Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane

Baumstark, A. L.; Franklin, P. J.; Vasquez, P. C.; Crow, B. S.

doi:10.3390/90300117

Open AccessArticle

Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane

by

A. L. Baumstark

^*,

P. J. Franklin

,

P. C. Vasquez

and

B. S. Crow

Department of Chemistry, Center for Biotech and Drug Design, Georgia State University, Atlanta, Georgia 30303-3083, USA

^*

Author to whom correspondence should be addressed.

Molecules 2004, 9(3), 117-124; https://doi.org/10.3390/90300117

Submission received: 5 February 2004 / Accepted: 12 February 2004 / Published: 28 February 2004

(This article belongs to the Special Issue Biologically Relevant Heterocyclic Compounds)

Download

Browse Figure

Versions Notes

Abstract

:

The mono-epoxidation of geraniol by dimethyldioxirane was carried out in various solvents. In all cases, the product ratios for the 2,3 and 6,7 mono-epoxides were in agreement with literature values. Kinetic studies were carried out at 23 °C in the following dried solvent systems: acetone (k₂ = 1.49 M^-1s^-1), carbon tetrachloride/acetone (9/1, k₂=2.19 M^-1s^-1), and methanol/acetone (9/1, k₂ = 17 M^-1s^-1). Individual k₂ values were calculated for epoxidation of the 2,3 and 6,7 positions in geraniol. The non-conjugated diene system was modeled employing two simple independent alkenes: 2‑methyl-2-pentene and 3-methyl-2-buten-1-ol by determining the respective k₂ values for epoxidation in various solvents. The kinetic results for each independent alkene showed that the relative reactivity of the two epoxidation sites in geraniol as a function of solvent was not simply a summation of the independent alkene systems.

Keywords:

Mono-epoxidation; selectivity

Introduction

Dioxiranes are powerful oxidants that efficiently transfer an oxygen atom to a wide variety of organic substrates [1]. Numerous synthetically useful transformations have been carried out employing dioxiranes. Dioxirane chemistry provides a model for mechanistic insights into electrophilic oxygen-atom transfer in biological systems. Dimethyldioxirane (1), either generated in situ [2] or in isolated solution [3], has been found to be a versatile epoxidizing reagent for a wide variety of alkenes. Epoxidation by 1 has been shown to be stereospecific and quantitative and to occur via a concerted electrophilic process with a “spiro” transition state [4]. The reaction of alkenes with 1 has been shown to be sensitive to steric factors. In general, cis alkenes have been found [4] to show greater reactivity than the corresponding trans compounds. Recently, product studies on the epoxidation of alkenes containing hydroxy groups have suggested [5,6] that (intermolecular) hydrogen bonding increases reactivity and affects product distributions. Computational studies have predicted [7] that hydrogen bonding of the hydroxy group of geraniol would lower the enthalpy of activation for epoxidation by a dioxirane. We report here a kinetics study on the mono-epoxidation of geraniol and selected model compounds by dimethyldioxirane in various solvents.

Results and Discussion

The reaction of dimethyldioxirane 1 with geraniol 2 in dried acetone, carbon tetrachloride/dried acetone (9/1) and methanol/acetone (9/1 wet and dried) was carried out at 23 °C under conditions [5,6] in which only the mono-epoxides 3 and 4 were formed (Reaction 1). The combined yields of 3 and 4 were essentially quantitative with respect to 1, the limiting reagent under these conditions. The products were isolated and characterized by NMR and GC/MS techniques. Results are summarized in Table 1.

Table 1. Product distributions for the mono-epoxidation of geraniol by dimethyldioxirane at 23 °C in various solvents.

