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Listed below are the ionization energies for the first six ionizations of an imaginary element: 1st IE= 1,100 kJ/mol 2nd IE = 1,950 kJ/mol 3rd IE = 5,890 kJ/mol 4th IE = 6,740 kJ/mol 5th IE= 8,120 kJ/mol 6th IE= 9,050 kJ/mol Why is the 2nd ionization energy higher than the 1st ionization energy? Check the two that apply. The 2nd electron removed is a core electron and core electrons are closer to the nucleus and experience a higher effective nuclear charge. The attractive force between the 2nd electron and the nucleus is weaker and requires more energy to overcome than the attractive force between the 1st electron and the nucleus. The 2nd electron removed is a valence electron, but it is closer to the nucleus because the 1+ cation that it was removed from is smaller than the neutral atom. The attractive force between the 2nd electron and the nucleus is stronger and requires more energy to overcome than the attractive force between the 1st electron and the nucleus.

Listed below are the ionization energies for the first six ionizations of an imaginary element: 1st IE= 1,100 kJ/mol 2nd IE = 1,950 kJ/mol 3rd IE = 5,890 kJ/mol 4th IE = 6,740 kJ/mol 5th IE= 8,120 kJ/mol 6th IE= 9,050 kJ/mol Why is the 2nd ionization energy higher than the 1st ionization energy? Check the two that apply. The 2nd electron removed is a core electron and core electrons are closer to the nucleus and experience a higher effective nuclear charge. The attractive force between the 2nd electron and the nucleus is weaker and requires more energy to overcome than the attractive force between the 1st electron and the nucleus. The 2nd electron removed is a valence electron, but it is closer to the nucleus because the 1+ cation that it was removed from is smaller than the neutral atom. The attractive force between the 2nd electron and the nucleus is stronger and requires more energy to overcome than the attractive force between the 1st electron and the nucleus.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter8: Electron Configurations And Periodicity
Section: Chapter Questions
Problem 8.29QP: Periodic Properties I A hypothetical element, X, has the following ionization energy values: First...
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Listed below are the ionization energies for the first six ionizations of an imaginary element: 1st IE= 1,100 kJ/mol 2nd IE = 1,950 kJ/mol 3rd IE = 5,890 kJ/mol 4th IE= 6,740 kJ/mol 5th IE= 8,120 kJ/mol 6th IE= 9,050 kJ/mol Why is the 2nd ionization energy higher than the 1st ionization energy? Check the two that apply. The 2nd electron removed is a core electron and core electrons are closer to the nucleus and experience a higher effective nuclear charge. The attractive force between the 2nd electron and the nucleus is weaker and requires more energy to overcome than the attractive force between the 1st electron and the nucleus. The 2nd electron removed is a valence electron, but it is closer to the nucleus because the 1+ cation that it was removed from is smaller than the neutral atom. The attractive force between the 2nd electron and the nucleus is stronger and requires more energy to overcome than the attractive force between the 1st electron and the nucleus.
Transcribed Image Text:Listed below are the ionization energies for the first six ionizations of an imaginary element: 1st IE= 1,100 kJ/mol 2nd IE = 1,950 kJ/mol 3rd IE = 5,890 kJ/mol 4th IE= 6,740 kJ/mol 5th IE= 8,120 kJ/mol 6th IE= 9,050 kJ/mol Why is the 2nd ionization energy higher than the 1st ionization energy? Check the two that apply. The 2nd electron removed is a core electron and core electrons are closer to the nucleus and experience a higher effective nuclear charge. The attractive force between the 2nd electron and the nucleus is weaker and requires more energy to overcome than the attractive force between the 1st electron and the nucleus. The 2nd electron removed is a valence electron, but it is closer to the nucleus because the 1+ cation that it was removed from is smaller than the neutral atom. The attractive force between the 2nd electron and the nucleus is stronger and requires more energy to overcome than the attractive force between the 1st electron and the nucleus.
Use the data table for the first eight ionization energies found for a particular element shown here to predict and explain which element would you expect to show this trend in successive ionization energies? Ionization Number 1st 2nd 3rd 4th 5th 6th 7th 8th 1. F 2. O Because 1 and 3 1 and 4 3. Core electrons are more strongly attracted to the nucleus than valence electrons. 4. Valence electrons release more energy when they are removed from the atom. O2 and 4 Energy (kJ/mol) O 2 and 3 1,314 3,388 5,300 7,469 10,990 13,327 71,330 84,078
Transcribed Image Text:Use the data table for the first eight ionization energies found for a particular element shown here to predict and explain which element would you expect to show this trend in successive ionization energies? Ionization Number 1st 2nd 3rd 4th 5th 6th 7th 8th 1. F 2. O Because 1 and 3 1 and 4 3. Core electrons are more strongly attracted to the nucleus than valence electrons. 4. Valence electrons release more energy when they are removed from the atom. O2 and 4 Energy (kJ/mol) O 2 and 3 1,314 3,388 5,300 7,469 10,990 13,327 71,330 84,078
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