Author: JMcAulay
Date: 2003-04-30 03:50
Henry: You are correct, it is indeed simple. And when things are oversimplified, they tend to become less than perfectly accurate. Of course, complexity multiplies as greater detail is examined. For example, it's easy to say that fermentation of glucose yields ethanol and carbon dioxide, but it's even easier to overlook the more than a dozen intermediate compounds produced, some of which will remain in trace quantities.
For the responsible party, here I am. That was written by me and me alone. Had I quoted someone else, I would have cited the source.
Even water, H2O, that stable, electrically neutral molecule, frequenntly separates into constituent ions and then recombines. The H2O2 molecule will do the same, except its recombination often fails.
Henry is correct that the H2O2 molecule is in itself neutral. But as a practical matter, the "soup" in which it resides contains plenty of H2O, HO-, H+, and e- particles. What takes place immediately after any separation of the H2O2 molecule occurs (and it will) involves charged particles from other sources, and recombinination may be prevented due to the negative ionization of two HO components into HO- particles. Separation of one of these HO- particles into H+ and O-- could then result, with the H+ ion combining with some other HO- ion to form a water molecule, leaving the O-- particle alone. And that is only one possible outcome at this level, as other reactions also may be proceeding. The probability of specific reactions occurring makes a difference, even within a system as simple as this.
Such a reaction is driven by ionization energies and related characteristics of the consitutents (energy needed to remove an electron from an atom, corollary to the strength with which a nuclide hangs on to an electron). For example, oxygen's ionization energy is greater than that of hydrogen. This is why, in the absence of external force, water molecules that separate will form HO- and H+ ions rather than non-ionized atoms.
Any free oxygen atoms which lack electrical charge (non-ionized) will rapidly combine with one another. They can share electrons easily. Hence, the O2 molecule is quite stable. However, oxygen atoms which have acquired an extra electron will not combine as readily, and two O-- ions will hardly combine at all (I'd like to say "they won't," but y'never know....). So while some oxygen will no doubt leave the "soup" as O2, some takes off as O-, and likely a larger amount than that goes away as O--. The more ionized nascent oxygen is far more active. If you want to see instant rust, put a drop of H2O2 on a piece of warm iron.
It's been almost three years since I taught Chemistry, so my brain is likely fogged. In any event, nothing that I write is cast in concrete. I am always pleased to amend any position or statement based on more accurate information. Anyway, I forgot -- what does this have to do with Clarinets?
Regards,
John
|
|
The Clarinet BBoard
.jpg){kind=small}
.jpg){kind=small}
.jpg){kind=small}
.jpg){kind=small}
.jpg){kind=small}
.jpg){kind=small}
