Final answer:
The fact that the wavelengths of the four lines in the Balmer series fit a regular pattern was evidence supporting the idea of quantized energy levels in the hydrogen atom. Johann Balmer derived an empirical equation, known as the Balmer formula, to describe the visible wavelengths emitted by hydrogen atoms. This equation showed that the wavelengths followed a mathematical pattern, indicating that energy levels in the hydrogen atom were discrete.
Step-by-step explanation:
The fact that wavelengths of the four lines in the Balmer series fit a regular pattern was evidence supporting the idea that the hydrogen emission spectrum is quantized. In 1885, Johann Balmer derived an empirical equation that related the visible wavelengths of light emitted by hydrogen atoms to whole integers. This equation, known as the Balmer formula, demonstrated that the wavelengths followed a mathematical pattern, which indicated that energy levels in the hydrogen atom were discrete rather than continuous.
For example, the Balmer series consists of spectral lines corresponding to transitions from higher energy levels down to the second energy level, which is represented by the quantum number n=2. These transitions result in visible light wavelengths. Other series, such as the Lyman series, Paschen series, and Brackett series, correspond to different energy level transitions and result in wavelengths in the ultraviolet or infrared region of the spectrum. The fact that the Balmer series wavelengths could be described by a simple equation showed that there was a regularity and predictability to the behavior of the hydrogen atom.