Ampoule containing ICl3 and its dimer formula
| IUPAC name
| Other names
Diiodine hexachloride (dimer)
| ICl3 (monomer)|
|Molar mass|| 233.264 g/mol (monomer)|
466.5281 g/mol (dimer)
|Appearance||Yellow or red solid|
|Density|| 3.203 g/cm3 (-40 °C)|
3.11 g/cm3 (15 °C)
|Melting point||63 °C (145 °F; 336 K)|
|Solubility|| Reacts with alcohols|
Soluble in acetic acid, acetone, arsenic trichloride, bromine, dichloroacetic acid, methyl ethyl ketone, phosgene, phosphoryl chloride, sulfuryl chloride
Slightly soluble in liq. SO2
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Iodine trichloride slowly fumes in open air, more vigorously in liquid form. It reacts with water, slowly with cold water and rapidly with warm/hot water. It also reacts vigorously with alkalis.
- 2 ICl3 + 3 H2O → 5 HCl + HIO3 + ICl (cold water)
- 5 ICl3 + 9 H2O → 15 HCl + 3 HIO3 + I2 (hot water)
- ICl3 → ICl + Cl2
Iodine trichloride is a bright yellow solid which upon exposure to light turns red due to the presence of elemental iodine.
Iodine trichloride is sold by chemical suppliers, but it's not easy to acquire.
Can be prepared by reacting iodine with an excess of liquid chlorine at −70 °C.
- Compound collecting
- Pyrotechnic demonstrations
Iodine trichloride is highly corrosive and toxic. Wear proper protection when handling it.
The only safe way to store this compound is in glass ampoules.
Iodine trichloride can be safely neutralized by adding it in very cold water containing very diluted solution of sodium hydroxide and sodium thiosulfate.
- Finkelstein, W.; Zh. Russ. Fiz. - Khim. O - va., Chast Khim.; vol. 58; (1926); p. 565
- Beckmann, E.; Junker, F.; Z. Anorg. Chem.; vol. 55; (1907); p. 375 - 375