Nickel(II) iodide

Nickel(II) iodide
Names
IUPAC name
Nickel(II) iodide
Other names
Nickelous iodide
Identifiers
13462-90-3 YesY
3D model (Jmol) Interactive image
ECHA InfoCard 100.033.319
PubChem 26038
Properties
I2Ni
Molar mass 312.50 g·mol−1
Appearance iron-black solid (anhydrous)
bluish-green solid (hexahydrate)
Density 5.384 g/cm3
Melting point 780 °C (1,440 °F; 1,050 K) (anhydrous)
43 °C (hexahydrate, loses water)
124.2 g/100 mL (0 °C)
188.2 g/100 mL (100 °C)
Solubility alcohols
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
0
2
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 [77 °F], 100 kPa).
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Infobox references

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.[1] 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.[2]

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.[3] It is also has niche uses as a reagent in organic synthesis, especially in conjunction with samarium(II) iodide.[4]

References

  1. ↑ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): 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.
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