Question

What is the strongest type of intermolecular force between solute and solvent in each solution?

1. ${\mathbf{CH}}_{\mathbf{3}}{\mathbf{OCH}}_{\mathbf{3}}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$
   
2. $\mathbf{Ne}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$
   
3. ${\mathbf{N}}_{\mathbf{2}}\left(\mathbf{g}\right){\mathbf{inC}}_{\mathbf{4}}{\mathbf{H}}_{\mathbf{10}}\left(\mathbf{g}\right)$
   

Short answer

1. ${\mathbf{CH}}_{\mathbf{3}}{\mathbf{OCH}}_{\mathbf{3}}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$: Hydrogen bonding
2. $\mathbf{Ne}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$: London Dispersion force
3. ${\mathbf{N}}_{\mathbf{2}}\left(\mathbf{g}\right){\mathbf{inC}}_{\mathbf{4}}{\mathbf{H}}_{\mathbf{10}}\left(\mathbf{g}\right)$: London Dispersion force

Step-by-step solution

Definition of intermolecular force

In a solution, the intermolecular force is defined as the attractive force among the molecules of solute and solvent which is determined by from the relative strength within and between the solute and the solvent.

Respective intermolecular force between solute and solvent in each solution

${\mathbf{CH}}_{\mathbf{3}}{\mathbf{OCH}}_{\mathbf{3}}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$:Hydrogen bonding

Hydrogen bonding is the strongest because of the polar ether molecule dissolves in polar solvent i.e., water.

$\mathbf{Ne}\left(\mathbf{g}\right){\mathbf{inH}}_{\mathbf{2}}\mathbf{O}\left(\mathbf{l}\right)$: London Dispersion force

Neon is nonpolar in nature, so the strongest intermolecular force between neon and water is London Dispersion force.

${\mathbf{N}}_{\mathbf{2}}\left(\mathbf{g}\right){\mathbf{inC}}_{\mathbf{4}}{\mathbf{H}}_{\mathbf{10}}\left(\mathbf{g}\right)$: London Dispersion force

Both nitrogen and butane are nonpolar in nature, so the strongest intermolecular force between nitrogen and butane is London Dispersion force.