Journal articles: 'Nickel(II) oxide'

1

Young, Jay A. "Nickel(II) Oxide." Journal of Chemical Education 82, no. 6 (June 2005): 831. http://dx.doi.org/10.1021/ed082p831.

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2

Cochran, SJ, and FP Larkins. "An X-Ray Photoelectron Study of Doped and Supported Nickel Oxide." Australian Journal of Chemistry 38, no. 9 (1985): 1293. http://dx.doi.org/10.1071/ch9851293.

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The surfaces of lithium-and chromium-doped nickel oxide and of nickel oxide supported on alumina have been examined by X-ray photoelectron spectroscopy. The concentration of the nickel(III) species increased for the lithium-doped oxide and decreased for the chromium-doped oxide relative to the undoped oxide. The effects of doping were manifested most clearly however by the amount of oxygen-containing species adsorbed on the oxide surface rather than by variations in the nickel(III) peak intensity. Lithium-doped oxides were also shown to reduce more readily than undoped or chromium-doped oxides in the presence of carbon-containing impurities. The rate of reduction is influenced by the activation energy for electron transport which is related to the availability of the nickel(III) species. Supported oxides showed significant surface enhancement of nickel(II) as well as an absence of the nickel(III) species. The nickel(II) species in the supported oxide was not easily reduced to nickel(0).

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3

Pourroy, G., J. L. Guille, and P. Poix. "Reactivity of metal oxides copper(I) oxide, manganese(II) oxide, cobalt(II) oxide, nickel(II) oxide, copper(II) oxide and zinc oxide with indialite." Chemistry of Materials 2, no. 2 (March 1990): 101–5. http://dx.doi.org/10.1021/cm00008a007.

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4

Moreno-Fuquen, Rodolfo, Olga Cifuentes, Jaime Valderrama Naranjo, Luis Manuel Serratto, and Alan R. Kennedy. "Dichlorobis(triphenylphosphine oxide-κO)nickel(II)." Acta Crystallographica Section E Structure Reports Online 60, no. 12 (November 20, 2004): m1861—m1862. http://dx.doi.org/10.1107/s1600536804029125.

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5

Sharma, S. K., F. J. Vastola, and P. L. Walker. "Reduction of nickel oxide by carbon: II. Interaction between nickel oxide and natural graphite." Carbon 35, no. 4 (1997): 529–33. http://dx.doi.org/10.1016/s0008-6223(97)83727-x.

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6

SAWATARI, Katsuhiko. "Differential determination of nickel (II) oxide and nickel (III) oxide in airborne particulate substances." INDUSTRIAL HEALTH 26, no. 2 (1988): 115–23. http://dx.doi.org/10.2486/indhealth.26.115.

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7

Sathiyaraj, Ethiraj, Govindasamy Gurumoorthy, and Subbiah Thirumaran. "Nickel(ii) dithiocarbamate complexes containing the pyrrole moiety for sensing anions and synthesis of nickel sulfide and nickel oxide nanoparticles." New Journal of Chemistry 39, no. 7 (2015): 5336–49. http://dx.doi.org/10.1039/c4nj02250e.

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Rare anagostic interaction is observed in (N-(pyrrol-2-ylmethyl)-N-furfuryldithiocarbamato-S,S′)(thiocyanato-N)(triphenylphosphine)nickel(ii). Bis(N-(pyrrol-2-ylmethyl)-N-furfuryldithiocarbamato-S,S′)nickel(ii) is used for the preparation of spherical nickel sulfide and nickel oxide nanoparticles.

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8

Markov, L., and K. Petrov. "Nickel-cobalt oxide spinels prepared by thermal decomposition of nickel(II)-cobalt(II) hydroxide nitrates." Reactivity of Solids 1, no. 4 (August 1986): 319–27. http://dx.doi.org/10.1016/0168-7336(86)80024-9.

