Pretty Pictures (2)

Pretty sure its Copper(I) Oxide Reference

Quote: Originally posted by sparkgap

If it's not much trouble, do you have similar pictures using other triphenylmethane/phthalein pigments? sparky (~_~)

Not really, we have circa 20kg phenolphthalein, but I never photographed it, maybe once(:

But here is a nice one:


I tried a trifluoromethyation with sodium trifluoroacetate in dimethylformamide on trinitrobenzene.

While heating the reaction mixture, the trifluoroacetate decomposed to give carbon dioxide, difluorocarbene and sodium fluoride. Since the sodium fluoride is an enough strong base in DMF to remove a proton from the trinitrobenzene, this red/orange thing formed what indicates the trinitrophenyl anion.

One of the most simple tests to show an organic compound present in a reaction mixture is irradiating the sample with UV light. If you know, that the product of the reaction should fluorescence blue, while the starting materials do not emit any light after irradiating the sample with UV, could help a lot while doing a reaction.

In this case a side product formed from the reaction above 130 °C, while the desired product formed at 100 °C. The starting material and the product did not emit any light under UV, while the side product did. So after taking the picture, I was sure, that the reaction is ready.

For more pics, visit: http://labphoto.tumblr.com/

Just a nicely backlit picture some boiling copper sulfate solution, nothing too special, but I think it looks pretty cool.

Quote: Originally posted by zts16

I think it looks pretty cool.

Anyone want to hazard a guess what this is?

clue: It isn't an organic compund

Quote: Originally posted by Oscilllator

Anyone want to hazard a guess what this is? clue: It isn't an organic compund

Just a wild guess, is it a copper sulfate, sodium dichloroisocyanurate complex? Otherwise no clue.
Although it's too light for that, I would like to make some,whatever it is, that color is... unseen.

U2U the name please? If you don't want to give it away here...

Fun with Copper!

Copper oxychloride (Dicopper chloride trihydroxide), freshly precipitated from a copper (II) chloride solution.



A vial in which I was conducting Fehlig's test for reducing sugars. The top layer is partially hydrolyzed starch, the middle is Fehlig's solution, and the bottom shows some hydrated copper (I) oxide precipitating, indicating glucose in the starch.



I don't find this as pretty as I do just neat, but these are some US nickels freshly plated in copper from a hot copper (II) acetate solution.

Quote: Originally posted by No Tears Only Dreams Now

Oscillator, I recently precipitated an unknown copper(surprising, right?) compound that looked just like that by accident, waxy texture and everything. I am very interested in finding out what it is.[Edited on 6-10-2014 by No Tears Only Dreams Now]

Quote: Originally posted by numos

What did you precipitate it from? I collect copper salts, and I have never seen this...

I was going for precipitating cuprous oxide for my collection by reducing copper sulfate by the method in the second half of this video: http://www.youtube.com/watch?v=IIHZ_zFu9lA

Long story short, it requires citric acid; I was impatient and tried to use kool-aid powder (cheap american drink mix)

It requires heating to complete the reaction; however, this curious precipitate formed almost immediately. And what is even more strange is that I can light it with a lighter, and it will weakly smolder for a bit.

An interesting blob of MEKP prior to detonation

Quote: Originally posted by Oscilllator

Hmmm, people seem to be jumping to the conclusion that this is a copper compound. Understandable, but nonetheless incorrect. Keep guessing!

Quote: Originally posted by Oscilllator

Anyone want to hazard a guess what this is? clue: It isn't an organic compund

Quote: Originally posted by No Tears Only Dreams Now

Can you tell us if it is wet or dry in the picture?

Cool image, BUT IT'S SIZE! I just can't get over it's size...

Quote: Originally posted by DraconicAcid

Quote: Originally posted by Oscilllator   Anyone want to hazard a guess what this is? clue: It isn't an organic compund It looks the right colour for hexamminenickel(II) chloride.

@ B&F : tragic waste of iodine!

Quote: Originally posted by Cheddite Cheese

@ B&F : tragic waste of iodine!

*stares mournfully at vapors*
But what did biologist want with I2? (I'm not exacly a biologist so this may be stupid)

Quote: Originally posted by DraconicAcid

It looks the right colour for hexamminenickel(II) chloride.

