.
Angewandte
Communications
DOI: 10.1002/anie.201200961
Photochemistry
Visible-Light Photoredox Catalysis in Flow**
Joseph W. Tucker, Yuan Zhang, Timothy F. Jamison, and Corey R. J. Stephenson*
Photoredox catalysts have recently been used as powerful
tools for synthetic chemists to exploit the energy gained by
the absorption of low-energy light within the visible spectrum
to initiate a variety of organic transformations.[1] The devel-
opment of methods based on the single-electron transfer
properties of photoredox catalysts, particularly in the last
several years, has represented a shift in models with respect to
the way synthetic chemists consider both photochemistry and
redox manipulations of organic molecules.[2–4]In addition, the
advent of new technologies has enabled chemists to conduct
Figure 1. Photoredox catalysis in flow. Enabling increased efficiency by
reactions with greater efficiency than ever before. Among
these new technologies is the development and wide imple-
mentation of flow reactors.[5,6] Conducting transformations in
flow has many advantages compared to the more traditional
batch reactions, in particular: a more predictable reaction
scale-up, decreased safety hazards, and improved reproduci-
bility. In addition, for photochemical transformations, the
high surface-area-to-volume ratios typical of flow reactors
allow for more efficient irradiation of a reaction mixture.[7]
Due to this feature, we reasoned that a mesofluidic photo-
chemical flow reactor would be amenable to our groupꢀs
ongoing study of visible-light-induced organic transforma-
tions mediated by photoredox catalysts (Figure 1).[8]
reactor technology (SET=single-electron transfer).
problem we sought to design a reactor having a considerably
smaller path length through which the light must travel. In
addition, a reactor having a greater surface-area-to-volume
ratio would result in an increased photon flux density,
potentially accelerating the reaction.[12] Commercially avail-
able PFA (perfluoro alkoxy alkane) tubing having an internal
diameter of 0.762 mm was identified as a viable choice
because of its chemical resistance and optical transparency.
Furthermore, a photoreactor of this size will allow for optimal
absorbance at typical catalyst concentrations (around
1.0 mm). For instance, the molar extinction coefficient of
Ru(bpy)3Cl2 (bpy = 2,2’-bipyridine) has been measured to be
13000mÀ1 cmÀ1,[13] as such the thickest portion of the tubing
allows for the absorption of 90% of the incident radiation.
Likewise, when carried out in batch reactors, 99% of the
incident radiation is absorbed by the reaction medium
residing within 1.5 mm of the reactor surface while the
remaining internal volume receives little productive radia-
tion.[14]
In designing our reactor, we sought to make it as simple as
possible without using specialized equipment in the hopes
that a similar design could be readily implemented in other
laboratories. Our optimized reactor involved wrapping
105 cm (corresponding to a 479 mL reactor volume) of PFA
tubing in figure-eights around a pair of glass test tubes. We
then used a peristaltic pump to pump the reaction mixture
through the tubing with irradiation from a commercially
available assembly of seven blue light emitting diodes
(LEDs).[15] Finally a silver-mirrored Erlenmeyer flask was
positioned above the reactor to reflect any incident light back
onto the tubing.[16]
Our group has studied the use of both the oxidative and
reductive quenching cycles of photoredox catalysts to initiate
synthetically useful manipulations of organic molecules such
as intra- and intermolecular radical reactions,[8] formal C H
À
oxidation reactions,[9] and the halogenation of alcohols.[10]
During these studies, it was commonly observed that large-
scale reactions were often slower than those conducted on
smaller scale.[11] As a consequence of the Beer–Lambert law,
the penetration of visible light through a reaction medium
decreases exponentially with increasing path length. We
hypothesized that this may be one reason for the observed
loss of reaction efficiency. To potentially circumvent this
[*] J. W. Tucker, Prof. Dr. C. R. J. Stephenson
Department of Chemistry, Boston University
Boston, MA 02215 (USA)
E-mail: crjsteph@bu.edu
Dr. Y. Zhang, Prof. Dr. T. F. Jamison
Department of Chemistry, Massachusetts Institute of Technology
Cambridge, MA 02139 (USA)
[**] Financial support for this research from the NSF (grant number
CHE-1056568), the NIH-NIGMS (grant number R01-GM096129),
the Alfred P. Sloan Foundation, Amgen, and Boehringer Ingelheim
is gratefully acknowledged. J.W.T. thanks The American Chemical
Society, Division of Organic Chemistry and Amgen for a graduate
fellowship. NMR (CHE-0619339) and MS (CHE-0443618) facilities
at BU are supported by the NSF.
Our initial experiments focused on the oxidative gener-
ation of iminium ions from N-aryl tetrahydroisoquinolines,
using reaction conditions similar to those we recently
reported.[9c] Employing BrCCl3 as the terminal oxidant, we
observed rapid formation of the iminium ion, 2, from the
corresponding tetrahydroisoquinoline, 1. Optimization stud-
ies showed that subjecting a solution of 1, BrCCl3, and
Ru(bpy)3Cl2 (0.5 mol%) in dimethylformamide (DMF) to
Supporting information for this article is available on the WWW
4144
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Angew. Chem. Int. Ed. 2012, 51, 4144 –4147