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The Art of Writing Reasonable Organic Reaction Mechanisms

The Art of Writing Reasonable Organic Reaction Mechanisms. University of Kentucky Professor of Chemistry Synthetic Organic Chemistry 1987 B.A., Princeton University 1992 Ph. D., Massachusetts Institute of Technology 1992-1994 Post-doctoral Fellow, Cambridge University.

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The Art of Writing Reasonable Organic Reaction Mechanisms

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  1. The Art of Writing Reasonable Organic Reaction Mechanisms University of Kentucky Professor of Chemistry SyntheticOrganic Chemistry 1987 B.A., Princeton University 1992 Ph. D., Massachusetts Institute of Technology 1992-1994 Post-doctoral Fellow, Cambridge University Robert B. Grossman

  2. 課程須知 參考書目 Organic Synthesis Organic Reaction Mechanisms Robert B. Grossman University of Kentucky A. C. Knipe University of Ulster Michael B. Smith University of Connecticut

  3. 課程須知 授課大綱 評量方式 一、有機化學反應機制的基本原則 (Basics of Organic Reactions) 二、鹼性條件下的有機化學反應 (Reactions under Basic Conditions) 三、酸性條件下的有機化學反應 (Reactions under Acid Conditions) 四、環化反應 (Pericyclic Reactions) 五、自由基反應 (Free Radical Reactions) *六、過渡金屬催化有機反應 (Metal-Catalyzed Reactions) 期末考範圍: 整學期授課內容 隨堂測驗: 每節課開始, 共兩題。 期末報告: 最後一節課分組報告，兩人一組， 每組5分鐘，並於課後繳交報告。

  4. 課程須知 Mechanisms are the means by which organic reactions are discovered, rationalized, optimized, and incorporated into the canon. They represent the framework that allows us to understand organic chemistry. The purpose of this book is to help you learn how to draw reasonable mechanisms for organic reactions. The general approach is to familiarize you with the classes and types of reaction mechanisms that are known and to give you the tools to learn how to draw mechanisms for reactions that you have never seen before. *Common error alerts are scattered throughout the text to warn you about common pitfalls and misconceptions that bedevil students. Pay attention to these alerts, as failure to observe their strictures has caused many, many exam points to be lost over the years.

  5. Chapter One The Basics of Organic Chemistry

  6. Common Abbreviations for Organic Substructures

  7. Formal Charge Formal Charge Formal charges are a useful tool for ensuring that electrons are not gained or lost in the course of a reaction. EX: Calculate the formal charge of Al, N, Br, C *Common error alert: Formal charges are not a reliabe guide to chemical reactivity. CH3+ NH4+which is more stable? 6e- 8e-

  8. Resonance Structure Resonance Structure For each σ bonding pattern, there are often several ways in which π and nonbonding electrons can be distributed. These different ways are called resonance structures. The true electronic picture of a compound is a weighted average of the different resonance structures. Benzene is neither this nor this. (1+2)/2= 1(1/2) bond Diazomethane is neither this nor this. Which structure is more important? Electronegativity: F> O> N> Cl

  9. Resonance Structure Types of Resonance Structure: 1. Look for a electron-deficient atom adjacent to a π bond. Which structure is more important? 5. The two electrons of a πbond can be divided evenly or unevenly between the two atoms making up that bond . 2. Look for a radicaladjacent to a π bond. 3. Look for a lone pairadjacent to a π bond. Draw the reasonable resonance structure of following compounds? 4. In aromatic compounds, π bonds move around to form new resonance structure. naphthalene

  10. Hyperconjugation: The bonding pair of electrons in the σ orbitals can delocalize into partly P orbital. 1ocabocation 3 adjacent C-H bonds 2ocabocation 6 adjacent C-H bonds Stability 3ocabocation 9 adjacent C-H bonds > >

  11. Molecular Shape: Lewis Structure and Molecular Orbitals Lewis Structure 1. 劃出分子結構，並使所有原子符合八隅體(H例外)，統計其電子數A 2. 計算所有原子的價電子數總和B 3.(A- B)/2為共用電子對，一般形成共用電子對的方法為環、雙鍵或三鍵 Linear SP Trigonal SP2 Tetrahedron SP3 eg. COCl2 A= 26 B= 4+6+(7*2)= 24 (26-24)/2= 1 SP2 trigonal Draw the Lewis structure for following molecules and determinate the molecular shape? HI, C22-, CH3OH, SiO2, O2, CS2, CN-

  12. Molecular Orbitals Hybrid Orbitals 1. Atomic Orbital(A.O.) Molecular Orbital(M.O.) H2 Antionding Why hydrogen exits as H2, but helium is monoatomic? Bonding 2. sp hybrids produce linear structure: 1800 degree results from minimizes electron repulsion BeH2 Be 1S22S22P0 . 2 H+

  13. Molecular Shape Hybrid Orbitals 3. sp2hybrids create trigonal structure BH3 B 1S22S22P1 4. sp3 hybridization explain the shape of tetrahedral carbon compounds CH4

  14. Structure and Stability of Organic Compounds Bond energy and bond length Determine the hybridization of C, N, O, B and F atoms in each of following compounds? NH3, H2O, BF3,

  15. Aromaticity Aromatic 1. Cyclic. 2. P orbitals. 3. Planar. 4. total e-= 4n+2 Aromatic compounds Stability: cyclic > acyclic > naphthalene azulenephenanthrene furan thiophenepyrroleindole Cyclopentadienidetropyliumpyrylium Explain why they are nonromatic compounds?

