mississippichem

I'll add that everyone should be careful with diazonium salts as they can be explosively unstable above 5 C. Always keep a thermometer in the reaction mixture! But yes, the HCl after sodium nitrite is a Sandemeyer reaction and it leads to the diazonium salt which is different from an azo-compound. vs.

You can approximate the integral heights of the peaks by treating them as simple triangles, if you're not the type that likes to integrate. This will be troublesome though if you don't have a decoupled spectrum. Could you give us a list of peaks with chemical shifts and multiplet designations? For example: a triplet at 7.3 ppm. Or 7.3(t)

It causes further splitting of the already quantized energy levels. Without it, the Pauli Exclusion principle wouldn't hold. Much chemistry is governed by the pairing and spin rules of fermions, namely electrons.

True, the mechanism of n-alkane combustion is not completely understood. IIRC though, the conversion of oxygen from the doubly degenerate triplet state to the non-degenerate singlet state is in fact the rate limiting step (it can take a while waiting for a random spin pair as entropy doesn't like this much). There is actually some evidence to suggest a pericyclic C-O-O-C transition state [not intermediate!] but this is far from conclusive. Lemur, Though it is somewhat poorly understood, it is known that the combustion of hydrocarbons does not involve ions. It is a radical process, meaning it involves unpaired electrons and no full charge separation. As far as the angular momentum is concerned, do you mean of the constituent electrons? or the angular momentum involved in the torisional and translational movement of the molecule itself?

Basically yes. The Jahn-Teller effect also becomes less pronounced as the ratio of metal ionic radius to dative bond length becomes smaller which kinetically speaking allows greater probability of a a gerad symmetric d-d overlap event [remember the analogous [imath]\pi[/imath] bonds have the opposite ungerad symmetry]. Breaking it down even further, the reduced Jahn-Teller effect ends up allowing a greater MO overlap integral. These high order bond clusters are more thermodynamically stable than their observed temperature ranges would have one believe. The major "road-block" is in the kinetics of the formation of the bond. Strongly [imath]\pi[/imath]-accepting ligands also serve to stabilize these species as the probability distribution of the electrons in the [imath]\delta[/imath]-orbitals becomes less concentrated and more "through-space" hyperconjugative geometry effects are allowed. This creates somewhat of a feedback loop that can serve to stabilize these high order bonds, albeit somewhat marginally.

It's just a rare case that a metal in at least a [imath]d^3[/imath] configuration has three non-bonding d-orbitals with the correct symmetry to get the multiple delta bonds. Usually, something called Jahn-Teller distortion prevents this from happening in already singly-bonded bimetallic species. These M-M multiple bonds are most common in second row d-block metals like Rhodium, ruthenium, osmium...you know, all the expensive ones. You should have a look at "Wade's Rules" and the "isolobal principle" if you are really interested.

Actually swansont's answer is the paragon of simple and explanatory. I imagine he is saying that with basic knowledge of the behaviors of gravity and magnetism, the "electric universe" hypothesis is falsified [proven wrong] without much mathematical rigor, deep thought, or experiments. The force of gravity diminishes as an inverse square. The force of magnetism diminishes as an inverse cube. There's not much that is cryptic or technical about that.

Be careful not to mix up a phenomenon like reflection with others like absorption and emission (things like fluorescence and phosphorescence). Radio waves are very low energy compared to things like UV or even visible light. They are only energetic enough to move electrons around in metals or cause molecules to vibrate a little faster. It takes much higher energy, generally speaking, to cause much chemistry to happen directly; including your physiological chemistry.

Are you familiar with the [imath] [x.y.z...n] [/imath] IUPAC naming convention for multicyclics? Or do you have a copy of the ChemDraw software?

In a plasma, coulombic interactions would almost completely drown out Van der Waals Forces. Van der Waals (especially the induced dipole, induced dipole interactions; London dispersion) forces are the weakest of the the intermolecular forces, where as coulombic interactions (electric forces between ions) are the strongest. Larger molecules have a larger Van der Waals surface and therefore experience more energetic London dispersion force interactions. Polarizability adds to the effect as well. I'm really talking mostly about the London dispersion forces here. Dipole-Dipole forces are just that; Permanent dipoles interacting between polar molecules.

