Baeyer–Villiger oxidation

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Baeyer-Villiger oxidation
Named after Adolf von Baeyer
Victor Villiger
Reaction type Organic redox reaction
Organic Chemistry Portal baeyer-villiger-oxidation
RSC ontology ID RXNO:0000031

The Baeyer-Villiger oxidation (also called Baeyer-Villiger rearrangement) is an organic reaction that forms an ester from a ketone or a lactone from a cyclic ketone.[1] Peroxyacids or peroxides are used as the oxidant.[1] The reaction is named after Adolf Baeyer and Victor Villiger who first reported the reaction in 1899.[1]

Baeyer-Villiger oxidation

Reaction mechanism[edit]

In the first step of the reaction mechanism, the peroxyacid protonates the oxygen of the carbonyl group.[1] This makes the carbonyl group more susceptible to attack by the peroxyacid.[1] In the next step of the reaction mechanism, the peroxyacid attacks the carbon of the carbonyl group forming what is known as the Criegee intermediate.[1] Through a concerted mechanism, one of the substituents on the ketone migrates to the oxygen of the peroxide group while a carboxylic acid leaves.[1] This migration step is thought to be the rate determining step.[2] Finally, deprotonation of the oxygen of the carbonyl group produces the ester.[1]

Reaction mechanism of the Baeyer-Villiger oxidation

The products of the Baeyer-Villiger oxidation are believed to be controlled through both primary and secondary stereoelectronic effects.[3] The primary stereoelectronic effect in the Baeyer-Villiger oxidation refers to the necessity of the oxygen-oxygen bond in the peroxide group to be antiperiplanar to the group that migrates.[3] This orientation facilitates optimum overlap of the 𝛔 orbital of the migrating group to the 𝛔* orbital of the peroxide group.[1] The secondary stereoelectronic effect refers to the necessity of the lone pair on the oxygen of the hydroxyl group to be antiperiplanar to the migrating group.[3] This allows for optimum overlap of the oxygen nonbonding orbital with the 𝛔* orbital of the migrating group.[4] This migration step is also (at least in silico) assisted by two or three peroxyacid units enabling the hydroxyl proton to shuttle to its new position.[5]

Stereoelectronic effects

The migratory ability is ranked tertiary ≻ secondary ≻ phenyl ≻ primary.[6] Allylic groups also migrate better than primary groups but not as well as secondary groups.[4] If there is an electron withdrawing group on the substituent, then it decreases the rate of migration.[7] There are two explanations for this trend in migration ability.[8] One explanation relies on the carbocation resonance structure of the Criegee intermediate.[8] Keeping this structure in mind, it makes sense that the substituent that can maintain positive charge the best would be most likely to migrate.[8] Tertiary groups are more stable carbocations than secondary groups, and secondary groups are more stable than primary.[9] Therefore, the tertiary ≻ secondary ≻ primary trend is observed.

Resonance structures of the Criegee intermediate

Another explanation uses stereoelectronic effects and steric bulk to explain the trend.[10] As mentioned, the substituent that is antiperiplanar to the peroxide group in the transition state will be the group that migrates.[3] This transition state has a gauche interaction between the peroxyacid and the non-migrating substituent.[10] If the bulkier group is placed antiperiplanar to the peroxide group, the gauche interaction between the substituent on the forming ester and the carbonyl group of the peroxyacid will be reduced.[10] Thus, it is the bulkier group that ends up antiperiplanar to the peroxide group making it the group that migrates.[10] This explains the trend of tertiary ≻ secondary ≻ primary because tertiary groups are generally bulkier than secondary and primary groups.

Steric bulk influencing migration

Historical background[edit]

In 1899, Adolf Baeyer and Victor Villiger first published a demonstration of the reaction that we now know as the Baeyer-Villiger oxidation.[11][12] They used peroxymonosulfuric acid to make the corresponding lactones from camphor, menthone, and tetrahydrocarvone.[12][13]

Original reactions reported by Baeyer and Villiger

There were three suggested reaction mechanisms of the Baeyer-Villiger oxidation that seemed to fit with observed reaction outcomes.[14] These three reaction mechanisms can really be split into two pathways of peroxyacid attack.[15] The first pathway has the peroxyacid attack the oxygen of the carbonyl group.[15] The second pathway has the peroxyacid attack the carbon of the carbonyl group.[15] The first pathway could lead to two possible intermediates: Baeyer and Villiger suggested a dioxirane intermediate, while Georg Wittig and Gustav Pieper suggested a peroxide intermediate with no dioxirane formation.[15] A second pathway was suggested by Rudolf Criegee.[15] In this pathway, the peracid attacks the carbonyl carbon producing what is now known as the Criegee intermediate.[15]

