Please like this comment to alert people to the fact that: Francium just cant be done Its half-life is way too low to exist in any size you could experiment with
Not realistically, but Bill Gates IS an enthusiastic element collector. With the right amount of money, fire/radiation suits, some liquid nitrogen to keep it from vaporizing and a glass of water, it MAY be possible to synthesize 1 gram of it!..lol. Let's do this!! (j/k..just a dream..lol)
@@inbredbanana8156 Because that part isn't what's actually said; it's me editing the quote for clarity because the context is missing. Like, if someone did an interview for a newspaper which went like this: "Did you get a good look at the robber?" "He was about 6 feet tall with red hair." Then the newspaper might quote him as saying "[The robber] was about 6 feet tall with red hair."
*Descripion of how alkali's react with water Lithium: fizzles in water, very dull Sodium: sometimes catches fire, reacts slightly more vigorously Potassium: catches fire, sometimes explodes Rubidium: usually explodes violently and dramatically Cesium: explodes with so much power, it can break the glass where the water is stored Francium: probably stronger than Cesium, never been observed
Francium loses the electron less easily than Cesium because of how many there are and how fast they move, but not by much. It would probably be slightly less explosive than Cesium
Actually sodium is more likely to explode than potassium due to the build up of hydrogen gas. Whereas, it's less likely to explode with potassium as the hydrogen is being used up. Also, the lithium can burst into flames as well depending on the surface area of the lithium and the amount.
I remember seeing this on tv in the early 80s. Loved it at the time and still do. I'm sure it's one of the main influences in sparking my love of chemistry.
For anyone wondering: Francium is radioactive, and with a very fast half life at that (22min), so no one has obtained enough francium for any adequate reaction at the scale that was shown here... ...though one can imagine.
The best part is that there is a sixth alkali metal that they did not mention, called Francium. Francium is extremely radioactive and unstable, and since it is one of the rarest naturally-occurring elements, doing a test such as this with Francium would be very difficult. But one can imagine the results of such a test would be quite disastrous, anyway.
I am so eager to see what would happen if you put Francium in water. I know it's almost impossible and the reaction would be too big but I'm so interested!
Yuki James Yes. The most stable isotope has a half life of a few minutes. It also isn't produced naturally (in meaningful quantities), and can only be made thousands of atoms at a time in particle accelerators. It is so rare that the reactions aren't well known. However, theoretical calculations and simulations show that it would be very similar to caesium, but slightly less reactive (not more).
One3673241 Wasn't that a nuclear explosion during the US nuclear bomb testing in the 50's/60's? I would wonder what would happen if you had a particle accelerator create a boulder of francium at the bottom of the Mariana trench.
***** Yes, but of a Francium bomb, I'm sure. My guess is that it'd explode on impact, possibly go pretty deep into the trench, and cause a radial tidal wave that would hit the surrounding countries, most notably Japan.
me: im gonna put cesium in my mouth my friend: try potassium me: wtf ill just go eat a banana my friend: i mean raw potassium me: a raw banana my friend: boi if u dont
Love this so much. Watched it in IB Chem (For those of you that don't know, that's basically just below or at college level) after we reacted lithium and sodium in distilled water. It was great, and every day is good when a flame is involved.
I always have an insanely absurd question in regards with alkaline metal, particularly Caesium: Alright, so these metals clearly react violently in water. One liquid that shares common properties with water is blood. Human blood is roughly 80% water. I'm wondering if alkaline metals can explode within contact with blood. It gives me this brutal image of an arrow tipped with Caesium being fired into someone's arm, causing the entire arm to explode without a fire or a gun. In short, the question I'm trying to ask here is: can Alkaline metals explode with blood contact as well as explode in contact with water?
It may be possible, but then again the dissolved compounds present in the blood plasma may interfere with the reaction. I'll see if I can ask one of my professors about it later
this reaction wouldn't work as alkali metals are highly reactive so as cesium gets in contact with air it will react creating cesium oxide and be useless.
