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Article

Triazolium Salt Organocatalysis: Mechanistic Evaluation of Unusual Ortho-Substituent Effects on Deprotonation

by
Peter Quinn
,
Matthew S. Smith
,
Jiayun Zhu
,
David R. W. Hodgson
* and
AnnMarie C. O’Donoghue
*
Department of Chemistry, Durham University, South Road, Durham DH1 3LE, UK
*
Authors to whom correspondence should be addressed.
Catalysts 2021, 11(9), 1055; https://doi.org/10.3390/catal11091055
Submission received: 7 August 2021 / Revised: 22 August 2021 / Accepted: 25 August 2021 / Published: 30 August 2021
(This article belongs to the Special Issue Organocatalysis: Mechanistic Investigations, Design, and Applications)
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Abstract

:
Organocatalysis by N-heterocyclic carbenes is normally initiated by the deprotonation of precursor azolium ions to form active nucleophilic species. Substituent effects on deprotonation have an impact on catalytic efficiency and provide insight into general catalytic mechanisms by commonly used azolium systems. Using an NMR kinetic method for the analysis of C(3)-H/D exchange, we determined log kex–pD profiles for three ortho-substituted N-aryl triazolium salts, which enables a detailed analysis of ortho-substituent effects on deprotonation. This includes N-5-methoxypyrid-2-yl triazolium salt 7 and di-ortho-methoxy and di-ortho-isopropoxyphenyl triazolium salts 8 and 9, and we acquired additional kinetic data to supplement our previously published analysis of N-pyrid-2-yl triazolium salt 6. For 2-pyridyl triazoliums 6 and 7, novel acid catalysis of C(3)-H/D exchange is observed under acidic conditions. These kinetic data were supplemented by DFT analyses of the conformational preferences of 6 upon N-protonation. A C(3) deprotonation mechanism involving intramolecular general base deprotonation by the pyridyl nitrogen of the N(1)-deuterated dicationic triazolium salt is most consistent with the data. We also report kDO values (protofugalities) for deuteroxide-catalyzed exchange for 6–9. The protofugalities for 8 and 9 are the lowest values to date in the N-aryl triazolium series.

Graphical Abstract

1. Introduction

The organocatalytic properties of N-heterocyclic carbenes (NHCs) are well documented for a broad range of synthetic transformations, including benzoin- and acyloin-type reactions [1,2,3,4,5,6,7,8], transesterifications [9,10,11,12,13,14,15,16,17,18,19], and annulations [20,21,22,23,24,25,26,27,28], among many others [29,30,31,32]. For the majority of these synthetic procedures, NHCs are typically generated in situ by the deprotonation of a conjugate acid heterocyclic azolium salt. In particular, triazolium salts 1 are widely employed as precatalysts: C(3) deprotonation of 1 generates the NHC, triazolylidene 2, which also has an ylidic/carbanion resonance form 2′ (Figure 1) [33]. First described in 1995 by Enders and Teles [34,35,36], the triazolyl scaffold has been proven to be broadly efficient in a range of NHC-catalyzed transformations [33,37,38,39,40,41,42,43]. In particular, the bicyclic pyrrolidine-based triazolyl scaffold 3 reported by Knight and Leeper [44] and related triazolium systems with morpholine- and aminoindane-based structures deliver increased yields and selectivities [45,46,47,48,49]. In addition to the fused ring, the choice of an appropriate N-aryl triazolium substituent is also key to reaction efficiency and product selectivity for a given transformation [50,51,52,53,54,55,56,57,58]. For example, the N-pentafluorophenyl catalyst 4 designed by Connon and Zeitler still holds the record, to our knowledge, of being the most efficient and stereoselective catalyst for the asymmetric benzoin reaction [47].
As the initial proton transfer step for the formation of triazolylidene 2 is common to a broad range of transformations, we reported both rate constants for deprotonation (kinetic acidities or protofugalities [59]) and carbon acid pKa values for a large series of triazolium salts in aqueous solution, which included 36 N-aryl examples [60,61,62,63,64]. In addition, there is an increasingly large body of literature data pertaining to the pKa values of the conjugate acids of NHCs in a range of solvents [65,66,67,68,69,70,71,72,73,74,75]. These datasets enable a detailed evaluation of the N-aryl substituent effect, which provides useful insight into the catalytic options for these commonly used NHC scaffolds.
As part of these studies, we reported unusual ortho-substituent effects on the proton transfer reactions of N-aryl triazolium salts [50,51,63]. For triazolium salts without ortho-substituents, H/D exchange of C(3)-H in D2O solution shows a simple first-order kinetic dependence on the concentration of deuteroxide, evident from a slope of +1 on a plot of log kex versus pD and consistent with a base-catalyzed mechanism for H/D exchange (Figure 2a). By contrast, for ortho-halo-substituted N-aryl triazolium salts (e.g., N-pentafluorophenyl triazolium 5 (Figure 2b)), significant changes in slope from log kex–pD proportionality were observed at low pDs consistent with H/D exchange via alternative mechanism(s). We previously proposed mechanistic options to explain the altered kinetic behaviors of ortho-halo-substituted N-aryl triazolium salts [61]. Although there are several potential options consistent with the data, the most likely mechanistic explanation is a pathway via N(1)-deuteration at lower pD values, which facilitates H/D exchange of the resulting N(1)-deuterated dicationic triazolium salt (Figure 2b). To account for the dominance of this altered behavior for ortho-halo-substituted triazolium salts 5, an increase in the extent of N(1) deuteration, and hence a more basic N(1), is required.
Triazolium salt 6 with an ortho-nitrogen atom in the N-pyrid-2-yl aryl substituent (Figure 2c) uniquely demonstrated formal acid catalysis of H/D exchange at lower pD values, evident from a slope of close to −1 on a plot of log kex versus pD, which was not observed for any other triazolium ion [63]. This provided evidence for the potential role of the N-pyrid-2-yl substituent as an intramolecular catalyst, although the precise form of catalysis has not been unequivocally established. Related studies involving mechanistic analysis of triazolium-catalyzed benzoin and Stetter-type reactions have highlighted that these ortho-substituent effects have also been observed in other steps in addition to the initial NHC-generating step. Rate and equilibrium constants for the formation of the first tetrahedral intermediate from the addition of NHC to aldehyde are substantially altered with ortho-heteroatom aryl substituents in both the N-aryl of catalyst and aldehyde, in comparison with analogues bearing para- or ortho-alkyl substitution [51].
To further probe the mechanistic origin of N-aryl ortho-substituent effects, and in particular to investigate the dominant form of catalysis for the N-pyrid-2-yl triazolium salt 6, we herein report a detailed kinetic evaluation by 1H NMR of the H/D exchange reactions of three additional triazolium salts, 7, 8, and 9. By tuning the basicity of the pyridyl nitrogen through the introduction of an electron-donating methoxy substituent in 7, it was postulated that any resulting changes in the log kex–pD profile would provide mechanistic insight into the role of the pyridyl substituent. In addition, the study of ortho-alkoxy-substituted triazolium salts in 8 and 9 would reveal whether the alternative proton transfer pathways observed for the ortho-halo analogues were unique or could extend to other ortho-heteroatoms. Our previous results suggest that ortho-alkyl substituents do not show any unusual behavior [61]. For N-mesityl triazolium salts with ortho-methyl substituents, there was no significant deviation from a slope of +1 except for slight upward deviation of one datapoint at the lowest pD value.
Our quantitative kinetic and structure–activity analyses provide useful insight into the mechanistic intricacies of triazolium catalysis. Although triazolium salts are a well-studied NHC organocatalyst class, there remain challenges in their usage in relation to both the stereo- and chemoselectivity of product formation, particularly in more polar media such as water. As one example of the benefits of heteroatom substitution in the NHC scaffold, recent intriguing results from Milo and coworkers demonstrated the importance of secondary sphere interactions in improving enantioselectivity in NHC organocatalysis of the benzoin reaction (as an archetypal NHC-catalyzed process) [76,77]. By invoking dynamic covalent interactions between boronic acid secondary sphere modifiers and the hydroxy substituent on the scaffold of chiral N-pentafluorophenyl triazolium salt 4, enantioselectivities were significantly increased. Thus, we hypothesize that alternative heteroatom substitution in the NHC scaffold, such as the ortho-pyridyl nitrogen of 6 and 7, could facilitate the greater adoption of this approach towards improving enantioselectivity in a broader range of transformations and different solvents.

