|Molar mass||115.928 g/mol|
|Melting point||927 °C (1,701 °F; 1,200 K)|
|cobalt(III) oxide, cobalt(III) chloride|
|iron(III) fluoride, rhodium(III) fluoride|
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
|what is: / ?)(|
Cobalt(III) fluoride is the inorganic compound with the formula CoF3. This highly reactive, hygroscopic brown solid is used to synthesize organofluorine compounds. CoF3 is a powerful fluorinating agent that leaves CoF2 as the byproduct.
- CoCl2 + 3/2 F2 → CoF3 + Cl2
This conversion is a redox reaction: Co2+ and Cl− are oxidized to Co3+ and Cl2, respectively, while F2 is reduced to F−. Cobalt(II) oxide (CoO) and cobalt(II) fluoride (CoF2) can also be converted to cobalt(III) fluoride using fluorine.
CoF3 decomposes upon contact with water to give oxygen:
- 4 CoF3 + 2 H2O → 4 HF + 4 CoF2 + O2
CoF3 is hygroscopic, forming a dihydrate (CAS#54496-71-8). It reacts with fluoride sources to give the anion [CoF6]3−, which is a rare example of a high-spin, octahedral cobalt(III) complex.
- 2CoF3 + R-H → 2CoF2 + R-F + HF
- Coe, P. L. "Cobalt(III) Fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289X.rc185.
- Priest, H. F. "Anhydrous Metal Fluorides" Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183. doi:10.1002/9780470132340.ch47
- Coe, P. L. "Potassium Tetrafluorocobaltate(III)" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289X.rp251.
|Wikimedia Commons has media related to Cobalt(III) fluoride.|
- National Pollutant Inventory - Cobalt fact sheet
- National Pollutant Inventory - Fluoride and compounds fact sheet