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Preferred IUPAC name
Other names
3D model (JSmol)
  • InChI=1S/C3F6S/c4-2(5,6)1(10)3(7,8)9[1]
  • FC(F)(F)C(=S)C(F)(F)F
Molar mass 182.08 g·mol−1
Appearance blue gas
Boiling point 8 °C (46 °F; 281 K)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Hexafluorothioacetone is an organic perfluoro thione compound with formula CF3CSCF3. At standard conditions it is a blue gas.[2]


Hexafluorothioacetone was first produced by Middleton in 1961 by boiling bis-(perfluoroisopropyl)mercury with sulfur.


Hexafluorothioacetone boils at 8 °C.[3] Below this it is a blue liquid.[2]


The blue colour is due to absorption in the visible light range with bands at 800–675 nm and 725–400 nm. These bands are due to T1–S0 and S1–S0 transitions.[2] There is also a strong absorption in ultraviolet around 230-190 nm.[2]


Hexafluorothioacetone acts more like a true thiocarbonyl (C=S) than many other thiocarbonyl compounds, because it is not able to form thioenol compounds (=C-S-H), and the sulfur is not in a negative ionized state (C-S).[4] Hexafluorothioacetone is not attacked by water or oxygen at standard conditions as are many other thiocarbonyls.[2]

Bases trigger the formation of a dimer 2,2,4,4-tetrakis-(trifluoromethyl)-1,3-dithietane.[2] Bases includes amines.[4]

The dimer can be heated to regenerate the hexafluorothioacetone monomer.[2]

The dimer is also produced in a reaction with hexafluoropropene and sulfur with some potassium fluoride.[2][5]

Hexafluorothioacetone reacts with bisulfite to form a Bunte salt CH(CF3)2SSO2.[4]

Mercaptans reacting with hexafluorothioacetone yield disulfides or a thiohemiketal:

R-SH + C(CF3)2S → R-S-S-CH(CF3)2.[4]
R-SH + C(CF3)2S → RSC(CF3)2SH (for example in methyl mercaptan or ethyl mercaptan).[4]

With mercaptoacetic acid, instead of a thiohemiketal, water elimination yields a ring shaped molecule called a dithiolanone -CH2C(O)SC(CF3)2S- (2,2-di(trifluoromethyl)-1,3-dithiolan-4-one).[4] Aqueous hydrogen chloride results in the formation of a dimeric disulfide CH(CF3)2SSC(CF3)2Cl.[4] Hydrogen bromide with water yields the similar CH(CF3)2SSC(CF3)2Br.[4] Dry hydrogen iodide does something different and reduces the sulfur making CH(CF3)2SH. Wet hydrogen iodide only reduces to a disulfide CH(CF3)2SSC(CF3)2H. Strong organic acids add water to yield a disulfide compound CH(CF3)2SSC(CF3)2OH.[4]

Chlorine and bromine add to hexafluorothioacetone to make CCl(CF3)2SCl and CBr(CF3)2SBr.[4]

With diazomethane hexafluorothioacetone produces 2,2,5,5-tetrakis(trifluoromethyl)-l,3-dithiolane, another substituted dithiolane.[4] Diphenyldiazoniethane reacts to form a three membered ring called a thiirane (di-2,2-trifluoromethyl-di-3,3-phenyl-thiirane)

Trialkylphosphites (P(OR)3) react to make a trialkoxybis(trifluoromethyl)methylenephosphorane (RO)3P=C(CF3)2 and a thiophosphite (RO)3PS.[4]

Hexafluorothioacetone can act as a ligand on nickel.[6]

Hexafluorothioacetone is highly reactive to alkenes and dienes combining via addition reactions. With butadiene it reacts even as low as -78 °C to yield 2,2-bis-(trifluoromethyl)-3,6-dihydro-2H-l-thiapyran.[7]

See also[edit]


  1. ^ Gupta, Kartick; Giri, Santanab; Chattaraj, P. K. (February 2013). "Charge-based DFT descriptors for Diels-Alder reactions". Journal of Physical Organic Chemistry. 26 (2): 187–193. doi:10.1002/poc.2987.
  2. ^ a b c d e f g h Clouthier, Dennis J.; Joo, Duck-Lae (8 May 1997). "The spectroscopy of hexafluorothioacetone, a blue gas". The Journal of Chemical Physics. 106 (18): 7479–7490. Bibcode:1997JChPh.106.7479C. doi:10.1063/1.473753.
  3. ^ Knunyants, I. L.; Yakobson, G. G. (2012). Syntheses of Fluoroorganic Compounds. Springer Science & Business Media. pp. 45–46. ISBN 9783642702075.
  4. ^ a b c d e f g h i j k l Middleton, W. J.; Sharkey, W. H. (May 1965). "Fluorothiocarbonyl Compounds. II. Reactions of Hexafluorothioacetone". The Journal of Organic Chemistry. 30 (5): 1384–1390. doi:10.1021/jo01016a009.
  5. ^ Dyatkin, B.L.; Sterlin, S.R.; Zhuravkova, L.G.; Martynov, B.I.; Mysov, E.I.; Knunyants, I.L. (January 1973). "Reactions of perfluoroalkylcarbanions with sulphur". Tetrahedron. 29 (18): 2759–2767. doi:10.1016/S0040-4020(01)93398-8.
  6. ^ Browning, Jane; Cundy, C. S.; Green, M.; Stone, F. G. A. (1969). "Hexafluoroacetone and hexafluorothioacetone nickel complexes". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 20. doi:10.1039/J19690000020.
  7. ^ Middleton, W. J.; Howard, E. G.; Sharkey, W. H. (June 1961). "Perfluorothiocarbonyl Compounds". Journal of the American Chemical Society. 83 (11): 2589–2590. doi:10.1021/ja01472a045.

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