Titanium tetrafluoride

Titanium(IV) fluoride
Names
	IUPAC name Titanium(IV) fluoride
	Other names Titanium tetrafluoride
Identifiers
CAS Number	7783-63-3 ;
3D model (JSmol)	Interactive image;
ChemSpider	7988529 ;
ECHA InfoCard	100.029.106
EC Number	232-017-6;
PubChem CID	121824;
UNII	T08RW8YRG1 ;
CompTox Dashboard (EPA)	DTXSID50894996 ;
	InChI InChI=1S/4FH.Ti/h41H;/q;;;;+4/p-4 Key: XROWMBWRMNHXMF-UHFFFAOYSA-J ; InChI=1/4FH.Ti/h41H;/q;;;;+4/p-4 Key: XROWMBWRMNHXMF-XBHQNQODAM;
	SMILES F[Ti](F)(F)F;
Properties
Chemical formula	TiF4
Molar mass	123.861 g/mol
Appearance	white powder
Density	2.798 g/cm3
Melting point	377 °C (711 °F; 650 K)
Boiling point	sublimes
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H312, H314, H332
Precautionary statements	P260, P261, P264, P270, P271, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P310, P312, P322, P330, P363, P405
NFPA 704 (fire diamond)	3 0 0
Related compounds
Other anions	Titanium(IV) bromide ; Titanium(IV) chloride ; Titanium(IV) iodide
Related compounds	Titanium(III) fluoride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	(what is ?)
	Infobox references

Titanium(IV) fluoride is the inorganic compound with the formula TiF₄. It is a white hygroscopic solid. In contrast to the other tetrahalides of titanium, it adopts a polymeric structure.^[2] In common with the other tetrahalides, TiF₄ is a strong Lewis acid.

Preparation, structure, reactions[]

The traditional method involves treatment of titanium tetrachloride with excess hydrogen fluoride:

TiCl₄ + 4 HF → TiF₄ + 4 HCl

Purification is by sublimation, which involves reversible cracking of the polymeric structure.^[3] X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.^[4]

TiF₄ forms adducts with many ligands. One example is cis-TiF₄(MeCN)₂, which is formed by treatment with acetonitrile.^[5]

References[]

^ "Titanium tetrafluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.
^ Bialowons, H.; Mueller, M.; Mueller, B.G. (1995). "Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 621: 1227–1231. doi:10.1002/zaac.19956210720.
^ Nikiforov, Grigory B.; Roesky, Herbert W.; Koley, Debasis (2014). "A survey of titanium fluoride complexes, their preparation, reactivity, and applications". Coordination Chemistry Reviews. 258–259: 16–57. doi:10.1016/j.ccr.2013.09.002.

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[1] "Titanium tetrafluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 12 December 2021.

[2] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[3] Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.

[4] Bialowons, H.; Mueller, M.; Mueller, B.G. (1995). "Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 621: 1227–1231. doi:10.1002/zaac.19956210720.

[5] Nikiforov, Grigory B.; Roesky, Herbert W.; Koley, Debasis (2014). "A survey of titanium fluoride complexes, their preparation, reactivity, and applications". Coordination Chemistry Reviews. 258–259: 16–57. doi:10.1016/j.ccr.2013.09.002.

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