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Solid–Solid Solutions01:24

Solid–Solid Solutions

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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.
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Liquid–Solid Solutions01:29

Liquid–Solid Solutions

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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...
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Recrystallization: Solid–Solution Equilibria01:10

Recrystallization: Solid–Solution Equilibria

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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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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.
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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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Metallic Solids

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Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
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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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Containerless solidification of undercooled SrO-Al2O3 binary melts.

Katsuyoshi Kato1, Atsunobu Masuno, Hiroyuki Inoue

  • 1Institute of Industrial Science, The University of Tokyo, 4-6-1 Komaba, Meguro-ku, Tokyo 153-8505, Japan. masuno@iis.u-tokyo.ac.jp.

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The SrO-Al2O3 system exhibits excellent glass-forming ability under containerless conditions. This study reveals insights into melt solidification and crystallization behavior, crucial for material science applications.

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Area of Science:

  • Materials Science
  • Physical Chemistry
  • Solid State Physics

Background:

  • Understanding the solidification behavior of binary oxide systems is critical for developing new materials.
  • Containerless processing minimizes heterogeneous nucleation, allowing for the study of intrinsic melt properties.
  • The SrO-Al2O3 system is of interest for its potential glass and ceramic applications.

Purpose of the Study:

  • To investigate the glass-forming ability and solidification characteristics of the SrO-Al2O3 binary system.
  • To determine the influence of cooling rates on crystallization behavior under containerless conditions.
  • To establish continuous cooling transformation diagrams for undercooled SrO-Al2O3 melts.

Main Methods:

  • Utilized an aerodynamic levitation furnace for containerless processing of SrO-Al2O3 samples.
  • Obtained cooling curves at various constant cooling rates (1-1000 °C s(-1)).
  • Analyzed crystallization and melting temperatures to assess glass-forming ability.

Main Results:

  • Glass formation was observed in specific SrO-Al2O3 compositions (35-45 mol% SrO and 55-75 mol% SrO).
  • Crystallization temperature showed independence from cooling rate for fully crystallized samples, indicating high glass-forming ability.
  • A decrease in crystallization temperature was noted for partially crystallized samples.

Conclusions:

  • The SrO-Al2O3 system possesses high glass-forming ability, supported by time-independent crystallization temperatures.
  • Containerless processing and continuous cooling transformation diagrams offer valuable insights into undercooled melt solidification.
  • The findings contribute to a deeper understanding of glass transition and crystallization kinetics in binary oxide systems.