Research Article | Open Access
Malcolm J. D’Souza, Olivia N. Hampton, Brett M. Sansbury, Dennis N. Kevill, "Evaluation of Electronic Effects in the Solvolyses of p-Methylphenyl and p-Chlorophenyl Chlorothionoformate Esters", Journal of Chemistry, vol. 2013, Article ID 248534, 9 pages, 2013. https://doi.org/10.1155/2013/248534
Evaluation of Electronic Effects in the Solvolyses of p-Methylphenyl and p-Chlorophenyl Chlorothionoformate Esters
The solvolyses of p-tolyl chlorothionoformate and p-chlorophenyl chlorothionoformate are studied in a variety of organic mixtures of widely varying nucleophilicity and ionizing power values. This solvolytic data is accumulated at 25.0°C using the titration method. An analysis of the rate data using the extended (two-term) Grunwald-Winstein equation and the concept of similarity of substrates based on their l/m ratios shows the occurrence of simultaneous side-by-side addition-elimination and unimolecular 1 mechanisms.
Chlorothionoformate esters are useful as derivatizing agents  and common organic building blocks in the synthesis of commercial thiocarbonate esters, nitriles, and isonitriles [2, 3]. High fungicidal activity was demonstrated  for the p-substituted aryl thiocarbamate analogs which are also cytotoxic .
McKinnon and Queen  affirmed that phenyl chlorothionoformate (PhOCSCl, 1, Figure 1), and alkyl chlorothionoformates (ROCSCl) in general hydrolyze rapidly to yield hydrochloric acid, carbonyl sulfide, and the corresponding alcohol. In water at 4.96°C, they obtained rates of s−1, s−1, and s−1, for PhOCSCl, methyl chlorothionoformate (MeOCSCl), and ethyl chlorothionoformate (EtOCSCl), respectively. The increase in reactivity observed with the increase in the electron-donating ability of the alkyl group, coupled with the positive entropy of activation, and a solvent deuterium isotope effect, k(D2O)/k(H2O) of 0.78 for the hydrolysis of MeOCSCl, made them conclude  that such aryl and alkyl chlorothionoformate esters hydrolyze by unimolecular 1 mechanisms.
Lee at al. [7–9] expanded on Queen’s MeOCSCl and PhOCSCl mechanistic work to include in their study the substrates ethanolyses, methanolyses, and solvolyses in water, aqueous ethanol, and aqueous acetone. They then proposed that MeSCOCl [7, 8] had 1 character in the water-rich solvents and a greater 2 character in the more organic mixtures. For PhOCSCl, Koo and others  also suggested a general base catalyzed 2 mechanism in the aqueous binary mixtures of ethanol (EtOH), methanol (MeOH), and acetone.
On the basis of large negative cross-interaction coefficients obtained for the aminolysis of substituted aryl chlorothionoformates with substituted anilines in acetonitrile, Oh et al.  proposed a concerted mechanism with a four-membered hydrogen-bonded cyclic transition state. On the other hand, Castro and coworkers [11–16] proposed that the aminolysis of chlorothionoformates using pyridine, alicyclic, and bicyclic amines is a stepwise process with the formation of a zwitterionic tetrahedral intermediate while their phenolysis  is concerted.
In a recently summarized  and ongoing solvolytic mechanistic study of nucleophilic substitution in chloroformate (ROCOCl), chlorothioformate (RSCOCl), chlorothionoformate (ROCSCl), and chlorodithioformate (RSCSCl) esters, we have successfully correlated their solvolytic rate coefficients in a series of binary aqueous organic mixtures of varying solvent nucleophilicity () [19, 20] and ionizing power () [21–23] values using the extended (two-term) Grunwald-Winstein (G-W) equation (1) :
In (1), and are the specific rates of solvolysis of a substrate in a given solvent and the standard solvent (80% ethanol), respectively, l is the sensitivity to changes in solvent nucleophilicity (N), m represents the sensitivity that controls the importance of the solvent ionizing power value (Y), and c is a constant (residual) term.
A thorough Grunwald-Winstein analysis in 49 solvents yielded an l value of 1.66, and an m value of 0.56 for phenyl chloroformate (PhOCOCl, 2) [25, 26]. The l/m ratio of 2.96 obtained was advanced as being characteristic for a stepwise addition-elimination (A-E) process that is associated with the formation of a rate-determining tetrahedral intermediate . For phenyl chlorodithionoformate (PhSCSCl, 3), we obtained , , and and proposed a unimolecular 1 ionization with strong rear-side nucleophilic solvation of the developing dithioacylium cation [26, 27]. We further recommended  that the l and m values for 2 and 3 can be taken as typical values for bimolecular addition-elimination (A-E) and unimolecular ionization (SN1) mechanisms occurring in alkyl and aryl ROCOCl substrates, including those where sulfur is substituted for one or both oxygens.
