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Article

Quantum Chemical Topological Analysis of [2Fe2S] Core in Novel [FeFe]-Hydrogenase Mimics

Department of Physical Chemistry, Faculty of Chemistry, University of Lodz, Pomorska 163/165, 90236 Lodz, Poland
Crystals 2025, 15(1), 52; https://doi.org/10.3390/cryst15010052
Submission received: 28 November 2024 / Revised: 26 December 2024 / Accepted: 1 January 2025 / Published: 3 January 2025
(This article belongs to the Section Materials for Energy Applications)

Abstract

:
Synthetic mimics of the active site of [FeFe]-hydrogenase enzymes are important in the context of catalytic hydrogen production for future energetic applications. Providing a detailed quantum chemical description of the catalytic center of such mimics contributes to a better understanding of their behavior in hydrogen production processes. In this work, the analysis of bonds in the butterfly [2Fe2S] core in a series of complexes based on recently synthesized [FeFe]-hydrogenase mimics has been carried out using a wide range of quantum chemical topological methods. This series includes hexacarbonyl diiron dithiolate-bridged complexes with the bridging ligand bearing a five-membered carbon ring functionalized with diverse groups. The quantum theory of atoms in molecules (QTAIM) and the electron localization function (ELF) provided detailed characteristics of Fe–Fe and Fe–S bonds in the [2Fe2S] core of the complexes. A relatively small amount of strongly delocalized electron charge is attributed to the Fe–Fe bond. It was established how the topological parameters of the Fe–Fe and Fe–S bonds are affected by the five-membered carbon ring and its functionalization in the bridging dithiolate ligand. Next, one of the first applications of the interacting quantum atoms (IQA) method to [FeFe]-hydrogenase mimics was presented. The pairwise interaction between the metal centers in the [2Fe2S] core turns out to be destabilizing in contrast to the Fe–S interactions responsible for the stabilization of the entire core.

Graphical Abstract

1. Introduction

Synthetic organometallic complexes inspired by the active site of [FeFe]-hydrogenase enzymes have attracted much attention for the past two decades [1,2,3,4,5,6,7]. [FeFe]-Hydrogenases are well known in nature for their catalytic activity toward the reversible conversion of protons and electrons into dihydrogen with high turnover frequencies [5,6,7], which nowadays is also recognized as a promising approach for H2 production within green energy solutions [8,9]. In naturally occurring [FeFe]-hydrogenases, this conversion is thought to take place in a dithiolate-bridged diiron subsite [10], whose [2Fe2S] core displays a butterfly geometrical arrangement [1]. The potential of H2 production processes for future energetic applications has generated a great deal of interest in the design and consequent synthesis of organometallic complexes demonstrating structural and functional resemblance to the catalytic site of [FeFe]-hydrogenase enzymes [6,7,11]. The resulting [FeFe]-hydrogenase mimics are often based on the [2Fe2S] core with its metal centers coordinated by terminally bound CO ligands and by a bridging dithiolate, in which two sulfur atoms may be linked via three carbon atoms (μ-S2C3) of a larger substituted moiety [6]. For example, a series of hexacarbonyl diiron dithiolate-bridged complexes with the bridging ligand bearing a five-membered carbon ring functionalized by aryl, hetaryl, and/or ferrocenyl groups have quite recently been synthesized and structurally characterized by X-ray crystallography [12]. However, most [FeFe]-hydrogenase mimics are much less efficient in H2 production than the naturally occurring enzymes [1,2,3]. What is worse, many mimics tend to form a catalytically inactive μ-hydride complex [13]. Changes in the bridging and terminal ligands of the mimics have an influence on the electronic properties of their Fe centers, and consequently, on the probability of μ-hydride complex formation [14]. Thus, a detailed characterization of the electronic structure features of the [2Fe2S] core in [FeFe]-hydrogenase mimics may help in a better understanding of their behavior in the reduction of protons to dihydrogen [14].
In continuation of our ongoing interest in the reactivity and properties of aromatic thioketones [15,16,17,18], a series of novel [FeFe]-hydrogenase mimics 1, 35, and 7 (Figure 1) have recently been synthesized in reactions of α,β-unsaturated aromatic thioketones (that is, thiochalcones) with triiron dodecacarbonyl Fe3(CO)12 [12]. For 3, 5, and 7, their single crystals suitable for X-ray diffractometry have been obtained [12] and their XRD structures have also been used to benchmark density functional theory (DFT) methods [19]. In the present work, these newly synthesized mimics, their congeners with diverse Ar1 and Ar2 groups (Figure 1), the archetype of the [FeFe]-hydrogenase catalytic site, namely [Fe2(pdt)(CO)6] (pdt = propanedithiolate) 10, as well as the by-product 11 from the synthesis of 4, were considered to provide insight into the nature of bonds in their [2Fe2S] core and to establish whether these bonds are affected by the five-membered carbon ring of the dithiolate ligand and its functionalization with Ar1 and Ar2. To that end, the [2Fe2S] core of complexes 111 was analyzed from a quantum chemical topology (QCT) perspective.
In general, the computational QCT methods [20] operate on real physical space in which the spatial distributions of scalar fields such as the charge density (ρ) in the quantum theory of atoms in molecules (QTAIM) [21] and the electron localization function (ELF) [22] are studied to provide detailed information on the nature of chemical bonds. As an extension of the long-known QTAIM, the non-covalent interactions (NCI) index [23,24] later introduced an additional scalar field, namely the reduced density gradient (RDG), into the analysis of ρ to identify, in a semi-quantitative fashion, the real-space regions of weak interactions. By modifying the RDG slightly, the interaction region indicator (IRI) [25] was also proposed to visually reveal both strong covalent bonds and weak interactions in chemical systems. The theory of interacting quantum atoms (IQA) [26] is a profound extension of the QTAIM that has lately gained great popularity because it provides an exact partition of total molecular energies into intra- and inter-atomic quantities with clear physical meaning and no external references [27].
The aforementioned QCT methods were employed in this work to shed light on the nature of bonds in the [2Fe2S] core of 111. In addition to the metal–metal interaction in this core, we particularly focus on the bonds between the metal centers and the bridging dithiolate of 111 because generally much less is known about such metal–ligand bonds in contrast to a wealth of information on transition metal–carbonyl bonds [28,29]. To the best of our knowledge, the use of QCT methods for studying [FeFe]-hydrogenase mimics with the μ-S2C3 linker of a dithiolate ligand has been restricted mostly to the QTAIM analysis of archetypical complex 10 so far [30,31,32,33]. This methodological narrowing prompted us to utilize here a wide range of QCT methods.

2. Computational Details

The geometrical structures of complexes 111 in the singlet ground state were fully optimized at a spin-unrestricted DFT level of theory. The initial molecular geometries of 3, 5, 7, 10, and 11 were extracted directly from the corresponding XRD crystal structures [12,34]. These structures were also employed to generate the initial geometries of the remaining mimics by replacing Ar1 and Ar2 with the appropriate substituents (Figure 1). The geometry optimizations were carried out at the TPSSh/def2-SVP level of theory [35,36], which is in compliance with the computational methodology of our previous study [12]. Harmonic vibrational frequency calculations were carried out at the same level of theory to verify that each optimized geometrical structure corresponded to a local energy minimum. For comparison, an additional set of geometry optimizations and harmonic vibrational frequency calculations was performed using the B3LYP functional [37,38]. Aside from another functional, a more extended Karlsruhe basis set, that is, def2-TZVP [36], was also used in single-point energy calculations. The charge density generated from the unrestricted wave function at the resulting DFT levels was the starting point for analyses by means of such QCT methods as the IRI, the QTAIM, the source function (SF) [39], and the ELF. Because of its immense computational cost and available implementation, the IQA method was applied to the charge density obtained from the B3LYP/def2-SVP single-point energy calculations. Within the IQA partition of energy, a generalization based on grouping atoms into fragments in an approach referred to as the interacting quantum fragments (IQF) analysis [40] was also taken into account.
Geometry optimizations and harmonic vibrational frequency calculations were carried out using the TURBOMOLE 7.7 program [41]. Extended wavefunction files (.wfx files) were provided by the Gaussian 16 program [42] in a series of single-point energy calculations. The IRI and the ELF were computed with the latest development version of Multiwfn 3.8 [43]. The QTAIM, SF, and IQA implementations available in AIMAll 19.10.12 were used [44]. Graphical representations were generated by means of the VMD 1.9.3 [45] and AIMStudio 19.10.12 [44] programs. Further computational details can be found in Section S1 in Supplementary Materials. A link to the repository of Cartesian coordinates for the optimized structures of 111 is provided in Section S2.

