Related Experiment Video
Updated: Jul 19, 2026
08:02
A Computer Vision System for the Assessment of Ice Cream Melting Behavior
Published on: October 4, 2024
A universal criterion of melting
1Department of Chemistry, University of Houston, Houston, Texas 77204-5003, USA. vas@uh.edu
The Journal of Physical Chemistry. B
|September 22, 2006
Summary
This study reveals a universal melting criterion based on molecular spacing at interfaces, applicable even with system-specific interactions. It also analyzes supercooled liquids and their surface tension contributions.
Area of Science:
- Materials Science
- Condensed Matter Physics
- Physical Chemistry
Background:
- Melting dynamics at liquid-solid interfaces are complex.
- Understanding molecular behavior near phase transitions is crucial.
Purpose of the Study:
- To dynamically analyze melting as a localization problem at interfaces.
- To derive and validate a Lindemann-like melting criterion.
- To investigate molecular translations in supercooled fluids and surface tension contributions.
Main Methods:
- Dynamic analysis of melting.
- Derivation of a Lindemann-like criterion.
- Computation of molecular translations and surface tension components.
Main Results:
- A universal Lindemann ratio (approx. 0.1) for melting at interfaces was derived.
- A non-universal criterion for bulk solids, dependent on harmonic properties, was established.
- Surface tension in supercooled liquids is split between entropic and energetic factors.
Conclusions:
- Overdamped dynamics near melting contribute to the universality of the Lindemann ratio.
- The study provides insights into the physics of melting, supercooled liquids, and interfacial phenomena.
More Related Videos
Related Concept Videos
02:39Phase Transitions: Melting and Freezing
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...
02:34Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility
Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
01:24Solid–Solid Solutions
The temperature-composition phase diagram of two solids, A and B, which are immiscible in the solid phase but form miscible liquids, shows that when the temperature is low, these two exist as separate, pure solids (A and B). As the temperature increases, they transition into a single-phase liquid solution where A and B coexist. Moving from point a1 to a2 in the phase diagram, the composition changes such that solid B begins to separate from the solution, enriching the remaining liquid with A.
02:54Molecular and Ionic Solids
Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...
01:29Liquid–Solid Solutions
The process of a solid dissolving in a liquid to form a solution is governed by the solubility limit, which is the maximum amount of the solid substance, or solute, that can be dissolved in a specific volume of the liquid or solvent. As the solute dissolves, it reaches a point where no more solute can be dissolved at a given temperature - this is known as the saturation point. However, if further solute is added and it manages to dissolve, the solution becomes supersaturated. Supersaturated...
02:44Heating and Cooling Curves
When a substance—isolated from its environment—is subjected to heat changes, corresponding changes in temperature and phase of the substance is observed; this is graphically represented by heating and cooling curves.
For instance, the addition of heat raises the temperature of a solid; the amount of heat absorbed depends on the heat capacity of the solid (q = mcsolidΔT). According to thermochemistry, the relation between the amount of heat absorbed or released by a substance, q, and its...
For instance, the addition of heat raises the temperature of a solid; the amount of heat absorbed depends on the heat capacity of the solid (q = mcsolidΔT). According to thermochemistry, the relation between the amount of heat absorbed or released by a substance, q, and its...