text{T}}\u2022{k}_{\text{PCKT}}^{\text{bi}}+{k}_{\text{ET}}$$

(14)

where [Phosphate]_{T} is the total concentration of phosphate buffer and
$\chi ({\text{HPO}}_{4}^{2-})$ is the mole fraction of
${\text{HPO}}_{4}^{2-}$, which can be calculated as a function of pH using the relation

$$\chi ({\text{HPO}}_{4}^{2-})={({10}^{{\text{p}K}_{\text{a}}-PH}+1)}^{-1}$$

(15)

with pK_{a} of 7.2 for HPO_{4}^{2−}. In Eq. (14),
${k}_{\text{PCET}}^{\text{bi}}$ is the bimolecular rate constant for the PCET reaction in which the proton is transferred to HPO_{4}^{2−}, and *k*_{ET} is the rate constant for an ET reaction that is followed by rapid PT to the solvent.[54] The ET rate constant was determined to be *k*_{ET} = 1.0 ± 0.2 × 10^{5} s^{−1} from experimental measurements in the absence of phosphate buffer. The bimolecular PCET rate constant was determined to be
${k}_{\text{PCET}}^{\text{bi}}=1.7\pm 0.1\times {10}^{7}{\text{M}}^{-1}{\text{s}}^{-1}$ from measurements of *k _{q}* as a function of phosphate buffer concentration at different pH values. The H/D KIE for the bimolecular PCET rate constant
${k}_{\text{PCET}}^{\text{bi}}$ was determined to be ~3.0 from measurements of

We calculated the overall rate *k _{q}* for hydrogen and deuterium transfer using the expression in Eq. (14) in conjunction with our PCET expression in Eq. (3) for

Analysis of the PCET calculations provides insight into the reorganization energies, reaction free energies, activation free energies, and vibronic couplings for the various pairs of reactant/product vibronic states for both hydrogen and deuterium transfer. Based on experimental measurements for a related system, [56] the inner-sphere reorganization energy is estimated to be 9.8 kcal/mol. The calculated outer-sphere reorganization energy for the overall PCET reaction was ~ 33 kcal/mol for all pairs of vibronic states. The dominant contribution to the rate arose from nonadiabatic transitions between the ground reactant state and the third product state for hydrogen transfer and the fourth product state for deuterium transfer. These contributions exceed the contributions from the nonadiabatic transition between the ground reactant and product states because the larger vibronic coupling overrides the slightly higher activation free energy barrier. The larger vibronic coupling is due mainly to the greater overlap between the reactant and product proton vibrational wavefunctions. This effect is more pronounced for deuterium than for hydrogen. The free energy surfaces and the corresponding proton vibrational wavefunctions are depicted in Figure 3.

Analysis of the free energy surfaces for the PCET reaction in the phosphate-acceptor model for the rhenium-tyrosine complex. In the center frame are slices of the two-dimensional ET diabatic free energy surfaces as functions of the solvent coordinates. **...**

These calculations provide insight into the fundamental mechanism of tyrosyl radical generation. Such insights have implications for PCET in PS II. For example, the conclusion that the phosphate serves as a proton acceptor is consistent with experimental observations in D1-His190 mutants of PSII, where the rates of P680^{+•} reduction by Y_{z} increased dramatically in the presence of imidazole and other small organic bases.[57,58]

We have calculated the vibronic couplings for the phenoxyl/phenol and the benzyl/toluene self-exchange reactions. As discussed above, the vibronic couplings significantly impact the rates and kinetic isotope effects, as well as their temperature dependences, for general PCET reactions. Although the splittings between the ground and excited electronic states are significantly larger than the thermal energy *k _{B}T* at room temperature for these systems, the vibronic couplings for both systems were found to be smaller than

