Synthesis and Characterization of Bidentate Isonitrile Iron Complexes.

The divalent iron complexes trans-[FeBr2(BINC)2], [Cp*FeCl(BINC)] (Cp* = Me5C5), and [FeBr2(CNAr3NC)2] with the chelating bis(isonitrile) ligands BINC (bis(2-isocyanophenyl)phenylphosphonate) and CNAr3NC (2,2″-diisocyano-3,5,3″,5"tetramethyl-1,1':3',1″-terphenyl) have been prepared and characterized. Their subsequent reduction yields the di- and trinuclear compounds [Fe3(BINC)6], [Cp*Fe(BINC)]2, [Fe(CNAr3NC)2]2, and [K(Et2O)]2[Fe(CNAr3NC)2]2. The molecular structures of all new species were determined by X-ray crystallography and compared to those of related iron carbonyl complexes, demonstrating that the bidentate isonitrile ligands are capable surrogates for two CO ligands with only minimal distortion of the tetrahedral or octahedral geometry of the parent complexes. The complexes were further characterized by NMR and IR spectroscopy, and the electrochemical properties of selected compounds were analyzed by UV-vis-NIR spectroelectrochemistry.

Introduction

With the discovery of n class="Chemical">isonitriles by Lieke[1] in 1859 came a new and emerging field within organometallic chemistry.[2] Isonitriles show stronger σ-donating character and weaker π-acceptor properties in comparison to carbon monoxide. However, they feature similar behavior when they coordinate to metals as both terminal and bridging ligands.[3,4] Isonitriles can be electronically and sterically tuned through modification of their organic substituents, which makes them versatile ligands for metal catalysis.[5] Chelating bis(isonitriles) confer rigidity to metal complexes, which has been proven to be especially valuable for the design of 3d-metal complexes with sufficient excited-state lifetimes to efficiently initiate single-electron-transfer (SET) processes. This approach has been successful for copper,[6] molybdenum,[7] and rhenium,[8] providing alternatives to established but scarce ruthenium- and iridium-based photocatalysts.[9]

Extending this concept to n class="Chemical">iron holds the promise of making this metal broadly available for photocatalysis. This is especially challenging, given that excited-state lifetimes of iron complexes are often in the picosecond range and have been reported at best in the low-nanosecond range.[10] However, there is only limited data available on coordination complexes of iron with bidentate isonitriles,[20−23] in contrast with monodentate isonitrile iron complexes, which have attracted considerable attention due to the high prevalence of iron carbonyl complexes.[11] For example, dinuclear iron complexes such as [CpFe(CNPh)2][12] (A, Ph = C6H5) and [Fe2(CNPh)9][13] (B) feature terminal and bridging isonitrile ligands (Figure ).

Figure 1

Selected examples of di- and trinuclear iron isonitrile complexes.

The trinuclear compound [n class="Chemical">Fe3(CO)10(CNPh)2] (C)[14] possesses both CO and monodentate isonitrile ligands, having replaced two of the axial CO ligands in [Fe3(CO)12]. Iron isonitrile analogues of [Fe(CO)4]2–, [Fe(CNXyl)4]2– (Xyl = 2,6-Me2C6H3)[15] and [Fe(CNArMes2)4]2– (ArMes2 = 2,6-(2,4,6-Me3C6H2)2C6H3),[16] further demonstrate the propensity of monodentate isonitriles to act as surrogates for CO.

In comparison to monodentate n class="Chemical">isonitrile ligands, the reactivity and coordination chemistry of bidentate isonitriles has been generally unexplored.[5] Given the linear structure of the isonitrile unit, such ligands need to form much larger chelates relative to the typical N,N- or P,P-ligands that are commonly found in five- and six-membered rings. The minimal ring size in a bidentate isonitrile–metal complex was found to be 12.[19] With this design concept, a number of iron(II) complexes with bidentate isonitrile ligands were realized; representative examples are D–G (Figure ).[5,20−23]

Some of us have previously been interested in the synthesis and reactivity of low-oxidation-state polyarene and n class="Chemical">alkene ferrates.[24] Such complexes have been used for various applications, including the activation of small molecules (e.g., P4 and CO2) and as catalysts for hydrogenation and hydroboration reactions.[25] Taking advantage of the well-known ability of isonitriles to stabilize low-oxidation-state transition-metal complexes,[15−18,26] in combination with imposing rigidity, we were interested in exploring the potential of the aforementioned chelating isonitrile ligands in the stabilization of highly reduced iron complexes. We particularly questioned if polynuclear iron complexes with chelating bis(isonitrile) ligands can still be formed, for which to the best of our knowledge no previous examples have been described in the literature. Here, we report the synthesis and characterization of new iron complexes with the ligands BINC (bis(2-isocyanophenyl)phenylphosphonate) and CNAr3NC (2,2″-diisocyano-3,5,3″,5”tetramethyl-1,1′:3′,1″-terphenyl, demonstrating that indeed di- and trinuclear structures can be realized.

Results and Discussion

Treating anhydrous Fen class="Chemical">Br2 with 2 equiv of BINC resulted in the formation of trans-[FeBr2(BINC)2] (1) as a blue solid in 33% isolated yield (Scheme ). Compound 1 displays structural and spectroscopic features similar to those of compounds D–G (see Figure S34 in the Supporting Information for a graphical representation of the structure).

Scheme 1

Synthesis of [FeBr2(BINC)2] (1) and [Fe3(BINC)6] (2)

Reduction of 1 with an excess of KC8 in n class="Chemical">THF afforded an orange-brown solution from which brown crystals of [Fe3(BINC)6] (2) were isolated in a yield of 26% by slow diffusion of n-hexane into the reaction mixture.

Single-crystal X-ray diffraction (XRD, Figure ) revealed that 2 crystallizes in the space group P1̅ with two molecules in the unit cell. At first glance, the structure of 2 resembles that of [n class="Chemical">Fe3(CO)12] (H) with respect to the Fe1–Fe2–Fe3 core (Table ), showing that the the BINC ligand can displace the carbonyl groups without imposing constraints due to its chelating structure. Each atom in the triiron core is coordinated by two BINC ligands, displaying one shorter and two longer Fe–Fe bonds (Fe2–Fe3 2.495(6) Å vs Fe1–Fe2 2.682(6) Å and Fe1–Fe3 2.685(6) Å) resembling an isosceles triangle. The shorter Fe2–Fe3 bond features two bridging isonitrile donor moieties, similar to the case for H which possesses ten terminal and two bridging carbonyl ligands.[27] Nevertheless, due to the chelate ring in the bis(isonitrile) ligand the triiron core of 2 shows slightly widened bond angles of 62.37 and 62.23° for Fe1–Fe2–Fe3 and Fe2–Fe3–Fe1, respectively, and a more acute angle of 55.41° for Fe2–Fe1–Fe3 in comparison with H (61.6, 61.2, and 57.2°, respectively).

Figure 2

Solid-state molecular structure of the complex [Fe3(BINC)6] (2). Ellipsoids are drawn at the 40% probability level. H atoms and disorder in the phenyl groups are omitted for clarity. Selected bond lengths (Å) and angles (deg): Fe1–C1 1.839(3), C1–N1 1.176(4), Fe2–C81 2.014(3), Fe3–C81 1.945(3), C81–N10 1.235(4), Fe2–C41 1.853(3), C41–N5 1.168(4); Fe2–C81–Fe3 78.10(1), Fe1–Fe2–C81 89.64(8), C81–Fe3–Fe1 91.04(8). Fe–Fe distances and Fe–Fe–Fe angles are given in Table .

