# N-centered, yet persistent: isolation of N 2 O-based radicals through FLP-type stabilization

Andrea Orellana Ben Amor, Laure Vendier, Vincent César, Vincent Maurel, Julien Panetier, Nicolas Queyriaux

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Andrea Orellana Ben Amor, Laure Vendier, Vincent César, Vincent Maurel, Julien Panetier, et al. N-centered, yet persistent: isolation of N 2 O-based radicals through FLP-type stabilization. Chemical Science, 2025, 17 (4), pp.2140 - 2147. 10.1039/d5sc08152a. hal-05506586

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Cite this: *Chem. Sci.*, 2026, 17, 2140

All publication charges for this article have been paid for by the Royal Society of Chemistry

Received 21st October 2025

Accepted 25th November 2025

DOI: 10.1039/d5sc08152a

rsc.li/chemical-science

# N-centered, yet persistent: isolation of N₂O-based radicals through FLP-type stabilization

Andrea Orellana Ben Amor, IDª Laure Vendier, IDª Vincent César, IDª Vincent Maurel, ID*b Julien Panetier, ID*c and Nicolas Queyriaux ID*a

The electrochemical one-electron reduction of IDipp·N₂O (IDipp = 1,3-bis(2,6-diisopropylphenyl) imidazol-2-ylidene) is inherently irreversible, highlighting the short-lived nature of the corresponding radical anion. However, stabilization by Lewis acidic boranes enables electrochemically reversible behavior, unlocking access to persistent radical species. These radicals are synthesized *via* chemical reduction and fully characterized, revealing a highly N-centered nature alongside remarkable persistence at room temperature under an inert atmosphere. A comprehensive investigation of their electronic structure is presented, integrating electron paramagnetic resonance techniques (both continuous-wave and pulsed) with theoretical analysis to provide deeper insight into their properties.

## Introduction

N-heterocyclic carbenes (NHCs) have recently emerged as powerful molecular tools capable of stabilizing N-centered radicals.¹⁻⁴ Through a combination of both steric protection and π-accepting properties, NHCs greatly limit the reactivity of the radicals, typically resulting in persistent derivatives. In this context, a series of NHC-stabilized aminyl radicals has been isolated by the Severin group (Scheme 1A).⁵ Those radicals – stable under an inert atmosphere – are characterized by a significant localization of the spin density of the unpaired electron (ca. 41%) on one of the nitrogen atoms of the diazenyl group. Open-shell diradicals, bridged by a permethylated biphenyl unit, were similarly isolated (Scheme 1B). When exposed to air, these diradicaloid derivatives were found to be significantly less stable than their monoradical analogues. This was attributed to increased steric congestion, which limits the coplanarity of the diazenyl units with the adjacent arene ring, thereby accounting for low electron delocalization. Related tri-azenyl radicals were also synthesized by the Lee group (Scheme 1C).⁶ Although displaying a greater N-centered character (ca. 55%), the spin density of the radical is, again, computed to be significantly delocalized throughout the molecule.

Further stabilization of a radical species may also be achieved through the combined use of NHCs and Lewis acid partners, employing a Frustrated Lewis Pair (FLP) approach, which provides increased steric protection and electronic

delocalization. Hence, Lee and co-workers demonstrated that the stabilization of an iminoxyl radical induced by a NHC alone was insufficient, resulting in progressive decomposition in solution.⁷ Conversely, a redox-active FLP system was recently reported to split NO through single electron oxidation.⁸ A dramatic increase in stability was achieved upon reaction with tris(pentafluorophenyl)borane (1ª), with the resulting zwitter-ionic radical displaying remarkable stability towards both air and moisture (Scheme 1D and E).⁹

In γ-radiolysis, nitrous oxide (N₂O) has been used for a long time as a chain transfer agent, facilitating the increased generation of hydroxyl radicals in water.¹⁰,¹¹ While undoubtedly involved in the process, the N₂O⁻ radical anion has never been experimentally evidenced. A notable result in this context was the *in situ* EPR characterization of a silyl-stabilized N₂O radical – embedded on a SiO₂ surface – by the group of Radtsig.¹² From this perspective, it is therefore appealing to deploy NHC-based strategies that have proven successful in stabilizing related

