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CH4 has weaker London forces than CCl4 because it is smaller and has fewer electrons, which means the intermolecular forces in CH4 are weaker than those in CCl4 since both molecules are nonpolar. This means it takes less energy to break the attractions between molecules in a sample of CH4, resulting in a lower boiling point.
When it comes to boiling point, we have to look at the intermolecular forces (e.g. dipole-dipole and london dispersion forces) not the intramolecular strength (like bond strength within a molecule). Since both CH4 and CCl4 are nonpolar, they both only have london dispersion forces for intermolecular forces. What determines the strength of london dispersion forces is the size of the molecules. Cl is larger than H, so CCL4 has the stronger intermolecular forces. With stronger intermolecular forces, it is harder to break apart CCl4 molecules into gas, meaning a higher boiling point.
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