Tetrakis(acetonitrile)copper(I) hexafluorophosphate
copper(I)_hexafluorophosphate.png) | |
copper(I)_hexafluorophosphate_3D_spacefill.png) | |
| Names | |
|---|---|
| IUPAC name
Tetrakis(acetonitrile)copper(I) hexafluorophosphate | |
| Identifiers | |
64443-05-6  | |
| Properties | |
| [Cu(CH3CN)4]PF6 | |
| Molar mass | 372.7198 g/mol |
| Appearance | White powder |
| Melting point | 160 °C (320 °F; 433 K) |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
verify (what is  ?) | |
| Infobox references | |
Tetrakis(acetonitrile)copper(I) hexafluorophosphate is a coordination compound with the formula [Cu(CH3CN)4]PF6. It is a colourless solid that is used in the synthesis of copper complexes.[1]
Structure
As confirmed by X-ray crystallographic studies, copper(I) ion is coordinated to four almost linear acetonitrile ligands in a nearly ideal tetrahedral geometry.[2] Related complexes are known with other anions including the perchlorate, tetrafluoroborate, and nitrate. With the weakly coordinating anion B(C6F5)4−, salts of [Cu(CH3CN)2]+ are obtained.[1]
The acetonitrile ligands protect the Cu+ ion from oxidation to Cu2+. However, acetonitrile is not bound very strongly to the copper ion, thus the complex is a useful source of Cu(I).
Synthesis
The cation was first reported in 1923 with a nitrate anion as a byproduct of the reduction of silver nitrate with a suspension of copper powder in acetonitrile.[3] [Cu(CH3CN)4]PF6 is generally produced by the addition of HPF6 to a suspension of copper(I) oxide in acetonitrile:[4]
- Cu2O + 2 HPF6 + 8 CH3CN → 2 [Cu(CH3CN)4]PF6 + H2O
The reaction is highly exothermic, and may bring the solution to a boil. Upon crystallization, the resulting microcrystals should be white, though a blue tinge is common, indicating the presence of a Cu2+ species.[4]
Reactions and applications
As the coordinated acetonitrile ligands may be displaced in other solvents, the [Cu(CH3CN)4]PF6 compound may serve as a precursor in the non-aqueous syntheses of other Cu(I) compounds.[4]
Water-immiscible organic nitriles have been shown to selectively extract Cu2+ from aqueous chloride solutions.[5] Through this method, copper can be separated from a mixture of other metals. Dilution of acetonitrile solutions with water induces disproportionation:
- 2 [Cu(CH3CN)4]+ + 6 H2O → [Cu(H2O)6]2+ + Cu + 8 CH3CN
References
- 1 2 Silvana F. Rach, Fritz E. Kühn "Nitrile Ligated Transition Metal Complexes with Weakly Coordinating Counteranions and Their Catalytic Applications" Chem. Rev., 2009, volume 109, pp 2061–2080. doi:10.1021/cr800270h
- ↑ Kierkegaard C.P.; Norrestam R. (1975). "Copper(I) tetraacetonitrile perchlorate". Acta Crystallogr. B 31: 314–317. doi:10.1107/S0567740875002634.J. R. Black, W. Levason and M. Webster "Tetrakis(acetonitrile-N)copper(I) Hexafluorophosphate(V) Acetonitrile Solvate"Acta Crystallogr. (1995). C51, pp. 623-625. doi:10.1107/S0108270194012527
- ↑ Morgan, H.H.; Sand, Henry Julics Salomon (1923). "Preparation and Stability of Cuprous Nitrate and Other Cuprous Salts in the Presence of Nitriles". J. Chem. Soc. 19: 2901. doi:10.1039/CT9232302891.
- 1 2 3 Kubas, G.J. (1990). "Tetrakis(acetonitirile)copper(I) Hexaflurorophosphate". Inorganic Syntheses 19: 90–91. doi:10.1002/9780470132593.ch15.
- ↑ Preston, J.S.; Muhr D.M; Parker A.J. (1980). "Cuprous hydrometallurgy: Part VIII. Solvent extraction and recovery of copper(I) chloride with organic nitriles from an iron(III), copper(II) chloride, two-step oxidative leach of chalcopyrite concentrate". Hydrometallurgy 5: 227. doi:10.1016/0304-386X(80)90041-9.