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Chapter 7: Problem 124

For each of the following pairs of elements $$(\mathrm{Mg} \text { and } \mathrm{K}) \quad(\mathrm{F} \text { and } \mathrm{Cl})$$ pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

Short Answer

Expert verified
In summary: For Mg and K: a. Mg has a more favorable electron affinity. b. Mg has a higher ionization energy. c. K has a larger atomic size. For F and Cl: a. F has a more favorable electron affinity. b. F has a higher ionization energy. c. Cl has a larger atomic size.

Step by step solution

01

a. More favorable (exothermic) electron affinity

Since Mg and K belong to different periods, but Mg is higher up in the periodic table than K, Mg has a more favorable electron affinity.
02

b. Higher ionization energy

Since Mg and K belong to different groups, but Mg is to the right of K, Mg has a higher ionization energy.
03

c. Larger size

Since Mg and K belong to different periods, but Mg is higher up in the periodic table than K, K has a larger atomic size. For F (Fluorine) and Cl (Chlorine):
04

a. More favorable (exothermic) electron affinity

F and Cl belong to the same group, but F is higher up than Cl, F has a more favorable electron affinity.
05

b. Higher ionization energy

F and Cl belong to the same group, but F is higher up than Cl, F has a higher ionization energy.
06

c. Larger size

Since F and Cl belong to the same group, but F is higher up in the periodic table than Cl, Cl has a larger atomic size.

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