<figure><img src="image_3.png" /><figcaption>Scheme 1 Molecular structures of NHC-stabilized N-centered radicals.</figcaption></figure>

<footnote>ªUniv. Toulouse, CNRS, LCC, Toulouse, France. E-mail: nicolas.queyriaux@lcc.toulouse.fr</footnote>

<footnote>ᵇUniv. Grenoble Alpes, CEA, CNRS, IRIG, SyMMES, 38000 Grenoble, France. E-mail: vincent.maurel@cea.fr</footnote>

<footnote>Department of Chemistry, State University of New York at Binghamton, Binghamton, NY 13902, USA. E-mail: panetier@binghamton.edu</footnote>
<figure><img src="image_4.png" /></figure>

aminyl and iminoxyl radicals to the N₂O motif. Interestingly, the group of Severin reported the preparation of NHC·N₂O adducts that may serve as convenient entry points in such an approach.¹³⁻¹⁵ Although they display a rich and diverse chemistry,¹⁶⁻²¹ their redox behavior remains virtually unexplored to date.

Here, we report the preparation of new FLP-type adducts of N₂O varying in the nature of their Lewis acid partners. Examination of their redox behavior specifically highlights the remarkable persistence of the corresponding radical anions. Accordingly, such radicals were isolated and fully characterized. A specific focus has been dedicated to elucidating the electronic structures of these species through the use of electron paramagnetic resonance techniques and theoretical investigations. The aminyl nature of the N₂O-based radical is evidenced, with a high degree of N-centered character.

## Results and discussion

Adducts 3ª⁻ᶜ were synthesized through a two-step synthetic route. 1,3-Bis(2,6-diisopropylphenyl)-2H-imidazol-2-ylidene (IDipp) was initially exposed to N₂O following a reported procedure to produce the stable IDipp·N₂O adduct 2 (Scheme 2).¹³,¹⁴ Subsequent reactions with selected boranes (1ª⁻ᶜ) were carried out in dichloromethane at room temperature, resulting in the formation of adducts 3ª⁻ᶜ in yields exceeding 80%. The relative Lewis acid strengths of these boranes were assessed using the Gutmann–Beckett method, employing triethylphosphine oxide (Et₃PO) as the Lewis base probe (refer to the SI for more details).²² When normalized to tri(s(pentafluorophenyl)borane (B(C₆F₅)₃), 1ª: 100%), the values obtained for 1ᵇ⁻ᶜ reveal the selected boranes to cover a significant range of Lewis acidity (1ᵇ: 85%, 1ᶜ: 57%).

Compounds 3ª⁻ᶜ display spectroscopic signatures similar to related species.¹⁷,¹⁹ More specifically, the formation of adducts diagnostically influences chemical shifts of the imidazolium backbone protons. In the ¹H NMR spectra, the corresponding singlet indeed experiences strong deshielding in comparison to the parent IDipp·N₂O compound (2: 7.25 ppm, 3ª: 7.99 ppm, 3ᵇ: 7.78 ppm, 3ᶜ: 7.70 ppm). As the Lewis acid becomes stronger, an enhanced weight of the diazotate mesomeric form is expected in the hybrid structure of the corresponding adducts (Scheme 2). As a result, the resonance of the backbone protons is progressively shifted downfield, in line with an increased aromatic character. For comparison purposes, the 2-phenyl imidazolium analogue, 4·BF₄ (1,3-bis(2,6-diisopropylphenyl)-2-

<figure><img src="image_5.png" /><figcaption>Scheme 2 Synthesis of the IDipp·N₂O·BAr₃ compounds 3ª⁻ᶜ.</figcaption></figure>

phenylimidazolium tetrafluoroborate), whose aromaticity is unambiguous, exhibits signals for these same protons at a value of 8.52 ppm. In the ¹³C{¹H} NMR spectra, the resonances for the carbene carbon atom of 3ª⁻ᶜ are in the region of δ = 144–148 ppm, in good agreement with previous findings.¹⁷,¹⁹ ¹¹B{¹H} NMR spectra display sharp resonances at close-to-zero δB values, confirming the expected tetrahedral geometry around the boron atom. When present, signals of the fluorine atoms lying on the phenyl groups of the boranes are observed at chemical shifts consistent with adduct formation.

