Not sure how I missed your comment man, but yeah its honestly crazy how many colors you can get out of copper. Didn't even realize how little blue copper I had in this video until you pointed it out lol
Right!? I'm slowly working on a video (that will probably be like 90 minutes long at this point) of every possible thing you can do with copper in the lab. I'll do several other metals eventually but copper felt like a good starting point given it can do so many crazy things.
This is exactly reason why I love inorganic chemistry. Beautiful colors. Nice video as always! Btw. Cu(I)-chloride complexes aren't brown, but colorless. Try dissolve some CuCl in HCl, you obtain colourless [CuCl2]- solution. The brown colour comes from mixed valence Cu(I)/Cu(II)-chloride complex. Try to combine Cu+/Cu2+ solutions in HCl, you obtain this brown solution.
huh that actually makes perfect sense now that I think about it, especially considering the pure copper (I) chloride is completely colorless. Thanks for letting me know, I honestly wasn't sure where the brown came from
I know longer do laboratory work, but grew up with a love of the sciences and eventually practiced biochemistry. I love your demonstrations of practical chemistry because they can be reproduced, tweaked, and used to evolve our knowledge by anyone with both the curiosity and the means. Thank you!
I see you mentioned Cobalt at the end of the video. You should definitely make a topical video on the importance of organometallic compounds within the human body. You could tie it all together.
I certainly intend to touch on that to a degree when I do the cobalt complex video! The cobalt compound I'm making has a structural center that is nearly identical to B-12 (and in fact it's main use is to study B-12)
That's awesome, looking forward to it with great anticipation, cobalamin is a compound and topic I am very interested in because of my own medical history.
Thank you so much! I've been trying to get back into doing chemistry since I moved and I've been using transition metal projects like these since they are so beautiful while relatively simple
if you cool the first copper iodide complex to liquid nitrogen temperatures, the fluorescence changes color to blue. nurdrage made a video about these complexes a long time ago
I loved the discussion about complexes and bonding! So fun to think about the physics happening underneath the hood as it were to the chemistry happening
Organometallic chemistry is something different. I would definitely have to start studying inorganic chemistry more to begin to understand how metallic bonds form complexes. This was pretty cool demonstration!
The likely names are: Green: copperdiiodobis(pyridine) Yellow: copperiodo(pyridine) I'm thinking the green compound would be square planar and the yellow linear. But that's only describing the molecules in isolation. Things could be different if it forms solvates in the crystal.
woah. its almost blue. that yellow one looks like the stereotypical "uranium cake" colours. those test tubes mounted behind a uv light would make a cool movie prop for scifi radioactivity
You could actually take a mechochemical path and mortar the copper iodide with pyridine Then you could add triphenylphosphan and mole again The complex you get has pretty cool properties in terms of luminescence At room temperature, only fluorescence from the singlet mlct can be observed under irradiation with UV light and at 77 kelvin the phosphorescence from the triplet mlct can be observed
Ah you noticed! I bought one just after we discussed it (you convinced me it was worth the investment) Actually though the first part of the video where I make the copper iodide was filmed with my new camera, but the actual synthesis along with the shots of the stuff under UV were filmed using my old camera.
I actually got so caught up researching whether I could after last time you asked that I forgot whether to ever reply. I do have the ruthenium and everything else I'd need based on the synthesis I was reading, but it seems making bipyridine is a bit more involved than simply squishing two pyridines together lol. Do you have any insight on the synthesis of bipyridine perhaps?
It's a nickel-catalysed reaction. And it must be ensured that the product isn't contaminated with pyrrol before you use it to synthesize the complex. Ch*miolis already did this synthesis but I think it's not to much to have it twice on this platform... 😉
At 12:45 there’s a yellow intruder in the green floculation :p. Do you use quartz tubes or normal borosilicate glass? Also at 3:47 ‘highly reccomend’ lol :p
While watching the video, I wondered if there was a mineral made of copper iodide. It turns out there is one called marshite (CuI), and it fluoresces red!
