Final answer:
CH3 group typically exhibits sp3 hybridization, not sp2, due to being bonded to four areas of electron density, resulting in a tetrahedral geometry with bond angles of approximately 109 degrees.
Step-by-step explanation:
The CH3 group does not have sp2 hybridization. In a molecule where carbon is surrounded by three regions of electron density, sp2 hybridization occurs, which manifests in trigonal planar geometry with 120° bond angles as seen in molecules like ethene (H2C=CH2).
In CH3 group, typically part of a larger molecule, each carbon atom is usually sp3 hybridized, indicating it is linked to four areas of electron density, which can be four single bonds, resulting in a tetrahedral geometry with approximately 109° bond angles.