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An international journal of inorganic chemistryrsc.li/dalton
ISSN 0306-0012
COMMUNICATION Douglas W. Stephen et al.
N-Heterocyclic carbene stabilized parent sulfenyl, selenenyl, and tellurenyl cations (XH+, X = S, Se, Te)
Volume 46 Number 10 14 March 2017 Pages 3073-3412
Dalton
Transactions
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Le, V. V. Thuy, V. D. Thao, M. Hatsukano, K. Higashimine, S. Maenosono, S. Chun and T. V. Thu, Dalton Trans., 2020, DOI: 10.1039/D0DT01177K.
Facile synthesis of Mn-doped NiCo
2O
4nanoparticles with enhanced electrochemical performance for battery-type
supercapacitor electrode
To Van Nguyen1, Le The Son1,2, Vu Van Thuy1, Vu Dinh Thao1, Masahito Hatsukano2, Koichi Higashimine2, Shinya Maenosono2, Sang-Eun Chun3, and Tran Viet Thu4
1Department of Chemical Engineering, Le Quy Don Technical University, 236 Hoang Quoc Viet, Hanoi 100000, Vietnam
2School of Materials Science, Japan Advanced Institute of Science and Technology, 1-1 Asahidai, Nomi, Ishikawa 923-1292, Japan
3School of Materials Sciences and Engineering, Kyungpook National University, Daegu 41566, Republic of Korea
4Institute of Research and Development, Duy Tan University, Danang 550000, Vietnam
Corresponding authors: E-mail: sangeun@knu.ac.kr; tranvietthu1@duytan.edu.vn;Tel: +84 964 793 732
Abstract
We report the synthesis of manganese-doped nickel cobalt oxide (Mn-doped NiCo2O4) nanoparticles (NPs) by an efficient hydrothermal and subsequent calcination route. The material exhibits a homogeneous distribution of Mn dopants and a battery-type behavior when tested as a supercapacitor electrode material. Mn-doped NiCo2O4 NPs show an excellent specific capacity of 417 C g-1 at scan rate of 10 mV s−1 and 204.3 C g-1 at current density of 1 A g−1 in standard three- electrode configuration, ca. 152-466 % higher than that of the pristineNiCo2O4 or MnCo2O4. In addition, Mn-doped NiCo2O4 NPs showed excellent capacitance retention of 99% after 1,000 charge- discharge cycles at current density of 2 A g−1. The symmetric solid-state supercapacitor device assembled using this material delivered an energy density of 0.87 Wh cm−2 at a power density of 25
Wh cm−2, and 0.39 Wh cm−2 at a high power density of 500 Wh cm−2. The cost-effective synthesis and high electrochemical performance suggest that Mn-doped NiCo2O4 is a promising material for supercapacitors.
Keyword: Energy storage materials; NiCo2O4; chemical synthesis; doping; supercapacitor.
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1. Introduction
The rapid development of portable electronics and electric vehicles has recently imposed additional requirements for power sources, such as enhanced durability and safety, improved mechanical strength, smaller size, and lower weight [1-3]. Popular power sources such as lithium-ion batteries have numerous advantages, including high energy density and low self-discharge; however, they also suffer several disadvantages, including low power density (ca. 101000 W kg-1), short lifecycle (ca. 4001200 cycles), high cost, and limited resource that restrict their range of applications [4]. Supercapacitors have emerged as a promising complimentary power source for batteries because of their numerous advantages, such as high power density, excellent durability, and high Coulombic efficiency [5]. The specific power of supercapacitors is typically 10 to 100 times greater that of batteries and can reach values up to 15 kW kg-1 [4].
Supercapacitor electrodes are generally classified into three main categories according to their energy storage mechanism: (1) Electrochemical double-layer electrodes, in which charge storage is relied on the absorption/desorption of electrolyte ions at the electrolyte/electrode interface. Typical electrodes are based on carbonaceous materials with large specific surface area [6-8] for attaining high energy density. (2) Pseudocapacitive electrodes, which rely on the transfer of electrical charges through redox reactions and intercalation/de-intercalation processes of electrode material beyond electrostatic adsorption, typically RuO2 and MnO2 [9-11]. Their capacitance values are relatively constant within potential window. (3) Battery-type electrodes, in which the charge storage is also faradaic in nature, but their specific capacity values vary with voltage window and their specific capacity is better expressed in C g-1 or mAh g-1 [12]. Typical battery-type electrode materials are transitional metal oxides/sulfides [13-16], and they are frequently coupled with pseudocapacitive electrodes in hybrid supercapacitors to obtain high specific power and high specific energy [15, 17].
Therefore, the electrode material is a critical factor that determines the charging mechanism, electrochemical performance, and practical applications of a supercapacitor in which the electrode material is incorporated. Over the past decade, numerous efforts have been dedicated to developing novel materials as well as to improving the performance of existing electrode materials [14, 18].
