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F r o m W i k i p e d i a , t h e f r e e e n c y c l o p e d i a
( R e d i r e c t e d f r o m F 2 O )
Oxygen difluoride
Names
IUPAC name
Oxygen difluoride
Other names
Identifiers
CAS Number
3D model (JSmol )
ChEBI
ChemSpider
ECHA InfoCard
100.029.087
EC Number
PubChem CID
RTECS number
UNII
CompTox Dashboard (EPA )
InChI=1S/F2O/c1-3-2 Y
Key: UJMWVICAENGCRF-UHFFFAOYSA-N Y
Key: UJMWVICAENGCRF-UHFFFAOYAI
Properties
Chemical formula
OF 2
Molar mass
53.9962 g/mol
Appearance
colorless gas, pale yellow liquid when condensed
Odor
peculiar, foul
Density
1.90 g/cm3 (−224 °C, liquid)
1.719 g/cm3 (−183 °C, liquid)
1.521 g/cm3 (liquid at −145 °C)
1.88 g/L (gas at room temperature)
Melting point
−223.8 °C (−370.8 °F; 49.3 K )
Boiling point
−144.75 °C (−228.55 °F; 128.40 K )
Solubility in water
hydrolyzes[1] slowly
Vapor pressure
48.9 atm (at −58.0 °C or −72.4 °F or 215.2 K [a] )
Thermochemistry
Heat capacity (C )
43.3 J/mol K
Std molar entropy (S ⦵ 298 )
246.98 J/mol K
Std enthalpy of formation (Δf H ⦵ 298 )
−24.5 kJ mol−1
Gibbs free energy (Δf G ⦵ )
42.5 kJ/mol
Hazards
GHS labelling :[4]
Pictograms
Signal word
Danger
Hazard statements
H270 , H280 , H314 , H330
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
LC 50 (median concentration )
1.5 ppm (mouse, 1 hour)
26 ppm (dog, 1 hour)
16 ppm (monkey, 1 hour)
[3]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 0.05 ppm (0.1 mg/m3 )[2]
REL (Recommended)
C 0.05 ppm (0.1 mg/m3 )[2]
IDLH (Immediate danger)
0.5 ppm[2]
Related compounds
Related compounds
O 2 F 2
NHF2
NF 3
SCl2
H 2 O
Cl 2 O
Br 2 O
I 2 O
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound
Oxygen difluoride is a chemical compound with the formula OF 2 . As predicted by VSEPR theory , the molecule adopts a bent molecular geometry . It is a strong oxidizer and has attracted attention in rocketry for this reason.[5] With a boiling point of −144.75 °C, OF2 is the most volatile (isolable) triatomic compound.[6] The compound is one of many known oxygen fluorides .
Preparation [ edit ]
Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and hydrofluoric acid containing small quantities of water .[7] [8] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide , with sodium fluoride as a side-product:
2 F2 + 2 NaOH → OF2 + 2 NaF + H2 O
Structure and bonding [ edit ]
It is a covalently bonded molecule with a bent molecular geometry and a F-O-F bond angle of 103 degrees. Its powerful oxidizing properties are suggested by the oxidation number of +2 for the oxygen atom instead of its normal −2.
Reactions [ edit ]
Above 200 °C, OF 2 decomposes to oxygen and fluorine by a radical mechanism.
2 OF2 → O2 + 2 F2
OF 2 reacts with many metals to yield oxides and fluorides . Nonmetals also react: phosphorus reacts with OF 2 to form PF 5 and POF3 ; sulfur gives SO 2 and SF 4 ; and unusually for a noble gas , xenon reacts (at elevated temperatures) yielding XeF4 and xenon oxyfluorides.
Oxygen difluoride reacts very slowly with water to form hydrofluoric acid :
OF 2 + H2 O → 2 HF + O2
It can oxidize sulphur dioxide to sulfur trioxide and elemental fluorine :
OF 2 + SO2 → SO3 + F2
However, in the presence of UV radiation , the products are sulfuryl fluoride (SO 2 F 2 ) and pyrosulfuryl fluoride (S 2 O 5 F 2 ):
OF 2 + 2 SO2 → S2 O 5 F 2
This section
needs expansion . You can help by
adding to it .
