Alicia
Casitas
a,
Amanda E.
King
b,
Teodor
Parella
c,
Miquel
Costas
a,
Shannon S.
Stahl
*b and
Xavi
Ribas
*a
aDepartament de Química, Universitat de Girona, Campus de Montilivi, 17071, Girona, Catalonia, Spain. E-mail: xavi.ribas@udg.edu; Fax: +34-972418150; Tel: +34-972419842
bDepartment of Chemistry, University of Wisconsin-Madison, 1101 University Avenue, Madison, WI 53706, USA. E-mail: stahl@chem.wisc.edu; Fax: +1-608-262-6143; Tel: +1-608-265-6288
cServei de RMN, Facultat de Ciències, Universitat Autònoma de Barcelona, Campus UAB, Bellaterra, E-08193, Catalonia, Spain
First published on 15th June 2010
A series of aryl–copper(III)-halide complexes have been synthesized and characterized by NMR and UV-visible spectroscopy, cyclic voltammetry and X-ray crystallography. These complexes closely resemble elusive intermediates often invoked in catalytic reactions, such as Ullmann–Goldberg cross-coupling reactions, and their preparation has enabled direct observation and preliminary characterization of aryl halide reductive elimination from CuIII and oxidative addition to CuI centers. In situ spectroscopic studies (1H NMR, UV-visible) of a Cu-catalyzed C–N coupling reaction provides definitive evidence for the involvement of an aryl-copper(III)-halide intermediate in the catalytic mechanism. These results provide the first direct observation of the CuI/CuIII redox steps relevant to Ullmann-type coupling reactions.
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Fig. 1 (a) Synthesis of [aryl–CuIII-X]X complexes. Their X-ray structures are depicted in (b) 1Cl, (c) 1Br, (d) 1I and (e) 2Cl. The ellipsoid representation is at 50% probability. The hydrogen atoms and respective second halide counteranion are omitted for clarity. Selected bond lengths [Å] for 1Cl: Cu(1)–C(1) 1.908(3), Cu(1)–Cl(1) 2.455(2), Cu(1)–N(1) 1.972(3), Cu(1)–N(2) 2.037(3), Cu(1)–N(3) 1.971(3); for 1Br: Cu(1)–C(1) 1.914(3), Cu(1)–Br(1) 2.600(1), Cu(1)–N(1) 1.974(3), Cu(1)–N(2) 2.034(2), Cu(1)–N(3) 1.974(2); for 1I: Cu(1)–C(1) 1.905(3), Cu(1)–I(1) 2.900(1), Cu(1)–N(1) 1.972(2), Cu(1)–N(2) 2.017(2), Cu(1)–N(3) 1.968(2); for 2Cl: Cu(1)–C(1) 1.898(3), Cu(1)–Cl(1) 2.468(1), Cu(1)–N(1) 1.986(5), Cu(1)–N(2) 1.999(3), Cu(1)–N(3) 1.974(4). |
Electronic spectra for [aryl–CuIII-X]X species exhibit halide-to-metal charge transfer bands in the 360–640 nm range, and the energies of these bands vary systematically with the identity of the halide. The aryl–CuIII-Cl compounds (1Cl, 2Cl) show two bands centred at 369 and 521 nm, the aryl–CuIII-Br compounds (1Br, 2Br) at 399 and 550 nm, and the aryl–CuIII-I compounds (1I, 2I) at 422 and 635 nm. The red-shift observed in the bands upon changing from Cl− to Br− to I− is in agreement with the ligand-field strength of the halide ligands (Cl− > Br− > I−), indicating that the bands correspond to ligand-to-metal charge transfer (LMCT) electronic transitions.
The diamagnetic character of all aryl–CuIII-X species permitted their characterization by NMR spectroscopy. Diagnostic 1H NMR peaks are evident in the 4–5 ppm range corresponding to the benzylic protons, and the 13C NMR spectrum exhibits a distinctive low field resonance for the Cipso–CuIII at about 180 ppm.8 Indeed, NOESY (Nuclear Overhauser Effect Spectroscopy) and HMBC (Heteronuclear Multiple Bond Correlation) experiments reveal that the rigid structure found in the solid state is retained in solution (see ESI†).