Spinel-type metal oxides with general formula AB2O4 (where A and B represent first-row transition metals such as Co, Fe, Ni, and Mn) have received intensive attention as a promising material for energy storage because of their high specific capacity, cost-effectiveness, and high earth- abundance [18-23]. Among them, NiCo2O4 is a very promising candidate because of their excellent charge storage capacity which is much higher than that of both neat NiO and Co3O4 [24-27]. The developments of high-performance NiCo2O4-based electrodes for supercapacitors have included different strategies such as tuning the morphology, forming the hetero-structures, and hybridizing
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with high surface area conductive support [23, 26-28]. Recently, it was shown that the composition of nickel-cobalt oxides has significant effects on their microstructures and electrochemical properties [29]. A substitution of Ni with Cu of up to 50% could increase the Cs of NiCo2O4 from 280.3 F g−1 to 367.4 F g−1 at a discharge rate of 1 A g−1 [30]. Whereas, the substitution of Ni with Mo could double the Cs of NiCo2O4 [31], and the substitution of Co with Fe could increase the Cs of NiCo2O4
up to 45.7 % [32]. Doping has also been demonstrated as a promising strategy for tuning the chemical composition and modulating the electrochemical property of NiCo2O4 materials [24, 33]. Among various dopants, Mn has many advantages such as multi-valence states, earth-abundance and environmental benign [34]. Mn-doped NiMoO4 nanorods as positive electrode in supercapacitor exhibit an improved electrochemical performance and cycle life due to synergistic effects of Ni and Mn elements [35]. 10% Mn-doped ZnCo2O4 synthesized by hydrothermal route exhibited a maximum capacitance of 707.4 F g−1 at a current density of 0.5 A g−1, and a high Coulombic efficiency of 96.3%
after 500 CV cycles in KOH electrolyte [34]. 5% Mn-doped NiCo2O4 nanosheets were found to show excellent lithium storage due to hierarchical structure and the combination of Mn dopants and the NiCo2O4 host structure [36]. However, the study of Mn-doped NiCo2O4 for supercapacitor application has not been reported.
In this work, we report a facile combined hydrothermal treatment/calcination route to prepare Mn-doped NiCo2O4 nanoparticles (NPs) with a doping content as high as 10 at%. The crystal structure, morphology, chemical composition, and chemical state of the as-prepared Mn-doped NiCo2O4 NPs was systematically characterized. We found that Mn-doped NiCo2O4 NPs display battery-type behavior with enhanced specific capacity compared with those of pristine NiCo2O4 and MnCo2O4, indicating a synergistic effect of Mn dopant and NiCo2O4 host structure. The cycling test indicated that the Mn-doped NiCo2O4 NPs demonstrate a long-term cycle stability with 99% capacity retention after 1000 charge–discharge cycles.
2. Experimental
2.1. Chemicals: Nickel(II) chloride hexahydrate (NiCl2·6H2O), cobalt(II) chloride hexahydrate (CoCl2·6H2O), manganese(II) chloride (MnCl2), urea (CO(NH2)2), hydrochloric acid (HCl), Ni foam, acetylene black, polyvinylidene fluoride (PVDF), N-methyl-2-pyrrolidone (NMP), and polyvinyl alcohol (PVA) were purchased from Shanghai Aladdin Bio-Chem Technology Co., Ltd. All of the reagents were of analytical grade and were used without further purification. All solutions in the experiments were prepared with deionized (D.I.) water (18 M cm).
2.2. Materials synthesis: NiCo2O4 (NCO), Mn-doped NiCo2O4 (NMCO), and MnCo2Ox (MCO) NPs were synthesized by a combined hydrothermal treatment/calcination route (Fig. 1a). In a typical
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procedure, 0.9 g of urea (15 mmol) and predetermined amounts of M2+ salts (M = Ni, Mn, Co) were dissolved into 75 mL of D.I. water by magnetic stirring for 30 min, resulting in the formation of a pinkish solution. The total amount of M2+ salts was fixed at 15 mmol, where Ni2+/Mn2+/Co2+ (molar ratio) was varied: 5/0/10 (NCO); 4/1/10 (NMCO); or 0/5/10 (MCO). The resulting mixture was transferred to a 150 mL Teflon-lined autoclave and heated to 120 oC for 6 h in air for hydrothermal treatment. After the autoclave was cooled to room temperature, the product in it was washed with D.I. water and ethanol several times. The washed product was calcined at 400 oC in air for 2 h. The amount of each precursor in synthesized samples are given in Table 1.
