| Hexafluoroacetone | |
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1,1,1,3,3,3-hexafluoro- |
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Other names
perfluoroacetone |
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| Identifiers | |
| CAS number | 684-16-2 |
| ChemSpider | 13846015 |
| ChEBI | CHEBI:39429 |
| RTECS number | UC2450000 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | C3F6O |
| Molar mass | 166.02 g/mol |
| Appearance | Colorless gas |
| Density | 1.32 g/ml, liquid |
| Melting point |
−129 °C (144 K) |
| Boiling point |
−28 °C (245 K) |
| Solubility in water | Reacts with water |
| Hazards | |
| R-phrases | R14, R23/24/25, R34, R60, R63 |
| S-phrases | S7/9, S26, S28, S36, S45, S53 |
| Main hazards | Toxic (T), Corrosive (C) |
| NFPA 704 |
0
3
2
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| Flash point | N/A |
| Related compounds | |
| Related organofluorides | Hexafluoro-2-propanol |
| (verify) (what is: /?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 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. The most common form of this substance is hexafluoroacetone sesquihydrate (1.5 H2O), which is a gem-diol.
Contents |
(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.[1]
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 a reactive substance, acting primarily as an electrophile. In water hexafluoroacetone is highly reactive as its equilibrium sharply favors (~106) forming a gem-diol hydrate, unlike the identical unfavorable equilibrium with acetone (10-3).[2] This makes the equilibria of two chemicals differ by about a billion regarding this addition of water.[2] 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.[3]