The substitution of one sulfur for the ether oxygen in PhOCOCl yields phenyl chlorothioformate (PhSCOCl, 4). For 4 in the more nucleophilic solvents, we obtained  , , , and , , and in the highly ionizing fluoroalcohol mixtures. On the other hand, for PhOCSCl (1), an l value of 1.88, an m value of 0.56, and an l/m ratio of 3.36 were obtained [26, 27] in nucleophilic solvents favoring the stepwise addition-elimination pathway (Scheme 1), and an l value of 0.34, an m value of 0.93, and an l/m ratio of 0.37 were obtained in the highly ionizing solvents suggesting a dissociative SN1 mechanism (Scheme 2) with moderate rear-side nucleophilic solvation of the developing carbocation. These results and others recently obtained [18, 25–43] clearly demonstrate that the introduction of one sulfur in ROCOCl substrates does induce a variety of superimposed mechanisms and the ranges of dominance are dependent on the R group, the presence of one or two sulfurs, and the types of solvent studied (i.e., on the and values).
Drawing upon extensive literature data and using (1) for benzoyl chloride (PhCOCl), we obtained  , , and in the less ionizing solvents, and , , and in the highly ionizing aqueous-organic mixtures. Recently, Bentley and Koo, Bentley and Harris [45, 46] provided convincing evidence that concurrent interchange mechanisms involving one dissociative and one an associative pathway do indeed occur in the solvolyses of p-substituted benzoyl chlorides.
Bentley  also calculated the Gaussian 03 (G3) values at 298K for the differences in heterolytic bond dissociation energies (HBDEs) differences and arrived at values of PhOCOCl = +4.7 kcal/mol, PhSCSCl = −18.4 kcal/mol, PhOCSCl = −13.1 kcal/mol, PhSCOCl = −8.5 kcal/mol, and PhCOCl = −11.7 kcal/mol. The calculations involve comparisons with acetyl chloride and the acetyl cation  and support the possible operation of a heterolytic fission of the covalent carbon chlorine bond in PhSCSCl, PhOCSCl, PhSCOCl, and PhCOCl, to generate a positively charged acylium (or thioacylium) ion.
Like many other ROCOCl substrates, benzyl chloroformate (PhCH2OCOCl) proceeds through a stepwise A-E process in all of the typical aqueous organic solvents except in the aqueous fluoroalcohols where a solvolysis-decomposition type mechanism with loss carbon dioxide is dominant .
Choi et al.  showed that phenyl fluorothionoformate (5) solvolyses by a bimolecular pathway in all solvents (including the fluoroalcohols) studied with the addition step of the addition-elimination reaction being rate-determining. They obtained an l value of 1.32, an m value of 0.39, an l/m ratio of 3.38, a solvent deuterium isotope effect value for methanolysis (/) of 2.11, and entropies of activation in the range of −26.2 to −21.0 cal mol−1 K−1.
An analysis of the solvolytic data for p-fluorophenyl chlorothionoformate (8) using (1) recently confirmed dual mechanistic channels (Schemes 1 and 2) occurring in the fifteen binary aqueous organic solvents studied at 35.0°C and these pathways were shown to be highly dependent on the solvents ionizing ability .
We now present the first-order specific rate constants at 25.0°C for the solvolyses of p-tolyl (p-methylphenyl) chlorothionoformate (6) and p-chlorophenyl chlorothionoformate(7) in ethanol and methanol and binary mixtures of aqueous ethanol (EtOH), aqueous methanol (MeOH), aqueous acetone, aqueous 2,2,2-trifluoroethanol (TFE), and aqueous 1,1,1,3,3,3-hexafluoro-2-propanol (HFIP). We compare the experimental rate data of 6 and 7 and their correlation results obtained using the two-term Grunwald-Winstein equation (1) to those previously published [9, 25–28, 40, 49–51] for compounds 1–5 and 8.
2. Results and Discussion
The first-order specific rates of solvolysis of 6 and 7 at 25.0°C in pure and aqueous organic mixtures of widely varying nucleophilicity () and ionizing power values () are reported in Table 1. In 6 and 7, there is a gradual rate increase that coincides with the increase of water content in the aqueous-organic mixtures (with increasing values). On the other hand, in the strongly hydrogen-bonding aqueous-HFIP mixtures, the first-order specific rates for 6 and 7 decrease with increasing water content (and increasing and decreasing values). One can also observe that 7 is approximately 10-fold faster than 6 in the aqueous ethanol solvents and 2- to 3-fold faster in the aqueous methanol and acetone mixtures, but this situation is reversed with 6 being the faster in the aqueous fluoroalcohol (TFE and HFIP) mixtures.
