<P> The Balmer series or Balmer lines in atomic physics, is the designation of one of a set of six named series describing the spectral line emissions of the hydrogen atom . The Balmer series is calculated using the Balmer formula, an empirical equation discovered by Johann Balmer in 1885 . </P> <P> The visible spectrum of light from hydrogen displays four wavelengths, 410 nm, 434 nm, 486 nm, and 656 nm, that correspond to emissions of photons by electrons in excited states transitioning to the quantum level described by the principal quantum number n equals 2 . There are several prominent ultraviolet Balmer lines with wavelengths shorter than 400 nm . The number of these lines is an infinite continuum as it approaches a limit of 364.6 nm in the ultraviolet . </P> <P> The Balmer series is characterized by the electron transitioning from n ≥ 3 to n = 2, where n refers to the radial quantum number or principal quantum number of the electron . The transitions are named sequentially by Greek letter: n = 3 to n = 2 is called H - α, 4 to 2 is H - β, 5 to 2 is H - γ, and 6 to 2 is H - δ . As the first spectral lines associated with this series are located in the visible part of the electromagnetic spectrum, these lines are historically referred to as "H - alpha", "H - beta", "H - gamma" and so on, where H is the element hydrogen . </P>

A wavelength in the balmer series is 486 nm. is. what transition is this
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