2. Results and Discussion

2.1. Kinetic Analysis of the C(3)-H/D Exchange Reactions of N-Pyridyl Triazolium Salts 6 and 7

N-pyrid-2-yl triazolium tetrafluoroborate 6 was prepared as described previously [63]. A synthesis of N-5-methoxy-pyrid-2-yl triazolium salt 7 was not reported previously, and we employed the route shown in Scheme 1. A Buchwald–Hartwig amination [78,79,80] using benzophenone hydrazone 10 and 2-chloro-4-methoxypyridine 11 was employed, which yielded N-aryl hydrazone 12. Subsequent acid-catalyzed hydrolysis, initially to the hydrazinium chloride, followed by neutralization using sodium hydroxide, yielded the aryl hydrazine 13. Onward conversion to triazolium tetrafluoroborate 7 employed the widely used method reported by Rovis [81]: reaction of aryl hydrazine 13 with 5-methoxy-3,4-dihydro-2H-pyrrol-1-ium tetrafluoroborate yielded amidrazone 14 with subsequent cyclization being elicited by triethylorthoformate to afford 7. The X-ray crystal structures (CCDC 2100846–2100847) obtained in the course of this work of both triazolium tetrafluoroborate salts 6 and 7 are shown in Figure 3.
The N-5-methoxy-pyrid-2-yl triazolium salt 7 had not been studied previously; thus a log kex–pD profile was determined in the pD range 0–4. Exchange reactions were performed in both DCl and formate buffer solutions at 25 °C and ionic strength, I = 1.0 (KCl). For the N-pyrid-2-yl analogue 6, we previously reported a log kex–pD profile [63]; however, additional data were acquired in the present study in the pD 3–4 region to assist with mechanistic evaluation and more robust kinetic fitting. For both 6 and 7, reactions were too fast above pD 4 for NMR analysis. The kinetic and NMR methods used for the analysis of the C(3)-H/D exchange reactions described herein were identical to those reported by us previously [60,61,63,64]. Over time, the disappearance of the singlet at ~10.3 ppm due to the C(3)-H is observed; however, there is no change in the integrals of all other signals, nor in the appearance of new signals. Figures S1–S2 in Supplementary Materials include representative 1H NMR spectral overlays at three time points during C(3)-H/D exchange for 6 and 7, respectively. The observed first-order rate constants for C(3)-H/D exchange at a given pD, kex (s−1), were obtained as slopes of semilogarithmic plots of the fraction of the remaining unexchanged substrate, f(s), against time according to Equation (1) (Figures S3–S5). Reaction progress was defined by values of f(s) calculated using Equation (2), where AC(3)-H and Astd are the integrated areas of the singlet at ~10.3 ppm due to the C(3)-H of the substrate and the broad triplet at 3.3 ppm owing to the methyl hydrogens of the internal standard, tetramethylammonium deuteriosulfate. The resulting kex (s−1) values obtained at each pD are collected in Tables S1 and S2 for 6 and 7.
ln f(s) =−kex t
f ( s ) = ( A C ( 3 ) - H / A std ) t / ( A C ( 3 ) - H / A std ) 0
Figure 4a shows the corresponding log kex–pD profiles for 6 and 7. Pleasingly, the same overall kinetic behavior is observed for the H/D exchange reactions of the 5-methoxy-2-pyridyl triazolium salt 7, as previously observed for 6. Both profiles show distinct regions of close to –1 and +1 slopes consistent with first-order kinetic dependencies on D3O+ and DO–, respectively. The formal dependence on D3O+ is unique to these 2-pyridyl salts, whereas all triazolium salts to date have shown a kinetic dependence on DO–. Significantly, log kex values in the lower pD region are substantially higher for 7 than for 6, showing that the 5-methoxy substituent on the pyridyl ring has increased reactivity to H/D exchange. For comparison, the plots in Figure 4b include log kex–pD data for N-pentafluorophenyl triazolium tetrafluoroborate 5 and N-phenyl triazolium tetrafluoroborate 15 taken from our previously published studies [61].
The solid lines in Figure 4a show the fits of the reaction data to Equation (3) [82], which was used in our previous analysis of reaction data for 6. In this equation, the H/D exchange reaction of the substrate in the region of close to +1 slope is described by the rate constant, kDO (M−1s−1), the second-order rate constant for deuteroxide-catalyzed exchange of the triazolium salts. Kw = 10−14.87 is the ion product of D2O at 25 °C, and γDO = 0.73 is the activity coefficient for deuteroxide ion under our experimental conditions. The H/D exchange reaction of the substrate in the region of close to −1 slope is described by the rate constant, kH (s−1) [83].
log k ex = log k H 10 − p D + K a N k DO K W γ DO 10 p D K a N + 10 − p D
This equation allows for speciation between the monocationic triazolium ion (6 or 7) and a conjugate acid dication obtained by protonation at either the triazolyl N(1) or 2-pyridyl N as pD is decreased, and defined by the acid dissociation constant, KaN. Excellent fits of the reaction data are observed for both 6 and 7 at the two ends of the plots, and values obtained from this fitting for both kDO and kH are shown in Table 1. There is more uncertainty associated with a potential value for KaN. The plots do not level to a plateau at the lowest pD values in a manner consistent with full protonation. Linear plots of only log kex values at the lowest pDs (Figure S6) yield slopes of –0.73 and –0.93 for 6 and 7, which are slightly below unity, suggesting the beginning of curvature. However, as this curvature is not substantial, there will be large errors associated with the determination of KaN. The fit to Equation (3) yields KaN = 0.86 (±0.39) and 0.57 (±0.29) for 6 and 7, respectively. By fixing KaN at defined values of 1, 10, 100, and 1000 (i.e., pKaN = 0, –1, –2, –3), both visible inspection and the magnitude of R2 indicate that the best fit is obtained for KaN = 1 in both cases (See Figure S7).
In the middle region of the pD-rate profile for the lowest log kex values, where the transition occurs between negative and positive slopes, there are several datapoints that deviate above the curve described by Equation (3). This is more significant for the 5-methoxy-2-pyridyl triazolium salt 7 and could potentially be explained by an additional pD-independent process. To allow for this third option, we included a pD-independent term, defined by the rate constant kin (s−1) in Equation (4) (Figure 4a, dashed line) [82]. The overall fit for 6 is similar, but there is a significant improvement in the overall fit for 7 (R2 = 0.999 versus 0.976); however, we must caution that the inclusion of an additional variable will always lead to an improvement in overall kinetic fitting whether its inclusion is mechanistically justified or not. In addition, there is a large increase in the error for kH when using Equation (4).
log k ex = log k H 10 − p D + k in + K a N k DO K W γ DO 10 p D K a N + 10 − p D
The following sections will evaluate the potential mechanistic options that can be aligned with the different regions of the log kex–pD profiles.

