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Chapter 8: Problem 101

The ionization energies of sodium (in \(\mathrm{kJ} / \mathrm{mol}\) ), starting with the first and ending with the eleventh, are 495.9,4560,6900,9540,13,400,16,600,20,120 \(25,490,28,930,141,360,170,000 .\) Plot the log of ionization energy \((y\) axis \()\) versus the number of ionization \((x\) axis \() ;\) for example, \(\log 495.9\) is plotted versus 1 (labeled \(I_{1}\), the first ionization energy), log 4560 is plotted versus 2 (labeled \(I_{2}\), the second ionization energy), and so on. (a) Label \(I_{1}\) through \(I_{11}\) with the electrons in orbitals such as \(1 s, 2 s, 2 p,\) and \(3 s .\) (b) What can you deduce about electron shells from the breaks in the curve?

Short Answer

Expert verified
Interpreting from the plot of log of ionization energies versus the number of ionization, the breaks in the curve indicates the completion of one shell and the start of another. A break in the curve means the next electron is considerably harder to remove, and hence, it must be in a filled lower energy level.

Step by step solution

01

Getting the Logarithmic Values

First of all, we need to find the logarithmic values of the given ionization energies. They will be plotted on the y-axis. By using the logarithmic formula \( \log x \), find the log values for each ionization energy.
02

Creating the Plot

Next, create a plot where the y-axis represents the log ionization energy and the x-axis represents the number of ionization, ranging from \( I_{1} \) to \( I_{11} \). Plot the log values found in Step 1 versus their corresponding ionization number.
03

Labeling the Electrons in Orbitals

Once the graph is plotted, label \( I_{1} \) through \( I_{11} \) with the electrons in orbitals such as \(1 s, 2 s, 2 p,\) and \(3 s \). This represents the orbitals that the electrons were in before ionization.
04

Deduction from the Breaks in the Curve

We need to analyze the breaks in the curve on the graph. From these breaks, we can deduce which energy level (shell) the electron moved from during the ionization process. A much larger jump in ionization energy typically indicates that we have removed all the electrons from a shell and the remaining ones are closer to the nucleus and more strongly attracted to it.

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Most popular questions from this chapter

Define valence electrons. For representative elements, the number of yalence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\).

An ion \(\mathrm{M}^{2+}\) derived from a metal in the first transition metal series has four and only four electrons in the \(3 d\) subshell. What element might \(\mathrm{M}\) be?

Explain which of these ions is larger, and why: \(\mathrm{Cu}^{+}\) or \(\mathrm{Cu}^{2+}\).

Write the empirical (or molecular) formulas of compounds that the elements in the third period (sodium to chlorine) are expected to form with (a) molecular oxygen and (b) molecular chlorine. In each case indicate whether you expect the compound to be ionic or molecular.

Describe the general layout of a modern periodic table.
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