Question

why ionization enthalpy of Be is more then B and of N is more than O explain?

Answer 1

It is known that full filled orbitals are most stable and after than half filled atomic orbitals are most stable. In the above case,
(i) Be has most stable full filled configuration
Be = 1s^2, 2s^2
while in B one unpaired electron is present
B = 1s^2, 2s^2, 2p^1

So,in order to remove electron from Be we have to supply very high amount of energy because it has full filled elecronic configuration but in B one unpaired electron is present so it is easy to remove electron from B
That's why ionisation enthalpy of Be is more than B

(ii) Similarly,in the case of Nitrogen and Oxygen nitrogen has half filled electronic configuration
N = 1s^2, 2s^2, 2p^3
while in oxygen one more electron is present than nitrogen
O = 1s^2, 2s^2, 2p^4
So it is easy to remove electron from oxygen
but in nitrogen we have to supply a high amount of energy in order to remove the electron
That is why ionisation enthalpy of N is more than O

Answer 2

Explanation:

here is the ans

have it

hope it helps