Ionization potential:- the amount of energy required to remove a
e− from the outermost shell of the neutral atom.
Factors affecting:-
(i) Atomic radii:-
as atomic radii increase ⟶ the outermost e− is loosely held by the nucleus and hence ionization potential decreases and vice versa.
(ii) Effective nuclear charge:-
as effective nuclear charge increases the e−s are held more tightly with the nucleus and hence ionization potential increases.
(iii) Shielding effect:-
with an increase in shielding effect⟶ ionization potential decreases. Due to this shielding, e−s are loosely held and hence low ionization potential.
(iv) Penetrating effect:-
Penetration effect is the ability of an orbital to attract a e−. So as penetrating effect increases ionization potential increases.
(v) Stability of half-filled and full-filled orbitals
ionization potential has maximum value due to the extra stability of the half-filled and full filled electron configuration.