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Octet rule (including exceptions) In covalent molecules the atoms “want to” reach a stable 8-electron noble gas The central atom has formally
“octet rule” by sharing two electrons only Two hydrogen atoms form a covalent bond to make a hydrogen molecule Each contributes one electron
Carbon, nitrogen, oxygen, and fluorine must always follow the octet rule How to draw Lewis dot structures: 1) Determine the central atom
If no electrons are left and the central atom is not yet surrounded by four electron pairs (octet rule), convert one or more lone pairs from a terminal atom to
number of electrons in the valence shell of the central atom in a hypervalent molecule is less than 8; in other words, the modified octet rule is obeyed
Exceptions to the Octet Rule ? In those cases where the octet rule does not apply, the substituents attached to the central atom nearly
For example, sulfur, the central atom in SF6, has 12 electrons around it, exceeding the octet rule See pg 601 of your text ASSIGNING FORMAL CHARGE ON ATOMS