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Article

Reactivity and Mechanism of Photo- and Electrocatalytic Hydrogen Evolution by a Diimine Copper(I) Complex

by
Maria Drosou
1,
Fotios Kamatsos
1,
George Ioannidis
1,
Athanasios Zarkadoulas
1,
Christiana A. Mitsopoulou
1,*,
Constantina Papatriantafyllopoulou
2 and
Demeter Tzeli
3,4
1
Inorganic Chemistry Laboratory, Chemistry Department, National and Kapodistrian University of Athens Panepistimiopolis, 157 71 Zografou, Greece
2
School of Chemistry, NUI Galway, H91 TK33 Galway, Ireland
3
Theoretical and Physical Chemistry Institute, National Hellenic Research Foundation, 48 Vassileos Constantinou, 116 35 Athens, Greece
4
Physical Chemistry Laboratory, Chemistry Department, National and Kapodistrian University of Athens, Panepistimiopolis Zografou, 157 71 Athens, Greece
*
Author to whom correspondence should be addressed.
Catalysts 2020, 10(11), 1302; https://doi.org/10.3390/catal10111302
Submission received: 25 October 2020 / Revised: 9 November 2020 / Accepted: 9 November 2020 / Published: 11 November 2020
(This article belongs to the Section Photocatalysis)
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Abstract

:
The tetrahedral copper(I) diimine complex [Cu(pq)2]BF4 displays high photocatalytic activity for the H2 evolution reaction with a turnover number of 3564, thus representing the first type of a Cu(I) quinoxaline complex capable of catalyzing proton reduction. Electrochemical experiments indicate that molecular mechanisms prevail and DFT calculations provide in-depth insight into the catalytic pathway, suggesting that the coordinating nitrogens play crucial roles in proton exchange and hydrogen formation.

Graphical Abstract

1. Introduction

Copper catalysts for proton reduction have recently gained special attention in facilitating solar and electrochemical energy storage via the formation of hydrogen fuel. The abundance, price and diverse redox activity of copper have attracted particular interest [1,2,3,4] and many copper complexes have been used as photosensitizers [5,6] redox mediators [7,8] and catalysts for CO2 reduction [9,10] and water oxidation [11,12,13]. Several Cu-based H2 evolution heterogeneous [14,15,16] electrocatalysts with good performance have been reported, involving Cu(0), Cu2O [17,18,19,20,21,22], and Cu2S [23] materials. However, there are only a few examples of molecular copper catalysts with well-defined, rationally tunable structures and a comprehensive H2 formation mechanism.
Distorted trigonal bipyramidal and square pyramidal Cu(II) complexes bearing polypyridine chelates, which are supposed to minimize the inherent lability of the d10 Cu(I) ion, have been extensively explored as proton reduction electrocatalysts and photocatalysts. Their proposed catalytic pathways involve proton coupled electron transfer (PCET) processes leading to a Cu(II)-hydride that evolves H2 via intramolecular coupling between the hydride and the proton of a pendant pyridine nitrogen [24,25,26,27]. Square planar copper corroles can evolve H2 electrocatalytically via an heterolytic pathway, where a Cu hydride reacts with a solution proton [28], while a Cu(II) complex bearing a non-innocent thiosemicarbazone ligand exhibits metal-assisted ligand-centered electrocatalytic H2 evolution [29]. Other Cu(II) molecular catalysts involving tetradendate triazenido [30], Schiff base [31,32], oxamato [33], oxamido [34], phenanthroline [35] and imidazole-based [36] ligands have been recently presented. Notably, many of those catalysts decompose under reductive conditions to afford H2 evolving materials, thus part of their activity is attributed to heterogeneous deposits of nanoparticles [19].
Herein, we examined the photocatalytic H2 production behavior of [CuI(pq)2](BF4) ([1]BF4), a homoleptic tetrahedral Cu(I) diimine complex bearing the bidentate 2-pyridin-2-yl-quinoxaline (pq) ligand (Figure 1a). A complex like [1]+ but carrying two methyl groups on quinoxaline ring, has been previously reported to be an intermediate in CO2 fixation catalysed by molecular [Cu(pq)2(H2O)](ClO4)2 [9]. Evaluation of the H2 evolution mechanism by electrochemical and density functional theory (DFT) methods indicates that the quinoxaline nitrogen atoms are primarily protonated and subsequent metal centered PCET leads to the formation of a Cu(II)-hydride, that can evolve H2 via a low energy transition state.

