a - to accommodate all of the substituents. 5. Compounds of...

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1. a. The formal charges of all atoms must sum to 0 in molecules. b. The formal charges must sum to the ion’s charge for a polyatomic ion. Formal Charge Cl 7 – (2+4) = +1 N 5 – (3+2) = 0 O 6 – (1+6) = -1 Cl 7 – (1+6) = 0 N 5 – (3+2) = 0 O 6 – (2+4) = 0 Writing Lewis Formulas: Limitations of the Octet Rule There are some molecules that violate the octet rule. For these molecules the N - A = S rule does not apply: 1. The covalent compounds of Be. 2. The covalent compounds of the IIIA Group. 3. Species which contain an odd number of electrons. 4. Species in which the central element must have a share of more than 8 valence electrons
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Unformatted text preview: to accommodate all of the substituents. 5. Compounds of the d- and f-transition metals. Writing Lewis Formulas: Limitations of the Octet Rule In those cases where the octet rule does not apply, the substituents attached to the central atom nearly always attain noble gas configurations. The central atom does not have a noble gas configuration but may have fewer than 8 (exceptions 1, 2, & 3) or more than 8 (exceptions 4 & 5)....
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This note was uploaded on 11/25/2011 for the course CHEM 1211 taught by Professor Atwood during the Fall '07 term at UGA.

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