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Communication

In-Site Growth of Efficient NiFeOOH/NiFe-LDH Electrodes: A Streamlined One-Step Methodology

by
Jing Ning
1,2,3,†,
Li Xu
1,2,3,4,†,
Wei Xu
4,
Guizhen Li
4 and
Wen Zhang
1,2,3,*
1
School of Chemical Engineering and Technology, Tianjin University, Tianjin 300350, China
2
National Industry-Education Integration Platform of Energy Storage, Tianjin University, Tianjin 300350, China
3
Tianjin Key Laboratory of Membrane Science and Desalination Technology, Tianjin 300350, China
4
Tianjin Mainland Hydrogen Equipment Co., Ltd., Tianjin 301609, China
*
Author to whom correspondence should be addressed.
†
These authors contributed equally to this work.
Chemistry 2024, 6(2), 312-322; https://doi.org/10.3390/chemistry6020017
Submission received: 28 February 2024 / Revised: 23 March 2024 / Accepted: 28 March 2024 / Published: 31 March 2024
(This article belongs to the Section Electrochemistry and Photoredox Processes)
Browse Figures
Versions Notes

Abstract

:
Oxygen evolution reactions (OER) are often the decisive step in determining the water electrolysis rate. The first row of transition metals and their derivatives, represented by Ni and Fe, have attracted much attention due to their excellent OER performance. Here, we develop a one-step strategy for preparing oxygen-evolving electrodes, in which the NiFeOOH-modified NiFe layered double hydroxide (NiFe-LDH) nanosheet is supported by nickel foam. At 100 mA·cm−2, the overpotential of NiFeOOH-NiFe-LDH was just 227 mV, and the duration times were over 200 h in 1 mol·L−1 KOH. Furthermore, the co-existence of LDH and hydroxyl oxides helps the oxygen evolution reaction. These results suggest the potential for this synthesis strategy to provide a low-cost, highly active OER electrocatalyst for industrial water splitting.

1. Introduction

Hydrogen energy is a great choice to replace fossil energy because of its advantages of being green, clean, renewable, and easy to transport [1,2,3,4,5]. Among the many ways to produce hydrogen, alkaline electrolytic water is a promising method because of its lower cost and extended stability [6,7,8,9,10]. There are two electrocatalytic reactions, the hydrogen evolution reaction (HER) and oxygen evolution reaction (OER). The OER at the anode side is a four-electron reaction with slow kinetic rates [11,12,13,14,15,16]. The efficiency of water splitting is mainly dependent on the OER. Therefore, decreasing the OER overpotential becomes the bottleneck to promote the process of alkaline electrolytic water.
The first-row transition metal derivatives, including their oxides [17], hydroxides [18], phosphides [19], sulfides [20], selenides [21] and nitrides [22], have demonstrated a catalytic activity for OER reaction. Many studies have shown that electrodes prepared from the transition metal elements of Ni and Fe have good OER catalytic properties and good prospects for application. In particular, Ni- and Fe-based layered double hydroxides (LDHs) have been considered by many researchers as one of the most promising OER electrodes due to their adjustable electronic configuration, flexible chemical composition, and exchangeable interlayer construction [23,24,25,26].
When participating in water electrolysis, the LDH also generates hydroxyl oxides, an intermediate, for the OER catalytic process. Many studies have attempted to prepare hydroxyl oxides as the OER catalysts for efficient electrolytic water. However, the preparation processes of hydroxyl oxides are complicated and often require several reaction steps. Most current preparation methods will first form nano-arrays of metal or metal derivatives on a nickel foam substrate, which are further oxidized to hydroxyl oxides by anodic electro-oxidation or chemical means [2,27,28]. A phase interface exists between the original nano-arrays and the hydroxyl oxides. The electron transfer across the phase interface is also believed to be a decisive factor in promoting electrolytic water catalysis [2]. Therefore, there is a need to develop novel and simple synthesis strategies for the fabrication of hydroxyl oxides.
In this work, hydroxyl oxide-based OER electrodes were prepared by means of a simple one-step method. NiFeOOH-NiFe-LDH nanosheets were synthesized by immersing nickel foam (NF) in a precursor solution containing nickel ions, iron ions and urea, and heated at 75 °C for 12 h at atmospheric pressure. During this process, the NiFeOOH can be generated on the surface layer of NiFe-LDH supported by NF and accelerate up the OER reaction process. The nanosheets of the two substances are laminated to each other, creating a large number of phase interfaces that help electrons transfer faster. With the overpotential of 0.23 V at 100 mA·cm−2, the NiFeOOH-NiFe-LDH exhibits remarkable OER efficiency. The electrode also shows good stability, holding steady in 1.0 mol/L KOH for at least 120 h at 200 mA·cm−2.

2. Materials and Methods

2.1. Materials

The nickel foam (NF) was obtained from Tianjin Leviathan Science & Technology Co., Ltd. (Tianjin, China), with a thickness of 1.0 mm and a porosity of 98%. Ethanol (AR, 99.5%) was purchased from Tianjin Yuanli Chemicals Co., Ltd. (Tianjin, China); Tianjin Hience Optech Technology Company (Tianjin, China) provide Ni(NO3)2·6H2O and CO(NH2)2. Shanghai Aladdin Biochemical Technology Co., Ltd. (Shanghai, China) offered Fe(NO3)3·9H2O and KOH. Industrial titanium-based iridium oxide electrodes (Ti/IrO2) were purchased from Kunshan Yiwanlin Electronic Technology Co., Ltd. (Kushan, China). Analytical grade reagents were utilized as supplied. Deionized water was used to prepare the aqueous solution.

2.2. Materials Synthesis

NF was used to support NiFeOOH-NiFe-LDH nanosheets via a straightforward one-step water bath process. In brief, a 3 cm × 4 cm area of NF was sonicated in 3 mol/L hydrogen chloride (HCl) solution, and deionized water and ethanol were used to remove the surface nickel oxides and organic molecules. To synthesize NiFeOOH-NiFe-LDH/NF, the solution was made by dissolving 178.0 mg Ni(NO3)2·6H2O, 122.4 mg Fe(NO3)3·9H2O (the atomic ratio of Ni: Fe is 2: 1) and 106.2 mg CO(NH2)2 in 50 mL deionized water under stirring for 30 min. The cleaned NF was added into this beaker and kept at 75 °C over a period of 12 h. After the sample had completely fallen to room temperature, it was taken out of the beaker. After cooling down to room temperature and washing by deionized water and alcohol, the NiFeOOH-NiFe-LDH was obtained. The sample was dried under 60 °C for 3 h, marked as NiFeOOH-NiFe-LDH.
NiFe-LDH/NF was prepared in the same precursor solution, comprising 178.0 mg Ni(NO3)2·6H2O, 122.4 mg Fe(NO3)3·9H2O and 106.2 mg CO(NH2)2 in 50 mL of deionized water. They were kept in a sealed PTFE-lined stainless steel at 120 °C for 12 h. The obtained product was denoted as NiFe-LDH. The empty NF electrode and the purchased industrial Ti/IrO2 electrode were also used as the control groups.
The synthesis methods for electrodes is illustrated in Figure S1.

2.3. Materials Characterization

The structural information of NiFeOOH-NiFe-LDH were studied by an X-ray diffraction (XRD, Bruker D8, Bruker Corporation, Karlsruhe, Germany). Microstructure and elemental distribution are characterized by scanning electron microstructure (SEM with EDS, Apreo S LoVac, Thermo Fisher Scientific, Hillsboro, Oregon, United States) and transmission electron microscopy (TEM, JEM 2100F, JEOL Ltd., Tokyo, Japan). The chemical state data were obtained via X-ray photoelectron spectroscopy (XPS, Thermo 250Xi, Thermo Fisher Scientific, Waltham, MA, USA). The composition of substances was further verified by Raman spectroscopy (Raman spectra, Horiba, Horiba Jobin Yvon, Palaiseau, France).

2.4. Electrochemical Measurements

The OER activity in 1 mol·L−1 KOH was evaluated using an AUTOLAB PGSTAT302N workstation, where NiFe-LDH, NF and Ti/IrO2 were used directly as the working electrode, and the Hg/HgO was the reference one and the Pt foil electrodes were the counter electrode. Reversible hydrogen electrode (RHE) was used to calibrate the potential. The calibrated equation is ERHE = EHg/HgO + 0.0591 × pH + 0.098 V. In addition, the iR drop of each polarization curve was compensated using an electrochemical workstation.
Linear sweep voltammetry (LSV) was collected under the rate of 5 mV·s−1. Electrochemical impedance spectroscopy (EIS) was tested at 1.42 V Versus RHE (VRHE) within the frequency from 105 Hz to 0.01 Hz with the amplitude of 5 mV. Electrochemical surface areas (ECSA) were studied in a non-Faradic potential window. The potentials were between 1.275 VRHE and 1.355 VRHE and the scan rates between 40 and 200 mV·s−1. Chrono potentiometric measurements were made for 120 h at 100 and 200 mA·cm−2 in order to test durability. The geometric area of the NF was used to normalize the current density.