2. Results and Discussion

2.1. Synthesis

Complex [1]+ was readily prepared from one equivalent of the Cu(I) starting [Cu(MeCN)4BF4] [37] and two equivalents of 2-pyridin-2-yl-quinoxaline (pq) [38] in acetonitrile. All operations were performed under a pure nitrogen atmosphere, using Schlenk and syringe techniques. [Cu(I)(MeCN)4BF4] [37] 1.0 mmol were dissolved in 5 mL acetonitrile and after a few minutes, 2-pyridin-2-yl-quinoxaline (pq) [38] 2.0 mmol dissolved in 10 mL acetonitrile was added and the mixture was stirred for 2 h. After this time, a deep purple solution was formed. Then the solvent was evaporated to dryness. The product was isolated in crystalline form with a yield of 63%. Calculated elemental analysis: C, 55.29; H, 3.21; N, 14.88; Found: C 55.46, H, 3.49; N, 15.01.
Complex [1]BF4 was also characterized by X-ray crystallography (Figure 1a, Tables S1–S7), UV-visible (Figure 1b) 1H-NMR (Figure S1) and cyclic voltammetry. Although its crystal structure was reported before [39], we repeated it for accuracy reasons and for taking into consideration the different anion of the complex. Time dependent density functional theory (TD-DFT) calculations with the B3LYP functional adequately reproduce the key features of the absorption spectrum and, thus, allow a reliable band assignment (Figure 1b, Table S8). The absorption bands centered at 550 nm are attributed to metal to ligand charge transfer (MLCT) transitions of the Cu(I) d orbitals to the pq π* antibonding orbitals.

2.2. Photocatalytic H2 Production

The photocatalytic H2 production activity of [1]+ was assessed in a multicomponent artificial photosynthesis system in N,N-dimethylformamide-water (DMF:H2O) mixture, using fluorescein (Fl) as a photosensitizer (PS) and triethanolamine (TEOA) as a sacrificial electron donor and the sample pH was 10.55. Under optimal conditions ([PS] = 0.3 mM, [1]+ = 0.85 μM, [TEOA] = 0.5 M in Ar saturated DMF:H2O 2:8, v/v solution under λ > 400 irradiation) [1]+ can photocatalyze H2 production efficiently, achieving 3564 TON (turnover number) with respect to the catalyst after 24 h (Table 1). Importantly, [1]+ can also serve as a photocatalyst for water reduction in a fully aqueous solution, reaching 182 mol of H2 per mole of catalyst. Keeping concentrations of [1]+, Fl and TEOA unchanged, the effect of solvent on H2 evolution was investigated as shown in Figure 2a which compares the catalytic efficiencies of three different solvent mixtures, namely H2O, DMF/H2O 2:8 and DMF/H2O 1/13. Photocatalytic systems with [1]+ as catalyst and CdTe quantum dots (QDs) as the photosensitizer showed a maximum performance of 132.53 TON after 24 h with TEOA as the electron donor, while systems with ascorbic acid as electron donor were inactive (Table S9).
Control experiments in the absence of light or any component of the system led to zero catalytic activity under the same conditions. In addition, mercury poisoning test was employed to investigate if catalytically active colloidal particles were formed during the catalytic process. Addition of mercury to this catalytic system resulted in a 30% reduction of the catalytic activity after 24 h of irradiation (Table 1), suggesting that the complex acts as a molecular photocatalyst, even though hydrogen evolution is partly attributed to in situ formed heterogeneous species.
In photocatalytic H2 evolution, the catalyst may accept electrons either from the excited PS or the reduced PS, resulting in oxidative and reductive quenching, respectively. The luminescence of the excited photosensitizer FL*, in a deaerated H2O solution of fluorescein, was plotted as a function of catalyst concentration and Stern-Volmer analysis yielded a quenching constant ksv = 1.3*105 M−1, indicating that the excited fluorescein can provide the potential needed to drive reduction of the catalyst (Figure 2b). However, the reductive quenching possibly predominates the photocatalytic process, because the TEOA concentration is six orders of magnitude higher than the concentration of the catalyst.
Due to the non-innocent nature of the pq ligand and the proposed ligand centered proton reduction mechanism (vide infra), a zinc analogue of complex [1]+, [Zn(pq)2]2+ was synthesized and was employed as a photocatalyst in identical conditions to complex [1]+, in order to elucidate whether the process is entirely ligand centered or mediated by the participation of the metal center (Figure S2). The zinc complex showed no catalytic activity. In addition, photocatalytic hydrogen production experiments were performed using pq as a catalyst where the catalytic performance did not exceed 3 TON proving that copper is an essential component in the proton reduction process.

