Iodine trichloride

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Iodine trichloride
Full structural formula of the dimer Iodine trichloride.svg
Full structural formula of the dimer
Space-filling model of the dimer Iodine-trichloride-dimer-3D-vdW.png
Space-filling model of the dimer
Commercial sample of iodine trichloride Iodine trichloride cropped.jpg
Commercial sample of iodine trichloride
Names
IUPAC name
Iodine trichloride
Other names
Diiodine hexachloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.011.582 OOjs UI icon edit-ltr-progressive.svg
PubChem CID
UNII
  • InChI=1S/Cl3I/c1-4(2)3 Yes check.svgY
    Key: PAWIVBWALDNUJP-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/Cl3I/c1-4(2)3
    Key: PAWIVBWALDNUJP-UHFFFAOYAF
Properties
I2Cl6
Molar mass 466.5281 g/mol
Appearanceyellow solid
Density 3.11 g/cm3
Melting point 63 °C (145 °F; 336 K)
−90.2×10−6 cm3/mol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Iodine trichloride is an interhalogen compound of iodine and chlorine. It is bright yellow but with time and upon exposure to light it turns red due to decomposition with formation of elemental iodine. In the solid state is present as a planar dimer I2Cl6, with two bridging Cl atoms. [1]

It can be prepared by reacting iodine with an excess of liquid chlorine at −70 °C, [2] or heating a mixture of liquid iodine and chlorine gas to 105 °C.[ citation needed ] In the molten state it is conductive, which may indicate disproportionation into ions: [2]

I2Cl6ICl+
2
+ ICl
4

It is an oxidizing agent, capable of causing fire on contact with organic materials.[ citation needed ] That oxidizing power also makes it a useful catalyst for organic chlorination reactions. [3]

Iodine trichloride reacts with concentrated hydrochloric acid, forming tetrachloroiodic acid: [4]

ICl3 + HCl → HICl4

References

  1. K. H. Boswijk; E. H. Wiebenga (1954). "The crystal structure of I2Cl6 (ICl3)". Acta Crystallographica. 7 (5): 417–423. doi: 10.1107/S0365110X54001260 .
  2. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8.
  3. Sabatier, Paul (1922). Catalysis in Organic Chemistry (PDF). Translated by Reid, E. Emmet. New York, NY: Van Nostrand. p. 2.
  4. Bateman, Richard J.; Bateman, Linda R. (February 1972). "Solid-state structure, nuclear quadrupole resonance spectrum, and the resultant symmetry implications for tetrachloroiodic acid tetrahydrate" . Journal of the American Chemical Society. 94 (4): 1130–1134. doi:10.1021/ja00759a017. ISSN   0002-7863.