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Related Concept Videos

States of Water01:23

States of Water

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Water exists in any one of the three classical states: solid (ice), liquid (water), and gas (steam or water vapor). The state of water depends on i) the intermolecular forces that draw molecules together and ii) the kinetic energy that leads to movements that pull them apart.
Water freezes when the intermolecular forces are greater than the kinetic energy. Unlike most other substances, water is less dense in its solid state than in its liquid state. This is because each water molecule can form...
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Phase Transitions: Melting and Freezing02:39

Phase Transitions: Melting and Freezing

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Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
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Entropy and Solvation02:05

Entropy and Solvation

8.8K
The process of surrounding a solute with solvent is called solvation. It involves evenly distributing the solute within the solvent. The rule of thumb for determining a solvent for a given compound is that like dissolves like. A good solvent has molecular characteristics similar to those of the compound to be dissolved. For example, polar solutions dissolve polar solutes, and apolar solvents dissolve apolar solutes. A polar solvent is a solvent that has a high dielectric constant (ϵ...
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Hydrogen Bonds01:04

Hydrogen Bonds

16.3K
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...
16.3K
Hydrogen Bonds00:26

Hydrogen Bonds

136.4K
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....
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Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

21.0K
Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
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Related Experiment Video

Updated: Apr 5, 2026

A Microfluidic Approach for the Study of Ice and Clathrate Hydrate Crystallization
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A Microfluidic Approach for the Study of Ice and Clathrate Hydrate Crystallization

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Evolution of Hydrogen Dynamics in Amorphous Ice with Density.

A Parmentier1, J J Shephard2,3, G Romanelli1

  • 1†Dipartimento di Fisica and NAST Centre, Università degli Studi di Roma Tor Vergata, Via della Ricerca Scientifica 1, 00133 Roma, Italy.

The Journal of Physical Chemistry Letters
|August 13, 2015
PubMed
Summary

Deep inelastic neutron scattering (DINS) and inelastic neutron scattering (INS) reveal how hydrogen atoms move in amorphous ices. Higher density weakens hydrogen bonds and increases hydrogen kinetic energy, with DINS offering superior insights into O-H stretching dynamics.

Keywords:
Raman spectroscopydeep inelastic neutron scatteringhydrogen bondingiceinelastic neutron scattering

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An Externally-Heated Diamond Anvil Cell for Synthesis and Single-Crystal Elasticity Determination of Ice-VII at High Pressure-Temperature Conditions
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Analyzing Melts and Fluids from Ab Initio Molecular Dynamics Simulations with the UMD Package

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Area of Science:

  • Condensed matter physics
  • Materials science
  • Physical chemistry

Background:

  • Amorphous ices are technologically relevant materials.
  • Understanding single-particle dynamics is crucial for characterizing material properties.
  • Hydrogen bonding significantly influences the behavior of amorphous ices.

Purpose of the Study:

  • To investigate the single-particle dynamics of hydrogen atoms in amorphous ices.
  • To determine the effect of density on hydrogen kinetic energy and bonding.
  • To compare the capabilities of DINS, INS, and Raman spectroscopy for probing O-H stretching modes.

Main Methods:

  • Deep inelastic neutron scattering (DINS)
  • Inelastic neutron scattering (INS)
  • Analysis of hydrogen kinetic energies and vibrational potentials

Main Results:

  • Mean kinetic energies of hydrogen nuclei increase with density.
  • Increasing density weakens hydrogen bonds and leads to more harmonic potentials.
  • DINS reveals more significant changes in O-H stretching kinetic energy than INS or Raman spectroscopy.
  • Anharmonicity constants for O-H stretching modes were determined.

Conclusions:

  • DINS is a powerful technique for accurate ground-state kinetic energy determination beyond the harmonic approximation.
  • The study provides benchmark kinetic energy data for path-integral Monte Carlo simulations.
  • Density plays a critical role in modifying hydrogen bonding and dynamics in amorphous ices.