2.3. Electrocatalytic Proton Reduction

The cyclic voltammogram (CV) of [1]+ recorded in DMF with 0.1 M tetrabutylammonium hexafluorophosphate (n-Bu4NPF6) as supporting electrolyte (Figure 3a) features an irreversible redox process at −0.18 V vs. ferrocenium/ferrocene (Fc+/Fc), which may be assigned to CuII/CuI. Two irreversible reduction events at −1.70 V and −1.97 V are attributed mostly to the pq ligand with some contribution from the Cu metal center. The free ligand reduction potential in DMF is −2.0 V vs. Fc+/Fc (Figure S3). The assignment of these reduction waves to the ligand-centered reduction processes is further supported by the calculated spin density of 0.18 on Cu at the reduced intermediate [1]0, as well as by the fact that the homoleptic Cu(I) complex with 2,2’-biquinoline (bq) has a similar redox process at the same potential window, which is attributed to bq/bq•− reduction [40]. The computationally derived oxidation and reduction potentials of [1]+ are −0.25 V, −1.77 V and −2.18 V, respectively, which supports a reliable peak assignment.
Subsequently, [1]+ was investigated with respect to its activity for electrocatalytic H2 production. As displayed in Figure 3b, upon addition of trifluoroacetic acid (TFA, pKaDMF = 6.0) [41] in a DMF solution of [1]+, a new reduction peak appears at −1.10 V and a significant catalytic current was observed over the potential of −1.66 V, attributed to catalytic H2 evolution. The overpotential of the catalyst was calculated [42] to be 720 mV, based on the reduction potential of TFA in a 5 mM DMF solution was calculated to be −0.94 V [43]. Several pieces of evidence suggest that the catalytic system is homogeneous. The linear dependence of catalytic current on the square of the scan rate (Figure 4a,b) indicates that the copper complex functions in a diffusion-controlled regime under the experimental conditions, and that it is a molecular catalyst. Also, rinse test experiment (Figure 4c) indicates that absorbed materials on the electrode surface are not catalytically active. Furthermore, the current increases linearly with an increase in the acid concentration (Figure 4d).
The electrocatalytic activity of [1]+ was also assessed in aqueous solution in the presence of acetic acid as a source of protons (Figure 5a,b). A very useful method to investigate the possibility of a concerted electron and proton transfer process (proton coupled electron transfer, PCET) instead of two separate consecutive electron transfer (ET) and proton transfer (PT) processes is the construction of the Pourbaix diagram, in which the reduction potential versus the pH of the solution is plotted [44]. The Pourbaix diagram (Figure 5c) shows that the reduction potential of the first reduction peak shifts linearly with the pH value in the range of 2.5 to 6.0, with a slope of 66.1 mV, which indicates that electron reduction is coupled with proton uptake. Similar ligand centered PCET processes have been reported for polypyridine copper proton reduction catalysts [24,25,26,27].

