A one step processed advanced interwoven architecture of Ni(OH)₂ and Cu nanosheets with ultrahigh supercapacitor performance

Abstract

In this work, an interwoven nanoscale structure of Ni(OH)₂ and copper is successfully grown on Ni foam (NF) by using a one-step cheap chemical method. The concurrently formed structure with active Ni(OH)₂ growing together with the conductive Cu network facilitates fast electron transport throughout the electrode. As a result of enhanced conductivity by Cu and ultrathin nanosheet morphology of the active material, the Ni(OH)₂–Cu hybrid electrode delivers an ultrahigh areal capacitance (8.66 F cm⁻² at 1 mA cm⁻²), superior rate capability (79.1% capacitance retention at 20 mA cm⁻² and 61.8% capacitance retention at 50 mA cm⁻²vs. 1 mA cm⁻²) and outstanding cycling stability (98.5% capacitance retention after being charged/discharged at a series of current densities for 3500 cycles). Furthermore, the full cell, with Ni(OH)₂–Cu/NF as the positive electrode and reduced graphene oxide (RGO) as the negative electrode, delivers high areal capacitances and superior energy densities especially at high rates. The involved mechanisms are analyzed and discussed.

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1. Introduction

Supercapacitors (SCs), featured with fast charge–discharge rates, long cycle life time and high power density, have triggered tremendous interest in the energy storage field especially in the last few years.¹ SCs store energy based either on electrode/electrolyte interface charge separation, known as electric double-layer capacitors (EDLCs), or on reversible surface faradaic reactions, known as pseudocapacitors.² Due to relatively low specific capacitance and energy density, it is very difficult for EDLCs to satisfy the ever-growing demand for applications such as peak-power assistance in electric vehicles.³ Thus, tremendous attention has been focused on pseudocapacitors that can exhibit capacitances at least one order of magnitude higher than EDLCs.³

Transition metal oxides and hydroxides, such as NiO, Co₃O₄, Fe₃O₄, MnO₂, Ni(OH)₂, Co(OH)₂ and their binary systems, are among the most promising pseudocapacitor electrode materials for their various oxidation states, high electrochemical activity and abundance of sources in nature.⁴ However the poor conductivity and short mean free path of these semiconductor materials seriously hinder their realization of their high theoretical capacitance, especially at high charging/discharging rates.⁵ To address this problem, extensive research has been carried out to fabricate a hybrid structure of metal oxide/hydroxide with conductive materials, most of which are carbon based materials (graphene, carbon nanotubes, etc.,),^6–10 conductive polymers^11,12 and expensive metals such as Au^13,14 and Ag.^15,16 Copper, with conductivity ranking only second to silver and of low cost, however, has not been widely studied for conductive reinforcement in oxide/hydroxide composite design.

The existing technologies for fabricating hybrids with conductive reinforcement usually involve multi-step procedures: the synthesis of conductive nanostructure cores or skeletons (such as carbon nanotubes, Co₃O₄ nanowires, etc.,) followed by the growth of active material shells.¹⁷ The problems of a multi-step process include the possible core surface contamination or change prior to the growth of the active material shells, which may affect the electrical properties of the final products arising from the core–shell interface. Also, the multi-step process will result in an increase in the production cost and poor utilization of space due to the existence of empty regions among the core–shell structures. It will be beneficial if the hybrid structure of active material and conductive reinforcement can be synthesized through a one-step process.

Furthermore, the hydrothermal method, a popular method for the synthesis of metal oxide/hydroxide due to the convenient operation and ultrafine crystallization of the products, has been reported to rely on precipitants, such as alkali sources,^18,19 oxidants^7,9,20 and toxic solvents,⁴ for OH⁻ sources. To the best of our knowledge, a clean and green hydrothermal method purely based on the reaction between metal precursors and water to produce a hybrid structure of hydroxide and metal network has not been reported.

