Isolation and electronic structures of derivatized manganocene, ferrocene and cobaltocene anions.

The discovery of ferrocene nearly 70 years ago marked the genesis of metallocene chemistry. Although the ferrocenium cation was discovered soon afterwards, a derivatized ferrocenium dication was only isolated in 2016 and the monoanion of ferrocene has only been observed in low-temperature electrochemical studies. Here we report the isolation of a derivatized ferrocene anion in the solid state as part of an isostructural family of 3d metallocenates, which consist of anionic complexes of a metal centre (manganese, iron or cobalt) sandwiched between two bulky Cpttt ligands (where Cpttt is {1,2,4-C5H2 tBu3}). These thermally and air-sensitive complexes decompose rapidly above -30 °C; however, we were able to characterize all metallocenates by a wide range of physical techniques and ab initio calculations. These data have allowed us to map the electronic structures of this metallocenate family, including an unexpected high-spin S = 3/2 ground state for the 19e- derivatized ferrocene anion.

The iconic organon class="Chemical">metallic complex ferrocene, [Cp2Fe] (FcH, Cp = cyclopentadienyl, η[5]-C5H5), wasfirst reported in 1951[1,2], andthe ferrocenium cation [Cp2Fe]+ (FcH+) was isolated soon after.[3]These discoveries were the harbingers of metallocene chemistry, which rapidly spread to cover most of the Periodic Table[4,5]. In the interim ferrocene has become a versatile workhorse in nanotechnology[6], electrochemistry, catalysis, medicine, and functional materials[7]; industrial applications include fuel additives and the synthesis of agrochemicals and pharmaceuticals[8]. A defining feature of ferrocene is its facile oxidation to ferrocenium, with the fully reversible FcH+/0 redox couple a standard reference in non-aqueous electrochemical processes[9].

Whilst metallocenes are strictly defined as the homoleptic [Cp2M] family, Cp derivatization to CpR ligands (C5RnH5-n -) provides tuneable physin class="Chemical">cochemical properties[4,5]; for example, decamethylferrocene, [Cp*2Fe] (Cp* = C5Me5), can be doubly oxidized to yield dicationic [Cp*2Fe]2+ salts[10]. Isolated metallocene anions are conspicuous by their absence in the literature, with “[Cp2M]-” (M = V[11], Cr[11], Fe[12,13], Co[14,15], Ni[11]) and “[Cp2M]2-” (M = Co, Ni)[15] anions only identified as transient species in seminal low temperature solution-phase electrochemical studies. Notable synthetic results include the reduction of [Cp*2Mn] to an orange powder formulated as “Na[Cp*2Mn]”[16,17], the preparation of white powders of “A[Cp2Re]” (A = Li[18], K[19]) from [Cp2ReH] and nBuLi or PhCH2K, and the structural characterization of a derivatized bis(indenyl) Co anion, [Na(THF)6][Co{C9H5-1,3-(SiMe3)2}2][20]. Recently, potassium salts of [Cp*2Mn]- were structurally authenticated[21]. It was previously shownthat replacement of a CpR ligand with an arene (C6R6) can provide neutral 19e- mixed sandwich Fe complexes; some of the [(CpR)Fe(C6Me6)] family are stable at room temperature, allowing characterization by single crystal XRD[22,23]. Finally, the related 19e- Fe bis-stannole complex [Li(THF)4][Fe{SnC4(SiMe3)2-1,3-Me2-2,4}2] was recently isolated and structurally authenticated[24].

Here we report the isolation of an isostructural series of derivatized metallocene anions for n class="CellLine">Mn, Fe and Co; despite their facile thermal decomposition above -30 °C these complexes were characterised by a wide range of physical techniques. Together with ab initio calculations these studies provide new insights into the electronic structures of metallocenes, including a19e-Fe metallocene anion with a high-spinS = 3/2 ground state rather than the low-spin S = 1/2 ground state observed in formally isoelectronic cobaltocenes[4,5].

Results and Discussion

Electrochemistry

We targeted [(Cpttt)2M]- (Cpttt = {1,2,4-C5H2 Bu3}) anions as the six bulky aliphatic n class="Chemical">tBu substituents impart solubility and kinetic stability.[(Cpttt)2M] precursors are known for M = Mn (1),[25,26]Fe (2)[27]and Co (3);[28,29]here we prepared 3 from CoCl2 and two equivalents of KCpttt30. We performed cyclic voltammetryon DME solutions of1-3 at -50 °C with [NnBu4][BF4] as the supporting electrolyte to determine reduction potentials and to assess metallocenate stabilities (Fig. 1). The quasi-reversible reduction processes (ΔEox/red (mV) = 760, 1; 390, 2; 270, 3) are similar for 2 and 3, whilst 1 shows evidence of reactivity on the experimental timescale at negative potentials (E½ (V)vsFcH+/0= -3.39, 2; -2.49, 3; for 1 Ep1 = -3.26 V, Ep2 = -2.50 V at peak current density). These reduction waves are all irreversible above -30 °C, and are formally assigned as M2+/M1+ processes from their similarity with the respective voltammograms of [Cp2M] (M = Fe, -3.45 to -3.57 V; Co, -2.40 to -2.55 V; vsFcH+/0)[12-15] and [Cp*2Mn] (-2.68 V; vsFcH+/0)[16]; note that for 1 we cannot definitively assign if Ep1 and Ep2 belong to the same redox couple.

