110325 - The chemical bond (Chapter 12 447-458) Lewis...

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1 CHM3400 - Lecture 29 Mar 25 The chemical bond (Chapter 12 447-458) Lewis structures Valence bond theory Hybridization Electronegativity Dipole moment
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2 Lewis structures Guideline when drawing Lewis structures is the octet rule : “each atom (other than hydrogen) tends to form bonds in order to be surrounded by eight valence electrons” Can draw resonance structures (e.g. NO 2 - ): Structures for O 3 , CO? Only a simplified theory: No information on bond strengths Examples of complexes that do not follow octet rule (e.g. NO)
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3 Valence bond theory Sharing of the electrons between both nuclei: d ) = experimental ly determined a ) Combination of two atomic orbitals : ) 2 ( ) 1 ( B A ψ ψ= Electrons A + B, nuclei 1 + 2 b ) Electrons are indistinguishable : ) 1 ( ) 2 ( ) 2 ( ) 1 ( B A B A + = c ) Include ionic bonds ( λ = weight): )] 1 ( ) 2 ( ) 2 ( ) 1 ( [ ) 1 ( ) 2 ( ) 2 ( ) 1 ( B A B A B A B A ψψ λ + + + = What is the bond energy?
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This note was uploaded on 05/29/2011 for the course CHM 3400 taught by Professor Seabra during the Spring '08 term at University of Florida.

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110325 - The chemical bond (Chapter 12 447-458) Lewis...

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