Question

9. Arrange the following elements in order of increasing lonisation
energy B,C,N,O​

Answer 1

Answer:

the following elements can be arranged in order of increasing ionization as B<C<O<N

Explanation:

B<C follow the rule i. e. ionization ionisation energy increases if you go from left to right along any period

O<N THIS EXCEPTION CAN BE SEEN BECAUSE OF THE EXCEPTIONAL STABILITY OF ELECTRONS OF NITROGEN DUE TO THE EXCHANGE ENERGY OF HALF FILLED 2P ORBITAL .

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Answer 2

Answer :

◈ Ionization enthalpy :

• The energy required to remove the most loosely bound electron from an isolated gaseous atom is called the ionization enthalpy.
• In general, the first ionization enthalpy decreases in a regular way on descending the main groups. There is gradual overall increase in ionization enthalpy as we move from left to right across a period, although the horizontal variation is somewhat irregular.

Correct order : B < C < O < N

◈ Why ionization enthalpy of nitrogen is higher than oxygen ?

• N : [He] 2s(2) 2p(3)
• O : [He] 2s(2) 2p(4)

Nitrogen has half-filled p orbital and we know that half-filled or full-filled orbitals are more stable because of high exchange energy that's why ionization enthalpy of N is higher than O$.$