Nickel(II) acetate

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Nickel(II) acetate
Nickel(II) acetate tetrahydrate.jpg
Names
Systematic IUPAC name
Nickel(2+) diacetate
Identifiers
373-02-4 YesY
6018-89-9 (tetrahydrate) YesY
EC number 239-086-1
Jmol-3D images Image
PubChem 9756
Properties
C4H6NiO4
Molar mass 176.78 g·mol−1
Appearance Green Solid
Odor slight acetic acid
Density 1.798 g/cm3 (anyhdrous)
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
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY verify (what isYesY/N?)
Infobox references

Nickel(II) acetate is the name for inorganic compound with the formula Ni(CH3CO2)2(H2O)n. The green tetrahydrate is more 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(H2O)4 + 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.[3] It may be dehydrated in vacuo, by reaction with acetic anhydride,[4] or by heat.[5]

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. ^ 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 Cryst. 6 (7): 609–612. doi:10.1107/S0365110X5300171X. 
  4. ^ 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 
  5. ^ 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.