Sulfur hexafluoride

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Sulfur hexafluoride
General
Systematic name	sulfur(VI) fluoride
Other names	sulphur hexafluoride
Molecular formula	SF6
SMILES	FS(F)(F)(F)(F)F
Molar mass	146.06 g/mol
Appearance	colorless, odorless gas
CAS number	[2551-62-4]
Properties
Density and phase	6.164 g/L, gas phase at 1 bar (~5.1 times denser than air) 1.329 kg/L, liquid phase at 25C 2,510kg/M3 or 2.510 kg/L, solid phase at -50.8C
Solubility in water	low
Melting point	-64 °C (209 K) (Sublimes), Decomposes at 500 °C (773 K)
Boiling point	Sublimes at Standard Pressure
Structure
Coordination geometry	octahedral
Dipole moment	0 D
Hazards
MSDS	External MSDS
Main hazards	highly inert, quite safe
NFPA 704
RTECS number	WS4900000
Supplementary data page
Structure and properties	n, εr=1.002, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Related compounds
Related compounds	SF4, CF4
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references

Sulfur hexafluoride is an inorganic compound with the formula SF₆. This species is a gas at standard conditions. SF₆ has an octahedral geometry, consisting of six fluorine atoms attached to a central sulfur atom. It is a colorless, odorless, non-toxic and non-flammable gas. Typical for a nonpolar gas, it is poorly soluble in water but soluble in nonpolar organic solvents. It is generally transported as a liquified compressed gas. It has a density of 6.13 g/L at sea level conditions.

Contents 1 Synthesis and chemistry 2 Notable characteristics 3 Applications 4 Greenhouse gas 5 Physiological effects and precautions 6 References 7 Further reading 8 See also 9 External links

[edit] Synthesis and chemistry

SF₆ can be prepared from the elements, that is exposure of S₈ to F₂. Some other sulfur fluorides are cogenerated, but these are removed by heating the mixture to disproportionate any S₂F₁₀ and then scrubbing the product with NaOH to destroy remaining SF₄.

There is virtually no reaction chemistry for SF₆. It does not react with molten sodium.

Starting from SF₄, one can prepare SF₅Cl, which is structurally related to SF₆. The monochloride is, however, a strong oxidant and readily hydrolyzed to sulfate.

[edit] Notable characteristics

Because the gas has a high density (over five times denser than air), it can be poured into open containers, like beakers and fishtanks. Moreover, light objects (e.g. made out of light wood or aluminium foil) can float on the gas.^[1]

[edit] Applications

SF₆ is used by the electrical industry as a gaseous dielectric medium for high-voltage (1 kV and above) circuit breakers, switchgear, and other electrical equipment, often replacing harmful PCBs. SF₆ 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. Although most of the decomposition products tend to quickly re-form SF₆, arcing or corona can produce disulfur decafluoride (S₂F₁₀), a highly toxic gas, with toxicity similar to phosgene. S₂F₁₀ 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.

SF₆ plasma is also used in the semiconductor industry as an etchant and in the magnesium industry. It has been used successfully as a tracer in oceanography to study diapycnal mixing and air-sea gas exchange. It is also emitted during the aluminium smelting process.

Because SF₆ is relatively slowly absorbed by the bloodstream, it is used to provide a long-term tamponade (plug) of a retinal hole in retinal detachment repair operations.

In a further medical application, SF₆ is employed as a contrast agent for ultrasound imaging. Sulfur hexafluoride microbubbles are administered in solution through injection into a peripheral vein. These microbubbles enhance their visibility of blood vessels, to ultrasound. This application has been utilised to examine the vascularity of tumours amongst other things.

Gaseous SF₆ is still a commonly used tracer gas for use in short-term experiments of ventilation efficiency in buildings and indoor enclosures, and for determining infiltration rates. Several 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 SF₆.

Sulfur hexafluoride was used as a harmless test gas in an experiment at St John's Wood tube station in London, England on 25 March 2007.^[2] 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.

[edit] Greenhouse gas

According to the Intergovernmental Panel on Climate Change, SF₆ is the most potent greenhouse gas that it has evaluated, with a global warming potential of 22,200 times that of CO₂ over a 100 year period (for countries reporting their emissions to the UNFCCC, a GWP of 23,900 for SF₆ is used as it was decreted at the third Conference of the Parties: GWP used in Kyoto protocol).^[3] Its mixing ratio in the atmosphere is lower than that of CO₂ (about 4 parts per trillion ppt in 1990 versus 365 ppm of carbon dioxide),^[4] its contribution to global warming is accordingly low.

[edit] Physiological effects and precautions

Sulfur hexafluoride can affect the sound of a person's voice if it is inhaled in small quantities. When SF₆ is inhaled, the pitch of a person's voice decreases dramatically.

Although inhaling SF₆ can be a novel amusement, the practice can be dangerous because, like all gases other than oxygen, the SF₆ displaces the oxygen needed for breathing (a phenomenon known as asphyxiation). A myth exists that SF₆ is too heavy for the lungs to expel unassisted, and that after inhaling SF₆, it is necessary to bend over completely at the waist to allow the excess gas to "spill" out of the body. In fact, the lungs mix gases very effectively and rapidly, such that SF₆ would be purged from the lungs within a breath or two.^[5] In general, dense, odourless gases in confined areas present the hazard of suffocation.

[edit] References

[edit] Further reading

• (1991) Gaseous Dielectrics VI. Plenum Press. ISBN 0-306-43894-1. 
• Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
• Khalifa, from Maller and Naidu (1981)

[edit] See also

• Tellurium hexafluoride
• hypervalent molecule
• Paschen's Law
• Electric power
• Process for Measuring the Degradation of Sulfur Hexafluoride in High-voltage Systems U.S. Patent 4,633,082 

[edit] External links

• Fluorocarbons and SF6 applications
• National Pollutant Inventory - Fluoride and compounds fact sheet
• High GWP Gases and Climate Change from the U.S. EPA website.
• Links to external chemical sources