As shown in Figure 4, the electronic wavefunctions for the two systems are qualitatively different at the transition state. In the phenoxyl/phenol system, the two highest-energy occupied molecular orbitals are dominated by 2*p* orbitals on the donor and acceptor oxygen atoms that are perpendicular to the hydrogen donor-acceptor axis. In the ground state, the doubly occupied molecular orbital corresponds to π-bonding, and the singly occupied molecular orbital corresponds to π-antibonding. In the benzyl/toluene system, the two highest-energy occupied molecular orbitals are dominated by σ orbitals on the donor and acceptor carbon atoms and are oriented along the hydrogen donor-acceptor axis. In the ground state, the highest doubly occupied molecular orbital corresponds to σ-bonding, and the singly occupied molecular orbital corresponds to σ-antibonding. Previously Mayer, Borden, and coworkers[59] used these differences in the singly occupied molecular orbitals of the transition state wavefunctions to designate the phenoxyl/phenol and benzyl/tolune systems as PCET and hydrogen atom transfer (HAT), respectively.

The two highest-energy occupied electronic molecular orbitals for (a) the phenoxyl/phenol and (b) the benzyl/toluene system. The electronic wavefunctions for diabatic states I and II are calculated at the minima of the ground state electronically adiabatic **...**

Figure 5 depicts the potential energy curves along the transferring hydrogen coordinate for the phenoxyl/phenol and the benzyl/toluene systems. The CASSCF electronically adiabatic ground and excited state curves, as well as the electronically diabatic curves corresponding to the reactant and product electron transfer states, are depicted. Note that the splitting between the electronically adiabatic ground and excited states is more than an order of magnitude larger for the benzyl/toluene system than for the phenoxyl/phenol system. As a result, the diabatic curves are very similar to the adiabatic curves for the phenoxyl/phenol system but are significantly different from the adiabatic curves for the benzyl/toluene system.

State-averaged CASSCF ground and excited state electronically adiabatic potential energy curves along the transferring hydrogen coordinate for (a) the phenoxyl/phenol and (b) the benzyl/toluene system. The coordinates of all nuclei except the transferring **...**

The fundamental nature of the proton tunneling is different for the two systems. For the phenoxyl/phenol system, the adiabaticity parameter *p* is very small,
$\kappa \approx \sqrt{2\pi p}$, and *τ*_{e} ≈ 80*τ*_{p}. In this case, the electronic transition time is significantly greater than the proton tunneling time. As a result, the electrons are not able to rearrange fast enough for the proton to move on the electronically adiabatic ground state surface, and the proton transfer reaction is electronically nonadiabatic. For the benzyl/toluene system, the adiabaticity parameter *p* is larger, *κ* ≈ 1, and *τ*_{p} ≈ 4*τ*_{e}. In this case, the electronic transition time is less than the proton tunneling time. Thus, the electrons can respond instantaneously to the proton motion, and the proton moves on the electronically adiabatic ground state surface. This analysis indicates that the proton tunneling is electronically nonadiabatic for the phenoxyl/phenol system but electronically adiabatic for the benzyl/toluene system.

Figure 6 illustrates the physical principles underlying the electronically nonadiabatic and adiabatic limits. For the electronically nonadiabatic phenoxyl/phenol reaction, the vibronic coupling is the product of the electronic coupling between the diabatic states and the overlap of the reactant and product proton vibrational wavefunctions corresponding to these diabatic states. For the electronically adiabatic benzyl/toluene reaction, the vibronic coupling is half the energy splitting between the states corresponding to the symmetric and antisymmetric proton vibrational wavefunctions for the electronically adiabatic ground state.

(a) Diabatic potential energy curves corresponding to the two localized diabatic electron transfer states I and II and the corresponding proton vibrational wavefunctions
${\varphi}_{\mu}^{(\text{I})}$ (blue) and
${\varphi}_{\nu}^{(\text{II})}$ (red) for the phenoxyl/phenol **...**

We also examined the dependence of the vibronic coupling on the proton donor-acceptor distance and the dependence of the KIE on both the magnitude and the distance dependence of the vibronic coupling. The vibronic coupling decreases exponentially with the proton donor-acceptor distance for both electronically adiabatic and electronically nonadiabatic reactions in the range of chemically relevant distances. For a given proton donor-acceptor distance, the vibronic couplings are significantly smaller for deuterium than for hydrogen because of the smaller overlap between the reactant and product proton vibrational wavefunctions for deuterium. Moreover, the value of the exponential decay parameter *α* is larger for deuterium than for hydrogen because the overlap between the reactant and product deuterium wavefunctions falls off faster with distance than the corresponding overlap for the hydrogen wavefunctions. These trends are directly relevant to the study of general PCET reactions.

