Final answer:
The hydrogen emission spectrum provides evidence for energy levels through distinct spectral lines, each corresponding to an electron transitioning between specific energy states, as described in Bohr's model and observable in series such as the Lyman and Balmer series.
Step-by-step explanation:
Understanding the Hydrogen Emission Spectrum and Energy Levels
The hydrogen emission spectrum provides evidence for the existence of distinct energy levels within an atom. This evidence is captured through the observation of spectral lines which correspond to the transition of an electron between these levels. When an electron jumps from a higher energy level to a lower one, it emits a photon whose energy is precisely the difference between the two levels. The transition to and from the ground state, known as the Lyman series, emits or absorbs ultraviolet light. Similarly, transitions to the second orbit, or n = 2, are part of the Balmer series and result in visible spectral lines, with each transition corresponding to a specific wavelength. This was mathematically described by Niels Bohr, who used the observed wavelengths of the spectral lines to calculate the energies of the electron in its allowed states. For instance, a transition from n = 3 to n = 2 emits light at the wavelength of 656 nm (red), and this is just one of the specific transitions that can be observed within this spectrum.
The spectral lines of hydrogen are characteristic and predictable because the energy difference between the orbits is fixed and unique for each transition, much like a fingerprint. The emission spectrum thus serves as a confirmation of the quantized nature of energy levels in atomic physics.