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Lecture-14 - Chem111 Fall 2005 Lecture 14 Bonding and...

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Chem111 Fall, 2005 51 Lewis Dot Structures accounting of all of the valence electrons – where do they go? 1916, Gilbert Lewis bond involves a pair of electrons ± "shared" by the atoms ± why 2? why not 1 or 3 or 7? Lewis derives a simple method for predicting bonding in molecules Octet Rule : atoms want to have/share 8 electrons in their valence (outer) shells ± accounts for a wide range of stable molecules ± lots of exceptions ± manifestation of the stability of the inert/noble gas e- configuration ± F ± F- and Ca ± Ca 2+ because of this! Examples. Let's get back to CO 2 and H 2 O … why does CO 2 have double bonds but H 2 O only has single bonds? H 2 O each H contributes 1 valence e- = 2 e- the O contributes 6 valence e- = 6 e- Total valence e- = 8 e- first, draw the molecule in its bonding arrangement H O H then put in the bonding electrons – 2 per bond – leaves 8-4=4 e- to distribute H O H then put in the remaining 4 electrons … H O H Lecture 14: Bonding and Molecules Lewis Dot Structures VSEPR (I&II) ** see the Lewis Dot Structure Handout! ** two O-H single bonds
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