Cyclic voltammetry (CV) measurements of the aryl–CuIII-X species show chemically reversible 1e− processes associated with the CuIII/CuII redox couple. The CuIII/CuIIE1/2 values for these complexes follow the trend E1/2Cl < E1/2Br < E1/2I, and the compounds bearing L2, with a secondary amine trans to the aryl ligand, exhibit E1/2 values 40–70 mV lower than the corresponding complexes bearing L1, with a tertiary amine in the trans position (see ESI†). Overall, the redox potentials for CuIII/CuII are substantially lower (up to 250 mV) than those measured previously for the corresponding perchlorate or triflate salts,8 indicating that halide coordination stabilizes the CuIII oxidation state.
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Fig. 2 (a) Acid-triggered quantitative aryl-X reductive elimination from aryl–CuIII-X at room temperature (counteranions omitted for clarity). (b) UV-vis monitoring of reductive elimination of complex [L1C–CuIII-Br]Br (1Br) upon addition of 1.5 equiv. of acid ([1Br] = 0.5 mM, [CF3SO3H] = 0.75 mM, CH3CN, 288 K). Inset shows decay profile at 420 nm (circles = experimental data, solid line = first-order theoretical fit). (c) Electrochemical (vs. SSCE, [complex] = 1 mM, scan rate = 0.2 V s−1, TBAPF6 0.1 M, CH3CN, 263 K) and kinetic data associated with aryl halide reductive elimination from aryl–CuIII-X species ([complex] = 0.5 mM, [CF3SO3H] = 0.75 mM, CH3CN, 253–283 K for 1Cl, 278–298 K for 1Br and 2Cl). (d) Proposed interaction of triflic acid with 1Br through weak axial coordination of the triflate anion to the CuIII center with concomitant protonation of the central amine. |
The reactions of 1Cl, 1Br and 2Cl were investigated in more detail by UV-visible spectroscopy. The kinetic profiles of the decay of the aryl–CuIII-X LMCT bands exhibited first-order behaviour, with rates following the trend: 1Cl > 2Cl > 1Br (Fig. 2b–c). Activation parameters obtained from Eyring analyses (Fig. 2c) reveal that the reductive elimination reactions exhibit a relatively large enthalpy of activation (21.5–23.2 kcal mol−1), consistent with significant Cu–X bond cleavage in the transition state. The reactions of 2Br, 1I and 2I were much slower, and systematic kinetic studies of these complexes were not performed. The aryl–CuIII-I compound 1I undergoes reductive elimination to afford (L1-I–H)+ in slightly lower yields (85%). The reaction of 2I requires extended reaction time (days), is complicated by side-reactions and (L2-I–H)+ is not observed. The faster rate of C–Cl reductive elimination from 1Cl relative to 2Cl is consistent with the higher reduction potential of 1Cl relative to 2Cl. In contrast, 1Br exhibits the slowest reductive elimination rate of the three complexes, despite having the highest reduction potential (Fig. 2c). The latter observation is amplified by the even-slower qualitative rates of C–I reductive elimination from 1I and 2I, which have the highest reduction potentials of the six aryl–CuIII-X compounds (E1/2 = −230 and −290 mV, respectively). Thus, the C–X reductive elimination rates do not correlate with the reduction potentials of the aryl–CuIII-X species across the halide series. Rather, these observations suggest that the trends in the rates of C–X reductive elimination are controlled by the relative carbon–halogen bond strengths: C–Cl > C–Br > C–I. A different trend has been observed for aryl carbon–halogen reductive elimination from PdII complexes, for which the relative rates kC–Br > kC–I > kC–Cl were measured.9
The mechanistic origin of the H+-triggered aryl-X reductive elimination event is not fully understood; however, electrochemical data indicate that CF3SO3H destabilizes the aryl–CuIII-X species. Cyclic voltammetry studies of 1Cl, 1Br and 2Cl in acetonitrile reveal that the CuIII/CuII reduction potential increases by 70–170 mV when CF3SO3H is present in solution (see ESI†). In addition, electronic absorption spectra of acidified solutions of these complexes show a 5 nm, 9 nm and 8 nm red-shift in the UV-visible bands, respectively, consistent with formation of new species. Our current hypothesis is that CF3SO3H protonates the central amine of the macrocyclic ligand, thereby destabilizing the CuIII oxidation state and facilitating C–X bond formation (Fig. 2d). The strong trans effect of the aryl ligand, as visualized in the larger CuIII–N(2) bond distances of all compounds, also is in agreement with a preferential protonation to the central amine. Preliminary experimental support for this hypothesis is available from 1H NMR spectroscopic studies of 1Br. Triflic acid (1.5 equiv) was added to a solution of 1Br in CD3CN at −30 °C. No aryl-Br reductive elimination was observed under these conditions; however, resonances corresponding to the N–CH3 group and the C–H protons of the adjacent methylene group undergo a noticeable upfield shift, while the other resonances remain essentially unchanged (see ESI†). We suspect that weak axial coordination of the triflate anion to the CuIII center, approaching from the face opposite to the halide, facilitates the protonation of the central amine (Fig. 2d).
