Nickel(II) acetate

Nickel(II) acetate

Names
Systematic IUPAC name Nickel(2+) diacetate
Identifiers
CAS Number	373-02-4 Y 6018-89-9 (tetrahydrate) Y
3D model (JSmol)	Interactive image
ECHA InfoCard	100.006.147
EC Number	239-086-1
PubChem CID	9756
InChI InChI=1S/2C2H4O2.Ni/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
SMILES [Ni+2].[O-]C(=O)C.[O-]C(=O)C
Properties
Chemical formula	C4H6NiO4
Molar mass	176.78 g·mol−1
Appearance	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 Å α = 90°, β = 93.6°, γ = 90°[3] tetrahydrate
Lattice volume (V)	471.5
Formula units (Z)	2
Coordination geometry	distorted octahedral
Hazards
NFPA 704	0 2 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).
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Infobox references

Nickel(II) acetate is the name for chemical compound with the formula Ni(CH₃CO₂)₂·2 H₂O or Ni(CH₃COO)₂·2 H₂O also abbreviated Ni(OAc)₂·2 H₂O. The green tetrahydrate Ni(CH₃COO)₂·4 H₂O is more common. It is used for electroplating.

Synthesis and structure

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]

Safety

Nickel salts are carcinogenic and irritate the skin.

References

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. 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.