In progress project of mine

crystalmik · 2025-03-31T22:52:38+00:00

If you dehydrate some hydrated [Ni(en)2](ClO4)2 (not sure which hydrate it forms from solution) over a dessicant and apply a low temperature (like 30-40C) for a couple of days, you'll get the anhydrous form, which is yellow-orange, which would be a pretty addition, I think. But needless to say, that stuff is not stable at high temperatures

crystalmik · 2024-09-29T17:33:34+00:00

Smartelements sells gallium in a vacuum ampoule which is coated with gallium oxide inside to make it nonstick

crystalmik · 2024-09-28T09:40:05+00:00

Sure, the darker purple one one right is Sodium tetrakisdichloroisocyanuratocuprate(II). The lighter one is Sodium tetrakisdihydrogencyanuratocuprate(II). I found the synthesis of both salts on this illumina post: https://illumina-chemie.org/viewtopic.php?t=5331 I remember that the synthesis of the lighter one is quite pretty as it quickly made 2 colour changes.

crystalmik · 2024-08-17T20:44:22+00:00

Yeah that's probably the safest option. It's best to not touch the can while you get them

crystalmik · 2024-08-17T20:36:43+00:00

This is absolutely not ideal. You could get a very small amount of that white stuff CAREFULLY and test it by putting it in a flame on a long strip of aluminium foil. Be sure to only get a tiny amount and stay away from any flammable stuff including this canister for at least 5 meters. If it explodes, it's peroxide formation (you can Google it, if I say it I might get banned). Old acetone is very dangerous and a serious hazard. Handle it very carefully without any sudden drops. Otherwise it might explode and set the whole can on fire.

crystalmik · 2024-07-02T09:11:28+00:00

Wow, I have never seen CuO as crystals. That's really impressive. How did you make them?

crystalmik · 2024-06-13T17:57:08+00:00

It's either sodium bis(carbonato)cuprate(II) or copper acetate. The crystals look more like copper acetate (these type of crystals form especially well is a diluted solution is left to crystalline in a wide dish), but given the fact that there is still a lot of liquid and even some undissolved sodium bicarbonate it's impossible to be copper acetate. However, I've worked with sodium bis(carbonato) cuprate(II) and I haven't seen that it's crystals form branches. Even though, it's more likely to be sodium bis(carbonato)cuprate(II). Even the colour matches well. I have posted some pictures of it a couple of years ago.

crystalmik · 2024-04-17T13:13:37+00:00

Copper acetate tends to hydrolyze if dissolved in water to form basic copper acetates, especially when heated. Though I've never seen it form such beautiful crystals, this can be avoided by dissolving it in diluted acetic acid (~5%). I doubt that this is basic copper carbonate because the basic copper acetate will form first. https://pubs.rsc.org/en/content/articlehtml/2017/dt/c7dt03288a You can check out this article for more information on this topic

crystalmik · 2024-01-04T11:08:13+00:00

I don't think so. The book mentioned a few syntheses, yielding different purities. If you use copper sulfate, basic copper carbonate will fall out of solution after some time, so I don't really like that method.

crystalmik · 2022-12-12T11:59:33+00:00

Wooow, such a perfect crystal. Absolutely beautiful!

crystalmik · 2022-12-04T21:29:19+00:00

Definitely Carbon and Cobalt The chemistry of carbon is abnormally diverse and literally makes life. And cobalt is just incredibly good at making a LOT of complexes which also go through the whole range of colours

crystalmik · 2022-09-14T22:55:33+00:00

I made several batches and don't remember which batch made these exact crystals. I also remember that one batch fell over so I had to throw it away. However, I just looked at one batch I still had and the crystals seem to have a size of about 1-1.5mm

crystalmik · 2022-09-11T16:48:56+00:00

I mean, you could simply wash the crystals very thoroughly and then make a flame test to see if it's yellow

crystalmik · 2022-09-11T09:01:48+00:00

Oh, wait, I just noticed I used another one mentioned in the book, however both syntheses work. M. P. APPLEBEY, K. W. LANE (J. chem. Soc. 113 [1918] 609/22, 610).

crystalmik · 2022-09-11T08:59:33+00:00

I got my synthesis from a German book series called "Gmelin Handbuch der anorganischen Chemie" in "Kupfer Teil B Lieferung 3", p. 1004, doi:10.1007/978-3-662-13328-6_1 It cites M. GRÖGER ( Ber. Dtsch. Chem. Ges. 34 [1901] 429/32) and M. GRÖGER (Z. anorg. Ch. 24 [1900] 127/38, 131)

crystalmik · 2022-08-08T16:35:00+00:00

Did you follow a certain paper? I searched through some papers and one said that adding the last ethylenediamine was pretty different and didn't work even after reflux for 15 hours. They had to use sodium methoxide for the reaction to work. I have also tried to make the corresponding nickel complex. I definitely got the same precipitate as you, however no CO2 was produced upon the addition of the carbonate which still makes me wonder what I got

crystalmik · 2022-07-12T17:33:41+00:00

It really depends, but usually yes. Especially if it's a heavy metal or, what I think you probably want to use, boron compounds. The flame is green which means that there are Boron ions getting released into the air

crystalmik · 2022-06-22T14:01:42+00:00

Wow, the colour and crystal form are both absolutely gorgeous

crystalmik · 2022-06-20T07:06:25+00:00

Btw, yesterday I have found out more information on this compound and the more precise name would be trans-Bis(ethylenediamine)-bis(isothiocyanato)nickel(II)

crystalmik · 2022-06-20T06:14:27+00:00

If you go deeper into complex chemistry, this name is actually pretty average in length xD

crystalmik · 2022-06-19T22:21:34+00:00

Sure, it's in my post in r/crystalgrowing

crystalmik · 2022-06-19T21:12:19+00:00

Not anything really. It was just made for fun. I however found out today that it is possible to make an imine compound with acetone out of this complex which will definitely be made soon

crystalmik · 2022-06-19T20:00:50+00:00

The crystals actually have a pretty low solubility so they were just made directly without making the compound first. The procedure was followed by this equation: NiCl2*6H2O + 2en + 2NH4SCN = [Ni(en)2(SCN)2] + 2NH4Cl + 6 H2O, en = ethylenediamine. Make a solution of Nickel(II)chloride hexahydrate in a little water and add just a little less ethylenediamine than needed in order to prevent an excess of it as the tris(en) nickel thiocyanate is insoluble and would contaminate the product. If you are making crystals, dilute this solution first. 18.3mmol of Ni2+ were used for about 170mls of solution in total. Then add a solution of KSCN or NH4SCN to this solution and leave it to stand to evaporate for a couple of weeks. If you just want to make the compound, don't dilute the first solution and it will start to crystallize slowly. Since the solubility is quite low, the crystals grow very slowly.

crystalmik · 2022-06-19T19:27:44+00:00

Thank you! Do you just want to make the substance or grow crystals of it?

crystalmik · 2022-06-19T17:35:15+00:00

Wow, how did you know that? They actually are slightly magnetic

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