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Titanium tetrafluoride

Titanium(IV) fluoride
Titanium(IV) fluoride
IUPAC name
Titanium(IV) fluoride
Other names
Titanium tetrafluoride
3D model (JSmol)
ECHA InfoCard 100.029.106
EC Number
  • 232-017-6
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
not listed
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
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).
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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.[1] 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.[2] X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.[3]

TiF4 forms adducts with many ligands. One example is cis-TiF4(MeCN)2, which is formed by treatment with acetonitrile.[4]


  1. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  2. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.
  3. ^ 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.
  4. ^ 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.