SUMMARY
The electronic transition of He II that emits a photon at 468.6 nm corresponds to the Pashen-alpha line. This transition can be analyzed using the equation \(\frac{1}{\lambda}=4R\left(\frac{1}{m^2}-\frac{1}{n^2}\right)\), where \(R\) is the Rydberg constant, \(m\) is the final energy level, and \(n\) is the initial energy level. The energy levels of He II, which is a once-ionized helium atom, can be modeled using the Bohr model with \(Z=2\). The values of \(n\) and \(m\) can be determined through trial and error, as they must be integer values close to the calculated wavelength.
PREREQUISITES
- Understanding of the Bohr model of the hydrogen atom
- Familiarity with the Rydberg formula for spectral lines
- Knowledge of electronic transitions in atomic physics
- Basic algebra for solving equations with two unknowns
NEXT STEPS
- Study the Rydberg formula in detail for various elements
- Learn about the differences between He I and He II in terms of electronic structure
- Explore the concept of spectral lines and their significance in quantum mechanics
- Investigate the application of the Bohr model to multi-electron systems
USEFUL FOR
Students of atomic physics, educators teaching quantum mechanics, and anyone interested in understanding electronic transitions in helium and other elements.