How To Make Sodium Metal
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- čas přidán 27. 08. 2024
- This is one way sodium metal can be isolated using NaOH and Mg. Mg has a strong enough desire for oxygen to tear it from the NaOH, leaving ingots of elemental sodium behind.
2Mg + 2NaOH = 2MgO + 2Na + H2
Thanks to NurdRage for the equation.
/ nurdrage #NightHawkInLight
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I grew up loving chemistry but became a carpenter now that I'm old I'm falling in love with chemistry again. Spare time to create awesomeness. Thanks for sharing.
Have you watch Dr.Stone? There's a carpenter that love making chemistry apparatus for main character. :)
@@zafeerahrifin2056 thanks buddy
@@nothingnew69 you're welcome
Can you learn me chemistry
@@user-ig3pn8hq8k teach ?
I'd say I like sodium hydroxide, but that would be a lye.
good one!
*chuckles*
*slaps knee*
Lmao
These chemistry comments are killing me 😂
Lol its funny cause it's the same thing
Yes. The salt needs to be heated to it's melting point then a strong electric current is passed through it to split the sodium from the chlorine. It's quite dangerous.
Can this be done with table salt?
@@jerometruitt2731 don't do it. just don't. You would be working with such dangerous materials and at high heat which adds even more danger. did you know molten salt explodes when it touches water? I'm betting you didn't, and who knows how many other hidden dangers there are.
@@jerometruitt2731 Yes sodium metal can be extracted from table salt but the melting point is about 801'C. Some calcium chloride is added to lower its melting point to about 600'C
Potassium will become unstable in mineral oil eventually, but sodium has been safe to store indefinitely by my experience.
What should potassium be stored in???
@@ekeene11 A vacuum ampule
@@NighthawkinlightYou replied after 10 years😂😂
@@The.RandomTubeI got recommended today
@@ekeene11Liquid paraffin wax.
@jeremiahswee Very true. This is not a typical displacement reaction. Rather than trading places with the sodium, the magnesium attacks the oxygen contained in the hydroxide group. This creates MgO, leaving Na and H on their own, unable to bond together. The Mg does not force the Na out because it is more reactive, but because it has a stronger desire for the oxygen than the hydroxide group does. If the hydroxide group is decomposed, any metal attached to it is freed, regardless of reactivity.
Magnesium is so expensive, wouldn't it be better to use five-karat electrolytic sodium hydroxide?
Loved the spoon reaction.
Sodium hydroxide is a popular drain cleaner, and is often sold in solid form. Be sure to read the ingredients on the label, though. Magnesium can be found in firestarters, in the sporting goods section of your local supermarket. They're sold as solid blocks with a large flint glued to it, though, so you have to powder it yourself. You can also check online, though powdered magnesium is probably expensive to ship.
You can also find magnesium at a plumbing store for real cheap. It's used in boiler tanks. Ask for a magnesium rod.
Don’t do this. Any amateurish mistake can cause severe burns.
I was gonna make a Sodium joke...
But Na
***** Pls laugh!
This is the best copy-pasted joke ever.
***** Tnx m8!
You're worth your salt, Dank Prince.
OH you're funny.
That was sodium stupid.
Sodium was stuck to the surface of the block of steel. Scraping it with the spoon exposed fresh sodium to the air, which caused it to rapidly oxidize, releasing enough heat to catch fire.
@Khalastas Try not grinding the NaOH. If you leave it in prill form it will react more slowly and leave more sodium. If you use a thick piece of steel as a lid like I have much of the sodium will condense on it because it's so much cooler than the reaction vessel itself. It can then simply be scraped off.
Why not just heat the whole mixture under oil? Sodium melts at around 208F, and MgOH does not. The sodium could coalesce like on Nurdrage.
Magneto! Go
sodium isn't magnetic...
Sodium does not contain iron and is not magnetic
@@OGJessie why would it have to be magnetic? it coalesces because of the strong surface tension of molten sodium.