**Table 1.** Product distributions for the mono-epoxidation of geraniol by dimethyldioxirane at 23 °C in various solvents.
Entry	Solvent	Product distribution, %
Entry	Solvent	3		4
1	Acetone^a	68	(74)^c	32	(26)^c
2	CCl₄/Acetone (9:1)^a	52	(51)^d	48	(49)^d
3	Methanol/Acetone (9:1)^a	79	--	21	--
4	Methanol/Acetone (9:1)^b	84	(88)^d	16 (12)^d	(12)^d

a) dried; b) wet; c) Ref. [5]; d) Ref. [6]

The product distributions (as determined by GC/MS and NMR spectroscopy ± 4%) were in good agreement with published studies [5,6]. The results in dried acetone/methanol (entry 3) have not been previously reported. The presence of fortuitous water seems to result in a slight increase in the yield of epoxide 3 at the expense of 4. The reaction of two independent alkenes: 2-methyl-2-pentene (5) and 3-methyl-2-buten-1-ol (6), with 1 as a model for the geraniol system yielded the corresponding epoxides in quantitative yield, respectively (reactions 2 and 3), independent of solvent. The results for 5 in acetone were in agreement with published data [8].

(2)

(3)

The reaction of 1 with the various alkenes was shown to be of the second order overall as expected (first order in both alkene and dioxirane). The second order rate constants (k₂s) were measured at 23 °C by monitoring the UV absorbance decay of 1 at 330 nm. The reactions were carried out in the following solvents: a) dried acetone, b) carbon tetrachloride/ dried acetone (9:1) and c) dried methanol/ dried acetone (9:1). The k₂ values for geraniol are reflective of those for the overall molecule (both sites). Pseudo first order conditions were employed for most of the k₂ determinations. Those in methanolic solvent for 5 and 6 were carried out under equal molar conditions.

Figure 1. Representative Data for the Mono-Epoxidation of Geraniol by 1 in Various Dried Solvents at 23 °C.

Figure 1 shows representative results for mono-epoxidation of geraniol by 1 in the three solvent systems. The k₂ values for epoxidation of alkenes 2, 5 and 6 are listed in Table 2.

Table 2. Second order rate constants for the mono-epoxidation of alkenes 2, 5 and 6 by 1 in various solvents at 23 °C.

**Table 2.** Second order rate constants for the mono-epoxidation of alkenes 2, 5 and 6 by 1 in various solvents at 23 °C.
Alkene	Structure	Solvent^a	k₂ (M^-1s^-1)	k_rel
2		Acetone	1.49 ± 0.02^b	≡1.0
		CCl₄/Acetone (9:1)	2.19 ± 0.05 ^b	1.5
		MeOH/Acetone (9:1)	17 ± 1 ^b	11.4
5		Acetone	0.99 ± 0.02	≡1.0
		CCl₄/Acetone (9:1)	1.10 ± 0.05	1.1
		MeOH/Acetone (9:1)	27 ± 2	27
6		Acetone	0.68 ± 0.02	≡1.0
		CCl₄/Acetone (9:1)	2.03 ± 0.10	3.0
		MeOH/Acetone (9:1)	7.5 ± 0.5	11.5

a) dried; b) per molecule (both olefinic sites)

The separate second order rate constants for epoxidation of the 6,7 and 2,3 sites in geraniol were calculated from the overall k₂ values (Table 2) and the observed product distributions (Table 1). The results as well as the relative rate calculations in the three solvent systems are listed in Table 3. Interestingly, the relative behavior of the two independent sites in geraniol is different. The results for 2,3 and 6,7 epoxidation show some of the characteristics observed for the model systems (5 and 6) with interesting differences (vide infra).

Table 3. Calculated second order rate constants of epoxidation of 6,7 and 2,3 sites of geraniol at 23 °C.

