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Related Concept Videos

Crystal Growth: Principles of Crystallization01:25

Crystal Growth: Principles of Crystallization

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Crystallization is a phase transformation process in which crystals are precipitated from a supersaturated solution or formed from other sources. During crystallization, atoms or molecules arrange themselves into a well-defined, rigid crystal lattice to minimize energy.
Initiating crystallization involves manipulating the concentration of the solute and the temperature of the solution. Since crystal growth occurs when the ratio of concentration and solubility of the solute in the solvent...
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Recrystallization: Solid–Solution Equilibria01:10

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Recrystallization is a purification technique used to separate impurities from solid compounds. In this technique, no chemical reactions occur. Instead, it exploits physical properties only, specifically, the solubility differences between the desired compound and impurities, either at a single temperature or at different temperatures, and under other selected conditions. The solid-solution equilibrium (solubility equilibrium) of each component in the solution represents a binary phase...
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Phase Transitions: Melting and Freezing02:39

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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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Molecular and Ionic Solids02:54

Molecular and Ionic Solids

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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...
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Sublimation01:03

Sublimation

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Sublimation is the direct transformation of a solid to a gaseous state. For instance, at standard pressure and room temperature, solid carbon dioxide sublimes to gaseous carbon dioxide. The phase diagram depicts the conditions required for sublimation. This process occurs at the solid-gas phase boundary and is not observed above the triple point of the substance. The reverse of sublimation is called deposition, where a gaseous substance condenses directly into a solid. Sublimation and...
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Phase Transitions: Vaporization and Condensation02:39

Phase Transitions: Vaporization and Condensation

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The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules...
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Updated: Nov 18, 2025

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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How a supercooled liquid borrows structure from the crystal.

Ulf R Pedersen1, Ian Douglass1, Peter Harrowell2

  • 1Glass and Time, IMFUFA, Department of Science and Environment, Roskilde University, P.O. Box 260, DK-4000 Roskilde, Denmark.

The Journal of Chemical Physics
|February 9, 2021
PubMed
Summary
This summary is machine-generated.

Supercooled liquids can adopt crystal-like structures, like the Laves phase, without losing their liquid state. This borrowing of crystal structure may explain favored local structures in many liquids.

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Area of Science:

  • Condensed matter physics
  • Materials science
  • Computational chemistry

Background:

  • Supercooled liquids exhibit complex structural dynamics.
  • Understanding the local structure of supercooled liquids is crucial for predicting their behavior.

Purpose of the Study:

  • To investigate the local atomic structure in a supercooled binary atomic liquid mixture.
  • To determine if supercooled liquids can exhibit crystalline structures without destabilization.

Main Methods:

  • Utilizing advanced computer simulations.
  • Analyzing common neighbor structures within the supercooled liquid.
  • Comparing simulated structures to known equilibrium crystal phases, specifically the Laves structure.

Main Results:

  • The supercooled liquid mixture exhibits common neighbor structures analogous to the equilibrium Laves crystal phase.
  • A significant accumulation of crystal-like (Laves) structures was observed.
  • The liquid remained a true metastable liquid despite the presence of these crystalline structures.

Conclusions:

  • Supercooled liquids can incorporate crystalline structures without losing their metastability.
  • The ability to "borrow" crystal structures may be a fundamental characteristic of liquids with strong local ordering.