N.
Queyriaux‡
*a,
K.
Abel
a,
J.
Fize
b,
J.
Pécaut
c,
M.
Orio
*d and
L.
Hammarström
*a
aDepartment of Chemistry, Ångström Laboratories, Uppsala University, Box 523, 751 20 Uppsala, Sweden. E-mail: nicolas.queyriaux@lcc-toulouse.fr; leif.hammarstrom@kemi.uu.se
bUniv. Grenoble Alpes, CNRS, CEA, IRIG, Laboratoire de Chimie et Biologie des Métaux, 17 rue des Martyrs, F-38054, Grenoble Cedex, France
cUniv. Grenoble Alpes, CEA, CNRS, IRIG, SYMMES, 38000 Grenoble, France
dAix Marseille Univ., CNRS, Centrale Marseille, iSm2, 13397 Marseille, France. E-mail: maylis.orio@univ-amu.fr
First published on 13th May 2020
The electrochemical behavior of [Co(bapbpy)Cl]+ [1-Cl]+, a pentacoordinated polypyridyl cobalt(II) complex containing a redox-active tetradentate ligand (bapbpy: 6,6′-bis-(2-aminopyridyl)-2,2′-bipyridine) has been investigated in DMF. Cyclic voltammograms (CV), recorded in the presence of increasing amounts of chloride anions, highlighted the existence of an equilibrium with the neutral hexacoordinated complex. Under a CO2 atmosphere, CVs of [Co(bapbpy)Cl]+ exhibit significant current enhancement assigned to CO2 catalytic reduction. Controlled-potential electrolysis experiments confirmed formation of CO and HCOOH as the only identifiable products. The addition of water or chloride ions was shown to affect the distribution of the products obtained, as well as the faradaic efficiency associated with their electrocatalytic generation. A combination of electrochemical techniques, chemical reductions, spectroscopic measurements (UV-vis and IR) and quantum chemical calculations suggests that the ability of the bapbpy ligand to be reduced at moderately negative potentials drastically limits the catalytic performances of [1-Cl]+, by stabilizing the formation of a catalytically-competent CO2-adduct that only slowly reacts with oxide acceptors to evolve towards the desired reduction products.
CO2 + e− → CO2˙− (Eo′ = −1.90 V vs. NHE) | (1) |
CO2 + 2H+ + 2e− → CO + H2O (Eo′ = −0.53 V vs. NHE) | (2) |
CO2 + 2H+ + 2e− → HCO2H (Eo′ = −0.61 V vs. NHE) | (3) |
CO2 + 4H+ + 4e− → HCHO + H2O (Eo′ = −0.48 V vs. NHE) | (4) |
CO2 + 6H+ + 6e− → CH3OH + H2O (Eo′ = −0.38 V vs. NHE) | (5) |
CO2 + 8H+ + 8e− → CH4 + H2O (Eo′ = −0.24 V vs. NHE) | (6) |
2H+ + 2e− → H2 (Eo′ = −0.42 V vs. NHE) | (7) |
Transition metal catalysts usually favor the desired multielectron processes, owing to their ability to accommodate multiple reduction steps within the range of considered potentials. Their relatively versatile and tunable properties have allowed rapid development of a wide diversity of electro- and photocatalytic systems, some of the most efficient and selective catalysts being based on rhenium9–11 and ruthenium12–14 complexes. Although studies on these two families of compounds have clearly demonstrated the essential role played by the metal center during the catalytic cycle,15,16 it is interesting to note that the first reduction steps initiating the catalytic process are centered on the ligand. This mechanistic specificity, associated with the cost-prohibitive nature of the rare metals being used, has certainly contributed to the great attention and efforts directed towards the development of first-row transition metal complexes capable to efficiently reduce CO2.17 While several complexes based on Fe,18,19 Co,20–22 Ni23,24 or Mn25,26 have been reported, improvements in terms of both selectivity and stability are still demanded.
