sharing Awesome Chemical Pictures (Read first comment)

Hi everyone
So i wanted to do a topic to share pictures of chemicals; interesting, expensive, rare, dangerous, synthetic, or what ever you want us to see.
I have the rather odd hobby of looking at new substances for quite a bit of time, and not to mention using it i think i'm not the only one. So i wanted us to share pictures so we can enjoy looking at things we don't have access to.
Here are the RULES:
1) Picture of a sample of compound
2) Attach a structure or formula or name o f the substance
3) If you like, a little explication of its uses
4) It must be a picture of a compound you own yourself. (woelen)



I'm starting !! Mercuric Cyanide Hg(CN)2
Double fun .. toxic mercury .. toxic cyanide ...uses ?? ... no idea realy :/



[Edited on 20-3-2019 by Chem Science]

I would like to add an additional rule: It must be a picture of a compound you own yourself.

I add a picture of a saturated solution of Cl2 in CCl4. Its color is much closer to the color of liquid chlorine than normal saseous chlorine, which is more green.




I made this by dissolving dried gaseous chlorine in pure CCl4, until no more gas could be dissolved. CCl4 dissolves quite some chlorine. I did not measure it, but it is many times the volume of liquid. According to solubility info I found on internet, a saturated solution of Cl2 in CCl4 will contain 7% to 8% by weight of chlorine. With a density of almost 1.6 grams per ml, this leads to roughly 0.11 to 0.12 grams of chlorine per ml of liquid. Gaseous chlorine has a density of appr. 0.003 grams per ml, so this solution has 35 to 40 times more chlorine per unit of volume and hence has a much stronger color.

I have no specific use for this sample. I use it as part of my element collection, displaying elemental chlorine at high concentration, without the need to have liquid (and hence highly pressurized) chlorine around. I chose CCl4 as solvent. This cannot react with Cl2 anymore, the solution is light-fast and stable on long-term storage.



[Edited on 20-3-19 by woelen]

Quote: Originally posted by Ubya

https://www.sciencemadness.org/whisper/viewthread.php?tid=26... There's already a thread to post pretty pictures

Yes but i want one of Reagents hehe (^.^)

Awesome sample woelen !! I edited the post and added your rule that yellow is beautiful

Quote: Originally posted by Chem Science

Quote: Originally posted by Ubya   https://www.sciencemadness.org/whisper/viewthread.php?tid=26... There's already a thread to post pretty pictures Yes but i want one of Reagents hehe (^.^)

Copper Citrate To make ultra fine copper powder. how ever the copper powder these gives is not pure, meaby these citrate is impure or the cooking i performed was bad.

Isatin .. for synthesis

A few more elements. I did not yet post them on my web page, they are fairly recent additions to my collection of elements:


A very pure sample of manganese, 99.99% purity, in an ampoule under Argon.





White phosphorus, little sticks, under water.

Harmine and harmaline hydrochloride crystals

Harmala alkaloids extracted from Peganum harmala (syrian rue) seeds, further purified by crystallization from brine.
These alkaloids are MAO inhibitors.
I further separate harmine and harmaline (DHH, dihydroharmine), the latter is further reduced to tetrahydroharmine (THH, leptaflorine) which is a weak SSRI with interesting benefits for central nervous system (could promote neuroplasticity).



[Edited on 23-3-2019 by nimgoldman]

Woow woelen That manganese seems awesome !!
i never heard of Harmine nimgoldman. very nice sample Awesome to see !!

Hi DraconicAcid .. haha there's always someone that has to do it wrong xD But it's not bad to smell lemon
Here are some Cobalt Complexes

Some Organic compounds The Nitrophthalhydrazide was synthesized by me

Some Inorganic chemicals

These two are very obvious when they are side by side like these

PETN and Gelignite when i was young and mad in science !



[Edited on 25-3-2019 by Waffles SS]

Wow nice pictures Waffles SS , first time looking at Pentaerythritol tetranitrate and Gelignite !! Here's some interesting stuff, Trifluoroacetic anhydride and bis(2,4,6-Tribromo)Oxalate

Trifluoroacetic anhydride. Something which still is on my wish list. I can buy it, but it is very expensive, so up to now I did not buy it.