3. Results

3.1. Structural and Morphological Characterizations of the Electrocatalysts

NiFeOOH-NiFe-LDH prepared in a one-step process was obtained by placing the treated nickel foam directly into a beaker with precursor solution and heating the beaker directly in an oven at 75 °C for 12h (Figure 1). As the temperature rises, the dissolved urea slowly decomposes and breaks down to form an alkaline environment. In the early stage, NiFe-LDH crystals nucleate and grow attached to the nickel foam to form nanosheets. Then, with the decomposition of urea, the metal ions foam hydroxyl oxides attached to nanosheets.
XRD tests were performed on the NiFeOOH-NiFe-LDH and NiFe-LDH samples attached to nickel foam surface (Figure S2). However, due to the low content of the surface catalytic layer, the diffraction peaks of the catalytic layer cannot be observed. Therefore, the ultrasonic oscillation was used to strip the catalytic layer from nickel foam, and the XRD of exfoliated samples are shown in Figure 2a. The diffraction peaks at 11.4°, 22.9°, 38.9° and 61.2° are the (003), (006), (015) and (113) lattice planes of the NiFe-LDH sample, respectively [23,24]. The diffraction peaks at 34.9°, 40.2°, 53.4° and 62.7° are the (110), (101), (102) and (110) facets of (Fe0.67Ni0.33)OOH [28], respectively.
The surface of catalysts was obtained via the SEM. In Figure 2b,c, the SEM images showed that the interconnected ultrathin nanosheets agglomerated into nanocluster structures, growing vertically on the NF surface. The SEM images at low magnification are shown in Figures S3 and S4. The cross-sectional view of the catalyst layer is shown in Figure S5, and the thickness of the NiFeOOH-NiFe-LDH/NF and NiFe-LDH/NF catalyst layers is approximately 3 μm.
The transmission electron microscopy (TEM) images suggest that the nanosheet thickness is thinner, indicating that more reactive sites can be exposed (Figure 2d). In TEM images (Figure 2e and Figure S6), there are visible lattice stripes with the spacing of 0.224 nm, due to the (101) plane of (Fe0.67Ni0.33)OOH [28]. The lattice spacing of 0.260 nm is due to the (012) lattice plane of NiFe-LDH [29]. Selected area electron diffraction (SAED) patterns showing diffraction rings (Figure 2f) were also consistent with the above findings. The TEM images and the related EDS mapping (Figure 2g) demonstrated that Ni, Fe and O were uniformly distributed on the nanosheets.
Phase detection was tested using Raman spectroscopy in Figure 3a to verify the substance composition further. The characteristic NiFe-LDH peaks at 453 cm−1 and 536 cm−1 are due to the vibration of the Ni(II)-O bond in Ni(OH)2 [30]. The peaks at the corresponding positions in NiFeOOH-NiFe-LDH are 470 cm−1 and 544 cm−1, which are considered to be the result of the Ni(III)-O in NiOOH and Ni(II)-O in Ni(OH)2 [31,32]. Two strong peaks at 308 cm−1 and 679 cm−1 were detected, corresponding to Fe-O’s bending and stretching vibrations in FeOOH, respectively [33,34].
XPS was utilized to study compositions of the NiFeOOH-NiFe-LDH and NiFe-LDH samples. In Figure 3b, the XPS reveals the existence of Ni, Fe and O, which is in accordance with EDS mapping images. The prominent Ni 2p peaks in Figure 3c are at 855.3 eV and 872.7 eV, identified as the Ni 2p3/2 and Ni 2p1/2 peaks, respectively. The typical satellite of Ni 2p3/2 and Ni 2p1/2 are the broad peaks at 861.4 and 879.7 eV [35]. The Ni 2p peak fitting analysis indicates the existence of two states of Ni 2p, Ni2+( t 2 g 6 e g 2 ) and Ni3+ ( t 2 g 6 e g 1 ), which can be attributed to Ni species in Ni(OH)2 and NiOOH, respectively. It is shown in Figure S7 that the prepared sample NiFeOOH-NiFe-LDH contains a high percentage of Ni3+ (30.8%). Many reports have shown that the introduction of high-valent Ni can effectively enhance the electron-withdrawing effect, and the electronic configuration of Ni3+ ( t 2 g 6 e g 1 ) is more favorable to the OER by forming σ-bonds with adsorbed oxygen [11,36].
Fe 2p in Figure 3d shows the peaks of NiFeOOH-NiFe-LDH at 710.3 eV and 723.6 eV, with the satellites at 717.0 eV and 732.6 eV, corresponding to the Fe 2p3/2 and Fe 2p1/2, respectively. The peak fitting of NiFeOOH-NiFe-LDH suggests that Fe3+ exists in different compositions. The peak located at 712.1 eV is attributed to FeOOH, and the peak at 710.2 eV is attributed to Fe(OH)3. These results agree with the finding of XRD [37,38,39].
The split-peak fitting of the O 1s spectra in Figure 3e shows that the lattice oxygen (M-O) is at 529.6 eV, the metal hydroxide (M-OH) is at 531.4 eV and the oxygen vacancy (Ov) is at 533.1 eV. It is clear from Figure 3f that the percentage of M-O of NiFeOOH-NiFe-LDH is considerably higher than the percentage of NiFe-LDH, suggesting the generation of hydroxyl oxides in NiFeOOH-NiFe-LDH.
NiFeOOH-NiFe-LDH has more oxygen vacancies than NiFe-LDH (Figure S5), suggesting the presence of high valence Ni in NiFeOOH-NiFe-LDH, which is beneficial to the OER reaction [40,41].

