13 posts • Page 1 of 1
Hybridization comes from the random dispersion of electrons in an atom or molecule. The e- are in constant motion, so if they randomly all happen to be mostly to one side, that creates a dipole dispersion, allowing for another dipole molecule to bond via Van der Waals forces to the opposite charge of the dipole. Hybridization is the inducing of the dipole allowing this to happen.
Hybridization is what occurs when the atomic orbitals in the atom (s, p, and sometimes d) overlap consequently creating a larger orbital. This happens when bonds are formed and the electrons of one atom are interacting with those of another. Hybridized orbitals allow for stronger and more stable bonds.
Yeah I was in discussion today and I am still confused about hybridization. I just remember it being an interaction with the P & S orbitals but I am still confused. If there is any visual representation to help us visualize it, that would be soo helpful.