To solve the problem, we need to identify which of the given electronic configurations violates Hund's rule.
1. Understanding Hund's Rule:
Hund's rule states that when electrons occupy degenerate orbitals (orbitals of the same energy), they will first fill each orbital singly with parallel spins before pairing up. In other words, each orbital in a subshell should get one electron before any orbital gets a second electron.
2. Analyzing the Given Configurations:
- Option (A): The configuration shows that all electrons are paired up in the orbital. This violates Hund's rule because the electrons should be unpaired and occupy degenerate orbitals with parallel spins before pairing.
- Option (B): This configuration follows Hund's rule because the electrons are unpaired in the orbitals with parallel spins.
- Option (C): This configuration also follows Hund's rule as the electrons are unpaired in the orbitals with parallel spins.
- Option (D): This configuration violates Hund's rule because there is a single electron in the orbital with a lower energy level being paired before occupying the degenerate orbitals in a way that violates the rule.
Final Answer:
The configuration in Option (D) violates Hund's rule.
