Selective Sulfide Oxidation to Sulfoxides with 30% H2O2 and Silica-Tungstate Catalyst, Notas de estudo de Química

Baixe Selective Sulfide Oxidation to Sulfoxides with 30% H2O2 and Silica-Tungstate Catalyst e outras Notas de estudo em PDF para Química, somente na Docsity! Selective Oxidation of Sulfides to Sulfoxides Using 30% Hydrogen Peroxide Catalyzed with a Recoverable Silica-Based Tungstate Interphase Catalyst Babak Karimi,*,†,‡ Maryam Ghoreishi-Nezhad,† and James H. Clark§ Department of Chemistry, Institute for AdVanced Studies in Basic Sciences (IASBS), P.O.Box 45195-1159, GaVa Zang, Zanjan, Iran, Institute for Fundamental Research (IPM), Farmanieh, P.O.Box 19395-5531, Tehran, Iran, and Clean Technology Center, UniVersity of York, York YO10 5DD, England karimi@iasbs.ac.ir Received November 17, 2004 ABSTRACT Various types of aromatic and aliphatic sulfides are selectively oxidized to sulfoxides and sulfones in good to excellent yields using 30% H2O2 in the presence of catalytic amounts of a novel recoverable silica-based tungstate interphase catalyst at room temperature. The catalyst can be recovered and reused for at least eight reaction cycles under the described reaction conditions without considerable loss of reactivity. The selective oxidation of sulfides to sulfoxides is an attractive and important method in organic chemistry, since sulfoxides are useful building blocks especially as chiral auxiliaries in organic synthesis1 They also play key roles in the activation of enzymes.2 However, this transformation is conventionally achieved using stoichiometric amounts of both organic3 and inorganic3h,4 reagents, most of which are not suitable for medium to large scale operations and which also lead to large a volume of toxic wastes. Moreover, over- oxidation of the sulfoxides to their sulfones is a common problem during the oxidation of sulfides. In recent years, the newly coined term “green chemistry” has become increasingly important, with the objective to create new products, industrial and laboratory processes, and services that achieve social and economic progress without environ- mental detriment.5 The use of H2O2 as final oxidant offers the advantages that it is a cheap, environmentally benign, and readily available reagent and produces water as the only † Institute for Advanced Studies in Basic Sciences. ‡ Institute for Fundamental Research. § University of York. (1) (a) Soladie, G. Synthesis 1981, 185. (b) Carreno, M. C. Chem. ReV. 1995, 95, 1917. (2) (a) Fuhrhop, J.; Penzlin, G. Organic Synthesis, Concepts, Methods, Starting materials, 2nd ed.; VCH: Weinheim, 1994. (b) Block, E. Reaction of Organosulfur Compounds; Academic Press: New York, 1978. (3) (a) Venier, C. G.; Squires, T. G.; Chen, Y.-Y.; Hussmann, G. P.; Shei, J. C.; Smith, B. F. J. Org. Chem. 1982, 47, 3773. (b) Murray, R. W.; Jeyaraman, R. J. Org. Chem. 1985, 50, 2847. (c) Adam, W.; Hadjiarapoglou, L. Tetrahedron Lett. 1992, 33, 469. (d) Breton, G. W.; Fields, J. D.; Kropp, P. J. Tetrahedron Lett. 1995, 36, 3825. (e) Kaldor, S. W.; Hammond, M. Tetrahedron Lett. 1991, 32, 5043. (f) Paquette, L. A.; Carr, R. V. C. Organic Syntheses; Wiley: New York, 1990; Collect. Vol. VII, p 453. (g) Xiong, Z.-X.; Huang, N.-P.; Zhong, P. Synth. Commun. 2001, 31, 245. For a review see: (h) Mata, E. G. Phosphrus, Sulfur Silicon 1996, 117, 231. (4) (a) Barton, D. H. R.; Li, W.; Smith, J. A. Tetrahedron Lett. 1998, 39, 7055. (b) Hirano, M.; Yakabe, S.; Clark, J. H.; Morimoto, T. J. Chem. Soc., Perkin Trans. 1 1996, 2693. ORGANIC LETTERS 2005 Vol. 7, No. 4 625-628 10.1021/ol047635d CCC: $30.25 © 2005 American Chemical Society Published on Web 01/25/2005 byproduct.6 This feature has stimulated the development of useful procedures for H2O2 oxidation, especially with the use of various types of tungsten-based catalyst systems.7 Very recently, the elegant work of Noyori and co-workers has shown that a combination of Na2WO4/C6H5PO3H2 and a quaternary ammonium hydrogen sulfate as an acidic phase transfer catalyst can be effectively applied for selective oxidation of sulfide to sulfoxides or sulfones using 30% H2O2 under halide-free conditions.8 Although using this protocol represents a considerable progress, the protocol needs homogeneous reaction conditions, and therefore the catalyst is difficult to recover and reuse. Since the replacement of current homogeneous oxidation procedures for the production of fine chemicals by environmentally acceptable protocols based on recoverable catalysts is one of the major tasks in green chemistry, solid oxidation catalysts are called to play a crucial role to accomplish this issue.9 One way to attain this goal