Proposed Baeyer-Villiger oxidation intermediates

In 1953, William von Eggers Doering and Edwin Dorfman elucidated the correct pathway for the reaction mechanism of the Baeyer-Villiger oxidation by using oxygen-18 to label benzophenone.[14] The three different mechanisms each lead to a different distribution of labelled products. The Criegee intermediate leads to a product that is only labelled on the oxygen of the carbonyl group.[14] The product of the Wittig and Pieper intermediate is only labeled on the oxygen of the ester.[14] The Baeyer and Villiger intermediate leads to a 1:1 distribution of both of the above products.[14] The outcome of the labelling experiment supported the Criegee intermediate.[14] It is now believed that the mechanism follows the Criegee intermediate.[1]

The different possible outcomes of Dorfman and Doering's labelling experiment


The migration does not change the stereochemistry of the group that transfers.[16][17] Therefore, if it is a chiral group that migrates, the chirality of that group will not be changed.


Although many different peroxyacids are used for the Baeyer-Villiger oxidation, some of the more common oxidants include meta-chloroperbenzoic acid (mCPBA) and trifluoroperacetic acid (TFPAA).[2] The reactivity differs depending on the choice of the peroxyacid.[4] The general trend of reactivity correlates to the strength of the corresponding acid (or alcohol in the case of the peroxides).[4] The stronger the acid, the more reactive will the corresponding peroxyacid be in performing the Baeyer-Villiger oxidation.[4] The trend of reactivity of some reagents is TFPAA ≻ 4-nitroperbenzoic acid ≻ mCPBA and performic acidperacetic acidhydrogen peroxidetert-butyl hydroperoxide.[4] The peroxides are much less reactive than the peroxyacids.[2] In fact, hydrogen peroxide requires a catalyst in order to be used as an oxidant in the Baeyer-Villiger oxidation.[6][18] In addition, using organic peroxides and hydrogen peroxide tends to generate more byproducts because these reagents can favour the formation of reactive alkenyl peroxides over migration.[19]


The use of peroxyacids and peroxides when performing the Baeyer-Villiger oxidation can cause the undesirable oxidation of other functional groups.[20] Alkenes and amines are a few of the groups that can be oxidized.[20] However, methods have been developed that will allow for the tolerance of these functional groups.[20] For instance, if there is an alkene present in the ketone, the alkene could potentially undergo oxidation to the epoxide.[20] In general, electron-poor alkenes will prefer the Baeyer-Villiger oxidation, while electron-rich will prefer the epoxidation.[21] However, it may depend on the reagents that are used.[21] For example, there are methods that will selectively choose the formation of the epoxide or the ester.[22] In 1962, G. B. Payne reported that the use of hydrogen peroxide in the presence of a selenium catalyst will produce the epoxide, while use of peroxyacetic acid will form the ester.[22]

Payne reported that different reagents will give different outcomes when there are more than one functional group


Catalytic Baeyer-Villiger oxidation[edit]

There has been interest in making the Baeyer-Villiger oxidation work with hydrogen peroxide as an oxidant in the presence of a catalyst.[6] Using hydrogen peroxide as an oxidant makes the reaction more environmentally friendly as the waste produced would just be water.[6] The use of benzeneseleninic acid derivatives as a catalyst has been reported to give high selectivity with hydrogen peroxide as the REDUCTANT .[23]

Baeyer-Villiger monooxygenases[edit]

Another way to create a catalytic Baeyer-Villiger oxidation is by using enzymes as the catalyst.[6] Baeyer-Villiger monooxygenases (BVMOs) use dioxygen to perform the Baeyer-Villiger oxidation.[6] These enzymes are capable of enantioselective oxidations of prochiral substrates.[6]

Asymmetric Baeyer-Villiger oxidation[edit]

There have been attempts to use organometallic catalysts to perform an enantioselective Baeyer-Villiger oxidation. [6] The first reported instance of an asymmetric Baeyer-Villiger oxidation on a prochiral ketone used dioxygen as the oxidant and a copper catalyst.[21] Other catalysts followed such as platinum and aluminum catalysts.[21]



