CHEM 101 Midterm: EXAM III Review
4 Nov 2016
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6. 3: writing lewis structures for molecular compounds and polyatomic. 6. 5: exceptions to the octet rule: odd-electron species, incomplete. 6. 7: vsepr theory: the five basic shapes. 6. 8: vsepr theory: the effect of lone pairs. Chapter 8: chemical reactions and chemical qualities. 8. 5: limiting reactant, theoretical yield, and percent yield. Indicates how the valence electrons are distributed in a molecule. An atom is most stable when its outermost shell of electrons is empty/full. Resonance: where the correct lewis structure cannot be accurately represented by a single lewis structure. These structures switch and change between each other almost instantaneously (why we have to show the resonance structures) Formal charge (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.
