Copper(II) trifluoroacetate
| Names | |
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| IUPAC name
copper;2,2,2-trifluoroacetate
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| (CF3COO)2Cu | |
| Molar mass | 289.576 g·mol−1 |
| Appearance | |
| soluble[3] | |
| Hazards | |
| GHS labelling:[4] | |
| Warning | |
| H315, H319 | |
| P264, P280, P302+P352, P305+P351+P338, P321, P332+P313, P337+P313, P337+P317, P362+P364 | |
| NFPA 704 (fire diamond) | |
| NIOSH (US health exposure limits):[6] | |
REL (Recommended)
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1 mg/m3 (TWA, as Copper) |
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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Copper(II) trifluoroacetate is the trifluoroacetate of divalent copper with the chemical formula Cu(CF3COO)2.
Properties
It exists as the anhydride, hydrate and adducts of other solvents. The hydrate begins to lose two waters of crystallisation at 108 °C (226 °F), and loses all crystal water at 173 °C (343 °F) to form the anhydrous form. This begins to decompose at 220 °C (428 °F).
Preparation
Copper trifluoroacetate can be obtained by reacting trifluoroacetic acid with copper oxide, copper hydroxide or basic copper carbonate. Acetone can replace the water molecules in copper trifluoroacetate hydrate, and under reduced pressure conditions, the acetone can be removed to obtain anhydrous material.[1]
Use
Copper trifluoroacetate finds some use as a reagent in organic chemistry.[7] For example, it mediates the C–H bond arylation of arenes with arylboronic acids and is used in the arylation of indoles with triphenylbismuth bis-trifluoroacetate.[7] It is also a catalyst for the aerobic oxidation of ethers.[7]
Adducts
Copper trifluoroacetate forms adducts with a variety of Lewis bases, such as ammonia, water, dioxane, and quinoline. The Lewis bases bind to the axial positions.[8][9]
References
- ^ a b Cotton, F.A.; Dikarev, E.V.; Petrukhina, M.A. (2000). "Syntheses and crystal structures of "unligated" copper(I) and copper(II) trifluoroacetates". Inorganic Chemistry. 39: 6072-6079. doi:10.1021/ic000663h.
- ^ Karpova, Elena V.; Boltalin, Alexander I.; Zakharov, Maxim A.; Sorokina, Nataliya I.; Korenev, Yuri M.; Troyanov, Sergei I. (Apr 1998). <741::aid-zaac741>3.0.co;2-4 "Synthesis and Crystal Structure of Copper(II) Trifluoroacetates, Cu2(CF3COO)4 · 2 CH3CN and Cu(CF3COO)2(H2O)4". Zeitschrift für anorganische und allgemeine Chemie. 624 (4): 741–744. doi:10.1002/(sici)1521-3749(199804)624:4<741::aid-zaac741>3.0.co;2-4. ISSN 0044-2313.
- ^ Baillie, M. J.; Brown, D. H.; Moss, K. C.; Sharp, D. W. A. (1968). "Anhydrous metal trifluoroacetates". Journal of the Chemical Society A: Inorganic, Physical, Theoretical: 3110–14. doi:10.1039/j19680003110.
- ^ "COPPER(II) TRIFLUOROACETATE, hydrate - Safety Data Sheet" (PDF). gelest.com. Gelest. 13 January 2016. CXCU080. Retrieved 16 November 2025.
- ^ "SDS - Copper(II) trifluoroacetate hydrate". fisherschi.com. ThermoFisher Scientific. 31 March 2024. Retrieved 17 November 2025.
- ^ "NIOSH Pocket Guide to Chemical Hazards".
- ^ a b c Ollevier, Thierry (2001-04-15), "Copper(II) Trifluoroacetate", Encyclopedia of Reagents for Organic Synthesis, Chichester, UK: John Wiley & Sons, Ltd, p. 1, doi:10.1002/047084289x.rn01852, ISBN 978-0-470-84289-8
- ^ Calvo, V.; Corteés, P.; Moreno, Y.; Vegas, A.; Spodine, E. (2000). "Influence of Hydrogen Bridges on the Magnetic Properties of Copper(II) Bis(trifluoroacetate) Complexes". Bol. Soc. Chil. Quím. 45. doi:10.4067/S0366-16442000000200013. hdl:10533/240302.
- ^ Moreland, James A.; Doedens, Robert J. (Feb 1975). "Synthesis, crystal structure, and magnetic properties of a dimeric quinoline adduct of copper(II) trifluoroacetate". Journal of the American Chemical Society. 97 (3): 508–513. doi:10.1021/ja00836a007. ISSN 0002-7863.