# Production of Reduced Graphene Oxide Platelets from Graphite Flakes Using the Fenton Reaction as an Alternative to Harmful Oxidizing Agents

Authors: Jean A. V. Piñas; Tatiana S. Andrade; Andreia T. Oliveira; Pedro E. A. Salomão; Mariandry Rodriguez; Adilson C. Silva; Henrique S. Oliveira; Douglas S. Monteiro; Márcio C. Pereira
Journal: Journal of Nanomaterials
 (2019)

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## Abstract

The conventional chemical methods to produce graphene using strong oxidizing agents produce toxic gases during synthesis; therefore, these methods do not meet the principles of green chemistry. In this work, an alternative top-down method for the synthesis of a few layers of graphene sheets has been produced by a Fenton reaction- (a mixture of Fe2+/H2O2) assisted exfoliation process in water using graphite flakes as a starting material. Based on X-ray diffraction data and Fourier transform infrared (FTIR), Raman spectroscopy, and transmission electron microscopy measurements, it is proposed that the oxidation of graphite by Fenton chemistry facilitates the exfoliation of graphene sheets under mild sonication. Subsequent chemical reduction with ascorbic acid produced a few layers of reduced graphene oxide. Compared to Hummers’ method, the Fenton reagent has similar exfoliation efficiency, but due to the Fenton reagent’s preference to react with the edges of graphite, the chemical reduction can lead to the formation of less defective reduced graphene oxides. Moreover, since Fe and H2O2 are cheap and environmentally innocuous, their use in large-scale graphene production is environmentally friendlier than conventional methods that use toxic oxidizing agents.


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## Body

## 1. Introduction

Graphene is a two-dimensional (2D) graphitic structure which is the basic unit for making graphitic materials of other dimensionalities such as 0D fullerene, 1D carbon nanotube, or 3D graphite [1]. Because of its exceptional electronic, thermal, and mechanical properties [2–4], graphene has been investigated in several fields of science including catalysis [5–7], adsorption [8–10], electrocatalysis [11, 12], energy storage [13–15], and sensors [16, 17].Graphene is commonly synthesized by top-down methods using graphite as a precursor [18–26]. By this method, graphite is first converted into graphite oxide (GO) by strong oxidizing agents. This is generally exemplified by Hummers’ method (a mixture of KMnO4, NaNO3, and H2SO4) [27] or modified Hummers’ methods [28–31]. Dichromate and potassium chlorate in fuming nitric acid have also been used as oxidizing agents to produce GO [32, 33]. Then, GO can be converted into graphene oxide sheets by exfoliation and subsequently into graphene by reduction treatment using different methods such as thermal, chemical, or photocatalytic reduction [34–36].The disadvantages of using conventional oxidizing agents for chemical exfoliation of graphite by Hummers’ method or potassium chlorate is the generation of toxic gases such as NO2, N2O4, and ClO2, which are profoundly harmful to the environment; therefore, they are unsuitable for large-scale green production of graphene. Recently, Agarwal et al. [37] reported a promising approach to produce a few layers of graphene by chemical exfoliation with Fenton chemistry. However, the use of organic solvent in the exfoliation process by sonication makes the process less green according to the principles of green chemistry [38].In this work, we report an alternative aqueous route to prepare reduced graphene oxide (RGO) from graphite flakes using the Fenton reaction (Fe2+/H2O2) as an oxidizing agent. By this method, graphite is first oxidized by the Fenton reagent to produce graphite oxide. Then, graphite oxide is exfoliated by sonication and reduced by ascorbic acid to form RGO. Although the liquid waste from this synthesis contains H2SO4, the use of the Fenton reaction is attractive because Fe and H2O2 are environmentally innocuous, H2O2 activation takes place at room temperature and under atmospheric pressure, and the chemical reactions do not generate toxic gases. Moreover, the standard reduction potential of the •OH radicals (Eɵ=2.80V) is higher than those of permanganate (Eɵ=1.51V) and dichromate (Eɵ=1.33V), which are the most commonly used oxidizing agents for this purpose. Therefore, from a chemistry viewpoint, the graphene sheets and their derivatives should also react with the hydroxyl radicals generated by the Fenton reaction.