2.4. Computational Study of the Catalytic Mechanism

DFT calculations were performed, in an effort to provide further insight on the electrocatalytic mechanism by exploring the possible steps of the H2 formation. The computed structures of all the intermediates involved in the catalytic pathways are presented in the Supplementary Information. The proposed proton reduction mechanism derived from the calculated free energies of possible intermediates of the reaction pathway is shown in Figure 6a.
In the presence of TFA (pKa = 6.0 in DMF) the first reduction to generate the doublet species [2]+ is a PCET process, in which ligand reduction is concomitant with a nitrogen atom protonation. Three different isomers can be considered in terms of whether the site of protonation is the coordinating pyridine nitrogen (N1), the coordinating quinoxaline nitrogen (N2) or the non-coordinating quinoxaline nitrogen (N3) (Figure S5).
The [Cu–N3–H]+ isomer was found to be the most stable one, while the free energies of [Cu–N2–H]+ and [Cu–N1–H]+ are 7.2 and 10.6 kcal mol−1 higher than that of [Cu–N3–H]+, respectively. Protonation of CuI to form a CuIII hydride was also considered, but the energy of this step is found to be 28.5 kcal mol−1 higher than the most stable species.
This redox peak assignment is also supported by the cyclic voltammetry data of the free ligand, where a new reduction peak at −1.1 V appears in the presence of TFA (Figure S3).
A second PCET step to afford intermediate [3]+ is feasible on the basis of thermodynamics with a calculated potential of −0.90 V. The most favourable protonation site when the N3 is already protonated is the N2 ligating atom, on the same quinoxaline ring, which takes a tetrahedral conformation, thus it maintains the Cu–N2 bond as well as the N2–H bond. Protonation of the non-coordinating quinoxaline N3 is accompanied by reduction of the quinoxaline moiety under applied potential, which increases the basicity of the coordinating N2. Upon the second PCET, N2 protonation induces loss of the π-conjugation of the pyrazine ring, which is reflected in the calculated C–C and C–N bond lengths, and N2 now lies above the plane of the pyrazine C atoms without being dechelated from the metal ([3]+, Figure S6). Other possible protonation sites and the corresponding relative free energies are shown in Figure S6. Notably, the formation of a Cu hydride is 30.2 kcal mol−1 energetically higher. Two further PCET processes result in protonation of the second quinoxaline ligand and the 4H+/4e− reduced intermediate [5]+ is generated. Since protonation of the ligating nitrogens induces weakening of the Cu–N bonds, the possibility of [5]+ decomposition was examined, but was found unfavorable (Figure S7). In the presence of acid, five oxidation peaks appear at the anodic scan of the cyclic voltammogram at −0.70 V, −0.62 V, −0.41 and −0.26 V, which can be assigned to the four ligand centered redox processes, and at −0.07 V which is attributed to CuI/CuII oxidation (Figure 3b). Cyclic voltammogram within a narrow potential region (0.3 to −1.2 V) to prevent the formation of Cu(0) species, show that the four anodic peaks are attributed to the first reduction peak (Figure 5b). The reduction potential of intermediate [5]+ to generate Cu(0) species is calculated to be −2.58 V, while a metal centered PCET at a calculated potential of −1.92 V (experimental −1.66 V) in the presence of TFA affords a trigonal pyramidal Cu(II) hydride, [6]+, which is proposed to be the H2 evolving species. [6]+ can evolve H2 via a low energy (+6.8 kcal mol−1) transition state (TS, Figure 6b) with a single imaginary frequency at 1245.6, that corresponds to H2 formation, as confirmed by IRC (integrated reaction coordinates) calculation. The energy coordinate diagram of the hydrogen evolution reaction was generated from the free energy change of each step in the catalytic cycle (Figure 7).

3. Conclusions

We have presented that the Cu(I) diimine complex [1]+ can serve as a molecular photocatalyst for water reduction in combination with fluorescein as a photosensitizer and triethanolamine as a sacrificial electron donor achieving 3564 turnovers, after 24 h of irradiation. Mechanistic studies based on electrochemical experiments and DFT calculations support that protonation of the nitrogen atoms of the pq ligand via consecutive PCET processes allows more anodic reduction potentials for the Cu(II)-hydride formation and lowers the overpotential needed for proton reduction. Furthermore, the non-ligating quinoxaline nitrogen also increases the stability of the catalyst under reductive conditions and, thus, the present study provides important guidelines for future robust catalysts design. Detailed mechanistic studies using spectroelectrochemistry experiments are at the center of ongoing work, as well as the development of polydentate quinoxaline containing ligands, that are expected to further stabilize the Cu(I) species.

