**The Balmer Series in the Hydrogen Spectrum**

The hydrogen spectrum is a series of lines observed when atomic hydrogen emits light. These lines correspond to specific wavelengths of light that are emitted or absorbed by the hydrogen atoms as they transition between different energy levels.

One of the most prominent series in the hydrogen spectrum is the Balmer series. This series lies in the visible region of the electromagnetic spectrum, which ranges from approximately 350 to 700 nm. The Balmer series consists of several distinct lines, each corresponding to a specific transition between energy levels in the hydrogen atom.

**Understanding the Balmer Series Transitions**

The Balmer series is formed when electrons in hydrogen atoms transition from higher energy levels to the second energy level (n = 2). This series can be explained using the Balmer formula, which relates the observed wavelength of the emitted or absorbed light to the energy levels involved:

1/λ = R(1/4 - 1/n²)

Where:
- λ represents the observed wavelength
- R is the Rydberg constant (1.097 × 10^7 m⁻¹)
- n is the principal quantum number of the higher energy level

By plugging in different integer values for n, we can calculate the corresponding wavelengths for the Balmer series lines.

**The Balmer Series Lines**

The Balmer series lines can be calculated using the Balmer formula. Here are the wavelengths for some of the key lines in the Balmer series:

- n = 3 to n = 2 transition: This corresponds to the Hα line, which has a wavelength of approximately 656 nm. It falls within the red region of the visible spectrum.
- n = 4 to n = 2 transition: This corresponds to the Hβ line, which has a wavelength of approximately 486 nm. It falls within the blue-green region of the visible spectrum.
- n = 5 to n = 2 transition: This corresponds to the Hγ line, which has a wavelength of approximately 434 nm. It falls within the violet region of the visible spectrum.

The Balmer series lines continue with higher-order transitions, but they become closer together and shift towards shorter wavelengths, eventually entering the ultraviolet region of the spectrum.

**Conclusion**

In summary, the Balmer series in the hydrogen spectrum lies in the wavelength range of 350 to 700 nm, which falls within the visible region of the electromagnetic spectrum. This series corresponds to transitions of electrons from higher energy levels to the second energy level (n = 2) in the hydrogen atom. The Balmer series lines, such as Hα, Hβ, and Hγ, have specific wavelengths that can be calculated using the Balmer formula. These lines contribute to the characteristic spectral lines observed in the hydrogen spectrum.

Balmer series