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Alcohols, Epoxides and Ethers

By James Ashenhurst

Protecting Groups For Alcohols

Last updated: September 13th, 2019 |

Alcohol Protecting Groups

Summary for today’s post on Protecting Groups for Alcohols:

summary

Table of Contents

  1. When Alcohols Get In The Way
  2. Protecting Groups Are Like “Painter’s Tape”
  3. What Would Be A Chemical Equivalent of “Painter’s Tape”?
  4. One Potential Solution: Ethers (Spoiler: They’re Not Great)
  5. A Better Way To Do It: Silyl Ethers
  6. A Successful Application of a Silyl Protecting Group Strategy
  7. Summary: Protecting Groups For Alcohols
  8. Notes

1. When Alcohols Get In the Way

As we’ve seen in previous posts in this series, alcohols are very versatile functional groups that participate in a variety of reactions. They can be deprotonated with base (making them good nucleophiles in substitution reactions), protonated (making them good leaving groups in substitution and elimination reactions), oxidized to aldehydes or ketones, or transformed into better leaving groups (alkyl halides, or alkyl tosylates) allowing for a host of substitution and elimination reactions.

All this this versatility comes with a drawback, however. Sometimes alcohol functional groups can  get in the way of other reactions we might like to do. Let me show you what I mean.

We’ve seen by now one of the most useful C-C bond forming reactions you learn in Org 1: nucleophilic substitution (SN2) of alkyl halides with acetylides (the conjugate base of acetylenes)

1-alkynes

Since alkynes are like a blank canvas, this reaction can set up the introduction of many different types of functional groups through addition reactions.

Now let’s modify our substrate a bit. We’ll attach a hydroxyl group (OH) to the end of the molecule. Now let’s see what happens.

2-alkyne alkylation fail

Look at what happened – we now formed a new O-CH3 bond instead of a C-C bond. What gives?

The answer, of course, is that our strong base NaNH2 deprotonated the strongest acid [OH, pKa of 16 versus acetylide C-H, pKa of 25] and the resulting alkoxide [R–O ] then attacked  CH3-I, resulting in a substitution reaction with displacement of iodide ion [note 1]

Here’s another example of the the principle at work. Here, we’d like to perform a substitution reaction of C-Br with C-C . So why does this reaction not lead to formation of a C-C bond?

3-cyclic ether formation

Same reason! Our acetylide ion is a strong base, and deprotonates the O-H group, which then participates in an SN2 reaction with the alkyl halide 4 bonds away (forming a five membered ring).

This is a textbook example of what we saw in our last post – an intramolecular SN2 reaction. [Why doesn’t it do substitution first? Acid-base reactions are fast, relative to substitution reactions].

So how could we have prevented this from occurring?

2. Protecting Groups Are Like Painter’s Tape

It’s reminiscent of a problem anyone who has painted a room would understand. Imagine you’re helping your cousin paint his room in a hideous shade of yellow-green so completely uncool to the untrained eye that only a hipster could appreciate it.  Then you come to one of those annoying wall outlets. You could paint over it of course.

A_power_outlet_painted_over
A wall color only a hipster could love. But now the wall outlet is useless. Fail

But now it’s useless if your cousin wants to plug in that 1965 Smith-Corona electric typewriter he found at a thrift store that he’s using to write his “novel”. Surely there’s a way to do this that doesn’t destroy our outlet. So what do you do?

Painter’s tape to the rescue!

Unknown
So what’s the chemical “equivalent” of painter’s tape?

Cover the outlet with painter’s tape, paint to your heart’s content, then remove the tape. THEN you can plug in the typewriter. Simple!

3. A Chemical Equivalent Of Painter’s Tape

Wouldn’t it be nice if we had a “chemical equivalent” of painter’s tape for alcohols. Something that could

  1. mask the reactivity of the OH group
  2. be inert to a large set of reaction conditions, and
  3. be easily and selectively removed to reveal the OH group once we’re done.

That would allow us to perform a synthesis of our desired molecule (second scheme above). Here I’m using “PG” to stand for “protective group”.

4-prot group scheme

Well, you might have guessed by now that enterprising chemists have developed a solution for this problem. It’s very clever, in fact.

4. One Potential Solution: Ethers

As we’ve discussed earlier, ethers are quite possibly the most boring functional group you can encounter. The only important reaction of ethers you cover in Org 1 is how to cleave them with very strong acid (e.g. with hydroiodic acid, HI). That’s it. Other than that, ethers are inert to pretty much any other reaction condition you can name.

For the chemical equivalent of “painter’s tape”, boring is good! It means that we can “protect” a hydroxyl group as an ether without worrying about it being affected by reactions we might like to do on the rest of the molecule (like addition of an acetylide to an alkyl halide, for example).

There’s just one problem: ethers require very harsh conditions in order to break (hydroiodic acid, HI). That’s like destroying the village in order to save it: such conditions will likely torch whatever other functional groups are on your molecule.

protect as ether

5. A Better Way To Do It: Silyl Ethers

Fortunately a very clever solution has been devised. Instead of making a typical ether (e.g. forming an O-C bond), we form a silyl ether (i.e. make an O-Si bond, not an O–C bond). It’s even easier to form than a “normal” ether, and shares  the property of being inert to many types of reaction conditions. In most introductory courses the most common silyl ether used is trimethylsilyl (TMS) although there are others [Generally, the bulkier the groups around silicon, the harder it is to cleave the O–Si bond]

silyl ethers

The main advantage of silyl ethers is that they’re easily cleavable. The Si-F bond is unusually strong – even stronger than Si-O.  Addition of a source of fluoride ion (F-)  will lead to cleavage of Si-O bonds without affecting the rest of the molecule.  A typical source of fluoride ion is the salt tetrabutylammonium fluoride (TBAF).