Table 1. Ratio between precursor chemicals for different samples Amount (mmol)
NiCl2∙6H2O MnCl2 CoCl2∙6H2O Total
NCO 5 0 10 15
NMCO 4 1 10 15
MCO 0 5 10 15
2.3. Characterization: All synthesized cobaltites were characterized by X-ray diffraction (XRD), scanning electron microscopy (SEM), transmission electron microscopy (TEM), scanning TEM (STEM) on an instrument equipped with a high-angle annular dark-field (HAADF) detector, energy- dispersive X-ray spectroscopy (EDS) elemental mapping, X-ray photoelectron spectroscopy (XPS), X-ray fluorescence (XRF) spectroscopy, and inductively coupled plasma (ICP). XRD measurements were conducted on a Siemens D5005 X-ray diffractometer equipped with a Cu-Kα radiation source (wavelength 1.5418 Å, acceleration voltage/current 30 kV/40 mA, scan rate 0.9 o min−1, scan step 0.03 o, 2θ range from 10 o to 70 o). SEM analysis was conducted on a Hitachi S4800 field-emission scanning electron microscope. TEM observations were performed on a Jeol JEM-1010 microscope.
STEM-HAADF imaging and EDS elemental mapping were carried out on a JEOL JEM-ARM200F microscope operated at an acceleration voltage of 200 kV and equipped with a spherical aberration corrector; the nominal resolution was 0.8 Å. XPS analysis was performed on a Shimadzu Kratos AXIS-ULTRA DLD high-performance XPS system. Monochromated Al Kα radiation was used to excite photoelectrons. The chemical composition was estimated by XRF spectroscopy (X-MET 5100, Oxford Instruments). The elemental compositions of the synthesized samples were further confirmed by ICP conducted on a Optima 7300DV. Each sample was quantified twice to ensure reproducibility.
2.4. Electrochemical measurements: To evaluate the electrochemical behavior and performance of the synthesized materials, a homogeneous slurry was prepared by mixing active material, acetylene black, and PVDF (weight ratio 75:12.5:12.5) in a small amount of NMP solvent. The working
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electrode was prepared by pasting the prepared slurry onto a Ni foam sheet (coating area 1.0 × 1.0 cm2) and drying in a vacuum oven at 60 °C for 5 h. The mass loading of active materials was approximately 2 mg cm−2. Cyclic voltammetry (CV), galvanostatic charge–discharge (GCD), and electrochemical impedance spectroscopy (EIS) measurements were performed on Metrohm Autolab PGSTAT 302N using a standard three-electrode cell system with a Ag/AgCl reference electrode (in 3 M KCl solution) and Pt counter electrode (sheet). In all of the electrochemical measurements, a 3 M KOH aqueous solution was used as the electrolyte. CV measurements were performed between
−0.1 and 0.5 V at different scan rates (10, 20, 40, 60, 80, and 100 mV s−1). GCD measurements were performed at different current densities (1.0, 1.5, 2.0, 2.5 and 3.0 A g−1) in the potential range from
−0.1 to 0.45 V. EIS analyses were carried out in the frequency range from 0.01 Hz to 100 kHz at open-circuit potential with an AC amplitude of 10 mV. The specific capacity (Cs, C g-1) of the electrochemically active material was subsequently calculated from cyclic voltammograms using the formula Cs = (IdV)/(×m), where I (A), V (V), (V s-1), and m (g) represent the current, potential, scan rate, and mass of active material, respectively. Cs was also calculated from the GCD curves at different current densities using Cs = (I×t)/m, where I is the discharge current (A) and t is the discharge time (s).
2.5. Fabrication of supercapacitor device: The symmetric all-solid-state supercapacitor device was fabricated with NMCO as the active material and PVA–KOH as a gel-type electrolyte. First, an electrode was prepared by pasting the prepared slurry of NMCO onto nickel sheets (width × length × thickness = 2.0 × 2.5 × 0.15 mm3) and dried in a vacuum oven at 60 oC for 5 h. The mass loading of active material on each electrode was approximately 10 mg cm−2. The gel-type electrolyte was prepared by dissolving 3 g of PVA in 30 mL of D.I. water with constant stirring at 100 oC for 2 h.
After the PVA solution became clear, 1.5 g of KOH in 10 mL of D.I. water was added to the solution at 80 oC under vigorous stirring. Two electrodes prepared with NMCO were immersed in PVA–KOH solution for 15 min. The electrodes were assembled with a PVA–KOH gel electrolyte between them.
Finally, the PVA–KOH gel was solidified by evaporating the contained water at room temperature, resulting in all-solid-state supercapacitor. Furthermore, the electrochemical characteristics of the supercapacitor device were studied using CV and GCD. The areal capacitance (Ca, F m-2) of the supercapacitor device was calculated from GCD using the formula Ca = (It)/(SV), where I (A), t (s), S (m2), and V (V) represent discharge current, discharge time, geometrical area of the electrode, and potential window (V). The specific energy density (E) and specific power density (P) were calculated using the equations E = Ca×(V)2/2 and P = E/t, respectively.
3. Results and Discussion
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3.1. Structural and morphological characterization
Phase identification: As shown in Fig. 1b, the XRD patterns of the as-synthesized cobaltites are almost identical and can be assigned to NiCo2O4 (JCPDS #20-0781) and/or MnCo2O4.5 (JCPDS
#32−0297); both have the same cubic spinel structure and crystallize in space group Fd-3m (227).
