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Brain&Force
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That is the most beautiful sample of fluorite I've ever seen.
At the end of the day, simulating atoms doesn't beat working with the real things...
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Jylliana
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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.
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j_sum1
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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.
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Molecular Manipulations
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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?
-The manipulator
We are all here on earth to help others; what on earth the others are here for I don't know. -W. H. Auden
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Jylliana
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Crystallized Gallium 
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blargish
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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"
 
BLaRgISH
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Zombie
Forum Hillbilly
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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]
They tried to have me "put to sleep" so I came back to return the favor.
Zom.
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sasan
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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]
 
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Hegi
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What about these fluorite crystals? 
 
Our webpage has been shut down forever cause nobody was willing to contribute. Shame on you all!!!
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Loptr
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Sodium
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]
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The Volatile Chemist
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That's gorgeous! A nice, collect-able form, minus the stirbar (or with, we all have our preferences....)
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Loptr
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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.
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The Volatile Chemist
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Nice! I thought that was your stirbar coated in sodium
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Mailinmypocket
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Crude sulfanilic acid has a pretty purple iridescence to it:
Note to self: Tare the damned flask.
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The Volatile Chemist
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Huh. Procedure, please?
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Mailinmypocket
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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...
Note to self: Tare the damned flask.
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Firmware21
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Mood: Ņ͈̣̭̺̈ͬ͊̔i̓̿͑ͯ̂ͪ҉̸̺̀t͉̣͕͙̟̪̅͐͂̏͌ͭ͗̑͝ṙ̶̛̙̥̝̻̟̓ͬ̾ͧ͒͘ͅa͒͊ͯ̾̑̏̌̓̕҉͚͚͓͔͙͚̥t͆̌͑ͩ̐͗
͖̻̲̪̲̙͘ͅe͙͕͙̙̤̤̫̒ͩͣ̅̊̍̉͒ͬ́͟ͅs͈̬̮̥̻͂ͥͨ̂ͮͨ͒́͠ !!!
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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".
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bismuthate
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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
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Mailinmypocket
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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?
Note to self: Tare the damned flask.
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bismuthate
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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.
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Mailinmypocket
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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.
Note to self: Tare the damned flask.
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The Volatile Chemist
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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]
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bismuthate
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It was bismuth nitrate.
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Zephyr
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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]
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bismuthate
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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?
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