Why is the first ionization energy of aluminum lower than the first ionization of magnesium?

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Why is the first ionization energy of aluminum lower than the first ionization of magnesium?

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Answer 1 · 2015-11-30T07:27:43

Consider the nucleus-electron attraction for a $s$ $s$ orbital electron versus a $p$ $p$ orbital electron.

Explanation:

Electronic configuration of atomic $M g$ $Mg$ : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$ $1s^(2)2s^(2)2p^(6)3s^2$ , versus $A l$ $Al$ , $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$ $1s^(2)2s^(2)2p^(6)3s^(2)3p^1$ .

Would you expect it to be easier to remove an electron from a $p$ $p$ orbital (with zero electron density at the nucleus), versus an $s$ $s$ orbital, which has density at the nucleus? Why?

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Why is the first ionization energy of aluminum lower than the first ionization of magnesium?

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