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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
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∙ 11y ago
The intermolecular force between NF3 molecules in the liquid state is primarily dipole-dipole interactions. This is because NF3 is a polar molecule with a permanent dipole moment due to the difference in electronegativity between nitrogen and fluorine atoms. These dipole-dipole interactions result in the attraction between neighboring NF3 molecules in the liquid state.
Wiki User
∙ 12y agodipole-dipole i believe! the only molecules that have hydrogen bonding are the ones with either OH, HF, and NH. and i believe the only London forces are non polar! I hope i'm not wrong here, but good luck anyways!
Wiki User
∙ 8y agoNF3 is a polar molecule, but it lacks the hydrogen bonding that water has, so its chief intermolecular force is dipole-dipole interaction. (there is also some dispersion force associated with NF3 as well, but it is quite small by comparison.)
Wiki User
∙ 12y agoN2 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.
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∙ 13y agodipole-dipole and dispersion forces.
Wiki User
∙ 13y agodipole-dipole
Wiki User
∙ 11y agoDispersion and dipole-dipole forces.
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What is the intermolecular force between BF3 in liquid state?
The intermolecular force between BF3 molecules in liquid state is London dispersion forces. This is because BF3 is a nonpolar molecule and London dispersion forces are the primary intermolecular force among nonpolar molecules.
What intermolecular forces explain why water is a liquid at room temperature?
Hydrogen bonding is the intermolecular force responsible for water being a liquid at room temperature. The hydrogen bonds between water molecules are relatively strong, allowing them to remain in a liquid state rather than vaporizing at room temperature.
Why is ethanol liquid?
Ethanol is a liquid at room temperature due to its intermolecular forces. The strong hydrogen bonding between ethanol molecules requires more energy to break the bonds, keeping it in a liquid state.
What is the relationship between the strength of intermolecular forces and phase change and density?
Stronger intermolecular forces generally lead to higher melting and boiling points, which are phase changes from solid to liquid and liquid to gas, respectively. Higher intermolecular forces also tend to result in higher densities due to molecules being more tightly packed together in the solid or liquid state.
What are Factors affecting state of a substance?
Factors affecting the state of a substance include temperature, pressure, and the intermolecular forces between the particles of the substance. Changes in these factors can lead to a substance transitioning between solid, liquid, and gas states.
What is the intermolecular force between BF3 in liquid state?
The intermolecular force between BF3 molecules in liquid state is London dispersion forces. This is because BF3 is a nonpolar molecule and London dispersion forces are the primary intermolecular force among nonpolar molecules.
When 2 molecules of a solid are kept some distance apart and the force between them is measured solid is then melted to form a liquid. Two molecules are now kept the same distance apart and the force?
The force between the molecules in the liquid state will be weaker compared to the solid state. This is because the intermolecular forces holding the molecules together in a liquid are generally weaker than those in a solid.
What is responsible for holding water molecules together in the liquid state?
The main intermolecular force holding water molecules together in hydrogen bonding. Also, there are diplole-dipole interactions and London dispersion forces. But hydrogen bonds are the major force keeping water in the liquid state.
What intermolecular forces explain why water is a liquid at room temperature?
Hydrogen bonding is the intermolecular force responsible for water being a liquid at room temperature. The hydrogen bonds between water molecules are relatively strong, allowing them to remain in a liquid state rather than vaporizing at room temperature.
Which matter has the maximum intermolecular force?
Solid matter typically has the maximum intermolecular forces compared to liquids and gases. This is because the particles in a solid are closely packed together, allowing for stronger attractions between them such as van der Waals forces, hydrogen bonding, and dipole-dipole interactions.
Does water expand when heated and why?
Yes... When water is heated, the intermolecular force of attraction between water atoms become weak and they start losing the intermolecular force of attraction... at temperature known as boiling point of water this intermolecular force become so weak that water lose its state and converts into gasious state... but this expansion is not considerable... :)
Why is ethanol liquid?
Ethanol is a liquid at room temperature due to its intermolecular forces. The strong hydrogen bonding between ethanol molecules requires more energy to break the bonds, keeping it in a liquid state.
Do inter-molecular forces occur as a result of being in the liquid state or does a liquid state exist because of inter-molecular forces?
The liquid state is caused by intermolecular forces.
What is the relationship between the strength of intermolecular forces and phase change and density?
Stronger intermolecular forces generally lead to higher melting and boiling points, which are phase changes from solid to liquid and liquid to gas, respectively. Higher intermolecular forces also tend to result in higher densities due to molecules being more tightly packed together in the solid or liquid state.
What force has to be overcome in order to change a solid into a liquid?
The force that has to be overcome is the intermolecular forces holding the solid particles in place. As heat is applied, these forces weaken, allowing the particles to move more freely and change from a solid to a liquid state.
What is the importance of intermolecular forces with regards to state of matter?
Intermolecular forces are responsible for holding molecules together in a substance, determining its physical properties such as melting point, boiling point, and viscosity. The strength of these forces influences the state of matter a substance is in (solid, liquid, gas), as they dictate how close together molecules can pack and how easily they can move past each other.
What are Factors affecting state of a substance?
Factors affecting the state of a substance include temperature, pressure, and the intermolecular forces between the particles of the substance. Changes in these factors can lead to a substance transitioning between solid, liquid, and gas states.