**Table 3.** Calculated second order rate constants of epoxidation of 6,7 and 2,3 sites of geraniol at 23 °C.
Entry	Solvent^a	k_6,7 (M^-1s^-1)	k_rel	k_2,3 (M^-1s^-1)	k_rel
1	Acetone	2.03	≡1.0	0.95	≡1.0
2	CCl₄/Acetone (9:1)	2.28	1.1	2.10	2.2
3	MeOH/Acetone (9:1)	26	13	6.9	7.3

a) dried

Product studies for mono-epoxidation of geraniol by dimethyldioxirane are well documented [5,6]. Adam et al. [5,6] found that the reaction of dioxirane 1 with equimolar geraniol in acetone yielded 9% bis-epoxide and the mono-epoxides 3 and 4 in a 73:17 ratio. No bis-epoxide was noted when 0.3 equivalents of 1 were used. The present yield data, obtained under the latter conditions, are in good to excellent agreement with the published work, especially when one notes that adventitious moisture affects the 3 to 4 ratios. In addition, the variation in product ratio as a function of solvent is also in good agreement with published results.

The geraniol study was designed as an intramolecular competition experiment in which absolute rate studies were not necessary [6]. The results were explained as a combination of inductive effects and intermolecular/intramolecular hydrogen bonding dependent on solvent characteristics. In hydrogen-bonding solvents, the greater reactivity of the 6,7 site over that of the 2,3 position was ascribed to the greater nucleophilicity of the 6,7 position over the inductively deactivated 2,3 site. In the non-polar carbon tetrachloride solvent system, intramolecular hydrogen bonding at the 2,3 olefinic site was postulated to be responsible for the increased yield of 4.

The absolute rate studies on geraniol show the situation to be complex. The studies on 5 and 6 provide insights and facilitate interpretation since they model each site in geraniol as if it were independent. Interestingly, other than the present work, there is only one other major kinetics study of dimethyldioxirane reactivity in various solvents. Gilbert et al. [13] reported the k₂ values for epoxidation of cis-stilbene by “acetone-free” 1. At 2 °C, epoxidation in CCl₄ was found to be ~3-fold slower than in acetone.

The present study on 5 noted a very slight increase in relative reactivity upon addition of carbon tetrachloride relative to that in acetone, the opposite of that reported in the literature [13]. In addition, reactions carried out with added methanol showed a 27-fold increase, in agreement with our previous data on addition of water [3b]. The results for 6 provide interesting differences from those of 5. In acetone, the k₂ value is somewhat lower than expected for a trisubstituted alkene. This lower reactivity is in agreement with our earlier observations [3b] on hydroxy-substituted alkenes. Deactivation of the alkene by an inductive effect is a possible explanation although gas phase calculations have suggested [7] that in the case of the 2,3 site of geraniol inductive effects are not involved. An explanation in which the hydroxy group interacts with acetone could also lead to reduced reactivity. The hydroxy-containing model compound 6 shows a larger increase in reactivity in carbon tetrachloride and a smaller one in methanol than those observed for 5. This latter observation indicates that strong hydrogen bonding to the solvent may increase steric interactions and slow attack by 1 on 6.

The k_rel values for geraniol (Table 2) indicate intermediate behavior as compared to that of 5 and 6. Calculation of the individual k₂ values for sites 2,3 and 6,7 and subsequent comparison to the model systems provide important insights that can not be gained solely from the product studies. Both the calculated k₂ values and the k_rel values need to be analyzed. In methanol, the k_6,7 value is essentially identical to the k₂ value for 5. However, the k_rel value for the formation of 3 is low. This indicates that the k_6,7 values in acetone and carbon tetrachloride are faster than expected. This suggests that the remote hydroxy group is exerting an effect on the 6,7-position that increases the reactivity in the less polar/less hydrogen-bonding solvents. This effect could be an intramolecular hydrogen-bonding effect or a solvation effect. Analysis of product studies, alone, would not lead to this conclusion.

The analysis of the 2,3 site rate constant data reveals additional interesting insights. In methanolic solvent, the k_2,3 value is very similar to that for 6. However, both those numbers are 3-fold less than the k_6,7 value and that for 5 in the same solvent. This clearly cannot be solely due to an inductive effect of a hydroxy group. It appears that hydrogen bonding between methanol and the hydroxy group results in decreased reactivity at the 2,3 position due to increased steric interactions (with essentially no effect at the 6,7 position). The k_2,3 and corresponding k_rel values in acetone and carbon tetrachloride are very similar to those for the model alkene 6.

