No, not every hydrogen atom has the same wavelength. The wavelength associated with a hydrogen atom depends on its energy level transitions. In the context of atomic spectroscopy, the energy levels of a hydrogen atom are quantized, meaning they can only occupy specific energy states.
When an electron in a hydrogen atom transitions between energy levels, it emits or absorbs electromagnetic radiation with a specific wavelength. The wavelengths associated with hydrogen atom transitions are well-known and have been experimentally determined.
The most commonly referenced wavelengths are those associated with the Balmer series, which involve transitions to or from the second energy level (n=2). The Balmer series includes visible light wavelengths, such as the famous Balmer-alpha line at approximately 656.3 nm (red light).
However, hydrogen atoms can also exhibit transitions involving other energy levels, leading to different wavelengths. For example, the Lyman series involves transitions to or from the first energy level (n=1) and corresponds to ultraviolet wavelengths.
So, in summary, the wavelength associated with a hydrogen atom depends on its energy level transitions, and different energy level transitions produce different wavelengths.