# Transition Metal Oxides on Reduced Graphene Oxide Nanocomposites: Evaluation of Physicochemical Properties

Authors: Vincenza Modafferi; Saveria Santangelo; Michele Fiore; Enza Fazio; Claudia Triolo; Salvatore Patanè; Riccardo Ruffo; Maria G. Musolino
Journal: Journal of Nanomaterials
 (2019)

---

## Abstract

Transition metal oxides on reduced graphene oxide (TMO@rGO) nanocomposites were successfully prepared via a very simple one-step solvothermal process, involving the simultaneous (thermal) reduction of graphene oxide to graphene and the deposition of TMO nanoparticles over its surface. Texture and morphology, microstructure, and chemical and surface compositions of the nanocomposites were investigated via scanning electron microscopy, X-ray diffraction, micro-Raman spectroscopy, and X-ray photoelectron spectroscopy, respectively. The results prove that Fe2O3@rGO, CoFe2O4@rGO, and CoO@rGO are obtained by using Fe and/or Co acetates as oxide precursors, with the TMO nanoparticles uniformly anchored onto the surface of graphene sheets. The electrochemical performance of the most promising nanocomposite was evaluated as anode material for sodium ion batteries. The preliminary results of galvanostatic cycling prove that Fe2O3@rGO nanocomposite exhibits better rate capability and stability than both bare Fe2O3 and Fe2O3+rGO physical mixture.


---

## Body

## 1. Introduction

Recently, graphene-based nanocomposites have captured considerable attention due to their unique properties and the large variety of possible applications, ranging from sensing and energy storage to heterogeneous, electro-, and photocatalysis [1–6]. Thanks to the striking combination of high specific surface area [7], chemical inertness [8], great mechanical strength [9], and excellent electrical and thermal conductivities [10], the utilization of graphene as an active support framework for functional nanoparticles (NPs) has open promising research areas. Various methods have been developed for the synthesis of graphene, through either chemical or physical routes [3, 11–14]. Among them, chemical oxidation of graphite to graphene oxide (GO), followed by reduction to produce graphene nanosheets, results to be the most appealing due to its low cost, ease, and high yield [8, 15]. GO possesses a considerable fraction of sp3-hybridized carbon atoms, covalently decorated with oxygen-containing functional groups. These oxygen-containing functional groups, including hydroxyl and epoxy groups mainly at basal planes of the carbon sheets and carbonyl and carboxylic groups prevailingly at the edges, provide GO with a remarkable hydrophilic character and chemical reactivity. Furthermore, the oxygen-containing functionalities can act as potential anchoring sites for adsorbing diverse metal oxide NPs [4, 7, 16].Graphite powders represent nowadays the standard anode material for commercial secondary Li+ ion batteries. Recently, many metal oxides have been evaluated as alternative anode materials both in Li+ and Na+ ion batteries (LIBs and SIBs) [17–19]. Among transition metal oxides (TMOs), which store Li+ or Na+ ions via conversion reactions [20], hematite (α-Fe2O3), magnetite (Fe3O4), and spinel cobalt oxide (Co3O4) are attracting great attention, thanks to their high theoretical specific capacities (1007 mAh/g, 926 mAh/g, and 890 mAh/g, respectively) [21–24]. Unfortunately, most of the TMO anodes suffer from limited cycle life as an effect of the large volume changes occurring during the conversion reactions. It is well accepted that graphene is able to buffer the volume expansion/contraction of TMOs in the composites during electrochemical reactions [25–28], thus limiting their pulverisation. Indeed, the iron oxide-rGO composites synthesized via microwave-assisted methods by Zhang et al. [29] taking advantage of the small particle size and the beneficial properties of rGO can deliver up to 300 mAh/g for more than 140 cycles. The specific capacity of ordered nitrogen-doped carbon/γ-Fe2O3 synthesized by Qiang et al. [30] through a multistep approach exceeded 200 mA/g at 100 mA/g (C/10), whereas the iron oxide-rGO composite prepared by the microwave-assisted method by Liu et al. [31] delivered 289 mAh/g at 100 mA/g, remaining stable for 50 cycles.In this work, we report the synthesis of nanostructured composites, consisting of cobalt and/or iron oxide anchored on GO, by the one-step solvothermal approach. The main advantage of this method is that since the reduction of GO to rGO occurs simultaneously to the deposition of the TMO NPs, it does not require the use of any chemical-reducing agent. Textural, structural, and morphological properties of the nanocomposites are studied by several complementary analysis techniques in view of their possible application as electrode materials in rechargeable batteries. Preliminary results relative to the electrochemical performance of the most promising of them are presented revealing that the carbon oxide nanocomposite shows good electrochemical performance in terms of specific capacity and capacity retention.


## 2. Materials and Methods

### 2.1. Materials

Sodium nitrate (NaNO3, 99.5% purity), sulfuric acid (H2SO4, 95-97% purity), and propylene carbonate (anhydrous, purity≥99.9%) were purchased from Merck. Potassium permanganate (KMnO4, ACS reagent purity≥99.0%), graphite powder (purum, particle size≤0.1 mm), iron (II) acetate (Fe(CH3COO)2, 95% purity), cobalt (II) acetate tetrahydrate (Co(CH3COO)2·4H2O, 99.999% purity), N-methyl-2-pyrrolidone (ACS reagent, 99% purity), sodium perchlorate (NaClO4, ACS reagent, purity≥98%), and fluoroethylene carbonate (99.9% purity) were supplied from Sigma-Aldrich. Hydrochloric acid (HCl, 36% wt) was obtained from Alfa Aesar. Hydrogen peroxide (H2O2, 30% wt) and ethanol 96° were purchased from Carlo Erba Reagents. All the chemicals were used as received without further purification. Distilled water was used throughout the experiments.


### 2.2. Synthesis of Graphene Oxide

Graphene oxide was prepared by exfoliation of graphite powder following a slightly modified Hummers method [32]. In a typical synthesis, 2 g of graphite and 1 g of NaNO3 were mixed with 50 ml of concentrated H2SO4 and stirred in an ice bath. Subsequently, KMnO4 (7 g) was slowly added into the mixture under stirring and cooling. The mixture was stirred for 2 h at 35°C. The temperature was then increased to about 98°C, and distilled water (400 ml) was added followed by a slow addition of 10 ml of H2O2 under stirring. The colour of the suspension turned from brown to yellow. The as-obtained GO was then recovered through centrifugation and thoroughly washed with HCl aqueous solution and with distilled water, in sequence. Finally, the solid was dried at 50°C in a vacuum oven for 2 days. Upon the solvothermal treatment, at 170°C for 3 h (see below), GO thermally reduced to rGO.


### 2.3. Synthesis of TMO/rGO Nanocomposite

The nanocomposites were obtained by the solvothermal treatment sketched in FigureS1. 200 mg of GO was dispersed in 60 ml of ethanol through sonication for 2 h. Then, 10 ml of a 0.2 M solution of Fe(CH3COO)2 or of Co(CH3COO)2·4H2O was added. The reaction mixture was stirred at 80°C for 10 h and, subsequently, was transferred in a Teflon beaker and sealed in a stainless steel autoclave for the solvothermal treatment at 170°C for 3 h. The resulting product was centrifuged, washed with ethanol and distilled water for several times, and then dried in air. A nanocomposite based on mixed metal oxides on GO was also prepared (the molar ratio of the Fe/Co precursors was 1 : 1). For comparison purposes, Fe2O3 NPs were also synthesized by the same procedure except for the absence of GO.


### 2.4. Material Characterization

The sample texture and morphology were investigated by scanning electron microscopy (SEM). Analysis was performed using a Phenom ProX scanning electron microscope equipped with an energy-dispersive X-ray (EDX) spectrometer.The formation of GO and its subsequent reduction to rGO upon thermal treatment were ascertained by means of X-ray powder diffraction (XRD) and micro-Raman spectroscopy (MRS). The XRD patterns were recorded at RT by using the Niβ-filtered Cu-Kα radiation (λ=0.15404 nm) at 40 kV. Analyses were registered in the 2θ range of 10–80° at a scan speed of 0.5°/min. Diffraction peak identification was performed on the basis of the JCPDS database of reference compounds. MRS analysis was carried out in air at room temperature. Raman scattering from the samples excited by an Nd:YAG laser operating at 532 nm (2.33 eV) aligned to a confocal microscope (NTEGRA-Spectra SPM from NT-MDT) and equipped with a 100x objective. A very low laser power (250 μW at the sample surface) was used in order to avoid local heating of the samples and annealing effects.The crystalline phase of the oxide was identified via XRD and MRS analyses. Surface composition of the samples and chemical environment of the component species were investigated by X-ray photoelectron spectroscopy (XPS). Spectra were acquired using a K-Alpha system of Thermo Scientific, equipped with a monochromatic Al-Kα source (1486.6 eV) and operating in a constant analyzer energy (CAE) mode with a pass energy of 50 eV for high-resolution spectra and a spot size of 400 μm. The binding energy shifts were calibrated keeping the C 1s position fixed at 284.5 eV. Identification and quantification of the surface species were carried out by decomposing the high-resolution photoelectron spectra of C 1s, O 1s, Fe 2p, and Co 2p core levels. The elemental concentrations were estimated from the areas under the photoelectron peaks weighed by the relative sensitivity factors. The results obtained are reported in Table S1.


### 2.5. Electrochemical Testing

Galvanostatic cycling with potential limitation (GCPL) was carried out with the Bio-Logic VSP-300 multichannel potentiostat/galvanostat on two-electrode coin cells CR2032 assembled in an argon-filled glove box (MBraun), with sodium acting both as counter and reference electrodes. The working electrode for galvanostatic cycling was prepared mixing Fe2O3@rGO composite, the carbon matrix (Super P, MM Carbon), and the polymer binder (polyacrylic acid Mw ~450,000, Sigma-Aldrich) in the weight ratio 8 : 1 : 1, respectively. A second electrode was made by using a physical mixture of Fe2O3 powder and rGO (Fe2O3+rGO) as an active material. For this purpose, Fe2O3 powder and rGO, synthesized separately, were mixed in the same ratio as Fe2O3@rGO nanocomposite. Finally, a third electrode was prepared by adding a higher carbon black content to bare Fe2O3 in order to obtain a comparable total carbon content with respect to the other electrodes. The conductive carbon matrix used in the preparation of the electrode was pretreated at 800°C under argon atmosphere, to remove the adsorbed water and impurities, reducing the typical irreversibility that occurs during the first charge and discharge in such systems [22]. The slurry obtained suspending the solid in N-methyl-2-pyrrolidone solvent was casted onto a copper foil using the doctor blade technique and subsequently dried at 80°C under vacuum overnight. The working electrode was then roll pressed, and 16 mm diameter disks were punched out. The load of active material was about 1 mg/cm2. The electrolyte was a 1 M solution of NaClO4 in anhydrous propylene carbonate with a 2% wt fluoroethylene carbonate additive. The GCPL tests were performed between 0.01 V and 3.00 V vs. Na/Na+ at different C-rates.


## 2.1. Materials

Sodium nitrate (NaNO3, 99.5% purity), sulfuric acid (H2SO4, 95-97% purity), and propylene carbonate (anhydrous, purity≥99.9%) were purchased from Merck. Potassium permanganate (KMnO4, ACS reagent purity≥99.0%), graphite powder (purum, particle size≤0.1 mm), iron (II) acetate (Fe(CH3COO)2, 95% purity), cobalt (II) acetate tetrahydrate (Co(CH3COO)2·4H2O, 99.999% purity), N-methyl-2-pyrrolidone (ACS reagent, 99% purity), sodium perchlorate (NaClO4, ACS reagent, purity≥98%), and fluoroethylene carbonate (99.9% purity) were supplied from Sigma-Aldrich. Hydrochloric acid (HCl, 36% wt) was obtained from Alfa Aesar. Hydrogen peroxide (H2O2, 30% wt) and ethanol 96° were purchased from Carlo Erba Reagents. All the chemicals were used as received without further purification. Distilled water was used throughout the experiments.


