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In basic conditions copper typically forms a hydroxide precipitate (copper (II) is hexadentate and so is octadehral). Alkalis (such as NaOH) and dilute lewis bases (such as ammonia) will produce the precipitate. The net reaction could be summarised:

Cu(s) + 2OH-+ 4H2O → [Cu(H2O)4(OH)2](s)

The aqueous copper can ligate with lewis bases. Excess ammonia would produce the following reaction:

[Cu(H2O)4(OH)2](s) + 4NH3 → [Cu(NH3)4(H2O)2]2+(aq)+ 2OH- + 2H2O

In a similar way copper metal can react with carbonate ions to form CuCO3. Similar to the example of ammonia above, there are other lewis bases that can result in ligand exchange (chloride and Iodide are two such examples).

Note: The above examples all involve copper (II) / Cu2+. Copper (I) compounds do not readily form in solution as it will disproportinate to form Cu and Cu2+.

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