Related Experiment Video
Updated: Aug 16, 2025

12:37
Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers
Published on: September 4, 2015
12.5K
Summary
Bloch-Zener oscillations in non-Hermitian lattices can transition from aperiodic to periodic, exhibiting unique smooth or sharp phase transitions. This phenomenon was observed in a photonic quantum walk experiment.
Area of Science:
- Wave Physics
- Quantum Mechanics
- Photonics
Background:
- Bloch-Zener oscillations (BZO) involve Bloch oscillations and Zener tunneling in two-band lattices under DC force.
- In Hermitian systems, BZO are typically aperiodic, only accidentally periodic.
- Non-Hermitian (NH) systems offer novel phenomena not seen in their Hermitian counterparts.
Purpose of the Study:
- To investigate the transition from aperiodic to periodic Bloch-Zener oscillations in non-Hermitian lattices.
- To explore the nature of phase transitions in NH BZO, specifically smooth vs. sharp transitions.
- To propose an experimental method for observing these phenomena.
Main Methods:
- Theoretical analysis of Bloch-Zener oscillations in two-band lattices under DC force.
- Investigation of non-Hermitian lattice parameters and their effect on BZO periodicity.
- Proposal of a discrete-time photonic quantum walk on a synthetic lattice for experimental realization.
Main Results:
- Non-Hermitian lattices allow for a transition from aperiodic to periodic BZO as a NH parameter is varied.
- The phase transition in NH BZO can be either smooth or sharp.
- This contrasts with other NH phase transitions, which are universally sharp.
Conclusions:
- Bloch-Zener oscillations in non-Hermitian systems exhibit unique phase transition properties.
- A photonic quantum walk provides a viable platform for experimentally observing smooth BZO phase transitions.
- The findings expand the understanding of wave physics in non-Hermitian systems.
More Related Videos
Related Concept Videos
Phase Transitions
19.5K
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...
19.5K
Phase Transitions: Melting and Freezing
12.6K
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...
12.6K
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
Phase Transitions: Sublimation and Deposition
17.4K
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...
17.4K
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
States of Matter and Phase Changes
1.2K
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...
1.2K

