1.The model only worked for hydrogen-like atoms.
ohr was not able to explain electron orbits of large atom w/ many electrons.
Bohr's model could not explain why the intensity of the spectra lines were NOT all equal.

The Brainliest Answer!

This Is a Certified Answer

Certified answers contain reliable, trustworthy information vouched for by a hand-picked team of experts. Brainly has millions of high quality answers, all of them carefully moderated by our most trusted community members, but certified answers are the finest of the finest.
Spectra of Large atoms:The Bohr model could only successfully explain the hydrogen spectrum.It could NOT accurately calculate the spectral lines of larger atoms.The model only worked for hydrogen-like atomsThat is, if the atom had only one electron.Relative Spectra IntensityBohr's model could not explain why the intensity of the spectra lines were NOT all equal.This suggests that some transitions are favoured more than others.Hyperfine spectral linesWith better equipment and careful observation, it was found that there were previously undiscovered spectral linesThese were named Hyperfine lines and they accompanied the other more visible lines.Bohr's model could not explain why this was the case due to the lack of equipment and development in quantum physics.The reason for these lines is actually because of a hyperfine structure of atoms.Solved through developments into Matrix MechanicsThe Zeeman effectIt was found that, when hydrogen gas was excited in a magnetic field, the produced emission spectrum was split.Bohr's model could not account for thisSolved by accounting for the existence of a tiny magnetic moment of each electron.Stationary statesAlthough Bohr stated that electrons were in stationary states, he could not explain why.The reason is covered laterMixture of SciencesThe Bohr model was a mixture of quantum and classical physicsThis is an issue because it was thought that quantum physics was completely irrelevant and different to classical physics.
1 5 1