Consider the first ionization energy for nitrogen (N) and oxygen (O). Of the two, which one has the highest first ionization energy? 1. Nitrogen 2. Oxygen Because 1. It is easier to remove an electron from a px orbital compared to a py 2. It is easier to remove an electron if there are only five valence electrons vs. six. 3. It is easier to remove an electron from a doubly occupied orbital due to electron-electron repulsion. 4. It is easier to remove an electron from a singly occupied orbital because electrons want to be paired.
Consider the first ionization energy for nitrogen (N) and oxygen (O). Of the two, which one has the highest first ionization energy? 1. Nitrogen 2. Oxygen Because 1. It is easier to remove an electron from a px orbital compared to a py 2. It is easier to remove an electron if there are only five valence electrons vs. six. 3. It is easier to remove an electron from a doubly occupied orbital due to electron-electron repulsion. 4. It is easier to remove an electron from a singly occupied orbital because electrons want to be paired.
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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Consider the first ionization energy for nitrogen (N) and oxygen (O). Of the two, which one has the highest first ionization energy?
1. Nitrogen
2. Oxygen
Because
1. It is easier to remove an electron from a px orbital compared to a py
2. It is easier to remove an electron if there are only five valence electrons vs. six.
3. It is easier to remove an electron from a doubly occupied orbital due to electron-electron repulsion.
4. It is easier to remove an electron from a singly occupied orbital because electrons want to be paired.
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