London dispersion forces are the primary intermolecular forces present in non-polar molecules. Arrange the following hydrocarbons in the increasing order of the magnitude of London dispersion forces between their molecules: (a) 2,2-Dimethylbutane (b) n-Butane (c) n-Hexane (d) 2-Methylpropane (e) n-Pentane Choose the correct answer from the options given below:

Step-by-step solution

London dispersion forces depend on the molecular mass and the surface area of the molecules. The magnitude of these forces increases with an increase in molecular mass due to higher polarizability. The molecular formulas of the given hydrocarbons are: (a) 2,2-Dimethylbutane: C₆H₁₄ (b) n-Butane: C₄H₁₀ (c) n-Hexane: C₆H₁₄ (d) 2-Methylpropane: C₄H₁₀ (e) n-Pentane: C₅H₁₂ Based on molecular mass, the general order of dispersion forces is C₄H₁₀ For isomers having the same molecular mass, branching decreases the surface a