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Nickel(II) iodide

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Nickel(II) iodide
Nickel(II) iodide hexahydrate, NiI2•6H2O
Nickel(II) iodide hexahydrate, NiI2•6H2O
Nickel(II) iodide
Nickel(II) iodide
Names
IUPAC name Nickel(II) iodide
Other names Nickelous iodide
Identifiers
CAS Number
ECHA InfoCard 100.033.319 Edit this at Wikidata
PubChem CID
CompTox Dashboard (EPA)
Properties
Chemical formula I2Ni
Molar mass 312.5023 g·mol
Appearance black solid, hydrate is green
Density 5.38 g/cm
Melting point 780 °C (1,440 °F; 1,050 K)
Boiling point 797 °C (1,467 °F; 1,070 K)
Solubility in water good
Solubility alcohols
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2 0 0
Related compounds
Other anions nickel(II) chloride, nickel(II) bromide, nickel(II) fluoride
Other cations cobalt iodide, copper iodide,
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Nickel(II) iodide is an inorganic compound with the formula NiI2. This paramagnetic black solid dissolves readily in water to give blue-green solutions of the aquo complexes. This blue-green colour is typical of hydrated nickel(II) compounds. Nickel iodides find some applications in homogeneous catalysis.

Structure and synthesis

The anhydrous material crystallizes in the CdCl2 motif, featuring octahedral coordination geometry at each Ni(II) center. NiI2 is prepared by dehydration of the pentahydrate.

NiI2 readily hydrates, and the hydrated form can be prepared by dissolution of nickel oxide, hydroxide, or carbonate in hydroiodic acid. The anhydrous form can be produced by treating powdered nickel with iodine.

NiI2 has found some industrial applications as a catalyst in carbonylation reactions. It is also has niche uses as a reagent in organic synthesis, especially in conjunction with samarium(II) iodide.

References

  1. Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton, Florida: CRC Press. ISBN 0-8493-0486-5.
  2. Laird G. L. Ward, "Anhydrous Nickel (II) Halides and their Tetrakis(Ethanol) and 1,2-Dimethoxyethane Complexes" Inorganic Syntheses, 1972, Volume 13, Pages: 154–164, 2007. doi:10.1002/9780470132449.ch30
  3. W. Bertleff, M. Roeper, X. Sava, “Carbonylation” in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH: Weinheim, 2003. DOI: 10.1002/14356007.a05 217.
  4. Shinichi Saito, Nickel(II) Iodide" in Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, 2008. DOI: 10.1002/047084289X.rn00843. Article Online Posting Date: March 14, 2008.
Nickel compounds
Nickel(0)
Nickel(II)
Nickel(III)
Nickel(IV)


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