Authors
Contact Us

Sign In

A subscription to JoVE is required to view this content. Sign in or start your free trial.

In This Article

  • Summary
  • Abstract
  • Introduction
  • Protocol
  • Results
  • Discussion
  • Disclosures
  • Acknowledgements
  • Materials
  • References
  • Reprints and Permissions

Summary

Nickel hydroxide nanosheets are synthesized by a microwave-assisted hydrothermal reaction. This protocol demonstrates that the reaction temperature and time used for microwave synthesis affects the reaction yield, crystal structure, and local coordination environment.

Abstract

A protocol for rapid, microwave-assisted hydrothermal synthesis of nickel hydroxide nanosheets under mildly acidic conditions is presented, and the effect of reaction temperature and time on the material's structure is examined. All reaction conditions studied result in aggregates of layered α-Ni(OH)2 nanosheets. The reaction temperature and time strongly influence the structure of the material and product yield. Synthesizing α-Ni(OH)2 at higher temperatures increases the reaction yield, lowers the interlayer spacing, increases crystalline domain size, shifts the frequencies of interlayer anion vibrational modes, and lowers the pore diameter. Longer reaction times increase reaction yields and result in similar crystalline domain sizes. Monitoring the reaction pressure in situ shows that higher pressures are obtained at higher reaction temperatures. This microwave-assisted synthesis route provides a rapid, high-throughput, scalable process that can be applied to the synthesis and production of a variety of transition metal hydroxides used for numerous energy storage, catalysis, sensor, and other applications.

Introduction

Nickel hydroxide, Ni(OH)2, is used for numerous applications including nickel-zinc and nickel-metal hydride batteries1,2,3,4, fuel cells4, water electrolyzers4,5,6,7,8,9, supercapacitors4, photocatalysts4, anion exchangers10, and many other analytical, electrochemical, and sensor applications4,5. Ni(OH)2 has two predominant crystal structures: β-Ni(OH)2 and α-Ni(OH)211. β-Ni(OH)2 adopts a brucite-type Mg(OH)2 crystal structure, while α-Ni(OH)2 is a turbostratically layered form of β-Ni(OH)2 intercalated with residual anions and water molecules from the chemical synthesis4. Within α-Ni(OH)2, the intercalated molecules are not within fixed crystallographic positions but have a degree of orientational freedom, and also function as an interlayer glue stabilizing the Ni(OH)2 layers4,12. The interlayer anions of α-Ni(OH)2 affect the average Ni oxidation state13 and influence the electrochemical performance of α-Ni(OH)2 (relative to β-Ni(OH)2) toward battery2,13,14,15, capacitor16, and water-electrolysis applications17,18.

Ni(OH)2 can be synthesized by chemical precipitation, electrochemical precipitation, sol-gel synthesis, or hydrothermal/solvothermal synthesis4. Chemical precipitation and hydrothermal synthesis routes are widely utilized in the production of Ni(OH)2, and different synthetic conditions alter the morphology, crystal structure, and electrochemical performance. The chemical precipitation of Ni(OH)2 involves adding a highly basic solution to an aqueous nickel (II) salt solution. The phase and crystallinity of the precipitate are determined by the temperature and identities and concentrations of the nickel (II) salt and basic solution used4.

Hydrothermal synthesis of Ni(OH)2 involves heating an aqueous solution of precursor nickel (II) salt in a pressurized reaction vial, allowing the reaction to proceed at higher temperatures than ordinarily allowed under ambient pressure4. Hydrothermal reaction conditions typically favor β-Ni(OH)2, but α-Ni(OH)2 can be synthesized by (i) using an intercalation agent, (ii) using a non-aqueous solution (solvothermal synthesis), (iii) lowering the reaction temperature, or (iv) including urea in the reaction, resulting in ammonia-intercalated α-Ni(OH)24. The hydrothermal synthesis of Ni(OH)2 from nickel salts occurs via a two-step process that involves a hydrolysis reaction (equation 1) followed by an olation condensation reaction (equation 2).19

