hydrogen bonding between the nitrogen of one molecule and the hydrogen of another, followed by dipole-dipole interactions and finally the very weak but ever present Van Der Waals forces.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
attractive force present between ammonia ions repulsive force also exist but not at high rate
NH3 exhibits hydrogen bonding in addition to dispersion forces. This significantly increases the intermolecular force, and raises the boiling point. PH3 does not exhibit hydrogen bonding and the dominant intermolecular force holding these molecules together is dispersion forces. (Dispersion forces also known as Van Der Waal Force)
Ion-dipole force
Dipole forces and London forces are present between these molecules.
predominant force
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
attractive force present between ammonia ions repulsive force also exist but not at high rate
The molecule CH3Cl has covalent bonds. In all chemical bonds, the type of force involved is electromagnetic.
Since the covalent bond between sulfur and oxygen is polar, dipole dipole attractions are present as intermolecular forces.
Induced dipole forced
AgNO3 is an ionic compound- so no molecules!
No, covalency does not have its own intermolecular force
force of attraction between molecules in solid is very great due to strong cohesive force holding them together
The intermolecular forces are London dispersion forces.C2H4 is ethene molecule. The bonding is calledthe covalent compound,which the molecules share their electrons in order to achieve the stable electron arrangement.
London Force
Solid state matter has maximum intermolecular force.