Atomic Orbitals — s, p, d Orbitals Explained
What is an orbital?
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.
Key NEET Facts
- •Orbital = region in space with high electron probability, not a path
- •s orbitals: spherical shape, 1 per subshell, holds 2 electrons
- •p orbitals: dumbbell shape, 3 per subshell (px, py, pz), hold 6 electrons total
- •d orbitals: cloverleaf shape, 5 per subshell, hold 10 electrons total
- •Nodes = regions where electron probability = zero. More nodes = higher energy.
- •1s < 2s < 2p < 3s < 3p < 4s < 3d order (Aufbau principle)
Common Mistakes
- ✕Thinking orbits are like planetary paths — they're not. Orbitals are probability clouds.
- ✕Confusing orbital shape with electron path — an electron in a p orbital doesn't travel in a figure-8.
- ✕Assuming all s orbitals look identical — 2s has 1 node, 3s has 2 nodes, 4s has 3 nodes.
NEET Frequency: 2-3 questions per year
Frequently Asked Questions
Why is an orbital not an electron's path?›
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.
What does orbital shape tell us?›
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.
How many electrons can one orbital hold?›
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⁻.
What are nodes in orbitals?›
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.
Ready to see this in action?
Visualize atomic orbitals — s, p, d orbitals explained with an interactive 3D simulation.
Explore Atomic Orbitals Lab→