Hydrogen Spectrum Simulation | Physics & Chemistry

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Hydrogen Spectrum Simulation

Concept Quiz

Bohr Model & The Rydberg Equation

Niels Bohr proposed that electrons orbit the nucleus in specific, quantized energy levels ($n=1, 2, 3...$). An electron transitioning between these states emits or absorbs a photon of specific energy, creating spectral lines.

$$ \Delta E = \left| -13.6 \text{ eV} \left( \frac{1}{n_f^2} - \frac{1}{n_i^2} \right) \right| = \frac{hc}{\lambda} $$

$n_i$ = Initial Orbit  |  $n_f$ = Final Orbit
Lyman Series: Transitions down to $n=1$ (Ultraviolet)
Balmer Series: Transitions down to $n=2$ (Visible Light)
Paschen Series: Transitions down to $n=3$ (Infrared)

Note: Orbit radii in the animation use a pseudo-linear scale for visual clarity, rather than the exact $r \propto n^2$ scale which would push outer orbits off-screen.

Transition Controls

Initial State ($n_i$) n = 1 (Ground State) n = 2 n = 3 n = 4 n = 5 n = 6

Final State ($n_f$) n = 1 (Ground State) n = 2 n = 3 n = 4 n = 5 n = 6

Quick Presets

Photon Data

Emission

Initial Energy ($E_i$) -1.51 eV

Final Energy ($E_f$) -3.40 eV

Energy Diff ($\Delta E$) 1.89 eV

Photon Wavelength (λ)

656.3 nm Visible (Red)

Energy Level Diagram

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