An Adaptable N-Heterocyclic Carbene Macrocycle Hosting Copper in Three Oxidation States.

A neutral hybrid macrocycle with two trans-positioned N-heterocyclic carbenes (NHCs) and two pyridine donors hosts copper in three oxidation states (+I-+III) in a series of structurally characterized complexes (1-3). Redox interconversion of [LCu]+/2+/3+ is electrochemically (quasi)reversible and occurs at moderate potentials (E1/2 =-0.45 V and +0.82 V (vs. Fc/Fc+ )). A linear CNHC -Cu-CNHC arrangement and hemilability of the two pyridine donors allows the ligand to adapt to the different stereoelectronic and coordination requirements of CuI versus CuII /CuIII . Analytical methods such as NMR, UV/Vis, IR, electron paramagnetic resonance, and Cu Kβ high-energy-resolution fluorescence detection X-ray absorption spectroscopies, as well as DFT calculations, give insight into the geometric and electronic structures of the complexes. The XAS signatures of 1-3 are textbook examples for CuI , CuII , and CuIII species. Facile 2-electron interconversion combined with the exposure of two basic pyridine N sites in the reduced CuI form suggest that [LCu]+/2+/3+ may operate in catalysis via coupled 2 e- /2 H+ transfer.

Introduction

Copper complexes attract significant interest because of their various applications as catalysts in organic transformations such as C−C/X bond formation and C−H bond activation reactions, and also for their involvement in biological oxidation and oxygenation processes.1, 2 These n class="Chemical">copper‐mediated reactions generally exploit oxidation state changes of the metal ion, and proposed mechanistic scenarios primarily involve the CuI/CuII or CuI/CuIII couples. However, in contrast to numerous examples of organometallic copper(I) and copper(II) complexes, organocopper(III) species have rarely been isolated and authenticated because of their limited stability.1d, 3, 4 The majority of recently reported organocopper(III) complexes are stabilized by anionic C/N‐based macrocycles, such as Ribas's4a triazamacrocycles, Wang's4b azacalix[1]arene[3]pyridines, Furuta's4c, 4d, 4i N‐confused porphyrins/corroles, and Srinivasan's4g biphenyl‐ embedded porphyrinoides (Figure 1 a). In all the aforementioned complexes, the formally CuIII ion adopts a square planar coordination geometry. However, the assignment of the physical oxidation states of copper—especially when ligated by redox non‐innocent ligands—should be considered with caution.5 For example, it was recently suggested that the formally 3d8 CuIII species [Cu(CF3)4]− features an inverted ligand field and that it is best described as having a 3d10 CuI electronic configuration.5a, 5b, 5d In such ambiguous cases, the combination of K‐edge X‐ray absorption spectroscopy (XAS) and theoretical calculations is a useful toolbox for assigning oxidation states.5, 6

Figure 1

Examples of previously reported organocopper(III) complexes.

Over the last decades, N‐heterocyclic carbenes (NHCs) have become one of the most popular ligand classes in organon class="Chemical">metallic chemistry and catalysis.7 As a consequence of their strong σ‐donating and variable π‐accepting abilities, NHCs are capable of supporting metal complexes in a range of oxidation states, and they are now emerging as useful scaffolds for the stabilization of 3d metal ion species in high oxidation states.8

NHC‐n class="Chemical">copper chemistry has developed rapidly since the first NHC‐CuI complex [(NHC)2Cu][OTf] was reported in 1993 by Arduengo.9, 10 To date, numerous examples of CuI complexes are known, and they usually adopt a linear geometry that is common to d10 coinage metal ions. In contrast, NHC‐ligated CuII complexes are much rarer,8 and a single NHC‐CuIII complex has been authenticated; the latter is based on a rigid tetra(N‐heterocyclic) carbene macrocycle (Figure 1 b) and is the only organocopper(III) complex of a neutral ligand reported to date.11

Most of the reported NHC‐n class="Chemical">CuII complexes require appended chelating N‐ or O‐donors, and they often contain anionic co‐ligands.12 The groups of K. Meyer and J. Long prepared two examples of CuII complexes with neutral N‐anchored tripodal tris(NHC) or NHC‐bridged polypyridyl ligands, respectively.13 Several computational studies suggested the existence of NHC‐CuIII species during carbene‐halide/aryl reductive elimination and oxidative coupling of carbenes,14 but such intermediates have so far eluded isolation. The seminal tetra(NHC)‐CuIII complex shown in Figure 1 b was synthesized by a disproportionation reaction starting from the corresponding tetra(imidazolium) salt and Cu2(OAc)4, and it shows the square planar coordination geometry expected for a low‐spin d8 ion.11 However, details on its electronic structure and valence state were not reported. Furthermore, in this case, as well as in most CuIII systems reported to date, the drastically different coordination geometry preferences for CuI versus CuII and CuIII prevented any reversible redox shuttling between the different oxidation states, because redox changes are usually accompanied by major structural changes. Accordingly, the CuI complex of Kühn's tetra(NHC) macrocycle, obtained when using CuOAc as the copper source, exhibits a tetranuclear structure composed of two tetra(NHC) ligands and four linearly coordinated CuI ions.11

To circumvent major structural rearrangements or changes in nuclearity during redox interconversion and allow for isolation of the n class="Chemical">Cu‐NHC system in three oxidation states from CuI to CuIII, we have exploited the concept of ligand hemilability in a macrocyclic NHC/pyridine hybrid scaffold. This system can adapt to the different metal ion coordination environments required (Figure 1 b). A number of bi‐, tri‐, tetra‐, and penta‐dentate cyclic or acyclic NHC/pyridine hybrid ligands have previously been introduced in organometallic chemistry,7c, 13b, 15 as these may favorably combine the strong σ‐donor properties of NHCs with the relatively weak σ‐N‐donor character of pyridine groups. Among them, the macrocyclic ligand derived from [H2L][PF6]2 (Scheme 1) with two trans disposed NHC moieties and two pyridine moieties has been utilized for the synthesis of NiII and FeII complexes.15a, 15d The latter can be further oxidized to the corresponding FeIII congener, indicating the ability of this ligand to stabilize higher valent metal complexes.

