Physics · Interactive learning companion

Bohr Atomic Spectra of Hydrogen-Like Atoms

Explain line spectra through quantized energy gaps and clearly state the hydrogen-like approximation.

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📝 Description

Bohr Atomic Spectra of Hydrogen-Like Atoms is a visual simulation for exploring energy levels and spectral lines. Students connect atomic transitions with emitted or absorbed radiation, supporting understanding of the Bohr model, hydrogen-like atoms, and spectroscopy.

📋 Instructions

Adjust the available controls and observe transitions between energy levels. Compare spectral lines and use the simulation for atomic-structure revision.

🎓 Learning Guide: Bohr Atomic Spectra of Hydrogen-Like Atoms

Learning focus: Explain line spectra through quantized energy gaps and clearly state the hydrogen-like approximation.

Physics Interactive learning companion

Learning objectives

Recognize hydrogen-like ions as one-electron systems.
Connect bound-state transitions with discrete photon energies.

Concepts and principles

In the nonrelativistic Bohr model, E_n≈−13.6 Z²/n² eV for a hydrogen-like ion.
A downward transition emits a photon with energy equal to the difference between the levels.

Examples and worked solutions

For H, what is the photon energy for n=2 to n=1 in the Bohr approximation?: Worked solution: 13.6×(1−1/4)=10.2 eV.

Try this activity

Observe any selected initial and final energy levels in the simulation.
If atomic number Z or n levels are adjustable, change one at a time and compare energy gaps.
Clarify that the Bohr model is a simplified historical model and does not describe all atomic effects.

Expected observations and explanations

Larger energy gaps correspond to higher photon frequencies.

Assessment questions and answers

Why do one-electron ions have different line energies from hydrogen?: Answer: Their nuclear charge Z changes the Coulomb attraction; Bohr energies scale approximately as Z².