Introduction
As one of the green supercapacitor electrode materials, MnO2 shows potential to replace RuO2 due to its high specific capacitance, environmental compatibility, low cost, and abundance in nature. In general, the fabrication of MnO2 can be readily realized on large scale using traditional chemical co-precipitation methods 12. However, MnO2 powders produced by these methods suffer some disadvantages, like low specific surface area, and thus low specific capacitance in most cases. To improve the electrochemical performance, the strategy of direct deposition of MnO2 on large-surface-area materials, such as carbon blacks, carbon nanotubes, activated or mesoporous carbons 3456789, is quite promising. Recently, graphene oxide (GO), a shining-star material, has been widely investigated as a suitable support for MnO2 loading 1011. Thanks to the large accessible surface area provided by GO, more ions can transport onto the material surface, achieving high electric-double-layer capacitance in aqueous electrolytes. Furthermore, nanostructured MnO2 modified on GO support can effectually prevent the aggregation of GO nanosheets caused by van der Waals interactions. As a result, the available electrochemical active surface area for energy storage can be greatly enhanced.
Structurally, a single-layer of graphite oxide, also called GO, consists of a honeycomb lattice of carbon atoms with oxygen-containing functional groups which are proposed to present in the form of carboxyl, hydroxyl, and epoxy groups 1213. These functional groups can enlarge the gap between adjacent GO sheets. For instance, the (002) diffraction peak of pristine graphite is located at approximately 26°, and the interplane distance is 0.34 nm. After oxidation of graphite, the diffraction peak shifts to a lower angle, indicative of a larger interplane gap. The functional groups and the larger interplane gap enable GO sheets to be easily decorated or intercalated by polymers, quantum dots, and metal/metal oxide nanoparticles (NPs), etc. 101114151617181920, which are favorable and much desired for various applications. Nevertheless, until now, few reports have focused on the effects of functional groups and interplane gap of GO on the loading amount of quantum dots or metal/metal oxide nanoparticles, and so on.
In this work, we study the influences of GO supports on the electrochemical behavior of MnO2-GO nanocomposites. Two types of GO nanosheets, denoted as GO(1) and GO(2), made from commercial expanded graphite (CEG) and commercial graphite powder (CGP), respectively, are employed as MnO2 supports for comparative study. GO(1) nanosheets are proved to have more functional groups and larger interplane gap compared to GO(2) nanosheets, which might be capable of enhancing the loading amount of MnO2. As a result, MnO2-GO(1) nanocomposite exhibits higher energy and powder densities in neutral aqueous electrolytes.
Experimental
Materials
Commercial expanded graphite, commercial graphite powder, 98% H2SO4, 30% H2O2, potassium permanganate (KMnO4) and NaNO3 were used as received. Distilled water was used in all the processes of aqueous solution preparation and washing.
Material characterization
Scanning electron microscopy images were obtained on a field-emission scanning electron microscope (FE-SEM JEOL JSM-6700F; JEOL, Tokyo, Japan). Transmission electron microscopy (TEM) analyses were carried out using an electron microscope (JEM 2010F; JEOL, Tokyo, Japan) operating at 120 kV. The Raman spectra were recorded using a WITEC-CRM200 Raman system (WITEC, Germany). The excitation source is 532-nm laser (2.33 eV). X-ray photoelectron spectroscopy (XPS) measurement, was carried out on a thermo scientific ESCALAB 250 (Thermo Fisher Scientific, UK). The nanocomposites X-ray diffraction (XRD) studies were charactered by a Bruker D8 ADVANCE XRD (Bruker AXS, Germany). Nitrogen adsorption-desorption experiments were investigated at 77 K on an automatic volumetric sorption analyzer (Quantachrome, NOVA1200; Micromeritics, USA). The surface area was calculated using the Brunauer-Emmett-Teller equation. Pore size distributions were calculated by the Barrett-Joyner-Halenda (BJH) method using the adsorption branches. Quantitative elemental determinations were performed by firstly dissolving the solid samples with a CEM Mars microwave digester (Matthews, NC, USA), followed by analysis with a Thermo Scientific iCAP 6000 series inductively coupled plasma optical emission spectroscopy (ICP-OES, Thermo Scientific, England).
Synthesis of GO
Two kinds of graphite were used for synthesizing GO by a modified Hummers method 212223. In brief, 2 g of CEG (or CGP) and 1.5 g of NaNO3 were added into 150 mL of 98% H2SO4 solution in a flask which was immersed in an ice bath. Afterwards, 9 g of KMnO4 was slowly added in the solution. Meanwhile, the temperature of the mixed solution was maintained below 20°C for 2 h to avoid overheating and explosion. The mixture was stirred for 5 days. Then, 10 mL of 30% H2O2 was added into the solution in order to completely react with the remaining KMnO4, leading to a bright yellow solution. Finally, the resulting mixture was washed by 3% H2SO4 and H2O until the pH value of the solution was approximately 5-6. GO powder was obtained after freeze drying the suspension, labeled as GO(1)/GO(2).
