Question

what is the strongest type of intermolecular force between solute and solvent in each solution?
a.) Cu (s) in Ag (s)
b.) CH3CH3 (g) in CH3CH2CH2NH2 (l)
c.) CH3Cl (g) in CH3OCH3 (g)

My guess would be:
a.) they are 2 different metals that are monotomic ions so...ionic bonding?
b.) the first is nonpolar? and second is polar? so....dipole induced dipole? or is the second nonpolar?
C.) H-bonding with the O and H? or would it be dipole -dipole because they're both polar?

Thanks!

Answer 1

Concepts and reason

The set of repulsive and attractive forcesbetween molecules that result from the polarity is represented as intermolecular force. There are four types of intermolecular forces; they are given below:

• Hydrogen bonding,

• London dispersion force,

• Ion-dipole force,

• Dipole-dipole force.

Fundamentals

Ion-dipole force is an intermolecular interaction that arises due the induced dipole moment in non-polar molecules by ions.

Hydrogen bond: Hydrogen is bonded to strong electronegative atoms.

Dipole-dipole: This force takes place between two polar compounds.

London dispersion force: This force is present in all compounds (weak force).

(a)

Both the constituents of the alloys are metals in their neutral state. They are composed of neutral atoms. Hence, the forces prevalent between the solute $\left( {{\rm{Cu}}} \right)$ and the solvent $\left( {{\rm{Ag}}} \right)$ would be weak London forces.

(b)

${\rm{Ethane}}$ molecules are non-polar. ${\rm{Propanamine}}$ molecules are slightly polar. Thus, there could be dipole-induced dipole interactions.

(c)

${\rm{Chloromethane}}$ and ${\rm{dimethyl}}\,{\rm{ether}}$ are both polar molecules with a significant dipole moment for each. Thus, the strongest interaction would be a dipole-dipole interaction.

Ans: Part a

The prevalent forces would be London dispersion forces.

Part b

The prevalent forces are dipole-induced dipole interactions.

Part c

The strongest interactions are dipole-dipole interactions.