By Luigi E. Picasso
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ChemActivity 3: Electron Orbitals Consider the incomplete orbital representation of O2, below right. a. Identify which lobes are hybrid orbitals (identify the type) and which lobes are p orbitals. b. Use dotted lines to show any π bonds. c. Use up or down arrows to show electron occupation of each hybrid orbital or bond. A double bond consists of one σ overlap and one π overlap. σ bond (or vice versa) O O π bond (or vice versa) Orbital Drawing of O2 Lewis Drawing of O2 5. Consider the following orbital representation of HCCH (ethyne).
15. Construct an explanation for why an H attached to an N or O atom can participate in a hydrogen bond (H-bond) while an H attached to a carbon atom cannot. 16. Circle each molecule below that you expect to be capable of hydrogen bonding to itself. O O R NH2 C N H HO C H2 H2 C CH3 C C H2 HO OH HOCH3 C H2 O H2 C H3C Cl C H2 H Cl H2 C H3C H2 C O CH3 C CH3 H C H2 17. An “hydrogen-bond donor” has an H suitable for hydrogen bonding. An “hydrogen-bond acceptor” has a lone pair suitable for hydrogen bonding.
B. C atom? N atom? O atom? Consider the molecules AlCl3 (aluminum chloride) and CF4 (carbon tetrafluoride). a. Draw the valence shell representation of each. b. Predict the value of the XYX bond angle, and explain your reasoning. 5 o; then draw a different bent molecule with a bond angle of about 120 o. 14 7. 5o or 90o. (circled charges indicate the charge on the molecule or fragment) H H C H H F H O H H N H H O O H H N H H 8. Make a model of each of the following molecules: Cl H O H Cl N Cl H H C H H C C C H H H C H C H C H H H H 9.