Complexes as Catalysts for Hydrocarbon and Catechol Oxidation Reactions with Hydrogen Peroxide and Molecular Oxygen

Dois ligantes tridentados, HL1, [(2-hidroxibenzil)(2-(imidazol-2-il)etil)]amina, e HL2, [(2-hidroxibenzil)(2-(piridil2-il)etil]amina, foram usados na síntese dos complexos binucleares [Cu 2 (L1) 2 ]Cl 2 •2H 2 O, complexo 1, e [Cu 2 (L2) 2 ] (ClO 4 ) 2 •1.5H 2 O, complexo 2, para serem empregados como catalisadores em processos de oxidação. Os complexos foram caracterizados por análise elementar e espectroscopias na região do infravermelho, ultravioleta-visível e ressonância paramagnética eletrônica. Foram também estudados por voltametria cíclica e titulação potenciométrica, a fim de caracterizar seus comportamentos em solução. A resolução da estrutura cristalina do complexo 1 mostrou um cátion binuclear contendo dois grupos fenóxido em ponte. Este arranjo possui uma distância Cu...Cu de 3.043(10) Å, similar à observada na catecol oxidase (2.90 Å). Os comportamentos catalíticos destes complexos foram investigados nas oxidações de cicloexano e de catecol. Na oxidação de cicloexano observou-se baixa atividade para ambos os complexos, que pode ser atribuída ao estereoimpedimento produzido pela falta de coplanaridade entre os anéis aromáticos do arcabouço dos ligantes, sugerindo que a aproximação entre o substrato e o centro ativo binuclear é uma etapa determinante no mecanismo da reação. Com relação à atividade de catecolase, foram observadas altas eficiências, com o complexo 2 sendo mais ativo que o complexo 1. Isto indica que o ligante piridina é capaz de estabilizar melhor o intermediário proposto para esse processo, que contém o centro CuCu. Isto é corroborado pela grande participação da piridina no LUMO (lowest unoccupied molecular orbital) do complexo 2, que pode ajudar a acomodar a carga negativa adicional quando o complexo é reduzido da forma CuCu para CuCu.


Introduction
Bleaching processes are among the most outstanding oxidative processes worldwide.They are largely employed in household, hospitals, commercial installations and in a variety of industries, such as textile, pulp and paper, and detergents. 1 Actually, chlorine-based bleaching systems including chlorine gas, chlorites (Ca(ClO 2 ) 2 and NaClO 2 ), hypochlorites (NaOCl, Ca(OCl) 2 ) and chlorine dioxide (ClO 2 ) are largely employed. 2However, environmental concerns have led to restrict their use mainly because of the resulting chlorine-based residuals. 3his restriction focuses basically on their chlorinated organic subproducts that are potentially hazardous, present low biodegradability, are recalcitrant, and then considered not environmentally friendly.In order to overcome the disadvantages of chlorine-containing products, totally chlorine free (TCF) systems emerged as an alternative, including molecular oxygen, ozone, hydrogen peroxide, perborates, percarbonates, enzymes and others. 4Under the green chemistry concept, some strategies are being spread out, as the use of enzymes able to activate oxygen, or hydrogen peroxide, to perform oxidation reactions. 5,6This class of enzymes is called oxidoreductases and comprises several copper-containing metalloenzymes such as laccases, 7 tyrosinase, 8,9 catechol oxidase 10 and Cu-containing quercetinase. 11,12Laccase is probably the most employed in bleaching studies.It is a multi-copper containing oxidoreductase (EC 1.10.3.2) with four copper centers (one type 1, one type 2 and two type 3 Cu atoms), which catalyzes the oxidation of a variety of phenols to quinones through the activation of molecular oxygen. 13Laccase has been studied in several organic transformations such as the preparation of phenolderivatives, aldehydes, ketones, lactones, oxidations of azo-dyes, hormones, polymerization reactions, and others. 13 addition to copper-containing laccase, tyrosinase and catechol oxidase have also received special attention related to their use as green catalysts because of their catecholase activity, i.e., their ability to convert 1,2-dihydroxyphenols (o-diphenol or catechol) to the respective o-quinones.However, besides this feature, tyrosinase is also able to promote the o-hydroxylation of phenols (cresolase activity) and may contribute to bioremediation of phenol-containing industrial residues. 7Unlike laccase, both tyrosinase and catechol oxidase are binuclear (type 3) copper enzymes.Despite tyrosinase crystal structure has not been solved, several spectroscopic studies indicate a close similarity with catechol oxidase.In the met form, catechol oxidase presents two Cu II ions coordinated to three histidine residues each, bridged by a hydroxo group 2.87 Å apart. 14onsidering the high academic and industrial interest on these enzyme systems, and that their use is sometimes limited mainly because of the optimal pH and temperature ranges, 15 model complexes are considered as an alternative.Because of this, several compounds have been synthesized, characterized and tested as catalysts for oxidative processes involving molecular oxygen and hydrogen peroxide. 16It is a matter of great concern to understand how small changes on the ligand scaffold can interfere in the reactivity of copper-containing coordination complexes, in order to improve their efficiency. 17n view of our previous interest in copper model complexes and in polipodal ligands, [18][19][20][21][22] we present here two new binuclear Cu II complexes (1 and 2, Figure 1) employing the tridentate N,O-donor ligands HL1, [(2-hydroxybenzyl)(2-(imidazol-2-yl)ethyl)]amine, and HL2, [(2-hydroxybenzyl)(2-(pyridil-2-yl)ethyl]amine.These complexes were designed intending to develop new catalysts for oxidative processes, and their reactivity towards cyclohexane and catechol oxidation reactions were investigated using hydrogen peroxide or molecular oxygen as oxidants.