Figure 1

Electrochemical studies for 1-3.

Cyclic voltammograms (current in arbitrary units, a.u., vs Potential, V vs FcH+/0) of 1 (Mn, purple), 2 (Fe, orange), 3 (Co, blue) at -50 °C, 1 mM in DME with 0.5 M [NnBu4][BF4] (1 and 3, 200 mV/s; 2, 100 mV/s), with redox processes labelled with formal metal oxidation states and arrows to indicate scan direction. As the formal Mn2+/+ redox couple of 1 is not reversible, the peak potentials are denoted (Ep1/Ep2) at the point of peak current density. The table compiles The table compiles half-wave (E1/2) or peak potential values (V vs FcH+/0) for the electrochemical redox processes [(Cpttt)2M]0/-, [(Cpttt)2M]+/0, and [(Cpttt)2M]2+/+ for complexes 1-3 when observed.

Synthesis

Given the large negative reduction potentials and temperature sensitivity seen in electrochemical studies, we reasoned that low temperature alkali metal reductions would be required to isolate 3d n class="Chemical">metallocenates; such conditions previously opened up elusive formal +2 oxidation states for f-element CpR complexes[31]. Thus potassium graphite (KC8) reductions of 1-3 in THF at -40 °C, in the presence of 2.2.2-cryptand to sequester potassium cations, gave the substituted metallocenates, [K(2.2.2-cryptand)][(Cpttt)2M] (M = Mn, 4; Fe, 5; Co, 6) (Fig. 2). Complex 4 reproducibly co-crystallized with one equivalent of [K(2.2.2-cryptand)][Cpttt], thus is formally 4·K(2.2.2-cryptand)Cp; an analogous contaminant [K(2.2.2-crypt)]2[(Cpttt)2Co][Cpttt] (7) was sometimes observed in batches of 6. The formulations of 4-6 were consistent with values obtained from elemental microanalysis, indicating that the single crystal XRD data is representative of the bulk samples. Intensely coloured THF or DME solutions of 4 (orange), 5 (brown) and 6 (brown) at room temperature change colour within 10 minutes and crystals of 1-3 were isolated from the resultant mixtures, thus all analytical data for 4-6 were collected below -30 °C. Surprisingly the 18e- complex 4 is the most thermally sensitive of the series; this is in stark contrast to the derivatized manganocene anion [Cp*2Mn]-, which has recently been synthesized by refluxing [Cp*2Mn] with molten K in THF[21]. This temperature sensitivity precluded the collection of reliable magnetic and NMR spectroscopic data for 4-6 despite multiple attempts, but otherwise we were able to fully characterise this family.

Figure 2

Synthesis of 4-6 and molecular structure of 5.

a, Synthesis of complexes4-6. b, Molecular structure of 5 with selective atom labelling (Fe, orange; K, violet; O, red; N, blue; C, grey). Displacement ellipsoids set at 50 % probability level and hydrogen atoms are omitted for clarity.

Structural characterisation

The solid-state structures of 1-7 and [K(2.2.2-crypt)][Cpttt] (8) were determined by single n class="Chemical">crystal X-ray diffraction at 150 K. As the [(Cpttt)2M]fragments are structurally analogous only the structure of 5 is depicted in Fig. 2 and selected bond lengths and angles are compiled in Table 1; the structures of 1-3 have been reported previously[25-27,29]. In common with 1-3 [25-27,29], near-eclipsed conformations of the C5 rings are observed for 4-7, with the quaternary carbons of tBu groups displaced from the Cpttt C5 planes away from the metal due to steric crowding. This also causes all the Cpttt centroid⋯M⋯Cpttt centroid angles to deviate from linearity, with 5 exhibiting the most bent geometry at 169.38(11)°; in contrast to 4-6, [K(18-crown-6)(THF)2][Cp*2Mn] exhibits a highly axial geometry (Cp*centroid⋯Mn⋯Cp*centroid: 179.5(2)°)[21]. The M–CCp and M⋯Cpttt centroid distances for 1-7 approximately correlate with valence electron counts, with the shortest values seen for 18e- 2 and 4, and longer distances for 19e- 3 and 5, and 20e- 6 and 7, presumably due to the partial occupancy of antibonding orbitals. As expected, these bond distances increase upon reduction of 2 to 5 and from 3 to 6 or 7. The seemingly anomalous long distances for 17e- 1 are due to its high-spin configuration, which results in significant electron density in antibonding orbitals[26]. The mean Mn⋯Cpttt centroid distances for 4 (1.750(3) Å) are longer than the corresponding distances in [K(18-crown-6)(THF)2][Cp*2Mn] (mean M⋯Cp*centroid: 1.673(7) Å)[21], due to the greater steric bulk of Cptttvs Cp*. 19e- 5 exhibits longer M⋯Cpttt centroid distances than seen for 19e- 3, and 20e- 6 and 7, motivating us to analyse their electronic structures.

