Coordination of Al(C₆F₅)₃vs. B(C₆F₅)₃ on group 6 end-on dinitrogen complexes: chemical and structural divergences

Abstract

The coordination of the Lewis superacid tris(pentafluorophenyl)alane (AlCF) to phosphine-supported, group 6 bis(dinitrogen) complexes [ML₂(N₂)₂] is explored, with M = Cr, Mo or W and L = dppe (1,2-bis(diphenylphosphino)ethane), depe (1,2-bis(diethylphosphino)ethane), dmpe (1,2-bis(dimethylphosphino)ethane) or 2 × PMe₂Ph. Akin to tris(pentafluorophenyl)borane (BCF), AlCF can form 1 : 1 adducts by coordination to one distal nitrogen of general formula trans-[ML₂(N₂){(μ-η¹:η¹-N₂)Al(C₆F₅)₃}]. The boron and aluminium adducts are structurally similar, showing a comparable level of N₂ push–pull activation. A notable exception is a bent (BCF adducts) vs. linear (AlCF adducts) M–N–N–LA motif (LA = Lewis acid), explained computationally as the result of steric repulsion. A striking difference arose when the formation of two-fold adducts was conducted. While in the case of BCF the 2 : 1 Lewis pairs could be observed in equilibrium with the 1 : 1 adduct and free borane but resisted isolation, AlCF forms robust 2 : 1 adducts trans-[ML₂{(μ-η¹:η¹-N₂)Al(C₆F₅)₃}₂] that isomerise into a more stable cis configuration. These compounds could be isolated and structurally characterized, and represent the first examples of trinuclear heterometallic complexes formed by Lewis acid–base interaction exhibiting p and d elements. Calculations also demonstrate that from the bare complex to the two-fold aluminium adduct, substantial decrease of the HOMO–LUMO gap is observed, and, unlike the trans adducts (1 : 1 and 1 : 2) for which the HOMO was computed to be a pure d orbital, the one of the cis-trinuclear compounds mixes a d orbital with a π* one of each N₂ ligands. This may translate into a more favourable electrophilic attack on the N₂ ligands instead of the metal centre, while a stabilized N₂-centered LUMO should ease electron transfer, suggesting Lewis acids could be co-activators for electro-catalysed N₂ reduction. Experimental UV-vis spectra for the tungsten family of compounds were compared with TD-DFT calculations (CAM-B3LYP/def2-TZVP), allowing to assign the low extinction bands found in the visible spectrum to unusual low-lying MLCT involving N₂-centered orbitals. As significant red-shifts are observed upon LA coordination, this could have important implications for the development of visible light-driven nitrogen fixation.

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Introduction

Since the discovery of the first transition metal (TM) dinitrogen complex in 1965,¹ the quest for an efficient and mild process for dinitrogen transformation embodies an ultimate goal for chemists. Although much progress has been made in the last two decades in the field of artificial nitrogen fixation, the number of catalytic systems for N₂ conversion under homogeneous conditions remains limited.^2,3 Therefore, new molecular design strategies must be explored to overcome the current scientific barriers and to gain access to optimised N₂ conversion.

Donor–acceptor activation is a strategy that has not been largely implemented in N₂ chemistry involving molecular complexes. This parallels neither its success for other small molecules activation, e.g., CO₂ ^4–6 or H₂,^7–9 both well exemplified through frustrated Lewis pair (FLP) chemistry^10–17 and metal–ligand cooperativity,^18,19 nor the fact that this concept finds echo in the two main processes responsible for nitrogen fixation. With regard to the nitrogenase enzymes, the “push–pull hypothesis” surmises that the acidic residues found in the active site build H-bonds with the distal N of N₂ bound to the FeMo-cofactor,^20–24 thus increasing polarization of the diatomic molecule and facilitating its protonation.^25,26 Besides, promotion of the Haber–Bosch catalysts with electropositive elements lowers the barrier for N₂ dissociation due to electrostatic effects, which can be seen as another manifestation of N₂ donor–acceptor activation.^27–30

At the molecular level, it can be achieved by the Lewis acid–base pairing of terminal N₂ complexes with Lewis acids,^31–33 which results in increased N₂ polarisation due to enhanced back-bonding from the donor metal. This was pioneered by the Chatt group^34–36 with neutral main-group Lewis acids, and was later further exemplified by the Fryzuk,³⁷ Tuczek,³⁸ Szymczak²⁵ and Simonneau^39,40 groups. Main group^41,42 and transition metal cations⁴³ have also been shown to participate in such type of donor–acceptor systems. The “donor” partner is generally an early-to-mid transition metal with a low formal oxidation state, although a model of purely main-group N₂ donor–acceptor activation system was proposed by the Stephan group.⁴⁴ By providing an access to a highly polarised N₂ unit, opportunities for the discovery of new reactivity patterns for dinitrogen complexes can arise, for instance N₂ protonation,²⁵ silylation or borylation.³⁹ In this context, the team of Szymczak and ours have focused on the coordination of the strong boron Lewis acid tris(pentafluorophenyl)borane, B(C₆F₅)₃ (BCF) with a series of group 6 and 8 (M = Mo, W, and Fe) phosphine N₂-complexes and have studied with DFT the implications for the N₂ ligand.^25,39,43 We have recently shown in a computational study that binding LAs to transition-metal N₂-complexes may shift their molecular orbital ordering.⁴⁵ Thus, by levelling basicity and redox potentials, Lewis acid coordination to the N₂ ligand may be an interesting way to mitigate overpotentials in homogeneous ammonia synthesis (electro)catalysed with metal complexes. Recently, we turned our interest towards Lewis Super Acids (LSA),⁴⁶ driven by the curiosity of gauging the push–pull effect when the acceptor is an extremely electron-deficient species. We have shown that a two-channel activation by the means of a strongly electrophilic bis(borane) C₆F₄{B(C₆F₅)₂}₂ (B₂CF) imparts significant activation to the diatomic molecule, up to the diazene-diide (N₂²⁻) state.⁴⁰ In the continuation of this work, we decided to study the coordination of the aluminium analogue of BCF, tris(pentafluorophenyl)alane – Al(C₆F₅)₃ (AlCF)^47–56 – to group 6 dinitrogen complexes, in order to assess how the resulting Lewis pairs differ or not in terms of structure and reactivity with respect to BCF.

