Final answer:
A methane (CH4) molecule is nonpolar due to its symmetrical tetrahedral structure and equal sharing of electrons in non-polar covalent bonds, resulting in a balanced distribution of charge.
Step-by-step explanation:
The molecule of methane, CH4, is nonpolar because its molecular structure is tetrahedral, with each of the four hydrogen atoms symmetrically arranged around the central carbon atom. This symmetrical arrangement allows the electrons to be shared equally among the C-H bonds, resulting in a molecule with no net dipole moment. The carbon and hydrogen atoms also have similar electronegativities, leading to non-polar covalent bonds. Thus, overall, the distribution of charge throughout the molecule is even, making methane nonpolar.
Furthermore, the tetrahedral geometry of methane ensures spatial symmetry, preventing any concentration of charge in a particular direction. This molecular symmetry, combined with the homogeneity of carbon-hydrogen bonds, results in a nonpolar molecule, underscoring the significance of both structural and electronegativity factors in determining the overall polarity of compounds. This molecular characteristic is vital in understanding methane's behavior in various chemical and physical interactions.