What kind of intermolecular forces act between a dichloroethylene (CHCl2) molecule and dichlorine monoxide molecule?
The Correct Answer and Explanation is:
Answer:
The intermolecular forces acting between a dichloroethylene (CHCl₂) molecule and a dichlorine monoxide (Cl₂O) molecule are primarily dipole-dipole interactions and London dispersion forces (LDFs).
Explanation
Intermolecular forces are the attractive forces between molecules that influence the physical properties of substances, such as boiling point, solubility, and state of matter. The strength and type of these forces depend on the molecular structure and polarity of the molecules involved.
1. Molecular Structure and Polarity:
- Dichloroethylene (CHCl₂): This molecule consists of a carbon-carbon double bond (C=C) with two chlorine atoms and two hydrogen atoms (depending on isomer). In the most relevant isomer here, 1,1-dichloroethylene (CH₂=CCl₂), the two electronegative chlorine atoms are bonded to the same carbon, creating a polar molecule. The molecule has a permanent dipole moment due to the electron-withdrawing effect of the chlorines.
- Dichlorine monoxide (Cl₂O): Cl₂O has a bent molecular geometry similar to water, with a lone pair on the oxygen atom. The difference in electronegativity between Cl and O makes Cl₂O polar as well, with a net dipole pointing toward the oxygen.
2. Types of Intermolecular Forces Present:
- Dipole-Dipole Interactions: Because both CHCl₂ and Cl₂O are polar molecules, they will experience dipole-dipole interactions. These occur when the partial positive charge on one molecule is attracted to the partial negative charge on another.
- London Dispersion Forces (LDFs): These are weak, temporary forces caused by the instantaneous distribution of electrons. LDFs are present between all molecules, regardless of polarity. Since both CHCl₂ and Cl₂O have relatively large electron clouds (especially with chlorine atoms), their LDFs are stronger than those in smaller molecules.
3. No Hydrogen Bonding: Although oxygen is present in Cl₂O, hydrogen bonding does not occur because neither molecule contains hydrogen directly bonded to a highly electronegative atom (O, N, or F).
In summary, the intermolecular forces between dichloroethylene and dichlorine monoxide are dipole-dipole interactions and London dispersion forces.
