Yes nitrogen does have dispersion forces due to the Lewis structure of the nitrogen.
Yes, the London dispersion force is very weak.
Please be more specific about who do you refer to as "he", when you ask about dispersion force. This way you can get an exact answer.
Dipole-dipole and dispersion
dispersion force (London)
N2 is a linear molecule represented by two nitrogen atoms held together by a triple bond. Since this bond is non-polar, the only force present is the London Dispersion force.
The dispersion force is responsible for holding nitrogen crystals together
LiF - dispersion force and ionic bonding BeF_2 - dispersion force and ionic bonding BF_3 - dispersion force CF_4 - dispersion force NF_3 - dispersion force and diople-diople interaction OF_2 - dispersion force and diople-diople interaction F_2 - dispersion force They all have at least dispersion force
Yes, the London dispersion force is very weak.
Please be more specific about who do you refer to as "he", when you ask about dispersion force. This way you can get an exact answer.
Dispersion forces
Dipole-Dipole and covalent sigma bond forces.
Dipole-dipole and dispersion
dispersion force (London)
N2 is a linear molecule represented by two nitrogen atoms held together by a triple bond. Since this bond is non-polar, the only force present is the London Dispersion force.
Correct answers from Mastering Chemistry: NH3 - hydrogen bonding CH4 - Dispersion forces NF3 - dipole-dipole
London or vanderwal force
Dispersion forces