According to the concept of spectral lines, what can different transitions in a hydrogen atom produce?

The correct choice highlights that different transitions in a hydrogen atom produce different light frequencies. When an electron in a hydrogen atom moves between energy levels, it either absorbs or emits a photon of light. The energy of this photon corresponds to the difference in energy between the two levels. According to the equation (E = hf) (where (E) is energy, (h) is Planck's constant, and (f) is frequency), different energy transitions will result in photons of various frequencies.

Each frequency of light falls within the electromagnetic spectrum, resulting in visible light for some transitions, and ultraviolet or infrared light for others. This is why the spectral lines of hydrogen can be distinctive; they represent specific frequencies (or wavelengths) of light emitted or absorbed during these electron transitions. Factors such as the Rydberg formula describe how these energy transitions correspond to specific spectral lines as they relate to the hydrogen atom's spectral emissions.

The other options relate more to aspects of atomic structure rather than the direct consequence of electron transitions: isotopes pertain to variations in neutron number, masses relate to the total number of protons and neutrons, and colors of atomic nuclei do not apply in the context of spectral lines.