Arrange the following oxides in the correct o | vedclass

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(B) The acidic character of oxides of group $15$ elements depends on the oxidation state of the central atom and its electronegativity.$1$. Higher oxi

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$III > I > II > IV$

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(B) The acidic character of oxides of group $15$ elements depends on the oxidation state of the central atom and its electronegativity.$1$. Higher oxidation state leads to higher acidic character. $N_2O_5$ $(III)$ has $N$ in $+5$ oxidation state,while $N_2O_3$ $(I)$,$P_2O_3$ $(II)$,and $As_2O_3$ $(IV)$ have the central atom in $+3$ oxidation state.$2$. Among oxides with the same oxidation state $(+3)$,the acidic character decreases down the group as electronegativity decreases and atomic size increases.$3$. Comparing the $+3$ oxides: $N_2O_3 > P_2O_3 > As_2O_3$ $(I > II > IV)$.$4$. Combining these,the overall order is $N_2O_5 > N_2O_3 > P_2O_3 > As_2O_3$,which corresponds to $III > I > II > IV$.

Arrange the following oxides in the correct order of their acidic character:
$N_2O_3$ $(I)$,$P_2O_3$ $(II)$,$N_2O_5$ $(III)$,$As_2O_3$ $(IV)$

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Arrange the following oxides in the correct order of their acidic character:$N_2O_3$ $(I)$,$P_2O_3$ $(II)$,$N_2O_5$ $(III)$,$As_2O_3$ $(IV)$