Points to Remember:
- The question asks for the name of a specific series of spectral lines.
- The answer requires factual knowledge of atomic physics and spectroscopy.
Introduction:
Atomic hydrogen, the simplest atom with one proton and one electron, emits light when its electron transitions between different energy levels. These transitions result in a series of discrete spectral lines, each corresponding to a specific wavelength of light. The wavelengths of these lines are precisely defined by the Rydberg formula and are crucial in understanding atomic structure and quantum mechanics. The study of these spectral lines was pivotal in the development of modern physics, leading to the Bohr model and ultimately the quantum mechanical model of the atom.
Body:
The Lyman Series:
The question specifically asks for the name of a series, and while there are several series for atomic hydrogen, the most commonly discussed and the first discovered is the Lyman series. The Lyman series describes the transitions of the electron from higher energy levels (n > 1) to the ground state (n = 1). These transitions produce ultraviolet light. The lines are designated as Lyman-α, Lyman-β, Lyman-γ, and so on, corresponding to transitions from n=2, n=3, n=4, etc., respectively.
Other Series:
While not directly asked for, it’s important to note that other series exist for atomic hydrogen, including:
- Balmer Series: Transitions to the n=2 energy level, producing visible light. This series is historically significant as it was the first to be observed.
- Paschen Series: Transitions to the n=3 energy level, producing infrared light.
- Brackett Series: Transitions to the n=4 energy level, producing infrared 75.5c-23.5 6.3-42 24.9-48.3 48.6-11.4 42.9-11.4 132.3-11.4 132.3s0 89.4 11.4 132.3c6.3 23.7 24.8 41.5 48.3 47.8C117.2 448 288 448 288 448s170.8 0 213.4-11.5c23.5-6.3 42-24.2 48.3-47.8 11.4-42.9 11.4-132.3 11.4-132.3s0-89.4-11.4-132.3zm-317.5 213.5V175.2l142.7 81.2-142.7 81.2z"/> Subscribe on YouTube