Cobalt(II) fluoride

Cobalt(II) fluoride
Names
IUPAC name
Cobalt(II) fluoride
Other names
cobalt difluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.044
EC Number
  • 233-061-9
RTECS number
  • GG0770000
CompTox Dashboard (EPA)
SMILES
  • F[Co]F
Properties
CoF2
Molar mass 96.93 g/mol
Appearance Red crystalline solid
Density 4.46 g/cm3 (anhydrous)
2.22 g/cm3 (tetrahydrate)
Melting point 1,217 °C (2,223 °F; 1,490 K)
Boiling point 1,400 °C (2,550 °F; 1,670 K)
1.4 g/100 mL (25 °C)
Solubility soluble in HF
insoluble in alcohol, ether, benzene
Structure
tetragonal (a,hydrous)
orthorhombic (tetrahydrate)
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
3
0
2
Lethal dose or concentration (LD, LC):
LD50 (median dose)
 oral (rat): 150 mg/kg
Related compounds
Other anions
 cobalt(II) oxide, cobalt(II) chloride
Other cations
 iron(II) fluoride, nickel(II) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Cobalt(II) fluoride, also known as cobaltous fluoride, is a chemical compound. Its chemical formula is CoF2. It contains cobalt in its +2 oxidation state. It also contains fluoride ions.

Properties

It is a reddish crystalline solid. It only dissolves a little in water. The hydrate (type with water molecules attached) can dissolve in water. It can dissolve in acid. It can react with hydrogen at 300 °C (572 °F) to make cobalt and hydrogen fluoride.

Preparation

It can be made by reacting anhydrous (without any water molecules attached) cobalt(II) oxide or cobalt(II) chloride with a stream of hydrogen fluoride. This reaction makes the anhydrous form. The hydrated (with water molecules attached) form is made by reacting any cobalt(II) compound with hydrofluoric acid. When fluorine is reacted with cobalt at a high temperature, it makes both cobalt(II) fluoride and cobalt(III) fluoride.

Uses

It is used as a catalyst. It can be used as a source of the fluoride ion in dentist care. It is used in lenses.

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