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Texium
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[*] posted on 18-10-2016 at 10:44


I'm really surprised that you got V(II) to work just using aluminum. You didn't even have to activate it with mercury or gallium? I tried using Al/Ga once for reducing V(III) to V(II) and that didn't even work.



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[*] posted on 18-10-2016 at 12:29


Quote: Originally posted by zts16  
I'm really surprised that you got V(II) to work just using aluminum. You didn't even have to activate it with mercury or gallium? I tried using Al/Ga once for reducing V(III) to V(II) and that didn't even work.


So was I. It didn't react at all in sulphuric acid solution, but adding a few mL of 6 M HCl got it going well.




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[*] posted on 18-10-2016 at 14:47


A bit of HCl will activate your Al just nicely. Al does not like chloride ions. :)



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[*] posted on 18-10-2016 at 19:18


I'll be interested to see pics of the crystals you manage. :o
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[*] posted on 25-10-2016 at 11:32


Quote: Originally posted by zts16  
I'm really surprised that you got V(II) to work just using aluminum. You didn't even have to activate it with mercury or gallium? I tried using Al/Ga once for reducing V(III) to V(II) and that didn't even work.


If you look at the picture of my V(II) two pages ago I did it the same way. Tested a lot of possible reducing agents and pH environments and finally settled with using Aluminium. It works quite well. I think most of my reductions (Ox-states) on Youtube were done using just Acid/Base and Al foil wrapped around a glas rod to keep it in solution. The only thing where it didnt work was for Boron from Boric Acid. I got an orange powder but never further processed or tested it. I guess althouth from a Redox perspective this could be possible the B-O-Bonds are just too strong.




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[*] posted on 27-10-2016 at 15:17


Erythritol, slow evaporation method. (the rest is here)


all-sizeDSC02707.JPG - 695kB

[Edited on 27-10-2016 by Dmishin]
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[*] posted on 27-10-2016 at 18:59


Very cool. I am impressed.
I am more likely to play with xylitol though since I can easily get it. Does it also exhibit birefringence?




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[*] posted on 28-10-2016 at 08:20


J_sum1, you might know this but if you're chasing Erythritol, check your local Coles or Woolies: http://shop.coles.com.au/online/mobile/national/norbu-sweete... Don't believe all that 'completely natural' crap. I nitrate it directly and it behaves well, I don't think there's much of this 'monk fruit' in there at all really
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[*] posted on 28-10-2016 at 08:43


This brand of Erythritol is good too J https://www.woolworths.com.au/Shop/Browse/spreads-breakfast-...
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[*] posted on 28-10-2016 at 09:28


To follow up on the issue of the preservation of mushroom as specimens (not for consumption):

I did a trial run preserving mushrooms under three fluids: mineral oil, isopropanol, and glycerine.

For the mineral oil I used a generic brown-white front yard mushroom. Over the course of a couple weeks submerged underneath it remained in remarkably good condition; fine structures like the veil remained intact and the only change in shape was a slow loss of turgor. Decomposition did set in gradually, with a brownish watery liquid oozing out of very localized points (apparently associated with clinging air bubbles), and the appearence of fine fuzz after ~2 weeks. There didn't appear to be much discoloration but it was drab to begin with so it's hard to say.

Glycerine and rubbing alcohol, I gathered two smallish red mushrooms (Russula, I think ) . Both liquids appeared to slow or stop decomp over several weeks, but both significantly leached the pigment from the specimen (in the alcohol it pooled at the bottom of the jar, in the glycerine it floated to the top, lol).

I have photos but they don't add much and definitely aren't pretty.

(Glycerine was an idea from an old tip I read on preserving spiders, which will shrivel if pinned like butterflies but bleach if kept in alcohol)




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[*] posted on 28-10-2016 at 12:45


Quote: Originally posted by j_sum1  
Very cool. I am impressed.
I am more likely to play with xylitol though since I can easily get it. Does it also exhibit birefringence?

Thanks! I don't see any sign of birefringence in my xylitol samples.

By the way, here is sodium trioxalatoferrate(III). It is much more soluble than K salt. Unfortunately, crystals are not stable.

[Edited on 29-10-2016 by Dmishin]

DSC02794.JPG - 445kB

[Edited on 29-10-2016 by Dmishin]
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[*] posted on 30-10-2016 at 15:42


Dmishin,
I am amazed at all the beautiful crystals you grow.
I have been trying to find a chemical that will grow clear beauties like those Erythritol, so I will try that out, thanks for the great examples for inspiration.
I have a bag of pure saccharin, I wonder how it crystallizes. :).
Here are a few of my early (lol this spring) crystals

Copper II sulfate
Potassium ferricyanide
Copper sulfate, nickel sulfate Combination
Ferrous chloride

Keep up the great work

Cheers,

Dwarven



7LxChAU.jpg - 1.4MB




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[*] posted on 6-11-2016 at 08:21


Quote: Originally posted by Dmishin  
Quote: Originally posted by j_sum1  
Very cool. I am impressed.
I am more likely to play with xylitol though since I can easily get it. Does it also exhibit birefringence?

Thanks! I don't see any sign of birefringence in my xylitol samples.

