Orbitale atomowe

The shape of an atomic orbital is determined by the angular momentum quantum number, l. The value of l ranges from 0 to n − 1, where n is the principal quantum number. Each value of l corresponds to a specific orbital type: s, p, d, or f. These distinct shapes represent the three-dimensional regions where electrons are most likely to be found.

Probability density alone suggests electrons are most likely at the nucleus, which contradicts electrostatic repulsion between protons and electrons. The radial distribution function multiplies probability density by the volume of thin spherical shells at distance r from the nucleus, providing a more accurate representation of where electrons actually reside in an atom.

Radial nodes are distances from the nucleus where the probability of finding an electron is zero. The number of radial nodes in an orbital is calculated as n − l − 1. For example, 2s orbitals have one radial node, while 3s orbitals have two radial nodes, making higher energy orbitals increasingly complex.

While s orbitals are spherically symmetric, p orbitals have a lobe-shaped structure with two lobes and a node at the nucleus. Each principal level with n ≥ 2 contains three p orbitals that are mutually perpendicular (orthogonal) to each other. Higher p orbitals like 3p and 4p have similar shapes but are larger with additional radial nodes.

D orbitals appear in principal levels with n ≥ 3 and consist of five orbitals total. Four have a cloverleaf shape with four electron-dense lobes and two perpendicular nodal planes intersecting at the nucleus. One d orbital differs slightly, featuring two lobes along the z-axis with a donut-shaped ring in the xy plane.

Individual atomic orbitals have distinct shapes—spherical s orbitals, lobe-shaped p orbitals, cloverleaf d orbitals, and complex f orbitals. However, when all orbitals are overlaid on top of one another, they combine to form a roughly spherical shape. This combined electron cloud appearance explains why atoms are typically depicted as spheres in chemistry.

The 1s orbital is the lowest energy orbital and is spherically symmetric. For hydrogen, the radial distribution function shows the greatest probability of finding an electron at 52.9 picometers from the nucleus. This distance defines the effective radius of the 1s orbital and represents where the electron cloud is most concentrated.