Cobalt(II) fluoride
| Names | |
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| IUPAC name
Cobalt(II) fluoride
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| Other names
cobalt difluoride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.044 |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| 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 | |
| GHS labelling:[1] | |
| Danger | |
| H301, H314, H317, H351 | |
| P203, P260, P264, P270, P272, P280, P301+P316, P301+P330+P331, P302+P352, P302+P361+P354, P304+P340, P305+P354+P338, P316, P318, P321, P330, P333+P317, P362+P364, P363, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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oral (rat): 150 mg/kg |
| Related compounds | |
Other anions
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Other cations
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Related compounds
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Cobalt trifluoride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
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Cobalt(II) fluoride is an inorganic compound with the formula CoF2. It is a pink paramagnetic solid.[2] Like some other metal difluorides, CoF2 crystallizes in the rutile structure, which features octahedral Co centers and planar fluorides.[3]
Preparation
Treating anhydrous cobalt chloride with hydrogen fluoride gives cobalt(II) fluoride:[4]
- CoCl2 + 2 HF → CoF2 + 2 HCl
Tetrahydrated cobalt(II) fluoride is formed by dissolving cobalt(II) in hydrofluoric acid. The anhydrous fluoride can be extracted from this by dehydration. Other synthesis can occur at higher temperatures.[5]
Reactions
Cobalt(II) fluoride reacts with fluorine to give cobalt(III) fluoride:
- CoF2 + 0.5 F2 → CoF3
The latter is a catalyst for fluorination reactions.
References
- ^ PubChem. "Cobalt difluoride". pubchem.ncbi.nlm.nih.gov. Retrieved 2026-03-11.
- ^ Donaldson, John Dallas; Beyersmann, Detmar (2005). "Cobalt and Cobalt Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Vol. 52. pp. 363–472. doi:10.1002/14356007.a07_281.pub2. ISBN 978-3-527-30385-4. PMC 7682369. PMID 1960848.
- ^ 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.
- ^ W. Kwasnik; R. Sauer (1963). "Cobalt(II) Fluoride". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY,NY: Academic Press. p. 267.
- ^ J.C. Bailar (1973), Comprehensive Inorganic Chemistry, Pergoamon
External links
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