Zoapatanol is a biologically active molecule that occurs naturally in the zeopatle plant.[24] The zeopatle plant has been used in Mexico to make a tea that can induce menstruation and labor.[24] In 1981, Vinayak Kane and Donald Doyle reported a synthesis of zoapatanol.[25][26] They used the Baeyer-Villiger oxidation to make a lactone that served as a crucial building block that ultimately led to the synthesis of zoapatanol.[25][26]

Kane and Doyle used a Baeyer-Villiger oxidation to synthesize zoapatanol


Steroids are an important class of molecules for use in therapeutics.[27] For instance, testololactone has been identified as an anticancer agent.[27] In 2013, Alina Świzdor reported the transformation of dehydroepiandrosterone to testololactone by use of a fungus that produces Baeyer-Villiger monooxygenases.[27] The fungus formed testololactone from dehydroepiandrosterone via a Baeyer-Villiger oxidation.[27]

Świzdor reported that a Baeyer-Villiger monooxygenase could change dehydroepiandrosterone into testololactone

See also[edit]


  1. ^ a b c d e f g h i j Kürti, László; Czakó, Barbara (2005). Strategic Applications of Named Reactions in Organic Synthesis. Burlington; San Diego; London: Elsevier Academic Press. p. 28. ISBN 978-0-12-369483-6. 
  2. ^ a b c Krow, Grant R. (1993). "The Baeyer-Villiger Oxidation of Ketones and Aldehydes". Organic Reactions. 43 (3): 251–798. doi:10.1002/0471264180.or043.03. 
  3. ^ a b c d Crudden, Cathleen M.; Chen, Austin C.; Calhoun, Larry A. (2000). "A Demonstration of the Primary Stereoelectronic Effect in the Baeyer-Villiger Oxidation of α-Fluorocyclohexanones". Angew. Chem. Int. Ed. 39 (16): 2851–2855. doi:10.1002/1521-3773(20000818)39:16<2851::aid-anie2851>;2-y. 
  4. ^ a b c d e f Myers, Andrew G. "Chemistry 115 Handouts: Oxidation" (PDF). 
  5. ^ The Role of Hydrogen Bonds in Baeyer-Villiger Reactions Shinichi Yamabe and Shoko Yamazaki J. Org. Chem.; 2007; 72(8) pp 3031–41; (Article) doi:10.1021/jo0626562
  6. ^ a b c d e f g h ten Brink, G.-J.; Arends, W. C. E.; Sheldon, R. A. (2004). "The Baeyer-Villiger Reaction: New Developments toward Greener Procedures". Chem. Rev. 104 (9): 4105–4123. doi:10.1021/cr030011l. 
  7. ^ Li, Jie Jack; Corey, E. J., eds. (2007). Name Reactions of Functional Group Transformations. Hoboken, NJ: Wiley-Interscience. 
  8. ^ a b c Hawthorne, M. Frederick; Emmons, William D.; McCallum, K. S. (1958). "A Re-examination of the Peroxyacid Cleavage of Ketones. I. Relative Migratory Aptitudes". J. Am. Chem. Soc. 80 (23): 6393–6398. doi:10.1021/ja01556a057. 
  9. ^ Jones, Jr., Maitland; Fleming, Steven A. (2010). Organic Chemistry (4th ed.). Canada: W. W. Norton & Company. p. 293. ISBN 978-0-393-93149-5. 
  10. ^ a b c d Evans, D. A. "Stereoelectronic Effects-2" (PDF). Chemistry 206 (Fall 2006-2007). 
  11. ^ Baeyer, Adolf; Villiger, Victor (1899). "Einwirkung des Caro'schen Reagens auf Ketone". Ber. Dtsch. Chem. Ges. 32 (3): 3625–3633. doi:10.1002/cber.189903203151. 
  12. ^ a b Hassall, C. H. (1957). "The Baeyer-Villiger Oxidation of Aldehydes and Ketones". Organic Reactions. 9 (3): 73–106. doi:10.1002/0471264180.or009.03. 
