5 An Overview of Organic Reactions Based on

5. An Overview of Organic Reactions Based on Mc. Murry’s Organic Chemistry, 6 th edition, Chapter 5 © 2003 Ronald Kluger Department of Chemistry University of Toronto Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 1

5. 1 Kinds of Organic Reactions n In general, we look at what occurs and try to learn how it happens n Common patterns describe the changes n Addition reactions – two molecules combine n Elimination reactions – one molecule splits into two n Substitution – parts from two molecules exchange n Rearrangement reactions – a molecule undergoes changes in the way its atoms are connected Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 2

5. 2 How Organic Reactions Occur: Mechanisms n In a clock the hands move but the mechanism behind the face is what causes the movement n In an organic reaction, we see the transformation that has occurred. The mechanism describes the steps behind the changes that we can observe n Reactions occur in defined steps that lead from reactant to product Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 3

Steps in Mechanisms n We classify the types of steps in a sequence n A step involves either the formation or breaking of a covalent bond n Steps can occur in individually or in combination with other steps n When several steps occur at the same time they are said to be concerted Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 4

Types of Steps in Reaction Mechanisms n Formation of a covalent bond Homogenic or heterogenic n Breaking of a covalent bond n Homogenic or heterogenic n Oxidation of a functional group n Reduction of a functional group n Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 5

Homogenic Formation of a Bond n One electron comes from each fragment n No electronic charges are involved n Not common in organic chemistry Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 6

Heterogenic Formation of a Bond n One fragment supplies two electrons n One fragment supplies no electrons n Combination can involve electronic charges n Common in organic chemistry Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 7

Homolytic Breaking of Covalent Bonds n Each product gets one electron from the bond

Heterolytic Breaking of Covalent Bonds n Both electrons from the bond that is broken become associated with one resulting fragment n A common pattern in reaction mechanisms Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 9

Indicating Steps in Mechanisms n Curved arrows indicate breaking and forming of bonds n Arrowheads with a “half” head (“fish-hook”) indicate homolytic and homogenic steps (called ‘radical processes’) n Arrowheads with a complete head indicate heterolytic and heterogenic steps (called ‘polar processes’) Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 10

Radicals n Alkyl groups are abbreviate “R” for radical Example: Methyl iodide = CH 3 I, Ethyl iodide = CH 3 CH 2 I, Alkyl iodides (in general) = RI n A “free radical” is an “R” group on its own: n CH 3 is a “free radical” or simply “radical” n Has a single unpaired electron, shown as: CH 3. n Its valence shell is one electron short of being complete n Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 11

5. 3 Radical Reactions and How They Occur n Note: Polar reactions are more common n Radicals react to complete electron octet of valence shell n A radical can break a bond in another molecule and abstract a partner with an electron, giving substitution in the original molecule n A radical can add to an alkene to give a new radical, causing an addition reaction Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 12

Steps in Radical Substitution n Three types of steps n n n Initiation – homolytic formation of two reactive species with unpaired electrons n Example – formation of Cl atoms form Cl 2 and light Propagation – reaction with molecule to generate radical n Example - reaction of chlorine atom with methane to give HCl and CH 3. Termination – combination of two radicals to form a stable product: CH 3. + CH 3 Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 13

5. 4 Polar Reactions and How They Occur n Molecules can contain local unsymmetrical electron distributions due to differences in electronegativities n This causes a partial negative charge on an atom and a compensating partial positive charge on an adjacent atom n The more electronegative atom has the greater electron density Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 14

Electronegativity of Some Common Elements n The relative electronegativity is indicated n Higher numbers indicate greater electronegativity n Carbon bonded to a more electronegative element has a partial positive charge ( +) Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 15

Polarizability n Polarization is a change in electron distribution as a response to change in electronic nature of the surroundings n Polarizability is the tendency to undergo polarization n Polar reactions occur between regions of high electron density and regions of low electron density Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 16

Generalized Polar Reactions n An electrophile, an electron-poor species, combines with a nucleophile, an electron-rich species n An electrophile is a Lewis acid n A nucleophile is a Lewis base n The combination is indicate with a curved arrow from nucleophile to electrophile Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 17

5. 5 An Example of a Polar Reaction: Addition of HBr to Ethylene n HBr adds to the part of C-C double bond n The bond is electron-rich, allowing it to function as a nucleophile n H-Br is electron deficient at the H since Br is much more electronegative, making HBr an electrophile Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 18

Mechanism of Addition of HBr to Ethylene n HBr electrophile is attacked by electrons of ethylene (nucleophile) to form a carbocation intermediate and bromide ion n Bromide adds to the positive center of the carbocation, which is an electrophile, forming a C-Br bond n The result is that ethylene and HBr combine to form bromoethane n All polar reactions occur by combination of an electron-rich site of a nucleophile and an electrondeficient site of an electrophile Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 19

