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why o has lower ionisation enthalpy than N and F?

  1. n has half filled electronic configuration so its i.e is high 
  2. f is highest electronegative element it never looses electrons so its i.e is high
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ionization energy depend on size

nitrogen has half filled electronic configurationand hence it is stable so its i.e is high

and F has small size

hope u got it

  • 0

oxygen has outer electronic configuration2s2 2p4

removal of ine electron from the 2p subshell will make its configuration

2s22p3

thus it attains a half filled configuration

thus lesser energy is required to remove an elecron from oxygen

whereas in nitrogen

the electronic configuration is

2s2 2p3

it has a stable half filled configuration

and thus more energy is required to remove an electron from nitrogen

in case of flourine

the electronic configuration is

2s2 2p5

it has to gain one more electron to attain noble gas configuration and become stable

thus more energy is required to remove an electron from flourine

thus ionisation enthalpy of oxygen is lesser than nitrogen or flourine

  • 24
nitrogen has higher i.e. as it has less number of electrons as compaired to O and F . by this nucleus holds the electrons tightly .
and shielding effect is also less in nitrogen . as comparied to O and F . and hence O and F have lower i.e.

hope you like it
  • 6
Pls tell why o is lower than n

  • -1
kkkmmm
  • -4
check some other website
  • 0
O is the lower ionisation enthalpy than the Band f
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