Given the water content of blood, I would say your theory of Caesium-blood interactions isn't fart from reality. However, I don't believe that an arrow tipped with an alkali metal like Caesium would be plausible, as Caesium is reactive enough to violently react with the water vapor present in even minorly moist air. So say we were to somehow install it within a bullet and could shoot it out of a gun so the Caesium doesn't react with the meteorological status of the air. If that bullet were delivered to someone through their arm, what would allow the Caesium to be released which then would allow it to react with the victim's blood? It's just too many variables to consider, and is much easier to make explosive arrows and bullets that already exist, given how the element works and might behave in a manufacturer. However, I wouldn't rule it out as impossible if you can design a suitable container for the Caesium to be carried with on the projectile, and guarantee its interaction with the desired molecules to cause an explosive reaction.
Actually It is counter intuitive, but Francium is actually less chemically reactive than Cesium... Of course, any amount of francium is dangerous, due to its radioactivity...
Love that caesium! One thing I don't understand is why the reactions are bigger on the way down the group. With the valence shell farther away from the nucleus, I'd imagine the opposite to be true. (Maybe, you can see why I did not major in chemistry for my undergrad degree. Please be gentle with any replies. I already know that I'm a chemical idiot. I don't need any reminders.)
On the contrary, the reason why they react so vigorously down the group is because of their ease in losing their valence electron. The easier it is for a metal to lose an electron shell, the more reactive it is, because it can form more easily ionic compounds with non-metals. Alkali metals have only one electron so it is easier to take off their shell, and down the group, the affinity for these electrons is weaker. All this just means that the alkali metals are very unstable, so it is easy for them to react, and when they do, they form really stable compounds (table salt for example). The formation of stable compounds usually means very exothermic reactions (give out a lot of heat) that happen almost instantaneously.
Wow time flies i watched this video in my school the same year it was uploaded. Unfortunately i took 14 years to get my recognition of like so here we go ,you earned it. 👍
It's also possible that the white solid is NaOH, produced when the water from a concentrated NaOH sol'n produced rapidly evaporates due to the heat. It would be possible to determine if it's NaOH, Na2O, or a combination of both, by dissolving some in H2O and titrating.
Those are neat reactions. I got to see the one with sodium during a demonstration for an intro chem class, and from there on, I never saw the metal again. Funny thing is, we worked a lot with Halogens (Iodine, in particular), but didn't do so much stuff with Alkali Metals, even though both are pretty dangerous.
@denelson83 Yes, it will sink because of its density but it cannot sink because it will react instantly with water. In this video, however, Caesium sank instead of reacting with water instantly like Rubidium.This is because Caesium is highly reactive and will form a layer of oxide very quickly when exposed to the air. This layer of oxide prevents the Caesium from reacting instantly upon contact with water. If Caesium sinks because it was very dense, then Rubidium should have sank too.
I remember watching this in school too. After Cesium, I expected him to say "and now, francium" and for everyone to say "NOO!", the a shot of someone dropping it in the water, then a mushroom cloud.
+Jim Li, and if you do find any francium, (there is an estimated 30 grams or about an ounce of it *in the entire planet crust*, scattered as one atom here and another there), be quick: the half-life of the most stable isotope is only 23 minutes.
Ronald Cheng someone got expelled for dropping pure Na in a toilet and flushing before the reaction took hold. Now we can't observe chemical reactions except when the teacher performs them.
@SNLSniping The reason you don't see Francium done, is because it is very unstable and its almost impossible to get a hold of because it doesn't last very long before it breaks down. You would have to make it yourself to even try to get a water reaction. If its anything like cesium, it will be in liquid form at room temperature. cesium melts at around 70 to 80 degrees F
The whistle became kind of a catch phrase for everyone who grew up watching this on TV, mostly old Open University programs. I whistled when I saw the video here tonight, for what was the first time in years. CSI:NY s09 e02 sent me here. :)
"You can see that things gradually become more terrifying as we go down the group." understatement of the century! I'm quite scared to think what francium would do, if any reasonable amount of it could be gathered up.
Actually due to the size of the molecule and the effects quantum mechanics have on its electron states (and probably other physics stuff I don't really understand too well), it's theorised that Francium would be LESS reactive that caesium.
