Minna M.
Karjalainen
,
Clara
Sanchez-Perez
,
J. Mikko
Rautiainen
,
Raija
Oilunkaniemi
and
Risto S.
Laitinen
*
Laboratory of Inorganic Chemistry, University of Oulu, P.O. Box 3000 FI-90014, Finland. E-mail: risto.laitinen@oulu.fi; Tel: +358 294 481611
First published on 29th April 2016
The solid-state structures of all members in the series of trichalcogenaferrocenophanes [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) (1–9) have been explored to understand the trends in secondary bonding interactions (SBIs) between chalcogen elements sulfur, selenium, and tellurium. To complete the series, the crystal structures of the four hitherto unknown complexes [Fe(C5H4S)2Te] (3), [Fe(C5H4Se)2S] (4), [Fe(C5H4Se)2Te] (6), and [Fe(C5H4Te)2S] (7) have been determined in this contribution. The packings of all complexes 1–9 were considered by DFT calculations at the PBE0/pob-TZVP level of theory using periodic boundary conditions. The intermolecular close contacts were considered by QTAIM and NBO analyses. The isomorphous complexes [Fe(C5H4S)2S] (1), [Fe(C5H4S)2Se] (2), and [Fe(C5H4Se)2Se] (5a) form dimers via weak interactions between the central chalcogen atoms of the two trichalcogena chains of adjacent complexes. In the second isomorphous series consisting of [Fe(C5H4Se)2S] (4) and 5b, the complexes are linked together into continuous chains by short contacts via the terminal selenium atoms. The intermolecular chalcogen–chalcogen interactions are significantly stronger in complexes [Fe(C5H4S)2Te] (3), [Fe(C5H4Se)2Te] (6), and [Fe(C5H4Te)2E′] (E′ = S, Se, Te) (7–9), which contain tellurium. The NBO comparison of donor–acceptor interactions in the lattices of [Fe(C5H4S)2S] (1), [Fe(C5H4Se)2Se] (5a and 5b), and [Fe(C5H4Te)2Te] (9) indeed shows that the n(5pTe)2 → σ*(Te–Te) interactions in 9 are the strongest. All other interaction energies are significantly smaller even in the case of tellurium. The computed natural charges of the chalcogen atoms indicate that electrostatic effects strengthen the attractive interactions in the case of all chalcogen atoms.
Secondary bonding interactions are currently considered to be due to electrostatic and dispersion effects in which the so-called σ-hole and polarizability play important roles.2 On the other hand, the interactions involving chalcogen compounds have traditionally been described as donor–acceptor interactions n2(D) → σ*(E–X) in which the lone pair of a donor atom D interacts with the antibonding σ* orbital of the heavy atom (E) and a more electronegative atom (X). This 3c–4e arrangement is of variable strength, from a very weak interaction to that of a hypervalent single bond.3a The energy difference between the σ(E–X) and σ*(E–X) orbitals diminishes upon going down the periodic table and therefore SBIs are stronger for tellurium compared to those of selenium and sulfur.4 However, even in the case of lighter chalcogen compounds, the complete description of the SBIs also requires the consideration of orbital interactions, as well as electrostatic and dispersion contributions.2,3 The different nature of interactions even in related compounds is exemplified by the observation that telluradiazoles show predominantly covalent interactions,5 but those in isotellurazole N-oxides are electrostatic,6 and the interactions in bis(alkynyl)tellurides are mainly due to dispersion.4 It has, however, been concluded several times that there is no real difference between charge transfer and electrostatic attraction combined with polarization effects.2c,7 Furthermore, it has also been pointed out that while several procedures to decompose secondary bonding interaction energies into contributions by different components, such as “electrostatics, exchange, Pauli exclusion, polarization, charge transfer, dispersion, induction, orbital interactions, electronic correlation, delocalization, deformation, etc.”,2c have been proposed, they cannot be considered independent contributions, and the results are likely not to be even qualitatively meaningful.
When considering interactions in chalcogen compounds, the strongest SBIs are found when the donor atom is oxygen or nitrogen, but chalcogen–chalcogen interactions are also known.3 Typical examples containing chalcogen–chalcogen SBIs are hexagonal allotropes of selenium8 and tellurium,9 in which the trigonal chains show close contacts expanding the formal coordination sphere of the chalcogen atoms to an octahedron.