Table 1

Selected distances (Å) and angles (°) for 1-7 (data for 1-3 agree with references 25, 27 and 29).

Complex	Range M–CCp	Mean M⋯Cpttt centroid	Cpttt centroid1⋯M⋯Cpttt centroid2	Formal e- count
1	2.347(2) – 2.516(2)	2.105(2)	169.63(3)	17
2	2.034(3) – 2.156(3)	1.715(2)	174.91(8)	18
3	2.121(2) – 2.227(2)	1.802(2)	174.77(4)	19
4	2.099(4) – 2.159(4)	1.750(3)	174.68(9)	18
5	2.262(5) – 2.511(6)	2.064(4)	169.38(11)	19
6	2.220(3) – 2.451(3)	1.958(2)	175.96(5)	20
7	2.225(2) – 2.415(2)	1.930(2)	176.20(5)	20

Ab initio electronic structure

Given that [Cp2Mn] is high-n class="Gene">spin[32,33], but becomes low-spin below 100 K when doped into a diamagnetic matrix of [Cp2Fe][34], and that [Cp*2Mn] is low-spin[16], it is evident that electron-electron repulsion and crystal field effects in 3d metallocenes have similar energy scales; indeed, at room temperature 1,1′-dimethylmanganocene shows evidence of both a sextet and doublet ground state[35]. A multiconfigurational wavefunction-based methodaccounting for electron correlation is therefore the only reliable way of treating the electronic structure, sowe performed state-average complete active space self-consistent field (SA-CASSCF) calculations with spin-orbit coupling (SOC) included a posteriori, as embodied by the OpenMOLCAS code[36]. For 2-7 the active space consisted of 12 orbitals (3dxz and 3dyz (π, e1g), 3dz2 (σ, a1g), 3dxy and 3dx2-y2 (δ, e2g), and 3dxz and 3dyz (π*, e1g) and ligand-hybridised 4d/5d orbitals), while for 1 this active space was not stable and our calculations only included five orbitals (3dz2 (σ, a1g), 3dxy and 3dx2-y2 (δ, e2g), and 3dxz and 3dyz (π*, e1g)). Here we focus on the metallocenates 4-7; see Supporting Information for discussion of 1-3.

For 4, using an active space of 10 electrons in 12 orbitals (CAS(10,12)+SO, Supplementary Table 13), the ground state is low-spin S = 0 ([1]A), with a first excited S = 1 state lying at ca. 15,000 cm-1. Thus, these calculations suggest that 4 is low-n class="Gene">spin diamagnetic just like its isoelectronic partner 2. For 5, using CAS(11,12)+SO (Supplementary Table 15) the ground state was found to be high-spin S = 3/2 ([4]E), but due to the low-symmetryof the molecule the orbital degeneracy of 3dxy and 3dx2-y2 pair is partly lifted, thus the[4]E is split into twoS = 3/2 states areseparated byca. 1,100 cm-1 (subsequent excited states ca. 10,000 cm-1). The ground S = 3/2 state has very large zero-field splitting that can be parameterised by D = -36.4 cm-1 and |E| = 0.15 cm-1, meaning that the lowest lying Kramers doublet is m = ±3/2, with the m ± 1/2 doublet lying at 72.8 cm-1. The g-value for the ground state is also anisotropic with g x = g y = 2.02, g z = 2.72, leading to effective g-values for the ground Kramers doublet of g x = g y = 0.02, g z = 8.11, while those for the first excited doublet are g x = g y = 4.02(3), g z = 2.82; the magnetic z-axis is parallel to the Cpttt centroid∙∙∙Fe∙∙∙Cpttt centroid vector. Thus, 5 is rather different to its isoelectronic partner 3 which is S = 1/2 ([2]E). Finally, for the Co metallocenate there are two crystal structures so calculations were performed on both; the first values are for 6 and those in braces are for 7. Using a CAS(12,12)+SO calculation (Supplementary Tables 17 and 18) the ground state was found to be high-spin S = 1 ([3]A), with a set of four excited S = 1 states lying between 11,000 – 12,000 cm-1 {12,000 – 13,000 cm-1}, and has a sizeable zero-field splitting that can be parameterised by D = +25.6 cm-1 and |E| = 0.21 cm-1{D = +23.6 cm-1 and |E| = 0.41 cm-1}, meaning that the lowest lying state is m = 0 with the m ± 1 pseudo-doublet lying at 24 – 26 cm-1, with an intra-doublet separation of 0.4 – 0.8cm-1. The g-value for the ground S = 1 state is anisotropic with g x = g y = 2.17(1) and g z = 2.00 {g x = g y = 2.15(1) and g z = 2.00}, where the magnetic z-axis is parallel to the Cpttt centroid∙∙∙Co∙∙∙Cpttt centroidvector.

