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Phase Transitions02:31

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Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to...
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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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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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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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Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3–12 are transition elements. The f-block elements, also called inner transition metals (the lanthanides and actinides), also meet this criterion because the d orbital is partially occupied before the f orbitals.
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Structural and magnetic phase transitions in Cs2[FeCl5(H2O)].

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Summary
This summary is machine-generated.

This study reveals a magnetoelectric compound with an erythrosiderite structure is not multiferroic. Investigations confirmed structural and antiferromagnetic transitions, excluding ferroelectric polarization.

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Area of Science:

  • Solid State Physics
  • Crystallography
  • Magnetism

Background:

  • The compound [Formula: see text] exhibits an erythrosiderite-related structure.
  • It is known to be magnetoelectric but not multiferroic.

Purpose of the Study:

  • To comprehensively investigate the structural and antiferromagnetic phase transitions.
  • To determine the compound's magnetoelectric and multiferroic properties.

Main Methods:

  • Polarization microscopy
  • Pyroelectric measurements
  • X-ray diffraction
  • Neutron diffraction

Main Results:

  • A structural phase transition from Cmcm to I2/c symmetry occurred at [Formula: see text] K, involving [Formula: see text] octahedra rotations and ordering of [Formula: see text] molecules and [Formula: see text] bonds.
  • Precise pyrocurrent measurements excluded significant ferroelectric polarization during this transition.
  • An antiferromagnetic phase transition at [Formula: see text] K resulted in the magnetic space group [Formula: see text], consistent with prior linear magnetoelectric effect and magnetization data.

Conclusions:

  • The compound [Formula: see text] is magnetoelectric but not multiferroic.
  • The observed structural transition is linked to molecular and bond ordering, not ferroelectricity.
  • The magnetic structure is well-defined and consistent with magnetoelectric coupling.