The first ionization enthalpies of C,N,and F | vedclass

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Question

(A) The correct value is $1310 \, kJ \, mol^{-1}$.In the periodic table,the first ionization enthalpy generally increases across a period from left to

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$1310 \, kJ \, mol^{-1}$

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(A) The correct value is $1310 \, kJ \, mol^{-1}$.In the periodic table,the first ionization enthalpy generally increases across a period from left to right.However,due to the stable half-filled $2p^3$ electronic configuration of Nitrogen $(1s^2 2s^2 2p^3)$,it has a higher ionization enthalpy than Oxygen $(1s^2 2s^2 2p^4)$.Therefore,the ionization enthalpy of Oxygen must be lower than that of Nitrogen $(1402 \, kJ \, mol^{-1})$.Thus,$1310 \, kJ \, mol^{-1}$ is the correct value.

The first ionization enthalpies of $C$,$N$,and $F$ are $1086$,$1402$,and $1681 \, kJ \, mol^{-1}$ respectively. Which of the following values is the most likely first ionization enthalpy of $O$ ($1310$ or $1510 \, kJ \, mol^{-1}$)?

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