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Molecules have hybridizations to form enough bonds. For example, CH4 has hybridization because normally C only has 2 unpaired electrons. With an sp3 hybrdization, C has 4 unpaired electrons that can bond with 4 H's. On the other hand, hybridization can also ensure the stability of a molecule. For example, NH3 has hybridization. While N has 3 unpaired electrons that could bond with each H, these electrons are all in the 2p orbital. When atoms bond to a central atom's p orbital, the bond angles will be 90 degrees. However, NH3 has bond angles that are NOT 90 degrees; instead, the angles are less than 109.5 degrees. To make the bond angles correct, which ensures the molecule's stability, N's orbitals are hybrdized to sp3. Therefore, each H atom binds to an sp3 orbital in N.
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