## 2.2. Synthesis of Graphene Oxide

Graphene oxide was prepared by exfoliation of graphite powder following a slightly modified Hummers method [32]. In a typical synthesis, 2 g of graphite and 1 g of NaNO3 were mixed with 50 ml of concentrated H2SO4 and stirred in an ice bath. Subsequently, KMnO4 (7 g) was slowly added into the mixture under stirring and cooling. The mixture was stirred for 2 h at 35°C. The temperature was then increased to about 98°C, and distilled water (400 ml) was added followed by a slow addition of 10 ml of H2O2 under stirring. The colour of the suspension turned from brown to yellow. The as-obtained GO was then recovered through centrifugation and thoroughly washed with HCl aqueous solution and with distilled water, in sequence. Finally, the solid was dried at 50°C in a vacuum oven for 2 days. Upon the solvothermal treatment, at 170°C for 3 h (see below), GO thermally reduced to rGO.


## 2.3. Synthesis of TMO/rGO Nanocomposite

The nanocomposites were obtained by the solvothermal treatment sketched in FigureS1. 200 mg of GO was dispersed in 60 ml of ethanol through sonication for 2 h. Then, 10 ml of a 0.2 M solution of Fe(CH3COO)2 or of Co(CH3COO)2·4H2O was added. The reaction mixture was stirred at 80°C for 10 h and, subsequently, was transferred in a Teflon beaker and sealed in a stainless steel autoclave for the solvothermal treatment at 170°C for 3 h. The resulting product was centrifuged, washed with ethanol and distilled water for several times, and then dried in air. A nanocomposite based on mixed metal oxides on GO was also prepared (the molar ratio of the Fe/Co precursors was 1 : 1). For comparison purposes, Fe2O3 NPs were also synthesized by the same procedure except for the absence of GO.


## 2.4. Material Characterization

The sample texture and morphology were investigated by scanning electron microscopy (SEM). Analysis was performed using a Phenom ProX scanning electron microscope equipped with an energy-dispersive X-ray (EDX) spectrometer.The formation of GO and its subsequent reduction to rGO upon thermal treatment were ascertained by means of X-ray powder diffraction (XRD) and micro-Raman spectroscopy (MRS). The XRD patterns were recorded at RT by using the Niβ-filtered Cu-Kα radiation (λ=0.15404 nm) at 40 kV. Analyses were registered in the 2θ range of 10–80° at a scan speed of 0.5°/min. Diffraction peak identification was performed on the basis of the JCPDS database of reference compounds. MRS analysis was carried out in air at room temperature. Raman scattering from the samples excited by an Nd:YAG laser operating at 532 nm (2.33 eV) aligned to a confocal microscope (NTEGRA-Spectra SPM from NT-MDT) and equipped with a 100x objective. A very low laser power (250 μW at the sample surface) was used in order to avoid local heating of the samples and annealing effects.The crystalline phase of the oxide was identified via XRD and MRS analyses. Surface composition of the samples and chemical environment of the component species were investigated by X-ray photoelectron spectroscopy (XPS). Spectra were acquired using a K-Alpha system of Thermo Scientific, equipped with a monochromatic Al-Kα source (1486.6 eV) and operating in a constant analyzer energy (CAE) mode with a pass energy of 50 eV for high-resolution spectra and a spot size of 400 μm. The binding energy shifts were calibrated keeping the C 1s position fixed at 284.5 eV. Identification and quantification of the surface species were carried out by decomposing the high-resolution photoelectron spectra of C 1s, O 1s, Fe 2p, and Co 2p core levels. The elemental concentrations were estimated from the areas under the photoelectron peaks weighed by the relative sensitivity factors. The results obtained are reported in Table S1.


## 2.5. Electrochemical Testing

Galvanostatic cycling with potential limitation (GCPL) was carried out with the Bio-Logic VSP-300 multichannel potentiostat/galvanostat on two-electrode coin cells CR2032 assembled in an argon-filled glove box (MBraun), with sodium acting both as counter and reference electrodes. The working electrode for galvanostatic cycling was prepared mixing Fe2O3@rGO composite, the carbon matrix (Super P, MM Carbon), and the polymer binder (polyacrylic acid Mw ~450,000, Sigma-Aldrich) in the weight ratio 8 : 1 : 1, respectively. A second electrode was made by using a physical mixture of Fe2O3 powder and rGO (Fe2O3+rGO) as an active material. For this purpose, Fe2O3 powder and rGO, synthesized separately, were mixed in the same ratio as Fe2O3@rGO nanocomposite. Finally, a third electrode was prepared by adding a higher carbon black content to bare Fe2O3 in order to obtain a comparable total carbon content with respect to the other electrodes. The conductive carbon matrix used in the preparation of the electrode was pretreated at 800°C under argon atmosphere, to remove the adsorbed water and impurities, reducing the typical irreversibility that occurs during the first charge and discharge in such systems [22]. The slurry obtained suspending the solid in N-methyl-2-pyrrolidone solvent was casted onto a copper foil using the doctor blade technique and subsequently dried at 80°C under vacuum overnight. The working electrode was then roll pressed, and 16 mm diameter disks were punched out. The load of active material was about 1 mg/cm2. The electrolyte was a 1 M solution of NaClO4 in anhydrous propylene carbonate with a 2% wt fluoroethylene carbonate additive. The GCPL tests were performed between 0.01 V and 3.00 V vs. Na/Na+ at different C-rates.


