The following table gives the first ionization energies for the second period elements. Using electron configurations,...

The following table gives the first ionization energies for the second period elements. Using electron configurations, explain why boron and oxygen have lower ionization energies than would be expected based on the general trend.

Element	Li	Be	B	C	N	O	F	NE
IE (KJ/mol)	520	899	801	1086	1402	1314	1681	2081

Solutions

Expert Solution

generally from left to right in periods ionisation energy increases.But from 2nd to 3rd group , 5th to 6th group ionisation energy decreases.

Reason : Be = Z = 4 = 1S2 2S2 , B = 1S2 2S2 3S1

Be is having fully filled orbital in its valence shell , so that it requires more energy than B.

similarly ,

N = 5 = 1s2 2s2 2p3 , O = 6 = 1s2 2s2 2p4

N , is half filled requires more energy than O.

queen_honey_blossom answered 1 year ago

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