Scheme 1

Synthesis of the CuI, CuII, and CuIII complexes of the NHC/pyridine hybrid macrocycle L.

Synthesis of the CuI, n class="Chemical">CuII, and CuIII complexes of the NHC/pyridine hybrid macrocycle L.

Herein we report a series of copper complexes in oxidation states +I, +II, and +III that can be (quasi)reversibly interconverted at moderate potentials. The n class="Chemical">copper ion is hosted within the neutral macrocyclic bis(NHC)‐bis(pyridine) ligand framework (L) throughout the series, and a suite of experimental methods (XRD, variable‐temperature (VT) NMR, XAS, absorption, superconducting quantum interference device (SQUID) magnetometry, and electron paramagnetic resonance (EPR) spectroscopy), as well as DFT calculations, have been employed to elucidate the geometric and electronic structures of the three complexes. To the best of our knowledge, this is the first system that can stabilize copper complexes in all three relevant oxidation states (+I, +II, and +III) within a single host scaffold, and without undergoing major structural changes.

Results and Discussion

Copper(I) complex and its dynamics. The n class="Chemical">copper(I) complex [LCu][PF6] (1) can be readily synthesized via two independent routes with good isolated yields (ca. 66 %). The complex is obtained either by reaction of the bis(imidazolium) salt [H2L][PF6]2 with mesitylcopper (MesCu, 2.0 equiv) in acetonitrile (MeCN) or by initial deprotonation of [H2L][PF6]2 with K[N(SiMe3)2] (2.0 equiv) followed by treatment with [Cu(NCMe)4][PF6] (1.0 equiv) in MeCN (Scheme 1). A yellow precipitate is generated in both reactions after long periods of reaction (1 week). 1 is isolated as a yellow powder after simple filtration. The electrospray ionization mass spectrum (ESI‐MS) of a MeCN solution of this yellow powder is dominated by a peak at m/z=405.1 amu characteristic for the cation [LCu]+ (Supporting Information, Figure S10), supporting the formation of the desired product [LCu][PF6].

At room temperature, complex 1 is stable both in the solid state and in MeCN solution under an inert atmosphere. However, it slowly decomposes in n class="Chemical">MeCN solution under air, as evidenced by UV/Vis monitoring (Figure S6). Interestingly, slow diffusion of Et2O into a saturated MeCN solution of the crude yellow powder yields not only the mononuclear complex 1 as yellow crystals in a large amount, but also a few colorless crystals of a different compound that turned out to be the dinuclear complex [L2Cu2][PF6]2 (1′). The structures of both 1 and 1′ were determined by X‐ray diffraction and are depicted without their anions in Figure 2 and Figure S2, respectively. In the minor product 1′, two macrocycles L are bridged by two CuI ions that are both ligated linearly by two NHC donors from the different ligands. This structural motif has previously been seen for the silver(I) and gold(I) analogues, [L2Ag2][PF6]2 16 and [L2Au2]Br2,17 and resembles the structure of a dinuclear copper(I) complex [LPh‐NHC 2Cu2][PF6]2 with a related bis(NHC) macrocycle lacking additional pyridine N donors.18 When dissolved in MeCN or acetone, 1′ immediately converts into the monomeric form 1, even at low temperatures, as evidenced by 1H NMR and ESI‐MS analysis (Supporting Information). This suggests a fast equilibrium between 1 and 1′ in solution that lies far on the side of mononuclear 1 in the above polar solvents.

Figure 2

a) Molecular structures of 1 (left, upside view; right, frontside view), b) 2, and c) 3 (only one of the two crystallographically independent molecules in the asymmetric unit is shown), with 50 % probability ellipsoids. Hydrogen atoms, lattice solvent (MeCN), and anions are omitted for clarity. Selected atom distances and angles of 1, 2, and 3 are listed in Table 1.

a) Molecular structures of 1 (left, upside view; right, frontside view), b) 2, and c) 3 (only one of the two crystallographically independent molen class="Chemical">cules in the asymmetric unit is shown), with 50 % probability ellipsoids. Hydrogen atoms, lattice solvent (MeCN), and anions are omitted for clarity. Selected atom distances and angles of 1, 2, and 3 are listed in Table 1.

