A re-examination of claims of aminoferrocene–graphene-based molecular magnets Open Access

Following reports that graphene oxide (GO) and reduced graphene oxide show weak magnetism at room temperature^1,2 and that GO modified by aminoferrocene (1) shows tunable magnetic properties,³ El-Gendy and co-workers published an article describing colossal superparamagnetic behavior at room temperature of GO⁴ modified by intercalation of aminoferrocene.^5, Figure 1 shows a redrawing⁶ of the published synthesis.⁵ The first step in the synthesis (step 1) is the direct nitration of ferrocene (2) by the nitronium ion—formed in a mixture of concentrated nitric and sulfuric acids—to give nitroferrocene 3. We were surprised by this claim as the direct nitration of 2 to give 3 has long been reported to fail.⁷ Indeed, the authors state that “nitration of ferrocene has been deemed un-attainable,” citing Woodward's classic 1952 paper which explains why direct nitration fails.⁸ The failure of direct nitration is due to the fact that electrophilic aromatic substitutions of 2 fail when the electrophile is also strongly oxidizing, since formation of the ferrocenium ion (2⁺) by oxidation of the iron center from Fe(II) to Fe(III) occurs instead and prevents subsequent substitution.⁹ Consequently alternative, albeit typically low-yielding, synthetic approaches have been developed for 3 that do not rely on direct nitration.^10–12 Intrigued by the authors claims that they were able to produce 3 by direct nitration we decided to attempt to reproduce their methodology.

In the first attempt, we followed the reported experimental and slowly added ferrocene to the HNO₃/H₂SO₄ mixture in an ice bath at 0 °C. CARE! Addition of >10 mg portions at a time led to spontaneous ignition, indeed, as the reaction progressed even addition of this amount led to ignition. Within the first few seconds of the first addition, a blue coloration was observed, consistent with the formation of the ferrocenium ion [2]⁺, followed by a rapid change to green and then the formation of a browny-black mixture which remained throughout the rest of the addition. After ∼50 min, we had added a total of ∼200 mg of ferrocene. After a total of ∼1 h reaction time, the mixture was carefully diluted with water and the organic components were extracted with ethyl acetate. Removal of the solvent from this mixture under reduced pressure gave a low yield (28 mg) of a brown solid. Separately, the aqueous phase was neutralized and then extracted (ethyl acetate) yielding an orange, gum-like residue (21 mg). The colors of the residues are not consistent with formation of nitroferrocene which is purple.¹¹ Neither the ¹H or ¹³C NMR spectra (see the supplementary material, Figs. S2, S3, S5, S6) of the residues are consistent with the reported spectra of nitroferrocene.¹² The absence of nitroferrocene in the first fraction was further indicated by both IR spectroscopy (Fig. S1), which showed no peaks at 1507 cm⁻¹ for the nitro group stretch of nitroferrocene,¹¹ and ESI-MS (Fig. S4) which showed no peaks at m/z = 231 consistent with the anticipated or reported mass spectrum of 3.¹² 

Subsequently, on request, the authors kindly provided further information regarding their methodology that was not available in the publication,¹³ stipulating that the reaction was performed at −80 to −30 °C under an inert atmosphere. Accordingly, in our second attempt, we cooled the HNO₃/H₂SO₄ mixture under a nitrogen atmosphere to −80 °C. This mixture was too viscous to stir at this temperature so we allowed the bath to warm to the point at which stirring could commence (∼−50 to −40 °C) and the bath was then maintained at this temperature for the addition of the ferrocene. In the first attempt, we used a total of 190 mg of ferrocene, which yielded trace amounts (∼4 mg) of precipitated material in contrast with the authors' description that the product forms as a suspension and can be collected and washed.¹³ The rest of the material stayed in solution, the dark blue coloration (see Fig. S10) of which was indicative of the formation of the ferrocenium ion 2⁺. The lack of reasonable amounts of isolable material may have been a consequence of the reduced scale of our attempt. So, for the third attempt, we planned a reaction on the same scale as the authors; unfortunately, the addition of the first portion of ferrocene led to rapid thermal runaway and spontaneous ignition, at which point further attempts to reproduce the purported synthetic protocol(s) or variations on them were abandoned in the interest of safety.

