Oxygen difluoride 1692055 203843838 2008-04-06T21:53:47Z 84.13.138.5 {{Chembox new | Name = Oxygen difluoride | ImageFile = Oxygen-difluoride-2D.png | ImageSize = 160px | ImageName = Structure and dimensions of the oxygen difluoride molecule | ImageFile1 = Oxygen-difluoride-3D-vdW.png | ImageSize1 = 160px | ImageName1 = Space-filling model of the oxygen difluoride molecule | OtherNames = difluorine monoxide<br />fluorine monoxide<br />oxygen difluoride<br />oxygen fluoride<br />hypofluorous anhydride | Section1 = {{Chembox Identifiers | CASOther = [7783-41-7] }} | Section2 = {{Chembox Properties | Formula = OF<sub>2</sub> | MolarMass = 53.9962 g mol<sup>−1</sup> | Solvent = other solvents | SolubleOther = 68 mL gaseous OF<sub>2</sub> in 1 L (0 °C)<ref>Yost, D. M. "Oxygen Fluoride" Inorganic Syntheses, 1939 volume, 1, pages 109-111.</ref> | MeltingPt = −224 °C | BoilingPt = −145 °C }} | Section4 = {{Chembox Thermochemistry | DeltaHf = 24.5 kJ mol<sup>−1</sup> }} | Section8 = {{Chembox Related | OtherCpds = [[Dioxygen difluoride|O<sub>2</sub>F<sub>2</sub>]]<br />[[difluoramine|NHF<sub>2</sub>]]<br />[[Nitrogen trifluoride|NF<sub>3</sub>]]<br />[[Sulfur dichloride|SCl<sub>2</sub>]]}} }} '''Oxygen difluoride''' is the [[chemical compound]] with the [[chemical formula|formula]] OF<sub>2</sub>. As predicted by [[VSEPR theory]], the molecule adopts a bent structure like [[water|H<sub>2</sub>O]], but it has very different properties, being a strong [[oxidizer|oxidant]]. ==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 (molecule)|water]].<ref>[[Paul Lebeau]]; Damiens, A. "A New Method for the Preparation of the Fluorine Oxide”<!--would be nice to get original titles in French-->Compt. rend. 1929, volume 188, 1253-5.</ref><ref>Lebeau, P.; Damiens, A. "The Existence of an Oxygen Compound of Fluorine"<!--would be nice to get original titles in French-->Compt. rend. 1927, volume 185, pages 652-4.</ref> The modern preparation entails the reaction of [[fluorine]] with a dilute aqueous solution of [[sodium hydroxide]]: :2F<sub>2</sub> + 2NaOH → OF<sub>2</sub> + [[Sodium fluoride|2NaF]] + H<sub>2</sub>O ==Reactions== Its powerful oxidizing properties are suggested by the [[oxidation number]] of +2 for the [[oxygen]] atom, which is unusual. Above 200 °C, OF<sub>2</sub> decomposes to oxygen and fluorine via a [[Radical (chemistry)|radical]] mechanism. OF<sub>2</sub> reacts with many metals to yield [[oxide]]s and [[fluoride]]s. [[Nonmetal]]s also react: [[phosphorus]] reacts with OF<sub>2</sub> to form [[Phosphorus pentafluoride | PF<sub>5</sub>]] and POF<sub>3</sub>; [[sulfur]] gives [[sulfur dioxide|SO<sub>2</sub>]] and [[sulfur tetrafluoride|SF<sub>4</sub>]]; and unusually for a [[noble gas]], [[xenon]] reacts, yielding [[Xenon tetrafluoride|XeF<sub>4</sub>]] and xenon oxyfluorides. Oxygen difluoride reacts very slowly with water to form [[hydrofluoric acid]]: :OF<sub>2</sub>(aq) + H<sub>2</sub>O(aq) → 2HF(aq) + O<sub>2</sub>(g) ==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]]. ==Safety== OF<sub>2</sub> is a dangerous chemical, as is the case for any strongly oxidizing gas. == References == {{Reflist}} ==External links== * [http://www.npi.gov.au/database/substance-info/profiles/44.html National Pollutant Inventory - Fluoride and compounds fact sheet] * [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7783417 WebBook page for OF<sub>2</sub>] [[Category:Oxygen compounds]] [[Category:Fluorides]] [[Category:Nonmetal halides]] [[Category:Rocket oxidizers]] [[bg:Кислороден дифлуорид]] [[cs:Difluorid kyslíku]] [[de:Sauerstoffdifluorid]] [[pl:Difluorek tlenu]] [[ru:Фторид кислорода(II)]] [[zh:二氟化氧]]