Why would you want to throw away any Copper or any Metal? Darn wasteful way to live in my opinion.😅 Thanks for sharing your experience and knowledge with me.😊
lol very good point. Funny enough I actually have a 5-gallon bucket that I toss any and all metal waste and scrap into (what I mean by throw away). I've got no idea what to do with any of it but as you said it feels darn wasteful to trash it. And no problem! Happy you enjoyed it :)
Hm... now i am curious if other amines could work, it would be nice school demo showing what different stochiometry in reaction can do to product, but pyridine XD
I don't really understand much else than energetics chemistry. Not a chemist, just here for the explosives. By "here" i mean literally the whole chemistry community.
tbh I think that's how most of us got here to begin with lol. Nonetheless happy to have you here! (It's the best community and I'm a scientist therefore cannot be biased)
@@integral_chemistryI got interested in chemistry through metallurgy. Then just sort of stumbled into the energetics and other chem. But then I turned it into a job and now I just ship chems all over the world and watch everyone else make the chem videos. I hate that I'm not making many videos these days, but making sure certain stuff is available to the community makes up for it. Let's keep this going though, how did the rest of you all get into chemistry?
I'm doing fine, thanks for checking in! I guess yesterday someone went out and mass reported every energetic video I've made. UA-cam ignored the reports and found my videos fine, but Patreon terminated my account.. I'm currently appealing the decision and I'll try and give a better update soon. Regardless, it's pretty annoying and very weird that patreon doesn't even issue a warning and goes straight to termination..
Yeah i guess they're less tolerant of energetics there than even UA-cam, which is the opposite of what I heard.. I'll try and appeal it as I genuinely was not trying to violate their policies 😅
@Apoptosis I´ve noticed a little mistake: the second reaction should be CuO + 2 HCl = CuCl2 + H2O. You´ve accidently put the equation as CuO + 2 HCl = CuCl2 + H2.
ohh good catch! See I was trying to edit the video together super fast to get it out today so I didn't catch that, but I did have a second where in passing I thought "hm you know, I didn't notice any gasses being evolved when I did this step.. oh well!"
@@integral_chemistry I understand, it happens and it´s not that serious. I just like to help in a positive way in any way I can do and think of, I can´t help it and I´m proud of that.🙂
Couldn’t you have made the copper(I) iodide by mixing copper sulfate with potassium iodide to make copper(I) iodide and then to get rid of the iodine add sodium thiosulfate to make soluble sodium iodide and sodium tetrathionate
Yeah that could work perfectly fine! I actually considered that as thiosulfate is more typically used to reduce iodine, plus I think its less apt to generate irritating sulfur dioxide. I only really settled on the sulfite because I felt it was likely easier for the average person to find
I wasn't prepared for so much non-blue copper chemistry, I'm gonna need a minute to reassess everything I thought I knew...
y e l l o w
Same here. I’m staring at a penny with a yellowish look on my face.
Not sure how I missed your comment man, but yeah its honestly crazy how many colors you can get out of copper. Didn't even realize how little blue copper I had in this video until you pointed it out lol
Who doesn't love some copper chemistry?
... didn't Explosions and Fire call copper a "shill metal"?
me i don't like copper chemistry, it was invented by inorganic chemist to sell more grants
Right!? I'm slowly working on a video (that will probably be like 90 minutes long at this point) of every possible thing you can do with copper in the lab. I'll do several other metals eventually but copper felt like a good starting point given it can do so many crazy things.
lol I can see that. Was his implication that its too easy/low effort since copper chemistry is so colorful?
@@Kay_Sea251 stop revealing the hidden parts
Man really said “if you already have some” like I have a single piece of chemistry equipment in my house 😂
Yes i am
This is exactly reason why I love inorganic chemistry. Beautiful colors. Nice video as always!
Btw. Cu(I)-chloride complexes aren't brown, but colorless. Try dissolve some CuCl in HCl, you obtain colourless [CuCl2]- solution. The brown colour comes from mixed valence Cu(I)/Cu(II)-chloride complex. Try to combine Cu+/Cu2+ solutions in HCl, you obtain this brown solution.
huh that actually makes perfect sense now that I think about it, especially considering the pure copper (I) chloride is completely colorless. Thanks for letting me know, I honestly wasn't sure where the brown came from
I know longer do laboratory work, but grew up with a love of the sciences and eventually practiced biochemistry. I love your demonstrations of practical chemistry because they can be reproduced, tweaked, and used to evolve our knowledge by anyone with both the curiosity and the means. Thank you!
