The correct order of ionisation energy of $C, N, O$ & $F$ is:

F < N < C < O

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C < N < O < F

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C < O < N < F

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F < O < N < C

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Solution

The correct option is C $C < O < N < F$
The correct order of ionization energy of $C, N, O$ & $F$ is $C < O < N < F$ .
In a period on moving from left to right, the ionization energy increases. This is due to increase in the effective nuclear charge.
However the ionization energy of $O$ is lower than the ionization energy of $N$ . This is because in case of $N$ an electron is to be removed from stable half filled $2 p$ sub-shell which requires large energy.

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Similar questions

Arrange F, Cl, O, and N in the decreasing order of electronegativity.

The van der waals radii of $O, N, C l, F$ and $N e$ increases in the order of:

The Van der Waals radii of $O, N, C l, F$ and $N e$ increases in the order?

The Van der walls radii of $O, N, C l, F$ and $N e$ increases in the order.

A. F, O, Ne, Cl
B. N, O, F, Ne, Cl
C.Ne, F, O, N, Cl
D. F, Cl, O, N, Ne

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