In the major product 1, the metal ion is hosted within the macrocyclic cavity and is bound to the two n class="Chemical">NHC donors in a quasi‐linear geometry (CNHC‐Cu‐CNHC: 169.6(1)°). The Cu−CNHC bond lengths of 1.939(2) Å and 1.946(2) Å agree with reported values for CuI−NHC complexes.11, 19, 20 The two pyridine rings adopt a near‐orthogonal orientation with respect to the plane defined by the two CNHC and the two pyridine N atoms, with interplanar angles of 78.6(1)° and 69.7(1)°, respectively. Furthermore, the distances between the pyridine N atoms and the central CuI ion (2.496(2) Å and 2.706(2) Å) are substantially longer than the Cu⋅⋅⋅Npy distances in other reported NHC‐CuI complexes with ancillary pyridine donors,21 though comparable to those in [(ItBuCNC)2Cu2][PF6]2 (2.422(2)–2.830(2) Å; ItBuCNC is a tridentate pyridine‐bridged dicarbene ligand);22 the Npy⋅⋅⋅Cu⋅⋅⋅Npy angle in 1 is 164.5(1)°. These structural features indicate weak interactions at best, in accordance with the preference of linear geometry of CuI−NHC complexes. However, weak Cu⋅⋅⋅py interactions may contribute to the predominance of the monomeric species 1 (see proceeding text) and the deviation of the CNHC‐Cu‐CNHC angle (169.6°) from linearity.

The mononuclear structure of 1 contrasts with the structures of the corresponding AgI and AuI complexes of the hybrid macrocycle L, and the CuI complex of a related macrocycle lacking the n class="Chemical">pyridine N donors, which were shown to exist as dinuclear or even tetranuclear ([L2Ag4][PF6]4) complexes in the solid state, with linearly coordinated metal ions bound to NHC or pyridine donors from two different macrocycles.16, 17, 18, 23 Dinuclear or tetranuclear structural motifs ([LNHCCu2]I2,20 [LNHC 2Cu4][PF6]4 11) have also been observed for copper(I) complexes of macrocyclic tetracarbene ligands. In iron complexes [LFeII(NCMe)2][PF6]2 15d and [LFeIII(NCMe)2][PF6]3,15d as well as in the nickel complex [LNiII]Br2,15a the macrocyclic ligand L binds as a typical tetradentate CNHC 2Npy 2 donor with the Fe−Npy and Ni−Npy bonds along the planes of the pyridine rings; the macrocycles are severely puckered and trans‐located imidazol‐2‐ylidene rings are twisted with respect to each other. In complex 1, the two imidazol‐2‐ylidene rings are almost coplanar (Figure 2 a).

In agreement with the crystallographic structure and the proposed weak interaction of the pyridyl groups with the metal center, the n class="Chemical">15N NMR resonance of Npy in 1 is shifted only slightly to lower field (−67.5 ppm) compared to the ligand precursor [H2L][PF6]2 (−77.6 ppm). The 13C NMR spectrum exhibits a down‐field shift of the signal for the carbene C from 153.9 ppm in [H2L][PF6]2 to 177.4 ppm in 1, which is characteristic of NHC‐CuI complexes.11, 20, 21 However, the simplicity of the room‐temperature 1H NMR spectrum of 1 (in [D3]MeCN), displaying a singlet at 5.20 ppm for the macrocyclic CH2 linkers and one set of signals for the pyridyl rings, suggests a highly dynamic behavior in solution with apparent D 2 symmetry of the complex on the NMR timescale. We attribute this to a flipping of the pyridyl rings via a process in which these rings become coplanar with the macrocyclic core and the Cu⋅⋅⋅NPy vector. DFT computations indicate such a conformation in which one of the pyridine rings has become coplanar with the macrocycle, reflecting the pyridine ring flip, to be only 8.2 kcal mol−1 higher in energy (Figure S47).

Similar diffusion coefficients of the imidazolium salt n class="Chemical">[H2L][PF6]2 (D 298K=1.05×10−9 m2 s−1) and 1 (D 298K=1.17×10−9 m2 s−1) derived from 1H diffusion ordered spectroscopy (DOSY) experiments support that the complex remains mononuclear with a 1:1 metal:ligand ratio in solution. The dynamic behavior of 1 in solution was probed by VT 1H NMR experiments in [D6]acetone (Figure 3; Figures S39,S40). Upon decreasing the temperature, signals arising from the pyridine groups and the imidazol‐2‐ylidene backbone shift slightly to lower and higher field, respectively (Figure S39), and become broad at −80 °C. The peak for the CH2 linkers exhibits a significant down‐field shift (Δδ=0.23 ppm) that begins to broaden at −50 °C and finally splits into a pair of apparent doublets at −80 °C (coalescence temperature T c=−62 °C, ΔG ≠=9.5 kcal mol−1), with a coupling constant of J ab=13.6 Hz that is typical for geminal coupling (Figure 3; Figure S40). This suggests that flipping of the pyridyl rings becomes slow on the NMR timescale at low temperatures. The activation energy (E a=17.8 kcal mol−1) and parameters (ΔH ≠=17.4 kcal mol−1 and ΔS ≠=37.2 cal mol−1 K−1) for this process were derived from Arrhenius and Eyring analyses of the VT NMR data (Figures S44,S45). The possible C 2 and C 2 symmetric isomers of 1 (with the two pyridine rings directed towards the same or opposite sides, respectively) are almost isoenergetic according to DFT calculations (Figure S47); broadening of all 1H NMR signals at low temperatures may reflect the presence of both isomers exhibiting very similar NMR shifts.

Figure 3

VT 1H NMR spectra for 1 in [D6]acetone (only regions 5.0–6.3 ppm and 6.8–8.5 ppm are shown for clarity).

