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Regular orbitals fill up in the typical way, with each orbital half filling (taking on only one electron) before any of them fill completely (2 electrons total) and then filling the next orbital in the same manner (Hund's Rule). Hybrid orbitals combine so that all the valence electrons are available to make bonding pairs with another atom. For example, instead of Carbon entirely filling its 2s orbital and having 2 unpaired electrons in its 2p orbital, it combines (hybridizes) its 2s and 2p orbitals in order to have 4 unpaired electrons available for bonding.
Hybridization of orbitals is usually greatly favored as this phenomena has lower energy compared to their separate counterparts. Since molecules and compounds form with the goal of attaining the lowest energy state of the interacting elements, it makes since that such an event occurs.
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