(August 2018 )
Oxygen difluoride is considered an unsafe gas due to its oxidizing properties. It reacts explosively with water.[9] Hydrofluoric acid produced by the hydrolysis of OF 2 with water is highly corrosive and toxic, capable of causing necrosis , leaching calcium from the bones and causing cardiovascular damage, among a host of other highly toxic effects. Other acute poisoning effects include: pulmonary edema , bleeding lungs, headaches, etc. [10] Chronic exposure to oxygen difluoride, like that of other chemicals that release fluoride ions, can lead to fluorosis and other symptoms of chronic fluoride poisoning. Oxygen difluoride may be associated with kidney damage. [10] The maximum workplace exposure limit is 0.05 ppm.[11] [10]
Popular culture [ edit ]
In Robert L. Forward 's science fiction novel Camelot 30K , oxygen difluoride was used as a biochemical solvent by fictional life forms living in the solar system's Kuiper belt . While OF 2 would be a solid at 30 K, the fictional alien lifeforms were described as endothermic , maintaining elevated body temperatures and liquid OF 2 blood by radiothermal heating.
References [ edit ]
^ "difluorine monoxide; oxygen difluoride, physical properties, suppliers, CAS, MSDS, structure, Molecular Formula, Molecular Weight, Solubility, boiling point, melting point" . www.chemyq.com .
^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0475" . National Institute for Occupational Safety and Health (NIOSH).
^ "Oxygen difluoride" . Immediately Dangerous to Life or Health Concentrations (IDLH) . National Institute for Occupational Safety and Health (NIOSH).
^ GHS: GESTIS 570242
^ "Oxygen Difluoride - an overview | ScienceDirect Topics" . www.sciencedirect.com . Retrieved 2023-11-03 .
^ Greenwood, Norman N. ; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann . p. 819. ISBN 978-0-08-037941-8 .
^ Lebeau, P. ; Damiens, A. (1929). "Sur un nouveau mode de préparation du fluorure d'oxygène" [A new method of preparation of oxygen fluoride]. Comptes rendus hebdomadaires des séances de l'Académie des Sciences (in French). 188 : 1253–1255. Retrieved February 21, 2013 .
^ Lebeau, P. ; Damiens, A. (1927). "Sur l'existence d'un composé oxygéné du fluor" [The existence of an oxygen compound of fluorine]. Comptes rendus hebdomadaires des séances de l'Académie des Sciences (in French). 185 : 652–654. Retrieved February 21, 2013 .
^ "OXYGEN DIFLUORIDE | CAMEO Chemicals | NOAA" . cameochemicals.noaa.gov . Retrieved 2024-05-14 .
^ a b c www.kdocs.cn https://www.kdocs.cn/singleSign4CST?cb=https%3A%2F%2Fwww.kdocs.cn%2Fl%2Fcn9j8vXb7Gq3%3Ff%3D201&ts=1715699652 . Retrieved 2024-05-14 .
^ "CDC - NIOSH Pocket Guide to Chemical Hazards - Oxygen difluoride" . www.cdc.gov . Retrieved 2024-05-14 .
External links [ edit ]
t
e
Salts and covalent derivatives of the
fluoride ion
t
e
PF 6 − , AsF6 − , SbF6 − compounds
AlF6 − compounds
chlorides, bromides, iodides and pseudohalogenides
SiF6 2- , GeF6 2- compounds
Oxyfluorides
Organofluorides
with transition metal, lanthanide, actinide, ammonium
nitric acids
bifluorides
thionyl, phosphoryl, and iodosyl
Chemical formulas
R e t r i e v e d f r o m " https://en.wikipedia.org/w/index.php?title=Oxygen_difluoride&oldid=1232931935 "
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