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Chapter 5: Problem 21

How does the core charge on the neutral atom change as we move from left to right across a row (period) of the periodic table?

Short Answer

Expert verified
The core charge on the neutral atom generally increases as we move from left to right across a row (period) of the periodic table. This is due to an increase in the atomic number with no significant change in the shielding effect.

Step by step solution

01

Understand the Concept of Core Charge

Core charge is the effective nuclear charge felt by the outermost (valence) electrons of an atom. It can be computed by subtracting the shielding effect from the atomic number. That is, Core charge = Atomic number – Shielding effect.
02

Understand the Structure of the Periodic Table

The periodic table is arranged in a way that elements with similar chemical properties line up in columns, also known as groups. The horizontal rows are called periods. As you move along a period from left to right, the atomic number (number of protons + number of veiling electrons) increases, but shielding effect usually stays the same.
03

Determine the Relationship between Core Charge and Position in the Periodic Table

As one moves from left to right across a period, the atomic number increases, adding protons to the nucleus and electrons to the same energy level, which does not significantly increase shielding effect. Therefore, the core charge generally increases as one moves from left to right across a period in the periodic table.

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Most popular questions from this chapter

Assuming that the valence shells of \(\mathrm{Li}\) and \(\mathrm{Be}\) are at approximately the same distance from their nuclei, explain how the core charges of \(\mathrm{Li}\) and \(\mathrm{Be}\) are consistent with the \(\mathrm{IE}_{1}\) values for \(\mathrm{Li}(0.52 \mathrm{MJ} / \mathrm{mole})\) and Be \((0.90 \mathrm{MJ} / \mathrm{mole})\).

How many electrons are in the valence shell of a) H? b) Li? C) He?

What is the core charge of Li?

Use the core charge concept to propose an explanation for the increase of \(\mathrm{IE}_{1}\) from Na through Ar. Clearly state any assumptions that you make.

Locate H, Li, and Na on the periodic table. a) Describe any relationship between the core charge of these atoms, the number of valence electrons, and their positions in the periodic table. b) Describe any relationship between the valence shell of these atoms and their positions in the periodic table. c) Based on its position in the periodic table, predict the valence shell, core charge, and number of valence electrons for \(\mathrm{Rb}\). d) Using the shell model and referring to the Coulombic Potential Energy relationship (equation in Model 1, CA3), explain clearly how the \(\mathrm{IE}_{1}\) for \(\mathrm{Rb}\) is consistent with your answer to part c.
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