Sciencemadness Discussion Board
Not logged in [Login ]
Go To Bottom

Printable Version  
Author: Subject: Vinconate identification
ZetekitoxinAB
Harmless
*




Posts: 19
Registered: 31-7-2019
Member Is Offline

Mood: Omberacetam

[*] posted on 31-7-2019 at 13:21
Vinconate identification


So I have recently rediscovered an old bottle of a substance, which I bought many years ago from a nootropics vendor, on ebay. It was advertised as vinpocetine and I remember it was very cheap, but he had good reviews so I decided to purchase it. At that time I had access to a chemistry lab and after taking it as vinpocetine (about 30-40 mg per day) for some time without any apparent side effects, I have decided to take a melting point. It turned out to be 119-121 °C, which was different from the literature value of real vinpocetine of 147-153 °C. Substance was pure according to TLC and I was able to send it, along some other chemicals, to an ESI-MS analysis which gave a Molecular weight of 296. Unfortunately I could not obtain a more advanced NMR spectra. Now I have moved away and dont have too many possibilities for quality analysis; I just have a few general reagents. I have reckoned after some web search that the slightly pale yellow crystalline substance was in fact vinconate - a synthetic chemical with purported nootropic effects but otherwise very obscure - likely substituted by the original trader for profit. The melting point and M do correspond to literature values of vinconate. I think that these circumstances strongly indicate that in fact it is vinconate, however I cant get over the fact that the substance is completely insoluble in 33% HCl, even after boiling. That is very strange in my opinion because of the supposed strongly basic tertiary N; even if synthetic it resembles a classical indole alkaloid. I mean even strychnine, which has a larger molecule and a similar basic N, form highly soluble salts with various acids. The substance is soluble in acetone giving a light yellow solution, which reacts with K dichromate in dilute sulfuric acid but not with iodine. Interestingly enough, I didnt find any reference to hydrochloride salts of vinconate or vinpocetine, instead they are sold as free bases. I would be really interested in possible explanations regarding the insolubility in conc. HCl and the lack of reaction with iodine, even though it has an isolated double C=C bound.
View user's profile View All Posts By User
Assured Fish
National Hazard
****




Posts: 304
Registered: 31-8-2015
Location: Noo Z Land
Member Is Offline

Mood: Misanthropic

[*] posted on 1-8-2019 at 22:27


Electrophilic addition proceeds via a carbocation and carbocations cannot form next to an electron withdrawing group (as ive had pointed out to me).
An ester like the one seen in Vinconate is an electron withdrawing group and thus its not possible for the alpha carbon next to it to undergo electrophilic addition with iodine or any other halogens or hydrogen halides.

As for you solubility issue, you mention boiling it in conc HCl, i would assume under these conditions you would hydrolyze the ester producing a carboxylic acid. As the equilibrium lies quite heavily in favor of the carboxylic acid.
Perhaps you should instead try to add a stoichiometric quantity of HCl and then filter off any precipitate, then weigh the precipitate and titrate the filtrate.

If you get nearly the same amount of solid back out of solution as you started with then the filtrate should contain very little or practically no HCl, this would indicate that the hydrochloride salt has formed.

If you instead manage to dissolve the solid with dilute acid then well you've answered your question.

It should also be noted that not all protonated amines are necessarily highly soluble in H2O, the shier organic bulk of the compound may hinder its solubility by having a rather non polar end.

And to answer a question you may also pose, not sure if your already aware.
The indole amine is not basic, this is due to that alkene next to it which prevents the lone pair of electrons on the nitrogen from being available to accept a proton.
There is only one amine available for protonation on Vinconate.




Sufficiently advanced science is indistinguishable from madness.
View user's profile View All Posts By User
Metacelsus
International Hazard
*****




Posts: 2318
Registered: 26-12-2012
Location: Cambridge, MA
Member Is Offline

Mood: Double, double, toil and trouble

[*] posted on 1-8-2019 at 22:39


Quote: Originally posted by Assured Fish  

An ester like the one seen in Vinconate is an electron withdrawing group and thus its not possible for the alpha carbon next to it to undergo electrophilic addition with iodine or any other halogens or hydrogen halides.


