Modèle atomique et spectre de l'hydrogène
Hydrogen emits light only at specific wavelengths, and those lines are a direct readout of its energy levels. This simulation lets you excite the atom and watch electrons drop between levels, producing the matching spectral line each time.
Comment utiliser cette simulation
- Excite the electron to a chosen energy level
- Let it drop and watch the emitted photon
- Compare the emission and absorption spectra
Ce qu’il faut observer
- Only certain wavelengths appear — the spectrum is lines, not a continuum
- Bigger energy jumps produce shorter-wavelength photons
- Absorption lines fall at exactly the same wavelengths as emission lines
La physique derrière
Electrons occupy discrete energy levels with E_n = −13.6/n² eV. A transition from level n₁ to a lower n₂ emits a photon whose energy is exactly the difference, so hf = E₁ − E₂. Transitions ending at n = 2 give the visible Balmer series; those ending at n = 1 give ultraviolet Lyman lines.