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sp² orbital evidenceLive observation

Mix one s and two p orbitals to form three planar sp² directions.

MoleculeH—H
Hybrid type100%
Bond angle−28 kJ/mol
ShapeAttractive
3D sp² Hybridization LaboratoryPaused
Mode

Why do three sp² orbitals form a plane?

One s and two p orbitals combine into three sp² orbitals. Rotate the trigonal plane to see its 120° angles and the perpendicular p orbital.

  1. One s + two p → three sp² orbitals.
  2. One other p orbital remains.
  3. Three directions share a 120° plane.

sp² orbital controls

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

Evidence

sp² directions3 directions
Ideal angle120°
p orbitals left1 p orbital
GeometryTrigonal planar

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 sp² hybridization with a transforming triangular orbital plane.

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

1. What is hybridization?

Watch: One s and two p become three planar sp² orbitals.

Chapters

sp² hybridization and trigonal geometry

Orbital conservation: 1 s + 2 p → 3 sp² orbitals. One of the original three p orbitals remains unhybridized.

Trigonal plane: the three sp² directions have ideal pairwise angles of 120°. The remaining p axis is perpendicular to their plane.

Bonding: head-on overlap gives σ; side-on p overlap gives π. A C=C or C=O double bond contains 1 σ + 1 π.

Examples: BF₃ is trigonal planar at boron; formaldehyde and ethene have sp²-hybridized carbon centers.

This is a valence-bond classroom model. Orbital surfaces show probability and wave-function phase, not solid shapes, electric charges, or electron paths.

Learning objectives

  • Explain how one s and two p make three sp² orbitals.
  • Identify the 120° trigonal plane.
  • Locate the perpendicular unhybridized p orbital.
  • Distinguish sigma and pi parts of a double bond.

Suggested investigations

  • Rotate BF₃ face-on and edge-on.
  • Hide p, then reveal the orbital needed for pi bonding.
  • Compare formaldehyde's C=O with ethene's C=C.
  • Change mixing and count orbitals before and after.

Questions for exploration

  • Why is the third p orbital perpendicular to the plane?
  • Why are the three sp² directions 120° apart?
  • How does side-on p overlap add a pi bond?

Teacher whiteboard

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