|ubstrate concentration of ca. 0.0052 M; binary solvents on a volume-volume basis at 25.0°C, except for TFE-H2O and HFIP-H2O solvents which are on a weight-weight basis. T-E are TFE-ethanol mixtures. ith associated standard deviation. eferences [19, 20]. eferences [21–23].|
In 100% EtOH at 25.0°C, the rates of solvolysis for substrates 1-8 are s−1 , s−1 , s−1 , s−1 , s−1 (estimated from specific rates at lower temperature) , s−1, s−1, and s−1 , respectively. For compounds 1–5 and 8, a tetrahedral A-E transition state is proposed for their ethanolyses [25, 27, 28, 40, 49]. The rate order in pure ethanol of reveals that the rate of the dithioester is the slowest. This suggests that the inductive capacity of the thiophenoxy group in 3 is very inefficient.
A comparison of just the p-substituted aryl chlorothionoformate ethanolysis rate exhibits a rate order of . These observations are consistent with the Hammett values of +0.23, +0.06, and −0.17  for para-Cl, para-F, and para-CH3, respectively, with increased electron-withdrawing ability for the substituent favoring the rate-determining addition of a solvent molecule at the carbonyl carbon.
An addition-elimination mechanism with the addition step rate-determining is favored for phenyl fluorothionoformate (5) in all of the solvents studied at 10.0°C . Using the similarity model concept [29, 53], we first compared the log (k/) values for p-tolyl chlorothionoformate (6) to those obtained for 5. This plot is shown in Figure 2 for the seventeen common binary solvents studied. This xy-graph results in an abominable correlation coefficient (R) of 0.169, slope of , intercept (c) of , and F-test of 0.4. A review of the plot shows significant deviation for the 90 HFIP, 70HFIP, and 90 TFE values and a noticeable divergence from the line-of-best fit for the four TFE-EtOH mixtures, especially for the 80T-20E point. Removal of these seven data points does indeed improve the correlation significantly resulting in a R value of 0.973, slope of , and . This illustrates that, like 5, the A-E mechanism is the dominant pathway for 6 in the ten remaining ethanol, methanol, and binary mixtures of aqueous ethanol, methanol, and acetone. The slope of indicates that in these ten solvents there is a much later transition state for addition to 6 when compared to that seen for the solvolyses of 5.
Using the extended Grunwald-Winstein equation (1) for all of the twenty specific rates of solvolysis of 6 listed in Table 1 leads to a very inferior correlation coefficient (R) of 0.505, , , , and a very low F-test value of 2.9. For the two-term G-W analyses, these are unacceptable correlation and F-test values and this could reflect the presence of concurrent mechanisms.
In Table 2, we report the relevant G-W analyses for substrates 1-8. Figure 2 clearly shows that the highly ionizing common solvents (90 HFIP, 70HFIP, 90 TFE, and 80T-20E) deviate the most in the plot that is presented for log versus log . Removal of the three HFIP (97, 90, and 70) values, the three TFE (97, 90, and 80) values, and the 80T-20E rate value, in the G-W analyses of 6, results in a marginal , , , , and a F-test of 17. However, deletion of any additional TFE-EtOH points does not improve the correlation coefficient but the P value (probability value indicating that the results are statistically insignificant) for the l term rises and the F-test value decreases substantially. The resulting l/m ratio of 3.54 observed is in line with values observed in the aryl chlorothionoformate substrates 1 () and 8 () for solvents governed by a dissociative A-E mechanism shown in Scheme 1.
| is the number of solvents. ith associated standard error. orrelation coefficient. -test value. alues taken from [26, 27]. alues taken from [25, 26]. alues taken from . alues taken from . xcluding the data points in aqueous HFIP, aqueous TFE, and 80T-20E in regression calculations. sing only the data points in aqueous HFIP, aqueous TFE, and 80T-20E in regression calculations. alues taken from .|
For 6, in the seven strongly hydrogen-bonding solvents of 80T-20E, aqueous TFE, and aqueous HFIP, we get an l value of , an m value of , a c value of , an R value of 0.986, and a F-test value of 69, all derived from a G-W analyses using (1) (and listed in Table 2). The l value has an associated P value of 0.03, indicating that the result is statistically significant . A large negative c value is observed because the experimental value is the one applying to the other reaction channel. For 6 in the ionizing fluoroalchohol mixtures, the l and the m values and the l/m ratio of 0.42 are in the range previously observed for ionization reactions (Scheme 2) for 1 () and 8 ().
