Comparative explanation of the Balmer series

1. Comparative explanation of the Balmer series The part of the hydrogen emission spectrum that corresponds to electron transitions from higher orbicular states n>2 to the energy level with principal quantum number n=2 is a series of spectral lines known as the Balmer series. n=2 The Balmer series occur in both visible and ultraviolet regions of the electromagnetic spectrum. UV Visible region region The detailed electron transitions in both visible and ultraviolet zones of the Balmer series below The Wavelength data comparison for both the visible & ultraviolet regions of the Balmer series In the visible zone, we observe four spectral lines at wavelengths 656nm, 486nm, 434nm, and 410nm correspond to electron transitions from energy levels such as 3 to 2, 4 to 2, 5 to 2, 6 to 2 giving characteristic red, aqua, blue and violet colored emissions in the hydrogen spectrum. This portion of the Balmer series is also known as the visible hydrogen spectrum. The spectral line formed due to the electron transition from the static configuration n=7 to the normal state n=2 is known as hydrogen epsilon. The hydrogen zeta emission line is due to the electron transition from top energy level n=8 to the ground state n=2 at a wavelength of about 389 nm. Similarly, the electron movement from n=9 to n=2 results in a spectral line named hydrogen eta. Finally, the spectral emission that results from n=∞ to the Balmer series ground state n=2 at 364.5 nm is the series limit of the Balmer series. The Wavelength data for both visible & UV regions of the Balmer series in a single chart view. For more interesting topics in chemistry, kindly visit our blog at; https://jayamchemistrylearners.blogspot. com/