is to immobilize one or more components of the catalytic systems onto a large surface area solid carrier to create new organic-inorganic hybrid (interphase) catalysts.10 An interphase is defined as a region within a material in which a stationary (organic-inorganic hybrid catalyst) and mobile component (solvent and reactants) penetrate each other on a molecular level. According to the definition, an interphase catalyst is composed of three parts. An inert matrix (support), a flexible organic spacer, and an active center.8b In contrast to traditional physisorbed heterogeneous catalysts, in the interphase counterparts the organic spacer provides sufficient mobility of the reactive center and diminishes undesired steric effect of the matrix over the accessibility of the reactive center. Therefore, these systems are able to simulate homogeneous reaction conditions, and at the same time they have the advantage of easy separation and recovery of the heterogeneous catalysts. Owing to the relative mobility of the reactive center in the interphase catalyst, we hypoth- esized that it might be possible to replace the phase transfer catalyst in Noyori’s protocol with a silica matrix having a quaternary organic spacer. In the present work we wish to report the results obtained with a novel silica-functionalized ammonium tungstate as a recoverable heterogeneous catalyst for selective oxidation of sulfide to sulfoxides using 30% H2O2. The catalyst is simply prepared by building up an aminopropyl group on the surface of commercially available mesoporous silica followed by acidification of amino groups using triflic acid and ion exchange of triflate ion by tungstate (Scheme 1). Typically, a surface-bound amino group at a loading ca. 0.31 mmol‚g-1 (by TGA/DTG analysis) was obtained. However, from the simultaneous XRF analysis of the catalyst for tungsten and sodium it was calculated that the loading of the former in the solid was 0.15 mmol‚g-1, while a trace amount (less than 0.4 ppm) of the latter was detected. The major weight loss at high temperature in TGA is character- istic of chemisorbed materials and confirmed that the aminopropyl group is covalently bound on the surface of silica.11 From this result, in combination with those obtained from TGA and XRF analyses, we can clearly conclude that the catalyst corresponds to a 2:1 ratio between the surface- bound ammonium group and WO42- anion (Scheme 1, compound 1). To test the catalytic activity of 1 we selected the oxidation of sulfides using 30% H2O2 as the model reaction. To increase accessibility of the H2O2 to the catalyst we chose a solvent mixture CH2Cl2/MeOH (1:1). We first examined the oxidation of methyl phenyl sulfide (2 mmol) using 30% H2O2 (3 equiv) and 1 (1 mol %, 0.133 g) in CH2Cl2/MeOH (10 mL) at room temperature. We observed that the reaction was sluggish and only low yields of the corresponding sulfoxide were formed after 18 h. However, when a similar oxidation reaction was conducted in the presence of 1 (2 mol %, 0.266 g), methyl phenyl sulfoxide was efficiently formed in excellent yields within 1.5 h (Table 1, entry 1). In a blank experiment no considerable oxidation was observed under similar reaction conditions in the absence (5) (a) Clark, J. H. Pure Appl. Chem. 2001, 73, 103. (b) Clark, J. H. Green Chem. 1999, 1, 1. (c) Ghosh, A. et al. Pure Appl. Chem. 2001, 73, 113. (6) For a review on metal-catalyzed epoxidation using H2O2, see: Lane, B. S.; Burgess, K. Chem. ReV. 2003, 103, 2457. (7) (a) Schultz, H. S.; Freyemuth, H. B.; Buc, S. R. J. Org. Chem. 1963, 28, 1140. (b) Ishii, Y.; Tanaka, H.; Nisiyama, Y. Chem. Lett. 1994, 1. (c) Stec, Z.; Zawadiak, J.; Skibinski, A.; Pastuch, G. Polish J. Chem. 1996, 70, 1121. (d) Neumann, R.; Juwiler, D. Tetrahedron 1996, 52, 8781. (e) Cresley, N. M.; Griffith, W. P.; Laemmel, A. C.; Nogueira, H. I. S.; Perkin, B. C. J. Mol. Catal. 1997, 117, 397. (f) Collins, F. M.; Lucy, A. R.; Sharp, C. J. Mol. Catal. 1997, 117, 397. (8) (a) Sato, K.; Hyodo, M.; Aoki, M.; Zheng, X.-Q.; Noyori, R. Tetrahedron 2001, 57, 2469. (b) Noyori, R.; Aoki, M.; Sato, K. Chem. Commun. 2003, 1977. (9) (a) Corma, A.; Garcia, H. Chem. ReV. 2002, 102, 3837. (b) Mallat, T.; Baiker, A. Chem. ReV. 2004, 104, 3037. (10) (a) Corma, A.; Garcia, H. Chem. ReV. 2002, 102, 3879. (b) Lu, Z. L.; Lindner, E.; Mayer, H. A. Chem. ReV. 2002, 102, 3543. (c) Wight, A. P.; Davis, M. E. Chem. ReV. 2002, 102, 3589. (d) Lindner, E.; Kemmler, M.; Auer, F.; Mayer, H. A. Angew. Chem., Int. Ed. 1999, 38, 2155. (e) Clark, J. H.; Macquarrie, D. J. Chem. Commun. 1998, 853. (11) See Supporting Information for details. Scheme 1 626 Org. Lett., Vol. 7, No. 4, 2005