Titanium tetrafluoride: Difference between revisions
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| Name = Titanium(IV) fluoride |
| Name = Titanium(IV) fluoride |
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| ImageFile = TiF4.jpg |
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| ImageName = Titanium(IV) fluoride |
| ImageName = Titanium(IV) fluoride |
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| OtherNames = titanium tetrafluoride |
| OtherNames = titanium tetrafluoride |
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The traditional method involves treatment of titanium tetrachloride with excess [[hydrogen fluoride]], and purification by sublimation:<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref> |
The traditional method involves treatment of titanium tetrachloride with excess [[hydrogen fluoride]], and purification by sublimation:<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref> |
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:TiCl<sub>4</sub> + 4 HF → TiF<sub>4</sub> + 4 HCl |
:TiCl<sub>4</sub> + 4 HF → TiF<sub>4</sub> + 4 HCl |
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X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.<ref>{{cite journal|author1=Bialowons, H.|author2=Mueller, M.|author3=Mueller, B.G.|title=Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur|journal=Zeitschrift für Anorganische und Allgemeine Chemie|year=1950|volume= 621|pages=1227-1231|doi=10.1002/zaac.19956210720}}</ref> |
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==References== |
==References== |
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Revision as of 16:47, 31 December 2016
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| Names | |
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| Other names
titanium tetrafluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.106 |
| EC Number |
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PubChem CID
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CompTox Dashboard (EPA)
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| 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 | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 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 halides of titanium, it adopts a polymeric structure consisting of octahedral Ti centres.[1]
Preparation
The traditional method involves treatment of titanium tetrachloride with excess hydrogen fluoride, and purification by sublimation:[2]
- TiCl4 + 4 HF → TiF4 + 4 HCl
X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.[3]
References
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ 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. (1950). "Titantetrafluorid - Eine Überraschend einfache Kolumnarstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 621: 1227–1231. doi:10.1002/zaac.19956210720.
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