Given below are two statements:Statement (I): | vedclass

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(D) Statement $(I)$: The first ionisation enthalpy generally increases across a period from left to right. The correct order for these elements is $Ar

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Statement $I$ is false but Statement $II$ is true

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(D) Statement $(I)$: The first ionisation enthalpy generally increases across a period from left to right. The correct order for these elements is $Ar > Cl > Mg > Na$. Therefore, the given order $Na > Mg > Cl > Ar$ is incorrect. Thus, Statement $(I)$ is false.Statement $(II)$: The electronic configuration of $Ca$ $(Z=20)$ is $[Ar] 4s^2$. The first two electrons are removed from the $4s$ orbital. The third electron must be removed from the $3p^6$ orbital, which is a stable noble gas configuration (Argon core). Removing an electron from a stable, fully-filled shell requires a very high amount of energy. Thus, Statement $(II)$ is true.

Given below are two statements:
Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.
Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.

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Given below are two statements:Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.