This is not true. The addition of halogens proceeds through an enol-like intermediate. See for example: https://en.wikipedia.org/wiki/Hell%E2%80%93Volhard%E2%80%93Z...

Edit: and for vinconate in particular, it wouldn't even be an alpha-halogenation, but rather addition of the iodine across the double bond. However, iodine is often quite slow to react with alkenes, especially (as you mentioned) when there's an electron-withdrawing group. I expect that bromine or chlorine would react, however.

[Edited on 2019-8-2 by Metacelsus]




As below, so above.
View user's profile View All Posts By User
Assured Fish
National Hazard
****




Posts: 304
Registered: 31-8-2015
Location: Noo Z Land
Member Is Offline

Mood: Misanthropic

[*] posted on 1-8-2019 at 23:35


The Hell–Volhard–Zelinsky halogenation is not the same reaction that was attempted by ZetekitoxinAB.
He used straight elemental iodine, thus he was attempting an electrophilic addition reaction.
https://en.wikipedia.org/wiki/Electrophilic_addition

The reaction you are describing is also initiated by enolation of the carbonyl, meaning the alpha carbon is left with a free electron without needing be become a carbocation for the neucleophile to then pick up.
Take a look at both mechanisms.





Sufficiently advanced science is indistinguishable from madness.
View user's profile View All Posts By User
ZetekitoxinAB
Harmless
*




Posts: 19
Registered: 31-7-2019
Member Is Offline

Mood: Omberacetam

[*] posted on 2-8-2019 at 13:37


Thank you for your insights ! I have tried again dissolving the substance in acid: 1 mmol (0.29 g) was suspended in 10 ml cold water and 0.2 g (slight excess) 33% HCl were added. No modification was observed whatsoever, the quantity of the suspension seems visually the same I will filter it tomorrow and weight it.

I have also tried the reaction with bromine, as suggested: in a 20 ml flask equal volumes of hydrogen peroxide 3% and sulfuric acid 37,5% were mixed giving about 15 ml solution. To this a small quantity (less than 0.5g) KBr was added, the solution turned almost instantly yellow with a strong bromine odor. 10 ml dichlormethane were added and the mixture was stirred, giving the organic layer an orange color. In a separate flask, rinsed and dried previously with acetone, 0,3 g test substance and 10 ml DCM were added giving a clear yellow solution.

I took the bromine containing DCM with a pipette and added it to the test DCM solution. Decoloration was instant but interestingly it also started slightly fuming (HBr). I would say that if the substance is vinconate (which is highly likely as both M and melting point correspond), there was an addition of bromine to the isolated double C=C bond, followed by an elimination reaction. I have attached a possible mechanism; I would presume that the bromonium intermediate would more likely react with another bromide giving the dibromo derivate which would eliminate HBr giving product 2.

Here is a synthesis published for vinconate: https://www.eosmedchem.com/article/83.html

Condensation of ethyltryptamine with VINC 006 is very nice, but the structure of the intermediates until VINC 006 is very dubious. Maybe the other carboxylate group is selectively cleaved, the other esther group reduced with NaBH4 to the primary alcohol which is oxidized with PCC to the aldehyde. The synthesis just seems overly complicated with many steps; I am sure VINC 006 could be made on an easier route.

In any case, I have started to think if the insolubility of the stuff has anything to do with the spatial structure of the molecule, where the lone electron pair interacts with the esther conjugated double bond, lowering basicity.

Also very likely vinconate is a racemate, as suggested by pubmed; but pubmed also gives reference to HCl salts. Maybe these salt could be obtained by combining the drug with dry HCl in a solvent, who knows...

1.png - 29kB
View user's profile View All Posts By User

  Go To Top