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Catalytic Effect of Aqueous Solution in Water-Assisted Proton Transfer Mechanism of 8-hydroxy Guanine Radical Peng Liu, Chen Li, Shengyu Wang, and Dunyou Wang J. Phys. Chem. B, Just Accepted Manuscript • DOI: 10.1021/acs.jpcb.7b09965 • Publication Date (Web): 08 Mar 2018 Downloaded from http://pubs.acs.org on March 9, 2018

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The Journal of Physical Chemistry

Catalytic Effect of Aqueous Solution in Water-assisted Proton Transfer Mechanism of 8-hydroxy Guanine Radical Peng Liu, Chen Li, Shengyu Wang, and Dunyou Wang* College of Physics and Electronics, Shandong Normal University, Jinan, 250014, China

*Corresponding Author. Electronic mail: [email protected] 1

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ABSTRACT Water-assisted proton transfer process is a key step in guanine damage reaction by hydroxyl radical in aqueous solution. In this article, we quantitatively determined the solvent effect in water-assisted proton transfer mechanism of 8-hydroxy guanine radical using combined quantum mechanics and molecular mechanism with an explicit solvation model. Atomic-level reaction pathway was mapped, which shows a synchronized two-proton transfer mechanism between the assistant water molecule and 8-hydroxy guanine radical. The transition state dipole moment is the largest along the

reaction

pathway

which

electrostatically

stabilizes

the

proton-transfer

transition-state complex. The free energy reaction barrier for this water-assisted proton

transfer

reaction

was

calculated

at

19.2

kcal/mol

with

the

DFT/M08-SO/cc-pVTZ+/MM level of theory. The solvent effect not only has a big impact on geometries but also dramatically changes the energetics along the reaction pathway. Among the solvent effect contributions to the transition state, the solvent energy contribution is -28.5 kcal/mol and the polarization effect contribution is 19.9 kcal/mol. In total, the solvent effect contributes -8.6 kcal/mol to the free energy barrier height, which means the presence of aqueous solution has a catalytic effect on the reaction mechanism and enhances the proton-transfer reactivity in aqueous solution.

2


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I. INTRODUCTION The presence of a solvent can change the energetics of the chemical reactions dramatically from their corresponding ones in gas phase. Combined multi-level quantum mechanics and molecular dynamics studies1-4 show that the presence of an aqueous solution weakens the interactions between a nucleophile and a substrate at its transition state for the bimolecular nucleophilic substitution (SN2) reaction, which substantially raises the reaction barrier height compared with the one in gas phase. For example, for the normal Walden-inversion mechanism of the F− + CH3Cl reaction mechanism, the reaction barrier in gas phase is ~ 6.9 kcal/mol;5 however, it is substantially increased to 26.9 kcal/mol6 because of the presence of the aqueous solution. As a result, the reaction rate constant in gas phase is about 20 orders of magnitude larger than that in solution phase for this SN2 reaction. A solvent can also change the gas-phase reaction mechanism by participating in a chemical reaction directly. For example, for the tautomerization of formamide to formamidic acid reaction,7-9 it is found that the water molecule assists tautomerization of formamide in aqueous solution and lowers the barrier height comparing to the one in gas phase. Another study of the water-assisted SN2 reaction of OH− + CCl4 in aqueous solution10 found that a water molecule assists to form a new OH− in the favorable back-side attack conformation via the proton transfer process, then the newly formed OH− attacks the substrate CCl4. Furthermore, a solvent can also serve as a solvent and as a catalyst at the same time.11-13 Water-assisted proton transfer mechanisms have been observed in the reactions 3



