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: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter6: The Periodic Table And Periodic Law
Section: Chapter Questions
Problem 66A
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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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