Sciencemadness Discussion Board

Pretty Pictures (2)

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Zyklon-A - 17-3-2014 at 13:42

Looks like caramel to me.

Hegi - 17-3-2014 at 22:37

Quote: Originally posted by DraconicAcid  
Is that a mineral, or an oddly-shaped piece of chocolate?


It´s vanadinite :D

kristofvagyok - 17-3-2014 at 23:04



3,2,1, bang!

A gram of hexanitromannite initiated with some lead styphnate photographed just when it exploded.

The experiment was part of chemistry safety classes when the students learnt about how to handle explosives and other compounds. The audience was protected by a plexiglass shield and noone got hurt, besides the plastic bottle with full of water what was next to the explosive.

Zyklon-A - 18-3-2014 at 10:22

Wow, kristofvagyok , that looks great.

Not very pretty, but I just found a nice length of copper power wire on my street. I haven't taken off the insulation, but the whole chunk weighs 470 grams. I'm assuming that ~80% of it is copper, so I might get about 376 g's from it.:D


PICT0007.jpg - 195kB

DraconicAcid - 18-3-2014 at 12:17

Quote: Originally posted by Zyklonb  
Wow, kristofvagyok , that looks great.

Not very pretty, but I just found a nice length of copper power wire on my street. I haven't taken off the insulation, but the whole chunk weighs 470 grams. I'm assuming that ~80% of it is copper, so I might get about 376 g's from it.:D


The copper used for electrical wire is very pure, and the insulation probably doesn't weigh very much.

Zyklon-A - 18-3-2014 at 12:39

I know, it's an excellent source. I wonder where it came from, there were no power line near where I found it. Especially no broken lines. Copper thieves dropped it perhaps....:) Probably not.
I used to have to strip other electrical wire lying around for my copper, but this will last a long time.

MrHomeScientist - 18-3-2014 at 12:44

I found a similar piece of wire in an empty lot near my house, except it was made of aluminum. It should also be very pure! My neighborhood has a lot of construction going on, so I'm always hunting around the sites for scraps :)

EDIT: Hegi, I've never seen vanadinite that color before - it's always orange or red. Do you know why yours is different?

[Edited on 3-18-2014 by MrHomeScientist]

HgDinis25 - 18-3-2014 at 14:20




It's just some small scale Iodine extraction, not that fantastic or anything but I like the colours xD

violet sin - 21-3-2014 at 21:40

I built a little electroplating set up recently. thought I'd share as it is cheap and easy to make. haven't done a whole lot of work with it yet, but it's currently refining sterling scrap.
main components:
1- DC-DC stepdown transformer, http://www.ebay.com/itm/LM2596-DC-DC-Buck-Converter-Constant...
1- DC digital ammeter/voltmeter, http://www.ebay.com/itm/141164937042?ssPageName=STRK:MEWNX:I...
and some simple stuff,.. A shallow light switch box( 1.25$), piece of plexiglass, a small piece of terminal strip, some wire and a stand to attach it to... and a wine cork( generic non-conductive backing for adj. step-down board positioning)

0318142008.jpg - 75kB 0319140234a.jpg - 62kB 0321141230.jpg - 46kB 0321141230a.jpg - 44kB 0321141506.jpg - 89kB

pic 1) laid out the parts: stand, switch box, plexi and the new V/A meter
pic 2) assembled unit
pic 3) attached to the stand.
pic 4) side view, short foot on the display side, and long foot opposed it rests nicely under the plating tank to secure the stand from falling.
pic 5) action shot on initial run. in this one you can see the stainless spill tray, the stand and control unit with the silver cell peaking out behind it( in a plastic bowl for shock/spill hazard) a small glass bowl to set sterling electrode while looking, and a second plastic cover to keep debris out while cell is down.

the DC-DC stepdown unit is adjustable, and the adj. screws are set in the plexi face plate. it can be powered by a wall-wort( AC adapter > 5V), and tuned down within a given range of the supply voltage. the amperage control isn't that great. it floats up/down quickly with voltage adj. but your amperage adj. by itself has a short leash.

total cost to me ~15$ and a few hours works, as I already had spare project materials around. the actual cell is a single wall stainless steel travel coffee mug with handle and all plastic taken off. the lid is some sort of PVC gutter/drain pipe cover( ~1$ ace ). any tighter and the lid wouldn't fit. I'll have to put a few days through it and see how she handles, hopefully well.

plexiglass is a bitch to work with some times. or mine was just really brittle. I broke 2 pieces making the face plate. that was probably the single most time consuming aspect.