@Cosmic I was talking to Fred
2NaOH + Mg → Mg(OH)2 + 2Na
2Na + 2H2O → 2NaOH + H2
Maybe, it depends what it's to be used for. It is too soft and reactive to make a useful alloy for any structural purposes.
Super cool - though I wish you would explain the chemical reaction that is taking place with each step. It would help chemistry students understand what each elemental step contributes to the over all reaction process.
However ...totally awesome!
I'm new to this here. I've always been fascinated with things like this and I have been through so much in my life that caused me to never get my ambition started. I'm 54 years old now and if I don't start now I never will.
You can also use electrolysis to extract it from saltwater (lots of salt in the water)
Nice work!
Someday i'll get around to making a sodium video as well. i'll probably blatantly steal (with credit) a few of your techniques :)
Yo now u have 700ksub
Wouldnt the sodium react with the water making sodium hydroxide again?
Chris Love Yes It does to some extent. This is a very wasteful process because of that very issue and because your going to loose a lot of sodium with the heat of this reaction. That's why he leaves the lid on. To keep as much air out as possible and to let the Na cool as much as possible, because the cooler it is the less reactive it is. But in a way this reaction is nice too because it produces oxides which stick to the lid and help seal it, But none the less Na is still wasted.
Now he utilised several things here, he used the fact that Na floats, to his advantage, and that the heat formed will cause the Na prills to globulate into proper dense balls, and finally the fact that the slag is heavier than water.
All of this means that once dropped in to the water layered with oil, the Na sinks through the oil because it has a lot of slag and impurities attached. It then hits the water layer and reacts heating up and making a larger solid glob of Na and releasing the slag from the sodium which falls to the bottom as its heavier.
Now that the Na is pure it is now not weighted down by the slag And starts to float back up into the oil phase, Which upon arrival stops reacting.
So Yes the sodium reacts with the water but only a certain amount of it as it is not reactive enough to fully react instantaneously, and it is simply not in the water phase long enough to react fully before floating into the neutrality of the oil phase.
This I would like to add is a very ingenious method of separation for the home scientist. If NightHawkInLight came up with this part of the process I'm very impressed. As it requires an innate knowledge of how things work, how things behave and also Physics. But the most important thing here is to have the cerebral acuity to be able to come up with processes like this. there are just not that many people out there who understand the complexity but yet the shear staggeringly simple mechanics behind this. It is great to see.
To ***** skofilmz It would not be possible to make anything other than sodium or Lithium utilizing this method, as anything else would be too reactive. In the case of K it reacts very quickly with water very often in an explosive instant. but because it would be contained between an oil layer and the water, it would most probably react instantly with little explosions and a big mess.
As for the Cs Forget about it, it will react even more so. I don't know why people have a fascination with the lower end of the Alkali's they are nowhere near as powerful as they are in peoples minds. The power increase is not linear as you go down the table. Rb is not a whole lot more powerful than K . etc....
Even if you could make Cs you be much better off trying sigma's website they will sell to the public. But even for a few grams like 2gr it would be very expensive maybe $60 in your money. You would have just as much fun with K and 3/4 of the bang.
Robert Cece I disagree, the sodium he has at the end is very pure If he pulled that big globule out of the water at the very end, I.e just washed it once more there would be very little oxides or physical contaminants. I do think it is a very wasteful process, but it's wastefulness is off set by its practicality.
On final point NightHawkInLight if you had of made a strong alkaline solution (some experimenting might need to be done to determine the optimum conc) instead of water I would Imagine you would get higher yields as the Na would not react to such an extent. I don't think In my opinion that simply leaving the sodium to turn the water basic is going to result in a strong enough solution to make much of a difference.
That is why maybe try starting out with a strong basic solution instead of water might yield more favourable outcome. But I am only theorising here.
atourdeforce and the longest comment award goes to...!
Yes
AJ Pollard and there's the shortest answer ^_^
atourdeforce As far as your "strong basic solution", NaOH would surely be a good candidate, since you have that in the first place, and since that's what the sodium would otherwise be trying to form. Would a saturated solution mean more or less 100% of the sodium is freed?