[Ni(H2O)N]2+ + hH2O ↔ [Ni(OH)h(H2O) N-h](2-h)++ hH3O+ (1)

Ni-OH + Ni-OH2 Ni-OH-Ni + H2O (2)

Microwave chemistry has been used for the one-pot synthesis of a wide variety of nanostructured materials and is based on the ability of a specific molecule or material to convert microwave energy into heat20. In conventional hydrothermal reactions, the reaction is initiated by the direct absorption of heat through the reactor. In contrast, within microwave-assisted hydrothermal reactions, the heating mechanisms are dipolar polarization of the solvent oscillating in a microwave field and ionic conduction generating localized molecular friction20. Microwave chemistry can increase the reaction kinetics, selectivity, and yield of chemical reactions20, making it of significant interest for a scalable, industrially viable method to synthesize Ni(OH)2.

For alkaline battery cathodes, the α-Ni(OH)2 phase provides improved electrochemical capacity compared with the β-Ni(OH)2 phase13, and synthetic methods to synthesize α-Ni(OH)2 are of particular interest. α-Ni(OH)2 has been synthesized by a variety of microwave-assisted methods, which include microwave-assisted reflux21,22, microwave-assisted hydrothermal techniques23,24, and microwave-assisted base-catalyzed precipitation25. The inclusion of urea within the reaction solution significantly influences the reaction yield26, mechanism26,27, morphology, and crystal structure27. The microwave-assisted decomposition of urea was determined to be a critical component for obtaining α-Ni(OH)227. Water content in an ethylene glycol-water solution has been shown to impact the morphology of microwave-assisted synthesis of α-Ni(OH)2 nanosheets24. The reaction yield of α-Ni(OH)2, when synthesized by a microwave-assisted hydrothermal route using an aqueous nickel nitrate and urea solution, was found to depend on the solution pH26. A prior study of microwave synthesized α-Ni(OH)2 nanoflowers using a precursor solution of EtOH/H2O, nickel nitrate, and urea found that temperature (in the range of 80-120 °C) was not a critical factor, provided the reaction is conducted above the urea hydrolysis temperature (60 °C)27. A recent paper that studied the microwave synthesis of Ni(OH)2 using a precursor solution of nickel acetate tetrahydrate, urea, and water found that at a temperature of 150 °C, the material contained both α-Ni(OH)2 and β-Ni(OH)2 phases, which indicates that temperature can be a critical parameter in the synthesis of Ni(OH)228.

Microwave-assisted hydrothermal synthesis can be used to produce high-surface area α-Ni(OH)2 and α-Co(OH)2 by using a precursor solution composed of metal nitrates and urea dissolved in an ethylene glycol/H2O solution12,29,30,31. Metal-substituted α-Ni(OH)2 cathode materials for alkaline Ni-Zn batteries were synthesized using a scaled-up synthesis designed for a large-format microwave reactor12. Microwave-synthesized α-Ni(OH)2 was also used as a precursor for obtaining β-Ni(OH)2 nanosheets12, nickel-iridium nanoframes for oxygen evolution reaction (OER) electrocatalysts29, and bifunctional oxygen electrocatalysts for fuel cells and water electrolyzers30. This microwave reaction route has also been modified to synthesize Co(OH)2 as a precursor for cobalt-iridium nanoframes for acidic OER electrocatalysts31 and bifunctional electrocatalysts30. Microwave-assisted synthesis was also used to produce Fe-substituted α-Ni(OH)2 nanosheets, and the Fe substitution ratio alters the structure and magnetization32. However, a step-by-step procedure for microwave synthesis of α-Ni(OH)2 and the evaluation of how varying reaction time and temperature within a water-ethylene glycol solution affects the crystalline structure, surface area, and porosity, and local environment of interlayer anions within the material has not been previously reported.

