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Organic Chemistry

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: blou@mail.cgu.edu.tw Office Hours: Tuesday 10:10-12:00 am. Lecture & Assignment Schedule (NEW). Week Date Topics 1 09/19,20 Introduction & Structure & Bonding (1)

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Organic Chemistry

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  1. 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: blou@mail.cgu.edu.tw • Office Hours: Tuesday 10:10-12:00 am

  2. Lecture & Assignment Schedule (NEW) WeekDateTopics 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: Proteins 1801/16期末考(30%)

  3. Lecture & Assignment Schedule WeekDateTopics 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: Proteins 18 01/16期末考

  4. Text Book “Fundamentals of Organic Chemistry” 6th Edition, (Brooks/Cole Publishing Company) 2006 by John McMurry

  5. 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！

  6. Chapter 1 Structure and Bonding; Acids and Bases

  7. Chapter 1 Structure & Bonding • What is organic Chemistry? treat illnesses, protect crops, & clean clothes

  8. Why should we study it? • Which elements in organic compounds?

  9. Organic chemistryis 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)

  10. 1.1 Atomic Structure • Atom: (2x10-10 m) • Nucleus • Protons (+) 10-14 ~ 10-15 m • neutrons • Electrons (-) 10-10 m

  11. 1.1 Atomic Structure • Atomic number (Z) • Mass number (A) • Atomic weight • Orbital (): s, p, d, & f. (fig. 1.4)

  12. 1.2 Electron Configuration of Atoms • Ground-state electron configuration • Rules 1-3 at page 4 • See Table 1.1 as examples

  13. 1.3 Chemical Bonding Theory • 2D to 3D • Tetrahedral carbon atom

  14. 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)

  15. 1.4 The Nature of Chemical Bonds • Lewis structures

  16. Number of covalent bonds

  17. 1.4 The Nature of Chemical Bonds • Kekulé strutures (line-bond structure) • Table 1.2

  18. 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

  19. 1.5 Forming Covalent Bonds • Molecular orbitals

  20. 1.6~1.8 Hybridization • Hybridization: (1) SP3 orbitals : Methane

  21. Ethane: CH3-CH3

  22. 1.8 Double and Triple Bonds

  23. Ethylene • C2H4 • s bond • P bond

  24. Acetylene • C2H2 • One s-bond • & two p-bonds

  25. 1.9 Bond Polarity & Electronegativity • Covalent bond to ionic bond EN = 0 0< EN <2.0 EN>2.0

  26. 1.9 Bond Polarity & Electronegativity • Elctronegativity: ability of an atom to attract electrons in a covalent bond.

  27. 1.10 Bond Polarity & Electronegativity • Electrostatic potential maps • Electron rich (red) • Electron poor (blue)

  28. 1.10~11 Acids & Bases • Bronstered-Lowry definition • Donates/accepts a hydrogen ion (H+) • Conjugate A/B

  29. 1.10~11 Acids & Bases • Ka & pKa & relative strength of acid

  30. 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)

  31. Organic bases (red) • Have an atom with a lone pair of electrons that can bond to H+ • -O & -N

  32. Lewis definition • Accepts & donates an electron pair

  33. Lewis acids & bases Reactions

  34. 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

  35. 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 reaction http://tabriz-chemists.blogfa.com/post-379.aspx

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