Related Experiment Video
Updated: Mar 11, 2026
10:57
Synthesis and Performance Characterizations of Transition Metal Single Atom Catalyst for Electrochemical CO2 Reduction
Published on: April 10, 2018
19.3K
Electronic ground state of Ni2
V Zamudio-Bayer1, R Lindblad1, C Bülow1
1Institut für Methoden und Instrumentierung der Forschung mit Synchrotronstrahlung, Helmholtz-Zentrum Berlin für Materialien und Energie, Albert-Einstein-Straße 15, 12489 Berlin, Germany.
The Journal of Chemical Physics
|November 24, 2016
Summary
The ground state of the Ni2+ molecular cation was determined using X-ray magnetic circular dichroism. This study suggests 3d transition metal cations favor maximum spin magnetic moments in their ground states.
Area of Science:
- Atomic and Molecular Physics
- Quantum Chemistry
- Materials Science
Background:
- Understanding the electronic and magnetic properties of diatomic molecular cations is crucial for various fields.
- Nickel dimer cation (Ni2+) is a key species in transition metal chemistry.
Purpose of the Study:
- To experimentally determine the ground state properties of the Ni2+ molecular cation.
- To investigate the spin magnetic moment contribution in 3d transition metal diatomic cations.
Main Methods:
- Utilized temperature and magnetic-field-dependent X-ray Magnetic Circular Dichroism (XMCD) spectroscopy.
- Employed a cryogenic ion trap with buffer gas cooling to achieve low temperatures (7.4±0.2 K).
Main Results:
- The Φ9/24 ground state of Ni2+ was experimentally determined.
- The spin dipole operator contribution to the XMCD sum rule was found to be 0.17±0.06 μB per atom.
- This contribution represents approximately 11% of the total spin magnetic moment.
Conclusions:
- Homonuclear diatomic molecular cations of 3d transition metals generally exhibit maximum spin magnetic moments in their electronic ground states.
- The findings provide insights into the magnetic behavior of transition metal molecular ions.
Related Concept Videos
02:46Electron Configurations
27.3K
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,...
27.3K
03:26Electron Configuration of Multielectron Atoms
66.0K
The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...
66.0K
01:14Atomic Nuclei: Nuclear Spin State Population Distribution
2.5K
Near absolute zero temperatures, in the presence of a magnetic field, the majority of nuclei prefer the lower energy spin-up state to the higher energy spin-down state. As temperatures increase, the energy from thermal collisions distributes the spins more equally between the two states. The Boltzmann distribution equation gives the ratio of the number of spins predicted in the spin −½ (N−) and spin +½ (N+) states.
2.5K
01:03Atomic Nuclei: Nuclear Spin State Overview
2.1K
NMR-active nuclei have energy levels called 'spin states' that are associated with the orientations of their nuclear magnetic moments. In the absence of a magnetic field, the nuclear magnetic moments are randomly oriented, and the spin states are degenerate. When an external magnetic field is applied, the spin states have only 2 + 1 orientations available to them. A proton with = ½ has two available orientations. Similarly, for a quadrupolar nucleus with a nuclear spin value of one, the...
2.1K
03:51Molecular Orbital Theory II
28.1K
Molecular Orbital Energy Diagrams
28.1K
03:02The Aufbau Principle and Hund's Rule
77.6K
To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and continuing across the periods of the periodic table, we add one proton at a time to the nucleus and one electron to the proper subshell until we have described the electron configurations of all the elements. This procedure is called the aufbau principle, from the German word aufbau (“to build up”). Each added electron occupies the...
77.6K