AlCF is structurally close to BCF as they both feature three C₆F₅ ligands in their coordination sphere and a central trivalent group 13 element, differing by their metal radii and electronegativity.⁵⁷ This apparently anecdotic distinction turns out to change quite significantly their chemical properties. As a matter of fact, while BCF is notably stable in a trigonal planar geometry and do not interact with weak and even moderate donors (such as non-polar and aromatic molecules and even oxygen-based compounds),^58,59AlCF is highly reactive (thermal and shock sensitive) in this configuration and is only stable in a tetrahedral environment where the 4th position is occupied by a weak donor^49,51,53,60 or, in its unsolvated dimeric form, through double Al–F interactions between Al and the ortho-F atom of one C₆F₅ ring.⁵³ This singular aspect to form adducts with very weak donors (vide infra) suggests indeed higher electrophilic properties of AlCFvs.BCF, and it is now widely accepted that AlCF has a much stronger Lewis acid character than BCF.⁵⁶ From computational studies and compiled experimental data, AlCF is considered as an LSA, having a Fluoride Ion Affinity (FIA)⁶¹ – acknowledged to be a way to estimate Lewis acidity – of 530 kJ mol⁻¹. In ascending order, the latter has an FIA higher than B₂CF (523 kJ mol⁻¹), SbF₅ (490 kJ mol⁻¹) (the reference of the LSA scale), and much higher than BCF (450 kJ mol⁻¹).^{53,56,62–65}

In this work, we describe a new family of AlCF adducts with Chatt-Hidai type group 6 dinitrogen complexes, by the means of spectroscopy (NMR, IR, UV-vis), single crystal X-ray diffraction (sc-XRD), and DFT calculations. Notable chemical and structural discrepancies are observed by comparison to BCF (see Fig. 1), which are duly highlighted throughout the article. Remarkably, the switch from boron to aluminium allowed us to isolate bis(μ-η¹:η¹-N₂–AlCF) adducts that remained elusive in the case of BCF. These are the first examples of neutral two-fold adducts of a main group Lewis acid with a bis(dinitrogen) complex.

Fig. 1 Coordination of AlCFversusBCF on Group 6 end-on dinitrogen complexes leading to a new family of mono and double Al dinitrogen adducts.

Results and discussion

Syntheses of 1 : 1 adducts supported with bis(phosphines)

Stoichiometric treatment (1 : 1) of tris(pentafluorophenyl)alane toluene adduct⁵¹ with a series of dinitrogen complexes trans-[ML₂(N₂)₂] in toluene (M = W, Mo, and Cr; L = 1,2-bis(diethylphosphino)ethane [depe] or 1,2-bis(diphenylphosphino)ethane [dppe] or 1,2-bis(dimethylphosphino)ethane [dmpe])^43,66–75 under a dinitrogen atmosphere produced new 1 : 1 adducts [ML₂(N₂)(μ-N₂)Al(C₆F₅)₃] 1_Al, 2_Al, 5_Al, 6_Al, and 7_Al of trans configuration in moderate to excellent yields (Scheme 1 and Table 1). Note that better results in terms of analytical purity, yields, and reproducibility have been obtained with the depe and dmpe series (see ESI†). Adducts 1_Al, 2_Al, 5_Al, 6_Al and 7_Al were characterised in solution and in the solid-state by multi-nuclei NMR and IR spectroscopies as well as single-crystal XRD analysis. Similarities are found between the depe-supported complexes 1_Al, 2_Al and their boron analogues 1_B, 2_B. Indeed, NMR signatures of these species are very close especially when considering their ³¹P NMR resonance (see Table 3). Coordination of the LA (BCF or AlCF) at the distal nitrogen of the N₂ fragment induces a nearly equal bathochromic shift of the μ-N≡N IR band and hypsochromic shift of the terminal N≡N stretching mode (see Table 3).

Scheme 1 Reactivity of ML₂(N₂)₂ (M = W, Mo, Cr; L = depe, dppe, dmpe) complexes with (top) B(C₆F₅)₃ and (bottom) Al(C₆F₅)₃(tol) (1 equiv.) under a dinitrogen atmosphere.

Table 1 Description of the different adducts

Compound	LA^a	M	R	Config.	N2 motifs	Yield (%)
a LA = Lewis acid. b NMR yield.
1AL	AlCF	W	Et	trans	μ-N2, η-N2	89
1B ^43	BCF	W	Et	trans	μ-N2, η-N2	62
2AL	AlCF	Mo	Et	trans	μ-N2, η-N2	100
2B ^43	BCF	Mo	Et	trans	μ-N2, η-N2	53
3B	BCF	W	Ph	trans	μ-N2	{31}^b
4B	BCF	Mo	Ph	trans	μ-N2	{95}^b
5AL	AlCF	W	Ph	trans	μ-N2, η-N2	51
5B	BCF	W	Ph	trans	μ-N2, η-N2	{69}^b
6AL	AlCF	Mo	Ph	trans	μ-N2, η-N2	81
7AL	AlCF	Cr	Me	trans	μ-N2, η-N2	79

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Suitable single-crystals of 1_Al and 2_Al for XRD studies have been grown from a cold and saturated solution of toluene/n-pentane. The solid-state structures of 1_Al and 2_Al (see Fig. 3, left, for 1_Al and ESI† for 2_Al) depict a similar octahedral geometry around the group 6 metal to that of 1_B and 2_B. Expectedly, coordination of AlCF to the distal N atom in complexes 1_Al and 2_Al imparts a tetrahedral geometry around the Al center (angles averaged at 109.5° for 1_Al and 108.0° for 2_Al). The N₁–N₂ bond lengths are similar between the aluminium and boron analogues (see Table 3). The TM-N₁ distance is slightly shortened in the case of aluminium adducts (W–N₁ = 1.855 Å for 1_Alvs. 1.909 Å for 1_B and Mo–N₁ = 1.869 Å for 2_Alvs. 1.894 Å for 2_B).

Overall, these experimental data point to a diminished bond order for the N₂ unit as a result of enhanced back-donation with a similar “push–pull” activation level of μ-N₂ in species 1_Al, 2_Al and 1_B, 2_B. However, we noticed structural divergences between 1_Al, 2_Al and their boron analogues 1_B, 2_B. According to the Cambridge Structural Database (CSD), the Al₁–N₂ bond lengths – 1.817 Å for 1_Al and 1.842 Å for 2_Al – are found to be the shortest ones compared to the expected Al–N distances range for similar reported N–Al(C₆F₅)₃ motifs (from 1.853 Å ^76,77 to 2.167 Å ⁷⁸) and N₂–AlR₃ (R = alkyl) fragments (from 1.929 Å ⁷⁹ to 2.089 Å ⁸⁰). On the other hand, the B–N₂ length for the boron congeners (1.549 Å for 1_B and 1.562 Å for 2_B) are found in the expected B–N distances range for similar reported N–B(C₆F₅)₃ moieties (from 1.492 Å ⁸¹ to 1.807 Å ⁸²) but are slightly below the B–N distances range for comparable bridging diazo borane (μ-N₂)–B(C₆F₅)₃ and azido borane (μ-N₃)–B(C₆F₅)₃ fragments (from 1.575 Å ²⁵ to 1.678 Å ³⁸). These results thus advocate for the presence of robust interactions between the bridging N₂ and the LA centre, more prominent in the case of aluminium.

Experimentally, we demonstrated the stronger affinity of μ-N₂ motif for AlCFvs.BCF by treating adduct 1_B with one equivalent of Al(C₆F₅)₃(tol) that leads to the formation of 1_Al and free BCF with an NMR yield higher than 90% (see Scheme 1 and ESI†). Note that over time this equilibrium does not evolve showing that the formation of 1_Al from 1_B is thermodynamically favourable. This set of clues led us to analyse the N₁–N₂–LA angle. In the case of the aluminium adducts, a nearly straight N₁–N₂–Al angle is found – 168.4° and 167.8° for 1_Al and 2_Al, respectively. These data conflict with similar reported N=N–Al angles of bridging diazenido trialkylaluminum (μ-N=N)–AlR₃ and azido trialkylaluminum (μ-N=N=N)–AlR₃ species featuring values ranging from 105.5° ⁸⁰ to 158.9°.⁸⁴ These results also contrast with the bent N₁–N₂–B angle found for the boron analogues – 148.4° for 1_B and 150.9° for 2_B. While [M(depe)₂(N₂)₂] and [M(dppe)₂(N₂)₂] cleanly reacted with BCF to form quantitatively 1 : 1 adducts, we observed significant divergent behaviours when we engaged trans-[Cr(dmpe)₂(N₂)₂] with BCF. Indeed, this leads to a partial and unselective reaction towards a complex mixture of species (starting materials in equilibrium with other species, see ESI†) that we were not able to isolate from each other in the solid-state. Among them, we can assume that the 1 : 1 adduct is partly formed. On the opposite, the stoichiometric reaction of Al(C₆F₅)₃(tol) with [Cr(dmpe)₂(N₂)₂] cleanly produced a new 1 : 1 adduct 7_Al in good yields (Scheme 1, bottom). Spectroscopic and crystallographic parameters of 7_Al are nearly identical to those of tungsten and molybdenum analogues 1_Al and 2_Al (see Fig. 3 and Table 3) showing a similar N₂ activation degree (close N–N distances and N≡N IR stretches) and AlCF coordination (close Al–N distances and Al–N–N angles in particular).

DFT investigation on the N–N–LA angle

To shed light into these results, DFT calculations at the BP86/def2-TZVP level of theory were employed, including implicit solvation and dispersion corrections, starting from the crystal structures of the BCF and AlCF adducts. One explicit solvent molecule was added to the molecular models due to the aforementioned greater stability of AlCF in a tetrahedral environment; this is required for the analysis of the thermodynamics behind the LA binding.

The potential energy surface (PES) minima found upon geometry relaxation match well with experiment: M–N₁ and N₂–LA bonds were only ca. 0.050 Å longer than the experimental ones and other deviations were even smaller. The N₁–N₂–LA angles obtained for the computed structures of AlCF and BCF adducts were 170° and 148°, respectively. A detailed comparison of the computational and experimental structural and spectroscopic features is included in the ESI (Tables S5 and S6).† To further elucidate the PES regarding the binding angle of the LAs, constrained geometry optimisations with varying N–N–LA angles (148° to 172°) were carried out for both LA adducts (Fig. 2). The N≡N–B angle is in fact extremely flexible: in the case of the least sterically impeded adduct, we observe the energy minimum at ca. 150° (in agreement with experimental data) and a small dent close to 165°, separated by less than 0.5 kcal mol⁻¹. The latter is not a local minimum as it is due to a ca. 10° rotation of one ethyl phosphine substituent. The increase in energy along the bending motion is, overall, meagre, with an energetic cost of less than 1 kcal mol⁻¹. For the AlCF 1 : 1 adduct, in contrast, a continuous and steeper increase in energy is observed as the N≡N–LA angle is decreased.

Fig. 2 (a) Potential energy surface along the N–N–Lewis acid angle coordinate for the AlCF (crimson) and BCF (red) 1 : 1 adducts, energies reported relative to PES minimum; and (b) relevant angles of the optimized structures.

Fig. 3 Solid-state structures of 1_Al and 7_Al. Ellipsoids are represented with 30% probability. Hydrogen atoms have been omitted for clarity. Two independent molecules were found in the asymmetric unit (Z′ = 2) of 1_Al but one of them has been omitted for clarity. Selected bond distances (Å) and angles (°) have been averaged between both independent molecules for 1_Al: Al₁–N₂ 1.816(7), W₁–N₁ 1.855(2), W₁–N₃ 2.113(2), N₁–N₂ 1.203(6), N₃–N₄ 1.114(1), W₁–N₁–N₂ 178.6(6), W–N₃–N₄ 177.2(6), N₁–W₁–N₃ 177.3(6), N₁–N₂–Al₁ 168.3(6). For 7_Al: Al₁–N₂ 1.8473, Cr₁–N₁ 1.7507, Cr₁–N₃ 1.9766, N₁–N₂ 1.177(2), N₃–N₄ 1.100(3), N₃–Cr₁–N₁ 177.47(7), N₂–N₁–Cr₁ 178.55(2), N₄–N₃–Cr₁ 178.02(18), N₁–N₂–Al₁ 170.26(2).

There is a marginal stabilisation of the frontier occupied orbitals in both adducts as the angle is bent from 148° to 172° (Fig. S93†), suggesting that the differing angles obtained in the crystal structures are not rooted in electronic structure stabilisation effects but are instead mainly due to steric hindrances. Note that for the N≡N–LA angle to bend (blue in Fig. 1b), a simultaneous bending of the M–N₁≡N₂ angle (peach, in Fig. 1b) by 9° occurs to better accommodate the LA around the phosphine ligand arms. This is true for both LAs.

Influence of the atmosphere: N₂vs. Ar

It is important to mention that for adducts in the depe and dmpe series we observed the same reactivity whether working under dinitrogen or argon. Nevertheless, we noticed significant divergences for the dppe series. Indeed, when using B(C₆F₅)₃, our group had previously observed the elimination of one dinitrogen molecule during the reaction leading to the formation of [M(dppe)₂(μ-N₂)B(C₆F₅)₃] adducts where the apical site (left vacant by N₂ dissociation) is occupied by an agostic interaction with an ortho hydrogen of one of the phenyl groups in the solid-state.³⁹ This process occurred under argon (Scheme 2, middle). Under dinitrogen, we noticed the same reactivity for trans-[Mo(dppe)₂(N₂)₂] (i.e. loss of one of the N₂ ligands) but the stoichiometric treatment of trans-[W(dppe)₂(N₂)₂] with BCF leads, after one night, to a mixture of [W(dppe)₂(μ-N₂)B(C₆F₅)₃] 3_B and trans-[W(dppe)₂(N₂)(μ-N₂)B(C₆F₅)₃] 5_B in a 31 : 69 3_B : 5_B ratio, respectively. Of note, species 5_B was observed in solution but we did not succeed to isolate it (see Scheme 1, top left, and ESI†).

