Oxygen difluoride
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Oxygen difluoride is a chemical compound with the formula Template:Chem2. As predicted by VSEPR theory, the molecule adopts a bent molecular geometry.Template:Fact It is a strong oxidizer and has attracted attention in rocketry for this reason.[2] With a boiling point of −144.75 °C, OF2 is the most volatile (isolable) triatomic compound.[3] The compound is one of many known oxygen fluorides.
Preparation
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.[4][5] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide, with sodium fluoride as a side-product:
Structure and bonding
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
Above 200 °C, Template:Chem2 decomposes to oxygen and fluorine by a radical mechanism.
Template:Chem2 reacts with many metals to yield oxides and fluorides. Nonmetals also react: phosphorus reacts with Template:Chem2 to form [[Phosphorus pentafluoride|Template:Chem2]] and Template:Chem2; sulfur gives [[sulfur dioxide|Template:Chem2]] and [[sulfur tetrafluoride|Template:Chem2]]; and unusually for a noble gas, xenon reacts (at elevated temperatures) yielding [[Xenon tetrafluoride|Template:Chem2]] and xenon oxyfluorides.
Oxygen difluoride reacts with water to form hydrofluoric acid:
It can oxidize sulfur dioxide to sulfur trioxide and elemental fluorine:
However, in the presence of UV radiation, the products are sulfuryl fluoride (Template:Chem2) and pyrosulfuryl fluoride (Template:Chem2):
Safety
Script error: No such module "Unsubst". Oxygen difluoride is considered an unsafe gas due to its oxidizing properties. It reacts explosively with water.[6] Hydrofluoric acid produced by the hydrolysis of Template:Chem2 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.[7] 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.[7] The maximum workplace exposure limit is 0.05 ppm.[8][7]
Popular culture
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 Template:Chem2 would be a solid at 30Script error: No such module "String".K, the fictional alien lifeforms were described as endothermic, maintaining elevated body temperatures and liquid Template:Chem2 blood by radiothermal heating.
Notes
References
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External links
- National Pollutant Inventory - Fluoride and compounds fact sheet
- WebBook page for Template:Chem2
- CDC - NIOSH Pocket Guide to Chemical Hazards
Template:Fluorides Template:Oxygen compounds Template:Fluorine compounds