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Chapter 5: Problem 11

How does the core charge for Na compare to the core charge for \(\mathrm{Li} ?\)

Short Answer

Expert verified
The core charge for both Na (sodium) and Li (lithium) is +1, meaning they're the same.

Step by step solution

01

Determine the number of protons and inner shell electrons for Na

Sodium (Na) is the 11th element on the periodic table, which means it has 11 protons. As for inner shell electrons, sodium has 10. The first shell has 2 electrons and the second shell has 8 electrons.
02

Calculate the Core Charge for Na

The core charge is calculated using the formula: Core Charge = Number of protons - Number of inner shell electrons. So for sodium, the core charge = 11 (protons) - 10 (inner shell electrons) = +1.
03

Determine the number of protons and inner shell electrons for Li

Lithium (Li) is the third element on the periodic table, which means it has 3 protons. As for inner shell electrons, lithium has 2. The first shell has 2 electrons.
04

Calculate the Core Charge for Li

Using the formula from step 2, for lithium, the core charge = 3 (protons) - 2 (inner shell electrons) = +1.
05

Compare the Core Charges

Once both core charges are calculated, it's seen that both sodium and lithium have the same core charge, which is +1.

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Most popular questions from this chapter

a) Why is the nuclear charge of \(\mathrm{Be}^{\prime \prime}+4^{\prime \prime}\) ? b) How many inner-shell electrons does Be have? c) How many valence electrons does Be have? d) Show how the core charge for Be was calculated. e) Based on your answers to CTQs \(1,3 \mathrm{c}\), and \(3 \mathrm{~d}\), what is the relationship between the number of valence electrons and the core charge of a neutral atom?

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 \(\mathrm{Be}(0.90 \mathrm{MJ} / \mathrm{mole})\).

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

a) Based on its position in the periodic table, predict the valence shell, core charge, and number of valence electrons for \(\mathrm{Rb}\) and add these values to Table 1 . b) Using the shell model and referring to the Coulombic Potential Energy relationship (equation in Model 1, CA 3), explain clearly how the IE \(_{1}\) for \(\mathrm{Rb}\) is consistent with your answer to part a.

Complete the following table: $$ \begin{array}{|c|c|c|c|c|} \hline \text { Atom } & \begin{array}{c} \text { Total number } \\ \text { of electrons } \end{array} & \begin{array}{c} \text { Number of } \\ \text { valence shell } \\ \text { electrons } \end{array} & \begin{array}{c} \text { Number of } \\ \text { inner shell } \\ \text { electrons } \end{array} & \text { Core Charge } \\ \hline \text { H } & 1 & & & \\ \hline \text { He } & & & & \\ \hline \text { Li } & & & & \\ \hline \end{array} $$
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