This type of analysis provides a new perspective on the distinction between PCET and HAT reactions. A conventional method for distinguishing PCET from HAT is that the electron and proton are transferred between different donors and acceptors (or different sets of orbitals) for PCET. Within this framework, our analysis suggests that PCET reactions are electronically nonadiabatic, whereas HAT reactions are electronically adiabatic. These two mechanisms can be differentiated by calculating the adiabaticity parameter, which depends on the electronic coupling and other quantities that can be determined with quantum chemistry methods.

Furthermore, the distinction between electronic adiabaticity and nonadiabaticity has important experimental consequences because the vibronic couplings can be substantially different in the electronically adiabatic and nonadiabatic limits. As discussed above, the magnitude and distance dependence of the vibronic coupling can significantly impact the magnitudes and temperature dependences of the rates and the KIEs. Thus, the calculation of the vibronic coupling in the correct limit, or in the intermediate regime, is critical for the interpretation of experimental data and the generation of experimentally testable predictions.

We have examined the dynamical behavior and the temperature dependence of the kinetic isotope effects for the PCET reaction catalyzed by the enzyme soybean lipoxygenase (SLO).[35] Lipoxygenases catalyze the oxidation of unsaturated fatty acids. Kinetic studies have shown that the hydrogen abstraction step in SLO is rate-limiting above 32 °C.[60] In this step, the pro-*S* hydrogen atom from carbon atom C11 of the linoleic acid substrate is transferred to the Fe(III)–OH cofactor, forming a radical intermediate substrate and Fe(II)–OH_{2}.[61] Quantum mechanical calculations[62] and analysis of the thermodynamic properties based on electrochemical data[34,48] indicate that the hydrogen abstraction step occurs by a PCET mechanism, in which the electron transfers from the π-system of the substrate to the iron of the cofactor, while the proton transfers from the C11 carbon of the substrate to the hydroxyl ligand of the cofactor. This PCET reaction is depicted in Figure 7. The SLO reaction has been studied with a variety of theoretical approaches.[34,35,47,48,61–70]

The hydrogen abstraction step of the reaction catalyzed by soybean lipoxygenase with its natural substrate linoleic acid. In this step, a hydrogen is abstracted from the linoleic acid to the iron cofactor. Figure reproduced with permission from Ref.[ **...**

Our calculations of this reaction were based on the vibronically nonadiabatic formulation for PCET reactions that includes the quantum mechanical effects of the active electrons and the transferring proton, as well as the motions of all atoms in the complete solvated enzyme system.[27,39] As described above, the rate is represented by the time integral of a probability flux correlation function that depends on the vibronic coupling, the average of the energy gap and *R* coordinate, and the time correlation functions of the energy gap and *R* coordinate. The vibronic couplings were estimated to within a constant factor by calculating the overlaps between reactant and product hydrogen vibrational wavefunctions for model systems, and the other quantities were calculated from classical molecular dynamics simulations of the entire system.

We tested the underlying assumptions of this vibronically nonadiabatic formulation for the SLO enzyme reaction and investigated the dynamical behavior of the protein, substrate, and cofactor. Our estimates of the contributions to the vibronic couplings for this PCET reaction indicated that this reaction is vibronically nonadiabatic. Moreover, our molecular dynamics simulations of the entire solvated enzyme system provided an estimate of 39 kcal/mol for the total reorganization energy. We found that the dynamical behavior (i.e., the time dependence) of the probability flux correlation function is dominated by the equilibrium protein and solvent motions and is not significantly influenced by the proton donor-acceptor motion. The magnitude of the overall rate, however, is strongly influenced by the frequency of the proton donor-acceptor motion, the magnitude and distance dependence of the vibronic coupling, and the protein/solvent reorganization energy.

