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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 ...
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”.
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
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).
Two p-orbitals forming a pi-bond. A double bond has two shared pairs of electrons, one in a sigma bond and one in a pi bond with electron density concentrated on two opposite sides of the internuclear axis. A triple bond consists of three shared electron pairs, forming one sigma and two pi bonds. An example is nitrogen.
The double bond is also stronger, 636 kJ mol −1 versus 368 kJ mol −1 but not twice as much as the pi-bond is weaker than the sigma bond due to less effective pi-overlap. In an alternative representation, the double bond results from two overlapping sp 3 orbitals as in a bent bond. [3]
In chemistry, linkage isomerism or ambidentate isomerism is a form of structural isomerism in which certain coordination compounds have the same composition but differ in which atom of the ligand is bonded to the metal. Typical ligands that give rise to linkage isomers are: cyanide, CN − – isocyanide, NC −; cyanate, OCN − – isocyanate ...