In quantum mechanics, orbitals represent regions around the nucleus where electrons are most likely to be found. Their shapes come from solutions of the Schrödinger equation.
Here are the main orbital shapes:
- s orbital
- Shape: Spherical
- Electrons are spread uniformly around the nucleus.
- Example: 1s, 2s, 3s …
- The size increases with higher energy levels (n).
- p orbital
- Shape: Dumbbell-shaped (like two lobes on opposite sides of the nucleus).
- There are three orientations: px, py, and pz, oriented along the x, y, and z axes.
- d orbital
- Shape: Cloverleaf-shaped (four lobes), except one (dz²) which looks like a dumbbell with a donut around the center.
- There are five orientations: dxy, dxz, dyz, dx²–y², and dz².
- f orbital
- Shape: Complex and multi-lobed (often with 6–8 lobes).
- Very complicated, but generally described as “flower-shaped.”
- There are seven orientations.
In short:
- s = sphere
- p = dumbbell
- d = cloverleaf
- f = complex/flower-like