Question

What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (ch3oh), carbon tetrabromide (cbr4), and dichloromethane (ch2cl2)?

Answer 1

The predominant force in methanol would be the hydrogen bonding due to the presence of OH. For carbon tetrachloride, london dispersion forces is dominant. Ultimately, for methyl chloride, the most prevailing intermolecular force would be dipole-dipole because of the presence of a positive end and a negative end of the molecule.

Step-by-step explanation:

Answer 2

The predominant force in methanol would be the hydrogen bonding due to the presence of OH. For carbon tetrachloride, london dispersion forces is dominant. Ultimately, for methyl chloride, the most prevailing intermolecular force would be dipole-dipole because of the presence of a positive end and a negative end of the molecule.