Final answer:
A methane molecule consists of four sigma bonds creating a tetrahedral geometry with 109.5-degree bond angles and symmetrical C-H bond lengths.
Step-by-step explanation:
A methane (CH4) molecule consists of four sigma bonds and no pi bonds. These sigma bonds form when the 1s orbital of each hydrogen atom overlaps with one of the four sp³ orbitals of the carbon atom. Every bond in a methane molecule is a single covalent bond, evidencing strong, equivalent connections between the carbon atom and each hydrogen atom, leading to a tetrahedral shape with bond angles of 109.5°.
The tetrahedral geometry of methane is a result of the spatial arrangement of the four hydrogen atoms around the central carbon atom, optimizing the distance between each pair of bonded electrons. The bond length in all four C-H bonds is equal, ensuring that the shape of the molecule is symmetrical and balanced. This geometric arrangement illustrates the fundamental concepts of molecular shape and bond formation in simple hydrocarbons that are crucial to understanding more complex organic structures.