I see you mentioned Cobalt at the end of the video. You should definitely make a topical video on the importance of organometallic compounds within the human body. You could tie it all together.
I certainly intend to touch on that to a degree when I do the cobalt complex video! The cobalt compound I'm making has a structural center that is nearly identical to B-12 (and in fact it's main use is to study B-12)
That's awesome, looking forward to it with great anticipation, cobalamin is a compound and topic I am very interested in because of my own medical history.
Transition metal chemistry always offers some interesting colors, beautiful recrystallisation as always!
Thank you so much! I've been trying to get back into doing chemistry since I moved and I've been using transition metal projects like these since they are so beautiful while relatively simple
if you cool the first copper iodide complex to liquid nitrogen temperatures, the fluorescence changes color to blue. nurdrage made a video about these complexes a long time ago
I came here to suggest cryocooling it too. It exhibits brilliant fluorescence thermochromism.
I loved the discussion about complexes and bonding! So fun to think about the physics happening underneath the hood as it were to the chemistry happening
Yessssss! Keep the colors coming. It’s so groovy❤
Colourful! That is potent stuff.
Organometallic chemistry is something different. I would definitely have to start studying inorganic chemistry more to begin to understand how metallic bonds form complexes. This was pretty cool demonstration!
Cul forms beautiful diamond-like crystals when recrystallized from MeCN 😸
Really?? I'll absolutely have to give that a try now!
@@integral_chemistry Yes, they are fragile though and turn into dust shortly after removing from the solution. Still, beautiful
The likely names are:
Green: copperdiiodobis(pyridine)
Yellow: copperiodo(pyridine)
I'm thinking the green compound would be square planar and the yellow linear. But that's only describing the molecules in isolation. Things could be different if it forms solvates in the crystal.
woah. its almost blue. that yellow one looks like the stereotypical "uranium cake" colours.
those test tubes mounted behind a uv light would make a cool movie prop for scifi radioactivity
Do you think you might be able to make copper selenite dihydrate
Great. Try to incorporate the most stable of the two in a polymer matrix as PMMA of polystyrene.
ooh I like that idea! I do (in general) need to get more creative about follow-up projects I can do with some of the things I make in my videos.
You could actually take a mechochemical path and mortar the copper iodide with pyridine
Then you could add triphenylphosphan and mole again
The complex you get has pretty cool properties in terms of luminescence
At room temperature, only fluorescence from the singlet mlct can be observed under irradiation with UV light and at 77 kelvin the phosphorescence from the triplet mlct can be observed
I am also familiar with the structure of the complex
In fact, one of the possible structures is a heterocuban
Explosions and Fire would be a truly insane crossover. Like Timmy turner and jimmy neutron
Sounds like the green could be used as a timer dye too change color when done time had passed. Like an expire date paint
Great video! The footage quality appears to be improved, it is just me or you have upgraded your camera?
Ah you noticed! I bought one just after we discussed it (you convinced me it was worth the investment) Actually though the first part of the video where I make the copper iodide was filmed with my new camera, but the actual synthesis along with the shots of the stuff under UV were filmed using my old camera.
@@integral_chemistry Ah, glad it worked out for you, the improvement from new camera is definitely noticeable!
Good work, bud
Would it be possible for you to make some Ru(bpy) for a orange-red chemiluminescence reaction?
I actually got so caught up researching whether I could after last time you asked that I forgot whether to ever reply. I do have the ruthenium and everything else I'd need based on the synthesis I was reading, but it seems making bipyridine is a bit more involved than simply squishing two pyridines together lol. Do you have any insight on the synthesis of bipyridine perhaps?
It's a nickel-catalysed reaction. And it must be ensured that the product isn't contaminated with pyrrol before you use it to synthesize the complex.
Ch*miolis already did this synthesis but I think it's not to much to have it twice on this platform... 😉
At 12:45 there’s a yellow intruder in the green floculation :p. Do you use quartz tubes or normal borosilicate glass? Also at 3:47 ‘highly reccomend’ lol :p
While watching the video, I wondered if there was a mineral made of copper iodide. It turns out there is one called marshite (CuI), and it fluoresces red!
I frankly like the yellow complex more. Green is what you expect of copper. Yellow, not so much. :P
copper is the coolest metal.
