Question

first ionization energy of magnesium is higher than that of sodium but second ionization energy of sodium is higher than that of magnesium give reason

Answer 1

This is because in 1st ionisation energy of magnesium,Magnesium has more z-effective as compared to Na (due to its smaller size)..In the second case (When an electron has been removed from both) Na+ becomes stable while Mg+ does not (as it has to loose 2 electrons for stability) Thus removing electron from Mg requires less energy as compared to removing electron from stable Na+ ion.

This is the correct answer.Hope it helped.❤️

Answer 2

Second ionization energy of sodium is higher than that of magnesium because now electron is to be removed from stable noble gas configuration.

Explanation:

The ionization energy is the energy required to remove an electron from the valence shell of an isolated gaseous atom of an element.

Now the ionization energy depends upon

a) size of an element : larger the size more lesser the effective nuclear charge on electron thus lower the ionization energy.

b) the electronic configuration of an element: If on losing an electron an element attains noble gas configuration or half filled stability then it will easily lose an electron.

For $Na:11:1s^22s^22p^63s^1$

$Na^+:10:1s^22s^22p^6$

For $Mg:12:1s^22s^22p^63s^2$

$Mg^{+}:11:1s^22s^22p^63s^1$

For first ionization energy , as magnesium is smaller than sodium, more energy is need to remove first electron from magnesium. But when second electron is to be removed, sodium acquires stable noble gas configuration and thus more energy is required to remove the second electron.

Learn more about ionization energy

https://brainly.in/question/6571176

https://brainly.com/question/12606723