CHEM 251 1st Edition Lecture 7 Outline of Last Lecture I. Clicker QuestionsII. Covalent BondingIII. Lewis Dot StructuresIV. Molecular OrbitalsOutline of Current Lecture V. Clicker QuestionVI. Heteronuclear MO DiagramsVII. MixingVIII. VSEPR Theory Current LectureIX. Clicker Questiona. Productive overlapX. Heteronuclear MO Diagramsb. Ex: COi. S-orbitalsThese 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.1.2. higher electronegativity => lower energyii. p-orbitals1.iii. filling in the MO diagram1.XI. Mixingc. In CO, occurs because C 2s close in energy to O 2pd.e.f. Why does CO bind through carbon?i. C-based lone pair is highest in energyii. Polarization1. O is more electronegative, so the bonding MO is polarized toward O2. Anti-bonding MO have opposite polarization (polarized toward C)g. Things to consider:i. How much of a difference does electronegativity make?ii. How far up/down in energy are bonding pairs placed?iii. Do sigma bonds and pi bonds have the same energy changes?h. NOTE: mixing is NOT the same as hybridizationXII. VSEPR Theoryi. Predicts molecular shape of polyatomic moleculesj. Key: lone pairs affect molecular geometryk. How do we guess the right bent angle?i. Lone pairs are big so surrounding angles are slightly smaller1. Repel neighboring groups2. Remember VSEPR
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