## 2. Materials and Methods

### 2.1. Material Synthesis

Graphite oxide was prepared from expandable graphite (G), with an average flake size smaller than 300μm, using a mixture of Fe2+/H2O2 as an oxidant. In short, 0.2500 g of graphite was mixed with 10 mL of 0.1 M FeSO4⋅7H2O aqueous solution. Then, 1 mL of 98% H2SO4 was added to the Fe2+/graphite suspension, which was kept in an ice bath under constant stirring for 12 h. Then, 1 mL of 30% H2O2 aqueous solution was added over about 5 h with constant stirring at room temperature. The solid was separated from the reaction mixture by filtration, washed several times with deionized water and hot HCl/H2O2 to remove residual ions, and dried at room temperature. This sample was named GO(F). The resultant GO(F) was then readily resuspended in deionized water and sonicated at 40°C for 2 h. Then, the obtained suspension was centrifuged at 4000 rpm and the solid discarded to obtain a supernatant with a few layers of graphene oxide. The well-dispersed graphene oxide was finally reduced by ascorbic acid to form a few layers of reduced graphene oxide (RGO(F)). Subsequently, the mixture was centrifuged at 4000 rpm for 30 min to obtain a stable dispersion of RGO(F). The low-density material suspended at the top layer of the centrifuged solution was collected for further characterization. By this method, 0.3822 g of RGO(F) was produced from 0.2500 g of graphite. The steps for the RGO(F) preparation are shown in Figure 1. For comparison, the same procedure was repeated using Hummers’ method to obtain reduced graphene oxide. Hummers’ method produced 0.3321 g of RGO(H) from 0.2500 g of graphite.Figure 1
Steps for the preparation of a few layers of reduced graphene oxide from graphite flakes.


### 2.2. Materials Characterization

Powder X-ray diffraction (XRD) measurements were carried out at room temperature using a Rigaku Geigerflex diffractometer equipped with a graphite diffracted-beam monochromator. The data were collected in a 2θ range of 10° to 70° using Cu-Kα radiation (λ=1.5418Å), with an acceleration voltage of 40 kV, acceleration current of 20 mA, and scan speed of 1°/min. Fourier transform infrared (FTIR) spectra were obtained with a Nicolet 360 FTIR spectrometer equipped with a Smart OMNI sampler with a germanium crystal. Transmission electron microscopy (TEM) was performed on a JEOL JEM-2100F field emission transmission electron microscope with an accelerating voltage of 200 kV. The Raman spectra were obtained with a Senterra Raman microscope spectrometer (Bruker, HR800 Labram I, Horiba Jobin Yvon) with an excitation wavelength of 633 nm. The samples were focused with a 100x lens, and the spectra were obtained using a 20 s integration time, five coadditions, and 3.5 cm−1 resolution. To prevent heat-induced phase changes via the excitation source while the Raman spectra were being collected, a line focus was utilized producing a line shape for the excitation source at the sample surface with a dimension of 25 × 1000 μm and using a laser power of 1 mW. Thermogravimetric analysis (TGA) was performed on a TG/DTA thermogravimetric analyzer (PerkinElmer Thermal Analysis).


