The correct order of first ionization enthalp | vedclass

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Question

(C) The electronic configurations of the elements are as follows: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=

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$C < O < N < F$

Vedclass · Answer

(C) The electronic configurations of the elements are as follows: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^2 2p^5$ Across a period,ionization enthalpy generally increases due to increasing effective nuclear charge. However,nitrogen $(N)$ has a stable half-filled $2p^3$ configuration,which makes its ionization enthalpy higher than that of oxygen $(O)$. Therefore,the correct order is $C < O < N < F$.

The correct order of first ionization enthalpy for the given four elements is:

Similar Questions

Ionisation energy in group $I$ elements varies in the decreasing order as:

Which has maximum first ionization potential?

Which of the following orders regarding ionization energy is correct?

Identify the element having lowest first ionization enthalpy.

The correct order of first ionisation enthalpy of the given elements is:

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