Along a period from left to right, ionization enthalpy increases. But ionization enthalpy of nitrogen is unexpectedly higher than that of oxygen. Why?
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Unexpected increase in ionization enthalpy of nitrogen is because of stable half filled configuration of nitrogen..
Atomic number of Nitrogen (N) = 7
Electronic configuration =
1s2 2s2 2p3
---> Here, for 1s2 & 2s2 subshell have 1 orbital and 2 electrons are filled in it.
---> Considering 2p3 ,
For p orbital their will be 3 orbitals and 3 of them are filled parallel wise.
I.e , half filled configuration.
Atomic number of Oxygen (O) = 8
Electronic configuration = 1s2 2s2 2p4
---> Here, in p subshell electrons are not filled either half filled nor as full filled .
.: Along a period from left to right, ionization enthalpy increases for nitrogen than oxygen.
Atomic number of Nitrogen (N) = 7
Electronic configuration =
1s2 2s2 2p3
---> Here, for 1s2 & 2s2 subshell have 1 orbital and 2 electrons are filled in it.
---> Considering 2p3 ,
For p orbital their will be 3 orbitals and 3 of them are filled parallel wise.
I.e , half filled configuration.
Atomic number of Oxygen (O) = 8
Electronic configuration = 1s2 2s2 2p4
---> Here, in p subshell electrons are not filled either half filled nor as full filled .
.: Along a period from left to right, ionization enthalpy increases for nitrogen than oxygen.
Kimmus:
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