《有机化学》课程PPT教学课件（Official PPT of Organic Chemistry, 7th Edition, L. G. Wade, Jr.Pearson Education）Chapter 07 Structure and Synthesis of Alkenes

Organic Chemistry,7th Edition L.G.Wade,Jr. Chapter 7 Structure and Synthesis of Alkenes Copyright 2010 Pearson Education,Inc

Chapter 7 Copyright © 2010 Pearson Education, Inc. Organic Chemistry, 7th Edition L. G. Wade, Jr. Structure and Synthesis of Alkenes

Introduction Alkenes are hydrocarbon with carbon-carbon double bonds. Alkenes are also called olefins,meaning "oil- forming gas”. The functional group of alkenes is the carbon- carbon double bond,which is reactive. Chapter 7 2

Chapter 7 2 Introduction • Alkenes are hydrocarbon with carbon-carbon double bonds. • Alkenes are also called olefins, meaning “oil￾forming gas”. • The functional group of alkenes is the carbon￾carbon double bond, which is reactive

Sigma Bonds of Ethylene 2 p sp H H sigma bonding orbitals of ethylene Copyright2010 Pearson Prentice Hall,Inc. Chapter 7 3

Chapter 7 3 Sigma Bonds of Ethylene

Orbital Description ● Sigma bonds around the double-bonded carbon are sp2 hybridized. ·Angles are approximately12o°and the molecular geometry is trigonal planar. Unhybridized p orbitals with one electron will overlap forming the double bond (pi bond). Chapter 7 4

Chapter 7 4 Orbital Description • Sigma bonds around the double-bonded carbon are sp2 hybridized. • Angles are approximately 120ºand the molecular geometry is trigonal planar. • Unhybridized p orbitals with one electron will overlap forming the double bond (pi bond)

Bond Lengths and Angles 116.6° 121.7° H ethylene ethane Copyright2010 Pearson Prentice Hall,Inc. sp2 hybrid orbitals have more s character than the sp3 hybrid orbitals. Pi overlap brings carbon atoms closer shortening the C-C bond from 1.54 A in alkanes down to 1.33 A in alkenes. Chapter 7 5

Chapter 7 5 Bond Lengths and Angles • sp2 hybrid orbitals have more s character than the sp3 hybrid orbitals. • Pi overlap brings carbon atoms closer shortening the C—C bond from 1.54 Å in alkanes down to 1.33 Å in alkenes

Pi Bonding in Ethylene electrostatic potential map Copyright 2010 Pearson Prentice Hall,Inc. The pi bond in ethylene is formed by overlap of the unhybridized p orbitals of the sp2 hybrid carbon atoms. Each carbon has one unpaired electron in the p orbital. This overlap requires the two ends of the molecule to be coplanar. Chapter 7 6

Chapter 7 6 Pi Bonding in Ethylene • The pi bond in ethylene is formed by overlap of the unhybridized p orbitals of the sp2 hybrid carbon atoms. • Each carbon has one unpaired electron in the p orbital. • This overlap requires the two ends of the molecule to be coplanar

Cis-Trans Interconversion CH3 CH CH3 cis no overlap with the ends perpendicular trans Copyright2010 Pearson Prentice Hall,Inc. Cis and trans isomers cannot be interconverted. No rotation around the carbon-carbon bond is possible without breaking the pi bond(264 kJ/mole). Chapter 7 7

Chapter 7 7 Cis-Trans Interconversion • Cis and trans isomers cannot be interconverted. • No rotation around the carbon—carbon bond is possible without breaking the pi bond (264 kJ/mole)

Elements of Unsaturation Unsaturation:A structural element that decreases the number of hydrogens in the molecule by two. Double bonds and rings are elements of unsaturation. To calculate:Find number of hydrogens if they were saturated,subtract the actual number of hydrogens,then divide by 2. Chapter 7 8

Chapter 7 8 Elements of Unsaturation • Unsaturation: A structural element that decreases the number of hydrogens in the molecule by two. • Double bonds and rings are elements of unsaturation. • To calculate: Find number of hydrogens if they were saturated, subtract the actual number of hydrogens, then divide by 2

Example:Calculate the Unsaturations for a Compound with Formula C5Ha. First calculate the number of hydrogen atoms for a saturated compound with five carbons: (2×C)+2 (2X5)+2=12 Now subtract from this number the actual number of hydrogen atoms in the formula and divide by 2: 12-8=4=2 unsaturations 22 The compound has two unsaturations,they can be two double bonds,two rings,or one double bond and one ring. Chapter 7 9

Chapter 7 9 Example: Calculate the Unsaturations for a Compound with Formula C5H8 . • First calculate the number of hydrogen atoms for a saturated compound with five carbons: (2 x C) + 2 (2 x 5) + 2 = 12 • Now subtract from this number the actual number of hydrogen atoms in the formula and divide by 2: 12 – 8 = 4 = 2 unsaturations 2 2 • The compound has two unsaturations, they can be two double bonds, two rings, or one double bond and one ring

Elements of Unsaturation: Heteroatoms Halogens replace hydrogen atoms in hydrocarbons,so when calculating unsaturations,count halides as hydrogen atoms. Oxygen does not change the C:H ratio,so ignore oxygen in the formula. Nitrogen is trivalent,so it acts like half a carbon.Add the number of nitrogen atoms when calculating unsaturations. Chapter 7 10

Chapter 7 10 Elements of Unsaturation: Heteroatoms • Halogens replace hydrogen atoms in hydrocarbons, so when calculating unsaturations, count halides as hydrogen atoms. • Oxygen does not change the C:H ratio, so ignore oxygen in the formula. • Nitrogen is trivalent, so it acts like half a carbon. Add the number of nitrogen atoms when calculating unsaturations