Lecture 03_Ch14b - • A σ bond can be formed a number of...

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Unformatted text preview: • A σ bond can be formed a number of ways: – s, s overlap – s, p overlap – p, p overlap Forming Bonds Only orbitals of the same phase (+, +) can form bonds • For every bonding orbital we form, we also form an anti-bonding orbital: Anti-bonding Orbitals MO Theory in Bonding • Homonuclear atoms (H2, O2, F2, N2) H2 (Only 1s orbitals available for bonding) • AOs must overlap in space in order to participate in MOs • Covalent bonding is dominated by the valence orbitals (only valence orbitals are shown in the MOs) Covalent Bonding in Homonuclear Diatomics Covalent Bonding in Homonuclear Diatomics Region of shared e- density + + – Valence configurations of the 2nd row atoms: Li Be B C N O F 2s1 2s2 2s22p1 2s22p2 2s22p3 2s22p4 2s22p5 So far we have focused on bonding involving the s orbitals. What happens when we have to consider the p orbitals? For diatom ic m olecules containing atom s with valence electrons in the p orbitals, we m ust consider three possible bonding interactions: σ- type π- type π- type = nucleus Fig (+ ) constructive m ixing (–) destructive m ixing Fig 14.36 Major limitations of the LE model: 2) Doesn’t easily deal with unpaired electrons (incorrectly predicts physical properties in some cases) Example: O2- Lewis dot structure O=O- All electrons are paired Contradicts experiment! .. .. .. .. Experiments show O2 is paramagnetic A quick note on magnetism… Paramagnetic The molecule contains unpaired electrons and is attracted to (has a positive susceptibility to) an applied magnetic field Diamagnetic The molecule contains only paired electrons and is not attracted to (has a negative susceptibility to) an applied magnetic field N2 Video O2 Video ____...
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This note was uploaded on 04/11/2011 for the course CHEM 162 taught by Professor N. during the Spring '08 term at University of Washington.

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Lecture 03_Ch14b - • A σ bond can be formed a number of...

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