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 most important intermolecular force between nitrogen gas molecules is London dispersion forces, due to the nonpolar nature of N2. Although weaker than dipole-dipole or hydrogen bonding forces, London dispersion forces are still present in all molecules.
It's to do with the intermolecular bonds (the van Der Waals forces). If they are strong, the substance exists as a solid as the particles are held together with a strong force. If however they are weak, the substance will be a gas.
NO2 has a higher boiling point than CO2 because the nitrogen radii is larger than carbon. The bigger the atom the more intermolecular force that is created...this requires more energy to break causing a higher boiling point.
Among the options provided, nitrogen gas (N2) should have the lowest boiling point. Nitrogen is a diatomic molecule with weak van der Waals forces between its molecules, leading to a relatively low boiling point compared to ammonia (NH3), hydrogen fluoride (HF), water (H2O), and sodium sulfide (Na2S) which have stronger intermolecular forces due to hydrogen bonding or ionic interactions.
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.
The most important intermolecular force between nitrogen gas molecules is London dispersion forces, due to the nonpolar nature of N2. Although weaker than dipole-dipole or hydrogen bonding forces, London dispersion forces are still present in all molecules.
N2 has dispersion forces and covalent interactions between the two atoms due to the triple bond in it.
It's to do with the intermolecular bonds (the van Der Waals forces). If they are strong, the substance exists as a solid as the particles are held together with a strong force. If however they are weak, the substance will be a gas.
London or vanderwal force
NO2 has a higher boiling point than CO2 because the nitrogen radii is larger than carbon. The bigger the atom the more intermolecular force that is created...this requires more energy to break causing a higher boiling point.
Among the options provided, nitrogen gas (N2) should have the lowest boiling point. Nitrogen is a diatomic molecule with weak van der Waals forces between its molecules, leading to a relatively low boiling point compared to ammonia (NH3), hydrogen fluoride (HF), water (H2O), and sodium sulfide (Na2S) which have stronger intermolecular forces due to hydrogen bonding or ionic interactions.
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.
O2 has stronger London dispersion forces than N2 because O2 has more electrons, which allows for greater polarization and stronger temporary dipoles. This results in stronger attractive forces between O2 molecules compared to N2 molecules.
In vanderwaal's Equation 'a' measures the intermolecular force of attraction and 'b' measures the volume of the molecule. N2 has greater volume (due to it's larger size) and hence 'b' is greater for N2. NH3 has greater dipole moment and hence 'a' is greater for NH3.
yup. nitrogen gas-- N2
no
N2, OF2, and CH3OH exhibit only London dispersion forces. N2 is a nonpolar molecule, while OF2 and CH3OH have polar bonds but overall nonpolar structures which result in only London dispersion forces being present.