SUMMARY
The electronic configurations of chromium (Cr), copper (Cu), rhodium (Rh), and iridium (Ir) exhibit anomalies due to stability preferences in their d-orbitals. Specifically, Rh adopts the configuration [Kr] 4d8 5s1 instead of the expected [Kr] 4d7 5s2, while Ir prefers [Xe] 4f14 5d7 6s2 over [Xe] 4f14 5d8 6s1. These deviations are attributed to the increased stability associated with half-filled and fully filled d-orbitals, which lower the overall energy of the atom. Understanding these configurations is crucial for grasping transition metal chemistry.
PREREQUISITES
- Understanding of electron configurations and the Aufbau principle
- Familiarity with transition metals and their properties
- Knowledge of quantum mechanics principles related to atomic structure
- Basic grasp of periodic table trends and anomalies
NEXT STEPS
- Research the stability of half-filled and fully filled d-orbitals in transition metals
- Study the electronic configurations of other transition metals for comparison
- Explore the role of electron-electron repulsion in determining atomic stability
- Learn about the implications of electronic configuration on chemical reactivity and bonding
USEFUL FOR
Chemistry students, educators, and anyone interested in the electronic structure of transition metals and their implications in chemical behavior.