These calculations reproduced the experimentally observed[48,61] magnitude and temperature dependence of the KIE for the SLO enzyme reaction without fitting any parameters directly to the experimental kinetic data. A comparison of the experimental and calculated data is depicted in Figure 8. The temperature dependence of the KIE is determined mainly by the effective proton donor-acceptor frequency, which can be calculated from the *R* coordinate variance in the molecular dynamics simulations, and the distance dependence of the vibronic couplings for hydrogen and deuterium, which can be calculated from the vibrational wavefunctions for model systems. The ratio of the overlaps of the hydrogen and deuterium vibrational wavefunctions strongly impacts the magnitude of the KIE but does not significantly influence the temperature dependence. These trends are summarized in the relatively simple, approximate expression for the KIE given in Eq. (5). For the SLO reaction, the large magnitude of the KIE arises mainly from the dominance of tunneling between the ground vibronic states and the relatively large ratio of the overlaps between the corresponding hydrogen and deuterium vibrational wavefunctions. The weak temperature dependence of the KIE is due in part to the dominance of the local component of the proton donor-acceptor motion.

In this review, we described the vibronically nonadiabatic theoretical formulation for PCET reactions and presented rate expressions in various limits, as well as methods for calculating the vibronic couplings. We illustrated this methodology through three different applications. In the first application, we investigated tyrosyl radical generation in a tyrosine-bound rhenium polypyridyl complex. The experimental data and theoretical calculations indicate that the electron transfers from the tyrosine to the photoexcited rhenium concurrently with the proton transferring to the phosphate buffer. In the second application, we calculated the vibronic couplings for the phenoxyl/phenol and benzyl/toluene self-exchange reactions and found that the proton transfer reaction is electronically nonadiabatic for phenoxyl/phenol, which was designated as PCET, but electronically adiabatic for benzyl/toluene, which was designated as HAT. The analysis of these couplings provided a new diagnostic for differentiating between the conventionally defined PCET and HAT reactions. In the third application, we simulated the PCET reaction catalyzed by the enzyme lipoxygenase. The simulations elucidated the dynamical role of the enzyme and the physical basis for the experimental observations of an unusually large KIE with relatively weak temperature dependence.

These theoretical studies provide insight into fundamental concepts relevant to PCET mechanisms in bioenergetic processes. The feedback between experiment and theory plays an essential role in these types of studies. In principle, these theoretical approaches could be applied to model systems that are more directly related to specific biological systems such as PSII. The calculation of reorganization energies, vibronic couplings, rates, and KIEs for PCET reactions in complex bioenergetic systems would provide new insights into the overall mechanisms. Such calculations represent an exciting and challenging direction for future research.

We are grateful for support of this work by NSF grant CHE-05-01260 and NIH grant GM56207.

**Publisher's Disclaimer: **This is a PDF file of an unedited manuscript that has been accepted for publication. As a service to our customers we are providing this early version of the manuscript. The manuscript will undergo copyediting, typesetting, and review of the resulting proof before it is published in its final citable form. Please note that during the production process errors may be discovered which could affect the content, and all legal disclaimers that apply to the journal pertain.

1. Debus RJ. Biochimica et Biophysica Acta. 1992;1102:269. [PubMed]

2. Barber J, Andersson B. Nature. 1994;370:31.

3. Diner BA, Babcock GT. In: Oxygenic Photosynthesis: The Light Reactions. Ort DR, Yocum CF, editors. Kluwer; Dordrecht, The Netherlands: 1996. pp. 213–47.

4. Tommos C, Tang X-S, Warncke K, Hoganson CW, Styring S, McCracken J, Diner BA, Babcock GT. Journal of the American Chemical Society. 1995;117:10325–35.

5. Hoganson CW, Lydakis-Simantiris N, Tang X-S, Tommos C, Warncke K, Babcock GT, Diner BA, McCracken J, Styring S. Photosynthesis Research. 1995;47:177–84. [PubMed]

6. Hoganson CW, Babcock GT. Science. 1997;277:1953–56. [PubMed]

7. Blomberg MRA, Siegbahn PEM, Styring S, Babcock GT, Akermark B, Korall P. Journal of the American Chemical Society. 1997;119:8285–92.

