Redox Reaction: Holiday ChemisTree! Copper + Silver Nitrate (Holiday Chemistry)
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- Опубліковано 30 лис 2017
- Oh Chemistry...Oh Chemist-Tree!
Here's a video treat for the holiday season, or any time of the year!
As Copper reacts with silver nitrate, copper replaces silver ions in solution, causing the silver to precipitate out of solution as elemental silver crystals! - Наука та технологія
Beautiful demonstration of both a displacement and REDOX reaction to produce a work of art!
Oh chemist-tree, oh chemist-tree,
Thy copper limbs are silvery.
When silver gains electrons free,
No longer ions they will be.
The copper's metal, sweet and nice,
But silver steals its electrons, twice!
Oh chemist-tree, oh chemist-tree,
Forms copper ions, oxidatively.
Perfect. Love it.
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Looks great
Thanks Scott!
Great video - thanks:)
Hi! Nice video! My question is, why doesn't the same reaction happen with zinc? It should happen based on their reactiveness .
This looks so cool, although looking at the tree itself it looks very painful to touch
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What would the Independent, Dependent, and Controlled Variables be?
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Ha! That was great! Do they hold up after the tree dries? It would be cool to make trees for a train set display!
Yeah, I wish that it would maintain that shape and structure, but those little high density crystals need the solution's buoyancy to look like that. Once out of solution, the previously "healthy" tree looks like a rather sickly one.
What is the material of tree 🎄
Is there a way to stop this reaction at the "pretty" stage? I've seen a few other vids of this rxn, and after the pretty stage, it tends to start looking more like a brown/black mushroom cloud than a frosty tree. Is it just something where I'd have to test different molarities of AgNO3 until I had just enough to stop the rxn, or does light/oxidation or something make the ugliness inevitable?
You can try doing an ANOVA with the different concentrations of silver nitrate and letting us know, this makes one of the best christmas decorations
yeah I've had this same issue with copper and silver nitrate, I'm unsure what causes the ugly brown to start emerging, any ideas?
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What is the actual time duration that it takes for this reaction to occur? Can the tree just be life in the solution indefinitely so it does no fall apart ? If the jar, with the solution and tree still in it was moved, would the tree fall apart ?
As for the reaction, I'd say immediately, but I'm guessing you're asking how long it took for the tree to be all "full" as it is by the end of the video. That was about 4 or 5 minutes. If it's left in the solution, the reaction would continue until you run out of silver ions in the silver nitrate, or until you run out of copper. In the case of the solution concentration I was using, I'd have most definitely run out of the silver ions first.
If left undisturbed, it is *likely* that your silver would tarnish due to oxygen gas dissolved in the solution, and thus, turn a blackish brown due to the silver oxide present, but that could take several days. In addition, copper II oxide could form , leading to copper II carbonate from dissolved oxygen and carbon dioxide gas, but that's less likely as the copper is now coated from the silver around it.
As for the tree falling apart if removed, I did remove it, and it doesn't fall apart, but also, due to the lack of buoyant force that the solution was providing, once out of solution the tree looks much less impressive. The crystals of silver all hang down, and it ends up looking like a very wet, long haired, hairy sheep dog!
@@MrLundScience I'm planning on demo-ing this same reaction to my class this week. What I want to confirm is, this should move a bit faster if I use hyper thin (angel hair) copper wire, right?
@@somerandomguy84 That depends upon how you are interpreting "faster". With more surface area, yes, the rate of the reaction would be increased, and think copper wire should do that. However, just because there's more surface area doesn't mean it will visually look covered as quickly. In other words, the increased surface area also will make the immediate crystals have many places to start, and will not become as large as in this video as quickly. With all of the silver nitrate used in your solution, more surface area means the reaction will proceed faster, but there's likely to be smaller crystals of silver. With less surface area, the reaction proceeds slower, but the silver crystals that do grow will continue to have more silver reduce at those surfaces (and thus, produce larger crystals). When the copper is covered with silver, the reaction can continue, as it's a reduction-oxidation reaction, and electrons can pass through the conductive silver, causing elemental copper underneath the silver to still be oxidized into dissolved ions.