A plot of log against 1.63 + 0.46 in the twenty pure and binary solvents studied is shown in Figure 3. The seven fluoroalcohol-containing mixtures (80T-20E; 97, 90, 70, HFIP; 97, 90, 80 TFE) were excluded in the correlation analysis but are added on the plot to show their extent of deviation from the correlation line. In Figure 3, if one carefully scrutinizes the positioning of the 80T-20E data point, one can discern that there may well be some contribution from the A-E pathway in this solvent mixture. Using the equation log = 1.63 + 0.46 + 0.30, one can estimate the addition-elimination pathway specific rate for 6 in 80T-20E to be s−1. This would suggest that in 80T-20E there is a 22% contribution from the addition-elimination pathway.
In Figure 4, we show a plot of log for 4-chlorophenyl chlorothionoformate (7) against log for phenyl fluorothionoformate (5) in the seventeen common pure and binary solvents studied. This linear regression results in an inadequate correlation coefficient on 0.812, slope of , intercept of , and an F-test value of 29. It is apparent from Figure 4 that the 90 HFIP and 90 TFE values digress considerably from the correlation line. Excluding these two values leads to a significantly improved , slope of , intercept of , and an F-test value of 160. This analysis promotes the possibility that for 7 in the remaining fifteen solvents a similar bimolecular addition-elimination pathway is operative.
For 7 using (1) for all of the nineteen solvents listed in Table 1 results in a low correlation coefficient of 0.679 to values with high standard errors associated of , , , and a dismal F-test value of 7. Observing that the 90 HFIP and 90 TFE values deviated significantly in Figure 4, it would be expected that if specific rates for solvolysis of 5 had been available the deviations for 97 HFIP and 97 TFE would have been even greater.
Excluding the 97, and 90 HFIP, and 97, and 90 TFE data points in the G-W analyses using (1), we obtain improved values of , , , , and an F-test value of 41. Further omission of the three aqueous HFIP (97, 90, and 50) and the three aqueous TFE (97, 90, and 50) values leads to a much improved R=0.966, , , , and F-test value = 69 (reported in Table 2). The sensitivities l and m obtained are typical for substrates undergoing overall nucleophilic substitution (A-E mechanism) involving rate-determining formation of a tetrahedral intermediate (shown in Scheme 1). The l/m ratio of 3.98 observed is a little higher than those observed for solvolyses of aryl chlorothionoformate esters 1 (), 6 (), and 8 ().
We have used the l/m ratio to suggest earlier and later transition states within otherwise very similar mechanisms and as a useful indicator for the presence of general base catalysis [55, 56] in solvolytic reactions of this type . The l/m ratios for p-chlorobenzoyl chloride, p-nitrobenzoyl chloride, p-nitrophenyl chloroformate, and p-nitrobenzyl chloroformate of 3.19, 3.29, 3.67, and 3.50 [29, 44] are of similar values to those obtained for the aryl chlorothionoformate 1 and 6–8 when they are reacting by the addition-elimination channel.
A plot of log for 4-chlorophenyl chlorothionoformate (7) against 1.79 + 0.45 in the nineteen pure and binary solvents studied is shown in Figure 5. The six data points for 97, 90, and 50 HFIP and 97, 90, and 50 TFE were excluded from the G-W analyses using (1) but were added to the plot to show their positive deviations from the correlation line.
Examination of Figure 5 indicates that the 50 TFE point is quite adjacent to the correlation line. Hence for this solvent there is the possibility of having a concurrent contribution from the A-E pathway. Using the equation log (k/ko)7 = 1.79 + 0.45 – 0.05, we have estimated A-E rates of s−1, s−1, s−1, s−1, and s−1, for 97 TFE, 90 TFE, 50 TFE, 80T-20E, and 50 HFIP, respectively. These calculations correspond to 2%, 5%, 40%, 53%, and 7% contributions from the A-E pathway for the solvolyses in these solvents.
After subtracting out the A-E component in the rates of reaction of 7 that were indicated to be occurring in the seven fluoroalcohol mixtures (97-50 HFIP, 97-50 TFE, and 80T-20E), we can then carry out a correlation of the estimated specific rates remaining to get , , , (large negative value because is for the A-E pathway), and a F-test value of 10. The l/m ratio of 0.52 is typical for 1 mechanisms seen in acyl halides and of the type shown in Scheme 2.
For the aryl chlorothionoformate esters 1, 6, 7, and 8, the evidence for a change in mechanism from a bimolecular A-E pathway to an ionization (1) mechanism in the highly ionizing fluoroalcohol mixtures is compelling and occurs even in substrates (7 and 8) that contain electron-withdrawing halogen substituents in the para position. These observations are consistent with Bentley’s G3 calculations that a C=S bond strongly stabilizes the developing carbocation . This formation of a cationic transition-state, favored in the highly ionizing solvent mixtures, is in all probability due to sulfur’s ability to modify its electron cloud and therefore to be highly polarizable.