This protocol establishes procedures for high-throughput microwave synthesis of α-Ni(OH)2 nanosheets using a rapid and scalable technique. The effect of reaction temperature and time were varied and evaluated using in situ reaction monitoring, scanning electron microscopy, energy dispersive X-ray spectroscopy, nitrogen porosimetry, powder X-ray diffraction (XRD), and Fourier transform infrared spectroscopy to understand the effects of synthetic variables on reaction yield, morphology, crystal structure, pore size, and local coordination environment of α-Ni(OH)2 nanosheets.

Protocol

NOTE: The schematic overview of the microwave synthesis process is presented in Figure 1.

1. Microwave synthesis of α-Ni(OH)2 nanosheets

  1. Preparation of precursor solution
    1. Prepare the precursor solution by mixing 15 mL of ultrapure water (≥18 MΩ-cm) and 105 mL of ethylene glycol. Add 5.0 g of Ni(NO3)2 · 6 H2O and 4.1 g of urea to the solution and cover.
    2. Place the precursor solution in an ice and water-filled bath sonicator (40 kHz frequency) and sonicate at full power (no pulse) for 30 min.
  2. Microwave reaction of the precursor solution
    1. Transfer 20 mL of the precursor solution into a microwave-reaction vial with a polytetrafluoroethylene (PTFE) stir bar and seal the reaction vessel with a locking lid with a PTFE liner.
    2. Program the microwave reactor to heat to the reaction temperature using the setting as fast as possible (to 120 or 180 °C) and hold at that temperature for 13-30 min.
      NOTE: Heating as fast as possible is a microwave setting that applies maximum microwave power until the desired temperature is achieved; apply variable power thereafter to maintain the reaction temperature.
    3. After the reaction is complete, vent the reaction chamber with compressed air until the solution temperature reaches 55 °C. Each stage of the reaction (heating, holding, and cooling) is performed under magnetic stirring at 600 rpm.
  3. Centrifugation and washing the microwave-reaction precipitate.
    1. Transfer the post-reaction solution to 50 mL centrifuge tubes. Centrifuge the post-reaction solution at 6,000 rpm/6,198 rcf for 4 min at room temperature and then decant the supernatant.
    2. Add 25 mL of ultrapure water to resuspend the nanosheets. Centrifuge using the same conditions and then decant the supernatant.
    3. Repeat the washing, centrifuging, and decanting steps a total of five times using water, and then three times using ethanol.
      ​NOTE: Isopropyl alcohol can also be used in place of ethanol.
  4. Measuring the pH before and after the microwave reaction
    1. Measure the pH of the precursor solution before starting the microwave reaction and measure the pH of the supernatant immediately after the first centrifugation.
  5. Drying the sample
    1. Cover the centrifuge tubes with a tissue or paper towel to act as a porous cover to reduce potential contamination and dry them in a sample oven at 70 °C for 21 h under ambient atmosphere.
      ​NOTE: The drying time and conditions can influence the relative intensities and 2θ° values of (XRD) peaks, as described in the Representative Results.

