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Question: Answered & Verified by Expert
Among the second-period elements, the actual ionisation enthalpies are in the order Li < B < Be < C < O < N < F < Ne. Which of the following options explains why Be has a higher ionisation enthalpy than B?
ChemistryClassification of Elements and Periodicity in PropertiesNEET
Options:
  • A Beryllium has a smaller atomic size compared to boron.
  • B Beryllium has a higher effective nuclear charge (Zeff) than boron.
  • C The electronic configuration of Be has higher stability than the electronic configuration of B due to completely filled 2s orbital
  • D Beryllium has more protons in its nucleus compared to boron.
Solution:
2680 Upvotes Verified Answer
The correct answer is: The electronic configuration of Be has higher stability than the electronic configuration of B due to completely filled 2s orbital
Correct Option is : (C)
The electronic configuration of Be has higher stability than the electronic configuration of B due to completely filled 2s orbital

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