Experimental
Materials and measurements HL1 and HL2 were synthesized and purified as previously described. 23,24All chemicals for syntheses and analyses were of analytical grade and used without further purification.Infrared spectra (CsI pellet or film) were recorded using a NICOLET, MAGNA-IR 760 (4000 to 200 cm -1 ) spectrophotometer.Elemental analyses were performed using a Perkin-Elmer 2400 analyzer coupled to an AD-4 Perkin-Elmer microbalance.Electronic absorption spectra were recorded using a Perkin-Elmer Lambda-19 spectrophotometer.Cyclic voltammetry studies were performed with a Princeton Applied Research (PAR) 273 potentiostat, at room temperature (25 ± 1 °C), in acetonitrile solutions kept under argon atmosphere.The standard three-electrode cell was composed by the following electrodes: a glassy carbon working, a platinum auxiliary and a Ag/AgCl pseudo-reference.Hexafluorophosphate of tetrabutylammonium (tba(PF 6 ), 0.1 mol L -1 ) was used as supporting electrolyte and the ferrocenium-ferrocene couple 25 was employed to monitor the reference electrode potential.Molar conductivities were measured on a Digimed CD-21 conductivity meter in methanol solutions.

Syntheses
Complex 1 was obtained by the slow addition of CuCl 2 • 2H 2 O (0.17 g, 1 mmol in 20 mL of methanol) to a methanolic solution of HL1 (0.217 g, 1 mmol in 20 mL).The reaction mixture was heated under stirring for ca.15 min, filtered and left to crystallize on bench at room temperature (near 25 °C).After a few days, dark green single crystals suitable for X-ray crystallographic analysis were collected from the mother liquor.N 6.94 (6.54)%.L M = 162 Ω -1 mol -1 cm 2 (electrolyte 2:1 in methanol). 26arning: perchlorate salts are potentially explosive and must be handled very carefully and only in small quantities.

Potentiometric titration
Potentiometric studies were carried out in CH 3 CN/H 2 O (1:1 v/v) solution using a Micronal B375 pHmeter fitted with blue-glass and calomel reference electrodes calibrated to read -log[H + ] directly, designated as pH.Bidistilled water in the presence of KMnO 4 was used to prepare the CH 3 CN/H 2 O (1:1 v/v) solutions.The electrode was calibrated using the data obtained from a potentiometric titration of a known volume of a standard 0.0100 mol L -1 HCl solution (0.1 mol L -1 in KCl) with a standard CO 2free 0.100 mol L -1 KOH solution.The measurements were carried out in a thermostatized cell containing a solution of the complex (0.05 mol/50 mL) with ionic strength adjusted to 0.100 mol L -1 by addition of KCl, at 25.00 ± 0.05 °C.The experiments were performed under argon flow to eliminate the presence of atmospheric CO 2 .The samples were titrated by addition of fixed volumes of a standard CO 2 -free KOH solution (0.100 mol L -1 ).Computations were carried out with the BEST program, and species diagrams were obtained with SPE and SPEPLOT programs. 27ystal structure X-ray diffraction data collection for compound 1 was performed on a Bruker-Kappa-CCD diffractometer (LDRX) using graphite-monochromatized Mo-K a radiation (l = 0.71069 Å) at room temperature.Final unit cell parameters were based on the fitting of all reflections positions. 28Data integration and scaling of the reflections were performed with the EVALCCD suite. 29Empirical multiscan absorption corrections using equivalent reflections were performed with the program SADABS. 30he structure was solved by direct methods using the SHELXS 31 program.The positions of all atoms could be unambiguously assigned on consecutive difference Fourier maps.Refinements were performed using SHELXL 31 based on F 2 through full-matrix least square routine.All but hydrogen atoms were refined with anisotropic atomic displacement parameters.Hydrogen atoms were added to the structure and further refined according to the riding model. 32No disordered groups have been found in the structure refinements.All attempts to localize the hydrogen atoms around the water molecules failed.Thus, the hydrogen bonds of the N-H group of the imidazole towards the water molecules could not be properly assigned.Crystal structure and refinement data for complex 1 are summarized in Table 1.Selected bond distances and angles are indicated in Table 2. Atomic coordinates and complete crystal structure results are given as supplementary information (see SI).

