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Texium
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@B&F: I don't usually either for the same reason, but I might try crystalizing some for my crystal collection I'm working on.
Edit: Oh, and now that I've posted this, it's started a new page, fixing the image size problem you mentioned, at least for the current page!
[Edited on 6-14-2014 by zts16]
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Brain&Force
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Not my work, but here's a video of erbium-praseodymium powder spontaneously igniting in air:
https://www.youtube.com/watch?v=8i45S_YW2Hg
No ignition sources needed.
At the end of the day, simulating atoms doesn't beat working with the real things...
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kristofvagyok
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3,4-O-Isopropylidene-D-mannitol, purity over 99% according to NMR analysis.
I have a blog where I post my pictures from my work: http://labphoto.tumblr.com/
-Pictures from chemistry, check it out(:
"You can’t become a chemist and expect to live forever." |
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numos
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On the subject of needle crystals:
Recrystallized Salicylic acid:
Sublimation distillation of Phthalic acid to Phthalic anhydride
Nowhere as impressive as kristof's crystals, but still pleasant to look at.
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sasan
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pyranine solution in water under UV light
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Brain&Force
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Try adding some acid and base for some interesting effects - pyranine is a fluorescent pH indicator.
At the end of the day, simulating atoms doesn't beat working with the real things...
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sasan
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Violet hexamine nickel (II) chloride and Yellow dipotassium tetra chloro nickelate(II)
are they cool enough??
 
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Metacelsus
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What's the blue stuff on the far right?
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The Volatile Chemist
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Very nice pictures everyone!
I like the yellow complex 
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sasan
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It is hexamine nickel chloride too but it is under sunlight ,the left is under tungsten light0
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The Volatile Chemist
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^Oh my, that's a stunning difference!
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sasan
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6gr platinium metal
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The Volatile Chemist
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Where'd you pick up that?
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DraconicAcid
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The yellow tetrachloronickel(II) complex is particularly surprising. I've made the tetraethylammonium salt of that ion, and it's blue.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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sasan
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In fact in solution was green,apon drying was green too,but after heating to about 45 c,the color change to deep yellowish orane,after puverizing
change to light yellow with some green tint
In wiki the tetrachloronicklate ion is yellow
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DraconicAcid
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Quote: Originally posted by sasan  |
In fact in solution was green,apon drying was green too,but after heating to about 45 c,the color change to deep yellowish orane,after puverizing
change to light yellow with some green tint
In wiki the tetrachloronicklate ion is yellow |
How did you make it?
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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sasan
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I've prepared it months ago,but as I realize,first I dissolved NiCl2.6H2O in water(preferly concentrated) added drops of con HCl(aq)into sulotion
and added 2moles KCl for each moles of NiCl2.apaporated and heated to about 40 c or place it under of intense hot sunlight.this is the procedure but
I'm not sure if it will work or not.try it in stochiometric amounts
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sasan
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| Quote: Originally posted by DraconicAcid | | The yellow tetrachloronickel(II) complex is particularly surprising. I've made the tetraethylammonium salt of that ion, and it's blue.
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how did you make the tetraethylammonium salt??can you write the complete name and structure of this salt?it seems to nedd tetrammonium chloride
reagent(I don't have )
[Edited on 18-6-2014 by sasan]
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DraconicAcid
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| Quote: Originally posted by sasan | | Quote: Originally posted by DraconicAcid | | The yellow tetrachloronickel(II) complex is particularly surprising. I've made the tetraethylammonium salt of that ion, and it's blue.
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how did you make the tetraethylammonium salt??can you write the complete name and structure of this salt?it seems to nedd tetrammonium chloride
reagent(I don't have) |
Dissolve nickel chloride hexahydrate in absolute ethanol with triethyl formate, heat until the solution is brown. Then add a solution of
tetraethylammonium chloride in ethanol to get blue (NEt4)2[NiCl4].
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
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violet sin
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couple pics to post here,
antimony 95g
cadmium stick 1/2 lb
tellurium pics, 1) 2lb ingot, 2) chunks broken from ingot, 3) ingot remainder, and 4) end of bar showing crystalline structure
 
 
the gentleman who sold the Te has more of the 2# ingots for an affordable price if any one is interested. I'm going to get more. 120$/2 lb with
shipping to the US only. I will post in reagent acquisition shortly. in the ebay auction it said, 97%, but in personal email it was stated 99.7%,
which I believe after breaking this thing up a little. so stoked to find it at a good price
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numos
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Some Sulfur dichloride I prepared yesterday. The ampule on the right is very contaminated with disulfur dichloride, but the other three are quite
pure.
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Oscilllator
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Numos wouldn't it be unsafe to store disulfur dichloride for long periods of time? I thought that it decomposed to disulfur dichloride and chlorine
gas, building up pressure until the vessel explodes. Or is an equilibrium formed at a low enough pressure to be safe?
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HgDinis25
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| Quote: Originally posted by Oscilllator | | Numos wouldn't it be unsafe to store disulfur dichloride for long periods of time? I thought that it decomposed to disulfur dichloride and chlorine
gas, building up pressure until the vessel explodes. Or is an equilibrium formed at a low enough pressure to be safe? |
Actualy, he's storing Sulfur Dichloride, not Disulfur Dichloride. Sulfur Dichloride looses chlorine over time. However, in an ampoule, there will be a
slight higher pressure than 1atm, because of chlorine formation. However, like you said, the equilibrium is quickly reached and no pressure build up
actualy happens. The decomposition of Sulfur Dichloride may be reduced by placing it in an ampoule that had been previously filled with chlorine gas.
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numos
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| Quote: Originally posted by HgDinis25 | | Quote: Originally posted by Oscilllator | | Numos wouldn't it be unsafe to store disulfur dichloride for long periods of time? I thought that it decomposed to disulfur dichloride and chlorine
gas, building up pressure until the vessel explodes. Or is an equilibrium formed at a low enough pressure to be safe? |
Actualy, he's storing Sulfur Dichloride, not Disulfur Dichloride. Sulfur Dichloride looses chlorine over time. However, in an ampoule, there will be a
slight higher pressure than 1atm, because of chlorine formation. However, like you said, the equilibrium is quickly reached and no pressure build up
actualy happens. The decomposition of Sulfur Dichloride may be reduced by placing it in an ampoule that had been previously filled with chlorine gas.
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Yes, this is correct. The best way to store Sulfur dichloride is in an ample as it keeps the substance from decomposing. I think I'm going to make a
video on the preparation of this, it is pretty simple, but can be very messy and lethal if done incorrectly.
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arkoma
Redneck Overlord
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Beaut-i-mous to me. Rose leaves refluxing in acetone. The maid cleaned AROUND it. (Living in a motel ATM) Nevada puts up with anything if yer not
on dope or stealing LOL
"We believe the knowledge and cultural heritage of mankind should be accessible to all people around the world, regardless of their wealth, social
status, nationality, citizenship, etc" z-lib
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