Now that's how you teach these things. Not some dude talking in some class while the students are yawning their knowledge out their brains to oblivion.
I don't know about you, but in my Chemistry class, the teacher did regularly show us such things. I even (vaguely) recall experiments with radioactive stuff he had to do outside. That was about 20 years ago.
These chemistry videos make great teaching aids and give me ideas for variation experiments to demonstrate myself. One reaction that I was surprised wasn't shown was with the alkali metals - vigorous and beautiful reactions that produce common salts, in fact you probably know one of those - that being of course sodium chloride, AKA table salt, but there's also lithium chloride, potassium chloride, sodium iodide, etc.
Yes, now you're right: many transition metals show +2 and +3 oxidation states; Al is only +3 under normal conditions* - it's in the Boron group (a main group element). * This is a disclaimer: I think Al can show either +1 or +2 (can't remember which, but only in molten salt solution, such as dissolving Al metal in molten AlCl3 - might be wrong on the details here, but this is an unusual situation, almost never happens.
The fires are started by fluorine but most of the burning is actually from oxygen in the air because the fluorine doesn’t have time to reach the entire substance.
I guess that explains why oxygen is the oxidizer that keeps us alive. Fluorine may react and thus spend its energy before even having a chance to reach our cells.
No gases are produced. Aluminium and bromine give aluminium bromide which appears as aerosol (tiny solid particles). It is mixed with excess bromine vapor so it looks yellow-orange, but it's actually transparent crystals when pure. Aluminium bromide is very corrosive to tissues cause it reacts with water, increasing the acidity of the solution, but not inherently very toxic per se.
How about fluorine and water? Or chlorine and water? I've never seen either of those reactions demonstrated. I wonder how vigorously each react with water.
Vid #3: 16. 1. Fluorine-colorless 2. Chlorine-greenish-yellow 3. Bromine-orange-red 4. Iodine-purple. 16. (Should be 17 but she had a typo): The flouring is considered the most reactive. In the video, it shows a reaction of fluorine with iron wool. Then with charcoal, and then final,y with hydrogen gas in a balloon. All of these reactions show fast reactions with a large release of energy. The slow motion view of the hydrogen and fluorine created what compound? The slow motion view of the hydrogen and fluorine created a fireball. 17. The same reaction with hydrogen and chlorine is that the hydrogen flame, when dipped into the chlorine gas, burns a pale blue color. Produces Hs, HCl, HBr, and HI. 18. The video finally shows a series of reactions with Aluminum and Halogens. The reaction starts with Aluminum and Fluorine gas. This reaction is over very quickly and just flash burns and quits burning very quickly. 19. As the next three halogens are put into contact with aluminum the reaction becomes: Aluminum-Chlorine: the aluminum just burns relatively slowly. Aluminum-Bromine: the aluminum starts to dissolve and then begins to burn immensely. Aluminum-Iodine: Iodine gas is produced and it sparks and burns much more than bromine did. As the next three halogens are out into contact with aluminum the reactions become progressively more intense.
@panjapop its just baisicly (anyone else feel free to correct me if i'm wrong...) two (di) atoms bonded together, in this video, he's reffering to two of the same element bonded to itself, e.g chlorine= Cl2. it exists that way in gaseous form (as two of its own atoms). Hope that helps (even though its 5 months late!) :-)
@howtodoit13 usually if you need flourine you have to make it by oxidizing the flouride ion, its can not be easy contained and is very dangerous so its not worth manufacturing industrially
I have a question: a candle burns without problems in a fluorine atmosphere, a candle burns without problems in a chlorine atmosphere, but can a candle burn without problems also in a gaseous bromine and iodine gas atmosphere? What would have happened if the operator had placed the nozzle with the hydrogen in the containers of bromine and iodine? Would he give off a colored flame like with chlorine?
i know im late but i can try to answer your question! a candle can burn in a chlorine atmosphere because chlorine gas doesn't interfere with the combustion. however, when it comes to bromine and iodine gas atmospheres, things might be different. bromine and iodine are both halogens like chlorine, but they have different properties. bromine is a liquid at room temperature, and iodine is a solid. if the operator were to place the nozzle with hydrogen in containers of bromine or iodine, it could potentially react with the halogens and form hydrogen halides, which are corrosive and can be dangerous. as for the colored flame, bromine and iodine gas can produce colored flames when they react with hydrogen, but the colors may be different from the bright green flame produced by chlorine.
