Question

Problem page what kind of intermolecular forces act between a dichlorine monoxide molecule and a hydrogen bromide molecule?

Answer 1

Answer:

Intermolecular forces present between $Cl_{2}O and HBr$ are- London force and ion-dipole force.

Explanation:

All molecules contain electrons. Therefore London dispersion force is present between all molecules.

$Cl_{2}O$ is an angular molecule. Also oxygen atom is more electronegative than Cl atom. Therefore $Cl_{2}O$ is dipolar.

HBr is a strong acid. Therefore it is dissociated completely to give $H^{+} and Br^{-}$.

Hence an ion-dipole attractive force operates between dipolar $Cl_{2}O$ and $H^{+} and Br^{-}$ ions.

Answer 2

Dichlorine monoxide has the same structure like that of water. So, this is a polar molecule. For polar molecules, the dominant intermolecular force would be dipole-dipole forces. For HBr, there is a force between two oppositely charged ions, H⁺ and Br⁻. So, the dominant intermolecular force is electrostatic attraction.