5. 6 Using Curved Arrows in Polar Reaction Mechanisms n Curved arrows are a way to keep track of changes in n n bonding in polar reaction The arrows track “electron movement” Electrons always move in pairs Charges change during the reaction One curved arrow corresponds to one step in a reaction mechanism Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 20

Rules for Using Curved Arrows n The arrow goes from the nucleophilic reaction site to the electrophilic reaction site n The nucleophilic site can be neutral or negatively charged n The electrophilic site can be neutral or positively charged Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 21

5. 7 Describing a Reaction: Equilibria, Rates, and Energy Changes n Reactions can go either forward or backward to reach equilibrium The multiplied concentrations of the products divided by the multiplied concentrations of the reactant is the equilibrium constant, Keq n Each concentration is raised to the power of its coefficient in the balanced equation. n a. A + b. B c. C + d. D Keq = [Products]/[Reactants] = [C]c [D]d / [A]a[B]b Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 22

Magnitudes of Equilibrium Constants n If the value of Keq is greater than 1, this indicates that at equilibrium most of the material is present as products n If Keq is 10, then the concentration of the product is ten times that of the reactant n A value of Keq less than one indicates that at equilibrium most of the material is present as the reactant n If Keq is 0. 10, then the concentration of the reactant is ten times that of the product Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 23

Free Energy and Equilibrium n The ratio of products to reactants is controlled by their n n relative Gibbs free energy This energy is released on the favored side of an equilibrium reaction The change in Gibbs free energy between products and reacts is written as “DG” If Keq > 1, energy is released to the surrounding (exergonic reaction) If Keq < 1, energy is absorbed from the surroundings (endergonic reaction) Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 24

Numeric Relationship of Keq and Free Energy Change n The standard free energy change at 1 atm pressure and 298 K is DGº n The relationship between free energy change and an equilibrium constant is: n DGº = - RT ln Keq where n R = 1. 987 cal/(K x mol) n T = temperature in Kelvin n ln = natural logarithm of Keq n (See the example in the book for a calculation) Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 25

Changes in Energy at Equilibrium n Free energy changes (DGº) can be divided into n n a temperature-independent part called entropy (DSº) that measures the change in the amount of disorder in the system a temperature-dependent part called enthalpy (DHº) that is associated with heat given off (exothermic) or absorbed (endothermic) n Overall relationship: DGº = DHº - TDSº Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 26

5. 8 Describing a Reaction: Bond Dissociation Energies n Bond dissociation energy (D): Heat change that occurs when a bond is broken by homolysis n The energy is mostly determined by the type of bond, independent of the molecule n The C-H bond in methane requires a net heat input of 105 kcal/mol to be broken at 25 ºC. n Table 5. 3 lists energies for many bond types n Changes in bonds can be used to calculate net changes in heat Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 27

Calculation of an Energy Change from Bond Dissociation Energies n Addition of Cl-Cl to CH 4 (Table 5. 3) n Breaking: C-H D = 438 k. J/mol Cl-Cl D = 243 k. J/mol n Making: C-Cl D = 351 k. J/mol H-Cl D = 432 k. J/mol Energy of bonds broken = 438 + 243 = 681 k. J/mol Energy of bonds formed = 351 + 432 = 783 k. J/mol DHº = 681 – 783 k. J/mol = -102 k. J/mol Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 28

5. 9 Describing a Reaction: Energy Diagrams and Transition States n The highest energy point in a reaction step is called the transition state n The energy needed to go from reactant to transition state is the activation energy (DG‡) Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 29

First Step in Addition n In the addition of HBr the (conceptual) transition-state structure for the first step n The bond between carbons begins to break n The C–H bond begs to form n The H–Br bond begins to break Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 30

5. 10 Describing a Reaction: Intermediates n If a reaction occurs in more than one step, it must involve species that are neither the reactant nor the final product n These are called reaction intermediates or simply “intermediates” n Each step has its own free energy of activation n The complete diagram for the reaction shows the free energy changes associated with an intermediate Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 31

Formation of a Carbocation Intermediate n HBr, a Lewis acid, adds to the bond n This produces an intermediate with a positive charge on carbon - a carbocation n This is ready to react with bromide Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 32

Carbocation Intermediate Reactions with Anion n Bromide ion adds an electron pair to the carbocation n An alkyl halide produced n The carbocation is a reactive intermediate Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 33

Reaction Diagram for Addition of HBr to Ethylene n Two separate steps, each with a own transition state n Energy minimum between the steps belongs to the carbocation reaction intermediate. Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 34

Biological Reactions n Reactions in living organisms follow reaction n n diagrams too They take place in very controlled conditions They are promoted by catalysts that lower the activation barrier The catalysts are usually proteins, called enzymes Enzymes provide an alternative mechanism that is compatible with the conditions of life Mc. Murry Organic Chemistry 6 th edition Chapter 5 (c) 2003 35