Copper Chloride - Periodic Table of Videos

[@frepi]

My guess is that Pr Poliakov was fed up with that old and ugly carpet and he pulled that trick of educating the children to alleviate mommy's anger.

[@LeQuizle]

"We now have a new carpet."

[@NuclearSavety]

.... and this is why you cant transport copper cloride or mercury in an airplane....

[@kingemocut]

that carpet story... i cri evry tiem.

[@Brightred11]

I demo'd this reaction for my department today and it is now gonna be part of our year 8 scheme of work. Great little bit of chemistry this.

[@GiorgioCapocasa]

A couple of weeks ago, a bottle of Copper Chloride fell and broke in my tool shed. When I went and opened the door, there was a strong odor of mustard: the Chloride had been eating through all of the spray cans that were on the shelves and the gas had filled the whole place. Also, many pipes I was keeping there were covered in copper, though it didn't manage to get through. It's quite an incredible chemical :)

[@whatevzist]

I would just like to say, thank you so much for making all of these videos! They are so awesome! I learned so much

[@anapecanape]

Everytime I see a thumbnail of the professor, I have to fight not to click on it... *must not watch it, won't be able to stop later, must finish homework first*

[@yobar23]

Thanks, Prof, for this! It reminds me of my 8th grade chemistry class, growing copper choride and copper sulfate crystals. I also remember my teacher telling us that these chemicals were used to keep algae out of ponds and that the pond owners could not keep aluminum john boats on these ponds because of the above reaction.

[@busby3141592]

If anyone is interested the balanced reaction would be : 2Al + 3CuCl2 --> 2AlCl3 + Cu3 Where the metal's are both solid and the chlorides are in aqueous solution.

[@mrthunt5770]

Sweet vid bro

[@nickmt]

Top draw on Prof's past home chemistry antics ... nothing like a safe home demo that had a funny unplanned consequence :) Three cheers for Poliakoff ... hip-hip!

[@jeebersjumpincryst]

yay welcome back! withdrawal is finally over. ive been rewatching all my fav pv and 60 symbols vids over and over.

[@tehhhhhd]

Thanks for calling it aluminium and not aluminum, England.

[@Llamarama100]

I love these videos, especially as theres usually a story associated with it, thanks for the fantastic videos! :)

[@TheColdwontrise]

I love these videos! I always look up random elements on my phone when I'm bored and these videos are a higher octane version of that. Thanks :D

[@SkewScrew]

Reminds me of how I discovered that reaction. I wanted to deliver CuCl2 to the water layer in a 3 layer experiment used to explain polarity and densities. I had a creative spoon made of copper wire and aluminium foil, so I could get deep enough into the cylinder. As I passed the ethyl acetate layer and started dissolving the salt in the water layer, everything suddenly went all bubbling and dark. As I pulled out the wire, I noticed I no longer had the spoon. I had a good laugh later.

[@Alabastro945]

I did a similar reaction using mercury(i) cloride instead of copper cloride, but the result was different (I obtained elemental HG and a foam of aluminium oxide) it was a very beautyfull reaction :D

[@AssemblerGuy]

This reaction is similar to the one with thermite mix in the periodic video on iron: Aluminium is more reactive than copper, so even though the chloride ions are "stuck onto" the copper (in that green copper chloride), the aluminium manages to "snatch" the chloride off of the copper, which is left behind as brown metal on the "burned" cupcake holder.

[@flamedrag18]

this is a great video showing the reaction of metals in the reactivity series, aluminum is more reactive, so it takes the place of the copper and leave behind metallic copper. same thing happens when you introduce copper into a silver salt solution or even chloroauric acid as a result of dissolving gold into aqua regia. the less reactive metals like silver, gold and platinum will precipitate out of solution if you introduce copper or any or the more reactive metals.

[@HansVanIngelgom]

I discovered this reaction when I was a teenager although it was with some Copper (III) chlorate I found in the basement. Also, I didn't do it inside but in the garden. Result: a small patch where nothing has grown in over 10 years. Oh, and HCl also reacts very nicely with aluminium foil.

[@BlokenArrow]

That is essentially correct. Cu+3(3Cl-) becomes Al+3(3Cl-) However, if you were to do the reaction with Boron (B), you would not get an ionic salt, but an electron-deficient covalent compound of BCl3 and metalic Cu.

[@ghuegel]

Get the adblock extension for your browser. It eliminates the ads. Though it does have the nasty side-effect of denying money to channels that make money off of their videos.

[@dkamm65]

As soon as I saw this video in my subs box - I don't think I've ever clicked a video faster.

[@mikkikun91]

Simple Redox reaction in which aluminium is getting oxidized and copper reduced. This shows that copper is a much more noble than aluminium. Not a bad reaction though, the copper can be salvaged for electronics and AlCl3 is a nice Lewis acid which can be used in Friedel-Crafts alkylation/acylation in organic chemistry. Thanks for letting me know of this reaction, in case I ever need AlCl3 I know now how to do it myself in case it isn't available ;)

[@YdeckW]

I am definitely sure that this reaction is not at all a good method for obtaining AlCl3 of the grade needed for organic synthesis. Also, the fact that you were familiar with the Friedel-Crafts reaction and not this simple displacement reaction so many times mentioned while discussing the reactivity series, really dazes me. I'm quite sure the professor would agree.

[@TheDingiso]

Welcome back!! Really miss you and your videos, Brady :D

[@TheHumanSuitcase]

I love the way you say aluminum.

[@lukystreik]

I really love those stories. Great 👍 😂 Thanks for sharing

[@sirNemanjapro]

I want to see that new carpet

[@SkuzleB]

Yet, the label clearly states that it is a copper (II) chloride. Actually, the ligands in solution may alter its color quite substantially. Here, chloride ions make complexes with Cu2+ ion that appear green, but on addition of concentrated HCl it can even change color to yellow due to formation of [CuCl4]2- complex anion. On the contrary, copper (I) compounds are mostly quite insoluble in plain water and appear green because of copper (II) impurities.

[@FLPhotoCatcher]

Aluminum is a correct spelling, & the American (& Canadian) way of pronouncing it is also correct. British chemist & inventor Humphry Davy settled on aluminum by the time he published his 1812 book Chemical Philosophy. I think calling it aluminum honours Humphry Davy, who identified the existence of the metal base of alum.

[@ib9rt]

Too many comments to find if it was already mentioned, but I think this is an auto-catalytic reaction? I seem to recall that aluminium and halides often have this property, so they speed up dramatically once they start going.

[@mikeltv1]

Did the same experiment in my chemistry class except we put a piece of aluminum wire into the copper chloride solution which turned into a chunk of copper

[@0Sebek0]

I love playing with aluminium reactions, from dissolving it in NaOH to mixing it with Fe2O3, to get flaming hydrogen and molten iron, Al is my favourite one, with its powerful entalphies of reaction xD

[@leokimvideo]

great story, and i wonder if the gopro survived

[@ASMRunning]

FINALLY!!! Its been forever since you posted a video

[@SolarWebsite]

I cannot believe the aluminum/aluminium discussion pops up every time it's mentioned. Come on people, lighten up! What does it matter how it's called... It's science, it's interesting. @Professor: Once again, a fun and interesting video! I also drove my parents to despair with some carpet-destroying experiments when I was a kid. @Brady: To satisfy the aluminum/aluminium-people, maybe have the language department make a video about it for the Words of the World video series?

[@nybotheveg]

3Cu2+ + 6Cl- 2Al --> 3Cu + 6Cl- + 2Al3+ as you can see by the equation the chloride ions doesn't change.

[@megoesmo0]

Metal ions in solution form so called metal complexes, where they form weak bonds to the solvent molecules and negatively charged ions like chloride, sulfate etc. The color of the solution depends on the strength of the bonds, which depends on the ions in the solution. Chloride gives a this greenish color, the typical copper blue you get with sulfate. When you add ammonia to a copper sulfate sollution you get a realy dark blue color. /watch?v=deNWxchzDRg shows this quite well.

[@Subparanon]

Yay! Another video! I just had a sobering thought. One day, these videos will stop for good. All things come and go. What a sad day that will be when we have no periodicvideos to look forward to every week.

[@weiming1998]

The copper forms the typical complex erroneously called the Cu2+ ion, the [Cu(H2O)6]2+ complex/ion, which has a blue colour, instead of the green of CuCl4(2-). Please forgive me if I have made a mistake in my explanation, this colour difference is very complex indeed.

[@rageagainstthebath]

I think I got used to the videos with actual context, like experiments following some special occasion. Anyway, well, glad to see new content. :)

[@aluisious]

Wow...it takes a special kind of "curiosity" to taste test things in chemistry class.

[@RedMeansRecord]

I hope you took lots of footage for us to see it too!

[@gsurfer04]

It's to do with the oxidation states. Copper can exist as either a +1 or +2 ion. The +1 ion is green and the +2 ion is blue.

