The first ionization enthalpies of N and O ar | vedclass

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(A) The electronic configuration of Nitrogen ($N$,$Z=7$) is $1s^2 2s^2 2p^3$. Because of the stable half-filled $2p$ subshell,it has a higher ionizati

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$14.6, 13.6$

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(A) The electronic configuration of Nitrogen ($N$,$Z=7$) is $1s^2 2s^2 2p^3$. Because of the stable half-filled $2p$ subshell,it has a higher ionization enthalpy. The electronic configuration of Oxygen ($O$,$Z=8$) is $1s^2 2s^2 2p^4$. Due to the removal of an electron from a more stable $2p^3$ configuration in Nitrogen compared to the $2p^4$ configuration in Oxygen,Nitrogen has a higher first ionization enthalpy $(14.6 \ eV)$ than Oxygen $(13.6 \ eV)$.

The first ionization enthalpies of $N$ and $O$ are respectively....... $eV$.

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