![]() | |
Names | |
---|---|
Preferred IUPAC name
1,1,2,3,3,3-Hexachloroprop-1-ene | |
Identifiers | |
3D model (JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.015.965 |
EC Number |
|
PubChem CID
|
|
UNII | |
UN number | 3382 3082 |
CompTox Dashboard (EPA)
|
|
| |
| |
Properties | |
C3Cl6 | |
Molar mass | 248.75 g/mol |
Appearance | colourless liquid[1] |
Density | 1.765 g/cm3 (at 25 °C) |
Melting point | −73[1] °C (−99 °F; 200 K) |
Boiling point | 209–210[1] °C (408–410 °F; 482–483 K) |
0.25 g/L[1] | |
Solubility | soluble in carbon tetrachloride, ethanol and diethyl ether[2] |
Hazards | |
GHS labelling: | |
![]() ![]() | |
Danger | |
H315, H319, H330, H332, H335 | |
P260, P261, P264, P271, P280, P284, P302+P352, P304+P312, P304+P340, P305+P351+P338, P310, P312, P320, P321, P332+P313, P337+P313, P362, P403+P233, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Hexachloropropene is a compound of chlorine and carbon with the linear formula CCl3CCl=CCl2.[3] It is a colourless liquid at room temperature. It is toxic for humans.
Hexachloropropene can be produced by the dehydrochlorination reaction of 1,1,1,2,2,3,3-heptachloropropane by potassium hydroxide in methanol solution.[4] 1,1,1,2,2,3,3-Heptachloropropane is produced by the reaction of chloroform and tetrachloroethylene:
Hexachloropropene can be used to produce other compounds such as uranium tetrachloride, anhydrous niobium pentachloride and tungsten hexachloride.[5]
References
[edit]- ^ a b c d Hexachlorpropen
- ^ Gangolli, S.; Royal Society of Chemistry (1999). The dictionary of substances and their effects. Cambridge, UK. p. 607. ISBN 0-85404-803-0. OCLC 41660040.
{{cite book}}
: CS1 maint: location missing publisher (link) - ^ "Hexachloropropene96%". Sigma Aldrich. Retrieved Nov 27, 2013.
- ^ Friedrich Boberg (1964-11-16). "Über 1.2-Dithia-cyclopentene, V. 4.5-Dichlor-1.2-dithia-cyclopentenon-(3)". Justus Liebigs Annalen der Chemie (in German). 679 (1): 109–118. doi:10.1002/jlac.19646790115. Retrieved 2022-03-08.
- ^ W. W. Porterfield and S. Y. Tyree, Jr. (1967), S. Young Tyree, Jr. (ed.), Anhydrous metal chlorides, McGraw-Hill Book Company, Inc., pp. 133–136