4. Materials and Methods

4.1. General Information

Reagents (starting materials, solvents) used in the experiments were purchased from Sigma Aldrich (Darmstadt, Germany) Merck (Darmstadt, Germany), Alfa Aesar (Heysham, Lancashire, UK) and Panreac Applichem (Barcelona, Spain). It was at least analytical grade and underwent further purification, where it was necessary to carry out the experiments. The solvents used to measure the absorption and emission spectra were of spectroscopic purity and originated from the above companies. Also, the water used in the experiments was from the Milli-Q instrument. In complex synthesis [39], the reagents that were used were purchased from the above companies.
Absorption spectra were measured on a Cary 300 (Varian Inc.-Agilent Technologies, Grenoble, France) or a U-2000 (Hitachi, Berkshire, United Kingdom ) spectrophotometers at 25 °C. Quartz alveoli were used with a stopper, a 1.00 cm optical path. Emission spectra were measured on a RF-5301PC spectrophotometer (Shimadzu, Hesse, Germany). Quartz alveoli were used with a 1.00 cm optical path, using the software OriginPro 9.0 (Arezzo, Italia). 1H-NMR spectra were measured on a Unity Plus 300/54 spectrophotometer (Varian, Grenoble, France).
For the X-ray diffraction studies, suitable crystals covered with paratone-N oil were placed onto the tips of glass fibers or scooped up in cryo-loops at the end of a copper pin and transferred to a goniostat for data collection with a SuperNova A diffractometer (Oxford Diffraction, Frankfurt, Germany,) equipped with a CCD area detector and a graphite monochromator utilizing Mo-Kα radiation (λ = 0.71073 Å). Empirical absorption corrections were applied using CrysAlis RED software [45] (multi-scan based on symmetry-related measurements). Structures were solved using SIR92 [46] and refined on F2 using full-matrix least squares with SHELXL97 [47]. Software packages used: CrysAlis CCD for data collection, CrysAlis RED for cell refinement and data reduction, WINGX for geometric calculations [48] and MERCURY [49] for molecular graphics. The program SQUEEZE [50], a part of the PLATON crystallographic software package, was used to remove contribution of highly disordered solvent molecules. All non-hydrogen atoms were refined anisotropically, whereas the hydrogen atoms were placed in calculated, ideal positions and refined as riding atoms with relative isotropic displacement parameters. Unit cell data and structure refinement details are listed in Table S2.
Photocatalysis experiments were performed in special led headlamps where the emitted radiation is in the range of the visible radiation spectrum (λ > 400 nm). The samples were irradiated for at least 72 h until the maximum performance of each system was found. The gaseous composition of the mixture and therefore the hydrogen detection was done by gas chromatography. The gas chromatograph was a 430-GC type (Bruker, Karlsruhe, Germany) equipped with a thermal conductivity detector (TCD) and operated under the following conditions: carrier gas: nitrogen, oven temperature 70 °C, detector temperature 150 °C, injector temperature 80 °C, molecular sieves column 5Å. The analysis of the chromatograms was done using the Galaxie software (Varian). The flask under the photocatalyst experiment was degassed by argon for 15 min and the system was sealed and illuminated for as long as the experiment lasts to find the maximum hydrogen output. The hydrogen produced is measured by integration of the chromatographic peaks and the quantification of the amount of hydrogen was based on calibration using Zn in aqueous HCl solution. Turnover number (TON) is used to quantify catalyst performance and represents the overall number of moles of H2 produced upon irradiation of a photocatalytic system per mole of catalyst in the system.

4.2. Synthesis

[Zn(pq)2]Cl2 was synthesized with the following procedure: ZnCl2 (1.0 mmol) was dissolved in EtOH (5 mL). After a few minutes, 2-pyridin-2-yl-quinoxaline (pq, 2.0 mmol) dissolved in EtOH (10 mL) was added. The mixture was stirred for 2 h. Almost immediately white powder appeared. The solution filtered off, washed with ethanol and dried, with a yield of 73%. Elemental Anal. Calc: C, 66.08; H, 3.78; N, 17.51; Found: C 66.12, H, 3.90; N, 17.35 1H-NMR peaks CDCl3: 7.49 (s, 2H), 7.78 (d,4H), 7.94 (s, 2H), 8.19 (d, 6H), 8.62 (t, 2H), 8.81 (s, 2H).
CdTe QDs were prepared as reported previously [51] and the A-F notation in Table S9 refers to the QDs’ preparation time according to this reference. A 50 mL aqueous solution of Cd(CH3COO)2•2H2O (0.2 mmol), thioglycolic acid 90% (18 μL), K2TeO3 (0.04 mmol) and NaBH4 (80 mg) was refluxed under open-air conditions for (A) 15 min, (B) 30 min, (C) 1 h, (D) 3 h, (E) 7 h or (F) 13 h.

4.3. Cyclic Voltammetry

All cyclic voltammetry (CV) measurements were recorded using an AFCBP1 (Pine Instrument Company, Lyon, France) and using the Aftermath Data Organizer software version 1.4.7881. Experiments were conducted in a three-electrode single-compartment cell with a glassy carbon working electrode, Ag/AgCl reference electrode and Pt counter-electrode at room temperature and using degassed solutions by purging with N2. All measurements were performed in N,N-dimethylformamide (DMF) in the presence of 0.1 M tetrabutylammonium hexafluoro-phosphate (n-Bu4NPF6) as a supporting electrolyte and ferrocenium/ferrocene (Fc+/Fc) redox couple was used as an internal potential reference.