3. Results and Discussion

3.1. Molecular Geometries

Before the analysis of QCT results commences, a geometrical characterization of the [2Fe2S] core in complexes 111 optimized at the TPSSh/def2-SVP and B3LYP/def2-SVP levels of theory needs to be presented briefly. The bond lengths calculated for the [2Fe2S] core of 111 are collected in Table 1. The [2Fe2S] core of 19 and 11 displays a butterfly arrangement with different lengths of its four Fe–S metal–ligand bonds due to the asymmetry of the bridging dithiolate ligand. It is evident that the TPSSh density functional generally yields somewhat shorter metal–metal and metal–ligand bonds in the [2Fe2S] core than those obtained from B3LYP. Comparison with the available experimental results derived from single-crystal X-ray diffraction measurements [12,34] reveals that the structures of the [2Fe2S] core are calculated with an accuracy of several pm, which is typical of DFT optimizations with double-ζ basis sets [46] and the neglect of crystal packing [19,47]. Both TPSSh and B3LYP overestimate the Fe–S bond lengths of 3, 5, 7, 10, and 11, whereas the calculated Fe–Fe bond tends to be too short relative to the experimental results.
The distance between the metal centers in complexes 110 is only slightly longer than the typical value of 232 pm for a single Fe–Fe covalent bond [48]. This geometrical prerequisite, along with the attainment of the favored 18-electron metal configuration, suggests the formation of a direct Fe–Fe bond in 110. For 9 and 10, their calculated Fe–Fe bond lengths are practically identical, and thus, it can be concluded that the presence of the five-membered carbon ring in the dithiolate bridge of 9 has a marginal effect on the Fe–Fe bond length. On the other hand, the introduction of aryl, hetaryl, and ferrocenyl substituents into the five-membered carbon ring allows us to distinguish certain trends in the length of Fe–Fe. In general, the Fe–Fe bond lengths calculated for 18 cluster around the value observed for the simplified (that is, methyl-substituted) analog 9. However, complexes 14 demonstrate slightly shorter Fe–Fe bonds than complex 9. By contrast, the presence of ferrocenyl groups in 58 results in a minor elongation of Fe–Fe bond as compared to its length in 9.
As for the Fe–S metal–ligand bonds of 110, their calculated lengths exceed by 8–15 pm the typical value of 219 pm for a single Fe–S covalent bond [48]. Across the series of 110, it is difficult to notice a clear trend in the length between particular Fe and S atoms. Instead, keeping track of changes in the average length of four Fe–S bonds allows us to single out the effect of Ar1 and Ar2 conclusively (Table 1). Then, the Fe–S bonds of 14 are longer on average than those calculated for 9. The opposite trend can be observed for the average Fe–S bond lengths of 58.
Complex 11 adopts a distorted geometry of its [2Fe2S] core that strikingly stands out from the [2Fe2S] geometries found for 110. The Fe–Fe bond of 11 undergoes a noticeable elongation which is accompanied by a rearrangement in the coordination sphere of the Fe1 center (Figure 1). The S2 atom is moved away from the Fe1 center, while the C1 atom enters the coordination sphere of Fe1. As a result, the Fe1–S2 bond is longer by at least 57 pm than the remaining three Fe–S bonds. The calculated Fe1–C1 bond length amounts to 213.1 pm and 216.5 pm at the TPSSh/def2-SVP and B3LYP/def2-SVP levels, respectively. The former perfectly reproduces the experimental result.

3.2. IRI Analysis

A preliminary insight into the interactions occurring in the [2Fe2S] core of 111 was obtained by means of the IRI topological analysis yielding a visual representation of real-space regions where various kinds of interactions could be identified. In Figure 2, the IRI isosurface is plotted for the [2Fe2S] core of complexes 9 and 11 that were optimized at the TPSSh/def2-SVP level of theory.
The IRI isosurface for the [2Fe2S] core of 9 is essentially identical to those of 18 and 10. Within the [2Fe2S] core of 9, each Fe–S interaction is characterized by a blue IRI area that is practically round in shape with its center lying on the axis linking these Fe and S atoms. Such features of the IRI isosurface signal the presence of chemical (covalent) bonds, the metal–ligand bonds in our case. Similarly, a blue area of the IRI isosurface can be observed between Fe1 and Fe2, indicating the region of a covalent interaction involving the metal centers. This area turns into red while moving away from the Fe–Fe bond axis, which in turn signals the appearance of repulsive interactions due to steric congestion inside two three-membered rings formed by one S and two Fe atoms.
Within the [2Fe2S] core of 11, the IRI isosurface delineates a blue disk transversely across the Fe1–C1 axis, in addition to three Fe–S blue areas of attractive interactions. This implies the presence of four covalent metal–ligand bonds in complex 11. There is also an attractive interaction between the metal centers. The complex does not exhibit any covalent metal–ligand bond between Fe1 and S2 because no blue IRI area shows up between these atoms.

3.3. QTAIM Analysis

Next, the conventional QTAIM topological analysis of ρ was performed to characterize the properties of bonds in the [2Fe2S] core in 111. The QTAIM molecular graphs of 9 and 11 are plotted in Figure 3. With the aim of plotting these molecular graphs, the geometrical structure of the complexes and their ρ distribution were calculated at the TPSSh/def2-SVP level of theory. Again, complex 9 was selected as the representative of 110 because its molecular graph depicts the [2Fe2S] core sharing common topological features to the whole series of these complexes. The QTAIM analysis of the [2Fe2S] core in 9 detects a bond path (BP) connecting the metal centers, as well as four BPs associated with the Fe–S metal–ligand bonds. Along each of the BPs, which mark out the lines of concentrated ρ linking pairs of atomic centers, there is a saddle point in ρ, called the bond critical point (BCP). From the QTAIM point of view, the presence of a BP and a BCP between two atoms meets the necessary and sufficient condition that these atoms are bonded to one another [49]. The five BPs within the [2Fe2S] core form two adjacent rings, each of which involves one Fe–Fe and two Fe–S BPs, and thus, they give rise to two ring critical points. These ring critical points are located in the regions earlier encompassed by an IRI isosurface mapped with red color where repulsive interactions were revealed (Figure 2). The QTAIM molecular graph for complex 11 also shows five BPs within its [2Fe2S] core, yet the Fe1–S2 BP is replaced with the Fe1–C1 one. Obviously, the different QTAIM topology for the [2Fe2S] core of 11 reflects changes in its geometry and in the coordination of the Fe1 center.
To obtain more information about the nature of Fe–Fe and Fe–S bonds, the local topological properties of ρ at the corresponding BCPs were examined. The QTAIM characteristics of Fe–Fe bond locally at its BCP are summarized in Table 2 for 111 in their geometries optimized at the TPSSh/def2-SVP level of theory. The BCP between the Fe1 and Fe2 atoms of 111 is described by relatively low values of ρBCP (<0.1 atomic units) and its Laplacian (∇2ρBCP < 0.1 atomic units). The latter adopts the plus sign, suggesting a region of charge depletion around the BCP and the closed-shell category of inter-atomic interaction [21]. The magnitudes of ρBCP and ∇2ρBCP for the BCP of Fe–Fe in 111 are quite typical of formally single metal–metal bonds in binuclear complexes [50,51], including those with diiron centers [52]. Moreover, the ρBCP and ∇2ρBCP values calculated for 10 are in good agreement with earlier theoretical results reported for this archetypical complex [30]. There are also other local QTAIM parameters that are more sensitive to the nature of bonds than the ρBCP itself or ∇2ρBCP. The total energy density at the BCP of Fe–Fe (HBCP), which is the sum of the potential energy density (VBCP) and the kinetic energy density (GBCP), is negative yet close to zero. Thus, a certain amount of covalency may be assigned to the interaction between Fe1 and Fe2 [53]. The negative value of HBCP results from the domination of VBCP over GBCP; the total amount of kinetic energy (GBCP/ρBCP) is small (<<1). Moreover, the adimensional ratio of energy densities (|VBCP|/GBCP) falls into the range between 1.0 and 2.0, and therefore, it categorizes the Fe–Fe interaction as intermediate between pure closed shell (that is, ionic) and pure electron shared (that is, ‘classical’ covalent) [54]. The values of the energy densities at the BCP of Fe–Fe conform with the QTAIM criteria for metallic bonds [54,55]. The calculated values of the delocalization index (δ) [56] between Fe1 and Fe2 in 111 also support the conclusion on the partial covalent character of the Fe–Fe bond. These values are slightly smaller than 0.5, which means that approximately half an electron is shared between the metal centers.
Variations in the QTAIM characteristics at the BCP of Fe–Fe can be noticed upon the substitution of Ar1 and Ar2 in 18. These variations are rather small in magnitude, yet they disclose important regularities. The ρBCP and ∇2ρBCP values in 14 are larger than in 9, which is associated with the shortening of the Fe–Fe bond in the former. The opposite trend in ρBCP and ∇2ρBCP pertains to complexes 58, in which the elongation of their Fe–Fe bonds is observed. Comparison of the δ values between the metal centers of 19 and 10 indicates that the five-membered ring of dithiolate ligands leads to a decrease in the number of electrons shared between the metal centers. The decrease in the delocalization index between Fe1 and Fe2 is more evident for complex 11. The elongated Fe–Fe bond of this complex quenches the electron sharing, and this is accompanied by smaller ρBCP and ∇2ρBCP values.
In regard to the Fe–S bonds in 110, all four BCPs between the Fe and S atoms in each complex show much the same QTAIM characteristics. The following discussion relies on the data gathered in Table 3 for the BCP of Fe1–S1 in 110, but consistent findings come from the analysis of the remaining three BCPs (Tables S1–S3 in Supplementary Materials). The ρBCP parameter at the BCP of Fe–S is generally of the same order of magnitude as that at the BCP of Fe–Fe. By contrast, the ∇2ρBCP values for the Fe–S bonds are significantly more positive than for the Fe–Fe bond. The negative HBCP values evidence a certain covalent degree for the Fe–S bonds. Furthermore, the δ values of approximately 0.7 imply that less than one electron is shared (or exchanged) between Fe1 and S1. This is in line with the experimental and theoretical findings on the partial covalent character of Fe–S interactions in hydrogenase mimics [57,58]. It is also known that the δ parameter provides an effective way of quantifying Fe–S covalency [58] and its values prove lower Fe–S bond covalency for 110 than for biomimetic iron–sulfur clusters containing bridging sulfide and terminal thiolate ligands [58]. Both |VBCP|/GBCP and GBCP/ρBCP adopt values that are fairly close to unity for the Fe–S bonds in 110. The magnitudes of all these local QTAIM parameters essentially match the QTAIM characteristics of many Fe–S metal–ligand bonds reported previously for iron complexes [52,59,60]. On the basis of the values obtained for these parameters, the Fe–S bonds in 110 belong to a transit closed shell class [61], lying between purely ionic and purely covalent limits. More specifically, they can be described as a donor–acceptor kind of bonds [54,55].
The substitution of Ar1 and Ar2 in 19 affects the QTAIM parameters at the BCPs of individual Fe–S metal–ligand bonds, and the resulting trends in these parameters essentially follow variations in the lengths of these bonds. Accordingly, longer Fe–S metal–ligand bonds tend to show smaller values of ρBCP and δ. The same changes in the topological characteristics of Fe–S bonds in complex 10 are observed upon introducing the five-membered ring into the dithiolate ligand, as occurs in complex 9. For the Fe–S bonds of complex 10, their δ estimations presented in this work agree well with the results of previous calculations [31].
For complex 11, the shortening of its Fe1–S1 bond (as well as Fe2–S1 and Fe2–S2) results in an increase in the absolute values of the local topological parameters describing this bond, but it remains a donor–acceptor character, nonetheless. The QTAIM characteristics of the Fe1–C1 bond (Table S4) are essentially similar to that of Fe–S in 11.
The last aspect of the QTAIM analysis that deserves a word of comment is the dependence of the obtained results on the basis sets and DFT functionals used. Extending the basis set from def2-SVP to def2-TZVP usually results in noticeable variations in the values of QTAIM parameters for the [2Fe2S] core of 110 (Table 2 and Table 3). This means that the def2-SVP basis set does not suffice to approach the basis set saturation close enough to generate the reasonably converged charge density. Only the ρBCP and δ values for Fe1–Fe2 change marginally upon increasing the basis set size. It is worth emphasizing that no BP and the related BCP were found between Fe1 and Fe2 in 11 while using the charge densities obtained from the TPSSh/def2-TZVP and B3LYP/def2-TZVP single-point calculations. This revealed that the topology of the [2Fe2S] core in 11 is close to a catastrophe point relating to the Fe1−Fe2 bond path. In this sense, the QTAIM picture of Fe–Fe in 11 is similar to that reported for Fe2(μ-S2)(CO)6 and Fe2(CO)9, in which the presence or absence of an Fe–Fe BCP was also dependent on the basis set used [52,62]. As for the dependence on the density functional used, TPSSh and B3LYP yield quite close values of the QTAIM parameters for the [2Fe2S] core of 111 despite differences in the optimized geometries (Tables S5–S9). In consequence, both functionals produce consistent trends in these parameters.