I wonder if these are used in coloured fluorescent lamps.
Why would you want to throw away any Copper or any Metal? Darn wasteful way to live in my opinion.😅 Thanks for sharing your experience and knowledge with me.😊
lol very good point. Funny enough I actually have a 5-gallon bucket that I toss any and all metal waste and scrap into (what I mean by throw away). I've got no idea what to do with any of it but as you said it feels darn wasteful to trash it.
And no problem! Happy you enjoyed it :)
Hm... now i am curious if other amines could work, it would be nice school demo showing what different stochiometry in reaction can do to product, but pyridine XD
yeahhh pyridine is not fun.. I have some methylamine I could try as well as aniline.. neither of those are particularly pleasant either though.
@integral_chemistry true. I doubt that without aromatic system it will glow sadly :(
I don't really understand much else than energetics chemistry. Not a chemist, just here for the explosives.
By "here" i mean literally the whole chemistry community.
tbh I think that's how most of us got here to begin with lol.
Nonetheless happy to have you here! (It's the best community and I'm a scientist therefore cannot be biased)
@@integral_chemistryI got interested in chemistry through metallurgy. Then just sort of stumbled into the energetics and other chem. But then I turned it into a job and now I just ship chems all over the world and watch everyone else make the chem videos. I hate that I'm not making many videos these days, but making sure certain stuff is available to the community makes up for it.
Let's keep this going though, how did the rest of you all get into chemistry?
The whole reason i gained my love for home chem is from my misadventures into TATP, so i feel you.
@@TakeApartLabare you the person who made like a pound of it at home because you didn't realize how bad it was lol
Neat!
Its been a while since i last watched.
Do you use DaVinci Resolve for editing?
Grow a large crystal of it!
I'll give it a shot! I'm honestly not sure whether its soluble in any solvent, but then again I hadn't tried lol
can't seem to find your patreon, what's up? you doing okay?
I'm doing fine, thanks for checking in! I guess yesterday someone went out and mass reported every energetic video I've made. UA-cam ignored the reports and found my videos fine, but Patreon terminated my account.. I'm currently appealing the decision and I'll try and give a better update soon. Regardless, it's pretty annoying and very weird that patreon doesn't even issue a warning and goes straight to termination..
@@integral_chemistryoof, good luck, sorry. Was literally just trying to subscribe when I found the patreon was gone :(
@@integral_chemistryI hope it can be resolved soon. If there's anything you need, or a way to contribute until it gets settled, let us know.
Anyone ever tried dissolving this to see if you could get Lasing? Copper is known for super radiant lasing at what looks like those frequencies.
What happened to your Patreon? Says account deleted...
Yeah i guess they're less tolerant of energetics there than even UA-cam, which is the opposite of what I heard.. I'll try and appeal it as I genuinely was not trying to violate their policies 😅
@Apoptosis I´ve noticed a little mistake: the second reaction should be CuO + 2 HCl = CuCl2 + H2O. You´ve accidently put the equation as CuO + 2 HCl = CuCl2 + H2.
ohh good catch! See I was trying to edit the video together super fast to get it out today so I didn't catch that, but I did have a second where in passing I thought "hm you know, I didn't notice any gasses being evolved when I did this step.. oh well!"
@@integral_chemistry I understand, it happens and it´s not that serious. I just like to help in a positive way in any way I can do and think of, I can´t help it and I´m proud of that.🙂
@@chemicalmaster3267 I do genuinely appreciate it :) Please do let me know if you ever see another little mistake like that in the future
I don't know, but I feel like the word Tetrakis should be involved.
Couldn’t you have made the copper(I) iodide by mixing copper sulfate with potassium iodide to make copper(I) iodide and then to get rid of the iodine add sodium thiosulfate to make soluble sodium iodide and sodium tetrathionate
Yeah that could work perfectly fine! I actually considered that as thiosulfate is more typically used to reduce iodine, plus I think its less apt to generate irritating sulfur dioxide. I only really settled on the sulfite because I felt it was likely easier for the average person to find
😮😮😦😀🫨🫨😂😂🫤🫤🥹🥹😂😂🫨
Organometallic has only ever meant a direct bond between a metal and carbon
I like to act like I know what you’re talking about. Chemistry is not my forte.