How does Bohr's model of the atom differ from the quantum mechanical model?

The quantum mechanical model of the atom represents a significant advancement in understanding electron behavior compared to Bohr's model. In Bohr's model, electrons are depicted as occupying fixed, circular orbits around the nucleus at defined energy levels, and their positions can be specified exactly. However, this idea of fixed paths does not accurately reflect the nature of electrons, which exhibit both particle-like and wave-like properties.

The quantum mechanical model, on the other hand, introduces the concept of probability distributions. It does not assign precise locations to electrons but rather describes regions of space, known as orbitals, where there is a high likelihood of finding an electron. These orbitals are defined by complex wave functions that account for various quantum numbers. This probabilistic interpretation aligns more closely with experimental evidence and accommodates the uncertainty principle, which states that one cannot simultaneously know both the exact position and momentum of an electron.

By focusing on probable areas instead of specific paths, the quantum mechanical model captures the reality of how electrons behave and interact within an atom, making it a more comprehensive and accurate representation of atomic structure.