4.4. Theoretical Studies

Geometry optimizations were carried out using the B3LYP density functional [52,53] in combination with the 6-31 g(d,p) basis set [54,55] as implemented in the Gaussian16 software package [56]. The choice of this functional was made based on agreement between the calculated optimized geometry and the experimentally defined structure (Table S10) as well as on its successful implementation in previous studies on copper-based catalysts. Gibbs free energies were calculated as single-point corrections on the optimized structures employing the larger basis set 6-311+g(2d,p) and D3 dispersion corrections [57] to obtain a more accurate value of the absolute free energy of each species. The solvent effects were considered through single-point energy calculations using the SMD continuum solvation model [58]. Frequency calculations were performed on all the optimized structures at the same level of theory, to identify all the stationary points as minima (zero imaginary frequency) or transition states (only one imaginary frequency) and to obtain Gibbs free energy corrections at 298.15 K. Time-dependent DFT (TD-DFT) calculations were performed to simulate the absorption spectra of [1]+.
The reduction potential was determined using the equation E = ΔGo/nF − E(Fc+/Fc0), where the E(Fc+/Fc0) standard ferrocene couple (Fc+/Fc0 = 4.988) [59]. Trifluoroacetic acid (pKaTFA = 6.0) calculated at the same level of theory was used for the calculation of the free energies of each protonation step through following equation: A + CF3COOH → AH+ + CF3COO−, pKaAH+ = ΔGo/1.364 + pKaTFA. The redox potential for the PCET processes, A + e− + H+ → AH, was calculated using the equation, E(A/AH) = E°(A/A−) + RTln(10)(pKaAH − pKaTFA) (Table S11).

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4344/10/11/1302/s1, Figure S1: 1H-NMR of [1]BF4 in CDCl3, Figure S2: 1H-NMR of [Zn(pq)2]2+ in CDCl3, Figure S3: Cyclic voltammograms (CVs) of the pq ligand (5.0 mM) in the absence (black curve) and the presence (coloured curves) of 1 mM (red), 2 mM (blue) and 4 mM (purple) of TFA recorded in a DMF solution of n-Bu4NPF6 (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s−1, Figure S4: Absorption spectra of [1]BF4 in H2O:DMF 1:8 mixture with C = 2*10−4 M under visible light irradiation over a period of 24 h, Figure S5: Relative free energies of the 1H+ protonated and 1e− reduced species [2]+ tautomers, Figure S6: Relative free energies of the 2H+ protonated and 2e− reduced species [3]+ tautomers, Figure S7: Possible decomposition pathways of the intermediate [5]+ in water, Figure S8: Relative free energies of the 3H+ protonated and 3e− reduced species [4]+ tautomers, Figure S9: Relative free energies of the 4H+ protonated and 4e− reduced species [5]+ tautomers, Figure S10: Higher occupied molecular orbital diagrams of the catalytic intermediates and spin densities on Cu (ρCu) of intermediates with unpaired electrons, Table S1: Crystallographic data for complex [1]BF4, Table S2: Selected bond distances (Å) and angles (o) for [1]BF4, Table S3: Crystal data and structure refinement for C26 H18 B Cu F4 N6 at 100 K, Table S4: Atomic coordinates (×104) and equivalent isotropic displacement parameters (Å2 × 103) for C26 H18 B Cu F4 N6 at 100 K with estimated standard deviations in parentheses, Table S5: Anisotropic displacement parameters (Å2 × 103) for C26 H18 B Cu F4 N6 at 100 K with estimated standard deviations in parentheses, Table S6: Bond lengths [Å] for C26 H18 B Cu F4 N6 at 100 K with estimated standard deviations in parentheses, Table S7: Bond angles [°] for C26 H18 B Cu F4 N6 at 100 K with estimated standard deviations in parentheses, Table S8: Electronic transitions of [Cu(pq)2]+ calculated with the TDDFT method, Table S9: Performance of the photocatalytic systems with [1]+ as catalyst, different CdTe QDs as the photosensitizer and different e− donors in DMF:H2O 1:2 solvent mixture, Table S10: Comparison of the experimental (crystal structure) and DFT calculated (B3LYP/6-31G**, gas phase) values of selected structural parameters of [Cu(pq)2]BF4 ([1]BF4), Table S11: The free energy of H2 self-elimination from AH2 was calculated from the following equations.

Author Contributions

Conceptualization, C.A.M.; methodology, M.D., D.T., C.A.M.; synthesis, G.I., F.K., A.Z.; photocatalytic experiments, F.K.; electrocatalytic experiments, M.D., G.I.; Single crystal X-ray crystallography, C.P.; DFT calculations, M.D., D.T.; investigation, M.D.; resources, M.D.; data curation, M.D., F.K.; writing—review and editing, M.D.; supervision, C.A.M., D.T.; project administration, C.A.M. All authors have read and agreed to the published version of the manuscript.

Funding

Special Research Account of NKUA (No: 16672), Hellenic Foundation for Research and Innovation (HFRI) under the HFRI PhD Fellowship grant 16199, Operational Programme «Human Resources Development, Education and Lifelong Learning» in the context of the project “Strengthening Human Resources Research Potential via Doctorate Research” (MIS-5000432), implemented by the State Scholarships Foundation (ΙΚΥ).

