Question

The second ionization energies among $Li.Be.B$ and $C$ s lowest for:

• A. $Li$
• B. $Be$
• C. $B$
• D. $C$

Answer 1

Answer: (B)

$Be$

The ionisation energy is the energy required to remove an electron from the outermost shell of an isolated gaseous atom. When the first electron or the most loosely bound electron is removed, the amount of energy required is less than the energy required to remove the electron in the next successive shell. This ionisation energy goes on increasing with the number of electrons removed.
So the number of electrons removed from the successive no of shells and the energy involved is called successive ionization energy.

The second ionization energy is the energy required to remove an electron from a 1+ cation in the gaseous state.

$X^{+}\left(g\right)\to X^2\left(g\right)+e^{-}$

just like the first ionization energy, the second ionization energy is affected by size., effective nuclear charge, and electron configuration.

The order is $Be<C<B<N<F<O<Ne<Li$.