SUMMARY
The Bohr radius for single electron orbits is influenced by the nuclear charge of the ion. For ions such as He+, Li2+, and Be3+, the effective charge is represented as Ze, where Z is the number of protons and e is the elementary charge (1.60 × 10-19 C). Textbooks typically derive the Bohr radius using hydrogen as a reference and subsequently adjust for heavier, hydrogen-like ions. This adjustment is crucial for accurately calculating the radius in multi-proton systems.
PREREQUISITES
- Understanding of the Bohr model of the atom
- Familiarity with atomic structure and nuclear charge
- Basic knowledge of elementary charge (e)
- Concept of hydrogen-like ions
NEXT STEPS
- Study the derivation of the Bohr radius for hydrogen-like ions
- Explore the implications of nuclear charge on electron orbits
- Learn about quantum mechanics and its relation to atomic models
- Investigate the differences between hydrogen and multi-electron atoms
USEFUL FOR
Students of physics, educators teaching atomic theory, and researchers focusing on quantum mechanics and atomic structure will benefit from this discussion.