The observed diffraction peaks at 18.6, 31.4, 36.7, 44.3, 59.1, and 64.6 o are appropriately indexed to the (111), (220), (311), (422), (511), and (440) planes, respectively. No diffraction peaks due to impurities are observed in any of the XRD patterns. The similarity in both the positions and relative intensities of the peaks of these cobaltites indicates that their crystal structures and lattice parameters do not substantially differ. A very small deviation from each other’s diffraction peak is due to the difference in atomic radii of Ni (0.135 nm) and Mn (0.140 nm). The structural representation of the typical cobaltite (NiCo2O4, Fig. 1c) shows that Ni (or Mn) ions occupy octahedral sites, whereas Co ions occupy both octahedral and tetragonal sites.
Stirring 30 min
pink powder black powder
Calcination 400oC, 2h autoclave
NiCl2.6H2O CoCl2.6H2O MnCl2
Urea Hydrothermal
120oC, 6h
JCPDS #20-0781
JCPDS #32-0297 a b
c OCo NiCo
(a)
(b) (c)
10 20 30 40 50 60 70
MCO
NMCO
Normalized intensity
NCO
440
511
422
400
222311
220
2-theta (degree)
111
Figure 1. (a) Synthesis flowchart for NCO, MCO, and NMCO. (b) XRD patterns of the as- synthesized cobaltites along with those of reference materials of NiCo2O4 (JCPDS #20-0781, black
bars) and MnCo2O4.5 (JCPDS #32-0297, red bars). (c) Illustration of spinel-structured NiCo2O4. Morphology: Figs. 2(a,d,g) and 2(b,e,h) show SEM and TEM images of NCO, NMCO, and MCO, respectively. As shown in the SEM images, all of the obtained cobaltites have polyhedral
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shapes, and their agglomeration is likely resulting from the calcination step (at 400 oC). Other authors have found that urea acts as a facet-directing agent in the hydrothermal crystallization of binary and ternary oxides when KOH is used as a mineralizer [37, 38]. In our synthesis route, KOH was not used and urea was hydrolyzed during the thermal treatment to generate carbonate ions [39-41]. Metal ions then combined with carbonate ions to form metal carbonates (pink powder), which were ultimately transformed to metal cobaltites (black powder) during calcination. Although these polyhedra are not very well defined, their average size was typically smaller than 100 nm. Despite huge differences in their elemental compositions, the NMCO exhibits a morphology similar to that of NCO and MCO.
The selected-area electron diffraction (SAED) patterns, shown in Figs. 2(c,f,i) can be indexed as the (311), (222), (511), and (440) planes of spinel-structured NiCo2O4, consistent with the previously shown XRD results.
200 nm
200 nm
200 nm
(a) (b) (c)
(d) (e) (f)
(g) (h) (i)
Figure 2. SEM image, TEM image, and SAED patterns of NCO (a, b, c) NMCO (d, e, f), and MCO (g, h, i).
The distribution of Ni, Mn, Co, and O across the as-synthesized cobaltite particles was characterized using STEM-EDS elemental mapping. The STEM-HAADF images and EDS elemental mapping images of NCO, NMCO, and MCO are shown in Fig. 3(a–c), respectively. These images and mapping images confirm the presence of all of the aforementioned elements as well as their
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homogeneous distribution throughout the cobaltite particles. These results thus demonstrate that well- structured NMCO were successfully synthesized for all combinations of the precursors.
(a) (c)
(b)
Figure 3. STEM-HAADF images and corresponding STEM-EDS elemental mappings of typical (a) NCO, (b) NMCO, and (c) MCO. Scale bar for STEM: 20 nm.
Elemental composition and chemical state: The XPS survey spectra (Fig. S1) assert the presence of Ni, Co, O in NCO; Mn, Co, O in MCO; and Ni, Mn, Co, O in NMCO. The presence of other elements such as C (ca. 286–288 eV) and Fe (ca. 720 eV) is due to adventitious carbon contamination and iron-based sample holder used for the sample preparation, respectively. NMCO was selected as a representative cobaltite sample for further XPS studies. All core-level XPS spectra of Ni 2p, Mn 2p, Co 2p, and O 1s were calibrated (reference: C 1s line), background subtracted (linear-type), deconvoluted, and fitted (Gaussian fitting method). The Ni 2p spectrum (Fig. 4a) was deconvoluted into six peaks, four of which correspond to two characteristic spin–orbit doublets of Ni2+ (853.1 and 872.3 eV) and Ni3+ (856.4 and 873.9 eV) [42]. The two remaining peaks (861.2 and 879.7 eV) correspond to shake-up satellites of nickel [33]. Similar to Ni spectrum, the Mn 2p spectrum (Fig. 4b) was also deconvoluted into six peaks, corresponding to Mn2+ (641.3 and 652.5 eV), Mn3+ (642.6 and 653.8 eV) [43], and shake-up satellites (643.9 and 655.4 eV) of manganese.
