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In $\ce{KMnO4}$, the Oxidation state of $\ce{Mn}$ is +7, which results in an electronic configuration as $\ce{[Ar] 4s^0 3d^0}$

In $\ce{K2Cr2O7}$,the Oxidation state of $\ce{Cr}$ is +6, which results in an electronic configuration as $\ce{[Ar] 4s^0 3d^0}$

As it is clearly visible there are no $\ce{d}$ electrons in either of these compounds but still, they are coloured.

My Doubt:

  1. If there's no $\ce{d-d}$ transition in these compounds what gives these compounds their colour?

  2. Are there other transition element compounds whose colour is not because of $\ce{d-d}$ transition?

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marked as duplicate by pentavalentcarbon, Nilay Ghosh, M.A.R. ಠ_ಠ, Todd Minehardt, Mithoron Mar 6 '18 at 14:48

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