Under identical conditions, no oxygen was produced in the
absence of catalyst 4. Omitting the photosensitizer resulted in
no oxygen evolution, and switching off the light terminated
oxygen evolution, thus confirming that complex 4 and the
photosensitizer are essential for the light-induced water
oxidation.
The properties of complex 4 in solution were studied in
the presence of K3PO4 by 1H NMR spectroscopy and X-band
EPR spectroscopy in D2O and H2O, respectively (Figures S1–
S8). The relatively narrow chemical shift range in combina-
In conclusion, we have reported a homogeneous manga-
nese-based catalyst 4, which is capable of catalyzing oxidation
of water to molecular oxygen in the presence of a single-
electron oxidant [Ru(bpy)3]3+. More importantly, 4 also
catalyzes photochemical water oxidation when using either
[Ru(bpy)3]2+ or the related [Ru(bpy)2(deeb)]2+ complex as
photosensitizer. A major difference between catalyst 4 and a
series of related catalysts developed by us and other research
groups is that the benzylic amine function has been replaced
by imidazole, thus making the ligand more resistant towards
oxidation. Furthermore, it may be even more important that
imidazole, as in many natural systems, can promote proton-
transfer reactions as the oxidation states of the manganese
atoms change.
tion with the absence of any EPR signal at 77 K indicate the
III,III
presence of an antiferromagnetically coupled Mn2
com-
plex with a singlet ground state, that is, the Mn2II,III complex 4
III,III
was oxidized to Mn2
by atmospheric oxygen because the
redox potential is lowered as the pH value is increased. The
broadening of the NMR signals could be attributed to the
population of excited spin states at ambient temperature.
Received: June 23, 2011
Published online: October 7, 2011
During the course of the water oxidation, the complex is
III,III
Keywords: homogeneous catalysis · manganese · N,O ligands ·
photocatalysis · water oxidation
expected to cycle between the initial Mn2
oxidation state
.
and Mn2V,V. In contrast with the EPR experiments in aqueous
III,III
solution, where the complex had been oxidized to Mn2
,
the spectrum recorded in dimethyl sulfoxide (DMSO) at 77 K
shows a broad (100 mT) signal at g = 2.0 (Figure S11), which
is indicative of a Mn2II,III complex.[33] This signal is overlapped
[5] F. Bozoglian, S. Romain, M. Z. Ertem, T. K. Todorova, C. Sens, J.
Mola, M. Rodrꢁguez, I. Romero, J. Benet-Buchholz, X. Fontro-
by a sharp six-line signal from trace amounts of free Mn2+ ions
II,III
in solution. A similar broad signal from Mn2
observed upon reduction of the Mn2
was also
III,III
complex in aqueous
solution by addition of ascorbic acid (Figure S11). In this
spectrum, the six-line signal from free Mn2+ ions is absent,
thus indicating that the ligand backbone of complex 4 is intact
in solution under conditions similar to those used in the water
oxidation experiments.
[6] Z. Deng, H. Tseng, R. Zong, D. Wang, R. Thummel, Inorg.
[7] X. Sala, I. Romero, M. Rodrꢁguez, L. Escriche, A. Llobet,
[8] Y. V. Geletii, B. Botar, P. Kçgerler, D. A. Hillesheim, D. G.
[9] A. Sartorel, M. Carraro, G. Scorrano, R. D. Zorzi, S. Geremia,
[10] S. W. Kohl, L. Weiner, L. Schwartsburd, L. Konstantinovski,
L. J. W. Shimon, Y. Ben-David, M. A. Iron, D. Milstein, Science
[12] Y. Xu, A. Fischer, L. Duan, L. Tong, E. Gabrielsson, B.
[13] Y. V. Geletii, Z. Huang, Y. Hou, D. G. Musaev, T. Lian, C. L.
The NMR spectra recorded at 258C and low concentra-
tions (1.4–2.8 mm) of complex 4 show three broad signals with
chemical shifts of 7.52, 7.31, and 6.69 ppm, which correspond
to the aromatic protons of the ligand (Figures S1 and S2). The
sharp signals at 3.34, and 1.90 ppm correspond to methanol
and acetate ions, respectively, which are released into solution
upon dissolution of complex 4 in D2O in the presence of
K3PO4. The chemical shifts of the aromatic protons were
shown to be essentially independent of the concentration of
complex 4 (Figures S1–S4), which again indicates that the
backbone of complex 4 is intact in solution, that is, there is no
rapid equilibrium between the complex and the uncoordi-
nated ligand. However, at higher concentrations (5.6–
8.5 mm), a set of three new, very broad signals was observed
(Figures S3 and S4). This feature could be attributed to an
equilibrium between the monomeric and dimeric forms in
solution. At low concentrations, the monomer should be
favored, thus giving rise to the initial set of three signals, while
at higher concentrations a mixture of monomer and dimer
could be observed. In addition, NMR spectra recorded at
different temperatures (5, 25, 50, and 808C) indicate that the
dimerization is favored at higher temperatures (Figures S5–
S8), possibly because of entropic effects as coordinated
solvent molecules are released into solution. The changes
with temperature are reversible and on cooling to 258C, the
spectrum at 808C (Figure S8) reverts to the spectrum at 258C
(Figure S6).
[15] Y. Xu, T. ꢂkermark, V. Gyollai, D. Zou, L. Eriksson, L. Duan, R.
[17] Q. Yin, J. M. Tan, C. Besson, Y. V. Geletii, D. G. Musaev, A. E.
[18] W. C. Ellis, N. D. McDaniel, S. Bernhard, T. J. Collins, J. Am.
Angew. Chem. Int. Ed. 2011, 50, 11715 –11718
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