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Chapter 5: Problem 1

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

Short Answer

Expert verified
The completed table will be: \[ \begin{array}{|c|c|c|c|c|} \hline \text { Atom } & \begin{array}{c} \text { Total number } \ \text { of electrons } \end{array} & \begin{array}{c} \text { Number of } \ \text { valence shell } \ \text { electrons } \end{array} & \begin{array}{c} \text { Number of } \ \text { inner shell } \ \text { electrons } \end{array} & \text { Core Charge } \ \hline \text { H } & 1 & 1 & 0 & 1 \ \hline \text { He } & 2 & 2 & 0 & 2 \ \hline \text { Li } & 3 & 1 & 2 & 1 \ \hline \end{array} \]

Step by step solution

01

Filling up electron configuration table for Hydrogen (H)

Hydrogen has atomic number 1, so it has 1 electron. This single electron is also the valence electron as Hydrogen has only one energy level. Therefore, there are no inner shell electrons and the core charge is \(1-0 = 1\).
02

Filling up electron configuration table for Helium (He)

Helium has atomic number 2, therefore, it has 2 electrons. Both electrons fill the 1st energy level, so it has 2 valence electrons and no inner shell electrons. The core charge is \(2-0 = 2\).
03

Filling up electron configuration table for Lithium (Li)

Lithium's atomic number is 3, meaning it has 3 electrons. Two of these fill the 1st energy level (inner shell electrons) and the third is in the 2nd energy level (the valence electron). The core charge in this case is \(3-2 = 1\).

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Most popular questions from this chapter

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.

Within our model and referring to the Coulombic Potential Energy expression, explain why the \(\mathrm{IE}_{1}\) increases from left to right across a row of the periodic table.

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?

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

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