This evening I made pictures of attractive samples, which I made myself. Many of the chemicals displayed here, I made myself. Some of them I purchased.

The uploads are in multiple posts.

The first picture is a mix of Br2 and Cl2. I made this by filling a bottle of 250 ml with carefully dried Cl2 gas and then adding a small amount of Br2. This Br2 then quickly reacts with Cl2 (it evaporates much faster than it normally does, because it reacts with Cl2, forming gaseous BrCl). The resulting gas is a mix of BrCl and excess Cl2.
With a syringe I took 30 ml or so and blew this into an ampoule, which I sealed. This is the golden yellow gas in the big ampoule. To the remaining gas, I added a few ml of CCl4 and swirled this around. The gas mix dissolves in the CCl4 and gives a bright red/orange solution. This bright red/orange solution is a solution of BrCl together with excess Cl2 in CCl4. I also ampouled this solution.
This set of ampoules nicely shows that BrCl is orange/red in thick layers (or in higher concentration) and that it is golden yellow in thinner layers. The liquid ampoule also shows the golden yellow color in the neck of the ampoule, where only a thin layer of liquid is viewed.





The two pictures below show the same ampoule, filled with K3Cr(C2O4)3.3H2O, but it shows how it looks like in fluorescent light and in tungsten light. In fluorescent light it looks dark purple, in bright tungsten light it looks green. In daylight it looks grey.

Some more interesting compounds:

Mercury sulfide exists in two forms. A black form and a red form. The first sample contains lumps of HgS, which are pieces, containing both the black form and the red form. These are from a natural source.



The HgS, shown in the picture below is synthetic, both samples are pure and nicely demonstrate that this compound exists in two forms. Both forms are remarkably inert and do not dissolve in water, nor in strong acids.







Arsenic also forms interesting sulfides. There are two well-known sulfides, As2S3, knows as orpiment, and As4S4, known as realgar. Pure powdered As2S3 is golden yellow. Pure crystalline As2S3 is golden/yellow, with a greyish/brown tinge and a high polish. Such pure crystalline samples are rare and expensive. More mundane sample usually are not shiny and have orange or red streaks in them, being As4S4 impurities. Sometimes, natural As2S3 also contains white quartz, but that can easily be recognized, and that is easy to remove, because quartz is MUCH harder than As2S3. The picture below shows three crystals of As2S3, containing small amounts of As4S4, which make the crystals appear somewhat orange instead of yellow.






The final two pictures in this post show very pure WO₃ and WO_3-x, with x appr. equal to 0.1, meaning that it is WO3, which is slightly deficient in oxygen. It is well known that WO3 can be deficient in oxygen and if it is, this has a very strong impact on the color. Very pure WO3 is pale yellow (color like sulphur, but slightly paler), but even a percent of oxygen deficiency leads to strong coloration in the blue part of the spectrum. The color is very intense and hence the material is nearly black.





[Edited on 25-3-19 by woelen]

This is my recently acquired sample of cesium metal. It is large, a full 10 grams of metal.






This is some home-made PBr5, put in an ampoule. PBr5 is a very nasty chemical, which only can be stored indefinitely in a glass ampoule. It eats any cap, even the PTFE-lined GL45 red caps. It heavily fumes in contact with air. I made it and quickly ampouled it, I did not do any further experiments with it.






Below is a sample of P.A. grade FeSO4.7H2O. Normally, the material you buy is more like a dull grey/green, but the pure chemical has a very fine mint green color. In air, it quickly loses its beautiful color, due to oxidation by oxygen in air. For this reason I ampouled some om my FeSO4.7H2O to keep a rare and beautiful sample. For experimental purposes, one can better use (NH4)2SO4.FeSO4.12H2O, which has much better storage properties than FeSO4.7H2O.







The final two pictures are ethylene diamine complexes of copper(II) and nickel(II). I made the copper(II) complex by dissolving as much as possible of copper(II) oxide in 35% perchloric acid. I allowed the liquid to settle and decanted the blue solution of copper(II) perchlorate. To this I added a 30% solution of ethylene diamine in water, until. First you get a precipitate of copper(II) hydroxide, but on addition of more ethylene diamine, this redissolves. I added two more drops of ethylene diamine solution and then put the solution aside and let it slowly evaporate, until I had a nice crop of crystals. I did not let it evaporate to dryness. I decanted the liquid from the crystals, carefully dried the crystal mass in a coffee filter and then let the mass dry in warm air. The dark purple crystals are the copper complex, Cu(en)2(ClO4)2.

