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:[1]
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). verify (what is ?) Infobox references

Titanium(IV) fluoride is the inorganic compound with the formula Ti F₄. 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 and structure

The traditional method involves treatment of titanium tetrachloride with excess hydrogen fluoride:[3]

TiCl₄ + 4 HF → TiF₄ + 4 HCl

Purification is by sublimation, which involves reversible cracking of the polymeric structure.[4] X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.[5]

Reactions

Structure of the [Ti₄F₁₈]^2- dianion

TiF₄ forms adducts with many ligands. One example is the complex cis-TiF₄(CH₃CN)₂, which is formed by treatment with acetonitrile.[6] It is also used as a reagent in the preparation of organofluorine compounds.[7] With fluoride, the cluster [Ti₄F₁₈]^2- forms. It has an admantane-like Ti₄F₆ core.[8]

Related to its Lewis acidity, TiF₄ forms a variety of hexafluorides also called hexafluorotitanates. Hexafluorotitanic acid has been used commercially to clean metal surfaces. These salts are stable at pH<4 in the presence of hydrogen fluoride, otherwise they hydrolyze to give oxides.[3]

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.
Meshri, Dayal T. (2000). "Fluorine Compounds, Inorganic, Titanium". Kirk‐Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.2009200113051908.a01. ISBN 9780471484943.
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 (7): 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.
Blizzard, T. A.; Sikervar, Vikas (2014). "Titanium(IV) Fluoride". Encyclopedia of Reagents for Organic Synthesis. pp. 1–5. doi:10.1002/047084289X.rn00123.pub2. ISBN 9780470842898.
Mazej, Zoran; Goreshnik, Evgeny (2009). "Poly[perfluorotitanate(IV)] Salts of [H₃O]⁺, Cs⁺, [Me₄N]⁺, and [Ph₄P]⁺ and about the Existence of an Isolated [Ti₂F₉]⁻ Anion in the Solid State". Inorganic Chemistry. 48 (14): 6918–6923. doi:10.1021/ic9009338. PMID 19545141.

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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.

[KO-3] Meshri, Dayal T. (2000). "Fluorine Compounds, Inorganic, Titanium". Kirk‐Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.2009200113051908.a01. ISBN 9780471484943.

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

[5] Bialowons, H.; Mueller, M.; Mueller, B.G. (1995). "Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 621 (7): 1227–1231. doi:10.1002/zaac.19956210720.

[6] 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.

[7] Blizzard, T. A.; Sikervar, Vikas (2014). "Titanium(IV) Fluoride". Encyclopedia of Reagents for Organic Synthesis. pp. 1–5. doi:10.1002/047084289X.rn00123.pub2. ISBN 9780470842898.

[8] Mazej, Zoran; Goreshnik, Evgeny (2009). "Poly[perfluorotitanate(IV)] Salts of [H₃O]⁺, Cs⁺, [Me₄N]⁺, and [Ph₄P]⁺ and about the Existence of an Isolated [Ti₂F₉]⁻ Anion in the Solid State". Inorganic Chemistry. 48 (14): 6918–6923. doi:10.1021/ic9009338. PMID 19545141.