X-ray quality crystals were grown from THF/pentane solutions, allowing for X-ray diffraction analysis of all three compounds 3ª⁻ᶜ. In all cases, the resulting structures confirm the coordination of the borane moiety to the IDipp·N₂O adduct 2 (Fig. 1). The relevant bond lengths and angles for compounds 3ª⁻ᶜ are summarized in Table 1, together with a comparison with the parent compound 2.¹³

In detail, the N₂O motif adopts a bent geometry with its proximal nitrogen atom connected to the NHC carbon atom and its oxygen atom linked to the borane group. The N–N–O angles are in the range of 108–109°, thus showing increased bending compared to 2 (112.9°). Interestingly, the nature of the borane slightly – but coherently – influences the N–N–O angle: the stronger the Lewis acid is, the more bent the motifs are. As a general trend, the N=N bonds tend to contract in 3ª⁻ᶜ (1.27–1.28 Å) compared to 2 (1.35 Å), while the N–O bonds are elongated (1.30–1.32 Å in 3ª⁻ᶜ vs. 1.25 Å in 1). Such a bond length inversion aligns well with the results obtained other FLP-type adducts of N₂O.¹⁷,¹⁹,²³,²⁴ Upon increased acidity of the borane partner, enhanced coplanarity of the N₂O motif and the heterocycle is accessed: the solid angle formed by the mean planes associated with these two motifs is indeed shifting from 39.08° in 2 to 19.80, 23.55 and 35.35° for 3ª⁻ᶜ, respectively.

To gain further insight into the electronic structures of compounds 3ª⁻ᶜ, we conducted DFT calculations. Initial geometry optimizations were performed using the ωB97X-D²⁵ functional in solution (tetrahydrofuran, ε = 7.4257) with the SMD approach (see the SI for more details).²⁶ A good agreement was typically found between the X-ray and DFT geometries, with the most significant error being an underestimation of the N1–O1 bond distances by an average of 2.8% (Table S2). We note that, as observed experimentally, the computed N–N–O bond angle increases across the series in going from 3ª (110.7°) to 3ᶜ (111.0°), consistent with 3ª featuring the strongest Lewis acid borane moieties. Inspection of the frontier molecular orbitals in this series of compounds reveals that the lowest unoccupied molecular orbitals are primarily localized on the N₂O motif (see SI), suggesting that the one-electron reduced species will yield a N₂O-centered radical.

We then investigated the electrochemical behaviour of compounds 3ª⁻ᶜ, along with the parent compound 2, using cyclic voltammetry (CV). In dry THF (containing 0.1 M n⁶Bu₄PF₆ as the supporting electrolyte), 2 exhibits two irreversible one-electron processes at Eₚ,ᶜ = -2.86 V vs. Fc⁺/Fc and Eₚ,ᵃ = +0.68 V vs. Fc⁺/Fc (Fig. 2, green trace). Despite attempts to increase the scan rate (up to 1000 mV s⁻¹) or decrease the temperature (down to 5 °C), redox reversibility could not be
<figure><img src="image_6.png" /></figure>

<figure><img src="image_7.png" /><figcaption>Fig. 1 Molecular structures of 3ª (left), 3ᵇ (centre) and 3ᶜ (right), as determined by X-ray diffraction. Thermal ellipsoids shown at the 50% probability level. Hydrogen atoms and solvent molecules were omitted for sake of clarity.</figcaption></figure>