Awesome experiment, we did this as an experiment at school, it was great :-)
How did it go? I’m a chemistry teacher thinking about trying this
aaaaaand im on the goverment watchlist
yor masony
loomynarty why?
VoxNerdula Well someone learned a new word.
loomynarty Glad to be of assistance shit fuck fucker fuck
Why?
Okay, so that was essentially a thermite reaction, right? But I thought the elemental metal had to be more reactive than the metal that starts as a salt. That's why Al+Fe2O3 works, isn't it? Mg is definitely not more reactive than Na.
I thought the same thing but chemistry likes to break itself apparently.
In a normal thermite reaction only the metal oxide is being reduced. Here both the sodium ions and hydroxide ions are being reduced, to sodium metal and hydrogen gas respectively. The reaction is enthalpically favorable by the heat of formation of MgO and entropically favored by the formation of hydrogen gas. It's favored but kinetically slow hence why high temperatures or an alcohol catalyst is needed. Long story short normally yes, sodium is more reactive than magnesium, but in chemistry there are always exceptions.
A big enough chunk of the metal can be used as an exposive that denonates when submerged in water.
That, and maybe some experiments with other reactions, or with conduction.
Okay someone explain to me why this reaction still works even though sodium is higher on the activity series and therefore shouldn’t let the single replacement reaction occur.
Edit: never mind I figured it out
Could you please tell me how.
Making the sodium is almost as cool as the sodium.
Would Al powder work at all? NaOH reacts with Al because it is amphoteric, but if you lit it quick enough could it work?
No it would form sodium aluminate
@@spookywizard4980 and hydrogen + water
@@icarokaue7334 ohhh yeah it does ;)
Yes, you do it any time you dissolve the salt in water. When salt dissolves it dissociates into it's respective Na+ and Cl- ions.
sodium has a low melting point so when it hit the water it melted itself and formed a ball it held together like that because as soon as part of the ball hits the water it burns pushing the ball from all sides
That's beyond my knowledge. Maybe someday.
such an amazing comment
The most interesting thing I've watched today.
Thank you for the reply. I have always wondered, over the years, what aging might do to the various elements in that box. I don't think that chemistry sets are sold anymore, in the US, which is too bad. As a youngster, I was not interested in following recipes. So, the chemistry set sat around. It's mostly intact, but I did lose the spectroscope. Other young people who have patience no longer have easy access to beginner experiments. That's too bad.
Sealing it in an airtight container submersed in mineral oil be enough. You can store it in a jar like this for months. Unless where you live is extremely humid, even taking it out in open air likely won't cause ignition. As well, mineral oil has a density of about 0.8g/cm, making the sodium more dense and therefore will settle to the bottom over time, further decreasing exposure.
amazing, I love home chemistry
Hey, when you placed the slag in the measuring cup, why didn't it react how it did in the end of the video?
The mineral oil covered up the sodium before it could really begin to heavily react.
Sodium hydroxide is hygroscopic (readily absorbs moisture from the air). So it's probably best to grind it up (and quickly) after the magnesium is ready, unless you can work in an environment with very low humidity. Just leaving sodium hydroxide exposed to the air for 15 minutes or so can achieve noticeable amounts of moisture.
sodium in its elemental form is a soft metal and it is highly reactive heavy metal. when exposed to air it can react and spontaneously combust. that is why you are using the mineral oil, it coats the sodium.
why would someone dislike this video?
Because someone got sodium pills in their allergi medicine on April fools day
Some people are just naturally "salty".
Felony Videos da dum crash...
Not sure, but it seems to be a rule on CZcams that every video has to have at least some dislikes.
Because sodium Cant be created, it's an element hes just extracting it
where do you find sodium hydroxide and magnesium powder??
Sodium hydroxide is lye. It's sold and used a drain cleaner. It can be bought at hardware stores and such. Good luck with the magnesium. I'm sure it can be easily made with a metal file if one can find a sorce of solid magnesium.