2.1.1. Mechanistic Options for the Region of + 1 Slope in log kex–pD Profiles at Higher pD Values (First-Order Dependence on DO−)

The first-order dependence on deuteroxide ion in this region of the profile is consistent with a single mechanism for deuteroxide-catalyzed H/D exchange, as shown in Figure 5: C(3) deprotonation of the triazolium salts by deuteroxide results in the formation of a complex between the triazolyl NHCs and a molecule of HOD. Subsequent reorganization of NHC·HOD to NHC·DOL (L = H or D) to allow for the delivery of deuterium, followed by deuteration, leads to a C(3)-deuterated product. Owing to the large excess of bulk solvent over the substrate, the deuteration step is effectively irreversible; thus kex reflects a rate-limiting formation of solvent-equilibrated NHC from the triazolium salt and deuteroxide ion at a given pD. By definition, the second-order rate constant, kDO (M−1s−1), is the observed kex value in 1 M−solution (pD ~ 14). Experimentally, C(3)-H/D exchange for all triazolium ions is orders of magnitude too fast to monitor directly by NMR in 1 M DO− (half-lives ~ nanoseconds); thus kDO values are obtained by the assessment of a range of kex values at lower pDs, as described above. The reactivities to deprotonation by a common base, kDO, allow for the evaluation of the protofugalities of the C(3) hydrogens in the series of triazolium ions.
In our previous studies, kDO values for N-aryl triazolium ions spanned a range of ~30 fold across the large series [60,61,62,63,64]. Maximal kDO values (~8 × 108 M−1s−1) were observed for N-pentafluorophenyl-substituted triazolium salts, whereas the lowest value to date of 4.2 × 107 M−1s−1 was observed for an N-4-methoxyphenyltriazolium salt 16. Typically, values for kDO were observed to increase for electron-withdrawing N-aryl substituents. In the present study, values of kDO = 8.79 × 107 M−1s−1 and 8.02 × 107 M−1s−1 were obtained for 6 and 7 (Table 1), respectively, which fall midway in the range of previously observed values. The extra data obtained herein for 6 in pD regions 3–4 permit a more reliable determination of kDO. These kDO values for 6 and 7 are higher than for N-phenyl triazolium salt 15, indicating an overall electron-withdrawing effect of both pyridyl substituents. Electron-withdrawing N-aryl substituents will destabilize the cationic triazolium carbon acid relative to the formally neutral NHC conjugate base, thus favoring the deprotonation process. The kDO values obtained for 6 and 7 are closely similar, suggesting that the electron-withdrawing 2-pyridyl nitrogen dominates the N-aryl substituent effect for deuteroxide-catalyzed exchange. The value for 7 is ~10% lower than for 6, as would be expected with the additional presence of a donating 5-methoxy substituent. There is no evidence of intramolecular catalysis involving the pyridyl substituent in this region as the kDO values fall within the normal range observed to date and can be explained by the normal electron-withdrawing substituent effect of the 2-pyridyl group. A substantially higher kDO value would have been expected if intramolecular catalysis were operational. Presumably, the intrinsic reactivity to intermolecular deprotonation by DO− is so high in this pD region that there is no competition from an intramolecular reaction.

