CO₂
Carbon Dioxide
Geometry Analysis
Two double bonds act as two effective bonding domains. No lone pairs on Carbon.
Pairs of electrons repel each other. Lone pairs repel more strongly than bonding pairs, often forcing bond angles to be smaller than the ideal geometry.
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VSEPR Theory: Repulsion betw. Bonding & Lone Pairs
Explore how electron pairs repel each other to determine molecular shape. (Lone pairs create invisible repulsion)
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📚 Master VSEPR Theory
Learn the rules for predicting molecular shapes and understanding bond angles.
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
Related Simulations
Molecular Coplanarity & Collinearity
**Molecular Coplanarity & Collinearity** are spatial properties determined by atomic hybridization. This resource visualizes how **sp³**, **sp²**, and **sp** orbitals dictate the alignment of atoms in planes and lines.
Hybridization & Bonding
**Hybridization & Bonding** theory explains the geometric arrangement of organic molecules. This resource visualizes **sp³**, **sp²**, and **sp** hybrid orbitals and the formation of **σ (sigma)** and **π (pi)** bonds.
Chemical Bonds
**Chemical Bonds** are the attractive forces that hold atoms together to form molecules and ionic lattices. This resource visualizes **Ionic**, **Covalent**, and **Metallic** bonding through interactive animations.