  13. ^ Renz, Michael; Meunier, Bernard (1999). "100 Years of Baeyer-Villiger Oxidations". Eur. J. Org. Chem. 1999 (4): 737–750. doi:10.1002/(SICI)1099-0690(199904)1999:4<737::AID-EJOC737>3.0.CO;2-B. 
  14. ^ a b c d e f Doering, W. von E.; Dorfman, Edwin (1953). "Mechanism of the Peracid Ketone-Ester Conversion. Analysis of Organic Compounds for Oxygen-18". J. Am. Chem. Soc. 75 (22): 5595–5598. doi:10.1021/ja01118a035. 
  15. ^ a b c d e f Doering, W. von E.; Speers, Louise (1950). "The Peracetic Acid Cleavage of Unsymmetrical Ketones". 72 (12): 5515–5518. doi:10.1021/ja01168a041. 
  16. ^ Turner, Richard B. (1950). "Stereochemistry of the Peracid Oxidation of Ketones". J. Am. Chem. Soc. 72 (2): 878–882. doi:10.1021/ja01158a061. 
  17. ^ Gallagher, T. F.; Kritchevsky, Theodore H. (1950). "Perbenzoic Acid Oxidation of 20-Ketosteroids and the Stereochemistry of C-17". J. Am. Chem. Soc. 72 (2): 882–885. doi:10.1021/ja01158a062. 
  18. ^ Cavarzan, Alessandra; Scarso, Alessandro; Sgarbossa, Paolo; Michelin, Rino A.; Strukul, Giorgio (2010). "Green Catalytic Baeyer–Villiger Oxidation with Hydrogen Peroxide in Water Mediated by Pt(II) Catalysts". ChemCatChem. 2 (10): 1296–1302. doi:10.1002/cctc.201000088. 
  19. ^ B. Schweitzer-Chaput, T. Kurtén, M. Klussmann, Angew. Chem. Int. Ed. 2015, 54, 11848–11851.doi:10.1002/anie.201505648
  20. ^ a b c d Grant R. Krow (1991). Trost, Barry M.; Fleming, Ian, eds. Comprehensive Organic Synthesis - Selectivity, Strategy and Efficiency in Modern Organic Chemistry, Volumes 1 - 9. Elsevier. pp. 671–688. ISBN 978-0-08-035930-4. 
  21. ^ a b c d Seymour, Craig. "Page 1 The Asymmetric Baeyer-Villiger Oxidation" (PDF).  External link in |website= (help)
  22. ^ a b Payne, G. B. (1962). "A Simplified Procedure for Epoxidation by Benzonitrile-Hydrogen Peroxide. Selective Oxidation of 2-Allylcyclohexanone". Tetrahedron. 18 (6): 763–765. doi:10.1016/S0040-4020(01)92726-7. 
  23. ^ ten Brink, Gerd-Jan; Vis, Jan-Martijn; Arends, Isabel W. C. E.; Sheldon, Roger A. (2001). "Selenium-Catalyzed Oxidations with Aqueous Hydrogen Peroxide. 2. Baeyer−Villiger Reactions in Homogeneous Solution". J. Org. Chem. 66 (7): 2429–2433. doi:10.1021/jo0057710. 
  24. ^ a b Levine, Seymour D.; Adams, Richard E.; Chen, Robert; Cotter, Mary Lou; Hirsch, Allen F.; Kane, Vinayak V.; Kanojia, Ramesh M.; Shaw, Charles; Wachter, Michael P.; Chin, Eva; Huettemann, Richard; Ostrowski, Paul (1979). "Zoapatanol and Montanol, Novel Oxepane Diterpenoids, from the Mexican Plant Zoapatle (Montanoa tomentosa)". J. Am. Chem. Soc. 101 (12): 3405–3407. doi:10.1021/ja00506a057. 
  25. ^ a b Kane, Vinayak V.; Doyle, Donald L. (1981). "Total Synthesis of (±) Zoapatanol: A Stereospecific Synthesis of a Key Intermediate". Tetrahedron Lett. 22 (32): 3027–3030. doi:10.1016/S0040-4039(01)81818-9. 
  26. ^ a b Kane, Vinayak V.; Doyle, Donald L. (1981). "Total Synthesis of (±) Zoapatanol". Tetrahedron Lett. 22 (32): 3031–3034. doi:10.1016/S0040-4039(01)81819-0. 
  27. ^ a b c d Świzdor, Alina (2013). "Baeyer-Villiger Oxidation of Some C19 Steroids by Penicillium lanosocoeruleum". Molecules. 18 (11): 13812–13822. doi:10.3390/molecules181113812. 

External links[edit]