Notes 100809 - Sigma orbital (1 st )(lower case) Bond...

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Lewis Dot Structures Strengths -relatively simple -mostly effective at predicting bonding arrangement, bond order, molecular geometry Weakness -does not allow accurately predicted properties -need a substantial list of exceptions -conceptual band aids like resonance structures -no information about energy levels Forming Moledular Orbitals from Atomic Orbitals Two wave functions: 1s(a) + 1s (b) → bonding (MO1) [Constructively interfere] 1s(a) – 1s(b) → antibonding (MO2) [Deconstructively interfere] Rules for Electron Configurations Pauli exclusion principle- no two electrons on the same set of 4 quantum #s Aufbau principle- fill the lowest energy orbitals 1 st then move to the next lowest energy Hund Principle Molecular Orbitals for H2, H2 -, He2
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Unformatted text preview: Sigma orbital (1 st )(lower case) Bond Order-the number of bonds between the 2 atoms is half the difference b/w the # of electrons in bonding orbitals and the # of electrons in anti-bonding orbitals-B.O. (# of bonds) = (#bonding e - # anti-bonding) / 2-Higher bond order = shorter, stronger bonds Paramagnetism-Paramagnetism- a type of induced magnetism, associated with unpaired electrons, that causes a substance to be attracted into the inducing magnetic field-Dimagnetism- a type of magnetism, associated with paired electrons, that causes a substance to be repelled from the inducing magnetic field Known 2 Diagram Schemes*** (in HF, why theres more EN cuz its not diatomic) B2, C2, N2, O2, F2, Ne2...
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This note was uploaded on 11/18/2010 for the course CH 301 taught by Professor Fakhreddine/lyon during the Spring '07 term at University of Texas at Austin.

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