What is the molecular shape of methane (CH4)?

Methane (CH4) has a tetrahedral molecular shape due to the arrangement of its four hydrogen atoms around the central carbon atom. This geometry arises from the concept of electron pair repulsion outlined in VSEPR (Valence Shell Electron Pair Repulsion) theory.

In methane, the carbon atom forms four single covalent bonds with the hydrogen atoms. According to VSEPR theory, the repulsion between the bonding pairs of electrons on the carbon will lead to a spatial arrangement that minimizes this repulsion. The most effective way to achieve this is by positioning the hydrogen atoms at the corners of a tetrahedron, which allows for maximum separation between the electron pairs.

The bond angles in a tetrahedral shape are approximately 109.5 degrees, which is consistent with the observed angles in methane's molecular structure. This three-dimensional arrangement is crucial in determining not only the molecule's shape but also its physical and chemical properties.

In summary, the tetrahedral geometry of methane is a result of four equivalent bonds around the central atom, aimed at minimizing electron repulsion, leading to a stable molecular configuration.