Platinum (VI) fluoride

Structural formula
General
Surname	Platinum (VI) fluoride
other names	Platinum hexafluoride
Molecular formula	PtF 6
Brief description	dark red crystalline solid
External identifiers / databases
CAS number 13693-05-5 EC number 237-214-0 ECHA InfoCard 100,033,816 PubChem 3014771 Wikidata Q417309
properties
Molar mass	309.07 g mol −1
Physical state	firmly
density	5.21 g cm −3 (−140 ° C)
Melting point	61.3 ° C
boiling point	69.1 ° C
solubility	reacts violently with water
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 (VI) fluoride or platinum hexafluoride (PtF ₆ ) is a chemical compound of the elements platinum and fluorine . It is an extremely powerful oxidizing agent that is able to oxidize molecular oxygen or xenon . In doing so, platinum (VI) itself is reduced to platinum (V).

history

It played an important role in the chemistry of noble gases in the 1960s, as PtF _{6 was the} first to produce a noble gas compound . In 1962 , the American chemist Neil Bartlett succeeded in using PtF ₆ to oxidize the dioxygen molecule O ₂ :

${\displaystyle \mathrm {PtF_{6}+O_{2}\longrightarrow O_{2}^{+}(PtF_{6}^{-})} }$

He found that the first ionization energy of O ₂ is similar to that of xenon and that the dioxygenyl cation (O ₂ ) ^{+ is} roughly the same size as the Xe ⁺ ion. This is how he came to the conclusion that Xe must also be oxidized:

${\displaystyle \mathrm {PtF_{6}+Xe\longrightarrow Xe^{+}(PtF_{6}^{-})} }$

The first noble gas compound was synthesized and the assumption that noble gases did not form compounds was refuted.

presentation

• Reaction of platinum with F ₂ at 300 ° C in a brass apparatus:

${\displaystyle \mathrm {Pt+3\ F_{2}\longrightarrow PtF_{6}} }$

• Disproportionation of PtF ₅ from 130 ° C:

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

properties

Platinum hexafluoride is a dark red crystalline solid that melts at 61.3 ° C and boils at 69.1 ° C. Its gas is brown-red and thermally stable up to 200 ° C. It crystallizes in the orthorhombic crystal system (measured at −140 ° C) in the space group Pnma (space group no. 62) with the lattice parameters a  = 937.4  pm , b  = 852.7 pm and c  = 493.3 pm and four formula units per unit cell with a calculated density of 5.21 g · cm ⁻³ .

Individual evidence

1. ↑ ^{a b c d} David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-81.
2. ^ ^{A b} T. Drews, J. Supeł, A. Hagenbach, K. Seppelt: "Solid State Molecular Structures of Transition Metal Hexafluorides", in: Inorganic Chemistry , 2006 , 45  (9), pp. 3782-3788; doi : 10.1021 / ic052029f ; PMID 16634614 .
3. ^ 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.
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. ↑ ^{a b} Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 .
6. ↑ Georg Brauer , with the collaboration of Marianne Baudler a . a. (Ed.): Handbook of Preparative Inorganic Chemistry . 3rd, revised edition. tape I . Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , pp. 278 .

literature

• Janiak, Klapötke , Meyer: Moderne Anorganische Chemie , de Gruyter, Berlin New York 1999, pp. 40–41.
• B. Weinstock, HH Claassen, JG Malm: Platinum Hexafluoride. In: Journal of the American Chemical Society , 1957 , 79 , pp. 5832-5832; doi : 10.1021 / ja01578a073 .