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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
Mode

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.

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

sp orbital controls

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

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.

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

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