Are there other protecting groups for alcohols? You betcha. For more information, see Note 2.

6. A Successful Application of A Silyl Ether Protective Group Strategy

So let’s go back to our second example. How could we get this sequence to work? Let’s “protect” the free alcohol as a silyl ether (TMS) and follow along.

7-application

There you have it. All we needed to get our desired reaction to work was a way of masking the OH until we were done performing our surgery on the other half of the molecule.

7. Summary: Protecting Groups For Alcohols

This post barely scratches the surface of protecting groups for alcohols. Protecting groups are used for alcohols in a variety of different situations, far beyond the SN2 examples we covered here. For instance, when we talk about Grignard reagents, we’ll see that they can’t be formed in the presence of alcohols, so we have to protect them. Another example might be if you wanted to selectively oxidize one of two different alcohols in a molecule. We can add more posts on this topic as we go along.

You’ll notice that the vast majority of molecules you encounter in Org 1 and Org 2 have only one important functional group. It’s very rare that you’ll be given a substitution reaction, for example, that has two nucleophiles of comparable strength. Learning how to deal with molecules that have more than one key functional group is, in my opinion, where Org 2 ends and Org 3 begins.

It’s at that point that you need to learn understand the relative reactivity of different functional groups, their compatibility with different reagents, and also how to plan a synthesis such that only one key functional group will participate in the reaction.

Next Post – Thiols And Thioethers


Notes: THP and TBS

[note 1] Isn’t it possible that NaNH2 could have deprotonated a little bit of the alkyne? Sure! But remember that acid base reactions are equilibrium, and the alcohol is a far stronger acid (pKa ~16 ) than the alkyne (pka 25). Even if that acetylide formed, it would be quickly protonated by any spare alcohol R-OH swimming around, giving rise to the alkoxide. [back to article]

[note 2] Two more protecting groups that come up quite frequently are TBS (t-butyldimethylsilyl) and THP (tetrahydropyranyl)  ethers. TBS is installed the exact same way TMS is – by using TBSCl in the presence of a base like NEt3.

THP ethers are slightly different. They are installed by adding dihydropyran (an “enol ether”) in the presence of strong acid. The enol ether is protonated at carbon by the strong acid, resulting in an oxonium ion, which is then attacked by the alcohol to give the ether. This is actually a special type of ether where two OR groups are attached to the same carbon. It’s a masked ketone, which we refer to as an acetal. We talk about acetals here in this blog post. [back to article]

endnote

For even more protecting groups for alcohols,  see this handout by the group of Andy Myers at Harvard.  It’s phenomenal.

Comments

Comment section

25 thoughts on “Protecting Groups For Alcohols

  1. I am looking for ways to protect a hydroxyl group on the bone of a molecule that has a carboxyl group at the end that needs to remain active. Is it possible to mask an OH on the bone while to acid at the end of chain remains ” active ” ?

    1. Richard

      try to chlorinate the carboxyl group, then protect the hydroxyl group, and then add water to the molecule, producing your desired product. use a protecting agent that doesn’t react with aqueous hcl, which will be produced from the reaction of water with the cocl group on the end of your molecule.

    1. I wouldn’t say this a 100% restriction – there are likely exceptions – but if you’re being taught this, here’s at least two reasons.

      1. THP protection involves using strong acid, and strong acid might protonate the OH, resulting in loss of water to form a (stable) tertiary carbocation.

      2. Tertiary alcohols are quite sterically hindered, and the rate of attack of the tertiary alcohol at the electrophile produced by protonation of DHP might be slow.

      Hope this helps! James

  2. How does the addition/ removal of a protecting group affect stereochemistry? For example a hydroxyl OH group on a wedge or dash would it remain the same or be changed?

  3. I am trying to protect aryl OH with trimethyl silyl chloride using HMDS base. In the reaction it is showing different spot on TLC. But when we do column chromatography. It only gives starting back. Does silyl protection breaks during column chromatography?
    What is the solution? Please help me.

    1. TMS groups are extremely labile, especially on a phenol hydroxyl group. If you’re going to go with a silyl group, then pick TBS or something heavier.

  4. Hello,

    I had a few questions, as i’m learning organic synthesis,
    i understood that the silylmethylether can be attacted by R- if there is not a good leaving group such as (Br, Cl, OTs), is that correct because i didn’t read something about that here?

    Thank you very much!

    1. In theory primary alcohols are less sterically hindered than secondary alcohols. You would think that TMS might be selective for primary. It is, but to a very minor extent. In order to get very good selectivity for primary over secondary, you have to use a very bulky protecting group like TBDPSCl or TIPSCl or trityl chloride. But like I said you have to make the protecting group much bigger than TMS.

    1. Without knowing what your molecule looks like it’s hard to say. It would be easy to selectively protect the aromatic OH because it’s considerably more acidic, and once you form the alkoxide it will be far more nucleophilic. One idea would be to just protect both groups, and then selectively deprotect the aromatic OH afterwards.

    1. Deprotecting OMe is never fun. It depends on how stable the rest of your molecule is. I would employ basic conditions (RS- , polar aprotic solvent) since acidic conditions will likely ionize the CH2OH. Without knowing what the rest of the molecule looks like, it’s hard to say.

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