The nickel complex was made by dissolving a soluble nickel salt in water and precipitating this with a solution of NaOH. This gives a precipitate of Ni(OH)2, which on boiling for a while becomes coarser and easier to filter. I did not dry the Ni(OH)2, I simply rinsed it with water and then I dissolved it in as little as possible of 35% HClO4. To this solution I added 30% solution of ethylene diamine in water. First you get a precipitate again, next you get a dark blue liquid and finally you get a purple liquid. To this purple liquid I added a few more drops of ethylene diamine and then I let this evaporate and worked up the crystals just as for the copper complex. Again, I did not evaporate to dryness.

Both complexes form nice crystals and can be obtained perfectly dry in the form of beautiful free flowing crystals. I ampouled both chemicals, because they make very attractive display samples.

Woooww !! Awesome samples woelen Nice Interhalogens !! I did not know about the WO(3-x), i have WO3 can i make WO(3-x) ?
That PCl5 is super nice !! i envy the fact that you make it your self !!
That Cesium ... yeah that's an Element <3 never actually seen in real life cesium It's always nice to see pictures It's my first time looking at K3Cr(C2O4)3.3H2O, nice sample !! what is it used for ?
Okay .. it's difficult to keep up, let's see if you like these next samples

So First is Hematoporphyrin Dihydrochloride al 75% Then we have the Precursors and actual 2,4.Dinitrophenylhydrazine and last is 1,5-Diphenylcarbazide

Copper nitrate form a silver refining process, left the beaker aside an this single beauty grew.
Sadly I do not have better pictures as I gave it away as a present a year ago.

Quote: Originally posted by DrScrabs

Copper nitrate form a silver refining process, left the beaker aside an this single beauty grew. Sadly I do not have better pictures as I gave it away as a present a year ago.

That looks like sulphate instead

Nice crystal !!! DrScrabs, super nice. The best gif you can give to someone
here's some other samples.

Quote: Originally posted by Chem Science

These two are very obvious when they are side by side like these

Quote: Originally posted by monolithic

Quote: Originally posted by Chem Science   These two are very obvious when they are side by side like these Is one of them an aldehyde? [Edited on 27-3-2019 by monolithic]

Here are some more compounds





[Edited on 27-3-2019 by Chem Science]



[Edited on 27-3-2019 by Chem Science]

Here are some FLuorine Organic Compounds !!

From left to right, ZnS:Ag, ZnS:Mn, ZnS:Cu phosphors that I synthesized recently.

The ZnS:Ag emits a blue glow, but is so faint that the camera doesn't pick it up. I'm still trying to figure out what's wrong (maybe it's not that sensitive to 400nm UV light?).

The ZnS:Mn has been made with likely Fe-contaminated MnSO4, and has many dead spots. I'll need to recrystallize the MnSO4 and try again.

Nice phosphorescent powders beta 4 i had a funny experience with Zn and Cu .. the first time i made it, it worked .. ten times later i was never able to replicate .... i have to try again. any suggestions ? How did you make yours ? i made mine with Sulfur, zinc and copper powder ignition. Like i said it worked the first time, but never again F*** my luck

Fluorescence indeed is very interesting. I also tried making ZnS:Cu from Zn, S and Cu, but the stuff I obtained is very impure. It is a dark brown solid. Pure ZnS should be white, or pale yellow (??). With some copper included I would expect it to become brown or green (CuS is nearly black, very dark brown). Maybe I should use very fine copper powder. My copper powder probably is too coarse (65 micron particles). Anyway, the stuff I made does not show any fluorescence.

Years ago, someone donated me a small display sample of depleted uranyl nitrate (too little to do actual experiments with it, but very nice as remarkable display sample). This shows fantastic fluorescence under black light.

