Question

List the types of intermolecular forces that exist between molecules (or basic units) in each of the following species: (a) benzene (C6H6), (b) CH3Cl,
(c) PF3, (d) NaCl, (e) CS2.

Answer 1

Benzene (C6H6) = nonpolar molecules . Dispersion forces are present only. Chloroform (CH3Cl)= polar molecules . Dispersion and dipole-dipole forces are present. Phosphorus trifluoride (PF3) molecules are polar. Dispersion and dipole-dipole forces are present. Sodium chloride (NaCl) = ionic compound. Ion-ion and dispersion forces are present. Carbon disulfide (CS2) = nonpolar molecules . Dispersion forces are present only.

Answer 2

Answer:

Answer has been given below

Explanation:

• Every molecules contain electrons. So, London dispersion force exists in all molecules.
• For polar aprotic molecules, additional dipole-dipole force exists between molecules.
• For ionic compounds, additional ionic interaction force exist between ions.
• For non polar molecules, only London dispersion force exists between molecules.
• Benzene is a non-polar molecule. So London dispersion force exists between benzene molecules.
• $CH_{3}Cl$ is a polar molecule. So, dipole-dipole force and London dispersion force exists between $CH_{3}Cl$ molecules.

• $PF_{3}$ is a polar molecule. So, dipole-dipole force and London dispersion force exists between $PF_{3}$ molecules.
• NaCl is an ionic compound. So London dispersion force and ionic interaction force exists between NaCl molecules.
• $CS_{2}$ is a nonpolar molecule. So, London dispersion force exists between $CS_{2}$ molecules.