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Apr 24, 2008 Homework Statement Name of complex ion CuCl4^2- The Attempt at a Solution I wrote tetrachlorocuprate(II) ion and my teacher says it is incorrect. I should write tetrachlorocopper(II) ion. 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. The β form adopts a hexagonal close-packed structure of Ni 2+ and OH − ions. The LibreTexts libraries are Powered by MindTouch ® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 25481-21-4 - HTLPAEWBUABNNS-UHFFFAOYSA-L - Nickel(II) EDTA complex - Similar structures search, synonyms, formulas, resource links, and other chemical information.

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]

For a Ni(II) assay, a 10 μL aliquot of dimethylglyoxime (DMG) dissolved in an ethanol solution (80 mM) was first introduced into the “Ni” symbol, followed by an addition of 10 μL of a solution of NaF and Na 2 S 2 O 3 dissolved in Milli-Q water (20 and 80 mg/mL, respectively). The latter solution was used for masking the interference of Cu. Ni(H2O)62+ (aq) + 2 dmg- (aq) “ Ni(dmg)2 (aq) + 6 H2O. To Conduct Demonstration. Leave one beaker of six (or seven, if CN- is being used) filled with NiCl2 or NiSO4 solution as a control. Add approximately 3 mL of 6M NH3 to the second beaker. Add approximately 0.5 mL of. How many d electrons are there in Co2+? For each complex ion formed, indicate the coordination number of the copper atom. Name each complex. Do your best to sketch a 3D representation of each Are isomers possible? If so, what are they? Record the observed color of each solution. What does this suggest about the wavelength of light absorbed for.

Properties[edit]

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⁻

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]

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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.

External links[edit]

Nickel nitrate is the inorganic compound Ni(NO₃)₂ or any hydrate thereof. The anhydrous form is not commonly encountered, thus 'nickel nitrate' usually refers to nickel(II) nitrate hexahydrate. The formula for this species is written in two ways: Ni(NO₃)₂^.6H₂O and, more descriptively [Ni(H₂O)₆](NO₃)₂. The latter formula indicates that the nickel(II) center is surrounded by six water molecules in this hydrated salt. In the hexahydrate, the nitrate anions are not bonded to nickel. Also known are three other hydrates: Ni(NO₃)₂^.9H₂O, Ni(NO₃)₂^.4H₂O, and Ni(NO₃)₂^.2H₂O. Anhydrous Ni(NO₃)₂ is also known.^[2]

It is prepared by the reaction of nickel oxide with nitric acid:

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NiO + 2 HNO₃ + 5 H₂O → Ni(NO₃)₂^.6H₂O

The anhydrous nickel nitrate is typically not prepared by the heating the hydrates. Rather is generated by reaction of hydrates with dinitrogen pentoxide or of nickel carbonyl with dinitrogen tetroxide:^[2]

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Ni(CO)₄ + 2 N₂O₄ → Ni(NO₃)₂ + 2 NO + 4 CO

The hydrated nitrate is often used as a precursor to supported nickel catalysts.

Safety[edit]

Like other nitrates, nickel nitrate is oxidizing. It is also irritating to the eyes, skin and, upon inhalation of the dust, respiratory tract. It may cause skin allergy. Nickel nitrate is a carcinogen, along with most other nickel compounds. The nickel ion is also toxic to aquatic organisms.

Uses[edit]

Nickel(II) nitrate is used as the precursor for the explosive Nickel Hydrazine Nitrate, which is used as lead-free and safer alternative to Lead Azide and Lead Styphnate.

References[edit]

1. ^Perry's Chem Eng Handbook, 7th Ed
2. ^ ^abKeith Lascelles, Lindsay G. Morgan, David Nicholls, Detmar Beyersmann, 'Nickel Compounds' in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a17_235.pub2

Ni Dmg 2 2 Aq 3d Structure System

Ni Dmg 2 2 Aq 3d Structure Pdf