The correct order of first ionization enthalpy for the given four element is :
The correct order of first ionization enthalpy for the given four element is :
- C $ < $ N $ < $ F $ < \mathrm{O}$
- $\mathrm{C} < \mathrm{N} < \mathrm{O} < \mathrm{F}$
- $\mathrm{C} < \mathrm{O} < \mathrm{N} < \mathrm{F}$
- $\mathrm{C} < $ F $ < \mathrm{N} < \mathrm{O}$
Solution
$\begin{array}{|c|c|c|c|c|}\hline \text {Explanation: } & \mathrm{C} & \mathrm{N} & \mathrm{O} & \mathrm{F} \\ \hline \text{(Half-filled) } & 2 s^2 2 p^2 & 2 s^2 2 p^3 & 2 s^2 2 p^4 & 2 s^2 2 p^5 \\ \hline \end{array}$
Across the period $Z_{\text {eff }}$ increases but nitrogen has half-filled orbital which makes it more stable.
$\therefore$ Order of $\mathrm{IE}_1=\mathrm{C} < \mathrm{O} < \mathrm{N} < \mathrm{F}$
Asked in: NEET 2022 (Phase 2)
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