@@bethany.b. What if bromine and iodine were in gaseous form? Could an atmosphere containing 100% I2 or Br2 in gaseous form cause hydrogen to burn? If there was a planet with an atmosphere made up of I2 in a high percentage, such as 90% or even 100% could there be fires if there was combustible material?
@flashkillerffff nope As Aluminium-Ions carry a positive charge of 3, they can only accept 3 bondings with free electrons. Each halogen ion carries one of those, so they form Aluminium-Tri-Halides... I hope my phrasing/nomenclature is correct as I usually only do chemistry in German
@howtodoit13 Not worth it, trust me. Fluorine is the Houdini of the elements - it's almost impossible to contain securely. You'd also need to work with it under a fume hood, since it reacts with water to form poisonous HF gas.
SplinterCell521 You can get small vials from Metallium inc. Heres a link- elementsales.com However, in order to purchase highly reactive elements you need to be qualified to handle them.
Your aluminium was impure. Also, when reacting aluminium with hydrochloric acid, and evaporating the solution, you don't get aluminium chloride, but its hydrate, and if you heat it to remove crystal water, you get aluminium oxychloride. If you want AlCl3, you need direct synthesis from the elements.
The root "di-" means "two" so a "diatomic molecule" is a molecule composed of two atoms. You would almost never find a single atom of Br for example; pure bromine is Br2 (the 2 is subscript).
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@howtodoit13 Chemical Register (google it) has flourine gas for sale and will ship in and to the US, though the conversion rate right now is brutal what with the dollar being so weak and all.
![Noob To Max With DRAGON REWORK In Blox Fruits [FULL MOVIE]](http://i.ytimg.com/vi/LnBMOinoOvA/mqdefault.jpg)
homework during lockdown any one
Yep
You guys are still in lockdown?
#immadohomework
@@yfeboanvakenss8841 yep
Once the reaction starts going, it looks like a pit of hell. Oh you science
In the words of Prof Farnsworth: Hail Science!
Now that's how you teach these things. Not some dude talking in some class while the students are yawning their knowledge out their brains to oblivion.
I don't know about you, but in my Chemistry class, the teacher did regularly show us such things. I even (vaguely) recall experiments with radioactive stuff he had to do outside. That was about 20 years ago.
9 years ago you posted that comment
@@Nathanyel Yeah, after I said so!
These chemistry videos make great teaching aids and give me ideas for variation experiments to demonstrate myself. One reaction that I was surprised wasn't shown was with the alkali metals - vigorous and beautiful reactions that produce common salts, in fact you probably know one of those - that being of course sodium chloride, AKA table salt, but there's also lithium chloride, potassium chloride, sodium iodide, etc.
I love this guy, the way he so dryly and nonchalantly saying all these things just tickles me.
homework anyone?
Yesh soo relatable
yup
Glad to see teachers 3 years ago used this for homework as well- XD
Yea
:)
Does anyone know what the original documentary is called?
Nice vid!! I've never seen fluorine before...it's such a great element!!
god damnn 10 years ago
@@ryaenson8285 HAAAII
11 years ago you posted that comment i was 3 or 4
@@ryaenson8285 +3 years
@@realityinfake3765 lol ive even passed my exam now
how about the part with the aluminum and the fluorine, how did they manage to get such pure fluorine into the container?
So that's how mixtapes are made...
Yes, now you're right: many transition metals show +2 and +3 oxidation states; Al is only +3 under normal conditions* - it's in the Boron group (a main group element).
* This is a disclaimer: I think Al can show either +1 or +2 (can't remember which, but only in molten salt solution, such as dissolving Al metal in molten AlCl3 - might be wrong on the details here, but this is an unusual situation, almost never happens.
Hey, I love this video!
The fires are started by fluorine but most of the burning is actually from oxygen in the air because the fluorine doesn’t have time to reach the entire substance.
I guess that explains why oxygen is the oxidizer that keeps us alive. Fluorine may react and thus spend its energy before even having a chance to reach our cells.
No gases are produced. Aluminium and bromine give aluminium bromide which appears as aerosol (tiny solid particles). It is mixed with excess bromine vapor so it looks yellow-orange, but it's actually transparent crystals when pure.
