The was put together to try and explain , the in which electrons are shared by the two atoms.
This is not the case for , for which the difference in between the two atoms (or molecules) is large enough that electrons are no longer shared, but transferred – lost and gained.
This gives rise to a postively-charged and a negatively-charged ion, which are bonded together by the electrostatic force of attraction. No hybridization is needed for these since we know how bond – one atom loses electrons, the other one gains them.
On the other hand, hybrodization successfully explained . A classic example is ##C##’s abillity to form 4 bonds, despite the fact that it only has 2 unpaired electrons in its outermost shell.
One electron is promoted from the 2s-orbital to the 2p-orbital, creating four ##sp^3## hybridized orbitals that hold 1 unpaired electron each, thus explaining how four bonds can be possible.
When it comes to the shape of an , hybridization again cannot be used since these compounds have no definite shape.
The alternating positively-charged and negatively-charged ions which form an ionic compound arrange themselves in a tightly-packed crystal lattice structure.
This crystal lattice structure helps keep the ions tightly together, and is the reason for why ionic compounds are solid at room temperature.
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