3.4. SF Analysis

We have also involved the SF method to distinguish percentage contributions from individual atoms in the [2Fe2S] core of 111 to the accumulation of ρ at the BCPs of Fe–Fe and Fe–S. At the BCP of Fe–Fe in 110, two percentage source function (%SF) contributions from the metal centers sum up to merely 8–9%, while the contributions from S1 and S2 amount to 23–24% in total at the TPSSh/def2-SVP level (Table S10). The %SF contribution from the Fe2 atom in 11 becomes negative, which means this metal center behaves as a sink, rather than a source, for the ρBCP value. The %SF contributions originating from the CO ligands predominate at the BCP of Fe–Fe for all complexes. This seems to construe the Fe–Fe bond in 111 as a highly delocalized (non-local, multicenter) interaction that is strikingly different from a typical single covalent bond [63]. As for the ρBCP value of each Fe–S metal–ligand bond in 111, the S atom forming such a bond provides the leading %SF contribution, and the two linked atoms supply more than half of the ρBCP value (Table S11). These relatively high %SF contributions from the bonded atoms speak for a more local character of Fe–S with respect to Fe–Fe. They are also mirrored in the δ values of approximately 0.7 for Fe–S in 111.

3.5. ELF Analysis

We move now to the ELF method to inspect an alternative real-space scalar field that can be a valuable indicator of electron localization and the local pairing of electrons. The topology of the ELF for the [2Fe2S] core of 111 identifies a disynaptic valence bonding attractor (that is, a local maximum of the ELF) between Fe1 and Fe2. Its essential features are summarized in Table 4. The localization domain surrounding this attractor in complex 1 calculated at the TPSSh/def2-SVP level of theory is displayed in Figure 4. The Fe–Fe attractor signals a shared electron interaction, yet its small value (ELFmax < 0.5) means a great electron delocalization due to the Pauli repulsion exerted by the charge density concentrated in the core regions of the metal atoms. The basin of this attractor is populated by an average number of electrons ( N ¯ ) amounting to ca. 0.5e, mainly thanks to the charge density of the atomic basins of Fe1 and Fe2. The contributions from the Fe1 and Fe2 basins are almost equal for each complex except complex 11 for which a greater contribution from Fe2 is observed. The relative fluctuation (λ) of the Fe–Fe basin population is high, which in turn confirms that the charge density inside this basin is strongly delocalized. In that regard, the λ values for the Fe–Fe bond in 111 are similar to those reported for Fe–Fe in the Fe4 cluster [64]. The small population and the significant relative fluctuation of ρ for the disynaptic Fe–Fe basin in 111 are not typical features of a ‘classical’ covalent bond—rather, they highlight its metallic and essentially delocalized character. This finding agrees with our conclusions yielded by the QTAIM and SF analyses. Moreover, the calculated N ¯ values of Fe1–Fe2 in 110 confirm that the presence of the five-membered carbon ring in the dithiolate ligands decreases the Fe1–Fe2 basin population, which compares with the trend in δ.
The ELF topology of the [2Fe2S] core in 110 reveals four valence bonding attractors describing the Fe–S metal–ligand bonds. Not all of them are identified as disynaptic Fe–S attractors: depending on the complex analyzed, at least two are recognized as trisynaptic, corresponding to the basins in which one S atom and two Fe atoms participate. The localization domains connected with the four attractors in complex 1 are marked in color in Figure 4. Several ELF parameters for the Fe1–S1 basin of 111 as an example of Fe–S metal–ligand bonds in these complexes are collected in Table 5. In comparison to the Fe1–Fe2 basin, the Fe1–S1 one is characterized by much larger ELF values of its attractor, which suggests a low probability of local parallel spin electron pairing. Instead, finding an antiparallel spin pair may be expected in the region between Fe1 and S1. The λ values of the Fe1–S1 basin population in 111 are still high yet smaller than those of Fe1–Fe2. They reflect a noticeable delocalization of the charge density inside the Fe1–S1 basin. Integration of ρ over the Fe1–S1 basin yields an N ¯ value of ca. 1.6e. The population of this basin is determined by the dominant contribution from the atomic basin of S1, while the contribution from Fe1 does not exceed 0.25e. The second metal center provides a negligible contribution to the population of the Fe1–S1 basin. Even the Fe–S basins that are formally classified as trisynaptic show the contribution from one Fe atom being of one order of magnitude smaller than that from another Fe atom. Nonetheless, the occurrence of the trisynaptic basins suggests a certain degree of electron delocalization across two Fe–S bonds sharing the same sulfur atom. Thus, these bonds tend to become uniform. As a matter of fact, the ELF parameters of four Fe–S metal–ligand bonds in each of complexes 110 are very similar (Table 5 and Tables S12–S14) despite the fact that the coordinated sulfur atoms of the dithiolate ligands are formally three-electron donors. According to the ELF analysis, each of these coordinated sulfur atoms possesses a single monosynaptic valence non-bonding attractor corresponding to its lone pair that is not shared with the metal centers. The population of the sulfur lone pair basin is oversaturated by 0.5 to 0.7e, while the Fe–S basins conserve their non-saturated occupations (<2e). Bearing in mind the dominant S-atom contribution to the population of each Fe–S basin, the aforementioned ELF topological features of Fe–S bonds in 111 do not match the description of ‘classical’ covalent bonds but rather a donor–acceptor kind of bonds. Such a conclusion drawn from the ELF analysis is in accord with the previous ELF study of Fe–S bonds in iron–oxo porphyrin π-cation radical species [65].
The Fe1–C1 bond in complex 11 is characterized by a disynaptic valence bonding attractor between the Fe1 and C1 atoms. Similarly to the Fe1–S1 bond, the Fe1–C1 bond has ELF topological features of a donor–acceptor bond (Table S15). The contribution of ρ from the atomic basin of C1 predominates in the population of the Fe1–C1 valence bonding basin. There is no ELF bonding attractor between Fe1 and S2 in complex 11.
Trends in the ELF description of the Fe–Fe, Fe–S, and Fe–C bonds in the [2Fe2S] core of 111 calculated using the TPSSh functional are consistent with those obtained from the B3LYP functional (Tables S16–S20).

