Hexavalent Iron

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  • Опубліковано 22 гру 2024

КОМЕНТАРІ • 55

  • @IIHawkGamingII
    @IIHawkGamingII Рік тому +11

    The transition metals have such amazing colors

  • @aqdrobert
    @aqdrobert Рік тому +7

    Hexavalent Iron Man surrounds himself with six Avengers.

    • @grebulocities8225
      @grebulocities8225 Рік тому +2

      Three of them bugger off at the slightest provocation though.

    • @aqdrobert
      @aqdrobert Рік тому +1

      @@grebulocities8225 Tony: Thor? Captain America? Hulk? Uh, oh...

  • @andrewhaychemistry
    @andrewhaychemistry Рік тому +5

    I didn't know about hexavalent iron, might try this with my class. Excellent video, thanks.

  • @larry_k
    @larry_k Рік тому +7

    Would love to see some reactions showing its oxidative properties

  • @R-Tex.
    @R-Tex. Рік тому +18

    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!

    • @Hirotechnics
      @Hirotechnics Рік тому

      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.

    • @evildoctorcow
      @evildoctorcow Рік тому +2

      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.

    • @realryder2626
      @realryder2626 Рік тому

      Like Himalayan pink salt?

    • @R-Tex.
      @R-Tex. Рік тому

      @@Hirotechnics😂 seriously??? you've grammar pedantry syndrome.

    • @derschwarzgeist
      @derschwarzgeist 6 місяців тому +1

      @Hirotechnics
      _”You're _*_a_*_ obviously a”_
      Funny that you’re being a grammar pedant.

  • @XemplarSoft
    @XemplarSoft Рік тому +1

    Damn, this video was pretty cool, love the colors!

  • @Alexelectricalengineering
    @Alexelectricalengineering Рік тому +1

    So cool, and so colorful 😁👍👍👍👍

  • @experimental_chemistry
    @experimental_chemistry Рік тому +4

    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.

    • @integral_chemistry
      @integral_chemistry  Місяць тому

      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

  • @chir0pter
    @chir0pter Рік тому

    1:28 I would describe that more as 'Peridot', which makes sense since peridot is colored green by iron 2+!

  • @chemicalmaster3267
    @chemicalmaster3267 11 місяців тому

    @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

    • @MineK_FG
      @MineK_FG 8 місяців тому

      I think this reaction is actually 2FeCl2 + H2O2 -> 2FeOH(Cl)2 if there is not enough hydrochloric acid.

  • @PaulSteMarie
    @PaulSteMarie Рік тому +2

    The color of the FeVI is giving me flashbacks to freshman chemistry and various cobalt-amino complexes

  • @jimsvideos7201
    @jimsvideos7201 Рік тому +1

    That barium compound is a nice colour.

  • @lautaromorales2903
    @lautaromorales2903 Рік тому +1

    4:50 the iron complex is [FeSCN]2+

  • @Dyingtolive2025
    @Dyingtolive2025 Рік тому +1

    Nice video!

  • @fredericomba
    @fredericomba Рік тому

    Thanks for the demonstration.

  • @stamasd8500
    @stamasd8500 Рік тому +4

    Nice. I've been attempting to make ferrate by electrolysis but it's difficult. I'll try the hypochlorite oxidation too. :)

    • @integral_chemistry
      @integral_chemistry  Рік тому +1

      same! Electrolysis gets very difficult under extremely oxidizing conditions like this I've found.

    • @stamasd8500
      @stamasd8500 Рік тому

      @@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. :)

  • @Ithirahad
    @Ithirahad Рік тому

    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?

  • @mooseitself
    @mooseitself Рік тому +1

    That's some high grade rust yo, the good stuff.

  • @tahallium
    @tahallium Рік тому

    insane!

  • @Psychx_
    @Psychx_ Рік тому +1

    So ferrate +VI kinda acts like sulfate when it comes to its reactions with earth alkali metals?

  • @PS-vk6bn
    @PS-vk6bn Рік тому

    I would like to see Chromium-2 (Cr-II) compounds!

  • @NguyênKhoaCôngTy
    @NguyênKhoaCôngTy 22 години тому

    How long do you boil to form ferrate?

  • @juanaguiar4852
    @juanaguiar4852 Рік тому +1

    Amazing! Can it be used as a pigment?

    • @integral_chemistry
      @integral_chemistry  Рік тому +1

      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..

  • @dissolvedpeafowl
    @dissolvedpeafowl Рік тому +1

    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?

    • @integral_chemistry
      @integral_chemistry  Рік тому +1

      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

  • @LuckyCrab_
    @LuckyCrab_ Рік тому +1

    Bro.. 2:06 why do you show here some FeO(OH)?

    • @integral_chemistry
      @integral_chemistry  Рік тому

      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

  • @planellas6
    @planellas6 Рік тому +3

    does +6 iron taste better than +2 iron?

  • @qwerty-wt5dr
    @qwerty-wt5dr Рік тому +1

    Music is too quiet, I can hear someone is talking something

  • @Alberto_Travagin
    @Alberto_Travagin Рік тому

    Very cool! You are the first one that managed to cristallize ferrate !

    • @experimental_chemistry
      @experimental_chemistry Рік тому

      Making the barium salt is no rocket science: it's almost insoluble in water, quite stable and therefore easily isolatable.

  • @vx_nerve_agent
    @vx_nerve_agent Рік тому +1

    Tf why is fe(oh)3 present when you react fecl2 with h2o2

    • @R-Tex.
      @R-Tex. Рік тому +1

      I think:
      3H2O2 + 6FeCl2 → 2Fe(OH)3 + 4FeCl3

    • @zenongranatnik8370
      @zenongranatnik8370 Рік тому +1

      Exactly, if you want pure FeCl3 you can oxidize FeCl2 with chlorine
      Edit: or add some HCl along with H2O2

    • @vx_nerve_agent
      @vx_nerve_agent Рік тому +1

      My mistake

    • @Tom-to7dy
      @Tom-to7dy Рік тому

      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

    • @Tom-to7dy
      @Tom-to7dy Рік тому

      (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)

  • @gideonevans9717
    @gideonevans9717 8 місяців тому

    Next up Hexavalent Chromium 😂

  • @MichaelLapore-lk9jz
    @MichaelLapore-lk9jz Рік тому +1

    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!

    • @karlbergen6826
      @karlbergen6826 Рік тому +1

      Uranium is commonly hexavalent!. Ferrates needs extreme conditions to form and is unstable.

    • @integral_chemistry
      @integral_chemistry  Рік тому +1

      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.

    • @grebulocities8225
      @grebulocities8225 Рік тому

      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.