Math

QuestionIndicate which species in each pair has the higher ionization energy. Select one or more: a. Between K and I,I\mathrm{I}, \mathrm{I} b. Between K and I,K\mathrm{I}, \mathrm{K} c. Between Al and Al+,Al\mathrm{Al}^{+}, \mathrm{Al} d. Between Al2\mathrm{Al}^{2} and Al+,Al+\mathrm{Al}^{+}, \mathrm{Al}^{+} e. Between Ar and Cl\mathrm{Cl}^{-}; Ar f. Between Ar and Cl,Cl\mathrm{Cl}^{-}, \mathrm{Cl}^{-} g. Between Mg and Ca,Mg\mathrm{Ca}, \mathrm{Mg} h. Between Mg and Ca,Ca\mathrm{Ca}, \mathrm{Ca}

Studdy Solution
Compare Mg and Ca: - Mg (Magnesium) is above Ca (Calcium) in Group 2 of the periodic table. - Ionization energy decreases down a group, so Mg has a higher ionization energy than Ca.
The species with higher ionization energy for each pair are: a. I b. (not applicable, as I is higher) c. Al+ \mathrm{Al}^{+} d. Al2+ \mathrm{Al}^{2+} e. Ar f. (not applicable, as Ar is higher) g. Mg h. (not applicable, as Mg is higher)

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