跳转到内容

巴顿反应

维基百科，自由的百科全书

巴顿反应（Barton反应）以英国化学家德里克·巴顿命名，也称为巴顿亚硝酸酯反应[1]反应中亚硝酸酯光解生成δ-亚硝基醇。反应经由RO–NO键均裂，氧自由基夺氢，而后自由基结合的机理。[2]

Barton反应

类似的反应是以卤代胺为原料的Hofmann-Löffler-Freytag反应。

该反应是在1960年发现的，其发现者是诺贝尔奖获得者德里克·巴顿爵士。[3] 巴顿1969年的诺贝尔化学奖是因为他在理解有机分子构象方面的工作而获奖，这项工作对于实现巴顿反应的实用性至关重要。[4]

Barton反应涉及RO-NO均匀断裂，然后进行δ-夺氢反应，自由基重组和互变异构反应形成肟。[5]δ-氢的选择性是6-元基团中间体的构象的结果。 通常，可以容易地预测氢原子夺取的位置。 这允许区域选择性和立体选择性地将功能性引入到具有高产率的复杂分子中。 由于其独特的衍生其他惰性底物的能力，巴顿在20世纪60年代广泛使用这种反应来制造许多非天然的类固醇类似物。 [6]

虽然Barton反应尚未得到许多其他有机反应的普及或广泛使用，同样的是机理上类似的Hofmann-Löffler-Freytag反应，但它代表了碳氢键活化（英语：Carbon–hydrogen bond activation）化学的第一个例子，在工业和学术化学界这个领域现在是许多前沿研究的主题。[7]

亚硝酸烷基酯的制备

已隱藏部分未翻譯内容，歡迎參與翻譯。

The unusual alkyl nitrite starting material of the Barton reaction is prepared by attack of an alcohol on a nitrosylium cation generated in situ by dehydration of doubly protonated nitrous acid.[8] This series of steps is mechanistically identical to the first half of the mechanism formation of the more well-known aryl and alkyl diazonium salts.

While the synthesis of alkyl nitrites from nitrosyl chloride is known and oft-employed in the context of complex molecule synthesis, the reaction is reversible and the products are in thermodynamic equilibrium with the starting material. Furthermore, nitrosyl chloride is a powerful oxidizing agent, and oxidation of the alcohols with concomitant chlorination has been observed.[9] The reaction of nitrosyl chloride with aromatic alcohols generally yields nitroso compounds and other over-oxidation products.

反应机理和区域选择性

已隱藏部分未翻譯内容，歡迎參與翻譯。

The Barton reaction commences with a photochemically induced cleavage of the nitrite O-N bond, typically using a high pressure mercury lamp.[10] This produces an alkyoxyl radical which immediately abstracts a hydrogen atom from the δ-carbon. In the absence of other radical sources or other proximal reactive groups, the alkyl radical recombines with the nitrosyl radical. The resultant nitroso compounds undergoes tautomerization to the isolated oxime product.

The carbon centered radical can be intercepted by other radical sources such as iodine or acrylonitrile. The first instance results in the δ-hydrogen being replaced with iodine, then subsequent cyclization to a tetrahydrofuran by an SN2 reaction.[11] The second example results in a chain elongation product with the oxime formed 2 carbon units further from the oxygen than normal.[12]

This mechanistic hypothesis is supported by kinetic isotope effect experiments.[13] Isotopic labeling of the nitrite with 15N has shown the mechanism non-‘caged’ and that the nitrosyl radical formed from a given nitrite recombines randomly with other alkyl radicals. However, recombination of the nitrosyl radical with the alkoxyl radical (a reversal of the homolytic cleavage) has been shown to proceed without scrambling of isotope labels.[14] This lack of tight radical pairing is also supported by the observation that alkyl radicals generated by Barton conditions can undergo radical cyclization while analogous intermediates generated by lead tetraacetate oxidation do not.[15]

In rare cases, it appears that the alkoxyl radical may epimerize before hydrogen atom abstraction.[16]

Most commonly, including steroidal systems, the hydrogen atom is abstracted from a methyl group that has a 1,3 diaxial relationship with the alkoxyl radical.[17] In the absence of a hydrogen on the δ-carbon, or when the particular conformation of the substrate orients the ε-carbon close together, 1,6-hydrogen atom transfer is the favored process. However, these reactions tend to be an order of magnitude slower than the corresponding 1,5-hydrogen atom transfer.

Computational studies have shown that this preference for 1,5-hydrogen atom transfer over 1,6-hydrogen atom transfer appears to be entropically favored rather than a result of a particular stable ‘chair-like’ transition state.[18] In fact, it has been calculated that the 1,6-hydrogen atom transfer proceeds through a transition that is about 0.8 kcal/mol lower than that of the 1,5.

