Iron(II) fluoride or ferrous fluoride is an inorganic compound with the molecular formula FeF2. It forms a tetrahydrate FeF2·4H2O that is often referred to by the same names. The anhydrous and hydrated forms are white crystalline solids.
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||93.84 g/mol (anhydrous) |
165.902 g/mol (tetrahydrate)
|Appearance||colorless transparent crystals|
|Density||4.09 g/cm3 (anhydrous) |
2.20 g/cm3 (tetrahydrate)
|Melting point||970 °C (1,780 °F; 1,240 K) (anhydrous) |
100 °C (tetrahydrate)
|Boiling point||1,100 °C (2,010 °F; 1,370 K) (anhydrous)|
Solubility product (Ksp)
|Solubility||insoluble in ethanol, ether; |
dissolves in HF
|Rutile (tetragonal), tP6|
|P42/mnm, No. 136|
|Occupational safety and health (OHS/OSH):|
|Causes severe skin burns & eye damage; |
Hazardous decomposition products formed under fire conditions- Iron oxides
|NFPA 704 (fire diamond)|
|Flash point||not applicable|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Anhydrous FeF2 adopts the TiO2 rutile structure. As such, the iron cations are octahedral and fluoride anions are trigonal planar.
The tetrahydrate can exist in two structures, or polymorphs. One form is rhombohedral and the other is hexagonal, the former having a disorder.
Like most fluoride compounds, the anhydrous and hydrated forms of iron(II) fluoride feature high spin metal center. Low temperature neutron diffraction studies show that the FeF2 is antiferromagnetic. Heat capacity measurements reveal an event at 78.3 K corresponding to ordering of antiferromagnetic state.
FeF2 sublimes between 958 and 1178 K. Using Torsion and Knudsen methods, the heat of sublimation was experimentally determined and averaged to be 271 ± 2 kJ mole−1.
The following reaction is proposed in order to calculate the atomization energy for Fe+:
The anhydrous salt can be prepared by reaction of ferrous chloride with anhydrous hydrogen fluoride. It is slightly soluble in water (with solubility product Ksp = 2.36×10−6 at 25 °C) as well as dilute hydrofluoric acid, giving a pale green solution. It is insoluble in organic solvents.
The tetrahydrate can be prepared by dissolving iron in warm hydrated hydrofluoric acid and precipitating the result by addition of ethanol. It oxidizes in moist air to give, inter alia, a hydrate of iron(III) fluoride, (FeF3)2·9H2O.