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Consider the following ionization energies for aluminum : Al (g) → Al+ (g)  + e- I1 = 580 kJ/mol Al+(g) → Al2+ (g) + e- I2 = 1815 kJ/mol Al2+(g) → Al 3+ (g) + e- I3 = 2740 kJ/mol Al3+(g) → Al 4+ (g) + e- I4 = 11, 600kJ/mol a. Account for the trend in the values of the ionization energies. b. Explain the large increase between I3 and I4

Consider the following ionization energies for aluminum : Al (g) → Al+ (g)  + e- I1 = 580 kJ/mol Al+(g) → Al2+ (g) + e- I2 = 1815 kJ/mol Al2+(g) → Al 3+ (g) + e- I3 = 2740 kJ/mol Al3+(g) → Al 4+ (g) + e- I4 = 11, 600kJ/mol a. Account for the trend in the values of the ionization energies. b. Explain the large increase between I3 and I4

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the following ionization energies for aluminum :

Al (g) → Al+ (g)  + e- I1 = 580 kJ/mol

Al+(g) → Al2+ (g) + e- I2 = 1815 kJ/mol

Al2+(g) → Al 3+ (g) + e- I3 = 2740 kJ/mol

Al3+(g) → Al 4+ (g) + e- I4 = 11, 600kJ/mol

a. Account for the trend in the values of the ionization energies.

b. Explain the large increase between I3 and I4

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