## 3. Results and Discussion

### 3.1. Support

The formation of GO from graphite was ascertained by means of XRD (compare patterns a and b in FigureS2). The XRD pattern of GO shows the sharp and characteristic diffraction peak at 2θ=9.5°, corresponding to the (001) reflection of graphene oxide with d-spacing of 0.955 nm. Its 2θ angle position, shifted to lower angles with respect to strong and sharp diffraction (002) of pristine graphite at 26.7°, matches well with the values reported in the literature [15], suggesting that GO sheets are loosely stacked due to the presence of oxygen-containing functional groups (C=O, –COOH, –OH, and C–O–C) between the layer of graphite formed during oxidation. The minor reflection at 42.6° suggests a turbostratic disorder in graphene sheets [33].After the solvothermal treatment, the characteristic peak of GO disappears, confirming the occurrence of the thermal reduction to rGO. A very broad and intense peak around2θ=24.1° and a weaker one around at 2θ=43.2° are detected (pattern c in Figure S2). The latter can be ascribed to the reflection from (100) plane of rGO. The former corresponds to the reflection from (002) plane with a d-spacing value of 0.369 nm. The remarkable decrease of interlayer spacing confirms the removal of most of the oxygen-containing functional groups [34].The results of MRS and XPS analyses confirm the formation of rGO upon solvothermal reaction. The Raman spectra of GO and rGO (FigureS3) are dominated by two intense and broad bands at ~1360 cm–1 (D-band) and ~1590 cm–1 (G-band). The D-band is generated by finite size effects and by lattice defects breaking the translational symmetry of graphitic layers, while the G-band originates from the stretching of C=C pairs and is the fingerprint of the graphitic crystalline arrangement [35]. In the higher frequency region of the spectrum, overtones and combination bands are detected.The D/G integrated intensity ratio (ID/IG) is commonly utilized to monitor the sp2 defect density in the carbon lattice [36]. It enhances from 2.75 in GO to 3.01 in rGO, proving that the density of sp2 carbon defects (the only ones contributing to the D-band intensity [35]) increases at expenses of non-sp2 defects. In addition, the G-band, sensitive to charge transfer, local distortions, and hybridization changes of the C–C bonding [36], downshifts from 1600 cm–1 in GO to 1588 cm–1 in rGO owing to the oxidation degree lowering.The high-resolution photoelectron profiles of the C 1s core levels in GO and rGO (FigureS4) are very different. In both the spectra, the contribution at 284.5 eV binding energy (BE) arises from C=C/C−C bonds in aromatic rings. Contributions ascribed to oxygenated carbon species fall in the 286–290 eV BE range. They include C–O species in phenols and ethers (at 286.1−286.3 eV), C=O species in carbonyls/quinones (at ~287.5 eV), and O–C=O bonds in carboxylic acid and anhydrides and esters (at 288.7−289.3 eV) [36]. As evident, solvothermal treatment brings about a drastic decrease of the C–O and C=O species present on the carbon surface. In addition, the appearance in the HRXPS spectrum of rGO of a weak contribution at 290.5−291.0 eV (shake-up π–π∗ transition [36]), absent in the HRXPS spectrum of GO, indicates the partial restoration of the π network following the release of oxygenated functionalities upon thermal treatment. Finally, Figure S5 compares the morphology of GO support before and after solvothermal reaction. The GO sample shows highly porous agglomerates, while rGO exhibits a structure similar to crumpled and ripped flakes, confirming the reduction of GO.