Acknowledgments

We gratefully acknowledge financial support from the Special Research Account of NKUA (No: 16672). M.D.: The research work was supported by the Hellenic Foundation for Research and Innovation (HFRI) under the HFRI PhD Fellowship grant 16199. F.K. thanks the co-funding by Greece and the European Union (European Social Fund—ESF) through the Operational Programme «Human Resources Development, Education and Lifelong Learning» in the context of the project “Strengthening Human Resources Research Potential via Doctorate Research” (MIS-5000432), implemented by the State Scholarships Foundation (ΙΚΥ).

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 10 01302 g001 550
Figure 1. (a) ORTEP of [1]BF4. Thermal ellipsoids are drawn from 50% probability ([1]+) (b) Experimental and calculated absorption spectra of [1]+ in DMF solvent.
Figure 1. (a) ORTEP of [1]BF4. Thermal ellipsoids are drawn from 50% probability ([1]+) (b) Experimental and calculated absorption spectra of [1]+ in DMF solvent.
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Catalysts 10 01302 g002 550
Figure 2. (a) Light-driven hydrogen production from system containing complex [1]+ as catalyst (8.5*10−7 M), Fl 0.3 mM, TEOA (0.5 M) in DMF: H2O (1:13)(10.0 mL) (green), in DMF: H2O (2:8)(10.0 mL) (red) and in H2O (blue) (b) Photoluminescence spectra of fluorescein as a function of [1]+ and Stern-Volmer plot of quenching by [1]+.
Figure 2. (a) Light-driven hydrogen production from system containing complex [1]+ as catalyst (8.5*10−7 M), Fl 0.3 mM, TEOA (0.5 M) in DMF: H2O (1:13)(10.0 mL) (green), in DMF: H2O (2:8)(10.0 mL) (red) and in H2O (blue) (b) Photoluminescence spectra of fluorescein as a function of [1]+ and Stern-Volmer plot of quenching by [1]+.
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Catalysts 10 01302 g003 550
Figure 3. (a) Cyclic voltammogram (CV) of complex [1]+ (1mM) in DMF solution of n-Bu4NPF6 (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s-1 (b) CVs of [1]+ 1 mM in DMF (0.1 M Bu4NPF6) with increasing equivalents of TFA.
Figure 3. (a) Cyclic voltammogram (CV) of complex [1]+ (1mM) in DMF solution of n-Bu4NPF6 (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s-1 (b) CVs of [1]+ 1 mM in DMF (0.1 M Bu4NPF6) with increasing equivalents of TFA.
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Catalysts 10 01302 g004 550
Figure 4. (a) CVs of 1 mM [1]+ in 0.1 M Bu4NPF6 DMF solution with 24 eq TFA at different scan rates (b) Plot of icat/ip vs the square root of the scan rate (c) CV of [1]+ 1 mM in DMF (0.1 M Bu4NPF6) with 15 mM TFA added (black) and a subsequent CV (red) using the same electrode after performing electrolysis at a potential of −1.7 V for 5 min, then rinsing with DMF and transfer to fresh DMF/0.1 M Bu4NPF6 solution without adding [1]+ with 15 mM TFA (d) Dependence of the catalytic current, icat/ip, on the concentration of TFA in a 1 mM [1]+ and 0.1 M Bu4NPF6 DMF solution.
Figure 4. (a) CVs of 1 mM [1]+ in 0.1 M Bu4NPF6 DMF solution with 24 eq TFA at different scan rates (b) Plot of icat/ip vs the square root of the scan rate (c) CV of [1]+ 1 mM in DMF (0.1 M Bu4NPF6) with 15 mM TFA added (black) and a subsequent CV (red) using the same electrode after performing electrolysis at a potential of −1.7 V for 5 min, then rinsing with DMF and transfer to fresh DMF/0.1 M Bu4NPF6 solution without adding [1]+ with 15 mM TFA (d) Dependence of the catalytic current, icat/ip, on the concentration of TFA in a 1 mM [1]+ and 0.1 M Bu4NPF6 DMF solution.
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Catalysts 10 01302 g005 550
Figure 5. (a) CVs of [1]+ (0.5 mM) in the presence of various concentrations of AcOH (1.0–8.0 mM) recorded in an aqueous solution of NaCl (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s−1 (b) CV of [1]+ (0.5 mM) in the presence of 2 mM of acetic acid recorded in an aqueous solution of NaCl (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s−1 in the potential window of 0.3 to −1.1 V (c) Pourbaix diagram (reduction potential vs. pH): the reduction potential of the first CV peak vs. [Fe(CN)6]3−/[Fe(CN)6]4− shifts linearly with the pH value in the pH range of 2.5–6.0, with a slope of 0.066 mV per pH unit. The respective CVs were recorded in aqueous solutions of [1]+ (0.5 mM) in the presence of CH3COOH/CH3COONa buffer.