Trichalcogenaferrocenophanes are a useful class of compounds for studying the trend in the SBI strengths of the group 16 elements (see Chart 1). While [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) complexes have been known for a long time, crystal structures have been reported for only [Fe(C5H4S)2S] (1),10 [Fe(C5H4S)2Se] (2),11 [Fe(C5H4Se)2Se] (the monoclinic polymorph 5a and the orthorhombic polymorph 5b),12 [Fe(C5H4Te)2Se] (8),13 and [Fe(C5H4Te)2Te] (9).14 Structures of some related complexes in which the cyclopentadienyl rings of ferrocene have been modified are also known.15 Trithiaosmocenophane16 and triselenaruthenocenophane17 also show similar E⋯E close contacts to trichalcogenaferrocenophanes.10,12 In this contribution, we complement the structural and spectroscopic characterization of the whole series of [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) containing both homo- and heteronuclear chalcogen chains by reporting the preparation and crystal structures of 3, 4, 6, and 7. All structural data for complexes 1–9 are compared and discussed in terms of trends in the chalcogen–chalcogen secondary bonding interactions. The experimental information is complemented by solid-state DFT calculations, which provide insight into the nature of SBIs in these systems.
The optimization was started from the experimental X-ray structures. Both the lattice parameters and atomic positions were optimized in the calculations. Monkhorst–Pack-type grids of k-points in the reciprocal space were generated using a shrinking factor (SHRINK) of 8. For the evaluation of Coulomb and exchange integrals (TOLINTEG), tolerance factors of 7, 7, 7, 7, and 14 were used. Default optimization thresholds and integration grid for the density functional part were employed in all calculations. The effect of dispersion forces on energy was modeled using Grimme's empirical D2 model.26 The D2 model has a tendency to overemphasize weak interactions26b and therefore the SBIs in the optimized structures are shorter than the corresponding contacts in the experimental structures. Despite this overbinding, the calculated structures are considered to give meaningful relative strengths of the different chalcogen–chalcogen bonding interactions, which have been analyzed using topological analysis of the electron density.27
In previous studies, an empirical relationship between the hydrogen bond interaction energy and potential energy density at the bond critical point has been suggested by Espinosa et al. as Eint = VBCP/2.28 The use of this relationship has been extended by others to other weak closed-shell interactions29 and the relationship is adopted here as an additional descriptor for qualitatively comparing the relative strengths of chalcogen–chalcogen contacts and hydrogen bonds. It should be noted that the reliability of the results from the relationship has been questioned30 and they should be considered qualitative at most. Topological analysis was performed with the TOPOND module31 implemented in the CRYSTAL14 program. For TOPOND calculations, basis sets were modified by removing the f functions from iron and tellurium.
The donor–acceptor nature of the chalcogen–chalcogen interactions between trichalcogenaferrocenophanes has been studied using natural bond orbital (NBO) analysis32 on snapshots of the optimized crystal structures. Each of the snapshots included four molecules to represent the closest chalcogen–chalcogen interactions in the crystal structures (see the ESI†) and donor–acceptor interaction energies were estimated by second-order perturbation theory analysis between filled donor NBOs and vacant acceptor NBOs. The NBO analyses were carried out using NBO 5.9 software33 on Kohn–Sham orbitals from a PBE0/pob-TZVP single point Gaussian 09 calculation.34
Fig. 1 Molecular structure of [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) (1–9) indicating the labeling of the atoms. The crystal structures of 3, 4, 6, and 7 have been determined in this contribution. |
The variation in the packing of the [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) (1–9) complexes is shown in Fig. 2. [Fe(C5H4S)2S] (1),10 [Fe(C5H4S)2Se] (2),11 and [Fe(C5H4Se)2Se] (5a)12c are isomorphic, crystallizing in the monoclinic space group P21/c [see Fig. 2(a)].