VT 1H NMR spectra for 1 in n class="Chemical">[D6]acetone (only regions 5.0–6.3 ppm and 6.8–8.5 ppm are shown for clarity).

In contrast, the 1H NMR spectra of related n class="Chemical">iron(II) and nickel(II) complexes in which L binds as a tetradentate CNHC 2Npy 2 ligand, [LFeII(NCMe)2][PF6]2 15d and [LNiII]Br2,15a reveal a pair of doublets for the CH2 linkers at room temperature because of restricted flexibility of the puckered macrocycle. Compared with activation parameters for the conformational ring inversion in [LFeII(NCMe)2][PF6]2 (ΔH ≠=15.1 kcal mol−1, ΔS ≠=−4.7 cal mol−1 K−1)15d or in [LaFe(CH3CN)][PF6]2 (La=acyclic tetradentate bis(NHC)‐bis(pyridine) ligand; ΔH ≠=14.4 kcal mol−1, ΔS ≠=−0.2 cal mol−1 K−1),24 the large and positive activation entropy in case of complex 1 indicates a different dynamic process with a more disordered transition state, which is attributed to the pyridyl ring flip. Complex [LNiII]Br2 with square planar coordination geometry of the low‐spin d8 nickel(II) shows a stationary puckered conformation and no ring inversion dynamics on the NMR timescale, even at 80 °C.15a

Redox Properties and (Spectro)electrochemistry. The redox properties of 1 were examined by electrochemical methods. Cyclic voltammetry (CV) of 1 in MeCN reveals two redox events at potentials of −0.45 V and +0.82 V (E 1/2, vs. Fc/Fc+, Figure 4) assigned to the n class="Chemical">CuI/CuII and CuII/CuIII couples, respectively. The second process is reversible, as judged by the linear dependence of the current on the square root of the scan rate (Randles–Sevcik equation), the similar peak currents of forward and reverse scans (I rp/I fp=0.92), and the peak‐to‐peak separation (ΔE p=80 mV) that is very similar to that of the Fc/Fc+ couple (ΔE p=76 mV) under the same conditions (Supporting Information). ΔE p for the CuI/CuII couple is slightly larger (ΔE p=124 mV, I rp/I fp=0.86), likely because it involves some more significant reorganization associated with the movement of the pyridine rings and a planarization of the structure upon oxidation to CuII. For comparison, the copper complexes [Cu(I(R)CNC)][PF6] (where I(R)CNC is a pincer‐type bis(NHC)pyridine ligand; R=Me, Et, and iPr)21b and [(TIMEN)Cu][PF6]13a (TIMEN is a N‐anchored tripodal tetradentate tris(NHC) ligand) showed reversible CuI/CuII couples at much higher potential (E 1/2 in the range +0.02–+0.11 V vs. Fc/Fc+), while a macrocyclic tetra(NHC) ligand (Figure 1 b) leads to an irreversible CuI/CuII couple at very negative potential (cathodic peak potential −1.14 V at 100 mV s−1; vs. Fc/Fc+) and an only partially reversible CuII/CuIII couple at E 1/2=−0.75 V (vs. Fc/Fc+).11 Notably, the CuII/CuIII potential of complex 1 is higher than that of many previously reported CuII or CuIII complexes with ancillary anionic N‐ or C‐donor ligands.4a, 4f, 4i The mostly reversible redox behavior of 1 indicates that the macrocyclic NHC‐pyridine hybrid ligand L has sufficient structural and electronic flexibility to accommodate copper in all three oxidation states from CuI to CuIII.

Figure 4

Cyclic voltammogram (100 mV s−1) of complex 1 in MeCN (0.1 m [nBu4N][PF6]) at room temperature.

Cyclic voltammogram (100 mV s−1) of complex 1 in MeCN (0.1 m n class="Chemical">[nBu4N][PF6]) at room temperature.

The sequential oxidation of 1 to the CuII (2) and n class="Chemical">CuIII (3) species yielded characteristic electronic absorption changes as probed by UV/Vis spectroelectrochemistry (UV/Vis‐SEC; Figure 5). The UV/Vis spectrum of complex 1 shows two prominent bands at 280 nm (ϵ=13 600 m −1 cm−1) and 340 nm (ϵ=5000 m −1 cm−1) that can be assigned to CuI→ligand charge transfer transitions (metal‐to‐ligand, MLCT) based on time‐dependent density functional theory (TD‐DFT) calculations (B3LYP/tzvp; Figures S5,S48; Supporting Information, Table S5; calculated λ max(calc)=271 nm and 374 nm). Upon bulk oxidation at 0.8 V (vs. Ag wire), both absorptions at 280 and 340 nm of 1 vanish and two lower intensity bands at 370 nm (shoulder, ϵ=220 m −1 cm−1) and 490 nm (ϵ=120 m −1 cm−1) emerge corresponding to the CuII complex formation. This is in line with the observed color change from yellow to red. A clear isosbestic point at 440 nm indicates a single‐step conversion without intermediate step(s). The 370 nm feature of 2 largely originates from a ligand→ CuII(d ) charge transfer (ligand‐to‐metal, LMCT) and the 490 nm feature is from a CuII based d–d transition (dyz→d ), based on the TD‐DFT results (Figure S49, Table S6; λ max(calc)=335 nm and 452 nm). Upon further electrolysis at 1.5 V (vs. Ag wire), absorptivity increases and the two bands of in‐situ‐generated 2 are replaced by three more intense bands at 300, 350, and 530 nm, which is indicative of formation of the CuIII complex 3 and consistent with a color change from red to dark‐red. TD‐DFT calculations assign all these three bands as ligand→CuIII charge transfer transitions (LMCT; Figure S50, Table S7; λ max(calc)=310, 376, and 512 nm). All spectral changes are fully reversible upon re‐reduction. The results of the (spectro)electrochemical studies suggest that preparation of the oxidized copper complexes by chemical bulk oxidation, and their isolation, should be feasible.

