Hypofluorous acid
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| Hypofluorous acid | |
|---|---|
| IUPAC name | fluoranol |
| Other names | oxygen fluoride hydride |
| 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[2] | |
| Molecular geometry | bent: H–O = 96.4(10) pm, O–F = 144.2(1) pm, H–O–F = 97.2(6)° |
| Thermochemistry[3] | |
| 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, HOF, is an unstable compound arising from the reaction of gaseous fluorine with water. It was first isolated in weighable quantities in 1971.[4] Despite the name, formed by analogy with other halogen compounds of similar formula, HOF is not significantly acidic, and hypofluorite salts are unknown.
Preparation
Reported preparations of hypofluorous acid in the 1930s[5][6] are now considered erroneous.[4] The first clear observation of HOF was through the infrared spectrum of a matrix isolation sample, obtained by photolysis of a mixture of fluorine and water in a nitrogen matrix at 14–20 K.[7]
Notes and references
Notes
References
- ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; p 1003. ISBN 0-08-022057-6.
- ↑ Kim, Hyunyong; Pearson, Edwin F.; Appelman, Evan H. Millimeter‐Wave Spectrum and Structure of Hypofluorous Acid: HOF and DOF. J. Chem. Phys. 1972, 56 (1), 1–3. DOI: 10.1063/1.1676830.
- ↑ 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).
- ↑ 4.0 4.1 Studier, Martin H.; Appleman, Evan H. Hypofluorous Acid. J. Am. Chem. Soc. 1971, 93 (9), 2349–51. DOI: 10.1021/ja00738a059.
- ↑ Dennis, L. M.; Rochow, E. G. Oxyacids of Fluorine. J. Am. Chem. Soc. 1932, 54 (2), 832–33. DOI: 10.1021/ja01341a518.
- ↑ Dennis, L. M.; Rochow, E. G. Oxyacids of Fluorine. II. J. Am. Chem. Soc. 1933, 55 (6), 2431–34. DOI: 10.1021/ja01333a033.
- ↑ Noble, Paul N.; Pimentel, George C. Hypofluorous acid: Infrared spectrum and vibrational potential function. Spectrochim. Acta Part A 1968, 24 (7), 797–806. DOI: 10.1016/0584-8539(68)80177-1.
External links
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See also the corresponding article on Wikipedia. |
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