Hydrogen Spectrum Simulation

The Hydrogen Atom & Its Spectrum

The simplest atom, hydrogen, consists of a single proton and a single electron. The Bohr model successfully explains its distinct spectral lines. Electrons can only occupy specific quantized energy levels (orbits), denoted by the principal quantum number '$n$'.

When an electron jumps from a higher energy level to a lower one, it emits a photon of light with energy exactly equal to the difference between the levels. Conversely, it absorbs a photon to jump to a higher level. These emitted/absorbed photons correspond to specific wavelengths, forming the line spectrum of hydrogen.

How to Use the Simulation

• The Atomic View (top-left) shows the electron orbiting the nucleus.
• The Energy Level Diagram (bottom-left) shows the allowed energy states for the electron.
• The Spectral Series View (right) visualizes the different series of spectral lines.
• Click on any energy level in the Energy Level Diagram to move the electron to that orbit.
• Use "Excite Electron" to jump it to a random higher level (simulating absorption).
• Use "De-excite Electron" to make it fall to a random lower level (simulating emission).
• The Spectral Output at the bottom will show the calculated photon properties for each transition.