  16. Structure and Stability of Organic Compounds Antiaromatic 1. Cyclic. 2. P orbitals. 3. Planar. 4. total e- = 4n Stability: acyclic > cyclic > Nonaromatic Nonaromatic If there is no cyclic array of continuously overlapping p orbitals, then the compound is nonaromatic.

  17. Acidity Acidity stability 1. Electronegativity HFand H2O electronegativity: F > O acidity: HF > H2O 2. Size HI, HBr and HCl Size: I- > Br- > Cl- acidity: HI > HBr>HCl 3. Resonance Resonance forms:

  18. pKa Values Acidity pKa = -log

  19. Indicate which of each pair of compounds is likely to be more acidic and why?

  20. Kinetics and Thermodynamics Kinetics and Thermodynamics Chemical thermodynamics: determine the reaction will happen or not. ΔH0 is easier to measure and TΔS0 is small compared with ΔH0for most reaction(T<100oC). Chemical Kinetics: determine how fast of the reaction. TS ΔG‡: activation energy TS: trasition state ΔG‡

  21. Kinetic or thermodynamic control Kinetic or thermodynamic control Endo Rule Originate from an attractive interaction between the π system of the diene and dienophile. endo TS exo Intermediate One of the joys of orgaic chemistry is designing condition under which only the kinetic or themodynamic product is obtained. *Common error alert: Don’t confuse TS and Intermediate.

  22. Basics in Drawing a Mechanism Getting Started in Drawing a Mechanism

  23. Classes of Overall Transformation Classes of Overall Transformation 1. In a addition reaction, two S.M. combine to give a single product. Usually a π bond in one S.M. is replaced by two σ bond. 2. In a elimination reaction, one S.M. is divided into two products. Usually two σbond in one S.M. are replaced by a new πbond.

  24. Classes of Overall Transformation Classes of Overall Transformation 3. In a substitution reaction, an atom or group that is σbond to the rest of S.M. is replaced by another σbond atom or group. 4. In a rearrangement, one S.M. gives one product with a different structure.

  25. Classes of Mechanisms Classes of Mechanisms(polar, radical, pericyclic, metal-mediated reaction) 1. Polar Reaction: The chemistry of nuclephiles and electrophiles. Nuclephile a. Nucleophilicity increase as you go down the period table(polarizability). eg. I- > Cl-, Et2S > Et2O b. Nucleophilicity decrease with increase steric effect. eg. EtO- is good base and nuclephile, but tBuO- is good base bad nuclephile. Poor nuclephile and good base: LDA, LiN(SiMe3)3, DBU, TEA, EtN(i-Pr)2, t-BuLi c. Nucleophilicity increase in polar aprotic solvent.

  26. Polar Reaction Types of nuclephile a. Lone pair: N, O, S… b. Sigma bond: MHX, RMgBr, RLi, R2CuLi c. Pi bond: weak nuclephile and weak electrophile. When π bonds attach a electron-pull heteroatoms, it become much better nuclephile. Nu E+

  27. Polar Reaction Types of electrophile a. Lewis acid(BF3, AlCl3), Carbocation b. Sigma bondelectrophile: Good leaving group(X) c. Pi bond: When π bonds attach a electron-withdrawing group.

  28. Polar Reaction *Common error alert: If a reaction is under acidic conditions, no strong bases can be present! If a reaction is under basic conditions, no strong acids can be present! Basic condition No R2O+H present Acidic condition No RO- present Free H+ and R3C+ should not be drawn under basic conditions Good base and acid can’t exist in one structure.

  29. Free-Radical Reaction Generation ofFree-radical a. Sigma bond homolysis and peroxide compounds b. One-electron reagents: Oxidative: DDQ, p-Chlornail, CAN, Pb(OAc)4, Mn(OAc)3… Reductive: Na, Li, SmI2, … c. The cycloaromatization

  30. Free-Radical Reaction Chain Reaction Overall reaction Initiators: Br2, AIBN, (BzO)2, (t-Buo)2, AIBN with light a. Initiation more stable b. Propagation c. Termination dimerization elimination

  31. Pericyclic Reaction a. Electro cyclic reactions(ring opening or ring closing) b. Cycloadditions(two π bonds change to two σ bonds) c. Sigmatropic(σ bond cleavage) d. Ene reaction(six electrons, [4+2]cycloaddition and [1, 5]sigmatropic, allylic H)

  32. Exercises Define the classes of the following pericyclic reaction?

  33. Transition-Metal-Mediatd Reactions *Common error alert: a. TiCl4, FeCl3, AlCl3, AgOTf, ZnCl2 are common Lewis acids. b. FeCl2, TiCl3, SmI2, (NH4)2Ce(NO)6(CAN) are one-electron reducing or oxidizing agents. Transition-Metal-Mediated Reactions Pd, Os, Co, Rh, Ir, Cu…

  34. Exercises Classify each of the following reactions as polar, free radical, pericyclicor transition-metal-mediated. a. b. c. d. e. g. f. h.

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