Fig. 2 Packing of [Fe(C5H4E)2E′] (E, E′ = S, Se, Te) (1–9). (a) [Fe(C5H4S)2S] (1),10 [Fe(C5H4S)2Se] (2),11 and [Fe(C5H4Se)2Se] (5a),12c (b) [Fe(C5H4Se)2S] (4) and [Fe(C5H4Se)2Se] (5b),12a (c) [Fe(C5H4S)2Te] (3) and [Fe(C5H4Se)2Te] (6), (d) [Fe(C5H4Te)2S] (7), (e) [Fe(C5H4Te)2Se] (8),9 and (f) [Fe(C5H4Te)2Te] (9).10 The packings of 1, 2, 5a, 5b, 8, and 9 have been redrawn from crystallographic information in the appropriate references. |
They form loosely linked dimers with close contacts between the central chalcogen atoms. In 1, the S⋯S distance is 3.7056(11) Å (ref. 10) and in 2 and 5a, the corresponding Se⋯Se close contacts are 3.6394(8) (ref. 11) and 3.6348(11) Å,12c respectively [see Fig. 2(a)]. [Fe(C5H4Se)2S] (4) and [Fe(C5H4Se)2Se] (5b)12a are also mutually isomorphic (orthorhombic space group Pca21). These complexes form quasi-planar chains linked by terminal selenium atoms with the respective distances of 3.8705(12) Å and 3.9572(13) Å (ref. 12a) [see Fig. 2(b)]. Complexes 3 and 6–9 [see Fig. 2(c–f)] containing tellurium show supramolecular frameworks with more numerous and shorter intermolecular chalcogen–chalcogen contacts than complexes where the trichalcogena chain consists only of sulfur and selenium atoms. [Fe(C5H4S)2Te] (3) and [Fe(C5H4Se)2Te] (6) are mutually isomorphic (different monoclinic lattices from those of 1, 2, and 5a, though crystallizing also in the space group P21/c). The S⋯S, S⋯Te, and Te⋯Te close contacts in 3 are 3.5749(17), 3.4693(14) and 3.5119(13), and 3.8517(7) Å, respectively. The analogous Se⋯Se, Se⋯Te, and Te⋯Te distances in 6 are 3.5989(16) Å, 3.6239(15) Å and 3.6908(16) Å, and 3.8795(13) Å, respectively. The S⋯Te distance in 7 is 3.446(3) Å, the shortest Se⋯Te distance in 8 is 3.7044(14) Å,13 and the shortest Te⋯Te contacts in 7–9 are 3.5559(13), 3.7241(13)–3.9168(18),13 and 3.4552(17)–3.8691(17) Å,14 respectively. All these distances are well below the sums of van der Waals' radii of the elements in question.35
All complexes 1–9 are also linked together with H⋯E (E = chalcogen) bonds and also show E⋯π and H⋯π electron interactions involving the cyclopentadienyl rings. The shortest close contacts are exemplified in Fig. S1 (see the ESI†) for [Fe(C5H4S)2S] (1), [Fe(C5H4Se)2Se] (5a and 5b), and [Fe(C5H4Te)2Te] (9). The strength of these interactions does not seem to vary within the series. However, as the strength and the number of chalcogen–chalcogen interactions increase, the number of H⋯E, E⋯π and H⋯π interactions diminishes. Only the tellurium-containing complexes 3, 6, 8, and 9 exhibit π-stacking of the cyclopentadienyl rings.
Complex | BCPb | Contact | X-ray (Å) | R | Pauling BOd | DFT (Å) | Anglee | ρ BCP (e Å−3) | QTAIM BOg | V(bcp) (hartree bohr−3) | E INT (kJ mol−1) |
---|---|---|---|---|---|---|---|---|---|---|---|
a The entries of different complexes in the table have been sorted in the order of increasing QTAIM bond orders. b BCP = bond critical point. c Ratio of the interatomic distance and the sum of van der Waals' radii.35 d Pauling bond orders N have been calculated from intermolecular close contacts using the relationship ,36 in which Ro is the sum of covalent radii35 of the two atoms in question and Re is the interatomic distance in the experimental X-ray structure. e Optimized ∠E–E⋯E angle. f Electron density at bond critical point. g Relative QTAIM bond orders of intermolecular close contacts have been determined from bond critical point electron densities ρBCP calculated for the optimized structures using ρBCP of the intramolecular chalcogen–chalcogen bonds in [Fe(C5H4E)2E′] (1–9) as references for bonds with bond order of 1 (see the ESI). h Ref. 10. i Ref. 11. j Ref. 12. k Ref. 13. l Ref. 14. | |||||||||||