2.1.2. Mechanistic Options for the Region of –1 Slope in log kex–pD Profile (First-Order Dependence on D3O+)

Formal D3O+ catalysis, as observed in this region of the profile, is unique to 6 and 7 and has not been observed to date in proton transfer studies for any other N-aryl triazolium salt. For all other triazolium salts, including N-pentafluorophenyl triazolium 5, rate constants for H/D exchange continue to decrease as pD is decreased (e.g., as shown in Figure 4b for 5 and 15). To account for the increase in kex for 6 and 7 at lower pDs, it is necessary to invoke a mechanism that is not possible, or would be substantially slower, for other triazolium ions. Importantly, kex rate constants for 7 are at least 15-fold higher than for 6 in this region, and any mechanism should allow for this difference in reactivity.
As both 6 and 7 contain two nitrogen atoms with lone electron pairs, the most logical mechanisms for acid catalysis will involve deuteration at one of these atoms. N-deuteration of the triazolium salt will eventually occur as the pD decreases, although the precise Ka is unknown. Possibilities include N(1)-deuteration of the triazolium ring (Option a or d, Figure 6), deuteration of the 2-pyridyl nitrogen (Option b, Figure 6), and shared deuteration between both nitrogens (Option c, Figure 6). Mechanisms involving pre-equilibrium N-deuteration to any of these three dicationic species, followed by C(3) deprotonation by solvent, as shown in Options a–d, which are kinetically equivalent, would result in formal acid catalysis. Option d additionally involves the participation of the 2-pyridyl nitrogen as an intramolecular general base catalyst in the activation of water.
Option a can be excluded, as there is no reason why a nonparticipating remote 2-pyridyl substituent should result in orders of magnitude increases in rate constants in this region compared with other N-aryl substituents. In the DO− region of +1 slope, the kDO values obtained for 6 and 7 fall midway in the range of previously observed rate constants and are not unusually high. It is thus difficult to justify why a remote nonparticipating pyridyl could substantially increase a D2O reaction but not a DO− reaction.
Option b is potentially more chemically reasonable as the range of triazolium salts studied previously did not contain a more basic heteroatom in an ortho-position. This option, which involves electrophilic catalysis by an N-protonated pyridyl substituent, would be unique to the 2-pyridyl salts 6 and 7. However, the question then arises as to how protonation on the 2-pyridyl nitrogen could result in an increase in kex, whereas with N(1)-deuteration on the central triazolium ring, as proposed for ortho-halo salts (e.g., 5, Figure 2b and Figure 4b), rate constants continue to decrease with pD. A significantly higher pKaN for acid dissociation of the N-protonated pyridyl than triazolyl nitrogen could explain this difference in trends. A higher degree of pyridyl N-deuteration owing to a higher pKaN, and hence a higher formal cationic charge at this position, would enhance electron deficiency and facilitate the deprotonation at C(3) by solvent. As discussed earlier, however, there is no evidence from the pD profile that pKaN is significantly greater than zero for 6 or even the more basic 5-methoxypyridyl-substituted 7. Similar pKaN values ~−0.3 were estimated for ortho-halo-substituted salts from reaction data, albeit with relatively large errors in KaN. In a similar manner, Option c with a shared intramolecular deuteration would also require an elevated pKaN compared with other triazolium salts in order to account for the substantial increase in rate constants in the –1 region.
Option d is not reliant on an elevated pKaN and utilizes the pyridyl nitrogen as an intramolecular general base catalyst (i.e., protonation on the pyridyl nitrogen is not required). In particular, our present results for 7 also add support to this mechanism as intramolecular deprotonation by a more basic 4-methoxyl pyridyl nitrogen would be expected to be close to two orders of magnitude faster than for 6 (note: pKa (H2O) = 5.17 and 6.62 for pyridinium and 4-methoxypyridinium salts, respectively).
We computationally studied the conformational profiles of both the monocationic and dicationic N-2-pyridyl triazolium ion as a function of the change in dihedral angle between the N-aryl substituent and central triazolium ring using the B3LYP/6-311++g (d,p) [84,85,86] level of theory (Supplementary Materials, Section S10). The preferred lowest energy conformation for the monocationic triazolium ion in water (Figure 7, black) has a coplanar N-aryl substituent with the pyridyl nitrogen pointing towards the C(3)-H, as observed in the experimental X-ray crystal structure for both 6 and 7 (Figure 3).
Interestingly, upon N-protonation at either N(1) of the triazole or the 2-pyridyl nitrogen to give a dicationic species, the preference for coplanarity remains, however, with a 180° rotation of the pyridyl nitrogen such that it points towards N(1) (Figure 7, red and blue, respectively). Thus, there is a clear difference in the preferred orientation of the pyridyl nitrogen between the monocationic and dicationic triazolium species. The same conformational preferences were observed in both water and methanol as solvents (see Figure S15 for methanol calculations), and also using the M062X/6-311g++ (d,p) [85,86,88] level of theory for the dication calculations in water (Figure S16). In principle, this lends support to mechanistic Option c (Figure 7), which requires this preferred lowest energy conformation for the dication, but not to Option d. However, the energy barrier for rotation around the N(2)-Cipso(Ar) bond in all three cases (Figure 7) is only 4.0–4.1 kcal mol−1 at 25 °C, which would permit interconversion between conformers on a subsecond timescale. Thus, all conformations are rapidly accessible on the kinetic timescale of H/D exchange.

2.1.3. Mechanistic Options for the (Potential) Region of Zero Slope in log kex–pD Profile (pD-Independent Region)

In the case of 5-methoxy-2-pyridyl triazolium salt 7, there is some evidence for an additional pD-independent process at intermediate pD values. The observed kex values at pD 1.7–2.5 are significantly increased above the intersection point of the regions of negative and positive slopes. In the case of 6, some slight upward deviation of a couple of datapoints is observed, but the changes are smaller. Figure 8 shows a mechanism that could be aligned with this region of the profile: deprotonation at C(3) of the monocationic triazolium salt by solvent D2O with potential intramolecular assistance from the pyridyl nitrogen. This mechanism also unifies with the mechanism that seems most consistent with the –1 region (i.e., intramolecular deprotonation at C(3) by solvent (c.f. Figure 8) is facilitated by N(1)-protonation, explaining the large increase in rate constants at lower pDs (c.f. Figure 6d)).

