did not affect the oxidation significantly in the range of 5–30 bar
(entries 1–3). The noticeable effect of temperature reflects
partly an intrinsic response of the reaction rates and partly the
phase behaviour of the reaction medium. The rate of the
aldehyde auto-oxidation increases more strongly with increas-
ing temperature as compared to the Baeyer–Villiger process.
Consequently, a larger excess of aldehyde is required to achieve
similar ketone conversion at higher temperatures (entry 7, 8). At
the same time, the temperature increase results in transition
from a biphasic (liquid and gaseous CO2) to a monophasic
(supercritical) reaction mixture as confirmed by visual inspec-
tion. The resulting dilution of substrates over the whole reactor
volume makes the oxidation also less effective as demonstrated
by dilution with liquid CO2 at room temperature (entry 3, 4).
Similar observations were made in Baeyer–Villiger reactions of
3-benzylcyclobutanone and bicycloctanone.
The Baeyer–Villiger oxidation of A was run in conventional
organic solvents under conditions comparable to those of Table
1, entry 1 (3 equiv. of aldehyde, rt, atmospheric pressure of O2,
24 h). In the absence of steel, a modest conversion of 23% was
achieved in CH2Cl2 only. In the presence of steel shavings,
conversion were 44% (toluene), 25% (ethyl acetate) and 27%
(CH2Cl2). These data demonstrate that CO2 is a “greener”
replacement for CH2Cl2 providing significant advantages for
the efficiency of the oxidation process.
and cyclohexanone react smoothly under these conditions
giving d- and e-lactone, in 70% and 75% conversion, re-
spectively (entries 4 and 5). Larger rings, such as cyclohepta-
none and cyclooctanone, did not undergo ring expansion.5b The
bicyclic ketones, bicyclo[4.2.0]octan-7-one and bicyclo-
[2.2.1]heptan-2-one, were transformed readily into hexahy-
drobenzofuran-2-one (entry 6) and 2-oxabicyclo[3.2.1]octan-
3-one (entry 7), respectively, following the expected
regioselectivity. The acyclic substrates 3-phenylbutan-2-one
and p-methoxybenzophenone underwent oxidation too (entries
8 and 9), the higher conversion being obtained with the latter
substrate. Also in these cases, the oxygen inserted exclusively
into the C–C-bond between the carbonyl and the most
substituted carbon atom.
In conclusion, we have demonstrated that Baeyer–Villiger
reactions can be performed very efficiently in compressed CO2
at room temperature using oxygen as primary oxidant and an
aldehyde as co-reductant. No additional catalyst is required and
good to excellent yields were achieved for a wide range of
cyclic (up to C6) and acyclic ketones. These results emphasise
the large potential of compressed CO2 as a benign and safe
(‘green’) reaction medium for oxidation processes in fine
chemical synthesis.
Notes and references
An initial assessment of the scope of the reaction under a
standard set of reaction conditions demonstrated that a wide
range of ketones, both cyclic and acyclic can be oxidised
efficiently (Table 2).
Various 3-substituted cyclobutanones are readily converted
to their corresponding lactones (entries 1–3). Cyclopentanone
‡ The reactions were performed in a stainless steel high pressure reactor (25
mL) equipped with thick walled glass windows. In a typical experiment, the
ketone (1 mmol), the aldehyde (3 mmol) and a weighed amount of CO2 (9
g) were introduced into the reactor. The reactor was then charged with O2
from a storage vessel, whereby the partial pressure was controlled by the use
of calibration curves.5 After 18 h, the autoclave was carefully vented
through a cryo-trap (acetone–dry ice, 250 °C) to collect the product. The
autoclave and the trap were washed with MTBE and the combined sample
was directly submitted to GC and GC-MS analysis (n-decane was used as
internal standard).
a
Table 2 Baeyer–Villiger oxidation in compressed CO2
Entry Substrate
1
Co-reductant
Pivalaldehyde
Product
Conv. (%)b
100
1 (a) For comprehensive reviews concerning Baeyer–Villiger oxidations,
see: G. R. Krow, Org. React., 1993, 43, 251; (b) M. Renz and B.
Meunier, Eur. J. Org. Chem., 1999, 4, 737; (c) C. Bolm, in Advances in
Catalytic Processes, ed. M. P. Doyle, JAI Press, Greenwich, 1997, Vol.
2, p. 43; (d) C. Bolm, O. Beckmann and T. K. K. Luong in Transition
Metals for Organic Synthesis, ed. M. Beller and C. Bolm, Wiley-VCH,
Weinheim, 1998, p. 213.
2
Benzaldehyde
82
2 (a) R. A. Sheldon and J. M. Kochi, in Metal-Catalyzed Oxidation of
Organic Compounds, Academic Press, New York, 1981; (b) K. A.
Jørgensen, Chem Rev., 1989, 89, 431.
3 Chemical Synthesis Using Supercritical Fluids, ed. P. G. Jessop and W.
Leitner, Wiley-VCH, 1999, p. 478.
4 (a) X. W. Wu, Y. Oshima and S. Koda, Chem. Lett., 1997, 1045; (b) E.
R. Birbaum, R. M. Le Lacheur, A. C. Horton and W. Tumas, J. Mol.
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Kerler, Chem. Ing. Tech., 2000, 72, 382; (f) G. Jenzer, T. Mallat and A.
Baiker, Catal. Lett., 2001, 73, 5; (g) A. M. Steele, J. Zhu and S. C.
Tsang, Catal. Lett., 2001, 73, 9.
3
4
5
Pivalaldehyde
Pivalaldehyde
Benzaldehyde
75
70
75
6
7
Benzaldehyde
Benzaldehyde
64
92
5 (a) F. Loeker and W. Leitner, Chem. Eur. J., 2000, 6, 2011; (b) N.
Theyssen and W. Leitner, Chem. Commun., 2002, 410.
6 T. Mukaiyama and T. Yamada, Bull. Chem. Soc. Jpn., 1995, 68, 17 and
references therein.
8
9
Pivalaldehyde
Benzaldehyde
48
79
7 (a) K. Kaneda, S. Ueno, T. Imanaka, E. Shimotsuma, Y. Nishiyama and
Y. Ishii, J. Org. Chem., 1994, 59, 2915; (b) X. Li, F. Wang, H. Zhang,
C. Wang and G. Song, Synth. Commun., 1996, 26, 1613.
8 K. Neimann and R. Neumann, Org. Lett., 2000, 2, 2861.
9 G. J. Brink, J. M. Vis, I. W. C. E. Arends and R. A. Sheldon, J. Org.
Chem., 2001, 66, 2429.
10 M. Rüsch gen. Klaas and S. Warwel, Org. Lett., 1999, 7, 1025.
11 K. Yoruzu, T. Takai, T. Yamada and T. Mukaiyama, Bull. Chem. Soc.
Jpn., 1994, 67, 2195.
a For the reaction conditions see note‡. b Determined by GC using n-decane
as internal standard.
CHEM. COMMUN., 2002, 1588–1589
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