posted on Jan, 26 2005 @ 07:05 PM
I'm not entirely sure what you mean by "electron vibration". It is true that the position of an electron within an orbital is not precisley defined
(Heisenberg's uncertainty principle), and so is mathematically represented by the wavefunction phi. phi^2 is related to the "density" of the
electron cloud, which in real terms refers to the "probability" of finding an electron at any given location in its orbitals. Because classical
theory postulates that an electron should lose energy as they orbit the nucleus, and because atoms still seem to work, it was postulated by, among
others, Bohr (look up his absolutley brilliant analysis of the spectral lines of hyrdogen) that the electrons have to resonate with themselves, and
that their wavelength has to be a multiple of hbar/2, so that they reinforce themselves. If this were to change, then the atom would probably
collapse... I'm not too sure, but I'm thinking that the electrons would either fly off or impact the nucleus, which would probably cause at least
some form of radioactive decay. Problem is, electrons like staying where they are... I doubt you'd be able to have a non-integral path length.
"spin" is an intrinsic property of electrons that describes their angular momentum and various other quantum properties. Fermions, which are regular
matter, incl. electrons, have half-integer spin (1/2 for electrons). This means, roughly, that you have to rotate an electron through 720 deg. to
preserve symmetry. In any case, the spin number (Ms) can have two values, + or -. It roughly represents the fact that the electron rotates about
itself, and creates a magnetic field, as it is a moving charge. This is why things like iron can be ferromagnetic, as all the spins for some reason
align and add up to one big magnetic field.
Hope this sorta answers your question...