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with RNA and DNA bases, including uracil,14 cytosine,15-18 thymine,18,19 adenine,18,20 and guanine.18,21-25 Quantum chemical study of intramolecular proton transfer for monohydrated guanine complexes found that the reaction barrier height is approximately two times lower for the tautomeric oxo-hydro reaction compared with non-water-assisted processes.21 Ab initio study at the DFT and MP2 levels of theory of the intramolecular proton transfer in C8-oxidative guanine22 showed the assistance of a water molecule in the proton-transfer process greatly reduces the reaction barrier; furthermore, the presence of oxygen at C8 position lowers the activation energy by about 1 kcal/mol. First principle study using DFT and a continuum solvent model (IEF-PCM)23 found that a water molecule assisted proton-transfer process of tautomerization in 8-oxo-7,8-dehydropurine can significantly lower the activation Gibbs energy to less than 10 kcal/mol in aqueous solution. As for 8-hydroxy guanine radical (8-OHGrad), ab initio multiconfigurational MCSCF/DZP/MRPT2 study25 showed the activation barrier of water-assisted proton transfer in gas phase is 22.4 kcal/mol, which is about 26.3 kcal/mol less than the direct reaction process without the assistance of one water molecule. In aqueous solution, a DFT/B3LYP theory with the IEF-polarizable continuum solvation model24 found the water-assisted proton transfer of 8-OHGrad with one water molecule is at 18.6 kcal/mol. Although the authors characterized the stationary points along the reaction pathway of the water-assisted proton transfer process, the detailed, atomic-level evolution of the reaction pathway was not available, and the solvent effects and the quantitative contributions of the solvent to the reaction barrier are still unknown. 4


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It is well known that the proton transfer process has to be assisted by water molecules’ dipole moment distribution from reorganization of the first and second solvation shells, thus to correctly reproduce the microscopic rearrangements of water molecules, one should treat solution water molecules explicitly. However, till now, there have been no studies of water-assisted proton transfer of 8-OHGrad in aqueous solution to analyze the quantitative contribution of the solvent effect to the energetics along the reaction pathway, therefore, how much of the catalytic effect of the aqueous solution on the activation barrier was unknow. In addition, there has been no detailed reaction pathway mapped. Thus, in this paper, using an explicit SPC/E solvent model,26 we combined quantum mechanics and molecular mechanics theory1,27,28 to study the water-assisted intramolecular proton transfer of 8-OHGrad in water. Our purpose is i) not only to investigate the solvent effects on this reaction mechanism in aqueous solution, ii) also to calculate the quantitative contribution of the solvent effect to the potential of mean force, iii) to map a detailed, atomic-level, water-assisted proton-transfer mechanism in aqueous solution, and iv) to calculate the potential of mean force (PMF) and free energy activation barrier of the title reaction in aqueous solution.

II. METHODS Using combined quantum mechanics and molecular mechanics theory,1,27,28 we investigated the water-assisted intramolecular proton transfer of 8-OHGrad in water, where the 8-OHGrad complex with one water molecule was treated as the QM region 5



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with DFT and effective electrostatic potential (ESP) levels of theory during different stages of calculation, and the aqueous solution was treated as the classical MM region. The 8-OHGrad•H2O complex was embedded in a 39.9 Å cubic box consisting of 2137 water molecules described with an explicit SPC/E water model.26 As Truhlar and co-workers pointed out that the DFT/M08-SO/cc-pVTZ+ calculation gives comparable

accuracy

in

term

of

reaction

barrier

height

as

the

CCSD(T)(full)/aug-cc-pCV(T+d)Z calculation.29 Therefore, in this paper, the DFT/M08-SO/cc-pVTZ+ level of theory was employed here to treat the QM region to calculate PMFs along the reaction pathway. In addition, the solute interacts with water molecules via bonded interactions, electrostatic interactions, and van der Waals interactions, and the van der Waals parameters of the QM region were obtained from standard Amber force field.30 The calculations of PMFs were performed using the NWChem computational chemistry package.31 The potential energy of the whole reaction system can be written as,

V potential = Vqm +Vqm / mm +Vmm

(1)

in which Vqm has the same express as in the gas phase, representing the potential of QM region, and Vmm describes the classical molecular mechanical energy of the MM region. The middle term, Vqm/ mm , is the interaction energy between the QM and MM subsystems including the bonded interactions, electrostatic interactions, and van der Waals interactions. Moreover, the electrostatic interactions between the solute electron density ρ and solvent classical charges ZI can be approximated as32

Velectronstatic = ∑ ∫ I

Z I ρ (r' ) ZQ dr' = ∑ I i = VESP (r , R, Q) RI − r' i , I RI − ri

(2) 6


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Here, ESP charges Qi stands for the QM electronic density, which was fitted from the ab initio calculation of the electrostatic potential surface of the QM region. The potential of mean force under the DFT/MM level of theory can be obtained27 as, DFT DFT ←ESP ESP ∆WAB = (∆WAA + ∆WBBDFT ←ESP ) + ∆WAB

