Final answer:
True, The VSEPR theory correctly predicts that methane (CH4) has a tetrahedral geometry with H-C-H bond angles of approximately 109.5 degrees, not 120 degrees.
Step-by-step explanation:
The H-C-H angle in CH4 (methane) is predicted by the VSEPR theory to be 109.5° rather than 120°. This is because methane has a tetrahedral geometry where the carbon atom is at the centre with four hydrogen atoms symmetrically spaced around it. The three p orbitals (px, py, and pz) are indeed oriented at 90° relative to each other, but the hybridization of the carbon atom in methane involves the mixing of the 2s and 2p orbitals to form four equivalent sp3 hybrid orbitals. This results in the bond angles being approximately 109.5°, which optimizes the distance between the electron pairs in the four C-H bonds, minimizing repulsion.