By the way, here is sodium trioxalatoferrate(III). It is much more soluble than K salt. Unfortunately, crystals are not stable.

[Edited on 29-10-2016 by Dmishin]



[Edited on 29-10-2016 by Dmishin]


It seems that sodium ferrioxalate forms square and tabular crystals and potassium ferrioxalate tends to form flat, hexagonal crystals..
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[*] posted on 6-11-2016 at 11:16


Quote: Originally posted by stibium  
Phosphorescent alkaline earth sulfides activated with bismuth.
From left to right:
BaS / SrS / CaS

I was browsing through the archives of Pretty Pictures mega thread and I just want to say WOW:o.




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[*] posted on 7-11-2016 at 13:23


Aluminum with silver sand (i.e. rather pure SiO2) heated in an electric arc to the boiling point of aluminum (2500 C) and then allowed to cool.

Actual size: about 24x36mm.

The balls in the center are probably crystallized elemental silicon


IMG_1583.JPG - 1.1MB

[Edited on 2016-11-7 by metalresearcher]
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[*] posted on 18-11-2016 at 07:38


Definitely not the best quality picture by FAR, but one you might not have ever seen before. Diiodoacetylene just after formation.

IMG_20161118_103348.jpg - 136kB
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[*] posted on 1-12-2016 at 10:37


Some large crystals of nootkatone, a naturally occurring sesquiterpene, that I grew at work as one of my own side projects! Its aroma is sharp and assertive, reminiscent of fresh grapefruit peel. And since there wasn't a picture of it online before, I stuck it up on Wikipedia for good measure!

nootkatone_recrystallized.JPG - 1.7MB

[Edited on 12-1-2016 by Amos]




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[*] posted on 1-12-2016 at 11:10


Quote: Originally posted by Amos  
Some large crystals of nootkatone, a naturally occurring sesquiterpene, that I grew at work as one of my own side projects! Its aroma is sharp and assertive, reminiscent of fresh grapefruit peel. And since there wasn't a picture of it online before, I stuck it up on Wikipedia for good measure!



[Edited on 12-1-2016 by Amos]


Very nice crystals. Where did you get the compound? :)




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[*] posted on 1-12-2016 at 12:03


Quote: Originally posted by Hegi  
Quote: Originally posted by Amos  
Some large crystals of nootkatone, a naturally occurring sesquiterpene, that I grew at work as one of my own side projects! Its aroma is sharp and assertive, reminiscent of fresh grapefruit peel. And since there wasn't a picture of it online before, I stuck it up on Wikipedia for good measure!



[Edited on 12-1-2016 by Amos]


Very nice crystals. Where did you get the compound? :)


One of the company's biggest projects is biosynthesizing it in three steps using genetically modified yeast. They also chemically synthesize it for research purposes, and my crystals were grown from the latter, of which we had about 2 kilos of 97% pure material in the lab freezer :)




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[*] posted on 3-12-2016 at 07:22


Spotted a tiny scorpion today :

bookscorpion.JPG - 85kB

It is about 8mm long and turns out to be a Book Scorpion (<i>Chelifer cancroides</i>;), a type of pseudoscorpion (it has no stinging tail).




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[*] posted on 3-12-2016 at 08:49


Very nice Amos, I like the clarity. Have you tried to isolate one of those seeds and grow a single unit?
It amazes me as to the number of compounds that will grow amazing crystals.

Here are my latest :), a couple of easy syntheses and alum, my largest alum at 80.5g :)

Nickel ammonium sulphate, Cobalt ammonium sulphate, and Potassium aluminum sulphate.




Nickel ammonium sulphate SM.jpg - 814kB Cobalt ammonium sulphate.jpg - 737kB Alum 4 final 80.5gSC.jpg - 1.2MB Alum final 80.5g as grownSM.jpg - 2MB

[Edited on 2016-12-3 by Dwarvensilver]




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[*] posted on 3-12-2016 at 08:52


Nice Aga,

Have to say cool and interesting but not real pretty :D
I like it!

[Edited on 2016-12-3 by Dwarvensilver]




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[*] posted on 3-12-2016 at 12:05


Quote: Originally posted by Dwarvensilver  
cool and interesting but not real pretty :D

... says the guy with a 'stainless' rule, which is, er, stained !

Beautiful crystals BTW.

Did it take a while to make them ?




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[*] posted on 4-12-2016 at 01:17


I had an idea after watching the latest NurdRage video where he does some work with Tritium vials (https://www.youtube.com/watch?v=KKdzhPiOqqg) and my question is,

would it be possible to grow a crystal around a small vial of Tritium?

(I'm not a grower and I know little about it) but I think that would be awesome if it can be done,

I see you can get vials in white http://www.ebay.com.au/itm/Tritium-Lamp-Vial-Tube-Capsule-Tr... which would better illuminate the colour of the crystal

[Edited on 4-12-2016 by NedsHead]
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[*] posted on 4-12-2016 at 04:37


Whoever saw my video on trying to make Ti(III) from Ti metal will know how little Ti(III) I actually had in the end.

So I had to do a McMurry reaction at the University and in the end hydrolyzed the rests of my reactants to yield this beautiful purple solution.

Ti.jpg - 415kB




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