2.2. Kinetic Analysis of the C(3)-H/D Exchange Reactions of N-di-Ortho-Alkoxy Triazolium Salts 8 and 9

For the syntheses of N-di-ortho-methoxy- and N-di-ortho-isopropoxyphenyl triazolium tetrafluoroborate salts 8 and 9, we utilized modifications of a previously reported procedure for the preparation of the analogous chloride salt of 8 (Supplementary Materials, Section S9). The C(3)-H/D exchange reactions of 8 and 9 had not been studied previously, and log kex–pD profiles were determined in the pD range 0–3. Figures S8 and S9 (Supplementary Materials, Section S7) include representative 1H NMR spectral overlays at three time points during C(3)-H/D exchange for 8 and 9, respectively. As for 6 and 7, no parallel reactions were observed during the timescale for complete deuterium exchange. The observed first-order rate constants for C(3)-H/D exchange at a given pD, kex (s−1), were obtained as slopes of semilogarithmic plots of the fraction of the remaining unexchanged substrate, f(s), against time according to Equation (1) (Figures S10 and S12). As for all previous studies of H/D-deuterium exchange reactions of the conjugate acids of NHCs, buffer catalysis was not significant (Figures S11 and S13, Tables S5 and S6). The resulting kex (s−1) values obtained at each pD are collected in Tables S3 and S4 for 8 and 9.
Figure 9 shows the corresponding log kex–pD profiles for 8 and 9. For comparison, Figure 9 also includes log kex–pD data for N-phenyl triazolium tetrafluoroborate 15 taken from our previously published studies [61]. In both cases, the profile is mostly described by a region of +1 slope consistent with the mechanism in Figure 6. There is evidence of some slight upward deviation from the line of +1 slope for a few datapoints at the lowest pD values. Equation (5) is a simplified form of Equations (3) and (4) [82], which only allows for a first-order dependence on DO–. To determine a kDO value, only datapoints that fit a line of unit slope were included (open symbols), and those showing slight upward deviation (filled symbols) were excluded from the kinetic fitting to Equation (5). The slight upward deviation is not significant enough to justify application of Equations (3) or (4) for kinetic fitting.
log k ex   =   log k DO K W γ DO 10 p D
The kDO values for 8 and 9 (Table 1) are lower than for both N-phenyl 15 and N-mesityl 17 triazolium salts and also than the lowest kDO to date for the N-4-methoxyphenyltriazolium salt 16. Clearly, di-ortho-alkoxy substitution is very different from ortho-halo substitution in not facilitating alternative pathways for H/D exchange as pD is decreased. Furthermore, opposite effects on deuteroxide-catalyzed exchange are observed at higher pDs. Halo substituents result in increases in protofugality, whereas ortho-alkoxy substituents substantially decrease kDO, consistent with a net electron-donating substituent effect for the latter-reducing C(3) carbon acidity.

2.3. Estimation of Carbon Acid C(3)-H pKa Values

In the determination of aqueous pKa values of weak carbon acids, the main problem is the levelling effect and the quantitative deprotonation of water. Owing to the greater basicities of most NHCs relative to hydroxide ion, quantitative deprotonation of water occurs, which prevents the determination of pKa values by direct quantification of the relative concentrations of acid and conjugate base species at equilibrium. We previously employed an alternative kinetic approach by using the rate constants for the forward and reverse directions of the proton transfer equilibrium in the calculation of pKa using Equation (6) derived for Scheme 2 [60,61,63,64,65]. In this equation, kHO (M−1s−1) is the second-order rate constant for deprotonation at C(3) by hydroxide ion, which may be calculated from the corresponding kDO value using a value of kDO/ kHO = 2.4 for the secondary solvent isotope effect on the basicity of HO− in H2O versus DO− in D2O. As discussed previously [61], the absence of significant general base catalysis of deuterium exchange provides good evidence that the reverse protonation of the triazol-3-ylidene NHC by water is equal or close to the limiting rate constant for the physical process of solvent reorganization (kHOH ≤ kreorg = 1011 s–1). The main error in pKa determination using this method is associated with the value assumed for kHOH; hence these pKa values provide upper limit estimations. Using this same approach, C(3)-H pKa values were calculated for triazolium tetrafluoroborate salts 6–9, which range from 17.4 to 17.9 (Table 1). Given that values of kDO for 6–9 only vary by threefold (2.87 × 107 M−1s−1–8.79 × 107 M−1s−1), and the logarithmic relationship of kHO and pKa in Equation (6), the resulting C(3)-H pKa values vary by less than 1 unit. Consistent with our previous work, N-aryl substituent effects on pKa are relatively small. As commented previously [61], the main factor influencing the pKas of the conjugate acids of NHCs is the nature of the ring heteroatoms in the central heterocycle, while the effects of N-aryl substituent are substantially smaller.
p K a   =   p K w +   log k HOH k HO

3. Conclusions

The C(3) deprotonation of 1,2,4-triazolium salts is the first key step in all organocatalysis processes involving NHC catalysis by triazolylidenes. Structure–reactivity studies of substituent effects on this proton transfer step can provide valuable insight into the modes of catalysis possible for a given N-aryl substituent. In order to mechanistically interrogate ortho-substituent effects on proton transfer, we reported detailed hydrogen–deuterium kinetic studies of N-5-methoxypyrid-2-yl triazolium salt 7 and di-ortho-methoxy and di-ortho-isopropoxyphenyl triazolium salts 8 and 9. In each case, we evaluated the effect of a change in reaction pD on the rate constant for exchange, kex, and performed a detailed kinetic evaluation of the log kex–pD profiles.
In common with all triazolyl NHCs studied to date, the profiles for 7–9 all included a region of +1 slope consistent with a first-order dependence on deuteroxide ion. The second-order rate constants for deuteroxide-catalyzed exchange, kDO (also known as the protofugality), could be measured as 8.02 × 107 M−1s−1, 3.87 × 107 M−1s−1, and 2.87 × 107 M−1s−1 for 7–9, respectively. Relative to N-phenyl triazolium tetrafluoroborate 15, the 5-methoxy-2-pyridyl substituent of 7 increases kDO, whereas the di-ortho-alkoxy substituents of 8 and 9 decrease kDO consistent with electron-withdrawing and electron-donating substituent effects on protofugality, respectively. Using the values for kDO, we also estimated upper limits on pKa values for deprotonation at C(3).
The log kex–pD profile for the N-5-methoxypyrid-2-yl triazolium salt 7 also demonstrated an extensive region of close to –1 slope, which had only been observed previously for N-pyrid-2-yl analogue 6, but not for any other triazolium salt. Significantly, the effect of a 5-methoxy substituent in the pyridyl ring of 7 is to increase rate constants in this region by at least 15-fold compared with 6. As there is no evidence for significant protonation of the pyridyl substituent above pD 0 for either 6 or 7, we propose that a H/D exchange mechanism involving intramolecular general base deprotonation at C(3) by the pyridyl nitrogen of the N(1)-deuterated dicationic triazolium salt is more consistent with the data than one involving electrophilic catalysis with protonation on the pyridyl nitrogen.

