Assignment_1_Review - a Show the direction of the dipole...

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CHM 2120 – Assignment #1 In this assignment: - Lewis structures, formal charge - Electronegativity, dipoles - Resonance - Acid/base 1. Draw the following molecules as full Lewis structures. Many molecules below possess a charge that is not shown—calculate the formal charge on each atom and indicate the location of the charge where applicable. Hint: each atom has a full octet, so start by adding electrons to each atom to complete its octet. The only atoms we will encounter in this course that lack an octet are carbon (a carbocation lacks an octet) and metals (B, Al, Mg, Li, etc).
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Assignment 1 - Review 2 2. Circle the plausible structures and put an “X” through the impossible structures below: Note: lone pairs should be added as required in order to satisfy the formal charge shown. 3. For the following bonds,
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Unformatted text preview: a. Show the direction of the dipole moment using two methods. b. Is the bond ionic or polar covalent? Example: C-H i. C-B ii. Li-C iii. Mg-C iv. Li-O v. C-Br vi. C-N vii. N-Br viii. O-Cl ix. O-H x. S-H xi. N-H Assignment 1 - Review 3 4. For the following molecules: a. Draw the important resonance forms using arrows to show the movement of electrons b. Rank the structures in order of importance of contribution to the resonance hybrid. c. Show the resonance hybrid structures 5. Draw the direction of the dipole in the indicated bonds in each of the following molecules. a) b) c) d) e) f) 6. Write equations for the following reactions using arrow notation. Predict whether the reaction will favor the starting materials or products and justify your choice. Assignment 1 - Review 4...
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Assignment_1_Review - a Show the direction of the dipole...

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