(3)

the last term is the solvent contribution to the PMF, calculated by statistical samplings with classical ESP/MM description. The first term in parentheses denotes the internal energy of the solute region under DFT level of theory. First, we embedded the estimated reaction complex (RC) in water, optimizing the QM and MM subsystems with a multi-region optimization protocol. Then we fixed the solute region and equilibrated the solvent MM region using molecular dynamics simulation for 120 picoseconds at 298 K, where the fixed QM region was represented by the ESP charges obtained from the previous optimization step. Second, the whole system was optimized again and the optimized structure was used to search the product complex (PC) with a bond-breaking and bond-formation procedure.2 This PC was optimized and equilibrated as we did to the initial RC. Third, the transition state (TS) was identified based on the optimized RC and PC, and was confirmed using a numerical frequency calculation with one imaginary frequency. Subsequently, we obtained the final RC and PC by optimizing displacements of the TS along the imaginary frequency mode. Finally, using the final obtained RC and PC, the reaction pathway was mapped using the nudged elastic band (NEB) approach.33 The molecular dynamics simulation was used to equilibrate the solvent for 120 picoseconds along the whole reaction pathway and the whole NEB reaction path was then optimized. The last step was repeated until the final NEB reaction pathway was converged. Finally, the PMF was calculated with the DFT/MM level of theory according to Eq. 3. 7



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III. RESULTS AND DISCUSSION A. Stationary points along the reaction path. First of all, the •OH attacks C8 site of guanine and results in the reactant(8-OHGrad) for the proton transfer process. The •OH is attached to C8 cite in guanine as shown in Figure 1. In aqueous solution, the hydroxyl radical, O10H10 is attached to C8 with a bond distance at 1.402 Å and the bending angle of ∠C8O10H10 is 108.1º; the dihedral angle of ∠C5N7C8O10 at 123.3º and the dihedral angle with respect the proton H10 ∠N7C8O10H10 is 15.5º. The location of O10H10 radical in gas phase is similar to the one in the solution phase. The distance of C8O10 is 1.382 Å and the bending angle of ∠C8O10H10 is 108.8º ; the dihedral angle of ∠C5N7C8O10 is at 110.9º and the dihedral angle with respect the proton H10 ∠N7C8O10H10 is 58.0º. (The structures of the stationary points are provided in Table S1 of the Supporting Information). Comparisons of stationary points for water-assisted intramolecular proton transfer process of 8-OHGrad in gas phase and in aqueous solution are shown in Figure 1-3, where the stationary points in gas phase are from Chaban et al.25 The optimized structures of reactant complex in gas phase and in solution phase are compared in Figure 1. The distance of H10O11 is 1.823 Å in aqueous solution, which is about 0.236 Å shorter than that in gas phase; the distance of N7H11 is 2.045 Å in aqueous solution, which is about 0.162 Å shorter than that in gas phase. The biggest differences exist among dihedral angles between in gas phase and in solution phase: the dihedral angles of ∠N7C8O10H10, ∠C8O10H10O11, ∠O10H10O11H11, ∠H10O11H11N7, ∠O11H11N7C8 and ∠H11N7C8O10 are 58.0º, -26.2º, -10.9º, 11.8º, 13.4º and -51.4º in gas phase, while they are 15.5º, 5.3º, -2.4º, -17.7º, 35.4º and 8


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-25.3º respectively in aqueous solution, with a mean unsigned difference of 26.7º with respect to those in gas phase. We found that there are hydrogen bonds formed between N7, C8, O10, O11 H11 sites and the adjacent water molecules: there are two strong hydrogen bonds formed with the H11O11H12 water molecule with an average distance of 1.746 Å; one strong and one weak hydrogen bond are formed between the hydroxyl located at the C8 site and its adjacent water molecules, with an average distance of 1.939 Å. There are also two weak hydrogen bonds formed with N7, with an average distance of 2.653 Å. Thus, the interactions between the solute and solvent, especially the hydrogen bonds, affect the reactant geometry in aqueous solution. And solvent effect here has a much bigger impact on the torsion angles than on the bond distances and bending angles. Figure 2 shows the structures of transition state in gas phase25 and in aqueous solution, where the latter was confirmed by numerical frequency calculations with a single imaginary frequency of 793.7i cm-1. At transition state, the water molecule and the hydroxyl radical, O10H10, forms a closed-ring with N7C8 as H11 in the water molecule attached to N7 and O11 in the hydroxyl radical attached to H10. The biggest difference of these two transition states still remains in their dihedral angles. In gas phase,