We conclude that, in line with previous investigations,^7,8 the direct nitration of ferrocene by the nitronium ion formed in concentrated H₂SO₄/HNO₃ does not occur, instead the formation of the blue ferrocenium ion 2⁺ is observed, accompanied by decomposition. Consequently, in our hands, and in line with all previous reports, the reaction shown in step 1 of the sequence shown in Fig. 1 fails, and therefore, aminoferrocene 1 cannot be produced by this approach.

Fortunately, compound 1 can be readily made by multiple alternative approaches,¹⁴ or purchased from one of several commercial suppliers. It has been thoroughly spectroscopically, analytically, and structurally characterized and indeed has had its single crystal x-ray structure determined twice.^15,16 We recorded an IR spectrum of a genuine, commercial sample of 1 and this is shown in Fig. S16; comparison with the IR spectrum reported shows that the material described is not 1,⁵ similarly the reported x-ray powder diffraction does not fit that calculated for 1 (Fig. S18, determined using reported x-ray structural data for 1).¹⁶ El-Gendy and co-workers describe the material as being in the oxidized, ferrocenium form 1⁺ where, in direct contrast to the purported first step in Fig. 1, the sulfuric acid present has oxidized the ferrocene center. A personal communication from the authors described the obtained material as brown;^13,17 however, ferrocenium ions would be expected to be typically blue or green. Indeed, a small-scale oxidation of 1 with concentrated H₂SO₄ gave a purple solution (Fig. S12).

In addition to synthetic studies, we were also intrigued by the computational models obtained to explain the reported magnetic phenomena.⁵ Notwithstanding that aminoferrocene is not produced by the synthetic protocols, we undertook a re-examination of the computational findings reported by El-Gendy and co-workers on the nature of the intercalated aminoferrocene-GO material.⁵ 

Modeling GO, as produced by modifications of the Hummers' method,¹⁸ remains challenging. This is not least because of the heterogeneity of the GO structure, which contains hydroxyl, epoxy, and carboxylic acid residues as the oxygenated groups formed during the oxidation of graphite, as captured by the Lerf–Klinowski model.¹⁹ In this model, the carboxylic acid functions tend to localize at the edge of sheets while the rest tend to occur on sp³-hybridised carbons in the basal plane. While the Lerf–Klinowski model has been used to good effect in computational studies,²⁰ it tends to assume a random distribution of oxidized functionalities throughout the structure and this is open to question, not least because disruption of the sp² framework by oxidation means that proximate regions are more prone to subsequent oxidation.²¹ This leads to oxidized islands in otherwise unmodified seas of graphitic structure. Accordingly, more sophisticated models have been developed which capture these features.^22,23

Against this backdrop, a small, highly simplified [C₅₄(OH)₇] precursor model, 5, with protonated epoxy groups as the sole O-containing functions was originally reported to describe the GO and its aminoferrocene adduct.⁵ Specifically, the precursor 5 had 6 protonated epoxy groups sitting over the centers of C₆ rings at the edges of the ring and a 7th sitting over the central C ring [Fig. 2(a)].²⁴ The model was not capped with hydrogen atoms but retained unphysical open shell carbon atoms at its edge.²⁵ Two of these sheets were then arranged on either side of a dication of aminoferrocene [1²⁺; see below for discussion on the likely stability of this Fe(IV) structure] and then the structure was relaxed to give the unusual structure, 6, shown in Fig. 2(b) with two free hydroxy radicals between 1²⁺ and the two GO sheets. The two GO layers bulge away from the aminoferrocene/hydroxyl radical region, hinting that the magnetic properties might be modulated by varying pressure.⁵ Importantly, partial electron-transfer from the Fe center to the free hydroxy radicals appears to account for the metalization of the material and attendant magnetic properties.⁵ Free hydroxy radicals will not be present in the GO as prepared by the modified Hummers' method since these would have been removed during work-up or would have long since reacted directly with the GO.²⁶ Therefore, if they are indeed present in the intercalated structure, they presumably result from interaction of the GO layer with the intercalating aminoferrocene. We tested this hypothesis using the precursor model 5 previously described⁵ and subjecting it to geometry optimization in isolation (PBE-d3bj/def2-TZVP). This led to extrusion of the central hydroxy radical (along with the migration of the remaining six hydroxyls to the periphery), as shown in Fig. 2(c).²⁷ This demonstrates that the extrusion of the free hydroxy radicals is simply an artifact resulting from the unphysical nature of the starting model 5.²⁸ 

