When comparing h2, nh3, o2, and ch4, which of the following statements is correct? a. ch4 has the highest boiling point because it experiences dipole-dipole forces. b. h2 has the strongest intermolecular forces because it has the lowest mass. c. nh3 has the highest boiling point because it experiences hydrogen bonding. d. o2 has the strongest intermolecular force because it experiences london dispersion forces.

c. NH3 has the highest boiling point because it experiences hydrogen bonding.

Explanation:

NH3 has three N-H polar covalent bonds with N and H having partial negative and positive charges respectively. The partial negative dipole of N from one NH3 molecule forms a hydrogen bond with the partial positive dipole of H from one NH3 molecule.  

δ- δ+   δ- δ+

N-H...N-H

Thus NH3 experiences hydrogen bonding and has the highest boiling point.  

The C-H bond in CH4 is nonpolar. Dipoles exist in polar covalent bonds. Hence option A is incorrect.  

Higher the molecular mass the greater is the intermocleuclar force of attraction. Hence option C is incorrect.  

London dispersion forces are weaker intermolecular forces than hydrogen bonding. Hence option D is incorrect.