In acyclic systems, δ-hydrogen abstraction is still observed, however, alpha-hydrogen abstraction to form the corresponding ketone competes.[19]

In certain cases, particularly nitrites derived from cyclopentyl alcohols, the oxygen-centered radical prefers to react via C-C bond cleavage as opposed to H-atom abstraction.[11] For example, when subjected to Barton conditions, cyclopentyl nitrite forms glutaraldehyde monoxime. This is also observed in cases where the radical intermediate formed by fragmentation is particularly stable, such as the allylic radical formed by the fragmentation of isopulegol nitrite.[20]

变体

已隱藏部分未翻譯内容，歡迎參與翻譯。

In rigid systems such as aldosterone, the 1,5-hydrogen atom transfer is exceedingly fast, with a rate constant on the order of 10^7 s-1. Similar intermolecular H-atom transfer can be up to 100 times slower.[21] Furthermore, the hydrogen atom transfer benefits from the formation of a stronger O-H bond at the expense of a weaker C-H bond. For the formation of a primary, second, or tertiary alkyl radical from an alkoxyl radical, there is a driving force of 3 kcal/mol, 5 kcal/mol, and 9 kcal/mol, respectively.[17]

The alkyl radical formed after hydrogen atom transfer is susceptible to standard radical reactions when scavengers are present in sufficient excess to outcompete the nitrosyl radical. Soon after their initial disclosure, Barton and co-workers reported the trapping of the radical with I2 and CCl3Br (as Iodine and Bromine radical sources, respectively) to form the δ-halo-alcohol. These halohydrin species can be cyclized to the corresponding tetrahydropyran derivates under basic conditions.[22]

Large excesses of activated alkenes can be used to intercept the alkyl radical and results in formation of a C-C bond from an unactivated C-H bond.[23]

In the presence of oxygen, the alkyl radical is trapped and forms an organic peroxy radical. This intermediate is trapped by the nitrosyl radical and then isomerizes to give a δ-nitrate ester which, while both acid- and base-stable, can be reduced to the corresponding alcohol under mild conditions.[24]