8. Kuhne H, Brudvig GW. Journal of Physical Chemistry B. 2002;106:8189–96.

9. Loll B, Kern J, Saenger W, Zouni A, Biesiadka J. Nature. 2005;438:1040–44. [PubMed]

10. Groot ML, Pawlowicz NP, van Wilderen LJGW, Breton J, van Stokkum IHM, van Grondelle R. Proceedings of the National Academy USA. 2005;102:13087–92. [PubMed]

11. Rhile IJ, Mayer JM. Journal of the American Chemical Society. 2004;126:12718–19. [PubMed]

12. Fecenko CJ, Meyer TJ, Thorp HH. Journal of the American Chemical Society. 2006;128:11020–21. [PubMed]

13. Costentin C, Robert M, Saveant J-M. Journal of the American Chemical Society. 2006;128:4552–53. [PubMed]

14. Reece SY, Nocera DG. Journal of the American Chemical Society. 2005;127:9448–58. [PubMed]

15. Sjodin M, Styring S, Akermark B, Sun L, Hammarstrom L. Journal of the American Chemical Society. 2000;122:3932–36.

16. Sjodin M, Styring S, Akermark B, Sun L, Hammarstrom L. Phil Trans R Soc Lond B. 2002;357:1471–79. [PMC free article] [PubMed]

17. Sjodin M, Ghanem R, Polivka T, Pan J, Styring S, Sun L, Sundstrom V, Hammarstrom L. Phys Chem Chem Phys. 2004;6:4851–58.

18. Sjodin M, Styring S, Wolpher H, Xu Y, Sun L, Hammarstrom L. Journal of the American Chemical Society. 2005;127:3855–63. [PubMed]