Mössbauer Spectroscopy

Complexes 2 and 5 werestudied by57n class="Chemical">Fe Mössbauer spectroscopy (Fig. 3, Supplementary Fig. 68 and Supplementary Table 19). The spectrum of 2 recorded at 80 K consists of a single quadrupole doublet that is best fit with an isomer shift, δ = 0.66(2) mm/sec and a quadrupole splitting, ΔE Q = 2.60(2) mm/sec (Fig. 3a). The spectrum of 5 displays two quadrupole doublets, unambiguously indicating two Fe species are present in this sample. The first species is described by parameters identical to those of 2, therefore we assign this doublet to the presence of 2, which forms upon thermal decomposition of 5 during sample preparation. The second species, which we attribute to 5, features an asymmetric quadrupole doublet and is fit with δ = 1.25(2) mm/sec and ΔE Q = 1.23(2) mm/sec (Fig.3b). The observation of an asymmetric quadrupole doublet is commonfor Kramers systems, like 5, in a slow to intermediate relaxation regime, i.e., the relaxation rate is around the same order of magnitude as the 57Fe Larmor precession (see Supporting Information for further discussion)[37,38].

Figure 3

Zero-field 57Fe Mössbauer spectra for 2 and 5.

57Fe Mössbauer spectra of powders recorded under zero applied magnetic field and 80 K (% Absorption vs Velocity, mm/s): a) Sample of [(Cpttt)2Fe] (2); experimental (black) and simulated (red); b) Sample of [K(2.2.2-cryptand)][(Cpttt)2Fe] (5); the blue trace corresponds to the quadrupole doublet assigned to 5 (~75%) whilst the green trace originates from the presence of 2 that forms upon the thermal decomposition of 5 (~25%). The red trace is the weighted sum of the two sub-spectra. The table compiles the experimentally determined 57Fe Mössbauer parameters for the sites (independent Fe environments) in the two samples 2 and 5, with N referring to the parameters of the Neutral molecule [(Cpttt)2Fe], and A to the Anion, [(Cpttt)2Fe]-. The following parameters are shown: δ, the isomer shift; ΔE Q, the quadrupole splitting; ГL and ГR, the line widths at half maximum showing the asymmetry of the doublet for 5. Here, the numbers in parentheses indicate the estimated uncertainty in the last digit.

The isomer shift quantifies electron density at the 57Fe nuclei, and hence can be used to identify oxidation state; unfortunately, the isomer shifts in n class="Chemical">ferrocene (δ≈ 0.45-0.6)[39,40] and associated cations (δ≈ 0.51 – 0.62 for 1+[41], δ≈ 0.59 mm/sec for 2+[10]) are similar. The isomer shift range of previously reported formally Fe1+ sandwich complexes (~0.52 – 0.73 at 77 K)[23,24,38,42] are smaller than that observed for 5, but these literature examples almost exclusively exhibit low spin ground states; herein, we propose that 5 has a formal 4s03d[7] high spin ground state with a reduced Fe spin population of +2.82 (see below).

To rationalize the unusually large isomer shift we have performed DFT calculations with hybrid (B3LYP) and GGA (BP86) functionals (Supplementary Table 20). The calculated isomer shifts and quadrupole splitting parameters of 2 (δ = 0.61 – 0.69 mm/sec, |ΔE Q calc| = 2.51 – 3.37 mm/sec) are in excellent agreement with the experimental values (δ = 0.66(2) mm/sec, |ΔE Q| = 2.60(2) mm/sec). In the case of 5, the calculated isomer shift for the high (δ = 1.09 – 1.27 mm/sec) and low (δ = 1.14 – 1.31 mm/sec) spin state both agree with the experimental value (δ = 1.25(2) mm/sec). Unfortunately, n class="Chemical">comparison of the calculated quadrupole splitting for the high (|ΔE Q calc| = 0.65 – 0.68 mm/sec) and low (|ΔE Q calc| = 2.01 – 2.36 mm/sec) spin states to the experimental one (ΔE Q= 1.23(2) mm/sec) is not useful for determination of the spin state.

