Understanding electron orbitals involves recognizing that they represent stationary states where the electron's position is described by probability distributions rather than fixed trajectories, as dictated by Heisenberg's uncertainty principle. Orbitals can be visualized as regions where the likelihood of finding an electron varies, with different shapes and complexities such as the Bohr model's circular shells and the more accurate SPDF configurations. The probability of locating an electron is highest at certain points within these orbitals, with specific characteristics for S, P, D, and F orbitals. The Schrödinger equation underpins the behavior of electrons, detailing quantum numbers that define energy levels, orbital types, and electron spin. For a clearer visual representation of these concepts, resources like the Falstad simulation can be helpful.