[@BlokenArrow]

Copper(II) is highly oxidized to +3, Copper(III) is the normal +2 state. Copper(I), which i beleive is unstable, is +6.

[@Daedalus33]

I did this experiment as part of a larger one in my Chem class. We started off with some copper wire and went through a few different compounds of copper and ended up with this. Really fun except we just put some aluminium foil into our beaker and saw it go from there and decanted the solution from there.

[@IrateNub]

Happy Birthday!

[@Kenchan1337]

to admit to such a mistake and shrug it off with a laugh, this guy's my new hero

[@apoorv2711]

@werdnativ the aluminium atoms on the surface of the metal displaced the copper ions from the solution and the Cu2+ ions got deposited on the surface.... No melting needed!

[@kooksies5712]

im afraid to say that is wrong :/ Cu+ is colourless due to its complete d-subshell. it is greeny blue due to the copper(II) chloride impurites. and in fact they are both not even green or blue unless hydrated (by either moisture in the air or in solution)

[@ib9rt]

I guess since the container says "copper (II) chloride dihydrate, reagent grade" it might be difficult to ascertain with any certainty what exactly was in the container...?

[@Melthornal]

Easy: the mechanism youtube uses for counting views lags behind real time. It updates the number of views the video had x amount of time ago. For some reason, I imagine bandwidth consideration, the first 300 views are done in real time. But once it reaches 300 it steps up to a more robust counting mechanism, which lags behind real time.

[@ib9rt]

As I recall, aluminium filings added to liquid bromine makes for a nice volcano. But I guess you have to do that in a fume cupboard these days...

[@weiming1998]

No, no no. The truth is much more complex than that. Notice how the crystals are all green, and a concentrated solution is green? Contrary to what simply high school chemistry teaches you, copper almost never exists in solution as the unbound ion, it bonds with suitable ligands to form a complex. The green crystals probably results from the excess HCl contamination in the crystals, forming a negatively-charged complex CuCl4(2-) via the attraction of the positively charged-cont

[@Neiljnr]

Thank god your back!

[@jenkinstsang915]

As far as the gas goes it's probably a mix of steam (from the heat) and HCl; aluminium chloride, once formed in aqueous solutions, will hydrolyze immediately to form Al(OH)3 and HCl. I suspect that the reaction won't be as spectacular if one uses copper sulphate instead of copper chloride because aluminium sulphate doesn't hydrolyze as much as AlCl3 (but I could be wrong)

[@exactspace]

Interesting. I'll need to check out some experiments with those, thanks.

[@andrestrujado]

Have you tried scratching the inside of a soda can in a circle in the middle and adding the CuCl2 solution.? The can breaks cleanly in two after a few seconds.

[@mcharest24]

Hope you had a nice holiday. Your vacation allowed me to realize I can survive without my weekly dose of videos !!!

[@crazyhans]

It may be just a typo, but it's a damn important one to pick up on and clarify.

[@Queenmania2007]

Love the videos, Brady - I must've seen every single one! I have a suggestion for a future video that will be relevant to both you personally and Chemistry A-Level students across the nation! At Sixth Form, we've learned about a compound called 2,4-dinitrophenylhydrazine (2,4- DNPH), also called Brady's reagent. It's used to identify carbonyl groups in compounds, and I (and, I'm sure, many other Chem students) would love to hear the professor talk about it!

[@Blinkwing]

Actually, the solution of CuSO4 (Copper-II) is blue due to Copper-Sulfate-Pentahydrate-Complexes. CuO (also Copper-II) is black.

[@T3sl4]

What's really interesting is what DOESN'T happen when this is performed with copper sulfate or nitrate. The chloride is catalytic, and I'm not sure anyone yet has an explanation as to why.

[@themomaw]

You're possibly thinking of copper sulfate? A much more vivid shade of blue. To the video: "Chemists should be always careful when designing a reaction and a container to make sure they don't get an unexpected reaction" Like the experiment bubbling over onto the counter? :)

[@WeaselWJ]

Yes, you could indeed do this reaction with a silver salt; in fact, it would likely be more vigorous.

[@WeaselWJ]

There is a video on this channel where the professor answers the question and says the proper word is 'aluminium'.

[@ruadeil_zabelin]

What was the experiment you were actually trying to achieve with the copper chloride? I can understand the mistake with the cupcake holder, but what were you trying to show them?

[@danielbluesmoke]

It was in all the videos... And thanks, I found it!

[@123chemik123]

Concentrated solution of copper(II) chloride is green but when the concentration is lower, the solution is blue.