Table 1

Selected Bond Lengths (Å) and Angles (deg) of 2 and [Fe3(CO)12] (H)a

	2	[Fe3(CO)12]
Fe1–Fe2	2.682(6)	2.677(2)
Fe2–Fe3	2.495(6)	2.558(1)
Fe3–Fe1	2.685(6)	2.683(1)
Fe1–Fe2–Fe3	62.37(2)	61.6(2)
Fe2–Fe3–Fe1	62.23(2)	61.2(2)
Fe3–Fe1–Fe2	55.41(2)	57.2(2)

The data for 2 were collected at 123 K, while the data for H were collected at room temperature.[27]

Solid-state molecular structure of the n class="Chemical">complex [Fe3(BINC)6] (2). Ellipsoids are drawn at the 40% probability level. H atoms and disorder in the phenyl groups are omitted for clarity. Selected bond lengths (Å) and angles (deg): Fe1–C1 1.839(3), C1–N1 1.176(4), Fe2–C81 2.014(3), Fe3–C81 1.945(3), C81–N10 1.235(4), Fe2–C41 1.853(3), C41–N5 1.168(4); Fe2–C81–Fe3 78.10(1), Fe1–Fe2–C81 89.64(8), C81–Fe3–Fe1 91.04(8). Fe–Fe distances and Fe–Fe–Fe angles are given in Table .

The 31P{n class="Chemical">1H} NMR spectrum of 2 shows only one singlet at δ 13.2 ppm in THF-d8, indicating a fluxional behavior by fast exchange of the bridging C≡N units in solution. In agreement with this analysis, only one 13C{1H} NMR signal is observed for the isonitrile carbon atoms at δ 218.7 ppm, which is shifted downfield in comparison to the corresponding signal of the free BINC ligand (δ 172.4 ppm). The solid-state infrared spectrum of 2 features a broad band centered at 2035 cm–1 assignable to the isonitrile ν[CN] stretch, shifted to lower wavenumbers in comparison to the isonitrile ν[CN] stretch in 1 (2122 cm–1). The ν[CN] stretching frequency for the divalent complex 1 is similar to that of the free BINC (2126 cm–1), as the isonitrile functions essentially as a pure donor ligand. In contrast, compound 2, with an iron center in the formally zerovalent oxidation state, shows ν[CN] stretching frequencies shifted to lower energies, shortened terminal Fe–C bond lengths (av. 1.83(1) Å vs 1.87(4) Å in 1), and slightly more bent Fe–C–N angles (172.5(3)° vs 176.1(1)° in 1). When they are taken together, these data indicate substantial M(dπ) → π* back-bonding in 2.[28]

The electrochemical behavior of 2 (see Figure S41 in the Supporting Information) was analyzed with UV–vis–NIR spectroelectrochemistry (SEC) in an optically transparent thin-layered electrode (OTTLE) cell.[29] The cyclic voltammogram showed a single partially reversible oxidation at Epa = −0.6 V versus [FeCp2]0/+, which was used as the internal standard for all potentials reported herein unless otherwise noted. The neutral n class="Chemical">complex could be regenerated at Epc = −1.35 V. The SEC for the oxidation process showed that the bands at 350 and 715 nm were consumed and replaced by a band at 475 nm with a shoulder at 580 nm. The spectrum of 2 could be regenerated after a cathodic potential of <1.5 V was reached. The electrochemical behavior of [Fe3(CO)12] in THF was reported to show only irreversible processes.[30]

Other prominent motifs for iron(II) n class="Chemical">complexes are mononuclear and dinuclear iron carbonyl species such as [CpFeCl(CO)2] (I), which was first synthesized by Hubbard,[31] and [CpFe(CO)2]2 (J).[32] In the case of J it was demonstrated that the CO ligands could be substituted with monodentate isonitrile ligands, resulting in A (Figure ). Again, we questioned if substitution by the bidentate isonitrile ligand BINC is also tolerated.

With [Cp*FeCl(tmeda)][33] (Scheme ; K, n class="Chemical">tmeda = tetramethylethylene-1,2-diamine) as the starting material, the mononuclear [Cp*FeCl(BINC)] (3, Cp* = Me5C5) could be readily synthesized in 82% yield and fully characterized by NMR/IR spectroscopy and XRD (see Figure S35 in the Supporting Information). The iron atom possesses a distorted-tetrahedral geometry, being η5-coordinated by the Cp* ligand, the two isonitrile moieties of the BINC ligand, and a chloride ligand. The carbon monoxide analogue I has a similar distorted-tetrahedral geometry in which the chloride and the two CO ligands are sterically repelled by the η5-coordinated cyclopentadienyl ligand and possess a C–Fe–C angle of 95.6(2)° and a C–Fe–Cl angle of 90.4(2)° (vs angles in 3: C1–Fe–C20 88.4(7)°, C1–Fe–Cl 94.3(6)°, C20–Fe–Cl 91.4(6)°).[34] The 31P{1H} NMR spectrum of 3 gives rise to a sharp singlet at δ 15.2 ppm. The IR spectrum shows two broad bands at 2084 and 2023 cm–1, which are assigned to the symmetrical and asymmetrical CN stretching vibrations.

Scheme 2

Synthesis of [Cp*FeCl(BINC)] (3) and [Cp*Fe(BINC)]2 (4)

The reduction of 3 in THF at low temperatures with 1 equiv of n class="Chemical">KC8 affords green crystals of 4 in a yield of 18% after workup and crystallization from THF/n-hexane (Scheme ). Single-crystal XRD revealed that 4 crystallizes as the cis isomer, in which the Cp* groups are both coordinated above the Fe–Fe bond (Figure ). One C≡N unit of the BINC ligands links terminally to iron, while the other bridges the iron–iron bond. As a result of the double bridging isonitrile units there is an Fe–Fe bond of 2.575 Å. The iron-bound bridging isonitrile groups result in an almost planar butterfly motif (Fe1–C20–Fe2–C40) with a torsion angle of 7.82°.

Figure 3

Solid-state molecular structure of the complex [Cp*Fe(BINC)]2 (4). Ellipsoids are drawn at the 40% probability level. H atoms, solvent molecules, and disorder in the Cp* groups are omitted for clarity. Selected bond lengths (Å) and angles (deg): Fe1–Fe2 2.575(3), Fe1–C20 1.914(2), Fe2–C20 1.956(2), C20–N2 1.242(2), C21–N3 1.178(2), Fe1–C1 1.787(2), Fe2–C21 1.795(2) C1–N1 1.176(2), Fe1–C40 1.936(2), Fe2–C40 1.919(2), C40–N4 1.246(2); C1–Fe1–Fe2 95.48(3), C1–Fe1–C20 89.88(5), C21–Fe2–Fe1 96.85(5), Fe1–C1–N1 173.08(1), Fe2–C21–N3 173.93(1), C20–Fe1–C40 96.26(7), Fe1–C20–Fe2 83.43(7).

