SF6

Sulfur hexafluoride

Names
IUPAC name Sulfur hexafluoride
Systematic IUPAC name Hexafluoro-λ6-sulfane
Other names Elagas Esaflon Sulfur(VI) fluoride Sulfuric fluoride
Identifiers
CAS Number	2551-62-4 Y
3D model (Jmol)	Interactive image
ChEBI	CHEBI:30496 Y
ChemSpider	16425 Y
ECHA InfoCard	100.018.050
EC Number	219-854-2
Gmelin Reference	2752
KEGG	D05962 N
MeSH	Sulfur+hexafluoride
PubChem	17358
RTECS number	WS4900000
UNII	WS7LR3I1D6 N
UN number	1080
InChI InChI=1S/F6S/c1-7(2,3,4,5)6 Y Key: SFZCNBIFKDRMGX-UHFFFAOYSA-N Y
SMILES FS(F)(F)(F)(F)F
Properties
Chemical formula	SF6
Molar mass	146.06 g/mol
Appearance	Colorless gas
Odor	odorless
Density	6.17 g/L
Melting point	−50.8 °C (−59.4 °F; 222.3 K)
Boiling point	−64 °C; −83 °F; 209 K
Solubility in water	0.003% (25 °C)
Solubility	slightly soluble in water, very soluble in ethanol, hexane, benzene
Vapor pressure	2.9 MPa (at 21.1 °C)
Magnetic susceptibility (χ)	−44.0·10−6 cm3/mol
Structure
Crystal structure	Orthorhombic, oP28
Space group	Oh
Coordination geometry	Orthogonal hexagonal
Molecular shape	Octahedral
Dipole moment	0 D
Thermochemistry
Std molar entropy (So298)	292 J·mol−1·K−1
Std enthalpy of formation (ΔfHo298)	−1209 kJ·mol−1
Pharmacology
ATC code	V08DA05 (WHO)
Hazards
Safety data sheet	External MSDS
S-phrases	S38
NFPA 704	0 1 2
US health exposure limits (NIOSH):
PEL (Permissible)	TWA 1000 ppm (6000 mg/m3)
REL (Recommended)	TWA 1000 ppm (6000 mg/m3)
IDLH (Immediate danger)	N.D.
Related compounds
Related sulfur fluorides	Disulfur decafluoride Sulfur tetrafluoride
Related compounds	Selenium hexafluoride Sulfuryl fluoride Tellurium hexafluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N  (what is YN ?)
Infobox references

Esaflon
Sulfur(VI) fluoride

Sulfur tetrafluoride

Sulfuryl fluoride
Tellurium hexafluoride

Sulfur hexafluoride (SF₆) is an inorganic, colorless, odorless, non-flammable, extremely potent greenhouse gas, which is an excellent electrical insulator.SF
6 has an octahedral geometry, consisting of six fluorine atoms attached to a central sulfur atom. It is a hypervalent molecule. Typical for a nonpolar gas, it is poorly soluble in water but quite soluble in nonpolar organic solvents. It is generally transported as a liquefied compressed gas. It has a density of 6.12 g/L at sea level conditions, considerably higher than the density of air (1.225 g/L).

SF
6 can be prepared from the elements through exposure of S
8 to F
2. This was also the method used by the discoverers Henri Moissan and Paul Lebeau in 1901. Some other sulfur fluorides are cogenerated, but these are removed by heating the mixture to disproportionate any S
2F
10 (which is highly toxic) and then scrubbing the product with NaOH to destroy remaining SF
4.