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9

Liang-Gui, Wang. "Bis(2-pyridinecarboxylatoN-oxide-κ2O,O′)nickel(II)." Acta Crystallographica Section E Structure Reports Online 63, no. 12 (November 28, 2007): m3168. http://dx.doi.org/10.1107/s1600536807059958.

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10

Pretorius, Eugene B., and Arnulf Muan. "Activity of Nickel(II) Oxide in Silicate Melts." Journal of the American Ceramic Society 75, no. 6 (June 1992): 1490–96. http://dx.doi.org/10.1111/j.1151-2916.1992.tb04215.x.

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11

Ravindran Durai Nayagam, B., Samuel Robinson Jebas, J. P. Edward Rajkumar, and Dieter Schollmeyer. "Tetraaquabis[3-(2-pyridylsulfanyl)propionatoN-oxide]nickel(II)." Acta Crystallographica Section E Structure Reports Online 65, no. 4 (March 31, 2009): m470. http://dx.doi.org/10.1107/s1600536809011283.

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12

Feizi, Hadi, Farshad Shiri, Robabeh Bagheri, Jitendra Pal Singh, Keun Hwa Chae, Zhenlun Song, and Mohammad Mahdi Najafpour. "The application of a nickel(ii) Schiff base complex in water oxidation: the importance of nanosized materials." Catalysis Science & Technology 8, no. 15 (2018): 3954–68. http://dx.doi.org/10.1039/c8cy00582f.

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13

Raul, Prasanta K., Bodhaditya Das, Rashmi R. Devi, and Sanjai K. Dwivedi. "Nanoscale Copper II Oxide An Efficient and Reusable Adsorbent for Removal of Nickel II from Contaminated Water." Defence Life Science Journal 6, no. 2 (June 3, 2021): 146–54. http://dx.doi.org/10.14429/dlsj.6.16289.

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The present work describes the synthesis of copper(II) oxide nanoparticles (NPs) with high surface area (52.11 m2/g) and its Ni(II) adsorption efficiency from contaminated water at room temperature. Copper (II) oxide NPs are able to remove Ni(II) as 93.6 per cent and 93.7 per cent using 500 ppb & 1000 ppb initial concentration of nickel at near-neutral pH respectively. CuO NPs is very much effective to remove more than 75 per cent nickel over a wide range of pH even in presence of other competing ions like Cd2+, Pb2+, Cr6+, SO42-. Prepared CuO NPs can be used to remove Ni(II) from aqueous solution in real field application.

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14

Vasil’eva, M. S., V. S. Rudnev, O. E. Sklyarenko, L. M. Tyrina, and N. B. Kondrikov. "Titanium-supported nickel-copper oxide catalysts for oxidation of carbon(II) oxide." Russian Journal of General Chemistry 80, no. 8 (August 2010): 1557–62. http://dx.doi.org/10.1134/s1070363210080037.

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15

Shi, Jing Min, Zhe Liu, Jian Jun Lu, and Lian Dong Liu. "Diaquabis(isothiocyanato)bis(4-methylpyridineN-oxide)nickel(II) monohydrate." Acta Crystallographica Section E Structure Reports Online 61, no. 5 (April 16, 2005): m871—m872. http://dx.doi.org/10.1107/s1600536805010937.

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16

Polam, J. R., and L. C. Porter. "Structure of bis(hexafluoroacetylacetonato)bis(triphenylphosphine oxide)nickel(II)." Acta Crystallographica Section C Crystal Structure Communications 48, no. 10 (October 15, 1992): 1761–64. http://dx.doi.org/10.1107/s0108270192001975.

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17

Alidoust, Nima, Martina Lessio, and Emily A. Carter. "Cobalt (II) oxide and nickel (II) oxide alloys as potential intermediate-band semiconductors: A theoretical study." Journal of Applied Physics 119, no. 2 (January 14, 2016): 025102. http://dx.doi.org/10.1063/1.4939286.

