Atomic orbital
![The shapes of the first five atomic orbitals: 1s, 2s, 2px, 2py, and 2pz. The two colors show the phase or sign of the wave function in each region. These are graphs of ψ(x, y, z) functions which depend on the coordinates of one electron. To see the elongated shape of ψ(x, y, z)2 functions that show probability density more directly, see the graphs of d-orbitals below.](/Images/godic/202502/12/Neon_orbitals1230.JPG")
![False-color density images of some hydrogen-like atomic orbitals (f orbitals and higher are not shown)](/Images/godic/202502/12/HAtomOrbitals1230.png")
![The Rutherford–Bohr model of the hydrogen atom.](/Images/godic/202502/12/Bohr-atom-PAR.svg1230.png")
![Cross-section of computed hydrogen atom orbital (ψ(r, θ, φ)2) for the 6s (n = 6, ℓ = 0, m = 0) orbital. Note that s orbitals, though spherically symmetrical, have radially placed wave-nodes for n > 1. However, only s orbitals invariably have a center anti-node; the other types never do.](/Images/godic/202502/12/HydrogenOrbitalsN6L0M01230.png")
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term, atomic orbital, may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.