chem1b-w09-lecture_12 - Lewis structures for Molecules A-...

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1 Lewis structures for Molecules A- SINGLE BONDS ONLY B- MULTIPLE BONDS IN COVALENT BONDING: ELECTRONS ARE SHARED TO COMPLETE AN OCTET FOR EACH ATOM IN THE MOLECULE ( A DUET FOR HYDROGEN) Example in Lewis notation: : Cl . Cl : Cl – Cl 7 electrons 7 electrons A bond (-) is a shared electron pair each atom “feels” it has 8 electrons . . . . . . . . .
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2 Examples: Cl – Cl O = O Each bond (-) is a shared electron pair Fig. 9.16 Prob. 10.1 These electron pairs not engaged in bonding are called “lone pairs”
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3 The Bond Order : BO Number of shared electron pairs Number of 2-atom linkages = BO Cl Cl BO = 1/1 = 1 H - N N-H BO = 3/1 = 3 For the Cl-Cl bond For the N-N bond Prob. 10.2a next
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Prob. 10.3 RESONANCE The bonding and the lone electron pairs can be placed in different locations without changing the position of the atoms in the molecule Prob. 10.4 Which resonance structures are the most probable? Those that result in the lowest
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This note was uploaded on 10/24/2009 for the course CHEMISTRY CHEM taught by Professor Eastman during the Winter '07 term at East Central College.

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chem1b-w09-lecture_12 - Lewis structures for Molecules A-...

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