Which of the bonding forces from the list below would need to be overcome to convert NH3 from a liquid to a gas? (Enter the letters in order of all that apply, e. g. AB, ABD, ACDE, etc.) A) Ionic B) Covalent C) Dispersion D) Dipolar E) Metallic F) Hydrogen G) Molecular H) None of the above

The bonding forces to overcome in order to convert NH₃ from a liquid to a gas, are (C) Dispersion (D) Dipolar and (F) Hydrogen. (CDF)

Explanation:

Ammonia is a polar molecule and exhibits dipole-dipole attraction, London dispersion forces and hydrogen bonding.

dipole-dipole attraction: This is the attraction of one polar molecule for another, due to opposite charged ends of the molecules. This bond needs to overcome to convert ammonia to gas.London dispersion forces: this is a bond or force between all molecules and it is present in ammonia, which must be overcome.hydrogen bonding: in ammonia (NH₃ ) hydrogen is bonded to nitrogen and creates hydrogen bonding. This bond, although a weak covalent bond must be overcome to convert ammonia (NH₃) from liquid to gas.

Therefore, the bonding forces to overcome in order to convert NH3 from a liquid to a gas, are (C) Dispersion (D) Dipolar (F) Hydrogen. (CDF)