Inorganic Chemistry

I read an article back in 9th grade that glass was an uber viscous fluid. Apparently they measured the glass murals of ancient cathedrals and found that the bottom of the glass was thicker than the top of the glass. Any one know how or what contributes to its viscousness?

This is a nice experiment, which shows formation of the special salt KICl4, which is a member of a whole class of very reactive and unstable salts (e.g. KI3, KIBr2, CsICl2, KICl4). http://woelen.scheikunde.net/science/chem/exps/KIO3+HCl/index.html You only need fairly common reagents, which are not that hard to obtain.

Is there a way to convert oxide to sulfide Thanks

I recently tried using ammonia as a reactant for a reaction (no reaction occurred), and placed the test tube in my homemade storage box/ fume hood. The next day, some what crystals had formed at the top of the test tube. I am almost sure that no reaction occurred (at least in the test tube), as I have gotten these same crystals with other ammonia experiments. They are perfectly white, and have a texture almost like that of a feather. Does anyone know what these crystals are?

Does anyone know what pressure Hydrogen has to be at to be able to conduct Electricity? Thanks Tash. Edit: I am under the impression it is and incredibly high amount of pressure, close to the pressure of jupiters core. but was wondering if anyone had a rough estimate and a Number.

Remind Me: Silver Nitrate + Halide - Precipitate Colours Can somone remind me the precipiate colours? I seem too have forgotten them... This is for the tests by which you can identify them through adding the solutions of the halide salt and the Silver Nitrate. Fluoride = Soluable Chloride = Milky White? Bromide = ? Iodide = ? Thanks for the help, this is bugging the hell out of me, Ryan Jones

Ok im new to all this and im not to sure im putting this in the correct froum but here goes! I was wondering if anyone could describe to me how I would go about making one of the hand warmers I have seen in camping shops I no that Sodium acetate and water are activated by bending a metal disk inside a pouch which then creates heat but after that im at a loss, if anyone can help me out I would be very greatfull?

I'm sure this is a really stupid question but I have always sucked at sciences so bear with me. ^^; I've been wondering if there's any chance mercury vapour could leak out of an unbroken fluorescent light bulb - or, if that were to happen, the light bulb would just never work because by then it would have nothing inside?

Ok, I understand the general reaction of electrolysis; The anode takes water and creates oxygen molecules, hydrogen ions, and electrons. The cathode takes water and electrons and creates hydrogen molecules and hydroxide ions. Furthermore, when a salt is dissolved in the water, electrolysis separates the two components of the salt, the anion to the anode and the cation to the cathode. What I am confused about is the role the cathode and anode have in this process. Say I'm using copper electrodes and NaCl as the electrolyte. Sodium is drawn to the cathode, where it combines with hydroxide ions? The chlorine is drawn to the anode, and it combines with hy…

Ok, I've been doing some electrolysis but I cannot figure out how to make a salt bridge to keep the reactions separate. I've tried using yarn wet with the solution, but that didn't work. So I tried using thin strips of paper towel, and that failed as well. So then I took a piece of tubing and siphoned it so that it was full of solvent, and again I was left with no reaction. What am I doing wrong?

In Al anodization, object made of aluminium to be anodized is anode. In my text book, it said that oxygen is produced and oxidize aluminum to Al2O3. But, Al is a stronger reducing agent than OH-, why is OH- oxidized instead?

anyone know how to make this from household materials? or what kind of stores might sell it?

Why is it that big hydrocarbons like in petrol dissolve polystyrene cups where as the little molecules in lighter fuel, don't? p.s. yes I am being very careful with this.

This is pretty neat. A while ago I had made a post in regards to some gallium that I had which had taken on a bluish tint and was really confusing me. I had obtained a bunch more gallium to add to my collection and had melted it down so I could pour it into the container with my existing gallium. I also wanted to have a mirrorlike surface to it so I had to scrape away the little bit of oxide that floated to the top and stuck to the sides of the glass. To remove the oxide, I used some newly stripped copper wire bent into a little hook. The oxide stuck to the copper and I was able to clean my Gallium. When the gallium solidified, however, I noticed that it had taken o…

since the group 1 elements can be substituted for Hydrogen, I got to thinking about Sodium Aluminate, and the possibility of Hydrogen Aluminate. NaAlO2 to HAlO2. after a google search, it came up with nothing at all usefull, Does this compound or Can this compound actualy exist?