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18

Balch, Alan L., and Y. W. Chan. "A novel oxygen atom transfer reaction. Isomerization of nickel(II) octaethylporphyrin N-oxide to nickel(II) octaethyloxochlorin." Inorganica Chimica Acta 115, no. 2 (May 1986): L45—L46. http://dx.doi.org/10.1016/s0020-1693(00)84399-6.

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19

Hanifehpour, Younes, Babak Mirtamizdoust, Ruiyao Wang, Saeed Anbarteh, and Sang Woo Joo. "A Nano Nickel (II) Metal–Organic Coordination Compound for Nano Nickel (II) Oxide: Sonochemical Synthesis and Characterization." Journal of Inorganic and Organometallic Polymers and Materials 27, no. 4 (April 24, 2017): 1045–52. http://dx.doi.org/10.1007/s10904-017-0554-4.

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20

RAMASAMY, KARTHIK, WEERAKANYA MANEEPRAKORN, NASIR IQBAL, MOHAMMAD AZAD MALIK, and PAUL O'BRIEN. "COBALT(II)/NICKEL(II) COMPLEXES OF DITHIOACETYLACETONE [M(SacSac)2](M = Co, Ni) AS SINGLE SOURCE PRECURSORS FOR COBALT/NICKEL SULFIDE NANOSTRUCTURES." International Journal of Nanoscience 10, no. 04n05 (August 2011): 815–22. http://dx.doi.org/10.1142/s0219581x11009234.

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Cobalt(II)/Nickel(II) complexes of 4-thiopent-3-ene-2-thione (SacSac), [ M(SacSac) 2]( M = Co, Ni ) have been used as single source precursors (SSPs) for the preparation of cobalt/nickel sulfide thin films by aerosol-assisted chemical vapor deposition (AACVD). Cobalt or nickel sulfide nanoparticles were grown by thermal decomposition of the precursor in hot trioctylphosphine oxide (TOPO) or hexadecylamine (HDA). XRD analysis showed that all samples of cobalt or nickel sulfide are of the sulfur deficient phases ( Ni9S8, Co9S8, Ni7S6 , or Ni3S2 ). SEM and TEM analysis showed that nickel sulfide formed nanowires, nanorods and spheres; cobalt sulfide formed plate like structures and spheres. The chemical compositions of the nanoparticles can be controlled by varying temperature or the capping agents.

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21

Borisov, Georgui, Sabi G. Varbanov, Luigi M. Venanzi, Alberto Albinati, and Francesco Demartin. "Coordination of Dimethyl(aminomethyl)phosphine Oxide with Zinc(II), Nickel(II), and Palladium(II)." Inorganic Chemistry 33, no. 24 (November 1994): 5430–37. http://dx.doi.org/10.1021/ic00102a014.

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22

Teng, C. M., T. F. Kelly, J. P. Zhang, H. M. Lin, and Y. W. Kim. "HREM observation of NiO growth on submicron spheres of pure nickel." Proceedings, annual meeting, Electron Microscopy Society of America 47 (August 6, 1989): 548–49. http://dx.doi.org/10.1017/s0424820100154718.

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Spherical submicron particles of materials produced by electrohydrodynamic (EHD) atomization have been used to study a variety of materials processes including nucleation of alternative crystallization phases in iron-nickel and nickel-chromium alloys, amorphous solidification in submicron droplets of pure metals, and quasi-crystal formation in nickel-chromium alloys. Some experiments on pure nickel, nickel oxide single crystals, the nickel/nickel(II) oxide interface, and grain boundaries in nickel monoxide have been performed by STEM. For these latter studies, HREM is the most direct approach to obtain particle crystal structures at the atomic level. Grain boundaries in nickel oxide have also been investigated by HREM. In this paper, we present preliminary results of HREM observations of NiO growth on submicron spheres of pure nickel.Small particles of pure nickel were prepared by EHD atomization. For the study of pure nickel, 0.5 mm diameter pure nickel wire (99.9975%) is sprayed directly in the EHD process. The liquid droplets solidify in free-flight through a vacuum chamber operated at about 10-7 torr.

