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Copper has an electronic configuration of [Ar] 3d10 4s1

Copper is a transition metal and the simple concept of valence electrons is difficult to apply to these. You could say 1, expecting the 4s electron to be lost, which does happen to form Cu+ , cuprous, compounds. However copper readily forms Cu2+ in cupric compounds, e.g. in copper sulfate. In these one of the d electrons is also lost to give a d9 configuration.

Other oxidation states such as copper (III) and copper(IV) are known.

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