The p-tolyl chlorothionoformate (6) and the p-chlorophenyl chlorothionoformate (7) are shown to solvolyze by the generation of concurrent bimolecular stepwise addition-elimination and unimolecular ionization (1) mechanisms. The exact delineation of the change in mechanism is identified utilizing the concept of substrate similarity based on l/m ratios, and statistical results obtained through the application of the two-term extended Grunwald-Winstein equation (1).
For 6 in the more nucleophilic solvents, we obtain an l value of 1.63, an m value of 0.46, and an l/m ratio of 3.54. For 7 in a similar set of solvents, we obtain an l value of 1.79, an m value of 0.45, and an l/m ratio of 3.98. It is now proposed that in such nucleophilic solvents 6 and 7 undergo an addition-elimination (association-dissociation) process with the addition-step being rate determining.
In the strongly hydrogen-bonding aqueous HFIP, aqueous TFE, and 80T-20E mixtures, we obtain an l value of 0.45, an m value of 1.07, and an l/m ratio of 0.42 for 6, and an l value of 0.43, an m value of 0.82, and an l/m ratio of 0.52 for 7. The sensitivities for l and m obtained (for 6 and 7) are befitting the proposal of an ionization component with an appreciable nucleophilic solvation of the developing cationic transition state.
We also found that for solvolyses of 6 there is evidence for a superimposed addition-elimination component of 22% in 80T-20E, and for 7 there are contributions from the A-E pathway of 2%, 5%, 40%, 53%, and 7% in 97 TFE, 90 TFE, 50 TFE, 80T-20E, and 50 HFIP, respectively.
4. Experimental Section
The p-tolyl chlorothionoformate (97%, Sigma-Aldrich), and the p-chlorophenyl chlorothionoformate (98%, Sigma-Aldrich) were used as received. Solvents were purified and the kinetic runs carried out as described previously . A substrate concentration of approximately 0.005 M in a variety of solvents was employed. For some of the runs, calculation of the specific rates of solvolysis (first-order rate coefficients) was carried out by a process  in which the conventional Guggenheim treatment was modified so as to give an estimate of the infinity titer, which was then used to calculate for each run a series of integrated rate coefficients. The specific rates and associated standard deviations, as presented in Table 1, were obtained by averaging all of the values from, at least, duplicate runs.
Multiple regression analyses were carried out using the Excel 2010 package from the Microsoft Corporation, and the SigmaPlot 9.0 software version from Systat Software, Inc., San Jose, CA, was used for the Guggenheim treatments.
O. N. Hampton and B. M. Sansbury completed this research under the direction of M. J. D’Souza as undergraduate research assistants in the DE-INBRE/DE-EPSCR sponsored Wesley College Directed Research Program in Chemistry. D. N. Kevill is a collaborator on this project.
The undergraduate research is supported by grants (DE-INBRE and DE-EPSCoR programs) from the National Center for Research Resources (NCRR) (5P20RR016472-12) and the National Institute of General Medical Sciences (NIGMS) (8 P20 GM103446-12) from the National Institutes of Health (NIH); a National Science Foundation (NSF) Delaware EPSCoR Grant EPS-0814251; an NSF MRI grant 0520492; an NSF ARI-R2 Grant 0960503. The authors would also like to thank T. W. Bentley for helpful discussions.
- D. H. R. Barton, P. Blundell, J. Dorchak, D. O. Jang, and J. C. Jaszberenyi, “The invention of radical reactions. Part XXI. Simple methods for the radical deoxygenation of primary alcohols,” Tetrahedron, vol. 47, no. 43, pp. 8969–8984, 1991.
- D. Subhas Bose and P. Ravinder Goud, “Aryl chlorothionoformate: a new versatile reagent for the preparation of nitriles and isonitriles under mild conditions,” Tetrahedron Letters, vol. 40, no. 4, pp. 747–748, 1999.
- S. M. Rahmathullah, J. E. Hall, B. C. Bender, D. R. McCurdy, R. R. Tidwell, and D. W. Boykin, “Prodrugs for amidines: synthesis and anti-Pneumocystis carinii activity of carbamates of 2,5-bis(4-amidinophenyl)furan,” Journal of Medicinal Chemistry, vol. 42, no. 19, pp. 3994–4000, 1999.
- M. Albores-Velasco, J. Thorne, and R. L. Wain, “Fungicidal activity of phenyl N-(4-substituted-phenyl)thionocarbamates,” Journal of Agricultural and Food Chemistry, vol. 43, no. 8, pp. 2260–2261, 1995.
- M. A. H. Zahran, T. A. R. Salem, R. M. Samaka, H. S. Agwa, and A. R. Awad, “Design, synthesis and antitumor evaluation of novel thalidomide dithiocarbamate and dithioate analogs against Ehrlich ascites carcinoma-induced solid tumor in Swiss albino mice,” Bioorganic and Medicinal Chemistry, vol. 16, no. 22, pp. 9708–9718, 2008.
