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Isoelectronicity is a phenomenon observed when two or more molecules have the same structure (positions and connectivities among atoms) and the same electronic configurations, but differ by what specific elements are at certain locations in the structure. For example, CO, NO +, and N 2 are isoelectronic, while CH 3 COCH 3 and CH 3 N = NCH 3 are ...
This type of bond is sometimes called a "banana bond". B 2 H 6 is isoelectronic with C 2 H 6 2+, which would arise from the diprotonation of the planar molecule ethylene. [8] Diborane is one of many compounds with such unusual bonding. [9] Of the other elements in group IIIA, gallium is known to form a similar compound digallane, Ga 2 H 6.
The bond order itself is the number of electron pairs (covalent bonds) between two atoms. [3] For example, in diatomic nitrogen N≡N, the bond order between the two nitrogen atoms is 3 (triple bond). In acetylene H–C≡C–H, the bond order between the two carbon atoms is also 3, and the C–H bond order is 1 (single bond).
Borazine, also known as borazole, inorganic benzene, is an inorganic compound with the chemical formula B 3 H 6 N 3. In this cyclic compound, the three BH units and three NH units alternate. The compound is isoelectronic and isostructural with benzene. For this reason borazine is sometimes referred to as “inorganic benzene”.
Each oxygen must be bonded to the nitrogen, which uses four electrons—two in each bond. Place lone pairs. The 14 remaining electrons should initially be placed as 7 lone pairs. Each oxygen may take a maximum of 3 lone pairs, giving each oxygen 8 electrons including the bonding pair. The seventh lone pair must be placed on the nitrogen atom.
The compounds Co(NO)(CO) 3 and Ni(CO) 4 illustrate the analogy between NO + and CO. In an electron-counting sense, two linear NO ligands are equivalent to three CO groups. This trend is illustrated by the isoelectronic pair Fe(CO) 2 (NO) 2 and [Ni(CO) 4]. [3] These complexes are isoelectronic and, incidentally, both obey the 18-electron rule.
Isolobal compounds are analogues to isoelectronic compounds that share the same number of valence electrons and structure. A graphic representation of isolobal structures, with the isolobal pairs connected through a double-headed arrow with half an orbital below, is found in Figure 1. Figure 1: Basic example of the isolobal analogy
Compounds which are isoelectronic usually have similar chemical structures. For example, methane, CH 4, and the ammonium ion, NH 4 +, are isoelectric and are isostructural as both have a tetrahedral structure. The C-H and N-H bond lengths are different and crystal structures are completely different because the ammonium ion only occurs in salts.