Difference between revisions of "Hypofluorous acid"
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| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| − | | Reference = <ref | + | | Reference = <ref>{{citation | journal = J. Chem. Phys. | volume = 56 | issue = 1 | pages = 1–3 | year = 1972 | doi = 10.1063/1.1676830 | title = Millimeter‐Wave Spectrum and Structure of Hypofluorous Acid: HOF and DOF | first1 = Hyunyong | last1 = Kim | first2 = Edwin F. | last2 = Pearson | first3 = Evan H. | last3 = Appelman}}.</ref> |
| − | | MolShape = bent: H–O = 96.4 pm, O–F = 144.2 pm, H–O–F = 97. | + | | MolShape = bent: H–O = 96.4(10) pm, O–F = 144.2(1) pm, H–O–F = 97.2(6)° |
| SpaceGroup = | | SpaceGroup = | ||
| Coordination = | | Coordination = | ||
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}} | }} | ||
| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
| − | | OtherCpds = [[Hypochlorous acid]]<br/>[[ | + | | OtherCpds = [[Hypochlorous acid]]<br/>[[Hypobromous acid]]<br/>[[Hypoiodous acid]] |
}} | }} | ||
}} | }} | ||
| − | '''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.<ref>{{citation | last1 = Studier | first1 = | + | '''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.<ref>{{citation | last1 = Studier | first1 = Martin H. | last2 = Appleman | first2 = Evan H. | title = Hypofluorous Acid | journal = J. Am. Chem. Soc. | year = 1971 | volume = 93 | issue = 9 | pages = 2349–51 | doi = 10.1021/ja00738a059}}.</ref> |
==Notes and references== | ==Notes and references== | ||
Revision as of 04:55, 17 September 2010
| 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[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 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.[4]
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).
- ↑ Studier, Martin H.; Appleman, Evan H. Hypofluorous Acid. J. Am. Chem. Soc. 1971, 93 (9), 2349–51. DOI: 10.1021/ja00738a059.
External links
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See also the corresponding article on Wikipedia. |
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