Lec21_drobny_11 - Lewis Dot Structures Lecture 21 Reading...

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Lewis Dot Structures • Lecture 21 • Reading: Zumdahl 13.9-13.12 • Recommended Problems: 13.51, 13.53, 13.57, 13.59 • Outline – Lewis Dot Structure Basics – Resonance – Formal Charge
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Localized Bond Models • Consider our energy diagram for H 2 bonding:
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Localized Model Limitations It is important to keep in mind that the models we are discussing are just that…. .models. We are operating under the assumption that when forming bonds, atoms “share” electrons using atomic orbitals (AO). – Electrons involved in bonding: “bonding pairs”. – Electrons not involved in bonding: “lone pairs”. In reality, once atoms come together in a molecule, the electrons are no longer localized in AOs. ..they now occupy delocalized molecular orbitals. But don’t fret. ..molecular orbitals appear in Chem 162! Just remember that electrons don’t necessarily stay with the atom they came in with.
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Background J.J. Thomson (1914): Proposed that electrons (which he discovered) are arranged in shells within atoms. Outermost shell contains “valence electrons” which may not exceed 8. Valence electrons are transferred between atoms in ionic solids to achieve noble gas conFgurations. Gilbert N. Lewis (1916): Concerned with bonding in organic compounds. Originated idea of shared electron pairs between atomic pairs. “The chemical bond is at all times and in all molecules merely a pair of electrons jointly held by two atoms”. Proposed the “cubic” atom, now shown as a dot structure and “rule of eight”. Irving Langmuir (1919): Popularized and extended Lewis’ theory. Originated term “Octet Rule”.
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Lewis Dot Structures (cont.) • Developed by G. N. Lewis to serve as a way to describe bonding in polyatomic systems. • Central idea:
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This note was uploaded on 01/25/2012 for the course CHEM CHEM 152 taught by Professor Daruwala during the Spring '09 term at University of Washington.

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Lec21_drobny_11 - Lewis Dot Structures Lecture 21 Reading...

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