C O M M U N I C A T I O N S
by NMR spectroscopy is the poor solubility of ruthenium chloride
3 in toluene and the high viscosity of toluene at low temperature.
Sample preparation was performed by quick transfer of a -78 °C
preformed solution of the intermediate to an NMR tube via a
cannula. The sample was then frozen (-196 °C) and quickly
transferred to the precooled probe of the NMR spectrometer. The
low solubility and therefore low concentration made it difficult to
run 13C NMR experiments, since it was not possible to get a
reasonable signal-to-noise ratio for the carbonyl peaks. This problem
was solved by employing 13CO-labeled catalyst 3 (for its prepara-
tion, see the Supporting Information). With the 13CO-enriched
ruthenium chloride 3, it was possible to monitor the reaction by
13C NMR at low temperature. Acyl intermediate A was studied
and characterized at -32 °C (Scheme 2).
previous NMR studies of the alkoxide exchange,4 and therefore,
the reaction was slower here than in the previous experiments. The
failure to detect an intermediate in the alcohol-alkoxide exchange
is in accordance with the low computed barrier of activation for
this reaction via CO participation (12 kcal/mol).5,14
In conclusion, we have provided experimental evidence for CO
ligand participation in the exchange of chloride for tert-butoxide
in η5-(Ph5Cp)Ru(CO)2Cl (3). An acyl intermediate, A, was observed
by in situ FT-IR measurements and low-temperature NMR spec-
troscopy prior to formation of tert-butoxide complex 5. This shows
how high-energy intermediates (produced via ring slip or dissocia-
tion) can be avoided in ligand exchange15 and that this may be
common in complexes bearing CO ligands.
Acknowledgment. The Swedish Research Council, the Berze-
lius Center EXSELENT, and the Knut and Alice Wallenberg
Foundation are gratefully acknowledged for financial support.
Scheme 2. Detection of Acyl Intermediate A by 13C NMR in
Toluene-d8 at -32 °C
Supporting Information Available: Experimental procedures and
characterization data for all new compounds. This material is available
References
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F. B.; Ba¨ckvall, J.-E. J. Am. Chem. Soc. 2005, 127, 8817. (c) Ko, S. B.;
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Acyl intermediate A has CO peaks at 209.5 (CO) and 208.7 ppm
(acyl).10 The peak of the CO ligand is shifted downfield. This is
comparable to the chemical shifts reported for other anionic
complexes (e.g. 208.1 ppm for [PPN]+[Ru3(CO)11(CO2CH3)]- (8)
in THF-d8).11 The acyl peak of A appears at an unusually high
chemical shift compared with those of similar structures in the
literature.9b,d,11 For example, the acyl peak of 8 appears at 189
ppm, and the neutral cyclopentadienylruthenium complexes
[Cp*Ru(CO)2(COOMe)] and [Cp∧Ru(COOMe)(CO)2]12 also have
acyl peaks in this region [191.3 ppm (C6D6)9d and 193.7 ppm
(CD2Cl2),9b respectively]. However, none of these structures has a
chloride bound to ruthenium. We estimated the 13C NMR shifts of
intermediate A using density functional theory (DFT) calculations
and found that they are in agreement with the expected values for
this structure.13 When the temperature was raised to 0 °C, the peaks
at 209.5 and 208.7 ppm for intermediate A slowly disappeared,
and the peak at 202.8 ppm for the CO groups of tert-butoxide
complex 5 appeared. At room temperature, this transformation was
rapid.
In addition, we studied the alcohol-alkoxide exchange (Scheme
1, step ii), which also should occur via CO assistance.5 However,
no acyl intermediate similar to A has been detected to date by in
situ FT-IR measurements at room temperature and below (Figure
S1). At room temperature, the alcohol-alkoxide exchange was very
rapid (<1 min), but at -78 °C the tert-butoxide ligand of complex
5 was not exchanged by phenylethanol for at least 1 h. However,
at -50 °C, the reaction slowly took place (t1/2 ) 15 min) and the
CO peaks of sec-alkoxide complex 7 at 2026 and 1971 cm-1
(symmetric and asymmetric stretch, respectively) appeared. The rate
of disappearance of tert-butoxide complex 5 was the same as the
rate of formation of sec-alkoxide complex 7, and the reaction was
complete within 2.5 h. The ruthenium concentration in this
experiment was 12 mM, which is ∼5 times lower than in our
(4) Mart´ın-Matute, B.; Åberg, J. B.; Edin, M.; Ba¨ckvall, J.-E. Chem.sEur. J.
2007, 13, 6063.
(5) Nyhle´n, J.; Privalov, T.; Ba¨ckvall, J.-E. Chem.sEur. J. 2009, 15, 5220.
(6) The CO bands of 5 appear at 2021 and 1964 cm-1. For experimental details,
see the Supporting Information.
(7) The reaction mixture containing intermediate A also showed characteristic
peaks in the area of C-O stretching vibrations (t-BuO). However, the
mixture possibly contained t-BuOH (and t-BuOK), and the peaks in this
area were not easy to assign.
(8) H2O vapor in the system absorbed in the region of 1600 cm-1, and a
background spectrum was automatically subtracted from the collected data.
If the amount of H2O vapor was not constant (which it seldom is), a peak
in this region might not be visible. Indeed, in our first experiments, the
system contained so much humidity that a lot of noise in this region made
it difficult to detect the acyl peak.
(9) (a) Gross, D. C.; Ford, P. C. J. Am. Chem. Soc. 1985, 107, 585. (b) Dutta,
B.; Scopelliti, R.; Severin, K. Organometallics 2008, 27, 423. (c) Trautman,
R. J.; Gross, D. C.; Ford, P. C. J. Am. Chem. Soc. 1985, 107, 2355. (d)
Suzuki, H.; Omori, H.; Mor-oka, Y. J. Organomet. Chem. 1987, 327, C47.
(10) The shifts were too close to allow a definite assignment, and they may be
reversed (DFT calculations indicated that δCO > δacyl; see note 13). Even if
the shifts are reversed, the structural conclusions remain the same.
(11) Taube, D. J.; Rokicki, A.; Anstock, M.; Ford, P. C. Inorg. Chem. 1987,
26, 526.
(12) Cp* ) Me5Cp; Cp∧ ) 1-MeO-2,3,4-tris(neopentyl)Cp.
(13) The estimated 13C NMR shifts were 205.3 (acyl) and 211.4 ppm (CO). For
experimental details, see the Supporting Information.
(14) The computed barrier for the corresponding exchange of chloride for tert-
butoxide in 3 is 16.7 kcal/mol (see ref 5).
(15) For a discussion of avoiding high-energy pathways in ligand exchange,
see: Casey, C. P.; Vosejpka, P. C.; Underiner, T. L.; Slough, G. A.; Gavney,
J. A. J. Am. Chem. Soc. 1993, 115, 6680.
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