Explain why the stability of oxoacids of chlorine increases in the order given below:
$HClO < HClO_2 < HClO_3 < HClO_4$
$HClO < HClO_2 < HClO_3 < HClO_4$
(N/A) The stability and acidic strength of oxoacids depend on the oxidation state of the central atom and the dispersal of negative charge in the conjugate base.
$(i)$ As the number of oxygen atoms increases,the oxidation state of chlorine increases ($+1, +3, +5, +7$ respectively).
$(ii)$ The conjugate base formed,such as $ClO_4^-$,has the negative charge delocalized over four oxygen atoms due to resonance,making it the most stable.
$(iii)$ In $HClO_4$,the high oxidation state of chlorine and the effective dispersal of negative charge in the $ClO_4^-$ ion make it the most stable and strongest acid,whereas $HClO$ is the least stable.
$(i)$ As the number of oxygen atoms increases,the oxidation state of chlorine increases ($+1, +3, +5, +7$ respectively).
$(ii)$ The conjugate base formed,such as $ClO_4^-$,has the negative charge delocalized over four oxygen atoms due to resonance,making it the most stable.
$(iii)$ In $HClO_4$,the high oxidation state of chlorine and the effective dispersal of negative charge in the $ClO_4^-$ ion make it the most stable and strongest acid,whereas $HClO$ is the least stable.
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