[Fe(C5H4S)2S] (1) | A | S⋯S–S | 3.7056(11)h | 1.00 | 0.10 | 3.562 | 161.5 | 0.006 | 0.04 | −0.00282 | −3.7 |
[Fe(C5H4S)2Se] (2) | A | Se⋯Se–S | 3.6394(8)i | 0.91 | 0.16 | 3.375 | 159.0 | 0.014 | 0.13 | −0.00782 | −10.3 |
[Fe(C5H4Se)2Se] (5a) | A | Se⋯Se–Se | 3.6348(11) | 0.91 | 0.16 | 3.402 | 155.0 | 0.013 | 0.12 | −0.00746 | −9.8 |
[Fe(C5H4Se)2S] (4) | B | Se⋯Se–S | 3.8705(17) | 0.97 | 0.12 | 3.607 | 159.0 | 0.010 | 0.09 | −0.00507 | −6.7 |
[Fe(C5H4Se)2Se] (5b) | B | Se⋯Se–Se | 3.9572(13)j | 0.99 | 0.10 | 3.606 | 156.6 | 0.010 | 0.09 | −0.00509 | −6.7 |
[Fe(C5H4S)2Te] (3) | C | S⋯S–Te | 3.5751(15) | 0.97 | 0.12 | 3.359 | 150.9 | 0.010 | 0.07 | −0.00634 | −8.3 |
D | Te⋯S–C | 3.5121(11) | 0.87 | 0.21 | 3.431 | 164.6 | 0.012 | 0.12 | −0.00645 | −8.5 | |
F | Te⋯Te–S | 3.8517(7) | 0.88 | 0.21 | 3.792 | 177.2 | 0.021 | 0.16 | −0.00454 | −6.0 | |
E | S⋯Te–S | 3.4692(13) | 0.86 | 0.23 | 3.287 | 177.4 | 0.018 | 0.19 | −0.00957 | −12.6 | |
[Fe(C5H4Se)2Te] (6) | C | Se⋯Se–Te | 3.5997(16) | 0.90 | 0.17 | 3.336 | 146.5 | 0.016 | 0.14 | −0.00945 | −12.4 |
D | Te⋯Se–C | 3.6240(14) | 0.86 | 0.22 | 3.423 | 163.5 | 0.015 | 0.18 | −0.00825 | −10.8 | |
F | Te⋯Te–Se | 3.8790(13) | 0.88 | 0.20 | 3.743 | 179.3 | 0.012 | 0.18 | −0.00503 | −6.6 | |
E | Se⋯Te–Se | 3.6915(16) | 0.88 | 0.20 | 3.408 | 175.1 | 0.018 | 0.21 | −0.00898 | −11.8 | |
[Fe(C5H4Te)2S (7) | G | Te⋯Te | 4.0070(13) | 0.91 | 0.16 | 3.764 | −/73.2 | 0.015 | 0.22 | −0.00630 | −8.3 |
H | S⋯Te–S | 3.446(3) | 0.85 | 0.23 | 3.137 | 175.6 | 0.023 | 0.24 | −0.01363 | −17.9 | |
I | Te⋯Te–S | 3.5559(13) | 0.81 | 0.32 | 3.267 | 161.9 | 0.028 | 0.41 | −0.01430 | −18.8 | |
[Fe(C5H4Te)2Se (8) | J | Se⋯Te–C | 3.9634(15)k | 0.94 | 0.14 | 3.816 | 135.6 | 0.009 | 0.11 | −0.00451 | −5.9 |
K | Te⋯Se–Te | 4.005(3)k | 0.95 | 0.12 | 3.752 | 138.6 | 0.010 | 0.12 | −0.00441 | −5.8 | |
L | Te⋯Se–Te | 4.117(3)k | 0.98 | 0.11 | 3.769 | 140.2 | 0.010 | 0.12 | −0.00429 | −5.6 | |
M | Se⋯Te–C | 3.7044(14)k | 0.88 | 0.19 | 3.582 | 161.9 | 0.013 | 0.15 | −0.00626 | −8.2 | |
N | Te⋯Te–C | 3.8756(13)k | 0.88 | 0.20 | 3.848 | 137.4 | 0.010 | 0.15 | −0.00421 | −5.5 | |
O | Te⋯Te–C | 3.7241(13)k | 0.85 | 0.25 | 3.623 | 169.4 | 0.011 | 0.16 | −0.00527 | −6.9 | |
P | Te⋯Te–Se | 3.9168(18)k | 0.89 | 0.19 | 3.769 | 164.0 | 0.013 | 0.19 | −0.00475 | −6.2 | |
Q | Te⋯Te–Se | 3.727(2)k | 0.85 | 0.25 | 3.493 | 173.8 | 0.019 | 0.28 | −0.00865 | −11.4 | |
[Fe(C5H4Te)2Te] (9) | R | Te⋯Te–Te | 3.8806(19)l | 0.88 | 0.20 | 3.923 | 147.7 | 0.008 | 0.12 | −0.00319 | −4.2 |
S | Te⋯Te–C | 3.8691(17)l | 0.88 | 0.20 | 3.877 | 172.4 | 0.010 | 0.15 | −0.00403 | −5.3 | |
T | Te⋯Te–C | 3.7472(17)l | 0.85 | 0.24 | 3.659 | 161.9 | 0.012 | 0.18 | −0.00538 | −7.1 | |
U | Te⋯Te–Te | 3.7124(18)l | 0.84 | 0.25 | 3.663 | 176.2 | 0.014 | 0.20 | −0.00602 | −7.7 | |
