Final answer:
Transitions from higher energy levels to n=2 in the hydrogen atom produce the Balmer series, which consists of visible spectral lines. The Balmer series is just one of several spectral series described by the Bohr model, including others like the Lyman, Paschen, and Brackett series resulting from transitions to different final energy levels.
Step-by-step explanation:
Transitions from higher energy levels to n=2 result in the Balmer series of the hydrogen spectrum. When an electron in a hydrogen atom falls from a higher energy level to the second energy level, it emits a photon, producing a line in the visible part of the electromagnetic spectrum. This series includes several transitions, such as the n = 3 to n = 2 transition, which produces a red spectral line at 656 nm, and others that produce green, blue, and violet lines as the transition levels increase from n = 4 to n = 6, respectively.
The Balmer series is part of a larger set of spectral series described in the Bohr model of the hydrogen atom, where different series are named according to the value of the final energy level, nf, that the electron transitions to. Other series include the Lyman series (nf = 1), which is in the ultraviolet; the Paschen and Brackett series (nf = 3 and nf = 4, respectively), both of which are in the infrared region.