EPR Spectroscopy

To directly probe the spin ground states of 1-7 we performed n class="Chemical">continuous wave EPR spectroscopy at X- (ca. 9.4 GHz) and Q-band (ca. 34 GHz) on polycrystalline samples. For brevity, we focushere on the data for 3 and 5, and summarize the results of the remaining compounds while providing a full analysis in the Supporting Information; we note that a continuous wave X-band EPR spectrum of a DCM frozen solution of 3 at 100 K has been reported previously[28]. As expected for the 18e- ferrocene analogue 2, there is no EPR spectrum at any temperature at X- or Q-band, in agreement with an S = 0 ground state from CASSCF calculations. Similarly, the 18e- 4 is also EPR silent at X- and Q-band aside from signals arising from the presence of 1 (Supplementary Fig. 74). The X-band EPR spectrum at 5 K for 3 (Co2+) shows a single feature around g = 1.89 (Supplementary Fig. 72), suggesting a low-spin S = 1/2 ground state, but a Q-band spectrum at 11 K reveals additional structure (Fig. 4a). Frozen solution experiments confirm an extrinsic peak in the powder spectrum at g = 1.83 (Supplementary Fig. 73), and simulations of the solid state data with Easyspin[43]giveg = 2.00, g = 1.93 and g = 1.72 with hyperfine interaction with the 59Co I = 7/2 nuclear spinA= 400, A = 0 and A = 150 MHz (Fig. 4a; we note that these hyperfine coupling constants are approximate due to the unresolved nature of the hyperfine structure).

Figure 4

Continuous wave Q-band EPR spectra of 3 and 5.

a, 3 at 11 K (33.950645 GHz, red line is a simulation with S = 1/2, g = 2.00, g = 1.93 and g = 1.72 with A= 400, A = 0 and A = 150 MHz andlw = 30 mT using Easyspin[41]). b, 5 at 5 K (34.080627 GHz, red line is a simulations with S = 3/2, D = -4.42 cm-1 with E = 0 cm-1 and g = 2.06 and g = 2.37, lw = 12.9 and lw = 3.7 GHz using PHI[42]). Stars denote extrinsic peaks. The resonances observedfor5 are at different magnetic fields to those seen for 3, and consistent with an assignment of 5 having a S = 3/2 spin state.

X-band EPR spectra of 5 between 5 and 20 K show a broad resonance between 0.1 and 0.3 T that increases in intensity with inn class="Chemical">creasing temperature(Supplementary Fig. 75). Only a weak spectrum could be obtained at Q-band(Fig. 4b), which shows a large positive feature at 0.5 T and a smaller negative feature at 1 T, suggestive of an easy-plane-like effective doublet state. Taken together with the temperature dependence of the X-band spectra, these results are consistent with an EPR-active excited state with easy-plane anisotropy. We hypothesise that this signal arises from anS = 3/2 ground state with negative axial zero field splitting (ZFS, D < 0) such that the ground m = ±3/2 Kramers doublet (which would appear as easy-axis) is EPR silent and the excited m = ±1/2 doublet (which behaves as easy-plane) is EPR active. Fitting the variable temperature X-band and Q-band spectra simultaneously[44] gives D = -4.42 with E = 0 and g = 2.06 and g = 2.37 (Fig. 4b and Supplementary Fig. 75), though we note that the magnitude of D is given solely by the temperature dependence of the X-band spectra, and is thus not spectroscopically determined and should be treated as an estimate.

Resonances in the Q-band EPR spectra of 5 are at different magnetic fields to those seen for 3 (Fig. 4), indicating difn class="Chemical">ferent effective g-values, which are far from g = 2 for 5 (effective g-values are g z = 2.37 and g x/y = 4.12). This provides strong foundation for the assignment of 5 as arising from a S = 3/2 spin state, in addition to the temperature dependence, as the large effective g-values are very unlikely to arise from a S = 1/2 system. Indeed, Rajasekharan et al. show that the g-values for variously substituted low-spin d[7] mixed sandwich [(η[5]-C5R5)Fe(η[6]-C6R6)] complexes are between 1.2 and 2.1[45], which are consistent with our EPR data for 3 (g = 2.00, g = 1.93 and g = 1.72) but clearly distinct from the data for 5 (effective g-values of g z = 2.37 and g x/y = 4.12, arising from S = 3/2, D = -4.42 cm-1 with E = 0 cm-1 and g = 2.06 and g = 2.37). CASSCF-SO calculations agree well with experimental data, predicting an axially anisotropic S = 1/2 ground state for 3 with g-values of g x ≈ g y = 2.1, g z = 1.61, and a ground S = 3/2 spin state with negative uniaxial magnetic anisotropy for 5, however the experimental D value for 5 is far smaller than that calculated (-4.42 cf. -36.4 cm-1). Low g-values < 2 are unusual for greater-than-half-filled d-shell complexes such as 3 and [(η[5]-C5R5)Fe(η[6]-C6R6)][45], and arise from the low-spin configuration where a single unpaired electron resides in a near-degenerate pair of π* orbitals (Fig. 5) where the orbital doublet degeneracy is lifted by low-symmetry perturbations, which has a parallel to the electronic structure and EPR spectra of d[3] Fe5+ nitrido and oxo complexes[46]. The negative D value for 5 in the high-spin [4]E ground state is a result of the uneven occupation of three electrons in the near-degenerate dxy/x2-y2(δ symmetry) orbitals (Fig. 5) leading to a significant contribution of orbital angular momentum along the z-direction and domination of the D component of the D-tensor[47].