Aluminium bromide is very corrosive to tissues cause it reacts with water, increasing the acidity of the solution, but not inherently very toxic per se.
How do you store the fluorine in the glass without having it react?
Its a slow reaction.
How about fluorine and water? Or chlorine and water? I've never seen either of those reactions demonstrated. I wonder how vigorously each react with water.
where do you get fluorine?
@FortNikitaBullion But what about later when fluorine is added to aluminum?
+1 Al compounds have been reported (e.g. Al-F), but under extremely controlled conditions and in very low concentrations.
what show is this from?
IODINE is my favorite ELEMENT. 😊
does anyone know where to get these in the elemental form?
Alr if you’re here from Ms. Scott’s class imma just drop some helpful things
Vid #3: 16. 1. Fluorine-colorless 2. Chlorine-greenish-yellow 3. Bromine-orange-red 4. Iodine-purple. 16. (Should be 17 but she had a typo): The flouring is considered the most reactive. In the video, it shows a reaction of fluorine with iron wool. Then with charcoal, and then final,y with hydrogen gas in a balloon. All of these reactions show fast reactions with a large release of energy. The slow motion view of the hydrogen and fluorine created what compound? The slow motion view of the hydrogen and fluorine created a fireball. 17. The same reaction with hydrogen and chlorine is that the hydrogen flame, when dipped into the chlorine gas, burns a pale blue color. Produces Hs, HCl, HBr, and HI. 18. The video finally shows a series of reactions with Aluminum and Halogens. The reaction starts with Aluminum and Fluorine gas. This reaction is over very quickly and just flash burns and quits burning very quickly. 19. As the next three halogens are put into contact with aluminum the reaction becomes: Aluminum-Chlorine: the aluminum just burns relatively slowly. Aluminum-Bromine: the aluminum starts to dissolve and then begins to burn immensely. Aluminum-Iodine: Iodine gas is produced and it sparks and burns much more than bromine did. As the next three halogens are out into contact with aluminum the reactions become progressively more intense.
You’re welcome. Now go get some sleep.
Also 20. One and three. 21. Fluorine is the most reactive halogen.
Tuomo Kovanen ayy I gochu
@Timera Tenhage heyyy timera!
It said “pyrex” on the container containing the fluorine.
Very good demo for the halogens
Good work
All of them smell terrible, and their toxic, but I still love them
@panjapop its just baisicly (anyone else feel free to correct me if i'm wrong...) two (di) atoms bonded together, in this video, he's reffering to two of the same element bonded to itself, e.g chlorine= Cl2. it exists that way in gaseous form (as two of its own atoms). Hope that helps (even though its 5 months late!) :-)
@howtodoit13 usually if you need flourine you have to make it by oxidizing the flouride ion, its can not be easy contained and is very dangerous so its not worth manufacturing industrially
12 year ...
Very clear and concise!
I have a question: a candle burns without problems in a fluorine atmosphere, a candle burns without problems in a chlorine atmosphere, but can a candle burn without problems also in a gaseous bromine and iodine gas atmosphere? What would have happened if the operator had placed the nozzle with the hydrogen in the containers of bromine and iodine? Would he give off a colored flame like with chlorine?
i know im late but i can try to answer your question! a candle can burn in a chlorine atmosphere because chlorine gas doesn't interfere with the combustion. however, when it comes to bromine and iodine gas atmospheres, things might be different. bromine and iodine are both halogens like chlorine, but they have different properties. bromine is a liquid at room temperature, and iodine is a solid. if the operator were to place the nozzle with hydrogen in containers of bromine or iodine, it could potentially react with the halogens and form hydrogen halides, which are corrosive and can be dangerous. as for the colored flame, bromine and iodine gas can produce colored flames when they react with hydrogen, but the colors may be different from the bright green flame produced by chlorine.
@@bethany.b. What if bromine and iodine were in gaseous form? Could an atmosphere containing 100% I2 or Br2 in gaseous form cause hydrogen to burn? If there was a planet with an atmosphere made up of I2 in a high percentage, such as 90% or even 100% could there be fires if there was combustible material?
@flashkillerffff nope As Aluminium-Ions carry a positive charge of 3, they can only accept 3 bondings with free electrons. Each halogen ion carries one of those, so they form Aluminium-Tri-Halides...
