Question

n solid methane, the forces between neighboring CH4 molecules are best characterized as: a. ionic bonds b. covalent bonds c. hydrogen bonds d. ion-dipole forces e. London dispersion forces

Answer 1

The forces between neighboring molecules in solid methane are characterized by London dispersion forces. These result from temporary fluctuations in electron distribution within molecules. Other bond types like ionic, covalent, hydrogen bonds and ion-dipole forces aren't applicable to methane.

Step-by-step explanation:

In solid methane (CH4), the forces between neighboring molecules are characterized by London dispersion forces. These forces are weak intermolecular forces that occur between all atoms and molecules. They result from temporary fluctuations in electron distribution within molecules, creating temporary dipoles that induce similar dipoles in neighboring molecules. While ionic bonds occur between ions, covalent bonds happen within molecules, and hydrogen bonds and ion-dipole forces are stronger types of intermolecular forces, none of these are applicable to methane as it is a non-polar molecule with symmetry in its distribution of charge.

Learn more about London dispersion forces