Which statement best describes the intermolecular forces between H2 molecules and NH3 molecules in the liquid phase?A.Van der Waals forces are the strongest force between H2 molecules, and hydrogen bonding is the strongest force between the NH3 molecules.B.Van der Waals forces are the strongest force between H2 molecules and between NH3 molecules.C.Dipole-dipole forces are the strongest force between H2 molecules, and Van der Waals forces are the strongest force between NH3 molecules.D.Hydrogen bonding is the strongest force between H2 molecules and between NH3 molecules.SUBMITarrow_backPREVIOUS

To determine the correct statement about the intermolecular forces between H2 molecules and NH3 molecules in the liquid phase, let's analyze the types of intermolecular forces present in each substance.

1. H2 Molecules:

   • H2 is a nonpolar molecule because it consists of two hydrogen atoms sharing electrons equally.
   • The primary intermolecular force in nonpolar molecules like H2 is Van der Waals forces (also known as London dispersion forces).

2. NH3 Molecules:

   • NH3 (ammonia) is a polar molecule due to the difference in electronegativity between nitrogen and hydrogen, and the molecule's trigonal pyramidal shape.
   • NH3 can form hydrogen bonds because it has a nitrogen atom with a lone pair of electrons and hydrogen atoms bonded to nitrogen.
   • Hydrogen bonding is the strongest intermolecular force in NH3.

Now, let's evaluate each statement:

A. Van der Waals forces are the strongest force between H2 molecules, and hydrogen bonding is the strongest force between the NH3 molecules.

• This statement is correct. Van der Waals forces are indeed the strongest force in H2, and hydrogen bonding is the strongest force in NH3.

B. Van der Waals forces are the strongest force between H2 molecules and between NH3 molecules.

• This statement is incorrect. While Van der Waals forces are the strongest in H2, hydrogen bonding is the strongest in NH3, not Van der Waals forces.

C. Dipole-dipole forces are the strongest force between H2 molecules, and Van der Waals forces are the strongest force between NH3 molecules.

• This statement is incorrect. H2 molecules do not have dipole-dipole forces because they are nonpolar. Additionally, Van der Waals forces are not the strongest in NH3; hydrogen bonding is.

D. Hydrogen bonding is the strongest force between H2 molecules and between NH3 molecules.

• This statement is incorrect. H2 molecules do not exhibit hydrogen bonding; they exhibit Van der Waals forces.

Therefore, the correct statement is:

A. Van der Waals forces are the strongest force between H2 molecules, and hydrogen bonding is the strongest force between the NH3 molecules.