
A mathematical function describing the location and wave-like behavior of an electron in an atom or molecule.An orbital is a mathematical function that describes the location and wave-like behavior of an electron in an atom or molecule. It defines the probability distribution of finding an electron in a given region of space, replacing the older idea of fixed, planet-like electron paths. Orbitals come in various shapes (s, p, d, f) and energy levels, and their arrangement determines the chemical properties of elements and how atoms bond to form molecules.
The concept was developed in the 1920s by Erwin Schrödinger and Max Born, building on Niels Bohr's earlier atomic model. The term 'orbital' was coined by Robert S. Mulliken in 1932.
The orbital is a solution to the Schrödinger equation for an electron in a potential field created by the nucleus and other electrons. The square of the wave function gives the probability density of the electron's position. In molecules, orbitals combine to form bonding and antibonding orbitals, which dictate molecular structure and reactivity. In solids, orbitals overlap to form bands, explaining electrical conductivity and other bulk properties.
Orbitals are fundamental to quantum chemistry, materials science, and semiconductor physics, guiding the design of new molecules, drugs, and electronic devices.
The shapes of orbitals are not arbitrary; they arise from the symmetries of the underlying quantum mechanical equations, and the 'fuzzy' electron cloud of an orbital can be directly imaged using scanning tunneling microscopy.




