iron trifluoride, ferric fluoride
3D model (JSmol)
|Molar mass||112.840 g/mol (anhydrous) |
166.89 g/mol (trihydrate)
|Appearance||pale green crystals|
|Density||3.87 g/cm3 (anhydrous) |
2.3 g/cm3 (trihydrate)
|Melting point||> 1,000 °C (1,830 °F; 1,270 K)|
|slightly soluble (anhydrous) |
49.5 g/100 mL (trihydrate)
|Solubility||negligible in alcohol, ether, benzene|
|R-3c, No. 167|
|iron(III) oxide, iron(III) chloride|
|manganese trifluoride, cobalt trifluoride, ruthenium(III) fluoride|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Iron(III) fluoride, also known as ferric fluoride, is an inorganic compound. It exists in an anhydrous form (formula FeF3) as well as two hydrated forms (both formula FeF3·3H2O). It is produced commercially mostly for laboratory work and is not as useful as the related compound iron(III) chloride. Anhydrous iron(III) fluoride is white while the hydrated forms are light pink.
Chemical and physical properties
Iron(III) fluoride is a thermally robust, paramagnetic solid, consisting of high spin Fe(III) centers, which is consistent with the pale colors of all forms of this material. Both anhydrous iron(III) fluoride as well as its hydrates are hygroscopic.
The anhydrous form adopts a simple structure with octahedral Fe(III)F6 centres interconnected by linear Fe-F-Fe linkages. In the language of crystallography, the crystals are classified as rhombohedral with an R-3c space group. The structural motif is similar to that seen in ReO3. Although the solid is nonvolatile, it evaporates at high temperatures, the gas at 987 °C consists of FeF3, a planar molecule of D3h symmetry with three equal Fe-F bonds, each of length 176.3 pm. At very high temperatures, it decomposes to give FeF2 and F2.
Two crystalline forms—or more technically, polymorphs—of FeF3·3H2O are known, the α and β forms. These are prepared by evaporation of an HF solution containing Fe3+ at room temperature (α form) and above 50 °C (β form). The space group of the β form is P4/m, and the α form maintains a P4/m space group with a J6 substructure. The solid α form is unstable and converts to the β form within days. The two forms are distinguished by their difference in quadrupole splitting from their Mössbauer spectra.
Preparation, occurrence, reactions
Anhydrous iron(III) fluoride is prepared by treating virtually any anhydrous iron compound with fluorine. More practically and like most metal fluorides, it is prepared by treating the corresponding chloride with hydrogen fluoride:
- FeCl3 + 3 HF → FeF3 + 3 HCl
The primary commercial use of iron(III) fluoride in the production of ceramics.
Some cross coupling reaction are catalyzed by ferric fluoride-based compounds. Specifically the coupling of biaryl compounds are catalyzed by hydrated iron(II) fluoride complexes of N-heterocyclic carbene ligands. Other metal fluorides also catalyse similar reactions. Iron(III) fluoride has also been shown to catalyze chemoselective addition of cyanide to aldehydes to give the cyanohydrins.
The anhydrous material is a powerful dehydrating agent. The formation of ferric fluoride may have been responsible for the explosion of a cylinder of hydrogen fluoride gas.
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- "A recent explosion of a lecture-size cylinder of hydrogen fluoride ... has renewed concerns that compressed gas cylinders can be especially dangerous" (PDF). University of California San Francisco. Archived from the original (PDF) on 2006-09-01.
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