CHEM101 Lecture 14: February 6: Breaking the Octet Rule (continued), Formal Atom Charges, Resonance Structures, Electron Delocalization, Picking the Best Resonance Structures.
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CHEM101 Lecture 13: February 4: Introduction to Molecular Structure and Bonding, the Step-By-Step Approach to Writing Lewis Structures,
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CHEM101 Lecture 14: February 6: Breaking the Octet Rule (continued), Formal Atom Charges, Resonance Structures, Electron Delocalization, Picking the Best Resonance Structures.
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CHEM101 Lecture 15: February 8: Review, Lewis Dot Structures, Resonance Structures,Picking the Best Resonance Structures (continued), Molecular Shape and Structure (not on first midterm), Electron Group Arrangements and Molecular Shapes, VSEPR Guidelines
Document Summary
February 6: breaking the octet rule (continued), formal atom charges, Resonance structures, electron delocalization, picking the best resonance. The second type of molecule which breaks the octet rule is when the central atom has less than or equal to 4 bonds, but some of the bonds are multi-bonds. In the diagram it shows 4 bonds but 1 of the bonds is a double bond meaning that there are 10 electrons on the central atom, not only 8 electrons like it would be if following the octet rule. In this diagram we see that there are 3 bonds on the cl atom and then 2 lone pairs as well. The lone pairs are on the central atom because the terminal atoms don"t have any more places to fit electrons. Formal charge = total valence electrons - (#unshared valence e + #shared valence e) Formal charges should be as close as possible.
