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Iron oxide is perhaps one of my favorite Oxymorons of Chemistry that ever was. When you're younger, all these fancy chemicals sound exotic and hard to get. Then you get older and figure out (like this one) is basically Hot Rust.
Here in Arizona we have an incredible amount of magnetite in the soil. After it rains it settles out into a black deposit on the sand and can be gathered by the bucketful. A little washing with water and or separated with magnets purifies it
Some of my favourite memories from when I was little involved going to this beach we used to often go to and pulling the magnetite out of the sand with these big magnets we got from taking apart old speakers. Fun times.
Ah magnetite I think that's what my friend has. Does it attract lightning to the areA? Where my friend lives gets the most lightning strikes and its some metal in the soil.
Your video is very good. It provides us chemistry lovers with the opportunity to carry out chemical experiments without a professional experimental environment. Thank you very much. I hope to keep it updated.
Always great to find a new chemistry channel! Heads up from my blunders doing a similar thing - that rod doesnt look to be stainless steel, probably zinc plated, but from the nut you can end up with a bunch of toxic chromium ions which add a certain toxicity to thermite or other reactions. Videos I'd like to see: - Creating the different oxidation states of rust - Seeing how each of these oxidation states effect thermite ratios - Seeing if granulisation size (like black powder) effects thermite efficacy - Testing for presence of impurities (diy bodge electrophoresis is fun, plating a series of metals is also telling) Lastly in reference to your noble lithium attempts (the frustration only adds to the videos, every chemist has been there), the perfect collector is neither nickel nor iron - its a strip of pure lithium itself. Greatly increases purity (especially when you melt it together) - dont put it under mineral oil (till its melted into one piece) far better to keep it under a CO2 atmosphere from a beaker with a watch glass with a graphite rod connected to 0.5A (just under glowing). The speed and 'faraday per g' of your processes will greatly improve if you consider 'cross sectional area of anode / cathode + proximity. Having a copper wire that wraps several times round the inside of the beaker kept as close as possible to say the iron by using gauze to stop short circuit - 10x faster, way less losses From splitting water.
If the pH of the solution is high enough, iron can be oxidized to create ferrate(VI), which possesses a higher oxidation potential than permanganate. This process can be accomplished easily by mixing iron(III) hydroxide with hypochlorite bleach. Would you try this?
The product is quite fine and slightly attracted to a magnet and does not attract iron particles at all. Being so fine it would be highly reactive with water and everything else, so it would be hard to control any reaction that is half-way between the states.
that was cool but also a bit scary! i think of myself as agoodnatured if somewhat inquizative. i started of finding out that calcium was a metal,atfirst i couldnt believe it but when the dictionary even says it is well i must be more of an imbicile than i thought i was cos our bones are prettymuch calcium arent they? we've got iron in our blood and even bloods not just blood,youve got hemoglobin,mioglobin and then is blood another seperate thing,its twistin my mellon man,probly showin my age abit there,that was a whole century ago when we used too go too these things called acid house partys! mind i found the acid abit scary but when the ecstacy and the club dj scene kicked of and life was well selfexplanetry realy. anyway dont know why got sidetracked,anyway it just amazes me all the metals in our bodies like calcium,iron zinc am prettyshure we got some gold in us aswell,not enough too go cashin it in down the pawnshop! we are basicaly walking terminators. anyway the whole point of this was too tell you too watch what shit you tell people how too do on the internet cos we do not want anyone blowin shit up,you get me!!! these youngsters nowadays you dont know whos got a machette or a gun! having a child nowadays is allmost childcruelty,just cos the life their gonna have too live through just isnt fair!!!
The amount of energy used in these electrolysis projects pales in comparison to other household uses. An electric heater, a fridge, and stovetop all use orders of magnitude more power than this kind of reaction. At an absolute maximum, I might spend 15 cents (AUD) a week on electrolysis (more realistically, 2 or 3 cents a week would be a pretty good guess), and that's only on the weeks where I'm actually doing an experiment. (The exception to this is the time I tried to make heavy water by electrolysis, which took 2 years and over $100 of electricity - and ultimately failed, haha)
It was great to see this done in glass, I done the same method but used a 20 litre plastic tub so couldn't see anything.. I got a few kg of iron oxide ready so just need to get around to finishing my ball mill to powder up the pile of aluminium turnings I've been saving
One interesting thing about doing this is that if you dry the powder it will become brown reddish and very slightly magnetic. Upon further heating it becomes a very red fine powder and becomes strongly magnetic. I suspect although never gone towards proving it that it is in the form of maghemite.
Oh wow I was just wondering why it went darker red and hypothesised to myself that maybe it aligns the ions to make it look more red... I didnt say it out loud cos I thought it sounded dumb. But what you've said makes me think maybe I was right. I know whe. You temper steel with heat it helps align the iron somehow. God so much to learn. I'm just trying to dye a t shirt and now I'm down this rabbit hole! 😂
I cheated and went to the hardware store to get gardening and cleaning supplies then reacted a ferrous sulfate solution with sodium hydroxide. But what I would like to be able to do is work out how to easily plate iron onto things such as graphite painted 3D prints.