- D. M. McKinnon and A. Queen, “Kinetics and mechanism for the hydrolysis of chlorothionoformates and chlorodithioformate esters in water and aqueous acetone,” Canadian Journal of Chemistry, vol. 50, pp. 1401–1406, 1972.
- S. La, K. S. Koh, and I. Lee, “Nucleophilic substitution at a carbonyl carbon atom (XI). Solvolysis of methyl chloroformate and its thioanalogues in methanol, ethanol and ethanol-water mixtures,” Journal of the Korean Chemical Society, vol. 24, no. 1, pp. 1–7, 1980.
- S. La, K. S. Koh, and I. Lee, “Nucleophilic substitution at a carbonyl carbon atom (XII). Solvolysis of methyl chloroformate and its thioanalogues in CH3CN-H2O and CH3COCH3-H2O mixtures,” Journal of the Korean Chemical Society, vol. 24, no. 1, pp. 8–14, 1980.
- I. S. Koo, K. Yang, D. H. Kang, H. J. Park, K. Kang, and I. Lee, “Transition-state variation in the solvolyses of phenyl chlorothionoformate in alcohol-water mixtures,” Bulletin of the Korean Chemical Society, vol. 20, no. 5, pp. 577–580, 1999.
- H. K. Oh, J. S. Ha, D. D. Sung, and I. Lee, “Aminolysis of aryl chlorothionoformates with anilines in acetonitrile: effects of amine nature and solvent on the mechanism,” Journal of Organic Chemistry, vol. 69, no. 24, pp. 8219–8223, 2004.
- E. A. Castro, M. Cubillos, and J. G. Santos, “Kinetics and mechanism of the aminolysis of phenyl and 2-nitrophenyl chlorothionoformates,” Journal of Organic Chemistry, vol. 62, no. 13, pp. 4395–4397, 1997.
- E. A. Castro, “Kinetics and mechanisms of reactions of thiol, thiono, and dithio analogues of carboxylic esters with nucleophilies,” Chemical Reviews, vol. 99, no. 12, pp. 3505–3524, 1999.
- E. A. Castro, M. Cubillos, and J. G. Santos, “Kinetics and mechanisms of the pyridinolysis of phenyl and 4-nitrophenyl chlorothionoformates formation and hydrolysis of 1-(aryloxythiocarbonyl) pyridinium cations,” Journal of Organic Chemistry, vol. 69, no. 14, pp. 4802–4807, 2004.
- E. A. Castro, M. Aliaga, P. R. Campodonico, J. R. Leis, L. García-Río, and J. G. Santos, “Reactions of aryl chlorothionoformates with quinuclidines. A kinetic study,” Journal of Physical Organic Chemistry, vol. 21, no. 2, pp. 102–107, 2008.
- E. A. Castro, “Kinetics and mechanisms of reactions of thiol, thiono and dithio analogues of carboxylic esters with nucleophiles. An update,” Journal of Sulfur Chemistry, vol. 28, no. 4, pp. 407–435, 2007.
- E. A. Castro, M. Gazitúa, and J. G. Santos, “Kinetics and mechanism of the reactions of aryl chlorodithioformates with pyridines and secondary alicyclic amines,” Journal of Physical Organic Chemistry, vol. 22, no. 11, pp. 1030–1037, 2009.
- E. A. Castromaria Cubillos and J. G. Santos, “Concerted mechanisms of the reactions of phenyl and 4-nitrophenyl chlorothionoformates with substituted phenoxide ions,” Journal of Organic Chemistry, vol. 63, no. 20, pp. 6820–6823, 1998.
- D. N. Kevill and M. J. D'Souza, “Sixty years of the Grunwald-Winstein equation: development and recent applications,” Journal of Chemical Research, no. 2, pp. 61–66, 2008.
- D. N. Kevill and S. W. Anderson, “An improved scale of solvent nucleophilicity based on the solvolysis of the S-methyldibenzothiophenium ion,” Journal of Organic Chemistry, vol. 56, no. 5, pp. 1845–1850, 1991.
- D. N. Kevill, “Development and uses of scales of solvent nucleophilicity,” in Advances in Quantitative Structure-Property Relationships, M. Charton, Ed., vol. 1, pp. 81–115, JAI Press, Greenwich, Conn, USA, 1996.
- T. W. Bentley and G. E. Carter, “The 2-1 spectrum. 4. The 2 (intermediate) mechanism for solvolyses of tert-butyl chloride: a revised Y scale of solvent ionizing power based on solvolyses of 1-adamantyl chloride,” Journal of the American Chemical Society, vol. 104, no. 21, pp. 5741–5747, 1982.
- T. W. Bentley and G. Llewellyn, “ scales of solvent ionizing power,” Progress Physical Organic Chemistry, vol. 17, pp. 121–158, 1990.
