Electrochemical and Mechanistic Study of Structure – Activity Relationship of α - , β - , γ - , and δ -Tocopherol on Superoxide Elimination in N , N -Dimethylformamide through Proton-Cou-pled Electron Transfer

: Elimination of superoxide radical anion (O 2 •− ) by tocopherols (TOH) and related compounds was investigated on the basis of cyclic voltammetry and in situ electrolytic electron spin resonance spectrum in N , N -dimethylformamide (DMF) with the aid of density functional theory (DFT) calculations. Quasi-reversible O 2 /O 2 •− redox was modified by the presence of TOH, suggesting that the electrogenerated O 2 •− was eliminated by α - , β - , γ -TOH through proton-coupled electron transfer (PCE T), but not by δ -TOH. The structure –activity correlation of α - , β -, γ - , and δ -TOH characterized by the methyl group on the 6-chromanol ring was experimentally confirmed, where the methyl group promotes the PCET mechanism. Furthermore, comparative analyses using some related compounds suggested that para -oxygen-atom in the 6-chromanol ring is required for a successful electron transfer (ET) to O 2 •− through the PCET. The electrochemical and DFT results in de-hydrated DMF suggested that the PCET mechanism involves preceding proton transfer (PT) forming hydroperoxyl radical followed by a PCET (intermolecular ET – PT). The O 2 •− elimination by TOH proceeds efficiently along the PCET mechanism involving one ET and two PTs.

Webster et al. reported the electrochemically controlled reversible transformation of α-TOH into its phenoxonium cation [3,6,[8][9][10]. In their pioneering work, a combination of electrochemical and in situ spectroscopy experiments demonstrated that all redox states of α-TOH-capable of donating two electrons and one proton-are accessible in acetonitrile through the addition of an organic soluble acid or a Brønsted base coupled with electrochemical generation. As they showed, the stability of the redox states for α-TOH is related to its characteristic structure, which enables a quinone-hydroquinone -conjugated redox system, despite its single hydroxyl group. Considering the structure-activity correlation of vitamin E in ROS elimination, it is reasonable that the differences in the four structures, α-, β-, γ-, and δ-TOH, are derived from those in the bulky methyl groups at the 5, 7, and 8 (R1, R2, and R3) positions ( Figure 1). The R1, R2, and para-oxygen respectively, are mainly considered to be related to the cyclic voltammetry responses, with the substituents determining the electron-donating ability and stability of tocopheroxyl radical (TO • ) [3]. The differences in the electrochemical behavior of α-, β-, γ-, and δ-TOH were investigated, all of which were found to be similar, and showed little difference in the formal redox potentials of direct two-electron oxidation or oxidation of tocopheroxyl anions (TO − ) upon the addition of a Brønsted base [6]. However, there was a significant difference in the chemical reversibility of the redox behavior, suggesting that the stabilities of the produced intermediates, such as TO • and phenoxonium cations, were different. The physicochemical properties confirmed by these electrochemical behaviors are presumed to be associated with electron transfer (ET) and proton transfer (PT) in the ROS elimination mechanism, but are not dominant to decide the reaction parameter between each ROS and TOH, particularly regarding the thermodynamics, kinetics, and deeper insights concerning the proton-coupled electron transfer (PCET) pathway, i.e., sequential PCET, hydrogen atom transfer involving the concerted PCET [11][12][13][14][15][16], and sequential proton loss electron transfer [5,17].
