organic chemistry fall, 2006 by 駱碧秀老師 time: tue. 08:10-10:00 & wed. 13:00-14:00...
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Organic Chemistry Fall, 2006 by 駱碧秀老師
Time: Tue. 08:10-10:00 & Wed. 13:00-14:00
Office: 醫學大樓 5F, 分機 5018
E-mail: [email protected]
Office Hours: Tuesday 10:10-12:00 am
Lecture & Assignment Schedule (NEW) Week Date Topics
1 09/19,20 Introduction & Structure & Bonding (1)
2 09/26,27 Alkanes (2) 3 10/03,04 Alkenes (3) 4 10/10,11 Reaction of Alkenes & Alkynes (4)5 10/17,18 Aromatic Compounds (5) 6 10/24 期中考 (I) (20%)7 10/31,01 Stereochemistry (6) 8 11/07,08 Alkyl Halides (7)
9 11/14,15 Structure Determination (13) 10 11/21,22 Alcohols-1 (8)11 11/28,29 Alcohols-2 (8)12 12/05 期中考 (II) (20%)13 12/12,13 Aldehydes & Ketones (9)14 12/19,20 Carboxylic Acids & Derivatives (10)
15 12/26,27 Carbonyl Alpha-Substitution Reactions (11)16 01/02,03 Amines (12)17 01/08,09 Biomolecules: Proteins18 01/16 期末考 (30%)
Lecture & Assignment Schedule Week Date Topics
1 09/19,20 Introduction & 2 09/26,27 Structure & Bonding (1) 3 10/03,04 Alkanes (2) 4 10/10,11 Alkenes (3) 5 10/17,18 Reaction of Alkenes & Alkynes (4)6 10/24,25 Aromatic Compounds (5)
7 10/31,01 Stereochemistry (6) 8 11/07,08 Alkyl Halides (7) 9 11/14 期中考 10 11/21,22 Structure Determination (13) 11 11/28,29 Alcohols-1 (8)12 12/05,06 Alcohols-2 (8)13 12/12,13 Aldehydes & Ketones (9)14 12/19,20 Carboxylic Acids & Derivatives (10)
15 12/26,27 Carbonyl Alpha-Substitution Reactions (11)16 01/02,03 Amines (12)17 01/08,09 Biomolecules: Proteins18 01/16 期末考
Text Book
“Fundamentals of Organic Chemistry” 6th Edition,
(Brooks/Cole Publishing Company)
2006
by
John McMurry
Grading
課程參與度 : 10%平常小考 : 20%期中考 : 30%期末考 : 40%
「成績，不只是在於你知道什麼，而在於你表現什麼。」
成功法則第一招：一定要來上課！
Chapter 1
Structure and Bonding; Acids and Bases
Chapter 1 Structure & Bonding
What is organic Chemistry?treat illnesses, protect crops, & clean clothes
Why should we study it? Which elements in organic compounds?
Organic chemistry is the study of the compounds of carbon. Includes biological molecules, drugs,
solvents, dyes Does not include metal salts and materials
(inorganic) Does not include materials of large
repeating molecules without sequences (polymers)
1.1 Atomic Structure
Atom: (2x10-10 m)
Nucleus• Protons (+) 10-14 ~ 10-15 m• neutrons
Electrons (-) 10-10 m
1.1 Atomic Structure
Atomic number (Z) Mass number (A) Atomic weight Orbital (): s, p, d, & f. (fig. 1.4)
1.2 Electron Configuration of Atoms
Ground-state electron configuration Rules 1-3 at page 4
See Table 1.1 as examples
1.3 Chemical Bonding Theory
2D to 3D Tetrahedral carbon atom
1.4 The Nature of Chemical Bonds
Ionic Bonds Bond between ions due to the
electrostatic attraction : NaCl Covalent Bonds
Bonds formed by sharing electrons Lewis structures (electron-dot) Nonbonding electrons (lone-pair
electrons)
1.4 The Nature of Chemical Bonds
Lewis structures
Number of covalent bonds
Kekulé strutures (line-bond structure)
•Table 1.2
1.4 The Nature of Chemical Bonds
1.5 Forming Covalent Bonds
Valence Bond Theory How to electron sharing between atoms?
• Overlapping of two atomic orbital. Bond strength
• energy Bond length
• distance
1.5 Forming Covalent Bonds
Molecular orbitals
1.6~1.8 Hybridization
Hybridization:(1) SP3 orbitals : Methane
Ethane:CH3-CH3
1.8 Double and Triple Bonds
Ethylene C2H4
bond P bond
Acetylene C2H2
One -bond & two -bonds
1.9 Bond Polarity & Electronegativity
Covalent bond to ionic bond
EN = 0 0< EN <2.0 EN>2.0
1.9 Bond Polarity & Electronegativity
Elctronegativity: ability of an atom to attract electrons in a covalent bond.
1.10 Bond Polarity & Electronegativity
Electrostatic potential maps Electron rich (red) Electron poor (blue)
1.10~11 Acids & Bases
Bronstered-Lowry definition Donates/accepts a hydrogen ion (H+) Conjugate A/B
1.10~11 Acids & Bases
Ka & pKa & relative strength of acid
Organic acid (blue)
Those that lose a proton from O–H: methanol and acetic acid Those that lose a proton from C–H, a carbon atom next to a
C=O double bond (O=C–C–H)
Organic bases (red)
Have an atom with a lone pair of electrons that can bond to H+
-O & -N
Lewis definition
Accepts & donates an electron pair
Lewis acids & bases Reactions
Lewis Acids
The Lewis definition of acidity includes metal cations, such as Mg2+ : They accept a pair of electrons when they form a bond to a base
Group 3A elements, such as BF3 and AlCl3, are Lewis acids because they have unfilled valence orbitals and can accept electron pairs from Lewis bases
Transition-metal compounds, such as TiCl4, FeCl3, ZnCl2, and SnCl4, are Lewis acids
Organic compounds that undergo addition reactions with Lewis bases (discussed later) are called electrophiles and therefore Lewis Acids
Lewis Bases
Most oxygen- and nitrogen-containing organic compounds are Lewis bases because they have lone pairs of electrons
Some compounds can act as both acids and bases, depending on the reactionhttp://tabriz-
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