3.6. IQA and IQF Analyses

At the last stage of this QCT study, let us turn to the energetics of the Fe–Fe and Fe–S interactions occurring in the [2Fe2S] core of 111. The real-space energetic image of these interactions obtained from the IQA method allows us to present a new perspective on their nature and role in the stabilization of 111. An insight into this nature rests on the IQA pairwise inter-atomic interaction energy (Eint) partitioned into two components associated with the conventional notions of ionicity and covalency, namely a classical electrostatic component (Vcl) and a purely quantum–mechanical exchange–correlation component (Vxc), respectively. The IQA energies of Fe1–Fe2 and Fe1–S1 across the series of complexes 111 are collected in Table 6. The IQA results for Fe1–S1 share the main features with the remaining three pairs of Fe and S atoms in 110 (Table S21).
For each of the studied complexes, the interaction between its metal centers is characterized by a positive value of the Eint energy; thus, this interaction is associated with a destabilization. Its Vcl component adopts a positive value because there is an electrostatic repulsion between the positively charged metal centers (Table S22). The covalent-like Vxc component of Fe1–Fe2 is always stabilizing (i.e., negative) but the electron sharing between the metal centers is too small to compensate for the destabilizing Vcl component. The dominant role of Vcl in the destabilization of Fe–Fe interaction was also observed for a [Fe2(CO)8]2- complex showing a distance of 284.7 pm between its Fe atoms [66]. It is noteworthy that, despite the destabilizing Eint energy, a delocalized multicenter Fe–Fe bond involving carbonyl ligands was found to occur in the [Fe2(CO)8]2- complex. For complex 11, the elongation of its Fe–Fe bond diminishes the electron sharing between the bonded atoms and, in consequence, the Eint energy of Fe–Fe becomes even more positive than for 110.
It is instructive to elucidate the destabilizing Eint energy of Fe–Fe in light of the occurrence of the BP linking these atoms, the QTAIM implication being that the two atoms are bonded to one another. According to the IQA interpretation [67], the occurrence of this BP indicates the privileged exchange–correlation channel between the Fe atoms, and it is independent of the overall Eint destabilization due to electrostatic repulsion. The stabilizing Vxc component between the Fe atoms is intense enough to develop a BP linking them.
The pairwise interaction energy of Fe1–S1 is always stabilizing for complexes 110. The source of this stabilization is the highly negative Vxc component, highlighting the importance of the partial covalent character of the Fe–S bond. Additionally, the Vcl component of Fe1–S1 is also energetically favorable due to the electrostatic attraction between the positively charged Fe1 atom and the negatively charged S1 atom (Table S22). The IQA description of Fe1–S1 in 110 can be extended to the Fe1–S1 bond of complex 11. Furthermore, the IQA energies of Fe2–S1 and Fe1–C1 in 11 are actually of similar magnitudes to the corresponding energies of Fe1–S1 (Tables S21 and S23). However, the negligible charge acquired by the S2 atom in 11 (Table S22) diminishes the stabilizing electrostatic interaction of Fe2–S2. Bearing in mind that the S2 atom is pushed away from the Fe1 center of 11, their pairwise Eint energy is reduced by one order of magnitude in comparison to the Eint value of Fe1–S1. Interestingly, the Vcl value of Fe1–S2 becomes positive due to the destabilizing electrostatic contribution from higher atomic multipole moments (higher than monopoles).
Trends in the Eint energies of Fe–Fe and Fe–S in 18 essentially follow the changes in their bond lengths relative to those of the methyl-substituted analog 9. The shortened Fe–Fe bond of 14 is associated with the increased destabilization of Fe–Fe, while the elongation of Fe–Fe in 58 implies a lesser Fe–Fe destabilization than in 9. The summed Eint energies of all four Fe–S bonds in 14 is less stabilizing than that of complex 9, whose Fe–S bonds are shorter. These trends can be simply explained by the distance dependence of the dominant IQA contribution. Growing inter-atomic distances reduce both the electrostatic repulsion between two Fe atoms and the electron sharing between the Fe and S atoms. Compared to complexes 19, archetype 10 shows a less destabilizing Eint of Fe–Fe and simultaneously a less stabilizing Eint of all four Fe–S bonds. The introduction of the five-membered carbon ring into the dithiolate ligand of 19 results in the growing stabilization of Vcl for all four Fe–S bonds. The Vxc energies of Fe–Fe and Fe–S in 111 correlate with the corresponding δ values because both these quantities are a signature of electron sharing.
From the IQA results presented above, it can be inferred that the Fe–S interactions are the main source of [2Fe2S] stabilization in 111; even a single Fe–S interaction suffices to compensate the destabilization produced by the interaction between the metal centers. Within the [2Fe2S] core of 111, there is also a stabilizing interaction between S1 and S2, but this interaction is extremely weak and thus plays a negligible role in [2Fe2S] stabilization (Table S24).
Finally, the IQF analysis is employed to dissect the interaction between the diiron and dithiolate fragments of complexes 111 and thus to establish how the strength and nature of this interaction is affected by the dithiolate ligand as a whole. The calculated IQF Eint energies between these two fragments in 111 and their Vcl and Vxc components are listed in Table 7. The IQF Eint energy is stabilizing for all dithiolate ligands and its Vxc component provides the main stabilizing contribution to the interfragment interaction. This stresses again the great relevance of electron sharing to this interaction. From the negative value of the IQF Vcl component, it can be inferred that the interfragment interaction is strengthened by the electrostatic attraction between the positively charged diiron center and the dithiolate ligand, acquiring an ancillary electron charge of ca. –0.5e upon complex formation. A comparison between 9 and 10 reveals that the presence of the five-membered carbon ring in the dithiolate ligand results in an increase in the strength of the interfragment interaction even though the geometry of the [2Fe2S] core remains virtually unchanged (Table 1). Substituting the phenyl groups of 1 with hetaryl and/or ferrocenyl groups leads to more stabilizing IQF Eint energies. Interestingly, the substitution of these phenyl groups with the methyl ones in 9 strengthens the interfragment interaction owing to its greater stabilization from Vxc. The strongest interaction between the diiron center and the dithiolate ligand is observed for the coordination pattern occurring in complex 11.

4. Conclusions

In this work, the nature of bonds formed in the [2Fe2S] core of complexes 111 was analyzed from a QCT perspective. The results of the preliminary IRI analysis signals the occurrence of Fe–Fe and Fe–S chemical (that is, covalent) bonds in the [2Fe2S] core, but the subsequent in-depth QTAIM, SF, and ELF analyses agree that both the Fe–Fe and Fe–S bonds are not ‘classical’ covalent bonds.
The Fe–Fe bond in the [2Fe2S] core of 111 conforms to the QCT criteria of the metallic kind of bonds, and it is characterized by a relatively small amount of the strongly delocalized electron charge, partly originating from the carbonyl and dithiolate ligands. Four Fe–S bonds in the [2Fe2S] core of 110 are recognized as nearly identical and of donor–acceptor type, according to the QCT criteria. The IQA results indicate that the electrostatic repulsion between the positively charged Fe centers in the [2Fe2S] core of 111 cannot be counterbalanced by the stabilizing effect of electron sharing between these centers. Notwithstanding the energetically unfavorable IQA interaction between the Fe centers, the stabilization of the [2Fe2S] core is produced by the contributions from the IQA pairwise Fe–S interactions. The QCT results reveal that the effect of the functionalized five-membered carbon ring in the bridging dithiolate ligand on the bonds formed in the [2Fe2S] core of 111 is rather small in magnitude but shows regularity. The presence of the five-membered carbon ring decreases the amount of the electron charge shared between the metal centers, which further destabilizes the Fe–Fe interaction. On the other hand, this is accompanied by the growing strength of all four Fe–S interactions, with a regular increase in the stabilizing contribution from the classical electrostatic component. The functionalization of the five-membered carbon ring with ferrocenyl groups exerts an energetically favorable influence on the pairwise inter-atomic interactions in the [2Fe2S] core of complexes 58. It obviously means a strengthening of the Fe–S interactions but also a decreased destabilization between the Fe centers. Furthermore, a stronger attractive interaction acts between the entire bridging dithiolate ligand of 58 and their diiron center. Similarly, the different coordination pattern observed in complex 11 is associated with a stronger interaction between the dithiolate ligand and the diiron center than in 18.
From a practical viewpoint, the QCT perspective provides an insight into the charge density in the catalytic center of [FeFe]-hydrogenase mimics, and therefore, it may aid in determining the dominant site for protonation, which in turn is decisive in efficient hydrogen production processes. In our case, the QCT results for the [2Fe2S] core of complexes 111 reveal a relatively small amount of electron charge delocalized between the metal centers bearing highly positive charges. This indicates the occurrence of an electron-poor diiron center which seems to be not readily protonated, thereby affecting the probability of μ-hydride complex formation and the electrocatalytic behavior (redox potentials) of this center in general. It should, however, be stressed that there are also other factors that have not been taken into consideration here (e.g., the nature of terminal ligands), even though they significantly contribute to the electrocatalytic properties of the diiron center [4].
Furthermore, the QCT results show a small effect of dithiolate ligand functionalization on the [2Fe2S] core of 1, 35, and 7. This is reflected in their almost identical electrocatalytic behavior, as evidenced by cyclic voltammetry experiments [12].
In light of the above findings, the QCT methods prove to be a useful tool for the analysis of bonds in moderately large organometallic systems such as complexes based on the recently synthesized [FeFe]-hydrogenase mimics [12]. These methods produce a lot of chemically important details supplementing an orbital-based picture of the [2Fe2S] core of [FeFe]-hydrogenase mimics [68,69].

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/cryst15010052/s1, Section S1: Further computational details; Section S2: Cartesian coordinates for the optimized molecular geometries of 111; Section S3: Additional tables; References [70,71,72,73,74,75] are cited in Supplementary Materials.

Funding

This research received no external funding.

Data Availability Statement

The original contributions presented in this study are included in the article/Supplementary Material. Further inquiries can be directed to the corresponding author.

Acknowledgments

The author gratefully acknowledges Polish high-performance computing infrastructure PLGrid (HPC Center: ACK Cyfronet AGH) for providing computer facilities and support within computational grant no. PLG/2023/016589.

Conflicts of Interest

The author declares no conflict of interest.