Figure 5

UV/Vis (spectro)electrochemistry showing the continuous oxidation of a) 1 to 2 (at 0.8 V vs. Ag wire; 1 (black), 2 (red); the inset shows a magnified view of the 330–600 nm range) and b) from 2 to 3 (at 1.5 V vs. Ag wire; 2 (red), 3 (blue)) in an MeCN solution containing 0.1 m [nBu4N][PF6]. The isosbestic point is marked with an asterisk.

UV/Vis (spectro)electrochemistry showing the continuous oxidation of a) 1 to 2 (at 0.8 V vs. Ag wire; 1 (black), 2 (red); the inset shows a magnified view of the 330–600 nm range) and b) from 2 to 3 (at 1.5 V vs. Ag wire; 2 (red), 3 (blue)) in an MeCN solution containing 0.1 m n class="Chemical">[nBu4N][PF6]. The isosbestic point is marked with an asterisk.

Copper(II) complex. Using n class="Chemical">[Cp2Fe][PF6] as oxidant, the CuII complex [LCu][PF6]2 (2) is readily obtained as a red solid in high yield (ca. 86 %) (Scheme 1). An ESI mass spectrum of a MeCN solution of this red solid shows dominant peaks at m/z=550.1 amu and 202.2 amu, which are characteristic of the monocation [LCu(PF6)]+ and the dication [LCu]2+, respectively (Figure S11). Complex 2 is insensitive to air and moisture over prolonged times, both in solution and in the solid state.

Red block crystals of 2 were obtained by slow diffusion of Et2O into a saturated n class="Chemical">MeCN solution of the crude material. The molecular structure of the cation of 2 shows that the CuII ion is five coordinate in the solid state with the tetradentate L establishing a square planar donor environment (C2N2 donor set, sum of angles around Cu is 358.0°) and a MeCN ligand occupying an apical position at rather long distance d(Cu−NMeCN)=2.321(3) Å, as expected for a Jahn–Teller d9 ion (Figure 2 b). IR spectroscopy of a solid sample of 2 that was kept under vacuum overnight indicated that the MeCN is weakly bound and readily lost, in accordance with the combustion analysis of the dried product.

The overall coordination environment of the n class="Chemical">CuII ion in 2 is best described as a slightly distorted square pyramid with τ 5=0.016 (close to the τ 5 value of 0 for an ideal square pyramid).25 Trans angles CNHC‐Cu‐CNHC and Npy‐Cu‐Npy within the basal plane are 168.4(1)° and 169.8(1)°, respectively, and the displacement of the copper ion out of the basal plane is only 0.192(1) Å. Cu−CNHC bonds in 2 (1.907(3) Å and 1.909(3) Å) are clearly shorter than in 1 (1.939(2) Å and 1.946(2) Å), which is consistent with the expectation that the increased electron deficiency of the metal center enhances its interaction with the carbene donors. Cu−CNHC bonds in 2 are at the short end of Cu−C bond lengths of known CuII−NHC complexes (1.89–2.52 Å).26 Oxidation of 1 to 2 yields dramatically shortened Cu−Npy distances (2.155(2)/2.157(3) Å) that are comparable to those of reported five‐coordinate CuII complexes with chelating NHC‐pyridine ligands (2.12–2.21 Å).26 This leads to a puckered macrocycle with a saddle‐like shape and approximate C 2 symmetry in solid 2, featuring dihedral angles between opposing imidazol‐2‐ylidene rings and pyridyl rings of 56.1(2)° and 50.1(1)°, respectively. This is reminiscent of the conformations the macrocyclic ligand L adopts in the six‐coordinate iron complexes [LFeII(NCMe)2][PF6]2 and [LFeIII(NCMe)2][PF6]3, as well as in the four‐coordinate nickel complex [LNiII]Br2.15a, 15d

SQUID magnetometry of a solid sample of 2 (Figure S15) shows an almost constant χ Μ  T value of 0.44 cm3 mol−1 K (corresponding to μ eff=1.88 μB) over a wide temperature range from 12 to 295 K, as expected for an S=1/2 system with some orbital contributions (g iso=2.17). The X‐band EPR spectrum of 2 in n class="Chemical">MeCN recorded at 298 K displays a nearly isotropic pattern with obvious 63/65Cu (I=3/2) and 14N (I=1) hyperfine splitting (Figure 6). The signal could be well simulated with approximately equal g factors (g 1=2.077, g 2=2.079, g 3=2.057),27 large A Cu (up to 157×10−4 cm) and coupling with two 14N atoms (A N av=20×10−4 cm), suggesting that the unpaired spin resides partly on the ligand L. This is corroborated by DFT calculations which, as expected, show that the singly occupied orbital is antibonding and has large Cu(d ) character with some Npy(py) and CNHC(px) contributions (Figure S51). Calculated spin densities on Cu and on each pyridine N are 60 % and 10 %, respectively (Figure 6). The X‐band EPR spectrum of 2 measured in frozen MeCN solution at 147 K exhibits a broad rhombic signal with approximate g‐values [2.25, 2.12, 2.00] but without resolvable Cu hyperfine splitting (Figure S14). The rhombic character of the g‐tensor is indicative of mixing of the d into the d ground state for C 2 symmetry.28 The paramagnetism of the complex and unfavorable relaxation properties of CuII ions preclude any NMR spectroscopic characterization.

