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Titanium tetrafluoride

Titanium(IV) fluoride
Titanium(IV) fluoride
Names
IUPAC name
Titanium(IV) fluoride
Other names
Titanium tetrafluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.106
EC Number
  • 232-017-6
Properties
TiF4
Molar mass 123.861 g/mol
Appearance white powder
hygroscopic
Density 2.798 g/cm3
Melting point 377 °C (711 °F; 650 K)
Boiling point sublimes
Hazards
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
0
3
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).
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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]

References

  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.