Nickel(II) Acetate - Wikipedia

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• 1 Synthesis and structure
• 2 Safety
• 3 References

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Appearance move to sidebar hide From Wikipedia, the free encyclopedia Nickel(II) acetate

Names
Systematic IUPAC name Nickel(2+) diacetate
Identifiers
CAS Number	373-02-4 Y (tetrahydrate): 6018-89-9 Y
3D model (JSmol)	ionic form: Interactive image (tetrahydrate): Interactive image coordination form (anhydrate): Interactive image
ChemSpider	9373 N (tetrahydrate): 56360
ECHA InfoCard	100.006.147
EC Number	239-086-1
PubChem CID	9756 (tetrahydrate): 62601
UNII	99QP4ELX96 Y (tetrahydrate): 6SOA8L0560 Y
UN number	2811
CompTox Dashboard (EPA)	DTXSID7020926 (tetrahydrate): DTXSID9075458
InChI Key: AIYYMMQIMJOTBM-UHFFFAOYSA-L InChI=1S/2C2H4O2.Ni/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2 (tetrahydrate): InChI=1S/2C2H4O2.Ni.4H2O/c2*1-2(3)4;;;;;/h2*1H3,(H,3,4);;4*1H2/q;;+2;;;;/p-2Key: OINIXPNQKAZCRL-UHFFFAOYSA-L
SMILES ionic form: [Ni+2].[O-]C(=O)C.[O-]C(=O)C (tetrahydrate): CC(=O)[O-].CC(=O)[O-].O.O.O.O.[Ni+2] coordination form (anhydrate): O=C(C)O[Ni]OC(C)=O
Properties
Chemical formula	C4H6NiO4
Molar mass	176.781 g·mol−1
Appearance	Mint-green Solid
Odor	slight acetic acid
Density	1.798 g/cm3 (anhydrous) 1.744 g/cm3 (tetrahydrate)
Melting point	decomposes when heated [1][2]
Solubility in water	Easily soluble in cold water, hot water
Solubility	Soluble in methanol insoluble in diethyl ether, n-octanol
Magnetic susceptibility (χ)	+4,690.0·10−6 cm3/mol
Structure
Crystal structure	monoclinic
Space group	P21/c
Lattice constant	a = 4.764, b = 11.771, c = 8.425 Åα = 90°, β = 93.6°, γ = 90°[3]tetrahydrate
Lattice volume (V)	471.5
Formula units (Z)	2
Coordination geometry	distorted octahedral
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H317, H332, H334, H341, H350, H360, H372, H410
Precautionary statements	P203, P233, P260, P261, P264, P270, P271, P272, P273, P280, P284, P301+P317, P302+P352, P304+P340, P317, P318, P319, P321, P330, P333+P317, P342+P316, P362+P364, P391, P403, P405, P501
NFPA 704 (fire diamond)	2 0 0
Lethal dose or concentration (LD, LC):
LD50 (median dose)	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). Y verify (what is YN ?) Infobox references

Chemical compound

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 mint-green tetrahydrate Ni(CH3CO2)2·4 H2O is most common. It is used for electroplating.

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 mint-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]

Safety

[edit]

Nickel salts are toxic, 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. Bibcode:1971AcCrB..27..706D. doi:10.1107/S0567740871002802.
4. ^ "Nickel metal and other compounds (as Ni)". Immediately Dangerous to Life or Health Concentrations. National Institute for Occupational Safety and Health.
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. ISBN 978-3-527-30673-2.
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.

v t e Nickel compounds
Nickel(0)	Ni(CO)4 Ni(COD)2 Ni(PPh3)4
Nickel(II)	NiF2 K2NiF4 NiF2−4 NiCl2 NiCl2−4 NiBr2 NiBr2−4 NiI2 NiI2−4 Ni(CN)2 K2Ni(CN)4 Ni(SCN)2 NiO Ni(OH)2 NiCO3 NiSO4 Ni3(PO4)2 NiCrO4 NiTiO3 NiSeO4 NiS NiSe Ni(ClO4)2 Ni(NO3)2 Ni(NO2)2 Ni(NO2)3−5 / Ni(NO2)4−6 Ni(CO2H)2 C24H46NiO4 C36H70NiO4 Ni(acac)2
Nickel(III)	NiF3 Ni2O3 NiOOH
Nickel(IV)	NiF4 K2NiF6 MNiOx

v t e Acetyl halides and salts of the acetate ion

AcOH He LiOAc Be(OAc)2Be4O(OAc)6 B(OAc)3B2O(OAc)4 AcOAcROAc NH4OAc AcOOH FAcFOAc Ne NaOAcNaH(OAc)2 Mg(OAc)2 Al(OAc)3"ALSOL"Al(OAc)2OHAl(OH)2OAcAl2SO4(OAc)4 Si P S ClAcClOAc Ar KOAc Ca(OAc)2 Sc(OAc)3 Ti(OAc)4 VO(OAc)2 Cr(OAc)2Cr(OAc)3 Mn(OAc)2Mn(OAc)3 Fe(OAc)2Fe(OAc)3 Co(OAc)2 [CoO(OAc)py]4 Ni(OAc)2 CuOAcCu(OAc)2 Zn(OAc)2 Ga(OAc)3 Ge As(OAc)3 Se BrAcBrOAc Kr RbOAc Sr(OAc)2 Y(OAc)3 Zr(OAc)4 Nb Mo(OAc)2 Tc Ru2(OAc)4ClRu(OAc)3 Rh2(OAc)4 Pd(OAc)2 AgOAc Cd(OAc)2 In(OAc)3 Sn(OAc)2Sn(OAc)4 Sb(OAc)3 Te IAcIOAcI(OAc)3 Xe CsOAc Ba(OAc)2 * Lu(OAc)3 Hf Ta W Re Os Ir Pt(OAc)2 Au(OAc)3 Hg2(OAc)2Hg(OAc)2 TlOAcTl(OAc)3 Pb(OAc)2Pb(OAc)4 Bi(OAc)3 Po At Rn Fr Ra ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og   * La(OAc)3 Ce(OAc)3 Pr(OAc)3 Nd(OAc)3 Pm Sm(OAc)3 Eu(OAc)3 Gd(OAc)3 Tb(OAc)3 Dy(OAc)3 Ho(OAc)3 Er(OAc)3 Tm(OAc)3 Yb(OAc)3 ** Ac(OAc)3 Th(OAc)4 Pa U(OAc)4 UO2(OAc)2 NpO2OAcNpO2(OAc)2 PuO2(OAc)2 Am Cm Bk Cf Es Fm Md No

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