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Sulfur hexafluoride


Sulfur hexafluoride

Sulfur hexafluoride
Skeletal formula of sulfur hexafluoride with assorted dimensions
Spacefill model of sulfur hexafluoride
Ball and stick model of sulfur hexafluoride
IUPAC name
Sulfur hexafluoride
Systematic IUPAC name
Other names

Sulfur(VI) fluoride

Sulfuric fluoride
ATC code V08
ChemSpider  Y
EC number 219-854-2
Jmol-3D images Image
RTECS number WS4900000
UN number 1080
Molar mass 146.06 g/mol
Appearance Colorless gas
Odor odorless[2]
Density 6.17 g/L
Boiling point −64 °C; −83 °F; 209 K
0.003% (25 °C)[2]
Solubility slightly soluble in water, very soluble in ethanol, hexane, benzene
Vapor pressure 2.9 MPa (at 21.1 °C)
Orthorhombic, oP28
Orthogonal hexagonal
0 D
292 J·mol−1·K−1[3]
−1209 kJ·mol−1[3]
Safety data sheet External MSDS
S-phrases S38
NFPA 704
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 1000 ppm (6000 mg/m3)[2]
REL (Recommended)
TWA 1000 ppm (6000 mg/m3)[2]
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  (: Y/N?)

Sulfur hexafluoride (SF6) is an flammable, extremely potent greenhouse gas which is an excellent electrical insulator.[4] SF
has an liquefied compressed gas. It has a density of 6.12 g/L at sea level conditions, which is considerably higher than the density of air (1.225 g/L).


  • Synthesis and reactions 1
  • Applications 2
    • Dielectric medium 2.1
    • Medical use 2.2
    • Tracer compound 2.3
    • Other uses 2.4
  • Greenhouse gas 3
  • Physiological effects and precautions 4
  • Other properties 5
  • See also 6
  • References 7
  • Further reading 8
  • External links 9

Synthesis and reactions

can be prepared from the elements through exposure of S
to F
. 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
(which is highly toxic) and then scrubbing the product with NaOH to destroy remaining SF

There is virtually no reaction chemistry for SF
. A main contribution to the inertness of SF6 is the steric hindrance of the sulfur atom, whereas its heavier group 16 counterparts, such as SeF6 are more reactive than SF6 as a result of less steric hindrance (See hydrolysis example).[5] It does not react with molten sodium, but reacts exothermically with lithium.


More than 10,000 tons of SF
are produced per year, most of which (over 8,000 tons) is used as a gaseous dielectric medium in the electrical industry.[6] Other main uses include an inert gas for the casting of magnesium, and as an inert filling for insulated glazing windows.

Dielectric medium

is used in the electrical industry as a gaseous dielectric medium for high-voltage circuit breakers, switchgear, and other electrical equipment, often replacing oil filled circuit breakers (OCBs) that can contain harmful PCBs. SF
gas under pressure is used as an insulator in gas insulated switchgear (GIS) because it has a much higher dielectric strength than air or dry nitrogen. This property makes it possible to significantly reduce the size of electrical gear. This makes GIS more suitable for certain purposes such as indoor placement, as opposed to air-insulated electrical gear, which takes up considerably more room. Gas-insulated electrical gear is also more resistant to the effects of pollution and climate, as well as being more reliable in long-term operation because of its controlled operating environment. Exposure to an arc chemically breaks down SF
though most of the decomposition products tend to quickly re-form SF
, a process termed "self-healing,"[7] Arcing or corona can produce disulfur decafluoride (S
), a highly toxic gas, with toxicity similar to phosgene. S
was considered a potential chemical warfare agent in World War II because it does not produce lacrimation or skin irritation, thus providing little warning of exposure.

is also commonly encountered as a high voltage dielectric in the high voltage supplies of particle accelerators, such as Van de Graaff generators and Pelletrons and high voltage transmission electron microscopes.

Medical use

is used to provide a tamponade or plug of a retinal hole in retinal detachment repair operations[8] in the form of a gas bubble. It is inert in the vitreous chamber[9] and initially doubles its volume in 36 hours before being absorbed in the blood in 10–14 days.[10]

is used as a contrast agent for ultrasound imaging. Sulfur hexafluoride microbubbles are administered in solution through injection into a peripheral vein. These microbubbles enhance the visibility of blood vessels to ultrasound. This application has been used to examine the vascularity of tumours.[11]

Tracer compound

Sulfur hexafluoride was the tracer gas used in the first roadway air dispersion model calibration; this research program was sponsored by the U.S. Environmental Protection Agency and conducted in Sunnyvale, California on U.S. Highway 101.[12] Gaseous SF
is used as a tracer gas in short-term experiments of ventilation efficiency in buildings and indoor enclosures, and for determining infiltration rates. Two major factors recommend its use: its concentration can be measured with satisfactory accuracy at very low concentrations, and the Earth's atmosphere has a negligible concentration of SF

Sulfur hexafluoride was used as a non-toxic test gas in an experiment at St. John's Wood tube station in London, United Kingdom on 25 March 2007.[13] The gas was released throughout the station, and monitored as it drifted around. The purpose of the experiment, which had been announced earlier in March by the Secretary of State for Transport Douglas Alexander, was to investigate how toxic gas might spread throughout London Underground stations and buildings during a terrorist attack.