the

dihedral

angles

of

∠N7C8O10H10,

∠C8O10H10O11,

∠O10H10O11H11, ∠H10O11H11N7, ∠O11H11N7C8 and ∠H11N7C8O10 are 32.5º, -9.3º, -12.7º, 8.2º, 11.9º and -34.4º respectively, while in solution phase, they are 29.1º, -26.0º, 10.9º, -11.2º, 28.1º and -33.6º respectively, with a mean unsigned difference of 13.4º with respect to those in gas phase. Again, we notice that four strong hydrogen bonds are formed, one formed with O11 and three formed with O10, with an average distance of 1.673 Å; meanwhile, three weak hydrogen bonds, one with C8H8 and two with N7, occur with an average distance of 2.711 Å. Therefore, 9



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the big changes of torsion angles here compared to gas phase are strongly influenced by the hydrogen bonds formed between the solute and solvent. The product complexes, both in the gas25 and solution phases, are plotted in Figure 3. At the product state, H11, originated from the assistant water molecule, has been transferred to the N7 site, while H10, from hydroxyl on the C8 site, has been transferred to the O11 and formed a new water molecule, H10O11H12. Thus, the proton transfer process has finished with the assistance of one water molecule in aqueous solution. At this stage, the proton H10 has been broke up from the hydroxyl radical and been transferred O11. However, the biggest differences still exist in their dihedral

angles:

∠N7C8O10H10,

∠C8O10H10O11,

∠O10H10O11H11,

∠H10O11H11N7, ∠O11H11N7C8 and ∠H11N7C8O10 are 35.0º, -15.5º, -4.5º, 2.9º, 15.8º and -38.5º in gas phase, while they are 41.5º, -10.0º, -13.0º, 3.8º, 25.2º and -53.5º respectively in aqueous solution, with a mean unsigned difference of 7.6º between them. Two strong hydrogen bonds are formed around the new formed water molecule with an average distance of 1.812 Å; there are also two strong hydrogen bonds formed at O10 with an average distance of 1.648 Å, and five weak hydrogen bonds, three formed at N7H11 and two at C8H8, with an average distance of 2.652 Å. As a result, the solvent effect has a tremendous impact on the torsion angles, much more than on the bending angles and the bond distances, which is different from our previous investigation of SN2 reactions1-4 that the solvent effect can not only have a big influence on the angles but also on the bond lengths in aqueous solution. However, the current reaction system has a compact ring structure and the solvent effect is not strong enough to affect the strong bond interactions in the stationary points; while the more weaker torsion interactions can be easily affected by the solvent effect, especially by the hydrogen bonds formed in their hydrogen shells. Therefore, for the 10


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current system, the biggest difference of the conformations of the stationary points lies in their corresponding torsion angles between gas phase and solution phase. Mulliken spin density distribution of the reactant complex, transition state and product state were also calculated using the Gaussian program.34 Note that the hybrid density functional M08-SO is not included in the Gaussian program, instead we chose the IEF-PCM/M06-2X/aug-cc-pVTZ method to calculate the spin densities, as Truhlar and co-workers pointed out that the M06-2X/aug-cc-pVTZ level of theory produces very close results to the M08-SO/cc-pVTZ+.29 Figure 4 shows the spin density distribution of the reactant complex, transition state and product complex. As the OH radical is attached to the C8 site to form the reactant complex, 8-hydroxy guanine radical (8-OHGrad), the localized spin density of a separate O10H10 radical has been delocalized and widely distributed in the 8-OHGrad radical as O10 only has a small spin density of 0.040 while N7 with the largest spin density of 0.507 (Table 1). On one hand, as the reaction proceeds from reactant complex to transition state, then to product complex, the spin density of O10 has been further decreased from 0.040 to 0.028, then to 0.017, and H10 from -0.007 to -0.006, then to -0.005. On the other hand, since H11 is transferred to the N7 site, it gains spin density from -0.002 at reactant complex to -0.045 at transition state, then to -0.078 at product state while the spin density of N7 decreases from 0.507 to 0.497, then to 0.474. B. Detailed, atomic-level reaction mechanism. Ten snapshots along the NEB33 reaction pathway are displayed in Figure 5 to examine the atomic-level evolution of the reaction in detail. Snapshot (1) shows the reactant structure, snapshot (6) the transition state, and snapshot (10) the product structure. First, from snapshot (1) to snapshot (10), the charges distributed on the H10 are 0.519, 0.449, 0.498, 0.512, 0.549, 0.559, 0.530, 0.544, 0.621, and 0.481; the ones 11



