Question:
The correct order of ionisation energy of C, N, O, F is
The correct order of ionisation energy of C, N, O, F is
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N > O because Nitrogen has a stable half-filled $p$-subshell.
Updated On: Apr 10, 2026
- $F<O<N<C$
- $F<N<C<O$
- $C<N<O<F$
- $C<O<N<F$
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The Correct Option is D
Solution and Explanation
Step 1: Period Trend
Ionization energy generally increases from left to right across a period due to increasing nuclear charge.
Step 2: Exception
Nitrogen ($2p^{3}$) has a half-filled subshell, which is exceptionally stable.
Step 3: Comparison
Because of this stability, it is harder to remove an electron from N than from O ($2p^{4}$).
Step 4: Final Order
The order is $C<O<N<F$.
Final Answer: (d)
Ionization energy generally increases from left to right across a period due to increasing nuclear charge.
Step 2: Exception
Nitrogen ($2p^{3}$) has a half-filled subshell, which is exceptionally stable.
Step 3: Comparison
Because of this stability, it is harder to remove an electron from N than from O ($2p^{4}$).
Step 4: Final Order
The order is $C<O<N<F$.
Final Answer: (d)
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