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Hydrogen Bonds

Hydrogen Bonds

A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...

Hydrogen Bonds

Hydrogen Bonds

Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....

Alkyl Halides

Alkyl Halides

Structural Properties
Alkyl halides are halogen-substituted alkanes wherein one or more hydrogen atoms of an alkane is replaced by a halogen atom such as fluorine, chlorine, bromine, or iodine. The carbon atom in an alkyl halide is bonded to the halogen atom, which is sp3-hybridized and exhibits a tetrahedral shape.
Unlike alkyl halides, compounds in which a halogen atom is bonded to an sp2 -hybridized carbon atom of a carbon-carbon double bond (C=C) are called vinyl halides. Whereas aryl...

Molecular Shape and Polarity

Molecular Shape and Polarity

Dipole Moment of a Molecule

Formation of Halohydrin from Alkenes

Formation of Halohydrin from Alkenes

An alkene, such as propene, reacts with bromine in the presence of water to yield a halohydrin. Halohydrins contain a halogen and a hydroxyl group attached to adjacent carbons. When the halogen is bromine, it is called a bromohydrin, while a chlorohydrin has chlorine as the halogen.

Halogenation of Alkenes

Halogenation of Alkenes

Halogenation is the addition of chlorine or bromine across the double bond in an alkene to yield a vicinal dihalide. The reaction occurs in the presence of inert and non-nucleophilic solvents, such as methylene chloride, chloroform, or carbon tetrachloride.
Consider the bromination of cyclopentene. Molecular bromine is polarized in the proximity of the π electrons of cyclopentene. An electrophilic bromine atom adds across the double bond, forming a cyclic bromonium ion intermediate.

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Related Experiment Video

Updated: Apr 15, 2026

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

Halogen bonding in solution.

Anna-Carin C Carlsson¹, Alberte X Veiga, Máté Erdélyi

¹Department of Chemistry and Molecular Biology, Gothenburg University, Gothenburg, Sweden.

Topics in Current Chemistry

|March 26, 2015

Summary

This summary is machine-generated.

Solvent effects significantly influence halogen bonding interactions in chemistry and biology. Polar solvents can stabilize neutral bonds but destabilize charged ones, while hydrogen bond donors disrupt all halogen bonds.

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Area of Science:

Chemistry
Biochemistry
Molecular Interactions

Background:

Halogen bonding is crucial for molecular recognition in chemistry and biology.
Understanding solvent effects is vital as most interactions occur in solution.
Solution studies offer insights into forces like charge transfer, dispersion, and electrostatics in halogen bonds.

Purpose of the Study:

To review literature on halogen bonding, focusing on solvent effects.
To analyze the electronic characteristics of halogen-bonded complexes.
To discuss charged/neutral and two-/three-center halogen bonds.

Main Methods:

Literature review of halogen bonding studies.
Analysis of solvent effects on different types of halogen bonds.
Examination of electronic characteristics and contributing forces.

Main Results:

Solvent polarity slightly stabilizes neutral two-center bonds but destabilizes charged ones.
Polar solvents affect three-center bond geometry minimally but aid counter-ion dissociation.
Charged three-center bonds strengthen with polarity; hydrogen bond donors destabilize all bonds.
Electrostatic models are insufficient for polar systems; dispersion is key for neutral bonds, charge transfer for charged bonds.

Conclusions:

Solvent polarity and hydrogen bonding significantly modulate halogen bond strength and characteristics.
Accurate modeling of halogen bonds requires considering solvent interactions and specific electronic contributions.
Halogen bonding is a complex interaction influenced by multiple factors, necessitating detailed solvent effect analysis.