SUMMARY
The electron orbitals of Hydrogen (H) and Helium ion (He+) differ primarily due to the difference in nuclear charge. While both atoms have a single electron in a 1s orbital, He+ has a nuclear charge of +2 compared to H's +1. This increased positive charge in He+ results in a stronger electrostatic attraction between the nucleus and the electron, leading to lower energy levels for the electron in He+. Consequently, the energy levels of He+ are more negative than those of H, indicating that the electron in He+ is more tightly bound to the nucleus.
PREREQUISITES
- Understanding of the Bohr Model of the atom
- Basic knowledge of atomic structure and electron orbitals
- Familiarity with concepts of nuclear charge and electrostatic forces
- Ability to calculate energy levels using the formula for hydrogen-like atoms
NEXT STEPS
- Study the calculations for energy levels in hydrogen-like atoms using the formula E = -Z² * 13.6 eV/n²
- Explore the differences in electron configurations between hydrogen and helium
- Learn about the implications of increased nuclear charge on atomic spectra
- Investigate the quantum mechanical model of the atom for a deeper understanding of orbitals
USEFUL FOR
Students studying atomic physics, educators teaching quantum mechanics, and anyone interested in the differences between hydrogen and hydrogen-like ions.