Referring to these studies, we investigated the electrochemical mechanism of the scavenging reaction of electrogenerated superoxide radical anion (O2 •− ) by α-TOH in N,N-dimethylformamide (DMF) [18]. Furthermore, a detailed mechanism was analyzed using density functional theory (DFT) calculations, and we proposed that the mechanism is a PCET characterized by the quinone-hydroquinone system (Equation (1)). In this mechanism, two PTs and one ET are thermodynamically preferred; the first PT from the acidic α-TOH to the O2 •− forms α-TO − and hydroperoxyl radical (HO2 • ), followed by ET coupled with the second PT from another α-TOH. In our previous studies, it has been reported that O2 •− is eliminated by polyphenols [18], diphenols (hydroquinone [19] and catechol [20]), and mono-phenols [21], through PCET mechanism. In these studies, the PCET mechanism based on quinone-hydroquinone -conjugation involves two PTs and one ET for a successful O2 •− elimination. The reversible cyclic voltammograms (CVs) in an alkali solution shown by Webster et al. revealed that PT is closely related to ET, and that the thermodynamically preferred mechanism of O2 •− elimination is enabled by ET-PT coupling. It is reasonable to assume a similar PCET mechanism for β-, γ-, and δ-TOH involving two PTs and one ET between O2 •− and two molecules of TOH since two protons are required in the net reaction (Equation (1)). However, the mechanism and structure-activity relationship of each TOH characterized by the methyl groups have not been provided.
In this study, we analyzed the reaction between electrogenerated O2 •− and TOH in DMF, focusing on the structure-activity relationship of TOH on the O2 •− elimination in relation to the PCET by electrochemistry and DFT calculation. Accordingly, we here present valuable information regarding the deeper mechanistic insight of PCET for the O2 •− elimination reaction by TOH.
The solvent for electrochemical and electron spin resonance (ESR) spectral-measurements was spectrograde purity DMF available from Nacalai Tesque Inc. (Kyoto, Japan) and used as received. Tetrapropylammonium perchlorate (TPAP) was prepared as described previously [22] and used as a supporting electrolyte for DMF. Ferrocene (Fc), used as a potential reference compound, was commercially available from Nacalai Tesque Inc. and purified by repeated sublimation under reduced pressure immediately before use.

2.2.Electrochemical and In situ Electrolytic ESR Spectrum Measurements
Cyclicvoltammetry was performed with a three-electrode system comprising a glassy carbon (GC) working electrode, a coiled platinum counter electrode, and an Ag/AgNO3 reference electrode (containing acetonitrile solution of 0.1 mol dm −3 tetrabutylammonium perchlorate and 0.01 mol dm −3 AgNO3; BAS RE-5) at 25°C using a BAS 100B electrochemical workstation, coupled to a BAS electrochemical software to record data. In situ electrolytic ESR spectra were measured using a JEOL JES-FA200 X-band spectrometer. The controlled-potential electrolysis was performed at room temperature in an electrochemical ESR cell using a 0.5-mm-diameter straight Pt wire sealed in a glass capillary as a working electrode (Supplementary, Figure S1).
Samples were prepared in a glove box completely filled with dinitrogen (N2) gas to prevent contamination by moisture. The DMF solution containing 0.1 mol dm −3 TPAP as a supporting electrolyte was saturated with O2 by air-bubbling the gas for ca. 2−3 min and the gas was passed over the solutions during the electrochemical and ESR measurements to maintain the concentration of O2 at a constant level. The equilibrium concentration of O2 was calculated as 4.8  10 −3 mol dm −3 .

2.3.Calculation
All solution phase calculations were performed at the DFT level with the Becke threeparameter Lee-Yang-Parr (B3LYP) hybrid functional as implemented in Gaussian 16 Program package [23]. The geometry optimization, subsequent vibrational frequency calculations, and population analysis of each compound were performed by employing the standard split-valence triple  basis sets augmented by the polarization d,p and diffusion orbitals 6-311+G(d,p). The solvent contribution of DMF to the standard Gibbs free energies was computed employing the polarized continuum model (PCM) method at the default settings of the Gaussian 16, which is widely employed in the description of the thermodynamic characteristics of solvation. The zero-point energies and thermal correction, together with entropy, were used to convert the internal energies to standard Gibbs energy at 298.15 K. The natural bond orbital (NBO) technique was used for electron and spin calculations in population analysis [24].
