How would you explain the fact that first ionisation enthalpy of sodium is lower that magnesium but the second ionisation enthalpy of sodium is more than magnesium?
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Electronic configuration of Na and Mg are
Na = 1s 2s 2p 3s
Mg = 1s 2s 2p 3s
First electron in both cases has to be removed from 3s-orbital but the nuclear charge of Na (+ 11) is lower than that of Mg (+ 12) therefore first ionization energy of sodium is lower than that of magnesium.
After the loss of first electron, the electronic configuration of
Na = 1s 2s 2p
Mg = 1s 2s 2p 3s
Here electron is to be removed from inert (neon) gas configuration which is very stable and hence removal of second electron requires more energy in comparison to Mg.
Therefore, second ionization enthalpy of sodium is higher than that of magnesium.
Electronic configuration of Na and Mg are
Na = 1s 2s 2p 3s
Mg = 1s 2s 2p 3s
First electron in both cases has to be removed from 3s-orbital but the nuclear charge of Na (+ 11) is lower than that of Mg (+ 12) therefore first ionization energy of sodium is lower than that of magnesium.
After the loss of first electron, the electronic configuration of
Na = 1s 2s 2p
Mg = 1s 2s 2p 3s
Here electron is to be removed from inert (neon) gas configuration which is very stable and hence removal of second electron requires more energy in comparison to Mg.
Therefore, second ionization enthalpy of sodium is higher than that of magnesium.
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