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Related Concept Videos

Phase Transitions02:31

Phase Transitions

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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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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 Diagram01:19

Phase Diagram

6.0K
The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region provide considerable insights into the thermal properties of substances. Such plots are known as phase diagrams. For instance, in the phase diagram for water (Figure 1), the solid curve boundaries between the phases indicate phase transitions (i.e., temperatures and pressures at which the phases coexist).
6.0K
Phase Transitions: Vaporization and Condensation02:39

Phase Transitions: Vaporization and Condensation

17.8K
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...
17.8K
States of Matter and Phase Changes00:59

States of Matter and Phase Changes

1.1K
The internal energy of a substance—the total kinetic energy of all its molecules and the potential energy of their associated forces—depends on the strength of the intermolecular forces in the condensed phases and the pressure exerted on the substance. The internal energy of a substance is the highest in the gaseous state, the lowest in the solid state, and intermediate in the liquid state. Phase transitions are caused by changes in physical conditions, such as temperature and...
1.1K
Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

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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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Orientational Transition in a Liquid Crystal Triggered by the Thermodynamic Growth of Interfacial Wetting Sheets
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Heating a dipolar quantum fluid into a solid.

J Sánchez-Baena1,2, C Politi3,4, F Maucher5,6

  • 1Center for Complex Quantum Systems, Department of Physics and Astronomy, Aarhus University, DK-8000, Aarhus C, Denmark. jsbaena@phys.au.dk.

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Summary
This summary is machine-generated.

Heating ultracold dipolar quantum fluids can surprisingly create a supersolid state, breaking translational symmetry. This finding challenges conventional thermal phase transitions and opens new avenues in quantum fluid thermodynamics.

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Area of Science:

  • Quantum physics
  • Condensed matter physics
  • Atomic physics

Background:

  • Materials typically melt or vaporize when heated due to increased particle motion.
  • Dipolar quantum fluids possess unique properties due to long-range dipole-dipole interactions.

Purpose of the Study:

  • To investigate the finite-temperature behavior of dipolar quantum fluids.
  • To explore deviations from standard thermal phase transition phenomenology.
  • To understand the conditions leading to supersolid formation in these systems.

Main Methods:

  • Theoretical study of the finite-temperature physics of dipolar quantum fluids.
  • Analysis of phase transitions induced by temperature changes.
  • Experimental observations using ultracold dysprosium atoms.

Main Results:

  • Heating a dipolar superfluid can induce a phase transition to a supersolid state.
  • This transition involves a spontaneous breaking of translational symmetry.
  • The observed phenomenon deviates from typical melting or vaporization behavior.

Conclusions:

  • Dipolar quantum fluids exhibit unusual thermal properties.
  • The formation of a supersolid state via heating is a key finding.
  • This research provides a platform for studying novel quantum thermodynamics.