Jump to content

Triphosgene

From Wikipedia, the free encyclopedia

This is an old revision of this page, as edited by Dork (talk | contribs) at 02:12, 23 February 2016 (skeletal svg). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.

Triphosgene
Names
IUPAC name
Bis(trichloromethyl) carbonate
Other names
BTC
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.046.336 Edit this at Wikidata
  • InChI=1S/C3Cl6O3/c4-2(5,6)11-1(10)12-3(7,8)9 checkY
    Key: UCPYLLCMEDAXFR-UHFFFAOYSA-N checkY
  • InChI=1/C3Cl6O3/c4-2(5,6)11-1(10)12-3(7,8)9
    Key: UCPYLLCMEDAXFR-UHFFFAOYAA
  • ClC(Cl)(Cl)OC(=O)OC(Cl)(Cl)Cl
Properties
C3Cl6O3
Molar mass 296.748 g/mol
Appearance white crystals
Density 1.780 g/cm3
Melting point 80 °C (176 °F; 353 K)
Boiling point 206 °C (403 °F; 479 K)
Reacts
Hazards
Safety data sheet (SDS) Fisher MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Triphosgene (bis(trichloromethyl) carbonate (BTC), C3Cl6O3) is a chemical compound that is used as a safer substitute for phosgene, because at room temperature it is a solid crystal, as opposed to phosgene which is a gas.[1] Triphosgene crystals decompose above 200 °C[2]

Preparation

This compound is commercially available. It is prepared by exhaustive free radical chlorination of dimethyl carbonate:[1]

CH3OCO2CH3 + 6 Cl2 → CCl3OCO2CCl3 + 6 HCl

Triphosgene can be easily recrystallized from boiling hexanes to yield pure white crystals.

Uses

Triphosgene is used as a reagent in organic synthesis and is a less hazardous substitute for phosgene for a variety of chemical transformations including to bond one carbonyl group to two alcohols, and to convert an amine group into isocyanate.[1]

Safety

The toxicity of triphosgene is the same as phosgene since it decomposes to phosgene on heating and upon reaction with nucleophiles. Even trace moisture leads to formation of phosgene. Therefore, this reagent can be safely handled if one takes all the precautions as for phosgene.[3]

See also

References

  1. ^ a b c Dr. Heiner Eckert; Dr. Barbara Forster (1987). "Triphosgene, a Crystalline Phosgene Substitute". Angew. Chem. Int. Ed. Engl. 26 (9): 894–895. doi:10.1002/anie.198708941.
  2. ^ Dr. Heiner Eckert (2011). "Phosgenation Reactions with Phosgene from Triphosgene". Chim. Oggi Chem. Today. 29 (6): 40–46.
  3. ^ Suresh B. Damle (1993-02-08). "Safe handling of diphosgene, triphosgene". C&E News. 71 (6): 4.
Retrieved from "https://en.wikipedia.org/w/index.php?title=Triphosgene&oldid=706394454"