- Cobalt(II) fluoride (CoF₂) is an inorganic compound containing cobalt in its +2 oxidation state bonded to fluoride ions, important in both research and industrial applications.
- Physical properties include its appearance as rose-pink to red crystals with a rutile-type crystal structure. It has a high melting point of 1200°C and is relatively dense compared to other metal fluorides.
- Structure features a distorted octahedral geometry around each cobalt ion, with fluoride ions bridging between cobalt centers in the crystal lattice. This arrangement results in interesting magnetic properties.
- Chemical composition consists of cobalt and fluorine in a 1:2 ratio, reflecting the divalent nature of cobalt in this compound. The molecular weight is approximately 96.93 g/mol.
- Magnetic properties are particularly interesting, showing antiferromagnetic behavior below its Néel temperature. The compound contains unpaired electrons in the d-orbital of Co2+, contributing to its magnetic characteristics.
- Synthesis can be achieved through several methods, including direct reaction of cobalt metal with fluorine gas, or reaction of cobalt(II) carbonate or oxide with hydrofluoric acid.
- Solubility characteristics show it is slightly soluble in water, forming the hydrated complex [Co(H2O)6]2+, and the solution appears pink due to d-d transitions in the cobalt ion.
- Chemical reactivity includes its ability to act as a fluorinating agent in some organic reactions, though it is less reactive than many other metal fluorides.
- Industrial applications include its use as a catalyst in certain organic syntheses, as a component in some specialized glasses and optical materials, and in certain electrochemical applications.
- Coordination chemistry shows CoF2 can act as a starting material for preparing more complex cobalt compounds and coordination complexes.
- Electronic structure involves partially filled d-orbitals of Co2+, leading to its characteristic color and magnetic properties. The compound exhibits typical characteristics of transition metal fluorides.
- Safety considerations include its corrosive nature and the generation of hydrogen fluoride when exposed to moisture or acids. Proper handling and storage procedures are essential.
- Thermal behavior shows stability at high temperatures, making it useful in some high-temperature applications. It doesn’t decompose until very high temperatures.
- Spectroscopic properties include characteristic absorption bands in the visible region, responsible for its pink color, and distinctive patterns in infrared spectroscopy.
- Crystal field effects are important in determining its properties, with the fluoride ligands creating a specific splitting of the cobalt d-orbitals.
- Storage requirements include keeping it in dry, sealed containers due to its tendency to absorb moisture from the air.
- Commercial forms include anhydrous and hydrated versions, each with specific applications and handling requirements.