Synthesis of MnO2-GO nanocomposites
The MnO2-GO nanocomposites were prepared by an in situ reduction method 24. The detailed procedure was as follows: 200 mg of GO(1) (or GO(2)) was blended with 150 mL of 0.02 M KMnO4 solution in a three-necked round-bottomed flask. The as-obtained mixture was refluxed at 120°C for 12 h with sustained magnetic stirring. The nanocomposites, labeled as MnO2-GO(1) (or MnO2-GO(2)), was then centrifuged, washed, and finally dried in air at 55°C overnight.
Electrochemical measurement
The working electrode of the electrochemical capacitors was fabricated by mixing the nanocomposites (15 mg) with 15 wt.% acetylene black and 5 wt.% polytetrafluorene-ethylene binder of the total electrode mass. A small amount of ethanol was added to the mixture for more homogeneous paste. The mixture was then pressed onto nickel foam current collector (1.0 × 1.0 cm) (washed by acetone and 0.1 M HCl carefully before use) to make electrodes. Electrochemical characterizations were carried out in a conventional three-electrode cell with 1 M Na2SO4 as the electrolyte. A platinum foil and saturated Ag/AgCl electrode were used as the counter and reference electrode, respectively. All electrochemical measurements were conducted using CHI 660 electrochemical workstation.
Results and discussion
XRD patterns of CEG and CGP before and after oxidation are shown in Figure 1. As can be seen, the single peak at 2θ of 26.3° indicates the typical graphitic structure. Compared with CGP, the CEG shows a broad peak together with an upper shift of 0.4°, suggesting that CEG is amorphous and has a larger interlayer spacing. After chemical oxidation treatments, the GO(2) evolved from CGP still presents two XRD peaks corresponding to the typical graphitic faces, whereas the pattern of GO(1) from CEG only shows one peak. Thus, the XRD results reveal that the CEG can be more easily exfoliated than CGP. Two diffraction peaks of GO(2) at approximately 26.3° and approximately 42.5° can be clearly seen from Figure 1b, corresponding to (002) and (101) planes of graphitic framework, respectively 2526. All peaks are weak and broad, which illustrate an amorphous carbon framework. This occurs because the interlayer spacing of the few-layered graphene sheet is similar to that of normal graphite, indicating that CGP has been partially converted into GO. In addition, there is a main peak at 2θ of 12.1° in GO(2) and 10.6° in GO(1), corresponding to d-spacing of 0.73 and 0.83 nm, respectively. This peak is similar to the typical diffraction peak of GO and is a possible indication of the presence of inter-few-layered graphene containing defects 27. GO(1) has a larger interplane gap than GO(2), revealing its higher oxidation degree compared to GO(2).
<p>Figure 1</p>XRD of (a) CEG and CGP; (b) GO(1) and GO(2)
XRD of (a) CEG and CGP; (b) GO(1) and GO(2). Diffraction peaks of graphite* and GO Δ.
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Figure 2a and 2b reveal the morphology differences between CEG and CGP. CEG has bigger graphite piece than CGP, which leads to larger GO(1) sheets than GO(2) (Figure 2c and 2d). Figure 3a and 3b show that the MnO2-GO(1) and MnO2-GO(2) still maintain the skeleton structure of GO with diameters around 10 μm, even larger than pristine GO (Figure 2c and 2d). This means that after hydrothermal reaction, the nanocomposites became agglomerate. The TEM observations show the prepared nano-MnO2 with morphology of nanorod and nanoflake uniformly decorated on the surface of the GO sheets. It is notable that both MnO2 nanorods and nanoflakes can be found on GO(2). While for GO(1) support, there are only MnO2 nanoflakes on its surface. Park and Keane have found that the strong epitaxial interaction between the catalytic species and the graphitic planes leads to a homogeneous distribution of the loaded Pd 28. It is generally accepted that large interplanar spacing and high specific surface area of GO(1) would enhance the epitaxial interaction between nano-MnO2 and the GO planes. As a result, MnO2 nanoflakes can be distributed uniformly on GO(1) with smaller size than MnO2 nanorods and nanoflakes on the GO(2) 29.
<p>Figure 2</p>SEM (a b) and TEM (c d) images of: (a) CEG, (b) CGP, (c) GO(1) and (d) GO(2)
SEM (a b) and TEM (c d) images of: (a) CEG, (b) CGP, (c) GO(1) and (d) GO(2).
