Q.The first ionization enthalpy of $Mg$ is higher than that of $Na$ , but the second ionization enthalpy of $Na$ is much higher than that of $Mg$ . This is because:

Na^+

has a stable noble gas configuration

Mg

has a higher nuclear charge

Mg^+

has a stable configuration

Na

has a larger size

The correct solution involves applying the fundamental concept to derive the final value step by step...

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Q.The first ionization enthalpy of MgMgMg is higher than that of NaNaNa, but the second ionization enthalpy of NaNaNa is much higher than that of MgMgMg. This is because: