(a) Be and Mg are alkaline earth metals.(b) K | vedclass

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$(B)$ $Be$ and $Mg$ belong to Group $2$, which are alkaline earth metals. This statement is correct.$(b)$ $K^{+}$ ($18$ electrons) and $Ca^{2+}$ ($18$

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$b$ and $c$

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$(B)$ $Be$ and $Mg$ belong to Group $2$, which are alkaline earth metals. This statement is correct.$(b)$ $K^{+}$ ($18$ electrons) and $Ca^{2+}$ ($18$ electrons) are isoelectronic. For isoelectronic species, the ionic radius decreases as the nuclear charge $(Z)$ increases. Since $Z$ of $Ca$ $(20)$ is greater than $K$ $(19)$, $Ca^{2+}$ has a smaller radius than $K^{+}$. Thus, $K^{+}$ has a larger radius than $Ca^{2+}$. This statement is correct.$(c)$ Transition elements are defined as elements having partially filled $d$-orbitals in their ground state or any common oxidation state. Elements like $Zn$, $Cd$, and $Hg$ have fully filled $d^{10}$ configurations and are not considered transition elements, even though they are $d$-block elements. This statement is incorrect.$(d)$ The ionic radius of $H^{-}$ is approximately $208 \ pm$, while the ionic radius of $F^{-}$ is approximately $133 \ pm$. Thus, $H^{-}$ is larger than $F^{-}$. This statement is correct.Therefore, only statement $(c)$ is incorrect.

Element	$IE_1$	$IE_2$	$IE_3$	$IE_4$
$W$	$10.5$	$15.5$	$24.9$	$79.8$
$X$	$8$	$14.8$	$78.9$	$105.8$

$(a)$ $Be$ and $Mg$ are alkaline earth metals.
$(b)$ $K^{+}$ has larger radii than $Ca^{2+}$.
$(c)$ All $d$-block elements are transition elements.
$(d)$ $H^{-}$ ion is larger than $F^{-}$.
Incorrect statement is/are

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$(a)$ $Be$ and $Mg$ are alkaline earth metals.$(b)$ $K^{+}$ has larger radii than $Ca^{2+}$.$(c)$ All $d$-block elements are transition elements.$(d)$ $H^{-}$ ion is larger than $F^{-}$.Incorrect statement is/are