The structure of 4 is related to that of the phenyl n class="Chemical">isonitrile complex trans-[CpFe(CNPh)2]2 (A, see Figure ), which was already reported by Fehlhammer in 1980.[12] In contrast to 4, compound A crystallizes in a trans/anti configuration with a strictly planar Fe2C2 core. The Fe–Fe bond in A is 2.523(1) Å, which is shorter than that in complex 4 (2.575(3) Å). In both complexes the aryl groups of the bridging isonitrile units show an anti conformation.

The NMR spectroscopic measurements indicate 4 is in a cis/trans isomer equilin class="Chemical">brium in THF-d8 (Scheme ) that is not affected by temperature changes (see Figure S16 in the Supporting Information).

Scheme 3

cis/trans Isomer Equilibrium of Compound 4 in Solution

The ratio of the isomers depends on the isolated form of 4; the crystalline product gives rise to the cis isomer as the main component, while for an amorphous powder the trans isomer predominates (see the Supporting Information for spectra).

The occurrence of cis and trans isomers observed for 4 is also found in the dinuclear carbonyl analogue n class="Chemical">[CpFe(CO)2]2 (J).[35] X-ray crystal structures for both trans-J[32] and cis-J[36,37] were obtained. The structure of the cis isomer contains a shortened iron–iron bond (2.531(2) Å vs compound 4, Fe1–Fe2 2.575(3) Å; Table ) due to the smaller ligands coordinated to the iron centers.[36] It is noteworthy that the sterically more hindered permethylated derivative [Cp*Fe(CO)2]2[38] (L) appears to exist exclusively as the trans isomer, although the cis configuration has been observed as a short-lived, photogenerated species.[37] In contrast, 4 exists both as the cis and trans isomers in solution. Nevertheless, the structural parameters of A, J, L, and 4 are similar. This shows that the exchange of the ancillary ligands (Cp vs Cp*, and CO vs CNPh and BINC) influences the solution behavior, but it does not strongly affect Fe–C and C–N bond lengths and Fe–C–N angles.

Table 2

Comparison of Selected Bond Lengths (Å) and Angles (deg) of Compound 4, cis-[CpFe(CO)2]2 (J),[36]trans-[Cp*Fe(CO)2]2 (L),[39] and [CpFe(CNPh)2]2 (A)[12]

	4	J	L	A
Fe1–Fe2	2.575(3)	2.531(2)	2.560(1)	2.523(1)
Fe1–Cterminal	1.787(2)	1.730(7)	1.753(3)	1.775(6)
Cterminal–N/O	1.176(2)	1.159(9)	1.154(3)	1.161(8)
Fe1–Cbridged	1.914(2)	1.918(7)	1.936(2)	1.934(6)
Fe2–Cbridged	1.956(2)	1.908(7)	1.936(2)	1.905(6)
Cbridged–N/O	1.242(2)	1.178(9)	1.172(3)	1.242(8)
Cterminal–Fe1–Cbridged	89.88(5)	92.3(3)	95.2(1)
Fe1–Cterminal–N/O	173.08(1)	176.5(8)	175(8)	178.4(4)

The electrochemical behavior of 4 in 0.1 M nBu4NPF6/n class="Chemical">THF showed a partially reversible oxidation wave at Epa = −0.7 V versus [FeCp2]+/0 and two irreversible processes at Epa = −0.35 and 0.05 V. SEC of 4 showed that the bands at 600 and 390 nm decreased upon oxidation, and the process was irreversible (Figure S42 in the Supporting Information). In contrast, the CV of compound 4 in CH2Cl2 (Figure S43 in the Supporting Information) showed more resolved redox transitions at −0.7, – 0.15, 0.3, and 0.65 V. No reduction signal was observed. These transitions were partially reversible according to the UV–vis SEC spectrum, which showed that the absorption bands at 310 and 370 nm were consumed and a band at 290 nm appeared. Upon further oxidation the band at 600 nm was consumed and the band at 290 nm coalesced.

In hopes of isolating isonitrile ferrate n class="Chemical">complexes with greater kinetic shielding, BINC was substituted for the bulkier bidentate chelating isonitrile CNAr3NC.[7] The addition of 2 equiv of CNAr3NC to a solution of anhydrous FeBr2 in THF affords an orange suspension, from which [FeBr2(CNAr3NC)2] (5) can be isolated as orange crystals in 55% yield after crystallization from CH2Cl2/n-hexane (Scheme ). The solid-state molecular structure of 5 shows a distorted-octahedral geometry at the iron center with a cis configuration of the bromido ligands (Br1–Fe1–Br2 92.12(2)°; see the Supporting Information for a graphical representation of the structure and further characterization details).

Scheme 4

Synthesis of [FeBr2(CNAr3NC)2] (5), [Fe(CNAr3NC)2]2 (6), and [K(Et2O)]2[Fe(CNAr3NC)2]2 (7)

Reduction of 5 in THF at low temperature with 2 equiv of n class="Chemical">KC8 (Scheme ) results in an orange-red solution from which dark red crystals of [Fe(CNAr3NC)2]2 (6) were isolated in a yield of 12%. The 1H NMR spectra and two-dimensional experiments (1H,1H-NOESY) show that compound 6 is isolated in an equilibrium with one main isomer (cis isomer; see the solid-state molecular structure in Figure ) and two other species (presumably isomers) with minor populations (see the Supporting Information for spectra).

Figure 4

Solid-state molecular structures of [Fe(CNAr3NC)2]2 (6, on the left) and [K(Et2O)]2[Fe(CNAr3NC)2]2 (7, on the right). Ellipsoids are drawn at the 40% probability level. H atoms and solvent molecules are omitted for clarity. Selected bond lengths (Å) and angles (deg) of 6: Fe1–Fe2 2.434(6), Fe1–C1 1.835(3), C1–N1 1.165(4), Fe1–C25 1.977(3), Fe2–C25 1.900(3), C25–N3 1.244(4), Fe1–C24 1.860(3), C24–N2 1.176(4), Fe2–C48 1.800(3), C48–N4 1.186(4); Fe1–C25–Fe2 77.73(1), C1–Fe1–C24 87.39(1), Fe1–C1–N1 178.3(3). Selected bond lengths (Å) and angles (deg) of 7: Fe1–Fe2 2.552(8), Fe1–C1 1.747(5), Fe1–C24 1.838(5), Fe1–C25 1.951(4), Fe2–C25 1.963(4), Fe2–C48 1.789(4), Fe1–K1 3.439(1), Fe2–K2 3.410(1), C1–N1 1.214(9), C24–N2 1.176(6), C25–N3 1.266(5), C48–N4 1.206(5), Fe1–C25–Fe2 81.38(2), Fe1–C1–N1 146.0(6), Fe1–C24–N2 170.7(4), Fe1–C25–N3 142.9(3), Fe2–C25–N3 135.2(3).

Single-crystal XRD of 6 confirms the formation of a dimeric n class="Chemical">iron complex with four CNAr3NC isonitrile ligands, two of which are bridging the iron–iron bond. Compound 6 features a relatively short metal–metal bond (2.434(6) Å) because of the bridging isonitrile ligands and assumes a butterfly structural motif. The Fe1–C25–Fe2–C49 torsion angle is 17.9°, which indicates the Fe–C–Fe–C moiety is nearly planar.