3.2. Electrochemical Test Performance

By means of a three-electrode setup, we investigated the electrochemical OER performance of various electrodes in 1 mol·L−1 KOH solution. Commercial IrO2/Ti and NF were also tested for comparison. In Figure 4a, the onset potential of NiFeOOH-NiFe-LDH at 1 mA·cm−2 was 1.337 V. NiFeOOH-NiFe-LDH has an overpotential of only 227 mV at 100 mA·cm−2, which was not only the lowest overpotential among the electrodes (Figure 4b) but also better than recently reported catalysts (Table 1).
Additionally, the kinetic of electrodes was evaluated by calculating the Tafel curves based on the polarization curves. In Figure 4c, NiFeOOH-NiFe-LDH has the fastest OER reaction kinetics and lowest Tafel slope of 35.0 mV·dec−1. The enhanced kinetics are verified by the electrochemical impedance (Figure 4d) characterization, with the charge transfer resistance (Rct) of NiFeOOH-NiFe-LDH being the lowest among all of these samples (6.343 Ω·cm2, Table 2).
CV curves based on the non-Faraday region of 1.275 V–1.355 V vs. RHE were calculated from the ECSA (Figure 5a–d, Table S1). In this way, the corresponding double-layer capacitance (Cdl) can be calculated for different catalysts. In particular, the Cdl of NiFeOOH-NiFe-LDH is 7.19 mF·cm−2, more significant than those of the other electrodes (Figure 5e). In comparison to NiFe-LDH, the surface area of NiFeOOH-NiFe-LDH is effectively increased. In 1 mol·L−1 KOH, stability tests of NiFeOOH-NiFe-LDH were conducted at 100 mA·cm−2 for 200 h (Figure 5f). It is observed that even after 200 h, the catalytic activity of NiFeOOH-NiFe-LDH remains at a high level, demonstrating its remarkable stability. The excellent catalytic activity of NiFeOOH-NiFe-LDH can be attributed to NiFeOOH serving as an intermediate in the OER mechanism, which promotes faster reaction rates.