## 2.1. Material Synthesis

Graphite oxide was prepared from expandable graphite (G), with an average flake size smaller than 300μm, using a mixture of Fe2+/H2O2 as an oxidant. In short, 0.2500 g of graphite was mixed with 10 mL of 0.1 M FeSO4⋅7H2O aqueous solution. Then, 1 mL of 98% H2SO4 was added to the Fe2+/graphite suspension, which was kept in an ice bath under constant stirring for 12 h. Then, 1 mL of 30% H2O2 aqueous solution was added over about 5 h with constant stirring at room temperature. The solid was separated from the reaction mixture by filtration, washed several times with deionized water and hot HCl/H2O2 to remove residual ions, and dried at room temperature. This sample was named GO(F). The resultant GO(F) was then readily resuspended in deionized water and sonicated at 40°C for 2 h. Then, the obtained suspension was centrifuged at 4000 rpm and the solid discarded to obtain a supernatant with a few layers of graphene oxide. The well-dispersed graphene oxide was finally reduced by ascorbic acid to form a few layers of reduced graphene oxide (RGO(F)). Subsequently, the mixture was centrifuged at 4000 rpm for 30 min to obtain a stable dispersion of RGO(F). The low-density material suspended at the top layer of the centrifuged solution was collected for further characterization. By this method, 0.3822 g of RGO(F) was produced from 0.2500 g of graphite. The steps for the RGO(F) preparation are shown in Figure 1. For comparison, the same procedure was repeated using Hummers’ method to obtain reduced graphene oxide. Hummers’ method produced 0.3321 g of RGO(H) from 0.2500 g of graphite.Figure 1
Steps for the preparation of a few layers of reduced graphene oxide from graphite flakes.


## 2.2. Materials Characterization

Powder X-ray diffraction (XRD) measurements were carried out at room temperature using a Rigaku Geigerflex diffractometer equipped with a graphite diffracted-beam monochromator. The data were collected in a 2θ range of 10° to 70° using Cu-Kα radiation (λ=1.5418Å), with an acceleration voltage of 40 kV, acceleration current of 20 mA, and scan speed of 1°/min. Fourier transform infrared (FTIR) spectra were obtained with a Nicolet 360 FTIR spectrometer equipped with a Smart OMNI sampler with a germanium crystal. Transmission electron microscopy (TEM) was performed on a JEOL JEM-2100F field emission transmission electron microscope with an accelerating voltage of 200 kV. The Raman spectra were obtained with a Senterra Raman microscope spectrometer (Bruker, HR800 Labram I, Horiba Jobin Yvon) with an excitation wavelength of 633 nm. The samples were focused with a 100x lens, and the spectra were obtained using a 20 s integration time, five coadditions, and 3.5 cm−1 resolution. To prevent heat-induced phase changes via the excitation source while the Raman spectra were being collected, a line focus was utilized producing a line shape for the excitation source at the sample surface with a dimension of 25 × 1000 μm and using a laser power of 1 mW. Thermogravimetric analysis (TGA) was performed on a TG/DTA thermogravimetric analyzer (PerkinElmer Thermal Analysis).


