Pretty Pictures (1)

4 palladium coins in aqua regia. It quickly turned dark red then almost black.

<!-- bfesser_edit_tag -->[<a href="u2u.php?action=send&username=bfesser">bfesser</a>: serialized]

[Edited on 26.9.13 by bfesser]

Very nice, how much palladium is in there? Love those bright red colors.

I have some as well:

Copper mirror formation:
http://s405.photobucket.com/albums/pp133/Joris12345/?action=...
Mercury oxide decomp.:
http://s405.photobucket.com/albums/pp133/Joris12345/?action=...
SnI4 in the gas phase:
http://i405.photobucket.com/albums/pp133/Joris12345/P1110887...

Quote: Originally posted by blogfast25

One supplier I know advertises 50 g of PdCl2.2 H2O for £ 1460... Expensive water!

Very sexy palladium shot, worthy of a lab pin-up .

The copper mirror is quite sexy too.

Figured I add a few contributions of my own:

1) Formation of gold flakes from Auric Chloride by addition of sodium Metabisulfite.
2) Molten silver ingot.
3) Platinum mirror formed by addition of hydrazine sulfate to hexachloroplatinic acid.

A few pictures which I like very much:

This is the fluorescence of the iodide of a pyridine-copper(I) complex which I made by reacting copper(I) iodide with pyridine:





The following picture was made, simply by lighting an air/ethanol mix in a flask:




I also like this one very much, it is the glow of singlet oxygen, falling back to normal oxygen and while doing so it emits red light. The singlet oxygen can be made by adding 30% H2O2 to Na-DCCA (swimming pool shock chlorine treatment).

Quote: Originally posted by Rogeryermaw

ooh i love nerd porn! that is pretty! (ohh i love watching rare metal take it off! mmm bubble bubble...slower yeah...now react faster yeah!!)

Well,chemist like us always enjoy it!

Take a look at my picture!
I don't know if it is not beautiful,but I find it interesting!




Me holding mercury metal!





Burning copper(II) nitrate in granite mortar.


Me while burning a pile of blackpowder in the same granite mortar.


Sublimating iodine in aluminium-iodine reaction.



Sperrylite mineral (PtAs2) after a while in concentrate hydrochloric acid.

i'm sure you've seen the pictures in the phosphorus thread. i was trying to take some in the dark of the green glow but it's so faint my shitty cam barely pics it up... i did catch this nice vid of some P4 dissolved i benzene. as the benzene evaporates the P4 oxidizes but i only used a tiny bit so it would show the lovely glow rather than cause conflagration.

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here is the link to the vid on boobtube: http://www.youtube.com/watch?v=XA02M9yf1qg

there are other vids of the phosphorus making process on my channel. they were private but i opened the rest to the public cuz fuck it that's why. everyone should be able to share the information i have or that makes me a censoring government dick.

[Edited on 15-10-2010 by Rogeryermaw]

I'm glad you made the videos public, I never really saw anything controversial in them. I understand your reasons though.

I have a video of the aqua regia, maybe I should post that

Quote: Originally posted by mr.crow

I have a video of the aqua regia, maybe I should post that

Yes,please?

Quote: Originally posted by metalresearcher

@woelen: Pic 2 is really nice but is that not an explosion hazard ? Vaporized ethanol (or even supermarket-grade methylated spirit with the blue dye) with air is explosive ??

i wouldn't say it's impossible but this question made me curious so i put on my face sheild and tried it several times. no explosion but it sure looks cool!

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ok obviously it's not a true "barking dog" but the effect, while milder is quite similar. no CS2 or P4 or S but it's still pretty. woelen's was much nicer and the still he captured really does justice to the effect.

later i will upload a vid of elemental phosphorus reacting with chlorine gas. did that last night and it's niiiice

i know it says pretty "pictures" but i do hope video is ok?



[Edited on 16-10-2010 by Rogeryermaw]

[Edited on 16-10-2010 by Rogeryermaw]

Some very beautiful pictures in this thread. I wish I had more myself, I took hundreds of pictures of my experiments at home however my camera was a much older model, something like 256 KB quality so most of my pictures are grainy / blurry / bad color. Somehow when the elements were perfect however, by some quirk of fate, it would take a good picture, not as pretty as the rest in the thread but pretty enough:

Pulling off ammonia though a compressor with copper tubing created ammonia complex in wash bottle.



