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Chapter 9: Problem 55

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

Short Answer

Expert verified
Al has smaller atomic radius and lower first ionization energy than Ge. In has larger atomic radius and lower first ionization energy than Ge. Se has smaller atomic radius and higher first ionization energy than Ge.

Step by step solution

01

- Comparing with Aluminum (Al)

Aluminum (Al) is located above and to the left of Germanium (Ge) in the periodic table. Thus, relative to Ge, Al has a smaller atomic radius and a lower first ionization energy.
02

- Comparing with Indium (In)

Indium (In) is located below and to the left of Germanium (Ge) in the periodic table. Therefore, relative to Ge, In has a larger atomic radius and a lower first ionization energy.
03

- Comparing with Selenium (Se)

Selenium (Se) is located above and to the right of Germanium (Ge) in the periodic table. Thus, compared to Ge, Se has a smaller atomic radius and a higher first ionization energy.

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Most popular questions from this chapter

How much energy, in joules, must be absorbed to convert to \(\mathrm{Na}^{+}\) all the atoms present in \(1.00 \mathrm{mg}\) of gaseous Na? The first ionization energy of Na is \(495.8 \mathrm{kJ} / \mathrm{mol}.\)

Which of the following ions are unlikely to be found in chemical compounds: \(\mathrm{K}^{+}, \mathrm{Ga}^{4+}, \mathrm{Fe}^{6+} \mathrm{S}^{2-}, \mathrm{Ge}^{5+},\) or \(\mathrm{Br}^{-} ?\) Explain briefly.

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Give the symbol of the element (a) in group 14 that has the smallest atoms; (b) in period 5 that has the largest atoms; (c) in group 17 that has the lowest first ionization energy.
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