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Welcome to Chem 109 A. Chapter 1 E-mail: [email protected] 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

Welcome to Chem 109 A

Chapter 1

E-mail: [email protected]

Web-site: http://clas.sa.ucsb.edu/staff/terri/


Ch. 1

  • 1. Label the polarities of the bonds for the following molecules.

    • A. Methanol – CH3OH

    • B. Urea – CO(NH2)2


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


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*


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


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.


Ch. 1

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


Ch. 1

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


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