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Pretty Pictures (2)

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The Volatile Chemist - 9-1-2015 at 15:53

Wow. It's real pretty. Probably expensive, considering the nickel and ethylenediamine.

DraconicAcid - 9-1-2015 at 16:46

Not for me- I used some of the nickel waste generated by my students, and the college bought me my ethylenediamine.

UC235 - 9-1-2015 at 18:32

DraconicAcid: Perhaps this paper may be of use: DOI: 10.1039/dt9730001537 I suspect that bis-ethylenediamineoxolatonickel (II) may not exist as a simple complex, but there may be something to having a u-oxolato arrangement.

Tdep - 9-1-2015 at 19:29

May not appear to be the prettiest thing, but I was pretty impressed with myself.
Someone want to guess what the purple colour is?

Brain&Force - 9-1-2015 at 23:28

KMnO₄

Hegi - 10-1-2015 at 00:21

Quote: Originally posted by DraconicAcid

Crystals of tris(ethylenediamine)nickel(II) oxalate. I was trying to make a bis(en) complex with a coordinated oxalate, but refluxing was not taking off the third en ligand, nor was heating the solid to over 300 oC.

Hi, I really like these crystals but want to know more details about synthesis. I suppose you started with nickel oxalate (insoluble in water) and added ethylenediamine that formed soluble complex. Am I right?

How much of ethylediamine did you use? What would happen if you do this with molar ratio Ni:en 1:2? Did you try that?
____________________________________________________________________________________________________________________

If someone is interested in mineralogy, here is picture of beatiful vanadinite crystal, more pictures from this series you can find on my web -> Minerals series

<IMG SRC="http://chem.pieceofscience.com/wp-content/uploads/2015/01/vanadinite.jpg" ALT="some text" WIDTH=900 HEIGHT=600>

Tdep - 10-1-2015 at 04:37

Quote: Originally posted by Tdep

Someone want to guess what the purple colour is?

If I told you guys it was gold metal, would you believe me? Colloidal gold, sub micrometer particles resulting from the decomposition of 'gold fulminate'.
Pretty :3

DraconicAcid - 10-1-2015 at 17:45

Quote: Originally posted by Hegi

I seem to recall trying that, but finding that the nickel oxalate simply wouldn't dissolve until I added excess en, despite heating the aqueous suspension.

cyanureeves - 10-1-2015 at 18:34

Tdep i was just about to say it was a gold something because i have seen even gold plating turn reddish and rainbow even.today i was melting a sterling candle stick holder and there was some blackened charred stuff in my crucible. i thought the black stuff was burnt borax but when i poured out the sterling into cold water i noticed red/rainbow coloring.i scooped out the silver shot and all the silver is now gold colored and i cant even see silver.the only thing i melted on that crucible was a pair of gold filled eyeglass frames and i thought i plucked it all out.i had no idea that sterling cement filled candle stick holders had a very thin foil of silver on the outside,hell not much thicker than aluminum foil.i thought i hit pay dirt at first when i found that sterling.

Brain&Force - 10-1-2015 at 21:45

Quote: Originally posted by Tdep

Someone want to guess what the purple colour is?

If I told you guys it was gold metal, would you believe me? Colloidal gold, sub micrometer particles resulting from the decomposition of 'gold fulminate'.
Pretty :3

When can we expect a video?

Definitely post it here. Gold-based explosives are a REALLY exotic thing to see.

Molecular Manipulations - 10-1-2015 at 23:49

Wow Hegi, those are some beautiful crystals. I also have some vanadinite ore, but the crystals are smaller and less defined.
I'll post a picture when I can.

Tdep - 11-1-2015 at 02:36

Quote: Originally posted by Brain&Force

When can we expect a video?

Possibly Wednesday? It's a real shame gold is so expensive and rare, this compound is great fun to play with. And the metal is so pretty to look at...

Also, god I love good mineral shots. I have some vanadium minerals too, no where near as beautiful as the previous photo though!

Hegi - 11-1-2015 at 02:44

Quote: Originally posted by Molecular Manipulations

Wow Hegi, those are some beautiful crystals. I also have some vanadinite ore, but the crystals are smaller and less defined.
I'll post a picture when I can.

Thanks, this piece did not cost a lot, about 30 dollars. The most expensive is mimetite. I´ll be waiting for your picture.

The Volatile Chemist - 11-1-2015 at 11:45

What's you-all's favorite minerals? At the moment, mine are beryl, tourmaline, and apophylite, the middle being my fav.
I'll post some apophylite crystals I own, sometime.

