A R T I C L E S
Adamo et al.
(Scheme 1).7 This side-reaction was recently developed as a
main catalytic reaction in the presence of pure dioxygen or air
(Scheme 3).4,5a,e The homocoupling of arylboronic acids was
first reported by Moreno-Man˜as et al. in 1996, using as catalysts
Pd0 or PdII complexes associated with monodentate phosphines.4
This oxidatiVe coupling could be accelerated by an oxidant, e.g.,
Cu(NO3)2.5d The homocoupling was later extended to arylbo-
ronic esters by Yoshida et al. in 2003, using Pd(OAc)2 and dppp
(1,3-bis-(diphenylphosphino)propane) as catalyst and DMSO as
solvent.5f
However, very little is known about the reaction mechanism
of this oxidatiVe homocoupling. A first mechanism was proposed
involving the oxidative addition of ArB(OH)2 to Pd0 complexes
with the generation of ArPdII-[B(OH)2]L2 (L ) PPh3) com-
plexes.4 However, our attempts to observe this reaction in the
absence of dioxygen always failed, whereas a reaction was
observed between ArB(OH)2 and a peroxo complex (η2-O2)-
PdL2 (L ) PPh3), formed in the reaction of Pd0L4 with
dioxygen.8 Sheldon and Kochi have proposed the formation of
the intermediate complex Ar2PdL2 (L ) PPh3) by a double
transmetalation of ArB(OH)2 with (HO)Pd(OOH)L2 generated
by reaction of water with the peroxo complex (η2-O2)PdL2.9
Conversely, while we were performing this work, Yoshida et
al. proposed a reaction of arylboronic esters ArB(OR)2 with (η2-
O2)Pd(dppp), which would give ArPd-[OOB(OR)2](dppp)
complexes.5f A subsequent transmetalation of the latter complex
by ArB(OR)2 would give Ar2Pd(dppp) and henceforth the
homocoupling product ArAr by a reductive elimination.
We report herein evidences for the mechanism of the
palladium-catalyzed homocoupling of ArB(OH)2 in the presence
of dioxygen (Scheme 3). In this study, it is clearly mechanisti-
cally and kinetically established that a peroxo complex of
palladium, (η2-O2)PdL2 (L ) PPh3),10 plays a key role in the
catalytic homocoupling of arylboronic acids.
were carried out in a thermostated three-electrode cell connected to a
Schlenk line. The counterelectrode was a platinum wire of ca. 1 cm2
apparent surface area; the reference was a saturated calomel electrode
(Radiometer) separated from the solution by a bridge (3 mL) filled
with a 0.3 M n-Bu4NBF4 solution in chloroform (or DMF). Degassed
chloroform (or DMF) (15 mL) containing 0.3 M n-Bu4NBF4 was poured
into a cell. (η2-O2)Pd(PPh3)2 (20 mg, 30 µmol, 2 mM) was then
introduced into the cell. The kinetic measurements were performed at
a rotating gold disk electrode (diameter ) 2 mm, inserted into a Teflon
holder, EDI 65109, Radiometer) with an angular velocity of 105 rad‚s-1
(Radiometer controvit). The rotating electrode was polarized at +0.70
V (+0.48 in DMF) on the plateau of the oxidation wave of (η2-O2)-
Pd(PPh3)2. 4-MeO-C6H4-B(OH)2 (45 mg, 300 µmol, 20 mM) was then
added into the cell, and the decrease of the oxidation current was
recorded versus time up to 100% conversion.
Typical Procedure for NMR Experiments. All experiments were
performed under argon atmosphere. To a solution of (η2-O2)Pd(PPh3)2
(5 mg, 7.5 µmol) in 0.5 mL of degassed CDCl3 were added various
amounts of arylboronic acids 1a-c or esters 1′b (from 0.75 to 37.5
1
µmol). The 31P NMR and H NMR were then performed.
Characterization of [ArB(OH)2,(η2-O2)Pd(PPh3)2] 6a, 6b, 6c, and
6′b. All experiments were performed under argon atmosphere. The
complexes were generated by addition of 0.5 equiv of 1a, 1b, 1c, and
1′b, respectively, to (η2-O2)Pd(PPh3)2 in CDCl3. The 31P NMR data of
6a, 6b, 6c, and 6′b are collected in Table 2.
Characterization of trans-ArPd(OH)(PPh3)2 5a, 5b. All experi-
ments were performed under argon atmosphere. The complexes were
generated as above by addition of 5 equiv of 1a, 1b, respectively, to
(η2-O2)Pd(PPh3)2 in CDCl3. The 1H NMR and 31P NMR spectroscopies
and ESI MS spectrometry of 5a, 5b are collected in Table 1. The
characteristics of 5b were identical to those of an authentic sample
generated in situ by addition of 12 mg (46 µmol) of PPh3 to a solution
11a,b
of 3.4 mg (3.24 µmol) [PhPd(µ-OH)(PPh3)]2
in 0.5 mL of CDCl3.
Characterization of trans-ArPdAr′(PPh3)2 trans-8ac and trans-
8bc. All experiments were performed under argon atmosphere. The
complexes were generated in an NMR tube by addition of 1.1 equiv
of 1c to trans-ArPd(OH)(PPh3)2 5a or 5b generated as above in CDCl3.