Figure 5. (a) CVs of [1]+ (0.5 mM) in the presence of various concentrations of AcOH (1.0–8.0 mM) recorded in an aqueous solution of NaCl (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s−1 (b) CV of [1]+ (0.5 mM) in the presence of 2 mM of acetic acid recorded in an aqueous solution of NaCl (0.1 M) on a glassy carbon electrode at a scan rate of 0.1 V s−1 in the potential window of 0.3 to −1.1 V (c) Pourbaix diagram (reduction potential vs. pH): the reduction potential of the first CV peak vs. [Fe(CN)6]3−/[Fe(CN)6]4− shifts linearly with the pH value in the pH range of 2.5–6.0, with a slope of 0.066 mV per pH unit. The respective CVs were recorded in aqueous solutions of [1]+ (0.5 mM) in the presence of CH3COOH/CH3COONa buffer.
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Catalysts 10 01302 g006 550
Figure 6. (a) Proposed mechanism for the electrocatalytic H2 formation by [1]+ based on DFT calculations using the B3LYP-D3/6-311+g(2d,p) method for the calculation of redox potentials and protonation energies (b) Structure of the transition state (TS) for H2 formation.
Figure 6. (a) Proposed mechanism for the electrocatalytic H2 formation by [1]+ based on DFT calculations using the B3LYP-D3/6-311+g(2d,p) method for the calculation of redox potentials and protonation energies (b) Structure of the transition state (TS) for H2 formation.
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Figure 7. Free energy diagram depicting the possible electron transfer-followed by proton transfer (ET-PT, blue), proton transfer-followed by electron transfer (PT-ET, red) and concerted proton coupled electron transfer (PCET, black) processes of the H2 evolution catalytic pathway.
Figure 7. Free energy diagram depicting the possible electron transfer-followed by proton transfer (ET-PT, blue), proton transfer-followed by electron transfer (PT-ET, red) and concerted proton coupled electron transfer (PCET, black) processes of the H2 evolution catalytic pathway.
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Table
Table 1. Performance of the photocatalytic system under various conditions.
Table 1. Performance of the photocatalytic system under various conditions.
CatalystPhotosensitizere− DonorSolventEvolved H2
[1]+, μMFluorescein, mΜTriethanolamine, MDMF:H2OTON24 h
10010.51:228.04
1010.51:2154.96
110.51:2855.45
0.110.51:21130.72
120.51:2381.85
11.50.51:2724.77
10.80.51:2204.83
10.50.51:2773.89
10.30.51:2791.50
110.11:2836.91
1111:2781.31
0.850.30.51:43564.31
8.50.30.51:4547.98
0.850.30.51:132643.75
0.85 10.30.51:131837.82
0.850.30.5H2O182.00
1 In the presence of ca. 1 mL of mercury.
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Drosou, M.; Kamatsos, F.; Ioannidis, G.; Zarkadoulas, A.; Mitsopoulou, C.A.; Papatriantafyllopoulou, C.; Tzeli, D. Reactivity and Mechanism of Photo- and Electrocatalytic Hydrogen Evolution by a Diimine Copper(I) Complex. Catalysts 2020, 10, 1302. https://doi.org/10.3390/catal10111302

AMA Style

Drosou M, Kamatsos F, Ioannidis G, Zarkadoulas A, Mitsopoulou CA, Papatriantafyllopoulou C, Tzeli D. Reactivity and Mechanism of Photo- and Electrocatalytic Hydrogen Evolution by a Diimine Copper(I) Complex. Catalysts. 2020; 10(11):1302. https://doi.org/10.3390/catal10111302

Chicago/Turabian Style

Drosou, Maria, Fotios Kamatsos, George Ioannidis, Athanasios Zarkadoulas, Christiana A. Mitsopoulou, Constantina Papatriantafyllopoulou, and Demeter Tzeli. 2020. "Reactivity and Mechanism of Photo- and Electrocatalytic Hydrogen Evolution by a Diimine Copper(I) Complex" Catalysts 10, no. 11: 1302. https://doi.org/10.3390/catal10111302

APA Style

Drosou, M., Kamatsos, F., Ioannidis, G., Zarkadoulas, A., Mitsopoulou, C. A., Papatriantafyllopoulou, C., & Tzeli, D. (2020). Reactivity and Mechanism of Photo- and Electrocatalytic Hydrogen Evolution by a Diimine Copper(I) Complex. Catalysts, 10(11), 1302. https://doi.org/10.3390/catal10111302

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