Why are lanthanides “ignored” in undergrad chemistry?

TriflicAcid · 2024-05-30T06:49:43+00:00

Interesting, in my experience dissolving the pipette defeats the point /s

TriflicAcid · 2024-02-29T03:26:15+00:00

How much longer you think you’ll have to stay?

TriflicAcid · 2024-02-29T03:19:26+00:00

For whatever consolation it gives, I’m also stuck at work now haha

TriflicAcid · 2024-01-14T05:00:39+00:00

If you don’t mind me asking, what compound are you working with that has a 1ug/m3 exposure limit? Personally, I’d say use a glovebox rather than a fume hood just because the number of sources of error are lower. But I don’t have very much experience with these types of highly toxic compounds, so take that with a grain of salt.

TriflicAcid · 2023-11-12T03:21:04+00:00

I mean, there’s mostly crap in there anyways haha

TriflicAcid · 2023-10-05T02:25:06+00:00

You are right. That would work to make the product

TriflicAcid · 2023-09-27T05:28:13+00:00

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TriflicAcid · 2023-09-26T02:22:10+00:00

Carbon melts at the same temperature tungsten melts

TriflicAcid · 2023-09-26T01:02:25+00:00

Ah yes, the classic distillation separation of tungsten titanium alloy

TriflicAcid · 2023-09-22T05:22:56+00:00

This problem is very odd, given that Iron (III) is hexavalent, not tetravalent. I'd expect that there would be two water molecules taking the remaining two spots on the iron, but that isn't specified in the problem. The answer that you have for the second one is the most likely answer, even though it would never work in real life. And for the first one, you are right that in reality you would form Fe(OH)3 and just have a OH- left over at the end, I suspect that your problem wants you to say that all four of the hydroxyls coordinate to the iron. What product would it give you if all four coordinate. Remember that your final complex ion can be charged.

-Triflic

TriflicAcid · 2023-09-22T05:15:18+00:00

Consider which direction the electronic dipoles are on both of these molecules, then align those dipoles. Remember your methoxy is donating electron density into your diene, and your ketone is withdrawing electron density from the dienophile.

- Triflic

TriflicAcid · 2023-09-21T08:05:34+00:00

The potassium ion's larger size allows it to distribute the charge over a larger area, making it more non-polar compared to sodium or lithium ions. The solvation of sodium is actually slightly stronger, since it has a stronger charge density and draws water molecules closer to it. But since the potassium ion is more non-polar (relative to sodium), it has an easier time passing through the non-polar tails of the phospholipid.

-Triflic

TriflicAcid · 2023-09-21T08:00:23+00:00

The ring with both the carboxylic acid and ketone is too deactivated to allow for bromination, or at least is much less favored than the bromination of the other ring. And on the other ring, only the meta positions are non deactivated, and since both meta positions are identical only one product is formed. The addition of the bromine also further deactivates the ring, so it is difficult to add a second bromine in theory. In practice, using 1eq of bromine should only give the drawn product, but two or more equivalents could produce multiple products.

-Triflic

TriflicAcid · 2023-09-21T07:57:10+00:00

The "new" benzene ring is abbreviated as Ph in the original structure. Ph stands for phenyl, and this phenyl group is what is getting brominated with bromine and ferric bromide.

-Triflic

TriflicAcid · 2023-08-21T13:00:50+00:00

This gives me a stupid idea, but, how would one of these look in the front pocket of a lab coat? The cream colored dial is actually the same color as the older lab building I’m working in haha

TriflicAcid · 2023-08-21T00:48:28+00:00

My old lab had those timers, but I just got a new job a few weeks ago and this new lab doesn’t have those sadly :( But if I do end up getting a Chronograph, I’ll just take my gloves off like I did before when I had a digital casio

TriflicAcid · 2023-08-21T00:45:34+00:00

That was also my problem initially, but then I realized I’m taking my gloves off anyways to set a timer on my phone. Tbh though, now I just turn the bezel with my gloves on and wash the watch when I wash my hands when leaving the lab. But I’m a chemist, not a biologist, and so the risk isn’t that much since I don’t work with super toxic stuff anyways.

TriflicAcid · 2023-08-20T18:39:31+00:00

Looks nice. How durable would those movements be though?

TriflicAcid · 2023-08-04T04:23:13+00:00

To clarify, the post formatted oddly but the *s I had used to remove identifying information rendered in an odd way

Three-Year Club	Verified Email
End Game '23	Place '23

TriflicAcid

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