VSEPR Theory: Repulsion betw. Bonding & Lone Pairs
Explore how electron pairs repel each other to determine molecular shape. (Lone pairs create invisible repulsion)
About this simulation
- What
- An interactive Chemistry simulation of VSEPR Theory: Repulsion betw. Bonding & Lone Pairs.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-01-12
Key Concepts
VSEPR Theory
Valence Shell Electron Pair Repulsion: Electron groups repel each other and spread out as far as possible.
Lone Pair Repulsion
Lone pairs take up more space than bonding pairs, compressing adjacent bond angles (e.g., from 109.5° to 104.5° in H₂O).
Electron vs Molecular Geometry
Electron geometry includes all electron pairs. Molecular geometry describes only the arrangement of atoms.
Understanding VSEPR Theory
VSEPR theory (Valence Shell Electron Pair Repulsion) is the primary model used in chemistry to predict the spatial geometry of individual molecules by calculating the number of electron domains surrounding a central atom.
The fundamental principle relies on the fact that electron pairs (both bonding and lone pairs) carry negative charges and naturally repel each other, forcing atoms to arrange themselves as far apart as possible to minimize this repulsion.
By identifying the exact count of lone pairs and bonding domains, we can determine a molecule's 3D shape, which dictates its physical properties, chemical reactivity, and molecular polarity.
Common Molecular Geometries
| Electron Domains | Bonding Pairs | Lone Pairs | Molecular Shape | Ideal Angle |
|---|---|---|---|---|
| 2 | 2 | 0 | Linear | 180° |
| 3 | 3 | 0 | Trigonal Planar | 120° |
| 3 | 2 | 1 | Bent / V-shaped | < 120° |
| 4 | 4 | 0 | Tetrahedral | 109.5° |
| 4 | 3 | 1 | Trigonal Pyramidal | < 109.5° |
| 4 | 2 | 2 | Bent / V-shaped | << 109.5° |
| 5 | 5 | 0 | Trigonal Bipyramidal | 90°, 120° |
| 6 | 6 | 0 | Octahedral | 90° |
Frequently Asked Questions
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