2. Material characterization and analysis

  1. Characterizing the morphology and composition using scanning electron microscopy (SEM) and energy-dispersive X-ray spectroscopy (EDS)
    1. Prepare the samples for SEM and EDS analysis by suspending a small amount of Ni(OH)2 powder in 1 mL of ethanol using a water bath sonicator.
    2. Drop cast the Ni(OH)2/ethanol mixture on an SEM stub and evaporate the ethanol by placing the SEM stub in a sample oven at 70 °C.
    3. Collect SEM micrographs and EDS spectra. Collect SEM images using an accelerating voltage of 10 kV and a current of 0.34 nA at magnifications of 6.5 kX, 25 kX, and 100 kX. Collect EDS spectra on selected regions using an accelerating voltage of 10 kV, a current of 1.4 nA, and a magnification of 25 kX.
  2. Analyzing the surface area and porosity using nitrogen physisorption porosimetry
    1. Prepare the samples for analysis by adding 25 mg of Ni(OH)2 into the sample tube. Perform a pre-analysis degassing and drying procedure under vacuum at 120 °C for 16 h before analysis.
    2. Transfer the sample tube from the degassing port to the analysis port to collect nitrogen (N2) isotherms.
    3. Analyze the N2 isotherm data using Brunauer-Emmett-Teller (BET) analysis to determine the specific surface area. Perform the BET analysis according to International Union of Pure and Applied Chemistry (IUPAC) methodologies33. The specific analysis software package used to perform the BET analysis is included in the Table of Materials.
    4. Analyze the desorption branch of the isotherm using the Barrett-Joyner-Halenda (BJH) method to obtain pore volume, pore diameter, and pore size distribution. Perform the BJH analysis according to IUPAC methodologies.33 The specific analysis software package used to perform BJH analysis is included in the Table of Materials.
  3. Structural analysis using powder X-ray diffraction (XRD)
    1. Fill the sample well of a zero-background powder XRD holder with Ni(OH)2, ensuring the powder surface is flat.
    2. Collect powder X-ray diffractograms using a CuKα radiation source between 5°-80° 2θ using a 0.01-step increment.
    3. Analyze the d-spacing using Bragg's law,
      nλ = 2d sinθ,
      where n is an integer, λ is the wavelength of the X-rays, d is the d-spacing, and θ is the angle between the incident rays and the sample.
    4. Analyze the crystallite domain size, D, using the Scherrer equation,
      figure-protocol-5831
      where Ks is the Scherrer constant (a Scherrer constant of 0.92 was used for the analysis), λ is the wavelength of the X-rays, β2θ is the integral breadth of the diffraction peak, and θ is the Bragg angle (in radians). For analysis, β2θ was taken as the full width at half maximum (fwhm) and multiplied by a constant of 0.939434.
  4. Characterizing the material using attenuated total reflectance-Fourier transform infrared spectroscopy (ATR-FTIR)
    1. Equip the attenuated total reflectance (ATR) attachment to the Fourier transform infrared (FTIR) spectrometer.
    2. Press a small amount of Ni(OH)2 powder between two glass slides to create a small pellet.
    3. Place the Ni(OH)2 pellet on the silicon ATR crystal and obtain an FTIR spectrum between 400 and 4,000 cm-1. Infrared spectra represent the average of 16 individual scans with 4 cm-1 resolution.

Results

Influence of reaction temperature and time on the synthesis of α-Ni(OH)2
Before the reaction, the precursor solution [Ni(NO3)2 · 6 H2O, urea, ethylene glycol, and water] is a transparent green color with a pH of 4.41 ± 0.10 (Figure 2A and Table 1). The temperature of the microwave reaction (either 120 °C or 180 °C) influences the in situ reaction pressure and color of the sol...

Discussion

Microwave synthesis provides a route to generate Ni(OH)2 that is significantly faster (13-30 min reaction time) relative to conventional hydrothermal methods (typical reaction times of 4.5 h)38. Using this mildly acidic microwave synthesis route to produce ultrathin α-Ni(OH)2 nanosheets, it is observed that reaction time and temperature influence the reaction pH, yields, morphology, porosity, and structure of the resulting materials. Using an in situ reaction pr...

Disclosures

The authors have no conflicts of interest.

Acknowledgements

S.W.K. and C.P.R. gratefully acknowledge support from the Office of Naval Research Navy Undersea Research Program (Grant No. N00014-21-1-2072). S.W.K. acknowledges support from the Naval Research Enterprise Internship Program. C.P.R and C.M. acknowledge support from the National Science Foundation Partnerships for Research and Education in Materials (PREM) Center for Intelligent Materials Assembly, Award No. 2122041, for analysis of the reaction conditions.