### 3.2. Nanocomposites

Figure1 displays the morphology of TMO@rGO nanocomposites, resulting from the SEM analysis. As particularly evident in the higher magnification images (Figures 1(d)–1(f)), the TMO NPs are uniformly confined in the wrinkled sheet-like structure of rGO, indicating that TMO NPs are successfully anchored on the graphene flakes during the solvothermal process. The average size of the oxide grains ranges between 45 and 70 nm.Figure 1
SEM images of (a) CoO@rGO, (b) CoFe2O4@rGO, and (c–f) Fe2O3@rGO nanocomposites.
(a)
(b)
(c)
(d)
(e)
(f)Figure2 shows XRD patterns of the investigated TMO@rGO nanocomposites. No typical diffraction peak of GO is observed, proving the successful reduction of GO to rGO during the solvothermal treatment also in the presence of the salt precursor(s). However, due to their low intensity with respect to the diffraction peaks arising from the oxide, no signal from rGO is generally detected. Only in Figure 2(b), the broad peak corresponding to the reflection from (002) graphitic plane is visible at ~25° 2θ angle.Figure 2
XRD patterns of (a) Fe2O3@rGO, (b) CoO@rGO, and (c) CoFe2O4@ rGO nanocomposites.As for the crystalline phase of the TMOs, the formation of hematite is observed when Fe(CH3COO)2 alone is used as a precursor (Figure 2(a)). In fact, the diffraction peaks at 24.1°, 33.2°, 35.8°, 40.9°, 49.5°, 53.9°, 57. 5°, 62.6°, and 64.1° 2θ angles can be indexed to the (012), (104), (110), (113), (024), (116), (122), (214), and (300) crystal planes of the rhombohedral (hexagonal) structure of hematite (JCPDS card no. 33-0664), respectively [37]. The average size of α-Fe2O3 crystallites, evaluated from the main (104) peak of the diffractogram via the Scherrer equation, is 27.2 nm (i.e., smaller than the average grain size estimated from the higher-magnification SEM images), proving the polycrystalline nature of the oxide NPs.When Co(CH3COO)2·4H2O alone is utilized, no evident diffraction peaks are detected in the XRD pattern of the nanocomposite, probably due to the amorphous nature of the oxide formed (Figure 2(b)). Conversely, when both Fe(CH3COO)2 and Co(CH3COO)2·4H2O are used, broad and less sharp reflection peaks at 30.1°, 35.4°, 43.1°, 56.9°, and 62.5° 2θ angles are observed (Figure 2(c)), which, respectively, correspond to the (220), (311), (400), (511), and (440) crystal planes of the cubic spinel structure of cobalt ferrite (CoFe2O4, JCPDS card no. 22-1086) [38]. The results of EDX analysis (Figure S6) confirm the formation of CoFe2O4@rGO: the Fe/Co atomic ratio (~2 : 1) is found to be very close to the stoichiometric ratio of CoFe2O4.Figure3 displays micro-Raman spectra of the investigated nanocomposites. Hematite belongs to the trigonal D3d6 space group symmetry. Normal modes predicted by the factor group analysis include six IR-active vibrations (2A2u+4Eu) and seven Raman-active vibrations (2A1g+5Eg) [39–41]. Actually, six peaks at 224, 244, 293, 407, 496, and 609 cm–1 are detected in the Raman spectrum of bare hematite (Figure 3(a)), corresponding to the A1g1, Eg1, unresolved Eg2-Eg3, Eg4, A1g2, and Eg5 vibration modes, respectively. In addition, a very weak band near 660 cm–1 is observed, due to the presence of surface defects and/or reduced grain size which, relaxing selection rules, render Raman active the IR-active Eu mode [39]. The very intense asymmetric band peaking at ~1315 cm–1 is ascribed to two-phonon scattering or two-magnon scattering [42].Figure 3
Micro-Raman spectra of (a) bare Fe2O3, (b) Fe2O3@rGO, (c) CoO@rGO, and (d) CoFe2O4@rGO nanocomposites.The spectra of TMO@rGO nanocomposites (Figures3(b)–3(d)) are dominated by the D- and G-bands arising from the Csp2 modes of rGO support. In agreement with XRD analysis results, no additional modes are detected in the nanocomposite synthesized by using Co(CH3COO)2·4H2O as a precursor (Figure 3(c)), while the modes of hematite (with the most intense band overlapped to the D-band) are visible in Fe2O3@rGO nanocomposite (Figure 3(b)).Cobalt ferrite with a cubic structure belongs to the space group Fd3m [43, 44]. For the spinel structure, factor group analysis predicts five Raman active phonon modes (A1g+Eg+3T2g). In the spectrum of the CoFe2O4@rGO composite (Figure 3(d)), only three spectral features are visible at ~285, 471, and 683 cm–1, which can be ascribed to the Raman vibration modes of ferrimagnetic CoFe2O4.Figures4 and 5 show the high-resolution photoelectron spectra of the Fe 2p and Co 2p core levels in nanocomposites synthesized by the use of Fe(CH3COO)2 and/or of Co(CH3COO)2·4H2O precursor(s). In the Fe 2p spectra (Figure 4), the binding energy (BE) position and separation of 2p3/2 (710.4 eV) and 2p1/2 (724.0 eV) spin-orbit components and the presence of the corresponding shake-up satellites at 718.9 eV and 733.0 eV indicate that the dominant state of Fe ions is +3 [45]. For the CoFe2O4@rGO composite (Figure 4(b)), the broad band at 710.4 eV may indicate also the presence of some Fe2+ [46]. In the Co 2p spectra (Figures 5), the BE positions of the two spin-orbit components (2p3/2 at 780.6 eV and 2p1/2 at 798.0 eV) with the related shake-up satellites, respectively, at 786.6 eV and 803 eV are indicative of Co ions in the +2 state [47].Figure 4
High-resolution photoelectron spectra of the Fe 2p core levels in (a) Fe2O3@rGO and (b) CoFe2O4@rGO nanocomposites.Figure 5
High-resolution photoelectron spectra of the Co 2p core levels in (a) CoO@rGO and (b) CoFe2O4@rGO nanocomposites.The asymmetry featuring the spectral profile of the Co 2p core level photoelectron spectrum in CoFe2O4@rGO nanocomposite (Figures 5(b)) is indicative of the presence of two nonequivalent bonds of Co ions, typical of CoFe2O4 compounds [47].The indications emerging from XPS analysis allow understanding the lack of oxide-related contributions in the Raman spectrum of CoO@rGO nanocomposite (Figure3(c)). Cobalt oxide exists in two stable forms, Co3O4 and CoO. In Co(II) oxide, characterized by a face-centered cubic crystalline structure, the first-order phonon Raman scattering is forbidden, while the (allowed) second-order is visible in the 1000–1100 cm–1 spectral range as a large band with weak intensity [48]. The very intense D- and G-bands hinder its detection in the spectrum of CoO@rGO nanocomposite.Additional information is inferred from the high-resolution photoelectron spectra of the O 1s core level (FigureS7). Fe2O3@rGO and CoFe2O4@rGO nanocomposites exhibit similar spectral profiles (a and c in Figure S7). The most intense contribution, centered at about 530 eV in both the spectra, corresponds to the O2– typical of Fe2O3 lattice and is compatible with O2− anions in the CoFe2O4 coordination [49]. On the contrary, in CoO@rGO nanocomposite, the O 1s profile (b in Figure S7) is dominated by the contribution due to C=O species in carbonyl and/or carboxylic groups at 532.3 eV [50]. Indeed, in the high-resolution photoelectron spectra of the C 1s core level of CoO@rGO nanocomposite (b in Figure S8), a strong contribution ascribable to carboxylic groups is detected, and the highest O/C atomic ratio (Table S1) pertains to this composite. On the contrary, in Fe2O3@rGO and CoFe2O4@rGO nanocomposites, the carbonaceous support exhibits a higher reduction degree (i.e., lower O/C atomic ratio), as evident from the C 1s photoelectron spectra (a and c in Figure S8).The relative weight of the transition metal oxide (rGO) in the investigated nanocomposites, as estimated on the basis of the XPS compositional analysis (TableS1), is 55.1, 59.3, and 74.1 wt% (44.9, 40.7, and 25.9 wt%) for CoO@rGO, Fe2O3@rGO, and CoFe2O4@rGO, respectively.


