This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Trends in Ionization Energy: Across a period: Ionization energy generally increases*. For example, Li has I_1 = 520.2 kJ/mol, while Be has I_1 = 899.5 kJ/mol. This is due to increasing nuclear charge and decreasing atomic radius, which holds valence electrons more tightly. Down a group: Ionization energy generally decreases*. This occurs because atomic radius increases and inner electrons shield the valence electrons more effectively, making them easier to remove. (The provided table does not contain data to illustrate this trend). Alkali Metals (e.g., Lithium): Lithium (1s^2 2s^1) readily loses its single valence electron (I_1 = 520.2 kJ/mol) to form a stable Li^+ ion with a 1s^2 (noble gas) electron configuration. The second ionization energy (I_2 = 7298.2 kJ/mol) is significantly higher (approximately 14 times I_1) because it requires removing an electron from a stable, full inner shell. Therefore, forming +2 or +3 ions is energetically unfavorable. Alkaline Earth Metals (e.g., Beryllium): Beryllium (1s^2 2s^2) readily loses both its valence electrons (I_1 = 899.5 kJ/mol, I_2 = 1757.1 kJ/mol) to form a stable Be^2+ ion with a 1s^2 (noble gas) electron configuration. The third ionization energy (I_3 = 14848.8 kJ/mol) is significantly higher (approximately 8.5 times I_2) because it requires removing an electron from a stable, full inner shell. Therefore, forming +3 or +4 ions is energetically unfavorable. That's 2 down. 3 left today — send the next one.