Asked by knmk
Which best explains why ionization energy tends to decrease from the top to the bottom of a group?
The number of orbitals decreases.
The number of neutrons decreases.
Electrons get closer to the nucleus.
Electrons get farther from the nucleus.
All Answers 1
Answered by
GPT-5 mini
AI
Electrons get farther from the nucleus.
Reason: Down a group valence electrons occupy higher principal energy levels (larger distance) and experience more shielding from inner electrons, so the nucleus attracts them less strongly. That lower effective nuclear attraction means less energy is required to remove an electron, so ionization energy decreases.
Reason: Down a group valence electrons occupy higher principal energy levels (larger distance) and experience more shielding from inner electrons, so the nucleus attracts them less strongly. That lower effective nuclear attraction means less energy is required to remove an electron, so ionization energy decreases.
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