Iodine trichloride




































































Iodine trichloride

Full structural formula of the dimer

Space-filling model of the dimer

Commercial sample of iodine trichloride
Names

IUPAC name
iodine trichloride

Identifiers

CAS Number

  • 865-44-1 ☑Y

3D model (JSmol)
  • Interactive image

ChemSpider

  • 63265 ☑Y

ECHA InfoCard
100.011.582


PubChem CID
  • 70076




Properties

Chemical formula

 I2Cl6

Molar mass
 466.5281 g/mol
Appearance
 yellow solid

Density
 3.11 g/cm3

Melting point
 63 °C (145 °F; 336 K)


Magnetic susceptibility (χ)

 −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).


☑Y verify (what is ☑Y☒N ?)

Infobox references

Iodine trichloride is an interhalogen compound of iodine and chlorine. It is bright yellow and in the solid state is present as a planar dimer I2Cl6, Cl2I(μ-Cl)2ICl2, with two bridging Cl atoms.[1]


It can be prepared by reacting iodine with an excess of liquid chlorine at −70 °C. In the molten state it is conductive, which may indicate dissociation:[2]


I2Cl6 ⇌ ICl2+ + ICl4−

Iodine trichloride can be created by heating a mixture of liquid iodine and chlorine gas to 105 °C.


It is an oxidizing agent, capable of causing fire on contact with organic materials.



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..mw-parser-output cite.citation{font-style:inherit}.mw-parser-output .citation q{quotes:"""""""'""'"}.mw-parser-output .citation .cs1-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration{color:#555}.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration span{border-bottom:1px dotted;cursor:help}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output code.cs1-code{color:inherit;background:inherit;border:inherit;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;font-size:100%}.mw-parser-output .cs1-visible-error{font-size:100%}.mw-parser-output .cs1-maint{display:none;color:#33aa33;margin-left:0.3em}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-right{padding-right:0.2em}


  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.










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