Related Experiment Video
Updated: Jun 22, 2026
07:24
Quantitative Atomic-Site Analysis of Functional Dopants/Point Defects in Crystalline Materials by Electron-Channeling-Enhanced Microanalysis
Published on: May 10, 2021
Effect of Cerium codoping on Er:BaY(2)F(8) crystals.
Optics Express
|June 6, 2009
Summary
Adding Cerium (Ce) to Erbium (Er):BaY(2)F(8) crystals significantly reduces Er lifetimes and enhances fluorescence. This research paves the way for developing low-threshold 1.5 micrometer Erbium lasers.
Area of Science:
- Solid-state spectroscopy
- Luminescence and optical materials
Background:
- Erbium-doped materials are crucial for 1.5 micrometer lasers.
- Cerium co-doping can modify spectroscopic properties of rare-earth ions.
Purpose of the Study:
- To investigate the spectroscopic properties of Er3+,Ce3+:BaY(2)F(8) single crystals.
- To understand the effect of Cerium concentration on Erbium ion lifetimes and fluorescence.
- To assess the potential for low-threshold 1.5 micrometer Erbium lasers.
Main Methods:
- Complete polarized spectroscopic investigation of Er3+,Ce3+:BaY(2)F(8) single crystals.
- Room temperature lifetime measurements as a function of Cerium concentration.
- Analysis using a rate equation model.
Main Results:
- Co-doping with 4% Cerium reduced Erbium (4)I(13/2) lifetime from 15.6 ms to 10 ms.
- Significant reduction in Erbium (4)I(11/2) and (4)S(3/2) lifetimes observed with Cerium co-doping.
- A four-fold increase in (4)I(13/2) fluorescence intensity and undetectable 3 micrometer transition intensity with 4% Cerium.
Conclusions:
- Cerium co-doping strongly influences Erbium ion luminescence in BaY(2)F(8) crystals.
- The observed changes suggest potential for improved laser performance.
- Results are promising for developing low-threshold 1.5 micrometer Erbium lasers.
Related Concept Videos
03:26Electron Configuration of Multielectron Atoms
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...
02:58Crystal Field Theory - Octahedral Complexes
Crystal Field Theory
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...
02:46Crystal Field Theory - Tetrahedral and Square Planar Complexes
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,...
01:27Lattice Energies of Ionic Crystals
Lattice energy represents the energy released when gaseous cations and anions combine to form an ionic solid, reflecting the strength of electrostatic interactions within the crystal. This process is fundamentally governed by Coulombic attraction between oppositely charged ions, where the potential energy varies inversely with the interionic distance and directly with the product of ionic charges. As ions approach one another, the electrostatic energy becomes increasingly negative, indicating a...