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(B) The correct answer is $B$. $1$. The ionisation potential of $N$ $(2s^2 2p^3)$ is greater than $O$ $(2s^2 2p^4)$ due to the stable half-filled $p$-

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The electron affinity of fluorine is greater than that of chlorine

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(B) The correct answer is $B$. $1$. The ionisation potential of $N$ $(2s^2 2p^3)$ is greater than $O$ $(2s^2 2p^4)$ due to the stable half-filled $p$-orbital configuration. $2$. The electron affinity of $F$ is lower than that of $Cl$ because the small size of $F$ leads to strong inter-electronic repulsions,making it harder to add an electron compared to $Cl$. $3$. The ionisation potential of $Be$ $(2s^2)$ is greater than $B$ $(2s^2 2p^1)$ due to the stable fully-filled $s$-orbital. $4$. The electronegativity of $F$ is greater than $Cl$ due to its smaller atomic size.

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

Which one of the following is an incorrect statement?

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The change in enthalpy $[\Delta H]$ in $kJ\ mol^{-1}$ for the reaction is $Mg + 2F \rightarrow MgF_2$. Given: $EA$ of $F = 328\ kJ\ mol^{-1}$,$IE_1$ of $Mg = 737\ kJ\ mol^{-1}$,$IE_2$ of $Mg = 1451\ kJ\ mol^{-1}$.

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