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Rank the following in increasing order of ionization energy by numbering them in order from 1 through 5, with 1 having the lowest ionization energy and 5 having the highest ionization energy. Ва Mg Sr Ве Са

Rank the following in increasing order of ionization energy by numbering them in order from 1 through 5, with 1 having the lowest ionization energy and 5 having the highest ionization energy. Ва Mg Sr Ве Са

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Understanding Ionization Energy: The Role of Electronic Structure** To comprehend why ionization energy follows a specific sequence, it's crucial to examine the underlying electronic structure of elements. Ionization energy refers to the amount of energy required to remove an electron from an atom in its gaseous state. The factors influencing this energy include: 1. **Nuclear Charge**: As the number of protons in the nucleus increases, the positive charge also increases. This stronger attraction between the positively charged nucleus and the negatively charged electrons makes it harder to remove an electron, thus increasing ionization energy. 2. **Electron Shielding**: Inner electrons can shield outer electrons from the full effect of the nuclear charge. As a result, even if the nuclear charge increases, the ionization energy might not increase as significantly if there is significant shielding. 3. **Orbital Penetration**: Electrons in s orbitals are closer to the nucleus on average than those in p orbitals in the same energy level. This proximity translates into higher ionization energy for s electrons due to reduced shielding and increased nuclear attraction. By analyzing these factors, we can explain variations in ionization energy across different elements and their respective orders. This understanding highlights the intricate balance between nuclear forces and electron distribution within an atom.
Transcribed Image Text:**Understanding Ionization Energy: The Role of Electronic Structure** To comprehend why ionization energy follows a specific sequence, it's crucial to examine the underlying electronic structure of elements. Ionization energy refers to the amount of energy required to remove an electron from an atom in its gaseous state. The factors influencing this energy include: 1. **Nuclear Charge**: As the number of protons in the nucleus increases, the positive charge also increases. This stronger attraction between the positively charged nucleus and the negatively charged electrons makes it harder to remove an electron, thus increasing ionization energy. 2. **Electron Shielding**: Inner electrons can shield outer electrons from the full effect of the nuclear charge. As a result, even if the nuclear charge increases, the ionization energy might not increase as significantly if there is significant shielding. 3. **Orbital Penetration**: Electrons in s orbitals are closer to the nucleus on average than those in p orbitals in the same energy level. This proximity translates into higher ionization energy for s electrons due to reduced shielding and increased nuclear attraction. By analyzing these factors, we can explain variations in ionization energy across different elements and their respective orders. This understanding highlights the intricate balance between nuclear forces and electron distribution within an atom.
**Activity: Ranking Ionization Energies** Rank the following elements in increasing order of ionization energy by numbering them from 1 through 5. Assign 1 to the element with the lowest ionization energy and 5 to the element with the highest ionization energy. - Ba [ ] - Mg [ ] - Sr [ ] - Be [ ] - Ca [ ] **Instructions:** Fill in the blanks with numbers 1 to 5 based on the elements' ionization energies. Remember, ionization energy generally increases across a period and decreases down a group in the periodic table. Use your knowledge of periodic trends to determine the correct order.
Transcribed Image Text:**Activity: Ranking Ionization Energies** Rank the following elements in increasing order of ionization energy by numbering them from 1 through 5. Assign 1 to the element with the lowest ionization energy and 5 to the element with the highest ionization energy. - Ba [ ] - Mg [ ] - Sr [ ] - Be [ ] - Ca [ ] **Instructions:** Fill in the blanks with numbers 1 to 5 based on the elements' ionization energies. Remember, ionization energy generally increases across a period and decreases down a group in the periodic table. Use your knowledge of periodic trends to determine the correct order.
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