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(D) $(I)$ Incorrect: $Li^+$ has the smallest size among alkali metals,so it gets most extensively hydrated. The hydrated radius is $Li^+ > Na^+ > K^+

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$(II)$ and $(III)$

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(D) $(I)$ Incorrect: $Li^+$ has the smallest size among alkali metals,so it gets most extensively hydrated. The hydrated radius is $Li^+ > Na^+ > K^+ > Rb^+ > Cs^+$. Larger hydrated ions have lower ionic mobility. Thus,the ionic mobility of hydrated $Li^+$ is less than that of hydrated $Na^+$.$(II)$ Correct: $P$ $(3s^2 3p^3)$ has a stable half-filled $p$-orbital,making its $IE_1$ higher than $S$ $(3s^2 3p^4)$. For $IE_2$,$P^+$ $(3s^2 3p^2)$ and $S^+$ $(3s^2 3p^3)$. $S^+$ has a half-filled $p$-orbital,making its $IE_2$ higher than $P^+$.$(III)$ Correct: Lithium has the highest negative standard electrode potential $(E^\circ = -3.04 \ V)$ due to its very high hydration energy,making it the strongest reducing agent in aqueous solution.

Element Description	Element	$\Delta_{i}H_1$	$\Delta_{i}H_2$	$\Delta_{eg}H$
$(i)$ Most reactive non-metal	$(A)$	$419$	$3051$	$-48$
$(ii)$ Most reactive metal	$(B)$	$1681$	$3374$	$-328$
$(iii)$ Least reactive element	$(C)$	$738$	$1451$	$-40$
$(iv)$ Metal forming dihalide	$(D)$	$2372$	$5251$	$+48$

List-$I$	List-$II$
$A$. $Al^{3+} < Mg^{2+} < Na^{+} < F^{-}$	$I$. Ionisation Enthalpy
$B$. $B < C < O < N$	$II$. Metallic character
$C$. $B < Al < Mg < K$	$III$. Electronegativity
$D$. $Si < P < S < Cl$	$IV$. Ionic radii

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