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23

Maximov, Maxim, Denis Nazarov, Aleksander Rumyantsev, Yury Koshtyal, Ilya Ezhov, Ilya Mitrofanov, Artem Kim, Oleg Medvedev, and Anatoly Popovich. "Atomic Layer Deposition of Lithium–Nickel–Silicon Oxide Cathode Material for Thin-Film Lithium-Ion Batteries." Energies 13, no. 9 (May 8, 2020): 2345. http://dx.doi.org/10.3390/en13092345.

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Lithium nickelate (LiNiO2) and materials based on it are attractive positive electrode materials for lithium-ion batteries, owing to their large capacity. In this paper, the results of atomic layer deposition (ALD) of lithium–nickel–silicon oxide thin films using lithium hexamethyldisilazide (LiHMDS) and bis(cyclopentadienyl) nickel (II) (NiCp2) as precursors and remote oxygen plasma as a counter-reagent are reported. Two approaches were studied: ALD using supercycles and ALD of the multilayered structure of lithium oxide, lithium nickel oxide, and nickel oxides followed by annealing. The prepared films were studied by scanning electron microscopy, spectral ellipsometry, X-ray diffraction, X-ray reflectivity, X-ray photoelectron spectroscopy, time-of-flight secondary ion mass spectrometry, energy-dispersive X-ray spectroscopy, transmission electron microscopy, and selected-area electron diffraction. The pulse ratio of LiHMDS/Ni(Cp)2 precursors in one supercycle ranged from 1/1 to 1/10. Silicon was observed in the deposited films, and after annealing, crystalline Li2SiO3 and Li2Si2O5 were formed at 800 °C. Annealing of the multilayered sample caused the partial formation of LiNiO2. The obtained cathode materials possessed electrochemical activity comparable with the results for other thin-film cathodes.

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24

Ghosh, Somnath, Hemanta Deka, Yuvraj B. Dangat, Soumen Saha, Kuldeep Gogoi, Kumar Vanka, and Biplab Mondal. "Reductive nitrosylation of nickel(ii) complex by nitric oxide followed by nitrous oxide release." Dalton Transactions 45, no. 25 (2016): 10200–10208. http://dx.doi.org/10.1039/c6dt00826g.

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Ni(ii) complex of bis-(2-ethyl-4-methylimidazol-5-yl)methane in methanol undergoes reductive nitrosylation in presence of NO to afford the corresponding Ni(i)-nitrosyl intermediate. Subsequent reaction with additional NO releases N₂O with Ni(ii)-nitrito complex formation.

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25

Melnyk, Yuriy, Roman Starchevskyi, and Stepan Melnyk. "Technological Aspects of Vegetable Oils Transesterification with Ethanol in the Presence of Metal Oxides." Kemija u industriji 69, no. 7-8 (2020): 365–70. http://dx.doi.org/10.15255/kui.2019.059.

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Transesterification of vegetable oil with ethanol in the presence of fine metal oxide particles as catalysts has been investigated. Zinc and nickel(II) oxides were shown to have the highest catalytic activity. In their presence, the conversion of sunflower oil triglycerides, after 150 min, reached 95.3 and 94.2 %, respectively. The optimal mass fraction of zinc oxide catalyst was found to be 0.25–0.31 %. In the presence of zinc oxide, with mass fraction of water in ethanol of 5 and 10 %, the conversion of triglycerides was 98.5 and 94.8 %, respectively.

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26

Anchidin-Norocel, Liliana, Sonia Amariei, and Gheorghe Gutt. "Sensing of Nickel(II) Ions by Immobilizing Ligands and Using Different SPEs." Engineering Proceedings 6, no. 1 (May 17, 2021): 2. http://dx.doi.org/10.3390/i3s2021dresden-10106.

