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Chapter 7: Problem 104

In each of the following sets, which atom or ion has the smallest ionization energy? a. \(\mathrm{Ca}, \mathrm{Sr}, \mathrm{Ba}\) b. \(\mathrm{K}, \mathrm{Mn}, \mathrm{Ga}\) c. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) d. \(\mathrm{S}^{2-}, \mathrm{S}, \mathrm{S}^{2+}\) e. \(\mathrm{Cs}\), Ge, Ar

Short Answer

Expert verified
The atoms or ions with the smallest ionization energy in each set are: a. \(Ba\) b. \(K\) c. \(N\) d. \(S^{2-}\) e. \(Cs\)

Step by step solution

01

a. Ca, Sr, Ba

All three elements belong to Group 2 (alkaline earth metals) on the periodic table. As we move down the group from calcium (Ca) to strontium (Sr) to barium (Ba), ionization energy generally decreases. Therefore, the element with the smallest ionization energy in this set is \(Ba\).
02

b. K, Mn, Ga

All three elements belong to different groups in the same period (Period 4) on the periodic table. As we move across a period from left to right, ionization energy generally increases. Since potassium (K) is the furthest to the left in Period 4, it will have the smallest ionization energy in this set.
03

c. N, O, F

All three elements belong to different groups in the same period (Period 2) on the periodic table. As we move across a period from left to right, ionization energy generally increases. Nitrogen (N) is the furthest to the left, so it will have the smallest ionization energy in this set.
04

d. S²⁻, S, S²⁺

All three species have sulfur (S) with different oxidation states. The negatively charged ion (\(S^{2-}\)) has gained electrons and will require less energy to remove an electron compared to the neutral atom (S). The positively charged ion (\(S^{2+}\)) has lost electrons, making it more difficult to remove another electron. Thus, the species with the smallest ionization energy in this set is \(S^{2-}\).
05

e. Cs, Ge, Ar

In this set, we have elements from three different groups on the periodic table. Cesium (Cs) is in Group 1 and is the furthest down the periodic table, which means it will have the lowest ionization energy due to the increased distance between the nucleus and the outer electrons. Germanium (Ge) is in Group 14, and Argon (Ar) is in Group 18 (a noble gas), both having higher ionization energies than Cs. Therefore, the element with the smallest ionization energy in this set is \(Cs\).

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