With the generation of HO2 • , bielectronic CVs were observed derives from the reduction of HO2 • (Equation (4)) as shown in Figure 2(f-h), cathodic current 2c. Conversely, in the presence of (a-c, e) TOH, the bielectronic CVs don't appear due to the elimination of HO2 • by the subsequent ET (Equation (5)) from the TO − . In our previous study, the ET involved in the PCET mechanism for successful O2 •− elimination required two structural characteristics; 1) the quinone-hydroquinone -conjugated structure characterized by ortho/para-diphenol or aminophenol, and 2) the hydroxyl and amino proton for the second PT [18][19][20][21]27]. Notably, α-, β-, and γ-TOH showed the CV for the successful O2 •− /HO2 • elimination, although the two structural characteristics are not involved in their structures.
Considering these results, we rationalized that O2 •− formation after the primary electrode process associated with PT from the hydroxyl group leads to the irreversible overall reduction of O2 to H2O2, which is driven by the exergonic reduction of the resulting HO2 • /HO2 − . Therefore, the CV traces for O2/O2 •− in the presence of phenolic compounds are divided into two typical curves: type A, an irreversible two-electron process observed in electro-chemical-electro reactions (Equations (2)-(4)), and type B, an irreversible oneelectron process (Equations (2), (3), (5), and (6)) leading to O2 •− elimination. Figure 3 shows the plausible electrochemical mechanism of O2/O2 •− in the presence of (a) α-TOH and in the presence of (b) homogentisic acid γ-lactone, summarizing Equations (2)- (6).
In this scenario, each CV result in the presence of α-, β-, γ-TOH, and 2,2,5,7,8-pentamethyl-6-chromanol, demonstrates type B (elimination of O2 •− /HO2 • ). Conversely, the others demonstrate type A (O2 •− is not eliminated) showing the appearance of a cathodic current ascribed to HO2 • . Then, the O2 •− /HO2 • elimination by ET was confirmed via in situ electrolytic ESR measurements of the CV solutions at an applied potential of −1.3 V corresponding to the O2 reduction (Equation (2)) with ESR scanning during 4 minutes. ESR spectra were obtained only for (Figure 2(a-c, e)) α-, β-, γ-TOH and 2,2,5,7,8-pentamethyl-6-chromanol (no ESR spectral for others). The two ESR spectra of (a) α-TOH and (e) 2,2,5,7,8-pentamethyl-6-chromanol with the simulated hyperfine coupling constants (hfcc) of hydrogen (aH/mT, 0.220, 0.210, 0.090, and 0.080) [21], are identical, owing to the radical spin not being distributed on the 2-phytyl chain. For (b) β-TOH and (c) γ-TOH, a weak signal was observed, derived from their radicals [4,6,29,30]. With reference to (d) δ-TOH, ESR shows no signal and the CV shows minimal reactivity. The anodic peaks (2a) appearing in Figure 2(a-c, e) are inferred to be assigned to TO − /TO • oxidation, although the corresponding cathodic peak (reduction peak of TO • ) is not observed. Based on the ESR results with the ratio of loss reversibility in CVs of O2/O2 •− (1a), the O2 •− elimination ability can be estimated as the following order: (a) ~ (e) > (b) ~ (c). The CV and ESR results demonstrated that TOH (a-c, e) with their 6-chromanol ring and two or more methyl groups can eliminate O2 •− /HO2 • , whereas the other structural features contained in (f-h) and the phytyl chain in (a-d) are not effective. And, the number of the methyl group on the 6-chromanol ring is in good correlation with the O2 •− elimination ability. These results imply that the reaction mechanisms of (b) β-TOH and (c) γ-TOH are the same as that of (a) α-TOH (Equation (1)); PCET involving two PTs and one ET, however their reactivities are different.

CV Analyses of the PCET Between O2 •− and α-TOH Under Acid-base Interactions
To gain more insight into the mechanism, acid-base interactions of α-TOH in the CVs of O2/O2 •− were investigated. Figure 4a shows the CVs of 4.8 × 10 −3 mol dm −3 O2 in the presence of α-TOH at concentrations (×10 −3 mol dm −3 ) of 0, 1.0, 2.0, 3.0, and 5.0 (black line), and 7.0, 10.0, and 20.0 (red line). The bielectronic current (2c) on the peak of O2/O2 •− appears where the concentration is greater than 7.0. Then, a small anodic peak (2a) begins to become larger at concentrations greater than 7.0. These changes in the CV show that the electrochemical mechanism has changed at higher concentrations of α-TOH. Simultaneously, the reoxidation current of O2 •− is not further decreased at concentrations over 7.0 ×10 −3 mol dm −3 . Though the trigger of a series of reactions (type B) along with a generation of α-TO • (Equation (5)) is the initial one-electron reduction of O2/O2 •− (Equation (2)), peak 2c (Figure 2a, red lines) will derive from the reduction of α-TO • , demonstrating that these peaks (2a/2c) can be attributed to α-TO • /α-TO − .
