The recurrence of dense face-centered cubic cesium
Li-Min Guan1, Li Zhu2, Sheng-Yi Xie1
1School of Physics and Electronics, Hunan University, Changsha, 410082, People's Republic of China.
Summary
Alkali metal cesium (Cs) unexpectedly re-transforms to a face-centered cubic (fcc) phase above 180 GPa. This high-pressure fcc phase exhibits distinct electronic properties compared to its low-pressure counterpart.
Area of Science:
- Condensed Matter Physics
- Materials Science
- High-Pressure Physics
Background:
- Alkali metals like cesium (Cs) exhibit complex phase transitions under pressure.
- Cesium's known phases include body-centered cubic, face-centered cubic (fcc), oC84, tI4, oC16, and double hexagonal close-packed (dhcp).
Purpose of the Study:
- To investigate the high-pressure phase behavior of cesium beyond the dhcp phase.
- To predict and characterize novel high-pressure phases of Cs using computational methods.
Main Methods:
- First-principles structure searching prediction.
- Total-energy calculations.
- Transition state calculations.
Main Results:
- Cesium re-transforms to the fcc phase above 180 GPa, following the dhcp phase.
- This transition involves overcoming an energy barrier (144 meV/atom at 200 GPa) and a 0.3% volume collapse.
- The high-pressure fcc Cs phase shows distinct electronic properties, with d-electrons dominating the Fermi level and significant inner core electron overlap.
Conclusions:
- The fcc phase is a stable phase of cesium at extreme pressures.
- Similar phase transitions are predicted for potassium and rubidium at higher pressures.
- Understanding these transitions provides insight into the behavior of alkali metals under extreme conditions.
More Related Videos
Related Concept Videos
Ionic Crystal Structures
16.4K
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
16.4K
Lattice Centering and Coordination Number
11.0K
The structure of a crystalline solid, whether a metal or not, is best described by considering its simplest repeating unit, which is referred to as its unit cell. The unit cell consists of lattice points that represent the locations of atoms or ions. The entire structure then consists of this unit cell repeating in three dimensions. The three different types of unit cells present in the cubic lattice are illustrated in Figure 1.
Types of Unit Cells
Imagine taking a large number of identical...
Types of Unit Cells
Imagine taking a large number of identical...
11.0K
Structures of Solids
17.0K
Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds typically form ordered, crystalline solids. A crystalline solid has a precise melting temperature because each atom or molecule of the same type is held in place with the same forces or energy. Amorphous solids or non-crystalline solids (or, sometimes, glasses) which lack an ordered internal structure and are randomly arranged. Substances that...
17.0K
Metallic Solids
20.1K
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
20.1K
The Born-Haber Cycle
24.5K
Lattice Energy
24.5K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
46.7K
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
46.7K