The XPS spectrum of Co 2p (Fig. 4c) exhibits peaks at 781.1 and 796.2 eV ascribed to Co2+, two
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peaks at 779.6 and 794.6 eV corresponding to Co3+, and two pairs of shake-up satellites corresponding to Co2+ (785.2 and 799.6 eV) and Co3+ (790 and 804.3 eV) [21]. In addition, the XPS spectrum of Co 2p includes two small peaks at 777.9 and 792.9 eV, suggesting the presence of a small amount of Co0 in the surface materials. The XPS O 1s spectrum (Fig. 4d) indicates two O species: the peak at 529.3 eV corresponds to O involved in M–O bonding (M is the metal), and the peak at 531.0 eV corresponds to defect sites on the surface of the synthesized cobaltite[44]. Ni2+, Ni3+, Co0, Co2+, Co3+, and O species on the surface of NCO, and Mn2+, Mn3+, Co0, Co2+, Co3+, and O species on the surface of MCO were verified in the XPS spectra of NCO (Fig. S2) and MCO (Fig. S3), respectively. These data clearly indicate that the NCO, MCO, and NMCO cobaltites were successfully synthesized according to our proposed hydrothermal and calcination routes. Both XRF and ICP (Table S1) were used to quantify the elemental composition of NMCO sample, and the results were consistent. The Mn:Ni:Co atomic ratio was calculated to be 0.3:3:10, which indicates a Mn doping content of approximately 10 % (as compared to Ni content).
Figure 4. XPS spectra of (a) Ni 2p, (b) Mn 2p, (c) Co 2p, and (d) O 1s in NMCO.
3.2. Electrochemical characteristics
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CV analysis: Fig. 5(a–c) show the CV curves of NCO, NMCO, and MCO, respectively. In all of the CV curves, a pair of well-defined redox peaks is clearly observed, which is attributed to redox reactions involved in AO/AOOH (A = Ni, Mn, Co) conversions[19]. This suggests the materials display battery-type rather than pseudocapacitance-type behavior; accordingly, their specific capacity is better presented as C g-1 (or mAh g-1) instead of F g-1 due to the charge storage is non-constant over the working potential [12, 45, 46]. Therefore, the supercapacitor electrodes fabricated using these materials mainly store and release electrical charges through Faradaic reactions.
No additional redox peaks are detected in the CV curves of NMCO, indicating that the redox processes in NMCO are very similar to those in NCO and MCO. Fig. 5d shows CV curves for all of the samples, as recorded at a scan rate of 100 mV s−1. The CV curve for NMCO shows a much larger internal area than those of NCO and MCO, indicating that NMCO exhibits the largest Cs. The Randles–Sevcik plots of NMCO sample are shown in Fig. 5e. It can be seen that, as the scan rate is increased from 10 to 100 mV s−1, both the anodic peak current (Ipa) and the cathodic peak current (Ipc) increase. More specifically, both Ipa and Ipc vary linearly with the square root of the scan rate (1/2), as well described by the Randles–Sevcik equation[47, 48]. These observations indicate that the redox events occurring at the electrode–electrolyte interface are fast and quasi-reversible and are only limited by electrolyte diffusion[49]. Simultaneously, the separation between anodic and cathodic peaks also increases with increasing scan rate, which is attributed to the equivalent series resistance.
The Cs of these materials at different scan rates was calculated, and the results are plotted in Fig. 5f.
The Cs of all of the materials increase with decreasing scanning rate. At the same scan rate, the Cs
values increase in the order MCO < NCO < NMCO. Specifically, the Cs value of NMCO obtained at 10 mV s−1 was calculated to be 417.0 C g-1, much greater than that of NCO (274 C g-1) and MCO (98.0 C g-1). The enhancement of Cs in NMCO suggests that the Ni and Mn in NMCO synergistically behave as a faradaic charging site compared with the Ni or Mn sites alone in NCO and MCO.
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-0.1 0.0 0.1 0.2 0.3 0.4 0.5 -60
-40 -20 0 20 40 60 80
Current (A g-1 )
Potential vs. Ag/AgCl (V) 100 mV s-1
80 mV s-1 60 mV s-1 40 mV s-1 20 mV s-1 10 mV s-1
NCO
-0.1 0.0 0.1 0.2 0.3 0.4 0.5
-60 -30 0 30 60
90 100 mV s-1 80 mV s-1 60 mV s-1 40 mV s-1 20 mV s-1 10 mV s-1
Current (A g-1 )
Potential vs. Ag/AgCl (V)
NMCO
-0.1 0.0 0.1 0.2 0.3 0.4 0.5
-30 -20 -10 0 10 20
30 100 mV s-1 80 mV s-1 60 mV s-1 40 mV s-1 20 mV s-1 10 mV s-1
Current (A g-1 )
Potential vs. Ag/AgCl (V)
MCO
0 20 40 60 80 100
50 100 150 200 250 300 350 400 450
Specific Capacity (C g-1 )
Scan rate (mV s-1)
NCO NMCO MCO
(a) (b)
(c) (d)
-0.1 0.0 0.1 0.2 0.3 0.4 0.5
-80 -60 -40 -20 0 20 40 60 80 100
Current (A g-1)
Potential vs Ag/AgCl (V) NCO NMCO MCO
3 4 5 6 7 8 9 10 11
-60 -40 -20 0 20 40 60 80
y = -6.7063x + 7.7012 R² = 0.9982 y = 8.9765x - 5.5143 R² = 0.9971
Current (A/g)
v1/2 Ipa
Ipc
NMCO (e) (f)
Figure 5. CV curves at different scan rates of NCO (a), NMCO (b), and MCO (c); CV curves of NCO, NMCO, and MCO at 100 mV s−1 (d); Randles–Sevcik plots of NMCO (e); Cs of all of the
synthesized materials at different scan rates (f).