I do have some Uranium glass aswell but don´t want to isolate Uranium in any state. Did not find any place wich accepst radiocative waste, also caontamination of my lab space is unacceptable in that way. Beeing happy with UV glowing glass marbes
And yes I am very jelous of the compounds posted before!

Edit: writing

[Edited on 29-3-2019 by DrScrabs]

If someone is interested in making ZnS:Cu, I posted the procedure and an helpful reference in this thread https://www.sciencemadness.org/whisper/viewthread.php?tid=14....

From my little experience it's key to start from very pure materials. ZnS can be made as described in the Brauer by bubbling H₂S in an acidified ZnSO₄ solution, but I decided to just buy lab grade ZnS to avoid messing with H₂S.

The copper sulfate was tech grade but I recrystallized it, and the ammonium chloride was made from household reagents but has been recrystallized three times.

And given this is a thread about reagent pictures, here's a photo of some of my undoped ZnS starting material. I can confirm it's perfectly white.



@woelen: nice fluorescent sample. Does it have an afterglow?

Here are some nice stuff

Wow Chem Science, that ruthenium complex is on my list of compounds I want to synthesize, someday. It can be used to make OLED displays.

By the way, the oxalate in your next post looks structurally similar enough to TCPO, maybe it can be used to make a glow stick reaction.

Here are my pictures: triple recrystallized ammonium chloride (white), and copper acetate (dark green).

yes the TCPO like compound react similar to TCPO .. NileRed has a video about it[https://www.youtube.com/watch?v=Zn61XAGgJA0] I want to make OLED'S but have not get to that point.
Thar Copper Acetate is Nice !!Ammonium chloride is fairly common, but when it's triple recrystallized ammonium chloride, That gives it Power

Sorry, not the best quality of the image. But the PhNHNH2.HCl is triple recrystallized from EtOH and got a nice treat with activated C.
Made by the NaSO3/SO2 reduction(SnCl2 is bs here IMHO), If there is some interest I can post the synthesis next time I make some

MnSO₄ made by reacting Mn powder with sulfuric acid. The pure compound should be white, so mine has some impurities.

Amazing that PhNHNH2.HCl Very nice crystals !! Plis post your synthesis

Quote: Originally posted by DrScrabs

Sorry, not the best quality of the image. But the PhNHNH2.HCl is triple recrystallized from EtOH and got a nice treat with activated C. Made by the NaSO3/SO2 reduction(SnCl2 is bs here IMHO), If there is some interest I can post the synthesis next time I make some

Quote: Originally posted by Tsjerk

Is yours very fluffy? I have a commercially bought sample and it is very voluptuous. Like 0.3 grams filling a cubic centimeter.

Here follow pictures of a few compounds I made at home:


This is potassium, I made according to POK's method, first posted on the German forum Versuchschemie.de. This forum unfortunately does not exist anymore.





The following is KCrO3Cl, I made from K2Cr2O7 and conc. HCl.





The next one is N(CH3)4ICl4. Normally, salts of the complex ion ICl4(-) are not very stable and this compound easily loses ICl3 so that a simple chloride remains behind. With the big cation N(CH3)4(+), however, it forms a stable salt.





The final one is KVO4 (the yellow stuff) and KVO3 (the white stuff), made from V2O5 and KOH and H2O2.

Crude phenylhydrazine sulfate, thread coming tomorrow

Quote: Originally posted by DrScrabs

Crude phenylhydrazine sulfate, thread coming tomorrow

Quote: Originally posted by Tsjerk

Quote: Originally posted by DrScrabs   Crude phenylhydrazine sulfate, thread coming tomorrow Nice! Do you know why it is reddish?

Oxidation maybe.






Iodine from NaI + KHSO5, molten under H2SO4, forms a nice on cooling crystalline layer without I2 fumes!

Quote: Originally posted by DrScrabs

Iodine from NaI + KHSO5, molten under H2SO4, forms a nice on cooling crystalline layer without I2 fumes!

Quote: Originally posted by Ubya

do you have any problems with sulphuric acid bubbles in the solid I2 mass?

Here are some Manganese Chloride I synthesized a few years ago.
There might be a bit of iron contamination, because that was produced from "pottery grade" Manganese Carbonate, and hardware store HCl. But I doubt it because it has the proper color (I synthesized MnCl2 from regular C-batteries a few years back and it had a orange-ish tint)

Hello.

