Which statement explains why H2O has a higher boiling point than N2?

Answer 1

In liquid ammonia one hydrogen atom from an adjacent molecule can form an

intermolecular hydrogen bond with the nitrogen atom of the central ammonia

molecule. With an average of only one

intermolecular bond per ammonia molecule, less thermal energy is required to

break the liquid ammonia into individual gas phase molecules. Therefore a lower

boiling temperature results.

In the case of liquid water, one hydrogen atom from each of two adjacent water

molecules can form an intermolecular hydrogen bond with each lone pair on the

oxygen atom of the central water molecule. As

such, a greater amount of thermal energy is required to break the extensive

hydrogen bonding network and a higher boiling temperature results.

Answer 2

H2, N2 and O2 are bonded by dispersion forces, while NH3 and H2O are both bonded by hydrogen bonding. Since hydrogen bonding is much stronger than dispersion forces, the boiling points of the molecules that have hydrogen bonding is much higher than the molecules that only have dispersion forces.

Answer 3

H2O has stronger intermolecular forces than N2