In this paper, we fabricated one special interwoven structure of ultrathin Ni(OH)₂–Cu nanosheets together with a conductive Cu layer growing on NF. Notably, such a favourable structure is achieved with a facile, simple and totally green one-step hydrothermal process with only nickel salt, copper salt and water as precursors. In the as-obtained hybrid film, Ni(OH)₂ and Cu are firmly connected with each other. Benefiting from such an architecture and nano-scale morphology, the as-obtained Ni(OH)₂–Cu hybrid film exhibits a high capacitive performance and superior energy density. Especially the nano-scale conductive copper network and the clean interface between the core and shell provide fast electron transportation paths, making high performance possible even at high charge/discharge rates.

2. Experimental section

2.1 Synthesis of Ni(OH)₂–Cu on NF

All the chemicals are of analytical grade and used without further purification. 262.9 mg NiSO₄·6H₂O, and 30 mg CuSO₄·5H₂O were added to 35 mL of deionized water (DI water). The solution was magnetically stirred for 15 min and then transferred to a 45 mL Teflon-lined stainless steel autoclave. 2 cm × 2 cm NF, pretreated by 20 min of sonication in acetone, ethanol and DI water, respectively, was immersed into a Teflon liner. Then the autoclave was sealed and transferred to an oven for 5 h for the hydrothermal process to take place at 140 °C. After the completion of the hydrothermal process, the substrate was collected, rinsed with DI water several times and dried at 60 °C for 12 h.

2.2 Fabrication of the asymmetric supercapacitor (ASC) full cell

The asymmetric supercapacitor is constructed with Ni(OH)₂–Cu/NF as the positive electrode, reduced graphene oxide (RGO) as the negative electrode, and 2 M KOH as the electrolyte. The RGO negative electrode was prepared by mixing 80 wt% RGO (Graphene Supermarket), 10 wt% carbon black and 10 wt% PTFE and spreading the mixture onto 2 cm × 2 cm NF. The mass loading of the RGO electrode was adjusted based on the principle of Q₊ = Q₋, where Q₊ is the charge stored in the positive electrode, Q₋ is the charge stored in the negative electrode. Q₋ was calculated according to the gravimetric capacitance of the negative electrode measured in the three-electrode configuration.

2.3 Characterization

The morphology and composition of the sample were examined by using a scanning electron microscope (SEM, Zeiss SUPRA40) equipped with an energy dispersive X-ray spectrometer (EDS) and transmission electron microscope (TEM, JEOL 100CX 2010F), which was also used for acquiring the selected area electron diffraction (SAED) patterns. The crystal structure was determined by X-ray diffraction (XRD) (BRUKER AXS, Cu, K = 0.154060 nm) at 40 kV and 40 mA.

2.4 Electrochemical measurements

Electrochemical measurements of the Ni(OH)₂–Cu/NF sample were carried out on an electrochemical workstation (PARSTAT MC), using a three-electrode mode with the as-fabricated hybrid as the working electrode, Pt wire as the counter electrode and saturated calomel electrode (SCE) as the reference electrode. 2 M KOH was used as the electrolyte. Cyclic voltammetry (CV) curves were obtained within the potential range of 0 V–0.5 V at various scan rates (1 mV s⁻¹–20 mV s⁻¹). Charge–discharge performances were tested at constant current densities from 1 mA cm⁻² to 50 mA cm⁻². In the cycling test, the sample was charged and discharged at a series of current densities in the sequence of 40 mA cm⁻², 30 mA cm⁻², 20 mA cm⁻², 30 mA cm⁻² and 40 mA cm⁻², with 3500 cycles in total. Electrochemical impedance spectroscopy (EIS) was performed by applying an AC voltage with a perturbation amplitude of 5 mV versus the open circuit in the frequency range from 0.01 Hz to 100 kHz.