I hope my phrasing/nomenclature is correct as I usually only do chemistry in German
You've done great👏👏👏
hello from west bridgford
same :)
Isnt hydrgoen flouride dangerous?
you need pure chlorine (Cl2) and pure aluminum (Al)
3 Cl2 (g) + 2 Al (s) -> 2 AlCl3 (s)
2:42💫
could someone give me a brief definition of a diatomic molecule? :)
no
A diatomic molecule is an atom coupled to another atom of the same element. For Example, F+F= F2
@howtodoit13 Not worth it, trust me. Fluorine is the Houdini of the elements - it's almost impossible to contain securely. You'd also need to work with it under a fume hood, since it reacts with water to form poisonous HF gas.
one question,does the reaction between aluminum and bromine produce poisonous gas???
Yes they all are poisons
The One To The Left Is Actually Empty Florine Would React With The Glass
Fluorine reacts slowly with glass. Its not instantaneous.
At 3:07, you meant AlF3.
Good video, though.
SplinterCell521 You can get small vials from Metallium inc.
Heres a link- elementsales.com
However, in order to purchase highly reactive elements you need to be qualified to handle them.
*I dropped a piece of aluminum foil in my coffee and it started a fire*
I officially learned Halogens :)
Cool! 😄
Lok Lam Chan Finally someone that thinks it's real! YEAH!
I just like watching halogens year the absolute souls out of other elements
Their famous substitution reaction with alkanes would've been awesome.
whos here from my school?
Me
I'm not Alex at all I'm ur classmate
Awesome video! Thanks!
Thank you so much
Hydrogen is not a happy gas
Your aluminium was impure.
Also, when reacting aluminium with hydrochloric acid, and evaporating the solution, you don't get aluminium chloride, but its hydrate, and if you heat it to remove crystal water, you get aluminium oxychloride.
If you want AlCl3, you need direct synthesis from the elements.
@CrazyforDarkness Glass is inert, nonreactive. Most things are stored in glass
could someone give me a brief definition of diatomic molecule is... :)
The root "di-" means "two" so a "diatomic molecule" is a molecule composed of two atoms. You would almost never find a single atom of Br for example; pure bromine is Br2 (the 2 is subscript).
i have a pound of I2 and i've made Cl2 and Br2 before. i have the safety equipment, i just don't like going to all the trouble. thats all.
Nitrgen triiodide, great fun!
@endimion17 why can't they pronounce it correctly!!!
I you have questions click o the three dots then open transcript :))
That's very good
hello how are you
Once the reaction starts going, it looks like a pit of hell... That's my whole science essay done.
How much iodine and aluminium did that guy use (roughly)? I'm not going to do it, I just would like to know.
Error when talking about aluminum fluoride he says Al3 but should be AlF3
It's just the captions
I’m guessing Pyrex is resistant to fluorine.
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where do they get flourine !! : o
So cool!
Student Mdm Tarina hadir 🙋🏻♂️
Not just that, it is rare.
1:05
2:00
Cool! Very interesting.
@FortNikitaBullion You Don't The Glass Is Empty
@howtodoit13
Chemical Register (google it) has flourine gas for sale and will ship in and to the US, though the conversion rate right now is brutal what with the dollar being so weak and all.
aluminium+Iodine looks EPIC :D
i was 2 or 3 when you said this
Same !
Thanks for reminding me of this video!
aluminum + bromine = hell in a bowl
I love how this guy says aluminum
very helpful imo, ty
Ive got a sub
Magnesium reacts with halogens easier than alluminium,
I reacted HCl with metallic aluminum.. But I got a black powder..
Impurities maybe
You forgot astatine
I swear this video looks like it’s 50 years old
3:07 it should be AlF3 think
you mean 3:07?
and no i dont think so
Thumbs up again if cele sent you here
Awesome
the halogens rockz!
anyone from 7a3 here
No, you're mistaken: what he says on the video is correct.
BOOM!
Iodene + aluminium=Thundering bowl :D
Those things are often performed in school. Definetly here in germany too ;)
If not: Just ask your teacher.
Astatine is a halogen but extremely rare
Agreed! epic.
13 year...
I came here for the aesthetics
jk it's for online class
12 yrs Old😊
@wow1022 For special Americans, aluminum. For the rest of the world, aluminium.
We don't have these lab
I wish we would do cool thing like that in school =/
i concur