Outermost electronic configurations of four elements A, B, C, D are given below :
(A) $3 s^{2}$
(B) $3 s^{2} 3 p^{1}$
(C) $3 s^{2} 3 p^{3}$
(D) $3 s^{2} 3 p^{4}$
The correct order of first ionization enthalpy for them is :
Solution
Orbitals with fully filled and half-filled electronic configuration are stable, and require more energy for ionization
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Elements with greater electronegativity require more energy for ionisation
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Hence the correct order is $C>D>A>B$
About this question
Subject: Chemistry · Chapter: Atomic Structure · Topic: Bohr's Model
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