The electrochemical properties of the ASC were investigated with a two-electrode configuration using 2 M KOH as the electrolyte. CV curves were obtained within the potential range of 0 V–1.5 V at various scan rates (2 mV s⁻¹–30 mV s⁻¹). Charge–discharge performances were tested at constant current densities from 1 mA cm⁻² to 50 mA cm⁻². 3600 cycles of cycling stability test were carried out at the current densities of 40 mA cm⁻², 30 mA cm⁻², 20 mA cm⁻², 30 mA cm⁻² and 40 mA cm⁻² in sequence.

3. Results and discussion

3.1 Synthesis of a Ni(OH)₂–Cu hybrid electrode

In this report, we will show that by using a single-step hydrothermal method (see Fig. 1(a) and experimental section), Ni(OH)₂ and Cu hybrid is formed (see Fig. 1(b)). The hybrid film is composed of two parts: a Cu nanoparticle layer at the bottom and an upper layer of interwoven Ni(OH)₂ and Cu nanosheets. This interesting architecture, with a nano-scale conductive Cu network spreading all over Ni(OH)₂, enables fast electron transportation throughout the whole electrode. It shows great potential as a fast charging/discharging SC electrode material. The Ni(OH)₂ part in this hybrid is formed due to the hydrolysis effect (see eqn (1)). The zero-valent metallic Cu might be formed from a replacement reaction as shown in eqn (2). The replacement reaction can occur because the zero-valent Ni substrate has a lower oxidation potential compared to that of Cu. The loss of Ni from the NF substrate is evidenced from the unreasonably high gravimetric capacitance of 12 371.4 F g⁻¹ (at 1 mA cm⁻²) when the mass of the active material is calculated by using the weight gain of the sample after the single-step hydrothermal synthesis. Since the substrate takes part in the reaction and the traditional way of measuring the amount of active material will overestimate the gravimetric capacitance, areal capacitance is utilized to evaluate the electrode's performance in this report.

NiSO₄ + 2H₂O → Ni(OH)₂ + H₂SO₄ (1)

Ni + CuSO₄ → NiSO₄ + Cu (2)

Fig. 1 Schematic illustration of the (a) one-step hydrothermal method; (b) structure of Ni(OH)₂–Cu hybrid.

Fig. 2 shows the (a) plan-view and (b) cross-section SEM and EDS elemental mapping images of the as-synthesized film on the NF substrate. It can be seen from the Cu mapping image in Fig. 2(a) that copper is interconnected. A comparison of the Cu and O mapping images reveals that Cu appears in oxygen deficient regions generally, for example, regions (i) and (ii) in Fig. 2(a). Such a correspondence is an indication that Cu exists as copper metal rather than copper oxide, which is later proved true from the XRD pattern shown in Fig. 3. Nickel appears everywhere as seen in the Ni mapping image in Fig. 2(a). These observations suggest an interwoven architecture of Ni(OH)₂ and Cu, which can be further proved from the cross-sectional view in Fig. 2(b). From the cross-section SEM and elemental mapping images in Fig. 2(b), we can see an inner copper nanoparticle layer on the Ni substrate; furthermore, interconnected copper is distributed in the nickel hydroxide matrix across the upper layer. A comparison of Cu and O elemental images reveals that the Cu regions generally correspond to O deficient regions (for example, regions (iii) and (iv)), also indicating that copper exists as Cu metal rather than oxide/hydroxide. As seen in region (iii), the part of bright flower-like nanosheets are rich in Cu and poor in O and Ni, suggesting flaked Cu in morphology. The plain-view and cross-section SEM and elemental mapping images reveal that a copper nanoparticle layer is first deposited on NF, followed by a layer of interwoven nickel hydroxides and copper nanosheets.

Fig. 2 EDS mappings of the Ni(OH)₂–Cu film on NF: (a) top view and (b) cross sectional view (taken from the knife-scratched sample surface). Blue circles are used to mark some Cu-rich regions.

Fig. 3 XRD pattern of the Ni(OH)₂–Cu hybrid on NF.

