Copper(II) tetrafluoroborate
Jump to navigation
Jump to search
| Names | |
|---|---|
| IUPAC name
Copper(II) tetrafluoroborate
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
PubChem CID
|
|
| |
| |
| Properties | |
| Cu(BF4)2 | |
| Molar mass | 237.155 g/mol |
| Appearance | blue crystal |
| soluble in water | |
| Hazards | |
| US health exposure limits (NIOSH): | |
PEL (Permissible)
|
TWA 1 mg/m3 (as Cu)[2] |
REL (Recommended)
|
TWA 1 mg/m3 (as Cu)[2] |
IDLH (Immediate danger)
|
TWA 100 mg/m3 (as Cu)[2] |
| Related compounds | |
Other anions
|
Copper(II) chloride Copper(II) oxide Copper(II) triflate |
Other cations
|
Sodium tetrafluoroborate Lithium tetrafluoroborate Silver tetrafluoroborate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper(II) tetrafluoroborate is any inorganic compound with the formula Cu(H2O)x(BF4)2. As usually encountered, it is assumed to be the hexahydrate (x = 6), but this salt can be partially dehydrated to the tetrahydrate.[3] Regardless, these compounds are aquo complexes of copper in its +2 oxidation state, with two weakly coordinating tetrafluoroborate anions.
The compound is used in organic synthesis, e.g. as a Lewis acid for Diels Alder reactions and for cyclopropanation of alkenes with diazo reagents. In both applications, the copper(II) is reduced to a copper(I) catalyst.[3][4]
References[edit]
- ^ Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, Florida: CRC Press, pp. 4–56, ISBN 0-8493-0594-2
- ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ a b Ilhyong Ryu, Noboru Sonoda, "Copper(II) Tetrafluoroborate" Encyclopedia of Reagents for Organic Synthesis 2001, John Wiley & Sons. doi:10.1002/047084289X.rc249
- ^ Copper(II) Tetrafluorborate, chemicalland21.com
| This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |