The yellow colour of chromate ion and orange | vedclass

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Question

(B) In both chromate $(CrO_4^{2-})$ and dichromate $(Cr_2O_7^{2-})$ ions,$Cr$ is present in $+6$ oxidation state,which corresponds to a $d^0$ electron

Vedclass · Accepted Answer

charge transfer only

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(B) In both chromate $(CrO_4^{2-})$ and dichromate $(Cr_2O_7^{2-})$ ions,$Cr$ is present in $+6$ oxidation state,which corresponds to a $d^0$ electronic configuration.Since there are no electrons in the $d$-orbitals,$d-d$ transitions are impossible.The intense colours (yellow for $CrO_4^{2-}$ and orange for $Cr_2O_7^{2-}$) arise due to ligand-to-metal charge transfer $(LMCT)$,where electrons from oxygen are transferred to the vacant $d$-orbitals of $Cr(VI)$.

List-$I$ (Element)	List-$II$ (Block)
$A$. $Cd$	$I$. $f$-block
$B$. $Eu$	$II$. $s$-block
$C$. $Se$	$III$. $d$-block
$D$. $Ba$	$IV$. $p$-block

The yellow colour of chromate ion and orange colour of dichromate ion is due to

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Match the following:
List-$I$ (Element) List-$II$ (Block)
$A$. $Cd$ $I$. $f$-block
$B$. $Eu$ $II$. $s$-block
$C$. $Se$ $III$. $d$-block
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