Why ionization energy of Na is less than Mg?

Answer 1

Electron configurations indicate that from Be to B there are electrons in the 2p subshell, which has more energy than 2s. These 2p electrons are not as strongly attached to the nucleus as they contain more energy, therefore they are more easily removed.

In moving from Mg to Al there are electrons in 3p - the same logic as above applies.

Answer 2

mg occupies s orbital whereas al occupies p orbital. distance between p orbital and nucleus is more than that of s orbital due to which atomic radius of al is more than that of mg..........................................................................contd..........................................

by BIPIN SHARMA.

Answer 3

Fluorine is more electronegative than Mg. It is easier to remove the first electron from a Mg atom that it is to remove one from a F atom.

Electronegativity is the ability of an atom to attract electrons towards itself. That means that the electrons in Fluorine are held tighter than in Mg. And this is why the first ionization of Mg is lower that that of Fluorine :)

Hope it helps.

Answer 4

Ionization energy of Na is less than that of Mg because Na gives only one electron but Mg gives two electrons as valency of magnesium is 2 and that of sodium is 1. And the I.E successor after 1st electron is always greater than the predecessor.i.e, 1st I.E < 2nd I.E <3rd I.E OR

3rd I.E > 2nd I.E > 1st I.E

Answer 5

The ionization energy of sodium (Na) is less than magnesium (Mg) because sodium has a larger atomic radius and fewer electrons in its outer shell. This makes it easier to remove an electron from sodium compared to magnesium, which has a higher effective nuclear charge due to its smaller size and more electrons in its outer shell.

Answer 6

Mg looses 2 electrons Al looses 3.