Consider the elements Ne , Na , Mg. The element with highest first ionization enthalpy and element with lowest second ionization enthalpy respectively are

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Accepted Answer

Correct answer: B. (b) _10 Ne=1 s^22 s^22p^6 , _11 Na=1 s^22 s^22p^63 s^1 _12 Mg=1 s^22 s^22p^63 s^2 ⇒ Highest first ionization enthalpy = Ne, due to stable fully-filled configuration. ⇒ Lowest second ionization enthalpy = Mg, due to stable noble - gas configuration obtained after losing two electrons.

$Consider the elements Ne, Na, Mg . The element with highest first ionization enthalpy and element with lowest second ionization enthalpy respectively are$

Solution

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