SUMMARY
Copper (Cu) has one valence electron but can lose more than one when forming cupric compounds (Cu²⁺). This occurs due to the stability of filled orbitals, where an electron from the 4s orbital can transition to the 3d orbital, resulting in the electronic configuration of 3d¹⁰4s¹. The ability of copper to lose multiple electrons is attributed to the stability gained from having a fully filled 3d subshell, which allows for the loss of additional electrons beyond the single valence electron.
PREREQUISITES
- Understanding of atomic structure and electron configuration
- Familiarity with transition metals and their properties
- Knowledge of cupric compounds and oxidation states
- Basic principles of stability in electron orbitals
NEXT STEPS
- Research the electronic configuration of transition metals, focusing on copper
- Study the formation and properties of cupric compounds
- Learn about the stability of filled vs. half-filled orbitals in transition metals
- Explore the concept of oxidation states in transition metals
USEFUL FOR
Chemistry students, educators, and professionals interested in transition metal chemistry and the behavior of copper in various chemical contexts.