A structural arrangement n class="Chemical">comparable to that of 6 is the structure of the unsaturated dinuclear iron carbonyl complex [Fe2(CO)8] (M), which was first observed in 1971 by Poliakoff and Turner as one of the main products from the low-temperature photolysis of [Fe2(CO)9] conducted in CO matrixes.[40,41] On the basis of infrared spectroscopic measurements the CO-bridged and unbridged isomers of M were proposed.[40] The calculated iron–iron bond length (2.482 Å, Table , BP86/TZVP) of the singlet state of M with C symmetry (global minimum) matches with the symmetry (two bridged CO units) and bond lengths of the solid-state molecular structure of 6 (Fe1–Fe2 2.434(6) Å).

Table 3

Comparison of Selected Bond Lengths (Å) and Angles (deg) (Average Values) of 6 and [Fe2(CO)8] (M[40])a

	6	M
Fe–Fe	2.434(6)	2.482
Fe–Cbridged	1.939	1.982
Cbridged–N/O	1.240	1.177
Fe–Cterminal	1.848	1.802
Cterminal–N/O	1.171	1.154
Fe–Cterminal–N/O	174.88	178.00

Optimized singlet geometry in C symmetry (BP86/TZVP).

The heightened stability and analogous nature of 6 in comparison to M allows for the latter’s stn class="Chemical">ructural realization, something not possible previously due to its inherent instability. As expected for CN-bridged 6 with C symmetry, an analysis of the DFT calculated CN stretching frequencies determined six IR-active modes (for a comparison of the calculated IR spectra of M and 6, see the Supporting Information). The solid-state IR spectrum of 6 features two specific ν[CN] bands at 2070 and 2022 cm–1 (broad bands) for the terminally and bridged coordinated isonitrile units, respectively. These data are in good agreement with the DFT calculated values (see the Supporting Information for further details).

It was previously reported that when monodentate isonitrile ligands were used it was not possible to isolate a dinuclear n class="Chemical">iron complex bearing eight ligands. An example is [Fe2(CNPh)9] (B, Fe–Fe 2.458(1) Å; see Figure ), which is synthesized in a manner comparable to that of 6 except partial decomposition must occur to provide an extra isonitrile ligand.[13] This result shows that the use of the sterically demanding bidentate ligand CNAr3NC is key to the successful stabilization of 6, allowing for the isolation of a dinuclear iron complex with a lower coordination number.

When the reduction of 5 is repeated with 3 equiv of finely ground KC8 instead of 2 equiv in n class="Chemical">THF at −80 °C, a brownish orange solution forms from which [K(Et2O)]2[Fe(CNAr3NC)2]2 (7) can be isolated as a black solid in 46% yield by crystallization from Et2O (Scheme ). The solid-state molecular structure of 7 shows a motif similar to that for complex 6. The iron–iron bond is bridged by two isonitrile units, and the other ligands coordinate terminally to the iron centers. In the solid state, 7 is a contact-ion pair with significant interactions between the potassium and bridging isonitrile units.

The dinuclear dianionic complex [n class="Chemical">Fe2(CO)8]2– (N), which was first reported by Hieber and Brendel,[42] is the carbon monoxide analogue of compound 7. The solid-state structures of N feature different coordination modes depending on the counterion used. Single-crystal XRD of [Na(DMF)3]2[Fe2(CO)8] (Na-N) shows no bridging CO ligands, explaining why the Fe–Fe bond is significantly longer (2.804(1) Å) than the metal–metal bond in 7 (Fe–Fe 2.552(8) Å).[43] The solid-state structure of [Li(THF)3]2[Fe2(CO)8] (Li-N),[44] in which the lithium atoms are bonded to the oxygen atoms of bridging CO groups, shows the same symmetry (C2) and coordination motif as for compound 7, which results in similar bond lengths (Table , 2.551(1) Å vs 2.552(8) Å for 7). Because of the bridging CO/isonitrile ligands, complexes Li-N and 7 both assume a butterfly structural motif and show similar Fe–C–Fe–C torsion angles of 40.6(3)° for Li-N and 38.5(2)° for 7.

Table 4

Comparison of Selected Bond Lengths (Å) and Angles (deg) of 7, [Li(THF)3]2[Fe2(CO)8] (Li-N),[44] and [Na(DMF)3]2[Fe2(CO)8] (Na-N)[43]

	7	[Li-N]	[Na-N]
Fe–Fe	2.552(8)	2.551(1)	2.804(1)
Fe–Cbridged	1.951(4)	1.929(8)
Cbridged–N/O	1.266(6)	1.216(9)
Fe–Cterminal	1.838(5)	1.765(8)	1.781(2)
Cterminal–N/O	1.176(6)	1.164(1)	1.158(2)
Fe–Cterminal–N/O	170.7(4)	177.5(7)	176.8(2)

Conclusion

We have reported the synthesis and characterization of n class="Chemical">isonitrile analogues of the classic tri- and dinuclear iron carbonyl complexes. The reduction of the iron(II) precursors trans-[FeBr2(BINC)2] (1), [Cp*FeCl(BINC)] (3) and [FeBr2(CNAr3NC)2] (5) led to oligonuclear iron compounds with chelating bidentate isonitrile ligands. [Fe3(BINC)6] (2) possesses a triangular iron arrangement that is comparable to the structural motif of [Fe3CO12] and has been shown to have fluxional behavior with the bridging and terminal coordinated isonitrile units in solution. The reduction of compound 3 resulted in the dimeric heteroleptic complex [Cp*Fe(BINC)]2 (4) as a cis/trans isomer mixture. The reduction of 5 bearing a bulkier isonitrile ligand results in [Fe(CNAr3NC)2]2 (6) and [K(Et2O)]2[Fe(CNAr3NC)2]2 (7), both possessing a butterfly arrangement. In contrast to its CO analogue [Fe2(CO)8], compound 6 is stable and isolable at room temperature. A detailed comparison of the spectroscopic and structural parameters of complexes 4–7 to mono(isonitrile) and CO analogues shows that replacing these monodentate ligands with bidentate isonitrile molecules, such as BINC and CNAr3NC, does not dramatically affect the molecular or electronic structures. Thus, future investigations will be aimed at the synthesis of further highly reduced ferrate complexes and their utilization for electro- or photocatalysis, where the stable coordination of bidentate (chelating) isonitrile ligands might be beneficial.

Experimental Section

General Procedures

All experiments were performed under an atmosphere of dry argon (n class="Chemical">Argon 4.6, Linde) using standard Schlenk line techniques, a MBraun UniLab Glovebox, or a GS Glovebox (GS117717). Solvents were dried and degassed with the MBraun SPS800 solvent-purification system. THF, diethyl ether, and DCM were stored over molecular sieves (3 Å). n-Hexane was stored over a potassium mirror. Deuterated tetrahydrofuran was purchased from Sigma-Aldrich and used as received.

Elemental analyses were determined by the analytical department of the University of Regensburg with a Micro Vario Cube (Elementar).

NMR Spectroscopy

NMR spectra were recorded on n class="Chemical">Bruker Avance 300 (300 MHz) and Bruker Avance 400 (400 MHz) spectrometers at 300 K if not stated otherwise. 1H and 13C{1H} spectra were referenced internally to residual solvent resonances, while 31P{1H} spectra were referenced externally to 85% H3PO4(aq). The assignment of 1H and 13C NMR signals was confirmed by two-dimensional (1H,1H-COSY, 1H,1H-NOESY, 1H,13C-HSQC, 1H,13C-HMBC) experiments. The following abbreviations have been used for multiplicities: s, singlet; d, doublet; t, triplet; q, quartet; m, multiplet; dd, doublet of doublets.

