Atomic nitrogen has a higher ionization energy than atomic oxygen. This is best explained by

  1. A

    stable electronic configuration of nitrogen 

  2. B

    the greater effective nuclear charge of nitrogen

  3. C

    the fact that the electron ionized in N is from the 2s subshell, while that ionized from O is from the 2p subshell.

  4. D

    the fact that N has an odd number of electrons while O has an even number

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    Solution:

    Due to the lower electron-electron repulsion in atomic nitrogen has a higher ionization energy than atomic oxygen. 

    The atomic radius of nitrogen IS lower due ton which the  electrons are consequently closer together. 

    Due to the increased repulsion caused by the additional electron, more energy is needed for this action to take place.

     

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