Question:
In which of the following, elements are correctly arranged in the decreasing order of their second ionization enthalpies?
In which of the following, elements are correctly arranged in the decreasing order of their second ionization enthalpies?
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Second ionization enthalpy depends on effective nuclear charge and atomic size. Across a period, it generally increases from left to right.
Updated On: Jun 26, 2026
- O > F > N > C
- N > O > F > C
- F > O > N > C
- C > N > O > F
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The Correct Option is A
Solution and Explanation
Step 1: Recall the trend of second ionization enthalpy.
Second ionization enthalpy increases across a period from left to right due to increasing nuclear charge and decreasing atomic size.
Step 2: Analyze elements given.
The elements O, F, N, C are all in the second period. Their second ionization enthalpies generally follow: \[ O \gt F \gt N \gt C \] because oxygen and fluorine have more effective nuclear charge than nitrogen and carbon, thus requiring more energy to remove the second electron.
Step 3: Conclusion.
Therefore, the correct decreasing order of second ionization enthalpies is \[ O \gt F \gt N \gt C \]
Second ionization enthalpy increases across a period from left to right due to increasing nuclear charge and decreasing atomic size.
Step 2: Analyze elements given.
The elements O, F, N, C are all in the second period. Their second ionization enthalpies generally follow: \[ O \gt F \gt N \gt C \] because oxygen and fluorine have more effective nuclear charge than nitrogen and carbon, thus requiring more energy to remove the second electron.
Step 3: Conclusion.
Therefore, the correct decreasing order of second ionization enthalpies is \[ O \gt F \gt N \gt C \]
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