Scheme 2 Reactivity of ML₂(N₂)₂ (M = W, Mo; L = dppe) complexes with B(C₆F₅)₃ and Al(C₆F₅)₃(tol) under an argon atmosphere. {The yield in brackets followed by a star*} represents the NMR yield. The other complexes (L = depe or dmpe) reacted similarly as under a dinitrogen atmosphere (see Scheme 1).

By contrast, the reaction of Al(C₆F₅)₃ with trans-[M(dppe)₂(N₂)₂] (M = Mo and W) does not promote the elimination of N₂ when working under a dinitrogen atmosphere. This leads instead to a similar reactivity to that of the depe series i.e. the formation of products 5_Al and 6_Al where the terminal N₂ stays bonded to the metal centre (Scheme 1). Under an inert atmosphere of argon, the stoichiometric treatment of AlCF with trans-[Mo(dppe)₂(N₂)₂] leads predominantly (73% NMR yield, see ESI†) to the formation of the aluminium analogue of 4_B, [Mo(dppe)₂(μ-N₂)AlCF] 4_Al, in which the second dinitrogen ligand is lost during the reaction (Scheme 2, top). Identity of adduct 4_Al is successfully established by XRD studies. It should be noted, however, that the quality of XRD data was not good enough to discuss the metrical parameters in great detail but confirmed the atom connectivity and loss of one N₂ ligand (see ESI†).

Surprisingly, changing from Mo to W drastically impacts this chemistry since the 1 : 1 reaction of trans-[W(dppe)₂(N₂)₂] with AlCF under argon does not trigger N₂ dissociation and instead promotes the quantitative formation of 5_Al as under a dinitrogen atmosphere (see Scheme 2, bottom, and ESI†). This highlights the sensitivity of these species towards the retention of their second N₂ ligand, depending whether the reaction medium is N₂-saturated or not. We assumed that formation of adducts 3–4 involves first the formation of 5–6 as intermediates (coordination of the LA at the distal N), which can then lose their terminal N₂ ligand depending on the LA and the atmosphere. In this case, this second step is more feasible (in ascending order) for 4_B > 3_B > 4_Al > 3_Al. This translates into Mo- and/or B-containing species having a greater tendency to labilise the trans-N₂ ligand. Spectroscopic and crystallographic data of 3–4vs.5–6 revealed distinct features (Table 3). The IR μ-N≡N stretching mode is shifted to lower wavenumbers for adducts 3–4vs.5–6 and the bridging N–N distances are elongated in adducts 3–4vs.5–6. Therefore, the elimination of the terminal dinitrogen molecule induces a stronger polarisation of the M–N≡N–LA fragment (3_B, 4_Bvs.5_Al and 6_Al). Notably, comparable crystallographic data between 5_Al, 6_Al and 1_Al, 2_Al are found when it comes to the LA–N₂ distance and N₁–N₂–LA angle i.e. a short Al–N separation and a nearly linear Al–N≡N array, again contrasting with the boron adducts 3_B and 4_B featuring bent B–N≡N angles (see Table 3).

Also, similarly to the depe series, the stronger affinity of N₂ metal complexes for AlCFvs.BCF in the dppe series was verified experimentally by treating the BCF adducts 3_B–4_B with one equivalent of AlCF producing instantly (whether working under argon or dinitrogen) the aluminium adducts 4_Al, 5_Al, and 6_Al and free BCF (see Scheme 1, left, Scheme 2, and ESI†). These reactions demonstrate the stronger affinity of AlCFvs.BCF for the dinitrogen ligand.

Syntheses of 2 : 1 adducts

Since we employed bis(dinitrogen) complexes as Lewis base partner, we were curious to know whether the reaction of [ML₂(N₂)₂] with two equivalents of the Lewis acid (AlCF or BCF) could provide 2 : 1 adducts. When we added two equivalents of B(C₆F₅)₃ to [M(depe)₂(N₂)₂] (M = Mo, W) we noticed an immediate colour change from orange-brown to deep purple-blue. While in the case of molybdenum, NMR analyses suggested some degradation occurring upon addition of the second equivalent of BCF, the spectra recorded when the W species was employed suggests the formation of a new putative complex 8_B (see Scheme 3, top, and Table 2). This is evidenced by a gain in symmetry as indicated by undifferentiated alkyl protons in the ¹H NMR spectrum, as opposed to 1_B (see ESI†). However, we also cannot exclude that such ¹H NMR spectrum results from signal coalescence of 1_B due to a concentration phenomenon as already observed in the case of 1_Al (Fig. S1–S3 and S40†). This could explain why the ³¹P NMR spectrum showed no change with respect to the mono adduct 1_B (δ = 34.7 ppm). Surprisingly, only two large signals are observed in ¹⁹F NMR, contrasting with the well-resolved multiplets characterizing ortho, meta and para fluorine resonances in 1_B. This may suggest either a fluxional behaviour of 8_B or that a fast 1_B + BCF ⇌ 8_B equilibrium takes place at room temperature. Measuring ¹H and ¹⁹F NMR at low temperature (down to −60 °C) resulted in de-coalescence of the signals. In particular, broad resonances, which chemical shifts match those of 1_B and free BCF, are found in the ¹⁹F NMR spectrum, pointing to an equilibrated mixture. Shoulders on the peaks of the para and meta fluorine of 1_B might be assigned to the two-fold adduct 8_B (Scheme 1, top-right, and Fig. S40†). Unfortunately, our attempts to isolate such a two-fold adduct were unsuccessful: crystals of 1_B were systematically collected from the purple solutions.

Scheme 3 Reactivity of [ML₂(N₂)₂] (M = W, Mo, Cr; L = depe, dppe, dmpe) complexes with (top) two equivalents of B(C₆F₅)₃ and (bottom) two equivalents of Al(C₆F₅)₃(tol) under a dinitrogen atmosphere.

