Is the electric conductivity of chlorine ions influenced by its oxidation state? I'm a high school student researching the conductivity of electrolyte solutions. In this excerpt of the CRC Handbook, I noticed that different ions containing chlorine have different limiting molar conductivity, and there seems to be a trend between molar conductivity and the oxidation state of chlorine:




Ion
Oxidation state of chlorine
$\Lambda$ in $\pu{e-4 m2 S mol-1}$




$\ce{ClO2-}$
+3
52


$\ce{ClO3-}$
+5
64.6


$\ce{ClO4-}$
+7
67.3




Does the trend really exist? If so, why did it happen? I found previous researches on the conductivity of $\ce{Fe^2+}$ and $\ce{Fe^3+}$, and the difference seemed to be a result of electrons spinning.
It is the similar effect as for molar conductivity of cations of alkali metals, which grows from $\ce{Li+}$ toward $\ce{Cs+}$, in spite of increasing ionic radius.
The point is, the effective radius of the hydrated ions has the opposite trend as the &quot;naked&quot; ion radius trend. $\ce{Li+}$ ion with the smallest radius has the strongest electrostatic field and the largest hydration sphere and has therefore the lowest molar conductivity.
The similar effect I expect for chlorine oxyacid anions. In this case, there is also decreasing degree of delocalization of the negative charge in trend $\ce{ClO4-} \gt \ce{ClO3-} \gt \ce{ClO2-}$.