Which type of intermolecular force exists between two CH_4 molecules?

• A. London dispersion forces
• B. Dipole-dipole interactions
• C. Ion-dipole forces
• D. Hydrogen bonding

Answer: (A)

Verified step by step guidance

1. Identify the molecular structure of CH_4 (methane). It is a nonpolar molecule because the C-H bonds are relatively nonpolar and the molecule is symmetrical, causing the dipoles to cancel out.
2. Recall that intermolecular forces depend on the polarity of molecules. Since CH_4 is nonpolar, it cannot have dipole-dipole interactions or hydrogen bonding, which require polar molecules or specific atoms like N, O, or F bonded to hydrogen.
3. Understand that ion-dipole forces occur between ions and polar molecules, which is not applicable here because CH_4 is neither ionic nor polar.
4. Recognize that the only intermolecular force present between nonpolar molecules like CH_4 is London dispersion forces, which arise from temporary fluctuations in electron distribution creating instantaneous dipoles.
5. Conclude that the intermolecular force between two CH_4 molecules is London dispersion forces.