### 3.3. Electrochemical Behavior

The results of rate capability tests on bare Fe2O3, Fe2O3@rGO nanocomposite, and Fe2O3+rGO physical mixture are presented in Figure 6. The comparison between their specific capacities demonstrates the beneficial effect of the rGO support, in agreement with the results of other studies [29, 31]. Fe2O3@rGO nanocomposite exhibits a higher specific capacity compared with the bare hematite. Indeed, a first anodic specific capacity of 331.4 mAh/g is registered for the composite, while only 129.2 mAh/g is obtained for bare Fe2O3. However, the high initial specific capacity of the Fe2O3@rGO is not fully reversible, and after 10 cycles at a C/20 rate, the anodic specific capacity becomes 181.4 mAh/g. Nonetheless, in the subsequent cycles, the capacity retention increases, and in the last 10 cycles at a C/20 rate, a highly stable specific capacity of 166.0 mAh/g (40% higher than that for bare Fe2O3) is recovered.Figure 6
(a) Anodic specific capacity and columbic efficiency as a function of the number of cycles, as obtained from the GCPL for electrodes based on bare Fe2O3, Fe2O3@rGO nanocomposite, and Fe2O3+rGO physical mixture. (b) Voltage versus specific capacity for selected cycles of the Fe2O3@rGO nanocomposite.
(a)
(b)The comparison between specific capacities of Fe2O3@rGO nanocomposite and Fe2O3+rGO physical mixture demonstrates the importance of an intimate connection between the carbonaceous support and the oxide anchored on its surface. As a matter of fact, in the first cycles, the specific capacities of Fe2O3@rGO and Fe2O3+rGO are comparable, but at higher rates, the difference becomes more evident. At C/2 and 2C rates, the nanocomposite outperforms the physical mixture. This is particularly evident at the highest rate. At 2C, in Fe2O3+rGO, the specific capacity decreases down to 20 mAh/g, whereas Fe2O3@rGO can still deliver 65 mAh/g. Moreover, when the current is set back to C/20, a better stability of the nanocomposite is registered, which proves its greater ability to buffer the volume changes occurring during the sodiation/desodiation process (i.e., a superior structural stability) with respect to the physical mixture. Although a long-term cycling analysis is still needed, these preliminary results clearly prove that the intimate contact between iron oxide and conductive rGO support, peculiar to the nanocomposite, leads to improved structural stability and, hence, to better rate performance.The low columbic efficiency (CE) that all active materials exhibit in the first cycle is generally attributed to the decomposition of the electrolyte and the formation of the solid electrolyte interface (SEI) [51]. Indeed, by analyzing the first charge/discharge profiles of Fe2O3@rGO (CE=54.3%) presented in Figure 6(b), the process centered at 1.0 V, generally attributed to the SEI formation, appears only during the first sodiation [52].In the next cycles, CE rapidly increases reaching values higher than 99%. Finally, after the first cycle, during the sodiation, a two-step process takes place, which could be assigned to the insertion of sodium in the oxide and the conversion of iron [22, 53]. The results here reported are comparable with what were reported in literature, but the relative low temperature (170°C) and the easy scalability of the one-step hydrothermal synthesis can be surpassingly advantageous.As known from the literature [27, 29, 54], the solvothermal method allows obtaining a uniform and quasi-quantitative distribution of TMO on graphene. Moreover, the TMO to rGO mass ratio, which, as shown by Zhang et al. [29] and by Liu et al. [31], affects the electrochemical performance of the TMO@rGO nanocomposite, can be easily tuned. Finding the optimal TMO to rGO mass ratio for the investigated nanocomposites is out of the aims of the present work, and it might be the subject of a future study. Fe2O3@rGO nanocomposite with optimized Fe2O3 to rGO mass ratio might exhibit improved electrochemical performance with respect to that here presented.


## 3.1. Support

The formation of GO from graphite was ascertained by means of XRD (compare patterns a and b in FigureS2). The XRD pattern of GO shows the sharp and characteristic diffraction peak at 2θ=9.5°, corresponding to the (001) reflection of graphene oxide with d-spacing of 0.955 nm. Its 2θ angle position, shifted to lower angles with respect to strong and sharp diffraction (002) of pristine graphite at 26.7°, matches well with the values reported in the literature [15], suggesting that GO sheets are loosely stacked due to the presence of oxygen-containing functional groups (C=O, –COOH, –OH, and C–O–C) between the layer of graphite formed during oxidation. The minor reflection at 42.6° suggests a turbostratic disorder in graphene sheets [33].After the solvothermal treatment, the characteristic peak of GO disappears, confirming the occurrence of the thermal reduction to rGO. A very broad and intense peak around2θ=24.1° and a weaker one around at 2θ=43.2° are detected (pattern c in Figure S2). The latter can be ascribed to the reflection from (100) plane of rGO. The former corresponds to the reflection from (002) plane with a d-spacing value of 0.369 nm. The remarkable decrease of interlayer spacing confirms the removal of most of the oxygen-containing functional groups [34].The results of MRS and XPS analyses confirm the formation of rGO upon solvothermal reaction. The Raman spectra of GO and rGO (FigureS3) are dominated by two intense and broad bands at ~1360 cm–1 (D-band) and ~1590 cm–1 (G-band). The D-band is generated by finite size effects and by lattice defects breaking the translational symmetry of graphitic layers, while the G-band originates from the stretching of C=C pairs and is the fingerprint of the graphitic crystalline arrangement [35]. In the higher frequency region of the spectrum, overtones and combination bands are detected.The D/G integrated intensity ratio (ID/IG) is commonly utilized to monitor the sp2 defect density in the carbon lattice [36]. It enhances from 2.75 in GO to 3.01 in rGO, proving that the density of sp2 carbon defects (the only ones contributing to the D-band intensity [35]) increases at expenses of non-sp2 defects. In addition, the G-band, sensitive to charge transfer, local distortions, and hybridization changes of the C–C bonding [36], downshifts from 1600 cm–1 in GO to 1588 cm–1 in rGO owing to the oxidation degree lowering.The high-resolution photoelectron profiles of the C 1s core levels in GO and rGO (FigureS4) are very different. In both the spectra, the contribution at 284.5 eV binding energy (BE) arises from C=C/C−C bonds in aromatic rings. Contributions ascribed to oxygenated carbon species fall in the 286–290 eV BE range. They include C–O species in phenols and ethers (at 286.1−286.3 eV), C=O species in carbonyls/quinones (at ~287.5 eV), and O–C=O bonds in carboxylic acid and anhydrides and esters (at 288.7−289.3 eV) [36]. As evident, solvothermal treatment brings about a drastic decrease of the C–O and C=O species present on the carbon surface. In addition, the appearance in the HRXPS spectrum of rGO of a weak contribution at 290.5−291.0 eV (shake-up π–π∗ transition [36]), absent in the HRXPS spectrum of GO, indicates the partial restoration of the π network following the release of oxygenated functionalities upon thermal treatment. Finally, Figure S5 compares the morphology of GO support before and after solvothermal reaction. The GO sample shows highly porous agglomerates, while rGO exhibits a structure similar to crumpled and ripped flakes, confirming the reduction of GO.


