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(A) The oxidation state of $Cr$ in the given compounds is as follows:$K_2CrO_4$: $Cr$ is in $+6$ oxidation state.$CrO_2$: $Cr$ is in $+4$ oxidation st

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$K_2CrO_4$

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(A) The oxidation state of $Cr$ in the given compounds is as follows:$K_2CrO_4$: $Cr$ is in $+6$ oxidation state.$CrO_2$: $Cr$ is in $+4$ oxidation state.$CrCl_3$: $Cr$ is in $+3$ oxidation state.$CrF_2$: $Cr$ is in $+2$ oxidation state.As the positive oxidation state of a metal ion increases,the effective nuclear charge increases and the ionic radius decreases.Therefore,$Cr$ in the $+6$ oxidation state $(K_2CrO_4)$ will have the smallest ionic radius.

In which of the following compounds would the ionic radius of chromium be the smallest?

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