Which of the following electronic configurati | vedclass

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(C) Ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge.However,stability of ele

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$[Ne]\, 3s^2\, 3p^5$

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(C) Ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge.However,stability of electronic configurations plays a significant role.Option $A$ $([Ne]\, 3s^2\, 3p^3)$ represents a half-filled $p$-orbital,which is exceptionally stable.Option $D$ $([Ne]\, 3s^2)$ represents a fully-filled $s$-orbital,which is also stable,but it belongs to a lower group $(Group\, 2)$ compared to the $p$-block elements.Comparing elements in the same period $(Period\, 3)$: $3s^2$ (Magnesium),$3s^2\, 3p^3$ (Phosphorus),$3s^2\, 3p^4$ (Sulfur),and $3s^2\, 3p^5$ (Chlorine).Chlorine $(3s^2\, 3p^5)$ has the highest effective nuclear charge among these,making it the most difficult to remove an electron from.Therefore,$[Ne]\, 3s^2\, 3p^5$ has the highest ionization enthalpy.

Which of the following electronic configurations has the highest ionization enthalpy?

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