Hegi - 11-1-2015 at 11:55

Quote: Originally posted by The Volatile Chemist

What's you-all's favorite minerals? At the moment, mine are beryl, tourmaline, and apophylite, the middle being my fav.
I'll post some apophylite crystals I own, sometime.

I´ve got many minerals in my collection. I´m collecting sulfide minerals and also carbonates. But I have many other pieces. My favourite is tiny octahedral spinel. Here´s a photo.

Molecular Manipulations - 11-1-2015 at 18:41

Quote: Originally posted by Hegi

I´ll be waiting for your picture.

Well I hope you didn't think that I was a photographer

Literally taken on my GoPro...
While I'm at it I might as well post some other photo's too.

Here's the vanadinite:

See if you guys can guess the rest.

[Edited on 12-1-2015 by Molecular Manipulations]

Brain&Force - 11-1-2015 at 19:23

Man, I really wish I could get a GoPro - I want to shoot videos, and that would be convenient!

Do the below compounds contain vanadium?

[Edited on 12.1.2015 by Brain&Force]

Molecular Manipulations - 11-1-2015 at 19:43

Yeah, it's pretty nice, I got it for Christmas. Not great quality but it works. I've also started shooting for a YT channel I'm about to start.
None of the other pictures contain vanadium.

Brain&Force - 11-1-2015 at 20:19

Say, do you want to join Rador Labs (links in sig)? We all want to shoot some videos for our channel and it would be great if you could join us.

Mailinmypocket - 12-1-2015 at 16:44

The procedure behind the flask is what the target compound is. The picture was taken after removing ethanol from the reaction. The product can be used as a pH indicator, colorless below ~pH 6 and yellowish above that and becoming a faded yellow above pH 11 (to be tested)

The Volatile Chemist - 12-1-2015 at 17:06

Mercury compound and mercury? Say, HgS ? Looks a bit too pink for HgS, though...

The Volatile Chemist - 12-1-2015 at 17:08

Quote: Originally posted by Mailinmypocket

The procedure behind the flask is what the target compound is. The picture was taken after removing ethanol from the reaction. The product can be used as a pH indicator, colorless below ~pH 6 and yellowish above that and becoming a faded yellow above pH 11 (to be tested)

That's crazy! (Sorry for the double post. I have a hard time reading it, what is it, and what'd you use to make it?

Mailinmypocket - 12-1-2015 at 18:19

It it putatively 2-methoxy-4-((phenylimino)methyl) phenol... I have still not isolated the solid and done a m.p. yet. The procedure is found in this document, all you need is vanillin, aniline and ethanol.

http://download.portalgaruda.org/article.php?article=170688&...

Hawkguy - 12-1-2015 at 18:19

Molecular Manipulations - 12-1-2015 at 18:42

Quote: Originally posted by The Volatile Chemist

Mercury compound and mercury? Say, HgS ? Looks a bit too pink for HgS, though...

Mercury is right. Nobody will ever guess the pink crystal because it's a mineral not a pure substance, it's fluorite - calcium fluoride.

Brain&Force - 12-1-2015 at 21:14

That is the most beautiful sample of fluorite I've ever seen.

Jylliana - 13-1-2015 at 02:41

Sulfur heated with a torch and then dropped in cold water. According to the research I did, it should be 'plastic sulfur' or χ-sulfur.

The only strange thing is, that this is very dark in color and rubbery to the touch(feels like a gummy bear), while plastic sulfur should be very hard and pale yellow.

Unfortunately it's not stable. It will convert back to α-sulfur over time.

Any information about this is welcome.

j_sum1 - 13-1-2015 at 04:37

My experience with heating sulfur and quenching is that it is possible to get anything from near black to grey to bright yellow. Consistency can be gooey, tacky, like putty, brittle. As it decomposes back to S8 it becomes less plastic and often floury.
It depends on its heating history -- what temperature, how long and how quick the quench was. I think it affects the chain length. Sulfur has a remarkable number of allotropes, nit many of them particularly stable. It would not surprise me if it was discovered that plastic sulfur contained a good mix of these: affecting its properties. Add to that the possibility of some oxidation on heating and the common presence of impurities and you have another dimension of variability.

Your sample is quite interesting in a sci-fi-movie-prop kind of way.

Molecular Manipulations - 13-1-2015 at 08:22

Quote: Originally posted by Brain&Force

That is the most beautiful sample of fluorite I've ever seen.