#1 rule of finance: if it sounds too good to be true, it is. Currency markets (Forex) are already risky financial instruments. Even if you bet on lets say the BP/USD pair, two relatively stable currencies, you can loose your money quickly. The potential payout for the Dinar is huge, but the risk is proportionally huge.

So a photon collides with said "anti-photon" [i'll leave that one alone for the moment] to yield energy in the form of what?...more photons?

Nice link Horza. Thanks for that. I've often used the hand held UV-light technique as many of my compounds are colorless but fluoresce strongly in the near-UV. It's easy to forget the "old school" techniques in these days; many of which are still very valid and useful. There is also something rewarding about analyzing product mixtures without the aid of an automated Fourier Transform!

This is just [math] E = mc^{2} [/math] "re-expressed" in SI units: [math] 1J=1kg \cdot \frac{1 m^{2}}{1 s^{2}} [/math] This is the definition of the joule which is the SI unit for energy: [math] 1J =1 \frac{kg \cdot m^{2}}{s^{2}} [/math] This is basically what Klaynos showed a few posts ago, but I'm just expressing it in explicit units to show how it works. See the similarity? Don't think too hard here, you'll get confused. This is a case of the math making things easier.

Yes, as Hypervalent Iodine has stated. I strongly encourage that a student use the "curly arrow" notation for reactions. If one can follow the electrons, then they can follow the reaction. I like to tell students to use curly arrows because, even if you can't remember an exact mechanism, you can play with curly arrows until you find something that looks remotely like the mechanism you forgot. It has saved me on exams before. I used to never be able to remember the oxymercuration-demercuration mechanism.

More formally you would number that oxygen for that compound by nomenclature conventions and call it O1 or O2 etc. But carbonyl oxygen is a decent informal name.

I've always called it the carbonyl oxygen. Are you looking for a formal IUPAC name or something?

Plus the side effects of even mild selenosis are generally nasty and include an intense general body odor of garlic. Some things are worse than death And yes, Horza, I did some work with selenium dioxide a while back and was advised to proceed with extreme caution by my superiors.

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Some studies have shown selenium to be effective in the prevention of some cancers. However, the therapeutic window for selenium is quite narrow, so I would be very careful not to take too much. Personally, I would avoid micro-nutrient supplements unless you've been diagnosed as deficient by a licensed MD [which I am not]. This is just my opinion though, as many of the effects of trace nutrient deficiency or overdose are not that well understood. I would ere on the side of caution.

If you can't breathe, then you have high concentration of deoxygenated blood. Deoxygenated blood is blue/purple and causes the blue coloration of the skin.

I think they're just talking about the hydrochloride salt of glycine so don't worry about any HCl. Remember that: [math] K_{1}K_{2}=\beta[/math] So you can multiply two equilibrium constants to obtain an average value for a multi-protic molecule. I would use the Henderson-Hasselbalch equation: [math]pH=pK_{a}+log\frac{[A^{-}]}{[HA]}[/math] Or you can just set up both equilibrium expressions and solve accordingly.

A Grignard reagent exists in what's called the Schlenck Equilibrim. The alkyl magnesium bromide is in equilibrium with a dihalomagnesium and dialkylmagnesium species. It has been postulated but not confirmed that a halomagnesium cluster is involved as well.

Yes, and I doubt Harvard Press, Wiley-Interscience, or any national physics society (APS where I'm from) would approve of the unlabeled pictures with ambiguous vector arrows.

Yes, in the sense that the rules governing quantum objects roughly add up to the classical chemistry an physics that govern how our brains work. By that standard everything should be posted in quantum theory. Please provide evidence that our neurons behave as quantum objects. As far as I know, our neural processes occur at a scale neither small nor energetic enough to observe any quantum effects. I'm quite sure the physics of the brain can be explained well classically.