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chemistry/hydrogen-bonds
View PricingHydrogen 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.
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Hydrogen Bonds
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.
Frequently Asked Questions
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