Title | 220 rev chp 01 - chem |
---|---|
Author | Kate Smith |
Course | Organic Chemistry |
Institution | Orange Coast College |
Pages | 3 |
File Size | 101 KB |
File Type | |
Total Downloads | 82 |
Total Views | 151 |
chem...
Chem 220
Orange Coast College
Review Chapter 01 1. Draw Lewis structures of the compounds with the following molecular formulas: a) C3H4
b) HNO2
c) HCO2H
2. For each compound, state whether its bonding is ionic, covalent, or a mixture of ionic and covalent, then draw a Lewis structure to show the bonding in the compound: b) NaOCH3
a) CH2Cl2
c) HCO2Na
3. Complete the following Lewis structures by filling in lone pairs and calculating formal charges: a)
b) H H
C
+
O N
H
O
O
H
H
H
4. Each of the following compounds has a Lewis structure that violates the octet rule. Draw the octet rule violating Lewis structure, and briefly explain how and why it violates the octet rule: c) H3PO4
d) SOCl2
e) B(CH3)3
5. Redraw each of the following fully condensed structures as partially condensed structures and as line structures: a) CH3CH2CHClCH2CH3
b) CH3C(O)CH3
c) CH3C(CH3)2CH2CH3
© John Congleton
Chem 220
Review Problem Set 01
Page 2
6. Redraw each of the following Lewis structures as partially condensed structures and as line structures:
H
H
H
H
C H
C
C H
O
d) H
c) H
H
H
C
C
C
C
H
H
H
H
H
H
H
H
H
Cl
C
C
C
HH
H
H H
C
C
O
H
H
H
7. Each of the following compounds or ions has resonance. Draw two resonance structures of each of the compounds: a) NO2–
b) [CH2=CH–CH2]–
8. For each of the following structures, push electrons to create the indicated number of resonance structures. Label each structure as a major or minor contributor: a) (ONE additional GOOD structures) O CH3
C
CH2
Chem 220
Review Problem Set 01
b) (TWO additional structures) NH NH2
C
NH2
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