Question

First ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium. explain​

Answer 1

Answer:------------------------------------

The first ionization energy of magnesium is larger than sodium because magnesium has one more proton in its nucleus to hold on to the electrons in the 3s orbital

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The electronic configurations are as follows:

Na - [Ne] 3s

1

Mg - [Ne] 3s

2

Sodium has one valence electron in 3s

1

and by losing this electron it attains stable configuration. Therefore the 1st ionization energy of Na is less than Mg. After removing an electron the Na attains noble gas configuration whereas Mg has one electron left. To remove an electron from a noble gas configuration high energy is required.

Therefore the second ionization enthalpy is higher than that of magnesium.

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Answer 2

Answer:

The first ionization energy of magnesium is larger than sodium because magnesium has one more proton in its nucleus to hold on to the electrons in the 3s orbital