Plz tell me How H2SO4 in manufacrured.. the stages.. web sites r needed too.. thanks alot:confused:

As we know, some metal ions like Calcium ion , potassium ion and sodium ion are colorless, while Cobalt ion, Iron(II)/(III) ion have color. Why ? What is the physical nature beneath that phenomenon ? What theories are involved ?

I have heard about the separation of water into hydrogen and oxygen underwater by short circuiting a charge. The process uses most metals (I've heard of aluminum and carbon as common) as electrodes. One touches the two electrodes together underwater and applies a current through the two electrodes (either DC or AC). If there's enough power, the electrodes will spark and bubbling will proceed. I've done the reaction with carbon rods and have produced hydrogen alone. It seems the oxygen might have combined with the carbon which was melted to form CO2 (I'm not exactly sure whether this is happening). The discoveries have led me to the following questions: 1. What is…

I did an electrolysis experiment with 99.8% pure niobium metal as anode. I tried this, in an attempt to dissolve the very inert metal. My reasoning was that the metal either dissolves or allows all kinds of gases (such as chlorine) to be produced at the anode. The latter would be very nice, having a metal anode, which does not pulverize with electrolysis. In reality, however, something really stunning happens. This is so weird that I decided to devote a web page to it. The experimental results can be read here: http://woelen.scheikunde.net/science/chem/exps/niobium/index.html

Wow, first of all I'd just like to say I'm impressed with the population of this website, it looks very solid. I was wondering if anyone had any ideas on how a poor Kansas boy who lives in his parents basement could isolate some Xenon or Krypton to work with over the holiday break? I guess fractional distillation of air is the only method that can get this, but if that's the method to use are there any suggestions about trapping the air? As to why, I'm interested in experiencing them in solid form. I know that with my limited resources it would be difficult to reach down to 116K with high pressure, but, hopefully, I can figure it out as soon as I get the "stuff."…

Hi there all you chemistry fans! I remember a few years ago I bought a large "lump" of Bismuth in crystaline form. I have reently added a smaller piece to my mineral collection and so, I want to know if there is something the amature chemist can do with it? The lump is about 40 Grams incase you were wondering As long as it does not involve something explosive or very, very toxic and as long as it does not vreak the forum rules (For your sake and mine) then please post your suggestions! Cheers, Ryan Jones

(I am a 9th grade student. ) Acidified potassium dichromate (VI) is used to test for the presence of reducing agents. How do I derive the 6 electrons in the following ionic equation during which the test of a reducing agent like sulphur dioxide is carried out? Cr2 O7 2- (aq) + 14H+ (aq) +6e- ==> 2Cr3+ (aq) + 7H2O (l) How is dichromate (VI) ion reduced to chromium (III) ion? Cr2 O7 2- ---> 2Cr 3+ How can reduction result in a negative charge changed to a positive charge?

anyone know a reaction with aluminum foils that can be done with common household chemicals to yield powdered aluminum?

Non-toxic Mercury compounds? Hi there everyone! I've been looking through a lot of compounds latly and it seems Mercury compounds are pretty damn nasty, are there any that are not toxic? Organic Mercury compounds are toxic, Mercury is toxic and inorganic Mercury compounds seem nasty but are there any that are non-toxic or are they all toxic? If there are any that are non-toxic I'd be interested too know though I think the odds are slim too none. Cheers, Ryan Jones

I was planning on obtaining some metal samples by extracting them from exotic thermite reactions (ie. vanadium, chromium, nickel). Unfortunately, there really isn't a simple way to prevent the aluminum oxide from entering the molten metal during the reaction. I was wondering if anyone could help me devise a scheme that would allow for minimal aluminum oxide impurities in the metal.