19. Marcus RA. Annual Reviews of Physical Chemistry. 1964;15:155–96.

20. Marcus RA, Sutin N. Biochimica et Biophysica Acta. 1985;811:265–322.

21. Cukier RI. Journal of Physical Chemistry. 1996;100:15428–43.

22. Cukier RI, Nocera DG. Annual Reviews of Physical Chemistry. 1998;49:337–69. [PubMed]

23. Cukier RI. Biochimica et Biophysica Acta-Bioenergetics. 2004;1655:37–44. [PubMed]

24. Hammes-Schiffer S. Accounts of Chemical Research. 2001;34:273–81. [PubMed]

25. Soudackov A, Hammes-Schiffer S. Journal of Chemical Physics. 2000;113:2385–96.

26. Soudackov A, Hammes-Schiffer S. Journal of Chemical Physics. 1999;111:4672–87.

27. Soudackov A, Hatcher E, Hammes-Schiffer S. Journal of Chemical Physics. 2005;122:014505.

28. Georgievskii Y, Stuchebrukhov AA. Journal of Chemical Physics. 2000;113:10438–50.

29. Mayer JM. Annual Review of Physical Chemistry. 2004;55:363–90. [PubMed]

30. Costentin C, Robert M, Saveant J-M. Journal of Electroanalytical Chemistry. 2006;588:197–206.

31. Skone JH, Soudackov AV, Hammes-Schiffer S. Journal of the American Chemical Society. 2006;128:16655. [PubMed]

32. Carra C, Iordanova N, Hammes-Schiffer S. Journal of the American Chemical Society. 2003;125:10429–36. [PubMed]

33. Hammes-Schiffer S, Iordanova N. Biochimica et Biophysica Acta-Bioenergetics. 2004;1655:29–36. [PubMed]

34. Hatcher E, Soudackov AV, Hammes-Schiffer S. Journal of the American Chemical Society. 2004;126:5763–75. [PubMed]

35. Hatcher E, Soudackov AV, Hammes-Schiffer S. Journal of the American Chemical Society. 2007;129:187–96. [PubMed]

36. Costentin C, Robert M, Saveant J-M. Journal of the American Chemical Society. 2007;129:5870–79. [PubMed]

37. Ishikita H, Soudackov AV, Hammes-Schiffer S. Journal of the American Chemical Society. 2007 (in press)

38. Hatcher E, Soudackov A, Hammes-Schiffer S. Chemical Physics. 2005;319:93–100.

39. Hatcher E, Soudackov A, Hammes-Schiffer S. Journal of Physical Chemistry B. 2005;109:18565–74. [PubMed]

40. Borgis D, Lee S, Hynes JT. Chemical Physics Letters. 1989;162:19–26.

41. Borgis D, Hynes JT. Journal of Chemical Physics. 1991;94:3619–28.

42. Suarez A, Silbey R. Journal of Chemical Physics. 1991;94:4809–16.

43. Trakhtenberg LI, Klochikhin VL, Pshezhetsky SY. Chemical Physics. 1982;69:121–34.

44. Kiefer PM, Hynes JT. Solid State Ionics. 2004;168:219–24.

45. Kiefer PM, Hynes JT. Journal of Physical Chemistry A. 2004;108:11793–808.

46. Kuznetsov AM, Ulstrup J. Canadian Journal of Chemistry. 1999;77:1085–96.

47. Knapp MJ, Klinman JP. European Journal of Biochemistry. 2002;269:3113–21. [PubMed]

48. Knapp MJ, Rickert KW, Klinman JP. Journal of the American Chemical Society. 2002;124:3865–74. [PubMed]

49. Vorotyntsev MA, Dogonadze RR, Kuznetsov AM. Dokl Akad Nauk SSSR. 1973;209:1135.

50. Fain B. Theory of Rate Processes in Condensed Media. Springer; New York: 1980.

51. Webb SP, Iordanov T, Hammes-Schiffer S. Journal of Chemical Physics. 2002;117:4106–18.

52. Skone JH, Pak MV, Hammes-Schiffer S. Journal of Chemical Physics. 2005;123:134108. [PubMed]

53. Ludlow MK, Skone JH, Hammes-Schiffer S. Journal of Physical Chemistry B. 2007 (submitted)

54. Reece SY, Nocera DG. personal communication.

55. Alev-Behmoaras T, Toulme JJ, Helene C. Photochemistry and Photobiology. 1979;30:533–39.

56. Reece SY, Seyedsayamdost MR, Stubbe J, Nocera DG. Journal of the American Chemical Society. 2006;128:13654–55. [PubMed]

57. Hays A-MA, Vassiliev IR, Golbeck JH, Debus RJ. Biochemistry. 1998;37:11352–65. [PubMed]

58. Hays A-MA, Vassiliev IR, Golbeck JH, Debus RJ. Biochemistry. 1999;38:11851–65. [PubMed]

59. Mayer JM, Hrovat DA, Thomas JL, Borden WT. Journal of the American Chemical Society. 2002;124:11142–47. [PubMed]

60. Glickman MH, Klinman JP. Biochemistry. 1995;34:14077–92. [PubMed]

61. Rickert KW, Klinman JP. Biochemistry. 1999;38:12218–28. [PubMed]

62. Lehnert N, Solomon EI. J Biol Inorg Chem. 2003;8:294–305. [PubMed]

63. Kuznetsov AM, Ulstrup J. Canadian Journal of Chemistry. 1999;77:1085–96.

64. Tresadern G, McNamara JP, Mohr M, Wang H, Burton NA, Hillier IH. Chemical Physics Letters. 2002;358:489–94.

65. Olsson MHM, Siegbahn PEM, Warshel A. Journal of the American Chemical Society. 2004;126:2820–28. [PubMed]

66. Olsson MHM, Siegbahn PEM, Warshel A. Journal of Biological Inorganic Chemistry. 2004;9:96–99. [PubMed]

67. Siebrand W, Smedarchina Z. Journal of Physical Chemistry B. 2004;108:4185–95.

68. Borowski T, Krol M, Chruszcz M, Broclawik E. Journal of Physical Chemistry B. 2001;105:12212–20.

69. Borowski T, Broclawik E. Journal of Physical Chemistry B. 2003;107:4639–46.

70. Tejero I, Eriksson LA, Gonzalez-Lafont A, Marquet J, Lluch JM. Journal of Physical Chemistry B. 2004;108:13831–38.

PubMed Central Canada is a service of the Canadian Institutes of Health Research (CIHR) working in partnership with the National Research Council's national science library in cooperation with the National Center for Biotechnology Information at the U.S. National Library of Medicine(NCBI/NLM). It includes content provided to the PubMed Central International archive by participating publishers. |