Jack Berry They didn't show it because only a few atoms of Francium have ever been produced. Its half-life is somewhere around the 8-millisecond mark, it doesn't last long enough to be produced in large enough quantities.
sodium is only more explosive in larger amounts, because it builds up H gas before igniting it. all alkali metals above Na react to quickly and violently to produce this effect, thus Cs, Rb, and K are more reactive than Na. just a bit of info in case you didn't know!
@911650 yes it is but it is in very short supply and hard to find naturally in nature, but has been used as a military grade explosive. I believe it is not tested here for safety reasons
Yes. I'm sure there would be some NaOH, even if the main reaction was the burning of the Na. I doubt if the Na2O formed could avoid the water. I don't see how a flame photometer could tell if it's Na2O or NaOH. though. The ones I'm familiar with are purely qualitative.
@danagol1985 You are correct, the answer to both of those questions is no, and magnesium does not act vigerously with water. Only slowly unless in a powdered form. (Just going through comments)
They always attribute the explosion to ignition of the H2. I think it's more complicated than that. I've thrown chunks of Na into H2O. Little pieces behave as shown here, but if they're larger, there's an explosion. When this occurs, a white, vitreous solid is found scattered nearby. While I'm sure that the H2 ignites to get things going, I believe the metal then ignites, and that the deposit is Na2O. All of the Group I metals are highly flammable.
Please like this comment to alert people to the fact that:
Francium just cant be done
Its half-life is way too low to exist in any size you could experiment with
-9 years late but- you can pin the comment to let more people know
@@rekunan oh my god they actually pinned nine years after
@@minharmonia my job here is done
Not realistically, but Bill Gates IS an enthusiastic element collector. With the right amount of money, fire/radiation suits, some liquid nitrogen to keep it from vaporizing and a glass of water, it MAY be possible to synthesize 1 gram of it!..lol. Let's do this!! (j/k..just a dream..lol)
nerd
Love the dry, British reactions: "As you can see, [the reactions] become gradually more terrifying as we go down the group."
Why are the brackets there?
@@inbredbanana8156 Because that part isn't what's actually said; it's me editing the quote for clarity because the context is missing. Like, if someone did an interview for a newspaper which went like this:
"Did you get a good look at the robber?"
"He was about 6 feet tall with red hair."
Then the newspaper might quote him as saying "[The robber] was about 6 feet tall with red hair."
@@macdjord ah I see thanks man
@@inbredbanana8156
NOW’S YOUR CHANCE TO [[CAUSE A BIG BOOM]]
And then he founded the Dyson vacuum company..."because all other alkali metals lose suction..." (the narration reminds me of those commercials)
"Let's try cesium..."
HOW ABOUT WE *DON'T* TRY CESIUM
Imagine what francium would do if it weren’t so radioactive.
@@gamencraft818 Literal nuke
Caesium*
Gacha Editzzz I’m not British
@@gamencraft818 element 119
let's try cesium, our fifth alkali metal *bass drop*
Alkali metals will do anything to get rid of that extra electron.
They would even do it for a Klondike bar.
+Max Greyfeather LOLOLOLOLOLOL
Ozzie Castava
Nerd
WOAH
Lmao. A fellow scientists
I want someone to try this experiment: put close to each other an ampoule with Cs and another one with fluorine, then break them both with a hammer!
*Descripion of how alkali's react with water
Lithium: fizzles in water, very dull
Sodium: sometimes catches fire, reacts slightly more vigorously
Potassium: catches fire, sometimes explodes
Rubidium: usually explodes violently and dramatically
Cesium: explodes with so much power, it can break the glass where the water is stored
Francium: probably stronger than Cesium, never been observed
Francium is radioactive................. unwise
yeah not only that but francium is unbelievably rare
Francium loses the electron less easily than Cesium because of how many there are and how fast they move, but not by much. It would probably be slightly less explosive than Cesium
Actually sodium is more likely to explode than potassium due to the build up of hydrogen gas. Whereas, it's less likely to explode with potassium as the hydrogen is being used up. Also, the lithium can burst into flames as well depending on the surface area of the lithium and the amount.
Thanks 4 my chem hw m8
I always find it incredible how smoothly and easily the metals can be cut.
it looks oddly satisfying too when you cut it. i feel like cutting it again and again when it darkens
Pure metals are surprisingly soft.
