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The boiling point of the fluoromethane (CH3F) is higher than
Diflourine (F-F).
What are the point differences in terms of intermolecular forces?
1. London dispersion forces:
The London dispersion exerts a force of between all molecules. The intensity of the LDF is proportional to the polarizability of the molecule, which depends on the number of electrons and the surface area of the molecule. In the past, the London Scattered Force has been the weakest of the three van der Waals forces. Contrary to what some teachers and some authors say, London dispersion forces are often stronger than Keysome or Debye forces, surpassed only by hydrogen bonding. Some teachers are guilty of telling students that the strength of the London dispersion force depends on its molar mass. This is just a coincidence. Understand, however, that molar mass is not the reason for the fluctuations in the strength of the London dispersion force.
2. Keesom forces (dipole-dipole attraction):
The force by which one polar molecule attracts another polar molecule. The oppositely charged ends of the molecule experience electrostatic attraction.
3. Debye forces (induced attraction) :
The attractive force between polar and nonpolar molecules, where the polar molecule induces charge separation in the nonpolar molecule. Debye forces can exist between two polar molecules, even for similar molecules. In such cases, the induced charge can temporarily increase or decrease the material's dipole moment.
4. Hydrogen Bonds
A weak covalent bond between a hydrogen atom of a molecule attached to an N, O, or F and an N, O, or F of an adjacent molecule. A hydrogen atom acts as a bridge and forms a bond between two molecules. Hydrogen bonding is more than electrostatic attraction between molecules, instead there is evidence of orbital overlap and covalent bond formation.
Therefore, The boiling point of the fluoromethane (CH3F) is higher than
Diflourine (F-F).
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