what are typical wavelengths in atomic spectrum

In atomic spectra, the typical wavelengths of spectral lines depend on the element and its electron energy levels. These wavelengths are characteristic of each element and are used for identification. Here are some examples of typical wavelengths in atomic spectra.

Hydrogen Spectrum

Hydrogen is one of the most well-known elements in terms of its atomic spectrum. In the visible region of the spectrum, hydrogen exhibits several lines with the following wavelengths (in nanometers):

• Balmer Series:

  • Hα (Red): 656.3 nm
  • Hβ (Blue-Green): 486.1 nm
  • Hγ (Blue-Violet): 434.0 nm
  • Hδ (Violet): 410.2 nm

• Lyman Series (Ultraviolet):

  • Hα (Ultraviolet): 121.6 nm
  • Hβ (Ultraviolet): 102.6 nm

Sodium (Na) Spectrum

Sodium vapor lamps emit yellow-orange light due to the dominant sodium D-line doublet with wavelengths around 589.0 nm (D1) and 589.6 nm (D2).

Mercury (Hg) Spectrum

Mercury vapor lamps emit various spectral lines in the ultraviolet, visible, and near-infrared regions. The most prominent lines are at 365.0 nm (near-ultraviolet) and 546.1 nm (green).

Helium (He) Spectrum

Helium exhibits several lines in the visible spectrum, including 587.6 nm (yellow) and 667.8 nm (red).

Neon (Ne) Spectrum

Neon signs produce various colors, each associated with a specific spectral line of neon. For example, the red glow of neon signs is due to the 632.8 nm line.

Argon (Ar) Spectrum

Argon gas discharge tubes emit a bluish-violet light with prominent spectral lines at 488.0 nm and 484.9 nm.