Supplementary Materials

The following are available online at https://www.mdpi.com/article/10.3390/catal11091055/s1: Figure S1—Representative 1H NMR spectra between 11.2 and 6.8 ppm at 500 MHz of 6 (10 mM, pD 3.07) during exchange of C(3)-H (s, 8.33 ppm) for deuterium in D2O at 25 °C and I = 1.0 (KCl). [internal standard, tetramethylammonium deuteriosulphate (s, 3.17 ppm)]. Figure S2—Representative 1H NMR spectra between 11.2 and 6.8 ppm at 500 MHz of 7 (10 mM, pD 1.08) during exchange of C(3)-H (s, 10.39 ppm) for deuterium in DCl solution in D2O at 25 °C and I = 1.0 (KCl). [internal standard, tetramethylammonium deuteriosulphate (s, 3.17 ppm)]. Figure S3—Semilogarithmic plots of the fraction of unexchanged substrate against time for the C(3)-H/D exchange reaction of 6 in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). The majority of the data for 6 (for lower pD values) has been previously reported. Figure S4—Semilogarithmic plots between pD = 0.42 and pD = 1.73 of the fraction of unexchanged substrate against time for the C(3)-H/D exchange reaction of 7 in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Figure S5—Semilogarithmic plots between pD = 2.03 and pD = 3.66 of the fraction of unexchanged substrate against time for the C(3)-H/D exchange reaction of 7 in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Table S1—First order rate constants for exchange of the C3-H of triazolium salt 6 for deuterium, in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Data for pD values of 3.07—3.66 were obtained as part of this work. Table S2—First order rate constants for exchange of the C(3)-H of triazolium salt 7 for deuterium in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Figure S6—Linear plot of log kex against pD for the H/D exchange of triazolium salt 6 (●) and 7 (●) at pD values ≤ 1.1, 25 °C and I = 1.0 (KCl). Figure S7—Plot of log kex versus pD for the C(3)-H/D exchange of 6 (●) and 7 (●) using eqn. 3 (main text), with KaN fixed to different values. Figure S8—Representative 1H NMR at 400 MHz of 8 ( 10 mM, pD 1.08) during exchange of C(3)-H (s, 9.76 ppm) for deuterium in DCl solution in D2O at 25 °C and I = 1.0 (KCl). [internal standard, tetramethylammonium deuteriosulphate (s, 3.17 ppm)]. Figure S9—Representative 1H NMR at 400 MHz of 9 (10 mM, pD 1.08) during exchange of C(3)-H (s, 9.82 ppm) for deuterium in DCl solution in D2O at 25 °C and I = 1.0 (KCl). [internal standard, tetramethylammonium deuteriosulphate (s, 3.17 ppm)]. Figure S10—Semilogarithmic plot of the fraction of unexchanged substrate against time for the deuterium exchange reaction of 8 in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Figure S11—Semilogarithmic plot of the fraction of unexchanged substrate against time for the deuterium exchange reaction of 8 in solutions of varying formate buffer concentration in D2O at 25 °C and I = 1.0 (KCl). Figure S12—Semilogarithmic plots of the fraction of unexchanged substrate against time for the deuterium exchange reaction of 9 in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Figure S13—Semilogarithmic plots of the fraction of unexchanged substrate against time for the deuterium exchange reaction of 9 in solutions of varying formate buffer concentration in D2O at 25 °C and I = 1.0 (KCl). Table S3—First order rate constants for exchange of the C(3)-H of triazolium salt 8 for deuterium in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Table S4—First order rate constants for exchange of the C(3)-H of triazolium salt 9 for deuterium in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Table S5—First order rate constants for exchange of the C(3)-H of triazolium salt 8 for deuterium, with varying formate buffer concentration, in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Table S6—First order rate constants for exchange of the C(3)-H of triazolium salt 9 for deuterium, with varying formate buffer concentration, in solutions of DCl in D2O at 25 °C and I = 1.0 (KCl). Figure S14 – Structures of pyrid-2-yl triazolium salts for which DFT calculations were undertaken of energies as a function of dihedral angle of the monocation, dication from N1 protonation (N1 dication) and dication from protonation of the pyrid-2-yl nitrogen (pyridyl dication). Figure S15—Conformational profiles of monocationic N-5-methoxypyrid-2-yl 7 ( Catalysts 11 01055 i008) and the two dicationic forms afforded from N-protonation of the triazolyl N(1) ( Catalysts 11 01055 i009) or the pyridyl nitrogen ( Catalysts 11 01055 i010) obtained by DFT calculations using B3LYP (6-311G++(d,p) basis set, PCM methanol). Figure S16—The effect of dihedral angle between N-aryl and triazolium ring on the calculated energy of the dication of 6 resulting from pyrid-2-yl nitrogen protonation obtained using B3LYP/6-311g++ (d,p) or M062X/6-311g++ (d,p) with PCM (water). Points are calculated energies with the solid curve an interpolation between the data points.

