The first ionization energy of Boron () is less than that of Beryllium (), despite Boron having a higher nuclear charge. What is the fundamental reason for this anomaly?

Question

The first ionization energy of Boron ($B$) is less than that of Beryllium ($Be$), despite Boron having a higher nuclear charge. What is the fundamental reason for this anomaly?

Prashant Kotian · Accepted Answer

Correct answer: B. Beryllium has a highly stable, deeply penetrating configuration. Boron's outermost electron is in a higher-energy, less penetrating orbital, making it easier to remove.

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