The only intermolecular forces possiable between hexane and water are london dispersion forces because hexane only exhibits LDF while water is polar and exhibits LDF, dipole-dipole and hydrogen bonding.
For a hexane molecule, since it is not polar the intermolecular force that holds it together is London forces. Its the only force of attraction that can hold a nonpolar force to another.
Van der valls forces
I think its dispersion forces
non-polar molecular forces
dispersion AKA London forces only
hexafatelane
London Dispersion
No, they do not hold two compounds together. The forces that hold compounds together are intermolecular forces. Ionic and covalent bonds are intramolecular forces, and they hold the atoms of the molecule or formula unit together.
between molecules the forces are called intermolecular forces, and between the atoms in a molecule they are called inramolecular forces
1. Intermolecular forces are the forces between molecules, while chemical bonds are the forces within molecules. 2. Chemical bonds combine atoms into molecules, thus forming chemical substances, while intermolecular forces bind molecules together. 3. Chemical bonding involves the sharing or transferring of electrons, while intermolecular forces do not change the electron stucture of atoms. 4. Intermolecular forces hold objects together, while chemical bonds hold molecules together.
The intermolecular force that exists in HCI is Van der Waals. Ion-Ion forces are not present since H, C, and I are all gases. A hydrogen bond is not present since the H is bonded to a C and not a F, O, or N. The compound is not polar so it could not be dipole-dipole. Therefore, it must be Van der Waals since every compound has this molecular force.
NaOH has the higher melting point. The reason is since NaOH is an ionic compound, thus meaning that the intermolecular forces (the forces that hold the compound together) between Sodium+ and Hydroxide- are ionic - ionic forces. The charges keep them together. Ionic forces are ALOT stronger than other intermolecular forces such as dispersion, dipole-dipole, or even hydrogen bonding. CH3OH (Methanol) has a lower melting point that Sodium Hydroxide since the intermolecular forces it entails are: Dispersion, dipole-dipole, and hydrogen bonding between Hydrogen and Oxygen. It will take LESS energy to break these attractions, than the energy required to break the attraction forces between the ionic compound NaOH.
intermolecular forces D:
intermolecular forces examples are dispersion forces
London dispersion forces (also known as van der Waals forces) hold molecular solids together. or Intermolecular forces
No, they do not hold two compounds together. The forces that hold compounds together are intermolecular forces. Ionic and covalent bonds are intramolecular forces, and they hold the atoms of the molecule or formula unit together.
hydrogen bonds
Intermolecular force holds large numbers of different molecules together.