The boiling points of normal hydrocarbons are higher than those of branched hydrocarbons of similar molecular weight because the London-dispersion forces between normal hydrocarbons are greater than those between branched hydrocarbons.

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This statement is true. London-dispersion forces, also known as van der Waals forces, increase with increasing surface area of the molecule. Normal hydrocarbons have a linear structure and can pack more closely together, resulting in a greater surface area and stronger London-dispersion forces. In contrast, branched hydrocarbons have a more compact and twisted structure, which reduces their surface area and weakens their London-dispersion forces.

The Boiling Points of Normal Hydrocarbons Are Higher Than Those