Dmg Chemical Formula

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Nickel(II) acetate
Names
Systematic IUPAC name
Identifiers
3D model (JSmol)
  • ionic form: Interactive image
  • coordination form (anhydrate): Interactive image
  • coordination form (tetrahydrate): Interactive image
ECHA InfoCard100.006.147
EC Number
PubChemCID
CompTox Dashboard(EPA)
  • InChI=1S/2C2H4O2.Ni/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
  • ionic form: [Ni+2].[O-]C(=O)C.[O-]C(=O)C
  • coordination form (tetrahydrate): O=C(C)O[Ni-4](OC(C)=O)([O+H2])([O+H2])([O+H2])[O+H2]
Properties
C4H6NiO4
Molar mass176.781 g·mol−1
AppearanceGreen Solid
Odorslight acetic acid
Density1.798 g/cm3 (anhydrous)
1.744 g/cm3 (tetrahydrate)
Melting pointdecomposes when heated [1][2]
Easily soluble in cold water, hot water
SolubilitySoluble in methanol
insoluble in diethyl ether, n-octanol
+4,690.0·10−6 cm3/mol
Structure
monoclinic
P21/c
α = 90°, β = 93.6°, γ = 90°[3]
Lattice volume (V)
471.5
2
distorted octahedral
Hazards
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
350 mg/kg (rat, oral)
410 mg/kg (mouse, oral)[4]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Material Safety Data Sheet Dimethylglyoxime, 1% Alcoholic - 2 - Ingestion: May cause irritation of the digestive tract. Symptoms may include headache, excitement, fatigue. Enter a chemical formula to calculate its molar mass and elemental composition: Molar mass of Ni(dmg)2 is 288.9146 g/mol Formula in Hill system is C8H14N4NiO4.

Nickel(II) acetate is the name for the coordination compounds with the formula Ni(CH3CO2)2·x H2O where x can be 0, 2, and 4. The green tetrahydrate Ni(CH3CO2)2·4 H2O is most common. It is used for electroplating.

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Synthesis and structure[edit]

The compound can be prepared by treating nickel or nickel(II) carbonate with acetic acid:

NiCO3 + 2 CH3CO2H + 3 H2O → Ni(CH3CO2)2·4 H2O + CO2

The green tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central nickel centre being coordinated by four water molecules and two acetate ligands.[5] It may be dehydrated in vacuo, by reaction with acetic anhydride,[6] or by heat.[7]

Dmg Chemical Formula Calculator

Safety[edit]

Nickel salts are carcinogenic and irritate the skin.

References[edit]