## 3. Results and Discussion

The powder X-ray diffraction patterns of G, GO, and RGO synthesized by Fenton’s and Hummers’ methods are presented in Figure2. The XRD data confirm the hexagonal graphitic structure of the carbon materials according to the JCPDS # 8-415 (Figures 2(a) and 2(c)). It is worth noting that the XRD pattern of expandable graphite (G) exhibits a (002) basal plane with d002 spacing at 0.335 and 0.340 nm (Figure 2(b)), suggesting that the precursor had not expanded efficiently. The XRD pattern of sample GO(F) (Figures 2(a) and 2(b)) shows the 002 basal plane of graphite similar to that of sample G, except for the higher relative intensity ratio of d0.340/d0.335 for sample GO(F) (1.7) compared to that of sample G (1.3), suggesting that the Fenton oxidation caused some structural defects in the graphene sheets of graphite [39–41]. Also, the oxidation of graphene sheets led to the disappearance of the (100), (101), and (110) planes in sample GO(F) due to the loss of sp2 carbon rings caused by the functionalization of the graphene sheets with oxygenated groups. The XRD pattern of sample RGO(F) shows that the (002) basal plane of graphite has shifted to the d-spacing value of 0.343 nm, while the (002) plane at d=0.335nm utterly disappeared, suggesting a loss of the long-range order in graphene sheets due to the exfoliation process [39–41]. Notoriously, the (100), (101), and (110) planes were restored after the reduction of the oxidized graphene sheets by ascorbic acid, suggesting that the sp2 carbon rings have been restored. The XRD patterns of GO(H) and RGO(H) obtained by Hummers’ method (Figures 2(c) and 2(d)) were quite similar to those obtained by the Fenton method. The (002) basal plane of graphite had shifted to a d spacing of 0.342 nm, which is close to the expansion of the graphene sheets obtained with the Fenton method.Figure 2
Powder XRD patterns and expanded XRD region for the (002) crystallographic plane of G, GO, and RGO samples obtained by (a, b) the Fenton method and (c, d) Hummers’ method.
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(d)The functional groups generated by Fenton oxidation of graphene sheets were evaluated by FTIR (Figure3). The broad bands in the range of 3600–3400 cm−1 are due to the vibrations of water molecules. The bands at around 2995 cm−1 correspond to symmetric stretching vibrations of -CH2. In the GO(F) and GO(H) sample, the band at 2870 cm−1 is due to antisymmetric stretching vibrations of -CH2. Intense bands at 1660 and 1330 cm−1 are due to C=O and C-O stretching vibrations of the -COOH groups. These bands were more intense in the spectra of GO(F) and GO(H) samples, suggesting that graphite oxide is highly oxidized and consists mainly of -OH and other oxygenated functional groups. The intensities of the C=O, C-O, and -OH functional groups were greater in the GO(F) than in the GO(H) sample, indicating that the Fenton reaction was more effective in generating COOH and -OH in the graphene sheets of graphite than Hummers’ reagent. Interestingly, the intensities of the C=O and -OH bands decreased after chemical reduction with ascorbic acid, indicating a partial removal of those functional groups to restore the sp2 carbon rings. Indeed, the reappearance of -CH2 groups at 2995 cm−1 in the spectra of RGO(F) and RGO(H) confirms the restoration of sp2 carbon in the graphene sheets. Based on that, it is suggested that the C-O groups mainly occupy the basal planes while the -COOH and -OH groups are mostly found at the edges. Therefore, the C=O and -OH groups can be more easily reduced by ascorbic acid than the C-O groups.Figure 3
FTIR spectra of G, GO, and RGO samples obtained by (a) the Fenton method and (b) Hummers’ method.
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(b)The successful oxidation and exfoliation of graphite oxide were further verified by Raman spectroscopy. The Raman spectrum of carbon materials presents two main features, theD band at approximately 1350 cm−1 and the G band at around 1580 cm−1. The D band is due to defect-mediated zone-edge phonons near the k point in the Brillouin zone, and the G band is due to the first-order scattering of the E2g phonon of sp2 C atoms. Thus, the intensity ratio of the D and G bands (ID/IG ratio) can be used to estimate the number of defects in carbon materials. For an increasing number of defects, sp2 domains (G band) become smaller, and the intensity of the D band increases. Therefore, high ID/IG ratio values indicate the high functionalization degree of graphene sheets in carbon materials [42]. The Raman spectra of samples G, GO(F), and RGO(F) are shown in Figure 4(a). The spectra of all samples indicated two remarkable bands at around 1336 and 1581 cm−1, which correspond to the D and G bands, respectively. The ID/IG ratio for sample G (Figure 4(a)) was 0.42, indicating that this graphite precursor is highly defective. After the oxidation of graphite by the Fenton reaction, the ID/IG ratio in sample GO increased significantly to 0.64, suggesting the oxidation of graphene