Two compounds with the formula C6H12 are compared.
Compound A: n-hexane (an unbranched chain of six carbon atoms).
Compound B: cyclohexane (a six-membered saturated ring).
At 25 °C, the saturated vapor pressures are 0.16 atm for n-hexane and 0.13 atm for cyclohexane.
(a) Using the data above, determine which compound has the stronger intermolecular attractions at 25 °C. Support your answer with a brief calculation or verbal argument based on vapor pressure.
(b) Provide a particulate-level explanation for the difference in intermolecular attractions between Compound A and Compound B, focusing on molecular shape and contact surface area.
(c) Both compounds have the same number of electrons. Explain why polarizability alone cannot account for the difference in vapor pressure, and identify the structural factor that is most responsible.
(d) Predict how replacing one C–C single bond in cyclohexane with a C=C double bond (forming cyclohexene) is expected to affect its saturated vapor pressure at 25 °C. Justify your answer in terms of the factors that influence London dispersion forces.