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Ch.8 - Periodic Properties of the Elements
All textbooksTro 4th EditionCh.8 - Periodic Properties of the ElementsProblem 57
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Chapter 8, Problem 57

Which experience a greater effective nuclear charge: the valence electrons in beryllium or the valence electrons in nitrogen? Why?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Effective Nuclear Charge (Z_eff)

Effective nuclear charge refers to the net positive charge experienced by an electron in a multi-electron atom. It accounts for the actual nuclear charge (the number of protons) and the shielding effect caused by inner-shell electrons. The greater the effective nuclear charge, the stronger the attraction between the nucleus and the valence electrons.
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Shielding Effect

The shielding effect occurs when inner-shell electrons partially block the attraction between the nucleus and the outer-shell (valence) electrons. This results in a lower effective nuclear charge felt by the valence electrons. In elements with more inner electrons, the shielding effect is more pronounced, reducing the effective nuclear charge experienced by the valence electrons.
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Trends in the Periodic Table

Periodic trends, such as effective nuclear charge, vary across periods and groups in the periodic table. As you move from left to right across a period, the effective nuclear charge increases due to the addition of protons without a corresponding increase in shielding. This trend helps explain why elements like nitrogen, which is further right in the periodic table than beryllium, experience a greater effective nuclear charge on their valence electrons.
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Related Practice
Textbook Question

Which outer electron configurations would you expect to belong to a metalloid? ns2 b. ns2np6 c. ns2np5 d. ns2np2

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According to Coulomb's law, which pair of charged particles has the lowest potential energy? a. a particle with a 1- charge separated by 150 pm from a particle with a 2+ charge b. a particle with a 1- charge separated by 150 pm from a particle with a 1+ charge c. a particle with a 1- charge separated by 100 pm from a particle with a 3+ charge

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According to Coulomb's law, rank the interactions between charged particles from lowest potential energy to highest potential energy. a. a 1+ charge and a 1- charge separated by 100 pm b. a 2+ charge and a 1- charge separated by 100 pm c. a 1+ charge and a 1+ charge separated by 100 pm d. a 1+ charge and a 1- charge separated by 200 pm

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Arrange the atoms according to decreasing effective nuclear charge experienced by their valence electrons: S, Mg, Al, Si.

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Textbook Question

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? a. K

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Textbook Question

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? b. Ca

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