Comprender el mecanismo de dopaje de electrones en los nanotubos de carbono de pared única intercalados con potasio

Claudia Kröckel1, María Rosa Preciado-Rivas2, Victor Alexander Torres-Sánchez2

  • 1Department of Chemistry and Pharmacy and Joint Institute of Advanced Materials and Processes (ZMP) , Friedrich-Alexander University of Erlangen-Nuremberg , Nikolaus-Fiebiger-Strasse 10 , 91058 Erlangen , Germany.

Resumen

El dopaje de potasio de los nanotubos de carbono de pared única (SWCNT) debilita los enlaces carbono-carbono, reduciendo la frecuencia del modo de respiración radial (RBM). Este efecto se correlaciona con el diámetro SWCNT y la estructura electrónica, crucial para afinar las propiedades nanoelectrónicas.

Videos de Conceptos Relacionados

Electron Configuration of Multielectron Atoms03:26

Electron 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...
63.8K
Valence Bond Theory02:42

Valence Bond Theory

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...
10.9K
Electron Configurations02:46

Electron Configurations

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,...
24.9K