Question

construct a table comparing the fiollowing intermolecular forces, dipole-dipoleinteractions, hydrogen bonds, and London Forces

Answer 1

Intermolecular forces name itself indicates that the attraction forces that are occuring between the molecules.

dipole-dipole interactions	London dispersion forces	hydrogen bond
They are observed in polar covalent molecules.	They are observed in polar or non polar covalent molecules and in all atoms.	Hydrogen bond is a weak electrostatic force of attraction that exists between covalently bonded hydrogen atom of one molecule and a highly electronegative atom(F.O and N atoms only) of another molecule.
These are observed between the positive dipole of one molecule and negative dipole of another molecule.	This attractive forces are due to the movement of electrons.At one instant electron dipoles are generated. These are the attractions between the electron dipole of one atom(which has partial negative charge )and the nucleus(positive charge) of another atom.	These are due to covalently bonded H-atom and a highly electronegative atom like F or O or N.
ex: HCl H-Cl-------H-Cl Where Cl attains $\delta$- charge and H attains partial positive ($\delta$+) charge.	Between identical atoms. ex: He , H2 , F2	Ex: HF , H2O, NH3 H-F --------H-F---------H-F The dashed line represents Hydrogen bonding.
Weaker than intermolecular hydrogen bond.	In case of heavier atoms (example iodine) these forces dominate over other interactions.	Stronger than dipole dipole interactions.
Observed when the electronegativity difference between the atoms is between 0.4 to 1.7	Observed when the electronegativity difference between the atoms is less than 0.4	If intermolecular H-bond is present then the molecules will have high boiling point than their analogous molecules. Ex: water has high boiling point than H2S