In which of the following compounds would the | vedclass

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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.

Metal ion	Colour
$A. V^{4+}$	$I. Colourless$
$B. Ti^{3+}$	$II. Purple$
$C. Ti^{4+}$	$III. Green$
$D. Ni^{2+}$	$IV. Blue$
	$V. Yellow$

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

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Match the following metal ions with their respective colours:
Metal ion Colour
$A. V^{4+}$ $I. Colourless$
$B. Ti^{3+}$ $II. Purple$
$C. Ti^{4+}$ $III. Green$
$D. Ni^{2+}$ $IV. Blue$
$V. Yellow$

In chromyl chloride,the number of $d$-electrons present on chromium is same as in (Given atomic number of $Ti = 22, V = 23, Cr = 24, Mn = 25, Fe = 26$)

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