Dioxygen difluoride

Structural formula
General
Surname	Dioxygen difluoride
other names	Fluoroperoxide
Molecular formula	O 2 F 2
Brief description	brown gas
External identifiers / databases
CAS number 7783-44-0 PubChem 123257 ChemSpider 109870 Wikidata Q420640
properties
Molar mass	70.0 g mol −1
Physical state	gaseous
density	1.45 g cm −3 (at boiling point) 1.91 g cm −3 (at −165 ° C)
Melting point	−163.5 ° C
boiling point	−57 ° C
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Oxygen difluoride is a chemical compound from the group of fluorides , more precisely the oxygen fluorides .

Extraction and presentation

Oxygen difluoride can be obtained by reacting oxygen and fluorine using an electrical discharge . The first synthesis goes back to Otto Ruff in 1933.

${\displaystyle \mathrm {O_{2}+F_{2}\rightarrow O_{2}F_{2}} }$

properties

Oxygen difluoride is brown as a gas, cherry-red as a liquid and orange-yellow in the solid state. The structure of the solid corresponds to that of hydrogen peroxide .

It is unstable (decomposition from −95 ° C) and a strong oxidizing and fluoridating agent . It oxidizes chlorine to chlorofluoride and chlorotrifluoride , and hydrogen sulfide to sulfur hexafluoride .

use

Oxygen difluoride serves as a fluorinating agent in order to convert neptunium or plutonium compounds at low temperatures to the hexafluorides .

Neptunium dioxide and tetrafluoride are almost completely converted to volatile neptunium hexafluoride by dioxygen difluoride (O ₂ F ₂ ) . This is possible both in gas-solid reactions at moderate temperatures and in liquid anhydrous hydrogen fluoride at −78 ° C:

${\displaystyle \mathrm {NpO_{2}\ +\ 3\ O_{2}F_{2}\ \longrightarrow \ NpF_{6}\ +\ 4\ O_{2}} }$

${\displaystyle \mathrm {NpF_{4}\ +\ O_{2}F_{2}\ \longrightarrow \ NpF_{6}\ +\ O_{2}} }$

Individual evidence

1. ↑ ^{a b c d e f g} G. Brauer; Handbook of preparative inorganic chemistry, F. Enke Verlag 1978, ISBN 978-3-432-26081-5 .
2. ↑ ^{a b} Entry on Oxygen Fluoride. In: Römpp Online . Georg Thieme Verlag, accessed on June 12, 2017.
3. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
4. ↑ Otto Ruff , W. Menzel: "Neue Oxerstofffluoride: O ₂ F ₂ und OF", Journal for inorganic and general chemistry , 1933 , 211  (1–2), pp. 204–208 ( doi : 10.1002 / zaac.19332110122 ) .
5. ^ AJ Bridgeman, J. Rothery: "Bonding in mixed halogen and hydrogen peroxides", Journal of the Chemical Society, Dalton Transactions , 1999 , pp. 4077-4082 ( doi : 10.1039 / a904968a ).
6. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 .
7. ^ Streng AG: The Chemical Properties of Dioxygen Difluoride . In: Journal of the American Chemical Society . 85, No. 10, 1963, pp. 1380-1385. doi : 10.1021 / ja00893a004 .
8. ↑ Ralf Steudel : Chemistry of non-metals ; ISBN 978-3-11-012322-7 .
9. ^ P. Gary Eller, Larned B. Asprey, Scott A. Kinkead, Basil I. Swanson, Richard J. Kissane: "Reactions of Dioxygen Difluoride with Neptunium Oxides and Fluorides", in: Journal of Alloys and Compounds , 1998 , 269  ( 1-2), pp. 63-66 ( doi : 10.1016 / S0925-8388 (98) 00005-X ).

Web links

• Entry to perfluoroperoxides . In: P. J. Linstrom, W. G. Mallard (Eds.): NIST Chemistry WebBook, NIST Standard Reference Database Number 69 . National Institute of Standards and Technology , Gaithersburg MD
• Things I Won't Work With: Dioxygen Difluoride - Blog post (English) by chemist Derek Lowe on the devastating properties of O ₂ F ₂