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Chapter 9: Problem 80

The highest first ionization energy of the following is that of (a) \(\mathrm{Cs}_{i}\) (b) \(\mathrm{Cl}_{i}\) (c) I; (d) Li.

Short Answer

Expert verified
The element with the highest first ionization energy is Cl

Step by step solution

01

Understanding the concept of ionization energy

Ionization energy is the energy required to remove an electron from an atom. It increases from left to right across a period and decreases from top to bottom down a group in the Periodic Table.
02

Positioning the given elements on the Periodic Table

On a Periodic Table, you can observe that Cs is placed at the bottom left, I and Cl are in the same group (Group 17 - Halogens), but I is placed below Cl, and Li is placed at the top left.
03

Identifying the trend

Considering the periodic trends in ionization energy, we can infer that Cl should have the highest ionization energy among the given elements because it's further to the right of Li (meaning it's more electronegative and holds onto its electrons more tightly) and above I (meaning it's less shielded and its effective nuclear charge is greater, which also means it holds onto its electrons more tightly). In contrast, Cs should have the lowest ionization energy because it's at the bottom left of the Periodic Table.

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Most popular questions from this chapter

The element whose atoms have the electron configuration \([\mathrm{Kr}] 4 d^{10} 5 \mathrm{s}^{2} 5 p^{3}(\mathrm{a})\) is in group 13 of the periodic table; (b) bears a similarity to the element Bi; (c) is similar to the element \(\mathrm{Te} ;\) (d) is a transition element.

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. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

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