CO2 from the given compounds does not have dipole-dipole forces as its strongest force. While the other given compounds including CH2Br2, CH3Br, CHCl3 and CH3OCH3 have dipole-dipole forces as their strongest forces.
Further explanation:
CO2:
CO2 is a non polar molecule although it has polar bonds between its central carbon atom and two oxygen atoms. The dipoles are pointing in opposite direction so they cancel out each other and hence it only has London dispersion forces. The carbon and oxygen both are non metals so carbon dioxide has covalent bond in it.
CH2Br2, CH3Br and CHCl3:
In the compound CH2Br2, CH3Br and CHCl3, there exists an electronegative difference between the carbon atom and the halogen atom (Br or Cl). So these compounds have dipole-dipole forces in them these are polar compounds as well. In compound CH2Br2 both the dipole-dipole and London dispersion forces are present.
CH3OCH3:
The given compound is dimethyl ether. The carbon and oxygen bonds in methoxy methane (or dimethyl ether) are polar. It has angular geometry. There are dipole-dipole and London dispersion forces present in this molecule.
Dipole-dipole forces:
These are the attractive forces which are present between positive end of one polar molecule and the negative end of the other polar molecule. These are one percent as effective as a covalent bond.
Answer details
Subject: Chemistry
Level: College
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