I made some solution of sodium hypomanganate cca 8 months ago. I am really interested in manganese chemistry and I prepared every oxidation state from II-VI from KMnO4. But hypomanganate is really unstable and rare. This makes him really exotic compound.

I made him by reduction of KMnO4 by Na2S2O3 in 48% NaOH. All reagents was cooled in fridge before reaction because hypomanganates are more stable in lower temperatures. In to the solution of 48% NaOH I added few drops of 25% solution of Na2S2O3.5H2O (Na2S2O3 isn't dissolve in water, but in 20% NaOH). Then I added few drops of dilute aqueous solution of KMnO4. Colour of solution has turned in to green by presence of manganate. I returned solution in to the fridge and after ten minutes solution turned colour in to turquoise by presence of hypomanganate. Solution was little bit cloudy, because some NaOH in solution crystallized in the fridge before reaction.

On the internet I found that this compund have really interesting formula Na3MnO4.0,25NaOH.12H2O.

I plan to repeat this reaction in future and test how long solution stays turquoise and some redox chemistry with ethanol and acetone.

In the picture is solution of hypomanganate next to solutions of manganate and permanganate for comparison of colour MnO4(n-).

Sorry if my english is bad. I'm trying as much as I can writing correctly.





[Edited on 15-4-2019 by Bedlasky]

[Edited on 15-4-2019 by Bedlasky]

[Edited on 16-4-2019 by Bedlasky]

I made few experiments until it's finally working. First few experiments stopped on manganate. It needs very strong alkaline media and low temperature.

If you want to try prepare hypomanganate in solid I have read something about this in one document (but it's only in Czech ). Author made hypomanganate from K2CO3, MnCO3 and dry air (dried over conc. H2SO4) at 800°C. The reaction leasted 60 hours. But hypomanganate wasn't pure - the yield was 56,9% (impurities was MnO2 adn K2MnO4). Hypomanganates is very water sensitive. Trace of water in the air leads to disproportionation to MnO2 and K2MnO4.

[Edited on 17-4-2019 by Bedlasky]

Over the years I have accumulated a few pictures of unusual chemicals. Here are 4 I have taken over the years.
1. is Selenium dioxide crystals.
2. is a selection of phosphorus samples.
3. is Neodymium sulphate.
4. is Praseodymium sulphate.

And of course Europium 3+ in alkali fluorescing under a UV laser.

All of these samples are very nice, but the white phosphorus and the europium are really outstanding.
My white P is not transparent, it is more like off-white wax. I have seen such pure white P once before, made by Endimion17 some years ago.

I myself did a little experiment and made a few pictures again, which also may be interesting. A small experiment, dissolving some I2 in CCl4, which gives a nice purple solution. The picture shows a still very dilute solution, which best demonstrates the color.




Finally, I had a very dark purple solution. To this, I added a little amount of red P and swirled for a minute or so. The I2 reacts with the red P (which was in excess). This leads to formation of the red compound PI3, which also is soluble in CCl4 (but only sparingly so).





I ampouled some of this solution. This solution is quite nasty, it fumes in contact with humid air. These fumes are from HI, formed by reaction of water vapor in air with PI3, dissolved in CCl4.

I ampouled some PI3, dissolved in CCl4 to make a more permanent display:





Making more PI3 in this way is not easy, because its solubility in CCl4 is not that high. Also the solubility of I2 in CCl4 is not superb.

I also have a small sample of the solid compound (made with CS2 as a solvent which has much better solubility properties) and ampouled this in a 20 ml ampoule to keep it good. It is very air-sensitive and cannot be kept around in a normal bottle (it is very corrosive, like PCl5, PCl3 and PBr3, and eats caps and besides that, it gives nasty brown stains on anything nearby). I made the glass ampoule a few days ago and now it is safely stored and makes a nice display:

Another nice sample, this one is appr. 25 grams of reagent grade BBr3. This I purchased as shown. I did not ampoule this myself. Making BBr3 at home is very difficult, boron and Br2 do not react at room temperature. Making this compound requires the use of very high temperatures.



Pure BBr3 is colorless, but commercial samples always contain a little free bromine, giving a brown/orange color.

