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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.
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The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their electron configurations are added to the table, a periodic recurrence of similar electron configurations in the outer shells of these elements is observed. Because they are in the outer shells of an atom, valence electrons play the most important role in chemical reactions. The outer electrons have the highest energy of the electrons in an atom...
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As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping includes lithium (Li), sodium (Na), and potassium (K). All of these elements are shiny, conduct heat and electricity well, and have similar chemical properties. A second grouping includes calcium (Ca), strontium (Sr), and barium (Ba), which also are shiny, good conductors of heat and electricity, and have chemical properties in common. However,...
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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...
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The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name “noble” because they were assumed to be nonreactive since they have filled valence shells. In 1962, Dr. Neil Bartlett at the University of British Columbia proved this assumption to be false.
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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...
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Elementos del grupo principal como metales de transición.

Philip P Power1

  • 1Department of Chemistry, University of California, Davis, California 95616, USA.

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|January 16, 2010
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Resumen
Este resumen es generado por máquina.

Los avances recientes revelan que los compuestos de elementos más pesados del grupo principal exhiben propiedades electrónicas únicas, que difieren significativamente de los elementos más ligeros. Su química es cada vez más paralela a los metales de transición, mostrando potencial en la catálisis.

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Área de la Ciencia:

  • Química Inorgánica La Química Inorgánica es la química inorgánica.
  • Química de los Elementos del Grupo Principal de Elementos

Sus antecedentes:

  • A finales del siglo XX y principios del siglo XXI se han producido avances significativos en la química de los elementos más pesados del grupo principal.
  • Los compuestos recién sintetizados revelan propiedades electrónicas distintas en comparación con los elementos más ligeros, lo que desafía la comprensión previa.

Objetivo del estudio:

  • Explorar las características estructurales y de enlace únicas de los compuestos de elementos más pesados del grupo principal.
  • Investigar los paralelos entre la reactividad de estos compuestos y los complejos de metales de transición.

Principales métodos:

  • Síntesis de nuevos compuestos de elementos más pesados del grupo principal.
  • Caracterización de las propiedades electrónicas y características estructurales.
  • Estudios de reactividad con moléculas pequeñas (por ejemplo, H2+, NH3+, C2+, H4+, CO).

Principales resultados:

  • Destacó las diferencias fundamentales en las propiedades electrónicas entre los elementos más pesados y más ligeros del grupo principal.
  • Demostró que la química de los elementos más pesados del grupo principal se asemeja cada vez más a la de los complejos de metales de transición.
  • Reacciones observadas de nuevos compuestos con moléculas pequeñas en condiciones suaves.

Conclusiones:

  • El estudio proporciona nuevos conocimientos estructurales y de vinculación en los elementos más pesados del grupo principal.
  • La química de los elementos más pesados del grupo principal comparte similitudes significativas con la química de los metales de transición.
  • Estos compuestos muestran potencial para aplicaciones catalíticas debido a su reactividad.