IR Spectroscopy

IR spectra were recorded using a n class="Chemical">Bruker ALPHA spectrometer equipped with a diamond ATR unit. The following abbreviations were used for the intensities and characteristics of important IR absorption bands: vs, very strong; s, strong; m, medium; w, weak; br, broad.

Electrochemistry and UV–Vis–NIR Spectroelectrochemistry

UV–vis–NIR absorption spectra were recorded on a J&M TIDAS spectrophotometer. Cyclic voltammetry was n class="Gene">carried out in 0.1 M Bu4NPF6/THF solutions using a three-electrode configuration (Pt working, Pt-wire counter, and Ag quasi-reference electrodes) and was performed on a Metrohm Autolab potentiostat. THF was distilled from Na/K amalgam and degassed directly before use in the electrochemistry.

X-ray Crystallography

Single-crystal X-ray diffraction data were recorded on an Agilent Technologies SuperNova diffractometer with Cu Kα radiation (λ = 1.54184 Å). Crystals were selected under n class="Chemical">mineral oil, mounted on MicroMount loops, and quench-cooled using an Oxford Cryo-system open flow N2 cooling device. Either semiempirical multiscan absorption corrections[45] or analytical corrections[46] were applied to the data. Using Olex2,[47] the structures were solved with the SHELXT[48] structure solution program using intrinsic phasing and refined with the SHELXL[49] refinement package using least-squares refinements on F2.[50] The hydrogen atoms were located in idealized positions and refined isotropically with a riding model. Crystallographic data for the structures in this paper have been deposited with the Cambridge Crystallographic Data Centre, CCDC, 12 Union Road, Cambridge CB21EZ, UK. Copies of the data can be obtained free of charge on quoting the depository numbers: 2056040 (for 1), 2056041 (for 2), 2056042 (for 3), 2056043 (for 4), 2056044 (for 5), 2056046 (for 6), and 2056045 (for 7).

Starting Materials

The chelating bidentate isonitrile ligands bis(2-isocyanophenyl) phenylphosphonate (BINC)[6] and 2,2″-diisocyano-3,5,3″,5′′-tetramethyl-1,1′:3′,1″-terphenyl (CNAr3NC)[7] and [Cp*FeCl(tmeda)][33] were prepared according to reported procedures.

Synthesis of trans-[FeBr2(BINC)2] (1)

A solution of BINC (0.350 g, 0.970 mmol) in n class="Chemical">THF (10 mL) was added to a solution of FeBr2 (0.100 g, 0.460 mmol) in THF (60 mL) at ambient temperature. The brownish orange reaction mixture turned into a grayish suspension after 30 min. After the mixture was stirred overnight, product 1 could be isolated as a blue solid after decanting off the supernatant solution, washing with THF (3 × 10 mL), and drying in vacuo. Recrystallization by slow diffusion of n-hexane into a DCM solution resulted in blue crystals of 1. Yield: 154 mg, 33% (the calculated yield assumes the presence of 8% FeBr2 in the sample, vide infra). Anal. Calcd for C40H26Br2FeN4O6P2 (MW = 936.27 g/mol): C, 51.31; H 2.80; N, 5.98. Found: C, 50.27; H, 2.87; N, 5.77. Elemental analyses consistently gave low carbon and nitrogen, which indicated the presence of a persistent impurity. The impurity could not be removed by extraction or crystallization. We presume the impurity to be unreacted FeBr2. A calculated C, H, N analysis for 1·0.08FeBr2 (C, 50.39; H, 2.75; N, 5.88) fits well to the values found (C, 50.27; H, 2.87; N, 5.77). 1H NMR (400.13 MHz, 300 K, CD2Cl2): δ (ppm) 8.31–8.37 (m, 4H, H2), 7.71 (d, 3JHH = 8.5 Hz, 4H, H4), 7.65 (d, 3JHH = 7.9 Hz, 4H, H7), 7.6 (dt, 3JHH = 1.4 Hz, 3JHH = 7.5 Hz, 2H, H1), 7.46–7.50 (m, 2H, H3), 7.40 (dt, 3JHH = 1.6 Hz, 3JHH = 7.7 Hz, 4H, H5), 7.28 (t, 3JHH = 7.7 Hz, 4H, H6). 13C{1H}-NMR (100.61 MHz, 300 K, CD2Cl2) δ (ppm) 147.4 (d, J = 7.0 Hz, C9), 134.6 (d, J = 2.6 Hz, C1), 133.9 (d, J = 11.5 Hz, C2), 130.8 (s, C5), 129.4 (d, J = 16.4 Hz, C3), 127.6 (s, C7), 126.1 (s, C6), 123.8 (d, J = 190 Hz, C10), 121.9 (d, J = 2.7 Hz, C4), 121.2 (d, J = 5.1 Hz, C8), (C11 ≡ N) signals were not detected. 31P{1H}-NMR (161.98 MHz, 300 K, CD2Cl2): δ (ppm) 15.5 (s, 2P). IR: ν (cm–1) 2122 (ν[C≡N], vs), 1585 (w), 1486 (s), 1486 (m), 1439 (m), 1288 (m), 1239 (m), 1130 (s), 1100 (s), 1031 (m), 916 (br s), 799 (s), 755 (s), 713 (m), 596 (s), 563 (s), 531 (vs).

Synthesis of [Fe3(BINC)6] (2)

KC8 (n class="Chemical">coarse, 144 mg, 1.068 mmol) was added in portions to a suspension of 1 (500 mg, 0.534 mmol) in THF (30 mL) at −80 °C. After the mixture was stirred overnight and warmed to room temperature, a brownish yellow solution was formed. The solution was filtered, concentrated in vacuo (ca. 15 mL), and layered with n-hexane (20 mL). Product 2 could be isolated as brown crystals after decanting off the supernatant solution and drying under vacuum. Yield: 107 mg, 26%. Anal. Calcd for C120H78Fe3O18N12P6 (MW = 2329.39 g/mol): C, 61.88; H, 3.38; N, 7.22. Found: C, 61.47; H, 3.42; N, 6.95. 1H NMR (400,13 MHz, 300 K, THF-d8): δ (ppm) 8.50 (dd, 4JHH = 1.1 Hz, 3JHH = 8.1 Hz, 1H, H7), 8.29 (m, 2H, H2), 7.56 (d, 3JHH = 8.1 Hz, 1H, H4), 7.14–7.16 (m, 1H, H5), 7.13 (d, 3JHH = 8.0 Hz, 1H, H11), 6.94 (t, 3JHH = 8.1 Hz, 1H, H6), 6.83 (t, 3JHH = 7.4 Hz, 1H, H1), 6.68–6.75 (m, 2H, H3), 6.68–6.75 (m, 1H, H10), 6.53–6.57 (dt, 3JHH = 1.0 Hz, 3JHH = 7.8 Hz, 1H, H9), 5.48 (d, 3JHH = 7.8 Hz, 1H, H8). 13C{1H} NMR (100.61 MHz, 300 K, THF-d8): δ (ppm) 218.7 (s, C18), 188.1 (s, C17), 146.4 (d, J = 5.0 Hz, C16), 144.9 (d, J = 10.1 Hz, C13), 134.0 (d, J = 10.7 Hz, C2), 133.9 (d, J = 2.8 Hz, C1), 130.7 (d, J = 4.2 Hz, C14), 128.9 (d, J = 15.7 Hz, C3), 127.4 (s, C7), 126.9 (d, C5), 126.7 (s, C6), 126.6 (s, C10), 126.5 (d, J = 188.9 Hz, C12), 125.2 (s, C9), 124.9 (s, C8), 123.4 (d, J = 2.1 Hz, C4), 123.3 (d, J = 7.2 Hz, C15), 120.2 (s, C11). 31P{1H} NMR (161.98 MHz, 300, THF-d8): δ (ppm) 13.2 (s). IR: ν (cm–1) 2035 (ν[C≡N], br m), 1643 (m), 1581 (s), 1485 (s), 1451 (m), 1440 (m), 1282 (m), 1265 (s), 1247 (s), 1200 (w), 1130 (s), 1101 (s), 927 (vs), 809 (s), 753 (vs). 516 (s).

