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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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Entropy and Solvation02:05

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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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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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Phase Transitions: Vaporization and Condensation02:39

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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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Freezing Point Depression and Boiling Point Elevation03:12

Freezing Point Depression and Boiling Point Elevation

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Boiling Point Elevation
The boiling point of a liquid is the temperature at which its vapor pressure is equal to ambient atmospheric pressure. Since the vapor pressure of a solution is lowered due to the presence of nonvolatile solutes, it stands to reason that the solution’s boiling point will subsequently be increased. Vapor pressure increases with temperature, and so a solution will require a higher temperature than will pure solvent to achieve any given vapor pressure, including one...
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Recrystallization: Solid–Solution Equilibria01:10

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2.0K
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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Controlling the Size, Shape and Stability of Supramolecular Polymers in Water
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Supercooled Low-Entropy Water Clusters.

Kouki Oka1, Toshimichi Shibue2, Natsuhiko Sugimura2

  • 1Department of Applied Chemistry, Waseda University, 3-4-1 Okubo Shinjuku, Tokyo 165-8555, Japan.

The Journal of Physical Chemistry Letters
|April 23, 2020
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Summary
This summary is machine-generated.

Investigating low-entropy water clusters in hydrophobic solvents revealed distinct structural changes and singularity temperatures. These findings offer new insights into water

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Area of Science:

  • Physical Chemistry
  • Materials Science
  • Biophysics

Background:

  • Water exhibits complex structural dynamics, particularly in confined or non-bulk environments.
  • Understanding water's behavior at low temperatures and in hydrophobic media is crucial for various scientific fields.

Purpose of the Study:

  • To investigate the properties of low-entropy water clusters and small bulk water domains in a hydrophobic solvent.
  • To elucidate the structural transitions and singularity temperatures of water under varying thermal conditions.
  • To propose a model explaining the observed water structures and their temperature-dependent populations.

Main Methods:

  • Utilized 1H nuclear magnetic resonance (NMR) spectroscopy to probe water structures.
  • Investigated a wide temperature range, including supercooling conditions (235-333 K).
  • Developed a theoretical model to interpret NMR data and water structural dynamics.

Main Results:

  • Identified singularity temperatures at approximately 300, 250, 235, and 225 K.
  • Proposed a model where water structures transition between disordered normal-liquid structure (DNLS) and locally favored tetrahedral structure (LFTS).
  • Observed that LFTS dominates below 250 K, converging to LFTS at 225 K, with increased phase transition rates at 235 K, indicating primary ice nucleation.

Conclusions:

  • Low-entropy water clusters in hydrophobic solvents represent a unique morphology.
  • These clusters act as valuable probe materials for fundamental water research.
  • The proposed model successfully explains the temperature-dependent structural transitions of water in this specific environment.