Between bonded atoms and that electrons of each lone

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between bonded atoms and that electrons of each lone pari belong completely to one atom (and are not delocalized over several atoms). Recall COCl 2 : there are three possible resonance structures, which is the most stable and therefore lowest in energy? COCl 2 Rules for formal charges assigned to individual atoms 1. ½ of the electrons of a bond are assigned to each atom in the bond 2. Both electrons of a lone pair are assigned to the atom which the lone pair belongs. Formal Charge = (# of valence e-‘s in the free atom) – ½ (# of bonding e-‘s) - (# of lone pair e-‘s) Calculate the formal charge for EVERY atom in ALL of the resonance structures in COCl 2 When writing Lewis Structures for molecules: A. Choose the one having the lowest magnitude of formal charges (zero on all or as many atoms as possible) B. When 2 proposed Lewis structures have equal magnitudes of formal charge, choose the one having the formal negative charge on the MOST electronegative, and any formal positive charges on the LEAST electronegative atom. Try these: BF 3
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SOCl 2 Carbonyl compounds contain a C=O somewhere in the molecule like acetone and acetic acid. Draw the Lewis structures and all possible resonance structures (including formal charges) for acetic acid (HC 2 H 3 O 2 ) and acetone (CH 3 C=OCH 3 )
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