hydrogen bond
The strongest intermolecular force that NH3 will exhibit is hydrogen bonding. NH3 molecules can form hydrogen bonds with other NH3 molecules or with other molecules containing a hydrogen atom bonded to a highly electronegative atom such as nitrogen, oxygen, or fluorine.
The most significant intermolecular force in NH3 is hydrogen bonding. This occurs due to the large electronegativity difference between nitrogen and hydrogen, creating a strong dipole-dipole interaction.
The most significant intermolecular force in NH3 is hydrogen bonding. This is due to the presence of a hydrogen atom bonded to a highly electronegative nitrogen atom, leading to a strong dipole-dipole interaction with neighboring ammonia molecules.
H20 is water.HF is hydrogen fluoride.NH3 is ammonia.
In NH3 (ammonia), the intermolecular forces present are hydrogen bonding, which occurs between the hydrogen atom on one NH3 molecule and the lone pair of electrons on the nitrogen atom of another NH3 molecule. This is a type of dipole-dipole attraction.
The strongest intermolecular force that NH3 will exhibit is hydrogen bonding. NH3 molecules can form hydrogen bonds with other NH3 molecules or with other molecules containing a hydrogen atom bonded to a highly electronegative atom such as nitrogen, oxygen, or fluorine.
The most significant intermolecular force in NH3 is hydrogen bonding. This occurs due to the large electronegativity difference between nitrogen and hydrogen, creating a strong dipole-dipole interaction.
The most significant intermolecular force in NH3 is hydrogen bonding. This is due to the presence of a hydrogen atom bonded to a highly electronegative nitrogen atom, leading to a strong dipole-dipole interaction with neighboring ammonia molecules.
H20 ice and, its liquids H20/NH3.
H20 is water.HF is hydrogen fluoride.NH3 is ammonia.
BCl3 and NH3 would exhibit dipole-dipole intermolecular forces, as they have polar bonds. CF4, CO2, and Cl2 would not exhibit dipole-dipole forces, as they are nonpolar molecules.
Nh3 + h20 <-> nh4+ + oh-
In the liquid state of ammonia (NH3), the predominant intermolecular force is hydrogen bonding. This occurs due to the presence of a nitrogen atom bonded to hydrogen, where the nitrogen atom is highly electronegative, creating a dipole moment. The hydrogen bonds between NH3 molecules are responsible for its relatively high boiling point compared to similar-sized molecules that only exhibit weaker van der Waals forces. Additionally, dipole-dipole interactions also play a role, but hydrogen bonding is the dominant force.
In NH3 (ammonia), the intermolecular forces present are hydrogen bonding, which occurs between the hydrogen atom on one NH3 molecule and the lone pair of electrons on the nitrogen atom of another NH3 molecule. This is a type of dipole-dipole attraction.
The pair of molecules with the strongest dipole-dipole interactions would be NH3-NH3 because ammonia (NH3) is a polar molecule with a significant dipole moment, leading to stronger attractions compared to the other options listed.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
Hydrogen bonding is strongest in molecules of H2O (water) because oxygen is highly electronegative, creating a large difference in electronegativity between the hydrogen and oxygen atoms which strengthens the hydrogen bonding.