An orbital is a region of space where an electron has a high probability of being found. The size and shape of an orbital depends on its energy level (n) and subshell (s, p, d, f). An orbital can hold a maximum of 2 electrons.
An orbital is not an electron's path — it's a region in space where an electron is likely to be found. Orbitals come in shapes: s orbitals are spherical, p orbitals are dumbbell-shaped (3 of them per subshell), and d orbitals are cloverleaf-shaped (5 of them per subshell). Understanding orbital shapes helps you predict where electrons hang out and how they interact to form bonds.
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The uncertainty principle (Heisenberg) says we cannot know both an electron's exact position and velocity at the same time. Therefore, we cannot describe an electron following a specific path. Instead, we describe the probability cloud (orbital) where it's likely to be found.
Orbital shape describes where electron density is concentrated. s orbitals (spherical) are useful for bonding in all directions. p orbitals (dumbbell) have lobes that point in specific directions (x, y, z), so they're useful for directional bonding. Understanding shape helps predict bond angles and geometry.
One orbital can hold a maximum of 2 electrons. These two electrons must have opposite spins (one spin-up, one spin-down) — this is the Pauli exclusion principle. So 1 orbital = 2e⁻, 3 p-orbitals = 6e⁻, 5 d-orbitals = 10e⁻.
A node is a region where the orbital's electron probability density is zero. s orbitals have no angular nodes but may have radial nodes. p orbitals have 1 angular node (a plane). Higher-energy orbitals have more nodes. More nodes = higher energy.
Visualize atomic orbitals — s, p, d orbitals explained with an interactive 3D simulation.
Explore Atomic Orbitals Lab→