Hypofluorous acid

From Wikipedia, the free encyclopedia
Hypofluorous acid

Gas-phase structure
IUPAC name

Hypofluorous acid

Other names

Hydrogen hypofluorite
Hydrogen fluorate(I)
Fluoric(-I) acid
Hydrogen monofluoroxygenate(0)

Identifiers
CAS number 14034-79-8 YesY
PubChem 123334
ChemSpider 109936 N
Jmol-3D images Image 1
Properties
Molecular formula HOF
Molar mass 36.0057 g mol−1
Appearance pale yellow liquid above −117 °C
white solid below −117 °C
Melting point −117 °C; −179 °F; 156 K
Boiling point < 0 °C
decomposes at 0 °C
Related compounds
Other cations lithium hypofluorite, LiOF
Related compounds hypochlorous acid, HOCl
 N (verify) (what is: YesY/N?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Hypofluorous acid is the chemical compound with the formula HOF. It is an intermediate in the oxidation of water by fluorine, which produces hydrogen fluoride and oxygen. It is the only hypohalous acid that can be isolated as a solid. HOF is explosive, decomposing to oxygen and HF.[1] It was isolated in the pure form by fluorination of ice.

The compound has been characterized in the solid phase by X-ray crystallography[1] as a bent molecule with an angle of 101°. The O–F and O-H bond lengths are 144.2 and 96.4 picometres, respectively. The solid framework consists of chains with O–H---O linkages. The structure has also been analyzed in the gas phase, a state in which the H—O—F bond angle is slightly narrower (97.2°).

For fluorine, the only known oxoacid is hypofluorous acid, HOF. It can be made by passing F2 gas over ice at -40 °C, collecting the HOF gas, and condensing it:

F2 + H2O → HOF + HF

It decomposes explosively at room temperature to form HF and O2:

2 HOF → 2 HF + O2

Hypofluorous acid in acetonitrile (generated in situ by passing gaseous fluorine through "wet" acetonitrile) serves as a highly electrophilic oxygen-transfer agent.[2][3] Treating phenanthroline with this reagent yielded the previously elusive 1,10-phenanthroline dioxide,[4] more than 50 years after the first unsuccessful attempt.[5]

Hypofluorites

Hypofluorites are derivatives of OF−, which is the conjugate base of hypofluorous acid. One example is trifluoromethyl hypofluorite (CF3OF).

See also

  • Hypochlorous acid, a related compound that is more technologically important but has not been obtained in pure form.

References

  1. ↑ 1.0 1.1 W. Poll, G. Pawelke, D. Mootz, E. H. Appelman (1988). "The Crystal Structure of Hypofluorous Acid : Chain Formation by O-H · · · O Hydrogen Bonds". Angew. Chem. Int. Ed. Engl. 27 (3): 392–3. doi:10.1002/anie.198803921. 
  2. ↑ S. Rozen, M. Brand (1986). "Epoxidation of Olefins with Elemental Fluorine in Water/Acetonitrile Mixtures". Angew. Chem. Int. Ed. 25 (6): 554–5. doi:10.1002/anie.198605541. 
  3. ↑ S. Dayan, Y. Bareket, S. Rozen (1999). "An efficient α-hydroxylation of carbonyls using the HOF·CH3CN complex". Tetrahedron 55 (12): 3657. doi:10.1016/S0040-4020(98)01173-9. 
  4. ↑ S. Rozen, S. Dayan (1999). "At Last, 1,10-Phenanthroline-N,N'-dioxide, A New Type of Helicene, has been Synthesized using HOF·CH3CN". Angew. Chem. Int. Ed. 38 (23): 3471–3. doi:10.1002/(SICI)1521-3773(19991203)38:23<3471::AID-ANIE3471>3.0.CO;2-O. 
  5. ↑ F. Linsker, R.L. Evans (1946). "Phenanthroline Di-N-oxides". J. Am. Chem. Soc. 68 (3): 403. doi:10.1021/ja01207a019. 
This article is issued from Wikipedia. The text is available under the Creative Commons Attribution/Share Alike; additional terms may apply for the media files.