In which of the following electronic configur | vedclass

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(D) The ionization energy increases significantly when an electron is removed from a stable,noble gas-like configuration or a completely filled shell.

Vedclass · Accepted Answer

$1s^2\, 2s^2\, 2p^6\, 3s^2$

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(D) The ionization energy increases significantly when an electron is removed from a stable,noble gas-like configuration or a completely filled shell.For option $D$,the configuration is $1s^2\, 2s^2\, 2p^6\, 3s^2$ (Magnesium,$Z=12$).The first ionization energy removes one $3s$ electron.The second ionization energy removes the second $3s$ electron.After removing two electrons,the configuration becomes $1s^2\, 2s^2\, 2p^6$,which is the stable neon noble gas configuration.Therefore,removing the third electron requires a very high amount of energy,leading to a large difference between the second and third ionization energies.

In which of the following electronic configurations will there be a large difference between the second and third ionization energy?

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