Cobalt polypyridyl complexes have recently emerged as interesting candidates for both CO2 reduction and hydrogen evolution.21,27–29 This type of coordination sphere has been shown to offer a wide range of advantages, from their ability to stabilize low-valent cobalt centers involved over the course of the catalytic process to their synthetic modularity and robustness. Generally based on polydentate ligands, these ligand frameworks are also proposed to contribute to the high stability of the resulting cobalt complexes by virtue of the chelate effect. The relevance of cobalt polypyridyl complexes for the electrocatalytic reduction of CO2 was first evidenced with the use of [Co(phen)3]2+ by Durand and co-worker in 1988.30 Further investigations have led to the development of a range of bis-triimine complexes capable to electro-assist the reduction of CO2 to generate mixtures of C1-products whose selectivity can be preferentially oriented towards HCOOH or CO.31–33 More recently, tetradentate platforms have been developed and allowed good selectivity towards formation of carbon monoxide to be reached.21,34–37 These encouraging results have stimulated the development of heterogenization strategies, either by their attachment onto transparent conducting oxide and carbonaceous materials (graphene and carbon nanotubes, typically) or by integrating them into polymer chains.38–42
The role played by the ligand set in catalytic mechanisms has recently attracted much attention,43–45 different functions susceptible to increase catalytic performance being envisaged: proton relays (amine, thiol or phenol groups),18,21,46–48 electron reservoirs (pyrazine, dithiolene or quinone moieties),49–51 effective catalytic sites52 or a combination of those functions.53,54 In the case of the electro-assisted H2 evolution, proton relay sites and redox-active units have clearly demonstrated their ability to improve catalytic kinetic features or to significantly reduce the overpotential required to drive the reaction.55 Examples are scarcer when it comes to CO2 reduction and mechanistic dead-ends have been established in several situations. While Savéant, Costentin and co-workers found that introduction of multiple proton relays dramatically enhanced the CO2-to-CO electrocatalytic properties of iron porphyrin,18 similar modifications performed on a ruthenium(II) complex by the group of Fujita resulted in a catalytically-inactive complex under CO2 atmosphere.56 Such unexpected behavior has been assigned to new deactivation pathways in which a carbonate species has been formed by the reaction between the reduced ligand and CO2. Similarly, Elgrishi et al. investigated the electro-assisted CO2-to-CO conversion mediated by [M(tpy)2]2+ complexes (M = Mn, Fe, Co, Ni, Cu, Zn) and suggested carboxylation of the reduced tpy ligand as a potential deactivation pathway (tpy = 2,2′:6′,2′′-terpyridine).32
Herein, we describe the electrocatalytic behavior of a cobalt(II) polypyridyl complex displaying an unusual combination of features, containing both a redox-active moiety and protic sites,55,57 potentially capable to set up a stabilizing hydrogen bond network around the bound CO2 molecule. Electrochemical measurements provide insights on the nature of the doubly reduced cobalt catalyst, the first reduction having a predominantly metal-based character and the second electron transfer being mostly localized on the ligand scaffold. According to theoretical calculations, the interaction of CO2 with this two-electron reduced complex results in a poorly reactive adduct. Nevertheless, this catalytically-competent intermediate is capable to slowly release CO and HCOOH, with a product distribution depending on the reaction conditions.
Due to the steric constraints originating from the two hydrogen atoms in ortho positions on the pyridine units, the bapbpy ligand adopts a saddle-shaped structure. To gain some insight on this type of twisted configuration, Bonnet and co-workers introduced the use of specific dihedral angles (Table S2†).60 Interestingly, the angles measuring terminal pyridines (β) and coordination plane torsions (γ and γ′) remain mostly unaffected by the change in the coordination number. On the contrary, the one describing the degree of rotation between the two rings forming the bipyridine motif (α) is dramatically modified, rising up from 6.53° in the pentacoordinated structure [1-Cl]+ to 16.66° in the hexacoordinated configuration [2-Cl2]. A combination of DFT calculations and electrochemical measurements (vide infra) have been undertaken in order to investigate the respective weight of each of these two structures in solution, highlighting the prominence of the pentacoordinated structure [1-Cl]+.
In an effort to further support the assignments of the different redox processes observed for complex [1-Cl]+, DFT calculations were conducted. The geometries of [1-Cl]+ and these one- and two-electron reduced species were thus optimized (Fig. S3†) and their electronic structures investigated in detail. When compared with the experimentally-obtained X-ray structure, the DFT-optimized structure of [1-Cl]+ appears in good agreement confirming that the pentacoordinated complex can be best described as a high-spin CoII complex with a quartet ground spin state (S = 3/2, Table S3†). One-electron reduction is metal-based, forming a species with a triplet ground spin state (S = 1, Tables S3 and S4†): the singly occupied molecular orbitals (SOMO) of [1-Cl]0 indeed have a dominant metal-based character (Fig. 3). The lability of the chloride ligand following mono-reduction has been evaluated, suggesting that chloride loss provides a slightly more stable adduct (Table S5†).