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<p>Figure 3</p>TEM and HRTEM images of (a) MnO2-GO(1) and (b) MnO2-GO(2)
TEM and HRTEM images of (a) MnO2-GO(1) and (b) MnO2-GO(2).
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The inset HRTEM images in Figure 3 show the lattice fringes of the MnO2-GO(1) and MnO2-GO(2) nanocomposites. Three distinct sets of lattice spacing of ca. 0.237, 0.29, and 0.48 nm are shown, corresponding to the (211), (001), and (200) planes of α-MnO2, respectively. The inset image in Figure 3a and 3 the upper inset image in Figure 3b present the orientation of the three epitaxial growths of MnO2 nanoflakes on GO(1) and GO(2). Both epitaxial growths for the formation of the MnO2 nanorods on GO(2) were revealed by the lower inset image in Figure 3b. The presence of clear lattice fringes in the HRTEM images confirms the crystalline nature of the α-MnO2 nanorodes and nanoflakes. The following Raman and XPS characterization also prove the polymorph of the MnO2 is α-MnO2.
The typical Raman spectra taken from different regions of the samples are shown in Figure 4. They present one diagnostic Raman scattering band of α-MnO2, approximately 643 cm-1, which belongs to Ag spectroscopic species originating from breathing vibrations of MnO6 octahedra 30. Two weak peaks recorded at approximately 305 and 360 cm-1 corresponding to the bending modes of O-Mn-O were observed in the spectra of the nanocomposites, stemming from the formation of Mn2O3 or Mn3O4 induced by the laser heating 31. The appearance of a strong Ag-mode consists with our HRTEM result that the crystalline α-MnO2 has been readily formed on the GO support. Another two prominent peaks, D band (1,345 cm-1) and G band (1,597 cm-1), belong to GO 32333435. From Figure 4, we can also see that the ratio of α-MnO2 to G is very different. MnO2-GO(1) has a larger α-MnO2 to G ratio than MnO2-GO(2), which means that the content of MnO2 in MnO2-GO(1) is higher than that in MnO2-GO(2). The Raman results are consistent with the inductively coupled plasma (ICP) and XPS results.
<p>Figure 4</p>Raman Spectra of (a) MnO2-GO(1) and (b) MnO2-GO(2)sheets
Raman Spectra of (a) MnO2-GO(1) and (b) MnO2-GO(2)sheets. (* α-MnO2)
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The element analysis was further studied by inductively coupled plasma (ICP) to prove the different amount of Mn in the nanocomposites. ICP-OES analysis of the concentrations of Mn in the nanocomposits confirmed that MnO2-GO(1) (230.3 mg g-1) has higher Mn content than MnO2-GO(2) (153.6 mg g-1), which will affect the morphology and electrochemical performances of the nanocomposites.
The nanocomposites obtained by using different GO sources have been further studied by the nitrogen adsorption-desorption measurements. As can be seen from Figure 5, all samples display a type-IV isotherm, indicating the mesoporous structure. Although MnO2-GO(1) and MnO2-GO(2) reveal the same type of the adsorption-desorption isotherm, their surface areas and pore size distributions are quite different. As for MnO2-GO(1), the specific surface area and the total pore volume are measured to be approximately 238.1 m2 g-1 and approximately 0.711 cm3 g-1, which are correspondingly larger than those for MnO2-GO(2). Remarkably, these values are much higher than the data for MnO2 produced by traditional co-precipitation of KMnO4 and Mn2+in previous report 36. The pore size distribution plots of MnO2-GO(1) and MnO2-GO(2) are calculated by BJH method, using desorption branch of N2 isotherms. MnO2-GO(1) and MnO2-GO(2) have comparable pore volumes. However, MnO2-GO(2) shows narrower pore size distribution than MnO2-GO(1), with a pore diameter range of 20-50 nm. The results clearly demonstrate that the graphite source has a significant effect on the microstructure of GO. The specific surface area and effective pores (8-50 Å) are reported to be effective to increase the double-layer capacitance of carbon and multiply the redox active sites for metal oxides loading. Therefore, the pseudo-capacitance will increase significantly. As a result, the unique structure could be useful to enhance the capacity of MnO2-GO(1) 243738.
<p>Figure 5</p>Nitrogen adsorption-desorption isotherms of (a) MnO2-GO(1) and (b) MnO2-GO(2)
Nitrogen adsorption-desorption isotherms of (a) MnO2-GO(1) and (b) MnO2-GO(2). The inset shows BJH pore-size distributions.