sheets in the graphitic structure, as also verified by FTIR. Hence, the Fenton chemistry can efficiently be used to weaken the van der Waals interactions of graphene layers, enabling the delamination of graphite by sonication. Indeed, the exfoliation/reduction of graphite oxide restores the sp2 network of graphene sheets and decreases the ID/IG ratio to 0.21, suggesting that sample RGO(F) has less structural defects than its precursors. Furthermore, the D′ band (1623 cm−1), usually reported for disordered graphitic lattices such as those introduced by heteroatoms, increases with the oxidation treatment and decreases upon the exfoliation/reduction procedure, confirming that RGO(F) has less structural defects than the G and GO samples. The error for the calculated ID/IG ratio is 0.05.Figure 4
Raman spectra of samples G, GO, and RGO obtained by (a) the Fenton method and (b) Hummers’ method.
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(b)For comparison, the graphite flakes were previously oxidized by Hummers’ method followed by ultrasonication and reduction with ascorbic acid to produce reduced graphene oxide. The Raman spectra (Figure4(b)) showed that the ID/IG intensity ratio of graphite oxidized (GO(H)) by Hummers’ reagent was 0.47 while that obtained after Fenton oxidation was 0.64, suggesting that under the studied conditions the Fenton method was more efficient in oxidizing graphite than Hummers’ method. After reduction, the ID/IG intensity ratio of RGO(H) decreased to 0.28, while the reduction of RGO obtained by the Fenton method was 0.21. It has been demonstrated that the Fenton reagent oxidizes the edges of graphite preferentially [37], and therefore, the reduction of graphite obtained from the Fenton route is more readily reduced than that obtained by Hummers’ method.Figures5(a)–5(c) show the TEM images of samples G, GO(F), and RGO(F). Figures 5(a)–5(c) show that all the samples have the morphology of platelets. Figure 5(c) confirms that the Fenton oxidation favors the delamination of graphene layers from graphite by mild ultrasound. The EDX data for the RGO(F) (Figure 5(d)) present only signals of C, O, S, and Cu. S is due to the ferrous sulfate, and Cu is the support for the RGO. No signal of Fe was identified by EDX, suggesting that HCl/H2O2 was efficient in completely removing iron from the graphene sheets. HRTEM analysis (Figure 5(e)) displays a close-to-ideal crystalline-reduced graphene oxide that consists of 6 layers with a d002 spacing of 0.33 nm. It was noted from Figure 5(f) that the previous Fenton oxidation of a graphite precursor is essential for obtaining a few layers of reduced graphene oxide. If the Fenton oxidation of graphite is not previously performed, an RGO with multiple layers is obtained. Figure 5(g) shows the morphology of the RGO(H) obtained by Hummers’ method, which resulted in approximately 8 layers of reduced graphene oxide (Figure 5(h)), suggesting that the exfoliation by the Fenton method is comparable to that of Hummers’ method.Figure 5
TEM images of samples (a) G, (b) GO(F), and (c) RGO(F) obtained by the Fenton method. (d) EDX data for the RGO(F) sample. (e) HRTEM image of the RGO(F) sample. (f) TEM image of the RGO sample obtained without the previous oxidation treatment by the Fenton reaction. (g) TEM image of RGO(H) obtained by Hummers’ method. (h) HRTEM image of the RGO(H) sample.
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(h)The thermal stability of RGO obtained by Fenton’s and Hummers’ method using thermogravimetric analysis (TGA) is shown in Figure6. For both samples, the small mass loss around 100°C is due to the loss of adsorbed water. RGO(F) shows a gradual mass loss from 400 to 800°C due to the oxidation of carbon. For RGO(H), the mass loss takes place from 700 to 800°C, indicating that RGO(H) is thermally more stable than RGO(F) probably due to its higher number of graphene layers. Also, at 800°C the mass loss achieved 100%, confirming that iron was removed entirely from the graphene sheets in the RGO(F) sample.Figure 6
TGA profile for the RGO obtained by Fenton’s and Hummers’ method.


## 4. Conclusions

A convenient method for producing a few layers of reduced graphene oxide by the previous oxidation of graphite with a Fenton reagent was demonstrated. The Fenton chemistry takes advantage of the high oxidizing power of hydroxyl radicals, which can attack the graphene sheets of graphite, thus favoring its exfoliation with ultrasound to obtain a few layers of reduced graphene oxide. The efficiency of graphite delamination was similar to that obtained with Hummers’ method, but because the Fenton chemistry oxidizes the edges of graphite preferentially, further chemical reduction with ascorbic acid leads to a synthesis of less defective reduced graphene oxide. Also, the Fenton reagent is environmentally friendlier than other conventional oxidizing agents for this purpose, which makes this method more adequate for large-scale use.



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*Source: 5736563-2019-01-09.xml*