Magnetism in a 2D Hybrid Ruddlesden-Popper Perovskite through Charge Redistribution Driven by an Organic Functional
A Tofanello1, A L M Freitas1, T B de Queiroz1
1Center for Natural and Human Sciences (CCNH), Federal University of ABC (UFABC), Santo André 09210-580, Brazil.
The Journal of Physical Chemistry Letters
|February 4, 2022
Summary
This study introduces magnetism into two-dimensional Ruddlesden-Popper perovskites using histidine molecules. This novel approach creates a magnetic moment at the interface, potentially leading to new physical properties.
Area of Science:
- Materials Science
- Solid State Physics
- Chemistry
Background:
- Two-dimensional Ruddlesden-Popper (RP) perovskites exhibit tunable crystal structures and synthetic versatility.
- Introducing magnetism into these materials is an active area of research for novel electronic and spintronic applications.
Purpose of the Study:
- To develop a novel strategy for imparting magnetism to 2D RP perovskites.
- To investigate the mechanism of magnetism induction using histidine molecules as spacers.
Main Methods:
- Utilizing histidine molecules as organic spacers within the 2D RP perovskite structure.
- Analyzing the interaction between histidine functional groups (amide, imidazole, carboxyl) and lead ions.
- Characterizing the resulting magnetic properties and charge states.
Main Results:
- Histidine molecules successfully induce magnetism in 2D RP perovskites.
- The imidazole group, potentially aided by the carboxyl group, facilitates charge rearrangement from Pb2+ to paramagnetic Pb3+ ions.
- A positive magnetic moment is observed at the interface of the hybrid perovskite.
Conclusions:
- A novel class of magnetized 2D hybrid perovskites has been synthesized.
- The interface magnetism arises from Pb3+ formation mediated by histidine.
- These materials offer potential for unique physical properties due to coupled magnetism and quantum confinement effects.
Related Concept Videos
01:27π Electron Effects on Chemical Shift: Overview
1.2K
An applied magnetic field causes loosely bound π-electrons in organic molecules to circulate, producing a local or induced diamagnetic field over a large spatial volume. As the molecules tumble in solution, the field generated by π-electrons in spherical substituents results in a zero net field. However, the net field generated by π-electrons in non-spherical substituents is not zero. The effect of this induced field depends on the orientation of the molecule with respect to B0,...
1.2K
02:42Valence Bond Theory
9.8K
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...
9.8K
03:24Hybridization of Atomic Orbitals I
50.0K
The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
50.0K
03:02Colors and Magnetism
12.5K
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...
12.5K
03:35Hybridization of Atomic Orbitals II
34.5K
sp3d and sp3d 2 Hybridization
34.5K
02:38Valence Bond Theory and Hybridized Orbitals
23.7K
According to valence bond theory, a covalent bond results when: (1) an orbital on one atom overlaps an orbital on a second atom, and (2) the single electrons in each orbital combine to form an electron pair. The strength of a covalent bond depends on the extent of overlap of the orbitals involved. Maximum overlap is possible when the orbitals overlap on a direct line between the two nuclei.
A σ bond (single bond in a Lewis structure) is a covalent bond in which the electron density is...
A σ bond (single bond in a Lewis structure) is a covalent bond in which the electron density is...
23.7K