Platinum (V) fluoride

Crystal structure
__  Pt 5+      __  F -
General
Surname	Platinum (V) fluoride
other names	Platinum pentafluoride
Ratio formula	PtF 5
Brief description	deep red powder
External identifiers / databases
CAS number 13782-84-8 Wikidata Q4493223
properties
Molar mass	290.08 g mol −1
Physical state	firmly
Melting point	80 ° C
solubility	reacts violently with water soluble in bromine trifluoride
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 .

Platinum (V) fluoride is a chemical compound of the elements platinum and fluorine . It was first synthesized by Neil Bartlett in 1960 .

Extraction and presentation

Platinum (V) fluoride can be obtained from the elements:

${\displaystyle \mathrm {2\ Pt+5\ F_{2}\longrightarrow 2\ PtF_{5}} }$

In red heat, platinum and fluorine react at a molar ratio of 2: 5 to form platinum (V) fluoride.

It can also be produced by reacting platinum (II) chloride with fluorine at 350 ° C.

${\displaystyle \mathrm {2\ PtCl_{2}+5\ F_{2}\longrightarrow 2\ PtF_{5}+2\ Cl_{2}} }$

properties

Platinum (V) fluoride is a deep red salt that melts at 80 ° C and breaks down into platinum (IV) fluoride and platinum (VI) fluoride from 130 ° C.

${\displaystyle \mathrm {2\ PtF_{5}\longrightarrow PtF_{4}+PtF_{6}} }$

It crystallizes in the monoclinic crystal system in the space group P 2 ₁ / c (space group no. 14) with the lattice parameters a  = 552  pm ; b  = 994 pm; c  = 1243 pm and β  = 99.98 ° as well as 4 formula units per unit cell .

Platinum (V) fluoride is one of the most powerful oxidizing agents around. For example, it oxidizes water to oxygen :

${\displaystyle \mathrm {4\ PtF_{5}+10\ H_{2}O\longrightarrow 4\ Pt+20\ HF+5\ O_{2}} }$

With xenon difluoride as a strong fluoride donor, various ionic compounds are formed in a fluoride transfer reaction, depending on the mixing ratio.

${\displaystyle \mathrm {2\,XeF_{2}+PtF_{5}\rightarrow [Xe_{2}F_{3}][PtF_{6}]} }$

${\displaystyle \mathrm {XeF_{2}+PtF_{5}\rightarrow [XeF][PtF_{6}]} }$

${\displaystyle \mathrm {XeF_{2}+2\,PtF_{5}\rightarrow [XeF]Pt_{2}F_{11}]} }$

Individual evidence

1. ↑ ^{a b c} platinum (V) fluoride at webelements.com .
2. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , p. 1728.
3. ↑ ^{a b c} Georg Brauer (ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 278.
4. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
5. ^ N. Bartlett, DH Lohmann: Two new fluorides of platinum . In: Proceedings of the Chemical Society. 1960, pp. 14-15; doi : 10.1039 / PS9600000001 .
6. ^ BG Mueller, M. Serafin: Single-crystal investigations on platinum tetrafluoride and pentafluoride. In: European Journal of Solid State and Inorganic Chemistry . 1992, 29, 4-5, pp. 625-633.
7. ↑ Ralf Steudel : Chemistry of Nonmetals, Syntheses - Structures - Bonding - Use , 4th Edition, 2014 Walter de Gruyter GmbH & Co. KG, Berlin / Boston, ISBN 978-3-11-030439-8 , p. 570, ( accessed via De Gruyter Online).