Oxygen vs. OzoneAllotropesDifferent molecular forms of the same elementCarbon: graphite/ diamond/”buckyballs”Oxygen: O2/O3Formation of ozoneResonance Structures: OzoneResonance: when two or more equivalent Lewis structures can be drawn for one compoundResonance Structures: two or more Lewis structures with the same arrangement of atoms but different arrangement of bonding pairs of electronsFormal Charge (FC): determined by the difference between the number of valence e- in the free atom and the sum of lone pair+ ½ bonding e- in a moleculeFC = (# valence electrons)-- [(# unshared e-) + ½ (# of e- in bonding pairs)]Choosing the Best StructureMost stable resonance structures:Formal charges equal or close to zeroNegative formal charges on the more electronegative elementCHEM 111 1nd Edition Lecture 16 Outline of Last Lecture I. ElectronegativityII. Polar Covalent BondsIII. Bond PolarityIV. Electronegativity DifferencesOutline of Current Lecture II. Oxygen vs. OzoneIII. Resonance Structures Current Lecture Oxygen vs. Ozone- Allotropes o Different molecular forms of the same elemento Carbon: graphite/ diamond/”buckyballs”o Oxygen: O2/O3- Formation of ozone Resonance Structures: Ozone Resonance: when two or more equivalent Lewis structures can be drawn for one compound Resonance Structures: two or more Lewis structures with the same arrangement of atoms but different arrangement of bonding pairs of electrons Formal Charge (FC): determined by the difference between the number of valence e- in the free atom and the sum of lone pair+ ½ bonding e- in a molecule FC = (# valence electrons)-- [(# unshared e-) + ½ (# of e- in bonding pairs)]These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute. Choosing the Best StructureMost stable resonance structures:Formal charges equal or close to zeroNegative formal charges on the more electronegative
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