## 3.2. Nanocomposites

Figure1 displays the morphology of TMO@rGO nanocomposites, resulting from the SEM analysis. As particularly evident in the higher magnification images (Figures 1(d)–1(f)), the TMO NPs are uniformly confined in the wrinkled sheet-like structure of rGO, indicating that TMO NPs are successfully anchored on the graphene flakes during the solvothermal process. The average size of the oxide grains ranges between 45 and 70 nm.Figure 1
SEM images of (a) CoO@rGO, (b) CoFe2O4@rGO, and (c–f) Fe2O3@rGO nanocomposites.
(a)
(b)
(c)
(d)
(e)
(f)Figure2 shows XRD patterns of the investigated TMO@rGO nanocomposites. No typical diffraction peak of GO is observed, proving the successful reduction of GO to rGO during the solvothermal treatment also in the presence of the salt precursor(s). However, due to their low intensity with respect to the diffraction peaks arising from the oxide, no signal from rGO is generally detected. Only in Figure 2(b), the broad peak corresponding to the reflection from (002) graphitic plane is visible at ~25° 2θ angle.Figure 2
XRD patterns of (a) Fe2O3@rGO, (b) CoO@rGO, and (c) CoFe2O4@ rGO nanocomposites.As for the crystalline phase of the TMOs, the formation of hematite is observed when Fe(CH3COO)2 alone is used as a precursor (Figure 2(a)). In fact, the diffraction peaks at 24.1°, 33.2°, 35.8°, 40.9°, 49.5°, 53.9°, 57. 5°, 62.6°, and 64.1° 2θ angles can be indexed to the (012), (104), (110), (113), (024), (116), (122), (214), and (300) crystal planes of the rhombohedral (hexagonal) structure of hematite (JCPDS card no. 33-0664), respectively [37]. The average size of α-Fe2O3 crystallites, evaluated from the main (104) peak of the diffractogram via the Scherrer equation, is 27.2 nm (i.e., smaller than the average grain size estimated from the higher-magnification SEM images), proving the polycrystalline nature of the oxide NPs.When Co(CH3COO)2·4H2O alone is utilized, no evident diffraction peaks are detected in the XRD pattern of the nanocomposite, probably due to the amorphous nature of the oxide formed (Figure 2(b)). Conversely, when both Fe(CH3COO)2 and Co(CH3COO)2·4H2O are used, broad and less sharp reflection peaks at 30.1°, 35.4°, 43.1°, 56.9°, and 62.5° 2θ angles are observed (Figure 2(c)), which, respectively, correspond to the (220), (311), (400), (511), and (440) crystal planes of the cubic spinel structure of cobalt ferrite (CoFe2O4, JCPDS card no. 22-1086) [38]. The results of EDX analysis (Figure S6) confirm the formation of CoFe2O4@rGO: the Fe/Co atomic ratio (~2 : 1) is found to be very close to the stoichiometric ratio of CoFe2O4.Figure3 displays micro-Raman spectra of the investigated nanocomposites. Hematite belongs to the trigonal D3d6 space group symmetry. Normal modes predicted by the factor group analysis include six IR-active vibrations (2A2u+4Eu) and seven Raman-active vibrations (2A1g+5Eg) [39–41]. Actually, six peaks at 224, 244, 293, 407, 496, and 609 cm–1 are detected in the Raman spectrum of bare hematite (Figure 3(a)), corresponding to the A1g1, Eg1, unresolved Eg2-Eg3, Eg4, A1g2, and Eg5 vibration modes, respectively. In addition, a very weak band near 660 cm–1 is observed, due to the presence of surface defects and/or reduced grain size which, relaxing selection rules, render Raman active the IR-active Eu mode [39]. The very intense asymmetric band peaking at ~1315 cm–1 is ascribed to two-phonon scattering or two-magnon scattering [42].Figure 3
Micro-Raman spectra of (a) bare Fe2O3, (b) Fe2O3@rGO, (c) CoO@rGO, and (d) CoFe2O4@rGO nanocomposites.The spectra of TMO@rGO nanocomposites (Figures3(b)–3(d)) are dominated by the D- and G-bands arising from the Csp2 modes of rGO support. In agreement with XRD analysis results, no additional modes are detected in the nanocomposite synthesized by using Co(CH3COO)2·4H2O as a precursor (Figure 3(c)), while the modes of hematite (with the most intense band overlapped to the D-band) are visible in Fe2O3@rGO nanocomposite (Figure 3(b)).Cobalt ferrite with a cubic structure belongs to the space group Fd3m [43, 44]. For the spinel structure, factor group analysis predicts five Raman active phonon modes (A1g+Eg+3T2g). In the spectrum of the CoFe2O4@rGO composite (Figure 3(d)), only three spectral features are visible at ~285, 471, and 683 cm–1, which can be ascribed to the Raman vibration modes of ferrimagnetic CoFe2O4.Figures4 and 5 show the high-resolution photoelectron spectra of the Fe 2p and Co 2p core levels in nanocomposites synthesized by the use of Fe(CH3COO)2 and/or of Co(CH3COO)2·4H2O precursor(s). In the Fe 2p spectra (Figure 4), the binding energy (BE) position and separation of 2p3/2 (710.4 eV) and 2p1/2 (724.0 eV) spin-orbit components and the presence of the corresponding shake-up satellites at 718.9 eV and 733.0 eV indicate that the dominant state of Fe ions is +3 [45]. For the CoFe2O4@rGO composite (Figure 4(b)), the broad band at 710.4 eV may indicate also the presence of some Fe2+ [46]. In the Co 2p spectra (Figures 5), the BE positions of the two spin-orbit components (2p3/2 at 780.6 eV and 2p1/2 at 798.0 eV) with the related shake-up satellites, respectively, at 786.6 eV and 803 eV are indicative of Co ions in the +2 state [47].Figure 4
High-resolution photoelectron spectra of the Fe 2p core levels in (a) Fe2O3@rGO and (b) CoFe2O4@rGO nanocomposites.Figure 5
High-resolution photoelectron spectra of the Co 2p core levels in (a) CoO@rGO and (b) CoFe2O4@rGO nanocomposites.The asymmetry featuring the spectral profile of the Co 2p core level photoelectron spectrum in CoFe2O4@rGO nanocomposite (Figures 5(b)) is indicative of the presence of two nonequivalent bonds of Co ions, typical of CoFe2O4 compounds [47].The indications emerging from XPS analysis allow understanding the lack of oxide-related contributions in the Raman spectrum of CoO@rGO nanocomposite (Figure3(c)). Cobalt oxide exists in two stable forms, Co3O4 and CoO. In Co(II) oxide, characterized by a face-centered cubic crystalline structure, the first-order phonon Raman scattering is forbidden, while the (allowed) second-order is visible in the 1000–1100 cm–1 spectral range as a large band with weak intensity [48]. The very intense D- and G-bands hinder its detection in the spectrum of CoO@rGO nanocomposite.Additional information is inferred from the high-resolution photoelectron spectra of the O 1s core level (FigureS7). Fe2O3@rGO and CoFe2O4@rGO nanocomposites exhibit similar spectral profiles (a and c in Figure S7). The most intense contribution, centered at about 530 eV in both the spectra, corresponds to the O2– typical of Fe2O3 lattice and is compatible with O2− anions in the CoFe2O4 coordination [49]. On the contrary, in CoO@rGO nanocomposite, the O 1s profile (b in Figure S7) is dominated by the contribution due to C=O species in carbonyl and/or carboxylic groups at 532.3 eV [50]. Indeed, in the high-resolution photoelectron spectra of the C 1s core level of CoO@rGO nanocomposite (b in Figure S8), a strong contribution ascribable to carboxylic groups is detected, and the highest O/C atomic ratio (Table S1) pertains to this composite. On the contrary, in Fe2O3@rGO and CoFe2O4@rGO nanocomposites, the carbonaceous support exhibits a higher reduction degree (i.e., lower O/C atomic ratio), as evident from the C 1s photoelectron spectra (a and c in Figure S8).The relative weight of the transition metal oxide (rGO) in the investigated nanocomposites, as estimated on the basis of the XPS compositional analysis (TableS1), is 55.1, 59.3, and 74.1 wt% (44.9, 40.7, and 25.9 wt%) for CoO@rGO, Fe2O3@rGO, and CoFe2O4@rGO, respectively.


