Related Experiment Video
Updated: Feb 19, 2026
11:21
Cooling an Optically Trapped Ultracold Fermi Gas by Periodical Driving
Published on: March 30, 2017
7.9K
Quantum phase slips: from condensed matter to ultracold quantum gases
C D'Errico1,2, S Scaffidi Abbate2, G Modugno3,2
1Istituto Nazionale di Ottica, CNR, 50019 Sesto Fiorentino, Italy derrico@lens.unifi.it.
Summary
Quantum phase slips (QPS) are key excitations in 1D superfluids and superconductors. Recent experiments show QPS signatures in Bose superfluids, advancing our understanding of quantum phenomena.
Area of Science:
- Condensed matter physics
- Quantum gas superfluids
- Low-temperature physics
Background:
- Quantum phase slips (QPS) are fundamental excitations in 1D superfluids and superconductors.
- QPS have been extensively studied in condensed matter systems.
- Recent observations have detected QPS signatures in quantum gas superfluids.
Purpose of the Study:
- To review findings on quantum phase slips from superconductors to quantum gases.
- To highlight recent experimental evidence of QPS in 1D Bose superfluids.
- To discuss the role of QPS in dissipation in these systems.
Main Methods:
- Review of existing research on quantum phase slips.
- Analysis of experimental data from 1D Bose superfluids.
- Focus on dissipation measurements in superfluids within periodic potentials.
Main Results:
- Summarized key results concerning quantum phase slips across different systems.
- Presented experimental evidence for QPS in 1D Bose superfluids.
- Identified signatures of QPS in the dissipation of superfluids in periodic potentials.
Conclusions:
- Quantum phase slips are observable in both superconductors and quantum gases.
- Recent experiments provide strong evidence for QPS in 1D Bose superfluids.
- Understanding QPS is crucial for comprehending dissipation in quantum systems.
Related Concept Videos
02:31Phase Transitions
23.4K
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...
23.4K
02:39Phase Transitions: Vaporization and Condensation
21.7K
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...
21.7K
02:33Phase Transitions: Sublimation and Deposition
20.4K
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...
20.4K
02:39Phase Transitions: Melting and Freezing
15.3K
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...
15.3K
00:59States of Matter and Phase Changes
5.0K
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...
5.0K
01:19Phase Changes
5.4K
Phase transitions play an important theoretical and practical role in the study of heat flow. In melting or fusion, a solid turns into a liquid; the opposite process is freezing. In evaporation, a liquid turns into a gas; the opposite process is condensation.
A substance melts or freezes at a temperature called its melting point and boils or condenses at its boiling point. These temperatures depend on pressure. High pressure favors the denser form of the substance, so typically, high pressure...
A substance melts or freezes at a temperature called its melting point and boils or condenses at its boiling point. These temperatures depend on pressure. High pressure favors the denser form of the substance, so typically, high pressure...
5.4K