Final Review Sheet - Chapter 9 Chemical Bonding I Lewis...

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Chapter 9: Chemical Bonding I: Lewis Theory 1) Bond Relationships -the shorter the bond, the stronger the bond -relative strength: single bond < double bond < triple bond -increased electron density in bonding internuclear region -single bond rotation allowed, double bond no rotation 2) Polar Covalent, Nonpolar Covalent, and Ionic Bonds electronegativity difference bond type example small (0 - 0.4) covalent Cl 2 intermediate (0.4 - 2.0) polar covalent HCl large (2.0+) ionic NaCl -electronegativity trends -electron density models -red (negative), blue (positive) - 3) Lewis Structures -drawing structures 1) sum all valence electrons 2) write atom symbols to show connectivity 3) draw a single bond between each atom pair bonded together 4) complete octets 5) place leftover electrons on central atom 6) not enough electrons to give to central atom an octet, try multiple bonds -octet exceptions -less than octet: B, Be, H -more than octet: P, S, I, As (3 rd period or below) -resonance structures (example: CO 3 2- )
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