  1. ^M. A. Mohamed, S. A. Halawy, M. M. Ebrahim: 'Non-isothermal decomposition of nickel acetate tetrahydrate', in: Journal of Analytical and Applied Pyrolysis, 1993, 27 (2), S. 109–110. doi:10.1016/0165-2370(93)80002-H.
  2. ^G. A. M. Hussein, A. K. H. Nohman, K. M. A. Attyia: 'Characterization of the decomposition course of nickel acetate tetrahydrate in air', in: Journal of Thermal Analysis and Calorimetry, 1994, 42, S. 1155–1165; doi:10.1007/BF02546925.
  3. ^Downie, T. C.; Harrison, W.; Raper, E. S.; Hepworth, M. A. (15 March 1971). 'A three-dimensional study of the crystal structure of nickel acetate tetrahydrate'. Acta Crystallographica Section B. 27 (3): 706–712. doi:10.1107/S0567740871002802.
  4. ^'Nickel metal and other compounds (as Ni)'. Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  5. ^Van Niekerk, J. N.; Schoening, F. R. L. (1953). 'The crystal structures of nickel acetate, Ni(CH3COO)2·4H2O, and cobalt acetate, Co(CH3COO)2·4H2O'. Acta Crystallogr.6 (7): 609–612. doi:10.1107/S0365110X5300171X.
  6. ^Lascelles, Keith; Morgan, Lindsay G.; Nicholls, David; Beyersmann, Detmar (2005). 'Nickel Compounds'. Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_235.pub2.
  7. ^Tappmeyer, W. P.; Davidson, Arthur W. (1963). 'Cobalt and Nickel Acetates in Anhydrous Acetic Acid'. Inorg. Chem.2 (4): 823–825. doi:10.1021/ic50008a039.
AcOHHe
LiOAcBe(OAc)2
BeAcOH		B(OAc)3AcOAc
ROAc		NH4OAcAcOOHFAcNe
NaOAcMg(OAc)2Al(OAc)3
ALSOL
Al(OAc)2OH
Al2SO4(OAc)4		SiPSClAcAr
KOAcCa(OAc)2Sc(OAc)3Ti(OAc)4VO(OAc)3Cr(OAc)2
Cr(OAc)3		Mn(OAc)2
Mn(OAc)3		Fe(OAc)2
Fe(OAc)3		Co(OAc)2,
Co(OAc)3		Ni(OAc)2Cu(OAc)2Zn(OAc)2Ga(OAc)3GeAs(OAc)3SeBrAcKr
RbOAcSr(OAc)2Y(OAc)3Zr(OAc)4NbMo(OAc)2TcRu(OAc)2
Ru(OAc)3
Ru(OAc)4		Rh2(OAc)4Pd(OAc)2AgOAcCd(OAc)2InSn(OAc)2
Sn(OAc)4		Sb(OAc)3TeIAcXe
CsOAcBa(OAc)2HfTaWReOsIrPt(OAc)2AuHg2(OAc)2,
Hg(OAc)2		TlOAc
Tl(OAc)3		Pb(OAc)2
Pb(OAc)4		Bi(OAc)3PoAtRn
FrRaRfDbSgBhHsMtDsRgCnNhFlMcLvTsOg
↓
La(OAc)3Ce(OAc)xPrNdPmSm(OAc)3Eu(OAc)3Gd(OAc)3TbDy(OAc)3Ho(OAc)3ErTmYb(OAc)3Lu(OAc)3
AcThPaUO2(OAc)2NpPuAmCmBkCfEsFmMdNoLr
Retrieved from 'https://en.wikipedia.org/w/index.php?title=Nickel(II)_acetate&oldid=894460861'
Nickel(II) hydroxide
Names
IUPAC name
Other names
Nickel hydroxide, Theophrastite
Identifiers
  • 12054-48-7
  • 36897-37-7 (monohydrate)
ChemSpider
ECHA InfoCard100.031.813
EC Number
  • 235-008-5
RTECS number
CompTox Dashboard(EPA)
  • Key: BFDHFSHZJLFAMC-UHFFFAOYSA-L
  • Key: BFDHFSHZJLFAMC-NUQVWONBAJ
  • [Ni+2].[OH-].[OH-]
Properties
Ni(OH)2
Molar mass92.724 g/mol (anhydrous)
110.72 g/mol (monohydrate)
Appearancegreen crystals
Density4.10 g/cm3
Melting point 230 °C (446 °F; 503 K) (anhydrous, decomposes)
0.13 g/L
+4500.0·10−6 cm3/mol
Structure[1]
hexagonal, hP3
P3m1, No. 164
α = 90°, β = 90°, γ = 120°
Thermochemistry
79 J·mol−1·K−1[2]
Std enthalpy of
formation(ΔfH⦵298)
−538 kJ·mol−1[2]
Hazards
Safety data sheetExternal SDS
GHS pictograms[3]
GHS Signal wordDanger[3]
H302, H332, H315, H334, H317, H341, H350, H360, H372[3]
P260, P284, P201, P280, P405, P501[3]
Lethal dose or concentration (LD, LC):
1515 mg/kg (oral, rat)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
The test tube in the middle contains a precipitate of nickel(II) hydroxide

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]

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]

Dmg Chemical Formula Chart

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]

Dmg Chemical Formula 2

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]

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]

Dimethylglyoxime

Dmg chemical formula pdf

References[edit]

  1. ^Enoki, Toshiaki; Tsujikawa, Ikuji (1975). 'Magnetic Behaviours of a Random Magnet, NipMg(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]

Dmg Chemical Formula

Retrieved from 'https://en.wikipedia.org/w/index.php?title=Nickel(II)_hydroxide&oldid=904764643'