Thanks, I want to know why it's pink, but I don't want to destroy the sample - the chemist's dilemma!
Jylliana, I've noticed the black color of plastic sulfur only when using the 90% "graden grade" stuff, which contains 10% bentonite clay. I think the black color comes from the clay or it's reaction with molten sulfur. When using 99% sulfur I get a grey-brown color if heated quickly and a lighter yellow-red color if heated slowly over a long period of time.
What grade of sulfur did you use?

Jylliana - 16-1-2015 at 09:23

Crystallized Gallium

blargish - 16-1-2015 at 14:20

On the mineral trend, here is my own sample of fluorite (it's unfortunately in massive form) as well as one of my favs: a sample of labradorite (a plagioclase feldspar) showing its characteristic "labradorescence"

Zombie - 16-1-2015 at 14:50

Quote: Originally posted by wish i had a kraken!!!

It is not termite :-)

[Edited on 27-7-2014 by wish i had a kraken!!!]

I just read thru this whole thread, and I am impressed to the bone.
Some of the most beautiful and fascinating things I have ever seen.
Kudos to Everyone for their work, and even more so for sharing it all.

The post that stuck out... I know the silliest one of all.
It reminded me of this stunt performed yearly. Go figure!

[Edited on 16-1-2015 by Zombie]

sasan - 17-1-2015 at 07:06

Theses are the pictures of copper ores in IRAN.cotains some minerals of this elements such as covellite,chalkopyrite,bornite and some other.very beautiful and amazing colors.photographed in AM university in tehran/iran.

[Edited on 17-1-2015 by sasan]

Screenshot_2015-01-17-18-25-17.jpg - 1MB

Screenshot_2015-01-17-18-24-35.jpg - 819kB

Hegi - 17-1-2015 at 12:10

What about these fluorite crystals?

Sodium

Loptr - 19-1-2015 at 19:01

I heated sodium to its melting point while stirring, and once it broke into tiny globules, I cut the heat and let it cool. Next time I will cut both stirring and heat, which will hopefully result in tiny spherical sodium.

This form is very reactive, though! Exposure to air instantly tarnishes it.

[Edited on 20-1-2015 by Loptr]

The Volatile Chemist - 20-1-2015 at 09:11

That's gorgeous! A nice, collect-able form, minus the stirbar (or with, we all have our preferences....)

Loptr - 20-1-2015 at 09:33

Quote: Originally posted by The Volatile Chemist

That's gorgeous! A nice, collect-able form, minus the stirbar (or with, we all have our preferences....)

The stir-bar didn't join with the sodium. I was on my way to bed and decided to snap a picture before it had a chance to oxidize by the morning, so no clean up was done, etc.

I am assuming any water within the mineral oil I was using either distilled out of the mixture or was dried by the sodium, because when I got up this morning it was still as bright and shiny.

The Volatile Chemist - 20-1-2015 at 15:54

Nice! I thought that was your stirbar coated in sodium

Mailinmypocket - 21-1-2015 at 07:09

Crude sulfanilic acid has a pretty purple iridescence to it:

The Volatile Chemist - 21-1-2015 at 12:46

Huh. Procedure, please?

Mailinmypocket - 21-1-2015 at 12:53

Sulfonation of aniline. Simply heat aniline and concentrated sulfuric acid at 180-190 in an oil bath for 4-5 hours. Pouring the finished reaction into cold water precipitates it out and it can be recrystallized and washed. The procedure I used is from Norris Experimental Organic Chemistry. The pages are here:

http://www.books-about-california.com/Pages/Experimental_Org...

Firmware21 - 22-1-2015 at 05:15

These beauties crystallized out from a "homemade" FeCl3 etchant solution. Since I didn't want to use H2O2 to oxidize it (I like my solutions concentrated), FeCl2 was still present, even after 7 month of "oxidation".

bismuthate - 23-1-2015 at 08:27

F**K it I have no idea how to work the photos on this forum.
Here have a link. It's a bismuth thiocyanate complex.
http://imgur.com/dTrjWSk

Mailinmypocket - 23-1-2015 at 08:38

Quote: Originally posted by bismuthate

F**K it I have no idea how to work the photos on this forum.
Here have a link. It's a bismuth thiocyanate complex.

http://imgur.com/dTrjWSk

I hope you don't mind that I tried to see if it was a problem with the picture dimensions/file size and uploaded it quoted for you. Not sure why it seems to work for me. Are you clicking "upload file"? Does it give an error messages?

bismuthate - 23-1-2015 at 08:50

I was just inserting the link it gives for forums and I couldn't resize and it was giant.
Thank's for quoting it so that it's visible though.

