Final answer:
sp³ hybridization involves the combination of one s orbital with three p orbitals to create four sp³ hybrid orbitals, resulting in a tetrahedral molecular geometry, as exemplified by methane (CH₄).
Step-by-step explanation:
sp3 hybridization refers to the mixing of one s orbital with three p orbitals resulting in four equivalent hybrid orbitals. This occurs in an atom surrounded by four regions of electron density. The newly formed sp3 hybrid orbitals have an equal mix of the characteristic of the contributing orbitals and arrange themselves in a tetrahedral geometry to minimize repulsions. Each of these hybrid orbitals is capable of forming a sigma bond by overlapping with orbitals from other atoms.
An example of sp3 hybridization can be seen in methane (CH4). Here, the carbon atom has four valence electrons and is surrounded by four hydrogen atoms. During hybridization, carbon's one 2s and three 2p orbitals mix to form four equivalent sp3 hybrid orbitals which then overlap with the 1s orbitals of hydrogen atoms to form methane with a tetrahedral shape.