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Week 8 Practice Problems

Week 8 Practice Problems - For each Lewis structure...

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CHEMISTRY 201X October 8-12, 2007 Practice Problems (62) The molecular orbital energy diagram for O 2 and F 2 (the one with no 2 s -2 p hybridization) is also appropriate to describe the molecular orbital energies for heteroatomic molecules like CO and NO. (a) Use this diagram, and draw the molecular orbitals for the CO molecule. (b) Use the diagram to predict the bond orders and numbers of unpaired electrons for BN, CN , NO + , NO, NO , BF, and BO. (63) Construct a molecular orbital energy diagram for the HF molecule. You may ignore the valence 2 s AO of fluorine, as it is very low in energy, and not heavily involved in chemical bonding. (64) For each of the following molecules or molecular ions, draw the Lewis structures, taking into account resonance.
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Unformatted text preview: For each Lewis structure, calculate the formal charge at each atomic site, and construct a qualitative molecular orbital diagram (labeling bonding, antibonding and nonbonding = lone pair orbitals). For each example, which orbital is the HOMO and which orbital is the LUMO? (a) O 3 (ozone) (b) CO 2 (carbon dioxide) (c) H 2 N-CH 2-COOH (glycine: an amino acid) (d) CH 3 NO 2 (nitromethane) (e) CH 3 CN (acetonitrile) (f) HN 3 (hydrazoic acid) (65) Draw Lewis structures for two possible forms of hydrogen cyanide (HCN): (a) for H bonded to the C atom; and (b) for H bonded to the N atom. Which isomer makes more sense? Now use a qualitative molecular orbital diagram to explain your choice....
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