Mailinmypocket - 23-1-2015 at 08:59

Ah righto. The roundabout way I use sometimes for that problem is to upload it to whatever image site you like, use that site to resize the photo, save the photo in its reformatted size to my computer. Then upload as attachment to sciencemadness. Obviously there are programs to do this instead of image hosting sites but this way works fine.

The Volatile Chemist - 23-1-2015 at 13:23

Both the bismuth complex and iron complexes are great! What was your bismuth source?
Looks like an iron thiocyanate complex, but not as deep...

[Edited on 1-23-2015 by The Volatile Chemist]

bismuthate - 23-1-2015 at 14:24

It was bismuth nitrate.

Zephyr - 23-1-2015 at 16:13

Bismuthate how did you make your bismuth complex?

Here is some barium chloride crystals and the disgusting iron impurities separated from it, iodine crystals, and some lead iodide.

[Edited on 1-24-2015 by Pinkhippo11]

bismuthate - 23-1-2015 at 19:02

I just mixed some potassium thiocyanate and bismuth nitrate solutions and crystallized. It's not pure of course. I'm working on recrystalizing it.
How did you make an iodine crystal that big?

kjpmi - 24-1-2015 at 17:17

Quote: Originally posted by Firmware21

These beauties crystallized out from a "homemade" FeCl3 etchant solution. Since I didn't want to use H2O2 to oxidize it (I like my solutions concentrated), FeCl2 was still present, even after 7 month of "oxidation".

Those crystals look so cool. I love that green color.

Firmware21 - 25-1-2015 at 11:10

Well, they already started to convert to FeCl3. Now they look a bit darker.
Too bad I can't keep them like this forever

blargish - 30-1-2015 at 10:04

Quote: Originally posted by Firmware21

Well, they already started to convert to FeCl3. Now they look a bit darker.
Too bad I can't keep them like this forever

I guess you could keep them in a container flushed with nitrogen or carbon dioxide to prevent aerial oxidation. That would keep the nice green colour

Zephyr - 2-2-2015 at 18:34

Bismuthate, the iodine crystal was created by melting the iodine under sulfuric acid. The bismuth nitrate and potassium thiocyanate formed this odd yellow solution with a white precipitate when mixed;

[Edited on 2-3-2015 by Pinkhippo11]

j_sum1 - 2-2-2015 at 18:37

Wow! That is stunning!

Brain&Force - 2-2-2015 at 18:39

What are those crystals?

Zephyr - 2-2-2015 at 18:41

Potassium permanganate! Cooled over eight hours.

Shivachemist - 2-2-2015 at 20:26

Calcium acetate: I made some attempts to prepare Aluminium acetate for making water proof cloth. When I was doing so, I had left some calcium acetate solution in a beaker (prepared by mixing calcium hydroxide and concentrated acetic acid) for later use. But, I completely forgot about it. After a couple of weeks, wow! calcium acetate crystallized out beautifully and you can see that in the pic

Ammonium tetraborate: I've crystallized this compound for my video posted a couple of days back in youtube

Hawkguy - 2-2-2015 at 20:48

Thats amazing, and not only for the beauty, it looks like you have the cleanest lab around to grow that accidentally without dust contamination or whatnot.

quantumcorespacealchemyst - 2-2-2015 at 22:54

Quote: Originally posted by Brain&Force

Man, I really wish I could get a GoPro - I want to shoot videos, and that would be convenient!

Do the below compounds contain vanadium?

[Edited on 12.1.2015 by Brain&Force]

I am thinking Google glass may be perfect for filming reactions while keeping the operator uninhibited.

And

Realgar: Paloma Mine, Castrovirreyna Province, Huancavelica Department, Peru

Size: 3.4 x 3.3 x 2.8 cm (miniature)

Weight: 55grams

Realgar on galena/with galena and orpiment coating

http://stores.ebay.com/jlminerals/

[Edited on 3-2-2015 by quantumcorespacealchemyst]

quantumcorespacealchemyst - 2-2-2015 at 23:26

[rquote]
The bismuth nitrate and potassium thiocyanate formed this odd yellow solution with a white precipitate when mixed;
[/rquote]

How does it turn red? Is it mixed longer and/or heated?

