Copyright © 2008 Pearson Prentice Hall, Inc. Chapter 23/1 The Nature of Organic Molecules • Carbon is tetravalent. It has four outer-shell electrons a...
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The Nature of Organic Molecules Organic Chemistry: The study of carbon compounds. •
Carbon is tetravalent. It has four outer-shell electrons and forms four bonds.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/1
The Nature of Organic Molecules •
Organic molecules have covalent bonds. In ethane, for instance, all bonds result from the sharing of two electrons.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/2
The Nature of Organic Molecules •
Organic molecules have polar covalent bonds when carbon bonds to an element on the right or left side of the periodic table.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/3
The Nature of Organic Molecules •
Carbon can form multiple covalent bonds by sharing more than two electrons with a neighboring atom.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/4
The Nature of Organic Molecules •
Organic molecules have specific three-dimensional shapes, which can be predicted by the VSEPR model.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/5
The Nature of Organic Molecules •
Organic molecules have specific three-dimensional shapes, which can be predicted by the VSEPR model.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/6
Alkanes and Their Isomers Hydrocarbons: Molecules that contain only carbon and hydrogen. Alkanes: Hydrocarbons that contain only single bonds. Space-filling models:
Structural formulas: Molecular formulas: Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/7
Alkanes and Their Isomers Isomers: Compounds with the same molecular formula but different chemical structures.
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/9
Drawing Organic Structures Structural Formula
Condensed Formula
Copyright © 2008 Pearson Prentice Hall, Inc.
Chapter 23/10
The Shapes of Organic Molecules
Determining Polarity of Molecules Step 1: Does the molecule have polar bonds? If no, the molecule is not polar. If yes, go to step 2. Step 2: Is there more than one polar bond? If no, the molecule is polar. If yes, go to step 3. Step 3: Do the bond dipoles cancel each other out? If no, the molecule is polar. If yes the molecule is not polar.
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Note: C—I, C—Br, C—Cl, C—F, C—O, O—H, N—H, and C—N are all common polar bonds.