4. Conclusions

In this study, we explored a strategy to prepare the NiFeOOH/NiFe-LDH electrode by in-site growth of NiFeOOH-decorated NiFe-LDH nanosheets on NF support and compared it with NiFe-LDH (Table S2). Mechanistic analysis showed that the presence of the reaction intermediate NiFeOOH promoted the rapid occurrence of OER. The prepared NiFeOOH-NiFe-LDH has a low overpotential of 227 mV while providing 100 mA·cm−2 current density. It also has a durability of up to 120 h in operation at 200 mA·cm−2. The outstanding electrochemical performance can be attributed to its unique composition and nanostructure and the abundance of phase interfaces that enhance the exposure of catalytically active sites. This work provides a new strategy for preparing NiFe-based electrodes for OER reactions.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/chemistry6020017/s1. Figure S1: synthesis methods for experimental electrodes; Figure S2: SEM images of NF; Figure S3: (a) SEM images and (b) TEM image of NiFe-LDH/NF; Figure S4: calculation of lattice stripes corresponding to two phase frame selection positions; Figure S5: percentage of Ni2+ and Ni3+ of NiFeOOH-NiFe-LDH; Figure S6: Calculation of lattice stripes corresponding to two phase frame selection positions; Figure S7: Percentage of Ni2+ and Ni3+ of NiFeOOH-NiFe-LDH; Table S1: The ECSA and Cdl values of different catalysts; Table S2: The comparisons between NiFeOOH-NiFe-LDH and NiFe-LDH.

Author Contributions

Conceptualization, J.N. and W.Z.; methodology, J.N., L.X. and W.X.; Validation, J.N. and L.X. and G.L.; formal analysis, J.N. and L.X.; investigation, J.N., L.X. and G.L.; resources, G.L. and W.X.; data curation, J.N.; writing—original draft preparation, J.N. and L.X.; writing—review and editing, W.Z.; visualization, J.N., G.L. and W.X.; supervision, W.Z. and L.X.; project administration, L.X.; funding acquisition, L.X. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the National Key R&D Program (No. 2021YFB4000303).

Data Availability Statement

The data presented in this study are available on request from the corresponding author. The data are not publicly available due to further research is being carried out.

Conflicts of Interest

Authors L.X., W.X. and G.L. were employed by company Tianjin Mainland Hydrogen Equipment Co., Ltd. The remaining authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

