Here's a breakdown:
* Balmer Series: This series produces visible light and is the most well-known. It corresponds to transitions where an electron jumps from higher energy levels (n ≥ 3) to the second energy level (n=2). The wavelengths in this series are:
* 656.3 nm (red)
* 486.1 nm (blue-green)
* 434.1 nm (blue)
* 410.2 nm (violet)
* ... and so on, with decreasing wavelengths as the initial energy level gets higher.
* Lyman Series: This series is in the ultraviolet range and corresponds to transitions from higher energy levels (n ≥ 2) to the first energy level (n=1).
* Paschen Series: This series is in the infrared range and corresponds to transitions from higher energy levels (n ≥ 4) to the third energy level (n=3).
* Brackett Series: This series is also in the infrared range and corresponds to transitions from higher energy levels (n ≥ 5) to the fourth energy level (n=4).
* Pfund Series: This series is in the far-infrared range and corresponds to transitions from higher energy levels (n ≥ 6) to the fifth energy level (n=5).
Important Notes:
* These wavelengths are just the most prominent ones. Hydrogen also emits other, less intense wavelengths corresponding to other transitions.
* The exact wavelengths can be calculated using the Rydberg formula.
* The wavelengths of hydrogen are incredibly important for understanding the structure of atoms and the behavior of light.
Let me know if you'd like me to elaborate on the Rydberg formula or any specific series in more detail!