Materials

NameCompanyCatalog NumberComments
ATR-FTIRBrukerTensor II FT-IR spectrometer equipped with a Harrick Scientific SplitPea ATR micro-sampling accessory
Bath sonicatorFisher Scientific15-337-409--
Ethanol VWR analyticalAC61509-0040200 proof
Ethylene GlycolVWR analyticalBDH1125-4LP99% purity
Falcon Centrifuge tubesVWR analytical21008-94050 mL
KimWipesVWR analytical21905-026--
Lab Quest 2Vernier LABQ2--
Microwave ReactorAnton Parr165741Monowave 450
Ni(NO3)2 · 6 H2OWard's Science470301-856Research lab grade
pH ProbeVernier PH-BTACalibrated vs standard pH solutions (pH= 4, 7, 11)
PorosemeterMicromeritics --ASAP 2020. Analysis software: Micromeritics, version 4.03
Powder x-ray diffactometerBrukerAXS Advanced Poweder x-ray diffractometer; d-spacing, and crystallite size analyses were performed using Highscore XRD software, and crystal structures were created using VESTA 3 software.
Reaction vialAnton Parr8272330 mL G30 wideneck, 20 mL max fill capacity
Reaction vial locking lidAnton Parr161724G30 Snap Cap
Reaction vial PTFE septumAnton Parr161728Wideneck
Scanning electron microscopeFEI--Helios Nanolab 400
UreaVWR analyticalBDH4602-500GACS grade