Sulfur hexafluoride is also routinely used as a tracer gas in laboratory fume hood containment testing. The gas is used in the final stage of ASHRAE 110 fume hood qualification. A plume of gas is generated inside of the fume hood and a battery of tests are performed while a gas analyzer arranged outside of the hood samples for SF6 to verify the containment properties of the fume hood.

It has been used successfully as a tracer in oceanography to study diapycnal mixing and air-sea gas exchange.

Other uses

  • SF
    plasma is also used in the semiconductor industry as an etchant. SF
    breaks down in the plasma into sulfur and fluorine, the fluorine plasma performing the etching.[15]
  • The magnesium industry uses large amounts of SF
    as inert gas to fill casting forms.[16]
  • Pressurizes waveguides in high-power microwave systems. The gas insulates the waveguide, preventing internal arcing.
  • Was used to fill Nike Air bags in all of their shoes from 1992-2006.[18]

Greenhouse gas

Mauna Loa sulfur hexafluoride timeseries.

According to the Intergovernmental Panel on Climate Change, SF
is the most potent greenhouse gas that it has evaluated, with a global warming potential of 23,900[20] times that of CO
when compared over a 100-year period. Measurements of SF6 show that its global average mixing ratio has increased by about 0.2 ppt (parts per trillion) per year to over 7 ppt.[21] Sulfur hexafluoride is also extremely long-lived, is inert in the troposphere and stratosphere and has an estimated atmospheric lifetime of 800–3200 years.[22] SF
is very stable (for countries reporting their emissions to the UNFCCC, a GWP of 23,900 for SF
was suggested at the third Conference of the Parties: GWP used in Kyoto protocol).[23] Average global SF6 concentrations increased by about seven percent per year during the 1980s and 1990s, mostly as the result of its use in the magnesium production industry, and by electrical utilities and electronics manufacturers. Given the low amounts of SF6 released compared to carbon dioxide, its overall contribution to global warming is estimated to be less than 0.2 percent.[24]

In Europe, SF
falls under the F-Gas directive which ban or control its use for several applications. Since 1 January 2006, SF
is banned as a tracer gas and in all applications except high-voltage switchgear.[25] It was reported in 2013 that a three-year effort by the United States Department of Energy to identify and fix leaks at its laboratories in the United States such as the Princeton Plasma Physics Laboratory, where the gas is used as a high voltage insulator, had been productive, cutting annual leaks by 35,000 pounds. This was done by comparing purchases with inventory, assuming the difference was leaked, then locating and fixing the leaks.[4]

Physiological effects and precautions

Like helium, sulfur hexafluoride is a non-toxic gas, yet by displacing oxygen in the lungs, it also carries the risk of asphyxia if too much is inhaled.[26] Being more dense than air, if a substantial quantity of gas is released it will settle in low-lying areas and present a significant risk of asphyxiation if the area is entered. This is particularly relevant to its use as an insulator in electrical equipment where workers may be in trenches or pits below equipment containing SF

As with all gases, the density of SF
affects the resonance frequencies of the vocal tract, thus changing drastically the vocal sound qualities, or timbre, of those who inhale it. It does not affect the vibrations of the vocal folds. The density of sulfur hexafluoride is relatively high at room temperature and pressure due to the gas's large molar mass. Unlike helium, which has a molar mass of about 4 grams/mol and gives the voice a childish and a "chipmunk like" quality, SF
has a molar mass of about 146 g/mol, and the speed of sound through the gas is about 134 m/s at room temperature.[28] For comparison, the molar mass of air, which is about 80% nitrogen and 20% oxygen, is approximately 30 g/mol which leads to a speed of sound of 343 m/s. Inhalation of SF
causes a lowering of the timbre, or frequency of the formants, of the vocal tract, by contrast with inhalation of helium, which raises it.[29]

Sulfur hexafluoride has an anesthetic potency slightly lower than nitrous oxide.[30]

Other properties

  • Thermal conductivity at STP (101.3 kPa and 0 °C) = 12.058 mW/(m·K)[31]
  • Heat capacity at constant pressure (Cp) (101.3 kPa and 21 °C) = 0.097 kJ/(mol·K)
  • Critical temperature: 45.5 °C
  • Critical pressure: 37.59 bar (3.759 MPa)[31]

