Hypofluorous acid

Source: Wikipedia, the free encyclopedia.
Hypofluorous acid
Hypofluorous acid
Gas-phase structure
Hypofluorous acid
  Hydrogen, H
  Oxygen, O
  Fluorine, F
Names
IUPAC name
Hypofluorous acid
Other names
  • Fluoranol
  • Fluoric(-I) acid
  • Hydrogen hypofluorite
  • Hydrogen fluorate(-I)
  • Hydrogen monofluoroxygenate(0)
  • Hydroxyl fluoride
Identifiers
3D model (
JSmol
)
ChemSpider
  • InChI=1S/FHO/c1-2/h2H ☒N
    Key: AQYSYJUIMQTRMV-UHFFFAOYSA-N ☒N
  • InChI=1/FHO/c1-2/h2H
    Key: AQYSYJUIMQTRMV-UHFFFAOYAN
  • OF
Properties
HOF
Molar mass 36.0057 g/mol
Appearance pale yellow liquid above −117 °C
white solid below −117 °C
Melting point −117 °C (−179 °F; 156 K)
Boiling point decomposes at 0 °C (32 °F; 273 K)[citation needed]
Structure
Cs
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Explosive, strong oxidizer, corrosive
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerinSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
4
0
4
OX
Related compounds
Other cations
 Lithium hypofluorite
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Hypofluorous acid,

oxidation of water by fluorine, which produces hydrogen fluoride, oxygen difluoride, hydrogen peroxide, ozone and oxygen. HOF is explosive at room temperature, forming HF and O2:[1]

2 HOF → 2 HF + O2

This reaction is catalyzed by water.[2]

It was isolated in the pure form by passing F2 gas over ice at −40 °C, rapidly collecting the HOF gas away from the ice, and condensing it:[2]

F2 + H2O → HOF + HF

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°).

Thiophene chemists commonly call a solution of hypofluorous acid in acetonitrile (generated in situ by passing gaseous fluorine through water in acetonitrile) Rozen's reagent.[3]

Hypofluorites

Hypofluorites are formally derivatives of OF−, which is the

trifluoromethyl ester of hypofluorous acid. The conjugate base is known in salts such as lithium hypofluorite
.

See also

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

References

  1. ^
    doi:10.1002/anie.198803921
    .
  2. ^
    ISSN 0001-4842
    .
  3. ^ For Rozen's original popularizations, see: For subsequent use, see, e.g.
Retrieved from "https://en.wikipedia.org/w/index.php?title=Hypofluorous_acid&oldid=1206735760"