Also, Pinkhippo11, how did you cool the KMnO4 over 8 hours? Was it in a kiln type of environment?

Also, has anyone read/seen about the salts made from BiI3 and halide salts? Bismuth(III) iodide forms iodobismuth(III) anions when heated with halide donors:[10]
2 NaI + BiI3 → Na2[BiI5]
http://en.wikipedia.org/wiki/Bismuth(III)_iodide
(10. ^ Norman, Nicholas C. (1998), Chemistry of Arsenic, Antimony and Bismuth, Springer, pp. 168–70, ISBN 0-7514-0389-X, retrieved 2008-06-19)

The Volatile Chemist - 3-2-2015 at 14:33

Put it in a tub of boiling water, let it sit, covered, and wrapped in towels. That's what I'd do....

fluorescence - 4-2-2015 at 13:49

Dissolved some natural Arsenic ore in Aqua Regia.

The Volatile Chemist - 4-2-2015 at 15:46

Great pic! What form of ore, and from where?

quantumcorespacealchemyst - 4-2-2015 at 16:13

That is awesome

quantumcorespacealchemyst - 4-2-2015 at 17:11

I found this after drinking the coffee that was in my window at least a few days. It was freezing and thawing and was partly thawed when I took it out to drink. I think I did the best I could to get the crystals pictures and it still doesn't look the way I see it. The camera only is 1 MP.

also there are these
it looks different in front of the computer compared to a light bulb. it is not a pure compound but has insoluble brown powder in it
More here> http://www.sciencemadness.org/talk/viewthread.php?tid=61446#...

[Edited on 5-2-2015 by quantumcorespacealchemyst]

[Edited on 5-2-2015 by quantumcorespacealchemyst]

[Edited on 5-2-2015 by quantumcorespacealchemyst]

Hawkguy - 4-2-2015 at 17:46

Liquid Chlorine

fluorescence - 5-2-2015 at 03:11

@The Volatile Chemist :

Not really sure. A friend sent it with some other chemicals. I didn't really know what to do with it so I thought since
I only have Sodium Arsenite and Sodium Biarsenate at home some more Arsenic Compounds would be good for the
collection. Actually tried to make Arsenic Acid from it but it somehow didn't turn out that well.

I though of dissolving it in Aqua Regia to gain like a crude form of Arsenic acid, than neutralizing it and hopefully precipitating it with Barium ( I think Barium Arsenate should be quite insoluble ). Filtering that of and mixing it again
with Sulfuric Acid to get insoluble Bariumsulfate and a clear Phase of Arsenic Acid. But while the reaction above white crystals fell out. I washed them but I'm not really sure what they are.

I've read that if you prepare Arsenic acid from the Oxide you will get crystalls of the Acid Hydrate so since the products for the Metal + acid and the oxide + acid are pretty much the same the crystalls could indeed be Arsenic Acid. But I can't find much in literature.

I've made a second attempt now with just Nitric Acid and we'll see whether there are crystalls, too or not.

The Ore is pretty clean, some dark grey stones with shining parts in it. At some points there are like yellow impurities but I've sorted them out. It should be somewhere from Germany (but I can ask for that).

EDIT:

Some Arsenic in conc. Nitric acid at room temperature and on the right close to it's boiling point. On the right is a indicator paper. That happens if you hold a dry indicator paper into Nitrous Gases. It get's pink and then white. Saw that at the university where I found dozens of pink strips after people worked with Aqua Regia. So I tested that out some time ago and found that they get that weird color when treated with Nitrous Gases. I guess the dye is destroyed in the reaction thus forming a color that is usually not found on the universal indicator.

[Edited on 5-2-2015 by fluorescence]

The Volatile Chemist - 6-2-2015 at 09:13

Nice job! I like the fume pictures.
The liquid chloride is impressive.

quantumcorespacealchemyst - 6-2-2015 at 12:22

Yea.

what do you think about putting a calculated amount of liquid chlorine in a super cold bomb flask?

(accounting for PTFE expansion/contraction, wiggling/turning/loosening on warming) I saw a corning glass article on the practice of acclimating PTFE joints to/from cold.

[Edited on 6-2-2015 by quantumcorespacealchemyst]

[Edited on 6-2-2015 by quantumcorespacealchemyst]

I guess not much would be containable due to gas pressure; nonetheless, it seems like a good, highly controllable source of Cl2 gas.

