Order of Boiling Point in CHCl3, CH2Cl2, CH3Cl, and CCl4
Understanding the boiling point of different compounds involves considering their intermolecular forces. The strength of these forces determines the energy required to overcome them and transition from the liquid phase to the gas phase.

Chloroform (CHCl3)
- Chloroform is a polar molecule with a net dipole moment due to the difference in electronegativity between carbon and chlorine.
- It can form dipole-dipole interactions and London dispersion forces, making it have moderate boiling points.
- However, the presence of three chlorine atoms increases the molecular weight, leading to stronger van der Waals forces compared to the other compounds.

Dichloromethane (CH2Cl2)
- Dichloromethane is also a polar molecule with dipole-dipole interactions and dispersion forces.
- It has a lower boiling point than chloroform due to the smaller molecular weight and lesser number of chlorine atoms.

Chloromethane (CH3Cl)
- Chloromethane is a polar molecule with dipole-dipole interactions and dispersion forces.
- It has the lowest boiling point among the chlorinated compounds considered due to its smaller molecular weight and weaker intermolecular forces.

Carbon Tetrachloride (CCl4)
- Carbon tetrachloride is a nonpolar molecule, resulting in only London dispersion forces between its molecules.
- Despite its larger molecular weight compared to the chloroform, the absence of dipole-dipole interactions leads to a lower boiling point compared to CHCl3.