You can get a magnesium rod out of a hot water heater or go to walmart or a hardware storeto buy one they cost around $7.50
dunno
You can easily buy pounds of magnesium powder on eBay.
@@chaoticchem what about Epsom salts?.
I like the different types of metals that reacts with water in a violent manner like that.
I still have a ChemCraft chemistry set from 1969. It's been under one pile of stuff, or another, since about 1974. I won it, in '69, but being a kindergartener, my parents would not let me play with it for the longest time. I believe that there is a vile of sodium metal, in there, and one other element, both of which came covered in mineral oil. To get to it, now, would be a major pain. I have often wondered, however, what kind of time bomb I have in my house.
Hmmm I just stumbled upon this video and I'm thinking if the U.S. government wasn't watching me before, they are now.
That sounds like me entire life
I always feel like somebody's watching me,
and I have no privacy.
you can buy sodium metal online anyway lol
@@fatherthyme4587 lol
Hey Nighthawk.
I've tried this experiment three times, twice with magnesium and once with dark aluminium.
The aluminium reacts significantly slower, similar to a burning candle. The magnesium burns similarly to yours. It leaves the large chunk of slag, and when I attempt to do the separation it all sinks and reacts away leaving no sodium ingots.
I'd love to attempt it again but I mineral oil is quite expensive for me. Do you have any suggestions?
Thankyou!
As a matter of fact I'm a physicist so i've had many chemistry classes. And if I'm not mistaken the guy in the video gets his Na from NaOH...so If i can get NaOH from NaCL into water....I think you proved me right.
im pretty sure the coating of oil will protect it from that. its just like a greasy plate. when you rinse it with pure water, it is somewhat "water" proof
How to make Caesium metal?
same process except caesium hydroxide. BUT IT IS EXPENSIVE AND IMPURE.
Konstantinos Myrianthefs NO, its hard to find, but their maybe a few samples online such as in Sigma-Aldrich Chemicals you can buy it there.
***** Where to get caesium salt?
***** Search it online. You might find something.
CuriouScienceDude That thing would be fluorine gas instead of Cs
Im a bit confused with the extraction. When the sodium passes through the mineral oil layer and reacts with the water why doesnt it produce NaOH?
+Badplum25 It does
NightHawkInLight Then how did you create Sodium?
sodium metal is less dense than water and mineral oil... so it floats to the surface of the oil and doesn't react fully with the water :D
Michael Schöllhorn oooo okay thanks that makes sense I was rlly confused :)
Some of the sodium is wasted and some keeps floating!! u can collect the floating part!
Hopefully, someday! I'm really interested in seeing real use of chemistry. Not even "Periodic Videos" shows anything more than stuff burning or blowing up. I'm outgrowing views of sudden color changes of flames, or gold dissolving into acid, or a cracked swimming pool, or a damaged driveway. Seeing one is seeing them all.
you can do many things, like drop it in water to make a entertaining explosion. it can also be the precursor to many chemicals and alloys.
Hey, I have a request: can you demo how to make some of the most useful chemicals of the last 100 years, like nylon and Lucite? Things that blow up give me some ideas for vandalism, but I'm really interested in constructive stuff. (Though, flushing a chunk of sodium, coated in a slow-dissolve material, down the toilet in a hated business establishment could be fun!)
just gotta put it in a pill capsule and flush it down my toilet
It wouldn't flush, sodium floats.
actually in the original VW bugs magnesium was used for the engine block and gear box. Around 20 kilos of magnesium was used in each car. In merica you can buy magnesium sticks they have flint on the side and you can use them to start camp fires.
With results, even if raw ( no complete chemical reactions written formulas, also for the collateral chemical reactions ).
Congratulations for this window to Chemistry-Universe !
Feel the wrath of the flaming spoon
=-O
I wish i would studied Chemistry....
Never too late to start. That's what I'm doing. Even if it is only as a hobby.
