Which of the following compounds is colored?

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(A) In $CuF_2$,the copper ion is in the $+2$ oxidation state $(Cu^{2+})$. The electronic configuration of $Cu^{2+}$ is $[Ar] 3d^9$. Due to the presenc

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$CuF_2$

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(A) In $CuF_2$,the copper ion is in the $+2$ oxidation state $(Cu^{2+})$. The electronic configuration of $Cu^{2+}$ is $[Ar] 3d^9$. Due to the presence of an unpaired electron in the $d$-orbital,$d-d$ transitions are possible,which makes the compound colored.In $CuI$,copper is in the $+1$ oxidation state $(Cu^+)$,which has a $3d^{10}$ configuration (no unpaired electrons).$NaCl$ and $H_2O$ do not contain transition metal ions with partially filled $d$-orbitals,so they are colorless.

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