VII Structure and Bonding B

# VII Structure and Bonding B - Structure and Bonding...

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Structure and Bonding Continued

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Using Lewis Structures Determining Formal Charge and Oxidation Number Formal Charge(FC) Charge an atom would have if the electrons in a bond were shared equally between the two atoms FC = # valence e on atom - (# of lone pair e) - (# bonding e associated with the atom) I.e. 1 electron from each bond to each atom in the bond Oxidation Number(ON) Charge an atom would have if the electrons in a bond belong solely to the more electronegative atom ON = # valence e on atom - (# of lone pair e) - (# bonding e associated with the atom) I.e both electrons in the bond go to the more electronegative atom
Determine the formal charge and oxidation number of all atoms In CO 3 - 2 . CO 3 - 2 (24) C O O O

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Determine the formal charge and oxidation number of all atoms In CO 3 - 2 . CO 3 - 2 (24) C O O O -2
Determine the formal charge and oxidation number of all atoms In CO 3 - 2 . CO 3 - 2 (24) C O C O A O B -2 Formal Charge C: 4 - 0 - 4 = 0 O A : 6 - 6 - 1 = - 1 O C : 6 - 6 - 1 = - 1 O B : 6 - 4 - 2 = 0 -2

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Determine the formal charge and oxidation number of all atoms In CO 3 - 2 . CO 3 - 2 (24) C O C O A O B -2 Formal Charge C: 4 - 0 - 4 = 0 O A : 6 - 6 - 1 = - 1 O C : 6 - 6 - 1 = - 1 O B : 6 - 4 - 2 = 0 -2 Oxidation Number C: 4 - 0 - 0 = + 4 O A : 6 - 6 - 2 = - 2 O C : 6 - 6 - 2 = - 2 O B : 6 - 4 - 4 = - 2 -2
Using Formal Charge to determine the “best” Resonance Form Magnitude of the formal charge to be as small as possible Negative charge on the more electronegative atom

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N 2 O (16) N N O N N O N N O N N O I II III
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