However, should the chloride ligand be released upon reduction to the CoI oxidation state, the reversibility of the CoII/CoI couple should be significantly affected. Indeed, [CoII(bapbpy)Cl]+ would be first reduced to [CoI(bapbpy)Cl]0, but only [CoI(bapbpy)]+ would be present for re-oxidation in the anodic sweep. As a consequence, the remarkable reversibility of the CoII/CoI electrochemical system is a strong evidence in favor of chloride retention on the timescale of the cyclic voltammetry measurements. This suggests slow kinetics associated with the chloride loss from the one-electron reduced species, [1-Cl]0. The second reduction process occurs on the bipyridine moiety of the bapbpy ligand and generates a delocalized ligand-based radical species having a quartet ground spin state (S = 3/2, Tables S3 and S6†), so that two-electron reduced species can be best described as a [CoI(bapbpy˙−)] complex, [1]0 (Fig. 4). Indeed, calculations strongly support chloride ligand expulsion upon reduction, providing a reasonable explanation to the poor reversibility of the more cathodic redox system (Table S7†).
As previously described, two different forms of the CoII complex have been identified in the solid state: the positively charged five-coordinate complex [1-Cl]+ and the neutral six-coordinate complex [2-Cl2]. If these two species coexist in solution, some measurable metrics describing their electrochemical behavior are likely to be affected by the equilibrium described in eqn (8).62,63 From that perspective, it is thus interesting to note that: (i) increasing scan rate leads to an apparent decrease of the current function (Fig. S4†) and (ii) the ratio ip,a/ip,c describing the reversibility of the CoII/CoI couple is maintained over the unity and further increases with scan rate (Fig. S5†). Taken together, these results provide evidences in favor of the existence of an equilibrium preceding the reduction process, according to a CE-type mechanism (where E corresponds to an electron transfer step and C to a chemical reaction).
[CoII(bapbpy)Cl]+ [1-Cl]+ + Cl− ↔ [CoII(bapbpy)Cl2] [2-Cl2], Ka | (8) |
To further support this assignment, we sought to change the balance between the pentacoordinated [1-Cl]+ and hexacoordinated [2-Cl2] complexes by modification of the free chloride anion concentration (Fig. S6†). Plotting the half-wave potential of the CoII/CoI couple as a function of the logarithm of the chloride concentration provides meaningful information related to the chloride coordination to the metal center (Fig. 5). From this data, two main regimes can be defined. At low concentration (≤1 mM), the half-wave potential of the CoII/CoI couple is only slightly modified suggesting the establishment of a plateau. At concentrations above 3 mM; a linear decrease of potential with log([Cl−]) is observed with a slope of −52 mV dec−1, the CoII/CoI potential shifting towards more negative potentials as the chloride concentration increases.
Theoretical description of similar system has previously been proposed by Savéant and Xu.64 However, the exact concentration of free chloride ions in solution prior to addition being unknown, only a rough estimate of the equilibrium constant −3.5 < log(Ka) < −2.5 can be determined from the intersection of the plateau and the linearly decaying trace. This set of data is in complete agreement with the existence of an equilibrium preceding the redox events, [1-Cl]+ being the dominant species in solution in the absence of any added chloride. Using tetrabutylammonium bromide in the same concentration range did not significantly affect the potential of the CoII/CoI couple, indicating that hard ligands – such as chloride anions – are required to trigger the formation of hexacoordinated species. DFT calculations further support the slightly higher stability of the pentacoordinated complex [1-Cl]+, when compared to [2-Cl2] (Table S8†).
