Video Experimental Relacionado
Updated: Feb 1, 2026
09:58
Light-driven Enzymatic Decarboxylation
Published on: May 22, 2016
12.2K
Covalencia impulsada por la degeneración energética en el enlace de actinuros
Jing Su1, Enrique R Batista1, Kevin S Boland1
1Los Alamos National Laboratory , P.O. Box 1663, Los Alamos , New Mexico 87545 , United States.
Journal of the American Chemical Society
|December 13, 2018
Resumen
El enlace actinídeo revela una mezcla orbital significativa en los compuestos AnCl62. La covalencia aumenta con la contribución orbital 5f en toda la serie de actinidos, lo que afecta la comprensión de los enlaces químicos.
Área de la Ciencia:
- Química de las actinidas
- Química inorgánica
- Química computacional
Sus antecedentes:
- Comprender el enlace químico en los elementos actínidos es crucial.
- La covalencia de las actinidas influye en sus propiedades químicas y su reactividad.
Objetivo del estudio:
- Evaluación cuantitativa de la covalencia An-Cl en los complejos AnCl62.
- Para investigar el papel de los orbitales 5f y 6d en la unión de los actinuros.
Principales métodos:
- Espectroscopia de absorción de rayos X de la línea K.
- Cálculos de la teoría funcional de la densidad relativista.
Principales resultados:
- Se observó una mezcla significativa entre los orbitales Cl 3p y An IV 5f/6d.
- Los orbitales 6d mostraron un enlace covalente más pronunciado que los orbitales 5f.
- La mezcla orbital de An-Cl cambió a través de la serie de actínidos (de Th a Pu).
Conclusiones:
- La covalencia del actinido 6d orbital disminuye de Th a Pu.
- La covalencia del actinido 5f-orbital aumenta en toda la serie.
- Este estudio proporciona información cuantitativa sobre la naturaleza de los enlaces actínidos.
Más Videos Relacionados
Videos de Conceptos Relacionados
01:29Covalent Bonds
162.1K
Overview
162.1K
01:08Covalent Bonds
10.8K
Overview
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally,...
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally,...
10.8K
02:46Covalent Bonding and Lewis Structures
61.3K
Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual attraction of atoms for a “shared” pair of electrons.
61.3K
02:49Bond Energies and Bond Lengths
31.5K
Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
31.5K
02:24Polar Covalent Bonds
29.3K
Covalent bonds are formed between two atoms when both have similar tendencies to attract electrons to themselves (i.e., when both atoms have identical or fairly similar ionization energies and electron affinities). Nonmetal atoms frequently form covalent bonds with other nonmetal atoms. For example, the hydrogen molecule, H2, contains a covalent bond between its two hydrogen atoms. When two separate hydrogen atoms with a particular potential energy approach each other, their valence orbitals...
29.3K
02:40MO Theory and Covalent Bonding
14.0K
The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
14.0K