Figure 6

a) EPR spectrum of 2 recorded in MeCN solution at 298 K (black line) and a simulation (S= ; g 1=2.077, g 2=2.079, g 3=2.057; A_Cu1=424 MHz, A_Cu2=388 MHz, A_Cu3=470 MHz; A_N1=60 MHz, A_N2=65 MHz, A_N3=57 MHz; full width at half maximum (FWHM)=13.3 G (red line). b) Overall Löwdin spin population of 2 (isodensity value 0.08 au). Color code: C (gray), N (blue), Cu (red).

a) EPR spectrum of 2 recorded in MeCN solution at 298 K (black line) and a simulation (S= ; g 1=2.077, g 2=2.079, g 3=2.057; A_n class="Chemical">Cu1=424 MHz, A_Cu2=388 MHz, A_Cu3=470 MHz; A_N1=60 MHz, A_N2=65 MHz, A_N3=57 MHz; full width at half maximum (FWHM)=13.3 G (red line). b) Overall Löwdin spin population of 2 (isodensity value 0.08 au). Color code: C (gray), N (blue), Cu (red).

Copper(III) complex. The n class="Chemical">CuII complex 2 can be further oxidized using [(2,4‐Br2‐C6H3)3N][SbF6] (a derivative of “Magic Blue” with E o′=+1.14 V vs. Fc/Fc+ in MeCN)29 as the one‐electron oxidant to give diamagnetic [LCu][PF6]2[SbF6] (3) as a dark‐red crystalline solid in moderate yield (ca. 60 %). At room temperature, 3 is stable both in solution and in solid state under inert atmosphere, but it gradually decomposes under aerobic conditions (Figure S7). Its ESI mass spectrum shows major peaks characteristic of 1 and 2, which possibly arise from the reduction of 3 during the electrospray ionization process.

Dark‐red crystals of 3 were obtained by slow diffusion of Et2O into a saturated n class="Chemical">MeCN solution of the crude material and were subjected to X‐ray diffraction. Two crystallographically independent but similar molecules were found in the asymmetric unit, representing enantiomers in different conformations (Figure S4); one of them is shown in Figure 2. The molecular structure of the trication of 3 in solid state is very similar to that of the dication of 2 (Figure 7 overlay). This suggests a very low reorganization energy for the 1 e− transfer when shuttling between 2 and 3, which is in accordance with the CV data. Oxidation of 2 leads to a significant further shortening of the Cu−CNHC (1.875(4)/1.880(4) Å) and Cu−Npy bonds (1.972(3)–1.974(3) Å) in 3 (Table 1), reflecting the removal of an electron from the antibonding d orbital. The Cu−CNHC bond lengths in 3 are comparable with those reported recently for the tricationic tetra(NHC)‐CuIII complex [LNHCCu][OTf]3 (1.879–1.884 Å; Figure 1 b).11 The apical Cu−NMeCN distance of 2.325(4) Å in 3 is almost unchanged from 2 (2.321(3) Å), but the MeCN ligation is more bent (angle Cu‐NMeCN‐CMeCN: 160.7(4)° in 3 vs. 173.8(3)° in 2). The invariant Cu−NMeCN bond length suggests that the interaction with the apical MeCN ligand is electronically insignificant, and that electronic changes upon oxidation of 2 to 3 occur within the basal plane. Similar to 2, the weakness of the apical interaction leads to facile removal of the MeCN when 3 is kept under vacuum, which is evidenced by IR spectroscopy and elemental analysis of a dried sample (Figure S8).

Figure 7

Overlay of the cations of 2 (red) and 3 (blue) with similar conformations.

Table 1

Selected atom distances (Å) and angles (°) of 1, 2, and 3 obtained from the crystallographic analyses.

Complexes	Cu−C1	Cu−C11	Cu−N1	Cu−N4	Cu−N7	C1‐Cu‐C11	N1‐Cu‐N4	C21‐N7‐Cu
1	1.939(2)	1.946(2)	2.706(2)	2.496(2)		169.62(8)	164.49(5)
2	1.909(3)	1.907(3)	2.157(3)	2.155(2)	2.321(3)	168.42(13)	169.83(9)	173.8(3)
3	1.880(4)	1.875(4)	1.974(3)	1.972(3)	2.325(4)	173.36(17)	173.14(13)	160.7(4)
3′ [a]	1.868(4)	1.868(4)	1.964(3)	1.974(3)	2.315(4)	172.55(17)	172.25(13)	165.9(4)

[a] The conformational enantiomer of 3 in the crystal unit.