[Edited on 17-4-19 by woelen]

The crystals of neodymium and praseodymium sulphate have really nice colours . Europium is also very nice. The sample of white phosphorus is very interesting - I've never seen sample like this.

Purple colour of iodine solution reminds me school labs - determining of partition coefficient. PI3 have nice colour .

Quote: Originally posted by Bedlasky

Hypomanganates is very water sensitive. Trace of water in the air leads to disproportionation to MnO2 and K2MnO4. [Edited on 17-4-2019 by Bedlasky]

Quote: Originally posted by Bedlasky

Hypomanganates is very water sensitive. Trace of water in the air leads to disproportionation to MnO2 and K2MnO4. [Edited on 17-4-2019 by Bedlasky]

Quote: Originally posted by fusso

Wait so how did you make a soln of MnO4 3-?

Quote: Originally posted by Bedlasky

Hello. I made some solution of sodium hypomanganate cca 8 months ago. I am really interested in manganese chemistry and I prepared every oxidation state from II-VI from KMnO4. But hypomanganate is really unstable and rare. This makes him really exotic compound. I made him by reduction of KMnO4 by Na2S2O3 in 48% NaOH. All reagents was cooled in fridge before reaction because hypomanganates are more stable in lower temperatures. In to the solution of 48% NaOH I added few drops of 25% solution of Na2S2O3.5H2O (Na2S2O3 isn't dissolve in water, but in 20% NaOH). Then I added few drops of dilute aqueous solution of KMnO4. Colour of solution has turned in to green by presence of manganate. I returned solution in to the fridge and after ten minutes solution turned colour in to turquoise by presence of hypomanganate. Solution was little bit cloudy, because some NaOH in solution crystallized in the fridge before reaction. On the internet I found that this compund have really interesting formula Na3MnO4.0,25NaOH.12H2O. I plan to repeat this reaction in future and test how long solution stays turquoise and some redox chemistry with ethanol and acetone.

Quote: Originally posted by maxstar

Again, dark blue sediment appears.

I made K2Cr3O10 and ampouled this.


I made this chemical by dissolving K2Cr2O7 and some CrO3 in boiling hot highly concentrated HNO3 (70% or so, maybe even a little more). The nitric acid I made by distillation from H2SO4 and KNO3 and a little water to make really concentrated acid. In such concentrated acid an amazingly large amount of K2Cr2O7 can be dissolved and when that is done, then it also is possible to dissolve some CrO3 in it as well. In order to do so, the liquid must be boiling hot, otherwise you don't get all of it dissolved.

After that, I put the flask with the acid and dissolved chromium compounds in a hot water bath, which I slowly let cool down. The next day I had a big crop of beautiful red K2Cr3O10. I put this on a glass fritte and used some paper tissue on the other side of the fritte to absorb the acid and any CrO3 which still is dissolved in it. This was quite scary, the acid with CrO3 is a very harsh oxidizer and after ten seconds or so, the paper tissue with acid soaked in it starts to fume and hiss. So, I had a bucket with water nearby and dumped the paper tissue with absorbed acid in that immediately. I repeated this procedure until no more acid could be absorbed in paper tissue. At this point, the solid already was quite dry.
Next, I put the solid in a petri dish and put it in an oven at 100 C for 20 minutes or so. I finally put the petri dish in a plastic jar, in which I also put a small dish, full of NaOH. This absorbs acid vapor and after several days I had a perfectly dry product, which could be ampouled nicely.

Below follow pictures of the ampouled product on a white background and on a black background:








I also made pictures where the compound is kept near the container of my K2Cr2O7. These pictures nicely show the difference between K2Cr2O7 and K3Cr3O10.





Once the K3Cr3O10 is completely dry and free of acid, it is not hygroscopic anymore, and it can be kept around very well. I will use this sample in my element collection as an addon to the chromium sample (together with Cr2O3, CsCr-alum, K2CrO4, K2Cr2O7).


[Edited on 18-5-19 by woelen]

Interesting compound with beautiful colour. Sadly I saw this compound only on pictures .

Hi.