Author Contributions

Conceptualization, A.C.O. and P.Q.; methodology, A.C.O. and P.Q.; kinetic experiments, P.Q.; synthesis, P.Q.; computational modelling, M.S.S., J.Z., and P.Q.; writing—original draft preparation, A.C.O. and M.S.S.; writing—review and editing, D.R.W.H.; supervision, A.C.O. and D.R.W.H. All authors have read and agreed to the published version of the manuscript.

Funding

We thank the EPSRC (PQ, EP/M506321/1; MSS, EP/S022791/1; JZ, EP/S020713/1) for funding.

Data Availability Statement

All kinetic data are contained within the article or Supplementary Materials.

Acknowledgments

We are grateful to the Durham Chemistry NMR service for their ongoing help and support. We also thank Dmitry S. Yufit of the Durham Chemistry Crystallography Service for X-ray crystallography for 6 and 7.

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 11 01055 g001 550
Figure 1. Triazolium salt precatalysts: C(3) deprotonation to generate NHC (N-heterocyclic carbene) and common scaffolds employed in organocatalysis.
Figure 1. Triazolium salt precatalysts: C(3) deprotonation to generate NHC (N-heterocyclic carbene) and common scaffolds employed in organocatalysis.
Catalysts 11 01055 g001
Catalysts 11 01055 g002 550
Figure 2. Mechanistic studies of the C(3) H/D exchange reactions of triazolium salts in D2O solution: (a) mechanism for DO–-catalyzed exchange consistent with a first-order kinetic dependence on deuteroxide ion, (b) potential mechanism for H/D exchange at low pDs accounting for altered dependence of log kex on pD for ortho-halo N-aryl triazolium salts (e.g., 5), (c) N-pyrid-2-yl and N-5-methoxypyrid-2-yl triazolium salts 6 and 7 and di-ortho-methoxy and di-ortho-isopropoxyphenyl triazolium salts 8 and 9.
Figure 2. Mechanistic studies of the C(3) H/D exchange reactions of triazolium salts in D2O solution: (a) mechanism for DO–-catalyzed exchange consistent with a first-order kinetic dependence on deuteroxide ion, (b) potential mechanism for H/D exchange at low pDs accounting for altered dependence of log kex on pD for ortho-halo N-aryl triazolium salts (e.g., 5), (c) N-pyrid-2-yl and N-5-methoxypyrid-2-yl triazolium salts 6 and 7 and di-ortho-methoxy and di-ortho-isopropoxyphenyl triazolium salts 8 and 9.
Catalysts 11 01055 g002
Catalysts 11 01055 sch001 550
Scheme 1. Synthesis of N-5-methoxy-pyrid-2-yl triazolium tetrafluoroborate 7.
Scheme 1. Synthesis of N-5-methoxy-pyrid-2-yl triazolium tetrafluoroborate 7.
Catalysts 11 01055 sch001
Catalysts 11 01055 g003 550
Figure 3. ORTEP diagrams from X-ray crystal structures of N-pyrid-2-yl and N-5-methoxy-pyrid-2-yl triazolium tetrafluoroborate salts 6 and 7 (counterions not shown).
Figure 3. ORTEP diagrams from X-ray crystal structures of N-pyrid-2-yl and N-5-methoxy-pyrid-2-yl triazolium tetrafluoroborate salts 6 and 7 (counterions not shown).
Catalysts 11 01055 g003
Catalysts 11 01055 g004 550
Figure 4. (a) pD-rate profiles for the C(3)-H/D exchange reactions of N-pyrid-2-yl 6 (○; ●, previously published data) and N-5-methoxy-pyrid-2-yl triazolium 7 (□) tetrafluoroborate salts in DCl or buffer solutions in D2O. The solid and dashed lines show the fits of reaction data to Equations (3) and (4), respectively. (b) Plotted for comparison are log kex–pD data taken from R. S. Massey et al. [61] for N-pentafluorophenyl triazolium tetrafluoroborate 5 (△; ▲, data not included in fitting) and N-phenyl triazolium tetrafluoroborate 15 (▽; ▼, data not included in fitting).
Figure 4. (a) pD-rate profiles for the C(3)-H/D exchange reactions of N-pyrid-2-yl 6 (○; ●, previously published data) and N-5-methoxy-pyrid-2-yl triazolium 7 (□) tetrafluoroborate salts in DCl or buffer solutions in D2O. The solid and dashed lines show the fits of reaction data to Equations (3) and (4), respectively. (b) Plotted for comparison are log kex–pD data taken from R. S. Massey et al. [61] for N-pentafluorophenyl triazolium tetrafluoroborate 5 (△; ▲, data not included in fitting) and N-phenyl triazolium tetrafluoroborate 15 (▽; ▼, data not included in fitting).
Catalysts 11 01055 g004
Catalysts 11 01055 g005 550
Figure 5. Mechanism for H/D exchange consistent with first-order dependence on DO−.
Figure 5. Mechanism for H/D exchange consistent with first-order dependence on DO−.
Catalysts 11 01055 g005
Catalysts 11 01055 g006 550
Figure 6. Mechanistic options for deprotonation consistent with a formal first-order dependence on D3O+: (a) N(1)-deuteration of triazolium with subsequent C(3)-deprotonation by solvent D2O; (b) N-pyridyl deuteration of triazolium followed by C(3)-deprotonation by solvent D2O; (c) Shared intramolecular deuteration of both N(1) and the 2-pyridyl nitrogen with subsequent C(3)-deprotonation by solvent D2O; (d) N(1)-deuteration of triazolium with subsequent C(3)-deprotonation by solvent D2O and general base catalysis by 2-pyridyl substituent.
Figure 6. Mechanistic options for deprotonation consistent with a formal first-order dependence on D3O+: (a) N(1)-deuteration of triazolium with subsequent C(3)-deprotonation by solvent D2O; (b) N-pyridyl deuteration of triazolium followed by C(3)-deprotonation by solvent D2O; (c) Shared intramolecular deuteration of both N(1) and the 2-pyridyl nitrogen with subsequent C(3)-deprotonation by solvent D2O; (d) N(1)-deuteration of triazolium with subsequent C(3)-deprotonation by solvent D2O and general base catalysis by 2-pyridyl substituent.