Due to its ability to serve as an oxide acceptor and to trigger proton-coupled electron transfers, addition of water has been shown to usually dramatically facilitate electro-assisted CO2 reduction.20,65–67 Increasing the water content of the electrolyte up to 3.0 vol% induces some noticeable changes on the CVs shape (Fig. 6B). The electrocatalytic wave was indeed anodically shifted together with a significant increase of the catalytic current, reaching a plateau above about 1% of water in the medium (Fig. S8†). This apparent enhancement of the catalytic ability of [1-Cl]+ in the presence of water also appears to affect the CoII/CoI couple. While maintaining its remarkable reversibility, the CoII/CoI couple is indeed shifted towards anodic potentials when increasing amounts of water are added. This observation strongly suggests the existence of protonation steps that are coupled to the first reduction of [1-Cl]+, as previously demonstrated in the presence of weak acids.55 Plotting the evolution of the CoII/CoI process as a function of the concentration of water in the electrolyte, resulted in a saturation curve (Fig. S9†): the CoII/CoI reduction is facilitated in the presence of low contents of water (<1.5%), any further addition having no observable effect.
As previously shown, the speciation of the cobalt complex [1-Cl]+ can be manipulated by adding excess chloride anions. In order to determine if the number of chloride ligands initially coordinated to the Co(II) center is likely to affect the electrocatalytic properties of the system, we investigated the electrochemical behavior of [1-Cl]+ under CO2 and in the presence of increasing amounts of tetrabutylammonium chloride (TBACl). Under CO2, the progressive addition of TBACl to the electrolyte solution resulted in some modifications of the electrochemical response of [1-Cl]+ (Fig. 6C). Beyond the changes observed on the CoII/CoI couple and previously investigated (vide supra), it is interesting to note that the electrocatalytic wave is doubly affected by: (i) an increased magnitude of the catalytic peak current (Fig. S10†) and (ii) a slight shift of the catalytic wave onset towards the more negative potentials. Such dual consequences probably emerge from conflicting effects of chloride addition to the medium. The increased catalytic current may arise from chloride assistance to the catalytic process as a kinetically-efficient carrier of proton traces, as previously demonstrated by Darensbourg and co-workers68,69 In contrast, the negative shift of the onset potential could be attributed either to (i) chloride coordination to the metal centre disfavoring CO2 binding or (ii) bapbpy ligand flexibility loss due to effective hydrogen bonds. Alternatively, chloride binding to a catalytic intermediate may contribute to both shift of the potential at more negative values and increased catalytic rate.
Entry | [1-Cl]+ (M) | Additives | Charge (C) | FECO (%) | FEHCOOH (%) | FEH2 (%) | FEtotal (%) |
---|---|---|---|---|---|---|---|
A | 1 × 10−3 | — | 5.93 | 7.4 | 7.9 | 0 | 15.3 |
B | 1 × 10−3 | H2O 2% | 7.85 | 15.7 | 5.4 | 2.9 | 24.0 |
C | 1 × 10−3 | H2O 10% | 11.59 | 11.3 | 7.7 | 7.9 | 26.9 |
D | 1 × 10−3 | TBACl 50 mM | 5.18 | 8.9 | 7.4 | 1.3 | 17.6 |
E | 0 | — | 0.503 | 0 | 0 | 0 | 0 |
When performed in DMF containing 2% of water (Table 1, entry B), CPE allows clear improvement of the product selectivity towards the generation of CO (FECO = 15.7% and FEHCOOH = 5.4%, at −1.95 V vs. Fc+/Fc). Increasing further the water content, however, has a negative impact on product distribution and faradaic efficiencies (Table 1, entry C). This behavior strongly contrasts with the situation found in the recent studies of McCrory65 and Fujita,28 where high faradaic efficiency towards CO or HCOOH formation was reached at high water contents only. It is interesting to note that, although still quite limited, hydrogen evolution starts to occur under such conditions. In the presence of a large excess of chloride anions (Table 1, entry D), only a slight increase of the faradaic efficiency associated with the formation of CO was observed.
Regardless the nature of the electrolyzed mixture, an initial current build-up was observed together with darkening of the initial yellow solution. Interestingly, this color change persists – even after the end of the CPE – as long as the solution is maintained under CO2 and kept free of oxygen. When opening the electrochemical cell to the air, the solution color turns back to the initial yellow color. This observation, associated with the modest faradaic efficiencies and UV-vis characterization of the chemically reduced catalyst (vide infra), suggest the existence of a reduced species that is able to trap two electrons and thus to hamper further catalytic processes. Such electron sink is expected to actually accounts for about 15 to 35% of the overall electrons passed through the system during CPE. In that prospect, three situations can be considered: (i) a poor interaction between the two-electron reduced cobalt complex [1]0 and CO2, (ii) a low reactivity of a [CoI(bapbpy˙−)(COO)] adduct towards the formation of the reduction products or (iii) a carbonyl-trapped cobalt complex.
TD-DFT calculations were performed on the series of complexes and the predicted spectroscopic data provides calculated spectra that compare well with the experimental observations (Tables S9–S11 and Fig. S11†). Our computations support that the UV-vis spectrum of [1-Cl]+ is dominated by three main absorption bands of different intensity while progressive reduction of the complex with one and two electrons resulted in the appearance of new electronic transitions in the [400–900] nm range. [1-Cl]0 and [1]0 display similar UV-vis spectra but with an increased intensity for the low-energy bands of the latter. The spectral features characterizing [1-Cl]+ are all assigned to charge transfers from the ligand to metal (LMCT, Fig. S12†). For [1-Cl]0 and [1]0 the additional transitions observed in the visible region display mixed characters with contributions from the metal and the ligand in the donor states and only from the ligand in the acceptor states. The NIR absorptions for the reduced complexes correspond to charge transfers with similar contributions from the metal and the ligand in both donor and acceptor states, but where the donor state involves the reduced bpy fragment of the ligand while the acceptor state involves the pyridine fragments with less excess electron density due to reduction of the complex (Fig. S13 and S14†). Our TD-DFT calculations thus adequately reproduce the energy of the key features of the experimental spectra which further support the geometries and electronic properties of [1-Cl]+, its reduced one- and two-electron reduced states.
The reactivity of [1-Cl]0 and [1]0 towards carbon dioxide was investigated by subjecting DMF solutions of the reduced species to 1 bar of CO2 in Fisher–Porter tubes. To avoid potential side reactions related to the presence of different cobalt species in the mixture, KC8 was employed as the reductant for this series of measurements providing similar UV-vis spectra for the one- and two-electron reduced species (Fig. S15A†). Whereas a rapid color change from dark brown to dark yellow was observed in the case of [1]0, no significant modifications were observed for the singly-reduced compound [1-Cl]0 within the same timeframe, indicating that CO2 is quickly reacting with the doubly reduced species (Fig. S15B†). Two main situations are possible: (i) the formation of a low-reactive CO2-adduct or (ii) the generation of a carbonyl-bearing cobalt complex. To deeper investigate these possibilities, the IR spectrum of the reduced species under CO2 was recorded. Due to the DMF absorptions, the IR region under investigation was limited to 1800–2700 cm−1 where cobalt carbonyl complexes have previously been evidenced.28,70 In our case, no new CO stretching bands were observed supporting the CO2-adduct hypothesis.
Interestingly, the CO2-adduct is best described as a [CoI(bapbpy˙−)(COO)] complex having a doublet ground spin state due to an effective antiferromagnetic coupling between the metal center and the ligand-based radical (Fig. S20, S21 and Table S14†). In consequence, coordination of CO2 to the metal center does not result in significant charge redistribution within the newly-bound CO2 ligand-centered orbitals. The merely increased electron density in the bound CO2 molecule only results in a moderate bending of the O–C–O angle of 32°. Such electronic reorganization has been proposed as a crucial step of the catalytic process.14,15 As a result, the bound CO2 molecule is only weakly activated due to an effective electron trapping within the bapbpy ligand platform. Further reactivity with oxide acceptors, such as carbon dioxide or protons, is thus expected to be significantly altered limiting catalytic performances.
A plausible mechanism for the electro-assisted reduction of CO2 by [1-Cl]+ is displayed on Fig. 8. Complex [1-Cl]+ undergoes two one-electron transfers associated with two different loci: a first metal-based reduction that generates [CoI(bapbpy)Cl]0 and a second ligand-centered process yielding [CoI(bapbpy˙−)Cl]−. Chloride loss, followed by CO2 binding produced the two-electron reduced complex [CoI(bapbpy˙−)(CO2)]0. The limited electronic reorganization of the two-electron reduced species upon CO2 binding is characteristic of an electron trapping within the bapbpy scaffold. Such behavior impedes the efficient formation of a metallocarboxylate intermediates and thus hampers further reactivity towards the formation of the two-electron reduced products (CO and HCOOH).
Footnotes |
† Electronic supplementary information (ESI) available. CCDC 1970564 and 1970565. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/d0se00570c |
‡ Current address: CNRS, LCC (Laboratoire de Chimie de Coordination), 31077 Toulouse, France. |
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