Answer Bank Effective nuclear charge decreases from left to right across a period on the periodic table. In a Be atom, a 1s electron has a greater Zer than a 2s electron. Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge. Across a period, as Zer increases, atomic size decreases. Effective nuclear charge does not depend on the number of electrons present in an atom. A ls electron in a Be atom has a smaller Zef than a 1s electron in a Li atom.
Answer Bank Effective nuclear charge decreases from left to right across a period on the periodic table. In a Be atom, a 1s electron has a greater Zer than a 2s electron. Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge. Across a period, as Zer increases, atomic size decreases. Effective nuclear charge does not depend on the number of electrons present in an atom. A ls electron in a Be atom has a smaller Zef than a 1s electron in a Li atom.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter6: The Structure Of Atoms
Section: Chapter Questions
Problem 47GQ: Which of the following are applicable when explaining the photoelectric effect? Correct any...
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Classify each statement about effective nuclear charge, ?eff , as true or false.
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