Question

decide which intermolecular forces act between the molecules of each compound in the table below. compound intermolecular forces (check all that apply) dispersion dipole hydrogen - bonding hydrogen fluoride ch₄ methane ch₃cl chloromethane carbon disulfide

Explanation:

Step1: Analyze hydrogen fluoride (HF)

HF has H - F bond. Fluorine is highly electronegative. Dispersion forces are present in all molecules. Dipole - dipole forces exist due to polar H - F bond. Hydrogen - bonding occurs as H is bonded to highly electronegative F. So it has dispersion, dipole, and hydrogen - bonding.

Step2: Analyze methane ($CH_4$)

$CH_4$ is a non - polar molecule. Only dispersion forces are present as there is no significant electronegativity difference to create a dipole and no hydrogen - bonding conditions are met.

Step3: Analyze chloromethane ($CH_3Cl$)

$CH_3Cl$ is a polar molecule due to the presence of the electronegative Cl atom. Dispersion forces are present in all molecules. Dipole - dipole forces exist because of the molecular polarity. There is no hydrogen - bonding as the hydrogen is not bonded to a highly electronegative atom like N, O, or F.

Step4: Analyze carbon disulfide ($CS_2$)

$CS_2$ is a non - polar molecule (linear geometry cancels out bond dipoles). Only dispersion forces are present.

Answer:

compound	dispersion	dipole	hydrogen - bonding
methane ($CH_4$)	√
chloromethane ($CH_3Cl$)	√	√
carbon disulfide ($CS_2$)	√