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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![**Question:**
Explain why the term symbols for an \( np^4 \) electron configuration are the same as for an \( np^2 \) electron configuration.
**Explanation:**
In atomic physics, term symbols provide important information about the angular momentum and spin states of electrons within an atom. The similarity in term symbols for \( np^4 \) and \( np^2 \) configurations arises from the inherent symmetry and complementary nature of electron pairing.
- **Electron Configuration:** For both \( np^2 \) and \( np^4 \), the term symbols reflect the possible arrangements of electrons and their resultant states. This is because a filled \( p \) shell has six electrons, and the complement of \( 2 \) electrons in a configuration (like \( np^4 \)) will have similar term symbols as the direct configuration (like \( np^2 \)) due to the addition of two missing electron spaces that mimic the presence of the electrons in the \( np^2 \) configuration.
- **Hund's Rule and Symmetry:** According to Hund's rule, the configurations will exhibit the same sets of term symbols due to their complementary nature—what one configuration lacks, the other has, leading to overall symmetrical arrangements in terms of orbital filling and electron pairing.
**Implications:**
Understanding these symmetries helps to predict and rationalize the behavior of elements based on their electron configurations, crucial for applications in spectroscopy and quantum chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3ac106f3-a177-400f-8063-f0df96f817c6%2F6afb34b9-90e5-4bbc-a9e2-d102d3b09151%2Fhsn7ggz_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
Explain why the term symbols for an \( np^4 \) electron configuration are the same as for an \( np^2 \) electron configuration.
**Explanation:**
In atomic physics, term symbols provide important information about the angular momentum and spin states of electrons within an atom. The similarity in term symbols for \( np^4 \) and \( np^2 \) configurations arises from the inherent symmetry and complementary nature of electron pairing.
- **Electron Configuration:** For both \( np^2 \) and \( np^4 \), the term symbols reflect the possible arrangements of electrons and their resultant states. This is because a filled \( p \) shell has six electrons, and the complement of \( 2 \) electrons in a configuration (like \( np^4 \)) will have similar term symbols as the direct configuration (like \( np^2 \)) due to the addition of two missing electron spaces that mimic the presence of the electrons in the \( np^2 \) configuration.
- **Hund's Rule and Symmetry:** According to Hund's rule, the configurations will exhibit the same sets of term symbols due to their complementary nature—what one configuration lacks, the other has, leading to overall symmetrical arrangements in terms of orbital filling and electron pairing.
**Implications:**
Understanding these symmetries helps to predict and rationalize the behavior of elements based on their electron configurations, crucial for applications in spectroscopy and quantum chemistry.
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