Modern Physics · Physics

Models of the Hydrogen Atom Simulation

Shine light on a hydrogen atom and compare the classical, plum-pudding and Bohr models. Only the Bohr atom absorbs and emits the exact lines the spectrometer records.

Interactive virtual lab · no download · works on phones and laptops

Chapter: Atoms
For: Class 12 · JEE · NEET
Time: ~15 min

Models of the Hydrogen Atom is a Pro simulation

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How to use it

1Choose a model, then switch on the light.
2Use white light, or a single wavelength from the slider.
3Watch the electron jump and the spectrometer collect emitted photons.
4Open the energy diagram to see each transition.

What to notice

Bohr energies are Eₙ = −13.6/n² eV, and orbit radii grow as n².
A photon is absorbed only if its energy matches a gap between levels.
Drops to n = 1 give the Lyman (UV) series, to n = 2 the visible Balmer series.
The classical atom would spiral in and collapse — the model fails.

For teachers

A ready-made teaching kit comes with this lab

Lesson plan
23 min, 4 steps
Ask the class
3 questions with answers
Quick quiz
7 questions, printable
Key formulas
3 formulas

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About the Models of the Hydrogen Atom simulation

Models of the hydrogen atom improved as experiments demanded. Thomson's plum pudding and a classical orbiting electron could not explain why hydrogen gives off light at only certain wavelengths. Bohr's model fixed the electron to allowed orbits with energy −13.6/n² eV; jumping between them emits or absorbs a photon of exactly the energy difference.

In this models of the hydrogen atom simulation you shine white light or one wavelength at a billiard-ball, plum-pudding, classical or Bohr atom, see which photons are absorbed and emitted, and follow the electron on an energy-level diagram. It covers Atoms in Class 12, JEE and NEET.

Also covers: bohr model, plum pudding, spectral lines, balmer, lyman, energy levels, rydberg.