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Q5. For each of the molecules below, redraw the expanded Lewis structures, Indicate which hybrid orbish label the Ï and Ï bonds. nb ltad on each central atom. Indicate which orbitals are overlapping in each bond. For each molecule, OH H3C-C-CH CI-C -CH Cl 06. H-C-H a) On the diagram, label the hybridization state of each atom. b) Although the lone pair electrons of the double-bonded oxygen atom (labeled with an 'x') could be located in an unhybridized p-orbital, why would these electrons tend to be in hybridized orbitals? ChemlA-Work Session 7: Valence Bond Theory and Molecular Orbital Theory
Q5. For each of the molecules below, redraw the expanded Lewis structures, Indicate which hybrid orbish label the Ï and Ï bonds. nb ltad on each central atom. Indicate which orbitals are overlapping in each bond. For each molecule, OH H3C-C-CH CI-C -CH Cl 06. H-C-H a) On the diagram, label the hybridization state of each atom. b) Although the lone pair electrons of the double-bonded oxygen atom (labeled with an 'x') could be located in an unhybridized p-orbital, why would these electrons tend to be in hybridized orbitals? ChemlA-Work Session 7: Valence Bond Theory and Molecular Orbital Theory
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Tod ThielLv2
2 Feb 2019
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