Figure 5

Orbital ordering, occupation, and approximate symmetry labels for the active space of 2-7 from CASSCF-SO.

Energy separation is not to scale and is merely indicative, visualised occupations are rounded (the occupations for 6 and 7 are identical, and those shown for 2 are Fe1; those for Fe2 are nearly identical), and the five excited 4d orbitals are excluded. Note that each diagram has four electrons more than the formal dn configuration, corresponding to the formally bonding π, e1g electrons.

The difference in the ground n class="Gene">spin states of 3 and 5 is likely a result of the compressed coordination sphere experienced by the metal in 3, due to stronger dipolar interactions and shorter bond lengths for Co2+ (Table 1). This effect is analogous to that of high- and low-spin monomeric manganocenes[26]. Such changes in bonding clearly affect 3d orbital energies, and it is commonplace to see orbital occupation diagrams of metallocenes from theoretical calculations. However, orbital energies are a single electron construct, and thus are non-existent in a wavefunction where electron correlation is explicitly considered. While we cannot produce orbital energy diagrams, we can use the state-averaged occupation of the active orbitals to infer their energetic ordering; that is, orbitals with greater occupation are lower in energy relative to those with lower occupation, Fig. 5. The orbital orderings for 2 and 4 are the same, but differ from the “traditional” picture[48] of dxz/dyz (π, e1g) < dxy/dx2-y2 (δ, e2g) < dz2 (σ, a1g) < dxz/dyz (π*, e1g) (recently echoed by a density-functional theory study[49]) and also from that determined with Hartree-Fock theory of dz2 (σ, a1g) < dxy/dx2-y2 (δ, e2g) < dxz/dyz (π, e1g) < dxz/dyz (π*, e1g)[50]. The orbital orderings for 5-7 are the same as one-another, yet differ from all other orderings already discussed, and are the same as that accepted for the ferrocenium cation[50]. Complex3 is the clear outlier from our results here, where the dxz/dyz (π, e1g) orbitals are the HOMO-1, and this ordering is in agreement with the Hartree-Fock results on ferrocene[50]. All of the occupation numbers (Supplementary Tables 8, 9, 11, 13, 15, 17, 18) suggest that dz2 (σ, a1g) lies lower than the dxy/dx2-y2 pair (δ, e2g), although for 2-4 and 6-7 the average occupations are quite close (1.97(1) and 1.93(2), respectively) so that these orbitals may be quite close in energy; for 5 there is a much more significant difference in the occupation numbers of 1.96 and 1.48, respectively, clearly indicating that dz2 is lower in energy than dxy/dx2-y2. The difference between this ordering and that of the “traditional” picture must owe to electron correlation effects, but we re-iterate that orbital energies do not exist in multi-reference wavefunctions such as those calculated here and so these orderings are only indicative.

The synthetic methodology presented herein should be transn class="Chemical">ferable to other d-block metallocenates with appropriate functionalization. We note that these results come over 50 years after the first published efforts to reduce ferrocene with alkali metals[51]. In the first report of the electrochemical reduction of cobaltocene in 1974, Geiger predicted that metallocene anions would be interesting candidates to study electrophilic attack at metallocene centres[14]; such reactivity studies on structurally authenticated ferrocene monoanions are now plausible. We envisage that the isolation of thermally stable examples will facilitate more rapid progress in this endeavour[21], as well as providing systems that are more amenable to magnetic and spectroscopic characterisation.

Methods

General procedures

All manipulations were performed using standard Schlenk techniques or in an Inert Purelab HE 2GB glovebox. Solvents were dried by passing through colun class="CellLine">mns containing activated alumina and molecular sieves, or by refluxing over potassium followed by distillation, and were degassed before use. Complexes were variously characterised by cyclic voltammetry, single crystal X-ray diffraction (a Rigaku XtalLAB AFC11 or Rigaku Oxford Diffraction SuperNova diffractometer equipped with CCD area detectors), elemental microanalysis, NMR, EPR, FTIR, Raman and UV-Vis-nIR spectroscopies, and DFT and CASSCF calculations; complexes 2 and 5 were additionally studied by 57Fe Mössbauer spectroscopy.[(Cpttt)2M] (1-3) were prepared by salt metathesis protocols from the parent MCl2 and two equivalents of KCpttt in THF under reflux conditions, and were isolated by removal of volatiles in vacuo followed by recrystallization from hexane, by adapting published procedures[25-27,29]. [K(2.2.2-crypt)][(Cpttt)2M] (4-6) were prepared by reduction of parent 1-3 with KC8 [52] in the presence of 2.2.2-cryptand in THF at -40 °C, and were isolated by filtration and layering with hexane at -40 °C. See below for example syntheses of 3 and 5.

