obesity
The main interaction between CH4 molecules are London dispersion forces, which result from temporary dipoles induced in the molecules. These forces are relatively weak compared to other intermolecular forces like hydrogen bonding.
It is intermolecular force of attraction, it may be 1- dipole - dipole interaction, 2- vander waal's force of attraction.
The intermolecular bonds between water molecules are hydrogen bonds.
Dispersion
i don't know kidding it means...........
Intermolecular because intermolecular forces occur between molecules, not within the same molecule. Specifically the forces are London dispersion forces, due to the interaction of instantaneous dipoles.
Intermolecular describes the interactions between separate molecules.
The main interaction between CH4 molecules are London dispersion forces, which result from temporary dipoles induced in the molecules. These forces are relatively weak compared to other intermolecular forces like hydrogen bonding.
A volatile liquid is easy to vaporize because there are weak intermolecular attractions between its molecules. A nonvolatile liquid is difficult to vaporize because there are strong intermolecular attractions between its molecules.
It is intermolecular force of attraction, it may be 1- dipole - dipole interaction, 2- vander waal's force of attraction.
The strongest intermolecular force between two molecules of water in ice is hydrogen bonding.
Intermolecular attraction
Yes, the vapor pressure decreases as the strength of intermolecular forces between molecules increases.
The intermolecular force of ClF is dipole-dipole interaction. This is because ClF is a polar molecule, with a significant difference in electronegativity between chlorine and fluorine causing a partial positive and partial negative charge, leading to attraction between the molecules.
Intermolecular spaces refer to the empty spaces or gaps between molecules in a substance. These spaces determine the physical properties of the substance, such as density and compressibility. The size of intermolecular spaces can affect how closely packed molecules are in a material.
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.
Polar molecules have a dipole moment and they have intermolecular forces that include dipole-dipole interaction. A hydrogen bond is the attraction between a hydrogen bonded to N, O, F atom with N, O, F lone pair. Small molecules that exhibit this effect are HF, H2O and NH3. The example molecules are all polar. The hydrogen bond interaction is stronger than a normal dipole-dipole interaction.