If we consider ionization enthalpies of elements in the second period from Li to Ne, they ordinarily increase but Be and N have higher ionization enthalpies than B and O respectively which succeed them. Why is it so ?

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Solution

$B e$ and $N$ have higher ionization enthalpies than B and O respectively because of $B e a n d N$ have exactly full filled and half-filled electronic orbital configuration to give more stability and therefore more energy is needed to ionize the $B e$ and $N$ atom.
$_{4} B e = 1 s^{2}, 2 s^{2} \to Full filled orbital$
$_{7} N = 1 s^{2}, 2 s^{2}, 2 p^{3} \to Half filled orbital$

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