References

  1. Evans, D.J.; Pickett, C.J. Chemistry and the Hydrogenases. Chem. Soc. Rev. 2003, 32, 268–275. [Google Scholar] [CrossRef] [PubMed]
  2. Liu, X.; Ibrahim, S.K.; Tard, C.; Pickett, C.J. Iron-Only Hydrogenase: Synthetic, Structural and Reactivity Studies of Model Compounds. Coord. Chem. Rev. 2005, 249, 1641–1652. [Google Scholar] [CrossRef]
  3. Vignais, P.M.; Billoud, B. Occurrence, Classification, and Biological Function of Hydrogenases: An Overview. Chem. Rev. 2007, 107, 4206–4272. [Google Scholar] [CrossRef]
  4. Schilter, D.; Camara, J.M.; Huynh, M.T.; Hammes-Schiffer, S.; Rauchfuss, T.B. Hydrogenase Enzymes and Their Synthetic Models: The Role of Metal Hydrides. Chem. Rev. 2016, 116, 8693–8749. [Google Scholar] [CrossRef] [PubMed]
  5. Wittkamp, F.; Senger, M.; Stripp, S.T.; Apfel, U.-P. [FeFe]-Hydrogenases: Recent Developments and Future Perspectives. Chem. Commun. 2018, 54, 5934–5942. [Google Scholar] [CrossRef]
  6. Gao, S.; Liu, Y.; Shao, Y.; Jiang, D.; Duan, Q. Iron Carbonyl Compounds with Aromatic Dithiolate Bridges as Organometallic Mimics of [FeFe] Hydrogenases. Coord. Chem. Rev. 2020, 402, 213081. [Google Scholar] [CrossRef]
  7. Hogarth, G. An Unexpected Leading Role for [Fe2(CO)6(μ-Pdt)] in Our Understanding of [FeFe]-H2ases and the Search for Clean Hydrogen Production. Coord. Chem. Rev. 2023, 490, 215174. [Google Scholar] [CrossRef]
  8. Ji, H.; Wan, L.; Gao, Y.; Du, P.; Li, W.; Luo, H.; Ning, J.; Zhao, Y.; Wang, H.; Zhang, L.; et al. Hydrogenase as the Basis for Green Hydrogen Production and Utilization. J. Energy Chem. 2023, 85, 348–362. [Google Scholar] [CrossRef]
  9. Grinberg, I.; Ben-Zvi, O.; Adler-Abramovich, L.; Yacoby, I. Peptide Self-assembly as a Strategy for Facile Immobilization of Redox Enzymes on Carbon Electrodes. Carbon Energy 2023, 5, e411. [Google Scholar] [CrossRef]
  10. Mulder, D.W.; Guo, Y.; Ratzloff, M.W.; King, P.W. Identification of a Catalytic Iron-Hydride at the H-cluster of [FeFe]-Hydrogenase. J. Am. Chem. Soc. 2017, 139, 83–86. [Google Scholar] [CrossRef]
  11. Li, Y.; Rauchfuss, T.B. Synthesis of Diiron(I) Dithiolato Carbonyl Complexes. Chem. Rev. 2016, 116, 7043–7077. [Google Scholar] [CrossRef] [PubMed]
  12. Buday, P.; Seeber, P.; Zens, C.; Abul-Futouh, H.; Görls, H.; Gräfe, S.; Matczak, P.; Kupfer, S.; Weigand, W.; Mlostoń, G. Iron(0)-Mediated Stereoselective (3+2)-Cycloaddition of Thiochalcones via a Diradical Intermediate. Chem. Eur. J. 2020, 26, 11412–11416. [Google Scholar] [CrossRef] [PubMed]
  13. Lansing, J.C.; Camara, J.M.; Gray, D.E.; Rauchfuss, T.B. Hydrogen Production Catalyzed by Bidirectional, Biomimetic Models of the [FeFe]-Hydrogenase Active Site. Organometallics 2014, 33, 5897–5906. [Google Scholar] [CrossRef]
  14. Kositzki, R.; Mebs, S.; Schuth, N.; Leidel, N.; Schwartz, L.; Karnahl, M.; Wittkamp, F.; Daunke, D.; Grohmann, A.; Apfel, U.-P.; et al. Electronic and Molecular Structure Relations in Diiron Compounds Mimicking the [FeFe]-Hydrogenase Active Site Studied by X-Ray Spectroscopy and Quantum Chemistry. Dalton Trans. 2017, 46, 12544–12557. [Google Scholar] [CrossRef]
  15. Matczak, P.; Domagała, M.; Domagała, S. Conformers of Diheteroaryl Ketones and Thioketones: A Quantum Chemical Study of Their Properties and Fundamental Intramolecular Energetic Effects. Struct. Chem. 2016, 27, 855–869. [Google Scholar] [CrossRef]
  16. Gröber, S.; Matczak, P.; Domagała, S.; Weisheit, T.; Görls, H.; Düver, A.; Mlostoń, G.; Weigand, W. Diferrocenyl Thioketone: Reactions with (Bisphosphane)Pt(0) Complexes—Electrochemical and Computational Studies. Materials 2019, 12, 2832. [Google Scholar] [CrossRef] [PubMed]
  17. Matczak, P.; Kupfer, S.; Mlostoń, G.; Buday, P.; Görls, H.; Weigand, W. Metal–Ligand Bonding in Tricarbonyliron(0) Complexes Bearing Thiochalcone Ligands. New J. Chem. 2022, 46, 12924–12933. [Google Scholar] [CrossRef]
  18. Matczak, P.; Domagała, S.; Weigand, W.; Mlostoń, G. A Comparative Analysis of UV–Vis Transitions in Hetaryl and Ferrocenyl Thioketones. Chem. Phys. 2023, 570, 111901. [Google Scholar] [CrossRef]
  19. Matczak, P.; Buday, P.; Kupfer, S.; Görls, H.; Mlostoń, G.; Weigand, W. Probing the Performance of DFT in the Structural Characterization of [FeFe] Hydrogenase Models. J. Comput. Chem. 2025, 46, e27515. [Google Scholar] [CrossRef]
  20. Popelier, P.L.A. On Quantum Chemical Topology. In Applications of Topological Methods in Molecular Chemistry; Chauvin, R., Lepetit, C., Silvi, B., Alikhani, E., Eds.; Challenges and Advances in Computational Chemistry and Physics; Springer International Publishing: Cham, Switzerland, 2016. [Google Scholar]
  21. Bader, R.F.W. Atoms in Molecules: A Quantum Theory; Clarendon: Oxford, UK, 1990. [Google Scholar]
  22. Silvi, B.; Savin, A. Classification of Chemical Bonds Based on Topological Analysis of Electron Localization Functions. Nature 1994, 371, 683–686. [Google Scholar] [CrossRef]
  23. Johnson, E.R.; Keinan, S.; Mori-Sánchez, P.; Contreras-García, J.; Cohen, A.J.; Yang, W. Revealing Noncovalent Interactions. J. Am. Chem. Soc. 2010, 132, 6498–6506. [Google Scholar] [CrossRef] [PubMed]
  24. Contreras-García, J.; Johnson, E.R.; Keinan, S.; Chaudret, R.; Piquemal, J.-P.; Beratan, D.N.; Yang, W. NCIPLOT: A Program for Plotting Noncovalent Interaction Regions. J. Chem. Theory Comput. 2011, 7, 625–632. [Google Scholar] [CrossRef]
  25. Lu, T.; Chen, Q. Interaction Region Indicator: A Simple Real Space Function Clearly Revealing Both Chemical Bonds and Weak Interactions. Chem. Methods 2021, 1, 231–239. [Google Scholar] [CrossRef]
  26. Blanco, M.A.; Martín Pendás, A.; Francisco, E. Interacting Quantum Atoms: A Correlated Energy Decomposition Scheme Based on the Quantum Theory of Atoms in Molecules. J. Chem. Theory Comput. 2005, 1, 1096–1109. [Google Scholar] [CrossRef] [PubMed]
  27. Guevara-Vela, J.M.; Francisco, E.; Rocha-Rinza, T.; Pendás, Á.M. Interacting Quantum Atoms—A Review. Molecules 2020, 25, 4028. [Google Scholar] [CrossRef] [PubMed]
  28. Macchi, P.; Sironi, A. Chemical Bonding in Transition Metal Carbonyl Clusters: Complementary Analysis of Theoretical and Experimental Electron Densities. Coord. Chem. Rev. 2003, 238–239, 383–412. [Google Scholar] [CrossRef]
  29. Frenking, G.; Fernández, I.; Holzmann, N.; Pan, S.; Krossing, I.; Zhou, M. Metal−CO Bonding in Mononuclear Transition Metal Carbonyl Complexes. JACS Au 2021, 1, 623–645. [Google Scholar] [CrossRef]
  30. Bertini, L.; Greco, C.; De Gioia, L.; Fantucci, P. DFT/TDDFT Exploration of the Potential Energy Surfaces of the Ground State and Excited States of Fe2(S2C3H6)(CO)6: A Simple Functional Model of the [FeFe] Hydrogenase Active Site. J. Phys. Chem. A 2009, 113, 5657–5670. [Google Scholar] [CrossRef]
  31. Bertini, L.; Greco, C.; Bruschi, M.; Fantucci, P.; De Gioia, L. CO Affinity and Bonding Properties of [FeFe] Hydrogenase Active Site Models. A DFT Study. Organometallics 2010, 29, 2013–2025. [Google Scholar] [CrossRef]