Fig. 3 displays the XRD pattern of the as-synthesized sample. Strong peaks belonging to metallic Ni (JCPDS 70-1849) and Cu (JCPDS 89-2838) can be seen from the graph. Ni peaks come from the NF substrate and Cu peaks suggest the formation of metallic copper during the hybrid film synthesis. The existence of metallic Cu explains why copper appears in oxygen deficient regions shown in Fig. 2. The signal of nickel hydroxide in this plot is very weak due to the very strong Cu and Ni signals.

Fig. 4 shows the flaked morphology of the hybrid film in low and high magnification SEM images. A good coverage on the NF substrate by the as-fabricated nanosheets can be seen from Fig. 4(a). As exhibited in Fig. 4(b), the outer hybrid film is mainly comprised of geometrically sheet-like 2D structures with thickness at a nanoscale level. As the charge storage mechanism of pseudocapacitor is mainly based on the surface/near-surface reaction, this morphology of porous ultrathin nanosheets is among the most favorable architectures for SC electrode materials owing to the large surface area and high exposure to electrolyte ions.

Fig. 4 SEM image of the Ni(OH)₂–Cu film on NF: (a) low magnification; (b) high magnification.

The Ni(OH)₂ phase in the sample is evidenced from Fig. 5. From Fig. 5(a), the magnified XRD pattern of Fig. 3, (101) and (110) peaks of Ni(OH)₂·0.75H₂O (JCPDS 38-0715) are observed. Since these peaks are very weak, TEM and SAED are further employed to examine the phases of the nanosheets. As exhibited in Fig. 5(b), the as-formed nanosheets show a foldaway silk-like morphology with high electron transparency, indicating an ultrathin nature,³ which is consistent with the SEM observation. The SAED pattern of the nanosheets is shown in Fig. 5(c). The d-spacings derived from these symmetric ring/spots reveal that two sets of rings exist in the SAED pattern. One set can be indexed to Ni(OH)₂·0.75H₂O (JCPDS 38-0715) crystal planes of (101), (015), (110) and (113), and the other set to Cu (JCPDS 89-2838) crystal planes of (111), (220) and (311). Such results suggest the outer nanosheet phases of the sample to be Ni(OH)₂·0.75H₂O and metallic Cu. The ratio of these two phases in the upper nanosheet layers are measured by XPS (see Fig. S1 and ESI†). The atomic ratio of Ni to Cu element is 11.58: 0.68 ≈ 17.03. The corresponding weight ratio of the Ni(OH)₂ phase (Ni(OH)₂·0.75H₂O) to Cu phase is calculated to be 28.46.

Fig. 5 (a) XRD pattern of Ni(OH)₂–Cu on a magnified scale; (b) TEM image and (c) SAED pattern of Ni(OH)₂–Cu nanosheets scratched down from the substrate.

3.2 Electrochemical properties of the Ni(OH)₂–Cu hybrid electrode

To explore the electrochemical properties of the as-synthesized electrode material, electrochemical tests in three-electrode configuration were performed. For comparison, we have also examined the pure Ni(OH)₂ sample (SEM image is shown in Fig. S2†) prepared under the same experimental conditions but without adding the copper source. The morphologies of the Ni(OH)₂–Cu sample and the pure Ni(OH)₂ sample are quite similar, although the Ni(OH)₂–Cu sample appears slightly more porous. As seen in Fig. 6(a), the typical cyclic voltammetry (CV) curve of the Ni(OH)₂–Cu hybrid exhibits a pair of well-defined redox peaks, indicating a strong pseudocapacitive behavior of the hybrid material.⁴ The redox reaction corresponds to the reversible conversion between Ni(II) and Ni(III):

Ni(OH)₂ + OH⁻ ↔ NiOOH + H₂O + e⁻ (3)

Fig. 6 (a) CV curves of Ni(OH)₂–Cu and Ni(OH)₂ electrodes at a scan rate of 2 mV s⁻¹; (b) galvanostatic discharge curves of Ni(OH)₂–Cu at various current densities; (c) corresponding areal capacitances of Ni(OH)₂–Cu and Ni(OH)₂ electrodes as a function of current densities; (d) comparison of Nyquist plots of Ni(OH)₂–Cu and Ni(OH)₂ electrodes (the inset is impedance in the high frequency region).

Compared to the pure Ni(OH)₂ electrode, the CV curve of the Ni(OH)₂–Cu electrode shows an evidently larger area, and the specific capacitances of the two electrodes are calculated to be 3.2 F cm⁻² and 5.95 F cm⁻² accordingly. The prominent enhancement in areal capacitance of Ni(OH)₂–Cu compared with Ni(OH)₂ appears to be mainly attributed to the interwoven structure of metallic Cu and Ni(OH)₂ nanosheets. The metallic Cu layer formed at the bottom of the hybrid film on NF provides a high conducting path and low contact resistance for charge carriers. More importantly, the upper interwoven metallic copper in the film provides a highly-conductive network that enables fast transportation of charge carriers within the electrode and benefits fast redox reaction kinetics of the active material.

Fig. 6(b) plots a series of discharging curves of the Ni(OH)₂–Cu electrode tested at increasing current densities. The expected non-linear shapes of the discharge curves confirm the pseudocapacitive nature of the electrode. The corresponding areal capacitances (shown in Fig. 6(c)) are calculated from the discharging curves based on eqn (4):

where C_A (F cm⁻²) is the areal capacitance, I_d (mA cm⁻²) is the discharging current density, Δt (s) is the total discharging time and ΔV (V) is the total discharging potential range. Encouragingly, the Ni(OH)₂–Cu electrode exhibits excellent areal capacitances of 8.66, 7.95, 7.41, 7.1, 6.85, 6.34 and 5.29 F cm⁻² at current densities of 1, 2, 5, 10, 20, 30 and 50 mA cm⁻², respectively. The result also suggests a good rate capability: 79.1% of the capacitance is retained when the discharge rate reaches 20 times that of the original 1 mA cm⁻². A very high capacitance of 5.29 F cm⁻² is still obtained at a high current density of 50 mA cm⁻², corresponding to 61.8% retention of capacitance at 1 mA cm⁻². As a comparison, we measured and obtained areal capacitances of 4.13 to 2.16 F cm⁻² from the Ni(OH)₂ sample at current densities from 1 to 20 F cm⁻². Notably, the corresponding capacitance retention is only 52.3% for Ni(OH)₂, much worse than that of the Ni(OH)₂–Cu sample. Such results reveal that the Ni(OH)₂–Cu hybrid film exhibits evidently enhanced specific capacitance and rate capability. This is probably due to the fact that the Cu network interconnects with Ni(OH)₂ nanosheets, facilitating more effective fast electron transport in the electrode.

To further understand the enhanced electron transportation capability of the Ni(OH)₂–Cu electrode, EIS analysis is performed on the Ni(OH)₂–Cu sample and Ni(OH)₂ reference (Fig. 6(d)). At very high frequencies, the intercept at the real axis (Z′) represents a combinational resistance of intrinsic resistance of the electrode material, contact resistance at the active material/current collector interface and ionic resistance of the electrolyte.²¹ The Ni(OH)₂–Cu sample exhibits a much smaller real axis intersection than Ni(OH)₂, indicating its significantly smaller internal resistance. The Ni(OH)₂–Cu electrode exhibits a much smaller depressed semicircle, which represents reduced charge-transfer resistance occurring in faradic reactions at the electrode–electrolyte interface. These results demonstrate that the Cu network in the active material helps to provide a favorable electron-transport pathway and improve the conductivity of the sample. In the low frequency area, the slope of the curve shows the Warburg impedance that is related to the electrolyte diffusion in a porous electrode and proton diffusion in host materials.²² As shown in the graph, the Ni(OH)₂–Cu electrode displays a more ideal straight line along the imaginary axis, indicating a lower diffusion resistance occurring in this electrode.

