Tetrasoxy fluoride

Structural formula
General
Surname	Tetrasoxy fluoride
other names	Difluorotetraoxide
Molecular formula	O 4 F 2
Brief description	red-brown solid (T <−191 ° C)
External identifiers / databases
CAS number 107782-11-6 Wikidata Q30301206
properties
Molar mass	102.00 g mol −1
Melting point	−191 ° 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 .

Tetrasoxygen difluoride is an inorganic chemical compound of oxygen from the group of oxygen fluorides . It consists of two O ₂ F molecule halves linked by a weak OO bond . It is the dimer of the O ₂ F radical.

Extraction and presentation

Tetrasoxygen difluoride can be obtained in two steps. In the first step, photochemically generated fluorine atoms are made to react with oxygen to generate dioxygen monofluoride radicals:

${\displaystyle \mathrm {2\ O_{2}+2\ F^{\cdot }\longrightarrow 2\ [O_{2}F]^{\cdot }} }$

Which then dimerize to tetrasoxygen difluoride in an equilibrium reaction, this happens at temperatures below −175 ° C:

${\displaystyle \mathrm {2\ [O_{2}F]^{\cdot }\rightleftharpoons O_{4}F_{2}} }$

At the same time, the dioxygen monofluoride radicals decompose to form dioxygen difluoride and oxygen , which shifts the above equilibrium autonomously to the left:

${\displaystyle \mathrm {2\ [O_{2}F]^{\cdot }\longrightarrow O_{2}+O_{2}F_{2}} }$

properties

As a solid, tetra- oxygen difluoride is dark red-brown and has a melting point of −191 ° C.

It is a strong fluorinating and oxidizing agent, even stronger than dioxygen difluoride . B. to oxidize Ag (II) to Ag (III), or Au (III) to Au (V). This process produces the corresponding fluoride anions or . With less noble substances, the oxidation leads to an explosion even at the lowest temperatures. B. is elemental sulfur even at -180 ° C explosively in sulfur hexafluoride transferred. ${\displaystyle {\ce {AgF4-}}}$ ${\displaystyle {\ce {AuF6-}}}$

Tetrasoxygen difluoride tends to react similarly to or to react with fluoride ion acceptors such as boron trifluoride ( ) to form salts with the oxygenyl ion ( ). In the case of , this leads to the formation of according to the formula: ${\displaystyle {\ce {[O2F]^{\cdot }}}}$ ${\displaystyle {\ce {O2F2}}}$ ${\displaystyle {\ce {BF3}}}$ ${\displaystyle {\ce {O2+}}}$ ${\displaystyle {\ce {BF3}}}$ ${\displaystyle {\ce {O2+BF4-}}}$

${\displaystyle {\ce {O_4F_2 + 2BF_3 -> 2O_2+BF_4^-}}}$

This behavior is also evident with arsenic pentafluoride , here it leads to . ${\displaystyle {\ce {O2+AsF6-}}}$

Individual evidence

1. ↑ ^{a b c d e f g h i j k} Basics and main group elements: Volume 1: Basics and main group elements , Walter de Gruyter GmbH & Co KG limited preview in the Google book search
2. ↑ 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. ↑ ^{a b c} Basics and main group elements: Volume 1: Basics and main group elements , Walter de Gruyter GmbH & Co KG limited preview in the Google book search