Hegi - 22-3-2014 at 03:02

Quote: Originally posted by MrHomeScientist  
I found a similar piece of wire in an empty lot near my house, except it was made of aluminum. It should also be very pure! My neighborhood has a lot of construction going on, so I'm always hunting around the sites for scraps :)

EDIT: Hegi, I've never seen vanadinite that color before - it's always orange or red. Do you know why yours is different?

[Edited on 3-18-2014 by MrHomeScientist]


I have no idea... I did not study it... :/

Potassium ferrioxalate crystals



And a little bit of analytical chemistry. Complexometric titration of Cu2+


BromicAcid - 22-3-2014 at 05:44

Quote: Originally posted by violet sin  
I built a little electroplating set up recently. thought I'd share as it is cheap and easy to make. haven't done a whole lot of work with it yet, but it's currently refining sterling scrap.


Love it, hopefully I see a lot of work come out of that apparatus :) There is such a low barrier to entry for electrochemisty and a vast number of experiments to be performed, I wish I saw more of it on this forum.

Töilet Plünger - 22-3-2014 at 17:44

Hegi, what reagents were used in the titration? And you should take pictures of the ferrioxalate in UV as well!

Hegi - 22-3-2014 at 23:32

Quote: Originally posted by Töilet Plünger  
Hegi, what reagents were used in the titration? And you should take pictures of the ferrioxalate in UV as well!


Definitely should but do not have UV right now... chelaton III as titrant and murexide as indicator were used :)

MrHomeScientist - 25-3-2014 at 17:03

Potassium nitrate crystals freshly decanted from their solution. I really liked how they formed this starburst pattern in the upper part of the beaker!


1.jpg - 143kB

Mailinmypocket - 28-3-2014 at 13:42

Came across a time lapse video (done on an iphone) of the Belousov-Zhabotinsky reaction in a petri dish using ferroin. Its not crazy good but the effect is neat.

https://www.youtube.com/watch?v=qFgnDs9GZj0

Zyklon-A - 28-3-2014 at 16:55

By "came across", you mean "uploaded"?:D

Mailinmypocket - 28-3-2014 at 17:07

Came across a video I uploaded a long time ago while looking at my YouTube account ;) is what I should have said. I plan on making a nicer one now that I have a better camera and apps for this type of filming. I have a few indicator mixes if like to try as well including a fluorescent one, so, we shall see how that works out

[Edited on 29-3-2014 by Mailinmypocket]

O-alkyl dithiocarbonates

Metacelsus - 28-3-2014 at 17:36



KiPrX recrystallization.jpg - 140kB iPrXA.jpg - 177kB

[Edited on 29-3-2014 by Cheddite Cheese]

Mailinmypocket - 29-3-2014 at 10:57

Just some chromium compounds


Chemistry_Keegan - 29-3-2014 at 17:02

Sodium aluminate crystals that formed over a course of several weeks after all the water evaporated on it's own :)

Sodium Aluminate.JPG - 72kB

BromicAcid - 29-3-2014 at 17:03

Quote: Originally posted by Mailinmypocket  
Just some chromium compounds


So pretty, they look like artist pigments. I believe at one time some oxidizing agents were used as pigments but the medium doesn't tend to hold up well to oxidizing agents.

Zyklon-A - 29-3-2014 at 21:09

I just got some potassium dichromate as well, I will post a picture of some nice big crystals as soon as I can make them, until then, it looks the same as Mailinmypocket's.

NeonPulse - 30-3-2014 at 02:35

Re-crystallizing some Trinitrophenol. Got a nice crop of well formed needle shaped crystals in the beaker....
:) i see alot of the pics here are of some type of crystalline formations. the silver metal on the copper wire look pretty neat. i tried the same but could not get decent close up pics.
picric crystals2.jpg - 75kB

Hegi - 31-3-2014 at 08:12

Quote: Originally posted by NeonPulse  
Re-crystallizing some Trinitrophenol. Got a nice crop of well formed needle shaped crystals in the beaker....
:) i see alot of the pics here are of some type of crystalline formations. the silver metal on the copper wire look pretty neat. i tried the same but could not get decent close up pics.


