Bohr's quantization condition
Electron angular momentum is quantized as discrete values.
Allowed stationary orbits
Electrons in stable, non-radiating orbits with quantized radii and velocities.
Energy absorption — process?
Electron absorbs photon energy to move to a higher energy level.
Energy emission — process?
Electron releases photon energy when transitioning to a lower level.
Hydrogen atom model
Electron orbits nucleus in quantized circular paths with negative total energy.
Energy levels — formula?
En = -13.6 eV / n², with n as quantum number.
Spectral lines — origin?
Electron transitions between quantized energy levels emit or absorb photons.
Hydrogen-like atoms
Atoms with one electron but different nuclear charges Z, like He⁺.
Effect of Z on radius
Radius scales as r ∝ n² / Z, decreasing with higher Z.
Effect of Z on energy
Energy levels Eₙ ∝ -Z² / n², more negative with higher Z.
Excitation energy
Minimum energy to raise an electron to an excited state.
Ionization energy
Energy needed to remove an electron completely from atom.
Limitations — multi-electron atoms?
Bohr's model cannot explain multi-electron interactions and spectra.
Limitations — spectral structure?
Fails to explain fine spectral line splitting and Zeeman effect.
Assumption of orbits?
Only circular orbits; ignores elliptical orbits and wave nature.
Spectral series — example?
Lyman (n=1), Balmer (n=2), Paschen (n=3) series.
Test your knowledge with 8 questions on Atomic Structure and Spectra.
1. How is Bohr's quantization condition applied to determine the properties of an electron's orbit in practice?
2. What is the key property that defines allowed stationary orbits in Bohr's model of the atom?
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