Table 2 Description of the two-fold adducts

Compound	LA^a	M	R	Config.	N2 motifs	Yield (%)
a LA = Lewis acid. b n.i. = not isolated.
8Al	AlCF	W	Et	trans	2× μ-N2	96
8B	BCF	W	Et	trans	2× μ-N2	n.i.^b
9Al	AlCF	Mo	Et	trans	2× μ-N2	n.i.^b
10Al	AlCF	Cr	Me	trans	2× μ-N2	n.i.^b
11Al	AlCF	W	Et	cis	2× μ-N2	77
12Al	AlCF	Mo	Et	cis	2× μ-N2	94
13Al	AlCF	Cr	Me	cis	2× μ-N2	77

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Gratifyingly, treatment of trans-[M(depe)₂(N₂)₂] (M = Mo, W) and trans-[M(dmpe)₂(N₂)₂] (M = Cr) with two equivalents of AlCF·toluene instantly triggered a quantitative reaction characterised by a colour change from reddish (ML₂(N₂)₂ starting materials) to blue azure/greenish within seconds. We attributed this colour change to the formation of a 2 : 1 adduct with a trans-configuration – species 8_Al (M = W), 9_Al (M = Mo), and 10_Al (M = Cr) (Scheme 3, Table 2, and Fig. 4, top). With time, we noticed an additional colour change from blue/green to brown/orange corresponding to the formation of another 2 : 1 adduct this time with a cis-configuration, namely products 11_Al (M = W), 12_Al (M = Mo), and 13_Al (M = Cr) (Scheme 3, bottom, and Fig. 4, bottom).

Fig. 4 Solid-state structures of 8_Al, 11_Al, and 13_Al. Ellipsoids are represented with 30% probability. Hydrogen atoms have been omitted for clarity. Two independent molecules were found in the asymmetric unit (Z′ = 2) of 11_Al, and 13_Al but one of them has been omitted for clarity. Selected bond distances (Å) and angles (°) have been averaged between both independent molecules for 11_Al and 13_Al. For 8_Al: Al₁–N₂ 1.927(2), Al₂–N₄ 1.919(2), W₁–N₁ 1.964(2), W₁–N₃ 1.956(3), N₁–N₂ 1.113(3), N₃–N₄ 1.114(3), N₃–W₁–N₁ 174.13(7), N₂–N₁–W₁ 176.88(2), N₄–N₃–W₁ 177.09(2), N₁–N₂–Al₁ 168.64(2), N₃–N₄–Al₂ 175.22(2). For 11_Al: Al₁–N₂ 1.901(4), Al₂–N₄ 1.894(0), W₁–N₁ 1.919(9), W₁–N₃ 1.901(0), N₁–N₂ 1.144(6), N₃–N₄ 1.156(6), W₁–N₁–N₂ 175.5(4), W₁–N₃–N₄ 175.8(4), N₁–W₁–N₃ 89.20(7), Al₁–N₂–N₁ 175.7(9), Al₂–N₄–N₃ 168.7(4). For 13_AL Al₁–N₂ 1.884(6), Al₂–N₄ 1.899(0), Cr₁–N₁ 1.784(2), Cr₁–N₃ 1.778(9), N₁–N₂ 1.156(1), N₃–N₄ 1.157(1), Cr₁–N₁–N₂ 175.6(9), Cr₂–N₃–N₄ 176.0(9), N₁–Cr₁–N₃ 89.19(2), Al₁–N₁–N₂ 170.8(4), Al₂–N₄–N₃ 172.0(0).

In the case of tungsten, intermediate 8_Al is stable enough (for one or two hours at room temperature) so that we succeeded to isolate it and analyse it by IR, XRD, and NMR. Then, 8_Al is progressively (within one day) converted into product 11_Al. However, intermediates 9_Al (M = Mo) and 10_Al (M = Cr) evolved within minutes towards products 12_Al and 13_Al, precluding their isolation (see ESI† for further details). The trans geometry of intermediate 8_Al is first evidenced by its ¹H NMR spectrum that exhibits 3 centrosymmetric signals (δ = 1.44, 1.13, and 0.68 ppm) and by its ³¹P NMR spectrum that displays a shielded pseudo-triplet (¹J_W–P = 141 Hz) at δ = 31.0 ppm (vs. 34.6 ppm for 1_Al). This configuration is confirmed by its structure in the solid-state (Fig. 4, top). Here, the Al₁–N₂–N₁–W₁–N₃–N₄–Al₂ atoms are almost perfectly aligned. Also, the coordination of a second AlCF moiety imparts a significant shortening of the N–N bonds (1.11 Å vs. 1.20 Å in 1_Al) and elongation of the W–N₁ (1.96 Å vs. 1.86 Å in 1_Al) and Al–N (1.92 Å vs. 1.82 Å in 1_Al) bonds (see Table 3) showing a decreased activation of the bridging dinitrogen fragments. These features are verified by IR where the ATR spectrum of 8_Al displays a single bridging N₂ stretch at higher wavenumber to that of 1_Al (1808 vs. 1778 cm⁻¹). Based on these data, we propose a formal bridging Al–N≡N–M depiction. The cis arrangement of products 11_Al and 12_Al is first demonstrated by NMR spectroscopy as their ¹H NMR spectra display asymmetrical depe resonances (see Fig. S44 and S54†) and their ³¹P NMR spectra feature two triplets (²J_P–P = 6 Hz and 14 Hz for 11_Al and 12_Al), each integrating for 2P (see Table 3 and ESI†). We could not analyse 13_Al (M = Cr, L = dmpe) by NMR spectroscopy as this species was not soluble in chemically compatible deuterated solvents (even ortho-dichlorobenzene). IR-ATR spectra of 11_Al, 12_Al, and 13_Al display two intense N≡N bands (see Table 3) assigned to symmetric and asymmetric N₂ stretches. Eventually, solid-state structures of 11_Al, 12_Al, and 13_Al (see Fig. 4-bottom and ESI†) confirmed the cis arrangement, with almost orthogonal N₁–M–N₃ angles. Of note, an elongation of the N–N bond is observed for 11_Al when compared to the trans adduct 8_Al (1.152 Å vs. 1.113 Å, respectively).