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The aim of this paper is the development of a sensor for the quantification of nickel ions in food raw materials and foods. It is believed that about 15% of the human population suffers from nickel allergy. In addition to digestive manifestations, food intolerance to nickel may also have systemic manifestations, such as diffuse dermatitis, diffuse itching, fever, rhinitis, headache, altered general condition. Therefore, it is necessary to control this content of nickel ions for the health of the human population by developing a new method that offers the advantages of a fast, not expensive, in situ, and accurate analysis. For this purpose, bismuth oxide-screen-printed electrodes (SPEs) and graphene-modified SPEs were used with a very small amount of dimethylglyoxime and amino acid L-histidine that were deposited. A potentiostat that displays the response in the form of a cyclic voltammogram was used to study the electrochemical properties of nickel standard solution with different concentrations. The results were compared and the most sensitive sensor proved to be bismuth oxide-SPEs with dimethylglyoxime (Bi2O3/C-dmgH2) with a linear response over a wide range (0.1–10 ppm) of nickel concentrations. Furthermore, the sensor shows excellent selectivity in the presence of common interfering species. The Bi2O3/C-dmgH2 sensor showed good viability for nickel analysis in food samples (cocoa, spinach, cabbage, and red wine) and demonstrated significant advancement in sensor technology for practical applications.

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27

Ahmad, Harith, Siti Aisyah Reduan, and Norazriena Yusoff. "Chitosan capped nickel oxide nanoparticles as a saturable absorber in a tunable passively Q-switched erbium doped fiber laser." RSC Advances 8, no. 45 (2018): 25592–601. http://dx.doi.org/10.1039/c8ra04380a.

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Nickel oxide (NiO) nanoparticles prepared from a nickel(ii) chloride hexahydrate precursor are used to form a chitosan capped NiO nanoparticle thin film that serves as a saturable absorber in a passively Q-switched erbium doped fiber laser.

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28

Zhu, Shan Shan, Fu Tao Hu, Dao Dong Pan, Wei Lian Xu, and Ning Gan. "Determination of Ultra Trace of Heavy Metals in Water by ICP-AES Based on Magnetic Enrichment." Advanced Materials Research 487 (March 2012): 658–62. http://dx.doi.org/10.4028/www.scientific.net/amr.487.658.

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A new method has been established for the pre-enrichment of trace heavy metals(lead(II), cadmium(II), chromium(VI) and nickel(II)) by magnetic iron oxide(core) / zirconium dioxide(shell) and determined by inductively coupled plasma atomic emission spectrometry (ICP-AES) in water samples. The factors affecting the separation and pre-enrichment of analytes such as amounts of magnetic iron oxide / zirconium dioxide, elution time and interfering ions were studied. The detection limits of the method (3σ) were 13.5ng/mL, 1.01ng/mL, 2.94ng/mL and 3.31mg/L respectively for lead(II), cadmium(II), chromium(VI) and nickel(II). The results showed that this method was simple, accurate, and sensitive which could be applied for the pre-enrichment, separation and determination of trace heavy metals in all kinds of water samples.

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29

Castellano, E. E., G. Oliva, and J. Zukerman-Schpector. "Structure of dibromobis(triphenylarsine oxide)nickel(II), NiBr2(Ph3AsO)2." Acta Crystallographica Section C Crystal Structure Communications 47, no. 3 (March 15, 1991): 654–55. http://dx.doi.org/10.1107/s0108270190009374.

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30

Stolyarova, V. L., S. I. Lopatin, and S. M. Shugurov. "Thermodynamic properties of gaseous salts formed by Nickel(II) oxide." Doklady Physical Chemistry 406, no. 2 (February 2006): 27–29. http://dx.doi.org/10.1134/s0012501606020011.

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31

Rathore, Bharatraj Singh, Narendra Pal Singh Chauhan, Sapana Jadoun, Suresh C. Ameta, and Rakshit Ameta. "Synthesis and characterization of chitosan-polyaniline-nickel(II) oxide nanocomposite." Journal of Molecular Structure 1242 (October 2021): 130750. http://dx.doi.org/10.1016/j.molstruc.2021.130750.

