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	{{chembox		{{chembox
			| Watchedfields = changed
⚫	| Name = Tellurium hexafluoride
			| verifiedrevid = 405721787
⚫	| ImageFileL1 = Tellurium-hexafluoride-dimensions-2D.png
		⚫	| Name = Tellurium hexafluoride
	| ImageNameL1 = Structure and dimensions of the molecule
	| ImageFileR1 = Tellurium-hexafluoride-from-xtal-1992-3D-balls.png		| ImageFileL1 = Tellurium-hexafluoride-dimensions-2D.png
	| ImageNameR1 = Ball-and-stick model of the molelcule		| ImageNameL1 = Structure and dimensions of the molecule
		⚫	| ImageFileR1 = Tellurium-hexafluoride-from-xtal-1992-3D-balls.png
	| IUPACName =
			| ImageNameR1 = Ball-and-stick model of the molelcule
⚫	| Section1 = {{Chembox Identifiers
	| CASNo = 7783-80-4		| IUPACName =
		⚫	|Section1={{Chembox Identifiers
	| SMILES = xxxxx
			| CASNo_Ref = {{cascite|correct|??}}
⚫	| PubChem = 24559
			| CASNo = 7783-80-4
			| UNII_Ref = {{fdacite|correct|FDA}}
			| UNII = JWI7143IXR
			| SMILES = F(F)(F)(F)(F)F
			| InChI = 1S/F6Te/c1-7(2,3,4,5)6
		⚫	| PubChem = 24559
			| EINECS = 232-027-0
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Formula = TeF<sub>6</sub>		| Formula = TeF<sub>6</sub>
	| MolarMass = 241.59 g/mol		| MolarMass = 241.590 g/mol
			| Appearance = colorless gas
	| Density = 0.0106 g/cm³
			| Odor = repulsive
⚫	| MeltingPt = −38.9 °C<ref name="CRC_HANDBOOK">'']'', 90. Auflage, CRC Press, Boca Raton, Florida, 2009, ISBN 978-1-4200-9084-0, Section 4, ''Physical Constants of Inorganic Compounds'', p.&nbsp;4-95.</ref>
			| Density = 0.0106 g/cm<sup>3</sup> (-10 °C) <br /> 4.006 g/cm<sup>3</sup> (-191 °C)
⚫	| BoilingPt = −37.6 °C<ref name="CRC_HANDBOOK"/>
			| MeltingPtC = −38.9
		⚫	| MeltingPt_ref = <ref name="CRC_HANDBOOK">'']'', 90. Auflage, CRC Press, Boca Raton, Florida, 2009, {{ISBN|978-1-4200-9084-0}}, Section 4, ''Physical Constants of Inorganic Compounds'', p.&nbsp;4-95.</ref>
			| BoilingPtC = −37.6
		⚫	| BoilingPt_ref = <ref name="CRC_HANDBOOK" />
			| Solubility = decomposes
			| RefractIndex = 1.0009
			| VaporPressure = >1 atm (20°C)<ref name="PGCH" />
			| MagSus = −66.0·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| CrystalStruct = ], ]		| CrystalStruct = ], ]
	| SpaceGroup = Pnma, No. 62		| SpaceGroup = Pnma, No. 62
	| Coordination = octahedral (''O<sub>h</sub>'')		| Coordination = octahedral (''O<sub>h</sub>'')
	| Dipole = 0		| Dipole = 0
	}}		}}
			|Section4={{Chembox Thermochemistry
			| HeatCapacity = 117.6 J/(mol K)
			| DeltaHf = -1318 kJ/mol
			}}
			|Section5={{Chembox Hazards
			| IDLH = 1 ppm<ref name=PGCH>{{PGCH|0588}}</ref>
			| REL = TWA 0.02 ppm (0.2 mg/m<sup>3</sup>)<ref name="PGCH" />
			| PEL = TWA 0.02 ppm (0.2 mg/m<sup>3</sup>)<ref name="PGCH" />
			| LCLo = 5 ppm (rat, 4 hr)<br />5 ppm (mouse, 1 hr)<br />5 ppm (rabbit, 4 hr)<br />5 ppm (guinea pig, 4 hr)<ref>{{IDLH|7783804|Tellurium hexafluoride (as Te)}}</ref>
			}}
	}}		}}
	'''Tellurium hexafluoride''' is the oldest known ] of ]. It is a colorless, highly toxic gas with an extremely unpleasant smell.		'''Tellurium hexafluoride''' is the ] of ] and ] with the chemical formula TeF<sub>6</sub>. It is a colorless, highly toxic gas with an unpleasant odor.<ref name=Brauer>{{cite book|author=W. Kwasnik|chapter=Tellurium Hexafluoride|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=1|pages=180}}</ref>
	==Preparation==		== Preparation ==
