Relativistic effects and pressure-induced phase transition in CsAu
Júlia F B Manfro1, Giovani L Rech1, Janete E Zorzi1
1Universidade de Caxias do Sul, 95070-560, Caxias do Sul, RS, Brazil. juliaflachm@gmail.com.
Physical Chemistry Chemical Physics : PCCP
|January 29, 2024
Summary
Relativistic effects significantly alter cesium auride (CsAu) properties, stabilizing its structure and influencing its transition to a conducting state under pressure. Simulations reveal key structural and electronic changes crucial for understanding CsAu
Area of Science:
- Computational Materials Science
- Solid-State Physics
- Quantum Chemistry
Background:
- Cesium auride (CsAu) exhibits unusual ionic salt properties despite being composed of two metals.
- Understanding the influence of relativistic effects is crucial for accurately modeling CsAu's behavior.
Purpose of the Study:
- To investigate the impact of relativistic effects on CsAu's structure and physical properties.
- To explore pressure-induced phase transitions and the transition to a conducting state in CsAu.
- To analyze the effect of high pressures on CsAu's electronic band gap.
Main Methods:
- Utilized computer simulations to model CsAu.
- Performed calculations with and without relativistic effects for comparison.
- Analyzed structural, volumetric, and electronic properties under varying pressures.
Main Results:
- Relativistic effects reduce CsAu's lattice parameter and enhance charge transfer, aligning volumetric properties with alkali halides.
- The electronic band gap of CsAu is predicted to close around 31.5 GPa.
- Relativistic effects stabilize the CsAu Pm3̄m structure and shift the transition to the P4/mmm phase to 14 GPa.
Conclusions:
- Relativistic effects are essential for accurate predictions of CsAu's properties and phase transitions.
- CsAu is expected to transition to a conducting state at high pressures.
- The P4/mmm phase may serve as an intermediate state towards a stable high-pressure CsAu phase.
Related Concept Videos
Phase Diagrams
40.8K
A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. These diagrams indicate the physical states that exist under specific conditions of pressure and temperature and also provide the pressure dependence of the phase-transition temperatures (melting points, sublimation points, boiling points). Regions or areas labeled solid, liquid, and gas represent single phases, while lines or curves represent...
40.8K
Phase Transitions
19.1K
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...
19.1K
Phase Diagram
5.9K
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).
5.9K
States of Matter and Phase Changes
953
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...
953
Phase Transitions: Melting and Freezing
12.4K
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...
12.4K
Phase Changes
4.3K
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...
4.3K


