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User:Mevans86/Selenoxide elimination

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Selenoxide elimination is a method for the synthesis of alkenes from selenoxides. It is most commonly used to synthesize α,β-unsaturated carbonyl compounds from the corresponding saturated analogues.[1]

Introduction

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After the development of sulfoxide elimination as an effective method for generating carbon-carbon double bonds,[2] it was discovered that selenoxides undergo a similar process, albeit much more rapidly. Most selenoxides decompose to the corresponding alkenes at temperatures between -50 and 40 °C. Evidence suggests that the elimination is syn; however, epimerization at both carbon and selenium (both of which are stereogenic) may occur during the reaction. As selenoxides can be readily prepared from nucleophilic carbonyl derivatives (enols and enolates),[3] selenoxide elimination has grown into a general method for the preparation of α,β-unsaturated carbonyl compounds.

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Mechanism and Stereochemistry

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Prevailing Mechanism

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Elimination of selenoxides takes place through an intramolecular, syn elimination pathway. The carbon-hydrogen and carbon-selenium bonds are co-planar in the transition state.[4]

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The reaction is highly trans-selective when acyclic α-phenylseleno carbonyl compounds are employed. Formation of conjugated double bonds is favored. Endocyclic double bonds tend to predominate over exocyclic ones, unless no syn hydrogen is available in the ring. Selenium in these reactions is almost always stereogenic, and the effect of epimerization at selenium (which is acid-catalyzed and occurs readily) on the elimination reaction is nearly unknown. In one example, separation and warming of selenoxides 1 and 2 revealed that 2 decomposes at 0 °C, while 1, which presumably has more difficulty accessing the necessary syn conformation for elimination, is stable to 5 °C.[5]

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Scope and Limitations

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Selenylating and Oxidizing Reagents

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α-Selenylation of carbonyl compounds can be accomplished with a variety of reagents, using either electrophilic or nucleophilic selenylating reagents. Usually, simple phenylseleno compounds are used in elimination reactions; although 2-nitrophenylselenides react more quickly, they are more expensive to prepare, and phenylselenides typically react in minutes. Electrophilic selenylating reagents can be used in conjunction with enols, enolates, or enol ethers. Phenylselenating reagents include:

  • Diphenyl diselenide
  • Benzeneselenyl chloride
  • Benzeneselinyl chloride
  • Sodium benzeneselenolate
  • Trimethylsilyl phenyl selenide

The most common oxidizing agent employed is hydrogen peroxide.[6] It is sometimes used in excess, to overcome catalytic decomposition of H2O2 by selenium; however, undesired oxidation of starting material has been observed under these conditions. Oxidation of products (via the Baeyer-Villiger reaction, for instance) has also been observed.[7]

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For substrates whose product olefins are sensitive to oxidation, meta-chloroperbenzoic acid (mCPBA) can be employed as an oxidant. It oxidizes selenides below the temperature at which they decompose to alkenes; thus, all oxidant is consumed before elimination begins. Buffering with an amine base is necessary before warming to avoid acid-mediated side reactions.[8]

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Ozone, which gives only dioxygen as a byproduct after oxidation, is used to oxidize selenides when special conditions are required for thermolysis or extreme care is necessary during workup. Quinones can be synthesized from the corresponding cyclic unsaturated carbonyl compounds using this method.[9]

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Substrates

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α-Phenylseleno aldehydes, which are usually prepared from the corresponding enol ethers, are usually oxidized with mCPBA or ozone, as hydrogen peroxide causes over-oxidation. α-Phenylseleno ketones can be prepared by kinetically controlled enolate formation and trapping with an electrophilic selenylating reagent such as benzeneselenyl chloride. A second deprotonation, forming a selenium-substituted enolate, allows alkylation or hydroxyalkylation of these substrates.[10]

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Base-sensitive substrates may be selenylated under acid-catalyzed conditions (as enols) using benzeneselenyl chloride. Hydrochloric acid generated during the selenylation of transient enol catalyzes tautomerization.[11]

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The seleno-Pummerer reaction is a significant side reaction that may occur under conditions when acid is present.[12] Protonation of the selenoxide intermediate, followed by elimination of hydroxide and hydrolysis, leads to α-dicarbonyl compounds. The reaction is not a problem for more electron-rich carbonyls—generally, fewer side reactions are observed in eliminations of esters and amides.[12]

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A second significant side reaction in reactions of ketones and aldehydes is selenylation of the intermediate selenoxide. This process leads to elimination products retaining a carbon-selenium bond,[13] and is more difficult to prevent than the seleno-Pummerer reaction. Tertiary selenoxides, which are unable to undergo enolization, do not react further with selenium electrophiles.

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Comparison with Other Methods

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Analogous sulfoxide eliminations are generally harder to implement than selenoxide eliminations. Formation of the carbon-sulfur bond is usually accomplished with highly reactive sulfenyl chlorides, which must be prepared for immediate use. However, sulfoxides are more stable than the corresponding selenoxides, and elimination is usually carried out as a distinct operation. This allows thermolysis conditions to be optimized (although the high temperatures required may cause other thermal processes). In addition, sulfoxides may be carried through multiple synthetic steps before elimination is carried out.[14]

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The combination of silyl enol ethers with palladium (II) acetate, the Saegusa oxidation, gives enones. However, the reaction requires stoichiometric amounts of Pd(OAc)2 and thus is not amenable to large-scale synthesis.[15] Catalytic variants have been developed.[16]

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For β-dicarbonyl compounds, DDQ can be used as an oxidizing agent in the synthesis of enediones. Additionally, some specialized systems give better yields upon DDQ oxidation.[17]

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Experimental Conditions and Procedure

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Typical Conditions

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Organoselenium reagents are toxic, and care should be taken to avoid undue exposure. Selenylation should be carried out using benzeneselenyl chloride whenever possible. Oxidation-elimination reactions should be carried out in non-polar solvents to avoid polar side reactions, such as the seleno-Pummerer reaction. Constrained or highly enolizable α-phenylseleno carbonyl compounds should be treated with ozone or mCPBA (rather than hydrogen peroxide) at low temperature to avoid side reactions.

The oxidation-elimination process produces a 1:1 molar ratio of benzeneseleninic acid and diphenyl diselenide. As the former slowly degrades in the presence of hydrogen peroxide, it should be promptly removed from the reaction mixture when the reaction is complete via base extraction. This extract can be treated with a reducing agent such as sodium thiosulfate.

Example Procedure[18]

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A solution of butyllithium in hexane (8 mL, 13.66 mmol) and diisopropylamine (fresly distilled, 1.94 mL, 13.66 mmol) in dry THF (14 mL) was stirred at 0° under argon. After cooling to –78°, the lactam starting material (1.2 g, 6.83 mmol) in dry THF (7 mL) was added. After 10 minutes benzeneselenenyl chloride(1.3 g, 6.83 mmol, recrystallized from hexane) in dry THF (8 mL) was slowly added. After 5 minutes, the reaction was allowed to warm to room temperature and then poured into formate buffer (pH 3; 180 mL) and extracted with ether. The extract was dried and evaporated, and the oily residue (2.35 g) was purified by flash chromatography (hexane-ethyl acetate, 7:3) to give the selenide (1.28 g, 3.86 mmol, 56.5% yield); 1H NMR δ 1.90–2.60 (2 H, m, CH2), 2.95 (1 H, m, CHD), 3.98 (1 H, m, CHSePh), 4.42 (2 H, s, CH2 benzylic), and 7.00–7.85 (10 H, aromatic complex); m/z: 331, 175, 157, 91 (100%). A sample was distilled for analytical purposes to afford pure selenide, bp 240° (0.2 mm Hg). Anal. Calcd for C17H16DNOSe: C, 61.6; H, 5.5; N, 4.2. Found: C, 61.5; H + D 5.4; N, 4.1.

