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	Ionization energy $1^{st}$ $(kJ/mol)$	Ionization energy $2^{nd}$ $(kJ/mol)$
$X$	$495$	$4563$
$Y$	$731$	$1450$

Which of the following elements has the lowest ionisation potential?

Similar Questions

Suppose a gaseous mixture of $He$, $Ne$, $Ar$ and $Kr$ is treated with photons of the frequency appropriate to ionize $Ar$. What ion$(s)$ will be present in the mixture?

Which is the correct order of ionisation energy?

Identify the elements $X$ and $Y$ using the ionisation energy values given below :

Element Ionization energy $1^{st}$ $(kJ/mol)$ Ionization energy $2^{nd}$ $(kJ/mol)$

$X$ $495$ $4563$

$Y$ $731$ $1450$

In the given graph,which point represents an alkali metal with the least atomic number (Period number $= 3$)?

Assertion $(A)$: $16$th group elements have higher ionisation enthalpy values than $15$th group elements in the corresponding periods.
Reason $(R)$: $15$th group elements have half-filled stable electronic configurations.

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