In Figure 4b, CVs of α-TOH in the absence (black line) and the presence of 20.0 × 10 −3 mol dm −3 sodium methoxide (red line) as a Brønsted base are shown. As reported by Wilson et al. [6], anodic oxidation of α-TO − (3a) was observed to yield α-TO • at a higher negative potential (E = −0.50 V vs Fc + /Fc) than α-TOH (4a, E = 0.3 V vs Fc + /Fc). Therefore, the resulting reversible peaks, 3a/3c, can be attributed to α-TO • /α-TO − redox couple. Similarly, α-TOH is deprotonated by O2 •− forming α-TO − (Equation (3)) in Figure 4a. However, the redox peaks of α-TO − /α-TO • are not observed at a lower concentration of α-TOH (black lines), owing to the following decomposition of α-TO • . Conversely, it is reasonable to assume that peak 2c/2a (redox of α-TO • /α-TO − ) is observable at higher concentration because α-TO − is also produced via the second PT (Equation (6)) from another α-TOH molecule to HO2 − . Furthermore, in a faster scan rate at 1.0 V s −1 (Figure 4c), the reduction of α-TO • /α-TO − (peak 5c) was reversibly observable on the anodic and returned cathodic scans (second cycle), despite that α-TO • is unstable. The redox potential of α-TO • /α-TO − is on the positive side of O2/O2 •− , but a cathodic peak is not observed in the first cycle because that α-TO • is not generated at the potential before the reduction of O2/O2 •− (Equation (2)), which is the trigger of a series of reactions. Under those conditions; fast scan, a higher concentration of α-TOH for the second PT (Equation (6)), and in the second cycle, the reduction peak of α-TO • /α-TO − is observable.
α-TO • + α-TO • → nonradical products (7) Next, Figure 4(d-e) shows the CVs of saturated O2 in the copresence of both 20.0 × 10 −3 mol dm −3 proton donor ((d) acetic acid, (e) phenol) and 0-5.0 × 10 −3 mol dm −3 α-TOH in a DMF solution. Irreversible bielectronic CVs of O2 associated with PT are observed in the presence of a proton donor, respectively. The addition of α-TOH to the solution for (d) acetic acid shows minimal reactivity in the bielectronic CV, conversely, that for (e) phenol results in the appearance of a new anodic peak at approximately −0.55 V, with a good correlation of concentrations of α-TOH (0-3.0 × 10 −3 mol dm −3 ). Judging from the peak potential, the new peak is assigned to the oxidation of α-TO − . In Figure 4f, the increasing concentration of phenol to the CV solution containing α-TOH (3.0 × 10 −3 mol dm −3 ) also resulted in the appearance of the anodic peak. Notably, the anodic peak only appears in the copresence of all three chemical species (O2 •− , α-TOH, and phenol). Without phenol (Figure 4f, solid line), or without α-TOH (Figure 4e, solid line), no peak appeared around this potential range, as is the case without O2. These results show that the π−planer ring of phenol supports the ET rather than proton donation in the intermolecular ET-PT: PCET. In the 1:2 mechanism shown in Equation (1), another molecule of α-TOH with its π−planer 6-chromanol ring will support the ET, as well as phenol.

