Question

Regarding the emmission spectra, are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model of the atom? Which lines, if any, are missing? Why might there be lines missing?

Answer 1

In general, Bohr's model of atom predicts emmission spectra for hydrogen atom and hydrogen like ions sucessfully. The experimentally calculated parameters of the spectral lines corresponding to Lyman, Balmer, Paschen, Brackett, Pfund and Humphry series are similar as calculated by Bohr.

However, when we consider groups of very fine spectral lines discovered due to the developement of high resolution spectroscopey a few years later, Bohr's prediction fails. Those are the lines missing.

Reason behind this is the Bohr' assumption that electron moves around the nucleus in certain permitted circular orbits and hence the energy of those orbits depends only on principal quantum number (n).  Which indeed was corrected by Sommerfeld. He explained that the electrons move in elliptical orbits instead of circular orbits and that the energy of these orbits depend not only on principal quantum number but also on azimuthal quantum number (arising from the quantised angular momentum from the ellitpical motion of the electron).
This theory in general known as Bohr-Sommerfeld model explains the occurance of groups of very fine lines for Hydrogen spectrum. It still could not explain the spectra of multi-electronic atoms.