3D sp Hybridization Simulation

sp orbital evidenceLive observation

Mix one s and one p orbital to form two opposite sp directions.

MoleculeH—H

Hybrid type100%

Bond angle−28 kJ/mol

ShapeAttractive

3D sp Hybridization LaboratoryPaused

ModeStudent

What makes two opposite sp orbitals?

One s and one p orbital on the same atom combine into two sp orbitals. Rotate the model to see a linear pair and the two unhybridized p axes.

One s + one p → two sp orbitals.
Two other p orbitals remain.
The sp directions are 180° apart.

sp orbital controls

Sound

Molecule

s–p mixing100%

Observation lens

3D orbital surface

Drag the scene to rotate the orbitals. The two p-lobe colors show opposite wave-function phases, not electric charges.

Simulation speed1×

Evidence

sp directions2 directions

Ideal angle180°

p orbitals left2 p orbitals

GeometryLinear

3D camera and focus

Drag to rotate the orbitals in 3D.

Orbital conservation

Teacher demonstrations

Guided visual lecture

Chapter 1 of 80%

Ready. The first ten seconds define sp hybridization with transforming 3D orbitals.

Language

Narrator

Playback speed1×

External recording: share this browser tab with tab audio enabled. No microphone is used.

1. What is hybridization?

Watch: One s and one p become two opposite sp orbitals.

Chapters

sp hybridization and linear geometry

Orbital conservation: 1 s + 1 p → 2 sp orbitals. Two of the original three p orbitals remain unhybridized.

Linear geometry: ideal sp–sp angle = 180°. Each sp hybrid has one larger forward lobe and one smaller opposite lobe.

Bonding: head-on overlap gives σ; side-on p overlap gives π. Ethyne C≡C = 1 σ + 2 π.

Examples: isolated gas-phase BeCl₂ is linear; CO₂ has a linear carbon center; C₂H₂ has sp-hybridized carbons.

This is a valence-bond classroom model. Orbital surfaces visualize probability, not solid shapes or electron paths. Solid BeCl₂ has an extended structure.

Learning objectives

Explain how one s and one p make two sp orbitals.
Identify the 180° linear arrangement.
Locate the two unhybridized p orbitals.
Distinguish sigma and pi overlap.

Suggested investigations

Rotate the sp pair to see its smaller opposite lobes.
Compare gas-phase BeCl₂ and CO₂.
Reveal ethyne's two perpendicular pi clouds.
Hide p orbitals, then reveal where pi bonding can form.

Questions for exploration

Why are the two sp directions opposite?
Why do two p orbitals remain?
How does ethyne form one sigma and two pi bonds?

Teacher whiteboard

Use a finger, stylus, mouse, Android device, or smart board. Ten full-size pages keep their own drawings.

Pen color

Line width4

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