<table><caption>Table 1 Selected bond lengths and angles for compounds 2 and 3a–c</caption><thead><tr><th></th><th>2<sup>13</sup></th><th>3a</th><th>3b</th><th>3c</th></tr></thead><tbody><tr><td>N1–N2 (Å)</td><td>1.352(4)</td><td>1.283(2)</td><td>1.284(2)</td><td>1.277(2)</td></tr><tr><td>N1–O1 (Å)</td><td>1.250(4)</td><td>1.317(2)</td><td>1.313(2)</td><td>1.310(1)</td></tr><tr><td>B1–O1 (Å)</td><td>—</td><td>1.537(3)</td><td>1.551(2)</td><td>1.593(2)</td></tr><tr><td>C1–N2 (Å)</td><td>1.358(4)</td><td>1.374(3)</td><td>1.374(2)</td><td>1.376(2)</td></tr><tr><td>N2–N1–O1 (°)</td><td>112.9(3)</td><td>108.0(2)</td><td>108.4(1)</td><td>109.1(1)</td></tr></tbody></table>

<figure><img src="image_8.png" /><figcaption>Fig. 2 Cyclic voltammograms of compounds 2 (green trace), 3ª (blue trace), 3ᵇ (red trace) and 4·BF₄ (dark grey trace), recorded in THF (0.1 M nBu₄NPF₆) at a glassy carbon electrode (analyte concentration: 1 mM, scan rate: 100 mV s⁻¹).</figcaption></figure>

achieved, even to a limited extent. Such a result suggests that the *in situ* electrogenerated radical is highly unstable and further evolves in solution. Interestingly, dramatic differences were observed when recording the CVs of compounds 3ª and 3ᵇ (Fig. 2, blue and red traces, respectively). In both cases, a single quasi-reversible process was observed to occur at strongly anodically-shifted potentials of −1.70 and −1.93 V vs. Fc⁺/Fc, for 3ª and 3ᵇ, respectively. The borane moiety thus appears to have a dual effect: (i) by providing an increased steric hindrance and a partial electronic density delocalization, it firstly results in increased kinetic stability of the radical, ultimately leading to

full reversibility recovery, and (ii), the decreased electronic density of the NHC·N₂O moiety simultaneously lowers the energy required to initiate electron transfer from the electrode, resulting in the observed anodic shift. As a result, the potential required can be tuned by the nature of the Lewis acid partner, as evidenced by the 230 mV gain in potential when switching from the partially fluorinated borane 1ᵇ to the perfluorinated one 1ª. Noteworthy, a similar beneficial effect of the addition of a Lewis-acidic borane was reported very recently in the one-electron reduction of NHC·CO₂ adducts.²⁷ Linear trends were observed when plotting the variation of the anodic and cathodic peak currents (iₚ,a and iₚ,c) of the electrochemical process versus the square root of the scan rate (from 100 mV s⁻¹ to 1000 mV s⁻¹, see SI), confirming the compounds to freely diffuse in solution. Meanwhile, the CV of 3ᶜ suggests that the Lewis acidity of the borane 1ᶜ is insufficient to achieve efficient stabilization of the associated radical species. An irreversible process was indeed observed, similar to parent compound 2 (see SI). Interestingly, the 2-phenyl imidazolium 4⁺ displays a reversible one-electron process at a similar potential of −2.18 V vs. Fc⁺/Fc (Fig. 2, dark grey trace). As previously investigated by the Ghadwal group,²⁸ the unpaired electron density of the resulting neutral radical was found to be partially located on the carbene carbon atom, with significant contributions from the carbon atoms of the aryl rings. This prior work thus questions the spin distribution in Lewis-acid stabilized radical anions [3ª⁻ᵇ·]⁻, and more specifically, the extent of their delocalization.

