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Among Be, B, Mg and Al, the second ionisation potential is maximum for
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B
Group II A Group III A
$\quad \quad \quad \mathrm{Be} \quad \quad \quad \mathrm{B}$
$\quad \quad \quad \mathrm{Mg} \quad \quad \quad \mathrm{Al}$
The electronic configuration of boron is $2 s^{2}2p$. And electronic configuration of $\mathrm{B}^{+}$ is $2 \mathrm{s}^{2}$. Hence it is difficult to remove second electron ty $2 s^{2}$ shell because half-filled and fully orbitals are more stable than others.
$\quad \quad \quad \mathrm{Be} \quad \quad \quad \mathrm{B}$
$\quad \quad \quad \mathrm{Mg} \quad \quad \quad \mathrm{Al}$
The electronic configuration of boron is $2 s^{2}2p$. And electronic configuration of $\mathrm{B}^{+}$ is $2 \mathrm{s}^{2}$. Hence it is difficult to remove second electron ty $2 s^{2}$ shell because half-filled and fully orbitals are more stable than others.
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