Correct! (or close enough as makes no difference). It is Hexaamine nickel nitrate, shown here before drying:

I prepared it by first drying the nickel nitrate as much as possible by azeotropic removal of water using toluene. The picture below is of the Nickel nitrate after drying. I presume it is the dihydrate, but it could be the trihydrate or even higher, I don't know. A lot of water was removed from the nickel nitrate though, so I suspect its a fairly low hydrate.

I then removed the toluene, dissolved the nickel nitrate in ethanol and bubbled ammonia gas through the mixture, creating a beautiful precipitate of the hexaamine complex. The precipitate was so fine some of it got through the filter, and I was unable to fully dry the sample. It is still wet with ethanol, since I can see no way to dry it without removing the ammonia ligands

@Brain&Force I very much doubt the complex you linked is nickel Hexaamine chloride. The hexaamine complexes are unstable in air (I sealed mine in a plastic vial glued shut) because the ammonia ligands get gradually replaced by water ones. The compound looks a lot more like cobalt chloride to me, but of course I could be wrong.

Quote: Originally posted by No Tears Only Dreams Now

Oscillator, every step of the whole synthesis looks amazing! Maybe I'll collect Nickel compounds next... [Edited on 6-11-2014 by No Tears Only Dreams Now]

Quote: Originally posted by Oscilllator

@Brain&Force I very much doubt the complex you linked is nickel Hexaamine chloride. The hexaamine complexes are unstable in air (I sealed mine in a plastic vial glued shut) because the ammonia ligands get gradually replaced by water ones. The compound looks a lot more like cobalt chloride to me, but of course I could be wrong.

Here's my preparation of hexaaminenickel(II) chloride - https://www.youtube.com/watch?v=49z5-Adw9QA

Mine was definitely purple:



My experience too is that you can't really dry it completely - if you leave it out in air the ammonia ligands escape and it returns to regular old green nickel(II) chloride (as seen in the video).


--------------------------------

And for my own Pretty Picture, the underside of a small "raft" of potassium sulfate crystals that formed on the surface of a saturated solution that I'm recrystallizing from. The little pyramids formed stalactites floating on solution!


[Edited on 6-11-2014 by MrHomeScientist]

Quote: Originally posted by Oscilllator

@Brain&Force I very much doubt the complex you linked is nickel Hexaamine chloride. The hexaamine complexes are unstable in air (I sealed mine in a plastic vial glued shut) because the ammonia ligands get gradually replaced by water ones. The compound looks a lot more like cobalt chloride to me, but of course I could be wrong.

I think it actually looks a lot more like anhydrous chromium(III) chloride rather than cobalt chloride. It has that same lustrous dark violet color, whereas cobalt chloride is more reddish purple.
Here's a picture of some for reference:


[Edited on 6-11-2014 by zts16]

MrHomeScientist: It's no longer necessary to resize photos if that's what you're doing. I personally use imgur.

It may be tris(ethylenediamine)nickel(II) chloride. Photo from woelen.

Cobalt chloride

Quote: Originally posted by zts16

Quote: Originally posted by Oscilllator   @Brain&Force I very much doubt the complex you linked is nickel Hexaamine chloride. The hexaamine complexes are unstable in air (I sealed mine in a plastic vial glued shut) because the ammonia ligands get gradually replaced by water ones. The compound looks a lot more like cobalt chloride to me, but of course I could be wrong. I think it actually looks a lot more like anhydrous chromium(III) chloride rather than cobalt chloride. It has that same lustrous dark violet color, whereas cobalt chloride is more reddish purple. Here's a picture of some for reference: [Edited on 6-11-2014 by zts16]

Anhydrous cobalt chloride is a light blue, and is only red in its hydrate form. Here are some pictures from a recent synthesis.




[Edited on 6-12-2014 by Pinkhippo11]

I dunno B&F, what happens when you do that...? (Innocent smile....)

Here's a test tube containing copper(II)bromide complex at different concentrations, prepared from sodium bromide and copper(II)sulfate. I prepared two solutions, one concentrated and one diluted, and then combined them in this tube. I love the way it changes colors so dramatically depending on concentration. After swirling the tube a bit, it became a uniform yellow color.

Iron trichloride hydrate. It's amazingly dark, will stain anything. Also quite dense.