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32

Mikhailov, Yu M., V. V. Aleshin, A. V. Bakeshko, V. I. Vershinnikov, T. I. Ignat'eva, and D. Yu Kovalev. "Combustion Modes of Mixtures of Nickel (II) Oxide with Titanium." Физика горения и взрыва 57, no. 4 (2021): 69–72. http://dx.doi.org/10.15372/fgv20210407.

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33

Zheng, Jun, Ling Xia, and Shaoxian Song. "Electrosorption of Pb(ii) in water using graphene oxide-bearing nickel foam as the electrodes." RSC Advances 7, no. 38 (2017): 23543–49. http://dx.doi.org/10.1039/c7ra02956j.

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34

Kaŝpárek, Frantiŝek, Zdenê Trávnicek, Martin Posolda, Zdenê Kŝindelár, and Jaromír Marek. "NICKEL(II), COPPER(II), ZINC(II), CADMIUM(II) AND MERCURY(II) COMPLEXES OF TRIS(2-AMINOETHYL)PHOSPHINE OXIDE." Journal of Coordination Chemistry 44, no. 1-2 (May 1, 1998): 61–70. http://dx.doi.org/10.1080/00958979808022880.

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35

Minigalieva, I., B. Katsnelson, L. Privalova, V. Gurvich, V. Shur, E. Shishkina, A. Varaksin, V. Panov, T. Slyshkina, and E. Grigorieva. "Experimental and mathematical modeling of combined subchronic toxicity of nickel(II) oxide and manganese(II,III) oxide nanoparticles." Toxicology Letters 238, no. 2 (October 2015): S279. http://dx.doi.org/10.1016/j.toxlet.2015.08.804.

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36

Seidel, Rüdiger W. "cis-Bis(nitrato-κ2O,O′)bis(triethylphosphine oxide-κO)nickel(II)." Acta Crystallographica Section E Structure Reports Online 65, no. 6 (May 7, 2009): m612. http://dx.doi.org/10.1107/s1600536809015724.

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In the title compound, [Ni(NO3)2(C6H15OP)2], the NiIIion, lying on a crystallographic twofold axis, adopts a distorted octahedral coordination, consisting ofO-donor atoms of two symmetry-related triethylphospine oxide and two bidentate nitrate ligands.

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37

Xie, Gang, Yoshiharu Sakamura, Keiko Ema, and Yasuhiko Ito. "Characterization of nickel oxide in molten carbonate II. In situ x-ray diffraction of higher nickel oxide in molten carbonate." Journal of Power Sources 32, no. 2 (August 1990): 135–41. http://dx.doi.org/10.1016/s0378-7753(12)80003-6.

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38

Atawneh, Majdoleen, Sami Makharza, Sahar Zahran, Kariman Titi, Fahed Takrori, and Silke Hampel. "The cross-talk between lateral sheet dimensions of pristine graphene oxide nanoparticles and Ni2+ adsorption." RSC Advances 11, no. 19 (2021): 11388–97. http://dx.doi.org/10.1039/d1ra00400j.

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39

Tonelli, Domenica, Barbara Ballarin, Mario Berrettoni, and Marcello Trevisani. "Electrochemical Study of Mannitol Oxidation at Nickel Oxide Electrode." Collection of Czechoslovak Chemical Communications 68, no. 9 (2003): 1636–46. http://dx.doi.org/10.1135/cccc20031636.

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The electrocatalytic oxidation of mannitol at a nickel oxide electrode was investigated. The experimental conditions for determining mannitol concentrations have been optimised taking into account the involved electrochemistry. Unlike what previously reported in the literature, our findings lead to the conclusion that both the electrochemical reaction involving the Ni(II)/Ni(III) couple and the chemical reaction between mannitol and Ni(III) are effective in determining the overall kinetics of the electrocatalytic process. The calibration line for mannitol was linear up to 20.0 mmol l-1. Mannitol determination with the nickel oxide electrode was performed in a liquid culture medium selective for Staphylococcus aureus in order to make an indirect calibration of bacterial viable cells, but the results were not satisfactory.