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distributed on the H11 are 0.381, 0.319, 0.408, 0.361, 0.470, 0.504, 0.442, 0.489, 0.373, and 0.484 respectively. Thus, the reaction mechanism is characterized by two synchronized-proton-transfer processes. One proton transfer process is H10 transferred to the assistant water molecule, while the other is H11 in the assistant water molecule transferred to N7 site concertedly. As can been seen, the H10O11 bond distance is 1.823 Å at reactant complex, decreases to 1.164 Å at transition state, and further decreases to 0.980 Å at product complex, which is the process of the breaking of the O10H10 bond in the 8-OHGrad and the forming of the new OH bond in the assistant water molecule. At the meantime, the H11N7 bond distance is 2.045 Å at reactant complex, decreases to 1.132 Å at transition state, and further decreases to 1.018 Å at product complex, which is process of the breaking of old OH bond in the assistant water molecule and the forming of H11N7 bond. This is a concerted two-proton-transfer processes. Furthermore, there are also big changes in their bending and dihedral angles during the proton transfer process. For instance, the angle of ∠C8O10H10 decreases from 108.1º at reactant complex to 105.9º at transition state, then to 101.8º at product complex; and the angle of ∠O10H10O11 decreases from 164.9º at reactant complex to 163.8º at transition state, then to 151.3º at product complex. In addition, the dihedral angle of ∠N7C8O10H10 increases from 15.5º at reactant complex to 29.1º at transition state, then to 41.5º at product complex; the dihedral angle of ∠H10O11H11N7 increases from -17.7º at reactant complex to -11.2º at transition state, then to 3.8º at product complex; the dihedral angle of ∠O11H11N7C8 decreases from 35.4º at reactant complex to 28.1º at transition state, then to 25.2º at product complex; and the dihedral angle of ∠H11N7C8O10 decreases from -25.3º at reactant complex to -33.6º at transition state, then to -53.5º at 12


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product complex. In short, the proton transfer process is assisted with one water molecule, which is a synchronized-two-proton-transfer processes: one process is one proton transferred from the hydroxyl to the assistant water molecule, the other from the assistant water molecule to the N7 site. This whole proton transfer process involves two bonds breaking and forming concertedly. The dipole moment evolution of the solute subsystem along the NEB reaction path was plotted in Figure 6. It shows that, at the transition state of point (6), the 8-OHGrad with the assistant-water molecule has the largest dipole moment. This means at the transition state the solute subsystem has the strongest electrostatic interactions with the surrounding water molecules in its solvation shells. The strongest electrostatic interaction here stabilizes the transition state, which indicates the activation energy will be lowered due to the strongest interaction between the solute and solvent at the transition state. In addition, the dipole moment of the reactant complex is smaller than the product complex because the reactant complex is more compact than the product complex. C. Potentials of mean force and solution contributions. We plotted the potential of mean force (PMF) as well as the solvent contribution along the NEB reaction path with the reactant as a reference point in Figure 7. It shows that the free energy reaction barrier is 19.2 kcal/mol and the reaction energy is 5.5 kcal/mol. Moreover, the water solvent contributes -28.5 kcal/mol to the TS, and -27.3 kcal/mol to the product complex, which indicates that the presence of solvent significantly reduces the reaction barrier height. This is consistent with our prediction on the analysis of the dipole moment that the largest electrostatic interaction with the surrounding waters at the transition state lowers the barrier height. The perturbation of 13