  32. Giles, L.J.; Grigoropoulos, A.; Szilagyi, R.K. Electron and Spin Density Topology of the H-Cluster and Its Biomimetic Complexes. Eur. J. Inorg. Chem. 2011, 2011, 2677–2690. [Google Scholar] [CrossRef]
  33. Arrigoni, F.; Zampella, G.; De Gioia, L.; Greco, C.; Bertini, L. The Photochemistry of Fe2(S2C3H6)(CO)6(µ-CO) and Its Oxidized Form, Two Simple [FeFe]-Hydrogenase CO-Inhibited Models. A DFT and TDDFT Investigation. Inorganics 2021, 9, 16. [Google Scholar] [CrossRef]
  34. Lyon, E.J.; Georgakaki, I.P.; Reibenspies, J.H.; Darensbourg, M.Y. Carbon Monoxide and Cyanide Ligands in a Classical Organometallic Complex Model for Fe-Only Hydrogenase. Angew. Chem. Int. Ed. 1999, 38, 3178–3180. [Google Scholar] [CrossRef]
  35. Staroverov, V.N.; Scuseria, G.E.; Tao, J.; Perdew, J.P. Comparative Assessment of a New Nonempirical Density Functional: Molecules and Hydrogen-Bonded Complexes. J. Chem. Phys. 2003, 119, 12129–12137. [Google Scholar] [CrossRef]
  36. Weigend, F.; Ahlrichs, R. Balanced Basis Sets of Split Valence, Triple Zeta Valence and Quadruple Zeta Valence Quality for H to Rn: Design and Assessment of Accuracy. Phys. Chem. Chem. Phys. 2005, 7, 3297–3305. [Google Scholar] [CrossRef]
  37. Becke, A.D. Density-Functional Thermochemistry. III. The Role of Exact Exchange. J. Chem. Phys. 1993, 98, 5648–5652. [Google Scholar] [CrossRef]
  38. Hertwig, R.H.; Koch, W. On the Parameterization of the Local Correlation Functional. What Is Becke-3-LYP? Chem. Phys. Lett. 1997, 268, 345–351. [Google Scholar] [CrossRef]
  39. Gatti, C.; Cargnoni, F.; Bertini, L. Chemical Information from the Source Function. J. Comput. Chem. 2003, 24, 422–436. [Google Scholar] [CrossRef] [PubMed]
  40. Martín Pendás, A.; Blanco, M.A.; Francisco, E. The Nature of the Hydrogen Bond: A Synthesis from the Interacting Quantum Atoms Picture. J. Chem. Phys. 2006, 125, 184112. [Google Scholar] [CrossRef] [PubMed]
  41. Ahlrichs, R.; Armbruster, M.K.; Bachorz, R.A.; Bahmann, H.; Baldes, A.; Bär, M.; Baron, H.; Bauernschmitt, R.; Bischof, F.A.; Böcker, S.; et al. TURBOMOLE 7.7; A Development of University of Karlsruhe and Forschungszentrum Karlsruhe GmbH, 1989–2007; TURBOMOLE GmbH: Karlsruhe, Germany, 2022. [Google Scholar]
  42. Frisch, M.J.; Trucks, G.W.; Schlegel, H.B.; Scuseria, G.E.; Robb, M.A.; Cheeseman, J.R.; Scalmani, G.; Barone, V.; Petersson, G.A.; Nakatsuji, H.; et al. Gaussian 16, Rev. C.01; Gaussian, Inc.: Wallingford, CT, USA, 2016. [Google Scholar]
  43. Lu, T.; Chen, F. Multiwfn: A Multifunctional Wavefunction Analyzer. J. Comput. Chem. 2012, 33, 580–592. [Google Scholar] [CrossRef]
  44. Keith, T.A. AIMAll 19.10.12; TK Gristmill Software: Overland Park, KS, USA, 2019. [Google Scholar]
  45. Humphrey, W.; Dalke, A.; Schulten, K. VMD—Visual Molecular Dynamics. J. Mol. Graph. 1996, 14, 33–38. [Google Scholar] [CrossRef] [PubMed]
  46. Zhao, C.; Wu, R.; Zhang, S.; Hong, X. Benchmark Study of Density Functional Theory Methods in Geometry Optimization of Transition Metal−Dinitrogen Complexes. J. Phys. Chem. A 2023, 127, 6791–6803. [Google Scholar] [CrossRef] [PubMed]
  47. Hargittai, M.; Hargittai, I. Gas-Solid Molecular Structure Differences. Phys. Chem. Minerals 1987, 14, 413–425. [Google Scholar] [CrossRef]
  48. Pyykkö, P.; Atsumi, M. Molecular Single-Bond Covalent Radii for Elements 1–118. Chem. Eur. J. 2009, 15, 186–197. [Google Scholar] [CrossRef] [PubMed]
  49. Bader, R.F.W. A Bond Path: A Universal Indicator of Bonded Interactions. J. Phys. Chem. A 1998, 102, 7314–7323. [Google Scholar] [CrossRef]
  50. Farrugia, L.J.; Macchi, P. Bond Orders in Metal–Metal Interactions through Electron Density Analysis. Struct. Bond. 2012, 146, 127–158. [Google Scholar]
  51. Malcek, M.; Vénosová, B.; Puškárová, I.; Kožíšek, J.; Gall, M.; Bucinský, L. Coordination Bonding in Dicopper and Dichromium Tetrakis (μ-Acetato)-Diaqua Complexes: Nature, Strength, Length, and Topology. J. Comput. Chem. 2020, 41, 698–714. [Google Scholar] [CrossRef] [PubMed]
  52. Farrugia, L.J.; Evans, C.; Senn, H.M.; Hänninen, M.M.; Sillanpäa, R. QTAIM View of Metal−Metal Bonding in Di- and Trinuclear Disulfido Carbonyl Clusters. Organometallics 2012, 31, 2559–2570. [Google Scholar] [CrossRef]
  53. Cremer, D.; Kraka, E. A Description of the Chemical Bond in Terms of Local Properties of Electron Density and Energy. Croat. Chem. Acta 1984, 57, 1259–1281. [Google Scholar]
  54. Bianchi, R.; Gervasio, G.; Marabello, D. Experimental Electron Density Analysis of Mn2(CO)10: Metal-Metal and Metal-Ligand Bond Characterization. Inorg. Chem. 2000, 39, 2360–2366. [Google Scholar] [CrossRef] [PubMed]
  55. Macchi, P.; Proserpio, D.M.; Sironi, A. Experimental Electron Density in a Transition Metal Dimer: Metal-Metal and Metal-Ligand Bonds. J. Am. Chem. Soc. 1998, 120, 13429–13435. [Google Scholar] [CrossRef]
  56. Fradera, X.; Austen, M.A.; Bader, R.F.W. The Lewis Model and Beyond. J. Phys. Chem. A 1999, 103, 304–314. [Google Scholar] [CrossRef]
  57. Rose, K.; Shadle, S.E.; Glaser, T.; de Vries, S.; Cherepanov, A.; Canters, G.W.; Hedman, B.; Hodgson, K.O.; Solomon, E.I. Investigation of the Electronic Structure of 2Fe-2S Model Complexes and the Rieske Protein Using Ligand K-Edge X-Ray Absorption Spectroscopy. J. Am. Chem. Soc. 1999, 121, 2353–2363. [Google Scholar] [CrossRef]
  58. Harris, T.V.; Szilagyi, R.K. Iron–Sulfur Bond Covalency from Electronic Structure Calculations for Classical Iron–Sulfur Clusters. J. Comput. Chem. 2014, 35, 540–552. [Google Scholar] [CrossRef] [PubMed]
  59. Lee, C.-R.; Hsu, I.-J.; Chen, H.-T.; Lee, G.-H.; Wang, Y. Charge Density Studies on [(NO)Fe(S2C6H4)2][PPN] and [(NO)3Fe(S2C6H4)3] Complexes. C. R. Chim. 2012, 15, 237–249. [Google Scholar] [CrossRef]
  60. Lebon, A.; Orain, P.-Y.; Memboeuf, A. Understanding the CO Dissociation in [Fe(CN)2(CO)2(Dithiolate)]2− Complexes with Quantum Chemical Topology Tools. J. Phys. Chem. A 2017, 121, 7031–7041. [Google Scholar] [CrossRef]
  61. Espinosa, E.; Alkorta, I.; Elguero, J.; Molins, E. From Weak to Strong Interactions: A Comprehensive Analysis of the Topological and Energetic Properties of the Electron Density Distribution Involving X–H···F–Y Systems. J. Chem. Phys. 2002, 117, 5529–5542. [Google Scholar] [CrossRef]
  62. Reinhold, J.; Kluge, O.; Mealli, C. Integration of Electron Density and Molecular Orbital Techniques to Reveal Questionable Bonds: The Test Case of the Direct Fe−Fe Bond in Fe2(CO)9. Inorg. Chem. 2007, 46, 7142–7147. [Google Scholar] [CrossRef] [PubMed]
  63. Gatti, C.; Lasi, D. Source Function Description of Metal–Metal Bonding in d-Block Organometallic Compounds. Faraday Discuss. 2007, 135, 55–78. [Google Scholar] [CrossRef]
  64. Berski, S.; Gutsev, G.L.; Mochena, M.D.; Andres, J. Toward Understanding the Electron Density Distribution in Magnetic Clusters: Insight from the ELF and AIM Analyses of Ground-State Fe4. J. Phys. Chem. A 2004, 108, 6025–6031. [Google Scholar] [CrossRef]
  65. Viciano, I.; Berski, S.; Marti, S.; Andres, J. New Insight into the Electronic Structure of Iron(IV)-Oxo Porphyrin Compound I. A Quantum Chemical Topological Analysis. J. Comput. Chem. 2013, 34, 780–789. [Google Scholar] [CrossRef] [PubMed]