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Figure 1. Diagram of the synthesis procedure for H-(Fe0.67Ni0.33)OOH-NiFe-LDH/NF.
Figure 1. Diagram of the synthesis procedure for H-(Fe0.67Ni0.33)OOH-NiFe-LDH/NF.
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Figure 2. (a) XRD pattern of exfoliated NiFeOOH-NiFe-LDH and exfoliated NiFe-LDH. (b,c) SEM images, (d,e) TEM images, (f) SAED patterns and (g) TEM images with EDS-mapping images of NiFeOOH-NiFe-LDH.
Figure 2. (a) XRD pattern of exfoliated NiFeOOH-NiFe-LDH and exfoliated NiFe-LDH. (b,c) SEM images, (d,e) TEM images, (f) SAED patterns and (g) TEM images with EDS-mapping images of NiFeOOH-NiFe-LDH.
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Figure 3. (a) Raman spectra, (b) XPS survey spectra and single-element spectra, (c) Ni 2p, (d) Fe 2p, (e) O 1s and (f) percentage of O element in different forms of NiFeOOH-NiFe-LDH and NiFe-LDH.
Figure 3. (a) Raman spectra, (b) XPS survey spectra and single-element spectra, (c) Ni 2p, (d) Fe 2p, (e) O 1s and (f) percentage of O element in different forms of NiFeOOH-NiFe-LDH and NiFe-LDH.
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Figure 4. Electrochemical performance of various catalysts in 1 mol·L−1 KOH. (a) Polarization curves. (b) The overpotentials required for current density of 100, 200 and 300 mA·cm−2. (c) Tafel plots. (d) Nyquist plots at 1.425 VRHE.
Figure 4. Electrochemical performance of various catalysts in 1 mol·L−1 KOH. (a) Polarization curves. (b) The overpotentials required for current density of 100, 200 and 300 mA·cm−2. (c) Tafel plots. (d) Nyquist plots at 1.425 VRHE.
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Figure 5. The Cdl measurement at the non-Faraday region potential window: (a) NiFeOOH-NiFe-LDH, (b) NiFe-LDH, (c) IrO2 and (d) NF. (e) The value of Cdl of different catalysts. (f) Chronoamperometric plots at 100 mA·cm−2 for NiFeOOH-NiFe-LDH.
Figure 5. The Cdl measurement at the non-Faraday region potential window: (a) NiFeOOH-NiFe-LDH, (b) NiFe-LDH, (c) IrO2 and (d) NF. (e) The value of Cdl of different catalysts. (f) Chronoamperometric plots at 100 mA·cm−2 for NiFeOOH-NiFe-LDH.
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Table 1. Comparison of OER performances between NiFeOOH-NiFe-LDH electrode and recently reported electrocatalysts in alkaline solution.
Table 1. Comparison of OER performances between NiFeOOH-NiFe-LDH electrode and recently reported electrocatalysts in alkaline solution.
CatalystSubstrateOverpotential (mV)Tafel Slope
(mV dec−1)		StabilityRef.
NiFeOOH-NiFe-LDHa NF227@100 mA cm−235.0120 h@200 mA cm−2
NiFe-LDH-NSb DG210@10 mA cm−252.010 h@10 mA cm−2[42]
NiFe-LDHc GCE270@10 mA cm−2-24 h@10 mA cm−2[37]
Mesoporous NiO/NiFe2O4GCE302@10 mA cm−2422 h @20 mA cm−2[43]
FePx/Fe-N-C/NPCNF325@10 mA cm−27924 h@10 mA cm−2[44]
Fe-NiO/NFNF264, 336@10, 100 mA cm−265.312 h@60 mA cm−2[45]
N-NiMoO4/NiS2d CF267, 335@10, 100 mA cm−2--[46]
N-CNTs@NiS2/Fe7S8GCE330@50 mA cm−251.4924 h@50 mA cm−2[47]
Amorphous (Fe-Ni)Cox-OH/Ni3S2NF280@100 mA cm−257100 h@200 mA cm−2[48]
NiFeCo-LDHe RDE249@10 mA cm−24680 h@100 mA cm−2[49]
Co@NiFe-LDHRDE253@10 mA cm−24450 h@10 mA cm−2[50]
Ni4FeW-LDHf CP248@20 mA cm−2686 h@10 mA cm−2[51]
Cr/FeNi-LDHg SS202, 242@10, 100 mA cm−232.515 h@10 mA cm−2[52]
FeOOH-NiCoMo-LDHNF252@50 mA cm−259.3950 h@50 mA cm−2[53]
S-NiMoO4@NiFe-LDHNF273@100 mA cm−29020 h@60 mA cm−2[17]
NiFe(OH)x/Ni3NNF260@10 mA cm−235-[54]
NiFeOx-LDHGEC227@10 mA cm−25420 h@100 mA cm−2[55]
Ru-NiFe-LDHCC246@10 mA cm−267.26 h@10 mA cm−2[38]
a NF; nickel foam, b DG; defective graphene, c GCE; glassy carbon electrode, d CF; carbon fiber, e RDE; glassy carbon electrode, f CP; carbon paper, g SS; stainless steel. All electrochemical tests were conducted in 1.0 M KOH except for Ref [14] (1.0 M KOH + 0.5 M NaCl freshwater).
Table 2. Equivalent circuit used for EIS data analysis and summary of the parameters obtained from various as-prepared electrodes.
Table 2. Equivalent circuit used for EIS data analysis and summary of the parameters obtained from various as-prepared electrodes.
SamplesRs (Ω)Rct (Ω)CPE.Y0 (F)CPE.N
NiFeOOH-NiFe-LDH0.90886.34291.10960.8192
NiFe-LDH0.94008.66661.83640.7585
IrO20.8736219.510.07250.8728
Nickel Foam2.70361321.40.01200.9700
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Ning, J.; Xu, L.; Xu, W.; Li, G.; Zhang, W. In-Site Growth of Efficient NiFeOOH/NiFe-LDH Electrodes: A Streamlined One-Step Methodology. Chemistry 2024, 6, 312-322. https://doi.org/10.3390/chemistry6020017

AMA Style

Ning J, Xu L, Xu W, Li G, Zhang W. In-Site Growth of Efficient NiFeOOH/NiFe-LDH Electrodes: A Streamlined One-Step Methodology. Chemistry. 2024; 6(2):312-322. https://doi.org/10.3390/chemistry6020017

Chicago/Turabian Style

Ning, Jing, Li Xu, Wei Xu, Guizhen Li, and Wen Zhang. 2024. "In-Site Growth of Efficient NiFeOOH/NiFe-LDH Electrodes: A Streamlined One-Step Methodology" Chemistry 6, no. 2: 312-322. https://doi.org/10.3390/chemistry6020017

APA Style

Ning, J., Xu, L., Xu, W., Li, G., & Zhang, W. (2024). In-Site Growth of Efficient NiFeOOH/NiFe-LDH Electrodes: A Streamlined One-Step Methodology. Chemistry, 6(2), 312-322. https://doi.org/10.3390/chemistry6020017

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