What solvent did you use? ... I prepared today few grams of TNP and then dissolved it in warm ethanol.. so now I´m waiting for crystals..

Chromuim Chemistry

Zyklon-A - 31-3-2014 at 09:03

Interesting color reaction:
Control: water
#1 reaction: water with 5 drops 3%H2O2
#2 reaction: water with 5 drops 3%H2O2
+ 5 drops 30%HCl
~50 mg potassium dichromate is added to each tube.
Control is on the right, #1 reaction in the middle and #2 reaction on left.

DSC01634.jpg - 95kB 10 seconds after addition. DSC01635.jpg - 95kB 2 minutes after addition. DSC01636.jpg - 73kB 5 minutes after addition. DSC01637.jpg - 81kB 10 minutes after addition.

[EDIT] Now 15-20 minutes after the last picture was taken, #2 reaction tube is nearly colorless, a bit of unreacted potassium dichromate has settled on the bottom, but the solution is very pale blue. The camera doesn't pick it up very well, it's slightly more colored then the picture shows.

[Edited on 31-3-2014 by Zyklonb]

DSC01638.jpg - 84kB

Iron(II) sulfate heptahydrate

Hegi - 31-3-2014 at 11:47

Been recrystallizing 1 kg of this compound and got nice crystals.. for more click here IRON SULPHATE CRYSTALS

<img src="http://chem.pieceofscience.com/wp-content/uploads/2014/03/2.jpg" width="900" height="597">

copperastic - 31-3-2014 at 11:57

How did you do this? I tried making crystals from iron II sulfate and the solution turned yellow. Im guessing from dissolved oxygen.

Brain&Force - 31-3-2014 at 11:58

Beautiful, Hegi, just beautiful! I tried making iron sulfate through replacement of copper sulfate and my crystals turned out a more greenish color rather than this aqua color.

kristofvagyok - 31-3-2014 at 14:40










After long-long time one of my compounds crystallized out. Sadly according to the recorded NMR spectra we are still not able to tell what is in the flask, but it still looks great.

Hegi - 31-3-2014 at 21:04

Quote: Originally posted by Brain&Force  
Beautiful, Hegi, just beautiful! I tried making iron sulfate through replacement of copper sulfate and my crystals turned out a more greenish color rather than this aqua color.


try to dissolve it in near boiling distilled water and add few milliliters of concentrated sulphuric acid, then let it overnight in fridge and you should be able to get that color. I´v been surprised too cause whenever I saw it before it was oxidized or rather hydrolyzed. ;)

Kristof - what is it suposed to be? ..

NeonPulse - 1-4-2014 at 01:26

Quote: Originally posted by Hegi  
Quote: Originally posted by NeonPulse  
Re-crystallizing some Trinitrophenol. Got a nice crop of well formed needle shaped crystals in the beaker....
:) i see alot of the pics here are of some type of crystalline formations. the silver metal on the copper wire look pretty neat. i tried the same but could not get decent close up pics.


What solvent did you use? ... I prepared today few grams of TNP and then dissolved it in warm ethanol.. so now I´m waiting for crystals..


I only dissolved the raw TNP in boiling distilled water to get a super saturated solution and very slow cooling the crystals grow as it cools. no solvent needed here. there are few helpful threads in the EM forum on this.

HgDinis25 - 1-4-2014 at 11:58






My sample of bismuth. Love that metal.

Zyklon-A - 1-4-2014 at 12:12

Made from this? https://www.youtube.com/watch?v=uRyPG6iJyjI

numos - 1-4-2014 at 19:49

Reaction between ~3gm pyrotechnical grade Aluminum powder, and ~8-10 drops of Mg2O7.
Reaction delay: ~22 seconds

I put a series of pictures taken within 5 seconds. (Excluding first and last, to show start/end)

1.jpg - 119kB 2.jpg - 105kB

3.jpg - 10kB 4.jpg - 63kB 5.jpg - 44kB 6.jpg - 50kB 7.jpg - 52kB 8.jpg - 63kB 9.jpg - 74kB

Oscilllator - 5-4-2014 at 21:12

magnesium heptoxide?
I doubt it

numos - 5-4-2014 at 23:46

Quote: Originally posted by Oscilllator  
magnesium heptoxide?
I doubt it


Why do you doubt it? I'm not the best at videos, so I went for screenshots of the video, but just for you, I'll upload the video - which should clear any doubts.

http://youtu.be/h4AuUNRXo-o

BlackDragon2712 - 6-4-2014 at 22:13

Quote: Originally posted by numos  
Quote: Originally posted by Oscilllator  
magnesium heptoxide?
I doubt it


Why do you doubt it? I'm not the best at videos, so I went for screenshots of the video, but just for you, I'll upload the video - which should clear any doubts.

http://youtu.be/h4AuUNRXo-o


'cause maybe you meant manganese heptoxide? Mn2O7?

numos - 6-4-2014 at 22:43

Quote: Originally posted by BlackDragon2712  
Quote: Originally posted by numos  
Quote: Originally posted by Oscilllator  
magnesium heptoxide?
I doubt it


Why do you doubt it? I'm not the best at videos, so I went for screenshots of the video, but just for you, I'll upload the video - which should clear any doubts.

http://youtu.be/h4AuUNRXo-o


'cause maybe you meant manganese heptoxide? Mn2O7?


oopsies... Your right. My bad. I feel silly, Mg and Mn:\



[Edited on 4-7-2014 by numos]

HeYBrO - 7-4-2014 at 01:03

I thought I'd try some Kristof/Hegi style photography... came out ok haha. Here is some Benzoic acid that i made by oxidising toluene via KMnO4

Benzoic acid.png - 544kB

[Edited on 7-4-2014 by HeYBrO]

Hegi - 7-4-2014 at 10:50

Quote: Originally posted by HeYBrO  
I thought I'd try some Kristof/Hegi style photography... came out ok haha. Here is some Benzoic acid that i made by oxidising toluene via KMnO4


nice try bro... I love that oxidation... fast and cheap way to produce your own benzoic acid..




HeYBrO - 7-4-2014 at 13:33

Quote: Originally posted by Hegi  


nice try bro... I love that oxidation... fast and cheap way to produce your own benzoic acid..



Thanks. I was going to edit the contrast and sharpness but i though against it. Looks much better, cheers. :)

[Edited on 7-4-2014 by HeYBrO]

kristofvagyok - 10-4-2014 at 14:59







Something special crystallized at the bottom of a flask, a cuneane based compound, what was obtained by the rearrangement of a cubane based molecule.

What is cubane and what is cuneane and what is this rearrangement? Cubane (1) is a square shaped and cuneane (2) is an wedge shaped molecule, both are strained.





For more information read this recently published article what was published by my supervisor:

Solvent-induced, selective rearrangement of hydrogen cubane-1,4-dicarboxylate to hydrogen cuneane-2,6-dicarboxylate
Gábor Durkó, István Jalsovszky
Tetrahedron, Volume 69, Issue 25, Pages 5160–5163

Brain&Force - 10-4-2014 at 16:02

Aw, come on! Nobody's going to top the brothers Hegedus!

I'm just wondering, kristofvagyok, what license, if any, do your photos fall under?

Hegi - 12-4-2014 at 09:45

Kristof, so epic, the picture and the molecule as well... high level organic chemistry.

Freshly prepared Mohr´s salt.


Texium (zts16) - 12-4-2014 at 21:28

Here is my first bromine isolation! I distilled it today from the reaction of NaBr+KMnO4+HCl. It has some water in it, but I don't really mind all that much, and I think it still looks really cool.

IMG_1205.jpg - 241kB

Zyklon-A - 12-4-2014 at 21:32

Nice! I've been isolating bromine several times this week, to find the cheapest method. Are you sealing it in an ampule?
[EDIT] Or is it in an ampule already? It's hard to see what kind of container it's in.

[Edited on 13-4-2014 by Zyklonb]

Texium (zts16) - 12-4-2014 at 22:04

Unfortunately, it's not in an ampule. It's just a normal vial with a teflon lined lid. It should keep it in, although I really wish I could have ampuled it.

Godspeed429 - 13-4-2014 at 10:21

52 gram crystal of Aluminum potassium sulfate.

Crystal.JPG - 307kB

Mailinmypocket - 13-4-2014 at 10:56

Some recrystallized KClO3, cooled very slowly overnight in a beaker...wrapped in a towel and then placed in a thermos lunch box. Some crystals are hard to capture on camera but a few plates are the size of dimes. Beautiful :)

kristofvagyok - 16-4-2014 at 18:16

Quote: Originally posted by Brain&Force  
I'm just wondering, kristofvagyok, what license, if any, do your photos fall under?
Attribution Non-commercial Share Alike (by-nc-sa)


And another picture:



Trying out a new UV lamp.

The mercury vapor lamp is placed in a double walled quartz tube what will serve as a water cooled, tempered UV light source, used for photochemistry.

Brain&Force - 19-4-2014 at 22:11

KRISTOF WITH A LIGHTSABER! OH YEAH! Now that's what I'm talking about!

Here are some bacteria I transformed. I don't know why the image is rotated.

<img src="http://i.imgur.com/gImIFam.jpg" title="I kept calling them my bacteria babies. That seemed to really creep everyone out." width=800>

My friends got better results:

<img src="http://i.imgur.com/u10WFLo.jpg" title="When the alt-text reaches a certain length, it seems to just enter a line break for some odd reason, like here. Anyone know why?" width=800>

confused - 19-4-2014 at 23:06

Nice, Im guessing the green is GFP. :D
Whats the blue and red protein?

kristofvagyok - 20-4-2014 at 03:18

I always wanted to work with those fluorescent things, they look adorable. Will you isolate the fluorescent protein from the cells?






On the pics: a little carbohydrate chemistry, 1,2:3,4:5,6-Tri-O-isopropylidene-D-mannitol what was made directly from mannitol and acetone with a little acid catalyst.

If you click on the pictures, you'll reach my portfolio, best pics from the past 2 years of the lab. Extra note: today I will post the 800.-th pics on my blog, so if anyone is bored here is a random post: http://labphoto.tumblr.com/random :D

Brain&Force - 20-4-2014 at 09:07

Different colors are different mutants of GFP. We were given unlabeled plasmid mixes, so we didn't know what colors we'd get when we transformed the bacteria.

I have no idea where the bacteria are now, and I don't think we're going to isolate the GFP from them. I have the procedure somewhere if you're interested (though you will need to have the correct plasmid and some E. coli available).

[Edited on 20.4.2014 by Brain&Force]

Brain&Force - 23-4-2014 at 15:03

<img src="http://i.imgur.com/b69MvRl.png" title="Might try it with boric acid next time." width=800>

"Thunder flasks" demo with methanol. Some copper chloride was added to color the flame, but with no success this time. (This is odd because my procedure had worked for the previous trial.)

<img src="http://i.imgur.com/TEXCsQy.jpg" title="I'm not sure which species this sample came from." width=800>

Stomata were viewed through a microscope by taking nail polish and drying it on the underside of a leaf to make a cast, then wet mounted on a slide.

Making sulfur chlorides:

Oscilllator - 23-4-2014 at 23:27


<a href="http://imgur.com/bUheqrS"><img src="http://i.imgur.com/bUheqrS.jpg?1" title="Hosted by imgur.com"/></a>

<a href="http://imgur.com/mBZluZN"><img src="http://i.imgur.com/mBZluZN.jpg?1" title="Hosted by imgur.com"/></a>

<a href="http://imgur.com/tcHHo4J"><img src="http://i.imgur.com/tcHHo4J.jpg?1" title="Hosted by imgur.com"/></a>

HeYBrO - 25-4-2014 at 14:59

That must of been hard to clean and dispose.

[Edited on 25-4-2014 by HeYBrO]

Oscilllator - 25-4-2014 at 15:23

Yeah my glassware still has what looks like sulfur powder on it. I'm thinking of blasting it in my over to try and burn the sulfur. Got any tips on how else I might go about it?

HgDinis25 - 25-4-2014 at 15:59

Quote: Originally posted by Oscilllator  
Yeah my glassware still has what looks like sulfur powder on it. I'm thinking of blasting it in my over to try and burn the sulfur. Got any tips on how else I might go about it?


Hot Toluene readly dissolves Sulfur (I've done it my self). Carbon Disulfide could also bee used...

The Volatile Chemist - 1-5-2014 at 19:17

GFP is definitely cool :) Anyone tried mutating bacterium who have the gene? Would be interesting... I don't have anything for such a procedure, but would love to see someone try! Maybe give them some light carcinogen...? If such a thing exists :)

Gold Pictures

Ionic Chemist - 6-5-2014 at 22:01



They might not be the best but I still consider this small collection pretty. All the pictures are from my recent attempts at gold purification via liquid-liquid extraction, with isopropyl alcohol as the secondary component in a water based mixture.

1). Separation of gold laden organic phase (left), from copper based aqueous impurities (right).

2). Addition of calcium chloride (layering inducer).

3). Formation of a biphasic layer accompanied by the production of calcium carbonate (from trace impurities of sodium carbonate used in processing).

4). Preparation for transfer of gold laden organic phase for further testing.

5). Microscopic view of reduced gold in a capillary tube.

6.) View of gold deposits in a separate section of the capillary tube.



Gold Purification.jpg - 58kB

Calcium Chloride Layering.jpg - 57kB

Full Triphase.jpg - 57kB

Gold Isolation.jpg - 72kB

Gold Capillary.jpg - 70kB

Gold Tube Capillary.jpg - 58kB

Etaoin Shrdlu - 7-5-2014 at 13:41

I really like that second-to-last picture, Ionic Chemist. Taken with a better camera it would probably be magnificent.

Zyklon-A - 8-5-2014 at 10:30


Can anyone guess what this is?
bubblebeaker.jpg - 73kB

DraconicAcid - 8-5-2014 at 10:35

Dilute manganate ion with dry ice.

Töilet Plünger - 8-5-2014 at 12:05

Bromothymol blue indicator with dry ice.

The Volatile Chemist - 8-5-2014 at 12:09

Quote: Originally posted by DraconicAcid  
Dilute manganate ion with dry ice.

Take It one step farther... Green Dye With dry ice... :)
Just Kidding. Though that definitely looks like something sublimating.

Töilet Plünger - 8-5-2014 at 12:09

Nickel ion with dry ice.

Manifest - 8-5-2014 at 15:05

I would imagine dry ice would float though.

Zyklon-A - 8-5-2014 at 16:25

Ok, nickel ion is my guess too. I didn't take this picture, and I don't know what it is. I saw it here, and wanted to see if you guys could makes some guesses.
I have been wanting to make a thread, on guessing a chemical based on a picture. Or is there already such a thread.

elementcollector1 - 8-5-2014 at 17:02

Pretty sure there is, somewhere in Whimsy. Something like "Where's Waldo for chemicals"...

Zyklon-A - 8-5-2014 at 19:20

Yes, I saw that, but isn't that where you try to guess where it is on the shelves?

MrHomeScientist - 9-5-2014 at 10:38

That's definitely dry ice, and almost certainly just green food coloring. Occam's razor, and all. I've done this a thousand times. Dry ice doesn't float.

kristofvagyok - 14-5-2014 at 11:56

Not strictly chemistry, but:




Two pieces of fluorite under UV light.

Fluorite (CaF2) is naturally occurring mineral, it is the far most common and well-known fluorine containing mineral found on earth. When pure, it is completely colorless and transmits light from 200 nm what means it lets through UVA, UVB and some of the UVC photons.

But when it is contaminated with other elements, usually with yttrium, cerium, iron, sodium, barium, aluminium, ect. it could change the color of the mineal and could also cause a fluorescence under UV light, just as in this case. Originally the fluorite on the right had a green color, but it emits strong blue light under UVB.

smaerd - 14-5-2014 at 17:05

Just out of curiousity Kristof how much do UV lamps like that light saber tend to cost? Euros or anything is fine. I was trying to think of a way to make one without shelling out tons and tons of money but I'm not sure it's practical.

Brain&Force - 14-5-2014 at 19:17

I have some fluorite, but it doesn't fluoresce at all. But I have some corundum that fluoresces red - if I find it I'll post a photo of it under UV.

smaerd, if it works for you, you can buy an ultraviolet (black light) compact fluorescent lamp from a party store (in the US Party City is one place. Most work fine, though there are a few duds that don't actually emit UV light. You can check by holding a US $20 bill behind the light

Here's potassium terbium sulfate fluorescing in a beaker, after separation from an iron-containing solution. Iron REALLY kills terbium fluorescence (which is why some of the crystals aren't as bright).

<img src="http://i.imgur.com/69Gz2yl.jpg" title="I just won $500 in the lottery and a $2500 scholarship. Amazing huh?" width=800>

[Edited on 15.5.2014 by Brain&Force]

smaerd - 15-5-2014 at 04:51

I have a nice little lamp, but if I want to run a reaction with semi-deep UV it would either need to be emersed in solution and protected with quartz or outside of a solution which is inside of something quartz. The quartz part is where things get tricky and expensive.

Also very nice terbium salt there B&F :).

[Edited on 15-5-2014 by smaerd]

Pyro - 15-5-2014 at 08:41

Heres a little quiz: What camera did I use for these macro shots?


WP_20140514_106.jpg - 111kB WP_20140514_137.jpg - 143kB WP_20140514_187.jpg - 116kB WP_20140514_191.jpg - 117kB

They are KMnO4 crystals

[Edited on 15-5-2014 by Pyro]

woelen - 15-5-2014 at 12:32

I looked at the match:

Just a few properties.
Nokia Lumia 620
1/30 s exposure time
Aperture F2.4
ISO 100
Colorspace sRGB

I can give more properties, but these are the most important ones.

kristofvagyok - 15-5-2014 at 13:40






Advanced chemistry: Growing crystals of a trifluoromethylthio substituted aromatic hydrocarbon.

Compounds that contain a trifluoromethylthio group (–SCF3) are found in many pharmaceutical and agrochemical products. Owing to their highlipophilicity and hydrophobicity, aryl trifluoromethylthio-ethers (ArSCF3) have attracted increasing attention from synthetic chemists to develop a efficient, high-yielded, and economical preparation of these molecules.

These crystals were prepared from an aryl thiolate with trifluoromethyl iodomethane (ICF3) what is a highly poisonous, carcinogen gas.

Pyro - 15-5-2014 at 14:17

Woelen, that was a lot faster than I expected!
I was amazed that these results were possible on a cell phone camera.

PS:where did you find this info?

arkoma - 15-5-2014 at 16:47




Electrolytic Copper Sulphate (creating) cell (per NurdRage) been running all afternoon in one of girly girls bud vases....started looking pretty so pulled the electrodes and took a back lit pic.

The Volatile Chemist - 16-5-2014 at 18:35

Arkoma, looks nice! Is the vase yours? :) Any flowers may not take copper sulfate (which happens to be sold as root kill) too well!

Quote: Originally posted by Pyro  
Woelen, that was a lot faster than I expected!
I was amazed that these results were possible on a cell phone camera.

PS:where did you find this info?


He likely found it in the picture itself. Some picture formats store information on how a photo was taken, if flash was used, etc. It's all in the file. Was that how you found it Woelen?

By the way, when you all buy chemicals, have you gotten any with nice crystals already? I got some ferric Ammonium Sulfate with some nice crystal lumps (single, imperfect crystals) over 1.5 cm3.

[Edited on 5-17-2014 by The Volatile Chemist]

arkoma - 16-5-2014 at 19:34

Quote: Originally posted by The Volatile Chemist  
Arkoma, looks nice! Is the vase yours? :)


LOL, no. It is my daughter-in-laws. The way it layered out and how I could see the anode actually pulling the blue tail of copper ions towards it was "purty". The good camera is out of town ATM--took that with daggum laptop.

Bert - 19-5-2014 at 12:47

Match head burning @ 4,000 frames/second

The Volatile Chemist - 19-5-2014 at 13:19

Quote: Originally posted by Bert  
Match head burning @ 4,000 frames/second

Wow, that's great! Thanks for posting it. I'd seen something like this, but much faster.

Zyklon-A - 19-5-2014 at 15:05

Quote: Originally posted by Bert  
Match head burning @ 4,000 frames/second

Wow, that was pretty cool. Here's some other cool slow motion videos by the same channel:
Lightning storm
Fire cracker
Very cool unknown fire balls
[EDIT] Can anyone guess what that last one is?

[Edited on 19-5-2014 by Zyklonb]

Brain&Force - 21-5-2014 at 13:45

I'm the 20000th viewer of this thread!

Two telescope shots. The first one is a crow I photographed with my telescope.
<img src="http://i.imgur.com/ELsu3jG.jpg" title="I also have a photo of a dove." width=800>

The second one is Jupiter, seen during the daytime. I couldn't see its moons.
<img src="http://i.imgur.com/w7p6O15.jpg" title="The best time to do this is when the moon passes directly over or under Jupiter." width=800>

The Volatile Chemist - 21-5-2014 at 14:04

Quote: Originally posted by Brain&Force  
I'm the 20000th viewer of this thread!

Nice pictures!


elements2.bmp - 829kB
An interesting graph I made (Using a Firefox Plugin)

[Edited on 5-21-2014 by The Volatile Chemist]

arkoma - 22-5-2014 at 08:59

@ Brain & Force. Nice. Have done some digizooms myself. 8" Celestron with a toilet paper tube spacer and duct-tape holding my little kodak easyshare. (click thumbs for bigger image)


Jupiter and three of the Galilean moons

Our moon

Photomicrograph of a piece of complex sulfide ore, using the same jury rig


Couldn't catch the true beauty of this Chrome/Nickel Chloride solution I got out of my salt bridge electrolytic cell this morning. Creme de Menthe, anyone?


(flower pot cell with cheap stainless steel anode, carbon rod cathode and NaCl electrolyte in both halves.)

Brain&Force - 22-5-2014 at 14:41

Quote: Originally posted by arkoma  
8" Celestron


I got one too! It's a black tube; don't know when it was made (I'm guessing the 90s) and it's on a fork mount.

kristofvagyok - 22-5-2014 at 14:50






Before and after the sublimation of ferrocene.

When we heat ferrocene (an organometallic compound with the formula Fe(C5H5)2, a sandwich compound) in vacuum, it sublimes and could be condensed with on a cooled glass surface to form perfectly pure needle like crystals (as seen on the bottom picture).

DraconicAcid - 22-5-2014 at 15:42

A sublimation that works nicely- a rare occurrence.

Way back when, I supervised an undergraduate lab that made ferrocene. Despite their sublimation, it generally looked like the stuff in the bottom of your second picture. I would tell them that if they wanted to see pure ferrocene, they should closely observe the crystals that formed halfway up their capillary tube after they measured their melting points.

arkoma - 22-5-2014 at 16:08

Wish I could say its mine, but its not. Belongs to one of my best mates.


Hegi - 29-5-2014 at 22:18

Quote: Originally posted by arkoma  
Wish I could say its mine, but its not. Belongs to one of my best mates.



But anyway, you have access to it and you can use it as well, no? ;)

Ethyl acetate layer, the yield of reaction was about 56%..

<img src="http://chem.pieceofscience.com/wp-content/uploads/2014/05/layeeeers.jpg" width="600" height="900">

The Volatile Chemist - 30-5-2014 at 12:49

Nice, Hegi! What process did you use?

Hegi - 31-5-2014 at 02:56

Quote: Originally posted by The Volatile Chemist  
Nice, Hegi! What process did you use?


I refluxed mix of 30 ml 98% acetic acid with 30 ml of 95% ethanol and about 8 ml of concentrated sulphuric acid for about 45 minutes, then washed it with sodium carbonate solution to get rid of free acetic/sulphuric acid. Separated layers. Into the organic layer I added calcium chloride to minimize the amount of water and redistilled the product.

Brain&Force - 4-6-2014 at 14:41

A 2 gram piece of terbium from the 6 gram piece I had, viewed under a dissection microscope. The dendritic structure of distilled terbium is easily apparent. The yellowness isn't the terbium, it's the color of the light on the microscope.

<img src="http://i.imgur.com/VqWZULj.jpg" title="SOMEBODY GIVE ME MORE TERBIUM! please? Pretty please?" width=800>

And the setting moon.

<a href=https://www.youtube.com/watch?v=X0nEkkpShsg&feature=kp><img src="http://i.imgur.com/IkDMOS3.jpg" title="I need one of those devices that hooks my camera securely onto my eyepieces." width=800></a>

[Edited on 4.6.2014 by Brain&Force]

The Volatile Chemist - 5-6-2014 at 14:10

Nice pictures! Once I move my microscope pictures over to my desktop, I'll post a few of some microscopic crystals. Sad, my mic. camera has better res. than my digital camera...

bismuthate - 5-6-2014 at 14:19

http://iconosquare.com/viewer.php#/detail/730604564436500586...
The oxidation states of copper. It's amazing how different they look!

kristofvagyok - 5-6-2014 at 23:21




Things what never-ever gets boring: fun with fluorescent dyes!

The red color is emitted by a fairly common dye: Rhodamine B. The green color is a bit more interesting, it is emitted by merbromin, an organomercury chemical:




Merbromin is one of the best antiseptics and it is still used in several countries, but because of its mercury content, it is no longer sold in the United States, Germany, or France. When used as a topical antiseptic, it stains the skin bright red and it is quite hard to remove. Luckily it is only used as a 2% solution, or more dilute, and since it is not readily absorbed by the skin, it is perfectly safe to use.

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