Question

arrange the following atoms in increasing order of their ionisation potential Boron beryllium oxygen nitrogen fluorine neon​

Answer 1

solution:

In case of Be electron has to be removed from an s-orbital whereas in Boron removal takes from p-orbital.

As s-orbital is closer to nucleus, hence removal of electron is difficult which raises its ionization enthalpy.

Comparing O and N, nitrogen has completely half filled p-orbitals, hence I.E. of nitrogen is greater than oxygen. [Half filled orbitals account for greater stability].

Comparing O and F, F has increased nuclear charge and small size, hence removal of electron is difficult. Therefore, I.E. of F is greater than O.

Answer 2

Explanation:

Second period: Neon > Fluorine > Oxygen > Nitrogen > Carbon > Boron > Beryllium > LithiumThird Period: Argon> Chlorine > Sulphur > Phosphorus > Silicon > Aluminum >Magnesium > Sodium