To specifically address this point, we decided to synthesize the radical anions corresponding to the reduction of 3ª and 3ᵇ. Encouraged by the reversible electrochemical behaviour of those compounds on the CV timescale, we thus turned our attention to their preparative chemical reduction. Notably, one-electron reduction using potassium graphite (KC₈) in dry tetrahydrofuran enabled the isolation of the desired species in reasonable yields (>50%), as dark red solids. The structures of [K][3ª⁻] and [K][3ᵇ⁻] were confirmed by single-crystal X-ray diffraction (Fig. 3, together with relevant bond lengths and angles summarized in Table 2). Upon comparison with the parent neutral compounds, notable modifications are identified. Increased bending of the N–N–O angles is observed, with
<figure><img src="image_9.png" /><figcaption>Fig. 3 Molecular structures of [K][3ª⁻] (left), [K][3ᵇ⁻] (centre) and [K][3ᶜ⁻] (right), as determined by X-ray diffraction. Thermal ellipsoids shown at the 50% probability level. Hydrogen atoms were omitted for sake of clarity.</figcaption></figure>

<table><caption>Table 2 Selected bond lengths and angles for compounds [K][3ª⁻]</caption><thead><tr><th></th><th>[K][3ª⁻]</th><th>[K][3ᵇ⁻]</th><th>[K][3ᶜ⁻]</th></tr></thead><tbody><tr><td>N1-N2 (Å)</td><td>1.354(3)</td><td>1.340(4)</td><td>1.359(3)</td></tr><tr><td>N1-O1 (Å)</td><td>1.412(4)</td><td>1.400(3)</td><td>1.392(3)</td></tr><tr><td>B1-O1 (Å)</td><td>1.488(3)</td><td>1.493(4)</td><td>1.525(4)</td></tr><tr><td>C1-N2 (Å)</td><td>1.316(4)</td><td>1.312(4)</td><td>1.315(4)</td></tr><tr><td>N2-N1-O1 (°)</td><td>103.2</td><td>103.7</td><td>102.9</td></tr></tbody></table>

values as low as 103.2° in [3ª⁻]⁻. To the best of our knowledge, it is one of the most acute angles reported for this structural motif so far, excluding cyclic derivatives.²⁹⁻³² Meanwhile, the elongation of both the N-N and N-O bonds in the N₂O motif is observed. The N-N bonds are observed in the range 1.34–1.35 Å in [3ª⁻]⁻ and [3ᵇ⁻]⁻, which are typically halfway between single and double bonds and thus suggest an overall bond order of 1.5. As for the N-O bonds, they range from 1.40 to 1.41 Å, consistent with single bond character. Conversely, contraction of the B-O and CₙHₙ-N bonds is observed, suggesting increased interactions within the FLP-type adducts that may account for the observed persistence of the radicals. A significant change in the structural features of these radicals lies in the increased coplanarity of the N₂O motif and the imidazolium ring: the dihedral angles associated with these two moieties shift from 19.80° and 23.55° in 3ª⁻ᵇ⁻ to 5.6° and 2.5° for [3ª⁻]⁻ and [3ᵇ⁻]⁻, respectively. Similarly observed in radicals based on NHC–CO₂-borne adducts,²⁷ this overall flattening probably arises from increased conjugation within the radical.

Interestingly, preparative one-electron reduction of 3ᶜ under identical conditions allowed the isolation of a few dark red crystals. Suitable for X-ray diffraction, they allowed the characterization of the molecular structure of [K][3ᶜ⁻] (Fig. 3). No particular structural differences were noticed when compared with [K][3ª⁻] and [K][3ᵇ⁻]. At first glance, this result may seem somewhat puzzling, as it is inconsistent with the electrochemical data that support a low-stability radical. We suspect, however, that the potassium cation derived from the reduction using KC₈ plays a significant role in the stabilization of the radical. Mougel's group recently demonstrated that the presence of Lewis acidic alkali cations (K⁺, Rb⁺, Cs⁺) is an effective

strategy for stabilizing low-valent iron-sulfur cubanes.³³ We believe that a similar scenario is at play here, with K⁺ supplementing the limited Lewis acidity of BPh₃.

