1. 8-1 Organic Chemistry William H. Brown Christopher S. Foote Brent L. Iverson William H. Brown Christopher S. Foote Brent L. Iverson

2. 8-2 Haloalkanes Chapter 8

3. 8-3 Structure  Haloalkane (alkyl halide):  Haloalkane (alkyl halide): a compound containing a halogen covalently bonded to an sp 3 hybridized carbon; given the symbol RX  Haloalkene (vinylic halide):  Haloalkene (vinylic halide): a compound containing a halogen bonded to an sp 2 hybridized carbon  Haloarene (aryl halide):  Haloarene (aryl halide): a compound containing a halogen bonded to a benzene ring; given the symbol ArX (we do not study vinylic or aryl halides in this chapter)

4. 8-4 Nomenclature number the parent chain to give the substituent encountered first the lowest number, whether it is halogen or an alkyl group indicate halogen substituents by the prefixes fluoro-, chloro-, bromo-, and iodo-, and list them in alphabetical order with other substituents locate each halogen on the parent chain by giving it a number preceding the name of the halogen in haloalkenes, number the parent chain to give carbon atoms of the double bond the lower set of numbers

5. 8-5 Nomenclature examples  Common names:  Common names: name the alkyl group followed by the name of the halide

6. 8-6 Nomenclature several polyhaloalkanes are common solvents and are generally referred to by their common or trivial names hydrocarbons in which all hydrogens are replaced by halogens are commonly named as perhaloalkanes or perhaloalkenes

7. 8-7 Dipole Moments  Dipole moment of RX depends on: the sizes of the partial charges the distance between them the polarizability of the unshared electrons on halogen

8. 8-8 van der Waals Forces  Haloalkanes are associated in the liquid state by van der Waals forces  van der Waals forces:  van der Waals forces: a group intermolecular attractive forces including dipole-dipole forces dipole-induced dipole forces induced dipole-induced dipole (dispersion) forces  van der Waals forces pull molecules together as molecules are brought closer and closer, van der Waals attractive forces are overcome by repulsive forces between electron clouds of adjacent atoms or molecules

9. 8-9 van der Waals Forces the energy minimum is where the attractive forces are the strongest van der Waals radiusnonbonded interatomic and intermolecular distances at these minima can be measured by x-ray crystallography and each atom and group of atoms can be assigned a van der Waals radius nonbonded atoms in a molecule cannot approach each other closer than the sum of their van der Waals radii without causing nonbonded interaction strain

10. 8-10 Boiling Points  For an alkane and a haloalkane of comparable size and shape, the haloalkane has the higher boiling point the difference is due almost entirely to the greater polarizability of the three unshared pairs of electrons on halogen compared with the low polarizability of shared electron pairs of covalent bonds polarizability:polarizability: a measure of the ease of distortion of the distribution of electron density about an atom in response to interaction with other molecules and ions; fluorine has a very low polarizability, iodine has a very high polarizability

11. 8-11 Boiling Points among constitutional isomers, branched isomers have a more compact shape, decreased area of contact, decreased van der Waals attractive forces between neighbors, and lower boiling points

12. 8-12 Boiling Points boiling points of fluoroalkanes are comparable to those of hydrocarbons of similar molecular weight and shape the low boiling points of fluoroalkanes are the result of the small size of fluorine, the tightness with which its electrons are held, and their particularly low polarizability

13. 8-13 Density  The densities of liquid haloalkanes are greater than those of hydrocarbons of comparable molecular weight a halogen has a greater mass per volume than a methyl or methylene group  All liquid bromoalkanes and iodoalkanes are more dense than water  Di- and polyhalogenated alkanes are more dense than water

14. 8-14 Bond Lengths, Strengths  C-F bonds are stronger than C-H bonds; C-Cl, C-Br, and C-I bonds are weaker

15. 8-15 Halogenation of Alkanes  If a mixture of methane and chlorine is kept in the dark at room temperature, no change occurs  If the mixture is heated or exposed to visible or ultraviolet light, reaction begins at once with the evolution of heat  Substitution:  Substitution: a reaction in which an atom or group of atoms is replaced by another atom or group of atoms

16. 8-16 Halogenation of Alkanes if chloromethane is allowed to react with more chlorine, a mixture of chloromethanes is formed

17. 8-17 Regioselectivity  Regioselectivity is high for bromination, but not as high for chlorination

18. 8-18 Regioselectivity  Regioselectivity is 3° > 2° > 1° for bromination, approximately 1600:80:1 for chlorination, approximately 5:4:1 Example: Example: draw all monobromination products and predict the percentage of each for this reaction

19. 8-19 Energetics  Bond Dissociation Enthalpies (BDE)

20. 8-20 Energetics  Using BDE, we can calculate the heat of reaction,  H 0, for the halogenation of an alkane

21. 8-21 Mechanism  Radical:  Radical: any chemical species that contains one or more unpaired electrons homolytic bond cleavageradicals are formed by homolytic bond cleavage the order of stability of alkyl radicals is 3° > 2° > 1° > methyl

22. 8-22 Radical Chain Mechanism  Chain initiation:  Chain initiation: a step in a chain reaction characterized by formation of reactive intermediates (radicals, anions, or cations) from nonradical or noncharged molecules

23. 8-23 Radical Chain Mechanism  Chain propagation:  Chain propagation: a step in a chain reaction characterized by the reaction of a reactive intermediate and a molecule to form a new reactive intermediate and a new molecule  Chain length:  Chain length: the number of times the cycle of chain propagation steps repeats in a chain reaction

