VSEPR Shape Visualizer - Interactive 3D Molecular Geometry Tool
Explore VSEPR theory with our interactive 3D molecular geometry visualizer. Rotate molecules in real-time to understand how electron pair repulsion determines molecular shapes. Perfect for chemistry students learning about hybridization, bond angles, and molecular polarity.
All 13 VSEPR Molecular Geometries
- 🔵 Linear: AX₂ (CO₂, BeH₂) - 180° bond angle, sp hybridization
- 🟢 Trigonal Planar: AX₃ (BF₃, CO₃²⁻) - 120° angles, sp² hybridization
- 🟣 Bent: AX₂E (SO₂, O₃) - ~117° angle with lone pair
- 🔷 Tetrahedral: AX₄ (CH₄, CCl₄) - 109.5° angles, sp³ hybridization
- 🔺 Trigonal Pyramidal: AX₃E (NH₃, PH₃) - ~107° angles
- 💧 Bent (Angular): AX₂E₂ (H₂O, H₂S) - ~104.5° angle
- ⭐ Trigonal Bipyramidal: AX₅ (PCl₅) - 90°, 120°, 180° angles
- ⚖️ Seesaw: AX₄E (SF₄) - distorted shape
- ➕ T-Shaped: AX₃E₂ (ClF₃) - ~87.5° angles
- 📏 Linear (5): AX₂E₃ (XeF₂, I₃⁻) - 180° angle
- 🎲 Octahedral: AX₆ (SF₆) - 90° and 180° angles
- 🏔️ Square Pyramidal: AX₅E (BrF₅) - ~85° angles
- ⬜ Square Planar: AX₄E₂ (XeF₄) - 90° angles
Understanding VSEPR Theory
The Valence Shell Electron Pair Repulsion (VSEPR) theory is fundamental to understanding molecular chemistry. It states that electron pairs around a central atom will arrange themselves as far apart as possible to minimize electrostatic repulsion.
Bonding Pairs
Shared between atoms to form chemical bonds. They determine the molecular framework.
Lone Pairs
Non-bonding electrons on the central atom. They push bonding pairs closer together.
Steric Number
Total of bonding + lone pairs. Determines electron geometry and hybridization.
Hybridization
Mixing of atomic orbitals (s, p, d) to form new equivalent orbitals for bonding.
How to Use the VSEPR Visualizer
- Select a Shape: Click on any molecular geometry from the grid
- View in 3D: Watch the molecule rotate or drag to rotate manually
- Study Details: See bond angles, hybridization, polarity, and examples
- Filter by Steric Number: Focus on related geometries
- Use the Reference Table: Compare all 13 shapes side-by-side
Perfect for Chemistry Education
This interactive VSEPR shape visualizer is designed for:
- • High school chemistry students studying molecular geometry
- • AP Chemistry and IB Chemistry exam preparation
- • College organic and inorganic chemistry courses
- • Teachers creating visual demonstrations for class
- • Anyone curious about how molecules are shaped!
💡 VSEPR Tip
Remember: Lone pairs occupy more space than bonding pairs! This is why H₂O (2 bonding + 2 lone pairs) has a 104.5° angle instead of the typical 109.5° tetrahedral angle. Lone pair-lone pair repulsion > lone pair-bonding pair repulsion > bonding pair-bonding pair repulsion.
Frequently Asked Questions
What is VSEPR theory?
VSEPR (Valence Shell Electron Pair Repulsion) theory predicts molecular geometry based on the idea that electron pairs around a central atom repel each other and arrange themselves to minimize this repulsion. It helps predict the shape of molecules based on the number of bonding and lone pairs of electrons.
What is a steric number in VSEPR?
The steric number is the total number of atoms bonded to the central atom plus the number of lone pairs on the central atom. It determines the electron pair geometry and is used to predict molecular shape. For example, a steric number of 4 gives tetrahedral electron geometry.
What is the difference between electron geometry and molecular geometry?
Electron geometry considers ALL electron pairs (bonding + lone pairs) around the central atom. Molecular geometry only considers the positions of bonded atoms, ignoring lone pairs. For example, water (H₂O) has tetrahedral electron geometry but bent molecular geometry.
How do lone pairs affect molecular shape?
Lone pairs occupy more space than bonding pairs because they're held closer to the nucleus. This causes them to exert greater repulsion on bonding pairs, compressing bond angles. For example, water's bond angle is 104.5° instead of the tetrahedral 109.5° due to two lone pairs.
What does AXnEm notation mean?
In VSEPR notation: A = central atom, X = number of bonded atoms, E = number of lone pairs. For example, AX₄E means 4 bonded atoms and 1 lone pair (like NH₃), while AX₂E₂ means 2 bonded atoms and 2 lone pairs (like H₂O).
How is hybridization related to VSEPR?
Hybridization predicts the mixing of atomic orbitals and is directly related to steric number: sp (2), sp² (3), sp³ (4), sp³d (5), sp³d² (6). The same steric number always gives the same hybridization regardless of lone pairs.
Why are some molecules polar and others non-polar?
Polarity depends on molecular symmetry. Symmetric molecules (like CO₂ or CH₄) are non-polar because dipole moments cancel out. Asymmetric molecules (like H₂O or NH₃) are polar because dipoles don't fully cancel. Lone pairs break symmetry and often create polarity.
What are the common VSEPR shapes for steric number 4?
Steric number 4 (sp³ hybridization) produces: Tetrahedral (AX₄, 0 lone pairs) like CH₄, Trigonal Pyramidal (AX₃E, 1 lone pair) like NH₃, and Bent (AX₂E₂, 2 lone pairs) like H₂O. Each has progressively smaller bond angles due to lone pair repulsion.