Explain the following.
"The first ionization energy of carbon atom is greater than that of boron whereas, the reverse is true for the second ionization energy".

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Solution

$I E_{1}$ of $C > I E_{1}$ of $B$ whereas $I E_{2}$ of $B > I E_{2}$ of $C$
$_{6} C ⟶ 1 s^{2} 2 s^{2} 2 p^{2}$ (full filled orbital)
$_{5} B ⟶ 1 s^{2} 2 s^{2} 2 p^{1}$
$∵ C$ has fully filled $p -$ orbital. And to remove an $e^{-}$ from a fully filled orbital is quite difficult as atom will tend to stay in stable form more.
In second case, after removal of an $e^{-}$ , $B$ has fully-filled $s -$ orbital and is having a stable configuration. Removing an $e^{-}$ from their stable form is difficult. Hence, $I E_{2}$ of $B$ is more than $I E_{2}$ of $C$ .

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