Chemistry:Swern oxidation

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Short description: Organic redox reaction
Swern oxidation
Named after Daniel Swern
Reaction type Organic redox reaction
Identifiers
Organic Chemistry Portal swern-oxidation
RSC ontology ID RXNO:0000154
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In organic chemistry, the Swern oxidation, named after Daniel Swern, is a chemical reaction whereby a primary or secondary alcohol (–OH) is oxidized to an aldehyde (–CH=O) or ketone (>C=O) using oxalyl chloride, dimethyl sulfoxide (DMSO) and an organic base, such as triethylamine.[1][2][3] It is one of the many oxidation reactions commonly referred to as 'activated DMSO' oxidations. The reaction is known for its mild character and wide tolerance of functional groups.[4][5][6][7]

The Swern oxidation.

The by-products are dimethyl sulfide ((CH3)2S), carbon monoxide (CO), carbon dioxide (CO2) and—when triethylamine is used as base—triethylammonium chloride (Et3NHCl). Of the volatile by-products, dimethyl sulfide has a strong, pervasive odour and carbon monoxide is acutely toxic, so the reaction and the work-up needs to be performed in a fume hood. Dimethyl sulfide is a volatile liquid (B.P. 37 °C) with an unpleasant odour at even low concentrations.[8][9][10]

Mechanism

The first step of the Swern oxidation is the low-temperature reaction of DMSO, 1a, formally as resonance contributor 1b, with oxalyl chloride, 2. The first intermediate, 3, quickly decomposes giving off carbon dioxide and carbon monoxide and producing chloro(dimethyl)sulfonium chloride, 4.

Dimethylchlorosulfonium chloride formation.

After addition of the alcohol 5, the chloro(dimethyl)sulfonium chloride 4 reacts with the alcohol to give the key alkoxysulfonium ion intermediate, 6. The addition of at least 2 equivalents of base — typically triethylamine — will deprotonate the alkoxysulfonium ion to give the sulfur ylide 7. In a five-membered ring transition state, the sulfur ylide 7 decomposes to give dimethyl sulfide and the desired carbonyl compound 8.

The mechanism of the Swern oxidation.

Variations

When using oxalyl chloride as the dehydration agent, the reaction must be kept colder than −60 °C to avoid side reactions. With cyanuric chloride[11] or trifluoroacetic anhydride[12] instead of oxalyl chloride, the reaction can be warmed to −30 °C without side reactions. Other methods for the activation of DMSO to initiate the formation of the key intermediate 6 are the use of carbodiimides (Pfitzner–Moffatt oxidation), a sulfur trioxide pyridine complex (Parikh–Doering oxidation) or acetic anhydride (Albright-Goldman oxidation). The intermediate 4 can also be prepared from dimethyl sulfide and N-chlorosuccinimide (the Corey–Kim oxidation).

In some cases, the use of triethylamine as the base can lead to epimerisation at the carbon alpha to the newly formed carbonyl. Using a bulkier base, such as diisopropylethylamine, can mitigate this side reaction.

Considerations

Dimethyl sulfide, a byproduct of the Swern oxidation, is one of the most notoriously unpleasant odors known in organic chemistry. Humans can detect this compound in concentrations as low as 0.02 to 0.1 parts per million.[13] A simple remedy for this problem is to rinse used glassware with bleach or oxone solution, which will oxidize the dimethyl sulfide back to dimethyl sulfoxide or to dimethyl sulfone, both of which are odourless and nontoxic.[14]

The reaction conditions allow oxidation of acid-sensitive compounds, which might decompose under the acidic oxidation conditions such as Jones oxidation. For example, in Thompson & Heathcock's synthesis of the sesquiterpene isovelleral,[15] the final step uses the Swern protocol, avoiding rearrangement of the acid-sensitive cyclopropanemethanol moiety.

IsovelleralPreparationViaSwernOxidation.png

See also

References

  1. ↑ Omura, K.; Swern, D. (1978). "Oxidation of alcohols by "activated" dimethyl sulfoxide. A preparative, steric and mechanistic study". Tetrahedron 34 (11): 1651–1660. doi:10.1016/0040-4020(78)80197-5. 
  2. ↑ Mancuso, A. J.; Brownfain, D. S.; Swern, D. (1979). "Structure of the dimethyl sulfoxide-oxalyl chloride reaction product. Oxidation of heteroaromatic and diverse alcohols to carbonyl compounds". J. Org. Chem. 44 (23): 4148–4150. doi:10.1021/jo01337a028. 
  3. ↑ Mancuso, A. J.; Huang, S.-L.; Swern, D. (1978). "Oxidation of long-chain and related alcohols to carbonyls by dimethyl sulfoxide "activated" by oxalyl chloride". J. Org. Chem. 43 (12): 2480–2482. doi:10.1021/jo00406a041. 
  4. ↑ Dondoni, A.; Perrone, D. (2004). "Synthesis of 1,1-Dimethyl Ethyl-(S)-4-formyl-2,2-dimethyl-3-oxazolidinecarboxylate by Oxidation of the Alcohol". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=v77p0064. ; Collective Volume, 10, pp. 320 
  5. ↑ Bishop, R. (1998). "9-Thiabicyclo[3.3.1]nonane-2,6-dione". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=cv9p0692. ; Collective Volume, 9, pp. 692 
  6. ↑ Leopold, E. J. (1990). "Selective hydroboration of a 1,3,7-triene: Homogeraniol". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=cv7p0258. ; Collective Volume, 7, pp. 258 
  7. ↑ Tojo, G.; Fernández, M. (2006). Oxidation of alcohols to aldehydes and ketones: A guide to current common practice. Springer. ISBN 0-387-23607-4. 
  8. ↑ Mancuso, A. J.; Swern, D. (1981). "Activated dimethyl sulfoxide: Useful reagents for synthesis". Synthesis 1981 (3): 165–185. doi:10.1055/s-1981-29377. 
  9. ↑ Tidwell, T. T. (1990). "Oxidation of alcohols to carbonyl compounds via alkoxysulfonium ylides: The Moffatt, Swern, and related oxidations". Org. React. 39: 297–572. doi:10.1002/0471264180.or039.03. ISBN 0471264180. 
  10. ↑ Tidwell, T. T. (1990). "Oxidation of alcohols by activated dimethyl sulfoxide and related reactions: An update". Synthesis 1990 (10): 857–870. doi:10.1055/s-1990-27036. 
  11. ↑ De Luca Lidia (2001). "A Mild and Efficient Alternative to the Classical Swern Oxidation". The Journal of Organic Chemistry 66 (23): 7907–7909. doi:10.1021/jo015935s. PMID 11701058. 
  12. ↑ Omura, Kanji; Sharma, Ashok K.; Swern, Daniel (1976). "Dimethyl Sulfoxide-Trifluoroacetic Anhydride. New Reagent for Oxidation of Alcohols to Carbonyls". J. Org. Chem. 41 (6): 957–962. doi:10.1021/jo00868a012. 
  13. ↑ Morton, T. H. (2000). "Archiving Odors". Of Molecules and Mind. Oxford: Oxford University Press. pp. 205–216. 
  14. ↑ Atkins, William J. Jr.; Burkhardt, Elizabeth R.; Matos, Karl (2006). "Safe Handling of Boranes at Scale". Org. Process Res. Dev. 10 (6): 1292–1295. doi:10.1021/op068011l. 
  15. ↑ Thompson, S. K.; Heathcock, C. H. (1992). "Total synthesis of some marasmane and lactarane sesquiterpenes". J. Org. Chem. 57 (22): 5979–5989. doi:10.1021/jo00048a036. 

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