	Tellurium hexafluoride is most commonly prepared by passing ] gas over tellurium metal at 150 °C. Below this temperature a mixture of lower fluorides form, including ] and ]. It can also be prepared by passing fluorine gas over TeO<sub>3</sub> or indirectly by reacting TeO<sub>2</sub> with SeF<sub>4</sub> to produce TeF<sub>4</sub> and then heating TeF<sub>4</sub> in excess of 200 °C to make TeF<sub>6</sub> and Te.		Tellurium hexafluoride can be prepared by treating tellurium with ] gas at 150 °C.<ref name="Brauer" /><ref>{{cite book |doi=10.1002/9780470132326.ch44|chapter=Sulfur, Selenium, and Tellurium Hexafluorides|year=2007|last1=Yost|first1=Don M.|title=Inorganic Syntheses|orig-year=1939|pages=121–122|volume=1|isbn=978-0-470-13232-6}}</ref> It can also be prepared by fluorination of ] with ]. Upon heating, ] disproportionates to give TeF<sub>6</sub> and Te.{{cn|date=March 2021}}
	==Properties==		== Properties ==
	Tellurium hexafluoride is a highly symmetric octahedral molecule. Its physical properties resemble the ] and ] analogs. It is less ], however, due to the increase in ]. At temperatures below −38 °C, tellurium hexafluoride condenses to a volatile white solid.		Tellurium hexafluoride is a highly symmetric octahedral molecule. Its physical properties resemble those of the hexafluorides of ] and ]. It is less ], however, due to the increase in ]. At temperatures below −38 °C, tellurium hexafluoride condenses to a volatile white solid.
			<gallery mode="packed" heights="150">
	<center>] ]</center>		File:Tellurium-hexafluoride-xtal-1992-3D-balls.png|Ball-and-stick model of the crystal structure
			File:Tellurium-hexafluoride-xtal-1992-3D-SF.png|Space-filling model of the crystal structure
			</gallery>
		⚫	== Reactivity ==
			Tellurium hexafluoride is much more chemically ] than SF<sub>6</sub>.<ref>{{Greenwood&Earnshaw2nd}}</ref> For example, TeF<sub>6</sub> slowly hydrolyzes to ]:
			:TeF<sub>6</sub> + 6 H<sub>2</sub>O → Te(OH)<sub>6</sub> + 6 HF
			Treatment of tellurium hexafluoride with ] (Me<sub>4</sub>NF) gives, sequentially, the hepta- and octafluorides:
			:TeF<sub>6</sub> + Me<sub>4</sub>NF → Me<sub>4</sub>NTeF<sub>7</sub>
			:Me<sub>4</sub>NTeF<sub>7</sub> + Me<sub>4</sub>NF → (Me<sub>4</sub>N)<sub>2</sub>TeF<sub>8</sub>
			== Further sources ==
⚫	==Reactivity==
		⚫	*W.C. Cooper, ''Tellurium'', Van Nostrand Reinhold Company, New York, USA, 1971.
	Unlike the ] analog, tellurium hexafluoride is not chemically ]. This can be attributed to the greater availability of the ''d'' orbitals and perhaps the availability of the ''f'' orbitals which neither sulfur or selenium have access to. TeF<sub>6</sub> is hydrolyzed in water to H<sub>6</sub>TeO<sub>6</sub> and reacts with Te below 200 °C.
		⚫	*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.
		⚫	*], 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.
	==Health Hazards==		== References ==
	People exposed to ] compounds exhibit "tellurium ]", which has a ]-like ]. This garlic odour is also present in ] and ]. Other symptoms of tellurium exposure include ], ], weakness, bluish-black markings on ]s, ], ] and ], ] taste in the mouth and skin rash. Death may occur from ]. People exposed to tellurium compounds should be removed from the area and seek medical attention.
	==References==
	{{reflist}}		{{reflist}}
		⚫	== External links ==
	==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==
⚫	*
⚫	*
			{{Hexafluorides}}
	{{Tellurium compounds}}		{{Tellurium compounds}}
			{{fluorine compounds}}
	{{DEFAULTSORT:Tellurium Hexafluoride}}		]
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