The transition from the n=3 to n=2 energy level in the hydrogen atom can produce a spectral line in the visible region of the emission spectrum.
The visible emission spectrum of hydrogen is a result of electrons transitioning between different energy levels within the atom. When an electron undergoes a transition from a higher energy level (such as n=3) to a lower energy level (such as n=2), energy is emitted in the form of light.
The specific wavelengths of light emitted during these transitions fall within the visible spectrum, producing the characteristic spectral lines observed in the visible region. In the case of hydrogen, the n=3 to n=2 transition corresponds to a spectral line in the visible spectrum, contributing to the distinct line spectrum associated with hydrogen's electronic transitions.