Among the following,the coloured compound is:

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(C) In $CuCl$,$Cu$ is in the $+1$ oxidation state ($d^{10}$ configuration),which is colourless.In $K_3[Cu(CN)_4]$,$Cu$ is in the $+1$ oxidation state

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$CuF_2$

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(C) In $CuCl$,$Cu$ is in the $+1$ oxidation state ($d^{10}$ configuration),which is colourless.In $K_3[Cu(CN)_4]$,$Cu$ is in the $+1$ oxidation state ($d^{10}$ configuration),which is colourless.In $[Cu(CH_3CN)_4]BF_4$,$Cu$ is in the $+1$ oxidation state ($d^{10}$ configuration),which is colourless.In $CuF_2$,$Cu$ is in the $+2$ oxidation state ($d^9$ configuration). Due to the presence of an unpaired electron,$d-d$ transitions occur,making it blue-coloured.

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