Tellurium hexafluoride

Tellurium hexafluoride

Identifiers
CAS number	7783-80-4
PubChem	24559
Jmol-3D images	Image 1
SMILES F[Te](F)(F)(F)(F)F
InChI InChI=1S/F6Te/c1-7(2,3,4,5)6
Properties
Molecular formula	TeF₆
Molar mass	241.590 g/mol
Odor	repulsive odor
Density	0.0106 g/cm³
Melting point	−38.9 °C
Boiling point	−37.6 °C
Solubility in water	decomposes
Structure
Crystal structure	Orthorhombic, oP28
Space group	Pnma, No. 62
Coordination geometry	octahedral (O_h)
Dipole moment	0
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Tellurium hexafluoride is the oldest^{[clarification needed]} known fluoride of tellurium. 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 metal 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]

CRC Handbook of Chemistry and Physics, 90. Auflage, CRC Press, Boca Raton, Florida, 2009, - get this book, Section 4, Physical Constants of Inorganic Compounds, p. 4-95.

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]

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

v t e Tellurium compounds

TeBr₂ TeBr₄ TeCl₂ TeCl₄ TeF₄ TeF₆ TeI₄ TeO TeO₂ TeO₃

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Information source: wikipedia.org

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