Why does the successive ionization enthalpy o | vedclass

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(C) The first ionization enthalpy is the energy required to remove the first electron from a neutral atom. After the removal of the first electron,the

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Due to the increased electrostatic attraction between the remaining electrons and the nucleus as the positive charge on the ion increases.

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(C) The first ionization enthalpy is the energy required to remove the first electron from a neutral atom. After the removal of the first electron,the remaining electrons are more strongly attracted by the nucleus because the effective nuclear charge per electron increases. Consequently,removing the second and third electrons requires significantly more energy,leading to the order $1^{st} < 2^{nd} < 3^{rd}$.

Why does the successive ionization enthalpy of an element increase in the order: $1^{st} < 2^{nd} < 3^{rd}$?

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