Tellurium hexafluoride

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Tellurium hexafluoride
Structure and dimensions of the molecule
Ball-and-stick model of the molelcule
Identifiers
7783-80-4 YesY
EC number 232-027-0
Jmol-3D images Image
PubChem 24559
Properties
TeF6
Molar mass 241.590 g/mol
Appearance colorless gas
Odor repulsive odor
Density 0.0106 g/cm³ (-10 °C)
4.006 g/cm3 (-191 °C)
Melting point −38.9 °C (−38.0 °F; 234.2 K)[1]
Boiling point −37.6 °C (−35.7 °F; 235.6 K)[1]
decomposes
Vapor pressure >1 atm (20°C)[2]
1.0009
Structure
Crystal structure Orthorhombic, oP28
Space group Pnma, No. 62
octahedral (Oh)
Dipole moment 0
Thermochemistry
117.6 J/(mol K)
-1318 kJ/mol
Hazards
US health exposure limits (NIOSH):
TWA 0.02 ppm (0.2 mg/m3)[2]
TWA 0.02 ppm (0.2 mg/m3)[2]
1 ppm[2]
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Tellurium hexafluoride is a chemical compound of tellurium and fluorine with the chemical formula TeF6. It is a colorless, highly toxic gas with an extremely unpleasant smell.

Preparation[edit]

Tellurium hexafluoride is most commonly prepared by passing fluorine gas over tellurium at 150 °C. Below this temperature a mixture of lower fluorides form, including tellurium tetrafluoride and ditellurium decafluoride. It can also be prepared by passing fluorine gas over TeO3 or indirectly by reacting TeO2 with SeF4 to produce TeF4 and then heating TeF4 in excess of 200 °C to make TeF6 and Te.

Properties[edit]

Tellurium hexafluoride is a highly symmetric octahedral molecule. Its physical properties resemble the sulfur and selenium analogs. It is less volatile, however, due to the increase in molecular weight. At temperatures below −38 °C, tellurium hexafluoride condenses to a volatile white solid.

Ball-and-stick model of the crystal structure Space-filling model of the crystal structure

Reactivity[edit]

Unlike the sulfur analog, tellurium hexafluoride is not chemically inert. This can be attributed to the larger atomic radius which can co-ordinate a maximum of eight atoms rather than six for sulfur and selenium which allows for nucleophilic attack. TeF6 is hydrolyzed in water to Te(OH)6 and reacts with Te below 200 °C.

References[edit]

  1. ^ a b CRC Handbook of Chemistry and Physics, 90. Auflage, CRC Press, Boca Raton, Florida, 2009, ISBN 978-1-4200-9084-0, Section 4, Physical Constants of Inorganic Compounds, p. 4-95.
  2. ^ a b c d "NIOSH Pocket Guide to Chemical Hazards #0588". National Institute for Occupational Safety and Health (NIOSH). 

Literature[edit]

  • W.C. Cooper; Tellurium, Van Nostrand Reinhold Company, New York, USA, 1971.
  • K.W. Bagnall; The Chemistry of Selenium, Tellurium and Polonium, Elsevier Publishing, New York, 1966.
  • R.T. Sanderson; Chemical Periodicity, Reinhold, New York, USA, 1960.
  • N.N. Greenwood and A. Earnshaw; Chemistry of the Elements, 2nd edition, Butterworth, UK, 1997.
  • F.A. Cotton, G. Wilkinson, C.A. Murillo, and M. Bochmann; Advanced Inorganic Chemistry, John Wiley & Sons, 1999.
  • G.J. Hathaway, N.H. Proctor; Chemical Hazards of the Workplace, 5th edition, Wiley-Interscience, New Jersey, 2004.

External links[edit]