Pretty cool man! I had no idea iron could be oxidized to +6! While your on the topic of coloured ions, It's be really interesting if you can extract and maybe precipitate out triiodide ion (from a starch-iodine complex) as a salt!
A better compound to crystallise is the tetramethylammonium triiodide. It gives beautiful crystals, but the pentaiodide can be formed from similar conditions and gives similarly beautiful crystals.
Nice work, rarely shown compound. Ferrate can also be made by electrolysis of an alkali hydroxide solution with an iron anode or by heating a mixture of iron powder and alkali nitrate until it ignites (needs to be carried out in a fireproof surrounding outside). If you want to proof that iron in a higher oxidation state has formed you can use the solid substance to decompose hydrogen peroxide to oxygen or conc. hydrochloric acid to chlorine.
Thank you! (and thanks for the info) Do you mean that ferrate can be made by alkaline electrolysis in a single-cell, or would it need to be a membrane-separated cell? I just Imagine the ferrate would be reduced at the cathode, but maybe that could be avoided by placing the cathode much higher in the cell? Definitely intend to give it a shot
@Apoptosis You´ve got the reaction equation wrong at 1:45. The correct reaction for the oxidation of iron(II) chloride to iron(III) chloride is: 6 FeCl2 + 3 H2O2 = 2 Fe(OH)3 + 4 FeCl3 If there´s excess hydrochloric acid present in the ferrous chloride solution then the reaction is: 2 FeCl2 + 2 HCl + H2O2 = 2 FeCl3 + 2 H2O
@@integral_chemistry LOL yeah. I've even endeavored to make my own ion exchange membranes for that, because Nafion is too expensive. It worked fairly well, but I won't post about it because it involved a substance on the watched list. :)
If it's such an aggressively powerful oxidizer, could you make a better solid rocket fuel or gunpowder by adding either some, or all, of a ferrate compound rather than the more common oxidizers?
probably not unfortunately. Pigments need to be chemically inert and this is a super strong oxidizer so it would likely react with and destroy any canvas or paper..
I suppose the barium ferrate partially explains why you had Ba(OAc)2 on hand for the NH4NO3 video, but I'm curious what other uses you have for such a nasty customer. Is it just because barium salts tend towards insolubility, or was there something specific you have/had in mind?
Honestly I just got it at a very good price a little over a year ago and figured I'd eventually find a use for it. I can't really think of too much else except maybe to precipitate hypomanganate so I might just precipitate the rest as the sulfate salt and start the disposal process bc I don't love having it around lol
I always learned in school that Iron (III) hydroxide doesn't really exist and it is actually an oxide-hydroxide where that oxygen coordinates to water. Its to show the structural difference but at the end of the day it could be just as easily shown as Fe(OH)3
Another way to look at it would be : H2O2 +2e = 2HO- So while the hydrogen peroxide oxidize a compound, the solution would turn more alkaline until you reach the pH of precipitation
(Btw let’s add that : Fe2+ = Fe3+ +e, so the oxidation of iron doesn’t produce H+ to counter it) (so basically you get to the equation mentioned above lmao)
Iron is NOT! hexavalent! It does not have the same degree of covalency! There are just 2 true hexavalent transition metals, chromium, and molybdenum! No other!
I'll have to do some research to find out exactly what you mean but I feel that if the quality you are referring to is shared by molybdenum than it is likely shared by tungsten and rhenium as well. Obviously group 6 metals are going to form the most stable hexavalent states because they have 6 valence electrons, but there are many other elements that can assume hexavalent states.. at least from what I was taught.
Tungsten has a strong preference for +6 as well, as found in e.g. WO3. Rhenium can be made hexavalent although it tends to prefer +7 in oxidizing environments. Hexavalent iron is real and is correctly shown in this video, although it is so strong that it oxidizes water to oxygen and gets reduced back to Fe(III) unless it is in a very strongly alkaline solution. Manganese can also form Mn(VI) aka manganate, and permanganate is reduced to manganate in strongly alkaline solutions. Finally, all of the platinum-group metals except palladium have hexafluorides that can form after reaction with F2, ClF3, or OF2, as do tungsten, rhenium, molybdenum, and technetium.
The transition metals have such amazing colors
Hexavalent Iron Man surrounds himself with six Avengers.
Three of them bugger off at the slightest provocation though.
@@grebulocities8225 Tony: Thor? Captain America? Hulk? Uh, oh...
I didn't know about hexavalent iron, might try this with my class. Excellent video, thanks.
Would love to see some reactions showing its oxidative properties
Pretty cool man! I had no idea iron could be oxidized to +6! While your on the topic of coloured ions, It's be really interesting if you can extract and maybe precipitate out triiodide ion (from a starch-iodine complex) as a salt!
You're*
You're a obviously a smart individual and know far more about chemistry than I do, so you're above simple grammar mistakes. C'mon.
A better compound to crystallise is the tetramethylammonium triiodide. It gives beautiful crystals, but the pentaiodide can be formed from similar conditions and gives similarly beautiful crystals.
Like Himalayan pink salt?
@@Hirotechnics😂 seriously??? you've grammar pedantry syndrome.
@Hirotechnics
_”You're _*_a_*_ obviously a”_
Funny that you’re being a grammar pedant.
Damn, this video was pretty cool, love the colors!
So cool, and so colorful 😁👍👍👍👍
Nice work, rarely shown compound.
