Compounds having the highest oxidation state | vedclass

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(D) The oxidation states of chlorine in the given compounds are: $1$. In $HOCl$,$O.S. = +1$ $2$. In $HClO_2$,$O.S. = +3$ $3$. In $HClO_4$,$O.S. = +7$

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(D) The oxidation states of chlorine in the given compounds are: $1$. In $HOCl$,$O.S. = +1$ $2$. In $HClO_2$,$O.S. = +3$ $3$. In $HClO_4$,$O.S. = +7$ For chlorine oxyacids,the acidic strength increases with the increase in oxidation state. $HClO_4$ $(+7)$ is a strong acid,$HClO_2$ $(+3)$ is an intermediate acid,and $HOCl$ $(+1)$ is the weakest acid. None of these act as amphoteric in the context of these specific oxyacids,as they all primarily exhibit acidic character.

Column-$I$	Column-$II$
$A$. Positively charged ion	$1$. $+7$
$B$. Oxidation number of all neutral atoms	$2$. $-1$
$C$. Oxidation number of hydrogen $(H^+)$	$3$. $+1$
$D$. Oxidation number of fluorine in $NaF$	$4$. $0$
$E$. Negatively charged ion	$5$. Cation
	$6$. Anion

Compounds having the highest oxidation state of the central atom act as acids,the lowest ones act as bases,and intermediate oxidation states act as amphoteric. Which one of the following is amphoteric?

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