Tellurium hexafluoride

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

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

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.

Reactivity

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

1 2 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.
1 2 3 4 "NIOSH Pocket Guide to Chemical Hazards #0588". National Institute for Occupational Safety and Health (NIOSH).
↑ "Tellurium hexafluoride (as Te)". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).

Literature

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

Binary hexafluorides

Known binary hexafluorides

Chalcogen binary hexafluorides	SF₆ SeF₆ TeF₆ PoF₆

Noble gas binary hexafluorides	XeF₆

Transition metal binary hexafluorides	MoF₆ TcF₆ RuF₆ RhF₆ WF₆ ReF₆ OsF₆ IrF₆ PtF₆

Actinide binary hexafluorides	UF₆ NpF₆ PuF₆

Predicted binary hexafluorides

Noble gas binary hexafluorides	KrF₆ RnF₆

Transition metal binary hexafluorides	CrF₆ PdF₆

Actinide binary hexafluorides	AmF₆

Tellurium compounds

Te₂Br TeBr₄ Te₃Cl₂ TeCl₄ TeF₄ TeF₆ TeI₄ TeO TeO₂ TeO₃ TeN

Fluorine compounds

AgF AgF₂ Ag₂F AlF₃ AmF₃ AmF₄ AsF₃ AsF₅ AuF₃ BF₃ B₂F₄ BaF₂ BeF₂ BiF₃ BiF₅ BrF₃ BrF₅ CF₄ C₂F₆ CaF₂ CdF₂ CeF₃ ClF₃ ClF₅ CoF₂ CoF₃ CrF₂ CrF₃ CrF₄ CrF₅ CrF₆ CsF CuF DyF₃ ErF₃ EuF₂ EuF₃ DF HF FI KF LiF NaF RbF TlF FeF₂ HgF₂ Hg₂F₂ KrF₂ MgF₂ MnF₂ NiF₂ F₂O F₂O₄ PbF₂ PdF₂ SnF₂ SrF₂ XeF₂ ZnF₂ ZrF₂ FeF₃ GaF₃ GdF₃ HoF₃ InF₃ LaF₃ LuF₃ MnF₃ F₃N NdF₃ F₃P PrF₃ PuF₃ SbF₃ ScF₃ SmF₃ TbF₃ TiF₃ TlF₃ TmF₃ UF₃ VF₃ YF₃ YbF₃ GeF₄ HfF₄ MoF₄ F₄N₂ PbF₄ PuF₄ SF₄ SeF₄ SiF₄ SnF₄ TeF₄ ThF₄ UF₄ VF₄ WF₄ XeF₄ ZrF₄ IF₅ NbF₅ PF₅ SbF₅ TaF₅ UF₅ VF₅ WF₅ MoF₆ OsF₆ PtF₆ ReF₆ SF₆ SeF₆ TeF₆ UF₆ WF₆ XeF₆ IF₇ ReF₇ IrF₃ IrF₆ OsF₄ OsF₅ PmF₃ PrF₄ PuF₆ ReF₄ ReF₅ RhF₆ RuF₃ RuF₄ RuF₅ RuF₆ TcF₅ TcF₆ VF₂ YbF₂ AgBF₄ AgPF₆ Cs₂AlF₅ K₃AlF₆ Na₃AlF₆ KAsF₆ LiAsF₆ NaAsF₆ HBF₄ KBF₄ LiBF₄ NaBF₄ RbBF₄ Ba(BF₄)₂ Ni(BF₄)₂ Pb(BF₄)₂ Sn(BF₄)₂ BaClF BaSiF₆ BaGeF₆ BrOF₃ BrO₂F CBrF₃ CBr₂F₂ CBr₃F CClF₃ CCl₂F₂ CCl₃F CFN CF₂O CF₃I CHF₃ CH₂F₂ CH₃F C₂Cl₃F₃ C₂H₃F C₆H₅F C₇H₅F₃ C₁₅F₃₃N ClFO₂ CrFO₄ CrF₂O₂ CsBF₄ NH₄F FNO FNO₂ FNO₃ KHF₂ NaHF₂ ThOF₂ NH₅F₂ F₂OS F₃OP F₃PS HPF₆ HSbF₆ KPF₆ KSbF₆ LiPF₆ NaPF₆ NaSbF₆ Na₂SiF₆ Na₂TiF₆ Na₂ZrF₆ TlPF₆ IOF₃ K₂NbF₇ K₂TaF₇ IO₃F

Chemical formulas

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