Jano L.
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Correct me if I am wrong but if electrons moved in trajectories around the nucleus, covalent bonds between atoms would be impossible and a big chunk of quantum chemistry would go out the window(e.g. H has just one electron and it's shared in the H2O molecule).
I do not understand how you can derive such conclusion. The theory of chemical bond is based on Schroedinger's equation for point-like charged particles. It is not based on rejection of existence of trajectories. Sure, it does not use the concept, but it also does not disprove it.
Covalent bond involves sharing of electrons and the probability distribution for positions is spread all over the molecule, so the natural way to imagine this is that electrons move all around the molecule, visiting randomly all the nuclei in the vicinity. Since electrons are negatively charged and with greatest probability in between the nuclei, they attract positive nuclei and keep them in some average distance despite their mutual repulsion. If some atoms are very attractive to electrons, they can leave some other atoms without the bonding electrons for long periods of time and the glueing effect of the latter may cease - hence the dissociation of polar molecules into ions that happens in solvents. I believe this is quite standard picture adopted in theoretical chemistry (see works by John Slater, David Cook, ...) It may not calculate exact trajectories, but for sure it does not disprove them either.