***** And outside. If you're really passionate about something, your interests usually leave the classroom.
Never too late. Not much older than me.
@martin27 I'm 32 and just getting into chemistry and not going to college. One doesn't need college to get into something like this. Just a willingness to learn and a live of science.
Think about it. When the sodium metal contacts the water hydrogen gas is produced in an exothermic reaction. Therefore the sodium metal is floating on a cushion of hydrogen causing it to glide along the surface in a very low friction way allowing it to bounce from edge to edge of the container.
you are a genius man....
I love chemistry and never though of magnesium to reduce sodium
(y)
thats how i feel when i stepped on a teemo shroom xD
Mexico is #1 on chemistry for drugs
Bruh :p
tip firework (flash) powder = magnesium powder, for sodium hydroxide make very concentrated salt water and run an electric current through it for a few hours then let the rest evaporate
moisture in the air/on the spoon can react with sodium, there must have been some on the spoon. the mineral oil prevents moisture from getting to it
ALCHEMY!
fucking where we going to get Sodium Hudroxide and Magnesium
Sodium hydroxide is a drain opener just check at your local hardware, make sure it's 100% NaOH.
You can buy also Sodium Hydroxide from a Hardware store. But I'm not sure where you can buy Magnesium powder, I get my Magnesium powder by grinding a piece of magnesium into a powder form. The piece of magnesium I use is a fire starter kit that you can get at Walmart or at Dollar General.
+Mason Poindexter I was thinking the same thing as I got 50 or so lying around. Say, what's your method of powdering the mag? I was using a sharp knife and scraping back and forth I did it for hour and then weighed my products turned out to be .3 man there has got to be better way
because it hadn't all reacted and the spoon scraping on the brick caused just enough friction heat to react what was left
Hey, you should have explained the bit about how sodium separates from the slag in between the layers of oil and water, by sacrificing some amount of itself.
SO THIS IS HOW YOU MAKE METH.
I would think so. I think electronegativity would come into play, but Mg should still be able to wrest K from K+.
brick go BOOM! have to try this sometime!
yes, group one metals are very reactive with water.
If you wrap the sodium in something that will insulate it from the water momentarily, and allow it to sink, the reaction of the sodium submerged reacting with the water can be spectacular. And dangerous.
Dude my son loves chemistry and my son is around 9 and he's quite interested to learn about compounds that contain sodium and sodium metal itself thanks for posting this video you can include more videos about sodium if you can or you can't do better.
I have a few more videos you'll find if you look for my alkali metal series. It's a dangerous project though, I wouldn't recommend sodium metal as a first project with your son.
you can also use molten salt and electrolysis it, this is a lot cheaper, and since you hopefully are venting your furnace anyway the chlorine gas wont be a issue (still better than sodium hydroxide).
Many notepads, phones etc use mag for the chassis -- not sure how pure but filings sparkle nicely in flames. Some cars have mag gearbox casings too.
I worked for DuPont for 32 years in niagara falls the only sodium producer in N America They made rail cars of the stuff 24/7 365 Threw a 10 lb chunk in the river took off like a hydroplane. So much smoke it stopped traffic 1/4 mile away for quite a while
i recommended my chemistry teacher to you. we watch your videos every week now
No, the sodium does not react with heat and oxygen, but with oxygen only. Sodium is a very reactive alkaline earth metal, so when it reacts with oxygen; lots of energy is released (reaction is exothermic) in the form of heat (fire), this produces NaO (sodium oxide).
In water, sodium reacts with H2O (water) and in doing so displaces a hydrogen; (re)forming NaOH. This reaction is also exothermic, which is why the sodium is both; on fire (heat energy) and moving around quickly (kinetic energy).
But in the metal reactivity series
Na>Mg
Then how magnesium displaces sodium from its compound.
Mix it with CaCl2. As I know it will lower the melting point of the mixture, however, it will be impure...
This video is really cool, but what are some practical uses to making sodium metal?