See also


  1. ^ "Sulfur Hexafluoride - PubChem Public Chemical Database". The PubChem Project. National Center for Biotechnology Information. Retrieved 22 February 2013. 
  2. ^ a b c d e "NIOSH Pocket Guide to Chemical Hazards #0576".  
  3. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23.  
  4. ^ a b Michael Wines (June 13, 2013). "Department of Energy’s Crusade Against Leaks of a Potent Greenhouse Gas Yields Results". The New York Times. Retrieved June 14, 2013. 
  5. ^ Duward Shriver, Peter Atkins (2010). Inorganic Chemistry. W. H. Freeman. p. 409.  
  6. ^ Constantine T. Dervos, Panayota Vassilou (2012). Sulfur Hexafluoride: Global Environmental Effects and Toxic Byproduct Formation. Taylor and Francis. 
  7. ^ Jakob, Fredi; Perjanik, Nicholas. "Sulfur Hexafluoride, A Unique Dielectric" (PDF). Analytical ChemTech International, Inc. 
  8. ^ Daniel A. Brinton, C. P. Wilkinson (2009). Retinal detachment: principles and practice. Oxford University Press. p. 183.  
  9. ^ Gholam A. Peyman, M.D., Stephen A. Meffert, M.D., Mandi D. Conway (2007). Vitreoretinal Surgical Techniques. Informa Healthcare. p. 157.  
  10. ^ Hilton, G. F.; Das, T.; Majji, A. B.; Jalali, S. (1996). "Pneumatic retinopexy: Principles and practice". Indian Journal of Ophthalmology 44 (3): 131–143.  
  11. ^ Lassau N, Chami L, Benatsou B, Peronneau P, Roche A (December 2007). "Dynamic contrast-enhanced ultrasonography (DCE-US) with quantification of tumor perfusion: a new diagnostic tool to evaluate the early effects of antiangiogenic treatment". Eur Radiol 17 (Suppl 6): F89–98.  
  12. ^ C Michael Hogan (September 10, 2011). "Air pollution line source". Encyclopedia of Earth. Retrieved 22 February 2013. 
  13. ^ Poison gas' test on Underground"'". BBC News. 25 March 2007. Retrieved 22 February 2013. 
  14. ^ Hughes, T.G.; Smith, R.B. and Kiely, D.H. (1983). "Stored Chemical Energy Propulsion System for Underwater Applications". Journal of Energy 7 (2): 128–133.  
  15. ^ Y. Tzeng and T.H. Lin (September 1987). Based Plasmas"SF
    "Dry Etching of Silicon Materials in (PDF). Journal of the Electrochemical Society. Retrieved 22 February 2013.
  16. ^ Scott C. Bartos (February 2002). "Update on EPA's manesium industry partnership for climate protection" (PDF).  
  17. ^ Dick Olsher (October 26, 2009). "Advances in loudspeaker technology - A 50 year prospective". The Absolute Sound. Retrieved December 14, 2013. 
  18. ^ Stanley Holmes (September 24, 2006). "Nike Goes For The Green". Bloomberg Business Week Magazine. Retrieved December 14, 2013. 
  19. ^ SPRI: Sulphur hexafluoride
  20. ^ "2.10.2 Direct Global Warming Potentials". Intergovernmental Panel on Climate Change. 2007. Retrieved 22 February 2013. 
  21. ^ Mixing Ratio"6"Chromatograph for Atmospheric Trace Species SF. US National Oceanic and Atmospheric Administration. Retrieved 22 February 2013. 
  22. ^ A. R. Ravishankara, S. Solomon, A. A. Turnipseed, R. F. Warren; Solomon; Turnipseed; Warren (8 January 1993). "Atmospheric Lifetimes of Long-Lived Halogenated Species". Science 259 (5092): 194–199.  
  23. ^ "6.12.2 Direct GWPs". Intergovernmental Panel on Climate Change. 2001. Retrieved 22 February 2013. 
  24. ^ Sulfur Hexafluoride"6"SF. PowerPlantCCS Blog. 19 March 2011. Retrieved 22 February 2013. 
  25. ^ "'"Climate: MEPs give F-gas bill a 'green boost. 13 October 2005. Retrieved 22 February 2013. 
  26. ^ "Sulfur Hexaflouride". Hazardous Substances Data Bank. U.S. National Library of Medicine. Retrieved 26 March 2013. 
  27. ^ "Guide to the safe use of SF6 in gas".  
  28. ^ "Thermophysical Properties of Fluid Systems". NIST. Retrieved 10 January 2014. 
  29. ^ "Physics in Speech". University of New South Wales. Retrieved 22 February 2013. 
  30. ^ Adriani, John (1962). The Chemistry and Physics of Anesthesia. Second Edition. Illinois: Thomas Books. p. 319.  
  31. ^ a b "Sulfur hexafluoride". Air Liquide Gas Encyclopedia. Retrieved 22 February 2013. 

Further reading

  • Christophorou, Loucas G.,  
  • Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  • Khalifa, Mohammad (1990). High-Voltage Engineering: Theory and Practice. New York: Marcel Dekker.  
  • Maller, V. N.; Naidu, M. S. (1981). Advantages in High Voltage Insulation and Arc Interruption in SF6 and Vacuum. Oxford; New York: Pergamon Press.  
  • Reduction Partnership for Electric Power Systems6SF

External links

  • Fluoride and compounds fact sheet— National Pollutant Inventory
  • High GWP Gases and Climate Change from the U.S. EPA website
  • and the Environment6International Conference on SF (related archive)
  • CDC - NIOSH Pocket Guide to Chemical Hazards
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