Synthesis of [Cp*FeCl(BINC)] (3)

A solution of BINC (420 mg, 1.17 mmol) in n class="Chemical">THF (5 mL) was added to a yellow solution of [Cp*FeCl(tmeda)][33] (400 mg, 1.17 mmol) in THF (15 mL). An immediate color change to dark red occurred. After the reaction mixture was stirred overnight, a red-brown suspension was formed. After the solvent was removed under reduced pressure, the brown solid was dried in vacuo. Recrystallization by slow diffusion of n-hexane into a DCM solution resulted in red-black crystals of 3. Yield: 560 mg, 82%. Anal. Calcd for C30H28ClFeN2O3P (MW = 586.83 g/mol): C, 61.40; H, 4.81; N, 4.77. Found: C, 60.78; H, 4.81; N, 4.70. The elemental analysis consistently indicates the presence of persistent impurities in samples of 3 prepared in the above manner. The unknown impurities could not be removed by washing or recrystallization of compound 3. 1H NMR (400.13 MHz, 300 K, CDCl3): δ (ppm) 8.17–8.11 (m, 2H, H2), 8.12 (d, 3JHH = 7.4 Hz, 1H, H3 or H3′), 7.56 (d, 3JHH = 8.1 Hz, 2H, H6), 7.48–7.42 (m, 3H, H1/H3), 7.27 (d, 3JHH = 7.6 Hz, 2H, H9), 7.15 (t, 3JHH = 7.6 Hz, 2H, H7), 7.08 (t, 3JHH = 7.6 Hz, 2H, H8), 1.75 (s, 15H, H-Cp*). 13C{1H} NMR (100.61 MHz, 300 K, CDCl3): δ (ppm) 188.7 (s, C11), 146.1 (d, J = 6.6 Hz, C5), 133.9 (d, J = 3.2 Hz, C1), 133.5 (d, J = 11.5 Hz, C2), 128.9 (d, J = 16.5 Hz, C3), 127.7 (d, J = 1.1 Hz, C7), 125.6 (s, C9), 125.4 (d, J = 1.0 Hz, C8), 123.4 (d, J = 189.9 Hz, C4), 123.2 (d, J = 6.2 Hz, C10), 121.4 (d, J = 2.8 Hz, C6), 93.1 (s, C12), 9.9 (s, C13). 31P{1H} NMR (161.98 MHz, 300 K, CDCl3): δ (ppm) 15.2 (s, 1P). IR: ν (cm–1) 2908 (w), 2084 (ν[C≡N], s), 2023 (ν[C≡N], s), 2011 (ν[C≡N], s), 1489 (s), 1439 (m), 1265 (m), 1244 (m), 1102 (s), 944 (vs), 923 (vs), 763 (vs), 573 (s).

Synthesis of [Cp*Fe(BINC)]2 (4)

KC8 (n class="Chemical">coarse, 138 mg, 1.023 mmol) was added to a red suspension of 3 (600 mg, 1.023 mmol) in THF (30 mL) at −80 °C. The green reaction solution obtained was stirred and warmed to room temperature overnight. After filtration and concentration under vacuum the green solution was layered with n-hexane. After the supernatant solution was decanted off and dried under vacuum, 4 was isolated as green crystals. Yield: 100 mg, 18%. Anal. Calcd for C60H56Fe2N4O6P2 (MW = 1102.77 g/mol): C, 65.35; H, 5.12; N, 5.08. Found: C, 65.06; H, 5.33; N, 4.84. 1H NMR (400.13 MHz, 300 K, THF-d8): δ (ppm) 8.14–8.09 (m, 4H, H2, cis), 8.10–8.05 (m, 1.3H, H2, trans), 7.77–7.72 (m, 1.3H, H2, trans), 7.66–7.63 (m, 2.3H, H1, cis (overlapping with trans)), 7.60–7.55 (m, 4.7H, H3, cis), 7.53–7.48 (m, 1.4H, H3, trans), 7.44 (d, 3J = 7.6 Hz, 0.8H, HAr, trans), 7.40–7.38 (m, 2.8H, H6, cis), 7.34–7.32 (m, 2.8H, H9, cis (overlapping with trans)), 7.29–7.22 (m, 2.6H, HAr, trans), 7.11–7.08 (m, 1H, HAr, trans), 7.05–7.02 (t, 3J = 7.6 Hz, 2.3H, H8, cis), 7.01–6.95 (m, 2.0H, trans), 6.88 (t, 3J = 7.6 Hz, 1H, HAr, trans), 6.70 (t, 3J = 7.6 Hz, 2.0H, H14, cis), 6.64 (t, 3J = 7.6 Hz, 2.8H, H7, cis), 6.54 (t, 3J = 7.6 Hz, 1H, HAr, trans), 6.48–6.44 (m, 1.3H, HAr, trans), 6.45–6.37 (m, 4H, H13 and H15, cis (overlapping with trans)), 6.32 (t, 3J = 7.6 Hz, 0.8H, HAr, trans), 6.27 (d, 3J = 7.6 Hz, 0.6H, H16, trans), 6.18 (d, 3J = 7.6 Hz, 2H, H16, cis), 6.14 (d, 3J = 7.6 Hz, 0.6H, H16, trans), 1.87 (s, 8.4H, H20, trans-Cp*), 1.74 (s, 30H, H20, cis-Cp*), 1.63 (s, 8.2H, H20, trans-Cp*). 13C{1H} NMR (100.61 MHz, 300 K, THF-d8): δ (ppm) 265.1 (s, C11, cis), 262.6 (s, C11, trans), 259.9 (s, C11, trans), 189.9 (s, C18, trans), 183.7 (s, C18, cis), 182.7 (s, C18, trans), 143.9 (d, J = 10.7 Hz, C12, cis), 144.0 (d, J = 10.4 Hz, C12, trans), 146.0 (m, C12, trans), 138.9 (d, J = 5.0 Hz, C5, cis), 138.6 (d, J = 5.0 Hz, C5, trans), 138.3 (d, J = 5.0 Hz, C5, trans), 137.4 (d, J = 6.3 Hz, C10, cis), 137.0 (d, J = 4.5 Hz, C10, trans), 137.8 (d, J = 6.0 Hz, C10, trans), 133.0 (d, J = 10.3 Hz, C2, trans), 132.9 (d, J = 11.3 Hz, C2, cis), 132.8 (d, J = 10.5 Hz, C2, trans), 132.6 (m, C1, cis), 128.2 (d, J = 15.8 Hz, C3, cis), 127.9 (d, J = 15.8 Hz, C3, trans), 127.7 (d, J = 15.5 Hz, C3, trans), 127.6 (s, CAr), 126.7 (d, J = 1.7 Hz, C16), 125.7 (s, CAr), 125.6 (dd, J = 1.8 Hz, J = 6.3 Hz, CAr), 125.1 (d, J = 1.7 Hz, C14), 124.8 (s, CAr), 124.6 (s, CAr, trans), 124.5 (s, C8, cis), 124.0 (d, J = 3.4 Hz, C17, cis), 123.6 (d, J = 190 Hz, C4, cis), 123.3 (d, J = 3.4 Hz, C13 and C15, cis), 123.8 (d, J = 3.4 Hz, CAr), 122.8 (s, C9, trans), 122.7 (s, C9, cis), 122.5 (s, C9, trans), 119.9 (d, J = 2.8 Hz, CAr), 119.7 (s, C6, cis), 119.6 (d, J = 2.8 Hz, C7, cis), 119.4 (s, CAr), 118.9 (d, J = 1.4 Hz, CAr), 118.7 (d, J = 2.5 Hz, CAr), 96.7 (s, C19, trans), 96.3 (s, C19, cis), 95.7 (s, C19, trans), 10.8 (s, C20, trans), 10.0 (s, C20, cis), 9.3 (s, C20, trans). 31P{1H} NMR (161.98 MHz, 300 K, THF-d8): δ (ppm) 14.5 (s, 2P, cis), 14.3 (s, 0.6P, trans), 12.1 (s, 0.6P, trans). IR: ν (cm–1) 3057 (w), 2899 (w), 2853 (w), 2053 (ν[C≡N], br s), 2028 (ν[C≡N], br s), 1656 (s), 1580 (s), 1478 (s), 1440 (m), 1256 (s), 1129 (s), 1098 (s), 924 (vs), 750 (vs), 645 (s), 580 (s), 533 (s), 501 (s).

