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O2, because it have more electrons than N2
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β 11y ago
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What type of intermolecular forces exist in N2?
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.
Which compound exhibits only London dispersion forces N2 HBr ICl5 PF5 OF2 CH3OH?
N2 IS CORRECT. The reason for this is because it is a non polar molecule, there are no polar bonds between each N-N atom and it the least polarizable of the ones listed.
Is N2 have a dipole moment?
N2 is a completely symmetrical molecule, therefore it has no dipole moment.
What molecules has a dipole moment A. O2 B. N2 C. CO2 D. HCl?
A. no dipole; only dissolutes using London dispersion forces B. same as A C. dipole outward towards 2 oxygens D. dipole towards chlorine atom
WHAT IS THE INTERMOLECULAR FORCE BETWEEN NF3 IN LIQUID STATE?
Every molecule has a london force (Induce dipole induce dipole force). In this molecule, the intermolecular force that hold these bonds together is dipole-diple interaction or dipolar interaction. There is no hydrogen bonding in here. If there is hydrogen bonding, H-atom must make bond with N,O,F. Therefore, intermolecular forces of NF3 is london force and dipole-diploe
What type of intermolecular forces exist in N2?
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.
What is the strongest intermolecular force in n2?
N2 has dispersion forces and covalent interactions between the two atoms due to the triple bond in it.
What is the intermolecular force of Nitrogen?
London or vanderwal force
Which is expected to have the largest dispersion forces CO2 C8H18 N2 C2H6?
C8h18
Which compound exhibits only London dispersion forces N2 HBr ICl5 PF5 OF2 CH3OH?
N2 IS CORRECT. The reason for this is because it is a non polar molecule, there are no polar bonds between each N-N atom and it the least polarizable of the ones listed.
Is N2 have a dipole moment?
N2 is a completely symmetrical molecule, therefore it has no dipole moment.
What molecules has a dipole moment A. O2 B. N2 C. CO2 D. HCl?
A. no dipole; only dissolutes using London dispersion forces B. same as A C. dipole outward towards 2 oxygens D. dipole towards chlorine atom
WHAT IS THE INTERMOLECULAR FORCE BETWEEN NF3 IN LIQUID STATE?
Every molecule has a london force (Induce dipole induce dipole force). In this molecule, the intermolecular force that hold these bonds together is dipole-diple interaction or dipolar interaction. There is no hydrogen bonding in here. If there is hydrogen bonding, H-atom must make bond with N,O,F. Therefore, intermolecular forces of NF3 is london force and dipole-diploe
What is the strongest molecular force that could occur between two molecules of each below?
Molecular Force Comparison What is the strongest molecular force that could occur between two molecules of each below? The strongest molecular force that could occur between two molecules is as follows: Hydrogen molecule (H2): Dipole-dipole interaction Oxygen molecule (O2): London Dispersion Forces Nitrogen molecule (N2): London Dispersion Forces Carbon dioxide (CO2): Dipole-dipole interaction Water (H2O): Hydrogen bonding Note: London Dispersion Forces are the weak attractive forces that occur between all molecules due to the fluctuation of their electron clouds. Dipole-dipole interactions are attractive forces between molecules that have a permanent dipole moment. Hydrogen bonding is a stronger attractive interaction that occurs between a hydrogen atom covalently bonded to a highly electronegative atom and another highly electronegative atom. πππ πππππ://π π π .ππππππππππΈπΊ.πππ/πππππ/πΉπ½πΈπ»π½πΌ/ππππππππ·πΈ/
Why N2 has lower boiling point then CO?
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.
Which statement explains why H2O has a higher boiling point than N2?
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.
Which of the following should have the lowest boiling point nh3 n2 hf H2O or na2s?
N2 would have the lowest BP because it has the weakest intermolecular forces.