GCD analysis: To evaluate the Cs and the rate performance of the obtained cobaltites, GCD measurements were conducted in the potential range from −0.1 to 0.45 V at different current densities ranging from 1 to 3 A g−1. Fig. 6(a–c) presents the GCD voltage profiles of NCO, NMCO, and MCO, respectively. The observed voltage plateaus in the discharging profiles match well with the peak potentials observed in the cyclic voltammograms, confirming their battery-type behavior and that their main mechanism for energy storage is based on redox reactions. The difference between the discharge and charge potential plateau in the GCD profile originates from the series resistance of the electrode. A smaller deviation indicates greater electrochemical reversibility; the GCD results in the current range from 1 to 3 A g−1 show that the NMCO exhibit excellent reversibility similar to that of neat NCO and MCO. Fig. 6d presents the GCD profiles for all of the samples, as recorded at a current
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density of 1 A g−1. The calculated Cs of NMCO is 204.3 C g−1, much higher than those of NCO (127 C g−1) and MCO (43.9 C g−1). It is also observed that the Cs of NMCO is always greater than those of NCO and MCO at other current densities, as shown in Fig. 6e. For all of the samples, the minimal decrease of Cs with increasing current density reveals remarkable rate capability, indicating fast kinetics of the faradaic reaction of the electrode materials. These results agree well with the results of the CV analysis and indicate the synergy of faradaic conversions between AO/AOOH (A = Ni, Mn, Co) pairs in NMCO. Given the similar structure and morphology of NMCO and NCO, the higher Cs of NMCO obviously arises from the composition difference due to Mn doping. It is therefore concluded that the Mn doping greatly enhanced the electrochemical properties of NiCo2O4 NPs.
0 50 100 150 200 250 300
-0.1 0.0 0.1 0.2 0.3
0.4 NCO
Potential vs. Ag/AgCl (V)
Time (sec)
1 A g-1 1.5 A g-1 2 A g-1 2.5 A g-1 3 A g-1
0 100 200 300 400
-0.1 0.0 0.1 0.2 0.3
0.4 1 A g-1
1.5 A g-1 2 A g-1 2.5 A g-1 3 A g-1
NMCO
Potential vs. Ag/AgCl (V)
Time (sec)
0 20 40 60 80 100
-0.1 0.0 0.1 0.2 0.3
0.4 MCO 1 A g-1
1.5 A g-1 2 A g-1 2.5 A g-1 3 A g-1
Potential vs. Ag/AgCl (V)
Time (sec)
(a) (b)
(c) (d)
0 200 400 600 800 1000
0 20 40 60 80 100 120
Capacitance retention (%)
Cycle number
NMCO
(e) (f)
1.0 1.5 2.0 2.5 3.0
0 30 60 90 120 150 180 210
Specific Capacity (C g-1 )
Current (A g-1)
NMCO
NCO
MCO
0 100 200 300 400
-0.1 0.0 0.1 0.2 0.3 0.4
Potential vs Ag/AgCl (V)
Time (sec)
NCO NMCO MCO
Figure 6. GCD curves of NCO, NMCO, and MCO at different current densities (a–c) and at 1 A g−1 (d); rate capability of all samples (e); and cycling performance of NMCO for 1,000 cycles at a
current density of 2 A g−1 (f).
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For comparison, the Cs of several supercapacitor electrodes fabricated from NiCo2O4
nanomaterials is summarized in Table 2. The specific capacity of NMCO NPs was 204.3 C g-1, which was much higher than that of NiCo2O4 nanosheets (92.1 F) [50], NiCo2O4 nanoflowers (122.5 C g−1) [12], NiCo2O4 nanosheets (145 C g−1) [51], NiCo2O4 hollow spheres (171.2 C g−1) [45], NiCo2O4
microspheres (112-202 C g−1) [52], and MnCo2O4 nanofibers (52 C g−1) [53] at the same discharge current of 1 A g-1, indicating the excellent performance of NMCO NPs. However, the Cs of NMCO NPs was still lower than that of NiCo2O4 nanoflowers grown on Ni foam (348.9 C g−1) [54] or rGONiCo2O4 nanocomposites (427 C g−1) [45]. This comparison suggests that further developments of this work should include the deposition of NMCO NPs on three-dimensional conductive scaffold or combination with other materials to form heterostructures.
