Nickel(II) acetate

Nickel(II) acetate
Names
	Systematic IUPAC name Nickel(2+) diacetate
Identifiers
CAS Number	373-02-4 ; 6018-89-9 (tetrahydrate) ;
3D model (JSmol)	Interactive image;
ECHA InfoCard	100.006.147
EC Number	239-086-1;
PubChem CID	9756;
CompTox Dashboard (EPA)	DTXSID7020926 ;
	InChI InChI=1S/2C2H4O2.Ni/c21-2(3)4;/h21H3,(H,3,4);/q;;+2/p-2;
	SMILES [Ni+2].[O-]C(=O)C.[O-]C(=O)C;
Properties
Chemical formula	C4H6NiO4
Molar mass	176.781 g·mol−1
Appearance	Green Solid
Odor	slight acetic acid
Density	1.798 g/cm3 (anyhdrous) ; 1.744 g/cm3 (tetrahydrate)
Melting point	250 °C (sublimes)
Boiling point	16.6 °C (tetrahydrate)
Solubility in water	Easily soluble in cold water, hot water
Solubility	Soluble in methanol ; insoluble in diethyl ether, n-octanol
Hazards
NFPA 704 (fire diamond)	2 0 0
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Nickel(II) acetate (Ni(CH₃COO)₂)is an inorganic compound of nickel and acetic acid. This inorganic compound is usually found as the tetrahydrate. It is used for electroplating.

It can be made by reacting nickel with Acetic acid or with nickel(II) carbonate.

Ni + CH₃COOH → C₄H₆NiO₄ + H₂O

NiCO₃ + CH₃COOH → C₄H₆NiO₄ + CO₂ + H₂O

The green tetrahydrate has been determined by X-ray crystallography to be octahedral about the central nickel atom, coordinated by four water molecules and two acetate fragments.^[1] It may be dehydrated in vacuo, by reaction with acetic anhydride,^[2] or by heat.^[3]

Safety

Nickel salts are carcinogenic and irritate the skin.

References

^ 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&middot4H₂O". Acta Cryst. 6 (7): 609–612. doi:10.1107/S0365110X5300171X.
^ 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 978-3527306732.
^ 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.

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[1] 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&middot4H₂O". Acta Cryst. 6 (7): 609–612. doi:10.1107/S0365110X5300171X.

[2] 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 978-3527306732.

[3] 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.

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