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SCAN0031 - 9-3 3 3 C-H bonds 4 8—6=2 5 2e‘ on C lone...

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Unformatted text preview: /\_ 9-3 3) 3 C-H bonds 4) 8—6=2 5) 2e‘ on C: lone pair 6) 7) 1—‘/2(2)=0 4—V2(6)—2=-l stresses” and 5 Vll. Resonance: having more than one valid, stable Lewis 1.8 Many molecules can be represented by 2 or more Lewis structures that differ only in the placement of electrons. In such cases electrons are delocalized, and the real electron distribution is a hybrid of e (mm-tutti contributing Lewis structures, each of which is called a resonance form. Rules for writing resonance structures: Not same as book rules Héillégfléét i 1) Individual resonance forms do not represent the reai molecule {doubEe-headed arrow) -. The real structure is a composite, or resonance hybrid of the different forms. They are single, unchanging structures, and they do not switch back and forth between resonance forms. The only diff. is they way they are written on paper. 2) Resonance forms differ only by position of TE and non—bonding electrons (double bonds and lone pairs). Neither the position nor the hybridization of atoms changes from one resonance form to another. 3) Resonance forms don’t have to be equivalent. Even though the two resonance forms aren’t equivalent (one has neg charge on C, the other on 0), they both contribute to the overall resonance hybrid. In this case the resonance hybrid is closer to the more stable form (0 with neg charge) than to the less stable form) . 9.. 0‘9 :01 l'll-i "He—’1“ \H H H H H H H H H H H H/ /©H<__>H ©\HHHMH H H H H H H H Best? a) maximize happy (fiiled shell) atoms (maximize the number ofbonds) I" b) minimize charge I? I c) minimize separation of charge ...
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