Synthesis of [FeBr2(CNAr3NC)2] (5)

A solution of CNAr3NC (98.3 mg, 0.292 mmol) in n class="Chemical">THF (15 mL) was added to a solution of FeBr2 (30 mg, 0.139 mmol) in THF (15 mL). After it was stirred overnight, the orange suspension was filtered and the remaining orange residue was washed with THF (2 × 5 mL) and dried in vacuo. Recrystallization by slow diffusion of n-hexane into a DCM solution resulted in orange crystals of 5. Yield: 73.6 mg, 55% (the calculated yield assumes the presence of 8% FeBr2 in the sample, vide infra). Anal. Calcd for C48H40Br2FeN4 (MW = 888.53 g/mol): C, 64.89; H, 4.54; N, 6.3. Found: C, 63.58; H, 4.80; N, 5.93. Elemental analyses consistently gave low carbon and nitrogen values, which indicated the presence of a persistent impurity. The impurity could not be removed by extraction or crystallization. We presume the impurity to be unreacted FeBr2. A calculated C, H, N analysis for 5·0.08FeBr2 (C, 63.65; H, 4.48; N, 6.19) fits well to the values found (C, 63.58; H, 4.80; N, 5.93). 1H NMR (400,13 MHz, 213 K, CD2Cl2): δ (ppm) 8.08 (ps t, 1H, HAr), 7.77 (ps t, 1H, HAr), 7.66 (t, 3JHH = 7.7 Hz, 1H, HAr), 7.63 (t, 3JHH = 7.7 Hz, 1H, HAr), 7.50 (d, 3JHH = 7.8 Hz, 1H, HAr), 7.46(d, 3JHH = 7.8 Hz, 1H, HAr), 7.42 (d, 3JHH = 7.8 Hz, 1H, HAr), 7.35 (d, 3JHH = 7.8 Hz, 1H, HAr), 7.18 (s, 1H, HAr), 7.14 (s, 1H, HAr), 7.12 (s, 1H, HAr), 7.09 (br. s, 2H, HAr), 7.05 (s, 1H, HAr), 6.94 (s, 1H, HAr), 6.91 (s, 1H, HAr), 2.64 (s, 3H, HMethyl), 2.55 (s, 3H, HMethyl), 2.53 (s, 3H, HMethyl), 2.37 (s, 6H, HMethyl), 2.33 (s, 3H, HMethyl), 2.26 (s, 3H, HMethyl), 1.53 (s, 3H, HMethyl). 13C{1H} NMR (100.61 MHz, 213 K, CD2Cl2): δ (ppm) 167.3 (s, CCN), 166.8 (s, CCN), 164.6 (s, CCN), 164.4 (s, CCN), 139.4 (s, CAr), 138.9 (s, CAr), 138.6 (s, CAr), 138.3 (s, CAr), 137.8 (s, CAr), 137.7 (s, CAr), 137.1 (s, CAr), 137.1 (s, CAr), 136.9 (s, CAr), 136.8 (s, CAr), 136.5 (s, CAr), 136.1 (s, CAr), 135.4 (s, CAr), 135.2 (s, CAr), 130.1 (s, CAr), 130.0 (s, CAr), 129.9 (s, CAr), 129.9 (s, CAr), 129.6 (s, CAr), 129.1 (s, CAr), 129.0 (s, CAr), 128.9 (s, CAr), 128.9 (s, CAr), 128.8 (s, CAr), 128.6 (s, CAr), 128.5 (s, CAr), 128.5 (s, CAr), 123.1 (s, CAr), 122.8 (s, CAr), 122.2 (s, CAr), 122.2 (s, CAr), 21.1 (s, CMethyl), 21.0 (s, CMethyl), 20.9 (s, CMethyl), 18.7 (s, CMethyl), 18.7 (s, CMethyl), 18.6 (s, CMethyl), 18.0 (s, CMethyl). Characterization by NMR spectroscopy at 300 K showed broadened signals in the 1H NMR spectra. Variable-temperature NMR confirmed the assumption of a cis/trans isomer mixture. The NMR characterization of compound 5 at 213 K (−60 °C) identified a 1:1 isomeric mixture. IR: ν (cm–1) 2158 (w), 2144 (ν[C≡N], vs), 2126 (ν[C≡N], vs), 1594 (w), 1462 (m), 860 (m), 805 (s), 733 (m), 705 (s), 607 (m), 567 (m).

