van de walls,
by shabbir makai
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.
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.
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
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.
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.
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.
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.
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.
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... :)
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.
The liquid state is caused by intermolecular forces.
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
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.
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.
If the intermolecular forces are great enough they can hold the molecules together as a liquid. If they are even stronger they will hold the molecules together as a solid. Water has nearly the same mass as methane and ammonia molecules, but the greater molecular forces between water molecules causes the water to be liquid at room temperature, while ammonia and methane, with weaker intermolecular forces, are gases at room temperature.
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.
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.