Hypofluorous acid
Revision as of 04:46, 17 September 2010 by Physchim62 (talk | contribs)
| Hypofluorous acid | |
|---|---|
| Identifiers | |
| InChI | InChI=1/FHO/c1-2/h2H |
| InChIKey | AQYSYJUIMQTRMV-UHFFFAOYAN |
| Standard InChI | InChI=1S/FHO/c1-2/h2H |
| Standard InChIKey | AQYSYJUIMQTRMV-UHFFFAOYSA-N |
| CAS number | [] |
| ChemSpider | |
| Properties[1] | |
| Chemical formula | HOF |
| Molar mass | 36.006 g mol−1 |
| Appearance | see text |
| Melting point |
−117 °C |
| Boiling point |
< 0 °C |
| Solubility in water | reacts |
| Structure[1] | |
| Molecular geometry | bent: H–O = 96.4 pm, O–F = 144.2 pm, H–O–F = 97.2° |
| Thermochemistry[2] | |
| Std enthalpy of formation ΔfH |
−98.32 kJ mol−1 |
| Standard molar entropy S |
226.77 J K−1 mol−1 |
| Related compounds | |
| Other compounds | Hypochlorous acid Hypobromous acid]] Hypoiodous acid |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Hypofluorous acid or oxygen fluoride hydride, HOF, is an unstable compound arising from the reaction of gaseous fluorine with water. It was first isolated in weighable quantities in 1971.[3]
Notes and references
Notes
References
- ↑ 1.0 1.1 Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; p 1003. ISBN 0-08-022057-6.
- ↑ Hypofluorous acid. In NIST Chemistry WebBook; National Institute for Standards and Technology, <http://webbook.nist.gov/cgi/inchi/InChI%3DInChI=1S/FHO/c1-2/h2H>. (accessed 17 September 2010).
- ↑ Studier, M. H.; Appleman, E. H. Hypofluorous Acid. J. Am. Chem. Soc. 1971, 93, 2349.
External links
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See also the corresponding article on Wikipedia. |
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