Barium iodide

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Barium iodide[1]
Cotunnite structure.png
IUPAC name
Barium iodide
Other names
Barium iodide, anhydrous
3D model (JSmol)
ECHA InfoCard 100.033.873
EC Number
  • 237-276-9
BaI2 (anhydrous)
BaI2·2H2O (dihydrate)
Molar mass 391.136 g/mol (anhydrous)
427.167 g/mol (dihydrate)
Appearance White orthorhombic crystals (anhydrous) colorless crystals (dihydrate)
Odor odorless
Density 5.15 g/cm3 (anhydrous)
4.916 g/cm3 (dihydrate)
Melting point 711 °C (1,312 °F; 984 K) (anhydrous)
decomposes at 740 °C (dihydrate)
166.7 g/100 mL (0 °C)
221 g/100 mL (20 °C)
246.6 g/100 mL (70 °C)
Solubility soluble in ethanol, acetone
-124.0·10−6 cm3/mol
Orthorhombic, oP12, SpaceGroup = Pnma, No. 62
-602.1 kJ·mol−1
Main hazards toxic
Related compounds
Other anions
barium fluoride
barium chloride
barium bromide
Other cations
beryllium iodide
magnesium iodide
calcium iodide
strontium 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

Barium iodide is an inorganic compound with the formula BaI2. The compound exists as an anhydrous and a hydrate (BaI2(H2O)2), both of which are white solids. When heated, hydrated barium iodide converts to the anhydrous salt. The hydrated form is freely soluble in water, ethanol, and acetone.


The structure of the anhydrous form resembles that of lead(II) chloride with each Ba center bound to nine iodide ligands[2] and has a crystalline packing structure that is quite similar to BaCl2.[3]


Anhydrous BaI2 can be prepared by treating Ba metal with 1,2-diiodoethane in ether.[4]

BaI2 reacts with alkyl potassium compounds to form organobarium compounds.[5]

BaI2 can be reduced with lithium biphenyl, to give a highly active form of barium metal.[6]


Like other soluble salts of barium, barium iodide is toxic.


  1. ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 4–44, ISBN 0-8493-0594-2
  2. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  3. ^ Brackett, E. B.; Brackett, T. E.; Sass, R. L.; The Crystal Structures of Barium Chloride, Barium Bromide, and Barium Iodide. J. Phys. Chem., 1963, volume 67, 2132 – 2135
  4. ^ Duval, E.; Zoltobroda, G.; Langlois, Y.; A new preparation of BaI2: application to (Z)-enol ether synthesis. Tetrahedron Letters, 2000, 41, 337-339
  5. ^ Walter, M. D.; Wolmershauser, G.; Sitzmann, H.; Calcium, Strontium, Barium, and Ytterbium Complexes with Cyclooctatetraenyl or Cyclononatetraenyl Ligands. J. Am. Chem. Soc., 2005, 127 (49), 17494 – 17503.
  6. ^ Yanagisawa, A.; Habaue, S.; Yasue, K.; Yamamoto, H.; Allylbarium Reagents: Unprecedented Regio- and Stereoselective Allylation Reactions of Carbonyl Compounds. J. Am. Chem. Soc.1994, 116,6130-6141