Inter Molecular Forces

Inter Molecular Forces are forces of attraction or repulsion which act between neighboring molecules. London Dispersion, Dipole Dipole, and Hydrogen Bonding are three inter molecular forces.

 London Dispersion- is when electrons in adjacent molecules are located in positions that can give the molecule a temporary pole or charge.  These are also called delta charges and can be positive and negative.

Dipole Dipole- is the attractive end of one molecule and the positive end of another molecule.  This can only take place in a polar (also know as charged) molecule.  Chloroform can also use London Dispersion.

Hydrogen Bonding- is a type of Dipole Dipole that only occurs in some polar molecules.  It is a force that attracts the Hydrogen of one molecule to the Nitrogen, Oxygen or Fluorine of another molecule.

The image above only illustrates Dipole Dipole forces because london Dispersion is an ongoing force.

          Two inter molecular forces that are active between two molecules of CHCl3 are Dipole Dipole, because it is a polar molecule, and London dispersion, because all molecules use them. 

     
       
          CHCl3 does not use Hydrogen bonding because it does no contain the atoms N, O, or F for the Hydrogen to bond to.

The red arrows show the flow of energy from lesser negativity to a higher negativity.  This helps explain that chlorine is a delta negative and Hydrogen is a Delta Positive (delta means temporary charge).  This is why the hydrogen atom in chloroform can bond with one of the chlorine atoms in another chloroform molecule.