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From: moroney@world.std.spaamtrap.com (Michael Moroney)
Newsgroups: sci.physics
Subject: Re: 2electronorbital.GIF
Date: Tue, 7 Feb 2017 19:09:20 +0000 (UTC)
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john <johnsefton288@gmail.com> writes:

>Anyway, I deduced that one rotation of the
> disc (one cycle), per two precessions of

Nature doesn't care what you "deduce".  Nature has her own rules. It is the job
of science to discover those rules.  And no, Nature isn't going to be so retarded
as to involve retarded spinny things, except as a mathematical curiosity perhaps.

>So, since applying ones classical theory
>to Benzene was the acid test for
>classical electron orbitals,

no, at the atomic scale you have to apply QM theory, classical mechanics doesn't
work at that level.

>Current theory
>would have it that this electron
>'delocalises' or whatever, 'spreading out'
>around the ring, somehow. I don't 
>see how this is possible, classically.

Again, classical mechanical theory doesn't work for that.

It's actually not so hard to see how "delocalized" electrons show up.
The wave functions of electrons in a bond (or antibond) are simply
the sums of the wave functions of the individual electrons involved.
Take the wave functions 6 p-orbital electrons for atoms arranged in a
hexago (the hexagon in the xy plane and the p orbitals pointed in the
z direction) with the "+" side of the 6 wave functions all on the same
side of the xy plane and add them, you'll get a wave function that is
mostly delocalized, with the function value between atoms close to that
directly above the atoms.

The electron density function is just the square of the wave function,
so you'll see the density between the individual p lobes is close
to that of the lobes themselves.

Maybe you can reprogram your 3d software to plot electron wave/density
functions for bonds instead of doing more silly spinny things.

>Look at the six green electrons in the
<snip babble>

> Isn't that sweet?

No, that is retarded.