Question
Copper(I) compounds are white and are dimagnetic. While copper(II) compounds are coloured and paramagnetic, explain.
✓
Answer
The electronic configuration of $Cu ^{+}( Z =28)$ is $1 s^2, 2 s^2 2 p^6, 3 s^2 3 p^6 3 d^{10}$, i.e., all orbitals are completely filled so it is dimagnetic in nature and form white compounds. The electronic configuration of $Cu ^{2+}( Z =27)$ is $1 s^2, 2 s^2 2 p^6, 3 s^2 3 p^6 3 p^9$ so it has 1 unpaired electron. Hence it is paramagnetic in nature and form coloured compounds.
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