Bohr Hydrogen Spectrum

The Bohr model of the hydrogen atom provides an educational framework for understanding discrete energy levels and spectral lines. In this model, the electron is confined to circular orbits with specific quantized energies. The energy of the electron in the n-th level is given by E_n = -13.6 / n² eV, where n is a positive integer (the principal quantum number). The radius of the orbit is r_n = a₀n², where a₀ is the Bohr radius.

Compare spectral transitions

Open the Bohr Hydrogen Spectrum module and use its labeled controls to explore the model.

1. Set Initial level ni to 3 and Final level nf to 2. This represents the first line of the Balmer series (H-alpha). The module calculates the photon energy as approximately 1.88888888889 eV and the wavelength as 656.386932706 nm, characteristic of visible red light.
2. Set Initial level ni to 1 and Final level nf to 3. The atom transitions from a lower to a higher energy state, meaning it undergoes an Absorption process, capturing a photon of roughly 12.0888888889 eV.
3. Try setting both levels equal, e.g., Initial level ni to 1 and Final level nf to 1. The energy change is exactly 0 eV, and the wavelength is correctly marked as Unavailable: no transition.
4. Drag the visual display to explore the drawn orbits up to n=6, and use Reset view to restore the centered framing.