The second ionisation energies of $\mathrm{Li}, \mathrm{Be}, \mathrm{B}$ and $\mathrm{C}$ are in the order

Question

Aicharya · Accepted Answer

The second ionisation energy is the energy required to remove an electron from a $\mathrm{I}+$ cation in the gaseous state. $X^{+}(g) \rightarrow X^{2+}(g)+e^{-}$ Just like the first ionisation energy, the second ionisation energy is affected by size, effective nuclear charge, and electron configuration. Li has highest $\mathrm{IE}_2$ than because the second electron remove from stable noble gas configuration and $B$ has higer $\mathrm{IE}_2$ than $\mathrm{C}$ due to the extra stability of the $2 s^2$ subshell in the $\mathrm{B}^{+}$ion. Therefore, the order is $\mathrm{Li} > \mathrm{B} > \mathrm{C} > \mathrm{Be}$ Hence, the correct option is (b).

The second ionisation energies of \(\mathrm{Li}, \mathrm{Be}, \mathrm{B}\) and \(\mathrm{C}\) are in the order

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