Hydrogen-spectrum wavelengths are specific wavelengths of light emitted or absorbed by hydrogen atoms as electrons transition between energy levels. These wavelengths form discrete lines in the spectrum, known as spectral lines.
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Hydrogen-spectrum wavelengths correspond to the energy differences between quantized electron orbits in a hydrogen atom.
The most important series of lines in the hydrogen spectrum are the Lyman, Balmer, and Paschen series.
Bohr's model of the atom successfully explained the observed spectral lines of hydrogen by quantizing electron orbits.
The Balmer series includes visible light wavelengths and is characterized by transitions where electrons fall to the n=2 orbit.
The formula for calculating hydrogen spectrum wavelengths is given by the Rydberg formula: $\frac{1}{\lambda} = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)$.
Review Questions
What are hydrogen-spectrum wavelengths, and how do they relate to electron transitions?
Which series in the hydrogen spectrum includes visible light wavelengths?
How does Bohr's model explain hydrogen-spectrum wavelengths?
Related terms
Rydberg Formula: A mathematical equation used to predict the wavelengths of spectral lines in various series of atomic spectra.
Balmer Series: A set of spectral lines for the hydrogen atom that involve electron transitions from higher energy levels down to n=2.
Bohr Model: An early atomic model proposing that electrons travel in fixed orbits around the nucleus with quantized energy levels.