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Fig. 3 (a) Reversible reductive elimination/oxidative addition induced by the presence of acid or base. (b) Monitoring of 1Br by UV-visible spectroscopy at 400 nm upon successive acid and base additions (initial conditions: [1Br] = 0.3 mM, addition of 2 equiv. of triflic acid and Proton Sponge® in the respective additions, CH3CN, 297 K). |
Reversible aryl halide oxidative addition to CuI is directly relevant to catalytic transformations. For example, Cohen and coworkers have provided kinetic evidence that the Ullmann coupling of o-bromonitrobenzene proceeds via reversible oxidative addition of aryl bromide to CuI in the first step of the mechanism.10 Copper(I) salts are also known to catalyze halogen exchange reactions with aryl halide substrates. In a noteworthy example reported recently by Buchwald and coworkers, CuI catalyzes the conversion of aryl bromides into aryl iodides in the presence of NaI.11
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Fig. 4 (a) Copper-catalyzed catalytic C–N bond forming reaction for the conversion of L1-Br and pyridone into 3·HBr at room temperature. (b) 1H NMR spectroscopic analysis of the Cu-catalyzed amination reaction: the catalytic resting state, aryl–CuIII-Br (1Br) is evident in the spectra obtained prior to t ∼ 120 min (for clarity only selected regions of the NMR spectrum are shown; full spectra are available in the ESI.† Conditions: [L1-Br] = 9 mM, [pyridone] = 10 mM, [CuI(CH3CN)4PF6] = 0.3 mM, CD3CN, 288 K). (c) Analysis of the catalytic reaction by UV-visible spectroscopy and the time-dependent progression of the absorbance at 542 nm (inset). Immediately upon mixing, the charge-transfer bands associated with 1Br are observed, and these features persist until most of the reaction is complete (same experimental conditions as in (b)). |
The aforementioned studies by Buchwald and Hartwig have provided evidence that, in reactions with bidentate nitrogen ligands, amide substrates react with CuI to form CuI-amidate intermediates prior to oxidative addition of the aryl halide. An alternative mechanistic possibility, as discussed in a recent review by Monnier and Taillefer,2c involves oxidative addition of the aryl halide, followed by reaction of the nucleophile with the aryl–CuIII intermediate. The results of the present study, together with previous observations of stoichiometric C–N coupling reactions,12 conform to the latter mechanism. It seems reasonable to expect that the mechanism of Ullmann–Goldberg-type coupling reactions will vary, depending on the identity of the substrates, ancillary ligand and/or the reaction conditions. Reactions involving nucleophiles that coordinate less readily to copper, or catalysts that feature higher-coordinate (e.g., tri- or tetradentate) ancillary ligands may disfavor pre-coordination of the nucleophile to CuI. In such cases, the reaction may proceed via a mechanism in which reaction of the aryl halide with CuI precedes that of the nucleophile. These issues will be important to address in future studies of Ullmann-type coupling reactions.
Footnote |
† Electronic supplementary information (ESI) available: Full experimental details for the synthesis, spectroscopic, and crystallographic characterization of 1X and 2X. Synthesis of reductive elimination L1-X and L2-X products. NMR and UV-vis monitoring of catalytic coupling of L1-Br with pyridone. Crystal data for 1Cl, 1Br, 1I, 2Cl and 2I. CCDC reference numbers 735508–735512. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c0sc00245c |
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