Reactivity Cyclohexane oxidation
The catalytic activities of complexes 1 and 2 towards cyclohexane oxidation were determined following previously published methods. 33The reaction was performed in acetonitrile at room temperature and inert atmosphere, using H 2 O 2 as oxidant.The catalyst:substrate:oxidant reaction ratio was 1:1000:1000, with a catalyst concentration of 7×10 -4 mol L -1 .In a typical experiment, the catalytic reaction was triggered with the addition of cyclohexane to a degassed acetonitrile solution containing the catalyst and the oxidant.The reaction was quenched after 24 h with the addition of an aqueous solution of Na 2 SO 4 (0.4 mol L -1 ).The products were extracted with diethyl ether; the organic fractions were dried over anhydrous Na 2 SO 4 and analyzed by gas chromatography.The results are expressed as relative yields. 33

Theoretical calculations
Geometry optimizations were performed as described before, using Gaussian 03 package with the B3LYP hybrid density functional theory combined with the 6-31G* basis sets and LANL2DZ for the Cu atom. 37

Results and Discussion
Synthesis and initial characterization L1 and L2 were chosen in order to provide insights about the influence of the substitution of pyridine by imidazole rings on the electronic structure and reactivity of the complexes.Both ligands are able to stabilize Cu II complexes.Infrared spectra of complexes 1 and 2 have shown characteristic bands of the ligands scaffold, and are shifted when compared to free HL1 and HL2, which is clear evidence of complexation.In order to help band attribution, theoretical studies were carried out using DFT (Figure S2).Considering the similarities of ligands and complexes spectra, the attribution data are summarized on Table S1, and only the main differences are discussed.In both spectra of complexes 1 and 2, the out-of-the-plane OH angular deformation band of the phenol group is absent, indicating the presence of phenolate groups coordinated to the metal centers.For complex 2, the presence of free perchlorate anions is evidenced by a broad band from 1130 to 1028 cm -1 assigned to the Cl-O stretchings of this anion as a counter ion. 38For both complexes, elemental analyses indicate the 1:1 ligand:metal ratio, and the presence of chloride or perchlorate anions.The binuclear arrangement for both complexes is firstly suggested by conductivity data obtained in freshly prepared methanol solutions (complex 1: L M = 151 Ω -1 mol -1 cm 2 , and complex 2: L M = 162 Ω -1 mol -1 cm 2 ), which are in the typical range of 2:1 electrolytes. 26

X-ray crystal structure
Crystallographic data and bond parameters for complex 1 are presented in Tables 1 and 2, respectively.An ORTEP 39 drawing of the cation complex is shown in Figure 2. The binuclear structure in the solid state is confirmed, where each Cu II atom is coordinated to a deprotonated L1, and bridged by the two phenoxo groups provided by the ligand.In close proximity, there are two chloride anions and two water molecules (Figure 2).In addition to the two  oxygen atoms from the phenoxo bridges, each Cu II atom is coordinated to one imidazole and the amine nitrogen atoms.Thus, the Cu II atoms can be considered as tetracoordinated, since their distances to the chloride anions and the water molecules are longer than 2.745(5) Å (Table 2).In fact, these Cu-Cl bond distances are longer than those reported for coordinated chloride anions. 19,40,41The geometries adopted by the Cu II centers are both distorted square-planar, with angles varying from 76.8(2) Å to 95.7(2) Å, for Cu(01), and from 77.9(2) Å to 96.9(2) Å, for Cu(02).

