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If you picture an atom as a miniature solar system with electrons orbiting like tiny planets, you are imagining a model that physics discarded nearly a century ago.
In 1926, Austrian physicist Erwin Schrödinger realized electrons act like 3D matter waves, meaning we cannot track their exact paths—only where they are most likely to be found.
An atomic orbital is a three-dimensional mathematical region around the nucleus where an electron has roughly a 90% probability of existing.
So what shapes do these probability clouds form as electrons gain energy?

Orbital Shapes: s, p, d, and f

Orbitals are categorized into four distinct sublevel geometries named s, p, d, and f based on historical spectral line descriptions.
An s orbital is shaped like a smooth sphere centered directly on the nucleus, meaning an electron is equally likely to be found in any direction.
A p orbital forms a two-lobed dumbbell or peanut shape oriented along three perpendicular spatial axes: pxp_x, pyp_y, and pzp_z.
Most d orbitals feature four lobes resembling a four-leaf clover, while f orbitals form even more complex eight-lobed flower-like structures.
Notice that the number of spatial orientations climbs by odd numbers: 1, 3, 5, and 7. But how many electrons can fit inside each of these shapes?

Sublevel Capacities and the Pauli Rule