Part 3ii Substitution Reactions: Solvent

1. Part 3ii Substitution Reactions: Solvent MeOH DMSO

2. Content of Part 3ii Solvent polarity and its effect on the SN1 reaction mechanism Solvent polarity and its effect on the SN2 reaction mechanism Protic and non-protic solvents and their effect on the SN2 mechanism Protic and polar non-protic solvents and change of mechanism from SN1 to SN2 Increasing solvent polarity and change of mechanism from SN2 to SN1

3. CHM1C3 – Introduction to Chemical Reactivity of Organic Compounds– – Learning Objectives Part 3ii – Substitution Reactions: Solvent • After completing PART 5ii of this course you should have an understanding of, and be able to demonstrate, the following terms, ideas and methods. • Understand how changes in the polarity of the solvent can change the rate of reaction in both SN2 and SN1 reaction mechanisms, • Understand what is meant by the dielectric constant of a solvent, (iii) Understand what is meant by protic and non-protic solvents, (iv) Understand what a hydrogen bond is, (v) Understand how protic solvents reduce the rate of reaction of nucleophiles with substrates, and (vi) Understand how increasing the polarity of the solvent can change the mechanism of substitution from SN2 to SN1.

4. Effect of Solvent Changing the solvent in which a reaction is carried out in can (i) Effect the reaction rate (ii) Result in a change in reaction mechanism

5. Solvent Polarity and SN1 Reactions Relative Rate Solvent: H2O/EtOH Rate = k[R-Br] 1 SN1 Solvent: H2O Rate = k[R-Br] 30 000 SN1 Why is reaction much faster in water alone?

6. Both reactions must involve the sp2 hybridised carbocation. The carbocation is obviously a very polar species. Polar species are most stable in polar solvents. The dielectric constant (e) of a solvent is a measure of the polarity of a solvent. The larger the e the more polar the solvent. e (H2O) = 78 e (EtOH) = 30 Thus, higher e solvent solvate and stabilise the carbocation more easily than lower e solvents. Thus, cations are generated more rapidly in higher e solvents.

7. Solvent Polarity and SN2 Reactions Increasing solvent polarity on substrates that undergo SN2 substitution reactions has a much less dramatic effect. As there is no cation formed there is nothing to stabilise. However, it is found that there is usually a slight decrease in rate with increasing polarity, especially when the nucleophile is charged, i.e. an anion. In much the same way as a carbocation is stabilised by higher polarity solvents, so are anions. Thus, in higher polarity solvents the nucleophile is more solvated and more stable, and therefore less reactive and the rate drops in higher polarity solvents.

8. Protic Solvents and Nucleophile Interaction A protic solvent is one in which there is hydrogen capable of forming a hydrogen bond to the nucleophile, i.e. a hydrogen attached to an electronegative heteroatom (O and N). e.g. H2O, MeOH, EtOH This results in a highly solvated and stable nucleophile, and therefore relative unreactive.

9. Non-Protic Solvents and the Nucleophile Interaction A non-protic solvent is one in which there is no hydrogen capable of forming a hydrogen bond to the nucleophile. This then results in the nucleophile being poorly solvated and relatively more reactive. DMSO DMF MeCN Acetone Ethylacetate Chloroform Dichloromethane Ether Alkanes

10. SN2 SN2 Rel. Rate Protic Solvent MeOH Rate = k[R-I][N3-] 1 Non-Protic Solvent DMF Rate = k[R-I][N3-] 45 000 It should be noted MeOH and DMF have similar e values, 33 and 37 respectively. Thus, any rate differences are not a result of solvating ability alone.

11. d- Polar Protic Solvent d+ Hydrogen Bond Lone pairs are rendered less effective in attacking the electrophilic centre Polar Non-Protic Solvent DMF None of the Hs are attached to electronegative atoms, therefore no H-bond donors, as above. Therefore, lone pairs on N3- are available for attaching the electrophilic centre

12. SN1 SN2 Protic and Polar Non-Protic Solvents and Change of Mechanism from SN1 to SN2 MeOH e = 33 Rate = k[R-Cl] Rate = k[R-I][N3-] DMSO e = 46