24. 8-24 Radical Chain Mechanism  Chain termination:  Chain termination: a step in a chain reaction that involves destruction of reactive intermediates

25. 8-25 Chain Propagation Steps  For any set of chain propagation steps, their equations add to the observed stoichiometry enthalpies add to the observed  H 0

26. 8-26 Regioselectivity?  The regioselectivity of chlorination and bromination can be accounted for in terms of the relative stabilities of alkyl radicals (3° > 2° > 1° > methyl)  But how do we account for the greater regioselectivity of bromination (1600:80:1) compared with chlorination (5:4:1)

27. 8-27 Hammond’s Postulate  Hammond’s Postulate:  Hammond’s Postulate: the structure of the transition state for an exothermic step looks more like the reactants of that step than the products for an endothermic step looks more like the products of that step than the reactants  This postulate applies equally well to the transition state for a one-step reaction and to each transition state in a multi-step reaction

28. 8-28 Hammond’s Postulate

29. 8-29 in halogenation of an alkane, hydrogen abstraction (the rate-determining step) is exothermic for chlorination but endothermic for bromination

30. 8-30 Hammond’s Postulate  Because hydrogen abstraction for chlorination is exothermic: the transition state resembles the alkane and a chlorine atom there is little radical character on carbon in the transition state regioselectivity is only slightly influenced by radical stability

31. 8-31 Hammond’s Postulate  Because hydrogen abstraction for bromination is endothermic: the transition state resembles an alkyl radical and HBr there is significant radical character on carbon in the transition state regioselectivity is greatly influenced by radical stability radical stability is 3° > 2° > 1° > methyl, and regioselectivity is in the same order

32. 8-32 Hammond’s Postulate

33. 8-33 Stereochemistry  When radical halogenation produces a chiral center or takes place at a hydrogen on a chiral center, the product is a mixture of R and S enantiomers as a racemic mixture for simple alkyl radicals, the carbon bearing the radical is sp 2 hybridized and the unpaired electron occupies the unhybridized 2p orbital (see next screen)

34. 8-34 Stereochemistry

35. 8-35 Allylic Halogenation  Allylic carbon:  Allylic carbon: a C adjacent to a C-C double bond  Allylic hydrogen:  Allylic hydrogen: an H on an allylic carbon an allylic C-H bond is weaker than a vinylic C-H bond

36. 8-36 Allylic Bromination  Allylic bromination using NBS

37. 8-37 Allylic Bromination  A radical chain mechanism Chain initiation Chain propagation

38. 8-38 Allylic Bromination chain termination  Br 2 is provided by the reaction of NBS with HBr

39. 8-39 The Allyl Radical  A hybrid of two equivalent contributing structures (Equivalent contributing structures) CH 2 CHCH 2 CHCH 2 CH 2

40. 8-40 The Allyl Radical  Molecular orbital model of the allyl radical

41. 8-41 The Allyl Radical  Unpaired electron spin density map of the allyl radical the unpaired electron density (green lobes) appears only on carbons 1 and 3

42. 8-42 Allylic Halogenation Example 8.5Example 8.5 Account for the fact that allylic bromination of 1-octene by NBS gives these isomeric products

43. 8-43 Radical Autoxidation  Autoxidation:  Autoxidation: oxidation requiring oxygen, O 2, and no other oxidizing agent occurs by a radical chain mechanism similar to that for allylic halogenation in this section, we concentrate on autoxidation of the hydrocarbon chains of polyunsaturated triglycerides the characteristic feature of the fatty acid chains in polyunsaturated triglycerides is the presence of 1,4- dienes radical abstraction of a doubly allylic hydrogen of a 1,4-diene forms a particularly stable radical

44. 8-44 Radical Autoxidation autoxidation begins when a radical initiator, X, abstracts a doubly allylic hydrogen this radical is stabilized by resonance with both double bonds

45. 8-45 Radical Autoxidation the doubly allylic radical reacts with oxygen, itself a diradical, to form a peroxy radical the peroxy radical then reacts with another 1,4-diene to give a new radical, R, and a hydroperoxide vitamin A, a naturally occurring antioxidant, reacts preferentially with the initial peroxy radical to give a resonance-stabilized phenoxy radical, which is very unreactive, and scavenges another peroxide radical

46. 8-46 Radical Autoxidation vitamin E as an antioxidant

47. 8-47 Radical Addition of HBr to Alkenes  Addition of HBr to alkenes gives either Markovnikov addition or non-Markovnikov addition depending on reaction conditions Markovnikov addition occurs when radicals are absent non-Markovnikov addition occurs when peroxides or other sources of radicals are present

48. 8-48 Radical Addition of HBr to Alkenes addition of HCl and HI gives only Markovnikov products to account for the the non-Markovnikov addition of HBr in the presence of peroxides, chemists proposed a radical chain mechanism  Chain initiation

49. 8-49 Radical Addition of HBr to Alkenes  Chain propagation

50. 8-50 Radical Addition of HBr to Alkenes  Chain termination  This pair of addition reactions illustrates how the products of a reaction can often be changed by a change in experimental conditions polar addition of HBr is regioselective, with Br adding to the more substituted carbon radical addition of HBr is also regioselective, with Br adding to the less substituted carbon

51. 8-51 Haloalkanes End Chapter 8