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Chapter 5: Problem 22

Based on its position in the periodic table, what is the valence shell and what is the core charge for C? Explain your reasoning.

Short Answer

Expert verified
For carbon (C), the valence shell is the second shell (2s2 2p2) and the core charge is +4. The reasoning is based on its position in the periodic table and understanding of atomic structure and electron configuration.

Step by step solution

01

Identify the Element's Position in the Periodic Table

You're being asked about C, carbon, which is found in group 14 and period 2 of the periodic table. This tells you about its electron configuration, which will help you determine the valence shell and core charge.
02

Determine the Electron Configuration

Referencing the periodic table, you can determine the electron configuration for carbon. Carbon, with atomic number 6, has 6 electrons. The electron configuration following the Aufbau principle is 1s2 2s2 2p2.
03

Determine the Valence Shell

The valence shell is identified as the highest principal quantum number in the electron configuration. Here it is \(n=2\), thus the valence shell for carbon is the \(2s2 2p2\). This is the outermost shell and contains the electrons that are associated with bonding.
04

Determine the Core Charge

The core charge is the effective nuclear charge felt by the valence electrons. It can be calculated as the number of protons in the nucleus (which is the atomic number, 6 for carbon) minus the number of electron in the inner shells (core electrons). Therefore, for carbon, the core charge is \(6 - 2 = 4\).

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Most popular questions from this chapter

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

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?

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.

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

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.
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