$X$,$Y$,and $Z$ are elements of the same period and belong to the $p$-block. $Y$ has a positive value of $\Delta_{eg}H$ (electron gain enthalpy),and $Z$ has the highest $2^{nd}$ ionization energy $(I.E.)$ among them. What is the correct order of their atomic numbers?
$(a)$ $X < Y < Z$
$(b)$ $X < Z < Y$
$(c)$ $Y < Z < X$
$(d)$ $Z < Y < X$

Which of the following statement$(s)$ is/are incorrect?

Match the items in List-$I$ with the items in List-$II$:

List-$I$	List-$II$
$(A)$ Rubidium	$(1)$ Germanium
$(B)$ Platinum	$(2)$ Radioactive chalcogen
$(C)$ Eka-silicon	$(3)$ $s$-block element
$(D)$ Polonium	$(4)$ Atomic number $78$

State whether the following statements are true or false:
$(i)$ As the atomic number increases in a period,the nuclear charge increases,therefore the ionization enthalpy increases.
$(ii)$ As the metallic character of elements increases,the atomic radius generally increases.
$(iii)$ $Mn$ $(Z = 25)$ is a transition element. Although it is a $3d$-orbital element,its position in the periodic table is in the $4^{th}$ period.

If the electronic configuration of $A^{-}$ is $[Ar] \ 4s^2 \ 3d^{10} \ 4p^1$,then $A^{+2}$ will belong to which group and period?

To which block do the elements with the following outer electronic configurations belong?
$(i)$ $6s^2 4f^3$
$(ii)$ $3s^2 3p^4$
$(iii)$ $3s^1$
$(iv)$ $3d^2 4s^2$