Table 2. Comparison of NiCo2O4–based electrode materials for supercapacitors
Electrode material Method of synthesis Electrolyte Cs from GCD
(at 1.0 A g−1) Ref.
NiCo2O4 nanosheets Hydrothermal 1 M KOH 92.1 C g−1 [50]
NiCo2O4 nanoflowers Hydrothermal 6 M KOH 122.5 C g−1 [12]
NiCo2O4 nanosheets Co-precipitation 2 M KOH 145 C g−1 [51]
NiCo2O4 hollow spheres Hydrothermal 3 M KOH 171.2 C g−1 [45]
NiCo2O4 microspheres Co-precipitation 6 M KOH 112-202 C g−1 [52]
MnCo2O4 nanofibers Hydrothermal 1 M KOH 52 C g−1 [53]
Mn-doped NiCo2O4
nanoparticles Hydrothermal/Calcination 3 M KOH 204.3 C g−1 This study
Cycling stability: The cycling performance of the cobaltites was evaluated by repeating GCD measurements for 1000 cycles at a current density of 2 A g−1 for NMCO, which exhibited the highest specific capacity among the synthesized materials. The Cs of NMCO increases upon cycling and reaches the maximum at approximately the 50th cycle (Fig. 6f). This maximum corresponds to full activation of the cobaltite. After 1,000 consecutive cycles, the NMCO sample maintained 99 % of its initial Cs. This high capacitance retention indicates that faradaic charging/discharging reactions in the NMCO is highly reversible. The overall electrochemical performance of the NMCO clearly demonstrates that it is attractive for supercapacitor applications and that its composition is critical for obtaining a large capacitance.
EIS analysis: EIS analysis was conducted to assess the electrochemical behavior of the electrode materials, and the results are presented in Fig. 7. In the high-frequency region, the intercept of the semicircle in EIS spectra with the real axis depicts the equivalent series resistance (ESR), which
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is contributed from several factors including the resistance of the electrode material/current collector, the resistance of the bulk electrolyte solution, and the resistance of the electrode material[55]. Since we used the same procedure for the preparation of electrodes and the identical geometrical arrangement of the electrochemical cell in EIS measurements, the difference in ESR is mainly originated from the resistance of the electrode material. As shown in the inset of Fig. 7 and Table S2, the ESR of NCO, MCO, and NMCO are 0.702, 0.663, and 0.649 , respectively. Here, NMCO exhibited the lowest ESR, which is agree well the maximum Cs according to the CV and GCD results.
In addition, NMCO might have unique MnO bondings and NiCo2O4MnCo2O4 interfaces which provide additional redox-active sites for charge storage. Moreover, EIS results also indicated that the NMCO has the lowest ESR. Therefore, Mn doping is beneficial for enhancing the performance of NiCo2O4 supercapacitor electrodes.
0 40 80 120 160 200
0 100 200 300 400 500
-Z" (Ohm)
Z' (Ohm) NCO
NMCO MCO
0.64 0.67 0.70 0.73 0.76 0.79 0.00
0.06 0.12 0.18 0.24 0.30
-Z" (Ohm)
Z' (Ohm)
Figure 7. Overall Nyquist plots of NCO, NMCO, and MCO. Inset: Enlarged Nyquist plots in the high-frequency region.
Electrochemical performance of the solid-state supercapacitor made from NMCO
To further evaluate the practical applicability of the NMCO materials, we constructed an all- solid-state, symmetric supercapacitor with NMCO as the active material and PVA–KOH as the gel electrolyte. The CV curves of the supercapacitor device recorded at different scan rates (Fig. 8a) exhibit a quasi-rectangular shape, and their internal areas increase with increasing scan rate, indicating that the device possesses pseudocapacitive behavior and that the faradaic reactions on its electrode surfaces are fast. The inset in Fig. 8a shows an image of the actual device during testing.
The GCD profiles measured at current densities of 0.1 to 2.0 mA cm−2 (Fig. 8b) are nearly symmetric, reflecting the electrochemical reversibility of the supercapacitor device. The areal capacitance of the supercapacitor device was calculated from the GCD measurements; the results are shown in Fig. 8c.