13. MeOH:Protic, e = 33 MeOH hydrogen bonds to CN- very efficiently, thus making the CN- a relatively poor nucleophile, under these conditions. Unreactive The C-Cl bond then has time to fragment to generate the carbocation and Cl-. Therefore, reaction proceeds via SN1 mechanism DMSO:Non-Protic, e = 47 There are no strong hydrogen bonding interactions between the cyanide and the DMSO. Thus, the cyanide anion lone pairs are ‘naked’ and, therefore is a relatively good nuclephile. DMSO i.e. the cyanide can react with R-Cl before the C-Cl bond fragments. Thus, reaction proceeds via an SN2 mechanism Reactive

14. Rate = k[I-][R-Br] I- SN2 B r I Br- Br- Rate = k[R-Br] SN1 B r I I- Increasing Solvent Polarity and Change of Mechanism from SN2 to SN1 Solvent: EtOEt e = 3 Solvent: H2O e = 78 This is fairly simple to conceptualise: If your start with a alkyl halide in a low dielectric solvent then the carbocation will not be formed as the dielectric of the solvent will not support the polar carbocation. Thus, SN2 reaction mechanism will predominate at low e. As the polarity of the solvent increases it becomes increasingly easier to support a carbocation, and the I- is hydrogen bonded as is a poor nuclephile. Thus, SN1 reaction mechanism will predominate at high e.

15. Polar Protic Polar Non-Protic Non-Polar Non-Protic Dielectric Constant 38 21 18 6 Solvent H2O MeOH EtOH 1-PrOH 1-BuOH 1 PeOH HCO2H CH3CO2H Dielectric Constant 80 33 24 20 18 15 58 6 Solvent HCONMe2 DMF MeCOMe acetone MeCOEt MeCO2Et Solvent CH2Cl2 CHCl3 CCl4 Dielectric Constant 9 5 2 Polar? THF tetrahydrofuran Et2O CCl4 MeS(O)Me DMSO MeNO2 nitromethane MeCN acetonitrile 47 39 37 9 3 2 2 2 2 2 n-Octane n-Hexane n-Pentane Benzene Polar? All values rounded to nearest integer http://www.asiinstruments.com/technical.asp

16. High e solvents: Cation formation promoted (if Nu is poor, i.e. attacks slowly) SN1 Promoted Low e solvents: Cation formation prevented SN2 Promoted Polar Protic solvents: Hydrogen bond to Nu, Ineffective Nu, R-X is able to cleave, before Nu attacks SN1 Promoted Polar Non-protic solvents Nu lone pair not hydrogen bonded Effective Nu, and attacks before R-X cleaves SN2 Promoted

17. – Summary Sheet Part 3ii – Substitution Reactions: Solvent CHM1C3 – Introduction to Chemical Reactivity of Organic Compounds– If one considers an SN1 reaction in which a carbocation is formed, then increasing the polarity of the solvent will lead to better solvation of the carbocation, and therefore greater stability. Thus, increasing the solvent polarity from, for example EtOH (e = 30) to H2O (e = 78), the rate of reaction increases by several orders of magnitude as the stability of the carbocation is so much greater in H2O than EtOH. Indeed, a reaction in a low dielectric solvent may go via an SN2 reaction (i.e. no requirement for stabilisation of a carbocation), but when transferred to a higher dielectric solvent may change mechanism to SN1. Not only is the stabilisation of the carbocation important by the solvent, but also the interaction of the nucleophile with the solvent. Nucleophiles have by definition a lone pair of electrons for donation to electrophilic centres, i.e. the carbon attached to the leaving group. However, if the solvent has a hydrogen atom attached to a electronegative heteroatom (O, S, N, such as an alcohol, amine or thiol) then this hydrogen atom will carry a partial positive charge and interact as hydrogen bond acceptor with the lone pair of electrons on the nucleophile. Thus, the lone pair of electrons will now be less effective in a nucleophilic sense. Thus, SN2 mechanisms might be slowed down on transferring to protic solvents, or even change to SN1 if the media is even just slight more polar due to the increased time available for scission of the C-leaving group bond.

18. Exercise 1: Substitution Reactions Identify the ethers B and C, and rationalise the difference in reaction outcomes.

19. Answer 1: Substitution Reactions Identify the ethers D and E, and rationalise the difference in reaction outcomes. SN1 SN2 DMSO does not hydrogen bond to the EtO- lone pairs, making EtO- a good nucleophile. Thus, EtO- attacks electrophilic centre before C-Br bond cleave. carbocationic reactive intermediate EtOH hydrogen bonds to the EtO-, making EtO- a poor nucleophile. Thus, C-Br bond cleaves before attack of EtO-. E D