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plante1999
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it look to be beatiful metalic sodium , you have the same glove than my.
I never asked for this.
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kuro96inlaila
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Tons of nude sodium!
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blogfast25
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Yep, 10 % is a bt of a bummer: it may prove hard to get much beyond that, considering circumstances...
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bfesser
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Mg is exceedingly cheap and easy to come by. 10% Na yield <em>is</em> worth sharing.
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m1tanker78
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Yes, 10% yield is better than 0%. For those in the US, Mg fire starter blocks are available at Wal-Fart, Harbor Freight and Academy, to name a few. I
don't know what impurities they have but I just picked one up from HF for $2.49 (though, not for Na production)...
EDIT: It weighs 40g including the flint that's glued to the side (I can't remove it w/o breaking it).
Tom
[Edited on 4-19-2011 by m1tanker78]
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Wizzard
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I get all my Mg from these, and laptop frames  Pure enough for me.
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Bot0nist
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Mood: Streching my cotyledons.
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Crude TNP that was laid to dry near an open beaker of of aqueous NH<sub>3</sub>. Suspected formation of ammonium picrate. Sample was pure
yellow the night before, but bright red crystals can be observed on the side near the beaker today. A beautiful surprise.
U.T.F.S.E. and learn the joys of autodidacticism!
Don't judge each day only by the harvest you reap, but also by the seeds you sow.
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kuro96inlaila
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Gold leaf suspended in water extracted from computer processor:
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m1tanker78
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Macro shots with a cell phone...
Unknown carbon compound that begins life as glossy planar flakes and (presumably) picks up moisture from the air and recrystallizes into a glassy
needle structure.
A small chunk broken off the block:
It looks like glass but is composed of many smaller 'fibers' that run parallel to each other. It's times like these I wish for a
microscope:
And finally, a small cluster ~8mm tall. It took a steady hand to pull this one off:
Tom
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hkparker
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Some pretty pictures of bismuth crystals I made my friend took. Too large to post in the forum.
<br><br>
<a target="tab" href="http://www.sciencemadness.org/scipics/bismuthcrystals1.JPG">Picture 1</a><br>
<a target="tab" href="http://www.sciencemadness.org/scipics/bismuthcrystals2.JPG">Picture 2</a><br>
<a target="tab" href="http://www.sciencemadness.org/scipics/bismuthcrystals3.JPG">Picture3</a>
My YouTube Channel
"Nothing is too wonderful to be true if it be consistent with the laws of nature." -Michael Faraday
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NurdRage
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Not a picture, but a video of gallium destroying a coke can:
<iframe sandbox title="YouTube video player" width="640" height="390" src="http://www.youtube.com/embed/FaMWxLCGY0U" frameborder="0"
allowfullscreen></iframe>
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blogfast25
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Interesting...
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NurdRage
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thanks
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mr.crow
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Excellent use of time lapse photography. I'm amazed the gallium absorbed so quickly, thought it was supposed to be a solid!
Double, double toil and trouble; Fire burn, and caldron bubble
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sternman318
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The first picture is some crystals of NaNO3
The second is of some copper being dissolved. I added some acetic acid, dumped some sodium chloride right in the middle, then poured in some hydrogen
peroxide and let it work its magic. Its like a lagoon By the way, those are the
actual colors-even though the copper looks dull.
 
[Edited on 25-4-2011 by sternman318]
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Boffis
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Organic metal salts
Hi I'm interested in organic anions that form crystalline metals salts. Check these out, they are the barium and strontium salts of alloxan 5 oxime;
Both the violet fishtail twins and the pink coral like material are barium salts but I don't yet know what the difference is.
Strontium forms crimson blades and small brick red balls in the same fashion.
 
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Rogeryermaw
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here is a rare look at sulfur naturally occurring in a volcanic steam vent from Kilauea in Hawaii on the Big Island.
although of questionable legality i could not help taking a sample...
sorry i should have put this on too. close up of the crystals. gorgeous long shiny needles, look how the light glints off the surface...
[Edited on 20-5-2011 by Rogeryermaw]
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blogfast25
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Very pretty but I think you mean ferric chloride hexahydrate.
http://en.wikipedia.org/wiki/Iron(III)_chloride
AlCl3 cannot be isolated as a hydrate.
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DJF90
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Way off the mark there...
[Edited on 26-5-2011 by DJF90]
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blogfast25
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Your product must be seriously contaminated with FeCl3.6H2O. The Al3+ ion, hydrated or not is colourless. See also most Al salts...
Your contamination may come from technical HCl or from your reactor.
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Megamarko94
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you are right i did some research and my HCl was very contaminated....
i tryed again with lab grade HCl and i got white cristals...
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blogfast25
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I'm a bit surprised one can crystallise the hydrate of AlCl3 at all, I'd have expected it to more or less completely hydrolyse. Live and learn!
Try washing your crystals with pure acetone: FeCl3 is highly soluble in it. I've done this with ZrOCl2.8H2O. Worked very well. But they won't be so
pretty anymore! 
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#maverick#
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first one some potassium nitrate crystals gotta love that
and second is potassium chlorate with a bit of permanganate contamination, used a MnO2 electrode and for got to apply an electrolitic layer of MnO2
taken with an iphone wish i had a better camera
<img src="http://i55.tinypic.com/i5w0up.jpg" width="800" />
[<a href="u2u.php?action=send&username=bfesser">bfesser</a>: fixed width]
[Edited on 7/7/13 by bfesser]
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LanthanumK
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Copper(II) chloride
Here is a shrunk image of some copper(II) chloride crystals I grew using the CuO + HCl method.
   
Here are some pictures of cobalt compounds I synthesized for the purpose of photography. They are some of the more colorful compounds I photographed.
[Edited on 27-5-2011 by LanthanumK]
[Edited on 27-5-2011 by LanthanumK]
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Megamarko94
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FeCl3 cristals....
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