SUMMARY
The discussion clarifies the definition of 'ground state' in quantum mechanics, specifically in relation to the hydrogen atom (H) and the hydrogen anion (H-). The ground state is defined as the lowest energy state of a system, which for the hydrogen atom is -13.6 eV, while the hydrogen anion has a lower energy of -14.35 eV. However, H- is not classified as a ground state because it represents a different system with distinct energy levels, not merely an extension of the proton-electron system. The orbital notation for the H- ion is confirmed to be 1s2.
PREREQUISITES
- Understanding of quantum mechanics principles
- Familiarity with atomic structure and energy levels
- Knowledge of hydrogen atom and hydrogen anion properties
- Basic skills in interpreting orbital notation
NEXT STEPS
- Research the energy levels of hydrogen anions and their implications
- Study the differences between proton-electron systems and multi-electron systems
- Explore quantum mechanics definitions of ground state and excited states
- Learn about orbital notation and its application in various atomic systems
USEFUL FOR
Students and professionals in physics, particularly those studying quantum mechanics, atomic structure, and anyone interested in the properties of hydrogen and its ions.