- D. N. Kevill and M. J. D’Souza, “Additional values and the correlation of the specific rates of solvolysis of tert-butyl chloride in terms of and scales,” Journal of Chemical Research, no. 5, pp. 174–175, 1993.
- S. Winstein, E. Grunwald, and H. Walter Jones, “The correlation of solvolysis rates and the classification of solvolysis reactions into mechanistic categories,” Journal of the American Chemical Society, vol. 73, no. 6, pp. 2700–2707, 1951.
- D. N. Kevill and M. J. D'Souza, “Correlation of the rates of solvolysis of phenyl chloroformate,” Journal of the Chemical Society, no. 9, pp. 1721–1724, 1997.
- D. N. Kevill, F. Koyoshi, and M. J. D'Souza, “Correlations of the specific rates of solvolysis of aromatic carbamoyl chlorides, chloroformates, chlorothionoformates, and chlorodithioformates revisited,” International Journal of Molecular Sciences, vol. 8, no. 4, pp. 346–362, 2007.
- D. N. Kevill and M. J. D'Souza, “Correlation of the rates of solvolysis of phenyl chlorothionoformate and phenyl chlorodithioformate,” Canadian Journal of Chemistry, vol. 77, no. 5-6, pp. 1118–1122, 1999.
- D. N. Kevill, M. W. Bond, and M. J. D'Souza, “Dual pathways in the solvolyses of phenyl chlorothioformate,” Journal of Organic Chemistry, vol. 62, no. 22, pp. 7869–7871, 1997.
- M. J. D'Souza, K. E. Shuman, S. E. Carter, and D. N. Kevill, “Extended Grunwald-Winstein analysis—LFER used to gauge solvent effects in p-nitrophenyl chloroformate solvolysis,” International Journal of Molecular Sciences, vol. 9, no. 11, pp. 2231–2242, 2008.
- M. J. D'Souza, D. N. Reed, K. J. Erdman, J. B. Kyong, and D. N. Kevill, “Grunwald-winstein analysis—isopropyl chloroformate solvolysis revisited,” International Journal of Molecular Sciences, vol. 10, no. 3, pp. 862–879, 2009.
- M. J. D'Souza, S. M. Hailey, and D. N. Kevil, “Use of empirical correlations to determine solvent effects in the solvolysis of S-methyl chlorothioformate,” International Journal of Molecular Sciences, vol. 11, no. 5, pp. 2253–2266, 2010.
- H. J. Koh, S. J. Kang, and D. N. Kevill, “Kinetic studies of the solvolyses of 2,2,2-trichloro-1,1-dimethylethyl chloroformate,” Bulletin of the Korean Chemical Society, vol. 31, no. 4, pp. 835–839, 2010.
- M. J. D'Souza, B. P. Mahon, and D. N. Kevill, “Analysis of the nucleophilic solvation effects in isopropyl chlorothioformate solvolysis,” International Journal of Molecular Sciences, vol. 11, no. 7, pp. 2597–2611, 2010.
- M. J. D'Souza, S. E. Carter, and D. N. Kevill, “Correlation of the rates of solvolysis of neopentyl chloroformate-A recommended protecting agent,” International Journal of Molecular Sciences, vol. 12, no. 2, pp. 1161–1174, 2011.
- D. H. Moon, M. H. Seong, J. B. Kyong, Y. Lee, and Y. W. Lee, “Correlation of the rates of solvolysis of 1- and 2-Naphthyl chloroformates using the extended grunwald-winstein equation,” Bulletin of the Korean Chemical Society, vol. 32, no. 7, pp. 2413–2417, 2011.
- M. J. D’Souza, A. M. Darrington, and D. N. Kevill, “A study of solvent effects in the solvolysis of propargyl chloroformate,” ISRN Organic Chemistry, vol. 2011, Article ID 7671411, 6 pages, 2011.
- H. J. Koh and S. J. Kang, “A kinetic study on solvolysis of 9-fluorenylmethyl chloroformate,” Bulletin of the Korean Chemical Society, vol. 32, no. 10, pp. 3799–3801, 2011.
- M. J. D'Souza, M. J. McAneny, D. N. Kevill, J. B. Kyong, and S. H. Choi, “Kinetic evaluation of the solvolysis of isobutyl chloro-and chlorothioformate esters,” Beilstein Journal of Organic Chemistry, vol. 7, pp. 543–552, 2011.
- M. J. D’Souza, K. E. Shuman, A. O. Omondi, and D. N. Kevill, “Detailed analysis for the solvolysis of isopropenyl chloroformate,” European Journal of Chemistry, vol. 2, no. 2, pp. 130–135, 2011.
