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Welcome to Chem 109 A

Welcome to Chem 109 A. Chapter 1 E-mail: benzene4president@gmail.com Web-site: http://clas.sa.ucsb.edu/staff/terri/. Ch. 1. 1. Label the polarities of the bonds for the following molecules. A. Methanol – CH 3 OH B. Urea – CO(NH 2 ) 2. Ch. 1.

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Welcome to Chem 109 A

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  1. Welcome to Chem 109 A Chapter 1 E-mail: benzene4president@gmail.com Web-site: http://clas.sa.ucsb.edu/staff/terri/

  2. Ch. 1 • 1. Label the polarities of the bonds for the following molecules. • A. Methanol – CH3OH • B. Urea – CO(NH2)2

  3. Ch. 1 • 2. Draw the Kekule, condensed and line structure for the following compounds. • A. 3-ethyl-2,4,4-trimethylhexane • B. 3-methyl-2-butanamine • C. 6-chloro-4-isopropyl-2,2-dimethyl-3-heptanol

  4. Ch. 1 • 3. Draw the following orbital before and after overlap. Label the nodes if any. • A. σ1s • B. σ1s* • C. σ2p • D. σ2p* • E. π2p • F. π2p*

  5. Ch. 1 4. For each of the following; draw the Lewis structure, assign formal charges, determine the hybridization of the central atom/s, determine the bond angles, describe the bonds (sigma vs pi and which orbitals are involved), and draw a 3D orbital structure a. C2H6 b. HCONH2 c. C2H2 d. CH2N2

  6. Ch. 1 • 5. Predict the relative lengths and strengths of the bonds in the following: • A. Chloromethane, bromoethane and iodoethane • B. Ethane, ethene and ethyne.

  7. Ch. 1 • 6. Describe the fundamental differences between a methyl cation, methyl anion and methyl radical.

  8. Ch. 1 7. In terms of dipole moments explain why BF3 has a molecular dipole moment of zero.

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