UC

Actually Cu2O (which is what is being discussed) is red (maroon, however is most likely copper). If the buildup is actually *on* the cathode, it is certainly copper metal. Please see here for making Cu2O by electrolysis: http://webpages.charter.net/dawill/tmoranwms/Chem_Cu.html

Yeesh, lots of questions. For proton NMR spectra, all you need to consider are 1: how many equivalent hydrogen are there for the peak (gives the integration, this is where symmetry matters) and how many hydrogen is it coupled to (ignore hydrogen attached to the same carbon, symmetry does not matter).You're first guess is correct, in that it is coupled to 8 hydrogens and thus is a nonet. For part D, you do need to count both methylene groups and thus you have a pentet. For questions 2 and 3, I want you to tell me why you are picking the reagents you picked. what does each do? what are the intermediate products? For 4, because acidified dichromate is a *powerful* oxidant. You can make aldehydes with dichromates, but it's fairly tricky. For 5, http://upload.wikimedia.org/wikipedia/commons/b/b9/PBr3_alcohol_rxn.jpg What kind of mechanism is that and what does it do to stereochemistry? For 6, because neopentyl groups are so hindered that they don't really undergo SN2 reactions. The alternative is SN1, which involves a carbocation and alkyl shifts can occur. For 7, look up zaitsev's rule.

I believe the answer you're looking for is spotting plate. Looks something like this? http://www.thesciencefair.com/Merchant2/graphics/00000001/SptingPlate%203765_M.jpg

Sulfonating just about anything makes it water soluble, but then it'd be nonvolatile. But you'd also probably cleave the ether if you use oleum.

You asked this as user thorazine on sciencemadness.org. You got their opinion. Indian and Chinese glassware is in general, garbage and you're better off buying pyrex or kimax stuff if you don't know the quality. It's pricier, but the odds of the pieces breaking in the long run is lower so you'll save money and much frustration.

Oxonium ions are not very happy ions, unlike ammoniums for example. They will slowly hydrolyze in strongly acidic conditions, but the equilibrium for [ce] R2OH^+ + H2O <-> R2O + H3O^+ [/ce] lies far to the right.

It's not about the size of the boiling chips. It's about surface area. One or two real boiling chips probably have the surface area of hundreds of crushed bottles. It provides a good place for bubbles to nucleate. The sulfuric acid fog *is* condensed, just not sticking well to itself. The shape of the graham condenser forces it to hit walls and coalesce into drops. The rationale for the upright 3-way adapter is to minimize strain on the glass joints and keep acid from pooling in the 3-way (and possibly seeping past the stopper).

No it wouldn't. Plaster of paris at least, which is what most people think of when they think of plaster. It's calcium sulfate. Sulfuric acid isn't going to do anything to it.

Turn the 3-way adapter right side up. Use a smaller heating flask or insulate the larger flask to get more vapor into the condenser. I'm surprized one condenser (or even an air condenser or no condenser) wasn't more than enough. Drop the leibig entirely. The graham just gives more surface area for the H2SO4 to condense on. Were you getting a "fog" of acid in the liebig? Use boiling chips. Activated carbon or maybe even some powdered plaster is probably acceptable as a crude replacement.

You should talk to YT about this stuff This is one of his specialties. He's probably asleep right now, so I'll give it 4 or 5 hours before he responds.

*SLOWLY* add conc. sulfuric to NaCl. Only use gentle heating when no more HCl is evolved by itself. If you dump the two together and heat, you will probably blow the connections on your apparatus open and end up inhaling a cloud of HCl, as will everyone nearby. Lead the gas to the surface of ice cold water. Bubbling probably isn't necessary as the solubility is quite high and you will end up with suckback.

I believe that [ce] 2KClO3 -> 2KCl + 3O2 [/ce] using a bit of [ce] MnO2 [/ce] as catalyst is going to be easier. It is my understanding that [ce] KClO4 [/ce] is quite a bit more stable and resistant to decomposition. As far as I can tell, this is just homework, so dangerous isn't really an issue. If it is actually being done, I suggest adding washing soda and activated carbon to some plain 3% hydrogen peroxide. The bubbles will be [ce] O2 [/ce]. As for big314mp's suggestion, that's not quite a reaction to some ears, although it will do as advertised.

