"About 50 years ago it was discovered that, under certain circumstances, the water molecule can split up in another, quite different, way. If, for instance, water is exposed to radiation such as X-rays or gamma rays, the two-electron bonds between the oxygen and the hydrogen atoms can briefly split, leaving one unpaired electron on the hydrogen and one on the oxygen, thus creating two radicals, both electrically neutral but both having only one spare electron. Thus, momentarily,there are two atoms each with only one electron in an outer orbital. These radicals are known, respectively, as the hydrogen radical and the hydroxyl radical, and both of them are highly reactive. The hydroxyl radical is the most reactive free radical known to chemistry and will attack almost every molecule in the area.
It is the unpaired electron that makes these radicals so chemically active. A group with an unpaired electron is highly unstable and is desperate either to pick up another electron from somewhere, or to give up its solitary electron.
Hydrogen atoms, which have only one electron, never exist individually for more than a fraction of a second, but immediately join up in pairs to produce a hydrogen molecule of two atoms with a stable pair of electrons (H2). The same applies to a hydrogen radical—which is, of course, simply an isolated hydrogen atom. It is this stable state that free radicals are always aiming for, and if a free radical is formed, it will at once attack the nearest molecule in order to steal or hand over an electron and achieve stability.
So now we have a definition of a free radical. A free radical is any atom or group of atoms that can exist independently and that contains at least one unpaired electron. Some free radicals exist for appreciable lengths of time. But the great majority have only a very brief independent existence before either grabbing an extra electron or giving one up."
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> According to this treatment of water-metal surface interaction by P. Thiel at Ames, and Madey at NIST,
> the adsorbed water molecule tends to dissociate into bound OH and H on the Nickel portion of
> the stainless steel.
> According to other Cr-Ni catalyst sources the presence of Chromium Oxide present on
> the surface keeps the exposed Ni area active.
>
>
Add the complexities in a electrolysis cell to this and....get back more than three orders of magnitude
energy multiplication without the hydrino formation?
Fred
