The first ionization enthalpies of four conse | vedclass

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Question

(B) The elements in the $2$nd period generally show an increase in ionization enthalpy from left to right.However,nitrogen $(N)$ has a higher first io

Vedclass · Accepted Answer

$14.5$

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(B) The elements in the $2$nd period generally show an increase in ionization enthalpy from left to right.However,nitrogen $(N)$ has a higher first ionization enthalpy than oxygen $(O)$ due to its stable half-filled $p$-orbital configuration $(2s^{2} 2p^{3})$.Among the given values $(8.3, 11.3, 14.5, 13.6)$,the value $14.5 \ eV$ corresponds to nitrogen because it is the peak in the trend before the drop at oxygen.Therefore,the first ionization enthalpy of nitrogen is $14.5 \ eV$.

The first ionization enthalpies of four consecutive elements present in the second period of the periodic table are $8.3, 11.3, 14.5$ and $13.6 \ eV,$ respectively. Which one of the following is the first ionization enthalpy of nitrogen?

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