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Remarkably, the areal capacitance only decreased ca. 55% (from 25.07 to 11.2 mF cm−2) as the current density was increased 20-fold (from 0.1 to 2.0 mA cm−2), which is an indication of excellent performance at high current density. The relationship between the power density and energy density of the supercapacitor device (Ragone plot) was calculated from GCD profiles; the results are shown in Fig. 8d. Our supercapacitor device delivers an energy density of 0.87 Wh cm−2 at a power density of 25 W cm−2, and 0.39 Wh cm−2 at a high-power density of 500 W cm−2. The energy density of our device is several times higher than that of ZnO/MnO2 [56], Mn3(PO4)2/graphene [17], NiCoSx/Cu/Ni [57], graphene fiber [58], carbon nanotube (CNT) fiber [49] and is comparable to that of graphene oxide/polyaniline (GO/PANI) [48]. Although the energy density of our device is slightly lower than that of NiO/MnO2 [59] and carbon-based hybrids such as mesoporous carbon/CNTs) [47], rGO/CNTs [60], Co3O4/CNTs [14], and carbon–carbon composites [47], its power density is one to two orders of magnitude higher than those of the aforementioned hybrids. In comparison to MnCo2O4/Ni/Cu [61], NiCo(OH)x/Ni/C [62], and MnCo(OH)x/NiO/Ni [63], our device has nearly comparable powder density but lower energy density. Therefore, combining NMCO with other metal/metal oxides could be a promising route for improvement of its energy density, especially for high power-supplying applications. Long-term GCD test of the supercapacitor device at 1.0 mA/cm2 (Fig. S4) reveals a capacity retention of 98.1 % after 1000 cycles, demonstrating its excellent stability.
0.0 0.1 0.2 0.3 0.4 0.5
-4 -2 0 2 4 6
Current (mA)
Potential vs. Ag/AgCl (V)
30 mV/s 20 mV/s 10 mV/s
0.0 0.5 1.0 1.5 2.0
0 4 8 12 16 20 24
Areal capacitance (mF/cm2 )
Current density (mA/cm2)
0 70 140 210 280 350
0.0 0.1 0.2 0.3 0.4 0.5
Potential vs. Ag/AgCl (V)
Time (sec)
0.1 mA/cm2 0.25 mA/cm2 0.5 mA/cm2 1 mA/cm2 2 mA/cm2
(a) (b)
(c) (d)
0.1 1 10
1 10 100 1000
Power density (W cm-2 )
Energy density (Wh cm-2)
ZnO/MnO2
Graphene fiber CNT fiber
Mn-doped NiCo2O4 (This work) Mn3(PO4)2/
graphene
C-C composite Co3O4/CNT
C/CNT rGO/CNT
NiO/MnO2 MnCo(OH)x/NiO/Ni
NiCo(OH)x/Ni/C MnCo2O4/Ni/Cu
NiCoSx/Cu/Ni
GO/PANI
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Figure 8. Electrochemical performances of the symmetric supercapacitor device: (a) CV curves (inset: a photo of the device); (b) GCD curves; (c) areal capacitance vs. current density; and (d) Ragone plot. The mass loading of active material on each electrode was approximately 10 mg cm−2.
4. Conclusions
In summary, Mn-doped NiCo2O4 NPs have been successfully prepared by a facile hydrothermal/calcination route and thoroughly characterized. The XRD, SEM, TEM, STEM, and XPS results confirmed the spinel structure, polyhedral shape, and chemical composition of the as- prepared Mn-doped NiCo2O4 NPs. CV and GCD measurements revealed battery-type behavior of all as-synthesized cobaltites and nearly two-fold enhancement in capacity of Mn-doped NiCo2O4 NPs as compared to that of the pristine NiCo2O4 NPs, which indicated the positive role of Mn doping. Mn- doped NiCo2O4 NPs exhibited an impressive Cs of 417 C g-1 at scan rate of 10 mV s g−1, and 204.3 C g-1 at discharge current density of 1 A g−1. EIS analysis supported that the enhanced Cs is related to decreased ESR. Mn-doped NiCo2O4 NPs also showed remarkable capacitance retention of ~99 % after 1,000 cycles at current density of 2 A g−1. The all-solid-state symmetric supercapacitor device fabricated from Mn-doped NiCo2O4 NPs exhibited promising electrochemical performance, resulting in enhanced power density at a comparable energy density. The cost-effective synthesis and high electrochemical performance suggest that Mn-doped NiCo2O4 is a promising material for supercapacitors. Further developments are being made including deposition of NiCo2O4 NPs on three-dimensional conductive scaffold and assembly of an asymmetric device for enhanced capacity.
Associated content
Supporting Information
XPS survey spectra of all samples (Fig. S1), core-level spectra of NCO (Fig. S2) and MCO (Fig. S3), cycling test of supercapacitor device (Fig. S4), results of ICP analysis (Table S1), and EIS fitting parameters (Table S2).
Author information
Corresponding Authors
E-mail: tranvietthu1@duytan.edu.vn (T. V. T); sangeun@knu.ac.kr (S.-E. C)
Conflicts of interest
There are no conflicts of interest to declare.
Acknowledgments
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This research was partly supported by the National Research Foundation of Korea (NRF) grant funded by the Korea government (Ministry of Science, ICT & Future Planning) (NRF- 2017R1C1B2005470) (NRF-2018R1A4A1022260).
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