Titanium tetrafluoride

In today's world, Titanium tetrafluoride has become a topic of great relevance and interest to a large number of people in different areas of society. Whether due to its impact on culture, the environment, politics or the economy, Titanium tetrafluoride has managed to capture the attention of academics, professionals and the general public. In this article, we will explore different aspects related to Titanium tetrafluoride, its importance and its influence on various aspects of daily life. From its origins to its possible future consequences, we will take an in-depth look at the relevance of Titanium tetrafluoride in today's world.

Titanium(IV) fluoride
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 Edit this at Wikidata
EC Number
  • 232-017-6
UNII
  • InChI=1S/4FH.Ti/h4*1H;/q;;;;+4/p-4 checkY
    Key: XROWMBWRMNHXMF-UHFFFAOYSA-J checkY
  • InChI=1/4FH.Ti/h4*1H;/q;;;;+4/p-4
    Key: XROWMBWRMNHXMF-XBHQNQODAM
  • F(F)(F)F
Properties
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]
GHS05: CorrosiveGHS07: Exclamation mark
Danger
H302, H312, H314, H332
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)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
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 , 100 kPa).
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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 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 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 2- forms. It has an adamantane-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

  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. ^ a b Meshri, Dayal T. (2000). "Fluorine Compounds, Inorganic, Titanium". Kirk-Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.2009200113051908.a01. ISBN 978-0-471-48494-3.
  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 978-0-470-84289-8.
  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.