Electron Paramagnetic Resonance (EPR) techniques were then used to gain further experimental insights into the electronic structure of the radicals [3ª⁻]⁻ and [3ᵇ⁻]⁻ (Fig. 4). The continuous wave (cw) EPR spectrum of [3ᵇ⁻]⁻, recorded at room temperature, exhibits three main features separated by 37.1 MHz (1.32 mT), consistent with the strong isotropic hyperfine coupling computed by DFT (Aᵢₐ₉,ₐ₉₉ = 29.1 MHz) for the N1 nucleus. Each main feature of the cw-EPR exhibits 7 lines separated by 3–5 MHz and additional shoulders. To better identify such smaller couplings, the HYSCORE spectrum of [3ᵇ⁻]⁻ was recorded at 70 K. In the left quadrant, two pairs of features are observed at [±5.00; ±8.71] and [±4.70; ±2.45] MHz. Their position and shape correspond to those expected for the double quantum/double quantum and double quantum/single quantum transitions of a nitrogen nucleus having a mainly isotropic hyperfine interaction (weak values of T tensor components compared to Aᵢₐ₉). In this case, the hyperfine Aᵢₐ₉ and quadrupolar K constants can be computed using the analysis developed by Dikanov and the relationship:³⁴

$$v_{dq\pm} = 2[v_{eff\pm}^2 + K^2(3 + \eta^2)]^{1/2}$$

with

$$v_{eff\pm} = |v_{14N} \pm \frac{a}{2}|$$

This analysis provides hyperfine coupling of Aᵢₐ₉,ₐ₉₉ = 5.9 MHz and a quadrupolar interaction in the range 0.81 < K < 0.93 (in MHz), in very good agreement with the values computed by DFT (Aᵢₐ₉,ₐ₉₉ = -5.4 MHz, Kₐ₉₉ = 0.87 MHz) for N2 (Table 3). In the right quadrant two very intense features are observed at [±4.71; ±2.44] MHz. They are typical of nitrogen nuclei with hyperfine coupling constants close to the so-called cancellation condition: A/2 ~ v(¹⁴N) (nuclear Larmor frequency for ¹⁴N, 1.07 MHz at 3460 G). These signals can be attributed to the N3 and N4 nuclei, as determined by DFT computations, since it is clear that, for some orientations of [3ᵇ⁻]⁻ vs. magnetic field, the hyperfine couplings of these nuclei fulfill the cancellation

<figure><img src="image_10.png" /></figure>
<figure><img src="image_11.png" /></figure>

<figure><img src="image_12.png" /><figcaption>Fig. 4 EPR spectra of $[^{3}\text{a}^{\cdot}]^{-}$ and $[^{3}\text{b}^{\cdot}]^{-}$, in solution at room temperature, together with their corresponding numerical simulations (left) and HYSCORE spectrum of $[^{3}\text{b}^{\cdot}]^{-}$ recorded at $T = 70$ K (right).</figcaption></figure>

condition. However, the pronounced anisotropic character of the hyperfine tensors of N3 and N4 predicted by DFT computations (see the higher values of *T* tensors for N3 and N4 compared with N2 in Table 3), does not allow the use of the same quantitative analysis as for the N2 nucleus. The last two features are observed centered on the diagonal at 1.6 MHz and 4.8 MHz, which can be attributed, respectively, to the $^{10}\text{B}$ and $^{11}\text{B}$ isotopes of the boron nucleus. The signal centered at 4.8 MHz extends over a range of ~3-4 MHz in the antidiagonal direction, in good agreement with the small and anisotropic hyperfine interaction computed by DFT for this $^{11}\text{B}$ nucleus (Table 3). Noteworthy, no significant signal was observed that could be attributed to $^{1}\text{H}$ or $^{19}\text{F}$ nuclei, beyond a weak signal close to the diagonal at 14.7 MHz, corresponding to very small hyperfine couplings (<2 MHz; see full scale spectrum in the SI).

Moreover, the experimental room-temperature cw-EPR spectrum can be numerically simulated (Easyspin software package), considering only the isotropic hyperfine coupling of N1, N2, N3, N4 and B nuclei. The agreement between the numerically fitted and the experimental spectrum is excellent. The $A_{\text{iso}}$ values extracted from this simulation match reasonably well those computed by DFT, which, in addition to the HYSCORE experiment, further validates experimentally the electronic structure of $[^{3}\text{b}^{\cdot}]^{-}$ calculated by DFT.