Synthesis of [Fe(CNAr3NC)2]2 (6)

KC8 (n class="Chemical">coarse, 30.4 mg, 0.225 mmol) was added in portions to a suspension of 5 (100.0 mg, 0.113 mmol) in THF (15 mL) at −80 °C. After 30 min a dark orange-red reaction solution was formed. The solution was stirred overnight and warmed to room temperature. The dark red reaction mixture was filtered and concentrated in vacuo (ca. 5 mL), and 6 was crystallized by slow diffusion of n-hexane into a THF solution. Compound 6 was isolated as red-brown crystals. Yield: 10 mg, 12%. Anal. Calcd for C96H80Fe2N8 (Mw = 1457.44 g/mol): C, 79.12; H, 5.53; N, 7.69. Found: C, 79.27; H, 5.89; N, 6.92. 1H NMR (400.13 MHz, 300 K, THF-d8): δ (ppm) 8.53 (s, 1H, HAr), 8.13 (s, 1H, HAr), 8.10 (s, 1H, HAr), 7.66 (s, 1H, HAr), 7.49 (s, 1H, HAr), 7.48 (t, 3J = 7.7 Hz 1H, HAr), 7.39 (t, 3J = 7.4 Hz 1H, HAr), 7.35 (m, 1H, HAr), 7.32 (m, 1H, HAr), 7.26 (t, 3J = 7.6 Hz 1H, HAr), 7.15 (d, 3J = 8.0 Hz, 1H, HAr), 7.10 (d, 3J = 8.0 Hz, 1H, HAr), 7.05 (m, 3H, HAr), 7.00 (m, 2H, HAr), 6.97 (m, 3H, HAr), 6.89 (m, 3H, HAr), 6.73 (m, 2H, HAr), 6.67 (m, 2H, HAr), 6.62 (m, 2H, HAr), 6.59 (m, 2H, HAr), 6.55 (m, 1H, HAr), 6.44 (d, 3J = 7.6 Hz, 1H, HAr), 6.40 (dd, 3J = 7.8 Hz, 3J = 1.5 Hz, 1H, HAr), 6.22 (s, 1H, HAr), 6.18 (d, 3J = 7.3 Hz, 1H, HAr), 6.05 (s, 1H, HAr), 5.40 (s, 1H, HAr), 5.36 (s, 1H, HAr), 2.62 (s, 3H, HMethyl), 2.54 (s, 3H, HMethyl), 2.46 (s, 6H, HMethyl), 2.34 (s, 3H, HMethyl), 2.28 (m, 6H, HMethyl), 2.18 (m, 9H, HMethyl), 2.10 (s, 3H, HMethyl), 1.83 (s, 3H, HMethyl), 1.75 (s, 3H, HMethyl), 1.70 (s, 3H, HMethyl), 1.65 (s, 3H, HMethyl), 1.23 (s, 3H, HMethyl), 1.13 (s, 3H, HMethyl), 0.53 (s, 3H, HMethyl). 13C{1H} NMR (150.88 MHz, 300 K, THF-d8): δ (ppm) 244.2 (s, CCN), 235.5(s, CCN), 208.7 (s, CCN), 191.1 (s, CCN), 142.2 (s, CAr), 140.9 (s, CAr), 140.5 (s, CAr), 139.5 (s, CAr), 138.3 (s, CAr), 138.1 (s, CAr), 137.9 (s, CAr), 137.4 (s, CAr), 136.4 (s, CAr), 136.2 (s, CAr), 135.8 (s, CAr), 135.6 (s, CAr), 135.5 (s, CAr), 134.9 (s, CAr), 134.7 (s, CAr), 134.1 (s, CAr), 134.0 (s, CAr), 132.9 (s, CAr), 132.8 (s, CAr), 129.6 (s, CAr), 129.5 (s, CAr), 129.4 (s, CAr), 129.2 (s, CAr), 128.7 (s, CAr), 128.4 (s, CAr), 127.9 (s, CAr), 127.8 (s, CAr), 126.1 (s, CAr), 125.1 (s, CAr), 29.6 (s, CMethyl), 27.0 (s, CMethyl), 25.4 (s, CMethyl), 22.0 (s, CMethyl), 20.8 (s, CMethyl), 20.5 (s, CMethyl), 20.2 (s, CMethyl), 20.1 (s, CMethyl), 20.0 (s, CMethyl), 19.9 (s, CMethyl), 19.8 (s, CMethyl), 19.7 (s, CMethyl), 18.8 (s, CMethyl), 18.5 (s, CMethyl), 18.4 (s, CMethyl), 17.8 (s, CMethyl), 17.5 (s, CMethyl), 17.1 (s, CMethyl). On the basis of the 1H,1H-NOESY of 6 showing three different sets of methyl groups (eight in each set) it can be concluded that compound 6 can be isolated as a mixture of three isomers. IR: ν (cm–1) 2914 (w), 2852 (w), 2070 (ν[C≡N], s), 2022 (ν[C≡N], s), 1676 (m), 1593 (m), 1460 (m), 1370 (s), 855 (vs), 733 (vs).

Synthesis of [K(Et2O)]2[Fe(CNAr3NC)2]2 (7)

KC8 (finely ground, 104.9 mg, 0.776 mmol) was added to a suspension of 5 (215.5 mg, 0.243 mmol) in n class="Chemical">THF (25 mL) at −80 °C. After 30 min a dark orange-brown reaction solution was formed. The red solution was stirred overnight and warmed to room temperature. The solvent was removed under reduced pressure, and the brown-red residue was extracted with Et2O (50 mL). After filtration the solution was concentrated in vacuo (ca. 20 mL) and stored at −30 °C. Compound 7 was isolated as black crystals. Yield: 98.8 mg, 46%. Anal. Calcd for C104H100Fe2N8O2K2 (MW = 1683.88 g/mol): C, 74.18; H, 5.99; N, 6.65. Found: C, 74.20; H, 6.17; N, 6.78. 1H NMR (400.13 MHz, 300 K, THF-d8): δ (ppm) 8.96 (s, 1H, H1 or H2), 8.31 (s, 1H, H1 or H2), 7.40 (t, 3J = 7.5 Hz, 1H, H3 or H4), 7.32 (t, 3J = 7.6 Hz, 1H, H3 or H4), 7.26 (d, 3J = 7.6 Hz, 1H, H5 or H7), 7.17 (d, 3J = 7.5 Hz, 2H, H6), 7.13 (d, 3J = 7.5 Hz, 1H, H5 or H7), 6.86 (s, 2H, H8), 6.81 (s, 1H, H8), 6.76 (s, 1H, H8), 6.65 (s, 1H, H8), 6.55 (s, 2H, H8), 6.43 (s, 1H, H8), 2.27 (s, 3H, H9), 2.24 (s, 3H, H9), 2.22 (s, 3H, H9), 2.19 (s, 6H, H9), 1.72 (s, 9H, H9, overlapping with THF-d8). 13C{1H}-NMR (100.61 MHz, 300 K, THF-d8): δ (ppm) 297.6 (m, CCN), 209.5 (m, CCN), 203.2 (m, CCN), 147.0 (m, CAr), 142.5 (m, CAr), 140.7 (m, CAr), 138.8 (m, CAr), 138.6 (d, J = 3.5 Hz, CAr), 134.5 (d, J = 12.3 Hz, C1 or C2), 133.7 (s, CAr), 133.4 (s, CAr), 133.0 (s, CAr), 131.5 (m, C8), 131.0 (s, CAr), 129.9 (s, CAr), 129.4 (d, J = 15.9 Hz, C8), 129.5 (m, CAr), 128.9 (m, C8), 128.8 (m, C8), 128.6 (s, C1 or C2), 128.1 (s, CAr), 127.8 (d, J = 7.0 Hz, C8), 127.5 (d, J = 6.0 Hz, C6), 127.2 (s, C3 or C4), 126.8 (s, C5 or C7), 126.5 (s, C5 or C7), 125.6 (s, C6), 20.2 (m, C9), 20.0 (m, C9), 19.7 (m, C9), 18.8 (m, C9). IR: ν (cm–1) 2968 (w), 2912 (w), 2853 (w), 1982 (ν[C≡N], w), 1961 (ν[C≡N], w), 1765 (br m), 1602 (w), 1514 (m), 1456 (m), 1381 (m), 1210 (m), 855 (vs), 744 (vs), 534 (vs).