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Cobalt(III) fluoride

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Title: Cobalt(III) fluoride  
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Subject: Cobalt, Cobalt(II) chlorate, Cobalt(II) oxalate, Cobalt(II) selenide, Cobalt(II) phosphide
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Cobalt(III) fluoride

Dangerous for the Environment (Nature) N|
Cobalt(III) fluoride
Cobalt(III) fluoride
Names
Other names
Cobalt trifluoride
Cobaltic fluoride
Cobalt fluoride
Cobaltic trifluoride
Identifiers
 YesY
ChemSpider  YesY
EC number 233-062-4
Jmol-3D images Image
PubChem
Properties
small=yes}}} }}} 0}}} 1=C|C} }}} 1=H|H} }}} 1=Ac|Ac} }}} 1=Ag|Ag} }}} 1=Al|Al} }}} 1=Am|Am} }}} 1=Ar|Ar} }}} 1=As|As} }}} 1=At|At} }}} 1=Au|Au} }}} 1=B|B} }}} 1=Ba|Ba} }}} 1=Be|Be} }}} 1=Bh|Bh} }}} 1=Bi|Bi} }}} 1=Bk|Bk} }}} 1=Br|Br} }}} 1=Ca|Ca} }}} 1=Cd|Cd} }}} 1=Ce|Ce} }}} 1=Cf|Cf} }}} 1=Cn|Cn} }}} 1=Cl|Cl} }}} 1=Cm|Cm} }}} 1=Co|Co} }}} 1=Cr|Cr} }}} 1=Cs|Cs} }}} 1=Cu|Cu} }}} 1=Db|Db} }}} 1=Ds|Ds} }}} 1=Dy|Dy} }}} 1=Er|Er} }}} 1=Es|Es} }}} 1=Eu|Eu} }}} 1=F|F} }}} 1=Fe|Fe} }}} 1=Fl|Fl} }}} 1=Fm|Fm} }}} 1=Fr|Fr} }}} 1=Ga|Ga} }}} 1=Gd|Gd} }}} 1=Ge|Ge} }}} 1=He|He} }}}}
Documentation

Appearance brown powder
Density 3.88 g/cm3
Melting point 92 °C (198 °F; 365 K)
reacts
Structure
hexagonal
Hazards
NFPA 704
0
3
2
Related compounds
Other anions
cobalt(III) oxide, cobalt(III) chloride
Other cations
iron(III) fluoride, rhodium(III) fluoride
Related compounds
cobalt(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 YesY  (: YesY/N?)

Cobalt(III) fluoride is the [1] CoF3 is a powerful fluorinating agent that leaves CoF2 as the byproduct.

Preparation

CoF3 is prepared in the laboratory by treating CoCl2 with fluorine at 250 °C:[2]

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.

Reactions

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.

Applications

Used as slurry, CoF3 converts hydrocarbons to the perfluorocarbons:

2CoF3 + R-H → 2CoF2 + R-F + HF

Such reactions are sometimes accompanied by rearrangements or other reactions.[1] The related reagent KCoF4 is more selective.[3]

References

  1. ^ a b 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.
  2. ^ Priest, H. F. "Anhydrous Metal Fluorides" Inorganic Syntheses McGraw-Hill: New York, 1950; Vol. 3, pages 171-183. doi:10.1002/9780470132340.ch47
  3. ^ 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.

External links

  • National Pollutant Inventory - Cobalt fact sheet
  • National Pollutant Inventory - Fluoride and compounds fact sheet
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