Compare the ionization enthalpy and electron gain enthalpy values of the elements given below:

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	$(D)$	$2372$	$5251$	$+48$

(A) $(i)$ The most reactive non-metal has a high negative electron gain enthalpy. Element $B$ has $\Delta_{eg}H = -328 \ kJ/mol$,which is the most negative.
$(ii)$ The most reactive metal has the lowest first ionization enthalpy $(\Delta_{i}H_1)$. Element $A$ has $\Delta_{i}H_1 = 419 \ kJ/mol$,which is the lowest.
$(iii)$ The least reactive element is a noble gas,which has very high ionization enthalpies and a positive electron gain enthalpy. Element $D$ has $\Delta_{i}H_1 = 2372 \ kJ/mol$ and $\Delta_{eg}H = +48 \ kJ/mol$.
$(iv)$ Metals forming dihalides are alkaline earth metals. Element $C$ has $\Delta_{i}H_1 = 738 \ kJ/mol$ and $\Delta_{i}H_2 = 1451 \ kJ/mol$,which is characteristic of group $2$ elements.