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Hexafluoropropanone 3D structure
IUPAC names
Other names
acetone hexafluoride
3D model (Jmol)
ECHA InfoCard 100.010.616
RTECS number UC2450000
Molar mass 166.02 g/mol
Appearance Colorless gas
Odor musty[1]
Density 1.32 g/ml, liquid
Melting point −129 °C (144 K)
Boiling point −28 °C (245 K)
Reacts with water
Vapor pressure 5.8 atm (20 °C)[1]
Main hazards Toxic (T),
Corrosive (C)
R-phrases R14, R23/24/25,
R34, R60, R63
S-phrases S7/9, S26, S28,
S36, S45, S53
NFPA 704
Flammability (red): no hazard code Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g., phosphorus Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
Flash point Nonflammable[1]
US health exposure limits (NIOSH):
PEL (Permissible)
REL (Recommended)
TWA 0.1 ppm (0.7 mg/m3) [skin][1]
IDLH (Immediate danger)
Related compounds
Related ketones;
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Hexafluoroacetone is a chemical compound with the formula CF3-CO-CF3. It is structurally similar to acetone, however its reactivity is markedly different. It comes in the form of a colourless, hygroscopic, nonflammable, highly reactive gas characterized by a musty odour.[2] The most common form of this substance is hexafluoroacetone sesquihydrate (1.5 H2O), which is a geminal diol.

Synthesis and reactions[edit]

(CF3)2CO is prepared in a two step process from perfluoropropene. In the first step KF catalyzes the reaction of the alkene with elemental sulfur to give the 1,3-dithete [(CF3)2CS]2. This species is then oxidized by iodate to give (CF3)2CO.[3]


Hexafluoroacetone is mostly employed in organic synthesis, but it is also the main chemical intermediate used in the production of hexafluoroisopropanol, as well as polymethyl methacrylates and polyesters for textile coating. Hexafluoroacetone can be employed as a solvent for acetal resins, polyamides, polyglycolide, polyacetals, and polyols or as a polymer adhesive. Hexafluoroacetone is used in the synthesis of the sedative drug midaflur.[citation needed]


Hexafluoroacetone is a reactive substance, acting primarily as an electrophile. In water hexafluoroacetone is highly reactive as its equilibrium sharply favors (~106) forming a geminal diol hydrate, unlike the identical unfavorable equilibrium with acetone (10−3).[4] This makes the equilibria of two chemicals differ by a factor of about a billion regarding this addition of water.[4] Hexafluoroacetone-hydrates are acidic and react with most metals to generate hydrogen. Hexafluoroacetone violently reacts in the presence of alkali. Related to its tendency to hydrate, (CF3)2CO adds ammonia to give (CF3)2C(OH)(NH2) which can be dehydrated with phosphoryl chloride to give (CF3)2CNH.[5]


  1. ^ a b c d e f "NIOSH Pocket Guide to Chemical Hazards #0319". National Institute for Occupational Safety and Health (NIOSH). 
  2. ^ CDC - NIOSH Pocket Guide to Chemical Hazards
  3. ^ Van Der Puy, M. ; Anello, L. G. (1990). "Hexafluoroacetone". Org. Synth.  ; Coll. Vol., 7, p. 251 
  4. ^ a b Lemal, David M. (2004). "Perspective on Fluorocarbon Chemistry". The Journal of Organic Chemistry. 69 (1): 1–11. doi:10.1021/jo0302556. PMID 14703372. 
  5. ^ Middleton, W. J.; Carlson, H. D. (1988). "Hexafluoroacetoneimine". Org. Synth.  ; Coll. Vol., 6, p. 664