What is the main difference between the schrödinger model and the bohr atomic model? schrödinger believed that electrons could only exist in orbits, but bohr stated that electrons could be found anywhere in the atom. bohr believed electron orbits were circular, but schrödinger’s equations represent complex shapes describing the probable locations of electrons. the bohr model did not explain the emission and absorption spectrum, but the energy levels described by schrödinger explained this property. bohr believed that the electrons circle the nucleus because positive particles attract negative particles, while schrödinger believed that an electron was a wave.

Bohr believed electron orbits were circular, but Schrödinger’s equations represent complex shapes describing the probable locations of electrons.

Explanation:

In Bohr's model of the atom, electrons orbit around the nucleus in circular orbits. In this model, each orbit corresponds to an energy level, so that the possible levels of energy of the electrons are discrete (an electron cannot stay between two orbits, but it must be in one precise orbit). Moreover, orbits in this model are circular.

Later, Schrodinger introduced his principle of uncertainty, that states that it is not possible to measure at the same time the position and the velocity of a particle. By applying this principle to the atom, the result is that electrons cannot be in a precise circular orbit, because we cannot know their exact position and velocity at the same time. Therefore, according to Schrödinger’s principle, electrons can be found in certain regions of space around the nucleus (called 'orbitals') where they have a certain probability to be found, and this probabilty is described by Schrödinger’s equation.

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