The diamagnetism of 3 is reflected by sharp 1H NMR signals in the normal range (0–9 ppm in n class="Chemical">[D3]MeCN). All peaks of 3 are dramatically shifted to lower field compared to those of 1, in line with the electron‐deficient nature of the CuIII center. In contrast to 1, however, the CH2 linkers of the macrocyclic ligand show an AB spin system at room temperature where the central peaks are no longer resolved but the small outer peaks are still visible; the central peak evolves into two strongly coupled doublets (J ab=17.0 Hz, ν ab/J ab<1) at lower temperatures (Figure 8; Figure S46; coalescence temperature T c=4 °C). In [D6]acetone, the CH2 linkers give rise to two apparent doublets at room temperature (J ab=16.8 Hz, ν ab/J ab=4.3; Figure 8). This indicates a more rigid macrocyclic skeleton in 3 compared to 1. Any dynamics of the puckered conformation in solution are slow on the NMR timescale, as was observed for [LNiII]Br2,15a which also reflects the shortened Cu−N/C bonds. As a consequence of the temperature limitation of the solvent and the instability of 3 at a higher temperature (it decomposes quickly at 50 °C in [D6]acetone), attempts to observe dynamic behavior and to derive reliable activation parameters from NMR spectroscopy were unsuccessful. The substantial high‐field shift of the 15N NMR resonance for the Npy atoms in complex 3 (−171.0 ppm) compared to −77.6 ppm for [H2L][PF6]2 and −67.5 ppm for 1 indicates a strong interaction of the pyridine donors with the oxidized metal ion. Remarkably, the 13C NMR signal for the imidazol‐2‐ylidene C2 atoms of 3 is shifted to a rather high‐field value (151.8 ppm), which is similar to what has been reported for the macrocyclic tetra(NHC) ligated CuIII (149.4 ppm) and AuIII complexes (ca. 146 ppm).11, 30 The diffusion coefficient of 3 (D 298K=9.14×10−10 m2 s−1, determined by 1H DOSY) is similar to those of 1 and the imidazolium salt [H2L][PF6]2, suggesting that the mononuclear structure is retained in solution.

Figure 8

1H NMR spectra of complex 3 in [D3]MeCN (top, 25 °C; middle, −40 °C) and [D6]acetone (bottom, 25 °C). Only regions 5.6–6.7 ppm and 7.4–9.0 ppm are shown for clarity. Inset: magnified range 5.8–6.1 ppm for 3 in [D3]MeCN at 25 °C.

1H NMR spectra of complex 3 in n class="Chemical">[D3]MeCN (top, 25 °C; middle, −40 °C) and [D6]acetone (bottom, 25 °C). Only regions 5.6–6.7 ppm and 7.4–9.0 ppm are shown for clarity. Inset: magnified range 5.8–6.1 ppm for 3 in [D3]MeCN at 25 °C.

Oxidation State Assignments. The redox non‐innocent character of many macrocyclic ligands used in previously reported formal CuIII complexes, such as n class="Chemical">carbaporphyrins and corroles (Figure 1 a),4e, 31 lends some ambiguity to the metal oxidation state assignments. Hence, the electronic structure of 3 was examined computationally as well as by XAS. Ground state DFT calculations suggest that 3 is best described as a closed shell singlet CuIII system with the triplet state being 25.2 kcal mol−1 higher in energy; broken‐symmetry calculations revealed the antiferromagnetically coupled open‐shell S=0 state to be even more unfavorable (Table 2; Table S8). Furthermore, both the calculated Cu−N/C bond distances after geometry optimization (Table 2), and the calculated UV/Vis spectrum (Figure S50) match the experimental data best for the closed shell singlet CuIII configuration. The lowest unoccupied molecular orbital (LUMO) of 3 is antibonding with significant Cu(d ) character, which is consistent with the removal of one electron from the singly occupied molecular orbital (SOMO) of 2, whereas the highest occupied molecular orbital (HOMO) to HOMO‐8 of 3 are mainly ligand‐centered orbitals with less than 4 % percent of Cu(d) contributions (Figure S52, Table S9).

Table 2

Comparison of the selected bond distances (Å) and relative single‐point energies (kcal mol−1) obtained from the optimized geometries of 3 at different spin states (closed shell singlet state and triplet state); BS (broken‐symmetry state) (1,1) at +26.6 kcal mol−1 (Supporting Information).

Complex	3 (S=0)	3 (S=1)	3 (Exp.)
Cu−C	1.8872/1.8874	1.9106/1.9104	1.867(4)–1.880(3)
Cu−NPy	2.0204/2.0201	2.2058/2.2061	1.965(3)–1.974(3)
Cu−NMeCN	2.3293	2.1730	2.315(3)/2.326(4)
E rel	0	25.2	–

Cu−n class="Gene">NPy

Cu−n class="Chemical">NMeCN

–

To corroborate the oxidation state assignments of the copper complexes of L reported herein, and specifically the n class="Chemical">CuIII character of 3, Cu Kβ high‐energy‐resolution fluorescence detection (HERFD) XAS was performed for the series of complexes 1–3. This detection technique records the Cu K‐edge absorption spectrum by monitoring a 3p→1s fluorescence signal with a large, high‐resolution emission spectrometer (ca. 1 eV resolution). The resultant narrower absorption linewidth is determined by the longer 3p core–hole lifetime, as opposed to the shorter 1s core–hole lifetime in traditional XAS measurements.

