Chemistry:Chromium trifluoride
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| Names | |
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| IUPAC name
Chromium(III) fluoride
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| Other names
Chromium trifluoride
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| Identifiers | |
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3D model (JSmol)
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PubChem CID
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| Properties | |
| CrF3 | |
| Molar mass | 108.9913 g/mol (anhydrous) 163.037 g/mol (trihydrate) 181.05 g/mol (tetrahydrate) |
| Appearance | green crystalline solid |
| Density | 3.8 g/cm3 (anhydrous) 2.2 g/cm3 (trihydrate) |
| Melting point | 1,100 °C (2,010 °F; 1,370 K) (sublimes) |
| negligible (anhydrous) sparingly soluble (trihydrate) | |
| Solubility | insoluble in alcohols soluble in HF, HCl |
| +4370.0·10−6 cm3/mol | |
| Structure | |
| Rhombohedral, hR24 | |
| R-3c, No. 167 | |
| Hazards | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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150 mg/kg (guinea pig, oral)[2] |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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TWA 1 mg/m3[1] |
REL (Recommended)
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TWA 0.5 mg/m3[1] |
IDLH (Immediate danger)
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250 mg/m3[1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Chromium(III) fluoride is the name for the inorganic compounds with the chemical formula CrF3 as well as several related hydrates. The compound CrF3 is a green crystalline solid that is insoluble in common solvents, but the coloured hydrates [Cr(H2O)6]F3 and [Cr(H2O)6]F3•3H2O are soluble in water. The trihydrate is green, and the hexahydrate is violet. The anhydrous form sublimes at 1100–1200 °C.[3]
Structures
Like almost all compounds of chromium(III), these compounds feature octahedral Cr centres. In the anhydrous form, the six coordination sites are occupied by fluoride ligands that bridge to adjacent Cr centres. In the hydrates, some or all of the fluoride ligands are replaced by water.[4]
Production
Chromium(III) fluoride is produced from the reaction of chromium(III) oxide and hydrofluoric acid:[5]
- Cr2O3 + 6 HF + 9 H2O → 2 [Cr(H2O)6]F3
The anhydrous form is produced from hydrogen fluoride and chromic chloride:[6]
- CrCl3 + 3 HF → CrF3 + 3 HCl
Another method of synthesis of CrF3 involves thermal decomposition of (NH3)CrF6: (NH4)3CrF6 → CrF3 + 3NH3 + 3HF A mixed valence Cr2F5 is also known.[7]
Uses
Chromium(III) fluoride finds some applications as a mordant in textiles and as a corrosion inhibitor. Chromium(III) fluoride catalyzes the fluorination of chlorocarbons by HF.[8] [9]
References
- ↑ 1.0 1.1 1.2 NIOSH Pocket Guide to Chemical Hazards. "#0141". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0141.html.
- ↑ "Chromium(III) compounds [as Cr(III)"]. Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/cr3m3.html.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ F.H. Herbstein, M. Kapon and G.M. Reisner, "Crystal structures of chromium(III) fluoride trihydrate. Structural chemistry of hydrated transition metal fluorides. Thermal decomposition of chromium(III) fluoride nonhydrate" Zeitschrift für Kristallographie 1985, volume 171, pp. 209
- ↑ Gerd Anger, Jost Halstenberg, Klaus Hochgeschwender, Christoph Scherhag, Ulrich Korallus, Herbert Knopf, Peter Schmidt, Manfred Ohlinger, "Chromium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.doi:10.1002/14356007.a07_067
- ↑ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN:0-7506-3365-4.
- ↑ Sturm. B.J. Phase Equilibria in the System Chromium(II)Fluoride-Chromium(III) Fluoride. Inorg. Chem., 1962, 1 (3), pp 665–672
- ↑ Mallikarjuna R. V. N.; Subramanian M. A. Fluoroolefin Manufacturing U.S. Patent 6,031,14, August 6, 1998; n.a.
- ↑ Ruh R. P.; Davis R. A. Proceess for Fluorinating Aliphatic Halohydrocarbons with a Chromium Fluoride catalyst and process for preparing the catalyst. U.S. Patent 2,745,886, May 15, 1956; n.a.
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