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The octet rule is a chemical rule of thumb that reflects the theory that main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas. The rule is especially applicable to carbon, nitrogen, oxygen, and the halogens; although more generally the ...
Since these compounds tend to be more reactive than compounds that obey their rule, electron counting is an important tool for identifying the reactivity of molecules. While the counting formalism considers each atom separately, these individual atoms (with their hypothetical assigned charge) do not generally exist as free species .
A Michael reaction is used as a mechanistic step by many covalent inhibitor drugs. Cancer drugs such as ibrutinib, osimertinib, and rociletinib have an acrylamide functional group as a Michael acceptor. The Michael donor on the drug reacts with a Michael acceptor in the active site of an enzyme. This is a viable cancer treatment because the ...
In 1960, Linnett originated a modification to the octet rule, originally proposed by Lewis, concerning valence electrons. He proposed that the octet should be considered as a double quartet of electrons rather than as four pairs, and hence the theory became known as "Linnett double-quartet theory". Using this method, he was able to explain the ...
On these views, he proposed the rule of eight or octet rule: Ions or atoms with a filled layer of eight electrons have a special stability. [17] Moreover, noting that a cube has eight corners Lewis envisioned an atom as having eight sides available for electrons, like the corner of a cube.
Satisfy the octet rule. Both oxygen atoms currently have 8 electrons assigned to them. The nitrogen atom has only 6 electrons assigned to it. One of the lone pairs on an oxygen atom must form a double bond, but either atom will work equally well. Therefore, there is a resonance structure. Tie up loose ends.
Valence Bond theory describes chemical bonding better than Lewis Theory, which states that atoms share or transfer electrons so that they achieve the octet rule. It does not take into account orbital interactions or bond angles, and treats all covalent bonds equally. [8]
The formulae of simple oxyanions are determined by the octet rule. The corresponding oxyacid of an oxyanion is the compound H z A x O y. The structures of condensed oxyanions can be rationalized in terms of AO n polyhedral units with sharing of corners or edges between polyhedra.