Spectroscopic analyses
The electronic spectra of complexes 1 and 2 were recorded in the solid state and acetonitrile solutions (Figure 3).In both cases, the two complexes present the same electronic features, indicating that their structures are maintained in solution.In acetonitrile, the spectra of both complexes are quite similar and show bands at 635 nm (e = 212 L mol -1 cm -1 ) and 398 nm (e = 3,340 L mol -1 cm -1 ) for complex 1, and at 640 nm (e = 280 L mol -1 cm -1 ) and 408 nm (e = 2,620 L mol -1 cm -1 ) for complex 2. The low molar extinction coefficients presented by the lower energy bands classify them as typical ligand field transitions in the Cu II centers. 47The higher energy bands can be assigned to ligand-to-metal charge transfer transitions (LMCT) from the phenoxo bridges to the Cu II ions, as proposed for other phenolate-coordinated Cu II complexes. 24,40,46,48 slight batochromic shift is observed for complex 2 when compared to complex 1.As observed before for cobalt(III) complexes with these same ligands, 49 this shift is a consequence of substitution of an imidazole by a pyridine ring in the ligand scaffold.In fact, we have also observed this behavior in other systems and assigned it to the greater basicity of 1-methylimidazole group compared to pyridine. 49,50Finally, electronic spectroscopy has been used to infer the geometry adopted by Cu II complexes in solution. 48Based on the similarities of the spectral data presented by complexes 1 and 2 we can conclude that they might present the same kind of geometry.The very broad shape of the spectra in the range of the low energy band makes a precise geometry attribution difficult, but points out to a distorted octahedron, 47 which suggests interaction of metal centers with solvent molecules.
EPR spectroscopy was used to give some insight on this issue.X-band spectra of complexes 1 and 2 were collected in frozen ethanol solutions at 77 K. Using the WINEPR SimFonia 51 program, the experimental data were simulated; both experimental and simulated spectra are presented in Figure 4.The following parameters were determined: g ⊥ = 2.068, g // = 2.268, A ⊥ = 20×10 -4 cm -1 , A // = 175×10 -4 cm -1 and g // / A // = 129 cm (for complex 1), and g ⊥ = 2.0590, g // = 2.261, A ⊥ = 20×10 -4 cm -1 , A // = 182×10 -4 cm -1 and g // /A // = 125 cm (for complex 2).The frozen solution spectra of both complexes (Figure 4) are typically axial, presenting four well-defined lines around g = 2, with g // > g ⊥ > 2.0 and A // > A ⊥ .These features are characteristic of elongated octahedral, square-pyramidal or square-planar geometries, 52 and have been observed for other binuclear Cu II complexes with two phenoxide bridges. 46,53The empirical g // / A // ratio can be employed to estimate the geometry distortion around Cu II centers, and values in the range of 105 to 135 cm are attributed to square-planar or octahedral (with tetragonal distortion) geometries. 54,55Considering the electronic spectroscopy data and the values observed for complexes 1 (g // / A // = 129 cm) and 2 (g // / A // = 125 cm), it is possible to infer that both complexes present interactions with solvent molecules in the axial positions.Additionally, the g // / A // ratio also provides evidence on the degree of covalency in the metal-ligand bond. 21,55Addison and Sakaguchi 55 reported that the replacement of "hard" by "soft" donor atoms around Cu II centers results in a decrease of g // , and consequently a decrease in the g // / A // ratio.This fact is interpreted as an increase in the electron delocalization away from the metal center, or an increase in covalency.For complexes 1 and 2, the g // values are very similar, but an increase in A // is observed when the softer base imidazole (complex 1) is replaced by pyridine (complex 2), which results in the decrease of the g // / A // ratio.This fact suggests a slight increase of the ligand field strength around the metal center for complex 2 compared to complex 1.In fact, as imidazole is a better s-donor than pyridine, [19][20][21]23,56 it was expected that HL1 presented higher ligand field strength than HL2, which is exactly the opposite behavior of the observed here.

