Nickel(II) acetate
Names
Systematic IUPAC name
Nickel(2+) diacetate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.006.147
EC Number
  • 239-086-1
UNII
  • 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 (anhydrate): O=C(C)O[Ni]OC(C)=O
  • coordination form (tetrahydrate): O=C(C)O[Ni-4](OC(C)=O)([O+H2])([O+H2])([O+H2])[O+H2]
Properties
C4H6NiO4
Molar mass 176.781 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]
Easily soluble in cold water, hot water
Solubility Soluble in methanol
insoluble in diethyl ether, n-octanol
+4,690.0·10−6 cm3/mol
Structure
monoclinic
P21/c
a = 4.764, b = 11.771, c = 8.425 Å
α = 90°, β = 93.6°, γ = 90°[3]
tetrahydrate
471.5
2
distorted octahedral
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
2
0
0
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

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.

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. Bibcode:1971AcCrB..27..706D. doi:10.1107/S0567740871002802.
  4. ↑ "Nickel metal and other compounds (as Ni)". Immediately Dangerous to Life or 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. ISBN 978-3527306732.
  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.
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