Catalysts 11 01055 g006
Catalysts 11 01055 g007 550
Figure 7. Conformational profiles of monocationic N-pyrid-2-yl 6 ( Catalysts 11 01055 i008) and the two dicationic forms afforded from N-protonation of the triazolyl N(1) ( Catalysts 11 01055 i009) or the pyridyl nitrogen ( Catalysts 11 01055 i010) obtained by DFT calculations using a B3LYP (6–311G++(d,p) basis set [84,85,86], PCM water [87]). The inset ball and stick diagrams show the structures corresponding to the lowest energy conformations of N-pyrid-2-yl triazolium monocation 6 ( Catalysts 11 01055 i008) and the two dicationic forms ( Catalysts 11 01055 i009) or ( Catalysts 11 01055 i010).
Figure 7. Conformational profiles of monocationic N-pyrid-2-yl 6 ( Catalysts 11 01055 i008) and the two dicationic forms afforded from N-protonation of the triazolyl N(1) ( Catalysts 11 01055 i009) or the pyridyl nitrogen ( Catalysts 11 01055 i010) obtained by DFT calculations using a B3LYP (6–311G++(d,p) basis set [84,85,86], PCM water [87]). The inset ball and stick diagrams show the structures corresponding to the lowest energy conformations of N-pyrid-2-yl triazolium monocation 6 ( Catalysts 11 01055 i008) and the two dicationic forms ( Catalysts 11 01055 i009) or ( Catalysts 11 01055 i010).
Catalysts 11 01055 g007
Catalysts 11 01055 g008 550
Figure 8. Mechanistic option for deprotonation consistent with pD-independent H/D exchange.
Figure 8. Mechanistic option for deprotonation consistent with pD-independent H/D exchange.
Catalysts 11 01055 g008
Catalysts 11 01055 g009 550
Figure 9. pD-rate profiles for the C(3)-H/D exchange reactions of N-di-ortho-methoxyphenyl 8 (♢; ♦, data not included in fitting) and N-di-ortho-isopropoxyphenyl 9 (◁; ◀, data not included in fitting) tetrafluoroborate salts. The solid lines show the fit of reaction data to Equation (5). Plotted for comparison are log kex–pD data taken from R. S. Massey et al. for N-phenyl triazolium tetrafluoroborate 15 (▽; ▼, data not included in fitting) [61].
Figure 9. pD-rate profiles for the C(3)-H/D exchange reactions of N-di-ortho-methoxyphenyl 8 (♢; ♦, data not included in fitting) and N-di-ortho-isopropoxyphenyl 9 (◁; ◀, data not included in fitting) tetrafluoroborate salts. The solid lines show the fit of reaction data to Equation (5). Plotted for comparison are log kex–pD data taken from R. S. Massey et al. for N-phenyl triazolium tetrafluoroborate 15 (▽; ▼, data not included in fitting) [61].
Catalysts 11 01055 g009
Catalysts 11 01055 sch002 550
Scheme 2. Determination of C(3)-H pKa using a kinetic approach.
Scheme 2. Determination of C(3)-H pKa using a kinetic approach.
Catalysts 11 01055 sch002
Table
Table 1. Kinetic parameters from fitting of H/D exchange kinetic data for 6–9 and comparison with previous data for 15–17.
Table 1. Kinetic parameters from fitting of H/D exchange kinetic data for 6–9 and comparison with previous data for 15–17.
Triazolium SaltkDO (M−1s−1)kH (s−1)kin (s−1)FitpKa [C(3)-H] 3
Catalysts 11 01055 i0011.01 (±0.05) × 1081.35 (±0.44) × 10−4-Equation (3)
(R2 = 0.991)		-
8.79 (±0.30) × 1074.36 (±3.52) × 10−41.97 × 10−5 1Equation (4)
(R2 = 0.998)		17.4
Catalysts 11 01055 i0029.57 (±0.84) × 1072.22 (±0.93) × 10−3-Equation (3)
(R2 = 0.976)		-
8.02 (±0.22) × 1072.30 (±35.9) × 10−12.59 × 10−3 1Equation (4)
(R2 = 0.999)		17.5
Catalysts 11 01055 i0033.87 (±0.07) × 107--Equation (5) 2
(R2 = 0.999)		17.8
Catalysts 11 01055 i0042.87 (±0.13) × 107--Equation (5) 2
(R2 = 0.999)		17.9
Catalysts 11 01055 i0056.82 × 107 4--Equation (5)17.5 4
Catalysts 11 01055 i0064.20 × 107 4--Equation (5)17.8 4
Catalysts 11 01055 i0075.29 × 107 4--Equation (5)17.7 4
1 The error in kin is high owing, in part, to the limited number of datapoints in this region.2 See Section 2.2. 3 Calculated as described in Section 2.3. 4 Determined by us previously (see R. S. Massey et al. [61]).
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Quinn, P.; Smith, M.S.; Zhu, J.; Hodgson, D.R.W.; O’Donoghue, A.C. Triazolium Salt Organocatalysis: Mechanistic Evaluation of Unusual Ortho-Substituent Effects on Deprotonation. Catalysts 2021, 11, 1055. https://doi.org/10.3390/catal11091055

AMA Style

Quinn P, Smith MS, Zhu J, Hodgson DRW, O’Donoghue AC. Triazolium Salt Organocatalysis: Mechanistic Evaluation of Unusual Ortho-Substituent Effects on Deprotonation. Catalysts. 2021; 11(9):1055. https://doi.org/10.3390/catal11091055

Chicago/Turabian Style

Quinn, Peter, Matthew S. Smith, Jiayun Zhu, David R. W. Hodgson, and AnnMarie C. O’Donoghue. 2021. "Triazolium Salt Organocatalysis: Mechanistic Evaluation of Unusual Ortho-Substituent Effects on Deprotonation" Catalysts 11, no. 9: 1055. https://doi.org/10.3390/catal11091055

APA Style

Quinn, P., Smith, M. S., Zhu, J., Hodgson, D. R. W., & O’Donoghue, A. C. (2021). Triazolium Salt Organocatalysis: Mechanistic Evaluation of Unusual Ortho-Substituent Effects on Deprotonation. Catalysts, 11(9), 1055. https://doi.org/10.3390/catal11091055

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