Yes, by melting it and doing electrolysis. Look at my channel, where I showed a way to separate lithium from lithium chloride. Sodium is similar, but temperatures are way higher.
I expected the sodium to react more violently...
Very nice video!
The sodium looked like a lump of clay before you dropped it in the water. Why does it appear white and form a sphere on the top of the water? Was it hot or molten?
Because that's not all sodium. We're calling it sodium, just like you're calling a rusty piece of steel "metal". The oxides react with the water, forming NaOH. This dissolves in the water, exposing the pure sodium metal underneath, which hasn't reacted with the atmosphere yet.
After 10 years I'm still coming back to your beautiful videos. Why doesn't the sodium fully burn up when you're separating it in the water?
The sodium floats on top of water so as soon as it starts reacting it floats to the top and gets coated in oil. That protects it from the water.
@@Nighthawkinlight That is straight up genius, and I just gushed to my partner about getting a response from a childhood hero :3333
@@MyCommentsRMaturelol No hero here, just a punk kid that grew up with a camera. Ha!
A kid my old teacher knew stole a brick of sodium from the science lab.(not knowing it was a highly unstable substance) The kid decided to get rid of it by throwing it into a local pond. I was told it was an impressive reaction.
Anyone noticed the 'chemical version' of the leidenfrost effect ? The rapid hydrogen production prevents the quick reaction of the piece of metal with the water :D
I could imagine that something, like that, if it sinks to the bottom of the pool (which maybe it wouldn't), but if it did, you could very well crack the pool. That would be a really expensive reaction.
"Ferb, I know what we're gonna do today!"
Is it possible to melt the sodium into a liquid in the mineral oil to collect a pure chunk of shiny metal?
same reaction with water only its way less reactive so less likely to burn but still makes hydrogengass and also don't drink from the alcohol after the reaction it forms sodium ethoxide wich is corrosive,harmfull and burns hard
Hey thats cool as soon as you dropped the flat crumbling piece of sodium into the water it basically immediately formed a sphere.
No, I replied to your comment, not theirs.
You asked 'Seriously' that apparently makes you care.
I pointed out that fact that you shouldn't care what people do and don't do on the internet unless it affects you or is illegal.
you can get it from street lamp bulbs too ( sodium vapour ones ) i blew up one of the toilet pans at school in the 80's with it.........happy days !
This is useful and helpful video for me.
Thanks dear
I like your videos
Aside from a Chemistry classroom, what is the value of this Sodium metal? What can I use it for? I love your videos by the way, and I am subscribed.
My chemistry teacher told me I could react sodium metal with whatever I want if I could find a displacement reaction to form it, as we're not allowed to buy it. Thanks!
nice idea, oil and water.
Simple and working!
I wonder if you could pop a few small pieces in a vial and bring it into the woods, and if you need to make a fire, just put a small amount of water over the metal and then light kindling with the reactive heat.
I think Sodium would take a loooooooot longer than the other metals that are more unstable. I'm not even sure if it will ever react to such a low level of moisture. Ones like Cesium, however...
Not pure, with elektrolyses you can form NaClO (in cold environment) or NaClO3 (hot environment) or NaOh and Cl2-water(or HCl) and with this video you can use NaOH to make Na. for making NaOH you need to seperate the place where the anode and kathode is inserted in the NaOH solution (a membrane between the solutions) and then react so that on 1 side you get NaOH and the other side chlorine gass wich is corrosive etc
I don't understand the separation step.
If the purpose of the water/oil interface is for Na to react with water so that it can get separated from the slag, why doesn't Na/water reaction oxidize Na into Na+ ?
Thanks!
It does,but Sodium metal is less dense than water and mineral oil,so some metal wil float.
not if from the electrolysis it is released as chlorine gas. It will be "left" as a byproduct of the reaction, but it should dissipate (do not inhale unless you want to suffocate in your own chest..). I havent done this myself, and am just guessing with basic chem knowledge.
I did this with my school we put a larger piece in a big glass cylinder it was awsome!!