参考文献

  1. ^ D. H. R. Barton, J. M. Beaton, L. E. Geller, and M. M. Pechet. A New Photochemical Reaction. Journal of the American Chemical Society. 1961, 83 (19): 4076–4083. doi:10.1021/ja01480a030. 
  2. ^ IUPAC Goldbook (PDF). [2008-06-27]. （原始内容 (PDF)存档于2007-06-09）. 
  3. ^ Barton, D. H. R.; Beaton, J. M.; Geller, L. E.; Pechet, M. M. A New Photochemical Reaction. Journal of the American Chemical Society. 1960, 82 (10): 2640–2641. doi:10.1021/ja01495a061. 
  4. ^ Barton, D. H. R.; Beaton, J. M.; Geller, L. E.; Pechet, M. M. A New Photochemical Reaction1. Journal of the American Chemical Society. 1961, 83 (19): 4076–4083. doi:10.1021/ja01480a030. 
  5. ^ 國際純化學和應用化學聯合會，化學術語概略，第二版。（金皮書）(1997)。在線校正版: (2006–) "Barton Reaction"。doi:10.1351/goldbook.B00599
  6. ^ Nussbaum, A. L.; Yuan, E. P.; Robinson, C. H.; Mitchell, A.; Oliveto, E. P.; Beaton, J. M.; Barton, D. H. R. The Photolysis of Organic Nitrites. VII. Fragmentation of the Steroidal Side Chain. The Journal of Organic Chemistry. 1962, 27: 20–23. doi:10.1021/jo01048a004. 
  7. ^ Gutekunst, W. R.; Baran, P. S. C–H functionalization logic in total synthesis. Chemical Society Reviews. 2011, 40 (4): 1976. doi:10.1039/c0cs00182a. 
  8. ^ N-Butyl Nitrite. Organic Syntheses. 1936, 16: 7. doi:10.15227/orgsyn.016.0007. 
  9. ^ Beckham, L. J.; Fessler, W. A.; Kise, M. A. Nitrosyl Chloride. Chemical Reviews. 1951, 48 (3): 319–396. PMID 24541207. doi:10.1021/cr60151a001. 
  10. ^ Sugimoto, A.; Fukuyama, T.; Sumino, Y.; Takagi, M.; Ryu, I. Microflow photo-radical reaction using a compact light source: Application to the Barton reaction leading to a key intermediate for myriceric acid A. Tetrahedron. 2009, 65 (8): 1593–1598. doi:10.1016/j.tet.2008.12.063. 
  11. ^ 11.0 11.1 Akhtar, M.; Barton, D. H. R.; Sammes, P. G. Some Radical Exchange Reactions during Nitrite Ester Photolysis1. Journal of the American Chemical Society. 1965, 87 (20): 4601–4607. doi:10.1021/ja00948a036. 
  12. ^ Petrovic, G.; Cekovic, Z. Free radical alkylation of the remote nonactivated δ-carbon atom. Tetrahedron Lett. 1997, 38 (4): 627–630. doi:10.1016/s0040-4039(96)02357-x. 
  13. ^ Barton, D. H. R.; Hesse, R. H.; Pechet, M. M.; Smith, L. C. The mechanism of the barton reaction. Journal of the Chemical Society, Perkin Transactions 1. 1979: 1159. doi:10.1039/P19790001159. 
  14. ^ Akhtar, M.; Pechet, M. M. The Mechanism of the Barton Reaction. Journal of the American Chemical Society. 1964, 86 (2): 265–268. doi:10.1021/ja01056a035. 
  15. ^ Čeković, Ẑ.; Ilijev, D. Intramolecular cyclization of alkenyl radicals generated by 1,5-hydrogen transfer to alkoxy radicals. Tetrahedron Letters. 1988, 29 (12): 1441–1444. doi:10.1016/S0040-4039(00)80319-6. 
  16. ^ Nickson, A.; Mahajan, J.; McGuire, F. Communications- Epimerization in a Nitrite Ester Photolysis. The Journal of Organic Chemistry. 1961, 26 (9): 3617–3618. doi:10.1021/jo01067a671. 
  17. ^ 17.0 17.1 Čeković, Ž. Reactions of δ-carbon radicals generated by 1,5-hydrogen transfer to alkoxyl radicals. Tetrahedron. 2003, 59 (41): 8073–8090. doi:10.1016/S0040-4020(03)01202-X. 
  18. ^ Dorigo, A. E.; McCarrick, M. A.; Loncharich, R. J.; Houk, K. N. Transition structures for hydrogen atom transfers to oxygen. Comparisons of intermolecular and intramolecular processes, and open- and closed-shell systems. Journal of the American Chemical Society. 1990, 112 (21): 7508–7514. doi:10.1021/ja00177a009. 
  19. ^ Ishmuratov, G. Y.; Kharisov, R. Y.; Shayakhmetova, A. K.; Botsman, L. P.; Shitikova, O. V.; Tolstikov, G. A. Ozonolysis of Ricinolic Acid Derivatives and Transformations of the Ozonolysis Products under Barton Reaction Conditions. Chemistry of Natural Compounds. 2005, 41 (6): 643–649. S2CID 43171151. doi:10.1007/s10600-006-0003-z. 
  20. ^ Bulliard, M.; Balme, G. V.; Gore, J. Fragmentation of isopulegol by a radical process. Tetrahedron Letters. 1989, 30 (17): 2213–2216. doi:10.1016/S0040-4039(00)99651-5. 
  21. ^ Robertson, J.; Pillai, J.; Lush, R. K. Radical translocation reactions in synthesis. Chemical Society Reviews. 2001, 30 (2): 94–103. doi:10.1039/b000705f. 
  22. ^ Akhtar, M.; Barton, D. H. R.; Sammes, P. G. Radical Exchange during Nitrite Photolysis. Journal of the American Chemical Society. 1964, 86 (16): 3394–3395. doi:10.1021/ja01070a039. 
  23. ^ Petrović, G.; Čeković, Ž. Alkylation of remote non-activated δ-carbon atoms: Addition of δ-carbon radicals, generated by 1,5-hydrogen transfer in alkoxy radical intermediates, to activated olefins. Tetrahedron. 1999, 55 (5): 1377–1390. doi:10.1016/S0040-4020(98)01110-7. 
  24. ^ Allen, J.; Boar, R. B.; McGhie, J. F.; Barton, D. H. R. Nitrite photolysis in the presence of oxygen. An improved synthesis of 32-oxygenated lanostanes. Journal of the Chemical Society, Perkin Transactions 1. 1973: 2402. doi:10.1039/P19730002402. 
  • László Kürti, Barbara Czakó: Strategic Applications of Named Reactions in Organic Synthesis; Elsevier Academic Press, Burlington-San Diego-London 2005, 1. Edition; ISBN 0-12-369483-3.
检索自“https://zh.wikipedia.org/w/index.php?title=巴顿反应&oldid=70296929”