Table 3 Relevant structural and spectroscopic parameters (distances (Å), angles (°), wavenumbers (cm⁻¹), chemical shift (ppm)) of the aluminium and boron adducts

Adduct	δ ^31P NMR^a	ν 1 (μ-N2)	ν 2 (N2)	N1–N2	N3–N4	N2–LA^b	N4–LA^b	M–N1	M–N3	N1–M–N3	N1–N2–LA^b	N3–N4–LA^b
a Recorded in C6D6. b LA = Lewis acid.
1Al	34.6	1778	2088	1.204	1.114	1.817	—	1.855	2.113	177.4	168.4	—
1B	34.7	1767	2076	1.181	1.082	1.549	—	1.909	2.015	175.7	148.4	—
2Al	52.6	1790	2137	1.168	1.103	1.842	—	1.869	2.128	177.7	167.8	—
2B	53.0	1789	2120	1.175	1.093	1.562	—	1.894	2.129	176.3	150.9	—
3B	69.2	1717	—	1.212	—	1.571	—	1.841	—	—	140.3	—
4Al	70.9	—	—	—	—	—	—	—	—	—	—	—
4B	73.1	1744	—	1.197	—	1.568	—	1.841	—	—	141.5	—
5Al	45.4	1773	2121	1.181	1.090	1.865	—	1.885	2.108	177.2	169.3	—
6Al	63.1	1786	2161	1.174	1.094	1.876	—	1.894	2.139	173.8	176.6	—
7Al	62.3	1802	2122	1.177	1.100	1.847	—	1.751	1.977	177.5	170.3	—
8Al	31.0	1808	—	1.113	1.114	1.927	1.919	1.964	1.956	174.1	168.6	175.2
11Al	28.6, 16.6	1903, 1802	—	1.145	1.157	1.901	1.894	1.920	1.901	89.2	175.8	168.7
12Al	44.4, 29.2	1927, 1821	—	1.148	1.138	1.892	1.907	1.910	1.921	88.6	173.9	170.7
13Al	—	1948, 1833	—	1.156	1.157	1.885	1.899	1.784	1.779	89.2	170.8	172.0
15Al	−18.8, −22.1, −25.5	1776	2037	—	—	—	—	—	—	—	—	—
16Al	−24.3, −26.5	1901, 1804	—	1.149	1.150	1.915	1.891	1.917	1.906	91.3	168.5	179.1

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DFT investigation on the 2 : 1 adduct formation

DFT calculations show that sequential binding of two equivalents of BCF or AlCF is thermodynamically favourable (Fig. 5), although binding of the second LA is associated with a relatively lower stabilisation of the adduct as may be expected from the trans effect. The individual contributions to the Gibbs energies can be found in the ESI, Tables S7 and S8.†

Fig. 5 Relative Gibbs energies (kcal mol⁻¹) of 1 : 1 (1_B and 1_Al) and 2 : 1 adduct formation. The cis isomer is more stable than the trans by ca. 3 kcal mol⁻¹.

The AlCF adducts are lower in relative energy than the BCF analogues. Conversion from trans to cis adducts was observed and indeed the cis isomeric form is shown to be more stable by 3.0 kcal mol⁻¹ over the trans 2 : 1 adduct. We analysed the MO diagrams of the AlCF adduct series to rationalise the degree of dinitrogen activation observed (Fig. 6). The complete frontier MO diagram as well as the depiction of the orbitals for the bare tungsten depe complex can be found in the ESI (Fig. S92).†

Fig. 6 (a) 2D depiction of the orbitals involved in the “push–pull” activation and metal s orbital used as reference and (b) MO diagram for the Al series of adducts (blue: LUMO/LUMO+1 average; green: HOMO; orange: HOMO−1, brown: HOMO−2, pink: σ antibonding interaction within the bridge). Orbital energies are plotted relative to the tungsten s orbital and thus all are positive (left vertical axis). Energies relative to proximally the midpoint of the HOMO/LUMO gap shown on the right vertical axis. Nomenclature of the orbitals considers symmetry.

The binding of LAs to the terminal atom of the nitrogen ligand has been shown to stabilise π* interactions in the N–N bridge, resulting in bond²⁵ weakening. In the case of the depe complexes, the same is observed when the formation of the 1 : 1 adduct occurs as a ca. 0.10 eV stabilisation from the bare complex to the AlCF 1 : 1 adduct (ν_N–N = 1778 cm⁻¹) is observed. However, in apparent contradiction to experimental results (ν_N–N = 1808 cm⁻¹ measured for the 2 : 1 trans adduct), a further ca. 0.08 eV stabilisation is noted upon binding of the second LA. As we have shown in previous work,⁴⁵ an analysis of the π interactions is insufficient to explain dinitrogen activation in such complexes. A concomitant destabilisation (0.65 eV) of the σ*–σ* orbital is observed that greatly exceeds the π stabilisation, explaining the increase in N–N stretching frequency (from the computed 1864 cm⁻¹ in W–Al₁ to 1880 cm⁻¹ in W–Al_2trans). The more stable cis adduct showed a slightly decreased bond strength (ν_N–N = 1802 cm⁻¹). The MO diagram for the cis 2 : 1 adduct shows a further 0.21 eV destabilisation of the σ*–σ* orbital, which should result in a stronger dinitrogen bond. It is not the case here, however, as the different coordination geometry allows for mixing of the metal d orbital that would form the δ MO in the trans adducts with the π orbitals of the dinitrogen bridge (Fig. 7). Therefore, the nature of the HOMO – a metal-centred orbital in the trans isomer – is significantly modified, forming an additional π–π* interaction in the cis isomer. This yields a total population of 6 electrons in N–N antibonding frontier orbitals instead of 4, leading to a greater overall activation of the N–N bond. The higher extent of the overlap between the metal and ligand orbitals is also likely responsible for the greater stability of this form.

Fig. 7 Cis (11_Al) vs. trans (8_Al) frontier orbitals (HOMO to HOMO−2). AlCF omitted for clarity. Orbitals of the cis isomer are shown in side and top views.

Case of a monophosphine-supported W–N₂ complex

To get more insights about the divergent chemical behaviours of AlCFvs.BCF towards bis-dinitrogen complexes, we also investigated their reactivity with cis-[ML′₄(N₂)₂] species (M = Mo or W, L′ = dimethylphenylphosphine). Stoichiometric treatment of BCF with cis-[WL′₄(N₂)₂] leads to the partial abstraction of one PMe₂Ph ligand to form a BCF-phosphine adduct – species 14 – (Scheme 4-top left) with a complex mixture of species (see ESI†) that we were not able to identify (except some remaining starting dinitrogen complex). From this experiment we concluded that adjunction of the Lewis acid mainly triggered decomposition. Furthermore, this highlights the ease for BCF to dissociate a monophosphine ligand suggesting its stronger affinity for PMe₂Ph vs. N₂. On the opposite, using similar conditions to that of the [M(depe)₂(N₂)₂] series, the reaction of AlCF with cis-[ML′₄(N₂)₂] (M = W) produces new LA-dinitrogen adducts – products 15_Al and 16_Al (Scheme 4, bottom). First clues about the identity of the mono adduct 15_Al is evidenced by NMR spectroscopy. Indeed, its ³¹P NMR spectrum displays three signals at chemical shifts of −18.8, −22.1, and −25.5 ppm integrating respectively for 1, 2 and 1 phosphorus nuclei. This NMR signature suggests that 15_Al is cis-[W(PMe₂Ph)₄(N₂){μ-N₂–Al(C₆F₅)₃}] having one terminal dinitrogen motif and one bridging dinitrogen fragment. These above aspects are confirmed by IR spectroscopy where coordination of one AlCF molecule at one distal nitrogen induces an averaged bathochromic shift of −171 cm⁻¹ of the μ-N≡N IR band −1776 vs. 1947 cm⁻¹ in cis-[W(PMe₂Ph)₄(N₂)₂]— and an averaged hypsochromic shift of +89 cm⁻¹ of the terminal N≡N stretching mode −2037 vs. 1947 cm⁻¹ in cis-[W(PMe₂Ph)₄(N₂)₂]. Unfortunately, despite the good purity of 15_Al verified by elemental and spectroscopic analysis, our attempts to get single crystals were unsuccessful.

