Intermolecular Forces Explorer

Identify London dispersion, dipole-dipole, and hydrogen bonding forces on interactive 3D molecules.

Water

H₂O

H-bonding
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Concepts

What Are Intermolecular Forces?

Intermolecular forces (IMFs) are attractions between molecules that determine boiling point, solubility, and physical state. There are three main types:

1. London Dispersion Forces (LDF)

Present in all molecules. Caused by temporary fluctuations in electron density. Stronger for larger, more polarizable molecules.

2. Dipole-Dipole Forces

Only in polar molecules. The δ+ end of one molecule attracts the δ− end of another. Stronger than LDF for similar-sized molecules.

3. Hydrogen Bonding

A special, strong type of dipole-dipole. Requires H bonded to N, O, or F (donor) and a lone pair on N, O, or F (acceptor).

Key idea: Forces are additive. A molecule with H-bonding also has dipole-dipole and LDF.

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About This Molecule

Water (H₂O)

Strongest force: H-bonding · 2 lone pairs