112. Consider the following ionization energies for aluminum. Al(g) → Alt(g) + e Alt(g) → Al²(g) + e Al²(g) → Al³+(g) + e 1₁ = 580 kJ/mol 12 = 1815 kJ/mol 13 = 2740 kJ/mol Al³+ (g) → Al4+(g) + e* 14 11600 kJ/mol a. Account for the increasing trend in the values of the ionization energies. Explain the large increase between 13 and 14. Which one of the four ions has the greatest electron affinity? Explain. List the four aluminum ions given in the preceding reactions in order of increasing size, and explain your ordering. (Hint: Remember that most of the size of an atom or ion is due to its electrons.) b. C. d.
112. Consider the following ionization energies for aluminum. Al(g) → Alt(g) + e Alt(g) → Al²(g) + e Al²(g) → Al³+(g) + e 1₁ = 580 kJ/mol 12 = 1815 kJ/mol 13 = 2740 kJ/mol Al³+ (g) → Al4+(g) + e* 14 11600 kJ/mol a. Account for the increasing trend in the values of the ionization energies. Explain the large increase between 13 and 14. Which one of the four ions has the greatest electron affinity? Explain. List the four aluminum ions given in the preceding reactions in order of increasing size, and explain your ordering. (Hint: Remember that most of the size of an atom or ion is due to its electrons.) b. C. d.
Introductory Chemistry: A Foundation
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Chapter12: Chemical Bonding
Section: Chapter Questions
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Transcribed Image Text:112. Consider the following ionization energies for aluminum.
Al(g) → Alt(g) + e
Al* (g) → Al²(g) + e
Al²(g) → Al³+(g) + e*
Al³+ (g) → AI4+(g) + e*
1₁ = 580 kJ/mol
1₂ = 1815 kJ/mol
13 = 2740 kJ/mol
14 = 11600 kJ/mol
Account for the increasing trend in the values of the ionization
energies.
b. Explain the large increase between 13 and 14.
C. Which one of the four ions has the greatest electron affinity? Explain.
d. List the four aluminum ions given in the preceding reactions in order
of increasing size, and explain your ordering. (Hint: Remember that
most of the size of an atom or ion is due to its electrons.)
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