Question

o O In all other cases.
How many following pairs in which ionisation energy of first element or ion is higher as compare to second?
(O, N), (Ne, Nat), (Sn, Pb), (Cu, Zn), (Li, Li+), (Lit, Be2+), (N3-, N), (Sn2+, Sn4+)​

Answer 1

Answer:

(O, N), (Ne, Na), (Sn, Pb)

Explanation:

The Ionization Energy is the energy required to remove an electron from its orbital around an atom to a point where it is no longer associated with that atom.

The ionization energy of an element increases as one moves across a period (left to right) in the periodic table because the electrons are held tighter by the higher effective nuclear charge. (harder to remove)

The ionization energy of the elements increases as one moves up a given group because the electrons are held in lower-energy orbitals, closer to the nucleus and therefore are more tightly bound (harder to remove).

The ionization energy is higher for cation of a atom, than ionization energy of the same atom because there it is already one or few electrons less than number of protons. Thus more energy is needed to remove one more electron.

Whereas, anions have more electrons than number of protons, so It is easier to remove an electron from their orbit