Why does oxygen have a lower ionization energy than nitrogen?
Understand the Problem
The question is asking for an explanation of why the element oxygen has a lower ionization energy compared to nitrogen. This involves understanding the concepts of ionization energy, atomic structure, and electron configuration.
Answer
Greater electron repulsion in oxygen's 2p subshell.
The final answer is that oxygen has a lower ionization energy than nitrogen due to greater electron repulsion in its 2p subshell.
Answer for screen readers
The final answer is that oxygen has a lower ionization energy than nitrogen due to greater electron repulsion in its 2p subshell.
More Information
Despite the general trend of increasing ionization energy across a period, the half-filled stability of nitrogen's 2p subshell makes it more stable than oxygen, which experiences higher electron repulsion.
Tips
Common mistakes include overlooking the role of electron-electron repulsion and half-filled orbital stability. Remember to consider subshell configurations.
Sources
- Why is ionization energy of oxygen lower than nitrogen? - lavelle.chem.ucla.edu
- Why does oxygen have a lower ionization energy than nitrogen? - socratic.org
- Why does nitrogen have a higher ionization energy than oxygen? - socratic.org
AI-generated content may contain errors. Please verify critical information