Synthesis of [(Cpttt)2Co] (3)

THF (20 mL) was added to a pre-n class="Chemical">cooled (-78 °C) mixture of CoCl2 (0.390 g, 3.0 mmol) and KCpttt (1.635 g, 6.0 mmol) in a grease-free Teflon stoppered vessel (Rotaflo), then allowed to warm slowly to room temperature. As the mixture warmed the solution slowly turned dark brown. The mixture was heated at 80 °C for 16 hrs, which produced dark brown solution with a pale precipitate. The mixture was cooled, and the volatiles were removed in vacuo to afford a brown solid. Hexane (30 mL) was added, and the mixture heated at 80 °C for 3 hrs, cooled to room temperature, and filtered away from pale solids. The solution was concentrated to ~1.5 mL and stored at 5 °C for 16 hrs, giving 3·(C as large brown plates (1.076 g, 59%). Anal. Calcd (%) for C34H58Co·C6H14: C, 78.51; H, 11.86. Found: C, 79.36; H, 11.82. [1]H NMR (C6D6, 400 or 500 MHz, 298 K): δ = 3.50 (br. s), 3.67 (br. s). [13]C{[1]H} NMR (C6D6, 125 MHz) No peaks were observed. FTIR (ATR, microcrystalline): ν̃ = 402 (w), 424 (w), 436 (w), 453 (w), 477 (w), 494 (w), 504 (w), 524 (m), 538 (w), 549 (w), 565 (w), 598 (m), 612 (w), 620 (w), 632 (w), 640 (w), 659 (w), 675 (w), 693 (w), 702 (w), 708 (w), 718 (w), 724 (w), 742 (w), 753 (w), 777 (w), 791 (w), 826 (w), 842 (w), 850 (w), 873 (w), 885 (w), 904 (w), 916 (w), 926 (w), 948 (w), 977 (w), 1003 (w), 1016 (w), 1056 (m), 1065 (m), 1073 (m), 1097 (m), 1128 (m), 1152 (w), 1163 (w), 1173 (w), 1201 (m), 1234 (s), 1260 (s), 1275 (m), 1297 (s), 1328 (m), 1354 (vs), 1387 (s), 1409 (m), 1446 (m), 1458 (m), 1477 (s), 1511 (m), 1540 (m), 1575 (m), 1589 (m), 1617 (w), 1634 (w), 1674 (w), 1699 (m), 1732 (w), 1758 (w), 1781 (m), 1819 (m), 1858 (m), 1882 (m), 1891 (m), 1909 (m), 1938 (m), 1962 (m), 1976 (s), 2009 (s), 2033 (m), 2048 (m), 2072 (m), 2131 (w), 2148 (m), 2156 (m), 2254 (m), 3016 (s).[1]H NMR spectroscopy was in agreement with earlier reports[28,29].

Synthesis of [K(2.2.2-crypt)][(Cpttt)2Fe] (5)

THF (2 mL) was added to a mixture of 2 (0.366 g, 0.7 mmol), and 2.2.2-n class="Chemical">cryptand (0.264 g, 0.7 mmol) to give a bright ruby-red solution. This solution was added rapidly to a pre-cooled (-78 °C) Schlenk vessel containing KC8 (0.095 g, 0.7 mmol) and a Teflon-coated stirrer bar. The slurry was stirred rapidly and allowed to warm to -40 °C over the course of 10 minutes, during which time the colour changed from ruby-red to dark brown. The mixture was stirred at -40 °C for 10 minutes, and then allowed to settle for a further 5 minutes. The brown solution was filtered cold to a pre-cooled (-40 °C) vessel, and concentrated at this temperature to ca. 1 mL. Hexane (4 mL) was carefully layered on top, which caused some crystals to immediately form. The vessel and cold bath were transferred to a freezer (-25 °C), to warm slowly to -25 °C overnight. Brown blocks of 5 were isolated by cold filtration (0.140 g, 21%). Anal. Calcd (%) for C52H94O6N2KFe: C, 66.57; H, 10.10; N, 2.99. Found: C, 66.60; H, 10.47; N, 3.03. [1]H NMR (C4D8O, 400 MHz, 298 K): δ = -8.12 (s, 18H, FWHM = 186 Hz, C5H2(CMe 3)), -2.70 (s, 36H, FWHM = 423 Hz, (C5H2(CMe 3)2), 2.28 – 2.78 (36H, 2.2.2-cryptand), Cpttt-CH not observed. [13]C{[1]H} NMR (C4D8O, 125 MHz) 35.76, 55.45, 57.43, 69.59, 70.51, 71.85, 72.96, 126.19, 127.00. FTIR (ATR, microcrystalline): ν̃ = 406 (m), 414 (w), 428 (m), 447 (w), 459 (w), 467 (w), 483 (w), 524 (m), 563 (m), 591 (w), 661 (w), 667 (w), 753 (m), 777 (m), 791 (m), 832 (m), 850 (w), 930 (m), 950 (s), 983 (m), 995 (m), 1026 (m), 1077 (s), 1085 (s), 1103 (vs), 1132 (s), 1195 (w), 1234 (m), 1260 (m), 1275 (w), 1295 (m), 1328 (w), 1352 (m), 1385 (m), 1446 (m), 1458 (m), 1477 (m), 1509 (w), 1542 (w), 1575 (w), 1591 (w), 1630 (w), 1644 (w), 1674 (w), 1699 (w), 1719 (w), 1734 (w), 1754 (w), 1781 (w), 1791 (w), 1821 (w), 1836 (w), 1852 (w), 1878 (w), 1895 (w), 1905 (w), 1915 (w), 1938 (w), 1962 (w), 1978 (w), 2009 (w), 2035 (w), 2046 (w), 2068 (w), 2164 (w), 2168 (w), 2239 (w), 2280 (w), 2317 (m), 2341 (w), 2372 (w), 2815 (m), 2882 (m), 2949 (m), 3018 (w), 3049 (w), 3059 (w), 3067 (w), 3076 (w), 3086 (w), 3096 (w), 3104 (w), 3114 (w), 3123 (w).

