Intermolecular forces are the attractive or repulsive interactions between molecules. These forces determine the physical properties of substances, such as melting and boiling points, viscosity, and solubility.
Ionic compounds have much stronger intermolecular forces compared to covalent compounds. This is because ionic compounds are formed by the transfer of electrons between atoms, creating strong electrostatic attractions between the oppositely charged ions.
No, ionic compounds do not have London dispersion forces. These forces are only present in covalent compounds where there are temporary dipoles created by the uneven distribution of electrons.
No, hydrogen bonds are not present in ionic compounds. Hydrogen bonds occur when a hydrogen atom is bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine. In ionic compounds, the bonds are between a metal and a nonmetal, so there is no hydrogen atom present.
Strong intermolecular forces in ionic compounds result in high melting and boiling points, as well as a high degree of solubility in polar solvents. These compounds also tend to be brittle and have high lattice energies due to the strong forces holding the ions together in a crystal lattice structure.