Sulfur chloride pentafluoride

Sulfur chloride pentafluoride
Skeletal formula of sulfur chloride pentafluoride	Ball-and-stick model of the sulfur chloride pentafluoride molecule
Names
	Other names Pentafluorochlorosulfanyl
Identifiers
CAS Number	13780-57-9 ;
3D model (JSmol)	Interactive image;
ChemSpider	109933 ;
ECHA InfoCard	100.034.014
PubChem CID	123330;
CompTox Dashboard (EPA)	DTXSID60160316 ;
	InChI InChI=1S/ClF5S/c1-7(2,3,4,5)6 Key: GSYNTTDHMKSMFY-UHFFFAOYSA-N ;
	SMILES S(Cl)(F)(F)(F)(F)F;
Properties
Chemical formula	SClF; 5
Molar mass	162.510 g mol−1
Appearance	Colorless gas
Density	6.642 g dm−3
Melting point	−64 °C (−83 °F; 209 K)
Boiling point	−19 °C (−2 °F; 254 K)
Hazards
Main hazards	Toxic
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Sulfur chloride pentafluoride is an inorganic compound with the formula SF
₅Cl. It exists as a colorless gas at room temperature and is highly toxic, like most inorganic compounds containing the pentafluorosulfide (SF₅) functional group.[1] The compound adopts an octahedral geometry with C
_4v symmetry. Sulfur chloride pentafluoride is the only commercially available reagent for adding the SF
₅ group to organic compounds.[2][3]

Reactivity

In contrast to the high reactivity and toxicity of SF
₅Cl, sulfur hexafluoride (SF
₆), is inert and nontoxic despite having a closely related chemical formula. This difference highlights the lability of the S-Cl bond in this molecule.

Under free-radical conditions, SF
₅Cl adds across double bonds. The following reaction involves the reaction of propene:

CH
₃CHCH
₂ + SF
₅Cl → CH₃CH(Cl)CH₂SF₅

The addition reaction is catalyzed by Et
₃B at around -30 °C. SF
₅Br is used similarly.[2]

SF
₅Cl is also a precursor to O(SF₅)₂ and F₂NSF₅ (from tetrafluorohydrazine).

Synthesis

Sulfur chloropentafluoride can be synthesized by several routes, starting from two lower sulfur fluorides, sulfur tetrafluoride and disulfur decafluoride:[1]

SF
₄ + Cl
₂ + CsF → SF
₅Cl + CsCl

ClF + SF
₄ → SF
₅Cl

S
₂F
₁₀ + Cl
₂ → 2 SF
₅Cl

The corresponding SF
₅Br is prepared similarly from in-situ generated bromine monofluoride.[4]

References

Nyman, F., Roberts, H. L., Seaton, T. "Sulfur Chloride Pentafluoride" Inorganic Syntheses, 1966, Volume 8, p. 160. doi:10.1002/9780470132395.ch42
Dolbier, William R.; et al. (2006). "A convenient and efficient method for incorporation of pentafluorosulfanyl (SF₅) substituents into aliphatic compounds". Journal of Fluorine Chemistry. 127 (10): 1302–10. doi:10.1016/j.jfluchem.2006.05.003.
Savoie, Paul R.; Welch, John T. (2015). "Preparation and Utility of Organic Pentafluorosulfanyl-Containing Compounds". Chemical Reviews. 115 (2): 1130–1190. doi:10.1021/cr500336u. PMID 25341449.
Winter, Rolf; Terjeson, Robin J.; Gard, Gary L. (1998). "An Improved and Facile Preparation of SF₅Br". Journal of Fluorine Chemistry. 89: 105–106. doi:10.1016/S0022-1139(98)00094-3.

[Nyman-1] Nyman, F., Roberts, H. L., Seaton, T. "Sulfur Chloride Pentafluoride" Inorganic Syntheses, 1966, Volume 8, p. 160. doi:10.1002/9780470132395.ch42

[multiple-2] Dolbier, William R.; et al. (2006). "A convenient and efficient method for incorporation of pentafluorosulfanyl (SF₅) substituents into aliphatic compounds". Journal of Fluorine Chemistry. 127 (10): 1302–10. doi:10.1016/j.jfluchem.2006.05.003.

[3] Savoie, Paul R.; Welch, John T. (2015). "Preparation and Utility of Organic Pentafluorosulfanyl-Containing Compounds". Chemical Reviews. 115 (2): 1130–1190. doi:10.1021/cr500336u. PMID 25341449.

[4] Winter, Rolf; Terjeson, Robin J.; Gard, Gary L. (1998). "An Improved and Facile Preparation of SF₅Br". Journal of Fluorine Chemistry. 89: 105–106. doi:10.1016/S0022-1139(98)00094-3.