Energy Levels of Singly-Ionized Platinum
Jean Blaise1, Jean-François Wyart1
1Laboratoire Aimé Cotton, 1 Bât. 505, C.N.R.S. Π, Centre Universitaire, F-91405-ORSAY ( France ).
Summary
Accurate wavelength measurements revealed 43 new even and 104 new odd energy levels for Platinum II (Pt II). The Slater-Condon method accurately interpreted these configurations, highlighting core interactions.
Area of Science:
- Atomic Physics
- Spectroscopy
- Quantum Mechanics
Background:
- The electronic structure of Platinum II (Pt II) is complex, requiring precise experimental data and theoretical models for accurate interpretation.
- Previous analyses of Pt II have provided a foundation, but further refinement is needed to fully understand its energy levels and configurations.
Purpose of the Study:
- To extend the analysis of Platinum II (Pt II) using new, accurate wavelength measurements.
- To identify and characterize new even and odd parity energy levels in Pt II.
- To interpret the observed energy levels using advanced theoretical methods, focusing on electron-shell interactions.
Main Methods:
- Utilized accurate wavelength measurements from Sansonetti et al. for the analysis of Pt II.
- Employed the Slater-Condon parametric method for theoretical interpretation of electronic configurations.
- Focused on low even configurations (5d⁹, 5d⁸6s, 5d⁷6s²) and high even configurations (5d⁸(7s+6d)).
Main Results:
- Discovered 43 new even and 104 new odd energy levels for Pt II.
- Achieved high accuracy in interpreting configurations, with root mean square deviations below 80 cm⁻¹.
- Demonstrated the critical role of the 5d⁸-5d⁷6s core interaction in explaining the even-parity levels.
Conclusions:
- The extended analysis significantly increases the number of known energy levels for Pt II.
- The Slater-Condon method, incorporating core interactions, provides a robust framework for understanding Pt II's atomic structure.
- Further investigation into core-shell interactions is crucial for a complete understanding of Pt II spectra.
More Related Videos
Related Concept Videos
Properties of Transition Metals
30.4K
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.
30.4K
Ionization Energy
44.1K
The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy (IE1). The first ionization energy for an element, X, is the energy required to form a cation with 1+ charge:
44.1K
Electron 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
Ionic Bonding and Electron Transfer
52.6K
Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions.
52.6K
The Energies of Atomic Orbitals
30.6K
In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
30.6K
Ions and Ionic Charges
80.1K
In ordinary chemical reactions, the nucleus — which contains the protons and neutrons of each atom and thus identifies the element — remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons to form electrically charged particles called...
80.1K