[Edited on 7-2-2015 by quantumcorespacealchemyst]

Silver Tree

Volanschemia - 7-2-2015 at 17:35

I'm not sure if pictures of this have been posted before but here's some I took of my Silver Tree.
The first one is when the crystals are still big enough to reflect light and in the second one the crystals are smaller and absorb light more, giving it a grey colour. Reminds me of a big storm cloud or something!

[Edited on 8-2-2015 by TheAustralianScientist]

quantumcorespacealchemyst - 9-2-2015 at 04:43

That's really cool

Molecular Manipulations - 9-2-2015 at 08:34

Nice TheAustralianScientist, looks to me like the ash and dust in a nuclear mushroom cloud! When I do the silver tree I use a less concentrated solution of silver nitrate (about 0.1 molar) and it makes larger crystals which reflect more light.
How'd you condense the chlorine Hawkguy? I've used dry ice in acetone with some success for that in the past. Don't use styrofoam Hehe.

[Edited on 9-2-2015 by Molecular Manipulations]

Volanschemia - 10-2-2015 at 18:00

Quote: Originally posted by Molecular Manipulations

Nice TheAustralianScientist, looks to me like the ash and dust in a nuclear mushroom cloud! When I do the silver tree I use a less concentrated solution of silver nitrate (about 0.1 molar) and it makes larger crystals which reflect more light.
How'd you condense the chlorine Hawkguy? I've used dry ice in acetone with some success for that in the past. Don't use styrofoam Hehe.

[Edited on 9-2-2015 by Molecular Manipulations]

Thanks! I thought it looked really nice. I used 1.6g of Silver(I) Nitrate in 50mL of distilled water which equals a 0.19M solution. I might try it again with a more dilute solution. I got a really good recovery of silver crystals, 0.995g, which I was really pleased with.

Hawkguy - 10-2-2015 at 19:41

Quote: Originally posted by quantumcorespacealchemyst

Yea.

what do you think about putting a calculated amount of liquid chlorine in a super cold bomb flask?

(accounting for PTFE expansion/contraction, wiggling/turning/loosening on warming) I saw a corning glass article on the practice of acclimating PTFE joints to/from cold.

[Edited on 6-2-2015 by quantumcorespacealchemyst]

[Edited on 6-2-2015 by quantumcorespacealchemyst]

I guess not much would be containable due to gas pressure; nonetheless, it seems like a good, highly controllable source of Cl2 gas.

[Edited on 7-2-2015 by quantumcorespacealchemyst]

I don't wanna store the stuff though, because of escapes, and Chlorinated Organics are often carcinogenic, apparently...

Hawkguy - 10-2-2015 at 19:43

Quote: Originally posted by Molecular Manipulations

I used the dry ice freezing mixture too, but I'm trying to adapt it to used propane or butane evaporation... Much more OTC..

quantumcorespacealchemyst - 11-2-2015 at 21:34

Does anyone know what the possible reactions going on in the arsenic ore dissolution are?
The Realgar As4s4 and Orpiment As2S3 seem to be the main parts of some ore, where AsO3 and even elemental Arsenic seem to be in other types.

I don't know about the pentoxide or supposed Arsenic dioxide, which Wikipedia says is a mixed valent compound of AS(iii) and AS(v).

Does HCl displace Sulphur? Can NO3 make nitrates? There doesn't seem to be much Arsenic chemistry here. I may have not found it yet. Nonetheless, the chemical working of Arsenic seems to be tough to find out about (besides analysis, Marsh test stuff).

woelen - 12-2-2015 at 04:31

There is a good reason for the low abundance of arsenic chemistry on this site. It is way too toxic to do anything more than the most basic things. Heating it, bubbling gas through arsenic-containing solutions, reducing it with strong reductors, they all are a no-go if you value your health. It is surprising that arsenic-containing chemicals can be obtained so easily (especially As4S4 and As2S3), but to a lesser extent also FeSAs.

Sulaiman - 12-2-2015 at 04:37

I made a video of tin crystals growing by electrolysis in real time,
I think it's pretty. https://www.youtube.com/watch?v=G1sq4hnrBgM
(I don't know how to copy it here)
After the video I just put the tin and electrolyte (HCl + SnCl2) in a beaker,
and stirred it to remake tin chloride ready for another run.

If not for the HCl it could make a nice re-usable toy.