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40

FUJII, Satoshi, Hiroshi KAKUNO, Yosohiro SUGIE, and Chiaki SAKAMOTO. "Adsorption of cobalt(II) and nickel(II) on titanium oxide in sodium citrate solution." NIPPON KAGAKU KAISHI, no. 8 (1985): 1635–37. http://dx.doi.org/10.1246/nikkashi.1985.1635.

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41

Yin, Lan, S. Balaji, and S. Seetharaman. "Effects of Nickel on Interface Morphology during Oxidation of Fe-Cu-Ni Alloys." Defect and Diffusion Forum 297-301 (April 2010): 318–29. http://dx.doi.org/10.4028/www.scientific.net/ddf.297-301.318.

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Steel produced in Electric Arc Furnaces (EAF) contain a high amount of copper that causes a detrimental surface cracking phenomenon called hot shortness. Studies have found that nickel can alleviate hot shortness by increasing copper solubility in the Fe phase, decreasing oxidation rate and promoting occlusion [1-3]. Occlusion is a phenomenon whereby the copper-rich phase becomes incorporated into iron oxides. Nickel promotes occlusion by causing an uneven interface and increasing the number of internal oxides. The uneven interface is likely a result of the two concentration fields resulting from ternary diffusion of nickel, copper and iron in the Fe phase. This work is aimed at explaining why nickel causes wavy oxide/liquid-Cu and liquid-Cu/Fe interfaces. Constitutional super-saturation criterion [4] was applied to explain uneven interfaces caused by nickel. A model simulating diffusion behaviors of copper and nickel in Fe was developed by coupling Comsol Multiphysics® and Matlab®. Interface concentrations of copper and nickel and perturbation criterion values were calculated as a function of time. Modeling results show that (i) the nickel interface concentration first increases to a peak value then decreases slowly during oxidation process as a result of the change in oxidation rates, and (ii) the alloys with higher nickel contents have more potential for interface breakdown and this occurs within the initial linear oxidation regime.

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42

Kennedy, A. R., S. W. Sloss, and M. D. Spicer. "cis-Di(nitrato-O,O')bis(tricyclohexylphosphine oxide-O)nickel(II)." Acta Crystallographica Section C Crystal Structure Communications 53, no. 3 (March 15, 1997): 292–93. http://dx.doi.org/10.1107/s0108270196014229.

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43

Liu, Winnie S., Roger K. Bunting, and Douglas X. West. "Heterocyclic amine adducts of bis(2-thiopyridine N-oxide)nickel(II)." Inorganica Chimica Acta 105, no. 3 (December 1985): 177–80. http://dx.doi.org/10.1016/s0020-1693(00)85225-1.

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44

Nattestad, Andrew, Michael Ferguson, Robert Kerr, Yi-Bing Cheng, and Udo Bach. "Dye-sensitized nickel(II)oxide photocathodes for tandem solar cell applications." Nanotechnology 19, no. 29 (June 10, 2008): 295304. http://dx.doi.org/10.1088/0957-4484/19/29/295304.

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45

Adolphe, Kouoh Sone Paul-Michel, Tagne Guy Merlain, Lekene Ngouateu René Blaise, Belibi Belibi Placide Desire, NdiNsami Julius, Kouotou Daouda, Ghogomu Numbonui Julius, Anagho Gabche Solomon, and Ketcha Mbadcam Joseph. "Kinetics and equilibrium studies of the adsorption of nickel (II) ions from aqueous solution onto modified natural and synthetic iron oxide." International Journal of Basic and Applied Sciences 4, no. 3 (June 20, 2015): 277. http://dx.doi.org/10.14419/ijbas.v4i3.4721.

