Beryllium iodide

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Beryllium iodide
Beryllium iodide.svg
Systematic IUPAC name
Beryllium iodide
7787-53-3 N
ChemSpider 74209 YesY
Jmol-3D images Image
PubChem 82231
Molar mass 262.821 g/mol
Appearance colorless needle-like crystals
Density 4.325 g/cm³
Melting point 480 °C (896 °F; 753 K)
Boiling point 590 °C (1,094 °F; 863 K) [1]
reacts explosively[1][citation needed]
Solubility Slightly soluble in CS2
Soluble in ethanol, diethyl ether[2]
71.14 J/(mol × K)
130 J/mol K
-192.62 kJ/mol
-210 kJ/mol
19 kJ/mol
Main hazards see Berylliosis
US health exposure limits (NIOSH):
TWA 0.002 mg/m3
C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[3]
Ca C 0.0005 mg/m3 (as Be)[3]
Ca [4 mg/m3 (as Be)][3]
Related compounds
Other anions
Beryllium fluoride
Beryllium chloride
Beryllium bromide
Other cations
magnesium iodide
calcium iodide
strontium iodide
barium iodide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 N verify (what isYesY/N?)
Infobox references

Beryllium iodide is the chemical compound with the formula BeI2. It is very hygroscopic and reacts violently with water, forming hydroiodic acid.


Beryllium iodide can be prepared by reacting beryllium metal with elemental iodine at temperatures of 500 °C to 700 °C:[1]

Be + I2 → BeI2

Beryllium iodide is also formed when beryllium carbide reacts with hydrogen iodide in the gas phase:

Be2C + 4 HI → 2 BeI2 + CH4

The iodine in beryllium iodide is easily replaced with the other halogens; it reacts with fluorine giving beryllium fluoride and fluorides of iodine, with chlorine giving beryllium chloride, and with bromine giving beryllium bromide. Beryllium iodide also reacts violently with oxidising agents such as chlorate and permanganate to give purple vapour of iodine. The solid and vapor are both flammable in air.[2]


Beryllium iodide can be used in the preparation of high-purity beryllium by the decomposition of the compound on a hot tungsten filament.


  1. ^ a b c Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press, p. 63, ISBN 0-8493-8671-3, retrieved 2007-12-10 
  2. ^ a b Parsons, Charles Lathrop (1909), The Chemistry and Literature of Beryllium, Easton, Pa.: Chemical Publishing, pp. 22–23, retrieved 2007-12-10 
  3. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0054". National Institute for Occupational Safety and Health (NIOSH).