Thiols And Thioethers JULY 5, 2015 BY JAMES 8 COMMENTS Here’s a summary of today’s post on thiols: Thiols and Thioethers One of the most powerful insights from learning the periodic table is the fact elements in the same period (column) have similar chemical properties. For instance Alkali metals (Li, Na, K…) all shed an electron relatively easily to form monovalent cations Halogens (F, Cl, Br) all gain an electron relatively easily to form halide ions. Noble gases (He, Ne, Ar, Kr…) tend to be chemically inert. So how does what we’ve learned about the reactivity of oxygen (O) based functional groups translate to its heavier cousins sulfur (S) , selenium (Se) and tellurium (Te)? Specifically, how does the chemistry of alcohols (ROH) and ethers (ROR) compare with the chemistry of thiols (RSH) and thioethers [aka sulfides] (RSR)?. Great question! That’s the topic of today’s post, specifically thiols and thioethers. We won’t really talk about selenium chemistry beyond briefly mentioning its acidity, and we definitely won’t go anywhere near tellurium chemistry, following Wöhler’s advice on diethyl tellurium that “its obnoxious and persistent smell is connected to unpleasantness, which one wouldn’t like to endure a second time“, and that “the smell is so persistent, that one has to avoid social life for several months in order not to molest other people“. Let’s start with what’s similar between alcohols/thiols, ethers/thioethers, and then move to what’s vastly different. 1. First Things First: Thiols Smell Bad Open a textbook that discusses thiols and one of the first things they’ll mention is their vile stench. We wouldn’t want to break with this honourable tradition here at MOC. Hydrogen sulfide (H2S) is responsible for the smell of rotten eggs and bad breath, among other unpleasant things. Thiols contribute to the smell of skunks and “skunky” beer. During my time in grad school one of the world’s leading organosulfur chemists had a lab across the hall. These were not people you wanted to be downwind from. Imagine getting on the city bus and having the people next to you get up from their seats and move down to the other end. Those stories were not uncommon from the people in that lab. BTW: the sulfur chemists’ best friend is bleach, which oxidizes stinky thiols to relatively odourless sulfoxides (see #5, below). 2. Thiols Are More Acidic Than Alcohols We’ve seen that alcohols are relatively acidic (pKa’s of about 16-17). Thiols are more acidic than alcohols by an average of about 5 pKa units or so ( pKa of about 11 for the thiol pictured below). Remember that pKa is logarithmic, so that means they’re about 105 times more acidic. Why might that be? When understanding acidity trends it greatly helps to think about the stability of the conjugate base Recall that acidity will be increased by any factor which stabilizes the conjugate base. [Since acid-base reactions are equilibria, if we stabilize the product (conjugate base) we therefore make the equilibrium where the starting material (acid) loses a proton more favourable, increasing Ka. In other words, we increase the acidity.] In the case of sulfur, the negative charge will be borne on a larger atom (sulfur > oxygen) and that negative charge dispersed over a greater volume. Greater volume = more diffuse charge = greater stability. Note the greater pKa of the molecule pictured above (about 10-11). The same holds true for selenium, which has an even larger atomic radius. I can’t find a pKa value for propaneselenol but would estimate it to be about 78. [If someone has a better number, please let me know!] A corollary of the fact that the conjugate base is more stable is that thiolates [the conjugate bases of thiols] are weaker bases than alkoxides. [“The stronger the acid, the weaker the conjugate base“]. 3. Sulfur: Less Basic, More Nucleophilic Remember how alkoxides [RO–] can act as nucleophiles in SN2 reactions as well as the base in elimination (E2) reactions? With thiolates [RS–], E2 reactions aren’t an issue. The weaker basicity of thiolates means that only SN2 reactions occur with alkyl halides. Thiols are more nucleophilic than alcohols, and thiolates are more nucleophilic than alkoxides. Since nucleophilicity is measured by reaction rate, that means that these sulfur nucleophiles tend to react faster with typical electrophiles (like alkyl halides) than their oxygen-based cousins. Why? As we’ve discussed before, the lower electronegativity of sulfur (relative to oxygen) means that its pairs of electrons are held onto less tightly than oxygen, making them more readily available for donation to electrophiles (like alkyl halides). This trend continues as we descend a column of the periodic table, so in general, nucleophilicity increases in this direction as well (i.e. RSe– is even more nucleophilic than RS– ). 4. Common Reactions of Thiolates: SN2 Reactions We’ve seen that one of the most important reactions to form ethers is the Williamson ether synthesis. Here’s a textbook example of the sulfur analogue of this reaction: substitution of alkyl halides with thiolates to form thioethers (also known as sulfides). This process resembles the Williamson to a tee. First, a strong base deprotonates the thiol (we use NaH here, but many other bases could also be used). Secondly, we add an alkyl halide, and an SN2 reaction results in formation of S-C and breakage of C-Br with inversion of stereochemistry. As mentioned above, note that if we were using an alkoxide, we’d have to worry about the E2 reaction competing with the SN2. With thiolates, it’s not an issue due to their decreased basicity. Since it comes up so much in exams, the intramolecular version is important to note. Note that we’re still forming C–S here and breaking a carbon-halide bond. Don’t forget that inversion occurs on the stereocenter on the secondary carbon! 5. Key Differences Between Alcohols And Thiols A. Oxidation In previous posts we saw that primary alcohols are oxidized to aldehydes and secondary alcohols are oxidized to ketones. This doesn’t work with thiols! Thiols aren’t oxidized to π bonds in the same way. The C–S π bond is actually quite weak due to poor orbital overlap. [note below] Instead, two different types of oxidation reactions occur with thiols. Thiols can be oxidized to disulfides through treatment with a mild oxidant like iodine (I2). A second oxidation pathway involves oxidation of sulfides to sulfoxides and sulfones through treatment with oxidants such as O3 (ozone) and peroxyacids such as m-chloroperoxybenzoic acid (mCPBA). Note that sulfur can exceed an octet of electrons whereas oxygen cannot. The oxidation of thiols to disulfides has important biological implications. The important amino acid cysteine contains a thiol group and disulfide bonds are responsible for the tertiary structures of proteins. They act like “hooks” that help to hold disparate parts of the peptide chain together. B. Hydrogen Bonding Isn’t As Significant With Thiols The electronegativity of sulfur is only 2.6 whereas hydrogen is 2.2. That means there isn’t much of a dipole in the S-H bond, and hydrogen bonding is not significant. Contrast H2O, with a boiling point of 100°C, with H2S and its boiling point of –60°C. Intermolecular forces are not very strong! C. Reactions With Acids Are Slightly Different In this series on alcohols and ethers we have seen countless examples of treating an alcohol or ether with H+ and converting it to its conjugate acid, making a better leaving group in the process. This isn’t as significant for thiols. The S-H bond is significantly weaker than the O-H bond [81 kcal/mol vs. 109 kcal/mol]. Secondly, due to the smaller dipole (electronegativity difference) of the S-H as opposed to O-H, there is less partial negative charge on sulfur and therefore less electrostatic attraction between S and the H of various acids. A better way of converting sulfur to a good leaving group is by treating it with Lewis acids such as Hg(OAc)2 . We haven’t really covered Hard-Soft Acid Base (HSAB) theory here on MOC (which is an advanced topic) but in order to further understand the differences in reactivity of O and S with various acids, the linked Wikipedia article is a useful primer.