Hmmm. I've genuinely never seen anyone perform effective electroplating with iron in a home setting. That's not to say it can't be done of course. I really don't know much about electroplating in general, but maybe this deserves some thought...
@@ScrapScience See Scientific American - Electro-Plating with Iron November 27, 1869. However I am not sure of the "art" that is also required to get it to really work well rather than just create a crust the is not smooth and solid.
When you do the same electrolysis in a bigger transparent container with a clear solution the iron hydroxide will form in an interesting way almost like stalactites in a dripping cave. Would be worth a time-lapse. At least that's what it did in my case.
Hello great teacher we want to prepare the lead oxide duo through the Hello great teacher we want to prepare the lead oxide duo through the house scrap ❤️❤️
That's great. Black Iron oxide is mixed with silicone sealer to make the black tambourine part of a drum head. The black full circle in the centre that provides and controls the pitch of the tones of the drum. This is a vital part of a drum. Thank you for your informative video.
Earned a subscription! Thank you. I'm looking to generate a bunch of this for red oxide needed in earthen construction. Would you have any recommendations if you wanted to make a lot of this? They use this in Rammed Earth and I want to have enough so I can adjust concentration when mixing to form different shades in my layers/courses. Thanks again!
I have a question. When rinsing the rust to purify it, how do you process? I'm only thinking of immerging with water and filtering again and again but this seems a little bit time consuming. Is there any other quicker way?
It's possible, but no, I didn't observe any significant chlorine generation (by that, I mean I couldn't ever smell any). It's generally much more difficult to oxidise chloride ions than to oxidise iron. With that said, there are probably small amounts being generated, especially at the start of the electrolysis run (I think you might be able to see a few bubbles forming on the anode at the start there - these are almost definitely chlorine).
I'm not certain, but I'm pretty sure it will happen at mild temperatures (a little over 100 C or so) if you wait long enough and make sure the material is finely divided. Heating it up further only speeds up the process. The hotter it is, the faster the reaction.
harry this is a barely related question but i reckon your the fella to ask. if i wanted to convert the lead sulfates removed from a dead acid battery back into lead oxides could i just mix the paste into a weak sulfuric acid as an electrolyte and run current through the cell via lead anode and cathode?
It might work to some degree, but lead sulfate is going to be extremely poorly soluble in weak sulfuric acid. For electrolytic oxidation to work, you need the lead sulfate to be either in solution or in mechanically perfect contact with the anode. There might be better ways to go about doing this. Are you trying to obtain lead(II) oxide or lead(IV) oxide?
@@ScrapScience honestly im not sure, which is reducable into lead eith application of fire and carbon ( i have plenty of both im a blacksmith shop and have plenty of coke and charcoal and VERY hot furnaces and kilns at my disposal) or conversion straight to lead nitrate via nitric acid.
Hang on, is your absolute end goal here to obtain lead metal, or are you doing this to make some other lead compound? Making lead(II) oxide is definitely the way to go if you want to reduce it to lead metal with carbon (though that kind of sounds like a good way to poison yourself with lead vapours). The sulfate is soluble (to some degree) in sulfuric acid or nitric acid. The oxide is soluble in most mineral acids. - If that's useful info at all.
I'm pretty sure I heated to about 700 C, and I just kept going until the material stopped giving off steam (Something like 20 min). The exact temperature and time is not important for the reaction, provided the dehydration is completed. Lower temperatures will also work, just slower.
@@ScrapScience Yes, but I am concerned with the color of the Iron Oxide. From what I know at higher temperature, the oxide gives a bright Red color. Is that true?
I'm pretty sure the colour has much more to do with the overall oxidation state of the iron in the material, as opposed to the temperature of the dehydration. If you allow the heated oxide mixture to have good exposure to air (or oxygen), it will form a much redder colour due to reduced Fe(II) presence. Heating without good oxygen exposure still gives you mostly Fe(III), but the traces of Fe(II) won't be removed, giving you a duller colour.
Breaking down some of the Fe(III) into Fe(II), when in the form of oxides, requires temperatures of nearly 2000 C before the reaction becomes spontaneous (by my calculations anyway). Anything below this will end up favouring the conversion of Fe(II) to Fe(III) instead.
Iron hydroxide is often blue when it contains a bit of iron in the +2 oxidation state. We probably just have a fair bit of Fe(II) in our hydroxide precipitate. In general, iron hydroxide can take on many colours (white, green, grey, blue, orange...) depending on the mixture of iron oxidation states and excess oxygen in the structure. By the time we've filtered everything and heated it, almost everything should have converted to Fe(III) however, so this isn't an issue.
@@ScrapScience Thanks for that clarification. Although I have learned and done quite a lot of chemistry, I did not know that iron could give blue color. Where can I read about this?
@@BigParadox There's a relatively good paper on the topic here: pubs.acs.org/doi/pdf/10.1021/j150487a005 (It's from the 50's but the information seems pretty okay to me)
