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Natural Science Forum / Physics / Particle Physics / April 2006New carbon ring animation the correct version.
This is my latest animation of a six-member carbon ring. http://users.accesscomm.ca/john/Hexane.GIF The last one had adjacent atoms with the same precession (spinning discs precess and yet remain parallel). It was not right. The electrons can't transfer while maintaining the same acceleration unless the edges of adjacent discs are momentarily following the same path. This can only happen when the discs have opposite precession,i.e. are UPSIDE-DOWN wrt each other. ( http://users.accesscomm.ca/john/Cyclohexane1.GIF to see INCORRECT version.) In order to bond, atoms have to be pointing the opposite way. And what determines the direction of the atom is the direction of the precession of the disc. John Galaxy Model for the Atom http://users.accesscomm.ca/john > This is my latest animation of a six-member > carbon ring. [quoted text clipped - 18 lines] > Galaxy Model for the Atom > http://users.accesscomm.ca/john Doesn't have the right geometry. The atoms in cyclohexane do not lie in a plane. PD Doesn't lie in a plane. Allow me to boot up my AutoCad and give you a different angle. This is the chair form. Next post. Here you go: http://users.accesscomm.ca/john/c6chair.GIF > Here you go: > http://users.accesscomm.ca/john/c6chair.GIF Couple quick questions, because the static projection hides things: In your left pane, you show 4 visible carbons. I'll call the one at top left 1, the one visible just below it 2, the one behind 2 but obscured is called 3, the one at bottom right 6, the one visible just above 6 is 4 and the one behind 4 but obscured is called 5. 1 2(3) \ 4(5) | 6 Questions: 1. It's not obvious from your GIF how 1 bonds to both 2 and 3. 2. It's not obvious why 2 bonds with 4 through the spot at roughly 5 o'clock on 2 (11 o'clock on 4) and not someplace else. Why not at one of the other spots, like the one at 3 o'clock (9 o'clock)? Note that conventional quantum mechanics answers both these questions nicely, and organic chemistry has made use of that for decades. PD > > Here you go: > > http://users.accesscomm.ca/john/c6chair.GIF [quoted text clipped - 23 lines] > > PD All bonds are at the points of tetrahedrons. See: http://users.accesscomm.ca/john/tetra.jpg Both chair and boat form rings are to be found within a tetrahedron lattice. John Galaxy Model for the Atom http://users.accesscomm.ca/john P.S. Would you like me to show you a tetrahedron lattice? That would take me 5 minutes. JS Actually, though, what is interesting, is that the actual bond-points ARE in the same plane, but the atoms aren't. John > > > Here you go: > > > http://users.accesscomm.ca/john/c6chair.GIF [quoted text clipped - 27 lines] > Both chair and boat form rings > are to be found within a tetrahedron lattice. The question's not so much whether your model says carbon atoms *can* form a tetrahedral lattice, but *why* they do. This is why I pointed out the rather arbitrary places where you have bonding happening. QM predicts that single-bonded carbons *should* form a tetrahedral lattice, and this is one of the strengths of that system. PD > John > Galaxy Model for the Atom > http://users.accesscomm.ca/john > P.S. Would you like me to show you a tetrahedron lattice? > That would take me 5 minutes. > JS > > > > Here you go: > > > > http://users.accesscomm.ca/john/c6chair.GIF [quoted text clipped - 34 lines] > QM predicts that single-bonded carbons *should* form a tetrahedral > lattice, and this is one of the strengths of that system. This gif shows the galaxy orbital pattern: http://users.accesscomm.ca/john/cubepath.GIF As you see, it centers on a cube. Here's a single path: http://users.accesscomm.ca/john/He.GIF You see there are two places where the line crosses over itself? That is where the corners of the cube hit. Now.........I'm sure QM has just such a straightforward explanation: go ahead, tell me 'one of the strengths of that system.' (He won't.) John > > > > > Here you go: > > > > > http://users.accesscomm.ca/john/c6chair.GIF [quoted text clipped - 52 lines] > > (He won't.) Sure. See the chapter on hybrid orbitals in any first-year chemistry textbook. You'll also see there why the bonding pattern (and the angles between bonds) changes when the bonds are double-bonds or triple-bonds. See for example, Chemistry, Brown, LeMay & Bursten, Chapter 9.5-9.6 (pages 319-331 in the 8th ed.). > John > > > > > > Here you go: > > > > > > http://users.accesscomm.ca/john/c6chair.GIF [quoted text clipped - 58 lines] > See for example, Chemistry, Brown, LeMay & Bursten, Chapter 9.5-9.6 > (pages 319-331 in the 8th ed.). Thanks, I'll do that. I might have one downstairs. But I want to explain it by discrete, constant-acceleration pathways. I achieved the molecular orbital on March 7, see the gifs below: http://users.accesscomm.ca/john/IWIN1.GIF http://users.accesscomm.ca/john/iwin4.GIF This shows the molecular pathway to be 25% shorter for each of the participants. ALSO, if you look closely, each participant must go on BOTH SIDES of each orbital. (I know- it necessitated 96 frames instead of 64- I noticed.) In the single atom it is confined to one side. This is a big advantage for each electron. But I haven't even considered double and triple bonds, I admit. Hey! It's an ongoing puzzle. But it's fun. This weekend I'm going to strap 200 pounds to the center of the frame I have on bearings on the axle of the Big Ball (see page) and roll it down a fairly large hill. Then I'm going to re-position the 200 pounds 6 inches to one side of center and do it again. John Galaxy Model for the Atom http://users.accesscomm.ca/john http://users.accesscomm.ca/john/IWIN1.GIF is the coolest one. It's too bad the yellow path is partially blue on the top view (because it overlays the blue from that angle). |
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