Free Energy Calculations of PCET Between Electrogenerated O2 •− and TOH
For a mechanistic analysis of the O2 •− elimination by TOH in DMF, DFT calculations were performed at the (U)B3LYP/PCM/6-311+G(d,p) level. In Figure 5, the equilibrium scheme and standard Gibbs free energy changes (ΔG°/kJ mol −1 , 298.15 K) of the six diabatic electronic states for the PCET involving two PTs and one ET between O2 •− and two molecules of α-TOH (1:2) are shown. The important factors in determining the sequential processes shown in this scheme are the ΔG°s for the acid-base interaction and the redox potentials of the components. ET1 (ΔG° = 325.9 kJ mol -1 ) is strongly endergonic; thus, PT1 (70.3) forming α-TO − to HO2 • will primarily occur, as shown in the CV result. The ΔG°s of the upper rectangle also show those of 1:1 reaction between O2 •− and one molecule of α-TOH. Since the cathodic current of HO2 • and the anodic current of α-TO − was not observed in the CV (Figure 4a), where the concentration of α-TOH is less than 5.0, the 1:1 PCET reaction corresponding to the upper rectangle will be feasible, resulting formation of HO2 − and α-TO2 • . On the other side, since the redox of α-TO − /α-TO • appeared in the CV at concentrations over 7.0 ×10 −3 mol dm −3 , the 1:2 reaction; the initial PT (PT1) forming HO2 • and following PCET corresponding to the lower rectangle, is feasible pathway. In the lower rectangle, PT3 (337.4) is strongly endergonic, thus, an exergonic ET2 (−50.3) followed by PT4 (−2.5) from another α-TOH is a thermodynamically feasible pathway.
For a comparative study, the ΔG° values of the PCET pathways for the other compounds were calculated (Table 1). From a thermodynamic viewpoint, the total values of ΔG° for the net PCET obtained from the sum of the values for the two PTs and one ET embody the energetic driving force of the net PCET. However, the total values cannot embody the energetic driving force because the ΔG° for the unfeasible single PT/ET has been summed in it. The important factor for the net PCET pathway comprised of PT1-ET2-PT4 to proceed as a sequential reaction is the ΔG° values of the individual reactions. In the pathway, the ΔG° of ET2 mainly constitutes an uphill energy barrier to the net PCET for homogentisic acid γ-lactone (20.7), 2,3-dihydro-2,2-dimethyl-7-hydroxybenzofuran (6.5), and trans-para-coumaric acid (155.8). Thus, these ΔG° values confirm that PCET is feasible for the 6-chromanol moiety in TOH but not for others, supporting the other experimental results. Furthermore, the ΔG°s of ET2 for α-TOH (−50.3), β-TOH (−40.1), γ-TOH (−38.6), δ-TOH (−28.4), and 2,2,5,7,8-pentamethyl-6-chromanol (−49.1) are in good correlation with the ratio of loss reversibility in the CVs of O2/O2 •− in the presence of TOH (Figure 2(a-e)).
The ΔG°s along the plausible pathway: PT1-ET2-PT4, indicate that the methyl groups on the 6-chromanol ring contribute to suppressing each of the PT (PT1, PT4) in the order of α-> β-> γ-> δ-TOH, and that in promoting ET2 in the same order. These results are thought to correspond to the increased electron density on the 6-chromanol ring with the electron-donating methyl group, thus suppressing PT and promoting ET. The increasing number of methyl group on the 6-chromanol ring promotes the total (net) PCET reaction, accelerating the CV modifications. These findings show that the key process in the net reaction pathway between O2 •− and TOH is the ET2, which determines the structureactivity relationship of TOH on the O2 •− elimination.  After the initial PT along the plausible pathway (PT1-ET2-PT4) in Figure 5, α-TO − , HO2 • , and α-TOH, are involved in the reaction system. Therefore, two reaction schemes for ET to HO2 • and subsequent PT (PT4) is feasible, where electron donor is different; α-TOH or α-TO − as shown in Scheme 1. These two reaction schemes show that TOH, HO2 • and TO − , primarily form a HB complex centering an oxygen species (TO − -HO2 • -TOH), and then transfer one proton and one electron. In the schemes, ET occurs between oxygenπ-orbitals orthogonal to the molecular framework, then, PT occurs between oxygen-σorbitals along the HBs. Besides a discussion on the concerted PCET or the sequential PCET, the two mechanisms (Scheme 1) are different in the direction of ET, (a) PCET; both ET and PT occur from the same molecule, and (b) intermolecular ET-PT (PCET in a broad sense); both ET and PT occur from different molecules. Calculated ΔG°s suggest that the intermolecular ET-PT, ET (ET2) between α-TO − and HO2 • (−50.3), is thermodynamically favorable rather than the PCET, ET between α-TOH and HO2 • (100.7). Similar comparisons of the ΔG°s for β-, γ-, and δ-TOH (Supplementary, Table S1) also showed thermodynamic superiority of (b) the intermolecular ET-PT, respectively. Scheme 1. Schemes of (a) PCET and (b) intermolecular ET-PT, between hydroxyl donor (ROH), corresponding anion (RO − ), and HO2 •− , formed after the initial PT.