One of my favorites, electrolysis of lithium chloride in DMSO with nickel electrodes



Trying to distill CS2 from carbon and sulfur and only ended up distilling sulfur



The first experiment I photographed, burning potassium after its creation

Such a beautiful science!

here are a couple of pics and the vid of P4 with Cl2


reaction flask inerted with CO2 with sand on bottom to mitigate breakage risk

the bottle of P4...ghetto home-made tag but better than unlabeled no?

cut a small piece to react

fresh chlorine gas for reaction

and finally the reaction. i drew some of the Cl2 gas into the syringe and "injected" it over the chunk of P4.

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shook the flask a little trying to get the syringe out and stopper on. don't sweat fellas. i'm using ventilation. last thing i want to do is gas myself with a nerve agent (PCl3).

the reaction is A LOT more energetic if you just drop the P4 in the chlorine flask but safety first you know.



[Edited on 16-10-2010 by Rogeryermaw]

Here is a video

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I also boiled it down successfully to PdCl2

Mr.crow, thanks for the wonderful picture, it's my desktop now

@ Blogfast25
Don't really know what that stuff is. You can see the bottom layer is turning blue/green from the nickel electrodes dissolving. The solids at the bottom are undissolved lithium chloride. When the current was jacked wayyyy up I could get a solid deposit on the cathode that reacted with water with hissing / spattering. My hope at the time was to make lithium, but when I looked into it more it seems some kind of methyl lithium complex was more likely. Don't remember exactly now but it was reported in the DMSO technical bulletin. As you can see however the colors are very vibrant. The red color becomes almost black when allowed to run for some time and solids start to precipitate.

@ BromicAcid my daughter about blew a gasket when she saw that bright pink fire! was that a thermite or electrolysis produced potassium or obtained by other means? would it be possible to share your method? i would love to reproduce this for her. pink just makes her day and that makes my day!

phosphine burning...



luminol + KOH in DMSO...

[Edited on 17-10-2010 by Magpie]

freshly distilled fuming nitric acid.



i know it's not doing anything spectacular but i think all the acids are pretty. it will likely go toward aqua regia...got a couple of cpu's i dont have a use for.

[Edited on 22-10-2010 by Rogeryermaw]

Here's my current self-made desktop background.
It's a picture of a part of an home-made ozonisator I'm currently working on.



Full size:
http://img231.imageshack.us/img231/8504/dsc01695y.jpg






[Edited on 22-10-2010 by Methansaeuretier]

[Edited on 22-10-2010 by Methansaeuretier]

Physical Laws in action: standing waves in a sauce pan of water about to be brought to the boil, vibrations supplied by a tumble drier about a yard away:





On occasion I’ve seen almost perfectly radially symmetrical standing waves in a half filled pop bottle stood on the drier.

These just show how hard it is to imagine the three dimensional standing waves in the quantum systems that are the electron clouds of our beloved atoms and molecules…

Sulphur mining Kawah Ijen volcano East Java, Indonesia

The pictures of burning sulfur are really neat, but what an environmental nightmare!

Here are a few from my shop that I'm particularly fond of:



This is of a water electrolysis cell I built using NaHCO3 solution as the electrolyte and stainless steel plates for electrodes.



I built it because I wanted an oxyhydrogen torch. Here's the picture of the nearly invisible flame igniting a bit of paper.



And my favorite: melting a chunk of refractory designed to take 1600C.

Construction details and pictures here if anyone's interested.

Quote: Originally posted by DougTheMapper

This is of a water electrolysis cell I built using NaHCO3 solution as the electrolyte and stainless steel plates for electrodes.

Quote: Originally posted by kuro96inlaila

Any explanation about molybdenum picture?

Quote: Originally posted by DougTheMapper

Mo has oxidation states of 6, 5, 4, 3, 2, 1, -1, and -2. IIRC it also easily forms complexes. I imagine that quite a few colors can be made with Mo compounds.

Quote: Originally posted by DougTheMapper

Mo has oxidation states of 6, 5, 4, 3, 2, 1, -1, and -2. IIRC it also easily forms complexes.

That's a quite naïve view of Mo chemistry. In reality Mo does all kind of crazy polyoxoanions (isolated, chains, sheets, 3D) where Mo has non-integer oxidation states. If you're (un)lucky it's incommensurate and every single Mo atom in your compound has a different oxidation state. That's in solid state - in solution it's probably even more complicated since the whole mess is dynamic. Just say no to Mo chemistry.

Crystals of elemental silver

Quote: Originally posted by NurdRage

Crystals of elemental silver

Quote: Originally posted by blogfast25

Nurd: Any idea of scale? This looks like a microscope shot with typically some areas in focus, some not. If so: good shots!

Yeah it's a microscope shot.