Conclusions

The kinetic data clearly show that the two epoxidation sites in geraniol are not simply a summation of the independent alkene system data. Instead there are subtle interactions between the two sites that mediate the final product distributions. Understanding of the mechanistic constraints on electrophilic oxygen-atom transfer chemistry provides important insights not only into synthetic applications but also into enzymatic-related systems.

Acknowledgments

Acknowledgment is made to the U.S. Army ERDEC (DAAA 15-94-K-0004) SEAS subcontract and to the Georgia State University Research Fund for support of this work.

Experimental

General

Glassware was treated by boiling in a solution containing 1% Na₂EDTA for approximately 1 h, washing with deionized water, rinsing with acetone and drying prior to use. All solvents (Aldrich) used were of either HPLC or anhydrous reagent grade. Kinetic experiments were carried out on a Shimadzu UV-1601 spectrometer connected to a HAAKE K constant temperature circulating water bath (T ± 0.3 °C). GC-MS data were collected on a Shimadzu GC-17A gas chromatograph coupled to a Shimadzu QP-5000 mass spectrometer. ¹H-NMR spectra (CDCl₃) were recorded on a Varian 300 MHz Unity spectrometer. Geraniol (1), 2-methyl-2-pentene (5), 3-methyl-2-buten-1-ol (6) and Oxone® (2HKSO₅•HKSO₄•K₂SO₄) were obtained commercially (Aldrich) and were used without further purification. Isolated dried dioxirane 1 (0.1 M, in acetone) was prepared by a procedure [4] that was an adaptation of the experimental approach of Murray and Jeyaraman [3a]. Also see W. Adam et al. [3d].

Product Studies

The reaction products for epoxidation of 2, 5 and 6 by dimethyldioxirane were analyzed by GC/MS and ¹H-NMR spectroscopy. For mono-epoxides 3 and 4 the data were in agreement with literature values [9,10] in each case [5,6]. In all cases, the percentage conversion was quantitative with respect to 1. The product study for geraniol was carried out under conditions [5] which only produced mono-epoxidation as follows: geraniol (50.0 mg, 0.325 mmol) was added to the appropriate dried solvent (11.25 mL) at ambient temperature. To this solution, 0.33 equivalents of 1 (1.25 mL, 0.078 M) in acetone were added followed by stirring for 1 h. The solvent was removed and the overall yield, as well as the product ratios for the mono-epoxides, were determined by integration of the olefinic and epoxide hydrogen peaks versus internal standard in the ¹H-NMR spectrum. GC/MS analysis was carried out to confirm the results. Product studies for the epoxides derived from 5 and 6 were carried out with a 3-fold excess of 1. Quantitative conversion of the alkene to the epoxides was observed in both cases. Spectral data for the epoxide were consistent with the respective literature values [11,12].

Kinetic Studies

All solutions for kinetic experiments were prepared with dried solvents. The reactions were studied at 23 ± 0.3 °C employing either a 10:1, 3:1, or 1:1 substrate to dimethyldioxirane ratio. The reactions were monitored by following the decrease in the absorbance at 330 nm (concentration of dioxirane). The following general approach was used in all kinetics experiments. A predetermined quantity of alkene of known concentration was placed in a standard UV quartz cuvette and allowed to equilibrate. The desired equivalents of dimethyldioxirane in dried acetone solution (≤ 0.1 M) were added via syringe and the solution was mixed rapidly. Under pseudo-first order conditions, the values of k_obs were calculated from linear plot of the natural log of the relative absorbance of the dioxirane against time. Data were collected for at least two half-lives for all the kinetic runs. The values for the second order rate constants were computed by dividing the k_obs value by the concentration of the reagent in excess. For the other conditions, the k₂ values were calculated using the standard approach for second order rate constants (for example, plots of the reciprocals of dioxirane concentration vs. time for equal molar conditions).