The specific areal capacitance of this sample is also compared with other Cu–Ni compound based electrodes reported in the literature in Table 1. The areal capacitances are calculated based on the mass loading and gravimetric capacitances provided in those papers. It can be seen that our Ni(OH)₂–Cu hybrid shows enormously enhanced capacitance, which is possibly due to its advanced structure.

Table 1 Comparison of areal capacitances of Ni, Cu based electrodes in references

No.	Material	Current density (mA cm^−2)	Areal capacitance (F cm^−2)	References
1	NiCu(OH)2CO3 nanowire on Cu foam	2.2	2.14	24
2	Ternary Ni–Cu–OH on the carbon nanofiber substrate	6	0.77	25
3	Nickel copper hydroxide (NCH) on the carbon fiber paper	2	2.88	26
4	Cu0.2Ni0.8O on Cu foam	5	2.97	27
5	Nickel copper oxide (NCO) nanowires on NF	2.5	2.24	28
6	Ni(OH) 2 –Cu hybrid on NF	2	7.95	Current work
		5	7.41
		10	7.1

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The cycling performance of the Ni(OH)₂–Cu electrode was evaluated by charge/discharge testing at a series of high current densities. As observed from Fig. 7, a slight increase in areal capacitance from 4.44 F cm⁻² to 4.54 F cm⁻² occurs during the first 160 cycles at 40 mA cm⁻², which corresponds to full activation of the electrode material as mentioned in several reports.^5,23 Then the capacitance goes through a slight decrease in each of the first three sections (700 cycles for each section) tested at reduced current densities, where a tendency shows up that smaller charging/discharging rate results in higher capacitance retention during the cycling test (90.5%, 95.3% and 97.1% retention after 700 cycles at 40, 30 and 20 mA cm⁻², respectively). Ultimately, the Ni(OH)₂–Cu electrode exhibits a capacitance of 4.47 F cm⁻² (at 40 mA cm⁻²) after 3500 cycles, corresponding to 98.5% retention of the highest capacitance achieved at 40 mA cm⁻², indicating an outstanding cycling stability.

Fig. 7 Cycling performance of the Ni(OH)₂–Cu electrode tested at various current densities.

To further evaluate the Ni(OH)₂–Cu electrode for real applications, the performance of the two-electrode asymmetric supercapacitor, with Ni(OH)₂–Cu as the positive electrode and RGO as the negative electrode, was tested. Fig. 8(a) shows typical CV curves of the ASC tested in a 2 M KOH electrolyte at various scan rates between 0 and 1.5 V. The clearly observed redox peaks indicate the pseudocapacitance contribution from the positive electrode.^29,30 The galvanostatic discharge curves acquired at different current densities are exhibited in Fig. 8(b). The nonlinearities of these discharge curves further confirm that the faradaic reaction occurred in the ASC. The specific areal capacitances of the ASC vs. various current densities were conducted and the corresponding results are shown in Fig. 8(c). A high areal capacitance of 2.48 F cm⁻² is achieved at the small current density of 1 mA cm⁻¹, while the capacitance retains 73% (1.81 F cm⁻²) and 61.7% (1.53 F cm⁻²) of the value at high current densities of 20 mA cm⁻² and 50 mA cm⁻², respectively. The results indicate a good performance of the ASC in both high specific capacitance and superior rate capability, which is mostly attributed to the advanced architecture of the positive electrode.

Fig. 8 (a) CV curves of Ni(OH)₂–Cu//RGO ASC at various scan rates; (b) galvanostatic discharge curves of Ni(OH)₂–Cu//RGO ASC at different current densities; (c) corresponding areal capacitances of Ni(OH)₂–Cu//RGO ASC as a function of current densities; (d) Ragone plots of Ni(OH)₂–Cu//RGO ASC and other Ni–Cu based ASCs from the literature.

