-fluoride-from-xtal-column-3D-bs-17.png) | |
| Names | |
|---|---|
| IUPAC name Titanium(IV) fluoride | |
| Other names Titanium tetrafluoride | |
| Identifiers | |
3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.029.106 |
| EC Number |
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| UNII | |
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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 labelling:[1] | |
  | |
| 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) | |
| Related compounds | |
Otheranions | Titanium(IV) bromide Titanium(IV) chloride Titanium(IV) iodide |
Related compounds | Titanium(III) fluoride |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Titanium(IV) fluoride is theinorganic compound with theformulaTiF4. It is a whitehygroscopic solid. In contrast to the other tetrahalides of titanium, it adopts a polymeric structure.[2] In common with the other tetrahalides, TiF4 is a strongLewis acid.
The traditional method involves treatment oftitanium tetrachloride with excesshydrogen fluoride:[3]
Purification is by sublimation, which involves reversiblecracking of the polymeric structure.[4]X-ray crystallography reveals that the Ti centres are octahedral, but conjoined in an unusual columnar structure.[5]
TiF4 forms adducts with many ligands. One example is the complexcis-TiF4(CH3CN)2, which is formed by treatment withacetonitrile.[6] It is also used as a reagent in the preparation oforganofluorine compounds.[7] With fluoride, the cluster [Ti4F18]2- forms. It has an adamantane-like Ti4F6 core.[8]
Related to itsLewis 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 ofhydrogen fluoride, otherwise they hydrolyze to giveoxides.[3]
