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

Answer 1

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

Electronic configuration of atomic #Mg#: #1s^(2)2s^(2)2p^(6)3s^2#, versus #Al#, #1s^(2)2s^(2)2p^(6)3s^(2)3p^1#.
Would you expect it to be easier to remove an electron from a #p# orbital (with zero electron density at the nucleus), versus an #s# orbital, which has density at the nucleus? Why?
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Answer 2

The first ionization energy of aluminum is lower than that of magnesium because aluminum has an outer electron in a higher energy level, which experiences increased shielding from inner electrons, making it easier to remove.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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