《有机化学》课程PPT教学课件（Official PPT of Organic Chemistry 6th LG Wade by Prentice Hall，L. G. Wade, Jr.）Chapter 01 Introduction and Review

Organic Chemistry,6th Edition L.G.Wade,Jr. Chapter 1 Introduction and Review Jo Blackburn Richland College,Dallas,TX Dallas County Community College District ©2006，Prentice Hall

Chapter 1 Introduction and Review Organic Chemistry, 6th Edition L. G. Wade, Jr. Jo Blackburn Richland College, Dallas, TX Dallas County Community College District © 2006, Prentice Hall

Definitions ·Old:“derived from living organisms” ·New:“chemistry of carbon compounds” From inorganic to organic,Wohler,1828 NH OCN heat、 urea 三> Chapter 1

Chapter 1 2 Definitions • Old: “derived from living organisms” • New: “chemistry of carbon compounds” • From inorganic to organic, Wöhler, 1828 heat NH4 + OCN - H2 N C NH2 O urea =>

Atomic Structure Atoms:protons,neutrons,and electrons. The number of protons determines the identity of the element. Some atoms of the same element have a different number of neutrons.These are called isotopes. Example:12C,13C,and 14C. => Chapter 1 3

Chapter 1 3 Atomic Structure • Atoms: protons, neutrons, and electrons. • The number of protons determines the identity of the element. • Some atoms of the same element have a different number of neutrons. These are called isotopes. • Example: 12C, 13C, and 14C. =>

Electronic Structure Electrons:outside the nucleus,in orbitals. Electrons have wave properties. Electron density is the probability of finding the electron in a particular part of an orbital. 。 Orbitals are grouped into“shells,”at different distances from the nucleus. > Chapter 1 4

Chapter 1 4 Electronic Structure • Electrons: outside the nucleus, in orbitals. • Electrons have wave properties. • Electron density is the probability of finding the electron in a particular part of an orbital. • Orbitals are grouped into “shells,” at different distances from the nucleus. =>

First Electron Shell electron density distance distance from the nucleus nucleus Copyright2005 Pearson Prentice Hall,Inc The 1s orbital holds two electrons. Chapter 1 5

Chapter 1 5 First Electron Shell The 1s orbital holds two electrons

Second Electron Shell 2p node clectron density node node electron distance from density the nucleus distance distance from the from the nucleus nucleus nucleus nucleus node nodal plane Cooyright 2005 Pearson Prentice Hall,ing 2s orbital (spherical) => 2p orbital Chapter 1 Three p orbitals 6

Chapter 1 6 Second Electron Shell 2s orbital (spherical) => Three p orbitals 2p orbital

Electronic Configurations ·Aufbau Principle: Place electrons in Relative orbital energies lowest energy 12p.↑2p,-2p. orbital first. ·Hund's Rule: energy ￥2s Equal energy orbitals are half- filled,then filled. Copyright2005 Pearson Prentice Hall,Inc. ·6C:1s22s22p2 二> Chapter 1

Chapter 1 7 Electronic Configurations • Aufbau Principle: Place electrons in lowest energy orbital first. • Hund’s Rule: Equal energy orbitals are half￾filled, then filled. • 6C: 1s 2 2s 2 2p 2    => 

Electronic Configurations TABLE 1-1 Electronlc Conflguratlons of the Elements of the FIrst and Second Rows Element Configuration Valence Electrons H 1s1 1 He 1s2 2 Li 1522s1 Be 1s22x2 2 B 1s2222p 3 C 1s22s22p2p 4 N 1s22522p12p2p 5 0 1s22s22p22p2p 6 F 1s22s22p22p2p 7 Ne 1s22s22p22p2p月 8 => Chapter 1

Chapter 1 8 Electronic Configurations =>

Bond Formation lonic bonding:electrons are transferred. Covalent bonding:electron pair is shared. HO:H -C Na+:CI nonpolar polar ionic bond covalent bond covalent bond Copyright2005 Pearson Prentice Hall.Inc. => Chapter 1 9

Chapter 1 9 Bond Formation • Ionic bonding: electrons are transferred. • Covalent bonding: electron pair is shared. =>

Lewis Structures ·Bonding electrons Nonbonding electrons or lone pairs H H Satisfy the octet rule! => Chapter 1 10

Chapter 1 10 Lewis Structures • Bonding electrons • Nonbonding electrons or lone pairs Satisfy the octet rule! => C H H H O H