短距离和远距离的磁性排序以及在 (Mn1-xNix) 2P2S6中出现的拓过渡
Nasaru Khan1, Deepu Kumar2, Shantanu Semwal3
1School of Physical Sciences, Indian Institute of Technology Mandi, Mandi, 175005, India. nasarukhan736@gmail.com.
Scientific reports
|February 5, 2025
概括
本研究使用拉曼光谱学研究二维 (Mn1-xNix) 2P2S6磁性材料中的相变. 兴奋剂调节多个过渡,包括在低温下潜在的拓相过渡.
科学领域:
- 凝聚物质物理学 凝聚物质物理学
- 材料科学 材料科学 材料科学
- 这就是Spintronics.
背景情况:
- 二维磁性材料为自旋电子和拓现象提供可调节的特性.
- 默明-瓦格纳定理一般禁止在有限温度的2D系统中长距离的磁性顺序,除了拓相位过渡.
研究的目的:
- 为了分析二维 (Mn1-xNix) 2P2S6.6.2 的散装单晶体中取决于温度的相变.
- 调查兴奋剂 (x = 1,0.7,0.3,0) 对这些转变的影响.
- 探索这些材料中潜在的拓相位过渡.
主要方法:
- 在 (Mn1-xNix) 2P2S6 单晶上使用温度依赖的拉曼光谱.
- 语音频率的第一原则计算.
- 分析声子自身能量参数,模式强度和动态拉曼易感性.
主要成果:
- 在 (Mn1-xNix) 2P2S6 中观察到多个温度依赖的相位过渡,可与兴奋剂度 (x) 调节.
- 识别了 ~ 150-170 K 和 ~ 60-153 K 之间的明显过渡,与旋转-旋转相关性相关.
- 检测到低温过渡 (~24-60 K),可能表明拓相位过渡.
结论:
- 在 (Mn1-xNix) 2P2S6 中的兴奋剂有效调整磁性相位过渡.
- 拉曼光谱揭示了与旋转相关性和潜在的拓现象相关的变化.
- 这些材料对探索拓物理和自旋电子应用具有前景.
相关概念视频
03:02Colors and Magnetism
11.5K
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
11.5K
02:28Electronic Structure of Atoms
20.9K
An atom comprises protons and neutrons, which are contained inside the dense, central core called the nucleus, with electrons present around the nucleus. Taking into account the wave–particle duality of electrons and the uncertainty in position around the nucleus, quantum mechanics provides a more accurate model for the atomic structure. It describes atomic orbitals as the regions around the nucleus where electrons of discrete energy exist, characterized by four quantum...
20.9K
02:42Valence Bond Theory
8.4K
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
8.4K
02:58Properties of Transition Metals
24.9K
Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3–12 are transition elements. The f-block elements, also called inner transition metals (the lanthanides and actinides), also meet this criterion because the d orbital is partially occupied before the f orbitals.
24.9K
04:00Periodic Classification of the Elements
45.0K
The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their electron configurations are added to the table, a periodic recurrence of similar electron configurations in the outer shells of these elements is observed. Because they are in the outer shells of an atom, valence electrons play the most important role in chemical reactions. The outer electrons have the highest energy of the electrons in an atom...
45.0K
02:46Electron Configurations
16.2K
Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest energy available), Pauli exclusion principle (no two electrons can have the same set of four quantum numbers), and Hund’s rule of maximum multiplicity (whenever possible, electrons retain unpaired spins in degenerate orbitals).
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p,...
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p,...
16.2K