Energy density and power density are two important parameters for characterizing the electrochemical performance of a supercapacitor. Based on the discharge curves, the areal energy density and power density can be calculated using the following equations:

where E (W h cm⁻²) is the energy density, I (A) is the discharge current, V(t) (V) is the discharge time, dt (s) is the time differential, A (cm²) is the area of the electrode, P (W cm⁻²) is the power density and Δt (s) is the discharge time. Fig. 8(d) depicts the Ragone plot of the as-fabricated Ni(OH)₂–Cu//RGO ASC and those reported in the literature listed in Table 1 with full cell data. The energy densities of the Ni(OH)₂–Cu//RGO ASC are 0.95, 0.9, 0.83, 0.75, 0.69 and 0.57 mW h cm⁻² at power densities of 2.01, 5.17, 10.28, 19.96, 29.06 and 44.78 mW cm⁻², respectively. As can be seen from Fig. 8(d), these energy densities are much higher than those of other Ni–Cu compound based ASCs, especially at high power densities. The results highlight the potential of the interwoven architecture of Ni(OH)₂–Cu for application in energy storage especially at high charge/discharge rates.

The cycling stability of the as-fabricated ASC was evaluated by performing 3600 cycles of the charge/discharge test at various current densities (see Fig. 9). An activation process of the electrode first takes place during the initial 80 cycles at 40 mA cm⁻² and the capacitance goes through an increase from 1.38 F cm⁻² to 1.68 F cm⁻². Then the capacitance suffers a minor decrease in each of the first two 720 cycles tested at 40 and 30 mA cm⁻², respectively. In the last three 720 cycles of testing, however, the capacitance of the ASC remains stable with no sign of further decrease. In the end, a capacitance of 1.43 F cm⁻² (85.1% of the highest capacitance achieved at 40 mA cm⁻²) is retained by the ASC after 3600 cycles, confirming its good cycling stability.

Fig. 9 Cycling performance of Ni(OH)₂–Cu//RGO ASC tested at various current densities.

4. Conclusion

In summary, the Ni(OH)₂–Cu hybrid electrode was synthesized through a facile and green one-step hydrothermal process. Only two metal salts and water were used as precursors without the need of adding alkali, oxidant or organic solutions. The as-fabricated electrode possesses an advanced architecture with the Cu nanoparticle layer at the bottom upon which grows an interwoven nanosheet layer of Ni(OH)₂ and Cu. Such a Ni(OH)₂–Cu hybrid electrode delivers an ultra-high areal capacitance of 8.66 F cm⁻² at 1 mA cm⁻², superior rate performance such that the capacitance of 6.85 and 5.29 F cm⁻² is retained when the current density goes up to 20 and 50 mA cm⁻², corresponding to 79.1% and 61.8% retention, respectively, and also outstanding cycling stability. Moreover, the as-obtained Ni(OH)₂–Cu//RGO ASC also exhibits high capacitive performance and superior energy densities especially at high power density. Therefore, the as-synthesized interwoven architecture of the Ni(OH)₂–Cu hybrid shows great potential in high-performance supercapacitor applications.

Acknowledgements

The support of Singapore Ministry of Education Academic Research Fund Tier 2 MOE Tier 2 MOE2013-T2-2-138, grant R-284-000-125-112 is appreciated.