Cyclic voltammetry studies
The cyclic voltammograms for complex 1 in acetonitrile solution (Figure S1) do not undergo significant variation upon several scan rate measurements, presenting a broad irreversible peak at -315 mV vs. NHE (normal hydrogen electrode).Considering that the coordination environments around the Cu II ions are identical, their reduction is expected to occur at very similar potentials, which can explain the broadening of the peak and allow us to consider it as a Cu II Cu II → Cu I Cu I process. 20This irreversibility indicates that HL1 might not be able to stabilize the reduced complex state leading it to break down (EC process).In contrast, complex 2 presents a redox activity dependent on the scan rate.As shown in Figure 5, from 50 and 100 mV s -1 , an irreversible wave is observed at -340 mV vs. NHE that is also tentatively attributed to the Cu II Cu II → Cu I Cu I process.The more negative value observed for complex 2 compared to complex 1 suggests that HL2 acts as a better electron donor than HL1, despite the expected behavior based on the s-donor ability of imidazole and pyridine groups.As reported before, 49 it is probably related to the LUMO features of these complexes.
When cyclic voltammograms of complex 2 are recorded at higher scan rates (125 to 250 mV s -1 ), an enhancement of the system reversibility is observed (125 mV s -1 : E 1/2 = -332 mV vs. NHE, DE p = 125 mV; 200 mV s -1 : E 1/2 = -328 mV vs. NHE, DE p = 135 mV; 250 mV s -1 : E 1/2 = -323 mV vs. NHE, DE p = 155 mV).This behavior suggests that, at least on the time scale of the measurements, the complex scaffold is maintained after reduction, and so a quasi-reversible process is detected.This fact can tentatively be rationalized in terms of the better p-acceptor properties of the pyridine ring which, by withdrawing electron density from the metal center after reduction, stabilizes the Cu I Cu I species under the time scale of the experiments.

Potentiometric titration
In order to examine the pK a of water molecules coordinated to the metal centers, potentiometric studies  were performed in acetonitrile/water mixture (1:1 v/v).As can be seen in Figure 6, two pK a values were observed for both complexes: for complex 1, pK a1 = 10.32 and pK a2 = 11.36, and for complex 2, pK a1 = 10.25 and pK a2 = 11.27.
Comparison of these results with those reported for other copper complexes in which the water molecules are considered completely coordinated to the metal center (pK a ca.8), 19,36,40 reveals that these pK a values are much higher.This fact can be tentatively explained by the existence of a weak metal-water interaction, as observed in the crystal structure of complex 1, in which the water molecule is 2.899 Å away from the Cu(02) center.In fact, a strong Jahn-Teller effect associated with the donating ability of the phenolate groups may weaken the Cu-O w bond, not permitting a significant polarization on the O-H bond of the closest water molecule and raising its pK a .It is worth to mention that the phenolate protonation constants could not be determined, probably because these groups are coordinated in a bridge mode and have very low pK a .

Theoretical calculations
As mentioned earlier, the EPR and the voltammetric data obtained for complexes 1 and 2 present an inverse behavior of that expected considering only the substitution of a pyridine by an imidazole group in the ligand scaffold.As previously reported, 49 this might be correlated to the features of the complexes frontier orbitals.Since the crystal structure of complex 1 revealed that the chloride anions and the water molecules are only interacting with the metal center, the geometry optimizations were carried out without them.As shown in Table 2, a good agreement was achieved between the experimental (X-ray) and the theoretical results for complex 1 and, then, the same approach was used to predict the geometry of complex 2. Figures 7 and 8 show the optimized geometries and the graphical representations of the frontier orbitals for complexes 1 and 2, respectively.
For complex 1, the HOMO (highest occupied molecular orbital) representation shows a small participation of the nitrogen atoms of the secondary amine and a strong contribution of both phenolate bridges.On the other hand, the LUMO has the participation of the nitrogen atoms of the secondary amine and the imidazole, the phenolate groups and the d x 2-y 2 orbital of the Cu center.For complex 2, the HOMO presents high similarity with that of complex 1, and shows a small participation of the amine nitrogen atoms and a large participation of the phenolate groups.However, the LUMO of complex 2 has strong contribution of the two pyridine rings.As the HOMO of both complexes are quite similar, the behavior observed for complexes 1 and 2 might be related to the different atomic contributions to the LUMO.While the LUMO of complex 1 is composed by the contribution of several atoms and is delocalized all over   the molecule, in complex 2 it has mainly the involvement of the pyridine rings and is localized over these groups.This fact can explain the more negative potential observed for complex 2 compared to complex 1, since the increase of electron density due to the reduction process might be more easily transferred to the LUMO of complex 1 than to the LUMO of complex 2.