Scheme 4 Reactivity of [M(PMe₂Ph)₄(N₂)₂] (M = W or Mo) complexes with (top) B(C₆F₅)₃ and (bottom) Al(C₆F₅)₃(tol).

Addition of two equivalents of Al(C₆F₅)₃(tol) on cis-[W(PMe₂Ph)₄(N₂)₂] produced a new two-fold adduct 16_Al —cis-[W(PMe₂Ph)₄{μ-N₂–Al(C₆F₅)₃}₂]— that was fully characterised in solution and in the solid-state. Spectroscopic and crystallographic data of 16_Al are very close to those of its congeners 11_Al (M = W), 12_Al (M = Mo), and 13_Al (M = Cr), showing a cis geometry for the AlCF-(μ-N₂) fragments (see Table 3). Indeed, aside from their ³¹P NMR chemical shifts, the IR and XRD data of 16_Alvs.11_Al are almost identical (see Table 3 and Fig. 8).

Fig. 8 Solid-state structure of 16_Al. Ellipsoids are represented with 30% probability. Hydrogen atoms have been omitted for clarity. Selected bond distances (Å) and angles (°): Al₁–N₂ 1.915(3), Al₂–N₄ 1.891(3), W₁–N₁ 1.917(3), W₁–N₃ 1.906(3), N₁–N₂ 1.149(4), N₃–N₄ 1.150(4), W₁–N₁–N₂ 179.2(3), W₁–N₃–N₄ 177.5(3), N₁–W₁–N₃ 91.34(1), Al₁–N₂–N₁ 168.5(3), Al₂–N₄–N₃ 179.1(3).

Electronic spectroscopy of the depe-supported W complexes

The recorded UV-vis absorption spectra of trans-[M(depe)₂(N₂)₂] (M = W and Mo) at 298 K display two types of bands, an intense transition (320–330 nm, ε ≈ 10⁵ M⁻¹ cm⁻¹) assigned to metal-to-ligand charge transfer (MLCT) involving a ligand phosphorus atom, and a less intense transition (440–500 nm, ε ≈ 10³ M⁻¹ cm⁻¹) assigned to a ligand field (LF) d–d transition.⁸⁵

The MLCT transition of the aluminium and boron adducts does not shift substantially (Δλ < 3 nm) compared to that of the W starting complex (Fig. 9). However, their intensities are about two times lower compared to the W starting complex. We thus assign these energetically similar UV signatures to the chemical environment around the W–P that does not change substantially upon coordination of the LA (unlike the dinitrogen ligand where the coordination of AlCF or BCF takes place). Fig. 10 (left side) displays the visible spectra of each sample at a concentration of 10⁻³ M. The trans-W(depe)₂(N₂)₂ starting complex displayed two LF (d–d transitions) bands at λ₁ = 467 nm and λ₂ = 509 nm in agreement with literature data.⁸⁵ For the Al mono adduct (W–Al, crimson line) we observed a significant blue shift of the first band —λ₁ = 411 nm— and a small red shift of the second band —λ₂ = 513 nm. For the boron mono-adduct (red line), we observed a slight blue shift for the first and second bands (λ₁ = 437 nm, λ₁ = 506 nm). The Al double adducts of trans configuration display two new bands (crimson dotted line), one at a wavenumber of 499 nm and the other at a high wavenumber of 633 nm (this complex has a green-cyan colour). For the cis-double adduct, the spectrum displays a single maximum in the visible region at 497 nm. Note that for all the Al and B adducts, we noticed absorption in the [550–700 nm] spectral window (unlike the W starting complex where there is no absorption at all in this area).

Fig. 9 Absorption spectra of trans-[W(depe)₂(N₂)₂] (W, grey line), trans-[W(depe)₂(N₂)(μ-N₂–Al(C₆F₅)₃)] (W–Al, crimson line), trans-[W(depe)₂{(μ-N₂–Al(C₆F₅)₃}₂] (trans-W–Al₂, dotted crimson line), cis-[W(depe)₂{(μ-N₂–Al(C₆F₅)₃}₂] (cis-W–Al₂, dashed crimson line), and trans-[W(depe)₂(N₂)(μ-N₂–B(C₆F₅)₃] (W–B, red line). The concentration of each sample is about 30 μM.

Fig. 10 Experimental (left) and computational (CAM-B3LYP, right) absorption spectra of trans-[W(depe)₂(N₂)₂] (W, grey line), trans-[W(depe)₂(N₂)(μ-N₂–Al(C₆F₅)₃)] (W–Al, crimson line), trans-[W(depe)₂{(μ-N₂–Al(C₆F₅)₃}₂] (trans-W–Al₂, dotted crimson line), cis-[W(depe)₂{(μ-N₂–Al(C₆F₅)₃}₂] (cis-W–Al₂, dashed crimson line), and trans-[W(depe)₂(N₂)(μ-N₂–B(C₆F₅)₃] (W–B, red line). The concentration of each sample is about 1000 μM. A Lorentzian line broadening with FWHM of 8 was applied to the computed peaks.

