Understanding Molecular Coplanarity & Collinearity
Explore the 3D structures of fundamental organic molecules to see how sp³, sp², and sp hybridization affects atomic alignment in space. Essential for understanding organic geometry.
About this simulation
- What
- An interactive Chemistry simulation of Understanding Molecular Coplanarity & Collinearity.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-02-25
Key Concepts
sp³ Hybridization (Tetrahedral)
In molecules like methane, the central carbon is sp³ hybridized, forming a tetrahedral shape with 109.5° angles. Any 3 atoms can be coplanar.
sp² Hybridization (Trigonal Planar)
In molecules like ethene and benzene, sp² hybridized carbons form planar structures with 120° angles, making large groups of atoms coplanar.
sp Hybridization (Linear)
In molecules like ethyne, sp hybridized carbons form a linear structure with 180° angles. Collinear atoms are always coplanar.
Single Bond Rotation
Single bonds (sigma bonds) can rotate freely, changing the spatial relationship between atoms on either side. Double and triple bonds cannot rotate.
Visualizing Covalent Geometry
Molecular Coplanarity and Collinearity refer to the geometric arrangement of atoms within a molecule. Atoms are considered coplanar if they lie within the same flat plane, and collinear if they are positioned along a single straight line.
These spatial arrangements are a direct consequence of the valence shell hybridization of the constituent atoms. For instance, sp² hybridization in ethene and benzene creates rigid planar frameworks, while sp hybridization in ethyne results in linear geometry.
Use our interactive 3D structures to highlight coplanar atom sets and collinear segments, and observe how sigma-bond rotation affects the maximum number of atoms that can simultaneously share a plane.
Frequently Asked Questions
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