The electronic configuration of an element wi | vedclass

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(A) The difference between the $1^{st}$ and $2^{nd}$ ionisation energies is largest when the removal of the second electron requires breaking a stable

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$1s^{2} 2s^{2} 2p^{6}$

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(A) The difference between the $1^{st}$ and $2^{nd}$ ionisation energies is largest when the removal of the second electron requires breaking a stable,fully-filled shell or subshell configuration.						Electronic configuration			Element/Group							$1s^{2} 2s^{2} 2p^{6}$			Neon (Group $18$)							$1s^{2} 2s^{2} 2p^{6} 3s^{1}$			Sodium (Group $1$)							$1s^{2} 2s^{2} 2p^{6} 3s^{2}$			Magnesium (Group $2$)							$1s^{2} 2s^{2} 2p^{1}$			Boron (Group $13$)			For $1s^{2} 2s^{2} 2p^{6}$ (Neon),the $1^{st}$ ionisation energy is very high due to its stable noble gas configuration. However,the $2^{nd}$ ionisation energy is significantly higher because it involves removing an electron from a stable $2p^{6}$ shell,which is extremely difficult. Thus,the jump between $IE_1$ and $IE_2$ is largest for this configuration.

The electronic configuration of an element with the largest difference between the $1^{st}$ and $2^{nd}$ ionisation energies is

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