V | Te⋯Te–Te | 3.7673(18)l | 0.86 | 0.24 | 3.677 | 165.6 | 0.015 | 0.22 | −0.00589 | −7.7 | |
W | Te⋯Te–Te | 3.5493(18)l | 0.81 | 0.32 | 3.487 | 177.8 | 0.016 | 0.23 | −0.00734 | −9.6 | |
X | Te⋯Te–Te | 3.6828(18)l | 0.84 | 0.27 | 3.503 | 172.4 | 0.019 | 0.28 | −0.00836 | −11.0 | |
Y | Te⋯Te–Te | 3.4552(17)l | 0.78 | 0.36 | 3.388 | 176.7 | 0.024 | 0.35 | −0.01087 | −14.3 |
Fig. 3 The QTAIM bond critical points in the optimized structures of (a) [Fe(C5H4S)2S] (1), [Fe(C5H4S)2Se] (2), and [Fe(C5H4Se)2Se] (5a), (b) [Fe(C5H4Se)2S] (4) and [Fe(C5H4Se)2Se] (5b), (c) [Fe(C5H4S)2Te] (3) and [Fe(C5H4Se)2Te] (6), (d) [Fe(C5H4Te)2S] (7), (e) [Fe(C5H4Te)2Se] (8), and (f) [Fe(C5H4Te)2Te] (9). For the intermolecular distances and bond orders, see Table 1. |
Consistent with the relatively long close contacts in complexes 1, 2, 4, and 5, which are near to the sums of the corresponding van der Waals radii of the atoms in question, the electron density values at bond critical points, as well as both the Pauling and QTAIM bond orders and interaction energies, indicate that the intermolecular chalcogen–chalcogen interactions in these complexes are weak (see Table 1). The electron density values at bond critical points, the bond orders, and the interaction energies are higher in complexes 3, 6, and 7–9, which contain tellurium. This is in accordance with the conclusions of previous studies.3,4
A simple model of donation of the p lone-pair electrons to the anti-bonding σ* orbital has been used to describe the chalcogen–chalcogen SBIs qualitatively,3,4 though they can also be accounted for by the presence of a σ-hole together with electrostatic and polarization effects.2 The correlation between QTAIM bond orders and the collinearity of the E⋯E′–X moieties (E, E′ = S, Se, Te; X = S, Se, Te, C) shown by the interactions (see Table 1) are in agreement with both models of the interactions.
In order to compare the relative donor–acceptor interaction strengths, we carried out NBO analyses for [Fe(C5H4S)2S] (1), [Fe(C5H4Se)2Se] (5a and 5b), and [Fe(C5H4Te)2Te] (9). The main interaction modes have been shown in Fig. 4.
[Fe(C5H4S)2S] (1) shows very weak interactions of types n(3p)2 → σ*(S–S) and n(3s)2 → σ*(S–S) shown in Fig. 4(a) and (d), respectively. In both cases, the NBO interaction energies are approximately 1.5 kJ mol−1. The corresponding interaction energies between the selenium atoms in the isomorphic [Fe(C5H4Se)2Se] (5a) are around 2.9 kJ mol−1. The interaction energies in 5b are comparable, though the donor–acceptor interaction n(3p)2 → σ*(Se–C) is somewhat stronger being 7.9 kJ mol−1. It is only with [Fe(C5H4Te)2Te] (9) that the interaction energies are significantly higher. The largest interaction energies in 9 are shown in Fig. 5 together with the observed and computed intermolecular distances. It can be seen that they correlate very well with the closest intermolecular contacts observed in the crystal structures and also with the relative QTAIM electron density values, bond orders, and interaction energies (see Table 1).
All significant interaction energies in 9, which are shown in Fig. 5, are found for n(5pTe)2 → σ*(Te–Te) interactions involving the donation from the terminal tellurium in the Te3 chain [see Fig. 4(a)]. All other interactions shown in Fig. 4 are below 16 kJ mol−1.
