See the General ChemistryNow CD-ROM or website, Screen 7.7...

See the General ChemistryNow CD-ROM or website, Screen 7.7 Bohr's Model of the Hydrogen Atom, Simulation. A photon with a wavelength of $97.3 \mathrm{nm}$ is fired at a hydrogen atom and leads to the emission of light. How many emission lines are emitted? Explain why more than one line is emitted.

Key Concepts

Bohr Model of the Hydrogen Atom

This model describes the hydrogen atom as having electrons in fixed, quantized orbits with specific energy levels. Electrons can move between these levels by absorbing or emitting discrete amounts of energy, which explains the distinct spectral lines observed in hydrogen's emission or absorption spectra.

Photon Absorption

When a photon with sufficient energy interacts with an electron in an atom, the electron can absorb the photon and jump to a higher energy level. The energy of the photon must exactly match the difference between the energy levels, making the process highly selective and quantized.

Electron Transitions and Cascade Emissions

After an electron is excited to a higher energy level, it does not necessarily return to the ground state in one step. Instead, it can transition through multiple lower intermediate levels, emitting one photon for each drop. This multi-step process, known as a cascade, results in the emission of multiple spectral lines.

Emission Spectrum

The emission spectrum, which is characteristic of the element, is generated by the photons emitted during the electron transitions between energy levels. Each emission line corresponds to a specific energy difference between two levels, explaining why more than one line is seen when an excited electron returns to the ground state.

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