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Related Concept Videos

Aqueous Solutions and Heats of Hydration02:42

Aqueous Solutions and Heats of Hydration

Water and other polar molecules are attracted to ions. The electrostatic attraction between an ion and a molecule with a dipole is called an ion-dipole attraction. These attractions play an important role in the dissolution of ionic compounds in water.
When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between them. This process...
Intermolecular Forces03:13

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
Intermolecular Forces03:13

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
Aldehydes and Ketones with Water: Hydrate Formation01:20

Aldehydes and Ketones with Water: Hydrate Formation

An oxygen-based nucleophile, like water, can undergo addition reactions with aldehydes and ketones. The reaction leads to the formation of hydrates, also referred to as 1,1-diols or geminal diols.
The formation of hydrates is a reversible reaction. Hydrate formation is influenced by steric and electronic factors accompanying the alkyl substituents on the carbonyl group: The rate of hydrate formation increases with a decrease in the number of alkyl groups attached to the carbonyl carbon. Hence,...
Van der Waals Interactions01:24

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions between particles with permanent, partial, or temporary charges. The intermolecular forces between neutral atoms and molecules are ion–dipole, dipole–dipole, and dispersion forces, collectively known as van der Waals forces.Polar molecules have a partial positive charge on one end and a partial negative charge on the other end of the molecule,...
The Electrical Double Layer01:30

The Electrical Double Layer

In the region where two bulk phases meet, an intricate electric charge distribution arises due to charge transfer, ion adsorption, molecular orientation, and charge distortion. This complex distribution is commonly referred to as the electrical double layer.When a solid electrode interfaces with ions in an electrolyte solution, the speed of electron transfer dictates the rates of oxidation and reduction. The electrode acquires a charge through the escape of atoms into the solution as cations or...

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Related Experiment Video

Updated: Jun 13, 2026

Total Internal Reflection Absorption Spectroscopy (TIRAS) for the Detection of Solvated Electrons at a Plasma-liquid Interface
08:50

Total Internal Reflection Absorption Spectroscopy (TIRAS) for the Detection of Solvated Electrons at a Plasma-liquid Interface

Published on: January 24, 2018

Hydrated electrons at the water/air interface.

D M Sagar1, Colin D Bain, Jan R R Verlet

  • 1Department of Chemistry, University of Durham, South Road, Durham DH1 3LE, UK.

Journal of the American Chemical Society
|May 4, 2010
PubMed
Summary
This summary is machine-generated.

Hydrated electrons at the water/air interface solvate within 1 picosecond and persist for over 750 picoseconds. Surfactant studies reveal these electrons reside hydrated in the interfacial region, below the dividing surface.

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Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

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Total Internal Reflection Absorption Spectroscopy (TIRAS) for the Detection of Solvated Electrons at a Plasma-liquid Interface
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Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics
10:52

Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

Published on: April 12, 2019

Area of Science:

  • Physical Chemistry
  • Surface Science
  • Spectroscopy

Background:

  • Understanding interfacial electron dynamics is crucial for various chemical processes.
  • The behavior of hydrated electrons at interfaces presents unique challenges due to complex interactions.

Purpose of the Study:

  • To investigate the temporal dynamics of hydrated electrons at the water/air interface.
  • To determine the precise location of hydrated electrons relative to the interface using chemical probes.

Main Methods:

  • Time-resolved second-harmonic generation spectroscopy was employed.
  • Surfactants were utilized to probe the electron's location within the interfacial region.

Main Results:

  • Initial solvation of hydrated electrons occurs within approximately 1 picosecond.
  • Electrons remain associated with the water/air interface for extended periods (>750 picoseconds).
  • Surfactant experiments indicate the electrons are hydrated below the dividing surface in the interfacial region.

Conclusions:

  • Hydrated electrons exhibit significant persistence at the water/air interface.
  • The electron's location is confirmed to be within the hydrated layer beneath the interface.
  • This study provides key insights into interfacial electron behavior and solvation dynamics.