[Edited on 12-2-2015 by Sulaiman]

morganbw - 12-2-2015 at 04:57

@Sulaiman
I liked that

quantumcorespacealchemyst - 12-2-2015 at 06:06

arsenic is only dangerous if the reactions and behaviour are unknown. chemistry at it's core deals with dangerous materials in a safe manner. lack of information is the real danger.

fluorescence - 12-2-2015 at 07:28

The question is what you want to do with it. I only made the Arsenic Acid because I always wanted to have that particular compound. There is a quite large variety of Arsenic Salts but I don't really know what to do with them. Your Sulfides belong to the few one that are even colored. So I'd rather keep them as they are...
I have some Sodium Arsenide and Arsenate but they just stand around as white powders and don't have any use for me. I worked with Arsenic at the university last semester where I had to find out whether it was in a given sample. So I did some testing with the Arsenic Compounds we had in our university lab. There are some interesting reactions with arsenic. There was a really efficient way to reduce it to the metal with the help of KCN that ended with a black sponge of metal in my testtube - I even managed to get an Arsenic mirror on the walls but that's pretty much all of it.

And I also have some bad memories on arsenic. A collegue gave me some testtubes to clean since I was cleaning mine and didn't tell me what was in it. Unfortunately it was conc. Sulphuric Acid with Arsenic(III)oxide in it. If he told me that there was acid in it I wouldn't have added water to it. The next thing I felt was boiling arsenic contaminated sulphuric acid running over my hand immediately leaving a red trail where it went.

Took like 3 weeks to fully heal. So I'm not really a fan of Aernic either.
Not because of it's toxicity but rather because of it's uses.

To add something to the thread: Here is some Cobalt(II)chloride (waterfree) dissolved in some absolute Ethanol. If you don't have water
in it you get a blue solution in stead of a pink one. Tried it with Nickel(II)chloride, too. This will leave you with a yellow solution but it's not that good.

quantumcorespacealchemyst - 12-2-2015 at 12:18

i worked out a theoretical equation of the action of nitric and hydrochloric acid on As4S4, realgar.

4HNO3 + As4S4 ---> 4HAsO + 4S + 4NO2
4HNO3 + As4S4 + 8HCl ---> 4HAsCl2 + 4S + 4NO2 + 4H2O
i don't know if that is likely to occur, the second equation mostly.
i guessed that Cl- is more attracted to the molecule (if it exists), being more basic than O-2, which seems to be more acidic and displaced easier.

i have seen a picture http://www.mindat.org/min-2328.html of a sulphur/selenium containing mineral, looks amazing.
and take a look at this (if you will), it looks like fiber optic cables http://www.mindat.org/min-4232.html.

edit: wrong link,fixed, also it doesn't seem HAsO and HAsCl2 are likely to form/exist.

Yvonite Cu(HAsO4) · 2H2O
http://www.mindat.org/min-7382.html

[Edited on 12-2-2015 by quantumcorespacealchemyst]

quantumcorespacealchemyst - 12-2-2015 at 13:06

www.mindat.org/min-4195.html
http://www.mindat.org/min-39333.html
http://www.mindat.org/min-3503.html
http://www.mindat.org/min-240.html

[Edited on 12-2-2015 by quantumcorespacealchemyst]

j_sum1 - 12-2-2015 at 17:06

Quote: Originally posted by Sulaiman

I made a video of tin crystals growing by electrolysis in real time,
I think it's pretty. https://www.youtube.com/watch?v=G1sq4hnrBgM
(I don't know how to copy it here)
After the video I just put the tin and electrolyte (HCl + SnCl2) in a beaker,
and stirred it to remake tin chloride ready for another run.

If not for the HCl it could make a nice re-usable toy.

[Edited on 12-2-2015 by Sulaiman]

That is AWESOME.
I now know how I am going to show tin in my element display.
J.

mayko - 12-2-2015 at 17:07

I recently made some iodine monochloride; here's some pictures from that ... adventure ... as the trichloride began to form and solidify. The last one is ~800x taken through the glass with a USB microscope. I kept thinking how the flask looked like a gas giant like Jupiter:

alexleyenda - 12-2-2015 at 21:59

[Et4N]3[Fe(SCN)6] complex I made today. The cristals are a very very dark green and when you crush them they become Red, which is a very rare thing. It has something to do with a difference in energy depending on the size of the cristals, I didn't look in details for the explaination, i,m very tired from my day. Anyway, enjoy :p

10966773_525631770912900_655408890_n.jpg - 89kB

10962246_525631774246233_591652556_n.jpg - 101kB

fluorescence - 13-2-2015 at 07:21

Wow that looks interesting. I didn't know that property even existed.