- M. J. D’Souza, S. M. Hailey, B. P. Mahon, and D. N. Kevill, “Understanding solvent effects in the solvolysis of 4-fluorophenyl chlorothionoformate,” Chemical Sciences Journal, vol. CSJ-35, pp. 1–9, 2011.
- H. J. Koh and S. J. Kang, “Correlation of the rates on solvolysis of 2,2,2-trichloroethyl chloroformate using the extended grunwald-winstein equation,” Bulletin of the Korean Chemical Society, vol. 33, no. 5, pp. 1729–1733, 2012.
- M. J. D'Souza, J. A. Knapp, G. A. Fernandez-Bueno, and D. N. Kevill, “Use of linear free energy relationships (LFERS) to elucidate the mechanisms of reaction of a γ-methyl-β-alkynyl and an ortho-infstituted aryl chloroformate ester,” International Journal of Molecular Sciences, vol. 13, no. 1, pp. 665–682, 2012.
- J. B. Kyong, Y. Lee, M. J. D’Souza, B. P. Mahon, and D. N. Kevill, “Correlation of the rates of solvolysis of tert-butyl chlorothioformate and observations concerning the reaction mechanism,” European Journal of Chemistry. In press.
- D. N. Kevill and M. J. D'Souza, “Correlation of the rates of solvolysis of benzoyl chloride and derivatives using extended forms of the Grunwald-Winstein equation,” Journal of Physical Organic Chemistry, vol. 15, no. 12, pp. 881–888, 2002.
- T. W. Bentley and I. S. Koo, “Concurrent pathways to explain solvent and substituent effects for solvolyses of benzoyl chlorides in ethanol-trifluoroethanol mixtures,” Arkivoc, vol. 2012, no. 7, pp. 25–34, 2012.
- T. W. Bentley and H. C. Harris, “Solvolyses of benzoyl chlorides in weakly nucleophilic media,” International Journal of Molecular Sciences, vol. 12, no. 8, pp. 4805–4818, 2011.
- T. W. Bentley, “Structural effects on the solvolytic reactivity of carboxylic and sulfonic acid chlorides. Comparisons with gas-phase data for cation formation,” Journal of Organic Chemistry, vol. 73, no. 16, pp. 6251–6257, 2008.
- J. B. Kyong, B. C. Park, C. B. Kim, and D. N. Kevill, “Rate and product studies with benzyl and p-nitrobenzyl chloroformates under solvolytic conditions,” Journal of Organic Chemistry, vol. 65, no. 23, pp. 8051–8058, 2000.
- S. H. Choi, M. H. Seong, Y. W. Lee, J. B. Kyong, and D. N. Kevill, “Correlation of the rates of solvolysis of phenyl fluorothionoformate,” Bulletin of the Korean Chemical Society, vol. 32, no. 4, pp. 1268–1272, 2011.
- K. H. Yew, H. J. Koh, H. W. Lee, and I. Lee, “Nucleophilic substitution reactions of phenyl chloroformates,” Journal of the Chemical Society, no. 12, pp. 2263–2268, 1995.
- S. K. An, J. S. Yang, J. M. Cho et al., “Correlation of the rates of solvolysis of phenyl chlorodithioformate,” Bulletin of the Korean Chemical Society, vol. 23, no. 10, pp. 1445–1450, 2002.
- C. Hansch and A. Leo, Substituent Constants for Correlation Analysis in Chemistry and Biology, Wiley-Interscience, New York, NY, USA, 1979.
- T. W. Bentley and M. S. Garley, “Correlations and predictions of solvent effects on reactivity: some limitations of multi-parameter equations and comparisons with similarity models based on one solvent parameter,” Journal of Physical Organic Chemistry, vol. 19, no. 6, pp. 341–349, 2006.
- M. D. Markel, “The power of a statistical test. What does insignificance mean?” Veterinary Surgery, vol. 20, no. 3, pp. 209–214, 1991.
- T. W. Bentley and H. C. Harris, “Separation of mass law and solvent effects in kinetics of solvolyses of p-nitrobenzoyl chloride in aqueous binary mixtures,” Journal of Organic Chemistry, vol. 53, no. 4, pp. 724–728, 1988.
- T. W. Bentley, H. C. Harris, Z. H. Ryu, G. T. Lim, D. D. Sung, and S. R. Szajda, “Mechanisms of solvolyses of acid chlorides and chloroformates. Chloroacetyl and phenylacetyl chloride as similarity models,” Journal of Organic Chemistry, vol. 70, no. 22, pp. 8963–8970, 2005.
- D. N. Kevill and M. H. Abduljaber, “Correlation of the rates of solvolysis of cyclopropylcarbinyl and cyclobutyl bromides using the extended Grunwald-Winstein equation,” Journal of Organic Chemistry, vol. 65, no. 8, pp. 2548–2554, 2000.
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