Reactivity Cyclohexane oxidation
Since our intention is to develop new catalysts for oxidative processes, and alkane oxidations have great industrial interest, 58,59 the cyclohexane oxidation was investigated using hydrogen peroxide at room temperature.Complexes 1 and 2 lead to low overall conversion values of 6.34 and 7.15%, respectively.For complex 1, only cyclohexanol (Cy-OH) and cyclohexanone (Cy=O) were isolated as reaction products, with selectivities of 68.1% for Cy-OH and 31.9% for Cy=O, and turnover number of 70.For complex 2, the formation of 31.9% of Cy-OH, 29% of Cy=O and 32% of Cy-OOH (cyclohexylhydroperoxide) was observed, and turnover number of 78.Comparing these values with other Cu II complexes presenting vacant positions on the metal coordination sphere, the overall yields are fairly lower. 60,61his fact may be explained by the non-coplanarity of the central square-plane core and the ligand aromatic rings, which can make difficult the substrate approach, even though both complexes (1 and 2) present two vacant positions per Cu II center.

Catechol oxidation
The most widely employed substrate to investigate the catecholase activity of model complexes is 3,5-ditert-butylcatechol (3,5-dtbc).It is due to its low redox potential that facilitates the oxidation to quinone, and the presence of bulky substituents that prevents further oxidation reactions. 62he pH dependence of the catecholase activities promoted by complexes 1 and 2 was investigated in a range (5.5 to 10) that includes the optimal pH activity range observed for the enzyme. 15The plots of v 0 (initial rate) vs. pH (Figure 9 for complex 1, and S2 for complex 2) show sigmoid-shape profiles and reveal pK a values of 9.1 for 1 and 8.0 for complex 2, which are the kinetic pK a .The difference between these values and those obtained by potentiometric titration can be explained by the fact that the kinetic pK a represents the water molecules deprotonation in the presence of substrate.In addition, the potentiometric pK a was determined in CH 3 CN/H 2 O (1:1 v/v) solution and the reactivity experiments were carried out in methanol.3][64] The substrate dependence was carried out at pH 9, and a Michaelis-Menten profile was obtained (Figure 10 for complex 1, and Figure S3 for complex 2).The parameters obtained by a non-linear fit are presented in Table 3.The values for complexes 1 and 2 indicate that they are very efficient compared to other complexes in the literature. 35,64,65The kinetic efficiency (k cat /K M ) shows that complex 2 is approximately 10 times more active than complex 1. Usually, the catecholase activity of model complexes is largely attributed to the distance Cu … Cu, but other effects such as redox potentials, neighboring groups, and the individual coordination spheres can play important roles. 66For complexes 1 and 2, the Cu … Cu distances are very similar (Table 2) and may not be the reason for their different activities.Since the first step in the proposed mechanism is the oxidation of one substrate molecule coupled to a two-electron reduction of  the active site, 67 it was expected that complex 1 presented higher activity than complex 2, which has a more negative reduction potential, but this kind of correlation has been questioned. 66he non-reversibility shown in the voltammograms of complex 1 indicates that, after reduction, the complex integrity is not maintained in solution and this can be a reason of its lower reactivity.On the other hand, the reversibility shown by complex 2 at high scan rates shows that this complex does not decompose as fast as complex 1 after reduction, leading to its higher reactivity.

Conclusions
The Cu II binuclear complexes 1 and 2 are reactive in the cyclohexane oxidation, with selectivity close to 70% for the formation of cyclohexanol (for complex 1), but with conversion values low for both complexes.This low hydrocarbon oxidation activity can be attributed to steric hindrance effects produced by the non-coplanar aromatic rings of the ligand scaffold.It seems that the access of the hydrocarbon molecule to the binuclear active center is a determinant step in the mechanism of this process.As mimetic for catecholase activity, both complexes were very efficient, with complex 2 being approximately 10 times more effective than complex 1.These high efficiencies indicate that the pyridine ligand is capable to stabilize an intermediate Cu I Cu I center, which is proposed to be formed in this process, avoiding the breaking down of the complex.This is corroborated by the strong participation of pyridine in the LUMO of complex 2, which can help to accommodate the additional negative charge when the complex is reduced from Cu II Cu II to Cu I Cu I .

Figure 5 .
Figure 5. Cyclic voltammograms of complex 2 in methanol at different scan rates.

Table 1 .
Crystal structure data collection and refinement for compound 1

Table 3 .
Kinetic parameters for complexes 1 and 2

Table S4 .
23perimental (X-ray diffraction data for HL123) and calculated (DFT) main bond distances (Å) and angles ( o ) for HL1 and HL2 Figure S1.Cyclic voltammograms registered for complex 1 in methanol at different scan rates.