All electrochemistry experiments were initially assessed at the open circuit potential and redox potentials are referenced to the n class="Chemical">FcH+/0 couple (unless otherwise stated) which was used as an internal standard. Cyclic voltammetry was carried out using a sealed cell and a three-electrode arrangement, with a Pt wire working electrode, Pt flag secondary electrode and an AgCl/Ag wire pseudo-reference electrode prepared by soaking a Ag wire in FeCl3(aq) before rinsing with water and acetone. Where measurements are performed at low temperature, the cell was equilibrated back to room temperature after each scan and stirred thoroughly before cooling in a –50°C acetone/liquid nitrogen bath without stirring (at least 1 minute to equilibrate) then transferred back into the Faraday cage and measurements performed promptly to minimize warming.

CASSCF calculations

OpenMolcas v18.09 was used for all calculations[36], employing the unoptimized XRD structure of each complex, with n class="Chemical">counterions and/or solvent removed, and include a sphere of point charges (+2 for M2+, +1 for M1+, -0.2 for Cp-ring carbon atoms, +1 for K+ counterions) of 40 Å radius to model the crystalline electric potential. Basis functions for all atoms are from the ANO-RCC library[53,54], using VTZP quality for the 3d metal atom, VDZP quality for the 10 Cp-ring carbon atoms, and VDZ quality for all other atoms. We use the second-order DKH transformation for the relativistic Hamiltonian and Cholesky decomposition with a threshold of 10-8 for the two-electron integrals. We start with an active space of five 3d orbitals (nominally 3dz2 (σ, a1g), 3dxy and 3dx2-y2 (δ, e2g), and 3dxz and 3dyz (π*, e1g)), and use the RAS probing method[55] to locate two bonding 3d (3dxz and 3dyz (π, e1g)) and five excited 4d orbitals to include them in the active space, and subsequently optimise the orbitals using SA-CASSCF for all states below ca. 40,000 cm-1 for each spin multiplicity (relative energies). Then, we re-optimise the orbitals by considering only the lowest-lying well-isolated states for each multiplicity. In the last step, we perform a configuration interaction expansion in the optimised active space to find roots that are below 30,000 cm-1 for each spin multiplicity (relative energies), and then mix all states with SOC.

Spectra were recorded at 80 K in zero applied field using a n class="Chemical">constant acceleration spectrometer and a 57Co/Rh source. The samples used for these measurements consisted of ground powders of 2 and 5 that were contained in PEEK (polyether ether ketone) sample cups with tightly fitted lids. The isomer shift is reported relative to that of α-Fe at room temperature. Spectral simulations were generated using the WMOSS software package (SEE Co. Minneapolis, MN).

EPR spectroscopy

EPR samples were prepared as ground powders and flame sealed under inert atmosphere while keeping the sample at 77 K in 2 mm Q-band and 4 mm X-band tubes. A frozen solution sample of 3 was prepared at 5 mM concentration in a mixed 9:1 n class="Chemical">toluene:n-hexane solvent system. The solution sample was frozen in liquid nitrogen then loaded into the spectrometer. Spectra were collected using Bruker EMX300 and E500 spectrometers. Low temperature measurements were achieved using liquid helium cooling to obtain 5 K. A strong pitch standard of g = 2.0028 was used to calibrate the magnetic field.