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Chapter 8: Problem 153

Using the following boiling-point data, estimate the boiling point of francium: $$ \begin{array}{l|l|l|l|l|l|l} \text { Metal } & \mathrm{Li} & \mathrm{Na} & \mathrm{K} & \mathrm{Rb} & \mathrm{Cs} & \mathrm{Fr} \\ \hline \text { B.p. }\left({ }^{\circ} \mathrm{C}\right) & 1347 & 882.9 & 774 & 688 & 678.4 & ? \end{array} $$

Short Answer

Expert verified
The exact prediction would depend on the calculated average decrease, however the boiling point of Francium should be less than 678.4 degrees Celsius.

Step by step solution

01

Identify Trend in Boiling Points

Examine the given data of the boiling points of alkali metals from Li to Cs. You can see a trend where the boiling point decreases as we go down the group in the periodic table.
02

Find Rate of Decrease

Calculate the rate of decrease of the boiling point from one alkali metal to the next, by subtracting the boiling point of an alkali metal from the boiling point of the metal above it in the periodic table. Average these values to get an overall rate of decrease.
03

Estimate the Boiling Point of Francium

Use the overall rate of decrease to estimate the boiling point of Francium by subtracting the rate from the boiling point of Cesium.

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Most popular questions from this chapter

Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

To prevent the formation of oxides, peroxides, and superoxides, alkali metals are sometimes stored in an inert atmosphere. Which of the following gases should not be used for lithium: \(\mathrm{Ne}, \mathrm{Ar}, \mathrm{N}_{2}, \mathrm{Kr} ?\) Explain. (Hint: As mentioned in the chapter, Li and Mg exhibit a diagonal relationship. Compare the common compounds of these two elements.)

Compare the work function for cesium ( \(206 \mathrm{~kJ} / \mathrm{mol}\) ) with its first ionization energy ( \(376 \mathrm{~kJ} / \mathrm{mol}\) ). Explain the difference.

Why do elements that have high ionization energies also have more positive electron affinities? Which group of elements would be an exception to this generalization?

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 \(I E_{1}\), the first ionization energy), \(\log 4560\) is plotted versus 2 (labeled \(I E_{2}\), the second ionization energy), and so on. (a) Label \(I E_{1}\) through \(I E_{11}\) 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?
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