It is possible that the calculated bulging of the GO layers observed in Fig. 2(b) is a function of the presence of the aminoferrocene moiety; indeed, this was suggested by El-Gendy and co-workers.⁵ Accordingly we modeled the interaction of aminoferrocene with optimized GO layers in the absence of free hydroxyl radicals. Geometry optimization [PBE-d3bj/def2-SVP(def2-TZVP on Fe)] of three models (6—^IS8; IS = intermediate spin) with intercalated 1, 1⁺, or 1²⁺ [Fe(II), Fe(III), and Fe(IV); Figs. 2(d)–2(f), respectively] gave structures that clearly show no bowing of the GO layers. Instead, the structures are largely unremarkable, formed by π-stacking of the cyclopentadienyl rings of the aminoferrocene moieties with the GO layers (see the supplementary material). Separately, we also modeled both (i) chemically more realistic²⁹ hydrogenated version of 6 and 7 with H atoms added to the peripheral carbons (9 and 10, respectively) and (ii) the effect of changing spin-state in 8. Neither modification had a profound effect on the overall structure of the species obtained (see the supplementary material).

It should be noted that when modeling varying oxidation states on ferrocenes, appropriate care must be spent on questioning the chemical likelihood of a given oxidation state under the conditions described. Looking at the oxidation states of the putative intercalating aminoferrocenes, 1 and 1⁺ are chemically reasonable under the conditions described by El-Gendy and co-workers,⁵ but the dication 1²⁺ is not. Ferrocene dications are remarkably rare due to their inherent extreme reactivity. To date, the only crystallographically characterized Fe(IV) ferrocene is [Fe(C₅Me₅)₂]²⁺,^30,31 which is extremely air- and moisture-sensitive and rapidly decomposes in organic solvents. Indeed, it can only be prepared and handled in anhydrous SO₂ and is produced by the oxidation of [Fe(C₅Me₅)₂] with powerful oxidizing agents, such as AsF₅, SbF₅, and ReF₆. No such potent oxidizing agents are present in the system reported by El-Gendy and co-workers:⁵  1²⁺ would be highly unlikely to form under their conditions³² and even if it did, it would not subsequently survive the reported reaction media.

In conclusion, inspired by the work of El-Gendy and co-workers, we have re-examined key synthetic and computational aspects of their claims. We conclude that while the material produced by the authors may well display the interesting magnetic properties claimed, it is clearly not the material the authors claim it to be. Furthermore, the interesting results obtained by El-Gendy and co-workers in their computational studies are unfortunately simply a result of chemical artifacts brought about as a consequence of the choice of starting model employed.

See the supplementary material for details of experimental procedures; spectroscopic details; computational methodology; and xyz coordinates of calculated structures.

The authors gratefully acknowledge the UK Catalysis Hub for resources and support provided via our membership of the UK Catalysis Hub Consortium and funded by EPSRC Grant Nos. EP/R026939/1, EP/R026815/1, EP/R026645/1, EP/R027129/1, or EP/M013219/1 (biocatalysis). This work was carried out using the computational facilities of the Advanced Computing Research Centre, University of Bristol—http://www.bristol.ac.uk/acrc/.

The authors have no conflicts to disclose.

Gayathri Athavan: Conceptualization (supporting); Investigation (equal); Methodology (equal); Writing – original draft (supporting); Writing – review & editing (supporting). François-Xavier Coudert: Conceptualization (supporting); Writing – original draft (supporting); Writing – review & editing (supporting). Robin B. Bedford: Conceptualization (lead); Data curation (lead); Funding acquisition (lead); Investigation (equal); Methodology (equal); Project administration (lead); Supervision (lead); Validation (equal); Visualization (equal); Writing – original draft (lead); Writing – review & editing (lead).

The data that support the findings of this study are available within the article and its supplementary material. In addition, the xyz coordinate files for the calculated structures are also available at the University of Bristol data repository, data.bris, at https://doi.org/10.5523/bris.mz85vyusop082j481j2ddl1rf.