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Related Concept Videos

Hydrogen Bonds01:04

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 Bonds00:26

Hydrogen Bonds

Hydrogen BondsHydrogen 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...
Hybridization of Atomic Orbitals II03:35

Hybridization of Atomic Orbitals II

sp3d and sp3d 2 Hybridization
Hybridization of Atomic Orbitals I03:24

Hybridization of Atomic Orbitals I

The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory
Valence Bond Theory02:42

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...

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Related Experiment Video

Updated: Jul 3, 2026

Synthesis of Terpolymers at Mild Temperatures Using Dynamic Sulfur Bonds in Poly(S-Divinylbenzene)
09:16

Synthesis of Terpolymers at Mild Temperatures Using Dynamic Sulfur Bonds in Poly(S-Divinylbenzene)

Published on: May 20, 2019

Hydrogen bonding to divalent sulfur.

Daryl L Howard1, Henrik G Kjaergaard

  • 1Department of Chemistry, University of Otago, P.O. Box 56, Dunedin, New Zealand.

Physical Chemistry Chemical Physics : PCCP
|July 10, 2008
PubMed
Summary
This summary is machine-generated.

Sulfur is nearly as effective as oxygen in accepting hydrogen bonds. This study compared the hydrogen bonding of methanol with dimethyl sulfide and dimethyl ether using spectroscopy and computational methods.

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Area of Science:

  • Physical Chemistry
  • Spectroscopy
  • Computational Chemistry

Background:

  • Hydrogen bonding is crucial in chemistry and biology.
  • Understanding the relative strengths of hydrogen bond acceptors is important.
  • Oxygen and sulfur are common elements involved in hydrogen bonding.

Purpose of the Study:

  • To compare the hydrogen bond accepting abilities of sulfur and oxygen.
  • To quantify the strength of hydrogen bonds formed by methanol with dimethyl sulfide and dimethyl ether.

Main Methods:

  • Vapor phase infrared spectroscopy was employed.
  • Ab initio calculations were performed for theoretical analysis.
  • Temperature dependence studies were used to determine enthalpies.

Main Results:

  • Sulfur is a weaker, yet nearly equivalent, hydrogen bond acceptor compared to oxygen.
  • Enthalpies of hydrogen bond formation were determined for methanol-dimethyl sulfide and methanol-dimethyl ether complexes.

Conclusions:

  • The findings provide insights into the subtle differences between oxygen and sulfur as hydrogen bond acceptors.
  • This research contributes to a deeper understanding of intermolecular interactions involving chalcogens.