Atomic Orbital Shapes – AP Chemistry | ShowMeClass

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Atomic Orbital Shapes

AP Chemistry · Unit 1: Atomic Structure

Learning Objectives

Describe the shape of s, p, and d orbitals

Identify nodes (regions of zero electron density)

Explain why orbitals have different energies

Connect orbital shapes to chemical bonding geometry

Quantum Numbers

Orbital Summary

s orbital: Spherical, 1 per sublevel, no node

p orbitals: Dumbbell, 3 per sublevel (x,y,z), 1 node

d orbitals: Cloverleaf, 5 per sublevel, 2 nodes

Phase: +/− lobes shown by color (wavefunction sign)

Key Insight

Orbitals show where electrons are likely to be found. The surface shown contains 90% of electron probability. Nodes are surfaces where ψ² = 0 — electrons are never found there.

OrbitalsQuantum NumbersAP ChemistryUnit 1

SELECT ORBITAL:

1s

Spherical shape centered on nucleus. One lobe, no angular nodes. Lowest energy orbital. All electrons in 1s have equal probability in all directions.

X → Y → Z ↑

Particle Count 3000

More particles = denser probability cloud

Opacity 0.70

Particle Size 3.0

Quantum Numbers

n = 1 (shell)

ℓ = 0 (subshell)

m_ℓ = 0

Nodes: 0

📝 Quick Quiz▼

1. How many orbitals are in the 3d subshell?

1 3 5 7

2. Which orbital has a "dumbbell" shape with one nodal plane?

s orbital p orbital d orbital f orbital

3. The number of angular nodes in an orbital equals:

n (principal quantum number) n − 1 ℓ (angular momentum quantum number) m_ℓ