CHEM 101 Lecture 6: Lecture Notes Week 6
2 Nov 2016
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Document Summary
H, he and b are the only elements that don"t need to fulfill the octet rule (they don"t need to reach 8, but there are elements that can have more than 8 valence electrons because of d orbitals) Predicts the lewis structure of molecules (valence e)-(all e in lone pairs)- (shared e)= formal charge. The more viable option is the first arrangement of co2, as the formal charge is lower than the second arrangement, even though both fulfill the octet rule. Formal charge has greater importance than the octet rule. Ions or molecules with an odd number of valence electrons. Ions or molecules with less than an octet (h, he, b) Ions or molecules with more than 8 valence electrons (d orbitals) These are normall ions or molecules involving the 3rd period or larger. If fulfilling the octet of a central atom results in an unfavorable formal charge, Unequal sharing of electrons results in a bond dipole.