Gotta love that Cesium
Paul Pyro Wow!!
Paul pyro think this is fake to?
It's my favorite element. And yes, I said that.
@@ducky4124 illiterate
i gotta be honest i have no memory of ever watching or commenting here, i think i’m in some sort of simulation
"Things gradually become more terrifying as we go down the group."
This is BRILLIANT.
saying "this gradually become more terrifying as we go down the group" in a calm voice like that just kills me
I remember seeing this on tv in the early 80s. Loved it at the time and still do. I'm sure it's one of the main influences in sparking my love of chemistry.
that whistle at the end.
When he said cesium I was like, "The whole dish is gonna explode..."
Lol awesome joke
I watched this during chemistry lesson! I love the ending (and whole class laughed too).
Do you remember this
@@freck2614 idk about her, but our teacher recommended the video weeks ago and I am just seeing it now. Laughed at the last part as well
@@inesjofremartins867 I got shown this by a teacher too haha
Whoa...I had no idea. Very cool.
U became verified wooo
@@fat1379 lmaooo ur user
Now you know
"Why don't you ask the smartest people in the universe Jerry? oh wait you can't, they blew up"
yesss i knew im not the only one
For anyone wondering:
Francium is radioactive, and with a very fast half life at that (22min), so no one has obtained enough francium for any adequate reaction at the scale that was shown here...
...though one can imagine.
The best part is that there is a sixth alkali metal that they did not mention, called Francium.
Francium is extremely radioactive and unstable, and since it is one of the rarest naturally-occurring elements, doing a test such as this with Francium would be very difficult.
But one can imagine the results of such a test would be quite disastrous, anyway.
But Francium is even more reactive than Caesium
I remember seeing this video in 5th form science... circa 1986, and it was old then...
also best description of a trend in the periodic table - more terrifying...
@@bulwynkl and now im watching it for school...
I am so eager to see what would happen if you put Francium in water. I know it's almost impossible and the reaction would be too big but I'm so interested!
Yuki James Yes. The most stable isotope has a half life of a few minutes. It also isn't produced naturally (in meaningful quantities), and can only be made thousands of atoms at a time in particle accelerators.
It is so rare that the reactions aren't well known. However, theoretical calculations and simulations show that it would be very similar to caesium, but slightly less reactive (not more).
its like a bomb
You know that explosion stock footage they used in the pie episode of Spongebob?
That was a Francium bomb.
One3673241 Wasn't that a nuclear explosion during the US nuclear bomb testing in the 50's/60's?
I would wonder what would happen if you had a particle accelerator create a boulder of francium at the bottom of the Mariana trench.
*****
Yes, but of a Francium bomb, I'm sure.
My guess is that it'd explode on impact, possibly go pretty deep into the trench, and cause a radial tidal wave that would hit the surrounding countries, most notably Japan.
Potassium + water = fire. Wait. "If we're underwater, how can there be a fire?" Patrick Star.
1:08 2Li + 2H2O → 2LiOH + H2
A bit uneventful
1:20 2Na + 2H2O → 2NaOH + H2
Na, it's starts to creep up
1:46 2K + 2H2O → 2KOH + H2
It's gettin' spectacular
1:56 2Rb + 2H2O → 2RbOH + H2
Most terrifying yet?
2:18 2Cs + 2H2O → 2CsOH + H2
RIP Container 2009-2009
I was gonna make a sodium joke but Na. *cringe*
Kevin Ho yeah that was Sodiam funny
Chemistry jokes. Lol
@@matthew78917 😂😂😂
K then ;)
My friend is very Gallium Yttrium. Lmk if u get it .
Cesium: "Don't...FUCK WITH ME, water!" 😡
DJ - W0LFB3AT5 LOL!
@timlin1111 to reactive/unstable to even handle or get your hand on
Macie Jay this is the last place I expected to see macie jay
@@shallteargf5974 dude same wtf LMAO
@Macie Jay lmao
@@shallteargf5974 same lmao i saw this and was like wtf, macie jay? here??
I remember watching this in a chemistry lesson at school in the 80's. Part of a very good series.
and we've watched it again in my school!
