Chemistry:Titanium tetrafluoride
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| Names | |
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| IUPAC name
Titanium(IV) fluoride
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| Other names
Titanium tetrafluoride
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| 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 pictograms |  
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| GHS Signal word | Danger |
| H302, H312, H314, H332 | |
| P260, P261, P264, P270, P271, P280, P301+312, P301+330+331, P302+352, P303+361+353, P304+312, P304+340, P305+351+338, P310, P312, P322, P330, P363, P405 | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other anions
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Titanium(IV) bromide Titanium(IV) chloride Titanium(IV) iodide |
Related compounds
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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   ?)
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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.[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
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 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
- ↑ "Titanium tetrafluoride" (in en). https://pubchem.ncbi.nlm.nih.gov/compound/121824#section=Safety-and-Hazards.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ 3.0 3.1 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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