It’s that cold in my lab right now: a frozen solution of 0.1 N KMnO4 in a burette. You’ve heard of permafrost, now you’ve seen permanganate frost!

Quote: Originally posted by bfesser

You might want to invest in a small electric space heater. Just be sure your volatile flammables are carefully stored away!

Quote: Originally posted by blogfast25

It’s that cold in my lab right now: a frozen solution of 0.1 N KMnO4 in a burette. You’ve heard of permafrost, now you’ve seen permanganate frost!

That must be crazily cold weather until that permanganate solution get freezed!

Well, at 0.1 N, the solution is only 0.02 M, so really quite dilute...

Crystallisation of FeCl3.6H2O from a concentrated solution:





[Edited on 19-12-2010 by blogfast25]

[Edited on 19-12-2010 by blogfast25]

Quote: Originally posted by NurdRage

no idea, probably less than 10ma for the slow growth videos. Maybe in the future i'll do more precise growth with controlled conditions.

Here is a picture of me working up a fluorescein-type (resorcinol malein) synthesis. It's more a matter of removing all of the other crap from your product, rather than vice-versa. The yields are *that* bad. Fortunately, the precursors are cheap.

Anyhow, here is some of it on silica gel eluting out with a manual (EtOAc:Hexanes:Methanol) gradient.

This was taken with an Iphone 3GS and an El cheapo blacklight.

Cheers,

O3



[Edited on 22-12-2010 by Ozone]

Quote: Originally posted by blogfast25

Quote: Originally posted by NurdRage   no idea, probably less than 10ma for the slow growth videos. Maybe in the future i'll do more precise growth with controlled conditions. Yes, it must be a very low current for such slow growth. With an SnCl2 solution I got crystals of almost a cm long with 4 A in about 1 - 2 mins...

Quote: Originally posted by crazedguy

Nurdrage Could that crystal growth be done with different elements? Could you give examples of ones that would work,thanks. [Edited on 22-12-2010 by crazedguy]

Quote: Originally posted by UnintentionalChaos

Quote: Originally posted by blogfast25   Quote: Originally posted by NurdRage   no idea, probably less than 10ma for the slow growth videos. Maybe in the future i'll do more precise growth with controlled conditions. Yes, it must be a very low current for such slow growth. With an SnCl2 solution I got crystals of almost a cm long with 4 A in about 1 - 2 mins... Hrm...in that case, the power source I'm using must be churning out a MUCH higher amperage than it is rated for...since it is also rated for 4A (no multimeter to check though). Anyway, Sn crystal growth in real time: http://www.youtube.com/watch?v=Af9GAUYDrlQ

Quote: Originally posted by blogfast25

Quote: Originally posted by bfesser   You might want to invest in a small electric space heater. Just be sure your volatile flammables are carefully stored away! Got one: in the current conditions it hardly makes a dent in it! We've had another 15 - 20 cm of snow overnight.

Have a look at this,very interesting!:

http://www.youtube.com/watch?v=HY7mTCMvpEM

Sure a lot of fish boiled there
Anyway it is old way to dispose sodium,old but fantastic!

Rightfully named Nurdrage, Teaser You gonna tell us how or just leave us hanging. Pretty cool. Someone should give there lady freind a glowing rose because if that don't say special I don't know what does.

Quote: Originally posted by NurdRage

actually it came off Nothing special really, just take a flower and stick it into highlighter fluid water and then shine a UV light on it after one day. Safe and cool looking.

Cool, glad I know whats going on because I recently for no reason lost sound on my computer.

Did you come up with this idea or have you seen other do the same as well? Im shocked I have never seen something so simple done. The dye and flower idea has been around for ages so I would expect someone to think of UV dye alone time ago I just have never seen such a thing.

Thanks for sharing.

@blogfast thanks


@sedit Came up with it myself.

I had a firm educated hypothesis though; i studied analytical chemistry and knew biological samples were routinely stained with fluorescent dyes. So i guess THOSE scientists get 80% of the credit. An old kids TV show i watched back when i was 5 gets 15% of the credit for showing me the plant and food coloring idea, 4% of the credit goes to my analytical chemistry professors, and i claim 1% for putting it together.

Damn man, you about as modest and humble as it gets aint ya.

Nice work no matter what, im glad to see it you gave it your all. When most people wish to put in 110% effort on things Dr Butyl is more then happy to suffice with just 1% and still get the job done

Bottom of the tube: NaCl (solid, about 11 g), top CuSO4.5H2O (solid, about 14 g, with 50 ml water poured over it all. Due to the high solubility of CuSO4.5H2O (> 30 g/100 g water) some of the CuSO4 dissolved immediately on pouring on the water, where the dissolved Cu2+ then reacts with NaCl to form the green CuCl4 (2-) complex anion. The green is so intense the white NaCl appears green!