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<p>The present paper reports on the kinetic and equilibrium studies of the adsorption of Nickel(II) ions from aqueous solution onto modified natural iron oxide (NAT) from Mbalam (East Region of Cameroon) and synthetic iron oxide (SYNTH). The parameters investigated using batch techniques include, the contact time, adsorbent mass, pH and initial metal ion concentration. The experimental results obtained showed that, the optimum pH of 6 for bothadsorbents with an equilibrium time of 30 minutes was sufficient. The kinetic data correlated well with the pseudo-first-order and pseudo-second-order kinetic models for both the adsorbents based on the correlation coefficients (R<sup>2</sup>) obtained. The adsorption processes followed both the Langmuir and the Tempkin adsorption models for the natural iron oxide, whereas the Freundlich and Tempkin adsorption models fitted well the adsorption data for the synthetic iron oxide. The maximum quantity of Nickel(II) ions adsorbed was 250 mg/g for the two adsorbents. These results revealed a high adsorption capacity of natural iron oxide which is comparable to that of synthetic iron oxide.</p>

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Minigalieva, Ilzira, Boris Katsnelson, Larisa Privalova, Marina Sutunkova, Vladimir Gurvich, Vladimir Shur, Ekaterina Shishkina, et al. "Attenuation of Combined Nickel(II) Oxide and Manganese(II, III) Oxide Nanoparticles’ Adverse Effects with a Complex of Bioprotectors." International Journal of Molecular Sciences 16, no. 9 (September 17, 2015): 22555–83. http://dx.doi.org/10.3390/ijms160922555.

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Musluoğlu, Emel, and Vefa Ahsen. "Synthesis and Characterization of 1,2-Bis(aziridin-N-yl)glyoxime and its Nickel(II), Palladium(II) and Cobalt(II) Complexes." Journal of Chemical Research 23, no. 2 (February 1999): 142–43. http://dx.doi.org/10.1177/174751989902300238.

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Illy-Cherrey, S., O. Tillement, J. M. Dubois, F. Massicot, Y. Fort, J. Ghanbaja, and S. Bégin-Colin. "Synthesis and characterization of nano-sized nickel(II), copper(I) and zinc(II) oxide nanoparticles." Materials Science and Engineering: A 338, no. 1-2 (December 2002): 70–75. http://dx.doi.org/10.1016/s0921-5093(02)00057-6.

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Nonoyama, Matsuo, and Kiyoko Nonoyama. "Cobalt(III), copper(II), and nickel(II) complexes of 1-thia-4,7-diazacyclononane-S-oxide." Transition Metal Chemistry 10, no. 10 (October 1985): 382–84. http://dx.doi.org/10.1007/bf00618848.

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Guillou, Nathalie, Carine Livage, Julienne Chaigneau, and Gérard Férey. "Structural investigation of the nickel 3-methylglutarate from powder diffraction demonstrating adaptability of the inorganic skeleton of MIL-77." Powder Diffraction 20, no. 4 (December 2005): 288–93. http://dx.doi.org/10.1154/1.2135311.

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Ni20[(C6H8O4)20(H2O)8]∙33H2O, a new nickel(II) 3-methylglutarate, was prepared hydrothermally (180 °C, 48 h, autogenous pressure) from a 1:1.5:2:180 mixture of nickel (II) sulphate hexahydrate, 3-methylglutaric acid, sodium hydroxide, and water. It crystallizes in the cubic system (space group P4332, Z=1) with a=16.8488(5) Å and V=4783.1(4) Å3. Its structure was solved from conventional X-ray powder diffraction data. It presents a three-dimensional network of edge-sharing nickel octahedra, lined by deprotonated organic anions. This remarkable oxide network with corrugated 20-membered rings is constructed from homochiral helices. The rings intersect each other to generate large crossing channels full of water along [111].

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Journal articles on the topic 'Nickel(II) oxide'

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