## 3.3. Electrochemical Behavior

The results of rate capability tests on bare Fe2O3, Fe2O3@rGO nanocomposite, and Fe2O3+rGO physical mixture are presented in Figure 6. The comparison between their specific capacities demonstrates the beneficial effect of the rGO support, in agreement with the results of other studies [29, 31]. Fe2O3@rGO nanocomposite exhibits a higher specific capacity compared with the bare hematite. Indeed, a first anodic specific capacity of 331.4 mAh/g is registered for the composite, while only 129.2 mAh/g is obtained for bare Fe2O3. However, the high initial specific capacity of the Fe2O3@rGO is not fully reversible, and after 10 cycles at a C/20 rate, the anodic specific capacity becomes 181.4 mAh/g. Nonetheless, in the subsequent cycles, the capacity retention increases, and in the last 10 cycles at a C/20 rate, a highly stable specific capacity of 166.0 mAh/g (40% higher than that for bare Fe2O3) is recovered.Figure 6
(a) Anodic specific capacity and columbic efficiency as a function of the number of cycles, as obtained from the GCPL for electrodes based on bare Fe2O3, Fe2O3@rGO nanocomposite, and Fe2O3+rGO physical mixture. (b) Voltage versus specific capacity for selected cycles of the Fe2O3@rGO nanocomposite.
(a)
(b)The comparison between specific capacities of Fe2O3@rGO nanocomposite and Fe2O3+rGO physical mixture demonstrates the importance of an intimate connection between the carbonaceous support and the oxide anchored on its surface. As a matter of fact, in the first cycles, the specific capacities of Fe2O3@rGO and Fe2O3+rGO are comparable, but at higher rates, the difference becomes more evident. At C/2 and 2C rates, the nanocomposite outperforms the physical mixture. This is particularly evident at the highest rate. At 2C, in Fe2O3+rGO, the specific capacity decreases down to 20 mAh/g, whereas Fe2O3@rGO can still deliver 65 mAh/g. Moreover, when the current is set back to C/20, a better stability of the nanocomposite is registered, which proves its greater ability to buffer the volume changes occurring during the sodiation/desodiation process (i.e., a superior structural stability) with respect to the physical mixture. Although a long-term cycling analysis is still needed, these preliminary results clearly prove that the intimate contact between iron oxide and conductive rGO support, peculiar to the nanocomposite, leads to improved structural stability and, hence, to better rate performance.The low columbic efficiency (CE) that all active materials exhibit in the first cycle is generally attributed to the decomposition of the electrolyte and the formation of the solid electrolyte interface (SEI) [51]. Indeed, by analyzing the first charge/discharge profiles of Fe2O3@rGO (CE=54.3%) presented in Figure 6(b), the process centered at 1.0 V, generally attributed to the SEI formation, appears only during the first sodiation [52].In the next cycles, CE rapidly increases reaching values higher than 99%. Finally, after the first cycle, during the sodiation, a two-step process takes place, which could be assigned to the insertion of sodium in the oxide and the conversion of iron [22, 53]. The results here reported are comparable with what were reported in literature, but the relative low temperature (170°C) and the easy scalability of the one-step hydrothermal synthesis can be surpassingly advantageous.As known from the literature [27, 29, 54], the solvothermal method allows obtaining a uniform and quasi-quantitative distribution of TMO on graphene. Moreover, the TMO to rGO mass ratio, which, as shown by Zhang et al. [29] and by Liu et al. [31], affects the electrochemical performance of the TMO@rGO nanocomposite, can be easily tuned. Finding the optimal TMO to rGO mass ratio for the investigated nanocomposites is out of the aims of the present work, and it might be the subject of a future study. Fe2O3@rGO nanocomposite with optimized Fe2O3 to rGO mass ratio might exhibit improved electrochemical performance with respect to that here presented.


## 4. Conclusions

In conclusion, transition metal oxides on reduced graphene oxide (TMO@rGO) nanocomposites, consisting of TMO nanoparticles uniformly anchored onto the surface of graphene nanosheets, were successfully synthesized via the one-step solvothermal process and characterized by means of a combination of complementary techniques. Fe2O3@rGO, CoFe2O4@rGO, and CoO@rGO were obtained by using Fe and/or Co acetates as oxide precursors.The results of preliminary tests aimed at evaluating the electrochemical performance of Fe2O3@rGO as anode material for sodium ion rechargeable batteries demonstrate that the intimate contact between the carbonaceous support and the oxide anchored on its surface plays a crucial role. Fe2O3@rGO nanocomposite exhibits better rate capability and stability with respect to both bare Fe2O3 and Fe2O3+rGO physical mixture, as it is able to buffer the volume changes occurring during the sodiation/desodiation process.



---

*Source: 1703218-2019-04-11.xml*