Ferrate can also be made by electrolysis of an alkali hydroxide solution with an iron anode or by heating a mixture of iron powder and alkali nitrate until it ignites (needs to be carried out in a fireproof surrounding outside).
If you want to proof that iron in a higher oxidation state has formed you can use the solid substance to decompose hydrogen peroxide to oxygen or conc. hydrochloric acid to chlorine.
Thank you! (and thanks for the info) Do you mean that ferrate can be made by alkaline electrolysis in a single-cell, or would it need to be a membrane-separated cell? I just Imagine the ferrate would be reduced at the cathode, but maybe that could be avoided by placing the cathode much higher in the cell? Definitely intend to give it a shot
1:28 I would describe that more as 'Peridot', which makes sense since peridot is colored green by iron 2+!
@Apoptosis You´ve got the reaction equation wrong at 1:45. The correct reaction for the oxidation of iron(II) chloride to iron(III) chloride is:
6 FeCl2 + 3 H2O2 = 2 Fe(OH)3 + 4 FeCl3
If there´s excess hydrochloric acid present in the ferrous chloride solution then the reaction is:
2 FeCl2 + 2 HCl + H2O2 = 2 FeCl3 + 2 H2O
I think this reaction is actually 2FeCl2 + H2O2 -> 2FeOH(Cl)2 if there is not enough hydrochloric acid.
The color of the FeVI is giving me flashbacks to freshman chemistry and various cobalt-amino complexes
That barium compound is a nice colour.
4:50 the iron complex is [FeSCN]2+
Nice video!
Thanks for the demonstration.
Nice. I've been attempting to make ferrate by electrolysis but it's difficult. I'll try the hypochlorite oxidation too. :)
same! Electrolysis gets very difficult under extremely oxidizing conditions like this I've found.
@@integral_chemistry LOL yeah. I've even endeavored to make my own ion exchange membranes for that, because Nafion is too expensive. It worked fairly well, but I won't post about it because it involved a substance on the watched list. :)
If it's such an aggressively powerful oxidizer, could you make a better solid rocket fuel or gunpowder by adding either some, or all, of a ferrate compound rather than the more common oxidizers?
That's some high grade rust yo, the good stuff.
insane!
So ferrate +VI kinda acts like sulfate when it comes to its reactions with earth alkali metals?
I would like to see Chromium-2 (Cr-II) compounds!
How long do you boil to form ferrate?
Amazing! Can it be used as a pigment?
probably not unfortunately. Pigments need to be chemically inert and this is a super strong oxidizer so it would likely react with and destroy any canvas or paper..
I suppose the barium ferrate partially explains why you had Ba(OAc)2 on hand for the NH4NO3 video, but I'm curious what other uses you have for such a nasty customer. Is it just because barium salts tend towards insolubility, or was there something specific you have/had in mind?
Honestly I just got it at a very good price a little over a year ago and figured I'd eventually find a use for it. I can't really think of too much else except maybe to precipitate hypomanganate so I might just precipitate the rest as the sulfate salt and start the disposal process bc I don't love having it around lol
Bro.. 2:06 why do you show here some FeO(OH)?
I always learned in school that Iron (III) hydroxide doesn't really exist and it is actually an oxide-hydroxide where that oxygen coordinates to water. Its to show the structural difference but at the end of the day it could be just as easily shown as Fe(OH)3
does +6 iron taste better than +2 iron?
not sure.. I wouldn't try either lmao
Music is too quiet, I can hear someone is talking something
Very cool! You are the first one that managed to cristallize ferrate !
Making the barium salt is no rocket science: it's almost insoluble in water, quite stable and therefore easily isolatable.
Tf why is fe(oh)3 present when you react fecl2 with h2o2
I think:
3H2O2 + 6FeCl2 → 2Fe(OH)3 + 4FeCl3
Exactly, if you want pure FeCl3 you can oxidize FeCl2 with chlorine
Edit: or add some HCl along with H2O2
My mistake
Another way to look at it would be : H2O2 +2e = 2HO-
So while the hydrogen peroxide oxidize a compound, the solution would turn more alkaline until you reach the pH of precipitation
(Btw let’s add that : Fe2+ = Fe3+ +e, so the oxidation of iron doesn’t produce H+ to counter it) (so basically you get to the equation mentioned above lmao)
Next up Hexavalent Chromium 😂
Iron is NOT! hexavalent! It does not have the same degree of covalency! There are just 2 true hexavalent transition metals, chromium, and molybdenum! No other!
Uranium is commonly hexavalent!. Ferrates needs extreme conditions to form and is unstable.
I'll have to do some research to find out exactly what you mean but I feel that if the quality you are referring to is shared by molybdenum than it is likely shared by tungsten and rhenium as well. Obviously group 6 metals are going to form the most stable hexavalent states because they have 6 valence electrons, but there are many other elements that can assume hexavalent states.. at least from what I was taught.
Tungsten has a strong preference for +6 as well, as found in e.g. WO3. Rhenium can be made hexavalent although it tends to prefer +7 in oxidizing environments. Hexavalent iron is real and is correctly shown in this video, although it is so strong that it oxidizes water to oxygen and gets reduced back to Fe(III) unless it is in a very strongly alkaline solution. Manganese can also form Mn(VI) aka manganate, and permanganate is reduced to manganate in strongly alkaline solutions. Finally, all of the platinum-group metals except palladium have hexafluorides that can form after reaction with F2, ClF3, or OF2, as do tungsten, rhenium, molybdenum, and technetium.