  66. Tiana, D.; Francisco, E.; Macchi, P.; Sironi, A.; Pendás, A.M. An Interacting Quantum Atoms Analysis of the Metal−Metal Bond in [M2(CO)8]n Systems. J. Phys. Chem. A 2015, 119, 2153–2160. [Google Scholar] [CrossRef] [PubMed]
  67. Martín Pendás, A.; Francisco, E.; Blanco, M.A.; Gatti, C. Bond Paths as Privileged Exchange Channels. Chem. Eur. J. 2007, 13, 9362–9371. [Google Scholar] [CrossRef]
  68. Schwab, D.E.; Tard, C.; Brecht, E.; Peters, J.W.; Pickett, C.J.; Szilagyi, R.K. On the Electronic Structure of the Hydrogenase H-Cluster. Chem. Commun. 2006, 3696–3698. [Google Scholar] [CrossRef]
  69. Chang, C.H. Computational Chemical Analysis of [FeFe] Hydrogenase H-Cluster Analogues to Discern Catalytically Relevant Features of the Natural Diatomic Ligand Configuration. J. Phys. Chem. A 2011, 115, 8691–8704. [Google Scholar] [CrossRef] [PubMed]
  70. Benediktsson, B.; Bjornsson, R. Analysis of the Geometric and Electronic Structure of Spin-Coupled Iron−sulfur Dimers with Broken-Symmetry DFT: Implications for FeMoco. J. Chem. Theory Comput. 2022, 18, 1437–1457. [Google Scholar] [CrossRef]
  71. Eichkorn, K.; Treutler, O.; Öhm, H.; Häser, M.; Ahlrichs, R. Auxiliary Basis Sets to Approximate Coulomb Potentials. Chem. Phys. Lett. 1995, 240, 283–290. [Google Scholar] [CrossRef]
  72. Eichkorn, K.; Weigend, F.; Treutler, O.; Ahlrichs, R. Auxiliary Basis Sets for Main Row Atoms and Transition Metals and Their Use to Approximate Coulomb Potentials. Theor. Chem. Acc. 1997, 97, 119–124. [Google Scholar] [CrossRef]
  73. Weigend, F. Accurate Coulomb-Fitting Basis Sets for H to Rn. Phys. Chem. Chem. Phys. 2006, 8, 1057–1065. [Google Scholar] [CrossRef] [PubMed]
  74. Furness, J.W.; Kaplan, A.D.; Ning, J.; Perdew, J.P.; Sun, J. Accurate and Numerically Efficient r2SCAN Meta-Generalized Gradient Approximation. J. Phys. Chem. Lett. 2020, 11, 8208–8215. [Google Scholar] [CrossRef]
  75. Kleinhaus, J.T.; Wittkamp, F.; Yadav, S.; Siegmund, D.; Apfel, U.-P. [FeFe]-Hydrogenases: Maturation and Reactivity of Enzymatic Systems and Overview of Biomimetic Models. Chem. Soc. Rev. 2021, 50, 1668–1784. [Google Scholar] [CrossRef] [PubMed]
Figure 1. [FeFe]-Hydrogenase mimics 111 studied in this work.
Figure 1. [FeFe]-Hydrogenase mimics 111 studied in this work.
Crystals 15 00052 g001
Figure 2. IRI isosurfaces for the [2Fe2S] core in complexes (a) 9 and (b) 11. The isosurfaces are plotted with an isovalue of 0.8 and colored from blue to red according to sign(λ2)ρ ranging from −0.04 to 0.02 atomic units. The term sign(λ2) stands for the sign of the second eigenvalue of the Hessian matrix of the charge density (ρ). Hydrogen, carbon, oxygen, sulfur, and iron are colored white, gray, red, yellow, and orange, respectively.
Figure 2. IRI isosurfaces for the [2Fe2S] core in complexes (a) 9 and (b) 11. The isosurfaces are plotted with an isovalue of 0.8 and colored from blue to red according to sign(λ2)ρ ranging from −0.04 to 0.02 atomic units. The term sign(λ2) stands for the sign of the second eigenvalue of the Hessian matrix of the charge density (ρ). Hydrogen, carbon, oxygen, sulfur, and iron are colored white, gray, red, yellow, and orange, respectively.
Crystals 15 00052 g002
Figure 3. QTAIM molecular graphs for complexes (a) 9 and (b) 11. Bond paths are drawn with black lines. Bond critical points are shown as small green spheres, ring critical points as small red spheres, and cage critical points as small blue spheres. Colors coding individual elements are the same as in Figure 2.
Figure 3. QTAIM molecular graphs for complexes (a) 9 and (b) 11. Bond paths are drawn with black lines. Bond critical points are shown as small green spheres, ring critical points as small red spheres, and cage critical points as small blue spheres. Colors coding individual elements are the same as in Figure 2.
Crystals 15 00052 g003
Figure 4. Localization domains plotted with an ELF isovalue of (a) 0.82 and (b) 0.42 for complex 1. Basins representing the Fe–Fe and Fe–S bonds are colored blue and green, respectively. Colors coding individual elements are the same as in Figure 2.
Figure 4. Localization domains plotted with an ELF isovalue of (a) 0.82 and (b) 0.42 for complex 1. Basins representing the Fe–Fe and Fe–S bonds are colored blue and green, respectively. Colors coding individual elements are the same as in Figure 2.
Crystals 15 00052 g004
Table 1. Calculated and available experimental bond lengths (in pm) for the [2Fe2S] core of complexes 111 a.
Table 1. Calculated and available experimental bond lengths (in pm) for the [2Fe2S] core of complexes 111 a.
ComplexFe1–Fe2Fe1–S1Fe1–S2Fe2–S1Fe2–S2Average Fe–S
1247.3
(249.9)
227.9
(230.4)
231.2
(234.0)
231.0
(233.7)
228.4
(230.6)
229.6
(232.2)
2247.6
(249.9)
227.7
(230.3)
230.7
(233.9)
230.6
(233.5)
228.1
(230.7)
229.3
(232.1)
3247.6
(250.2)
[251.5]
227.5
(230.1)
[224.1]
230.7
(233.5)
[227.9]
229.8
(232.6)
[226.2]
228.4
(230.7)
[225.1]
229.1
(231.7)
4247.8
(250.0)
227.5
(230.2)
230.5
(233.8)
229.5
(232.9)
228.3
(230.8)
229.0
(231.9)
5248.9
(251.3)
[250.8]
227.0
(229.3)
[224.1]
229.2
(232.1)
[227.3]
227.4
(230.1)
[225.3]
228.2
(230.6)
[224.9]
228.0
(230.5)
6248.5
(251.0)
228.2
(230.8)
228.4
(230.8)
227.2
(229.5)
229.5
(232.4)
228.3
(230.9)
7248.7
(251.3)
[251.5]
227.9
(230.3)
[223.2]
228.3
(230.7)
[224.8]
226.9
(229.2)
[225.2]
229.6
(232.2)
[225.0]
228.2
(230.6)
8248.6
(251.1)
228.0
(230.5)
228.2
(230.8)
226.7
(229.2)
229.7
(232.3)
228.2
(230.7)
9248.2
(250.8)
227.2
(229.7)
229.8
(232.4)
228.3
(230.9)
228.6
(230.9)
228.5
(231.0)
10248.4
(250.9)
[251.0]
228.2
(230.8)
[224.9]
228.2
(230.8)
[225.4]
228.9
(231.7)
[224.9]
228.9
(231.7)
[225.4]
228.6
(231.3)
11260.3
(264.3)
[263.7]
223.8
(225.5)
[221.4]
286.7
(291.5)
[286.5]
227.5
(230.4)
[224.3]
229.7
(233.1)
[226.4]
241.9
(245.1)
a Results obtained from the TPSSh/def2-SVP and B3LYP/def2-SVP calculations are shown without and in parentheses, respectively. Experimental results [12,34] are given in square brackets. The numbering of atoms is the same as in Figure 1.
Table 2. QTAIM parameters (in atomic units) at the BCP on the path linking Fe1 and Fe2 in complexes 111 a.
Table 2. QTAIM parameters (in atomic units) at the BCP on the path linking Fe1 and Fe2 in complexes 111 a.
ComplexρBCP2ρBCP|VBCP|/GBCPGBCP/ρBCPHBCPδ
10.0527
(0.0528)
0.0444
(0.0686)
1.604
(1.443)
0.5312
(0.5833)
−0.0169
(−0.0136)
0.470
(0.477)
20.0526
(0.0527)
0.0439
(0.0685)
1.606
(1.442)
0.5297
(0.5826)
−0.0169
(−0.0136)
0.470
(0.477)
30.0525
(0.0526)
0.0442
(0.0691)
1.604
(1.439)
0.5313
(0.5849)
−0.0169
(−0.0135)
0.471
(0.477)
40.0524
(0.0525)
0.0440
(0.0693)
1.606
(1.437)
0.5313
(0.5858)
−0.0169
(−0.0134)
0.470
(0.476)
50.0517
(0.0518)
0.0430
(0.0694)
1.608
(1.429)
0.5298
(0.5862)
−0.0167
(−0.0130)
0.467
(0.474)
60.0519
(0.0520)
0.0432
(0.0689)
1.607
(1.434)
0.5295
(0.5842)
−0.0167
(−0.0132)
0.471
(0.478)
70.0518
(0.0520)
0.0429
(0.0689)
1.608
(1.433)
0.5289
(0.5841)
−0.0167
(−0.0131)
0.470
(0.477)
80.0518
(0.0520)
0.0435
(0.0695)
1.605
(1.430)
0.5311
(0.5868)
−0.0167
(−0.0131)