[@mikkikun91]

True that, forgot the water while thinking about that (long day is long). That most probably will yield Al(OH)3 dissolved in water and protons and chloride ions (basically it can form to what I understood hydrochloric acid). At least I get copper to some degree when performing this reaction I hope. Kudos for pointing that out to me.

[@CHAS1422]

Question: Since the copper is an ion in solution does the copper and aluminum simply do an electron exchange, and the Chlorine ion stays the same?

[@Chaosdude341]

I absolutely love the professor. I want that on a shirt.

[@kurtilein3]

it went between the two layers, met two surfaces to react with, and boiled over. But in a lab thats no big deal. The desk surface is either a kind of chemically non-reactive and virtually impossible to destroy natural stone, or tiles of the same property. Burning coal or burning sulfur or corrosive acids or whatever wont do anything to such a lab table, instead of causing stains.

[@punishedexistence]

Actually,hot concentrated sodium hydroxide and hydrofluoric acid both react with glass pretty well, have to use polyethylene or teflon for those, dilute NaOH isn't too bad though.

[@weiming1998]

Cu2+ ions to the Cl- ions and acts as the ligand instead of water, because not much water is present. When the copper (II) chloride dries, water still remains as the hydrate, CuCl2.2H2O, in which the crystal is still green because the Cu2+ is still bound to the Cl-, making this more like CuCl4(2-).2H3O+ (approximation). When you dilute this with more water, the copper instead becomes attracted to the water molecule, because there are more water molecules than Cl-, so-cont

[@groezy]

Have you done a video on dihydrogen monoxide yet? I'd like to see one.

[@DannyandPatty]

I actually just did this experiment in my Grade 10 science class. Sooooo cool!

[@Comutix]

Top stuff Brady! Coming back down under any time soon? :)

[@WeaselWJ]

Ah yes, good point. I forgot that Ag+ ions are generally insoluble in water; I was merely focusing on the redox potentials to see if the reaction could occur.

[@Bongo1020]

Can't wait for more videos!

[@Higgs666]

My dad didn't agree when I was burning holes in his linoleum floor while playing with magnesium as a young teenager.

[@TheHubps]

you won't have any AlCl3 with this reaction, the main problem is that aluminum chloride undergoes on hydrolysis. Al has amphoteric proprietes (it can behave as an acid or a base). it's pretty hard to have pure AlCl3, believe me :)

[@nejustinas32]

I loved how it shot out of the jar on to the table :)

[@rohankunder1006]

How will u find the exact percentage of copper in cuprous chloride that has been prepared... By instrumental analysis... To determine its purity

[@PCWestOtzi]

wow, that was long time since last upload :)

[@nodariel]

I love the "splurge-shot" camera view

[@SgtCustard]

Fairy cakes are much smaller than cupcakes and have a less sweet base/topping :)

[@Subparanon]

Does anybody know why copper chloride reacts in this way but sodium chloride does not? I assume it's the reactive aluminum stealing the chlorine atoms away from the copper that causes this reaction to occur so is it that the sodium metal holds onto chlorine atoms better than the aluminum tries to take them away?

[@busby3141592]

Sure, 2Al --> 2Al(3+) + 6e 3Cu(2+) + 6e --> Cu3 So Aluminium loses electrons - is oxidised, Copper gains electrons - is reduced.

[@Gluttonysan]

I was taught in school that cooper in a solution turns blue. Why is this one green? Cool reaction though

[@retsaoter]

You don't replace the whole carpet, you steal a patch from under the couch or in a closet.

[@exactspace]

Do chemists perform any reactions that cannot take place in a glass beaker because it would have a bad reaction with the glass?

[@Nexus2Eden]

Thinking about how reactive Chlorine is - I don't think I would ever consider it to be innocuous lol. Is that Chlorine gas being released as vapor during the reaction, or just water vapor?

[@werdnativ]

I just looked up the melting point of copper, it's over 1000°C; aluminum is 660°C. Does this reaction really get that hot, or what is the resulting liquid? It's not liquid copper I assume, so does the copper separate from chlorine in a solid state? I guess the liquid must be the aluminum chloride, it has a relatively low melting point at 194°C.

[@Paldasan]

Is it possible to put the chemical equation in the info box? It's been far too many years since highschool for me to remember them.

[@mimiaslan8772]

what is the gas generated, if this is supposed to be a simple metathesis reaction?

[@RigelOrionBeta]

I used to have a chemistry lab professor whose hands shaked a lot more than him... it was very scary.

[@verkoopprijs]

you can do the same with a sodium hydroxide solution, right?