References

1. J. Yan, Q. Wang, T. Wei and Z. Fan, Adv. Energy Mater., 2014, 4, 1300816.
2. Y. Wang and Y. Xia, Adv. Mater., 2013, 25, 5336–5342.
3. C. Yuan, J. Li, L. Hou, X. Zhang, L. Shen and X. W. D. Lou, Adv. Funct. Mater., 2012, 22, 4592–4597.
4. H. Chen, L. Hu, M. Chen, Y. Yan and L. Wu, Adv. Funct. Mater., 2014, 24, 934–942.
5. J. Kang, A. Hirata, H. J. Qiu, L. Chen, X. Ge, T. Fujita and M. Chen, Adv. Mater., 2014, 26, 269–272.
6. X. A. Chen, X. Chen, F. Zhang, Z. Yang and S. Huang, J. Power Sources, 2013, 243, 555–561.
7. D. P. Dubal, G. S. Gund, C. D. Lokhande and R. Holze, ACS Appl. Mater. Interfaces, 2013, 5, 2446–2454.
8. S. Min, C. Zhao, G. Chen and X. Qian, Electrochim. Acta, 2014, 115, 155–164.
9. J. Xu, S. L. Gai, F. He, N. Niu, P. Gao, Y. J. Chen and P. P. Yang, J. Mater. Chem. A, 2014, 2, 1022–1031.
10. L. L. Zhang, Z. Xiong and X. S. Zhao, J. Power Sources, 2013, 222, 326–332.
11. X. H. Xia, D. L. Chao, Z. X. Fan, C. Guan, X. H. Cao, H. Zhang and H. J. Fan, Nano Lett., 2014, 14, 1651–1658.
12. W. C. Jiang, D. S. Yu, Q. Zhang, K. L. Goh, L. Wei, Y. L. Yong, R. R. Jiang, J. Wei and Y. Chen, Adv. Funct. Mater., 2015, 25, 1063–1073.
13. J. Zhu, Z. Xu and B. N. Lu, Nano Energy, 2014, 7, 114–123.
14. Z. G. Zeng, H. J. Zhou, X. Long, E. J. Guo and X. H. Wang, J. Alloys Compd., 2015, 632, 376–385.
15. Y. H. Li, Z. Y. Wang and Y. F. Zhang, J. Alloys Compd., 2015, 644, 47–53.
16. H. Xia, C. Y. Hong, X. Q. Shi, B. Li, G. L. Yuan, Q. F. Yao and J. P. Xie, J. Mater. Chem. A, 2015, 3, 1216–1221.
17. Z. Tang, C. H. Tang and H. Gong, Adv. Funct. Mater., 2012, 22, 1272–1278.
18. J. Li, W. Zhao, F. Huang, A. Manivannan and N. Wu, Nanoscale, 2011, 3, 5103–5109.
19. Y. X. Xu, X. Q. Huang, Z. Y. Lin, X. Zhong, Y. Huang and X. F. Duan, Nano Res., 2013, 6, 65–76.
20. M. M. Wang, W. L. Ma, J. Y. Xue, F. M. Zhang and H. T. Cui, Phys. Status Solidi A, 2016, 213, 215–220.
21. X. Chen, C. Long, C. Lin, T. Wei, J. Yan, L. Jiang and Z. Fan, Electrochim. Acta, 2014, 137, 352–358.
22. L. Mei, T. Yang, C. Xu, M. Zhang, L. B. Chen, Q. H. Li and T. H. Wang, Nano Energy, 2014, 3, 36–45.
23. X. H. Xiong, D. Ding, D. C. Chen, G. Waller, Y. F. Bu, Z. X. Wang and M. L. Liu, Nano Energy, 2015, 11, 154–161.
24. X. Zheng, Y. Ye, Q. Yang, B. Geng and X. Zhang, Chem. Eng. J., 2016, 290, 353–360.
25. N. A. Alhebshi and H. N. Alshareef, Mater. Renew. Sustain. Energy, 2015, 4, 9.
26. L. Zhang and H. Gong, Sci. Rep., 2015, 5, 18108.
27. L. Y. Zhang and H. Gong, ACS Appl. Mater. Interfaces, 2015, 7, 15277–15284.
28. L. Zhang, C. Tang and H. Gong, Nanoscale, 2014, 6, 12981–12989.
29. C. D. Wang, J. L. Xu, M. F. Yuen, J. Zhang, Y. Y. Li, X. F. Chen and W. J. Zhang, Adv. Funct. Mater., 2014, 24, 6372–6380.
30. A. Pendashteh, S. E. Moosavifard, M. S. Rahmanifar, Y. Wang, M. F. El-Kady, R. B. Kaner and M. F. Mousavi, Chem. Mater., 2015, 27, 3919–3926.

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Footnote

† Electronic supplementary information (ESI) available. See DOI: 10.1039/c6ta03336a

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