Correct order of oxidising nature is

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(A) The oxidising nature of the trioxides of group $6$ elements depends on the stability of the lower oxidation states. As we move down the group from

Vedclass · Accepted Answer

$CrO_3 > MoO_3 > WO_3$

Vedclass · Answer

(A) The oxidising nature of the trioxides of group $6$ elements depends on the stability of the lower oxidation states. As we move down the group from $Cr$ to $W$,the stability of the $+6$ oxidation state increases,while the stability of lower oxidation states decreases. Therefore,$CrO_3$ is a strong oxidising agent because $Cr$ prefers to be in the $+3$ oxidation state. In contrast,$MoO_3$ and $WO_3$ are much less oxidising because $Mo$ and $W$ are more stable in the $+6$ oxidation state. The correct order of oxidising nature is $CrO_3 > MoO_3 > WO_3$.

Column-$I$	Column-$II$
$A$. $Pb_3O_4$	$I$. Neutral oxide
$B$. $N_2O$	$II$. Acidic oxide
$C$. $Mn_2O_7$	$III$. Basic oxide
$D$. $Bi_2O_3$	$IV$. Mixed oxide

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Match the formulas given in Column-$I$ with the type of oxide given in Column-$II$ and select the correct option:-

Column-$I$ Column-$II$

$A$. $Pb_3O_4$ $I$. Neutral oxide

$B$. $N_2O$ $II$. Acidic oxide

$C$. $Mn_2O_7$ $III$. Basic oxide

$D$. $Bi_2O_3$ $IV$. Mixed oxide

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The electronic configuration of $Cu(II)$ is $3d^9$ whereas that of $Cu(I)$ is $3d^{10}$. Which of the following is correct?

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