Which of the following elements has the lowes | vedclass

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(B) The ionisation potential generally increases across a period from left to right due to an increase in effective nuclear charge and a decrease in a

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$O$

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(B) The ionisation potential generally increases across a period from left to right due to an increase in effective nuclear charge and a decrease in atomic size. All the given elements ($N$,$O$,$F$,$Ne$) belong to the $2^{nd}$ period. However,we must consider the electronic configurations: $N (1s^2 2s^2 2p^3)$ has a stable half-filled $p$-orbital. $O (1s^2 2s^2 2p^4)$ has a lower ionisation potential than $N$ due to inter-electronic repulsion. $F (1s^2 2s^2 2p^5)$ has a higher ionisation potential than $O$. $Ne (1s^2 2s^2 2p^6)$ has the highest ionisation potential due to a stable noble gas configuration. Comparing these,$O$ has the lowest ionisation potential among the given options.

Element	$IE_1 + IE_2$ $(kJ/mol)$	$IE_3 + IE_4$ $(kJ/mol)$
$P$	$2.45$	$8.82$
$Q$	$2.85$	$6.11$

Which of the following elements has the lowest ionisation potential?

Similar Questions

Which of the following elements has the lowest $IE_1$ value?

The sum of $IE_1 + IE_2$ and $IE_3 + IE_4$ for elements $P$ and $Q$ are given below:

Element $IE_1 + IE_2$ $(kJ/mol)$ $IE_3 + IE_4$ $(kJ/mol)$

$P$ $2.45$ $8.82$

$Q$ $2.85$ $6.11$

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