2:19 We’ll be right back
me: im gonna put cesium in my mouth
my friend: try potassium
me: wtf ill just go eat a banana
my friend: i mean raw potassium
me: a raw banana
my friend: boi if u dont
I remember the first time I saw this reaction. It blew my mind.
That last one is fantastic.
I like how he describes it as "gradually more terrifying" in such a happy tone of voice.. good god
Love this so much. Watched it in IB Chem (For those of you that don't know, that's basically just below or at college level) after we reacted lithium and sodium in distilled water. It was great, and every day is good when a flame is involved.
THAT SHIT WAS HELLA LIT FAM 10/10 WOULD WATCH AGAIN!
RAHHH MY G I AGREE INNIT THO
I always have an insanely absurd question in regards with alkaline metal, particularly Caesium:
Alright, so these metals clearly react violently in water. One liquid that shares common properties with water is blood. Human blood is roughly 80% water. I'm wondering if alkaline metals can explode within contact with blood. It gives me this brutal image of an arrow tipped with Caesium being fired into someone's arm, causing the entire arm to explode without a fire or a gun.
In short, the question I'm trying to ask here is: can Alkaline metals explode with blood contact as well as explode in contact with water?
This is some nazi scientist idea right here
These metals are generally too soft. We already have explosive arrows with cheaper and more efficient materials.
It may be possible, but then again the dissolved compounds present in the blood plasma may interfere with the reaction. I'll see if I can ask one of my professors about it later
this reaction wouldn't work as alkali metals are highly reactive so as cesium gets in contact with air it will react creating cesium oxide and be useless.
Given the water content of blood, I would say your theory of Caesium-blood interactions isn't fart from reality. However, I don't believe that an arrow tipped with an alkali metal like Caesium would be plausible, as Caesium is reactive enough to violently react with the water vapor present in even minorly moist air. So say we were to somehow install it within a bullet and could shoot it out of a gun so the Caesium doesn't react with the meteorological status of the air. If that bullet were delivered to someone through their arm, what would allow the Caesium to be released which then would allow it to react with the victim's blood?
It's just too many variables to consider, and is much easier to make explosive arrows and bullets that already exist, given how the element works and might behave in a manufacturer. However, I wouldn't rule it out as impossible if you can design a suitable container for the Caesium to be carried with on the projectile, and guarantee its interaction with the desired molecules to cause an explosive reaction.
I love how it just ends abruptly after the cesium explodes
I just love how abruptly the video ends
Has to watch cesium over and over again. The explosion is just so cool.
I remember watching this in year 10, about 19 years ago, and the reaction with caesium and water still gives me the giggles!
The cesium at the end makes me laugh every single time.
Actually
It is counter intuitive, but Francium is actually less chemically reactive than Cesium...
Of course, any amount of francium is dangerous, due to its radioactivity...
0:35 turn on the captions...
+Connor Steppie Nazi another reaction of the alkali metals the reaction. Really youtube... really?
+Connor Steppie those responsible for the moose comments have been sacked.
+Bradox Taylor wat
where does it say that
+Connor Steppie 1:55
+Connor Steppie 2:12 too, that last bang is an accurate representation
I just learned hours of chemistry in a 2 minute 22 second video
Good for you NASA :-)
No you learned 2 minutes and 22 seconds of chemistry.
* claps * Epic
0:33 "Sodium is kept on the oil to prevent reaction with f*ck"
subtitles. please.
omg xD
Sodium is kept under oil to prevent it reacting with air and water in the air.
playfulpippapony Apparently not, according to the subtitles.
They're sodium incorrect and made a Na-sty mistake, but let's not get salty over it
it got fixed fffffffffff
Here's a picture if you don't believe me: upurs.us/image/70414.png
It was probably made around that time. A lot of us who grew up in the UK remember seeing this video at school. :)
Summary:
Lithium: mild reaction
Sodium: slightly stronger reaction
Potassium: hydrogen catches fire
Rubidium: explodes immediately
Caesium: glass got broken
imagine francium, radium and the future elements discovered 119, and 120
HolaSoyAlejandro Ow! A more than a meter explosion radius!
I remember seeing this video very vividly 17 years ago! How awesome!
