Sulfur monochloride pentafluoride

Structural formula
General
Surname	Sulfur monochloride pentafluoride
other names	Sulfur chloride pentafluoride Sulfur chloride fluoride Sulfur pentafluorochloride Pentafluorosulfanyl chloride
Molecular formula	ClF 5 S
Brief description	colorless gas
External identifiers / databases
CAS number 13780-57-9 EC number 237-431-0 ECHA InfoCard 100.034.014 PubChem 123330 Wikidata Q2336792
properties
Molar mass	162.51 g mol −1
Physical state	gaseous
density	1.541 g cm −3 (−60 ° C)
Melting point	−64 ° C
boiling point	−17 ° C
solubility	soluble in most organic solvents
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 .

Sulfur monochloride pentafluoride is a chemical compound from the group of fluorides .

Extraction and presentation

Sulfur monochloride pentafluoride can be obtained by reacting sulfur tetrafluoride with chlorine and potassium fluoride or cesium fluoride at 175 ° C.

${\displaystyle \mathrm {SF_{4}+Cl_{2}+CsF\longrightarrow SClF_{5}+CsCl} }$

It is also possible to display it by reacting sulfur tetrafluoride with chlorofluoride at 380 ° C.

${\displaystyle \mathrm {SF_{4}+ClF\longrightarrow SClF_{5}} }$

Since cesium fluoride acts as a catalyst , the former reaction can be carried out at lower temperatures.

properties

Sulfur monochloride pentafluoride is a colorless gas and a strong oxidizing agent . It is much more reactive than sulfur hexafluoride because the S-Cl bond is weaker than the SF bonds. It therefore reacts on the one hand according to radical reaction mechanisms and on the other hand is much more easily hydrolyzed than sulfur hexafluoride.

When heated to over 400 ° C or under UV light, it decomposes via SF ₅ radicals to form sulfur tetrafluoride and sulfur hexafluoride.

${\displaystyle \mathrm {2\ ClF_{5}S\longrightarrow SF_{4}+SF_{6}+Cl_{2}} }$

Sulfur monochloride pentafluoride reacts with hydrogen and irradiation to form the extremely poisonous disulfur decafluoride .

${\displaystyle \mathrm {2\ SClF_{5}+H_{2}\longrightarrow F_{5}S-SF_{5}+2\ HCl} }$

use

Sulfur monochloride pentafluoride can be used to introduce SF ₅ groups.

${\displaystyle \mathrm {SClF_{5}+C_{2}F_{4}\longrightarrow F_{5}SC_{2}F_{4}Cl} }$

${\displaystyle \mathrm {2\ SClF_{5}+O_{2}\longrightarrow F_{5}SO_{2}SF_{5}+Cl_{2}} }$

In preparative chemistry, it is also used to represent organic components with carbon-sulfur double and triple bonds.

Individual evidence

1. ↑ ^{a b c d e f} Georg Brauer , with the assistance of Marianne Baudler u. a. (Ed.): Handbook of Preparative Inorganic Chemistry . 3rd, revised edition. tape I . Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , pp. 186 .
2. ^ ^{A b} Leo A. Paquette: Handbook of Reagents for Organic Synthesis, Sulfur-Containing Reagents . John Wiley & Sons, 2013, ISBN 978-1-118-63483-7 , pp. 426 ( limited preview in Google Book search).
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 d e} Ralf Steudel : Chemistry of non-metals: From structure and bond to application . Walter de Gruyter, 2008, ISBN 3-11-021128-9 , p. 565 ( limited preview in Google Book search).
5. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 475.
6. ↑ Konrad Seppelt: Sulfur / carbon double and triple bonds (PDF; 77 kB), in: Pure Appl. Chem. , 1987, Vol. 59, No. 8, pp. 1057-1062.