Copper(II) trifluoroacetate is the
trifluoroacetate of divalent
copper with the chemical formula Cu(CF3COO)2. It exists as the anhydride, hydrate and adducts of other solvents. The hydrate begins to lose two waters of crystallisation at 108 °C, and loses all crystal water at 173 °C to form the anhydrous form. This begins to decompose at 220 °C. It finds some use as a reagent in
organic chemistry.[6]
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]
Adducts
Copper trifluoroacetate forms adducts with a variety of Lewis bases, such as
ammonia,
water,
dioxane,[7], and
quinoline.[8] The Lewis bases bind to the axial positions.
References
^
abCotton FA , Dikarev EV , Petrukhina MA (2000). "Syntheses and crystal structures of "unligated" copper(I) and copper(II) trifluoroacetates". Inorganic Chemistry. 39: 6072-6079.
doi:
10.1021/ic000663h.{{
cite journal}}: CS1 maint: multiple names: authors list (
link)
^Elena V. Karpova, Alexander I. Boltalin, Maxim A. Zakharov, et al. Synthesis and Crystal Structure of Copper(II) Trifluoroacetates, Cu2(CF3COO)4 · 2 CH3CN and Cu(CF3COO)2(H2O)4. ZAAC, 1998. 624(4): 741-744
^MJ Baillie, DH Brown, KC Moss. Anhydrous metal trifluoroacetates. Journal of the Chemical Society A Inorganic Physical Theoretical, 1968: 3110-3114. DOI: 10.1039/j19680003110
^V. Calvo, P. Corteés, Y. Moreno, A. Vegas, E. Spodine (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.{{
cite journal}}: CS1 maint: multiple names: authors list (
link)