CHM 131 Lecture Notes - Lecture 12: Lone Pair, Chlorine, Covalent Bond

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Polyatomics represent molecular orbitals with bonding and lone pair electrons. Accounts for all valence electrons contributed to the molecule by each of its atoms. Resonance structures arise when there is more than one way to arrange the electrons. Formal charge correlates a lewis dot structures electron locations to number of valence electrons an atom donates to a molecule. Each atom of the representative elements donates the number of electrons equivalent to group number (ia viia). Sum all available electrons, the molecule (lewis dot structure) must have this number of electrons. If there is an odd number of electrons, the lone electron exists in a nonbonding orbital or a multiple bond. If the compound is an ion, add one electron for each negative charge and subtract one electron for each positive charge. First atom is central atom (unless hydrogen, which can never be central) .

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