In: Chemistry
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?
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.