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The high-resolution XPS spectra further confirm the different oxygen contents in GO(1) and GO(2), manganese contents and carbon contents in MnO2-GO(1) and MnO2-GO(2). As shown in Figure 6a and 6b, the curve fitting yields three components at sp2-C (approximately 284.5 eV), C-O (hydroxyl and epoxy, approximately 286.5 eV), and C=O (carboxyl, approximately 288 eV), respectively 394041. The contribution of C=C band decreases from 50% for GO(2) to 40% for GO(1). An obvious broadening of C=C band is also observed, indicating a more disordered structure for GO(1), which agrees well with the XRD results.
<p>Figure 6</p>C1s spectra: (a) GO(1), (b) GO(2)
C1s spectra: (a) GO(1), (b) GO(2). (c-d) Mn2p, (e-f) O1s spectra of MnO2-GO(1) and MnO2-GO(2).
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The spectra in Figure 6c and 6d illustrate the existence of MnO2 by the peaks assigned to Mn 2p3/2 (642.7 eV) and Mn 2p1/2 (653.9 eV), respectively. They have a spin-energy separation of 11.2 eV, further confirming the presence of α-MnO2 in the nanocomposite 4243.
Besides the oxygen (O 1s, 532.4 eV) signals from graphene sheets in Figure 6e and 6f, the O 1s peak observed at 530.0 eV is assigned to the oxygen bonded with manganese 44. On the basis of the quantitative analysis of XPS data, the corresponding atomic ratios of Mn to C for MnO2-GO(1) and MnO2-GO(2) in the nanocomposite are estimated to be 1:1.61 and 1:1.81 by integrating the area of each element peak areas, with their relative sensitive factor taken into account as well. It is worth noting that most carbon atoms in graphene sheets have not been substituted by Mn. However, MnO2-GO(1) still has more replacement Mn position in the nanocomposite than MnO2-GO(2). All of the data further confirm the existence of α-MnO2 and the loading of MnO2 is higher in MnO2-GO(1) than that in MnO2-GO(2).
The electrochemical performances of the GO obtained from different graphite sources before and after loading MnO2 were investigated by cyclic voltammograms (CVs) and galvanostatic charge/discharge measurements in 1 M Na2SO4 solution between -0.3 and 0.8 V (Figure 7). From Figure 7a, it can be seen that the plots show an almost rectangular profile induced by an ideal capacitive behavior. GO shows lack of symmetry 43. The poor electrochemical performance of GO is due to their poor electrical conductivity and low faradic reaction rate. However, the capacitance of GO(2) (21.39 F g-1) is higher than that of GO(1) (0.64 F g-1). Figure 7b shows the galvanostatic charge/discharge curves of the GO(1), GO(2), MnO2-GO(1), and MnO2-GO(2) at a current density of 100 mA g-1. After MnO2 loading, the capacity of MnO2-GO(1) is twice that of MnO2-GO(2) due to the high loading amount of MnO2 for GO(1) than that for GO(2).
<p>Figure 7</p>(a) CVs and (b) galvanostatic charge/discharge curves of GO(1), GO(2), MnO2-GO(1), respectively
(a) CVs and (b) galvanostatic charge/discharge curves of GO(1), GO(2), MnO2-GO(1), respectively.
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Figure 8a and 8b show the CV curves of MnO2-GO(1) and MnO2-GO(2) nanocomposites. MnO2-GO(1) shows the lack of symmetry at high scan rates (Figure 8b), which is probably due to pseudo-capacitance from MnO21043. Specific capacitances of the nanocomposites calculated at current densities of 100, 250, 500 mA g-1 from the discharge curves are 176.0, 165.8, 140.3 F g-1 for MnO2-GO(2) electrode, and 307.7, 297.3, 184.6 F g-1 for MnO2-GO(1) electrode (Figure 8c and 8d). The MnO2-GO(1) electrode has almost twice the specific capacitances of MnO2-GO(2). The enhanced electrochemical performance of MnO2-GO(1) electrode is due to the high MnO2 loading by using the GO(1) with abundant surface functionalities. High loading and homogeneous distribution of MnO2 on graphene oxide surface are advantageous for graphene oxide network to transport ions in the pore system and increasing the MnO2-electrolyte interfacial area. Therefore, the excellent capability of GO(1) makes it attractive particularly for energy storage applications. Different GO precursors obviously have significant effect on the electrochemical capacitive performance before or after loading other nanomaterials. Thus, it is important to obtain highly porous and surface-functionalized graphene for supercapacitor applications.
<p>Figure 8</p>(a-b) CVs and (c-d) galvanostatic charge/discharge curves of MnO2-GO(1) and (b) MnO2-GO(2), respectively
(a-b) CVs and (c-d) galvanostatic charge/discharge curves of MnO2-GO(1) and (b) MnO2-GO(2), respectively.
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