The Cu Kβ HERFD‐XAS of 1 reveals two sharp features at 8981.8 and 8984.8 eV (Figure 9). These lowest energy, intense transitions beginning at approximately 8982 eV are consistent with the d10 electronic configuration of n class="Chemical">CuI, where the first Cu K‐edge transitions correspond to dipole‐allowed 1s→4p transitions. The reduced local symmetry of the CuI center (where the z axis is along the CNHC−Cu−CNHC direction) lifts the degeneracy of the Cu 4p orbital energies. The first peak is assigned as the Cu 1s→4p with predominant CNHC(p) and Cu(p) character from an unoccupied C−Cu π‐like orbital (Figure S53). The higher energy feature corresponds to the Cu 1s→4p transitions of the orthogonal C−Cu π‐like interaction, with contributions from the pyridine σ (p) orbitals (Figure S53).

Figure 9

a) Cu Kβ HERFD‐XAS of 1–3 (up, solid lines). Inset: TD‐DFT‐calculated pre‐edge spectra of 2 and 3 (dashed lines). Each calculated pre‐edge consists of a single transition, broadened by 1.4 eV (FWHM). b) The transition difference density plots for each pre‐edge transition of 2 and 3 (bottom) are shown with isodensity value=0.003 au. Color code: C (gray), N (blue), Cu (red), hydrogen atoms omitted. Calculations shifted by +188.55 eV.

a) Cu Kβ HERFD‐XAS of 1–3 (up, solid lines). Inset: TD‐DFT‐can class="Chemical">lculated pre‐edge spectra of 2 and 3 (dashed lines). Each calculated pre‐edge consists of a single transition, broadened by 1.4 eV (FWHM). b) The transition difference density plots for each pre‐edge transition of 2 and 3 (bottom) are shown with isodensity value=0.003 au. Color code: C (gray), N (blue), Cu (red), hydrogen atoms omitted. Calculations shifted by +188.55 eV.

The Cu Kβ HERFD‐XAS of 2 is dramatically different from the spectrum of 1 (Figure 9); the intense dipole‐allowed transitions are gone in the spectrum of 2 and the rising edge is shifted to higher energy, reflecting a deeper 1s electron binding energy of the higher oxidation state. At 8979.5 eV, a weak pre‐edge feature is observed corresponding to a dipole‐forbidden 1s→3d transition into the single d electron–hole of the d9 n class="Chemical">CuII center.6b, 32

The most oxidized complex, 3, possesses the highest energy absorption edge—indicative of CuIII. A weak pre‐edge feature is observed at 8981.3 eV for 3, which is approximately 1.8 eV higher than the established n class="Chemical">CuII pre‐edge energy of 2 and consistent with previous reports for CuIII complexes.6b Furthermore, the observed shifts in the whiteline energies for 1, 2, and 3, at approximately 8994, 8996.5, and 9000 eV, respectively, are consistent with the increasing copper oxidation state.

TD‐DFT calculations of the n class="Chemical">Cu pre‐edge features of 2 and 3 each show a single transition into a predominantly d unoccupied orbital, as evidenced by the transition difference density plots (Figure 9). These calculations (using the PBE0 functional and def2‐TZVP basis set) reproduce the relative energies of the pre‐edges well, with the CuIII pre‐edge predicted to be 1.81 eV higher in energy than the CuII analogue.

Conclusion

In this study, we have shown that the bis(NHC)‐bis(n class="Chemical">pyridine) hybrid macrocycle L is capable of accommodating copper in three sequential oxidation states, from +I to +III. Structural characterization of the complexes [LCu]+/2+/3+ (1–3) evidences hemilability of the two pyridine donors, which allows the ligand to adapt to the very different stereoelectronic requirements and coordination preferences of CuI versus CuII/CuIII while retaining the linear CNHC‐Cu‐CNHC arrangement throughout the series. In the oxidized species 2 and 3, the two pyridine donors swing in to provide the additional two equatorial donors that establish the square planar environment required for hosting CuII and CuIII ions. While NHC‐CuI complexes are abundant, CuII complexes with NHC ligation are rare and their redox chemistry is generally associated with decomposition or major structural changes. A recently reported CuIII complex of a tetra(NHC) macrocycle has a strongly destabilized Cu(d ) orbital and lacks the ligand hemilability that is required to enable reduction to the CuI state.11 Hence the present system is unique in that it allows for accessing all three copper oxidation states with little structural reorganization and within a useful potential window for the redox interconversions, which occur at E 1/2=−0.45 V and +0.82 V (vs. Fc/Fc+). An interesting aspect for future reactivity studies is that the addition of two electrons upon reduction of 3 to 1 also exposes two basic pyridine N atoms, suggesting that the electron transfer might be coupled with proton transfer.

The electronic structure of formal CuIII complexes is a matter of active investigation and debate because, in many reported cases, ligand non‐innocence has to be considered.5, 31 For instance, [n class="Chemical">Cu(CF3)4]− and related systems have recently been described as having a 3d10 ground state electronic configuration because of an inverted ligand field (that is, CuI character with the LUMO having predominantly trifluoromethyl character).5d In contrast, X‐ray spectroscopic studies on the present series of [LCu]+/2+/3+ complexes have revealed textbook examples of XAS signatures for CuI, CuII, and CuIII, in 1, 2, and 3, respectively. These findings are also in accordance with the other data and DFT results, and they indicate that 3 is a genuine CuIII species. This is in line with NHC ligands being extremely strong σ‐donor ligands that are largely redox innocent and are capable of supporting high oxidation state 3d metal complexes.8

Conflict of interest

The authors declare no conflict of interest.

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Supplementary

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