Velcro Molecules: Intermolecular Forces
Why is water liquid but ethane gas? It's all about how sticky the molecules are. Drag them to find out.
About this simulation
- What
- An interactive Chemistry simulation of Velcro Molecules: Intermolecular Forces.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2025-10-11
Key Concepts
Intermolecular Forces (IMFs)
Attractions between adjacent molecules. Much weaker than covalent bonds, but they determine boiling points.
Hydrogen Bonding
The strongest IMF. Occurs when Hydrogen is bonded to highly electronegative atoms (N, O, F).
London Dispersion Forces
Weak, temporary dipoles caused by electron movement. Larger molecules = more electrons = stronger London forces.
Understanding Intermolecular Forces
Intermolecular Forces (IMFs) are the non-covalent attractive forces that exist between molecules. These forces are the primary determinants of bulk physical properties, including state of matter, boiling point, and volatility.
The three core IMF classifications include London Dispersion Forces (temporary dipoles present in all molecules), Dipole-Dipole interactions (permanent dipoles in polar molecules), and Hydrogen Bonding (exceptionally strong dipoles specifically involving H bonded to N, O, or F).
Our interactive simulator provides a tactile 'velcro' experience to quantify the relative energy required to overcome these secondary bonds, demonstrating why molecules like water remain liquid at room temperature while nonpolar molecules of similar size are gases.
Intermolecular Forces Comparison
| Force Type | Relative Strength | Occurs In |
|---|---|---|
| London Dispersion | Weak (Increases w/ size) | All molecules |
| Dipole-Dipole | Moderate | Polar molecules |
| Hydrogen Bonding | Strong | H bonded to N, O, F |
Frequently Asked Questions
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