Two or more molecular entities (atoms, molecules, ions) are described as being isoelectronic with each other if they have the same number of electrons[1] or the same electron configuration[2] and the same structure (number and connectivity of atoms), regardless of the nature of the elements involved.
The term valence isoelectronic is used when the above conditions are met but with only the same number of valence electrons[3]
The statement "These compounds or molecules are isoelectronic" is not just an implemetation of the above definition. It has significance by fact that calculations on molecules and electron density, and therefore capability of reaction, have been performed on quite a lot of common substances. By identifying a new, rare or odd compound as being isoelectronic with an already known one offers clues to possible properties and reactions.
Examples
The N atom and the O+ radical ion are isoelectronic because each has 5 electrons in the outer electronic shell. Similarly, the cations K+, Ca2+, and Sc3+, the anions Cl−, S2−, and P3− are all isoelectronic with the Ar atom. In such monatomic cases, there is a clear trend in the sizes of such species, with atomic radius decreasing as charge increases.
CO, N2 and NO+ are isoelectronic because each have 2 nuclei and 10 valence electrons (4+6, 5+5, and 5+5, respectively).
The uncharged H2C=C=O molecule and the zwitterionic CH2=N+=N- molecule are isoelectronic.
CH3COCH3 and CH3N2CH3 are not isoelectronic. They do have the same number of nuclei and the same number of valence electrons, but the atoms' connectivity is different: the first one has both methyl (CH3) groups attached to carbonyl's (CO's) carbon atom, forming a trigonal planar structure: H3C-C(=O)-CH3; the second molecule's structure is linear: H3C-N=N-CH3 and its methyl groups are not connected to the same nitrogen atom.
The amino acids cysteine and serine are also considered (at least valence) isoelectronic.
References
- ^ Isoelectronic Configurations iun.edu
- ^ Isoelectronic thefreedictionary.com
- ^ Advances in Organonmetallic chemistry. F.G.A. Stone page 190 google books link
See also
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