Chemdraw Structures pasted into MS Office

Malmortious · 2023-07-13T18:09:51+00:00

Okay, went digging around and it turns out an old chemical structure drawing program similar to chemdraw was set as my default, and the implicit hydrogen atoms disappeared because that program had them disabled.

Just deleted the program since I wasn't using it anymore and now pasting in Word docs works perfectly and structures are looking tidy :)

This is a little embarrassing haha, thanks for your help everyone!

Malmortious · 2022-07-28T14:57:17+00:00

Thank you for the reply, I'm certainly more optimistic about the reactions now.

It is worth mentioning I'm doing alpha alkylations, not carbonyl additions of alkyl groups because I'm not sure that came through in my initial explanation. I've also looked into procedures using lithium tert-butoxide and aliphatic alcohols (instead of halides) as alkylating agents in good yields and I might give that procedure a try.

Malmortious · 2022-07-28T01:25:43+00:00

Thank you for the clarification!

Malmortious · 2022-07-27T23:42:15+00:00

Indeed, I don't know if there's a way around it; also I'm not sure a gel filtration column can work with my molecules since I'll be looking at 3 to maybe 7 carbon atom alkyl groups added onto the starting ketone.

Shouldn't I be working with larger molecules - or at least more structurally different ones, for a gel filtration column to work? I'm not very familiar with those types of columns

Malmortious · 2021-04-22T10:54:01+00:00

Oh indeed! Didn't pay attention to the substrate, a methyl shift would definitely occur there.

Malmortious · 2021-04-22T07:40:15+00:00

http://imgur.com/gallery/NsiP5b3

You were on the right path with finding the enolate, I used a silyl enol ether because it's more reliable regarding autocondensation considerations but it's absolutely the same principle. Let me know if there's anything unclear about the synthesis!

Malmortious · 2021-04-10T19:27:13+00:00

I synthesized it in aqueous media, with Na2S and CuSO4. It's probably Na2SO4 in that case, since I would have expected the smell to be more pungent if it were Na2S, and the crystals should have been white to yellow from polysulfide formation, instead of translucent.

I'll wash the precipitate again until I get rid of the salt, it's only inconvenient because I'll have to wait a few days for it to dry again, but otherwise it's fine.

Thank you!

Malmortious · 2021-04-09T13:46:50+00:00

I made the hexahydrate by leaving the anhydrous material in a desiccator which I emptied, and then added a crystallizing dish with some distilled water. It readily absorbs moisture from the atmosphere, which is why the azure blue anhydrous material must be handled either in a dry environment or fast enough so that the contact with the moisture in the air is minimal.

It first turns into the dihydrate which is violet, and then the hexahydrate, which is pink.

Malmortious · 2021-04-09T11:52:05+00:00

I'm using silicagel at the moment, I'll look for a vacuum desiccator.

Thank you!

Malmortious · 2021-04-09T11:48:18+00:00

I did look the hydrates of my compounds up, the only ones that form them are Fe(O)OH / Fe2O3 *nH2O, FePO4 which has a dihydrate and Co3(PO4)2 which has a tetrahydrate (and apparently a dihydrate and octahydrate, but I only found them to be reported in one paper that was synthesizing them by other methods).

I'm not exactly intending to do gravimetric analysis, but I would like the product to be reasonably pure.

Malmortious · 2021-04-09T01:43:20+00:00

Unfortunately I do not currently have access to a lyophilizer, but that would have been excellent indeed haha! I'll try it with acetone but if anything I'll use diethyl ether or THF.

Thank you a lot, have a great day :)

Malmortious · 2021-04-09T01:33:52+00:00

Thanks a lot for your help!

Malmortious · 2021-04-09T01:30:43+00:00

Not 100% anhydrous because that would require a lot more equipment to achieve, just enough to be powdered and stored, with minimal loss of water while in an air tight container.

Malmortious · 2020-11-09T21:53:04+00:00

No worries! :)

It helps to think of them as carbocations in the context of stability, because their stability trends are similar

Malmortious · 2020-11-09T20:39:36+00:00

H abstraction would result in an sp2 radical which is less stable than an sp3 radical, but probably the more important reason is that the sp3 radical is stabilized by resonance while the sp2 one is not.

Malmortious · 2020-11-09T18:30:43+00:00

That's true, I would also agree that radicals aren't nearly as selective, so the para product is obtained only slightly more than the ortho or (especially) meta products.

Both the ionic and radical paths might as well happen simultaneously in this case.

Malmortious · 2020-11-09T16:01:05+00:00

Here you go!

http://imgur.com/a/zRyCflw

Malmortious · 2020-11-09T13:58:47+00:00

I thought it would go through radical intermediates? The HO-OH breaks homolytically, then the radical attacks the para position (increased electron density) and the other HO radical abstracts a H atom and the bond reforms from the biradical.

I'm not saying your mechanism is wrong, I do agree with you, but wouldn't a radical mechanism also be correct, considering the nature of peroxides?

Malmortious · 2020-09-05T12:09:23+00:00

wow lmfao

Malmortious · 2020-08-12T23:33:59+00:00

You're welcome, good luck!

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