UC

This is me not reaming you out, but you're wrong. nope.

The chalcogen is sulfur. It is even on wikipedia, although it doesn't have it's own page. It is to the best of my knowledge not comercially available. I am looking at what I think is the first published paper on it: september 2006

So, you want the answer?

Oh, but that would make it too easy.

What? I am unaware of any hemihdyrates. is there any chance that this solution contains a lot of chloride anion? Copper (II) ions form yellowish tetrachlorocuprate complexes in solutions with lots of chloride, which result in a green solution, since the water-coordinated copper ions are blue.

Well, it's in a glass beaker/erlenmeyer as it is, so yes. Just don't store it in glass.

no hydrogen.

sapphyrin Your first mistake was mentioning it in IRC a while back. I am a polycyclic aromatic molecule with a rather sunny name, consisting solely of carbon and a chalcogen. What am I?

That's because I didn't see it.

Meitnerium. Someone else post a riddle. I got nothin'.

http://en.wikipedia.org/wiki/Polyadenylation

A saturated solution of NaOH in water consists of 111g of NaOH dissolved in 100mL of water. This solution is thick, attacks glass over time (forming silicates), and is air sensitive, precipitating Na2CO3 as it absorbs CO2 from the air. It will happily cause chemical burns and damage clothing. Instead of a saturated solution, you may consider a 50%wt/wt solution, which is simply 100g of NaOH in 100mL of water. This is close to saturated and is comercially available. Even if you start with crushed ice, adding this much NaOH rapidly will result in solution more than hot enough to burn you, which may boil. It will put off plenty of steam either way, which carries small droplets of caustic solution. If you dump it in all at once, it will solidify into a brick in the bottom of your container. Wear gloves, goggles, and a lab coat (or at least a crummy shirt). Start with ice water and have an ice bath prepared. Slowly add the NaOH in portions to the water in a large erlenmeyer, swirling constantly. Chill the solution between additions. Store in an airtight HDPE container. Nalgene makes these if you're looking for a supplier. They are reasonably priced.

http://www.scienceforums.net/forum/showthread.php?t=31089 I had been using it long before coming to this forum. To make forum-friendly images, you need to save as a bitmap and then convert to a JPEG in another program, which drastically reduces the file size. I actually find it more usable than chemdraw, which costs @$400 IIRC. Of course, it does lack some of the advanced stuff chemdraw has, but for anything you'll need to post here, it's just fine.

Many solvents swell plastics and rubbers, but which solvents for which plastics and rubbers are important considerations. Try looking up a solvent incompatibility sheet. One I know off the top of my head: EPDM rubber is massively swollen by aromatic hydrocarbons (benzene, toluene, xylene, etc.)

No. You won't make any aluminum isopropoxide. Instead you'll make aluminum hydroxide until you run out of water, but Al(OH)3 is voluminous, so you probably would have sludge as your reaction mixture. Look at the drawing below. From left to right, I have drawn formaldehyde, benzaldehyde, neopentaldehyde, acetaldehyde, propionaldehyde, and cyclohexanal (formylcyclohexane). The alpha carbon is the carbon adjacent to the aldehyde carbonyl carbon. If the alpha carbon has no hydrogens (alpha-hydrogens) on it, the cannizzaro reaction will occur, with no condensation products. For formaldehyde, there is no alpha carbon at all, so it's good to go for cannizzaro. For benzaldehyde, the alpha-carbon is part of the aromatic ring, and has no hydrogens. For neopentaldehyde, the alpha-carbon is quaternary and has no hydrogens. Acetaldehyde, propionaldehyde, and cyclohexanal all have at least one alpha hydrogen, and are therefore capable of undergoing keto-enol tautomerism. Thus, they are capable of forming enolates, which participate in the aldol reaction/condensation. There is ALWAYS an equilibrium present, but sometimes it lies so far to one side of the reaction that it effectively goes to completion. Aluminum isopropoxide is picky about which things it reduces. I'm not sure it would even work on acetaldehyde, but some research on standard enthalpies of formation should tell you the answer.

Heme B does. http://en.wikipedia.org/wiki/Heme

Your avatar is hemoglobin. The first answer is porphyrins. Porphin has 11 double bonds. Element 20 is calcium, an appropriate choice for a membrane transport question. Using this page (http://users.rcn.com/jkimball.ma.ultranet/BiologyPages/M/MembraneTransport.html), [math] deltaG=2*(309.6)*ln(10/1) [/math] So, ΔG=1425.76cal/mol = 5965.38J/mol = 5.97kJ/mol -> 6 So, element 26, which is Iron.

Magnesium is an alkaline earth metal and will happily react with water to generate hydrogen. I think this is because the copper is laid down on the magnesium and forms a galvanic cell, which should predispose the magnesium to rapid reaction in water If you put some aluminum foil in saturated NaCl brine, you get no reaction. but it is rather vigorous upon the addition of a catalytic amount of copper salt. This is the same principle, and credit to Woelen for the experiment.

The Cannizarro reaction is only applicable to aldehydes that cannot undergo keto-enol tautomerism. The best known of these are benzaldehyde and formaldehyde. With acetaldehyde you will mainly get aldol reaction and aldol condensation products plus an enjoyable amount of tar. Salt will not generate anhydrous isopropanol. It will get you to 91% and no better. Take the 91%, shake with 10% of it's weight in NaOH flakes, remove the aqueous layer. Repeat with another small amount of NaOH, and distill to give an effectively anhydrous product. If you want better, use a little sodium metal and redistill in flame-dried glass. I can dig up the reference if you'd like. Also, proper nomenclature is aluminum isopropoxide.

Hence my use of "some." If you intend this as a means to neutralize bleach, then the production of any chlorine gas is unacceptable. Go try it. I guarantee the fumes coming off are not just oxygen.

Perhaps in theory, but bleach mixed with hydrogen peroxide will also make some chlorine gas.

I can't believe I forgot this one. This isn't tolerant of beta-haloethers though, which undergo elimination (see the Boord olefin synthesis), or of hydroxy groups, or other non-LiAlH4 responsive functional groups that do react with grignards.

LiAlH4 reduces primary and secondary alkyl halides to the alkanes, and in some cases tertiary alkyl halides. assuming the structure is relatively simple and insensitive, you could dehydrohalogenate the tertiary alkyl halide and then hydrogenate it over Pd/C. (palladium on carbon) Googling around also found me some stuff on tributyltin hydride with catalytic InCl3, which seems to occur via a radical mechanism.

In theory yes, but it's worthless in practice as hydrogen reductions of metal compounds need to be carried out in furnaces to get them to work.

Very little protein to speak of Perhaps gelatinization of starches is what you're looking for.