Potential Energy Scanning for the Stable HB Complex Along the PCET
For gaining deeper insight into the structure-activity relationship on the PCET mechanism, potential energy surfaces were investigated with the frontier molecular orbital and NBO analyses at the (U)B3LYP/PCM/6-311+G(d,p) level of theory. It is assumed that the reaction involves three elementary steps: i) formation of the prereactive HB complex (PRC) from the free reactants, ii) reaction to the product complex (PC) via a transition state (TS), and iii) dissociation of the product complex yielding free products. First, we start with an analysis of potential energy scanning for the stable HB complexes (PRC, intermediate HB complex, and PC) along the PCET reaction of α-, β-, γ-, and δ-TOH. Optimized structures of the 1:1 PRC (TOH-O2 •− ) resulting TO − -HO2 • formed after the initial PT (in step, i)) were obtained (Figure 6, upper), but were not the PC (TO • -HO2 − ). Thus, potential energy surface along the following ET (step ii)) is not obtained, suggesting that 1:1 PCET reaction don't occur for all of α-, β-, γ-, and δ-TOH.
Similarly, optimization for both of the 1:2 PRC (TOH-O2 •− -TOH), the 1:2 PC (TO • -H2O2-TO − ), and the intermediate HB complex (TO − -HO2 • -TOH) formed after the initial PT, centering an oxygen species bonded by a hydroxyl group of TOH were conducted. However, optimized stable structures of 1:2 HB complexes were not obtained, thus, their potential energy surfaces were not scanned. Since TOH have a long phytyl chain, it is difficult to form the 1:2 HB complexes. Conversely, the formation of HB complex between another molecule of TOH and HO2 • formed after iii) dissociation of TO − -HO2 • complex can occur, resulting in formation of TO • -H2O2 (Figure 6, lower). Spins are distributed on the electron donor (TO • ) side, demonstrating that ET coupled with the second PT (PCET) occurs. That is, the second PT from another molecule of β-, γ-TOH is necessary for the PCET, similar to α-TOH as reported in our previous study [18].
These results with the electrochemical results (Figures 2 and 3) reveal that β-, γ-TOH also bring about successful O2 •− elimination through the 1:2 PCET involving two PTs and one ET. Although the potential energy surfaces of the 1:2 PCET (Scheme 1) were unclarified for both mechanisms; (a) PCET and (b) intermolecular ET-PT, the intermolecular ET-PT predominates in the ΔG° results. Alternatively, assuming that HO2 • is released at a dissociation of the HB complex after the initial PT (TO − -HO2 • ), a 1:1 PCET between another TOH and HO2 • can occur. The reaction coordinate along ET-PT via TS between TOH and HO2 • can be found for α-, β-, γ-, and δ-TOH. However, the obtained activation energies (Ea, kJ mol −1 ) of TS (Supplementary, Figure S3) are not in a good correlation with the ratio of loss reversibility in the CVs of O2/O2 •− (Figure 2). Considering these results, the 1:2 PCET mechanism for a successful O2 •− elimination by β-TOH is shown in Figure 7; step i) formation of 1:2 PRC with the initial PT, followed by step ii) the intermolecular ET-PT, then step iii) dissociation of PC resulting formation of β-TO • , β-TO − , and H2O2.
