Isoelectronicity

As isoelectronic refers to two atoms, ions, or molecules when they have the same number of electrons and a very similar electron configuration, although they consist of other elements. This results in the case of compounds a matching binding geometry.

Physical and chemical properties of isoelectronic compounds often differ quite strong. Since the total charge and / or the charge distribution of isoelectronic compounds often differ significantly from each other, are properties that are particularly strongly affected hereof, less similar than others, which will remain less affected (see isosterism ). Some isoelectronic compounds have, for example, very similar qualities as a ligand or " Lewis base " in complex compounds, see the examples.

More broadly, the term " isoelectronic ". Only the valence must be structured in the same and filled with the same number of electrons. These include, for example, compounds in which one partner is replaced by the periodic table above or below him a standing item.

Examples

Isoelectronic:

  • O2 - F - Ne - Na
  • HF - OH - NH2
  • CO - CN - NO - N2
  • CO2 - N3

Isoelectronic:

  • O2 - Cl - Ne - K
  • CCl4 - SiCl4 - AlCl4 - - PBr4
  • H2SO4 - H2S2O3 - H2PO4 -
  • [Mo ( CO) 6] - [V (CO) 6 ] - [ Fe (CN ) 6] 4 -
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