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Chapter 7: Problem 44

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) $\mathrm{Cs}, \mathrm{Cl} ;(\mathbf{b}) \mathrm{Fe}, \mathrm{Zn} ;\( (c) \)\mathrm{I}, \mathrm{Cl} ;(\mathbf{d}) \mathrm{Se}, \mathrm{Sn}$

Short Answer

Expert verified
For each pair: (a) Cs has the smaller first ionization energy. (b) Fe has the smaller first ionization energy. (c) I has the smaller first ionization energy. (d) Sn has the smaller first ionization energy.

Step by step solution

01

Periodic Table Position

Locate Cs and Cl on the periodic table. Cs belongs to the alkali metal group (Group 1) and Cl belongs to the halogen group (Group 17).
02

Evaluate Ionization Energy Trend

Ionization energy increases from left to right across a period. Since Cl is located to the right of Cs within the same period, Cl has a higher first ionization energy than Cs. Thus, Cs has the smaller first ionization energy. #b) Fe vs Zn#
03

Periodic Table Position

Locate Fe and Zn on the periodic table. Both Fe (Iron) and Zn (Zinc) are part of the same period and belong to the transition metal group.
04

Evaluate Ionization Energy Trend

Ionization energy increases from left to right across a period. Since Fe is located to the left of Zn within the same period, Fe has a smaller first ionization energy than Zn. #c) I vs Cl#
05

Periodic Table Position

Locate I and Cl on the periodic table. Both elements belong to the halogen group (Group 17) and are in different periods.
06

Evaluate Ionization Energy Trend

Ionization energy decreases from top to bottom within a group. Since I is located below Cl within the same group, I has a smaller first ionization energy than Cl. #d) Se vs Sn#
07

Periodic Table Position

Locate Se and Sn on the periodic table. Se belongs to the Chalcogen group (Group 16) and Sn belongs to the Carbon group (Group 14).
08

Evaluate Ionization Energy Trend

Ionization energy decreases from top to bottom within a group and increases from left to right across a period. Since Se is located above and to the right of Sn, Se has a higher first ionization energy than Sn. Thus, Sn has the smaller first ionization energy.

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Most popular questions from this chapter

Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect? (i) The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom. (ii) Effective nuclear charge increases (iii) Valence going left to right across a row of the periodic table. electrons screen the nuclear charge more effectively than do core electrons. (iv) The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table. (v) The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table.

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