Here is photo of one of my crystals of ammonium-ferric sulfate. Crystal weight is 37,7g. On photos has beautiful pale violet colour but currently is transparent on edges (but middle is still pale violet) and surface is little bit rusty but it doesn't become rusty even more. I store it in paraffin oil to prevent water losses (on the air it lose water and becomes rusty).

Figure 1: I started stockpiling orange peels in my freezer, telling myself that I'd steam distill them some day. By the time the freezer was full & I got around to the project, I had 2.63 kg hoarded.


Figure 2: When I was done, I had 41.80 g of orange oil collected, for a dry mass percent of ~1.6% oil. I measured its density as 0.837 g/mL.

Also, my house smelled like Froot Loops the whole time

Quote: Originally posted by woelen

That's interesting. How much solvent did you need for this extraction? And what solvent did you use? Did you recover the solvent by distilling it off and using it again? Could you provide some more details on how the extraction was done? Another question I have is what you can do with this orange oil? Does it have some specific interesting chemical properties, which can be used in nice chemical experiments?

I hope he used steam distillation, it's relatively fast, in one morning I processed about 1kg of peels in a few batches, using a solvent would require lots of it (just to cover the peels) and even more for washings, the beta carotene would also be extracted so a distillation is mandatory. Meh steam distillation is better
The oil should be mainly limonene, it's used as a solvent

Quote: Originally posted by mayko

Got some orange peels steam-distilling, no broken glassware yet!

Yep, this was a steam distillation... actually several. I've never really gotten the hang of the technique so I decided to just do it over and over for practice. I hadn't thought as far ahead as a use for the orange oil! I might mix some with alcohol and spray it on paper to make scented stationery for my letter writing.

In the process I learned that orange oil is produced industrially from the waste from orange juice production by pressing rather than steam distillation.

Here's some Uranyl Nitrate sample and Thionyl Bromide

shouldn't uranyl nitrate be UO2 (NO3)2?
is that an uranium (IV) (with oxygen!?) nitrite?
i think you messed up the formula a bit

@Chemscience how much is that?

Quote: Originally posted by fusso

@Chemscience how much is that?

Just enough to convince me to get my own !

Oh please do post a picture in UV light

Fresh made Picric acid drying out befor being converted to Ammonium Picrate

https://en.wikipedia.org/wiki/Picric_acid

https://en.wikipedia.org/wiki/Dunnite





Some Iron 2 Sulphate for a 1,4, Dioxan synth I have planed along side some Copper Nitrate



[Edited on 3-6-2019 by XeonTheMGPony]

Ups ... Sorry Yup i did messed up the formula jej e.. Sorry .. Nex post is on UV for Herr Haber and the correct formula =) .. btw nice Ferrous Sulphate.I'm very interested in your synthesis of Dioxane, so i'm expectant for the post

Here's 20gr of Uranyl Nitrate in UV light

Quote: Originally posted by woelen

That sample of uranyl nitrate is beautiful. @Ubya: Uranyl ion has uranium in its +6 oxidation state. The ion is UO2(2+) and the nitrate salt is UO2(NO3)2.

yup i know, i was messing around trying to interpret the wrong formula

@chem science: beautiful sample, uranium is one of my favourite elements, if not the most

6-Monodeoxy-6-monoazido-beta-cyclodextrin synthesized via refluxingMono-6-O-(p-toluenesulfonyl)-β-cyclodextrin and sodium azide in an aqueous solution..
Used as synthetic intermediate. The azide is reduced to make 6-Monodeoxy-6-monoamino-beta-cyclodextrin or used in click chemistry to attatch subsituted functional groups which can be used to bind/trace movement in vivo. One example is performing an amidation reaction between the amino-cyclodextrin and biotin( biotinylation). When tested on mice, the movement of the cyclodextrin within the cell can be traced by introduction and binding of streptavidin or avidin. Cyclodextrins can act as "cages" for molecules such as steroids and facilitate drug delivery. B-cyclodextrin itself is combined with DMSO and a specific therapeutic drug to permit effective drug delivery through cellular walls.

some tetraphenylcyclopentadienone made at uni

AvB you are totally right, my bad.



ps can't edit my last post (can't edit any of mesagges on this thread but this one, the button is not there, wtf?)

[Edited on 14-6-2019 by Ubya]