where z is the number of electrons (1), F is the Faraday constant (9.648533 × 10 4 C mol −1 ). In the anodic scan for (d) 2,6-DTBO, two small peaks appeared on the positive side of the O2/O2 •− redox couple. It is unclear that which of the two peaks is assigned to PhO • /PhO − . Notably, in the second cycle of the CV, the reduction peak of PhO • is observable for (c) TTBP (red line) but not for (d) 2,6-DTBO, indicating that the PhO • of TTBP is stable. Therefore, we infer that one of the anodic peaks for 2,6-DTBO arises from the decomposition of a radical. Moreover, an ESR spectrum is detectable for (c) TTBP but not for (b) 2,6-DTBM, although the potential of PhO • /PhO − for TTBP (−0.6207) is less negative than that for 2,6-DTBM (−0.6577) in both the experimental and calculated results. These results suggest that the thermodynamic properties of PhO • (radical stability and redox potential) are not directly associated with the ET mechanism involved in the PCET, implying that the mechanism of the O2 •− elimination involves a concerted ET-PT.
Furthermore, spins are distributed on the tertiary carbons of tertiary butyl (t-Bu) group but not on the combined carbons in the α-positions of 2 and 6 t-Bu groups of the radicals (Figure 8(c-d)). For example, number of the line splitting observed in the ESR spectra for (d) 2,6-DTBO is 21 (3 ⋅ 7), the large 3 splitting is derived from two H a , and the hyperfine 7 splitting corresponds to the number of combined six α-carbons (c). The largest coupling constants (0.191, 0.330 mT) are assigned to the two hydrogens at positions 3 and 5 in the phenolic ring of (c) TTBP and (d) 2,6-DTBO, respectively. Other hfccs are assigned to the t-Bu groups at positions 2, 4, and 6 in TTBP (0.048, 0.030 mT) and positions 2 and 6 in 2,6-DTBO (0.032 mT); however, the hydrogen atom (H b ) is not directly combined to tertiary carbons. The splitting corresponds to the number of combined α-carbons, suggesting that radical electrons are distributed only on tertiary carbons and the electronic spins resonate to the hydrogens (H b ) in the β-position. Thus, effect of t-Bu groups at positions 2 and 6 on the O2 •− elimination is expected to be similar to that of the methyl group.
As a result of comparative analyses using the four 2,6-di-t-Bu-phenolic compounds, a higher electron-donating ability of the para-substituted group was required for the PCET, suggesting that the para-oxygen-atom in 6-chromanol ring of TOH is essential for successful O2 •− elimination through the PCET.

Conclusions
In conclusion, we have shown the structure-activity relationship of α-, β-, γ-, and δ-TOH on the O2 •− elimination through the PCET in DMF. As a result, we have clarified; • β-and γ-TOH eliminates O2 •− through the PCET involving two PTs and one ET, in a similar mechanism for α-TOH, conversely, δ-TOH does not • the net PCET mechanism involves the initial PT with forming a 1:2 HB complex (TO − -HO2 • -TOH) followed by intermolecular ET-PT as an intra-complex reaction • the increasing number of methyl groups on a 6-chromanol ring promotes the PCET reaction, especially the latter ET-PT, increasing the electron-donating ability of the 6chromanol ring • the expansion of the π−conjugated plane via the 1:2 HB complex plays an important role in the PCET mechanism • the electron-donating ability of the para-oxygen-atom in 6-chromanol ring of TOH is essential for successful O2 •− elimination through the PCET It was not clarified whether to proceed in a concerted PCET or a sequential PCET, however, the concerted pathway is reasonable for the findings that the net PCET involving the initial PT followed by intermolecular ET-PT occurs as an intra-complex reaction without dissociation of the HB complex.
Although the results presented in this manuscript are for a chemical reaction in aprotic DMF solvent rather than a biological system, the PCET theory is adaptable to biological processes involving both protic and aprotic conditions in such as a lipid bilayer. Therefore, we hope that the findings obtained in this study will provide evidence for the biological mechanistic actions of O2 •− elimination by TOH.