The spectra from 1H NMR, NMR 2D, and 31P NMR spectroscopies of
trans-8ac and trans-8bc are collected in Table 6.
Typical Procedure for (η2-O2)Pd(PPh3)2-Catalyzed Homocou-
pling of Arylboronic Acids (Scheme 5). To a solution of (η2-O2)Pd-
(PPh3)2 (3 mg, 4.6 µmol) in 0.5 mL of CDCl3 was added under dioxygen
500 µL (23 µmol) of the arylboronic acid 1b (or 1a) from a mother
solution of 1b (46 mM in CDCl3). After mixing for 10 min, the yield
of the homocoupling product PhPh 2b (or 4-MeO-C6H4-C6H4-OMe-4,
2a) was determined by 1H NMR spectroscopy after addition of a known
amount of toluene as internal standard. The 1H NMR spectrum of PhPh
(or 4-MeO-C6H4-C6H4-OMe-4) was identical to that of an authentic
commercial sample. The yield of the byproduct Ph-OH (or 4-MeO-
C6H4-OH) was determined in a similar way.
Experimental Section
General. 31P NMR spectra were recorded in CDCl3 or in DMF
containing 10% of acetone-d6 on a Bruker spectrometer (101 MHz)
1
with H3PO4 as an external reference. H NMR spectra were recorded
in CDCl3 on a Bruker spectrometer (250 MHz) with TMS as an internal
reference.
Chemicals. DMF was distilled from calcium hydride under vacuum
and kept under argon. PPh3, PhB(OH)2, 4-CN-C6H4-B(OH)2, 4-MeO-
C6H4-B(OH)2, and PhB(O-(CH2)3-O) were commercial and used as is.
8a
The peroxo complex (η2-O2)Pd(PPh3)2 and the dimeric complex
[PhPd(µ-OH)(PPh3)]211a,b were synthesized as reported in the literature.
Typical Procedure for the Kinetics of the Reaction of (η2-O2)-
Pd(PPh3)2 with Arylboronic Acids, As Monitored by Amperometry.
All experiments were performed under argon atmosphere. Experiments
Computational Methods. All calculations were carried out using
the Gaussian code.12 A hybrid Hartree-Fock/density functional model,
hereafter referred to as PBE0, was used throughout.13 In this functional,
derived from the PBE,14 the ratio of HF/DFT exchange is fixed a priori
to 1/4.15 A double ê quality LANL2 basis16 and corresponding
pseudopotential17 was used for all calculations. Such level of theory
was proven to provide reliable results both for thermochemical and
(7) (a) Campi, E. M.; Jackson, R.; Marcuccio, S.; Naeslund, C. G. M. J. Chem.
Soc. Chem. Commun. 1994, 2395-2395. (b) Gillmann, T.; Weeber, T.
Synlett 1994, 649-651. (c) Song, Z. Z.; Wong, H. N. C. J. Org. Chem.
1994, 59, 33-41.
(8) (a) Wilke, G.; Schott, H.; Heimbach, P. Angew. Chem., Int. Ed. 1967, 6,
92-93. (b) Amatore, C.; Aziz, S.; Jutand, A.; Meyer, G.; Cocolios, P. New
J. Chem. 1995, 19, 1047-1059.
(9) Sheldon, R. A.; Kochi, J. K. Activation of Molecular Oxygen by Metal
Complexes. In Metal-catalyzed Oxidations of Organic Compounds; Aca-
demic Press: New York, 1981; Chapter 4, pp 71-119.
(12) Frisch, M. J.; et al. Gaussian 03, Revision B5; Gaussian, Inc.: Pittsburgh,
PA, 2003.
(13) Adamo, C.; Barone, V. J. Chem. Phys. 1999, 110, 6158-6170.
(14) Perdew, J. P.; Burke, K.; Ernzerhof, M. Phys. ReV. Lett. 1996, 77, 3865-
3868.
(15) Adamo, C.; Barone, V. Chem. Phys. Lett. 1997, 274, 242-250.
(16) Dunning, T. H., Jr.; Hay, P. J. In Modern Theoretical Chemistry; Schaefer,
H. F., III, Ed.; Plenum: New York, 1976; pp 1-28.
(17) Hay, J.; Wadt, W. R. J. Chem. Phys. 1985, 82, 299-310.
(10) For a review on palladium peroxo complexes as intermediates in catalytic
reactions, see: Stahl, S. S. Angew. Chem., Int. Ed. 2004, 43, 3400-3420.
(11) (a) Grushin, V. V.; Alper, H. Organometallics 1993, 12, 1890-1901. (b)
Grushin, V. V.; Alper, H. Organometallics 1996, 15, 5242-5245. (c)
Amatore, C.; Carre´, E.; Jutand, A.; M’Barki, M. A.; Meyer, G. Organo-
metallics 1995, 14, 5605-5614. (d) Matos, K.; Soderquist, J. A. J. Org.
Chem. 1998, 63, 461-470.
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6830 J. AM. CHEM. SOC. VOL. 128, NO. 21, 2006