References

  1. Liu, B., et al. 120 Years of nickel-based cathodes for alkaline batteries. Journal of Alloys and Compounds. 834, 155185 (2020).
  2. Young, K. H., et al. Fabrications of high-capacity α-Ni(OH)2. Batteries. 3, 6 (2017).
  3. Huang, M., Li, M., Niu, C., Li, Q., Mai, L. Recent advances in rational electrode designs for high-performance alkaline rechargeable batteries. Advanced Functional Materials. 29 (11), 1807847 (2019).
  4. Hall, D. S., Lockwood, D. J., Bock, C., MacDougall, B. R. Nickel hydroxides and related materials: a review of their structures, synthesis and properties. Proceedings of the Royal Society A. Mathematical, Physical and Engineering Sciences. 471 (2174), 20140792 (2015).
  5. Miao, Y., et al. Electrocatalysis and electroanalysis of nickel, its oxides, hydroxides and oxyhydroxides toward small molecules. Biosensors and Bioelectronics. 53, 428-439 (2014).
  6. Suen, N. T., et al. Electrocatalysis for the oxygen evolution reaction: recent development and future perspectives. Chemical Society Reviews. 46 (2), 337-365 (2017).
  7. Diaz-Morales, O., Ledezma-Yanez, I., Koper, M. T., Calle-Vallejo, F. Guidelines for the rational design of Ni-based double hydroxide electrocatalysts for the oxygen evolution reaction. ACS Catalysis. 5 (9), 5380-5387 (2015).
  8. Rossini, P. d. O., et al. Ni-based double hydroxides as electrocatalysts in chemical sensors: a review. Trends in Analytical Chemistry. 126, 115859 (2020).
  9. Yu, Z., Bai, Y., Tsekouras, G., Cheng, Z. Recent advances in Ni-Fe (Oxy)hydroxide electrocatalysts for the oxygen evolution reaction in alkaline electrolyte targeting industrial applications. Nano Select. 3 (4), 766-791 (2021).
  10. Othman, M. R., Helwani, Z., Martunus, F. W. J. N. Synthetic hydrotalcites from different routes and their application as catalysts and gas adsorbents: a review. Applied Organometallic Chemistry. 23 (9), 335-346 (2009).
  11. Bode, V. H., Dehmelt, K., Witte, J. About the nickel hydroxide electrode. II. On the oxidation products of nickel(II) hydroxidesZeitschrift für Anorganische und Allgemeine Chemie. 366, 1-21 (1969).
  12. Kimmel, S. W., et al. Capacity and phase stability of metal-substituted α-Ni(OH)2 nanosheets in aqueous Ni-Zn batteries. Materials Advances. 2 (9), 3060-3074 (2021).
  13. Corrigan, D. A., Knight, S. L. Electrochemical and spectroscopic evidence on the participation of quadrivalent nickel in the nickel hydroxide redox reaction. Journal of the Electrochemical Society. 136 (3), 613-619 (1989).
  14. Shangguan, E., et al. A comparative study of structural and electrochemical properties of high-density aluminum substituted α-nickel hydroxide containing different interlayer anions. Journal of Power Sources. 282, 158-168 (2015).
  15. Li, Y. W., et al. Effect of interlayer anions on the electrochemical performance of Al-substituted α-type nickel hydroxide electrodes. International Journal of Hydrogen Energy. 35 (6), 2539-2545 (2010).
  16. Wang, C., Zhang, X., Xu, Z., Sun, X., Ma, Y. Ethylene glycol intercalated cobalt/nickel layered double hydroxide nanosheet assemblies with ultrahigh specific capacitance: structural design and green synthesis for advanced electrochemical storage. ACS Applied Materials & Interfaces. 7 (35), 19601-19610 (2015).
  17. Hunter, B. M., Hieringer, W., Winkler, J. R., Gray, H. B., Müller, A. M. Effect of interlayer anions on [NiFe]-LDH nanosheet water oxidation activity. Energy & Environmental Science. 9 (5), 1734-1743 (2016).
  18. Zhou, D., et al. Effects of redox-active interlayer anions on the oxygen evolution reactivity of NiFe-layered double hydroxide nanosheets. Nano Research. 11, 1358-1368 (2018).
  19. Cochran, E. A., Woods, K. N., Johnson, D. W., Page, C. J., Boettcher, S. W. Unique chemistries of metal-nitrate precursors to form metal-oxide thin films from solution: materials for electronic and energy applications. Journal of Materials Chemistry A. 7 (42), 24124-24149 (2019).
  20. Bilecka, I., Niederberger, M. Microwave chemistry for inorganic nanomaterials synthesis. Nanoscale. 2 (8), 1358-1374 (2010).
  21. Zhang, X., et al. Microwave-assisted synthesis of 3D flowerlike alpha-Ni(OH)2 nanostructures for supercapacitor application. Science China Technological Sciences. 58, 1871-1876 (2015).
