12
reaction of radical 1 with O2 could generate peroxide
(0.019 g, 0.13 mmol), K2CO3 (0.046 g, 0.33 mmol), and
1,4-dioxane (100 mL) was heated under reflux at 110 °C.
Molecular oxygen or air was bubbled into the system for 70 h.
When the reaction was finished as indicated by TLC, the
solvent was evaporated under vacuum for reusing, and the
residue was purified by flash column chromatography
(petroleum ether/ethyl acetate) to afford the desired product
3a (8.1 g, 48%) and 3a (3.48 g, 22%). Moreover, the results
showed that the turnover number (TON) increases with
the increasing amount of the substrate (see Supporting
Information). It indicates that this process might be conve-
niently scaled up in industry.
radical 2 which would give product A, another peroxide
radical 3, and product B followed by a series of electron
transfer and Cu-promoted homolysis of activated CꢀH and
CꢀC bonds in glycol ethers. This process should be far
more complicated than the present primary mechanism
which would be the subject of our future investigations.
To gain mechanistic insight, a competing kinetic isotope
effect (KIE) experiment was carried out (eq 6). As a result, a
significant KIE was observed with the kH/kD = 8.0 (see
Supporting Information). It suggests that the CꢀH bond
cleavage should be the rate-determining step of this proce-
dure. Furthermore, 1,4-dioxane gave 1,4-dioxan-2-ol as a
major product along with the mono- and diformates of 1,2-
ethanediol as minor products without carboxylic acid in this
system, which is similar to the results given by Jewett and
Lawless9 that autoxidation of p-dioxane gave formate esters
of 1,2-ethanediol. The addition of (2,2,6,6-tetramethyl-
piperidin-1-yl)oxyl (TEMPO) does not trap any radical
intermediate but stops the reaction. No reactions occur
when 4-methylmorpholine replaces dioxane. These two
experiments indicate that the copper catalyst may be deac-
tivated by coordination with a N-atom, which was further
confirmed by addition of several nitrogen ligands such as
N,N-dimethylethylenediamine (DMEDA), N,N,N,N-tetra-
methylethylenediamine (TMEDA), and 1,10-phenanthro-
line giving the same results as above. The minor product
cannot give the open-chain product by further reaction with
dioxane under the typical conditions. With the experimental
data and literature precedent in hand, a plausible mecha-
nism for this catalytic aerobic cleavage of CꢀC bonds is
depicted in Scheme 2. This procedure is most likely a copper-
catalyzed autoxidation rather than the copper-O2 pathways
in some enzymes such as tyrosinase and catechol oxidase.10
Radical intermediate 1 would be formed by hydrogen
abstraction from dioxane with a copper(II) peroxide radical,
which could be generated by a combination of molecular
oxygen with copper(I),11 and the CꢀH bond cleavage
should be the rate-determining-step. Auto-oxidation via
Scheme 2. Possible Mechanism
In conclusion, this work demonstrates an unexpected Cu-
catalyzed oxidative cleavage of the C(sp3)ꢀC(sp3) bond of
glycol ether by using air or molecular oxygen as the terminal
stoichiometric oxidant. As a result, the corresponding
R-acyloxy ethers and formates of 1,2-ethanediol are formed
by direct coupling of carboxylic acids and aldehydes with glycol
ethers under the reaction conditions. This system would
represent the first example of Cu-catalyzed aerobic cleavage
of the saturated CꢀC bond in ethers, which could be
potentially applied to the degradation of plastics and poly-
mers made by glycol. Additionally, it could also provide an
efficient and convenient protocol for large-scale preparation
of various valuable pharmaceuticals containing an R-acyloxy
ether subunit by simply coupling carboxylic acids and alde-
hydes with glycol ethers under mild conditions. Moreover,
this process not only could be conveniently scaled up but also
is atom-efficient and environmentally benign. This novel
system may draw much attention from scientists focused on
oxidation chemistry and copper enzymes in biology. Further
studies of this system on the mechanism and expansion of the
substrate scope are underway in our laboratory.
(9) Jewett, D.; Lawless, J. G. Bull. Environ. Contam. Toxicol. 1980,
25, 118.
(10) (a) Solomon, E. I.; Sundaram, U. M.; Machonkin, T. E. Chem.
Rev. 1996, 96, 2563. (b) Solomon, E. I.; Chen, P.; Metz, M.; Lee, S.-K.;
Palmer, A. E. Angew. Chem., Int. Ed. 2001, 40, 4570. (c) Gamez, P.;
Aubel, P. G.; Driessen, W. L.; Reedijk, J. Chem. Soc. Rev. 2001, 30, 376.
(d) Lewis, E. A.; Tolman, W. B. Chem. Rev. 2004, 104, 1047.
(11) (a) Cramer, C. J.; Tolman, W. B. Acc. Chem. Res. 2007, 40, 601.
(b) Arends, I.; Gamez, P.; Sheldon, R. A. Adv. Inorg. Chem. 2006, 58,
235. (c) Que, L., Jr.; Tolman, W. B. Nature 2008, 455, 333. (d) Wang, Y.;
DuBios, J. L.; Hedman, B.; Hodgson, K. O.; Stack, T. D. P. Science
1998, 279, 537. (e) Prigge, S. T.; Eipper, B. A.; Mains, R. E.; Amzel,
L. M. Science 2004, 304, 864. (f) Mirica, L. M.; Vance, M.; Rudd, D. J.;
Hedman, B.; Hodgson, K. O.; Solomon, E. I.; Stack, T. D. P. Science
2005, 308, 1890. (g) Rolff, M.; Schottenheim, J.; Decker, H.; Tuczek, F.
Chem. Soc. Rev. 2011, 40, 4077.
Acknowledgment. This project is supported by the Na-
tional Science Foundation of China (No. 21002045) and the
Fundamental Research Funds for the Central Universities
(lzujbky-2012-55). We also thank the State Key Laboratory
of Applied Organic Chemistry for financial support.
Supporting Information Available. Full experimental
details and characterization data for all products. This
material is available free of charge via the Internet at
(12) (a)Walling, C. InActive Oxygen in Chemistry; Foote, C. S., Valentine,
J. S., Greenberg, A., Liebman, J. F., Eds.; Blackie: 1995; pp 24ꢀ65. (b)
Chudasama, V.; Fitzmaurice, R. J.; Caddick, S. Nat. Chem. 2010, 2, 592.
The authors declare no competing financial interest.
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