The first to use Quantum Theory for Atomic Structure. After spending four years in Rutherford’s Lab, he took an interest to the Rutherford (planetary) atomic structure. A common objection to the Rutherford (planetary) model of the atom at the time was that the charged particles ought to have, according to classical physics, radiated energy and therefore crashed into the oppositely-charged nucleus. Bohr assumed that there were “stationary” orbits (i.e., where the electrons did not emit energy), and further assumed that these orbits happened when the electrons had angular momentums in relation to the Planck constant. Working from there, he deduced the energies for each of these orbits. Furthermore, he assumed that an emission of light occurred when an electron went from a higher-energy orbit to a lower-energy orbit, and an absorption of light occurred when the electron went vice versa. With this, he deduced a theoretical formula for the structure of the atom. While Bohr had the right General idea about electrons and their orbits, he, among other things, violated the Heisenberg uncertainty principle and even got the ground-state orbit momentum wrong.