The phenylselenopyrrolidinone (782 mg, 2.36 mmol) was dissolved in ethanol (8.6 mL) and the solution was cooled to 0°. Hydrogen peroxide (35%, 1.4 mL) was then added dropwise and the mixture was stirred at 0° (the reaction was monitored by TLC, dichloromethane-acetone, 85:15). After 30 minutes, a solution of ferrous sulfate heptahydrate (4.12 g, 14.8 mmol) in water (20 mL) was added slowly. The mixture was diluted with water (40 mL), and extracted with dichloromethane. The organic layer was washed with aqueous sodium bicarbonate and water, dried, and evaporated. The pyrrolone product (344 mg, 1.98 mmol), 83.7% yield was obtained after purification by flash chromatography (eluant dichloromethane-acetone 87: 13); IR 3000, 2150, 1675 cm–1; 1H NMR δ 3.85 (1 H, m, CDH), 4.61 (2 H, s, CH2 benzylic), 6.20 (1 H, d, CH, J = 6 Hz), 7.02 (1 H, d, CH, J = 6 Hz), and 7.26 (5 H, aromatic complex); [α]D = + 1.48° (c 5.19, CHCl3); m/z: 174 (M+), 173, 106, and 91 (100%). A sample crystallized from diisopropyl ether had mp 60–61°. Anal. Calcd for C11H10DNO: C, 75.8, H + D, 6.9; N, 8.0. Found: C, 75.6; H + D, 6.8; N, 7.9.

References

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  1. ^ Reich, H. J.; Wollowitz, S. Org. React. 1993, 44, 1. doi: (10.1002/0471264180.or044.01)
  2. ^ Emerson, D.; Craig, A.; Potts, I. J. Org. Chem., 1967, 32, 102.
  3. ^ Sharpless, K. B.; Lauer, R. F.; Teranishi, A. Y. J. Am. Chem. Soc. 1973, 95, 6137.
  4. ^ Sharpless, K. B.; Young, M. W.; Lauer, R. F. Tetrahedron Lett. 1973, 1979.
  5. ^ Jones, D. N.; Mundy, D.; Whitehouse, R. D. J. Chem. Soc., Chem. Commun. 1970, 86.
  6. ^ Figueredo, M.; Font, J.; Virgili, A. Tetrahedron, 1987, 43, 1881.
  7. ^ Vargas, D.; Fronczek, F. R.; Fischer, N. H.; Hostettmann, K. J. Nat. Products 1986, 49, 133.
  8. ^ Callant, P.; Ongena, R.; Vandewalle, M. Tetrahedron 1981, 37, 2085.
  9. ^ Waring, A. J.; Zaidi, J. H. J. Chem. Soc. Perkin Trans. 1, 1985, 631.
  10. ^ Solomon, M.; Hoekstra, W.; Zima, G.; Liotta, D. J. Org. Chem. 1988, 53, 5059.
  11. ^ Plieninger, H.; Gramlich, W. Chem. Ber. 1978, 111, 1944.
  12. ^ a b Reich, H. J.; Renga, J. M.; Reich, I. L. J. Org. Chem. 1974, 39, 2133.
  13. ^ Reich, H. J.; Renga, J. M.; Reich, I. L. J. Am. Chem. Soc. 1975, 97, 5434.
  14. ^ Wakamatsu, T.; Yamada, S.; Ban, Y. Heterocycles 1986, 24, 309.
  15. ^ Ito, Y.; Hirao, T.; Saegusa, T. J. Org. Chem. 1978, 43, 1011.
  16. ^ Tsuji, J.; Takahasi, K.; Minami, I.; Shimizu, I.; Tetrahedron Lett. 1984, 25, 4783.
  17. ^ Lott, R. S.; Breitholle, E. G.; Stammer, C. H. J. Org. Chem. 1980, 45, 1151.
  18. ^ Santaniello, E.; Casati, R.; Manzocchi, A. J. Chem. Soc. Perkin Trans. 1 1985, 2389.

Category:Organic redox reactions

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