[Edited on 14-6-2014 by Zyklonb]

Yeah, it's very messy to work with.
I made it from pure iron, hydrochloric acid and hydrogen peroxide.

It's reaction with a sodium carbonate solution is pretty cool looking if you add the iron chloride solution drop by drop to the carbonate solution.



[Edited on 14-6-2014 by Zyklonb]

3,4-O-Isopropylidene-D-mannitol, purity over 99% according to NMR analysis.

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.

pyranine solution in water under UV light

Violet hexamine nickel (II) chloride and Yellow dipotassium tetra chloro nickelate(II)

are they cool enough??

Very nice pictures everyone!
I like the yellow complex

6gr platinium metal

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

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.

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]

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. 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)

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

Some Sulfur dichloride I prepared yesterday. The ampule on the right is very contaminated with disulfur dichloride, but the other three are quite pure.

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?

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.

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

Crossing the road can also be messy and lethal if done incorrectly. And you won't film a video of how to cross the road (I thing). You should want to make the video because of the amazing chemistry going on, and all the complex thinking that designed the experiment

Received some hard to get chrysene. Here is 5mg in 3ml acetone under a blacklight. A neat and different fluorescent material! It is found in car exhaust, cigarette smoke and burnt BBQ foods I believe.
Quite carcinogenic and expensive. A small speck is seen in the bottom of the vial


[Edited on 22-6-2014 by Mailinmypocket]

KCl crystal I grew over the course of the last year and a half. ran out of room in the snapple tea bottle, destroyed the bottle to retrieve it. just mixed and set out for a long time, then put in with worn out CaCl₂ and checked periodically. turned out nice I think




pile of ammonium sulfate,... drying magnesium hydroxide,... some of the larger crystals of ammonium sulfate. I had made the magnesium hydroxide for a ceramic component. epsom salt and ammonia, MgSO₄ + 2 NH₄OH -> Mg(OH)₂ + (NH4)₂SO₄ and figured why not use my free dessicator( backyard) to salvage the ammonium sulfate also? I do already have 40#'s or so for the lawn in the shed, but better than down the drain. fertilizer and ceramic material, nothing to waste



[Edited on 22-6-2014 by violet sin]

The reaction of triphenylphosphine with lithium.

When adding lithium metal (those near shiny lumps floating over there) to a solution of triphenylphopshine in tetrahydrofuran, phenyl lithium and lithium diphenylphosphide will form (that orange colored thing at the surface of the lithium). The reaction will only happen if the solvent does not contain any water, but when it starts, the whole solution will turn blood red in a few minutes.

only camera I have since my digi broke is a crappy webcam *sigh*

Crude piperine being crashed out of isopropanol with ice cubes

Yes, extracted a quarter pound of "Safeway" brand ground black pepper. The oil is layering out nicely in the bottom of my beaker. Wish I had a better camera

Edit--Me, through a "rose" colored filter. Red rose pigment, aqueous extract dried on a glass plate



[Edited on 6-25-2014 by arkoma]

A sodium acetate solution made by boiling down vinegar & baking soda (hence the amber impurities).

benzoic acid from toluene. I should warn that it is important to limit exposure to toluene, as right now i feel dizzy and have headache. Manganese dioxide get absolutely everywhere too. Fun synth otherwise.





[Edited on 28-6-2014 by HeYBrO]

That's hilarious. Did she ask what it was ?
When and where did you get your rig?

Quote: Originally posted by arkoma

I had to ask my 19 year old niece WTF is this "XD" crap just last week.......

I didn't figure it out till a month ago lol, I don't have a phone (YOU can't track me murica, hahahaha!)

Quote: Originally posted by The Volatile Chemist

(YOU can't track me murica, hahahaha!)

Arkoma, what forum did you post that last bit about your rig in? I can't seem to access it

Quote: Originally posted by The Volatile Chemist

I didn't figure it out till a month ago lol, I don't have a phone (YOU can't track me murica, hahahaha!)

I don't have a phone either but hey, common it is used a lot on internet too !

Yea. I just meant they couldn't track my LOCATION every second by built in GPS, that's all

Concentrating rose hip extract (in acetone)

Cool, looks like you got your new camera.
Also, those duct-taped joints are looking great!