This page is quite useful: http://www.cem.msu.edu/~reusch/VirtualText/benzrx1.htm As for activating versus deactivating, more electrons make an aromatic ring more reactive. Are fluorines going to give or pull away electron density from a carbon? (look at electronegativities if you aren't sure) If that carbon is attached to an aromatic ring, is it going to give or borrow electron density to compensate for what the fluorines are doing to it? If you have any further questions, feel free to ask them here

Concentrated aqueous solutions of Cobalt chloride or Copper chloride will change color upon heating. Lower temperatures favor more water ligands around the metal ion, while higher termperatures favor chloride ligands. Cold CoCl2 solutions are pink, but become blue upon heating. CuCl2 solutions are blue when cold and become increasingly green when heated. This is a large temperature swing though and perhaps unsuitable for what you want.

Are pictures available? Was there any current running through the wires? Were the wires touching any dissimilar metals? Offhand, Id say galvanic corossion to aluminum hydroxide and iron contamination making the orange color, but I'd need to know more first.

Dissolve tin in moderate strength sulfuric acid and keep air out, or you'll make some stannic ions Sn(IV) out of your stannous Sn(II) ions. It probably needs excess acid around to be stable in solution.

Magic. No, eucalyptus oil is primarily 1,8-cineole (eucalyptol), a terpenoid and ether. It belongs in the same class of molecules as turpentine and as such behaves much like gasoline with respect to water solubility. To change the structure to make it soluble in water or solid at room temperature means it is no longer eucalyptus oil and probably would neither have the same properties nor smell (if any).

Decomposition of hydrogen peroxide? [ce] 2H2O2 -> 2H2O + O2 [/ce] Decomposition of calcium hypochlorite? [ce] Ca(OCl)2 -> CaCl2 + O2 [/ce] The way oxygen originally isolated, by decomposition of mercuric oxide? [ce] 2HgO -> 2Hg + O2 [/ce] To test, perhaps the very classic glowing splint experiment? A small piece of wood with an ember will flare up and burn in an oxygen atmosphere.

I've done this with 15% H2O2 and (I think) activated charcoal. The water was boiling by the time it ran out of H2O2 because the decomposition is quite exothermic. Before it got so hot that the steam interfered, I was doing the "glowing wooden splint" demonstration. It flares up quite impressively in a mostly oxygen atmosphere. The inhibitors and buffers in [math] H_2O_2 [/math] are almost always just phosphoric acid and acid phosphate salts to regulate the pH. [math] H_2O_2 [/math] is much less stable in alkaline solution. MnO2 is also a fantastic catalyst. Iodide ion is also good. Google "elephant toothpaste" for demonstrations that use soap to trap all the gas being produced. Liver is an excellent source of catalase. I did that experiment in 7th grade biology with blended raw liver and 3% hydrogen peroxide. There are also enzymes that catalyze the oxidation of compounds by [math] H_2O_2 [/math]. For example, blend peeled turnip and water and strain through cheesecloth. The liquid has a fair amount of peroxidase in it. Upon adding dilute hydrogen peroxide solution, buffer, and guiacol solution, the color goes from clear to yellow and then to browns as guiacol is oxidized to tetraguiacol. Without the peroxidase, the process only occurs very slowly.

precipitates from what? when you do what to what? I have an idea but you've given us a portion of the question and it doesn't make much sense.

kalt = cold? I snagged the link from an old thread over on sciencemadness.org. I believe some testing was done and better results were when everything had been prechilled as much as possible. My larger freezer at home reaches -20C. A problem though is measuring the temperature you achieve.

So you have something to discuss or any kind of opinion on this at all, or are you just adding clutter to the forum? Also, judging by title, you've referenced some article in a magazine meant for the public. I could be wrong however. Can you provide a link or the authors of said article. A title means very little and tells us nothing of credibility.

Correct The whole top row of transition metals, as you can see, are about the same size and many substitutional alloys are known between them. For example stainless steel is mostly iron, nickel, and chromium. Carbon is tiny by comparison, but has it's place in stainless steel as well, filling in some of the gaps between the Fe, Cr, and Ni.

In slightly more common terms, the difference in electronegativity between aluminum and oxygen is smaller than between magnesium and oxygen. The [math] Al_2O_3 [/math] therefore has more covalent character than MgO (which is more ionic in character). Ionic compounds tend to be high melting, while covalent have fairly low melting points.

http://boomeria.org/chemlectures/textass2/table10-9.jpg <-- what does this tell you?