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the solute wave function due to the presence of the solvent leads to the contribution of polarization effect, which is shown in Figure 8 by comparing the gas-phase reaction path and the solute internal energy along the NEB reaction path. Here the gas phase energy is obtained with the same 10 snapshots along the PMF reaction path without the solvent contribution and solute-solvent interactions; the solute internal energy is obtained excluding the solvent energy contribution. The comparison shows that the polarization effect contributes 32.2 kcal/mol to reactant state, 52.1 kcal/mol to transition state, and 52.9 kcal/mol to product state. Thus, the net polarization effect contributes 19.9 kcal/mol to transition state, and 20.7 kcal/mol to product state. In total, the aqueous solution contributes -8.6 kcal/mol to free energy barrier height, and -6.6 kcal/mol to reaction energy. So, the solvent energy and polarization effect have opposite contributions to the PMF: the former has an effect on reducing the barrier height, and the latter raises the barrier. Nonetheless, the total solvent effect has contributed -8.6 kcal/mol to the free energy barrier height, which means the presence of aqueous solution enhances the reactivity. In other words, the aqueous solution has a catalytic effect on this reaction mechanism by reducing the reaction barrier about 8.6 kcal/mol. This is also confirmed by comparison with the reaction barrier height in gas phase. In gas phase, the title reaction has a barrier height at 22.4 kcal/mol,25 and it is lowered to 19.2 kcal/mol here in aqueous solution. Therefore, the presence of aqueous solution indeed enhances the proton transfer reactivity. Our calculated barrier height at 19.2 kcal/mol has a very good agreement with the one at 18.6 kcal/mol by Munk et al.24 using a continuum solvation model with IEF-PCM/B3LYP/aug-cc-pVTZ//B3LYP/6-31G(d) level of theory. Usually, a system in solution treated with implicit and explicit solvent model would produce quite different results. For example, as Yang’s group35 compared the reactant structure of 14


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the Cl− + CH3Cl in solution optimized with implicit and explicit solvent model, they found the reactant structure optimized using implicit solvent model leads to a wrong symmetry conformation. Therefore, they pointed out that there are “risks of using conformations optimized in the gas phase or with a continuum solvent model for the study of solution or enzyme reactions”. In addition, the ring opening process of guanine damage by hydroxyl radical36 with an explicit SPC/E water model shows that reaction barrier height is 31.6 kcal/mol at the CCSD(T)/MM level of theory, which is much higher than the one at 19.5 kcal/mol obtained with the IEF-PCM implicit water model at DFT/B3LYP level of theory.24 Thus, the good agreement of the barrier height in this work between different solvent models might be a coincidence caused by the computational error produced from the implicit solvent model and the quantum level of theory used there. Our calculated free reaction energy, 5.5 kcal/mol, is about 2.5 kcal/mol lower than the one at 8.0 kcal/mol calculated by Munk et al. using a continuum solvation model. Since there is no experimental data of this reaction to compare with, here we used the method (the implicit, ICE-PCM solvation model in Gaussian program34) employed by Munk et al.24 to try to reproduce our explicit-water-model results to show the consistence between the two methods. Based on the same QM structures of the stationary points in aqueous solution from our explicit SPC/E water model results, the IEF-PCM/M06-2X/aug-cc-pVTZ calculation gives the barrier height at 19.3 kcal/mol and the free reaction energy at 7.1 kcal/mol, which are consistent with our explicit-water model results at 19.5 kcal/mol and 5.5 kcal/mol respectively at the DFT/M08-SO/cc-pVTZ+ level of theory.

IV. SUMMARY AND CONCLUSIONS 15



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Combining quantum mechanics with molecular mechanics theories, we investigated the water-assisted intramolecular proton transfer of 8-OHGrad in aqueous solution. An explicit SPC/E solvation model26 was used to describe the aqueous solution to describe the local rearrangements of water molecules. The stationary points comparison with the corresponding ones in gas phase shows that the aqueous solution affects the dihedral angles the most. Detailed, atomic-level reaction mechanism along the reaction pathway shows that the reaction mechanism is a synchronized two-proton transfer process: on one hand, the assistant water molecule accepts proton H10 from the hydroxyl attached at C8 site; on the other hand, it transfers its proton H11 to the N7 site of 8-OHGrad. The calculated free energy barrier is 19.2 kcal/mol at DFT/M08-SO/cc-pVTZ+ level of theory. The strongest electrostatic interaction at the transition state stabilized the proton-transfer process at the transition state, therefore it lowers the reaction barrier height in aqueous solution. The calculation also shows that, the solvent energy contributes -28.5 kcal/mol to the transition state and the polarization effect contributes 19.9 kcal/mol. In total, the water solution contributes -8.6 kcal/mol to the activation barrier, which means the water solution lowers the transition state in aqueous solution, and has a catalytic effect for this proton-transfer reaction mechanism.

