Which of the following electronic configurati | vedclass

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(B) The first ionization enthalpy depends on the stability of the electronic configuration and the effective nuclear charge. $ns^2 np^6$ represents a

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$ns^2 np^4$

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(B) The first ionization enthalpy depends on the stability of the electronic configuration and the effective nuclear charge. $ns^2 np^6$ represents a noble gas configuration,which is highly stable and has the highest ionization enthalpy. $ns^2 np^3$ represents a half-filled p-orbital,which is also extra stable. Comparing $ns^2 np^4$ and $ns^2 np^5$,the $ns^2 np^4$ configuration has a lower effective nuclear charge and less stability compared to the half-filled or fully-filled states,making it easier to remove an electron compared to the others listed in the context of periodic trends. However,among the given options,$ns^2 np^4$ has the lowest ionization energy because it is neither half-filled nor fully-filled,and it is further to the left in the period compared to $ns^2 np^5$ and $ns^2 np^6$.

Which of the following electronic configurations represents the atom with the lowest first ionization enthalpy?

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