CHEM 142 Lecture Notes - Lecture 9: Formal Charge, Octet Rule, Valence Electron
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Some atoms break the octet rule in forming bonds by either having less than or exceeding. The second-row elements c,n,o and f should always assume to obey the octet rule. The second row elements b and be often have fewer than 8 electrons. Third row and heavier elements often satisfy the octet rule but are assumed in the simplest model to exceed the octet rule by using their empty valenced orbitals. Requires that we compare: the number of valence electrons on the fine neutral atom and, the number of valence electrons belonging to a given atom. Valence electrons belonging = (# of lone pairs) + . 5 (# of shared pairs) Describes how homogenously the electron density is distributed. Structure w/ most homogeneous (min formal charge on all atoms) tend to be more correct. Carbon almost never appears with a lone pair. Oxygen almost never appears with a positive formal charge.
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