we had this in an assessment, except we had to 'analyse' instead of 'discuss'. here's my answer:
When an element is heated or ionised, it emits visible light and radiation, which can be manipulated into its components using a spectroscope and prism. A pattern is created of coloured lines on a dark background. This pattern is known as the emission spectrum, and is elementally unique. Passing white light through cool gas, however, creates an absorption spectrum, so called because the gas absorbs the same frequencies it would emit if heated. An absorption spectrum creates a pattern of dark lines on a coloured background.
Between 1884 and 1886, Johann Balmer suggested a mathematical formula to fit each of the known wavelengths of hydrogens spectrum, = b(m2 / (m2 22) ), where b is a constant and m varies with each line in the spectrum. This formula covered the four lines created in the visible portion of the spectrum, known as the Balmer series. Johannes Rydberg later generalised Balmers formula.
Rutherfords atomic model did not agree with the observable spectra, and Bohr set out to rectify this with his atomic model. He therefore kept the basic structure of the Rutherford model, necessary to explain the alpha particle scattering experiments. From his basic hypotheses, Bohr derived a number of equations. One of these was Rydbergs equation. The ability to derive this from his atomic model showed that Bohrs ideas were feasible, as they successfully explained observable hydrogen emission spectra.
Thus, the hydrogen spectrum was the basis for the scientific validity of Bohrs model of the atom, and had a significant contribution to its development. It also played a role in the stimulus for the creation of the Bohr model, since Bohrs aim was to account for the discrepancies between Rutherfords model and the observed hydrogen spectrum.
this got me 8/10, i lost two marks for not talking about quantisation of energy for electrons to change energy levels.
hope that's in some way helpful...
