2FeCl3 + FeCl2 + 8NH3 + 4H2O = Fe3O4 + 8NH4Cl Can I use any iron 2 and 3 salts?
Also I tried boiling iron hydroxide in water for 2 hours afterwards I filtered the powder and it seems to oxidised a little(it still works) what caused this? Was it left over iron hydroxide?
I'm making FeCl3 for etching metal by Fe (m) + HCl (aq) -> FeCl2 (aq) + O2 (g) -> FeCl3
Which is working, but how do I know when I'm done? The resulting solution is a very dark yellow and by color alone it's difficult to gauge the amount of iron II remaining. I can precipitate it out with a base but then I'm looking at a murky yellow-brown precipitate instead of a murky yellow-brown liquid.
I've found several analyses which depend on toxic or difficult-to-get reagents and are not suitable for the garage. Is there a simpler way to know when the reaction is done?
I am trying to make a terrain mesh that is similar to the games listed above, one that uses a heightmap, that way I can hopefully have the materials auto applied depending on the height. The only problem is that I can't find a way to make the heightmap's colors represent the height of a vertex on the mesh. If anyone knows how to do this, it would be very appriciated if you could tell me
Oh chemistry gods, lend me your wisdom. I'm a grad student working on a nanoparticle-based system and one synthesis method I'm looking at involves a combination of ferrous chloride and ferric chloride (iron(ii) and iron(iii)). We have over 1 kg of each of those in stock already, but they're each in hydrate form. Off the top of my head, I believe it's iron(ii) chloride hexahydrate and iron(iii) chloride nonahydrate. However, I'm convinced this residual water is causing some issues as the nanoparticles aren't taking the shapes I'd expect. Long story short, I'd like to dehydrate the salts instead of buying anhydrous ones, especially because shipping has been EXTREMELY unpredictable recently.
Ideas:
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Just grind them up, stick them in a vacuum furnace overnight/ over the weekend at approx 50C. I feel like this will do a little, but not a whole lot.
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I need this dissolved in ethanol anyways. So maybe I could dissolve in ethanol and then add either sodium sulfate or molecular sieves to suck up the water and voila. However, I can't find anything reliable on just how much sieves can absorb ions so I'm afraid of this method.
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Suck it up and buy anhydrous salts, wait a few weeks for them to come in.
Please advise.
A molecular diuranium(III) oxide was prepared. It undergoes cleavage of one U−O bonding and effects the reductive coupling of pyridine and the two‐electron reduction of bipyridine by delivering a “UII” synthon. These reactions provide a synthetic route to dinuclear UIII/UIII complexes bridged by redox‐active N‐heterocyclic ligands.
Abstract
Oxide is an attractive linker for building polymetallic complexes that provide molecular models for metal oxide activity, but studies of these systems are limited to metals in high oxidation states. Herein, we synthesized and characterized the molecular and electronic structure of diuranium bridged UIII/UIV and UIII/UIII complexes. Reactivity studies of these complexes revealed that the U−O bond is easily broken upon addition of N‐heterocycles resulting in the delivery of a formal equivalent of UIII and UII, respectively, along with the uranium(IV) terminal‐oxo coproduct. In particular, the UIII/UIII oxide complex effects the reductive coupling of pyridine and two‐electron reduction of 4,4′‐bipyridine affording unique examples of diuranium(III) complexes bridged by N‐heterocyclic redox‐active ligands. These results provide insight into the chemistry of low oxidation state metal oxides and demonstrate the use of oxo‐bridged UIII/UIII complexes as a strategy to explore UII reactivity.
https://ift.tt/2HkViN3
Poison IV, though, just made the victim extremely itchy.
I was told SnO2 is named Tin(IV) Oxide because of the charge on oxygen, which will have a total of 4+ charge, which is why it has (IV). But when I was naming Cr2O3 on homework the answer was chromium(III) oxide! Shouldn't it be (VI) because oxygen has +2 charge and that would be 6? Thanks
In my country soapmaking is not very popular and it can therefore be difficult to get supplies that are specifically made for soapmaking.
I found some Black oxide (iron) that is sold as cement color and was wondering if it can be used in soap or if there are different kinds of iron oxide.
I'm doing a Planning and Designing lab for A-level Chem, and the problem statement asks how the oxides of Vanadium can be prepared from Vanadium (V) oxide. Wikipedia says that the oxides can be prepared via successive thermal decomposition, but I can't find any temperature values online to support the claim. I've checked the CRC Handbook, (84th edition) and they don't have the decomposition temperatures for any of the vanadium oxides other than V2O5 on pg 789 on the pdf, which makes me wonder where the wiki gets the info from.
Oxide is an attractive linker for building polymetallic complexes that provide molecular models for metal oxides activity, but studies of these systems are limited to metals in high oxidation states. Herein, we synthesized and characterized the molecular and electronic structure of diuranium bridged U(III)/U(IV) and U(III)/U(III) complexes. Reactivity studies of these complexes revealed that the U‐O bond is easily broken upon addition of N‐heterocycles resulting in the delivery of a formal equivalent of U(III) and U(II), respectively, along with the uranium(IV) terminal‐oxo coproduct. In particular, the U(III)/U(III) oxide complex effects the reductive coupling of pyridine and two‐electron reduction of 4,4'‐bipyridine affording unique examples of diuranium(III) complexes bridged by N‐heterocyclic redox‐active ligands. These results provide insight into the chemistry of low oxidation state metal oxides and demonstrate the use of oxo‐bridged U(III)/U(III) complexes as a strategy to explore U(II) reactivity.
https://ift.tt/2HkViN3
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