Question

why ionization energy of nitrogen is more than ionization energy of oxygen ?

Answer 1

• Usually the ionization energy of a more electronegative element is more than that of a less electronegative or a more electropositive element...
• However, since Oxygen is a very reactive element as compared to Nitrogen, so it loses the first and the second valence electrons of its atom more easily, and with less application of energy, than in case of Nitrogen...
• Hence, the ionization energy of Nitrogen is more than that of Oxygen...

<Judge It Yourself...>

Answer 2

$\huge\underline{\underline{\bf Answer;-}}$

↔ Ionisation energy of Nitrogen is

greater than the Ionisation energy of

oxygen

↔Let us look at the electronic

configurations of Nitrogen and Oxygen

Nitrogen:-

Atomic number=7

Electronic configuration: 1s² 2s² 2p³

↔As we can see in 2p orbital,we have

half filled configuration

↔Half filled configuration is more stable

so it needs more energy inorder to

remove an electron from the outermost

orbit.

Oxygen:-

Atomic number=8

Electronic configuration: 1s² 2s² 2p⁴

↔Here we can see that there is

no half filled or completed filled

configuration

↔It needs less energy to remove the

electron from the outermost orbit

compared to nitrogen

$\sf I.E \: of \: Nitrogen >I.E \: of \: Oxygen$