Hydrogen Bonds - H2O, NH3, HF
Visualize hydrogen bond formation, tetrahedral coordination in ice, and the zigzag chain structure of HF. Learn why ice floats and why water has a high boiling point.
About this simulation
- What
- An interactive Chemistry simulation of Hydrogen Bonds - H2O, NH3, HF.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-03-17
Key Concepts
Hydrogen Bond
A strong intermolecular force between H (on N/O/F) and a lone pair.
Donor-Acceptor Match
Balanced H and lone pairs lead to the strongest networks (Water).
Tetrahedral Coord.
In ice, each water molecule connects to 4 others.
Anomalous Density
Ice is less dense than water due to its open hexagonal lattice.
Understanding Hydrogen Bonding
Hydrogen bonding is a special type of dipole-dipole attraction that occurs when a hydrogen atom bonded to a strongly electronegative atom (N, O, F) exists in the vicinity of another electronegative atom with a lone pair of electrons.
In water, this force is particularly strong and symmetrical. Each water molecule has two hydrogen atoms (donors) and two lone pairs (acceptors), allowing for a perfect 1:1 ratio that leads to a complex, three-dimensional network.
In contrast, Ammonia (NH₃) has 3 donors but only 1 acceptor, while Hydrogen Fluoride (HF) has 3 acceptors but only 1 donor. Both are 'limited' and cannot form the same level of interconnectivity as water.
This network is responsible for water's high boiling point, surface tension, and the fact that its solid state (ice) floats on its liquid state—a property essential for life on Earth.
Frequently Asked Questions
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