Recitation Chapter 1 - Practice Questions PDF

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Recitation Chapter 1 1. Assign formal charges to each carbon atom in the molecule shown to the right. All lone pairs have been drawn in. A) a: 0, b: 0 B) a: 0, b: +1 C) a: 0, b: -1 D) a: +1, b: -1 E) a: -1, b: +1 2. Assign formal charges to each N atom in the molecule shown to the right. All lone pairs have been drawn in. A) a: 0, b: 0, c: 0 B) a: 0, b: +1, c: 0 C) a: 0, b: +1, c: +1 D) a: 0, b: +1, c: -1 E) a: 0, b: -1, c: +1 3. Draw all reasonable resonance structures for the species shown on the right. A) B) C) D)

4. Draw all reasonable resonance structures for the species shown on the right. A

B

C

D

5. For the compound shown to the right, label each bond as ionic or covalent. A) a: ionic, b: ionic, c: covalent B) a: ionic, b: covalent, c: covalent C) a: ionic, b: covalent, c: ionic D) a: covalent, b: covalent, c: ionic E) a: covalent, b: ionic, c: covalent

6. How are the molecules or ions in each pair related? Classify them as resonance structures (abbreviated as "reson.", isomers, or neither. A) a,b: isomers c,d: neither B) a,b: isomers c,d: reson. C) a,b: res. struc. c: isomers d: neither D) a,b: isomers c: neither d: reson. E) a,b: isomers c: reson. d: neither

7. How many covalent bonds are predicted for each atom? a. N

b. Cl

c. Al

d. Si

e. H

8. Label each bond in the following compounds as ionic or covalent. a. LiBr

b. HBr

c. I 2

d. CH3OH

f. BrCl

g. H2O

h. NaNO3

e. CH 3ONa

i. CH3NH2

9. Assign the formal charge on each second row atom: a

NH4NO3

b

CH3-NC

c

CH3-CN

d

NaNH2

10. Draw a Lewis structure for each ion or molecule. a. CH3Oe. CH3NO2

b. HC2f. N2

c. (CH 3NH)-

d. -CH2CN

g. H6BN

h. BF4-

11. Convert each condensed formula to a Lewis structure. a. CH3(CH2)4CH(CH3)2 b. (CH3)2CHCH(CH2CH3)2 c. (CH3)3CCH(OH)CH2CH3 d. (CH3)2CHCOOH e. (CH3CH2)2CHCH2CO2CH3 f.

CH3CH2NHCH2CHO

12. Draw a second resonance structure for each structure below.

Chapter 1 (continued) 13. Label the resonance structures in each pair as major, minor or equal contributors to the hybrid. Then draw the hybrid.

14. Draw a valid resonance structure through the curved arrows if there is. If there is no valid resonance structure, explain why.

15. Predict all bond angles in each compound and the geometry around the second-row atoms. a. CH3Cl e. CH3COOH

b. NH2OH

c. CH3CH2CH3

d. (CH3)3N

f. BF4-

16. Predict the hybridization and geometry around each indicated atom.

b. (CH3)3O+ 17. Indicate the polarity of the labeled bonds using δ + or δ- . Br—Cl

NH2—OH

CH3—NH2

18. Use the observed bond lengths to answer each question: a, why is bond [1] longer than bond [2] b, why are bonds [3] and [4] equal in length, and shorter than bond [2]?

[3] 127 pm

d, 18. Questions about nicotine: a, what is the hybridization of each N atom in nicotine? b, what is the geometry around each N atom? c, in what type of orbital does the lone pair on each N atom reside? d, draw a constitutional isomer of nicotine. e, draw a resonance structure of nicotine....