• Nickel Dimethylglyoxime

1. Nickel(II) hydroxide is the inorganic compound with the formula Ni(OH) 2. It is an apple-green solid that dissolves with decomposition in ammonia and amines and is attacked by acids. It is an apple-green solid that dissolves with decomposition in ammonia and amines and is attacked by acids.
2. Starting with the mass of Ni(DMG) 2 (that is the red precipitate), show the calculation to obtain the moles of Ni 2+ that is present in your Ni-en complex you analyzed. Be sure to include any appropriate chemical reactions that were used in the calculation.
3. Jan 09, 2008  Ni(DMG)2(s) is a red precipitate. As you can see nickel has not been oxidized, nickel is not oxidized as the Ni2+ ion only forms a complex. DMG has to be in an alcohol solution because It is the conjugate base, not dmgH2 itself, that forms the complexes.

Nickel(II) hydroxide is the inorganic compound with the formula Ni(OH)₂. It is an apple-green solid that dissolves with decomposition in ammonia and amines and is attacked by acids. It is electroactive, being converted to the Ni(III) oxy-hydroxide, leading to widespread applications in rechargeable batteries.^[4]

Properties[edit]

We describe the high yield synthesis of multi-walled carbon nanotubes (MWCNTs) and the determination of the optimum production conclitions. The method involves the catalytic pyrolysis of solid Ni(dMg)(2) under an At atmosphere. In a typical preparation of Ni-DMG, 1 g Ni(NO 3) 2 6H2O was added to a 25 mL of DMG solution, followed by stirring for 30 min. The mixed solution was centrifuged, and the precipitate was washed for several times with distilled water and dried at room temperature.

Nickel(II) hydroxide has two well-characterized polymorphs, α and β. The α structure consists of Ni(OH)₂ layers with intercalated anions or water.^[5][6] The β form adopts a hexagonal close-packed structure of Ni²⁺ and OH⁻ ions.^[5][6] In the presence of water, the α polymorph typically recrystallizes to the β form.^[5][7] In addition to the α and β polymorphs, several γ nickel hydroxides have been described, distinguished by crystal structures with much larger inter-sheet distances.^[5]

The mineral form of Ni(OH)₂, theophrastite, was first identified in the Vermion region of northern Greece, in 1980. It is found naturally as a translucent emerald-green crystal formed in thin sheets near the boundaries of idocrase or chlorite crystals.^[8] A nickel-magnesium variant of the mineral, (Ni,Mg)(OH)₂ had been previously discovered at Hagdale on the island of Unst in Scotland.^[9]

Reactions[edit]

Nickel(II) hydroxide is frequently used in electrical car batteries.^[6] Specifically, Ni(OH)₂ readily oxidizes to nickel oxyhydroxide, NiOOH, in combination with a reduction reaction, often of a metal hydride (reaction 1 and 2).^[10]

Reaction 1 Ni(OH)₂ + OH⁻ → NiO(OH) + H₂O + e⁻

Dmg mori machines tools trading co ltd toronto. Machine nameMachine numberModel yearMachine heightWidthDepthMass of machineSpecificationsMSL 0071B200986 in.73 in.67 in.7,750 lbs.Max.

Reaction 2 M + H₂O + e⁻ → MH + OH⁻

Net Reaction (in H₂O)Ni(OH)₂ + M → NiOOH + MH

Of the two polymorphs, α-Ni(OH)₂ has a higher theoretical capacity and thus is generally considered to be preferable in electrochemical applications. However, it transforms to β-Ni(OH)₂ in alkaline solutions, leading to many investigations into the possibility of stabilized α-Ni(OH)₂ electrodes for industrial applications.^[7]

Synthesis[edit]

The synthesis entails treating aqueous solutions of nickel(II) salts with potassium hydroxide.^[11]

Toxicity[edit]

The Ni²⁺ ion is a known carcinogen. Toxicity and related safety concerns have driven research into increasing the energy density of Ni(OH)₂ electrodes, such as the addition of calcium or cobalt hydroxides.^[4]

See also[edit]

References[edit]

1. ^Enoki, Toshiaki; Tsujikawa, Ikuji (1975). 'Magnetic Behaviours of a Random Magnet, Ni_pMg_(1-p)(OH₂)'. Journal of the Physical Society of Japan. 39 (2): 317. doi:10.1143/JPSJ.39.317.
2. ^ ^abZumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN978-0-618-94690-7.
3. ^ ^abcd'Nickel Hydroxide'. American Elements. Retrieved 2018-08-30.
4. ^ ^abChen, J.; Bradhurst, D.H.; Dou, S.X.; Liu, H.K. (1999). 'Nickel Hydroxide as an Active Material for the Positive Electrode in Rechargeable Alkaline Batteries'. J. Electrochem. Soc. 146 (10): 3606–3612. doi:10.1149/1.1392522.
5. ^ ^abcdOliva, P.; Leonardi, J.; Laurent, J.F. (1982). 'Review of the structure and the electrochemistry of nickel hydroxides and oxy-hydroxides'. Journal of Power Sources. 8 (2): 229–255. doi:10.1016/0378-7753(82)80057-8.
6. ^ ^abcJeevanandam, P.; Koltypin, Y.; Gedanken, A. (2001). 'Synthesis of Nanosized α-Nickel Hydroxide by a Sonochemical Method'. Nano Letters. 1 (5): 263–266. doi:10.1021/nl010003p.
7. ^ ^abShukla, A.K.; Kumar, V.G.; Munichandriah, N. (1994). 'Stabilized α-Ni(OH)₂ as Electrode Material for Alkaline Secondary Cells'. J. Electrochem. Soc. 141 (11): 2956–2959. doi:10.1149/1.2059264.
8. ^Marcopoulos, T.; Economou, M. (1980). 'Theophrastite, Ni(OH)₂, a new mineral from northern Greece'(PDF). American Mineralogist. 66: 1020–1021.
9. ^Livingston, A.; Bish, D. L. (1982). 'On the new mineral theophrastite, a nickel hydroxide, from Unst, Shetland, Scotland'(PDF). Mineralogical Magazine. 46 (338): 1. doi:10.1180/minmag.1982.046.338.01.
10. ^Ovshinsky, S.R.; Fetcenko, M.A.; Ross, J. (1993). 'A nickel metal hydride battery for electric vehicles'. Science. 260 (5105): 176–181. doi:10.1126/science.260.5105.176. PMID17807176.
11. ^Glemser, O. (1963) 'Nickel(II) Hydroxide' in 'Handbook of Preparative Inorganic Chemistry, 2nd ed. G. Brauer (ed.), Academic Press, NY. Vol. 1. p. 1549.

Nickel Dimethylglyoxime

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