Wow....Rick and Morty wasn't lying
Me eating something that has potassium and drinking water right after:🔥🧨🧨
Love that caesium! One thing I don't understand is why the reactions are bigger on the way down the group. With the valence shell farther away from the nucleus, I'd imagine the opposite to be true. (Maybe, you can see why I did not major in chemistry for my undergrad degree. Please be gentle with any replies. I already know that I'm a chemical idiot. I don't need any reminders.)
On the contrary, the reason why they react so vigorously down the group is because of their ease in losing their valence electron. The easier it is for a metal to lose an electron shell, the more reactive it is, because it can form more easily ionic compounds with non-metals. Alkali metals have only one electron so it is easier to take off their shell, and down the group, the affinity for these electrons is weaker.
All this just means that the alkali metals are very unstable, so it is easy for them to react, and when they do, they form really stable compounds (table salt for example). The formation of stable compounds usually means very exothermic reactions (give out a lot of heat) that happen almost instantaneously.
The guy put Caesium in the water and caesium was all like "OH HELL NO!"
2:18
Imagine throwing hunks of that into a Lake...
Photon torpedo away!
Wow time flies i watched this video in my school the same year it was uploaded. Unfortunately i took 14 years to get my recognition of like so here we go ,you earned it. 👍
I remember seeing this video on a laser disc in high school. We had the teacher replay the Cesium explosion like 10 times. :)
“let’s try caesium, our 5th alkali metal.” *Famous last words*
"Let's try cesium."
Glass: Why do I hear boss music
Hahahhaha
One of my favourite UA-cam videos of all time, bar none.
I LOVE chemistry! What is interesting is the Alkali metals, the radioactive metals, the poisonous metals, and mercury!
This is GREAT! It helped me to answer my assignment questions. Thank you sooo much!
Lithium: Floats around, whizzing
Sodium: Floats and whizzes faster
Potassium: Flame
Rubidium: Fireworks
Cesium: Explodes (breaks glass)
Francium: ????????
HairMetalBrony1016 Fr: Whole lab explodes
Francium: about the same as cesium
“Let's try Cesium" *Explodes* *Silence*
Caesium, you're only supposed to blow the BLOODY DOORS OFF!
It's also possible that the white solid is NaOH, produced when the water from a concentrated NaOH sol'n produced rapidly evaporates due to the heat. It would be possible to determine if it's NaOH, Na2O, or a combination of both, by dissolving some in H2O and titrating.
wow cutting metal like that looks so satisfying
And the final ingredient...!
2:18
Finally someone who knows Rick and Morty references
How about...
"Let's try Cesium, our fifth alkali metal."
*puts chunk in*
*big explosion causes glass to break*
"Oops."
Those are neat reactions. I got to see the one with sodium during a demonstration for an intro chem class, and from there on, I never saw the metal again.
Funny thing is, we worked a lot with Halogens (Iodine, in particular), but didn't do so much stuff with Alkali Metals, even though both are pretty dangerous.
That last part where they react with water was terrifying.
@denelson83 Yes, it will sink because of its density but it cannot sink because it will react instantly with water. In this video, however, Caesium sank instead of reacting with water instantly like Rubidium.This is because Caesium is highly reactive and will form a layer of oxide very quickly when exposed to the air. This layer of oxide prevents the Caesium from reacting instantly upon contact with water. If Caesium sinks because it was very dense, then Rubidium should have sank too.
Anyone else here for school work help or using it in class as a resource?
sort of. im in chemistry i just showed my teacher this vid and hes goin to show it to the class
I remember watching this in school too. After Cesium, I expected him to say "and now, francium" and for everyone to say "NOO!", the a shot of someone dropping it in the water, then a mushroom cloud.
Where is Francium?😂. Try it! But be at least 1000 yards away
lmfao
+Jim Li It is, but good luck finding any
+Jim Li, and if you do find any francium, (there is an estimated 30 grams or about an ounce of it *in the entire planet crust*, scattered as one atom here and another there), be quick: the half-life of the most stable isotope is only 23 minutes.
lol. Try ten miles away! XD
We had them decades ago. It's not possible to synthesize macroscopic amounts of it.
it's so good to finally see this!
