Nickel(II) acetate

Nickel(II) acetate

Names
Systematic IUPAC name Nickel(2+) diacetate
Identifiers
CAS Number	373-02-4 6018-89-9 (tetrahydrate)
EC Number	239-086-1
Jmol interactive 3D	Image
PubChem	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/cm^3 (anyhdrous) 1.744 g/cm^3 (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
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)[3]
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 inorganic 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.^[4] It may be dehydrated in vacuo, by reaction with acetic anhydride,^[5] or by heat.^[6]

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. "Nickel metal and other compounds (as Ni)". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
4. 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.
5. 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
6. 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.

Salts and the ester of the Acetate ion
AcOH																	He
LiOAc	Be(OAc)2 BeAcOH											B(OAc)3	ROAc	NH4OAc	AcOAc	FAc	Ne
NaOAc	Mg(OAc)2											Al(OAc)3 ALSOL Al(OAc)2OH	Si	P	S	ClAc	Ar
KOAc	Ca(OAc)2	Sc(OAc)3	Ti(OAc)4	VO(OAc)3	Cr(OAc)2	Mn(OAc)2 MnAc3	Fe(OAc)2 FeAc3	Co(OAc)2, CoAc3	Ni(OAc)2	Cu(OAc)2	Zn(OAc)2	Ga(OAc)3	Ge	As	Se	BrAc	Kr
RbOAc	Sr(OAc)2	Y(OAc)3	Zr(OAc)4	Nb	Mo(OAc)2	Tc	Ru	Rh	Pd(OAc)2	AgOAc	Cd(OAc)2	In	Sn(OAc)2 SnAc4	Sb(OAc)3	Te	IAc	Xe
CsOAc	Ba(OAc)2		Hf	Ta	W	Re	Os	Ir	Pt(OAc)2	Au	Hg2(OAc)2, HgAc2	TlOAc Tl(OAc)3	Pb(OAc)2 Pb(OAc)4	Bi(OAc)3	Po	At	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Uut	Fl	Uup	Lv	Uus	Uuo
		↓
		La(OAc)3	Ce(OAc)x	Pr	Nd	Pm	Sm(OAc)3	Eu(OAc)3	Gd(OAc)3	Tb	Dy(OAc)3	Ho(OAc)3	Er	Tm	Yb(OAc)3	Lu(OAc)3
		Ac	Th	Pa	UO2(OAc)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr