Question

when removing successive outermost electrons from sodium. the first ionization energy is 495 kj/mol, while the second ionization energy is 4562 kj/mol. however, when removing successive electrons from magnesium, the first ionization energy is 738 kj/mol and the second ionization energy is 1451 kj/mol. why is there a bigger increase in second ionization energy for sodium than there is for magnesium?

Answer 1

There a bigger increase in second ionization energy for sodium than there is for magnesium because fully filled orbitals have extra stability.

The electronic configuration of Sodium is:

Na = 1s2 2s2 2p6 3s1

After removing one electron, the  electronic configuration is

Na⁺ = 1s2 2s2 2p6   ( I.E 1 = 495)

I.E 1 of sodium = 495 and I.E 2 of sodium = 4562

• I.E 1 < I.E 2 because half filled and fully filled orbitals have extra stability.

• Also ,  I.E 2 is very high because an electron is removed from fully filled p orbital.
• After losing an electron , sodium attains stable noble gas configuration

The electronic configuration of Magnesium is:

Mg = 1s2 2s2 2p6 3s2

There a bigger increase in second ionization energy for sodium than there is for magnesium because:

1. The electronic configuration of Na⁺ is Ne and electronic configuration of Mg⁺¹ is [Ne] 3s1  so removing an electron from 3s takes less energy than removing an electron from 2p
2. Since  Na⁺ ion is larger than Mg⁺ ion , it takes more energy to remove an electron from sodium ion

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