1004 - Section 5.8 Formal Charge vs Oxidation State...

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Unformatted text preview: Section 5.8 Formal Charge vs Oxidation State Consider NH 3 (ammonia): ER = (1 × 8) + (3 × 2) = 14 VE = 5 + (3 × 1) = 8 SP = 1/2(14 - 8) = 3 H N H H Formal Charge (for covalent bonds) Oxidation State (for ionic bonds) H N H H H N H H Assign all nonbonding and half of the bonding e ’s Assign all nonbonding Ox N = 5 - 8 = - 3 FC N = Old way: N+3(+1)=0 N = -3 F F C F F Oxidation State- Ionic limit F F C F F Formal Charge- Covalent limit Section 5.8 Formal Charge vs Oxidation State You can calculate ox state and formal charge for any bonded atom. Ex. CF (carbon tetrafluoride): Old way: C + 4(-1) = 0 C = +4 These are the “ limits ” of all ionic or all covalent. (Really somewhere in between!) OS F = - 1 F is more electronegative so it gets the bonded electrons N O Cl O N Cl Ex. NOCl (nitrosyl chloride): ER = 3 × 8 = 24 VE = 5 + 6 + 7 = 18 SP = 1 / 2 (24 - 18) = 3 +1-1 +1-1 N O Cl O N Cl +1-2 +1 Formal charges = 0 in a neutral molecule. THE BEST! Section 5.9 A Challenging Lewis Structure Not equal resonance structures!...
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This note was uploaded on 06/14/2009 for the course CH 101 taught by Professor Bigham during the Spring '08 term at N.C. State.

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1004 - Section 5.8 Formal Charge vs Oxidation State...

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