0.467
(0.474)
90.0521
(0.0521)
0.0441
(0.0700)
1.603
(1.429)
0.5331
(0.5888)
−0.0168
(−0.0132)
0.469
(0.475)
100.0518
(0.0517)
0.0451
(0.0717)
1.596
(1.418)
0.5383
(0.5954)
−0.0166
(−0.0129)
0.479
(0.484)
110.0445
(n/a)
0.0270
(n/a)
1.683
(n/a)
0.4777
(n/a)
−0.0145
(n/a)
0.429
(0.433)
a Results derived from the TPSSh/def2-SVP and TPSSh/def2-TZVP calculations are shown without and in parentheses, respectively. The numbering of atoms is the same as in Figure 1.
Table 3. QTAIM parameters (in atomic units) at the BCP on the path linking Fe1 and S1 in complexes 111 a.
Table 3. QTAIM parameters (in atomic units) at the BCP on the path linking Fe1 and S1 in complexes 111 a.
ComplexρBCP2ρBCP|VBCP|/GBCPGBCP/ρBCPHBCPδ
10.0744
(0.0790)
0.2306
(0.1749)
1.159
(1.369)
0.9213
(0.8766)
−0.0109
(−0.0255)
0.688
(0.721)
20.0747
(0.0793)
0.2313
(0.1753)
1.160
(1.370)
0.9218
(0.8768)
−0.0110
(−0.0257)
0.688
(0.722)
30.0749
(0.0796)
0.2336
(0.1772)
1.159
(1.368)
0.9272
(0.8814)
−0.0111
(−0.0258)
0.689
(0.723)
40.0749
(0.0796)
0.2338
(0.1774)
1.159
(1.368)
0.9279
(0.8821)
−0.0110
(−0.0258)
0.687
(0.721)
50.0765
(0.0811)
0.2296
(0.1719)
1.174
(1.385)
0.9081
(0.8620)
−0.0121
(−0.0269)
0.698
(0.731)
60.0740
(0.0785)
0.2276
(0.1723)
1.163
(1.371)
0.9183
(0.3972)
−0.0110
(−0.0254)
0.678
(0.711)
70.0745
(0.0790)
0.2293
(0.1735)
1.164
(1.372)
0.9204
(0.8741)
−0.0112
(−0.0256)
0.679
(0.713)
80.0741
(0.0786)
0.2281
(0.1725)
1.162
(1.371)
0.9184
(0.8727)
−0.0110
(−0.0255)
0.680
(0.713)
90.0757
(0.0803)
0.2324
(0.1755)
1.165
(1.375)
0.9191
(0.8739)
−0.0115
(−0.0263)
0.697
(0.731)
100.0747
(0.0792)
0.2323
(0.1756)
1.159
(1.368)
0.9245
(0.8774)
−0.0110
(−0.0256)
0.687
(0.723)
110.0818
(0.0866)
0.2514
(0.1870)
1.180
(1.391)
0.9374
(0.8871)
−0.0138
(−0.0300)
0.713
(0.754)
a Results derived from the TPSSh/def2-SVP and TPSSh/def2-TZVP calculations are shown without and in parentheses, respectively. The numbering of atoms is the same as in Figure 1.
Table 4. ELF parameters (in atomic units) for the bonding basin of Fe1–Fe2 in complexes 111 a.
Table 4. ELF parameters (in atomic units) for the bonding basin of Fe1–Fe2 in complexes 111 a.
ComplexELFmax N ¯ λ N ¯ ( Fe 1 ) N ¯ ( Fe 2 )
10.469
(0.430)
0.498
(0.457)
0.882
(0.889)
0.241
(0.225)
0.248
(0.230)
20.472
(0.433)
0.500
(0.459)
0.881
(0.889)
0.242
(0.225)
0.248
(0.230)
30.476
(0.437)
0.505
(0.462)
0.880
(0.888)
0.244
(0.228)
0.251
(0.231)
40.476
(0.436)
0.502
(0.457)
0.881
(0.888)
0.245
(0.227)
0.247
(0.228)
50.498
(0.456)
0.518
(0.477)
0.876
(0.884)
0.255
(0.237)
0.256
(0.236)
60.499
(0.458)
0.521
(0.482)
0.875
(0.883)
0.259
(0.240)
0.256
(0.238)
70.500
(0.458)
0.519
(0.482)
0.876
(0.883)
0.256
(0.238)
0.258
(0.240)
80.496
(0.455)
0.516
(0.478)
0.876
(0.883)
0.253
(0.237)
0.257
(0.237)
90.485
(0.445)
0.509
(0.465)
0.879
(0.887)
0.247
(0.230)
0.253
(0.232)
100.510
(0.470)
0.529
(0.489)
0.873
(0.881)
0.263
(0.237)
0.260
(0.247)
110.492
(0.451)
0.517
(0.474)
0.880
(0.887)
0.224
(0.207)
0.279
(0.257)
a Results derived from the TPSSh/def2-SVP and TPSSh/def2-TZVP calculations are shown without and in parentheses, respectively. The numbering of atoms is the same as in Figure 1.
Table 5. ELF parameters (in atomic units) for the bonding basin of Fe1–S1 in complexes 111 a.
Table 5. ELF parameters (in atomic units) for the bonding basin of Fe1–S1 in complexes 111 a.
ComplexELFmax N ¯ λ N ¯ ( Fe 1 ) N ¯ ( S 1 )
10.899
(0.898)
1.615
(1.641)
0.642
(0.640)
0.196
(0.210)
1.405
(1.415)
20.900
(0.898)
1.622
(1.646)
0.641
(0.639)
0.197
(0.211)
1.411
(1.420)
30.900
(0.898)
1.618
(1.645)
0.642
(0.639)
0.196
(0.210)
1.408
(1.419)
40.899
(0.897)
1.593
(1.629)
0.646
(0.642)
0.195
(0.210)
1.384
(1.404)
50.896
(0.895)
1.632
(1.650)
0.641
(0.640)
0.204
(0.217)
1.419
(1.423)
60.899
(0.898)
1.656
(1.645)
0.634
(0.633)
0.192
(0.201)
1.458
(1.441)
70.895
(0.898)
1.632
(1.647)
0.642
(0.634)
0.205
(0.203)
1.419
(1.428)
80.895
(0.897)
1.628
(1.650)
0.642
(0.635)
0.203
(0.205)
1.418
(1.438)
90.898
(0.896)
1.626
(1.651)
0.642
(0.639)
0.198
(0.213)
1.415
(1.423)
100.897
(0.896)
1.540
(1.601)
0.650
(0.644)
0.193
(0.206)
1.339
(1.384)
110.891
(0.889)
1.542
(1.587)
0.655
(0.650)
0.206
(0.221)
1.327
(1.357)
a Results derived from the TPSSh/def2-SVP and TPSSh/def2-TZVP calculations are shown without and in parentheses, respectively. The numbering of atoms is the same as in Figure 1.
Table 6. Pairwise IQA energies (in atomic units) for Fe1–Fe2, Fe1–S1, and four Fe–S bonds in total in complexes 111 a.
Table 6. Pairwise IQA energies (in atomic units) for Fe1–Fe2, Fe1–S1, and four Fe–S bonds in total in complexes 111 a.
ComplexFe1–Fe2Fe1–S1All Four Fe–S Bonds
EintVclVxcEintVclVxcEintVclVxc
10.03040.1096−0.0791−0.1974−0.0588−0.1386−0.7615−0.2273−0.5341
20.03060.1096−0.0790−0.1973−0.0585−0.1389−0.7617−0.2254−0.5363
30.03040.1093−0.0788−0.1946−0.0556−0.1390−0.7597−0.2228−0.5370
40.03060.1094−0.0788−0.1945−0.0556−0.1389−0.7596−0.2210−0.5385
50.02880.1073−0.0785−0.1987−0.0571−0.1416−0.7726−0.2213−0.5513
60.02850.1078−0.0793−0.1947−0.0579−0.1369−0.7689−0.2220−0.5469
70.02870.1077−0.0790−0.1949−0.0577−0.1372−0.7703−0.2221−0.5482
80.02930.1079−0.0786−0.1949−0.0580−0.1369−0.7743−0.2250−0.5493
90.02960.1083−0.0787−0.1990−0.0584−0.1405−0.7740−0.2276−0.5463
100.02600.1063−0.0803−0.1897−0.0516−0.1381−0.7550−0.2080−0.5470
110.03260.1014−0.0688−0.2028−0.0545−0.1483−0.5403−0.1073−0.4330
a Results derived from the B3LYP/def2-SVP single-point energies for the geometries optimized at the TPSSh/def2-SVP level of theory. The numbering of atoms is the same as in Figure 1.
Table 7. IQF energies (in atomic units) between the dithiolate fragment and the diiron Fe1–Fe2 fragment in complexes 111 a.
Table 7. IQF energies (in atomic units) between the dithiolate fragment and the diiron Fe1–Fe2 fragment in complexes 111 a.
ComplexEintVclVxc
1−0.7397−0.1836−0.5561
2−0.7429−0.1849−0.5580
3−0.7449−0.1868−0.5581
4−0.7468−0.1874−0.5594
5−0.7481−0.1776−0.5705
6−0.7463−0.1805−0.5658
7−0.7469−0.1795−0.5674
8−0.7440−0.1754−0.5687
9−0.7437−0.1792−0.5644
10−0.7374−0.1739−0.5635
11−0.7815−0.1858−0.5957
a Results derived from the B3LYP/def2-SVP single-point energies for the geometries optimized at the TPSSh/def2-SVP level of theory. The numbering of atoms is the same as in Figure 1.
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Matczak, P. Quantum Chemical Topological Analysis of [2Fe2S] Core in Novel [FeFe]-Hydrogenase Mimics. Crystals 2025, 15, 52. https://doi.org/10.3390/cryst15010052

AMA Style

Matczak P. Quantum Chemical Topological Analysis of [2Fe2S] Core in Novel [FeFe]-Hydrogenase Mimics. Crystals. 2025; 15(1):52. https://doi.org/10.3390/cryst15010052

Chicago/Turabian Style

Matczak, Piotr. 2025. "Quantum Chemical Topological Analysis of [2Fe2S] Core in Novel [FeFe]-Hydrogenase Mimics" Crystals 15, no. 1: 52. https://doi.org/10.3390/cryst15010052

APA Style

Matczak, P. (2025). Quantum Chemical Topological Analysis of [2Fe2S] Core in Novel [FeFe]-Hydrogenase Mimics. Crystals, 15(1), 52. https://doi.org/10.3390/cryst15010052

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