which substance has the weakest attractive forces based on the provided size of the molecule?\nc₆h₁₄\nc₄h₁₀\n…

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})