References and Notes

For selected reviews see: Curci, R. “Advances in Oxygenated Processes”; Vol. 2, Baumstark, A., Ed.; JAI Press: Greenwich, CT, 1990. [Google Scholar] Adam, W; Hadjiarapogolonu, L.; Curci, R.; Mello, R. Chapt. 4; “Organic Peroxides,”; Adam, W., Ed.; Wiley and Sons: Chichester, England, 1992. [Google Scholar] Adam, W.; Hadjiarapogolonu, L. Top. Curr. Chem. 1993, 164, 45. Curci, R.; Dinai, A.; Rubino, M. Pure Appl. Chem. 1995, 67, 811.
Denmark, S.E.; Wu, Z. J. Org. Chem. 1998, 63, 2810. Frohn, M.; Wang, Z.-X.; Shi, Y. ibid 1998, 63, 6425. Yang, D.; Wong, M.-K.; Yip, Y.-C. ibid 1995, 60, 3887. Adam, W.; Hadjiaarapogolonu, L.; Sherz, A. Chem. Ber. 1991, 124, 227. Curci, R.; Fiorentino, M.; Trisi, L.; Edwards, J.D.; Pater, R.H. J. Org. Chem. 1980, 45, 4758.
Murray, R.; Jeyaraman, R. J. Org. Chem. 1985, 50, 2847. Baumstark, A.L.; Vasquez, P.C. J. Org. Chem. 1988, 53, 3437. Baumstark, A.L.; Michelena-Baez, E.; Navarro, A.M.; Banks, H.D. Het. Comm. 1997, 3, 393. Adam, W.; Hadjiarapogolonu, L.; Bialas, J. Chem. Ber. 1991, 124, 2377.
Baumstark, A.L.; McCloskey, C.J. Tetrahedron Lett. 1987, 3311.
Adam, W.; Prechtl, F.; Richter, M.J.; Smerz, A.K. Tetrahedron Lett. 1993, 34, 8427.
Adam, W.; Smerz, A.K. J. Org. Chem. 1996, 61, 3506.
Miaskiewicz, K.; Smith, D.A. J. Am. Chem. Soc. 1998, 120, 1872.
Michelena-Baez, E.; Navarro-Eisenstein, A.M.; Banks, H.D.; Vasquez, P.C.; Baumstark, A.L. Het. Comm. 2000, 6, 119.
Onoda, T.; Shirai, R.; Koiso, Y.; Iwasaki, S. Tetrahedron 1996, 52, 14543.
Chavnan, S.M.S.; Parkash, S.; Mohaptra, P.P. Indian J. Chem. Sect. B 1997, 312.
Palombi, L.; Bonadies, F.; Scetti, A. Tetrahedron 1997, 53, 11369.
Robinson, P.L.; Barry, C.N.; Kelly, J.W.; Evans, S.A. J. Am. Chem. Soc. 1985, 107, 5210.
Gilbert, M.; Ferrer, M.; Sánchez-Baeza, F.; Messequer, A. Tetrahedron 1997, 53, 8643.

Share and Cite

MDPI and ACS Style

Baumstark, A.L.; Franklin, P.J.; Vasquez, P.C.; Crow, B.S. Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane. Molecules 2004, 9, 117-124. https://doi.org/10.3390/90300117

AMA Style

Baumstark AL, Franklin PJ, Vasquez PC, Crow BS. Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane. Molecules. 2004; 9(3):117-124. https://doi.org/10.3390/90300117

Chicago/Turabian Style

Baumstark, A. L., P. J. Franklin, P. C. Vasquez, and B. S. Crow. 2004. "Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane" Molecules 9, no. 3: 117-124. https://doi.org/10.3390/90300117

Article Menu

Kinetics of the Epoxidation of Geraniol and Model Systems by Dimethyldioxirane

Abstract

Introduction

Results and Discussion

Conclusions

Acknowledgments

Experimental

General

Product Studies

Kinetic Studies

References and Notes

Share and Cite

Article Metrics

Article Access Statistics

Further Information

Guidelines

MDPI Initiatives

Follow MDPI