Computing the electronic excitation spectra of transition-metal complexes with a high degree of quantitative accuracy is far from trivial.⁸⁶ Nevertheless TD-DFT calculations are key to provide understanding into the nature of the transitions responsible for the UV-vis bands. The peaks obtained via TD-DFT calculations (CAM-B3LYP/def2-TZVP) are in qualitative agreement with the recorded spectra, albeit being generally red shifted by ca. 30–60 nm, except for the bare tungsten complex in which an almost exact match is obtained. The mono-substituted adducts have almost overlapping spectra in both experiment and computations. Two peaks are observed in the experimental UV spectrum of 11_Al (trans-W–Al₂, Fig. 10-left) while the computed one displays just one. A second, considerably red-shifted peak is visible in the computed spectrum at wavelengths greater than 750 nm (Fig. S97†). An analysis of the Natural Transition Orbitals (NTOs) shows, however, that these do not correspond to d–d transitions, but instead to low-lying MLCT transitions from the metal to both nitrogen ligands (Fig. 11). Such low-lying charge transfer transitions had already been identified in a Ru(II) complex⁸⁷ that has, like the compounds studied here, a ligand-based LUMO orbital. Remaining relevant NTOs as well as the calculated peaks and associated difference densities can be found in Fig. S94–S96.†

Fig. 11 NTOs (occupied – bottom, vacant – top) of the 450 nm band of the bare tungsten complex.

Conclusions

This work was motivated by previous results from our groups having thoroughly investigated, experimentally on the one hand, the coordination of tris(pentafluorophenyl)borane, BCF, to formally zerovalent group 6 bis(dinitrogen) complexes supported with phosphine ligands, and computationally on the other hand, the influence of LA binding to a dinitrogen ligand. This combined experimental/theoretical study explores similar chemistry employing tris(pentafluorophenyl)alane, AlCF. The shift to a structurally comparable but more Lewis acidic species led to the isolation of related 1 : 1 adducts of an extensive family of dinitrogen complexes, including a chromium-based and monophosphine-based ones that could not be selectively formed when BCF was employed. A notable difference on the structural point of view is the linear N–N–Al vs. bent N–N–B motif that is explained by steric repulsion between the C₆F₅ groups with the ethyl substituents of the phosphines built up as a result of longer Al–C bonds.

Unlike BCF, AlCF makes robust two-fold μ-N₂ adducts with the bis(dinitrogen) complexes. They form with an initial trans arrangement that evolves in solution to a more stable cis one with a rate depending on the metal (Cr > Mo > W). To the best of our knowledge, these compounds are the first examples of trinuclear heterometallic complexes formed by Lewis acid–base interaction exhibiting p and d elements. Among the handful of N₂-bridged trinuclear heterobimetallic species^88–98 of general formula M₁(μ-N₂)M₂(μ-N₂)M₁ (M₁ = Cr,⁸⁹ Mo,^95–97 Re,⁹² Fe,⁹³ Co;^{90,91,93,94,98} M₂ = Na,⁹⁵ Mg,^{90,91,93–95,97,98} Ti,⁸⁹ Zr,^92,96 V,⁹⁶ Fe⁹⁶), many are based on a low diversity of metal/metal couples, typically on magnesium/early transition metals pairs, as a result of a formally anionic dinitrogen complex formed by reduction with an alkaline or alkaline-earth metal. For the synthesis of d-block-only congeners, a general strategy consists in halide substitution by an electron-rich N₂ ligand, a transformation that accompanies with formal oxidation of the N₂-ligated metal centre concomitant with reduction of N₂. Here, the novelty of our bis(μ-η¹:η¹-N₂–AlCF) specimens resides in the use of a p-block metal that interacts with neutral group 6 N₂ complexes through Lewis acid–base pair formation, through straightforward syntheses (no redox state change, no by-products, and no workup). Note that this synthetic approach parallels a recent work published by Mazzanti and coworkers where they reported the coordination of f-elements (lanthanides and uranium) to an end-on dinitrogen iron complex leading to the formation of N₂ bridged heterobimetallic adducts.⁹⁹ Last but not least, the close proximity of the two activated dinitrogen motifs in these adducts (imparted by their cis-configuration) may pave the way towards new type of N₂ reactivity. DFT calculations show that the diminished level of N₂ activation in these systems, evidenced experimentally by comparison of IR and XRD data to those of the 1 : 1 adducts, can be interpreted by a destabilisation of a σ-symmetric, W–N antibonding component of the W–N–N bonding. While the “bare” N₂ complexes, their 1 : 1 and trans-2:1 Lewis acid adducts have a HOMO of pure d character, in the cis-2:1 adducts this orbital overlaps with a π* orbital of each N₂ ligands. This could result, in terms of reactivity, into a selective reactivity of the N₂ ligands towards electrophiles vs. the metal centre. From the bare [W(depe)₂(N₂)₂] complex to the two-fold aluminium adduct, substantial decrease of the HOMO–LUMO gap is noticed. In particular, the stabilized N₂-centered LUMO should more easily accept electrons, suggesting Lewis acids could be co-activators for (electro) catalysed N₂ reduction.

Electronic spectroscopy was examined for the depe-supported W–N₂ complex and its adducts both experimentally and computationally. This investigation suggests that the nature of the observed absorptions in the visible spectrum is an unusual low-lying MLCT involving N₂-centered orbitals that significantly red-shifts upon LA coordination. This could have important implication for visible light-driven nitrogen fixation, and we are currently exploring the reactivity of LA-adducts of N₂ complexes towards this end.

Data availability

The datasets supporting this article have been uploaded as part of the ESI.† All the computational data have been uploaded (https://www.iochem-bd.org/handle/10/229000) onto the ioChem-BD platform (https://www.iochem-bd.org/) to facilitate data exchange and dissemination, according to the FAIR principles of OpenData sharing.

Author contributions

Conceptualization: A. S.; formal analysis: L. E., L. V., A. C., N. Q.; funding acquisition: A. S., V. K.; investigation L. E., A. C., N. Q., F. M.; methodology: L. E., A. C., N. Q., F. M., V. K., A. S.; project administration: V. K., A. S.; supervision V. K., A. S.; validation: L. E., F. M.; visualization: L. E., F. M.; writing – original draft: L. E., F. M.; writing – review & editing: V. K., A. S.

Conflicts of interest

There are no conflicts to declare.

Acknowledgements

L. E. and A. S. thanks the French Agence Nationale de la Recherche for funding (grant ANR-21-CE07-0003). N. Q. and A. S. are indebted to the European Research Council for funding (ERC Starting Grant no 757501). A. C. is grateful to the French Ministry of National and Superior Education and Research (MENESR) for a PhD fellowship. F. F. M. gratefully acknowledges a Career Bridging Grant from TU Darmstadt. We are grateful to the CNRS (Centre National de la Recherche Scientifique) and the Technische Universität Darmstadt for providing access to facilities, specifically the Lichtenberg II high performance computer at TU Darmstadt on which all calculations for this work were performed.

Notes and references

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Footnote

† Electronic supplementary information (ESI) available: General methods, experimental procedures, NMR spectra, crystallographic and computational details and CIF files. CCDC 2346952–2346961. For ESI and crystallographic data in CIF or other electronic format see DOI: https://doi.org/10.1039/d4sc02713b

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