Edit: Just tried that compound suggested in this thread
http://www.sciencemadness.org/talk/viewthread.php?tid=48176

After 5 min of gently heating and then letting it cool for about 10 min. I got that. Pretty satisfying how easy that went and how good the result looks.

All credits go to woelen who presented that compound first !

[Edited on 13-2-2015 by fluorescence]

The Volatile Chemist - 13-2-2015 at 09:12

Nice pictures! Could the crystals of the "[Et4N]3[Fe(SCN)6]" complex you made have oxidized? does the crushed powder show any signs of change? If not, that's amazing!

alexleyenda - 13-2-2015 at 15:06

The color change happens at the second you crush the crystals and no sign of oxidation is present. I'm gonna try to find an explanation.
Edit: I've done some research and nothing, I've only seen the compound and this property listed in an article from 2013, but no explanation. It seems it's a quite rare phenomenon and it hasn't been investigated much yet.

[Edited on 13-2-2015 by alexleyenda]

Zombie - 13-2-2015 at 16:50

I'm just going to make a simplified guess, and say it is a property of light diffraction in the crystalline structure vs the crushed state'.

Similar to lead crystal vs crushed.

With no oxidation or further interaction of compounds I don't see any other viable explanation.

[Edited on 14-2-2015 by Zombie]

woelen - 15-2-2015 at 08:36

I have been playing around with my PBr3 which I made a few years ago, see http://www.sciencemadness.org/talk/viewthread.php?tid=17228#... .
I have made nice collector's samples of some very rare compounds:

PBr3: http://woelen.homescience.net/science/chem/compounds/phospho...
PBr5: http://woelen.homescience.net/science/chem/compounds/phospho...
PBr7: http://woelen.homescience.net/science/chem/compounds/phospho...

Some time ago, I also added 200 mg of C60 (fullerene) to my element collection. I put some CS2 and C60 in an ampoule and keep this as another sample for my collection of compounds:

C60: http://woelen.homescience.net/science/chem/compounds/carbon....

Texium - 15-2-2015 at 10:10

Wow, great pictures as usual, woelen. I would have never expected that fullerenes would even dissolve, much less make such colorful solutions! Really fascinating stuff.

Mailinmypocket - 15-2-2015 at 11:29

That C60 is beautiful Woelens! I'm going to try and see what those nanotubes I got as samples recently look like in CS2 also, I wonder if the color will be similar or none at all? Haven't researched much but Wikipedia (not the best source) does indicate some sort of solubility.

The Volatile Chemist - 16-2-2015 at 14:29

Where did you purchase the fullerenes? Good price tags on 'em.

Potassium hexacyanochromate

Hegi - 17-2-2015 at 22:10

Hello everyone,

if someone´s interested in chromium compounds there is one that is really hard to get in its pure form. Yields up to 10%. You can find the whole synthesis here -> K3[Cr(CN)6]

<img src="http://chem.pieceofscience.com/wp-content/uploads/2015/01/hexacyanochromate.jpg" width="900" height="600" alt="Computer Hope">

<img src="http://chem.pieceofscience.com/wp-content/uploads/2014/01/hexacyanidochromate-II.jpg" width="900" height="600" alt="Computer Hope">

Zombie - 17-2-2015 at 22:20

Quote: Originally posted by woelen

I have been playing around with my PBr3 which I made a few years ago, see http://www.sciencemadness.org/talk/viewthread.php?tid=17228#... .
I have made nice collector's samples of some very rare compounds:

PBr3: http://woelen.homescience.net/science/chem/compounds/phospho...
PBr5: http://woelen.homescience.net/science/chem/compounds/phospho...
PBr7: http://woelen.homescience.net/science/chem/compounds/phospho...

Some time ago, I also added 200 mg of C60 (fullerene) to my element collection. I put some CS2 and C60 in an ampoule and keep this as another sample for my collection of compounds:

C60: http://woelen.homescience.net/science/chem/compounds/carbon....

Lovely Picts. and write up.

The Volatile Chemist - 18-2-2015 at 12:29

I bet they would (The Cr(III) and Co(III) complexes mentioned here and on his site, respectively) would make great indicators for metal ions, and selective precipitation salts.

alexleyenda - 19-2-2015 at 17:07

A little classic :p I managed to get my hands on AgNO3 for the first time

Zombie - 19-2-2015 at 18:47

Is that the one they call the silver tree?

How fragile is that? Dust? Powder?

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