After shaking the tube for some time:



This solution can be considered a solution of Cu2+, CuCl4 (2-), Na+ and SO4(2-).


[Edited on 9-4-2011 by blogfast25]

Now add some Aluminium foil a la woelen

Quote: Originally posted by DJF90

Now add some Aluminium foil a la woelen

I will!

So this is the CuSO4/NaCl tube after adding some aluminium (a few of these little levers you use for opening a pop can) and standing overnight:



Top layer is greyish CuCl with a wad of elemental copper ‘hidden’ in it, then follows a green layer and at the bottom of the tube is some CuCl. Here’s the wad of copper sponge recovered and rinsed:



What took me by surprise a bit was the heat generated by the reduction of Cu2+(aq) by Al(s). Of course the cell potential ΔE for 3 Cu2+(aq) + 2 Al(s) === > 3 Cu(s) + 2 Al3+(aq) is very healthy and thus ΔG = -nFΔE is too but in this case things appeared to even start boiling, which is why the copper was found in the top bit of the tube! Of course it was a concentrated solution too (almost saturated).

The CuCl was of course formed by Cu(s) + Cu2+(aq) + 2 Cl-(aq) === > 2 CuCl(s). The heat will have helped a lot! Here’s some of the CuCl transferred to another (smaller) test tube:



Left: the CuCl.

Right: after adding 4 M NaOH. The green precipitate is likely to be our old friend the Cu[+I]/Cu[+II] complex, due to some remaining Cu2+ (the suspension as slightly bueish).


Reaction with ammonia:



Middle: the left tube from above was decanted off, then fresh water added and then decanted again. 4 % NH3 solution was then added. The deep blue is the colour of the Cu+ ammonia complex: Cu [+I] forms the same complex as Cu2+ and it’s blue too. The weak ammonia dissolves all the CuCl!

Left: adding 4 M NaOH changes nothing for a few minutes, indicating strength of the complex. But then slowly precipitation starts…

Right: the same tube as above right, after a bit of standing what is more or less Cu2O has dropped out (CuO's colour depends on a lot of things...)

Made some CuSO₄·5H2O using 12% H₂O₂ and 98% H₂SO₄

50ml of 12% H₂O₂ was poured into a 100ml beaker and chilled to aprox. 5c. 10ml of 98% H₂SO₄ was added slowly while stirring. A 10g piece of cleaned copper pipe was added and the reaction preceded immediately and rather violently with a lot of fizzing and some splashing. The solution began to turn blue almost instantaneously and the color got darker as the reaction continued. The beaker was placed in a still area to sit overnight. Approximately 15 hours later I took these pictures. Aside from the crystals on the pipe, there is a great mass that formed on the bottom of the beaker as well.

My wife actually enjoyed this project, as opposed to some of my others


[Edited on 9-4-2011 by Bot0nist]

Bot0nist:

This is the first time I’ve seen a decent write-up of this quick and mean synth. of CuSO4, straight from conc. H2SO4 (but maybe I should get out more often? ). I only have H2O2 9% and H2SO4 about 95 % but I’ll definitely be trying this shortly, Thank you!

I'll check that out

Hi. I was cutting up some praseodymium recently and ended up with some filings. As a reactive metal I thought it would be interesting to mix with an oxidiser and ignite. I got a lovely "soft" explosion and clouds of dark brown smoke (Presumably an oxide of praseodymium). I have attached a Single frame and a slow motion video of the explosion.



Attachment: My Movie.wmv (1.1MB)
This file has been downloaded 1031 times

Quote: Originally posted by nezza

Hi. I was cutting up some praseodymium recently and ended up with some filings. As a reactive metal I thought it would be interesting to mix with an oxidiser and ignite. I got a lovely "soft" explosion and clouds of dark brown smoke (Presumably an oxide of praseodymium). I have attached a Single frame and a slow motion video of the explosion.

Hmm,exotic pyro composition!
Never see praseodymium flash powder before!

Sodium made by magnesium + sodium hydroxide process.

First shot is the synthesis right from the raw slag, and the second is after workup and cleaning.

Nurdrage:

This is still sodium by magnesiothermy, right? Not 'Pok's method'?

Very nice pix, BTW!

[Edited on 18-4-2011 by blogfast25]

Yeah its not pok's method.

So don't worry, i haven't beaten ya to it.

Don't judge a book by its cover?

Unrefined sodium nugget dissected to check internal integrity. Ugly outside; lustrous inside...