ACKNOWLEDGMENTS D.Y. Wang thanks Dr. Chaban for sending us the geometries of the stationary points in gas phase, and Dr. Zongliang Li for the advice on spin density. This work is supported by the National Natural Science Foundation of China (Grant No. 11774206,11374194) and the Taishan Scholarship fund. The computation work was carried out at the Shenzhen Supercomputer Center of China. 16


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Molecular Mechanics Study of Ring Opening Process of Guanine Damage by Hydroxyl Radical in Aqueous Solution. Sci. Rep. 2017, 7, 7798.

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Figure 1. Solvent effects on geometry. Comparison of reactant complexes for water-assisted proton transfer process of 8-OHGrad in gas phase and in aqueous solution. The indicated distances are in angstroms (bond lengths in black and hydrogen bonds in blue).

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Figure 2. Comparison of transition states for water-assisted proton transfer process of 8-OHGrad in gas phase and in aqueous solution. The indicated distances are in angstroms (bond lengths in black and hydrogen bonds in blue).

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Figure 3. Comparison of product complexes for water-assisted proton transfer process of 8-OHGrad in gas phase and in aqueous solution. The indicated distances are in angstroms (bond lengths in black and hydrogen bonds in blue).

25



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Figure 4. Spin density distribution of the reactant complex, transition state and product complex of QM solute obtained at the IEF-PCM/M06-2X/aug-cc-pVTZ level of theory.

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Figure 5. The structures of 10 snapshots along the NEB reaction path for the water-assisted proton transfer of 8-OHGrad in aqueous solution. Snapshot (1) is the structure of reactant complex, snapshot (6) transition state, and snapshot (10) product complex. The indicated distances are in Angstroms. 27



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Figure 6. Evolution of the dipole moment of the solute subsystem along the NEB reaction path for the water-assisted proton transfer of 8-OHGrad in aqueous solution.

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Figure 7. Potential of mean force and solvent contributions along the NEB reaction path. The potential of mean force was calculated at the DFT/MM level of theory with the reactant state as the energy reference point.

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Figure 8. Comparison between gas-phase and solute internal energies along the NEB reaction pathway under the DFT/MM level of theory using the gas-phase energy of the reactant complex as a reference point.

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Table 1. Mulliken Spin density of the reactant complex (RC), transition state (TS) and

product

complex

(PC)

of

QM

solute

obtained

at

the

IEF-PCM/M06-2X/aug-cc-pVTZ level of theory.

H9 N9 C8 H8 N7 C5 C6 O6 N1 H1 C2 N2 1H2 2H2 N3 C4 O10 H10 H11 O11 H12

RC

TS

PC

-0.00387 0.05800 0.00011 0.01726 0.50741 0.01026 0.08354 0.11623 -0.01468 -0.00173 0.04924 0.07398 -0.00627 -0.00620 -0.03058 0.10939 0.03997 -0.00683 -0.00156 0.00650 -0.00016

-0.00688 0.08265 -0.03917 0.01472 0.49693 0.24035 0.03501 0.13259 -0.00190 -0.00202 0.02484 0.06377 -0.00434 -0.00404 -0.00830 -0.00169 0.02838 -0.00622 -0.04529 -0.00003 0.00063

-0.01228 0.09599 -0.00507 0.00624 0.47369 0.28262 0.02806 0.13575 -0.00144 -0.00150 0.03264 0.05454 -0.00329 -0.00210 -0.01176 -0.00879 0.01723 -0.00457 -0.07706 0.00126 -0.00015

31



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TOC Graphic

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Catalytic Effect of Aqueous Solution in Water ... - ACS Publications

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