  22. Li, J., Wei, M., Chu, W., Wang, N. High-stable α-phase NiCo double hydroxide microspheres via microwave synthesis for supercapacitor electrode materials. Chemical Engineering Journal. 316, 277-287 (2017).
  23. Tao, Y., et al. Microwave synthesis of nickel/cobalt double hydroxide ultrathin flowerclusters with three-dimensional structures for high-performance supercapacitors. Electrochimica Acta. 111, 71-79 (2013).
  24. Zhu, Y., et al. Ultrathin nickel hydroxide and oxide nanosheets: synthesis, characterizations and excellent supercapacitor performances. Scientific Reports. 4, 1-7 (2014).
  25. Benito, P., Labajos, F. M., Rives, V. Microwave-treated layered double hydroxides containing Ni and Al: the effect of added Zn. Journal of Solid State Chemistry. 179 (12), 3784-3797 (2006).
  26. Soler-Illia, G. J. d. A., Jobbágy, M., Regazzoni, A. E., Blesa, M. A. Synthesis of nickel hydroxide by homogeneous alkalinization. precipitation mechanism. Chemistry of Materials. 11 (11), 3140-3146 (1999).
  27. Xu, L., et al. 3D flowerlike α-nickel hydroxide with enhanced electrochemical activity synthesized by microwave-assisted hydrothermal method. Chemistry of Materials. 20 (1), 308-316 (2008).
  28. Alshareef, S. F., Alhebshi, N. A., Almashhori, K., Alshaikheid, H. S., Al-Hazmi, F. A ten-minute synthesis of alpha-Ni(OH)2 nanoflakes assisted by microwave on flexible stainless-steel for energy storage devices. Nanomaterials. 12 (11), 1911 (2022).
  29. Godínez-Salomón, F., et al. Self-supported hydrous iridium-nickel oxide two-dimensional nanoframes for high activity oxygen evolution electrocatalysts. ACS Catalysis. 8 (11), 10498-10520 (2018).
  30. Godínez-Salomón, F., Albiter, L., Mendoza-Cruz, R., Rhodes, C. P. Bimetallic two-dimensional nanoframes: high activity acidic bifunctional oxygen reduction and evolution electrocatalysts. ACS Applied Energy Materials. 3 (3), 2404-2421 (2020).
  31. Ying, Y., et al. Hydrous cobalt-iridium oxide two-dimensional nanoframes: insights into activity and stability of bimetallic acidic oxygen evolution electrocatalysts. Nanoscale Advances. 3 (7), 1976-1996 (2021).
  32. Kimmel, S. W., et al. Structure and magnetism of iron-substituted nickel hydroxide nanosheets. Magnetochemistry. 9 (1), 25-47 (2023).
  33. Thommes, M., et al. Physisorption of gases, with special reference to the evaluation of surface area and pore size distribution (IUPAC Technical Report). Pure and Applied Chemistry. 87 (9-10), 1051-1069 (2015).
  34. Birkholz, M., Fewster, P. F., Genzel, C. . Thin Film Analysis by X-ray Scattering. , (2006).
  35. Hall, D. S., Lockwood, D. J., Poirier, S., Bock, C., MacDougall, B. R. Raman and infrared spectroscopy of alpha and beta phases of thin nickel hydroxide films electrochemically formed on nickel. Journal of Physical Chemistry A. 116 (25), 6771-6784 (2012).
  36. Choy, J. H., Kwon, Y. M., Han, K. S., Song, S. W., Chang, S. H. Intra- and inter-layer structures of layered hydroxy double salts, Ni1-xZn2x(OH)2(CH3CO2)2xnH2O. Materials Letters. 34 (3-6), 356-363 (1998).
  37. Momma, K., Izumi, F. VESTA for three-dimensional visualization of crystal, volumetric and morphology data. Journal of Applied Crystallography. 44 (6), 1272-1276 (2011).
  38. Godinez-Salomon, F., Mendoza-Cruz, R., Arellano-Jimenez, M. J., Jose-Yacaman, M., Rhodes, C. P. Metallic two-dimensional nanoframes: unsupported hierarchical nickel-platinum alloy nanoarchitectures with enhanced electrochemical oxygen reduction activity and stability. ACS Applied Materials & Interfaces. 9 (22), 18660-18674 (2017).
  39. Shakhashiri, B. Z., Dirreen, G. E., Juergens, F. Color, solubility, and complex ion equilibria of nickel (II) species in aqueous solution. Journal of Chemical Education. 57 (12), 900-901 (1980).

Reprints and Permissions

Request permission to reuse the text or figures of this JoVE article

Request Permission

Explore More Articles

Nickel HydroxideNanosheetsMicrowave SynthesisHydrothermal SynthesisReaction ConditionsCrystalline StructureSurface AreaPorosityReaction TemperatureReaction TimeAlpha Nickel HydroxideMetal HydroxidesMetal OxidesEnergy StorageCatalysisSensors

This article has been published

Video Coming Soon

JoVE Logo

Privacy

Terms of Use

Policies

Contact Us

Recommend to library

JoVE NEWSLETTERS

Research

Education

Authors

Librarians

ABOUT JoVE

Copyright © 2025 MyJoVE Corporation. All rights reserved