I hope this helps.
@@MrLundScience Sure does help. Thanks!!
Super cool! What happens when it is removed from the solution?
That is much prettier than the little trees they sell to accompany the Christmas village houses!
Well, the silver crystals are very light and not rigid at all. So, when taken out of solution, as they don't have the added buoyancy support from the solution, they all sort of hang down in a droopy fashion, not unlike a long haired dog when very wet! It's not nearly as stunning. If you didn't know it was silver, it'd look kind of gross. Like a very gray colored moss.
Wow it looks like the ones you buy from the store. Where do you get the copper at and the silver nitrate?
Where do I get it? From our school chemical supplier catalogs.
Where can the average non-chemistry teacher get it? Well, copper sheet metal can be purchased from either metal work suppliers (talk to your local scrap yard...they'll direct you in the right spot), or there's multiple online sources. Silver nitrate, meanwhile, is not something you can just pick up at the grocery store. It does have health hazards if used incorrectly. Still, it's not a controlled substance by any means, and there are online sources for it if you really want some. It's not cheap, though. Keep in mind, if you do use any, you *want to wear gloves* and avoid any and all skin contact. The silver ion can leach into your skin, and form silver oxide, which turns your skin a purple-ish black for a few days. If too much silver ion gets into your system, you wind up with gray rings around the irises of your eyes, and that's essentially permanent, and can lead to vision problems.
help please ok I have one question I have nitric acid and a heated magnetic Stirrer & some silver that I have made all most to dust now I know when I put the silver in the acid it reacts and will deserve now I am to put a copper bar in to the silver nitrate to recover the silver what do I need to do about the copper reacting with the acid all so ? add more silver? neutralize the acid? or? thank you
Kevin, my honest advice is to immediately *STOP* and do not attempt to perform the reaction you are suggesting here.
Nitric acid isn't your normal type of acid. If silver is placed in a dilute sample of it, nitric oxide gas, NO, (nitrogen monoxide) will be produced, which is a very VERY hazardous gas. In the US, nitric oxide is officially classified as "extremely hazardous". That's the *best case* scenario. If you use more concentrated nitric acid, you will produce brown NO2 gas, (nitrogen dioxide) which is *also* classified as an "extremely hazardous" substance. Exposure to this gas can cause skin irritation, internal bleeding of the throat and lungs, and if enough were exposed to your eyes, blindness. This is nothing to play around with.
Meanwhile, silver nitrate (both in crystal form or as a solution) is *readily* available online from chemical suppliers, and while it has its own safety concerns, it's NOT a hazardous chemical and is much easier to work with and manage.
I don't mean any offense. For all I know, you have proper safety equipment and have some training in chemistry. But even if that's true, just about every chemist I know would *avoid* doing what you propose and just get some silver nitrate, for proper chemistry always involves safety first, and there's never a reason to take unnecessary risks. With how affordable and available silver nitrate is, making it on your own is most definitely an unnecessary risk.
Please heed my warning, and stay safe!
thank u I would rather be warned by others than giving bad info yes I am in a save a place and have vent box and supplied-air full-face respirator for a fallback not doing this for the silver nitrate but for gold & silver recovery from the use of electrolysis just do not want any silver loss.
As a public school teacher, I can't go into detail as to *exactly* how I would do this. That said, find a *safe* way to dissolve the silver. Once you have the silver dissolved (be it as silver nitrate or otherwise), I would neutralize the acid, and then in a well ventilated area, I would perform electrolysis. This would minimize impurities. Electrolysis can be done as seen here with tin II chloride: ua-cam.com/video/r-YbQN_twpw/v-deo.html
Where did you buy the copper tree from
I cut it out of a copper sheet and bent it that way. Good luck! Oh, also, you could twist together a tree from copper wire.
Just read the other comments and replies!
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