Ahh the good ole days, pick up a lump of cesium from the stockroom and plant it in the teachers bathroom.
You'd be lucky if you don't get expelled for that. XD
+Ronald Cheng Yeah lol
Ronald Cheng someone got expelled for dropping pure Na in a toilet and flushing before the reaction took hold. Now we can't observe chemical reactions except when the teacher performs them.
Caesium was amazing. Thanks this really helped me with my revision! :)
Shoutout?
@SNLSniping The reason you don't see Francium done, is because it is very unstable and its almost impossible to get a hold of because it doesn't last very long before it breaks down. You would have to make it yourself to even try to get a water reaction. If its anything like cesium, it will be in liquid form at room temperature. cesium melts at around 70 to 80 degrees F
Do they make Cesium soap?
U will explode while taking a bath😂
The whistle became kind of a catch phrase for everyone who grew up watching this on TV, mostly old Open University programs. I whistled when I saw the video here tonight, for what was the first time in years.
CSI:NY s09 e02 sent me here. :)
"You can see that things gradually become more terrifying as we go down the group." understatement of the century! I'm quite scared to think what francium would do, if any reasonable amount of it could be gathered up.
my science teacher explained that it would have flying shrapnel like i think twice as far as cesium
Francium is used in bombs but only profesional people can have it or really experienced universities if they have a detailed explaination
Actually due to the size of the molecule and the effects quantum mechanics have on its electron states (and probably other physics stuff I don't really understand too well), it's theorised that Francium would be LESS reactive that caesium.
Francium is Radioactive, its why they didnt show it here.
Jack Berry They didn't show it because only a few atoms of Francium have ever been produced. Its half-life is somewhere around the 8-millisecond mark, it doesn't last long enough to be produced in large enough quantities.
sodium is only more explosive in larger amounts, because it builds up H gas before igniting it. all alkali metals above Na react to quickly and violently to produce this effect, thus Cs, Rb, and K are more reactive than Na. just a bit of info in case you didn't know!
R.I.P
Men: 0 / Cesium : 1
"You can see that thing gradually become more terrifying as we go down the group."
I loled.
I like how they ended it exactly after it broke😂
@911650 yes it is but it is in very short supply and hard to find naturally in nature, but has been used as a military grade explosive. I believe it is not tested here for safety reasons
Bath Bomb
Literally lol
Thank you for making this video!
I remember this from when i was in school XD
It’s like a fish dying in hot water
now where is the two parts plutonic quarks?
Yes. I'm sure there would be some NaOH, even if the main reaction was the burning of the Na. I doubt if the Na2O formed could avoid the water. I don't see how a flame photometer could tell if it's Na2O or NaOH. though. The ones I'm familiar with are purely qualitative.
I just laughed so hard with the cesium. funny
WOW! Caesium is SO explosive. I can't believe what ive just witnessed!!!!!!!!!!!!!! SIMON WALLER
Reminds me of cheese when he cuts into it.
@danagol1985 You are correct, the answer to both of those questions is no, and magnesium does not act vigerously with water. Only slowly unless in a powdered form. (Just going through comments)
lie for like?
@@lakikaki9413 😍
Nerd
@UCX5YEGgXUcJ_FbF0csAUrXw reported
They always attribute the explosion to ignition of the H2. I think it's more complicated than that. I've thrown chunks of Na into H2O. Little pieces behave as shown here, but if they're larger, there's an explosion. When this occurs, a white, vitreous solid is found scattered nearby. While I'm sure that the H2 ignites to get things going, I believe the metal then ignites, and that the deposit is Na2O. All of the Group I metals are highly flammable.
Why would anyone think this is fake?
Dennis Eluyefa who does?
1:45 can we all just appreciate that droplet sound for a second?
Anyone else watching this for school lmao?
1:07 "sizzle sizzle"
1:19 "sizzle fizz fizz sizzle"
1:44 "plop fizz crackle sizzle crackle"
2:01 "POP fizz CRACKLE sizzle fizz"
2:16 "EXPLOSION!!!"
You're about... one year too early.
This guy sounds like Anderson from Sherlock.
I love the mili second of peace before the cesium reacts