Nickel(II) acetate
{{Chembox
| Watchedfields = changed
| verifiedrevid = 433903788
| Name =
| ImageFile1 = Nickel(II) acetate tetrahydrate.jpg
| ImageFile2 = Nickel(II)-acetate-tetrahydrate-3D-balls.png
| IUPACName =
| SystematicName = Nickel(2+) diacetate
| OtherNames =
| Section1 = {{Chembox Identifiers
| Abbreviations =
| CASNo = 373-02-4
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo1 = 6018-89-9
| CASNo1_Ref = {{cascite|correct|CAS}}
| index1_label = (tetrahydrate)
| DTXSID1 = DTXSID9075458
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 99QP4ELX96
| UNII1 = 6SOA8L0560
| UNII1_Ref = {{fdacite|correct|FDA}}
| EINECS = 239-086-1
| PubChem = 9756
| PubChem1 = 62601
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 9373
| ChemSpiderID1 = 56360
| UNNumber = 2811
| SMILES = [Ni+2].[O-]C(=O)C.[O-]C(=O)C
| SMILES_Comment = ionic form
| SMILES3 = O=C(C)O[Ni]OC(C)=O
| SMILES3_Comment = coordination form (anhydrate)
| SMILES1 = CC(=O)[O-].CC(=O)[O-].O.O.O.O.[Ni+2]
| InChI1=1S/2C2H4O2.Ni.4H2O/c2*1-2(3)4;;;;;/h2*1H3,(H,3,4);;4*1H2/q;;+2;;;;/p-2
| InChIKey1 = OINIXPNQKAZCRL-UHFFFAOYSA-L
| InChI = InChI=1S/2C2H4O2.Ni/c2*1-2(3)4;/h2*1H3,(H,3,4);/q;;+2/p-2
| StdInChIKey = AIYYMMQIMJOTBM-UHFFFAOYSA-L
| RTECS =
| MeSHName =
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI =
| KEGG_Ref = {{keggcite|correct|kegg}}
| KEGG =
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| Section2 = {{Chembox Properties
| Ni=1 | O=4 | C=4 | H=6
| Appearance = Mint-green Solid
| Odor = slight acetic acid
| Density = 1.798 g/cm3 (anhydrous)
1.744 g/cm3 (tetrahydrate)
| MeltingPt = decomposes when heated 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}}.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}}.
| MeltingPt_notes =
| BoilingPt =
| BoilingPt_notes =
| Solubility = Easily soluble in cold water, hot water
| SolubleOther = Soluble in methanol
insoluble in diethyl ether, n-octanol
| Solvent =
| LogP =
| VaporPressure =
| HenryConstant =
| AtmosphericOHRateConstant =
| pKa =
| pKb =
| MagSus = +4,690.0·10−6 cm3/mol
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| Section3 = {{Chembox Structure
| CrystalStruct = monoclinic
| SpaceGroup = P21/c
| LattConst_a = 4.764
| LattConst_b = 11.771
| LattConst_c = 8.425 Å
| LattConst_beta = 93.6
| LattConst_Comment = tetrahydrate
| UnitCellVolume = 471.5
| UnitCellFormulas = 2
| Coordination = distorted octahedral
}}
| Section4 = {{Chembox Thermochemistry
| DeltaHf =
| DeltaHc =
| Entropy =
| HeatCapacity =
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| Section7 = {{Chembox Hazards
| ExternalSDS =
| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|H302|H317|H332|H334|H341|H350|H360|H372|H410}}
| PPhrases = {{P-phrases|P203|P233|P260|P261|P264|P270|P271|P272|P273|P280|P284|P301+P317|P302+P352|P304+P340|P317|P318|P319|P321|P330|P333+P317|P342+P316|P362+P364|P391|P403|P405|P501}}
| MainHazards =
| NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S =
| FlashPt =
| AutoignitionPt =
| ExploLimits =
| LD50 = 350 mg/kg (rat, oral)
410 mg/kg (mouse, oral){{IDLH|7440020|Nickel metal and other compounds (as Ni)}}
| PEL =
}}
| Section8 = {{Chembox Related
| OtherAnions =
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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 mint-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 mint-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.{{cite journal | doi = 10.1107/S0365110X5300171X | journal = Acta Crystallogr. | title = The crystal structures of nickel acetate, Ni(CH3COO)2·4H2O, and cobalt acetate, Co(CH3COO)2·4H2O | year = 1953 | last1 = Van Niekerk | first1 = J. N. | last2 = Schoening | first2 = F. R. L. | volume = 6 | issue = 7 | pages = 609–612}} It may be dehydrated in vacuo, by reaction with acetic anhydride{{Ullmann's | doi = 10.1002/14356007.a17_235.pub2 | title = Nickel Compounds | year = 2005 | last1 = Lascelles | first1 = Keith | last2 = Morgan | first2 = Lindsay G. | last3 = Nicholls | first3 = David | last4 = Beyersmann | first4 = Detmar}} or by heat.{{Cite journal | doi = 10.1021/ic50008a039 | journal = Inorg. Chem. | title = Cobalt and Nickel Acetates in Anhydrous Acetic Acid | year = 1963 | last1 = Tappmeyer | first1 = W. P. | last2 = Davidson | first2 = Arthur W. | volume = 2 | issue = 4 | pages = 823–825}}
Safety
Nickel salts are toxic, carcinogenic and irritate the skin.