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Author: Subject: Pretty Pictures (2)
smaerd
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[*] posted on 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]




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Pyro
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[*] posted on 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]




all above information is intellectual property of Pyro. :D
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[*] posted on 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.




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kristofvagyok
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[*] posted on 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.




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Pyro
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[*] posted on 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?




all above information is intellectual property of Pyro. :D
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[*] posted on 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.
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The Volatile Chemist
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[*] posted on 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]




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arkoma
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[*] posted on 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.
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[*] posted on 19-5-2014 at 12:47


Match head burning @ 4,000 frames/second



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[*] posted on 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.




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Zyklon-A
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[*] posted on 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]




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Brain&Force
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[*] posted on 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>




Raney nickel can't hydrogenate dank memes.
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The Volatile Chemist
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[*] posted on 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]




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[*] posted on 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.)
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Brain&Force
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[*] posted on 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.




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[*] posted on 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).




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[*] posted on 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.




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[*] posted on 22-5-2014 at 16:08


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

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[*] posted on 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">




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The Volatile Chemist
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[*] posted on 30-5-2014 at 12:49


Nice, Hegi! What process did you use?



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[*] posted on 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.




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[*] posted on 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]




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[*] posted on 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...



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[*] posted on 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!




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[*] posted on 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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-Pictures from chemistry, check it out(:

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