# Question #26e09

Jan 20, 2015

I'll assume you are referring to the charges on the ions which they form.

Zinc has the electron structure $\left[A r\right] 4 {s}^{2}$

This means the principal oxidation states are 0 and +2.
$Z {n}^{2 +}$ is quite stable in aqueous conditions.

Copper has the electron structure $\left[A r\right] 3 {d}^{10} 4 {s}^{1}$. The principal oxidation states are 0, +1 and +2

In aqueous conditions copper(I) is relatively unstable and it undergoes disproportionation to copper(II):

$2 C {u}^{+} \rightarrow C u + C {u}^{2 +}$