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 Edit this at Wikidata
EC Number
  • 233-061-9
RTECS number
  • GG0770000
UNII
  • InChI=1S/Co.2FH/h;2*1H/q+2;;/p-2 checkY
    Key: YCYBZKSMUPTWEE-UHFFFAOYSA-L checkY
  • InChI=1/Co.2FH/h;2*1H/q+2;;/p-2
    Key: YCYBZKSMUPTWEE-NUQVWONBAL
  • 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
+9490.0·10−6 cm3/mol
Structure
tetragonal (anhydrous)
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 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Lethal dose or concentration (LD, LC):
oral (rat): 150 mg/kg
Related compounds
Other anions
cobalt(II) oxide, cobalt(II) chloride
Other cations
iron(II) fluoride, nickel(II) fluoride
Related compounds
cobalt trifluoride
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 cobalt(II) fluoride
Anhydrous cobalt(II) fluoride

Cobalt(II) fluoride is a chemical compound with the formula (CoF2). It is a pink crystalline solid compound[1][2] which is antiferromagnetic at low temperatures (TN=37.7 K)[3] The formula is given for both the red tetragonal crystal, (CoF2), and the tetrahydrate red orthogonal crystal, (CoF2·4H2O). CoF2 is used in oxygen-sensitive fields, namely metal production. In low concentrations, it has public health uses. CoF2 is sparingly soluble in water. The compound can be dissolved in warm mineral acid, and will decompose in boiling water. Yet the hydrate is water-soluble, especially the di-hydrate CoF2·2H2O and tri-hydrate CoF2·3H2O forms of the compound. The hydrate will also decompose with heat.

Like some other metal difluorides, CoF2 crystallizes in the rutile structure, which features octahedral Co centers and planar fluorides.[4]

  1. ^ Pradyot Patnaik (2002), Handbook of Inorganic Chemicals, McGraw-Hill Professional, ISBN 978-0-07-049439-8
  2. ^ Pashkevich, D. S.; Radchenko S. M.; Mukhortov, D. A., "Article title Heat Exchange between Cobalt(II) Fluoride Powder and the Wall of Rotating Cylinder" (PDF), Russian Journal of Applied Chemistry, Consultants Bureau, ISSN 1070-4272, archived from the original (PDF) on 2004-09-29, retrieved 2007-03-07
  3. ^ Ashcroft/Mermin: Solid State Physics (Tab. 33.2)
  4. ^ Stout, J. W.; Reed, Stanley A. (1954). "The Crystal Structure of MnF2, FeF2, CoF2, NiF2 and ZnF2". J. Am. Chem. Soc. 76 (21): 5279–5281. doi:10.1021/ja01650a005.