Question

which substance has the weakest attractive forces based on the provided size of the molecule?
c₆h₁₄
c₄h₁₀
c₂h₆

Explanation:

Step1: Understand intermolecular forces

The strength of London - dispersion forces (a type of intermolecular force) is related to the size of the molecule. Larger molecules have more electrons and a greater surface - area, leading to stronger London - dispersion forces.

Step2: Compare molecule sizes

Among the given molecules, the smallest molecule will have the weakest attractive forces. Assuming the molecules are hydrocarbons, a smaller number of carbon and hydrogen atoms means a smaller molecule. Without knowing the exact identities of \(C_{x}H_{y}\) in full, generally, the molecule with the fewest number of atoms will have the weakest intermolecular forces. If we assume \(C_{2}H_{6}\), \(C_{4}H_{10}\) and \(C_{6}H_{14}\) are the options, \(C_{2}H_{6}\) is the smallest.

Answer:

The molecule with the fewest number of carbon and hydrogen atoms among the given options. If the options are \(C_{2}H_{6}\), \(C_{4}H_{10}\) and \(C_{6}H_{14}\), the answer is \(C_{2}H_{6}\)