EPR and HYSCORE investigations of the radical $[^{3}\text{a}^{\cdot}]^{-}$ yielded very similar results. The HYSCORE spectrum is similar to that of $[^{3}\text{b}^{\cdot}]^{-}$ (see SI). The EPR spectrum of $[^{3}\text{a}^{\cdot}]^{-}$ recorded at

room temperature is less resolved than the spectrum of $[^{3}\text{b}^{\cdot}]^{-}$, but careful numerical simulation leads to very similar hyperfine coupling constants in good agreement with DFT computations. As expected, the plot of the Mulliken spin density for the one-electron reduced species indicates that most of the electron density is localized on the $N_{2}\text{O}$ moiety (e.g., $\rho(N_{2}\text{O}) = 0.71$,

<figure><img src="image_13.png" /><figcaption>Fig. 5 (A) Isosurface (0.007 au) plot of the Mulliken spin population of the one-electron reduced species $[^{3}\text{a}^{\cdot}]^{-}$. Hydrogen atoms have been omitted for clarity. (B) Corresponding Lewis representation of the aminyl radical $[^{3}\text{a}^{\cdot}]^{-}$.</figcaption></figure>

<table><caption>Table 3 EPR parameters (in MHz) of $[^{3}\text{a}^{\cdot}]^{-}$ and $[^{3}\text{b}^{\cdot}]^{-}$ obtained by numerical simulation of spectra shown in Fig. 4 and comparison with DFT-computed ones</caption><thead><tr><th></th><th></th><th>N1</th><th>N2</th><th>N3</th><th>N4</th><th>B</th><th>Linewidth</th></tr></thead><tbody><tr><td rowspan="2">[^3a<sup>•</sup>]<sup>-</sup></td><td>A<sub>iso,exp</sub> (A<sub>iso,DFT</sub>)</td><td>36.8 (28.7)</td><td>EPR 4.3 (−4.4)<br>HYSCORE 5.9</td><td>3.6 (4.0)</td><td>4.1 (4.3)</td><td>1.4 (−3.7)</td><td>4.7</td></tr><tr><td>T<sub>DFT</sub><br>K<sub>exp</sub> (K<sub>DFT</sub>)</td><td>[-29.3 −30.5 59.8]<br>n.m. (1.13)</td><td>[2.8 −0.7 −2.1]<br>0.81 &lt; K &lt; 0.93 (0.86)</td><td>[-4.4 −4.6 9.0]<br>n.m. (−1.13)</td><td>[-4.1 −3.8 7.9]<br>n.m. (−1.14)</td><td>[2.7 −1.2 −1.5]<br>n.m. (0.04)</td><td></td></tr><tr><td rowspan="2">[^3b<sup>•</sup>]<sup>-</sup></td><td>A<sub>iso,exp</sub> (A<sub>iso,DFT</sub>)</td><td>37.1 (28.7)</td><td>EPR 4.6 (−5.3)<br>HYSCORE 5.9</td><td>3.8 (3.8)</td><td>4.5 (4.4)</td><td>1.7 (4.1)</td><td>3.4</td></tr><tr><td>T<sub>DFT</sub><br>K<sub>exp</sub> (K<sub>DFT</sub>)</td><td>[-29.3 −30.4 59.7]<br>n.m. (1.11)</td><td>[1.2 0.1 −1.3]<br>0.81 &lt; K &lt; 0.93 (0.86)</td><td>[-4.2 −4.4 8.6]<br>n.m. (−1.15)</td><td>[-4.0 −3.6 7.6]<br>n.m. (−1.15)</td><td>[2.8 −1.3 −1.5]<br>n.m. (0.06)</td><td></td></tr></tbody></table>
<figure><img src="image_14.png" /></figure>

Fig. 5A), in agreement with the EPR properties. We also note that the frontier molecular orbitals for [3a']- indicate that the highest occupied molecular orbital, which is located in the α-space, involves a π* orbital on the N₂O moiety, consistent with the experimentally observed elongation of both the N–N and N–O bonds. Taken together, structural information, spectroscopic data and DFT calculations all point towards the reduced species being best described as aminyl radicals (Fig. 5B).