Electrostatic effects involving the lone-pair electrons and the σ-holes of the chalcogen–chalcogen bonds strengthen the attractive interaction between the complexes in each case. This effect may be inferred by the PBE0/pob-TZVP natural charges of the chalcogen atoms, as shown in Table 2. The charge on the central chalcogen atom is nearly zero, as expected for atoms in the middle of homonuclear chains. The terminal chalcogen atoms, however, carry a significant positive charge. It is reasonable that these atoms are attracted by lone-pair electrons. Also, this effect is most prominent in the case of tellurium.
Complex | Bridging chalcogen atom | Terminal chalcogen atoms | ||
---|---|---|---|---|
Range | Average | Average | Range | |
[Fe(C5H4S)2S] (1) | −0.041 to −0.065 | −0.049 | +0.159 to +0.176 | +0.166 |
[Fe(C5H4Se)2Se] (5a) | −0.019 to −0.054 | −0.036 | +0.199 to +0.221 | +0.207 |
[Fe(C5H4Se)2Se] (5b) | −0.029 to −0.059 | −0.041 | +0.196 to +0.216 | +0.205 |
[Fe(C5H4Te)2Te] (9) | −0.043 to −0.113 | −0.084 | +0.204 to +0.355 | +0.284 |
Complex | Contact | Exptl. (Å) | Calc. (Å) | ρ (e Å−3) | V(bcp) (hartree bohr−3) | E INT (kJ mol−1) |
---|---|---|---|---|---|---|
a Ct denotes the centroid of the carbon atoms in the cyclopentadienyl ring. b Ref. 10. c Ref. 12. d Ref. 14. | ||||||
[Fe(C5H4S)2S] (1) | S⋯H | 2.9897(8)–3.1018(9)b | 2.568–2.738 | 0.0057–0.0138 | −0.00258–(−0.00687) | −3.4–(−9.0) |
S⋯Cta | 3.5803(10)b | 3.370 | ||||
H⋯Cta | 3.2626(9)–3.4998(11)b | 2.867–3.322 | ||||
[Fe(C5H4Se)2Se] (5a) | Se⋯H | 3.0271(6)–3.2309(6) | 2.636–2.865 | 0.0092–0.0157 | −0.00448–(−0.00794) | −5.9–(−10.4) |
Se⋯Cta | 3.6701(6)–3.9977(9) | 3.429–3.653 | ||||
H⋯Cta | 3.2477(6) | 2.781 | ||||
[Fe(C5H4Se)2Se] (5b) | Se⋯H | 3.0789(6)–3.2436(7)c | 2.664–3.039 | 0.0140 | −0.00779 | −10.2 |
Se⋯Cta | 3.8875(8)c | 3.603 | ||||
H⋯Cta | 3.2770(8)c | 2.812 | ||||
[Fe(C5H4Te)2Te] (9) | Te⋯H | 3.3573(12)–3.6521(13)d | 2.980–3.432 | 0.0061–0.0084 | −0.00249–(−0.00354) | −3.3–(−4.6) |
H⋯Cta | 3.2721(12)–3.4430(13)d | 3.031–3.346 | ||||
Ct⋯Cta | 3.7991(14)d | 3.741 |
It can also be verified in Table 3 that the cyclopentadienyl rings are only involved in π-stacking in the case of 9.
Complexes 1, 2, 4, 5a and 5b show only weak intermolecular interactions. The isomorphous 1, 2, and 5a form dimers where the most significant interaction is between the central chalcogen atoms of the two trichalcogena chains of adjacent complexes. In the second isomorphous series consisting of 4 and 5b, the complexes are linked together into continuous chains by short contacts via the terminal selenium atoms.
The intermolecular interactions are expectedly stronger in complexes 3, 6, and 7–9, which contain tellurium. The NBO comparison of donor–acceptor interactions in the lattices of [Fe(C5H4S)2S] (1), [Fe(C5H4Se)2Se] (5a and 5b), and [Fe(C5H4Te)2Te] (9) show that the n(5pTe)2 → σ*(Te–Te) interactions in 9 are the strongest. All other interaction energies are significantly smaller even in the case of tellurium. The computed natural charges of the chalcogen atoms indicate that electrostatic effects strengthen the attractive interactions in the case of all chalcogen atoms.
Footnote |
† Electronic supplementary information (ESI) available: X-ray crystallographic information, QTAIM bond orders and NBO analysis, and NMR spectroscopic information. CCDC 1455391–1455394, CIF files of PBE0/def2-TZVPP optimized crystal structures. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c6ce00451b |
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