Interestingly, we found that the radical anion [3a']- exhibits remarkable weeks-long persistence in solution at room temperature under an inert atmosphere (as determined by cw-EPR measurements compared to a TEMPO control). In contrast, exposure to oxygen leads to immediate re-oxidation to the neutral adduct 3ª, likely *via* an outer-sphere electron transfer mechanism. While extended stability has been reported for structurally related radicals, it remains surprising in this case due to the strongly N-centered character of the radical, which is typically associated with short-lived, highly reactive species.

These results, therefore, point to an important kinetic stabilization capable of balancing the thermodynamic drivers typically associated with strongly localized organic radicals.³⁵ The effective steric protection of the spin density provided by the highly congested molecular environment of our radicals is most probably responsible for this stabilization.

## Conclusions

In summary, we report the synthesis, isolation and full characterization of the first molecular examples of N₂O-based radical anions. Access to these species, best described as aminyl-type radicals, was enabled by a FLP-type strategy combining N-heterocyclic carbenes with boron-based Lewis acids. Electrochemical studies demonstrated that the nature and strength of the Lewis acid partner directly influence both the redox properties and the stability of the resulting radicals. A combination of cw-EPR spectroscopy, HYSCORE experiments and DFT calculations, confirmed that the spin density is primarily localized on the central nitrogen atom, yielding a highly N-centered radical. Remarkably, despite this localization, the radicals display significant persistence in solution under inert atmosphere – a feature attributed to the substantial steric protection afforded by the surrounding molecular environment.

## Author contributions

The manuscript was written through contributions of all authors. All authors have given approval to the final version of the manuscript.

## Conflicts of interest

There are no conflicts to declare.

## Data availability

CCDC 2440410 to 2440415 contain the supplementary crystallographic data for this paper.⁶⁰a–f

The authors have also cited additional references within the supporting information (SI).³⁶⁻⁵⁹ The data supporting this article (detailed synthetic procedures, NMR/IR/Raman spectra, additional EPR measurements, computational details and radical persistence assessment) have been included as part of the SI. Supplementary information is available. See DOI: https://doi.org/10.1039/d5sc08152a.

## Acknowledgements

Dr Dmitry Valyaev is kindly acknowledged for providing compound 4·BF₄. NMR Spectroscopy Service (A. Bonnet) from the Laboratoire de Chimie de Coordination is acknowledged for technical assistance with NMR experiments. Dr Baptiste Martin is acknowledged for preliminary EPR experiments. Marine Tassé is acknowledged for Raman spectroscopy measurements. Dr Alix Sournia-Saquet is gratefully acknowledged for granting access to the electrochemistry facility at LCC. Dr Sébastien Bontemps is thanked for fruitful discussions. N. Q. would like to thank the CNRS and the ANR (grant ANR-24-CE07-5771-01) for financial support. A. O. B. acknowledges funding from the University of Toulouse for her PhD fellowship. Financial support from the IR INFRANALYTICS FR2054 for conducting the research is similarly gratefully acknowledged. This material is also based upon work supported by the National Science Foundation under Grant No. CHE-2400072.

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60 (a) CCDC 2440410: Experimental Crystal Structure Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxfxx; (b) CCDC 2440411: Experimental Crystal Structure Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxfxx
Edge Article

Chemical Science

Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxfyy; (c)

CCDC 2440412: Experimental Crystal Structure

Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxfzz; (d)

CCDC 2440413: Experimental Crystal Structure

Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxg01; (e)

CCDC 2440414: Experimental Crystal Structure

Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxg12; (f)

CCDC 2440415: Experimental Crystal Structure

Determination, 2025, DOI: 10.5517/ccdc.csd.cc2mxg23.

<figure><img src="image_16.png" /></figure>